Electrovalent bonding
1. Which forms a crystal of NaCl [CPMT 1972; NCERT 1976; DPMT 1996] (a) molecules (b) Na and Cl ions (c) Na and Cl atoms (d) None of the above 2. When sodium and chlorine reacts then [NCERT 1973] (a) Energy is released and ionic bond is formed (b) Energy is released and a covalent bond is formed (c) Energy is absorbed and ionic bond is formed (d) Energy is absorbed and covalent bond is formed 3. Which one is least ionic in the following compounds [CPMT 1976; BHU 1998] (a) AgCl (b) KCl
(c) BaCl2 (d) CaCl2 4. The electronic configuration of four elements L, P, Q and R are given in brackets L 1s2, 2s2 2p4 ; Q 1s2, 2s2 2p6, 3s2 3p5 P 1s2, 2s2 2p6, 3s1 ; R 1s2, 2s2 2p6, 3s2 The formulae of ionic compounds that can be formed between these elements are [NCERT 1983]
(a) L2P, RL, PQ and R2Q (b) LP, RL, PQ and RQ
(c) P2L, RL, PQ and RQ2 (d) LP, R2L, P2Q and 5. Electrovalent compound's [MP PMT 1984] (a) Melting points are low (b) Boiling points are low (c) Conduct current in fused state (d) Insoluble in polar solvent 6. A electrovalent compound is made up of [CPMT 1978, 81; MNR 1979] (a) Electrically charged molecules (b) Neutral molecules (c) Neutral atoms (d) Electrically charged atoms or group of atoms 7. Electrovalent bond formation depends on (a) Ionization energy (b) Electron affinity (c) Lattice energy (d) All the three above 8. In the following which substance will have highest boiling point [NCERT 1973; MP PMT 1990]
(a) He (b) CsF
(c) NH 3 (d) CHCl3 9. An atom of sodium loses one electron and chlorine atom accepts one electron. This result the formation of sodium chloride molecule. This type of molecule will be [MP PMT 1987] (a) Coordinate (b) Covalent (c) Electrovalent (d) Matallic bond 10. Formula of a metallic oxide is MO. The formula of its phosphate will be [CPMT 1986, 93]
(a) M2 PO4 2 (b) MPO4
(c) M2PO4 (d) M3 PO4 2 11. From the following which group of elements easily forms cation (a) F, Cl, Br (b) Li, Na, K (c) O, S, Se (d) N, P, As 12. Which type of compounds show high melting and boiling points [CPMT 1996] (a) Electrovalent compounds (b) Covalent compounds (c) Coordinate compounds 23. In the transition of Zn atoms to Zn ions there is a decrease in (d) All the three types of compounds have equal melting and the [CPMT 1972] boiling points (a) Number of valency electrons 13. Lattice energy of an ionic compound depends upon (b) Atomic weight [AIEEE 2005] (c) Atomic number (a) Charge on the ion only (d) Equivalent weight (b) Size of the ion only 24. Phosphate of a metal M has the formula M PO . The formula (c) Packing of ions only 3 4 2 (d) Charge on the ion and size of the ion for its sulphate would be 14. In the given bonds which one is most ionic [CPMT 1973; MP PMT 1996]
[EAMCET 1980] (a) MSO 4 (b) MSO4 2 (a) Cs Cl (b) Al Cl (c) M 2 SO4 3 (d) M 3 SO4 2 (c) C Cl (d) H Cl 25. The molecular formula of chloride of a metal M is MCl . The 15. Element x is strongly electropositive and y is strongly 3 formula of its carbonate would be [CPMT 1987] electronegative. Both element are univalent, the compounds formed from their combination will be [IIT 1980] (a) MCO3 (b) M 2 CO 3 3 (a) x y (b) x y (c) M 2CO 3 (d) MCO 3 2 (c) x y (d) x y 26. Sodium chloride easily dissolves in water. This is because 16. In the formation of NaCl from Na and Cl [CPMT 1985] [NCERT 1972; BHU 1973] (a) Sodium and chlorine both give electrons (a) It is a covalent compound (b) Sodium and chlorine both accept electrons (b) Salt reacts with water (c) Sodium loses electron and chlorine accepts electron (c) It is a white substance (d) Sodium accepts electron and chlorine loses electron (d) Its ions are easily solvated 17. Which of the following is an electrovalent linkage 27. When is dissolved in water the sodium ion becomes [CPMT 1974; DPMT 1984, 91; AFMC 1988] [NCERT 1974; CPMT 1989; MP PMT 1999]
(a) CH 4 (b) MgCl2 (a) Oxidized (b) Reduced (c) Hydrolysed (d) Hydrated (c) SiCl4 (d) BF3 18. Electrovalent compounds do not have [CPMT 1991] 28. Solid is a bad conductor of electricity since (a) High M.P. and Low B.P. (b) High dielectric constant [AFMC 1980] (c) High M.P. and High B.P. (d) High polarity (a) In solid there are no ions 19. Many ionic crystals dissolve in water because (b) Solid is covalent [NCERT 1982] (a) Water is an amphiprotic solvent (c) In solid there is no motion of ions (b) Water is a high boiling liquid (d) In solid there are no electrons (c) The process is accompanied by a positive heat of solution 29. Favourable conditions for electrovalency are (d) Water decreases the interionic attraction in the crystal (a) Low charge on ions, large cation, small anion lattice due to solvation (b) High charge on ions, small cation, large anion 20. The electronic structure of four elements A, B, C, D are (c) High charge on ions, large cation, small anion (A) 1s 2 (B) 1s 2 , 2s 2 2p 2 (d) Low charge on ions, small cation, large anion 30. The sulphate of a metal has the formula M SO . The formula (C) 1s 2 , 2s 2 2p 5 (D) 1s 2 , 2s 2 2p 6 2 4 3 for its phosphate will be The tendency to form electrovalent bond is largest in [DPMT 1982; CPMT 1972; MP PMT 1995] [MNR 1987, 95] (a) MHPO4 (b) (a) A (b) B 2 (c) (d) (c) C (d) D 31. Ionic bonds are usually formed by combination of elements with [CBSE PMT 1993; MP PMT 1994] 21. Chloride of metal is MCl . The formula of its phosphate will be [CPMT 1979] 2 (a) High ionisation potential and low electron affinity (a) M 2 PO4 (b) M 3 PO4 2 (b) Low ionisation potential and high electron affinity (c) High ionisation potential and high electron affinity (c) M 2 PO4 3 (d) MPO4 (d) Low ionisation potential and low electron affinity 22. The phosphate of a metal has the formula . The formula of 32. Molten sodium chloride conducts electricity due to the presence of [IIT 1981] its nitrate will be [CPMT 1971; MP PMT 1996] (a) Free electrons
(a) MNO3 (b) M 2 NO 3 2 (b) Free ions (c) Free molecules (c) MNO (d) MNO 3 2 3 3 (d) Atoms of sodium and chlorine 45. Out of the following, which compound will have electrovalent 33. The phosphate of a metal has the formula MHPO4 . The formula bonding of its chloride would be [NCERT 1974; CPMT 1977] (a) Ammonia (b) Water (c) Calcium chloride (d) Chloromethane (a) MCl (b) MCl2 46. The force which holds atoms together in an electrovalent bond is (c) (d) MCl3 M 2 Cl 3 (a) Vander Waal's force
34. A number of ionic compounds e.g. AgCl, CaF2 , BaSO4 are (b) Dipole attraction force insoluble in water. This is because [NCERT 1984] (c) Electrostatic force of attraction (a) Ionic compounds do not dissolve in water (d) All the above (b) Water has a high dielectric constant 47. The main reaction during electrovalent bond formation is (c) Water is not a good ionizing solvent (a) Redox reaction (b) Substitution reaction (d) These molecules have exceptionally high alternative forces in (c) Addition reaction (d) Elimination reaction the lattice 48. Electrovalent compounds are [CPMT 1996] 35. What is the nature of chemical bonding between Cs and F (a) Good conductor of electricity [MP PMT 1987; CPMT 1976] (b) Polar in nature (a) Covalent (b) Ionic (c) Coordinate (d) Metallic (c) Low M.P. and low B.P. 36. Which one of the following compound is ionic (d) Easily available [MNR 1985] 49. Ionic compounds do not have [RPMT 1997] (a) Hard and brittle nature (a) KCl (b) CH 4 (b) High melting and boiling point (c) Diamond (d) H 2 (c) Directional properties 37. Which of the following compound has electrovalent linkage (d) Soluble in polar solvents [CPMT 1983, 84, 93] 50. Highest melting point would be of [RPMT 1999] (a) (b) CH 3 Cl NaCl (a) He (b) CsCl (c) (d) Cl 2 (c) NH 3 (d) CHCl 3 38. An ionic compound is generally a [MADT Bihar 1981] 51. What is the effect of more electronegative atom on the strength of (a) Good electrolyte (b) Weak electrolyte ionic bond [AMU 1999] (c) Non-electrolyte (d) Neutral (a) Decreases (b) Increases 39. What metals combine with non-metals, the metal atom tends to (c) Decreases[AMU 1982 slowly] (d) Remains the same (a) Lose electrons 52. An element X with the electronic configuration 1s 2 , 2s 2 2p 6 ,3s 2 (b) Gain electrons would be expected to form the chloride with the formula [JIPMER 2000] (c) Remain electrically neutral (a) XCl (b) XCl (d) None of these 3 2 (c) XCl (d) X Cl 40. Chemical formula for calcium pyrophosphate is Ca 2 P2O7 . The 2 formula for ferric pyrophosphate will be [NCERT 1977] 53. Two element have electronegativity of 1.2 and 3.0. Bond formed between them would be [CPMT 1982; DCE 2000] (a) Fe3 (P2O7 )3 (b) Fe4 P4 O14 (a) Ionic (b) Polar covalent (c) Fe4 (P2O7 )3 (d) Fe3 PO4 (c) Co-ordinate (d) Metallic 41. Among the bonds formed by a chlorine atom with atoms of 54. Which of the following is least ionic [MP PET 2002] hydrogen, chlorine, sodium and carbon, the strongest bond is (a) C H Cl (b) KCl formed between [EAMCET 1988; MP PMT 1993] 2 5 (a) H Cl (b) Cl Cl (c) BaCl2 (d) C6 H 5 N H 3 Cl (c) Na Cl (d) C Cl 55. Which type of bonding exists in Li2O and CaF2 respectively 42. Which of the following is least soluble [CPMT 1989] [RPET 2000]
(a) BeF2 (b) SrF2 (a) Ionic, ionic (b) Ionic, covalent (c) Covalent, ionic (d) Coordinate, ionic (c) CaF2 (d) MgF2 56. An atom with atomic number 20 is most likely to combine 43. Which of the following halides has maximum melting point chemically with the atom whose atomic number is (a) (b) NaBr [BHU 2000] (c) NaI (d) NaF (a) 11 (b) 14 44. The high melting point and insolubility in organic solvents of (c) 16 (d) 10 sulphanilic acid are due to its ...... structure. [IIT 1994] 57. Bond formed in crystal by anion and cation is (a) Simple ionic (b) Bipolar ionic [CBSE PMT 2000] (c) Cubic (d) Hexagonal (a) Ionic (b) Metallic (c) Covalent (d) Dipole (c) 6 (d) 10 58. Atoms or group of atoms which are electrically charged are known 3. The electronic[UPSEAT configuration 2001] of four elements are given in brackets (a) Anions (b) Cations 2 2 1 2 2 5 L 1s , 2s 2p ; M 1s , 2s 2p (c) Ions (d) Atoms 2 2 6 1 2 2 2 59. Which one is the strongest bond [Pb. PMT 2001] Q 1s , 2s 2p , 3s ; R 1s , 2s 2p (a) Br – F (b) F – F The element that would most readily form a diatomic molecule is
[NCERT 1983] (c) Cl – F (d) Br – Cl (a) Q (b) M 60. The interionic attraction depends on interaction of (c) R (d) L [Kerala CET (Med.) 2002] 4. In covalency [CPMT 1974, 76, 78, 81; AFMC 1982] (a) Solute-Solute (b) Solvent-Solvent (a) Electrons are transferred (c) The charges (d) Molecular properties (b) Electrons are equally shared 61. Which of the following compounds is ionic (c) The electron of one atom are shared between two atoms [UPSEAT 2002] (d) None of the above 5. Which compound is highest covalent (a) KI (b) CH 4 (a) LiCl (b) LiF (c) Diamond (d) H 2 (c) LiBr (d) LiI 62. Which of the following pairs of species has same electronic 6. The nature of bonding in graphite is configuration [UPSEAT 2002] [DPMT 1986; CPMT 1986] (a) Covalent (b) Ionic 2 2 3 4 (a) Zn and Ni (b) Co and Ni (c) Metallic (d) Coordinate 2 4 3 (c) Co and (d) Ti and V 7. Which of the following substances has giant covalent structure [DPMT 1985, 86; NCERT 1975] 63. The energy that opposes dissolution of a solvent is (a) Iodine crystal (b) Solid [CPMT 2002] CO2 (a) Hydration energy (b) Lattice energy (c) Silica (d) White phosphorus
8. With which of the given pairs CO resembles [BHU 2005] (c) Internal energy (d) Bond energy 2 (a) HgCl, CH (b) HgCl, SnCl 64. Which of the following has highest melting point 2 2 2 2 4 (c) CH, NO (d) NO and NO [RPET 2003] 2 2 2 2 2 9. The electron pair which forms a bond between two similar non- (a) BeCl (b) MgCl 2 2 metallic atoms will be [IIT 1986]
(a) Dissimilar shared between the two (c) CaCl 2 (d) BaCl2 (b) By complete transfer from one atom to other 65. Which of the following statements is not true for ionic compounds [RPET 2003] (c) In a similar spin condition (a) High melting point (d) Equally shared in between the two (b) Least lattice energy 10. For the formation of covalent bond, the difference in the value of (c) Least solubility in organic compounds electronegativities should be [EAMCET 1982] (d) Soluble in water (a) Equal to or less than 1.7 (b) More than 1.7 66. Electrolytes are compound containing [MADT Bihar 1981] (c) 1.7 or more (d) None of these 11. Which type of bond is formed between similar atoms (a) Electrovalent bond (b) Covalent bond (a) Ionic (b) Covalent (c) Coordinate bond (d) Hydrogen bond (c) Coordinate (d) Metallic 67. Which of the following hydrides are ionic [Roorkee 1999] 12. Covalent compounds are generally ...... in water [CPMT 1987] (a) CaH 2 (b) BaH2 (a) Soluble (b) Insoluble (c) SrH 2 (d) BeH 2 (c) Dissociated (d) Hydrolysed 68. Which of the following conduct electricity in the fused state 13. Which one is the electron deficient compound [AIIMS 1982]
[Roorkee 2000] (a) ICl (b) NH 3 (a) BeCl (b) MgCl 2 2 (c) BCl3 (d) PCl3 14. Which among the following elements has the tendency to form (c) SrCl2 (d) BaCl2 covalent compounds
(a) (b) Covalent bonding Ba Be (c) Mg (d) Ca 1. The valency of sulphur in sulphuric acid is [NCERT 1974] 15. Silicon has 4 electrons in the outermost orbit. In forming the bonds [EAMCET 1981] (a) 2 (b) 4 (a) It gains electrons (b) It loses electrons (c) 6 (d) 8 (c) It shares electrons (d) None of these 2. The number of electrons involved in the bond formation of 16. Which of the following occurs when two hydrogen atoms bond with each others N 2 molecule (a) Potential energy is lowered [IIT 1980; CPMT 1983, 84, 85; CBSE PMT 1992] (b) Kinetic energy is lowered (a) 2 (b) 4 (c) Electronic motion ceases (a) LiCl NaCl BeCl 2 (b) BeCl 2 NaCl LiCl (d) Energy is absorbed (c) NaCl LiCl BeCl (d) BeCl LiCl NaCl 17. A bond with maximum covalent character between non-metallic 2 2 elements is formed [NCERT 1982] 27. Bond energy of covalent O H bond in water is (a) Between identical atoms [EAMCET 1982] (b) Between chemically similar atoms (a) Greater than bond energy of H bond (c) Between atoms of widely different electronegativities (b) Equal to bond energy of bond (d) Between atoms of the same size (c) Less than bond energy of bond 18. Amongst the following covalent bonding is found in (d) None of these [CPMT 1973] [DPMT 1983] (a) Sodium chloride (b) Magnesium chloride 28. Solid CH 4 is (c) Water (d) Brass (a) Molecular solid (b) Ionic solid 19. Indicate the nature of bonding in diamond (c) Pseudo solid (d) Does not exist [EAMCET 1980; BHU 1996; KCET 2000] 29. A covalent bond is likely to be formed between two elements which [MP PMT 1987] (a) Covalent (b) Ionic (a) Have similar electronegativities (c) Coordinate (d) Hydrogen (b) Have low ionization energies 20. Octet rule is not valid for the molecule (c) Have low melting points [IIT 1979; MP PMT 1995] (d) Form ions with a small charge
(a) CO 2 (b) H 2 O 30. The bond between two identical non-metal atoms has a pair of electrons [CPMT 1986] (c) CO (d) O 2 (a) Unequally shared between the two 21. Which of the following compounds are covalent (b) Transferred fully from one atom to another [IIT 1980; MLNR 1982] (c) With identical spins
(a) H 2 (b) CaO (d) Equally shared between them 31. The valency of phosphorus in is [DPMT 1984] (c) KCl (d) Na 2 S H 3 PO4 (a) 2 (b) 5 22. Indicate the nature of bonding in CCl 4 and CaH 2 (c) 4 (d) 1 [NCERT 1973] 32. Which of the following substances has covalent bonding (a) Covalent in and electrovalent in [AMU 1985] (b) Electrovalent in both and (a) Germanium (b) Sodium chloride (c) Covalent in both and (c) Solid neon (d) Copper 33. The covalency of nitrogen in HNO is [CPMT 1987] (d) Electrovalent in and covalent in 3 (a) 0 (b) 3 23. If the atomic number of element X is 7, the best electron dot (c) 4 (d) 5 symbol for the element is [NCERT 1973; CPMT 2003] 34. Hydrogen chloride molecule contains a [CPMT 1984] (a) X . (b) . X . (a) Covalent bond (b) Double bond . .. (c) . X : (d) : X . (c) Coordinate bond (d) Electrovalent bond . .. 35. As compared to covalent compounds, electrovalent compounds 24. Which is the most covalent [AFMC 1982] generally have (a) C O (b) C Br [CPMT 1990, 94; MP PMT 1997] (c) C S (d) C F (a) Low melting points and low boiling points 25. The covalent compound HCl has the ionic character as (b) Low melting points and high boiling points [EAMCET 1980] (c) High melting points and low boiling points (a) The electronegativity of hydrogen is greater than that of (d) High melting points and high boiling points chlorine 36. The interatomic distances in and Cl molecules are 74 and (b) The electronegativity of hydrogen is equal to that of chlorine 2 198 pm respectively. The bond length of is (c) The electronegativity of chlorine is greater than that of hydrogen [MP PET 1993] (a) 272 pm (b) 136 pm (d) Hydrogen and chlorine are gases (c) 124 pm (d) 248 pm 26. The correct sequence of increasing covalent character is represented by [CBSE PMT 2005] 37. On analysis, a certain compound was found to contain iodine and oxygen in the ratio of 254 gm of iodine and 80 gm of oxygen. The atomic mass of iodine is 127 and that of oxygen is 16. Which of (e) M 3 A the following is the formula of the compound [CPMT 1981] 47. The table shown below gives the bond dissociation energies (E ) (a) IO (b) I O diss 2 for single covalent bonds of carbon (C) atoms with element
(c) I5 O2 (d) I2 O5 A, B, C and D. Which element has the smallest atoms[CBSE PMT 1994] 38. Ionic and covalent bonds are present in 1 Bond Ediss (kJ mol ) [CBSE PMT 1990; MNR 1990; KCET 2000; UPSEAT 2001] C A 240 (a) CCl 4 (b) CaCl 2 C B 328 (c) NH Cl (d) H O 4 2 C C 276 39. Highest covalent character is found in [EAMCET 1992] C D 485
(a) CaF2 (b) (a) A (b) B (c) C (d) D (c) CaBr2 (d) CaI2 48. If a molecule X has a triple bond, then X will have the electronic 40. Among the following which property is commonly exhibited by a 2 configuration [CET Pune 1998] covalent compound [MP PET 1994] 2 2 5 2 2 3 (a) High solubility in water (a) 1s 2s 2p (b) 1s 2s 2p (b) High electrical conductance (c) 1s 2 2s1 (d) 1s 2 2s 2 2p1 (c) Low boiling point 49. Which of the following compounds does not follow the octet rule for (d) High melting point electron distribution [CET Pune 1998] 41. Atoms in the water molecule are linked by [MP PAT 1996] (a) PCl5 (b) PCl3 (a) Electrovalent bond (c) (d) PH (b) Covalent bond 3 (c) Coordinate covalent bond 50. The valency of A 3 and B 2 , then the compound is (d) Odd electron bond [Bihar MEE 1997] (a) A2 B3 (b) A3 B2 42. Which is the correct electron dot structure of N 2 O molecule [MP PET 1996] (c) A3 B3 (d) A2 B2 .. .. (e) None of these (a) : N N O (b) : N N O : [AFMC 1998] .. .. 51. The number of electrons shared by each outermost shell of N 2 is (a) 2 (b) 3 ...... (c) N N O (d) : N N O : (c) 4 (d) 5 ...... 52. Which of the following substances when dissolved in water will give 43. A covalent bond between two atoms is formed by which of the a solution that does not conduct electricity following [MP PMT 1996] [JIPMER 1999] (a) Electron nuclear attraction (a) Hydrogen chloride (b) Potassium hydroxide (b) Electron sharing (c) Sodium acetate (d) Urea 53. Which of the following atoms has minimum covalent radius (c) Electron transfer [DPMT 2000] (d) Electrostatic attraction (a) B (b) C 44. The electronic configuration of a metal M is (c) N (d) Si 2 2 6 1 1s , 2s 2p , 3s . The formula of its oxides will be 54. Boron form covalent compound due to [Pb. PMT 2000] [MP PET/PMT 1998] (a) Small size (b) Higher ionization energy (c) Lower ionization energy (d) Both (a) and (b) (a) MO (b) M 2 O 55. Two elements X and Y have following electron configurations (c) M 2 O3 (d) MO2 X 2 2 6 2 6 2 45. Which of the following statements regarding covalent bond is not 1s , 2s 2p , 3s 3p , 4s true [MP PET/PMT 1998] 2 2 6 2 6 and Y 1s , 2s 2p , 3s 3p (a) The electrons are shared between atoms (b) The bond is non-directional The compound formed by combination of X and Y is (c) The strength of the bond depends upon the extent of [DPMT 2001] overlapping (a) (b) XY5 X 2 Y5 (d) The bond formed may or may not be polar (c) X Y (d) XY 46. If the electronic configuration of M 2, 8, 3 and that of 5 3 2 56. Covalent compounds have low melting point because A 2, 8, 7, the formula of the compound is [KCET 2002] [Bihar MEE 1996] (a) Covalent bond is less exothermic (a) M A (b) MA 2 3 2 (b) Covalent molecules have definite shape
