Review Sheet 1St Semester Honors Chemistry

REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY UNIT 1 INTRODUCTORY (A) 454 g 1. An example of a chemical change is (B) 1000 L (A) freezing of water. (C) 1 mg (B) burning a match. (D) 1 in3 (C) boiling carbon tetrachloride. 3 (D) dissolving alcohol in water. (E) 1 cm (E) stretching a rubber band. 10. 10.0 mL of a pure liquid substance has a mass of 25.0 2. Which involves a chemical change? g. What is the mass of 3.00 L of the substance? (A) powdering sugar (A) 83 g (B) condensing steam (B) 120 g (C) magnetizing an iron bar (C) 1,200 g (D) separating cream from milk (D) 7,500 g (E) exposing photographic film to light (E) 25,000 g

–6 3. Which process is a chemical change? 11. The metric prefix for 10 is (A) the melting of ice (A) mega– (B) the burning of a candle (B) kilo– (C) the magnetizing of steel (C) micro– (D) the liquefaction of oxygen (D) milli–

4. The graph was obtained by plotting the volume of a UNIT 2 MOLES material vs. the mass of that same material. 12. Which expression represents the number of atoms in 1.0 10–3 g of lead?

(B) What is the density of the material? (A) 1.5 g·cm (C) (B) 2.0 g·cm (C) 0.67 g·cm (D) (D) 0.50 g·cm (E) 5. Which is a unit for expressing volume? (A) mm 13. How many atoms are in one mole of hydrogen sulfide, H S? (B) g 2 (C) cm 23 (D) g·cm (A) 34 6.02 10 (B) 3 6.02 1023 6. The number 149,000,000 is usually written in (C) 3 scientific notation as (D) 34 (A) 0.149 109 6 (B) 149 x 10 14. A substance whose density is 4.00 g·cm–3 occupies a (C) 1.49 x 108 3 volume of 12.0 cm . What is its mass? (D) 1490 x 105 (A) 0.333 g (B) 8.00 g 7. Which measurement is the most uncertain? (C) 48.0 g (A) 1.00 ± 0.01 cm (D) 4.00 g (B) 2.00 ± 0.05 L (C) 10 ± 1 g 15. How many moles of oxygen atoms are present in one (D) 200 ± 1 mL mole of beryllium sulfate tetrahydrate, BeSO ·4H O? 4 2 8. Which unit represents l 10–3 mol? (A) eight (A) decimole (B) five (B) kilomole (C) four (C) millimole (D) two (D) micromole

9. The volume of one milliliter most nearly equals REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY 16. Which statement best accounts for the fact that gases 20. According to the Avogadro Principle, one liter of can be greatly compressed? gaseous hydrogen and one liter of gaseous ammonia (A) Molecules occupy space. contain the same number of (B) The collisions of molecules