(c) M 2 A (d) MA3 (c) Covalent bond is weaker than ionic bond (d) Covalent molecules are held by weak Vander Waal’s force of (a) 8 (b) 5
attraction (c) 6 (d) 7 57. p and n-type of semiconductors are formed due to 70. Hydrogen atoms are held together to form hydrogen molecules by [AMU 1982] [UPSEAT 2002] (a) Hydrogen bond (b) Ionic bond (c) Covalent bond (d) Dative bond (a) Covalent bonds (b) Metallic bonds 71. Strongest bond is [AFMC 1987] (c) Ionic bonds (d) Co-ordinate bond (a) C C (b) C H 58. Which of the following is Lewis acid [RPET 2003] (c) C N (d) C O (a) (b) BF3 NH 3 72. The major binding force of diamond, silicon and quartz is [Kerala CET (Med.) 2002]
(c) PH3 (d) SO 2 (a) Electrostatic force (b) Electrical attraction
(c) Co-valent bond force (d) Non-covalent bond force 59. Among the species : CO , CH COO , CO, CO 2, HCHO 2 3 3 73. Multiple covalent bonds exist in a molecule of [NCERT 1973] which has the weakest carbon- oxygen bond (a) H (b) F [Kerala PMT 2004] 2 2
(c) C2 H 4 (d) N 2 (a) CO2 (b) CH 3COO 74. Which of the following does not obey the octet rule (c) CO (d) CO 2 3 [EAMCET 1993]
(e) HCHO (a) CO (b) NH 3 60. Valency of sulphur in is [DPMT 1984] Na 2 S 2O3 (c) H 2 O (d) PCl5 (a) Two (b) Three 75. Which of the following statements is correct for covalent bond [BHU 1997] (c) Four (d) Six (a) Electrons are shared between two atoms 61. The acid having O O bond is (b) It may be polar or non-polar [IIT JEE Screening 2004] (c) Direction is non-polar (a) (b) (d) Valency electrons are attracted H 2 S 2O3 H 2 S 2O6 76. Among CaH , NH , NaH and B H , which are covalent (c) H S O (d) H S O 2 3 2 6 2 2 8 2 4 6 hydride [Orissa JEE 2005] 62. The following salt shows maximum covalent character (a) NH 3 and B2H6 (b) NaH and CaH 2 [UPSEAT 2004] (c) NaH and NH (d) CaH and (a) AlCl (b) MgCl 3 2 3 2
(c) CsCl (d) LaCl3 Co-ordinate or Dative bonding
63. Which type of bond is present in H 2S molecule 1. Which species has the maximum number of lone pair of electrons [MHCET 2003; Pb CET 2001] on the central atom? [IIT 2005] (a) Ionic bond (b) Covalent bond (a) [ClO] (b) XeF 3 4 (c) Co-ordinate (d) All of three (c) SF (d) [I] 4 3 64. is more acidic than H 2O , due to [BVP 2004] 2. A simple example of a coordinate covalent bond is exhibited by [NCERT 1984] (a) O is more electronegative than S (a) C2 H 2 (b) H 2 SO4 (b) O H bond is stronger than S H bond (c) (d) HCl (c) bond is weaker than bond
(d) None of these 3. The bond that exists between and BF3 is called 65. Which of the following has covalent bond [AFMC 1982; MP PMT 1985; MNR 1994; [AFMC 1988; DCE 2004] KCET 2000; MP PET 2001; UPSEAT 2001] (a) (b) Na 2S (a) Electrovalent (b) Covalent (c) NaH (d) (c) Coordinate (d) Hydrogen 66. The following element forms a molecule with eight its own weight 4. Which of the following does not have a coordinate bond atoms [MHCET 2004] [MADT Bihar 1984] (a) Si (b) (a) SO 2 (b) HNO 3 (c) Cl (d) P (c) H 2 SO3 (d) HNO 2 67. In H2O2 , the two oxygen atoms have (a) Electrovalent bond (b) Covalent bond 5. Coordinate covalent compounds are formed by (c) Coordinate bond (d) No bond [CPMT 1990, 94] 68. Carbon has a valency of 2 in CO and 4 in CO and CH . Its (a) Transfer of electrons (b) Sharing of electrons 2 4 (c) Donation of electrons (d) None of these process valency in acetylene C H is [NCERT 1971] 2 2 6. In the coordinate valency [CPMT 1989] (a) 1 (b) 2 (a) Electrons are equally shared by the atoms (c) 3 (d) 4 (b) Electrons of one atom are shared with two atoms 69. Number of electrons in the valence orbit of nitrogen in an ammonia molecule are [MH CET 2004] (c) Hydrogen bond is formed (d) None of the above [DPMT 1985]
7. Which of the following contains a coordinate covalent bond (a) BF3 (b) CCl 4 [MNR 1990; IIT 1986] (c) BeCl (d) All of these (a) N O (b) BaCl 2 2 5 2 3. Which molecule has the largest dipole moment (c) HCl (d) H 2 O [CPMT 1991] 8. A coordinate bond is formed when an atom in a molecule has [CBSE(a) PMT 1992] (b) HI (a) Electric charge on it (c) (d) (b) All its valency electrons shared 4. The unequal sharing of bonded pair of electrons between two atoms (c) A single unshared electron in a molecule causes [EAMCET 1986] (d) One or more unshared electron pair (a) Dipole 9. Which has a coordinate bond [RPMT 1997] (b) Radical formation 2 (c) Covalent bond (a) SO 3 (b) CH 4 (d) Decomposition of molecule (c) CO (d) NH 2 3 5. Which of the following will show least dipole character 10. The compound containing co-ordinate bond is [NCERT 1975; Kurukshetra CEE 1998] [AFMC 1999; Pb. CET 2002] (a) Water (b) Ethanol (a) O (b) SO 3 3 (c) Ethane (d) Ether
(c) H 2 SO4 (d) All of these 6. Which of the following molecules will show dipole moment 11. The number of dative bonds in sulphuric acid molecules is [NCERT 1972, 74; DPMT 1985] [MP PET 2002] (a) Methane (b) Carbon tetrachloride (a) 0 (b) 1 (c) Chloroform (d) Carbon dioxide (c) 2 (d) 4 7. Which of the following compounds possesses the dipole moment[NCERT 1978; EAMCET 1983; MP PMT 1995] 12. Which of the following compounds has coordinate (dative) bond (a) Water[RPET 2003] (b) Boron trifluoride (a) (b) (c) Benzene (d) Carbon tetrachloride CH 3 NC CH 3 OH
8. Which bond angle would result in the maximum dipole moment (c) CH 3 Cl (d) NH 3 for the triatomic molecule YXY [AIIMS 1980] 13. The structure of orthophosphoric acid is [KCET 2003] (a) 90o (b) 120o O H o o | (c) 150 (d) 180 (a) H O P O H (b) O P O H 9. Which of the following would have a permanent dipole moment[CBSE PMT 2005] | | O O (a) BF3 (b) SiF4 | | (c) (d) H H SF4 XeF4 10. Carbon tetrachloride has no net dipole moment because of O H [IIT 1982, 83; MP PMT 1985, 91; EAMCET 1988; | AMU 1999] (c) O P O H (d) H O P O | (a) Its planar structure H (b) Its regular tetrahedral structure 14. What is the nature of the bond between B and O in (c) Similar sizes of carbon and chlorine atoms (C H ) OBH [Orissa JEE 2003] (d) Similar electron affinities of carbon and chlorine 2 5 2 3 11. The molecule which has the largest dipole moment amongst the (a) Covalent (b) Co-ordinate covalent following [MNR 1983] (c) Ionic bond (d) Banana shaped bond (a) (b) CHCl 15. Sulphuric acid provides a example of 3 [Kerala CET (Med.) 2002] (c) CCl 4 (d) CHI3 (a) Co-ordinate bonds 12. Positive dipole moment is present in (b) Non-covalent compound [MNR 1986; MP PET 2000]
(c) Covalent and co-ordinate bond (a) (b) C6 H 6 (d) Non-covalent ion (c) BF (d) 3 Dipole moment 13. The polarity of a covalent bond between two atoms depends upon [AMU 1982] (a) Atomic size (b) Electronegativity
1. Which molecules has zero dipole moment (c) Ionic size (d) None of the above [AIIMS 1980, 82, 91; Roorkee 2000; MH CET 2001] 14. Pick out the molecule which has zero dipole moment [CPMT 1989; EAMCET 1993; MP PMT 1999] (a) H2O (b) CO2 (a) (b) (c) HF (d) HBr
2. In the following which one have zero dipole moment (c) BCl3 (d) SO 2 15. Zero dipole moment is present in [DPMT 1986; IIT 1987] (c) Sulphur dioxide (d) Water (a) NH 3 (b) H 2 O 28. is less reactive than due to [UPSEAT 2003] N 2 CN (c) cis 1, 2-dichloroethene (d) trans 1, 2-dichloroethene (a) Presence of more electrons in orbitals 16. Which of the following is the most polar [AFMC 1988] (b) Absence of dipole moment
(a) CCl 4 (b) CHCl 3 (c) Difference in spin quantum no (d) None of these (c) CH 3 OH (d) CH 3 Cl 10 17. Which one has minimum (nearly zero) dipole moment 29. In a polar molecule, the ionic charge is 4.8 10 e.s.u. If the [IIT Screening 1994; CBSE PMT 1996] inter ionic distance is one Å unit, then the dipole moment is [MH CET 2003] (a) Butene-1 (b) cis butene-2 (a) 41.8 debye (b) 4.18 debye
(c) trans butene-2 (d) 2-methyl-1-propene (c) 4.8 debye (d) 0.48 debye 18. Which one of the following is having zero dipole moment 30. Which of the following is a polar compound [RPMT 1997; EAMCET 1988; MNR 1991] [Pb. CET 2000] (a) (b) (a) (b) HCl H 2Se (c) CH 3 F (d) (c) CH (d) HI 19. Which of the following molecules does not possess a permanent 4 dipole moment [CBSE PMT 1994] 31. Which of the following has no dipole moment [DCE 2002] (a) H 2 S (b) SO 2 (a) (b) CO 2 SO3 (c) CS 2 (d) SO 3
20. Which of the following has zero dipole moment (c) O3 (d) H 2O [CPMT 1997; AFMC 1998; CBSE PMT 2001] 32. Which of the following is non-polar [DCE 2002] (a) CH 2 Cl 2 (b) CH 4 (a) PCl5 (b) PCl3 (c) (d) PH3 (c) SF (d) IF 21. Fluorine is more electronegative than either boron or phosphorus. 6 7 33. Identify the non-polar molecule in the set of compounds given : What conclusion can be drawn from the fact that BF3 has no HCl, HF, H2, HBr [UPSEAT 2004] dipole moment but PF3 does
[Pb. PMT 1998] (a) H 2 (b) (a) is not spherically symmetrical but is PF3 (c) HF, HBr (d) HBr (b) molecule must be linear 34. Dipole moment is shown by [IIT 1986] (c) The atomic radius of P is larger than the atomic radius of B (a) 1, 4-dichlorobenzene (d) The molecule must be planar triangular (b) cis 1, 2-dichloroethene 22. Which molecule does not show zero dipole moment (c) trans1, 2-dichloroethene [RPET 1997, 99] (d) 1, 2-dichloro-2-pentene (a) (b) BF3 NH 3 35. If HCl molecule is completely polarized, so expected value of dipole moment is 6.12D (deby), but experimental value of dipole moment is (c) CCl 4 (d) CH 4 1.03D. Calculate the percentage ionic character [Kerala CET 2005] 30 23. The dipole moment of HBr is 1.6 10 cm and interatomic (a) 17 (b) 83 spacing is 1Å. The % ionic character of HBr is [MP PMT 2000] (c) 50 (d) Zero (a) 7 (b) 10 (e) 90 (c) 15 (d) 27 24. Non-polar solvent is [RPET 2000] Polarisation and Fajan's rule (a) Dimethyl sulphoxide (b) Carbon tetrachloride (c) Ammonia (d) Ethyl alcohol 1. BF and NF both molecules are covalent, but is non-polar 3 3 25. Which shows the least dipole moment and is polar. Its reason is [UPSEAT 2001; DPMT 1982] [CPMT 1989; NCERT 1980] (a) (b) (a) In uncombined state boron is metal and nitrogen is gas (c) CH CH OH (d) CH COCH 3 2 3 3 (b) B F bond has no dipole moment whereas N F bond has 26. Which molecule has zero dipole moment [UPSEAT 2001] dipole moment (a) H O (b) AgI 2 (c) The size of boron atom is smaller than nitrogen
(c) PbSO4 (d) HBr (d) is planar whereas is pyramidal 27. The dipole moment is zero for the molecule 2. Which one is polar molecule among the following [IIT 1989; MP PMT 2002] (a) Ammonia (b) Boron trifluoride (a) CO (b) 2 2 (c) H 2 O (d) CH 4 (c) Na (d) Ca 3. If the electron pair forming a bond between two atoms A and B is 15. Maximum covalent character is associated with the compound [RPMT 1999] not in the centre, then the bond is [AIIMS 1984] (a) NaI (b) MgI2 (a) Single bond (b) Polar bond (c) (d) AlI3 (c) Non-polar bond (d) bond 16. Polarisibility of halide ions increases in the order 4. Which of the following liquids is not deflected by a non-uniform [DCE 1999] electrostatic field [NCERT 1978] (a) F , I , Br , Cl (b) Cl , Br , I , F (a) Water (b) Chloroform (c) I , Br , Cl , F (d) F , Cl , Br , I (c) Nitrobenzene (d) Hexane 17. According to Fajan’s rule, covalent bond is favoured by 5. Which of the following is non-polar [EAMCET 1983] [AIIMS 1999] (a) H 2 S (b) NaCl (a) Large cation and small anion (c) Cl (d) H SO (b) Large cation and large anion 2 2 4 (c) Small cation and large anion 6. Polarization is the distortion of the shape of an anion by an (d) Small cation and small anion adjacently placed cation. Which of the following statements is 18. Which of the following statements is correct [AMU 1999] correct [NCERT 1982] (a) Maximum polarization is brought about by a cation of high (a) SF4 is polar and non-reactive charge (b) SF6 is non-polar and very reactive (b) Minimum polarization is brought about by a cation of (c) is a strong fluorinating agent low radius
(c) A large cation is likely to bring about a large degree of (d) is prepared by fluorinating SCl 2 with NaF polarization 19. Choose the correct statement [RPMT 2000] (d) A small anion is likely to undergo a large degree of polarization (a) Amino polarisation is more pronounced by highly charged cation 7. The bonds between P atoms and Cl atoms in PCl5 are likely to be [MP PMT 1987] (b) Small cation has minimum capacity to polarise an anion. (a) Ionic with no covalent character (c) Small anion has maximum polarizability (b) Covalent with some ionic character (d) None of these (c) Covalent with no ionic character 20. The ICl molecule is [DPMT 2001] (d) Ionic with some metallic character (a) Purely electrovalent (b) Purely covalent 8. Two electrons of one atom A and two electrons of another atom B are utilized to form a compound AB. This is an example of (c) Polar[MNR with 1981] negative end on iodine (a) Polar covalent bond (b) Non-polar covalent bond (d) Polar with negative end on chlorine (c) Polar bond (d) Dative bond 21. Which of the following is a polar compound [AIIMS 2001] (a) HF (b) HCl 9. In which of the following molecule is the covalent bond most polar [AMU 1985; MP PET 2001] (c) HNO (d) H SO (a) HI (b) HBr 3 2 4 22. Which of the following has zero dipole moment (c) HCl (d) H 2 [MP PMT 2002]
10. Amongst ClF3 , BF3 and NH 3 molecules the one with non- (a) ClF (b) PCl3 planar geometry is [MP PMT 1999] (c) (d) SiF4 CFCl3 (a) ClF (b) 3 23. Which of the following compounds has least dipole moment
(c) BF3 (d) None of these [RPET 2003] (a) (b) 11. Which of the following possesses highest melting point PH3 CHCl 3 [CPMT 1999] (c) NH 3 (d) BF3 (a) Chlorobenzene (b) o-dichlorobenzene 24. Pauling’s electronegativity values for elements are useful in (c) m-dichlorobenzene (d) p-dichlorobenzene predicting [UPSEAT 2004] 12. The polar molecule among the following is (a) Polarity of bonds in molecules [Orissa JEE 1997] (b) Position of elements in electrochemical series
(a) CCl 4 (b) CO 2 (c) Co-ordination number (d) Dipole moment of various molecules (c) CH 2 Cl 2 (d) CH 2 CH 2 25. Amongst LiCl, RbCl, BeCl and MgCl the compounds with the 13. Which of the following have both polar and non-polar bonds [AIIMS 1997] 2 2 greatest and the least ionic character, respectively, are [UPSEAT 2002] (a) C2 H 6 (b) NH 4 Cl (a) LiCl and RbCl (b) RbCl and
(c) (d) AlCl3 (c) RbCl and (d) and 14. Which of the following has a high polarising power [CET Pune 1998] 26. Bond polarity of diatomic molecule is because of (a) Mg2 (b) Al3 [UPSEAT 2002] (a) Difference in electron affinities of the two atoms (b) Sidewise overlap of orbitals takes place (b) Difference in electronegativities of the two atoms (c) End to end overlap of orbitals takes place
(c) Difference in ionisation potential (d) None of the above (d) All of these 11. The number of sigma and pi bonds in 1-butene-3-yne are [IIT 1989] Overlaping- and - bonds (a) 5 sigma and 5 pi (b) 7 sigma and 3 pi (c) 8 sigma and 2 pi (d) 6 sigma and 4 pi 1. Triple bond in ethyne is formed from 12. The most acidic compound among the following is [MP PMT 1990; NCERT 1979; EAMCET 1978; AMU 1985; [MP PET 1993] CPMT 1988; MADT Bihar 1982; MH CET 2000] (a) CH 3 CH 2OH (b) C6 H 5 OH (a) Three sigma bonds (c) CH COOH (d) CH CH CH OH (b) Three pi bonds 3 3 2 2 (c) One sigma and two pi bonds 13. Which of the following is not correct [CBSE PMT 1990] (d) Two sigma and one pi bond (a) A sigma bond is weaker than bond 2. The bond in the formation of fluorine molecule will be (b) A sigma bond is stronger than bond [MP PMT 1987] (c) A double bond is stronger than a single bond (a) Due to s s overlapping (d) A double bond is shorter than a single bond (b) Due to s p overlapping 14. Strongest bond formed, when atomic orbitals (a) Maximum overlap (b) Minimum overlap (c) Due to p p overlapping (c) Overlapping not done (d) None of them (d) Due to hybridization 15. The p p orbital overlapping is present in the following molecule [MP PET 1994] 3. Which type of overlapping results the formation of a bond (a) Hydrogen (b) Hydrogen bromide [DPMT 1981] (c) Hydrogen chloride (d) Chlorine (a) Axial overlapping of orbitals 16. In N molecule, the atoms are bonded by (b) Lateral overlapping of orbitals 2 [MP PET 1996; UPSEAT 2001] (c) Axial overlapping of orbitals (a) One , Two (b) One , One (d) Axial overlapping of orbitals (c) Two , One (d) Three bonds 4. The number and type of bonds between two carbon atoms in calcium carbide are [AIEEE 2005] 17. In which of following there exists a p d bonding (a) One sigma, one pi (b) One sigma, two pi [AFMC 2001] (a) Diamond (b) Graphite (c) Two sigma, one pi (d) Two singma, two pi 5. In a double bond connecting two atoms, there is a sharing of (c) Dimethyl amine (d) Trisilylamine [CPMT 1977, 80, 81; NCERT 1975; 18. Number of bonds in SO 2 [DCE 2001] Bihar MEE 1980; MP PET 1999] (a) Two and two (a) 2 electrons (b) 1 electron (b) Two and one (c) 4 electrons (d) All electrons 6. Strongest bond is [DPMT 1990] (c) Two , two and one lone pair (a) C C (b) C C (d) None of these (c) C C (d) All are equally strong 19. Which of the following has bonding [CBSE 2002] 7. bond is formed [JIPMER 2002] (a) NO (b) 2 3 CO 3 (a) By overlapping of atomic orbitals on the axis of nuclei (c) BO3 (d) SO 2 (b) By mutual sharing of pi electron 3 3 (c) By sidewise overlapping of half filled p-orbitals 20. Number of sigma bonds in is [AIEEE 2002] P4 O10 (d) By overlapping of s-orbitals with p-orbitals (a) 6 (b) 7
8. The double bond between the two carbon atoms in ethylene consists (c) 17 (d) 16 of [NCERT 1981; EAMCET 1979] (a) Two sigma bonds at right angles to each other Hybridisation (b) One sigma bond and one pi bond (c) Two pi bonds at right angles to each other 1. Which molecule is not linear [CPMT 1994] (d) Two pi bonds at an angle of o to each other 60 (a) BeF2 (b) BeH 2 9. In the series ethane, ethylene and acetylene, the bond C H (c) CO (d) H O energy is [NCERT 1977] 2 2 (a) The same in all the three compounds 2. The bond angle in water molecule is nearly or Directed bonds in (b) Greatest in ethane water forms an angle of (c) Greatest in ethylene [NCERT 1980; EAMCET 1981; MNR 1983, 85; AIIMS 1982; CPMT 1989; MP PET 1994, 96; (d) Greatest in acetylene MP PET/PMT 1998] 10. In a sigma bond (a) Sidewise as well as end to end overlap of orbitals take place (a) 120o (b) 180o o o (c) 109 28' (d) 104 30' 12. The mode of hybridisation of carbon in CO 2 is [CPMT 1991] 2 3. The central atom in a molecule is in sp hybrid state. The shape of (a) sp (b) molecule will be [MP PMT 1987; CBSE PMT 1989] (c) 3 (d) None of these (a) Pyramidal (b) Tetrahedral sp (c) Octahedral (d) Trigonal planar 13. In which of the following the central atom does not use hybrid 4. Which molecule is linear orbitals in its bonding [MNR 1992] [MP PMT 1984; IIT 1982, 88; EAMCET 1993; CBSE PMT 1992; MP PET 1995; RPMT 1997] (a) BeF3 (b) OH3
(a) NO2 (b) ClO2 (c) NH 2 (d) NF3
(c) CO2 (d) H2S 14. XeF2 involves hybridisation [DPMT 1990] 5. Which of the following molecules has trigonal planer geometry [CBSE PMT 2005] (a) (b) sp3 d (a) IF3 (b) PCl3 (c) sp3 d 2 (d) None of these (c) NH 3 (d) BF3 15. Which of the following hybridisation results in non-planar orbitals [CBSE PMT 1991] 6. A sp3 hybridized orbital contains 2 [DPMT 1984; BHU 1985; CPMT 1976] (a) (b) dsp 1 1 (a) s character (b) s character (c) (d) 4 2 16. Octahedral molecular shape exists in ...... hybridisation 2 3 (c) s character (d) s character [DPMT 1990] 3 4 (a) (b) 7. Structure of ammonia is [MP PMT 1987, 89, 91; CPMT 1975, 82; (c) sp3 d 3 (d) None of these RPMT 1999; JIPMER 2002] 17. The electronic structure of molecule OF is a hybrid of (a) Trigonal (b) Tetrahedral 2 (c) Pyramidal (d) Trigonal pyramidal (a) (b) 8. The bond angle in ethylene is [CPMT 1987] (c) (d) sd3 (a) 180o (b) 120o 18. Percentage of s-character in hybrid orbital is (c) o (d) o 109 90 (a) 25 (b) 50 9. Compound formed by sp3d hybridization will have structure (c) 66 (d) 75 [BHU 1982; RPMT 1999] 19. Shape of XeF4 molecule is (a) Planar (b) Pyramidal [BHU 1987; AFMC 1992; CET Pune 1998; (c) Angular (d) Trigonal bipyramidal Roorkee Qualifying 1998; DCE 2002] 10. Which of the following formula does not correctly represent the (a) Linear (b) Pyramidal bonding capacity of the atom involved (c) Tetrahedral (d) Square planar [CBSE PMT 1990] 20. For which of the following hybridisation the bond angle is maximum [CBSE PMT 1991] H (a) (b) | F F (a) H P H (b) | O (c) (d) H 21. The C H bond distance is the longest in [MNR 1990]
O O (a) C2 H 2 (b) C2 H 4 (c) O N (d) H C C (c) C2 H 4 Br2 (d) C6 H 6 O H O H 22. The nature of hybridization in CH Cl CH Cl for carbon is 11. Which of the following statement is not correct 2 2 [AIIMS 1983] (a) (b)
(a) Hybridization is the mixing of atomic orbitals prior to their 2 combining into molecular orbitals (c) (d) sp d 23. Shape of methane molecule is [MNR 1983] (b) sp2 hybrid orbitals are formed from two p atomic orbitals (a) Tetrahedral (b) Pyramidal and one s atomic orbital (c) Octahedral (d) Square planer 2 3 (c) d sp hybrid orbitals are directed towards the corners of a 24. Which one amongst the following possesses an hybridized regular octahedron carbon in its structure [CBSE PMT 1989] 3 o (d) dsp hybrid orbitals are all at 90 to one another (a) CH 2 C.Cl CH CH 2 35. In the following molecule, the two carbon atoms marked by asterisk (b) C.Cl 2 C.Cl 2 (*) possess the following type of hybridized orbitals (c) CH 2 C CH 2 * * H 3 C C C CH 3 [NCERT 1984] (d) CH 2 CH CH CH 2 (a) orbital (b) orbital 25. Which of the following is the correct electronic formula of chlorine molecule [CPMT 1971] (c) orbital (d) s orbital ...... 36. The bond angle in carbon tetrachloride is approximately (a) : Cl : Cl : (b) :Cl : : Cl : [MNR 1981; MP PMT 1987] ...... (a) 90o (b) 109o ...... (c) : Cl : Cl : (d) : Cl : :Cl : (c) 120o (d) 180o 37. When two pairs of electrons are shared, bond is
26. In XeF4 hybridization is [MNR 1979] (a) Single covalent bond (b) Double covalent bond (a) sp3 d 2 (b) sp3 (c) Dative bond (d) Triple bond 3 2 (c) sp d (d) sp d 38. The nature of hybridization in the NH 3 molecule is 27. In HCHO, 'C' has hybridization [AIIMS 1987] [EAMCET 1982] (a) (b) (a) sp (b) sp2 (c) (d) (c) (d) All the above 39. Which one of the following compounds has bond angle as nearly 28. Which has the shortest C C bond length [MP PMT 1985] [NCERT 1982; CPMT 1989] (a) (b) H 2 S (a) C2 H 5 OH (b) C2 H 6 (c) (d) CH 4 (c) C H (d) C H 2 2 2 4 40. In ethene, the bond angle(s) is/are [CPMT 1976; AMU 1984; MP PMT 1985] 29. The hybridization of Ag in the linear complex AgNH 3 2 is [CPMT 1985; BHU 1981] (a) 109o 28' (b) (a) dsp2 (b) (c) (d) Different (c) (d) 41. Structure formula of H 2 O2 is [CPMT 1993] 30. Experiment shows that H 2 O has a dipole moment while CO 2 has H not. Point out the structures which best illustrate these facts [DPMT 1984; NCERT 1983; CPMT 1984] (a) O O O (a) (b) O C O; H O H H O C O ; H H (b) H O O H (straight line) (c) C ; H – H – O (d) O H || | H' O O CO ; OH (c) O O 31. Which species do not have hybridization H [DPMT 1985] Where H O O O O H' 101.5 o and all the four (a) Ammonia (b) Methane atoms are in the same plane (c) Water (d) Carbon dioxide 32. As compared to pure atomic orbitals, hybrid orbitals have (a) Low energy (b) Same energy (d) (c) High energy (d) None of these 33. The compound 1, 2-butadiene has Where H O O O O H' 97o and the angle [IIT 1983; MP PMT 1996] o (a) Only hybridized carbon atoms between H O O plane and O O H' plane is 101 42. Number of shared electrons in between carbon-carbon atoms in (b) Only hybridized carbon atoms ethylene molecule is [MADT Bihar 1983] (c) Both and hybridized carbon atoms (a) 2 (b) 4 (c) 6 (d) 3 2 (d) sp, sp and hybridized carbon atoms 43. The structural formula of a compound is
34. The number of unpaired electrons in O 2 molecule is CH 3 CH C CH 2 . The type of hybridization at the four [MNR 1983; Kerala PET 2002] carbons from left to right are [CBSE PMT 1989] (a) 0 (b) 1 (a) sp2 , sp, sp2 , sp3 (b) sp2 , sp3 , sp2 , sp (c) 2 (d) 3 (c) sp3 , sp2 , sp, sp2 (d) sp3 , sp2 , sp2 , sp2 55. In diborane, the H B H bond angle is . The hybridization of boron is likely to be 44. Acetate ion contains [AMU 1983] [BHU 1981; CBSE PMT 1999] (a) One C, O single bond and one double bond (a) (b) (b) Two single bonds (c) (d) (c) Two double bonds 56. The number of shared pairs of electrons in propane is (d) None of the above [BHU 1981] 45. The two carbon atoms in acetylene are (a) 2 (b) 4 [AMU 1984; MADT Bihar 1982] (c) 6 (d) 10 3 2 (a) sp hybridized (b) sp hybridized 57. s-character in hybridised orbitals are (c) hybridized (d) Unhybridized sp 1 1 (a) (b) 46. Among the following compounds which is planar in shape 3 2 [AMU 1992] 1 2 (a) Methane (b) Acetylene (c) (d) 4 3 (c) Benzene (d) Isobutene
47. In methane the bond angle is [AMU 1983] 58. The two types of bonds present in B2 H 6 are covalent and [IIT 1994] (a) 180o (b) 90o (a) Three centre bond (b) Hydrogen bond (c) 120o (d) 109o (c) Two centre bond (d) None of the above
48. The angle between orbitals in ethylene is 59. In the compound CH 3 OCl, which type of orbitals have been [BHU 1987, 95; AMU 1985] used by the circled carbon in bond formation [MP PET 1994] (a) (b) (a) (b) (c) (d) 109.5 o (c) (d) p 49. The species in which the central atom uses hybrid orbitals in 60. The correct order of the O O bond length in O , H O and its bonding is [IIT 1988] 2 2 2 O3 is [CBSE PMT 1995] (a) PH3 (b) NH 3 (a) (b) O2 O3 H 2O2 O3 H 2O2 O2 (c) H 3 C (d) SbH 3 (c) H O O O (d) O H O O 50. Carbon atoms in diamond are bonded to each other in a 2 2 3 2 2 2 2 3 configuration [CPMT 1981] 61. The structure of PF5 molecule is (a) Tetrahedral (b) Planar [AFMC 1995; JIPMER 2001] (c) Linear (d) Octahedral (a) Tetrahedral (b) Trigonal bipyramidal 51. Which of the following molecules can central atom said to adopt (c) Square planar (d) Pentagonal bipyramidal hybridization [CBSE PMT 1989; MP PET 1994] 62. Which of the following hybridisation has maximum s-characters [MP PET 1995] (a) (b) (a) BeF2 (b) BCl3 (c) (d) None of these (c) C2 H 2 (d) 63. The PCl5 molecule is a result of the hybridisation of 52. In Cu NH 3 SO4 , ;Cu has following hybridization 4 [MP PET 1995; DCE 2000; MP PMT 2002] [AIIMS 1988; UPSEAT 2001] (a) sp2 d 2 (b) sp3 d (a) dsp2 (b) (c) spd 3 (d) sp2 d 3 (c) (d) sp3 d 2 64. Hybridisation involves [MP PMT 1996] 53. The hybridization of carbon atoms in C C single bond of (a) Addition of an electron pair HC C CH CH 2 is [IIT 1991; MP PET 1995] (b) Mixing up of atomic orbitals (a) sp3 sp3 (b) sp2 sp3 (c) Removal of an electron pair (d) Separation of orbitals 2 3 (c) sp sp (d) sp sp 65. The geometry of sulphur trioxide molecule is 54. The compound in which C * uses hybrids for bond formation (a) Tetrahedral (b) Trigonal planar is [IIT 1989] (c) Pyramidal (d) Square planar
66. The shapes of BCl3 , PCl3 and ICl3 molecules are all (a) HCOOH (b) (NH ) CO 2 2 (a) Triangular (b) Pyramidal (c) T shaped (d) All above are incorrect (c) (NH 3 )3COH HgCl2 (d) CH 3CHO 67. In benzene molecule all bond lengths are equal because (a) All carbon atoms are equivalent (a) SnCl 2 (b) HCl (b) All carbon atoms are sp2 hybridised (c) (d) HgCl2 (c) All C C bonds in benzene, have same order 79. Which one of the following statements is true for ammonium ion [EAMCET 1997] (d) All bonds are single covalent bond (a) All bonds are ionic 68. Which one is false in the following statements (b) All bonds are coordinate covalent [MP PET 1997] (c) H atoms are situated at the corners of a square (a) Each carbon in ethylene is in hybridisation (d) atoms are situated at the corners of a tetrahedron (b) Each carbon in acetylene is in sp3 hybridisation 80. The bond angle in hybridisation is [RPMT 1997] (c) Each carbon in benzene is in hybridisation (a) 180o (b) (d) Each carbon in ethane is in hybridisation (c) 90o (d) 109o 2' 69. Out of the following hybrid orbitals, the one which forms the bond 81. The correct order towards bond angle is [RPMT 1997] at angle 120o , is [MP PMT 1997] (a) sp sp2 sp3 (a) d 2 sp3 (b) (b) sp2 sp sp3 (c) (d) sp (c) sp3 sp2 sp 70. As the p character increases, the bond angle in hybrid orbitals formed by s and atomic orbitals [MP PMT 1997] (d) Bond angle does not depend on hybridisation (a) Decreases (b) Increases 82. The geometry and the type of hybrid orbital present about the
(c) Doubles (d) Remains unchanged central atom in BF3 is [IIT 1998; BHU 2001] 71. hybridization leads to which shape of the molecule (a) Linear, (b) Trigonal planar, [MP PET/PMT 1998] (c) Tetrahedral, (d) Pyramidal, (a) Tetrahedron (b) Octahedron (c) Linear (d) Plane triangle 83. In graphite, electrons are [CBSE PMT 1997] 72. Which of the following will be octahedral [MP PET 1999] (a) Localised on every third C atom
(b) Present in antibonding orbital (a) SF6 (b) BF4 (c) Localised on each atom 3 (c) PCl5 (d) BO3 (d) Spread out between the structure [CET Pune 1998] 73. The hybrid orbitals used by central atoms in BeCl 2 , BCl3 and 84. The ammonium ion is (a) Tetrahedral (b) Trigonal pyramidal CCl 4 molecules are respectively [MP PMT 1999] (c) Square planar (d) Square pyramidal (a) sp2 , sp3 and (b) sp , sp2 and sp3 85. In hybridisation, shape is [Bihar MEE 1997] (c) sp3 , sp and sp2 (d) sp2 , sp and (a) Angular (b) Tetrahedral (c) Bipyramidal (d) Linear 74. The structure of H 2 O2 is [CBSE PMT 1999; AFMC 2003] (e) None of these (a) Planar (b) Non-planar (c) Spherical (d) Linear 86. When the hybridisation state of carbon atom changes from to 75. Which of the following is isoelectronic as well as has same structure to sp, the angle between the hybridised orbitals as that of [CPMT 1999] N 2 O [AIIMS 1998]
(a) N 3 H (b) H 2 O (a) Decreases gradually (b) Increases gradually (c) Decreases considerably (d) All of these (c) NO 2 (d) CO 2 87. The structure and hybridisation of is 76. has the hybridisation [DPMT 1996] Si(CH 3 )4 [CBSE PMT 1996] (a) sp3 d (b) dsp2 (a) Bent, (b) Trigonal, (c) (d) 77. Compound having planar symmetry is [DPMT 1996] (c) Octahedral, (d) Tetrahedral, 88. The type of hybridisation of boron in diborane is (a) H 2 SO4 (b) [BHU 1999] (c) HNO 3 (d) (a) sp - hybridisation (b) sp2 - hybridisation 78. Which of the following compounds is not linear 3 3 2 [CPMT 1996] (c) sp - hybridisation (d) sp d - hybridisation 89. Which compound does not possess linear geometry [RPET 1999] 101. The bond angle is minimum in [Pb. PMT 2001; MP PET 2003; UPSEAT 2004] (a) CH 2 CH 2 (b) HC CH (a) H 2 Te (b) H 2 Se (c) BeCl 2 (d) CO 2 (c) H O (d) H S 90. Which of the following molecule does not show tetrahedral shape [RPET 1999] 2 2 102. The correct order of hybridization of the central atom in the (a) CCl (b) SiCl 4 4 2 following species [PtCl4 ] , PCl5 and BCl3 is (c) SF (d) CF 4 4 [IIT Screening 2001; BHU 2005] 91. Pyramidal shape would be of [RPET 1999] 2 3 2 3 2 3 2 (a) dsp , dsp , sp and (b) sp , dsp , dsp , sp (a) NO (b) H O 3 2 (c) dsp2 , sp2 , sp3 , dsp3 (d) dsp2 , sp3 , sp2 , dsp3 (c) H 3 O (d) NH 4 103. Which of the following pairs has same structure [BHU 2001]
92. What is the correct mode of hybridization of the central atom in the (a) and BCl3 (b) and NH 3 following compounds : NO , SF PF 2 2 4, 6 (c) PCl5 and SF6 (d) NH 4 and SO 4 [AMU 1999] 104. The smallest bond angle is found in [AIIMS 2001] 2 3 2 3 3 3 2 3 2 (a) IF (b) CH (a) sp , sp , d sp (b) sp , sp d , sp d 7 4
3 3 2 2 3 (c) BeF (d) BF (c) sp, sp d, sp d (d) sp, sp , sp 2 3 105. Which of the following is not linear [DCE 2001] 93. The hybridization in PF is [DCE 2000] 3 (a) (b) CO 2 ClO2 3 2 (a) sp (b) sp (c) I3 (d) None of these (c) dsp3 (d) d 2 sp3 106. Which of the following is not tetrahedral [MP PMT 2001] 94. Which of the following molecule is linear [MP PMT 2000] (a) (b) SCl 4 (a) (b) NO 2 SO 2 2 (c) Ni(CO)4 (d) NiCl4 107. As the s-character of hybridisation orbital increases, the bond angle [BHU 2002; RPMT 2002] (c) NO 2 (d) SCl 2 (a) Increases (b) Decreases 3 2 95. The geometry of the molecule with sp d hybridised central atom (c) Becomes zero (d) Does not change is [NCERT 1981; AFMC 1982; RPMT 2000] 108. The shape of IF7 molecule is (a) Square planar (b) Trigonal bipyramidal [AFMC 2002; MHCET 2003] (c) Octahedral (d) Square pyramidal (a) Octahedral (b) Pentagonal bipyramidal
96. The bond angle in PH3 is [RPMT 2000] (c) Trigonal bipyramidal (d) Tetrahedral 109. A completely filled d orbital (d 10 ) [UPSEAT 2002] (a) Much less than NH 3 (a) Spherically symmetrical (b) Equal to that of (b) Has octahedral symmetry
(c) Much greater than (c) Has tetrahedral symmetry
(d) Depends on the atom (d) Slightly greater than 110. Which has hybridization of central atom 97. Which of the following has tetrahedral structure [UPSEAT 2002] [CPMT 2000] (a) PCl (b) SO 3 3 (a) CO 3 (b) (c) (d) NO 3 (c) (d) None of these K4 [Fe(CN )6 ] 111. In which of the following species is the interatomic bond angle is 98. The single, double and triple bond lengths of carbon in carbon 109o 28 [AIEEE 2002] dioxide are respectively [AIIMS 2000] (a) NH , (BF )1 (b) (NH ) , BF (a) 1.15, 1.22 and 1.10 Å (b) 1.22, 1.15 and 1.10 Å 3 4 4 3 1 (c) 1.10, 1.15 and 1.22 Å (d) 1.15, 1.10 and 1.22 Å (c) NH 3 , BF4 (d) (NH 2 ) , BF3 99. Shape of BF molecule is [CPMT 2000; Pb. CET 2002] 112. A square planar complex is formed by hybridisation of which atomic 3 orbitals [AIEEE 2002] (a) Linear (b) Planar (a) s, p , p , d (b) s, p , p , d x y yz x y x 2 y2 (c) Tetrahedral (d) Square pyramidal (c) s, p , p d (d) s, p , p ,d 2 3 x y, z 2 y z xy 100. In the complex [SbF5 ] , sp d hybridization is present. Geometry of the complex is [Pb. PMT 2000] 113. In benzene, all the six C – C bonds have the same length because (a) Square (b) Square pyramidal of [MP PET 2002] (c) Square bipyramidal (d) Tetrahedral (a) Tautomerism (b) hybridisation
(c) Isomerism (d) Inductive effect (c) SO3 (d) NO3 1 114. The bond energies of H H and Cl – Cl are 430 kJ mol and 125. Which of the following has a linear structure [MP PMT 2004] 242 kJ respectively, H for HCl is 91 kJ mol-1. The bond (a) (b) t CCl 4 C2H2 energy of HCl will be [MP PET 2003] (c) (d) C H (a) 427 kJ (b) 766 kJ 2 4
(c) 285 kJ (d) 245 kJ 126. In a regular octahedral molecule, MX6 , the number X M X bonds at 180° is [CBSE PMT 2004] 115. Which of the following has dsp2 hybridization (a) Six (b) Four
[MP PET 2003] (c) Three (d) Two 2 (a) NiCl (b) 3 2 4 SCl 4 127. sp d hybrid orbitals are [MP PET 2004] 2 (a) Linear bipyramidal (b) Pentagonal (c) NH 4 (d) PtCl4 (c) Trigonal bipyramidal (d) Octahedral 116. Which one of the following is a planar molecule [EAMCET 2003] 128. In an octahedral structure, the pair of d orbitals involved in d 2sp3 hybridization is [CBSE PMT 2004] (a) (b) H O NH 3 3 (a) d ,d (b) d ,d x 2 xz xy yz (c) BCl3 (d) PCl3 (c) d ,d (d) d ,d 117. Which one of the following is a correct set with respect to molecule, x 2 y 2 z 2 xz x 2 y 2 hybridisation and shape [EAMCET 2003] 129. The correct order of bond angles (smallest first) in 2 H S, NH ,BF and SiH is [AIEEE 2004] (a) BeCl 2 , sp , linear 2 3 3 4 (a) H S NH SiH BF (b) , , triangular planar 2 3 4 3
(b) NH 3 H2S SiH4 BF3 (c) BCl3 , , triangular planar (c) H2S SiH4 NH 3 BF3 3 (d) , sp , tetrahedral (d) H2S NH 3 BF3 SiH4 118. Which of the following compounds doesn’t have linear structure [RPET 1997,130. 2003] Which one of the following has the regular tetrahedral structure [AIEEE 2004] (a) CO (b) SO 2 2 (a) (b) BF4 SF4 (c) (d) BeCl 2 C2 H 2 (c) XeF (d) Ni(CN ) 2 119. Which of the following bonds require the largest amount of bond 4 4 energy to dissociate the atom concerned (Atomic no. : B 5,S 16, Ni 28, Xe 54 ) [UPSEAT 2003] 131. The states of hybridazation of boron and oxygen atoms in boric acid (a) H – H bond in H (b) bond in CH [AIEEE 2004] 2 C – C 4 (H3 BO3 ) are respectively (c) N N bond in N (d) O O bond in O 3 2 2 2 (a) sp and sp (b) and
(e) bond in ethane (c) and (d) and 120. The percentage s-character of the hybrid orbitals in methane, ethene and ethyne are respectively [KCET 2003] 132. The hybridisation in molecule is [Pb. PMT 2004] (a) 25, 33, 50 (b) 25, 50, 75 (a) sp (b)
(c) 50, 75, 100 (d) 10, 20, 40 (c) (d) sp3d 121. Arrange the hydra-acids of halogens in increasing order of acidity [Orissa JEE 2003] (a) HF HCl HBr HI (b) HI HBr HCl HF 133. Among the compounds, BF3, NCl 3,H2S,SF4 and BeCl2 ,
identify the ones in which the central atom has the same type of (c) (d) HF HBr HI HCl HF HI HBr HCl hybridisation [Kerala PMT 2004] 2 122. Which one has sp hybridisation [MP PMT 2004] (a) and (b) and NCl 3 H2S (a) (b) CO 2 N 2O (c) BF3, NCl 3 and (d) and (c) SO2 (d) CO 123. Among the following compounds the one that is polar and has (e) and central atom with hybridization is 134. The molecule of has 180° bond angle. It can be explanid on [MP PMT 2004; IIT 1997] the basis of [AFMC 2004] (a) H CO (b) BF 2 3 3 (a) hybridisation (b) hybridisation
(c) SiF4 (d) HClO2 124. The molecule which is pyramid shape is (c) hybridisation (d) hybridisation [MP PMT 2004; EAMCET 1985; IIT 1989] 135. sp3 hybridisation is found in (a) PCl (b) CO 2 3 3 [Pb. CET 2003; Orissa JEE 2005] (a) 2 (b) (c) or (d) 3 2 or 2 3 CO 3 BF3 d sp d sp
146. The valency of carbon is four. On what principle it can be explained (c) NO 3 (d) NH 3 in a better way 136. Which set hydridisation is correct for the following compounds[Pb. CET 2003] (a) Resonance (b) Hybridization (c) Electron transfer (d) None of the above NO , SF PF 2 4 6 147. Hybridization is due to the overlapping of [MADT Bihar 1983] (a) sp , sp2 , sp3 (a) Orbitals of different energy levels (b) , sp3d , sp3d 2 (b) Orbitals of different energy content
(c) Orbitals of same energy content 2 3 (c) , , d sp (d) None of the above
(d) , , 148. If a molecule MX3 has zero dipole moment, the sigma bonding orbital used by M are 137. The state of hybridisation of in is B BCl3 [IIT 1981; MP PMT 1994; Kerala PMT 2004] [Pb. CET 2000; BHU 2004] (a) sp3 d hybrid (b) sp hybrid (a) (b) 3 2 2 (c) sp d hybrid (d) sp hybrid (c) (d) sp2d 2 149. The linear structure is assumed by [IIT 1991] (a) SnCl 2 (b) NCO 138. The hybrid state of sulphur in SO3 molecule is [DCE 2004] (c) CS (d) NO (a) (b) 2 2
150. Hybridisation of central atom in NF3 is [Orissa JEE 2005] (c) (d) (a) sp3 (b) 139. Which of the following molecules has pyramidal shape 2 2 [DCE 2004; J&K CET 2005] (c) sp (d) dsp 151. The pair having similar geometry is [J&K CET 2005] (a) (b) PCl3 (a) PCl3, NH 3 (b) BeCl2, H2O (c) (d) (c) CH 4 , CCl 4 (d) IF5, PF5 140. The hybrdization of IF is [Pb. CET 2001] 7 152. The d-orbital involved in sp3d hybridisation is (a) sp3d 3 (b) sp2d [J&K CET 2005]
(a) d 2 2 (b) d xy (c) (d) x y (c) d (d) d 141. In which compound, the hydrogen bonding is the strongest in its z 2 zx liquid phase [Pb. CET 2001] ` Resonance (a) HF (b) HI
(c) CH (d) PH 4 3 1. Which one in the following is not the resonance structure of CO2 142. Geometry of ammonia molecule and the hybridization of nitrogen (a) O C O (b) O C O involved in it are [MH CET 2004] (a) -hybridization and tetrahedral geometry (c) O C O (d) O C O 2. Which of the following molecule contains one pair of non-bonding (b) -hybridization and distorted tetrahedral geometry electrons
(c) -hybridization and triangular geometry (a) CH 4 (b) NH 3 (d) None of these (c) H 2 O (d) 143. Be in BeCl 2 undergoes [MH CET 2004] 3. Resonance is due to [NCERT 1981; Kurukshetra CEE 1998] (a) Diagonal hybridization (a) Delocalization of sigma electrons (b) Trigonal hybridization (b) Delocalization of pi electrons (c) Tetrahedral hybridization (c) Migration of H atoms (d) No hybridization (d) Migration of protons 144. Which of the following is non-linear molecule [DCE 2003] 4. Resonating structures have different [AMU 1983] (a) CO (b) CO 3 2 (a) Atomic arrangements (b) Electronic arrangements (c) (d) CS 2 (c) Functional groups (d) Alkyl groups 145. The trigonal bipyramidal geometry results from the hybridisation[UPSEAT 2004]5. In the cyanide ion, the formal negative charge is on (a) dsp3 or (b) dsp2 or [AMU 1984]
(a) C (c) PF3 (d) NH 3 (b) N 4. Which has the least bond angle [NCERT 1973; (c) Both C and N DPMT 1990; CBSE PMT 1990; UPSEAT 2003]
(d) Resonate between C and N (a) (b) BeF2 6. Which does not show resonance [CPMT 1990] (c) H 2 O (d) (a) Benzene (b) Aniline 5. In compound X , all the bond angles are exactly 109o 28', X is [CBSE PMT 1991] (c) Ethyl amine (d) Toluene (a) Chloromethane (b) Iodoform 7. The enolic form of acetone contains (c) Carbon tetrachloride (d) Chloroform [IIT 1990; Bihar MEE 1997] 6. The shape of SO 2 ion is (a) 9 sigma bonds, 1 pi bond and 2 lone pairs 4 [CPMT 1982; DPMT 1983, 84, 96; Bihar MEE 1997] (b) 8 sigma bonds, 2 pi bonds and 2 lone pairs (a) Square planar (b) Tetrahedral (c) 10 sigma bonds, 1 pi bond and 1 lone pair (c) Trigonal bipyramidal (d) Hexagonal (d) 9 sigma bonds, 2 pi bonds and 1 lone pair 7. Which of the following molecules has one lone pair of electrons on 8. Point out incorrect statement about resonance the central atom [EAMCET 1980; AMU 1982; MNR 1989] [MP PET 1997] (a) (b) (a) Resonance structures should have equal energy (b) In resonance structures, the constituent atoms should be in the (c) (d) PCl5 same position 8. Of the following compounds, the one having a linear structure is[NCERT 1981; CPMT 1991; DPMT 1982; (c) In resonance structures, there should not be the same number MP PMT 1985; AIIMS 1996] of electron pairs (a) NH 2 (b)
(d) Resonance structures should differ only in the location of (c) C2 H 2 (d) electrons around the constituent atoms 9. XeF6 is 2 9. The number of possible resonance structures for CO 3 is (a) Octahedral (b) Distorted octahedral [MP PMT 2000] (c) Planar (d) Tetrahedral (a) 2 (b) 3 10. Which has maximum bond angle [CPMT 1993] (c) 6 (d) 9 (a) CHF3 10. Resonance hybrid of nitrate ion is [RPET 2000] (b) CHCl 3 (a) 1/2O...... N ...... O 1/2 (b) 2/3O...... N ...... O 2/3 (c) CHBr3 O 1/2 O 2/3 (d) All have maximum bond angle 11. Of the following species the one having a square planar structure is [NCERT 1981; MP PMT 1994] (c) 1/3O...... N ...... O 1/3 (d) 2 / 3 O...... N ...... O2 / 3 (a) NH 4 (b) BF4 1/3 O2 / 3 O (c) XeF4 (d) SCl 4 12. In which of the following is the angle between the two covalent 11. 2 anion has which of the following characteristics CO 3 bonds greatest [Roorkee 1999] [NCERT 1975; AMU 1982; MNR 1987; (a) Bonds of unequal length IIT 1981; CPMT 1988; MP PMT 1994] (b) sp2 hybridization of C atom (a) CO 2 (b) (c) Resonance stabilization (c) (d) (d) Same bond angles
13. As the s-character of hybridized orbital decreases, the bond angle [DPMT 1986]
VSEPR Theory (a) Decreases (b) Increases (c) Does not change (d) Becomes zero 1. The structure of Cu H 2 O4 ion is 14. XeF2 molecule is [BHU 1982] [NCERT 1983; MP PMT 1983] (a) Linear (b) Triangular planar (a) Square planar (b) Tetrahedral (c) Pyramidal (d) Square planar (c) Distorted rectangle (d) Octahedral 15. Of the following sets which one does NOT contain isoelectronic 2. The bond angle in PH3 would be expected to be close to species [AIEEE 2005] o o 3 2 2 (a) 90 (b) 105 (a) PO4 , SO4 ,ClO4 (b) CN , N 2,C2 o o (c) 109 (d) 120 2 2 3 2 (c) SO ,CO , NO (d) BO ,CO , NO 3. In which molecule are all atoms coplanar [MP PMT 1994] 3 3 3 3 3 3 16. A molecule which contains unpaired electrons is (a) CH 4 (b) BF3 [NCERT 1982] (b) C2 H 2 NH 3 H 2O CH 4 (a) Carbon monoxide (b) Molecular nitrogen (c) NH H O CH C H (c) Molecular oxygen (d) Hydrogen peroxide 3 2 4 2 2 (d) H 2O NH 3 CH 4 C2 H 2 17. H O is [MADT Bihar 1983] 2 28. Which compound has bond angle nearly to 90 (a) A linear triatomic molecule [Pb. PMT 2001] (a) (b) (b) A bent (angular) triatomic molecule H 2O H 2 S
(c) Both of these (c) NH 3 (d) CH 4 (d) None of these 29. A lone pair of electrons in an atom implies [KCET 2002] 18. Bond angle between two hybrid orbitals is 105o.% s-orbital (a) A pair of valence electrons not involved in bonding (b) A pair of electrons involved in bonding character of hybrid orbital is [MP PMT 1986] (c) A pair of electrons (a) Between 20 21% (b) Between 19 20% (d) A pair of valence electrons (c) Between 21 22% (d) Between 22 23% 30. The bond angle of water is 104.5 o due to [CPMT 2002] 19. The bond angle between H O H in ice is closest to (a) Repulsion between lone pair and bond pair [CPMT 1989; UPSEAT 2002] (b) sp3 hybridization of O (a) 120o 28' (b) 60o (c) Bonding of (c) 90o (d) 105o
20. Which of the following molecules does not have a linear (d) Higher electronegativity of O arrangement of atoms [CBSE PMT 1989] 31. The correct sequence of decrease in the bond angle of the following hybrides is [MP PET 2002] (a) H 2 S (b) C2 H 2 (a) NH 3 PH3 AsH3 SbH 3 (c) BeH 2 (d) CO 2 (b) NH 3 AsH3 PH3 SbH 3 21. BCl3 is a planar molecule while NCl 3 is pyramidal, because [CBSE PMT 1995] (c) SbH AsH PH NH (a) has no lone pair of electrons but has a lone pair 3 3 3 3 (d) PH NH AsH SbH of electrons 3 3 3 3 (b) B Cl bond is more polar than N Cl bond 32. Central atom of the following compound has one lone pair of electrons and (c) Nitrogen atom is smaller than boron atom three bond pairs of electrons [JIPMER 2002] (a) (b) (d) bond is more covalent than bond AlCl3
22. The isoelectronic pair is [AIIMS 2005] (c) (d) BF3 (a) Cl2O, ICl2 (b) ICl2 ,ClO2 33. Among KO 2 , AlO2 , BaO2 and NO 2 unpaired electron is (c) IF2 , I3 (d) ClO2 , CIF2 present in [MP PET 2003] 23. According to VSEPR theory, the most probable shape of the (a) and BaO (b) KO and AlO molecule having 4 electron pairs in the outer shell of the central 2 2 2 atom is [MP PET 1996, 2001] (c) only (d) only (a) Linear (b) Tetrahedral 34. True order of bond angle is [RPET 2003] (c) Hexahedral (d) Octahedral (a) H 2O H 2S H 2Se H 2Te 24. The molecular shapes of SF ,CF and XeF are 4 4 4 (b) H Te H Se H S H O [AIEEE 2005] 2 2 2 2
(a) The same with 2, 0 and 1 lone pairs of electrons on the central (c) H 2S H 2O H 2Se H 2Te atom, respectively (d) H O H S H Te H Se (b) The same with 1, 1 and 1 lone pair of electrons on the central 2 2 2 2 atoms, respectively 35. Which of the following has not a lone pair over the central atom [Orissa JEE 2003] (c) Different with 0, 1 and 2 lone pairs of electrons on the central (a) NH (b) PH 3 3 atom, respectively (d) Different with 1, 0 and 2 lone pairs of electrons on the central (c) (d) atom, respectively 36. In BrF3 molecule,the lone pairs occupy equatorial positions to 25. Which of the following species is planar [JIPMER 1997] minimize [CBSE PMT 2004] 2 (a) CO 3 (b) NH 2 (a) Lone pair- lone pair repuilsion and lone pair-bond pair repulsion (c) PCl (d) None of these 3 (b) Lone pair- lone pair repulsion only
26. The shape of CH 3 species is [RPET 1999] (c) Lone pair- bond pair repulsion only (a) Tetrahedral (b) Square planar (d) Bond pair- bond pair repulsion only
(c) Trigonal planar (d) Linear 37. H 2O is dipolar, whereas BeF2 is not. It is because 27. Which of the following is the correct reducing order of bond-angle [BHU 2000] [CBSE PMT 1989; 2004] (a) NH CH C H H O 3 4 2 2 2 (a) is linear and is angular (b) H O is angular and BeF is linear 2 2 2 (a) O2 (b) O2
(c) The electornegativity of F is greater than that of O 1 1 (c) O2 (d) O2 (d) involves hydrogen bonding whereas is a discrete 5. The bond order is maximum in molecule [AIIMS 1983, 85; CBSE PMT 1994; MP PET 2002] 38. Maximum bond angle is present in [BVP 2004] (a) (b) (a) (b) BCl3 BBr3 (c) (d) (c) BF3 (d) Same for all 6. Which of the following compounds of boron does not exist in the 39. The shape of a molecule of NH 3 , in which central atoms contains free form lone pair of electron, is [MHCET 2003] (a) BCl (b) BF (a) Tetrahedral (b) Planar trigonal 3 3
(c) Square planar (d) Pyramidal (c) BBr3 (d) BH3 40. The largest bond angle is in [DCE 2002; MNR 1984] 7. Molecular orbital theory was developed mainly by (a) (b) [BHU 1987; Pb. CET 2003] AsH3 (a) Pauling (b) Pauling and Slater (c) H 2O (d) PH3 (c) Mulliken (d) Thomson 41. The bond angle in ammonia molecule is [EAMCET 1980] 8. The bond order of a molecule is given by [NCERT 1984] o o (a) 91 8 (b) 93 3' (a) The difference between the number of electrons in bonding (c) 106o45' (d) 109o28' and antibonding orbitals 42. Which of the following gives correct arrangement of compounds (b) Total number of electrons in bonding and antibonding orbitals involved based on their bond strength (c) Twice the difference between the number of electrons in [BHU 2005] bonding and antibonding electrons (a) HF > HCl > HBr > HI (d) Half the difference between the number of electrons in bonding (b) HI > HBr > HCl > HF and antibonding electrons (c) HF > HBr > HCl > HI 9. Oxygen molecule is paramagnetic because (d) HCl > HF > HBr > HI [NCERT 1984; IIT 1984] 43. Which one has a pyramidal structure [CBSE PMT 1990] (a) Bonding electrons are more than antibonding electrons (b) Contains unpaired electrons (a) CH (b) NH 4 3 (c) Bonding electrons are less than antibonding electrons (c) H 2 O (d) CO 2 (d) Bonding electrons are equal to antibonding electrons 44. Among the following the pair in which the two species are not 10. Which one is paramagnetic from the following isostructural is [CBSE PMT 2004] [IIT 1989; CBSE PMT 1995] (a) and NH (b) PF and (a) O (b) BH4 4 6 SF6 2 (c) Both (a) and (b) (d) (c) SiF4 and SF4 (d) IO3 and XeO3 CN 45. The maximum number of 90° angles between bond pair-bond pair 11. The bond order in N 2 ion is [Pb. CET 2004] of electrons is observed in [AIEEE 2004] (a) 1 (b) 2 (a) dsp2 hybridization (b) sp3d hybridization (c) 2.5 (d) 3
12. Out of the following which has smallest bond length (c) dsp3 hybridization (d) sp3d 2 hybridization [RPMT 1997]
(a) O (b) O Molecular orbital theory 2 2 2 (c) (d) O 2 1. Bond order is a concept in the molecular orbital theory. It depends 13. Which of the following molecule is paramagnetic on the number of electrons in the bonding and antibonding orbitals. [CPMT 1980; RPET 1999;MP PMT 1999; RPMT 2000] Which of the following statements is true about it ? The bond order[AIIMS 1980] (a) Chlorine (b) Nitrogen (a) Can have a negative quantity (c) Oxygen (d) Hydrogen (b) Has always an integral value 14. Which molecule has the highest bond order (c) Can assume any positive or integral or fractional value (a) N (b) Li including zero 2 2
(d) Is a non zero quantity (c) He2 (d) 2. The bond order of NO molecule is [MP PET 1996] 15. The molecular electronic configuration of H 2 ion is (a) 1 (b) 2 2 2 x 2 (c) 2.5 (d) 3 (a) 1s (b) 1s 1s 3. When two atomic orbitals combine they form 2 1 3 (c) 1s x 1s (d) 1s (a) One molecular orbital (b) Two molecular orbital 16. The paramagnetic nature of oxygen molecule is best explained on (c) Three molecular orbital (d) Four molecular orbital the basis of [BHU 1996] 4. Which of the following species is the least stable (a) Valence bond theory (b) Resonance (c) Molecular orbital theory (d) Hybridization (c) Equal to that of orbital 17. In which case the bond length is minimum between carbon and nitrogen (d) Double that of orbital 29. In the electronic structure of acetic acid, there are (a) CH 3 NH 2 (b) C6 H 5 CH NOH [AMU 1983] (c) CH CONH (d) CH CN 3 2 3 (a) 16 shared and 8 unshared electrons 18. Which one of the following species is diamagnetic in nature [AIEEE 2005] (b) 8 shared and 16 unshared electrons (c) 12 shared and 12 unshared electrons (a) (b) H He2 2 (d) 18 shared and 6 unshared electrons (c) (d) H 2 H 2 30. Which of the following does not exist on the basis of molecular 19. Which one of the following oxides is expected exhibit paramagnetic orbital theory [AFMC 1990; MP PMT 1996] behaviour [CBSE PMT 2005] (a) (b) He2 (a) CO 2 (b) SO2 (c) He (d) Li (c) ClO2 (d) SiO2 2 2
20. The bond order in N 2 molecule is 31. In P4 O10 , the number of oxygen atoms attached to each [CBSE 1995; Pb. PMT 1999; MP PET 1997] phosphorus atom is [IIT 1995] (a) 1 (b) 2 (a) 2 (b) 3 (c) 3 (d) 4 (c) 4 (d) 2.5 21. Which one is paramagnetic and has the bond order 1/2 [NCERT 1983] 32. Of the following statements which one is correct
(a) O 2 (b) (a) Oxygen and nitric oxide molecules are both paramagnetic because both contain unpaired electrons (c) F (d) H 2 2 (b) Oxygen and nitric oxide molecules are both diamagnetic 22. When two atoms of chlorine combine to form one molecule of because both contain no unpaired electrons chlorine gas, the energy of the molecule [AMU 1982] (c) Oxygen is paramagnetic because it contains unpaired electrons, (a) Greater than that of separate atoms while nitric oxide is diamagnetic because it contains no (b) Equal to that of separate atoms unpaired electrons (c) Lower than that of separate atoms (d) None of the above statement is correct (d) Oxygen is diamagnetic because it contains no unpaired electrons, while nitric oxide is paramagnetic because it contains 23. An atom of an element A has three electrons in its outermost shell and that of B has six electrons in the outermost shell. The formula an unpaired electron
of the compound between these two will be 33. According to the molecular orbital theory, the bond order in C 2 [CPMT 1974, 84; RPMT 1999] molecule is (a) (b) A3 B4 A2 B3 (a) 0 (b) 1
(c) A3 B2 (d) A2 B (c) 2 (d) 3 24. The bond order of individual carbon-carbon bonds in benzene is 34. The molecular[IIT 1980] orbital configuration of a diatomic molecule is (a) One (b) Two 2p2 (c) Between 1 and 2 (d) One and two alternately 1s 2 * 1s 2 2s 2 * 2s 2 2p 2 y x 2p2 25. PCl5 exists but NCl 5 does not because z [EAMCET 1977; MP PET/PMT 1988] Its bond order is (a) Nitrogen has no vacant d-orbitals (a) 3 (b) 2.5 (b) is unstable (c) 2 (d) 1 (c) Nitrogen atom is much smaller (d) Nitrogen is highly inert 35. The difference in energy between the molecular orbital formed and 26. Paramagnetism is exhibited by molecules the combining atomic orbitals is called [NCERT 1979; MP PET 2002] (a) Bond energy (b) Activation energy (a) Not attracted into a magnetic field (c) Stabilization energy (d) Destabilization energy (b) Containing only paired electrons (c) Carrying a positive charge 36. According to molecular orbital theory, the paramagnetism of (d) Containing unpaired electrons molecule is due to presence of [MP PMT 1997] 27. Which one of the following is paramagnetic [DPMT 1985] (a) Unpaired electrons in the bonding molecular orbital
(a) H 2 O (b) NO 2 (b) Unpaired electrons in the antibonding molecular orbital (c) Unpaired electron in the bonding molecular orbital (c) SO 2 (d) CO 2 (d) Unpaired electrons in the antibonding molecular orbital 28. The energy of a 2p orbital except hydrogen atom is [MP PET 1999; BHU 2001] [AMU 1983] 37. The bond order in O 2 is (a) Less than that of 2s orbital (a) 2 (b) 2.5 (b) More than that of orbital (c) 1.5 (d) 3 38. Which of the following is paramagnetic [MP PET 1999] 50. The number of antibonding electron pairs in molecular ion on (a) O 2 (b) CN the basis of molecular orbital theory is [Pb. PMT 2000] (c) CO (d) NO (a) 4 (b) 3 (c) 2 (d) 5 39. If N x is the number of bonding orbitals of an atom and N y is the number of antibonding orbitals, then the molecule/atom will be 51. The bond order of He2 molecule ion is stable if [DPMT 1996] [Pb. PMT 2000; Pb CET 2001] (a) 1 (b) 2 (a) N x N y (b) N x N y 1 1 (c) N N (d) N N (c) (d) x y x y 2 4 40. Which of the following molecular orbitals has two nodal planes 52. Which one[KCET does 1996] not exhibit paramagnetism [DPMT 2000] (a) 2s (b) 2p y (a) ClO2 (b) ClO2 (c) (d) * * NO 2 (c) 2p y (d) 2p x 53. In which of the following pairs the two molecules have identical 41. The number of nodal planes 'd' orbital has [KCET 1996] bond order [MP PMT 2000] (a) Zero (b) One (a) N ,O 2 (b) 2 2 N 2 , (c) Two (d) Three (c) N (d) 42. Atomic number of an element is 26. The element shows 2 , , 54. The bond order is not three for [MP PMT 2001] [CPMT 1996] (a) N (b) O 2 (a) Ferromagnetism (b) Diamagnetism 2 2 (c) Paramagnetism (d) None of these (c) (d) NO 43. What is correct sequence of bond order [BHU 1997] 55. In H 2O2 molecule, the angle between the two O – H planes is [CBSE PMT 2002] (a) O O O (b) O O O 2 2 2 2 2 2 (a) 90o (b) 101o o o (c) O2 O2 O2 (d) O2 O2 O2 (c) 103 (d) 105 56. Which of the following molecule has highest bond energy 44. Which bond is strongest [RPMT 1997] [AIIMS 2002] (a) (b) F F Br F (a) (b) C – C
(c) Cl F (d) I F (c) N – N (d) O – O 45. Which of the following is not paramagnetic [AIIMS 1997] 57. Which of the following species would be expected paramagnetic [UPSEAT 2002] 2 (a) Copper crystals (b) (a) S (b) N 2 Cu (c) Cu (d) H 2 (c) O 2 (d) NO 58. Which of the following is correct for triple bond 46. Which one of the following molecules is paramagnetic [CPMT 2002] [Pb. PMT 1998] (a) 3s (b) 1p, 2s
(a) CO 2 (b) SO 2 (c) 2p, 1s (d) 3p 59. In which of the following pairs molecules have bond order three and (c) (d) H 2 O are isoelectronics [MP PET 2003] 47. N and are converted into monoanions N and 2 2 (a) CN , CO (b) NO , CO respectively, which of the following statements is wrong [CBSE PMT 1997] (c) , O 2 (d) CO, O 2
(a) In N 2 , the N N bond weakens 60. Which of the following is paramagnetic [MP PET 2003] (a) (b) (b) In O2 , the O O bond order increases (c) CO (d) (c) In bond length increases 61. How many bonding electron pairs are there in white phosphorous [MP PET 2003] (d) becomes diamagnetic (a) 6 (b) 12
48. With increasing bond order, stability of a bond (c) 4 (d) 8 [CET Pune 1998] 62. The atomicity of phosphorus is X and the PPˆ P bond angle in the (a) Remains unaltered (b) Decreases molecule is Y. What are X and Y [EAMCET 2003] (c) Increases (d) None of these (a) X = 4, Y = (b) X = 4, Y = 60o 49. Which is not paramagnetic [DCE 1999, 2000] o o (c) X = 3, Y = 120 (d) X = 2, Y = 180 (a) O 2 (b) O 2 2 (c) O 2 (d) 63. From elementary molecular orbital theory we can give the electronic (b) Bond length in is greater than in
configuration of the singly positive nitrogen molecular ion N as [UPSEAT 2003] 2 (c) Bond length in is greater than in (a) (1s)2 (1s)2(2s)2 (2s)2(2p)4(2p)1 (d) Bond length is unpredictable
2 2 2 2 1 3 73. Which of the following is diamagnetic [BVP 2004] (b) (1s) (1s) (2s) (2s) (2p) (2p) (a) Oxygen molecule (b) Boron molecule
2 2 2 2 4 (c) (1s) (1s) (2s) (2p) (2p) (c) N 2 (d) None 2 2 2 2 2 2 (d) (1s) (1s) (2s) (2s) (2p) (2p) 74. Bond energies in NO, NO and NO are such as 64. The paramagnetic property of the oxygen molecule due to the presence of unpaired electorns present in [Pb. CET 2004] [Kerala PMT 2004] (a) NO NO NO (b) NO NO NO
1 * 1 (a) ( 2p x ) and ( 2px ) (c) NO NO NO (d) NO NO NO (b) and 1 75. Which of the following is paramagnetic [UPSEAT 2004] ( 2p y ) (a) B (b) C 1 1 2 2 (c) ( * 2p y ) and ( * 2p z ) (c) N 2 (d) F2 1 (d) and ( 2p y ) 76. The paramagnetic molecule at ground state among the following is[UPSEAT 2004] 1 1 (a) H (b) O (e) ( * 2pz ) and ( 2pz ) 2 2 3 (c) (d) 65. In PO4 ion, the formal charge on each oxygen atom and 77. Which has the highest bond energy [DCE 2002] P O bond order respectively are [DPMT 2004] (a) (b) Cl (a) 0.75, 1.25 (b) 0.75, 1.0 2
(c) Br (d) I (c) 0.75, 0.6 (d) 3, 1.25 2 2 78. In O , and O 2 molecular species, the total number of 66. The bond order in CO 2 ion between C O is 2 2 3 antibonding electrons respectively are [DCE 2003] [Pb. PMT 2004] (a) 7, 6, 8 (b) 1, 0, 2 (a) Zero (b) 0.88 (c) 6, 6, 6 (d) 8, 6, 8 (c) 1.33 (d) 2 79. Which of the following is not paramagnetic [DCE 2002] 67. The bond order of O is the same as in [CPMT 2004] 2 (a) (b) O 2 2 (a) (b) CN N 2 2 (c) O 2 (d) O 2 (c) CO (d) NO 80. Which of the following species have maximum number of unpaired electrons [AIIMS 1983] 68. Bond order of O2 is [DPMT 2004] (a) 2 (b) 1.5 (a) (b) O 2
(c) 3 (d) 3.5 (c) (d) 69. The total number of electron that takes part in forming bonds in 81. The correct order in which the O – O bond length increases in the N 2 is [MP PET 2004] following is [BHU 2000; CBSE PMT 2005] (a) 2 (b) 4 (a) H2O2 O2 O3 (b) O2 H2O2 O3 (c) 6 (d) 10 (c) O2 O3 H2O2 (d) O3 H2O2 O2 70. The bond length the species O2,O2 and O2 are in the order of 82. Correct[MP order PET of 2004] bond length is [Orissa JEE 2005] (a) O O O (b) O O O (a) CO 2 CO CO (b) CO CO CO 2 2 2 2 2 2 2 3 2 2 3 (c) CO CO CO 2 (d) None of these (c) O2 O2 O2 (d) O2 O2 O2 2 3 71. According to molecular orbital theory which of the following 83. Which of the following is paramagnetic [DPMT 2005] statement about the magnetic character and bond order is correct (a) N 2 (b) C2 regarding [IIT JEE Screening 2004] 2 (c) N 2 (d) O2 (a) Paramagnetic and bond order< 84. Among the following molecules which one have smallest bond angle[Orissa JEE 2005] (a) (b) (b) Paramagnetic and bond order> NH 3 PH3
(c) H O (d) H Sc (c) Dimagnetic and bond order< 2 2 (e) H S (d) Dimagnetic and bond order> 2
72. The bond order in NO is 2.5 while that in is 3. Which of the Hydrogen bonding following statements is true for these two species 1. In the following which bond will be responsible for maximun value [AIEEE 2004] of hydrogen bond (a) Bond length in is equal to that in NO (a) O H (b) N H (c) S H (d) F H 13. The pairs of bases in DNA are held together by 2. In which of the following hydrogen bond is present [NCERT 1978; DPMT 1985; CBSE PMT 1992]
(a) H 2 (b) Ice (a) Hydrogen bonds (b) Ionic bonds (c) Sulphur (d) Hydrocarbon (c) Phosphate groups (d) Deoxyribose groups 3. In the following which has highest boiling point 14. Water has high heat of vaporisation due to [AFMC 1982] [MP PMT 1989; RPMT 1997] (a) HI (b) HF (a) Covalent bonding (b) H bonding (c) HBr (d) HCl (c) Ionic bonding (d) None of the above 4. Which contains hydrogen bond [MP PMT 1989] 15. In which of the following compounds does hydrogen bonding occur [CBSE PMT 1989] (a) (b) (a) SiH 4 (b) LiH (c) (d) (c) (d) 5. Contrary to other hydrogen halides, hydrogen fluoride is a liquid because [MP PMT 1990; AMU 1983; EAMCET 1980] 16. Which among the following compounds does not show hydrogen (a) Size of F atom is small bonding [MP PMT 1989] (a) Chloroform (b) Ethyl alcohol (b) is a weak acid (c) Acetic acid (d) Ethyl ether (c) molecule are hydrogen bonded 17. Acetic acid exists as dimer in benzene due to [CPMT 1982] (d) Fluorine is highly reactive (a) Condensation reaction 3 6. In the following which species does not contain sp hybridization (b) Hydrogen[DPMT 1985] bonding (c) Presence of carboxyl group (a) NH 3 (b) CH 4 (d) Presence of hydrogen atom at carbon (c) H2O (d) CO2 18. Which one among the following does not have the hydrogen bond [IIT 1983; MP PMT 1994; [IIT 1984] 7. As a result of sp hybridization, we get UPSEAT 2001] (a) Two mutual perpendicular orbitals (a) Phenol (b) Liquid o (b) Two orbitals at 180 (c) Water (d) Liquid (c) Four orbitals in tetrahedral directions 19. The bond that determines the secondary structure of a protein is[NCERT 1984; MP PET 1996] (d) Three orbitals in the same plane (a) Coordinate bond (b) Covalent bond 8. The reason for exceptionally high boiling point of water is (c) Hydrogen bond (d) Ionic bond [DPMT 1986; NCERT 1976; AMU 1984; EAMCET 1979; 20. is a gas but is a low boiling liquid. This is because MP PMT 1993; AIIMS 1996; KCET 2001; CPMT 2003] [NCERT 1984; MP PMT 2001] (a) Its high specific heat (a) H F bond is strong (b) Its high dielectric constant (b) bond is weak (c) Low ionization of water molecules (c) Molecules aggregate because of hydrogen bonding (d) Hydrogen bonding in the molecules of water 9. Which concept best explains that o-nitrophenol is more volatile than (d) is a weak acid p-nitrophenol 21. The relatively high boiling point of is due to [AIIMS 1980, 82; Kurukshetra CEE 1998; MP PET 2002] [NCERT 1984] (a) Resonance (b) Hyperconjugation (a) Hydrogen bonding (c) Hydrogen bonding (d) Steric hindrence (b) Covalent bonding 10. Which contains strongest H bond (c) Unshared electron pair on [IIT 1986; MP PET 1997, 2003; UPSEAT 2001, 03] (d) Being a halogen acid (a) O H..... S (b) S H..... O 22. Water is liquid due to [MADT Bihar 1983] (c) F H..... F (d) F H..... O (a) Hydrogen bonding (b) Covalent bond 11. Which of the following compound can form hydrogen bonds (c) Ionic bond (d) Vander Waals forces [NCERT 1978; MP PMT 1997] 23. The maximum possible number of hydrogen bonds in which an molecule can participate is (a) CH 4 (b) NaCl [MP PMT 1986; MNR 1991; IIT 1992;MP PET 1999] (c) (d) CHCl 3 H 2 O (a) 1 (b) 2 12. Of the following hydrides which has the lowest boiling point (c) 3 (d) 4 [CBSE PMT 1987] 24. Hydrogen bonding is maximum in
(a) NH 3 (b) PH3 [IIT 1987; MP PMT 1991; MP PET 1993, 2001; MNR 1995; CPMT 1999; KCET (Med.) 2002] (c) SbH (d) AsH 3 3 (a) Ethanol (b) Diethyl ether (c) Ethyl chloride (d) Triethyl amine 35. Ethanol and dimethyl ether form a pair of functional isomers. The 25. The hydrogen bond is strongest in boiling point of ethanol is higher than that of dimethyl ether due to the presence of [AIIMS 1998] [BHU 1987; CBSE PMT 1990, 92] (a) Hydrogen bonding in ethanol (a) Water (b) Ammonia (b) Hydrogen bonding in dimethyl ether (c) Hydrogen fluoride (d) Acetic acid (c) CH group in ethanol 26. The high boiling point of ethanol (78.2o C) compared to dimethyl 3 (d) group in dimethyl ether ether (23.6 o C) , though both having the same molecular formulae 36. Which of the following hydrogen bonds are strongest in vapour C H O , is due to [MP PMT 1993] 6 6 phase [AMU 1999] (a) Hydrogen bonding (a) HF HF (b) HF HCl (b) Ionic bonding (c) (d) (c) Coordinate covalent bonding HCl HCl HF HI (d) Resonance 37. Which of the following shows hydrogen bonding 27. Methanol and ethanol are miscible in water due to [CPMT 2000] [CPMT 1989] (a) (b) P (a) Covalent character (c) As (d) Sb (b) Hydrogen bonding character 38. The boiling point of a compound is raised by [DPMT 2001] (c) Oxygen bonding character (a) Intramolecular hydrogen bonding (d) None of these (b) Intermolecular hydrogen bonding o o 28. B.P. of H 2 O(100 C) and H 2 S (42 C) explained by (c) Covalent bonding (a) Vander Waal's forces (b) Covalent bond (d) Ionic covalent (c) Hydrogen bond (d) Ionic bond 39. The boiling point of water is exceptionally high because 29. Strength of hydrogen bond is intermediate between [KCET 2001] [DPMT 1991] (a) Water molecule is linear (a) Vander Waal and covalent (b) Water molecule is not linear (b) Ionic and covalent (c) There is covalent bond between H and O (c) Ionic and metallic (d) Water molecules associate due to hydrogen bonding (d) Metallic and covalent 40. has a much higher boiling point than because 30. In which of the following compounds intramolecular hydrogen bond [UPSEAT 2002; MNR 1994] is present [MP PET 1994] (a) Ethyl alcohol (b) Water (a) NH 3 has a larger molecular weight (c) Salicylaldehyde (d) Hydrogen sulphide (b) undergoes umbrella inversion 31. Hydrogen bonding is formed in compounds containing hydrogen and [MP PET 1995] (c) forms hydrogen bond (a) Highly electronegative atoms (d) contains ionic bonds whereas contains covalent (b) Highly electropositive atoms bonds (c) Metal atoms with d-orbitals occupied 41. Which one has the highest boiling point [MP PET 2002] (d) Metalloids (a) Acetone (b) Ethyl alcohol 32. Which of the following compounds in liquid state does not have (c) Diethyl ether (d) Chloroform hydrogen bonding [MP PMT 1996] 42. Which of the following compounds has the highest boiling point [JIPMER 2002] (a) H O (b) HF 2 (a) HCl (b) HBr
(c) NH 3 (d) C6 H 6 (c) (d) H 2 SO4 HNO 3
33. Compounds showing hydrogen bonding among HF, NH 3 , H 2 S 43. Which of the following has minimum melting point [UPSEAT 2003] and PH3 are (a) CsF (b) HCl
(a) Only HF, NH 3 and (c) HF (d) LiF (b) Only and 44. Hydrogen bond energy is equal to [UPSEAT 2003] (c) Only NH , H S and (a) 3 – 7 cals (b) 30 – 70 cals 3 2 (d) All the four (c) 3 – 10 kcals (d) 30 – 70 kcals 34. The high density of water compared to ice is due to 45. H 2O is a liquid while H 2 S is gas due to [BHU 2003] [CBSE PMT 1997; BHU 1999; AFMC 2001] (a) Covalent bonding (a) Hydrogen bonding interactions (b) Molecular attraction (b) Dipole-dipole interactions (c) Dipole-induced dipole interactions (c) H – bonding (d) Induced dipole-induced dipole interactions (d) H – bonding and molecular attraction 46. H – bonding is maximum in [BHU 2003] (a) Overlapping valency orbitals (a) (b) (b) Mobile valency electrons C6 H 5 OH C6 H 5 COOH (c) Delocalized electrons (c) CH 3 CH 2OH (d) CH 3 COCH 3 (d) Highly directed bonds 47. Select the compound from the following which dissolves in water 8. In melting[IIT lattice,1980] structure of solid [CPMT 1982] (a) Remains unchanged (b) Changes (a) CCl (b) CS 4 2 (c) Becomes compact (d) None of the above
(c) CHCl3 (d) C2H5OH 9. Which of the following has the highest melting point [CPMT 1994] 48. When two ice cubes are pressed over each other, they unit to form one cube. Which of the following force is responsible for holding (a) Pb (b) Diamond them together [NCERT 1978] (c) Fe (d) Na (a) Vander Waal's forces 10. In the formation of a molecule by an atom [AFMC 1995] (b) Hydrogen bond formation (a) Attractive forces operate (c) Covalent attraction (b) Repulsive forces operate (c) Both attractive and repulsive forces operate (d) Dipole–dipole attraction (d) None of these 49. Which is the weakest among the following types of bond 11. Which has weakest bond [RPMT 1997] [NCERT 1979; MADT Bihar 1984] (a) Diamond (b) Neon (Solid) (a) Ionic bond (b) Metallic bond (c) KCl (d) Ice (c) Covalent bond (d) Hydrogen bond 12. Which of the following exhibits the weakest intermolecular forces[AIIMS 1999; BHU 2000] 50. H-bond is not present in [BCECE 2005] (a) He (b) HCl (a) Water (b) Glycerol (c) NH 3 (d) H 2 O (c) Hydrogen fluoride (d) Hydrogen Sulphide 13. Glycerol has strong intermolecular bonding therefore it is
[RPET 2000] Types of bonding and Forces in solid (a) Sweet (b) Reactive (c) Explosive (d) Viscous 1. In a crystal cations and anions are held together by 14. Among the following the weakest one is [EAMCET 1982] [Pb. PMT 2004; CPMT 2002] (a) Electrons (b) Electrostatic forces (a) Metallic bond (b) Ionic bond
(c) Nuclear forces (d) Covalent bonds (c) Van der Waal's force (d) Covalent bond 2. In the following metals which one has lowest probable interatomic 15. Lattice energy of alkali metal chlorides follows the order forces [MP PMT 1990] [DPMT 2004] (a) Copper (b) Silver (a) LiCl NaCl KCl RbCl CsCl (b) (c) Zinc (d) Mercury CsCl NaCl KCl RbCl LiCl 3. In solid argon, the atoms are held together by (c) LiCl CsCl NaCl KCl RbCl [NCERT 1981; MP PET 1995] (d) NaCl LiCl KCl RbCl CsCl (a) Ionic bonds (b) Hydrogen bonds 16. In the following which molecule or ion possesses electrovalent, covalent and co-ordinate bond at the same time [CPMT 1987] (c) Vander Waals forces (d) Hydrophobic forces 4. Which one is the highest melting halide [AIIMS 1980] (a) (b) NH 4 (a) (b) NaCl NaBr (c) Cl (d) H2O2 (c) NaF (d) NaI 17. Both ionic and covalent bond is present in the following 5. The enhanced force of cohesion in metals is due to [MNR 1986; MP PMT 2004] [NCERT 1972] (a) CH (b) (a) The covalent linkages between atoms 4
(b) The electrovalent linkages between atoms (c) SO2 (d) NaOH (c) The lack of exchange of valency electrons 18. The formation of a chemical bond is accompanied by (d) The exchange energy of mobile electrons [MP PET 1995] 6. Which one of the following substances consists of small discrete (a) Decrease in energy molecules [CPMT 1987] (b) Increase in energy (a) (b) Graphite (c) Neither increase nor decrease in energy (c) Copper (d) Dry ice (d) None of these 7. Which of the following does not apply to metallic bond 19. Chemical bond implies [KCET 2002] [CBSE PMT 1989] (a) Attraction [UPSEAT 2001] (b) Repulsion (a) (b) N 2 H 5 BaCl2 (c) Neither attraction nor repulsion (c) HCl (d) (d) Both (a) and (b) H 2 O 20. Which of the following statements is true [AIEEE 2002] 6. Which combination is best explained by the co-ordinate covalent (a) HF is less polar than HBr bond [JIPMER 2001; CBSE PMT 1990] (b) Absolutely pure water does not contain any ions (a) (b) Cl + Cl H H 2 O (c) Chemical bond formation take place when forces of attraction 1 overcome the forces of repulsion (c) Mg O (d) H I 2 2 2 2 (d) In covalency transference of electron takes place 7. Arrange the following compounds in order of increasing dipole 21. Which of the following statements is true about Cu NH SO [CPMT 1988] 3 4 4 moment. (a) It has coordinate and covalent bonds (I) Toluene (II) m dichlorobenzene (b) It has only coordinate bonds (III) o dichlorobenzene (IV) p dichlorobenzene (c) It has only electrovalent bonds [IIT 1996] (d) It has electrovalent, covalent and coordinate bonds (a) I IV II III (b) IV I II III 22. Blue vitriol has (c) IV I III II (d) IV II I III (a) Ionic bond (b) Coordinate bond 8. The correct order of dipole moment is [Roorkee 1999] (c) Hydrogen bond (d) All the above (a) CH 4 NF3 NH 3 H 2O 23. The number of ionic, covalent and coordinate bonds in NH 4 Cl are respectively [MP PMT 1999] (b) NF3 CH 4 NH 3 H 2O (a) 1, 3 and 1 (b) 1, 3 and 2 (c) NH 3 NF3 CH 4 H 2O (c) 1, 2 and 3 (d) 1, 1 and 3 (d) H O NH NF CH 24. Covalent molecules are usually held in a crystal structure by 2 3 3 4 9. Which of the following has the highest dipole moment [MP PET 1995] [AIIMS 2002] (a) Dipole-dipole attraction H CH 3 (b) Electrostatic attraction H | | (a) C O (b) C C
(c) Hydrogen bonds H | | H (d) Vander Waal's attraction CH 3
CH 3 H Cl CH 3 | | | | (c) C C (d) C C | | | | CH H 3 CH 3 Cl 10. Which of the following arrangement of molecules is correct on the
basis of their dipole moments [AIIMS 2002] 1. The values of electronegativity of atoms A and B are 1.20 and 4.0 (a) BF3 NF3 NH 3 (b) NF3 BF3 NH 3 respectively. The percentage of ionic character of A – B bond is [MP PET 2003] (c) NH BF NF (d) NH NF BF (a) 50 % (b) 43 % 3 3 3 3 3 3
11. The type of hybrid orbitals used by the chlorine atom in ClO is [IIT 1992] (c) 55.3 % (d) 72.24% 2 (a) sp3 (b) sp2 2. O 2 is the symbol of ….. ion [EAMCET 2003] 2 (c) sp (d) None of these (a) Oxide (b) Superoxide 12. Among the following species, identify the isostructural pairs, (c) Peroxide (d) Monoxide NF3 , NO 3 , BF3 , H 3 O , HN3 [IIT 1996] 3. The number of electrons that are paired in oxygen molecule is [IIT 1995] (a) [NF3 , NO 3 ] and [BF3 , H 3 O ] (a) 7 (b) 8 (b) [NF , HN ] and [NO , BF ] (c) 14 (d) 16 3 3 3 3 (c) [NF , H O ] and 3 3 4. When N 2 goes to N 2 , the N N bond distance ..... and when (d) and [HN , BF ] 3 3 O 2 goes to O 2 , the O O bond distance ...... 13. In the compound CH CH CH CH C CH, the [IIT 1996] 2 2 2 C C bond is of the type [IIT 1999] (a) Decrease, increase (b) Increase, decrease 2 3 (c) Increase, increase (d) None of these (a) sp sp2 (b) sp3 sp3 5. Which of the following contains a coordinate covalent bond (c) sp sp3 (d) sp2 sp3 (d) Isoelectronic and weak field ligands 24. The number of S – S bonds in sulphur trioxide trimer S 3O9 is [IIT Screening 2001] 14. The correct order of increasing C O bond length of (a) Three (b) Two 2 CO, CO 3 , CO 2 is [IIT 1999] (c) One (d) Zero 25. Strongest intermolecular hydrogen bond is present in the following 2 2 (a) CO 3 CO 2 CO (b) CO 2 CO 3 CO molecules pairs [IIT 1981; DCE 2000] (a) SiH and SiF 2 2 4 (c) CO CO 3 CO 2 (d) CO CO 2 CO 3 O 15. In the dichromate dianion [IIT 1999] || (b) CH C CH and CHCl (a) 4 Cr O bonds are equivalent 3 3 3 O O (b) 6 Cr O bonds are equivalent || || (c) H C OH and CH 3 C OH (c) All Cr O bonds are equivalent (d) H 2 O and H 2 O2 (d) All bonds are non-equivalent 26. A compound contains atoms X, Y, Z. The oxidation number of 16. Bond length of ethane (I), ethene (II), acetylene (III) and benzene (IV) follows the order [CPMT 1999] X is 2, Y is + 5 and Z is 2 . Therefore, a possible formula of the compound is [CPMT 1988] (a) I II III IV (b) I II IV III (a) XYZ (b) X YZ (c) I IV II III (d) III IV II I 2 2 3 2
17. Hybridisation state of chlorine in ClF3 is [RPET 1999] (c) X 3 YZ 4 2 (d) X 3 Y4 Z2
3 3 (a) sp (b) sp d 27. Bonds present in CuSO 4 .5H 2O is [IIT 1983; DCE 2001] (a) Electrovalent and covalent (c) sp3 d 2 (d) sp3 d 3 (b) Electrovalent and coordinate 18. Molecular shapes of SF ,CF and XeF are 4 4 4 (c) Electrovalent, covalent and coordinate [IIT Screening 2000] (a) The same with 2, 0 and 1 lone pairs of electrons respectively (d) Covalent and coordinate (b) The same, with 1, 1 and 1 lone pairs of electrons respectively 28. The ionization of hydrogen atom would give rise to (c) Different, with 0, 1 and 2 lone pairs of electrons respectively [UPSEAT 2001] (d) Different, with 1, 0 and 2 lone pairs of electrons respectively (a) Hybrid ion (b) Hydronium ion 19. Structure of IF and hybridization of iodine in this structure are[UPSEAT 2001] 4 (c) Proton (d) Hydroxyl ion (a) , Linear 29. Which can be described as a molecule with residual bonding (b) , T-shaped capacity [JIPMER 2000] (a) BeCl (b) NaCl (c) sp3d , Irregular tetrahedral 2
(d) , Octahedral (c) CH 4 (d)
20. In which of the following the central atom does not use sp3 hybrid orbitals in its bonding [UPSEAT 2001, 02] (a) BeF (b) 3 OH3 (c) NH 2 (d) NF3
21. The magnetic moment of K3 [Fe(CN )6 ] is found to be 1.7 B.M. How many unpaired electron (s) is/are present per molecule Read the assertion[Orissa and JEE reason 2003] carefully to mark the correct option out of (a) 1 (b) 2 the options given below :
(c) 3 (d) 4 (a) If both assertion and reason are true and the reason is the correct explanation of the assertion. 22. N 2 and O 2 are converted into monocations N 2 and O 2 (b) If both assertion and reason are true but reason is not the correct respectively. Which is wrong [CBSE PMT 1997] explanation of the assertion.
(a) In N 2 , the N N bond weakens (c) If assertion is true but reason is false. (d) If the assertion and reason both are false. (b) In the bond order increases O2 , O O (e) If assertion is false but reason is true. (c) In paramagnetism decreases 1. Assertion : Water is a good solvent for ionic compounds but (d) becomes diamagnetic poor one for covalent compounds. 23. The common features among the species CN , CO and NO are Reason : Hydration energy of ions releases sufficient [IIT Screening 2001] energy to overcome lattice energy and break (a) Bond order three and isoelectronic hydrogen bonds in water, while covalent bonded (b) Bond order three and weak field ligands compounds interact so weakly that even Vander (c) Bond order two and -acceptors Wall's forces between molecules of covalent 16. Assertion : The crystal structure gets stabilized even though compounds cannot be broken. [AIIMS 1996] the sum of electron gain enthalpy and ionization enthalpy is positive. 2. Assertion : The atoms in a covalent molecule are said to share electrons, yet some covalent molecules are Reason : Energy is absorbed during the formation of polar. crystal lattice. 17. Assertion : Order of lattice energy for same halides are as Reason : In a polar covalent molecule, the shared electrons spend more time on the average near one of the LiX NaX KX . atoms. [AIIMS 1996] Reason : Size of alkaline – earth metal increases from Li 3. Assertion : Diborane is electron deficient to K . Reason : There are no enough valence electrons to form 18. Assertion : Born-Haber cycle is based on Hess’s law. the expected number of covalent bonds[AIIMS 2001] Reason : Lattice enthalpy can be calculated by Born- 4. Assertion : A resonance hybrid is always more stable than Haber cycle. any of its canonical structures 19. Assertion : Bond energy has order like Reason : This stability is due to delocalization of electrons[AIIMS 1999] C C C C C C . 5. Assertion : All F S F angle in SF greater than 90° but Reason : Bond energy increases with increase in bond 4 order. less than 180° 20. Assertion : Electron affinity refers to an isolated atom’s Reason : The lone pair-bond pair repulsion is weaker than attraction for an additional electron while bond pair-bond pair repulsion electronegativity is the ability of an element to [AIIMS 2004] attract electrons towards itself in a shared pair of O electrons. 6. Assertion : The electronic structure of O3 is O O Reason : Electron affinity is a relative number and electronegativity is experimentally measurable.
Reason : structure is not allowed because 21. Assertion : Geometry of SF4 molecule can be termed as distorted tetrahedron, a folded square or see saw. octet around cannot be expanded. Reason : Four fluorine atoms surround or form bond with [IIT 1998] sulphur molecule. 7. Assertion : Bond order can assume any value number 22. Assertion : BF3 has greater dipole moment than H 2 S . including zero Reason : Fluorine is more electronegative than sulphur. Reason : Higher the bond order, shorter is bond length and greater is bond energy 23. Assertion : The bond between two identical nonmetal atoms has a pair of electrons with identical spin. [AIIMS 1999] Reason : Electrons are transferred fully from one atom to 8. Assertion : Ortho nitrophenol molecules are associated due to the presence of intermolecular hydrogen bonding while another. 24. Assertion : B molecule is diamagnetic. paranitrophenol involves intramolecular, hydrogen 2 bonding Reason : The highest occupied molecular orbital is of Reason : Ortho nitrophenol is more volatile than the para type. [AIIMS 2005] nitrophenol [AIIMS 1999] 25. Assertion : The nearly tetrahedral arrangement of the 9. Assertion : Nitrogen molecule diamagnetic. orbitals about the oxygen atom allows each water Reason : N molecule have unpaired electrons. molecule to form hydrogen bonds with as many 2 as four neighbouring water molecules. 10. Assertion : Ice is less dense than liquid water. Reason : In ice each molecule forms four hydrogen bonds Reason : There are vacant spaces between hydrogen as each molecule is fixed in the space. bonded water molecules in ice. 26. Assertion : The bond order of helium is always zero. 11. Assertion : Water is liquid but H S is a gas. 2 Reason : The number of electrons in bonding molecular Reason : Oxygen is paramagnetic. orbital and antibonding molecular orbital is 12. Assertion : Iodine is more soluble in water then in carbon equal. tetrachloride. Reason : Iodine is a polar compound. 13. Assertion : o and p -nitrophenols can be separated by steam distillation. Reason : -nitrophenol have intramolecular hydrogen bonding while -nitrophenol exists as associated molecules. Electrovalent bonding
14. Assertion : The fluorine has lower reactivity. Reason : F F bond has low bond dissociation energy. 1 b 2 a 3 a 4 c 5 c 15. Assertion : is strong while is a weak bond. 6 d 7 d 8 b 9 c 10 d Reason : Atoms rotate freely about bond. 11 b 12 a 13 d 14 a 15 a 16 c 17 b 18 a 19 d 20 c 21 b 22 d 23 a 24 a 25 b Polarisation and Fajan’s rule
26 d 27 d 28 c 29 a 30 d 1 d 2 c 3 b 4 d 5 c 31 b 32 b 33 b 34 d 35 b 6 a 7 b 8 a 9 c 10 b 36 a 37 b 38 a 39 a 40 c 11 d 12 c 13 b 14 b 15 d 41 c 42 b 43 d 44 b 45 c 16 d 17 c 18 b 19 a 20 d 46 c 47 a 48 b 49 c 50 b 21 a 22 c 23 d 24 a 25 b 51 b 52 b 53 a 54 a 55 a 26 b 56 c 57 a 58 c 59 a 60 c
61 a 62 b 63 d 64 d 65 b Overlaping - and - bonds 66 a 67 abc 68 bd
1 c 2 c 3 b 4 b 5 c Covalent bonding 6 c 7 c 8 b 9 d 10 c 1 c 2 c 3 B 4 b 5 d 11 b 12 c 13 a 14 a 15 d 6 a 7 c 8 a 9 d 10 a 16 a 17 d 18 c 19 d 20 d 11 b 12 b 13 c 14 b 15 c 16 a 17 a 18 c 19 a 20 b Hybridisation
21 a 22 a 23 c 24 c 25 c 1 d 2 d 3 d 4 c 5 d 26 c 27 a 28 a 29 a 30 d 6 a 7 c 8 b 9 d 10 d 31 b 32 a 33 d 34 a 35 d 11 d 12 a 13 a 14 b 15 a 36 b 37 d 38 c 39 d 40 c 16 b 17 c 18 a 19 d 20 b 41 b 42 b 43 b 44 b 45 b 21 c 22 c 23 a 24 c 25 a 46 d 47 d 48 b 49 a 50 a 26 a 27 b 28 c 29 b 30 a 51 b 52 d 53 c 54 d 55 d 31 d 32 a 33 d 34 c 35 c 56 d 57 a 58 a 59 d 60 a 36 b 37 b 38 c 39 b 40 b 61 c 62 a 63 b 64 b 65 b 41 d 42 b 43 c 44 a 45 c 66 b 67 b 68 d 69 b 70 c 46 c 47 d 48 b 49 c 50 a 71 c 72 c 73 cd 74 ad 75 ab 51 b 52 a 53 c 54 c 55 c 76 a 56 d 57 b 58 a 59 b 60 c
Co-ordinate or Dative bonding 61 b 62 c 63 b 64 b 65 b 66 a 67 c 68 b 69 c 70 a 1 d 2 b 3 c 4 d 5 c 71 a 72 a 73 b 74 b 75 d 6 b 7 a 8 d 9 a 10 d 76 d 77 c 78 a 79 d 80 b 11 c 12 a 13 a 14 b 15 c 81 c 82 b 83 d 84 a 85 d
Dipole moment 86 b 87 d 88 c 89 a 90 c 91 c 92 c 93 a 94 b 95 c 1 b 2 d 3 d 4 a 5 c 96 a 97 b 98 b 99 b 100 b 6 c 7 a 8 a 9 c 10 b 101 a 102 b 103 d 104 a 105 b 11 b 12 d 13 b 14 c 15 d 106 a 107 a 108 b 109 b 110 a 16 c 17 c 18 a 19 c 20 b 111 a 112 b 113 b 114 d 115 d 21 d 22 b 23 b 24 b 25 a 116 c 117 c 118 b 119 c 120 a 26 b 27 b 28 b 29 c 30 a 121 a 122 c 123 a 124 a 125 b 31 a 32 c 33 a 34 bd 35 a 126 c 127 d 128 c 129 c 130 a
131 b 132 b 133 e 134 c 135 d 136 b 137 b 138 d 139 a 140 a 6 d 7 b 8 d 9 c 10 c 141 a 142 b 143 a 144 a 145 a 11 d 12 b 13 a 14 b 15 d 146 b 147 c 148 d 149 bcd 150 a 16 d 17 b 18 d 19 c 20 c 151 ac 152 a 21 a 22 a 23 d 24 a 25 c 26 a 27 b 28 c 29 a 30 c Resonance 31 a 32 b 33 d 34 a 35 a
36 a 37 a 38 b 39 d 40 c 1 d 2 b 3 b 4 b 5 b 41 a 42 c 43 b 44 c 45 c 6 c 7 a 8 c 9 b 10 c 46 b 47 d 48 b 49 d 50 d 11 abcd
Types of bonding and Forces in solid VSEPR Theory 1 b 2 d 3 c 4 c 5 d 1 a 2 a 3 b 4 c 5 c 6 d 7 d 8 b 9 b 10 c 6 b 7 b 8 c 9 b 10 a 11 d 12 a 13 d 14 c 15 a 11 c 12 a 13 a 14 a 15 c 16 b 17 d 18 a 19 d 20 c 16 c 17 b 18 d 19 d 20 a 21 d 22 d 23 a 24 d 21 a 22 d 23 b 24 d 25 a
26 c 27 b 28 b 29 a 30 a Critical Thinking Question 31 a 32 c 33 c 34 a 35 c 36 b 37 b 38 d 39 d 40 b 1 d 2 c 3 c 4 b 5 a 41 c 42 a 43 b 44 c 45 d 6 a 7 b 8 a 9 a 10 d
11 a 12 c 13 d 14 d 15 b Molecular orbital theory 16 c 17 b 18 d 19 c 20 a
21 a 22 d 23 a 24 d 25 c 1 a 2 c 3 b 4 b 5 c 26 c 27 c 28 c 29 a 6 d 7 c 8 b 9 c 10 b
11 c 12 b 13 c 14 a 15 c Assertion & Reason 16 c 17 d 18 b 19 c 20 c 1 a 2 a 3 a 4 a 5 c 21 d 22 c 23 b 24 c 25 a 6 b 7 b 8 e 9 c 10 a 26 d 27 b 28 b 29 a 30 c 11 b 12 d 13 a 14 e 15 c 31 c 32 a 33 c 34 a 35 c 16 c 17 c 18 b 19 a 20 c 36 d 37 b 38 a 39 a 40 c 21 b 22 e 23 d 24 d 25 a 41 c 42 a 43 b 44 a 45 a 26 a 46 c 47 b 48 c 49 c 50 a
51 c 52 b 53 a 54 a 55 a 56 c 57 c 58 c 59 a 60 a 61 a 62 b 63 a 64 c 65 a 66 c 67 a 68 a 69 c 70 a 71 b 72 b 73 d 74 c 75 a 76 b 77 b 78 a 79 c 80 a 81 c 82 a 83 c 84 d
Hydrogen bonding
1 d 2 b 3 b 4 a 5 c 24. (a) M3 (PO4 )2 means M is divalent so formula of its sulphate is
MSO4 .
25. (b) As the molecular formula of chloride of a metal M is MCl3 , it
is trivalent so formula of its carbonate will be M 2 (CO 3 )3 .
26. (d) Sodium chloride is electrovalent compound so it dissolves in Electrovalent bonding water which is a polar solvent.
27. (d) When sodium chloride is dissolved in water, the sodium ion is hydrated. 1. (b) NaCl is ionic crystal so it is formed by Na and Cl ions. 30. (d) Yet the formula of sulphate of a metal (M) is M (SO ) , it is 2. (a) Bond formation is always exothermic. Compounds of sodium 2 4 3 are ionic. M 3 ion so formula of its phosphate would be . 3. (a) According to Fajan’s rule ionic character is less. 32. (b) Molten sodium chloride conducts electricity due to the 4. (c) Valencies of L, Q, P and R is – 2, – 1, + 1 and + 2 respectively so presence of free ions.
they will form P2 L, RL, PQ and RQ2 . 33. (b) The phosphate of a metal has the formula MHPO4 it means
5. (c) Electrovalent compounds are good conductor of heat and metal is divalent so its chloride would be MCl2 . electricity in molten state or in aqueous solution. 34. (d) 7. (d) Electrovalent bond formation depends on ionization energy of 35. (b) Cs is highly electropositive while F is highly cation, electron affinity of anion and on lattice energy. electronegative so they will form ionic bond. 8. (b) Because CsF is electrovalent compound. 37. (b) Na is highly electropositive while Cl is highly electronegative so they will form ionic bond. 9. (c) NaCl is formed by electrovalent bonding. 38. (a) Ionic compounds are good conductors of heat and electricity so 10. (d) Valency of metal is + 2 by formula MO so its phosphate would they are good electrolyte. 39. (a) Metal tends to lose electrons due to low ionization energy. be M3 (PO4 )2 because valency of [PO4 ] is – 3. 40. (c) As the formula of calcium pyrophosphate is Ca P O means 11. (b) Li, Na and K are alkali metals with low ionization energy and 2 2 7 one electron in their outermost shell so they will form cation valency of pyrophosphate radical is – 4 so formula of ferric
easily. pyrophosphate is Fe4 P2O7 3 . 12. (a) Melting point and boiling point of electrovalent compounds are 41. (c) M X bond is a strongest bond so between Na Cl is a high due to strong electrostatic force of attraction between the strongest bond. ions. 42. (b) The solubility order is :
13. (d) The value of lattice energy depends on the charges present on BeF2 MgF2 CaF2 SrF2 so SrF2 is least soluble. the two ions and distance between them. It shell be high if 43. (d) NaF has maximum melting point, melting point decreases of charges are high and ionic radii are small. sodium halide with increase in size of halide their bond energy 14. (a) Cs is more electropositive. get lower. 15. (a) X loses electron, Y gains it. 44. (b) Sulphanilic acids have bipolar structure so their melting point is high and insoluble in organic solvents. 16. (c) Formation of occurs by Na and Cl . ion ion 45. (c) CaCl2 will have electrovalent bonding because calcium is 17. (b) MgCl has electrovalent linkage because magnesium is electropositive metal while chlorine is electronegative so they 2 will combined with electrovalent bond. electropositive metal while chlorine is electronegative. 47. (a) Electrovalent bond is formed by losing electrons from one atom 18. (a) Electrovalent compounds generally have high m.pt and high and gaining electron by other atom i.e. redox reaction. b.pt due to stronger coulombic forces of attractions. 48. (b) Electrovalent compound are polar in nature because they are 19. (d) Water is a polar solvent so it decreases the interionic attraction formed by ions. in the crystal lattice due to solvation. 50. (b) CsCl has ionic bonding. 20. (c) Element C has electronic structure 1s2 , 2s2 2p 5 , it requires 51. (b) As soon as the electronegativity increases, ionic bond strength increases. only one electron to complete its octet and it will form anion 52. (b) This X element is a second group element so its chloride will so it will form electrovalent bond. be XCl2 . 21. (b) Since the chloride of a metal is MCl therefore metal ‘M’ 2 53. (a) When electronegativity difference is from 1.7 to 3.0. This bond must be divalent i.e. M 2 . As a result the formula of its is called as ionic bond. phosphate is . 54. (a) Ethyl chloride is an organic compound so it will be covalent. 55. (a) Lithium oxide and calcium fluoride show ionic characters. 22. (d) In MPO the oxidation state of M is +3. Hence, the formula 4 57. (a) Generally cation and anion form ionic bond. of nitrate is M(NO 3 )3 . 58. (c) Those atoms which contain +ve and –ve sign are known as ion. 23. (a) Ion is formed by gaining or losing electrons. To form cation 59. (a) Generally Br-F contain maximum electronegativity difference electron are lost from the valency shell, so Zn atoms to Zn compare to other compound. ions there is a decrease in the no. of valency electron. 61. (a) Due to greater electronegativity difference. 3d 4s
4s
31. (b) Valency of phosphorus in H 3 PO4 is supposed ‘x’ then 62. (b) Co 3 3d 6 4s0 , 3 x 8 0 , x 5 0 , x 5 . 33. (d) (1) x 3(2) 0 1 x 6 0 x 6 1 5 .
34. (a) HCl molecule has covalent bond. 4 6 0 Ni 3d 4s , 35. (d) Electrovalent compounds have high melting point and high boiling point. 64. (d) BaCl2 contain higher ionic character.
66. (a) Electrolytes are compound which get dissociated into their ion 36. (b) Middle length of H 2 74 pm in water so it contains electrovalent bond. 74 67. (abc) CaH ,BaH ,SrH are ionic hydride. Length of H 37pm 2 2 2 2
68. (bcd) Generally MgCl2 , SrCl2 , are ionic compounds so Middle length of Cl 2 198 pm they conduct electricity in fused state. 198 Length of Cl 99 pm Covalent bonding 2 Bond length of HCl = Length of H + Length of Cl 2. (c) In N 2 molecule each Nitrogen atom contribute 3e so total = 37 + 99 = 136 pm no. of electron’s are 6. 254 37. (d) Compound has 254 gm of I means 2 mole, while 3. (b) Non-metals readily form diatomic molecules by sharing of 2 127 electrons. Element M (1s2 2s2 2p5 ) has seven electrons in its 80 80 gm O means 5 mole so they will form compound valence shell and thus needs one more electron to complete its 2 16 octet. Therefore, two atoms share one electron each to form a I2O5 . diatomic molecule (M 2 ) 38. (c) NH 4 Cl has covalent as well as ionic bond...... : M . . M : : M : M : H . . . . | . . . . H N H Cl 5. (d) Covalent character depend on the size of cation and anion. | H 6. (a) In graphite all carbon atoms are sp2 -hybridised and have covalent bond. 39. (d) Covalent character increases when we come down a group so 7. (c) Silica has tendency to form long chain covalent structure such CaI2 will have highest covalent character. as carbon so it has giant covalent structure. 41. (b) In water molecule three atom are linked by covalent bond. 8. (a) All have linear structure. O Structure is O = C = O, Cl – Hg – Cl, HC CH H H 9. (d) Similar atoms form covalent bond. .. 42. (b) : N N O : or N N O. 10. (a) Covalent bond forms when electronegativity difference of two .. atom is equal to 1.7 or less than 1.7 44. (b) The electronic configuration of Na (Z 11)is 11. (b) Similar atoms form covalent bond. 2 2 6 1 12. (b) Water is a polar solvent while covalent compounds are non- 1s , 2s 2p , 3s . The oxide of Na is Na 2O . polar so they usually insoluble in water. 45. (b) Covalent bond is directional. 13. (c) BCl 3 is electron deficient compound because it has only ‘6’ 47. (d) Bond dissociation energy decreases with increase in size. So D electrons after forming bond. is smallest. 14. (b) Due to its small size and 2 electrons in s-orbital Be forms 48. (b) Molecule X is nitrogen because nitrogen molecule has triple covalent compound. bond. It’s configuration will be 1s2 , 2s2 2p 3 .
18. (c) H 2O will formed by covalent bonding. 49. (a) PCl5 does not follow octet rule, it has 10 electrons in its
21. (a) Two identical atoms are joined with covalent bond so H 2 will valence shell.
be covalent. 50. (a) The compound will be A2 B3 (By criss cross rule). 23. (c) Element ‘X’ has atomic no. 7 so its electronic configuration will 51. (b) Each nitrogen share 3 electrons to form triple bond. . 52. (d) Urea solution does not conduct electricity because it is a be 2, 5. So its electron dot symbol would be : X . . covalent compound. 24. (c) C-S will be most covalent. Covalent character depend on the 54. (d) Due to the small size and higher ionization energy, boron size of cation and anion. forms covalent compound. 25. (c) HCl has ionic character yet it has covalent compound because 58. (a) BF 3 contain 6 electron so it is lewis acid. electronegativity of chlorine is greater than that of hydrogen. 59. (d) Among the given species. The bond dissociation energy of 26. (c) Order of polarising power Be Li Na 2 C O bond is minimum in case of CO3 by which
Hence order of covalent character BeCl 2 LiCl NaCl . 2 C O bond become more weaker in CO3 or the bond
order of (1.33) is minimum so the bond become weaker.
60. (a) Valency of Na 2S 2O3 is supposed to be x, then 2 2x (6) 0 , 2x 4 0 , x 2 .
O O || || 61. (c) H O S O O S O H (Marshall acid) || || O O 62. (a) Among the given choice Al is least electropositive therefore, the bond between Al and Cl will be least ionic or most covalent or the difference in electronegativeity of two atom is less than 1.8. 2. (b) H 2SO4 has co-ordinate covalent bond.
32 2 2 6 2 4 O 63. (b) Electronic configuration of 16 S 1s ,2s ,2p ,3s ,3p . In the last orbit it has only 6 electron. So it require 2 electron to H O S O H complete its octet, therefore it share 2 electron with two O hydrogen atom and forms 2 covalent bond with it. 3. (c) NH has lone pair of electron while BF is electron 64. (b) The acidity of hydrides of VI group elements increase from top 3 3 deficient compound so they form a co-ordinate bond. to bottom as the bond strength decrease from top to X H NF BF bottom 3 3 4. (d) HNO2 does not have co-ordinate bond. Structure is H2O H2S H2Se H2Te H O N O . 65. (b) We know that Al3 cation is smaller than Na (because of 7. (a) Structure of N 2O5 is O N O N O . greater nuclear change) According to Fajan's rule, small cation O O polarise anion upto greater extent. Hence Al3 polarise Cl 2 ion upto greater extent, therefore has covalent bond 9. (a) SO3 has one coordinate bond. O S O AlCl3 between Al and Cl atoms. O 66. (b) Sulphur has the second highest catenation property after 10. (d) Co-ordinate bond is a special type of covalent bond which is formed by sharing of electrons between two atoms, where both carbon. Its molecule has eight atom bonded together (i.e. ) S 8 the electrons of the shared pair are contributed by one atom.
67. (b) H 2O2 has open book structure. Since this type of sharing of electrons exits in O3 , SO3 and O H 2SO4 . Therefore all these contains coordinate bond. H O 12. (a) CH 3 N C contain dative bond. H 13. (a) H PO is orthophosphoric acid. 3 4 69. (b) The electronic configuration of nitrogen is O N 1s2,2s2,2p3 7 H O P O H It has 5 electrons in valency shell, hence in ammonia molecule | it complete its octet by sharing of three electron with three H O | atom, therefore it has 8 electrons in its valence shell in H ammonia molecule 15. (c) Sulphuric acid contain, covalent and co-ordinate bond. . . . . H N H or H N H Dipole moment . | H H 1. (b) CO 2 is a symmetrical molecule so its dipole moment is 71. (c) Multiple bonds have more bond energy so C N will be the zero. strongest. 2. (d) These all have zero dipole moment. 72. (c) Diamond, silicon and quartz molecule bounded by covalent 3. (d) HF has largest dipole moment because electronegativity bond. difference of both is high so it is highly polar. 5. (c) Due to its symmetrical structure. 73. (cd) C2 H 4 and N 2 has multiple bonds. 6. (c) Chloroform has 3 chlorine atom and one hydrogen atom 74. (ad) CO has only 6 electrons while PCl5 has 10 electrons after attached to the carbon so it is polarised and it will show dipole sharing so both don’t follow octet rule. moment.
76. (a) Among these, NaH and CaH 2 are ionic hydrides and B2 H6 8. (a) The dipole moment of two dipoles inclined at an angle is 2 2 and NH 3 are covalent hydrides. given by the equation X Y 2XY cos cos90 0 . Since the angle increases from 90 180 , the Co-ordinate or Dative bonding value of cos becomes more and more – ve and hence resultant decreases. Thus, dipole moment is maximum when 1. (d) 90 . – F F
Cl Xe
O O F F O
F F 9. (c) Due to distorted tetrahedral geometry SF has permanent 1.03 4 100 16.83% 17% dipole moment F 6.12 F Polarisation and Fajan's rule : S F F 1. (d) is planar while NF3 is pyramidal due to the presence of 10. (b) has no net dipole moment because of its regular CCl 4 lone pair of electron on nitrogen in . tetrahedral structure. 2. (c) is a polar molecule due to electronegativity difference of 12. (d) H-F is polar due to difference of electronegativity of hydrogen H 2O and fluorine so it shows positive dipole moment. hydrogen and oxygen. 14. (c) BCl has zero dipole moment because of its trigonal planar 3. (b) When electronegativity difference is more between two joined 3 atoms then covalent bond becomes polar and electron pair geometry. forming a bond don’t remain in the centre.
16. (c) Dipole moment of CH 3OH is maximum in it. 4. (d) Hexane has symmetrical structure so does not have polarity. 5. (c) When two identical atoms form a bond, bond is non-polar. 20. (b) CH 4 have regular tetrahedron so its dipole moment is zero. 22. (b) Ammonia have some dipole moment. 6. (a) According to Fajan’s rule, polarisation of anion is influenced by charge and size of cation more is the charge on cation, more is 23. (b) Charge of e 1.6 1019 polarisation of anion. Dipole moment of HBr 1.6 1030 8. (a) When two atoms shares two electrons it is an example of covalent bond. This covalent bond may be polar or may be Inter atomic spacing 1Å 11010 m non-polar depends on the electronegativity difference. In given % of ionic character in example formula is AB. So it is polar. 9. (c) HCl is most polar due to high electronegativity of Cl. dipolemoment ofHBr 100 HBr 3 interspacingdistance q 10. (b) NH 3 has sp hybridised central atom so it is non planar. 1.6 1030 11. (d) p-dichloro benzene have highest melting point.
19 10 100 1.6 10 10 13. (b) NH 4Cl has both types of bonds polar and non polar 1030 1029 100 101 100 0.1100 10% H 25. (a) Carbon tetrachloride has a zero dipole moment because of its | regular tetrahedral structure. H N H Cl | 27. (b) BF3 has zero dipole moment. H 29. (c) Given ionic charge 4.8 1010 e.s.u. and ionic distance 14. (b) Greater the charge of cation more will be its polarising power (according to Fajan’s rule). 1A 108 cm we know that dipole moment = ionic charge 15. (d) AlI Aluminiumtriiodide shows covalent character. According × ionic distance 4.8 1010 108 3 to Fajan’s rule. 8 4.8 10 e.s.u. per cm 4.8 debye. 16. (d) As the size of anion increases, polarity character increases. 30. (a) Higher is the difference in electronegativity of two covalently 20. (d) Due to the electronegativity difference. bonded atoms, higher is the polarity. In HCl there is high difference in the electronegativity of H and Cl atom so it is a 21. (a) We know that greater the difference in electronegativity of two polar compound. atoms forming a covalent bond. More is its polar nature. In HF there is a much difference in the electronegatives of hydrogen 31. (a) Linear molecular has zero dipole moment CO 2 has linear and flourine. Therefore (HF) is a polar compound. structure so it does not have the dipole moment O C O . 22. (c) Silicon tetrafloride has a centre of symmetry.
32. (c) SF6 is symmetrical and hence non polar because its net dipole 23. (d) have zero dipole moment. moment is zero. 25. (b) According to Fajan’s rule largest cation and smallest anion form 33. (a) Polarity create due to the difference in electronegativity of both ionic bond. atom in a molecule except H 2 all other molecule have the 26. (b) Polarity character is due to the difference in electronegativity of different atom so they will have the polarity while will be two atoms or molecule. non polar. Overlaping- and - bonds 34. (bd) cis isomer shows dipole moment while that of trans is zero or very low value. Trans 1, 2 di-chloro-2-pentene will
also show dipole moment due to unsymmetry. 1. (c) 35. (a) % of ionic character H – C C – H Experiment al value of dipole moment = Expected value of dipole moment 2. (c) In fluorine molecule formation p-p orbitals take part in bond formation. 3. (b) -bond is formed by lateral overlapping of unhybridised p-p 1 5. (d) No. of e– pair 3 [3 3] =0 orbitals. 2 C F No. of e– pair 3 +0 120° 4. (b) Ca 1 and 2 F B 120° C
120° 5. (c) In a double bond connecting two atom sharing of 4 electrons F take place as in . H 2C CH 2 No. of atom bonded to the central atom 6. (c) C C is a multiple bond so it is strongest. In case of 3, 3 geometry is Trigonal planar. 9. (d) As the bond order increases, C H bond energy also 6. (a) In –hybridisation each hybridised orbital has 1/4 s- increases so it will be greatest in acetylene because its B.O. is 3. character. H H o | | 8. (b) In ethylene both Carbon atoms are - hybridised so 120 . 11. (b) H C C C C 3 | 9. (d) Structure of sp d hybridized compound is Trigonal H bipyramidal.
16. (a) O N N ||
10. (d) In H C C O H the asterisked carbon has a valency of 17. (d) We know that trisilylamine is sp2 –hybridized therefore * p d bonding is possible due to the availability of vacant 5 and hence this formula is not correct. d-orbitals with silicon. 11. (d) dsp3 hybrid orbitals have bond angles 120o ,90o . 18. (c) 13. (a) In BeF , Be is not –hybridised it is hybridised. 3
S 17. (c) In molecule OF2 oxygen is hybridised.
2, 2 bond and one lone pair. 18. (a) In hybrid orbitals s-character is 1/4th means 25%. . . . . : O : O 3 2 19. (d) XeF4 molecule has ‘Xe’ sp d hybridised and its shape is . . . . square planar. 19. (d) : O S O : 5 atoms has 12 electrons in its outermost 20. (b) The bond angle is maximum for sp hybridisation because two || O : sp hybridised orbitals lies at angle of 180o . . . 21. (c) C H Br has all single bonds so bond distance is shell. One (S O) bond will be (p-p) bond while two 2 4 2 the largest. bond will be (p-d) bond. 23. (a) In methane molecule C is hybridised so its shape will be 20. (d) Structure of P O is 4 10 tetrahedral. O 3 2 1 24. (c) In compound CH C CH the second carbon sp- P 2 2 hybridised. O O .. .. 25. (a) : Cl Cl : is the correct electronic formula of Cl molecule O .. .. 2 O P P O O because each chlorine has 7 electrons in its valence shell. 26. (a) has sp3d 2 hybridisation, its shape is square planar. O O P 27. (b) In HCHO, carbon is hybridized H O | Each phosphorus is attached to 4 oxygen atoms. H C O 2 sp Hybridisation 28. (c) Because of the triple bond, the carbon-carbon bond distance in ethyne is shortest. 3 1. (d) H 2O is not linear because oxygen is sp hybridised in 29. (b) The hybridisation of Ag in complex [Ag(NH 3 )2 ] will be sp H O . 2 because it is a Linear complex. 2. (d) O 30. (a) Structure of is linear O C O while that of 95.7 pm (104.5)o O H H is i.e. bent structure so in resultant dipole
H H
4. (c) CO 2 has sp – hybridization and is linear. moment is zero while that of has some value. 31. (d) is not hybridised, it is sp hybridised. 32. (a) As compare to pure atomic orbitals, hybrid orbitals have low 70. (a) As p-character increases the bond angle decreases. energy. 1 In - p-character , bond angle - 180o sp 2 sp sp 2 sp 3 2 33. (d) CH 2 C CH – CH 3 1, 2-butadiene. 2 3 In - p-character , bond angle - 36. (b) CCl 4 is sp hybridised so bond angle will be approximately 3 109o . 3 In - p-character , bond angle - 40. (b) Ethene has sp2 hybridised carbon so bond angles are 120o . 4 O 71. (a) -hybridization called tetrahedral because it provides tetrahedral shape to the molecule. 44. (a) Acetate ion is CH 3 C i.e. one C O single bond 3 2 O 72. (a) S-atom in SF6 has sp d hybridisation. So, the structure of and one C O double bond. will be octahedral.
46. (c) Benzene has all carbons hybridised and planar in shape. 74. (b) Structure of H 2O2 is non-planar. It has open book structure.
o 75. (d) Structure of is similar to both have linear 47. (d) In methane C is hybridized and bond angle is 109 . N 2O CO 2 structure. H H H | | | 78. (a) SnCl 2 is V–shaped. 56. (d) H C C C H | | | 79. (d) In NH nitrogen is hybridised so 4 hydrogen situated H H H 4 at the corners of a tetrahedron. There are 10 shared pairs of electrons. 81. (c) Increasing order of bond angle is sp3 sp2 sp . 58. (a) The diborane molecule has two types of B – H bond : 109 120 180
(i) B Ht – It is a normal covalent bond. 84. (a) NH 4 has –hybridized nitrogen so its shape is tetrahedral.
(ii) B Hb – It is a three centred bond. 86. (b) Bond angle increases with change in hybridisation in following 3 2 order sp sp sp . H t 88. (c) In Diborane boron shows –hybridization. B B 89. (a) Alkene does not show linear structure but it has planar
structure due to –hybridisation. Hb 61. (b) PF involves sp3d hybridization and hence has trigonal 5 90. (c) Generally SF4 consist of 10 electrons, 4 bonding electron pair bipyramidal structure. and one lone pair of electron, hence it shows 1 62. (c) s-character in sp 100 50% hybridization. 2 92. (c) Atom/Ion Hybridisation 1 sp s-character in sp2 100 33.3% NO 2 3 with one lone pair of electron 3 1 s-character in sp 100 25% 4 PF6
Hence, maximum s-character is found in sp-hybridisation. 93. (a) PF3 consist of three bonding pair electrons and one lone pair 3 3 63. (b) The molecule of PCl5 has sp d hybridisation, structure is of electron hence it shows sp – hybridization. trigonal bipyramidal. 94. (b) shows sp–hybridization. So its shape is linear. 64. (b) Merging (mixing) of dissimilar orbitals of different energies to form new orbitals is known as hybridisation and the new 95. (c) Generally octahedral compound show – hybridization. orbital formed are known as hybrid oribitals. They have similar energy. 96. (a) In fifth group hydride bond angle decreases from top to bottom 65. (b) In SO sulphur is sp2 hybridized so its shape will be 3 NH PH AsH SbH BiH . trigonal planar. 3 3 3 3 3 66. (a) These all are triangular with hybridization. 97. (b) Generally NH 4 shows hybridization. 67. (c) Bond length depends upon bond order and in benzene all 98. (b) We know that single, double and triple bond lengths of carbon C C bonds have same bond order. in carbon dioxide are 1.22Å,1.15 Å and 1.10Å respectively.
68. (b) In each carbon has -hybridization 2 C2 H 2 sp 99. (b) It shows sp –hybridization so it is planar. H C C H sp sp 101. (a) Bond angle of hydrides decreases down the group. 3 2 125. (b) There is sp hybridization in C H so it has the linear 102. (b) Hybridization of N in NH 3 is sp that of Pt in [PtCl4 ] 2 2 structure. is dsp2 that P in PCl is sp3d and that of B in BCl is 5 3 126. (c) In octahedral molecule six hybrid orbitals directed towards the sp2 . corner of a regular octahedron with a bond angle of 90°.
103. (d) NH and SO 2 both show –hybridization and 4 4 X tetrahedral structure. X X 3 3 104. (a) It is shows sp d –hybridization. Hence the bond angle is M
about 72o . according to thisX geometry, the numberX of X M X bond 107. (a) s-character increases with increase in bond angle. at 180° must be three. X Hybridization s% Angle 127. (d) sp3d 2 hybrid orbital have octahedral shape sp 50 180o 128. (c) In the formation of d 2sp3 hybrid orbitals two (n 1)d orbitals 33.3 120o of e.g., set [i.e., (n 1)dz2 and (n 1)dx 2 y 2 orbitals] one 25 109.28o ns and three np [ npx ,npy and npz ] orbitals combine 3 1 20 o sp d 90 and together and form six hybrid orbitals.
108. (b) IF7 molecule show –hybridization. 129. (c) The correct order of bond angle (Smallest first) is H S NH SiH BF 110. (a) PCl3 contain three bonding and one lone pair electron. Hence 2 3 4 3 shows –hybridization. 92.6 107 10928' 120 H N 111. (a) Ammonia and (BF )1 shows –hybridization. 4 H 107° H 92.6° 112. (b) For square planar geometry hybridization is involving S H H
s, p , p and d 2 orbital. x y x y2 H F 113. (b) All carbon atoms of benzene consist of alternate single and 109° 28' double bond and show hybridization. 120° Si B H H 116. (c) molecule show –hybridization and planar F F structure. H 130. (a) 117. (c) Boron trichloride molecule show –hybridization and trigonal 2– F – planar structure. NC CN 2 F 118. (b) SO2 molecule shows sp –hybridization and bent structure. Ni B F 119. (c) Due to multiple bonding in N 2 molecule. NC CN F 120. (a) % of s-character in
100 100 Square planar Regular tetrahedral , , CH 4 25 C2 H 4 33 3 4 2 3 (sp ) (sp ) F F F F 100 C2 H 2 50 (sp ) 2 S F Xe
121. (a) Acidic character increases when we come down a group, so HI F F is the strongest acid. F
122. (c) SO has sp2 hybridization have the V shape structure See saw shaped Square planar 2 131. (b)
( 120) due to 2 lone pair of electron over S atom. CO 2 H
·· ·· O and N 2O have the sp hybridization.
123. (a) In H2CO3 and BF3 central atom are in hybridization
but in due to the ionic character of O H bond it B H ·· sp2 ·· H will be polar (High electronegativity of oxygen). O O 3 sp3 ·· ·· sp 3 124. (a) Due to sp hybridization and presence of lone pair of electron
on p atom PCl3 are of pyramidal shape like that of NH 3 . 132. (b) In the formation of BF3 molecule, one s and 2p orbital hybridise. Therefore it is sp2 hybridization. 2 5 133. (e) In NCl 3 and H2S the central atom of both (N and S) are in I [Xe] 5s ,5p hence 5p 5d sp3 hybridization state 5s I in ground state
·· ···· N S 5s 5p 5d
107° 92.5° I in excited state Cl H H Cl Cl 2 while in BF3 and central atoms are in sp and and I F7 in excited hybridization respectively. In and BeCl central state 2 F F F I F F F 3 2 3 2 atom are in sp and sp hybridization In BF3 , NCl 3 & IF shows sp d hybridization. So, its3 3structure is pentagonal 7 sp d bipyramidal. H 2 S central atom are in , & hybridization 141. (a) Compound containing highly electronegative element (F, O, N) and in the central atom are in and sp hybridization. attached to an electropositive element (H) show hydrogen bonding. Fluorine (F) is highly electronegative and has smaller 134. (c) C 2s2,2p 1p 1 ; C 2s1,2p 1p 1p 1 ground state x y excited state x y z size. So hydrogen fluoride shows the strongest hydrogen 2 2 1 1 bonding in the liquid phase. Oground state 2s ,2px py pz 3 In the formation of CO 2 molecule, hybridization of orbitals of 142. (b) In the ammonia molecule N atom is sp hybridized but due carbon occur only to a limited extent involving only one s and one to the presence of one lone pair of e (i.e. due to greater p orbitals there is thus sp hybridisation of valence shell orbitals of the carbon atom resulting in the formation of two sp hybrid Lp bp repulsion) it has distorted tetrahedral (or pyramidal) orbitals. geometry. Oxygen atom in ground state sp – p N bonded p – p Carbon atom in H H H excited state 143. (a) 2 2 0 4 Be 1s ,2s ,2p sp – p p – p
bonded Be in ground state Oxygen atom in 1s 2s 2p ground state 3 135. (d) In NH 3 , N undergoes sp hybridization. Due to the presence Be in excited state of one lone pair, it is pyramidal in shape.
BeCl2 136. (b) NO 2 SF4 PF6 sp sp3d sp3d 2 Cl Cl 137. (b) The configuration of B 1s 2 ,2s 2 2p1 5 sp hybridisation B in ground state (Linear diagonal hybridization) 144. (a) Except CO3 other choice CO2,CS 2 and BeCl2 have 1s 2s 2p sp hybridization and shows the linear structure while B in excited state have sp3 hybridization and show the non linear 1s 2s 2p structure because generate tetrahedral structure.
In BCl3 state 145. (a) dsp3 or sp3d hybridization exhibit trigonal bipyramidal 1s 2s 2p geometry e.g., PCl 5 Cl Cl Cl sp2hybridisation Cl Cl
138. (d) In SO molecule, S atom remains sp2 hybrid, hence it has 3 sp3d2 (Trigonal bipyramidal) trigonal planar structure O Cl P
Cl S Cl
O O 146. (b) Carbon has only two unpaired electrons by its configuration 3 139. (a) In PCl3 molecule, phosphorous is sp hybridised but due but hybridization is a concept by which we can explain its to presence of lone pair of electron, it has pyramidal structure valency 4.
147. (c) Hybridization is due to overlapping of orbitals of same energy
content. P 140. (a) The electronic configuration of Cl Cl Cl 2 2 3 3 148. (d) MX3 show the sp hybridization in which 3sp hybridized 9. (b) XeF6 is distorted Octahedral. It has sp d hybridisation orbital of M bonded by 3X from bond and having the with lone pair of electron on Xe, so its shape is distorted. 10. (a) zero dipole moment. 5s 5p 5d 11. (c) Xe ground state
149. (bcd) SnCl 2 has V–shaped geometry. Xe double excitation 5s 5p 5d 150. (a) NF is predominantly covalent in nature and has pyramidal 3 structure (the central atom is sp3 hybridised) with a lone pair 5s 5p 5d of electrons in the fourth orbital. XeF4
151. (ac) PCl , NH Pyramidal. 3 2 3 3 sp d - hybridization
o CH 4 , CCl 4 Tetrahedral. 12. (a) has bond angle 180 . 13. (a) As the s-character of hybridized orbitals decreases the bond 152. (a) dsp3 or sp3d : one s three p one d(d ). z2 angle also decreases In hybridisation: s-character 1/4, bond angle 109o Resonance o In hybridisation: s-character 1/3, bond angle 120
1. (d) Choice (a), (b), (c) are the resonance structures of CO 2 . In sp hybridisation: s-character 1/2, bond angle
2. (b) In NH 3 nitrogen has one lone pair of electron. 14. (a) XeF2 molecule is Linear because Xe is sp hybridised. 2 2 5. (b) In CN ion formal negative charge is on nitrogen atom due 15. (c) SO4 has 42 electrons; CO 3 has 32 electrons; NO 3 has to lone pair of electrons. 32 electrons. 16. (c) Molecular oxygen contains unpaired electron so it is O H | paramagnetic (according to MOT). 7. (a) has 9 , 1 and 2 lone pairs. CH 3 C CH 2 17. (b) Structure of H 2O is a bent structure due to repulsion of lone 8. (c) In resonance structure there should be the same number of pair of oxygen. electron pairs. 18. (d) Bond angle between two hybrid orbitals is 105o it means 9. (b) There are three resonance structure of CO 2 ion. 3 orbitals are hybridised but to lone pair repulsion bond O O O angle get changed from to 105o . So its % of s- C C C character is between 22-23%. – O O O O O O 22. (d) Number of electrons in ClO2 = 7 + 6 + 6 + 1 = 20 (I) (II) (III) Number of electrons in ClF + = 7+7+7 – 1=20. 11. (abcd) It has all the characteristics. 2 23. (b) Central atom having four electron pairs will be of tetrahedral shape. VSEPR Theory F . .
F F F F 2. (a) The bond angle in PH3 would be expected to be close to 24. (d) S C Xe o o . . 90 . (The bond angle H P H in PH3 is 93 ) F F F F F 2 F F . . 3. (b) In BF3 molecule Boron is sp hybridised so its all atoms are co-planar. 26. (c) It shows –hybridization and show trigonal planar structure. 4. (c) Due to lp lp repulsions, bond angle in H 2O is lower o o o o 28. (b) H S show bond angle nearly . (104 .5 ) than that in NH 3 (107 ) and CH 4 (109 28). 2
BeF2 on the other hand, has sp-hybridization and hence has a 31. (a) Bond angle of hydrides is decreases top to bottom in the group. o bond angle of 180 . NH 3 PH3 AsH3 SbH 3 32. (c) 5. (c) Compound is carbontetrachloride because CCl 4 has – hybridization 4 orbitals giving regular tetrahedron geometry. In N Three bond pair and one lone pair of electron. others the geometry is little distorted inspite of hybridization due to different atoms on the vertices of H H H tetrahedron. 2 33. (c) Unpaired electrons are present in KO2 while others have 6. (b) SO4 ion is tetrahedral since hybridization of S is . paired electron 7. (b) NH molecule has one lone pair of electrons on the central 3 atom i.e. Nitrogen. NO 2 = 22 electrons ; BaO2 = 72 electrons
8. (c) C2 H 2 has linear structure because carbons are sp-hybridised AlO2 30 electrons ; KO 2 35 electrons o and lies at 180 . 34. (a) Bond angle decreases from to H 2Te . 35. (c) BF does not contain lone pair of electron. 3 Molecular orbital theory 36. (b) Bent T-shaped geometry in which F both lone pairs occupy the . . No. of bonding e No. of antibonding e equatorial position of the trigonal 2. (c) B.O. bipyramidal here 2
Br F 8 3 5 (lp lp ) repulsion = 0 2.5 . 2 2 . . repulsion = 4 and (lp bp ) 3. (b) One bonding M.O. and one anti-bonding M.O. F repulsion =2 2 (bp bp ) 4. (b) O is least stable. 37. (b) The overall value of the dipole moment of a polar molecule 2 depends on its geometry and shape i.e., vectorial addition of 5. (c) B.O. of O is 2, B.O. of O 1 is 1.5, B.O. of O 1 is 2.5 and of dipole moment of the constituent bonds water has angular 2 2 2 structure with bond angle 105° as it has dipole moment. is 1. However BeF is a linear molecule since dipole moment 2 6. (d) Hydride of boron does not exist in BH3 form. It is stable as its summation of all the bonds present in the molecule cancel each dimer di borane . other. (B2 H6 ) 10. (c) O2 (2 8 1 17) has odd number of electrons and hence it is paramagnetic. All the remaining molecules/ions, i.e., O F Be F CN (6 7 1 14) diamagnetic
38. (d) BClH3 , BBr3 andH BF3 , all of these have same structure i.e. NO(7 8 15) has odd number of electrons and hence it is paramagnetic. trigonal planar ( sp2 hybridization) Hence bond angle is same No. of N No. of N 5 for all of them (i.e., equal to 120°) 11. (c) B.O. b a 2.5 . 2 2 39. (d) We know that molecule of (NH 3) has maximum repulsion due to lone pair of electron. Its shape is pyramidal and is 12. (b) Bond order of O2 is highest so its bond length is smallest. sp3 hybridization. 13. (c) Oxygen is paramagnetic due to the presence of two unpaired 40. (b) : O : . . electron : N 2 2 2 2 H 105° H O2 (1s) (1s) (2s) (2s) H H 107° 2 2 2 1 1 (2p x ) (2py ) (2p x ) (2py ) (2pz ) . .H . . As 17. (d) In CH CN bond order between C and N is 3 so its bond P 3 H H H H length is minimum. 18. (b) H H Less than 107° As the electronegativity of central atom decreases bond angle is He2 H 2 H 2 H 2 decreases (1s) NH has largest bond angle. * 3 (1s) 3 41. (c) In NH 3 ,sp -hybridization is present but bond angle is 1 1 1 B.O. 1 106o 45 because Nitrogen has lone pair of electron according 2 2 2 Magnetic to VSEPR theory due to bp-lp repulsion bond angle decreases P D P P from 109o 45' to 106o 45 . nature 42. (a) Bond strength decreases as the size of the halogen (P = Paramagnetic, D = Diamagnetic) increases from F to I. 19. (c) Due to unpaired e ClO2 is paramagnetic. 43. (b) NH has pyramidal structure, yet nitrogen is sp3 hybridised. 3 20. (c) The Bond order in molecule is 3, N N Here, This is due to the presence of lone pair of electron. N 2 3 Nb 2 4 2 8 and N a 2 44. (c) SiF4 has symmetrical tetrahedral shape which is due to sp hybridization of the central sulphur atom in its excited state B.O. (8 2)/ 2 3. configuration. has distorted tetrahedral or Sea- Saw SF4 1 21. (d) H has the bond order , it has only one electron so it will geometry which arise due to sp3d hybridization of central 2 2 sulphur atom and due to the presence of lone pair of electron be paramagnetic. in one of the equatorial hybrid orbital. 22. (c) When bond forms between two atom then their energy get 45. (d) lower than that of separate atoms because bond formation is an exothermic process. 23. (b) Valency of A is 3 while that of B is 2 so according to Criss O O O Cross rule the formula of the compound between these two
will be A2 B3 . dsp2 hybridization sp3d hybridization sp3d2 hybridization 24. (c) Due to resonance bond order of C C bonds in benzene is (Four 90° angles (Six 90° angle (Twelve 90° angle between 1 and 2. between bond pair between bond pair between bond pair
and bond pair) and bond pair) and bond pair) 25. (a) Nitrogen does not have vacant ‘d’-orbitals so it can’t have +5 55. (a) H 2O2 contain bond angle between two O H planes about oxidation state i.e. the reason PCl exists but NCl does 5 5 90o . not. 56. (c) Nitrogen molecule has highest bond energy due to presence of 26. (d) Molecules having unpaired electrons show paramagnetism. triple bond. 27. (b) NO 2 has unpaired electrons so it would be paramagnetic. 2 9 0 57. (c) Cu [Ar18 ]3d 4s it has one unpaired electron so it is 30. (c) Helium molecule does not exist as bond order of He2 0 . paramagnetic. 31. (c) Structure of P4 O10 is 59. (a) CN 14 electrons ; CO =14 electrons O 1 6 B.O. = [10 4] 3 . P 2 2 1 5 O O 60. (a) B.O. = [10 5] 2.5 , paramagnetic 2 2 O P O P P O O 61. (a) P P P O O 64. (c) The paramagnetic property in oxygen came through unpaired P electron which can be explained by molecular orbital theory.
Each phosphorus is attached to 4 oxygen atoms. O Antibonding N N 8 4 b a 33. (c) B.O. of carbon 2 . 2px* 2 2 N N 10 4 34. (a) B.O. b a 3 . 2 2
N N 8 3 5 2pz* 2py* 37. (b) B.O. b a 2.5 . 2 2 2
38. (a) Electronic configuration of O2 is 2 2 2 2 2 2 Px Py Pz Px Py Pz O2 (1s) (1s) (2s) (2s) (2px ) (2py )
2 1 1 (2pz ) (2py ) (2pz ) The molecule has two unpaired electrons So, it is paramagnetic
* 40. (c) 2p y has two nodal planes. So 2 unpaired of electron present in * * . 42. (a) Element with atomic number 26 is Fe. It is a ferromagnetic. 2py and 2pz 43. (b) Correct Sequence of bond order is Total number of bonds between atoms 2Px bonding 2 65. (a) Bond order O2 O2 O2 Total number of resonating structure B.O – 2.5 2 1.5 5 44. (a) Due to small bond length. 1.25 4 45. (a) S 2 have all paired electrons so it is diamagnetic. 66. (c) We know that carbonate ion has following resonating 46. (c) NO has 15 electrons. structures – – 47. (b) In the conversion of O2 into O2 bond order decreases. O O O – 2 C=O C – O– C – O 49. (c) O2 does not have any unpaired electron so it is diamagnetic. – – O O O 50. (a) consist of four antibonding electron pair [1s and 2s have two antibonding and have two antibonding electron Total number of bonds between atoms 2px 2py Bond order pair]. Total number of resonating structure 51. (c) The electron’s distribution in molecular orbitals is 2 1 1 1 2 4 1s , 2s 1.33 . 2 1 1 3 3 B.O. 0.5 . * 2 * 2 2 2 2 67. (a) O2 (15e ) K : K ( 2s) ( 2s) ( 2p x ) 52. (b) ClO has all paired electrons hence it does not show 2 2 * 1 * 0 2 ( 2py ) ( 2pz ) ( 2py ) ( 2pz ) paramagnetism. 1 1 Hence, bond order (10 5) 2.5 53. (a) B.O. [ N b N a ] 2 2 * 2 * 2 2 1 6 1 6 N 2 (13e ) KK ( 2s) ( 2s) ( 2p x ) N [10 4] 3 ; O 2 [10 4] 3. 2 2 2 2 2 2 2 1 ( 2py ) ( 2pz ) 1 1 5 54. (a) B.O. for N = [N N ]= [9 4] 2.5 . 1 2 2 b a 2 2 Hence, bond order (9 4) 2.5 . 2
68. (a) Electronic configuration of O2 is 2 * 2 2 * 2 * 2 2 So only exist unpaired electron and show the O2 (1s) ( 1s) ( 2s) ( 2s) ( 2s) ( 2pz ) 2 2 * 1 * 1 paramagnetism. ( 2p x 2py ) ( 2p x 2py ) 2p 2 * 2p 1 1 1 y y Hence bond order N N [10 6] 2 . 76. (b) O 1s2 , *1s2 , 2s2 , * 2s2 , 2p 2 2 b a 2 2 x 2p 2 * 2p 2 69. (c) Nitrogen form triple bond N N z z In which 6 electron take part. So two unpaired electron found in O2 at ground stage by 70. (a) As bond order increase bond length decrease the bond order of which it shows paramagnetism. species are 77. (b) Due to greater electron affinity Cl2 has the highest bond number of bonding electron - Number of a.b. electron energy. 2 78. (a) Molecular orbital electronic configuration of these species are : 10 6 For O 2 ; O(17e ) 1s 2 *1s 2 , 2s 2 * 2s 2 , 2p 2 , 2p 2 , 2 2 2 x y 10 5 2p 2, * 2p 2 * 2p 1 O 2.5 z y z 2 2 O (16e) 10 7 2 O 1.5 2 2 * 1 * 1 2 2pz 2py 2pz So, bond order O2 O2 O2 and bond length are 2 2 * 2 2 * 2 2 2 O2 (18e) 1s 1s , 2s 2s , 2px , 2py , . 2 * 2 * 2 2 * 1 2pz 2py 2pz 2p y 2p y Hence number of antibonding electrons are 7,6,and 8 71. (b) : 2 * 2 2 * 2 2 O2 1s , 1s , 2s , 2s , 2p x respectively. 2 * 1 2p z 2p z 79. (c) Species with unpaired electrons is paramagnetic O2 has 2 10 6 Bond order 2.0 unpaired electrons, O has one unpaired, O 2 has zero 2 2 2 2 (Two unpaired electrons in antibonding molecular unpaired electrons, O2 has one unpaired. orbital) 2 * 1 80. (a) O has 2 unpaired electron while O and O has one each 2 * 2 2 * 2 2 2py 2py 2 2 2 O :1s , 1s , 2s , 2s , 2p 2 x 2pz 2 * 2pz0 2 unpaired electrons while O2 does not have any unpaired 10 5 electron. Bond order 2.5 2 81. (c) H O O H , O O O , O O (One unpaired electron in antibonding molecular orbital so it is paramagnetic) O 72. (b) Higher the bond order, shorter will be the bond length, thus O O NO having the higher bond order that is 3 as compared to Due to resonance in O O O bond length will be in b/w NO having bond order 2 so NO has shorter bond length. 3 and O O . 73. (d) Oxygen molecule boron molecule and ion, all (O2 ) (B2 ) N 2 of them have unpaired electron, hence they all are 82. (a) From valency bond theory, bond order in CO, i.e. : C O : is paramagnetic. 2 3, that of O C O is 2 while that of CO 3 ion is 1.33. 74. (c) Bond order of NO , NO and NO are 3, 2.5 and 2 Since the bond length increases as the bond order decreases, respectively, bond energy bond order 2 i.e. CO CO2 CO3 . 75. (a) Paramagnetic property arise through unpaired electron. B 2 2 2 2 2 2 molecule have the unpaired electron so it show paramagnetism. 83. (c) N2 : KK(2s) *(2s) (2px ) (2py ) (2pz ) 2 * 2 2 * 2 1 1 (diamagnetic) B2 1s 1s , 2s 2s , 2px 2py (2 unpaired electron) 2 2 2 2 C2 : KK(2s) *(2s) (2px ) (2py ) (diamagnetic) 2 * 2 2 * 2 2 2 2 2 2 2 2 C2 1s 1s , 2s 2s , 2px . 2py N2 : KK(2s) *(2s) (2px ) (2py ) (2pz ) (No unpaired electron) (paramagnetic) 2 * 2 2 * 2 2 2 2 N 2 1s 1s , 2s 2s , 2px , 2py 2pz 2 2 2 2 2 2 (No unpaired electron) O2 : KK(2s) *(2s) (2pz ) (2px ) (2py ) 2 * 2 2 * 2 2 2 2 *(2p )2 *(2p )2 (diamagnetic) F2 s , 1s , 2s , 2s , 2px , 2py , 2pz , x y (No unpaired electron) 84. (d) NH 3 107, PH3 93, H2O 104.5 * 2 * 2 2py , 2pz H2Se 91, H2S 92.5
Hydrogen bonding 47. (d) C2 H5 OH will dissolve in water because it forms hydrogen bond with water molecule. 1. (d) Hydrogen bonding will be maximum in F-H bond due to 48. (b) In ice cube all molecules are held by inter molecular hydrogen greater electronegativity difference. bond. 2. (b) Ice has hydrogen bonding. 49. (d) Hydrogen bonding is developed due to inter atomic attraction 3. (b) H – F has highest boiling point because it has hydrogen so it is the weakest. bonding.
6. (d) CO 2 is sp-hybridised Types of bonding and Forces in solid
7. (b) sp-hybridization gives two orbitals at 180o with Linear 1. (b) In electrovalent crystal has cation and anion are attached by structure. electrostatic forces. 8. (d) Hydrogen bonding increases the boiling point of compound. 2. (d) Mercury has very weak interatomic forces so it remains in 9. (c) o-Nitrophenol has intramolecular hydrogen bonding but p- liquid state. Nitrophenol has intermolecular hydrogen bonding so boiling 3. (c) The melting and boiling points of argon is low hence, in solid point of p-Nitrophenol is more than o-Nitrophenol. argon atoms are held together by weak Vander Waal’s forces. 10. (c) The strongest hydrogen bond is in hydrogen fluoride because 4. (c) NaF is the strongest ionic crystal so its melting point would be the power of hydrogen bond electronegativity of atom and highest. 1 9. (b) Diamond is the hardest substance it’s melting point would be electronegativity atomic size highest. 10. (c) Bond is formed by attractive and repulsive forces of both the So fluorine has maximum electronegativity and minimum atoms. atomic size. 12. (a) Generally zero group elements are linked by the Vander Waal’s 11. (d) H 2O can form hydrogen bonds rest CH 4 and CHCl 3 are force. Hence these show weakest intermolecular forces. organic compound having no oxygen while NaCl has itself 13. (d) Glycerol has a three OH group hence it is viscous in nature. intraionic attraction in the molecule. 14. (c) Vander waal's forces is the weakest force of attraction.
12. (b) PH3 has the lowest boiling point because it does not form 16. (b) NH 4 contain all three types of bond in its structure Hydrogen bond. 14. (b) Hydrogen bonding increases heat of vaporisation. H | 15. (d) Only forms H-bonds. NH 3 H N H | 22. (a) Water molecule has hydrogen bonding so molecules get H dissociated so it is liquid. 23. (d) In case of water, five water molecules are attached together 17. (d) In NaOH covalent bond is present in O H bond while through four hydrogen bonding. ionic bond is formed between OH and Na . 25. (c) Hydrogen bond is strongest in hydrogen fluoride. 18. (a) Bond formation is an exothermic reaction so there is decrease in energy of product. 28. (c) Boiling point of H 2O is more than that of H 2 S because 22. (d) Blue vitriol is CuSO 4 . 5H 2O and it has all types of bonds. H 2O forms hydrogen bonding while does not. H | 30. (c) Interamolecular H-bonding. O H 23. (a) H N H Cl | C O H 31. (a) HydrogenH bond is formed when hydrogen is attached with the atom which is highly electronegative and having small radius. Ionic bond = 1, Covalent bond = 3 34. (a) Water is dense than ice because of hydrogen bonding Co-ordinate bond = 1.
interaction and structure of ice. 35. (a) Ethanol have hydrogen bonding so its boiling point is higher Critical Thinking Questions
than its isomer dimethyl ether. 1. (d) We know that ionic characters 36. (a) A compound having maximum electronegative element will 2 form strong Hydrogen bond. 16[EA EB] 3.5 [EA EB]
37. (a) Due to electronegativity difference of N 2 and H 2 , or ionic characters = 72.24%
form hydrogen bond. 3. (c) Configuration of O2 molecule is 38. (b) Intermolecular hydrogen bonding compound contain more b.p. 2 2 2 2 2 2 compare to intramolecular hydrogen bonding compound. [(1s) (1s) (2s) *(2s) (2p x ) (2py ) 39. (d) Water molecule contain hydrogen bonding. (2p )2 (2p )1 (2p )1 ] 40. (c) It contain intermolecular hydrogen bonding. z x y 41. (b) Ethyl alcohol has a intermolecular hydrogen bond. No. of pair are 7 so total no. of paired electrons are 14. 43. (b) HCl contain weak covalent bond. 45. (c) Due to intermolecular hydrogen bonding water molecules come 6. (a) H O : H H O H close to each other and exist in liquid state. | | 46. (b) Due to greater resonance stabilization. H H 7. (b) The correct order of increasing dipole moment is p-dichlorobenzene < Toluene < m-dichlorobenzene < o- 27. (c) CuSO 4 .5H 2O has electrovalent, covalent and coordinate dichlorobenzene. bonds. 8. (a) The dipole moment of CH 0D, 4 O NF3 0.2D, NH 3 1.47D and H 2O 1.85D . 2 Cu O S O.5H 2 O . Therefore the correct order of the dipole moment is O CH 4 NF3 NH 3 H2O . 10. (d) Ammonia molecule is more basic than nitrogen trifluoride and Boron trifluoride because ammonia molecule easily gives lone Assertion & Reason
pair of electron. 1. (a) Solubility in water depends on hydration energy and lattice 3 11. (a) Chlorine atom in ClO2 is sp hybridised but its shape is energy. angular. 2. (a) Polarity in covalent bond developed due to shifting of electrons towards one of the bonded atoms. 12. (c) [ NF3 and H 3 O ] are pyramidal while [ NO 3 and BF3 ] 3 are planar. Hence answer (c) is correct. 5. (c) SiF4 have sp hybridization & shape of regular tetrahedral where the bond angle of 13. (d) CH 2 CH CH 2 CH 2 C CH F 3 sp 2 sp F S F are found hybridised 109.5 o which is 109.5o 14. (d) B.O. in CO i.e., : C O : is 3, that of O C O is 2 while greater than 90o but 2 o S that of CO 3 ion is 1.33. Since the bond length increases as less than 180 . Repulsion sequence are F the bond order decreases i.e. CO CO CO 2 . Thus 2 3 Lp Lp Lp Bp Bp Bp F option (d) is correct. F so assertion are true 15. (b) Dichromate dianion has following structure but the reason are false. 2 O O 9. (c) N 2 molecule is diamagnetic. The diamagnetic character is due O Cr O Cr O to the presence of paired electron molecule does not O O contain any unpaired electron. Thus, assertion is coorect but the reason is false. 6, Cr O bonds are equivalent. 10. (a) It is correct that during formation of Ice from water there are 17. (b) ClF is a [AB ] type of molecule because it consist of three vacant spaces between hydrogen bonded molecules of Ice. Ice 3 3 has a cage like structure. Due to this reason Ice is less dense bonding pair and two lone pair of electrons hence this than liquid water. hence both assertion & reason are true & compound shows sp3 d hybridization. reason are the correct explanation of assertion. 11. (b) Water is liquid while H S is gas because oxygen is of small 20. (a) BeF does not show –hybridization because this 2 3 size & more electronegative in comparision to sulphur. Hence compound is not formed. water molecules exist as associated molecules to form liquid 21. (a) K3 [Fe(CN )6 ] state due to hydrogen bonding does not have hydrogen 2 6 bonding & can’t associated hence it is gas. Fe26 4s 3d 12. (d) Iodine is more soluble in CCl 4 than in H 2O because iodine Fe3 3d 5 4s0 is non polar & thus it dissolve in because like dissolves
like. = 13. (a) o & p -nitrophenols can be separated by steam distillation because -nitrophenol is steam volatile. Here, both assertion & reason are correct & reason is correct explanation of assertion. 14. (e) Fluorine is highly reactive F F bond has low bond 2 3 Unpaired electron d sp –hybridization dissociation energy. Here assertion is false but reason is true. 22. (d) N 2 has one unpaired electron so it would be paramagnetic. 15. (c) It is true that sigma () bond is stronger than pi () bond but 23. (a) Each of the species has 14 electron so isoelectronic and shows the reason that there is free rotation of atoms is false. bond order 3. 16. (c) Energy is released in the formation of the crystal lattice. It is qualitative measure of the stability of an ionic compound so 1 1 6 B.O. [N N ] [10 4] 3 . assertion is true & reason are false. 2 b a 2 2 17. (c) Li, Na & K are alkali metals & not alkaline earth metal so, 24. (d) O O O size of alkali metal increases So. Assertion is true & reason are false. S S 18. (b) Hess’s law states that the enthalpy of a reaction is the same, O O O whether it takes place in a single step or in more than one O S O step. In born haber cycle the formation of an cycle ionic compound may occur either by direct combination of the O Trimer of SO3 . element or by a stepwise process involving vaporization of elements, conversion of the gaseous atoms into ions & the combination of the gaseous ions to form the ionic solid. 19. (a) With increase in bond order, bond length decreases & hence bond energy increases so both assertion & reason are true & reason are the correct explanation of assertion. 20. (c) Electron affinity is experimentally measurable while electronegativity is a relative number so assertion is true but reason are false. 21. (b) Assertion & reason both are correct but reason is not the correct explanation of assertion sulphur has five electrons pairs whose arrangement should be trigonal bipyramidal according to VSEPR theory. Two structure are possible F .. F | F F S F : S F | F F (a) (b) Lone pair in the axial Lone pair in the equatorial position (three l.p – b.p position (two L.p – b.p repulsion at 90o) repulsion)
22. (e) BF3 has zero dipole moment because of its structure. F F B 0 F
H 2 S has two lone pairs on sulphur atom & hence. It has irregular shape. Thus it possess dipole moment. So assertion is false but reason are true. 23. (d) Both assertion & reason are false because pairs of electron will have different spins. Electrons are equally shared between them.
24. (d) In B2, total number of electrons = 10
B (1s)2 *(1s2) (2s)2 *(2s)2 (2p)1 (2p)1 2 x y Presence of unpaired electron shows the paramagnetic nature. The highest occupied molecular orbital is of -type. 25. (a) Both assertion & reason are true & reason is the correct explanation of the assertion because. At any given instant, at room temperature each water molecules forms hydrogen bonds
with other water molecules. The H 2O molecules are in continuous motion. So hydrogen bonds are constantly & rapidly broken & formed. In Ice molecules are however fixed in the space lattice. 26. (a) Both assertion & reason are true & reason is the correct explanation of assertion, because helium molecule is formed by linking two helium atoms. both have 1s orbitals. These will combine to form two molecular orbitals ( ) & * ( ) four available electrons are accommodated as (1s)2 & *(1s)2 .
1. Nature of the bond formed between two elements depends on the (c) H O (d) NH (a) Oxidation potential (b) Electronegativity 3 4 (c) Ionization potential (d) Electron affinity 12. The dipole moment of chlorobenzene is 1.73 D. The dipole moment of p -dichlorobenzene is expected to be 2. Two elements X and Y have following electronic configurations [CPMT 1991] 2 2 6 2 6 2 X 1s , 2s 2p , 3s 3p , 4s and (a) 3.46 D (b) 0.00 D Y 1s 2 , 2s 2 2p 6 , 3s 2 3p 5 . The expected compound formed by (c) 1.73 D (d) 1.00 D 13. Polarization of electrons in acrolein may be written as combination of and is [BHU 1990] [IIT 1988] (a) XY (b) X Y 2 5 2 (a) C H 2 CH C H O (b) C H 2 CH CH O (c) X 2 Y5 (d) XY5 3. Electricity do not pass through ionic compounds (c) C H C H CH O (d) C H CH CH O (a) In solution (b) In solid state 2 2 (c) In melted state (d) None of these 14. The order of dipole moments of the following molecules is [Roorkee 2000] 4. From the following which compound on heating readily sublimes (a) CHCl 3 CH 2Cl 2 CH 3 Cl CCl 4 (a) NaCl (b) MgCl2 (b) CH 2Cl 2 CH 3Cl CHCl 3 CCl 4 (c) BaCl2 (d) AlCl3 (c) CH Cl CH Cl CHCl CCl 5. Which one in the following contains ionic as well as covalent bond [IIT 1979; CPMT 1983; DPMT3 1983] 2 2 3 4 (d) CH 2Cl 2 CHCl 3 CH 3 Cl CCl 4 (a) CH 4 (b) H 2 (c) KCN (d) KCl 15. The electronegativity of C, H, O, N and S are 2.5, 2.1, 3.5, 3.0 6. The solution of sugar in water contains and 2.5 respectively. Which of the following bond is most polar [EAMCET 1986] [NCERT 1972; MP PET 2000] (a) O H (b) S H (a) Free atoms (c) N H (d) C H (b) Free molecules 16. Which of the following bond has the most polar character (c) Free ions [DPMT 1982; CBSE PMT 1992; CPMT 1999] (d) Free atoms and free molecules (a) C O (b) C Br 7. In which of the following reactions, there is no change in the valency (c) C S (d) C F [NCERT 1974; CPMT 1971, 78] 17. The geometry of H 2 S and its dipole moment are [IIT 1999] (a) 4KClO 3KClO KCl 3 4 (a) Angular and non-zero (b) Angular and zero (b) SO2 2H 2S 2H 2O 3S (c) Linear and non-zero (d) Linear and zero 18. How many and bonds are there in the molecule of (c) BaO2 H 2 SO4 BaSO4 H 2O2 tetracyanoethylene (d) 2BaO O 2BaO 2 2 N C C N C C 8. The octet rule is not followed in [BHU 1981] N C C N (a) (b) F2 NaF [NCERT 1980; MP PMT 1986, 95;Orissa JEE 1997]
(c) CaF2 (d) BF3 (a) Nine and nine (b) Five and nine 9. Sodium chloride is an ionic compound whereas hydrogen chloride is (c) Nine and seven (d) Five and eight a gas because [KCET 2002] 19. The shape of H O ion is [EAMCET 1993; CPMT 2001] (a) Sodium is reactive 3 (b) Covalent bond is weaker than ionic bond (a) Linear (b) Angular
(c) Hydrogen chloride is a gas (c) Trigonal planar (d) Triangular pyramidal (d) Covalent bond is stronger than ionic bond 20. The hybridization in sulphur dioxide is[IIT 1986; DPMT 1990] 10. Which one of the following molecules has a coordinate bond (a) sp[CPMT 1988, 94] (b) sp3 (a) NH Cl (b) AlCl 4 3 (c) sp2 (d) dsp2 (c) (d) Cl 2 21. The number and type of bonds between two carbon atoms in 11. Co-ordinate bond is absent in [RPMT 2002] CaC2 are [IIT 1996] (a) BH (b) CO 2 4 3 (a) One sigma () and one pi () bonds (a) 3 (b) 2 (b) One sigma () and two pi () bonds (c) 1 (d) 1/2 (c) One sigma and one and a half pi bonds 28. In the process, 2 the electron lost is from (d) One sigma bond O2 O2 e [Orissa JEE 2002] 22. Which of the following resonating structures of N 2 O is the most (a) Bonding -orbital (b) Antibonding -orbital contributing [Roorkee Qualifying 1998] (c) orbital (d) orbital (a) N N O (b) N N O 2p z 2p x (c) N N O (d) N N O 29. The maximum number of hydrogen bonds formed by a water molecule in ice is 23. The hybridization of atomic orbitals of nitrogen in NO 2 , NO 3 , [MP PET 1993; AFMC 2002;UPSEAT 1999, 2001, 02] (a) 4 (b) 3 and NH 4 are [IIT Screening 2000] (c) 2 (d) 1 (a) sp, sp3 and sp2 respectively 30. Hydrogen bonding is not present in (b) sp, sp2 and sp3 respectively [AIIMS 1998; MP PET/PMT 1998] (a) Glycerine 2 (c) sp , sp and respectively (b) Water (d) sp2 , sp3 and sp respectively (c) Hydrogen sulphide (d) Hydrogen fluoride 24. The molecule having one unpaired electron is [IIT 1985; MP PMT 1989] 31. The bonds in K4 [Fe(CN )6 ] are [EAMCET 1991] (a) NO (b) CO (a) All ionic (b) All covalent (c) CN (d) O 2 (c) Ionic and covalent 25. The geometry of ClO , according to valence shell electron pair 3 (d) Ionic, covalent and coordinate covalent repulsion (VSEPR) theory will be 32. In which of the following ionic, covalent and coordinate bonds are [KCET 1996; MP PET 1997] present [UPSEAT 2002] (a) Planar triangle (b) Pyramidal (a) Water (c) Tetrahedral (d) Square planar (b) Ammonia 26. Which of the following halogens has the highest bond energy [CPMT 1988] (c) Sodium cyanide (a) (b) F2 Cl 2 (d) Potassium bromide
(c) Br2 (d) I2
2 27. What bond order does O2 have [Pb. PMT 2001]
(SET -3) 1. (b) If the two elements have similar electronegativities,the bond 3. (b) Ionic compounds can’t pass electricity in solid state because between them will be covalent, while a large difference in they don’t have mobile ion in solid state. electronegativities leads to an ionic bond. 4. (d) AlCl sublimes readily on heating. 2. (a) From electronic configuration valencies of X and Y are + 2 and 3 . . –1 respectively so formula of compound is XY2 . 5. (c) Structure of KCN is [K (C N)]. 6. (b) Sugar is an organic compound which is covalently bonded so in 27. (c) O 2 have bond order one water it remains as free molecules. 2 1 2 2 6 2 6 B.O. [10 8] 1 . 7. (c) In the reaction BaO2 H 2SO4 BaSO4 H 2O valency 2 2 is not changing. 28. (b) Electron lost from antibonding orbital. 8. (d) BF does not have octet, it has only six electrons so it is 29. (a) In ice each water molecule forms four hydrogen bond through 3 which each water molecule is tetrahedrally attached with other electron deficient compound. water molecule. 9. (b) NaCl is a ionic compound because it consists of more elelctronegativity difference compare to HCl. H O 10. (a) NH 4 Cl has a coordinate bond besides covalent and ionic H H H H | O O bonds H N H Cl | H H H H H O O O H | H H H 11. (b) O C O has covalent bonds only. 12. (b) Due to symmetry dipole moment of p-dichloro benzene is zero. O O
13. (d) H H H H 14. (d) CCl 4 has zero dipole moment because of symmetric O O tetrahedral structure. CH 3Cl has slightly higher dipole 30. (c) Hydrogen bondingH is present in moleculesH which have F, O, or N atoms. moment which is equal to 1.86D. Now CH 3Cl has less 31. (d) Structure of K4 [Fe(CN )6 ] is electronegativity then CH 2Cl2 . But CH 2Cl2 has greater 4 dipole moment than CHCl . 3 C N 15. (a) More the difference in electronegativity of atoms. Bond C N between them will be more polar. C N 4 K Fe 16. (d) C F bond has the most polar character due to difference of their electronegativity. C N C N C N 17. (a) H S has angular geometry and have some value of dipole 2 moment. 32. (c) Sodium cyanide contain ionic, covalent and coordinate bond. N C C N 18. (a) C C N C C N 9 and 9 bonds. 3 19. (d) H 3O has sp hybridization and its shape is triangular pyramidal due to lone pair on oxygen. 2 20. (c) SO2 molecule has sp hybridisation. C *** 21. (b) In Ca two carbons are joined with 1 and 2 bonds. C
22. (a) In N 2O molecule N N O structure is most contributed. 23. (b) The shape of NO 2 , NO 3 and NH 4 are linear trigonal planar and tetrahedral respectively. Thus the hybridization of atomic orbitals of nitrogen in these species are sp, sp2 and respectively. 24. (a) NO has one unpaired electron with Nitrogen. .. : N ::O : . .. . . 25. (b) O Cl O | O
26. (b) Bond energy of Cl2 is highest among all halogen molecule.
Bond energies of F2, Cl2, Br2, I2 are 37, 58, 46 and 36 Kcal mol 1 respectively.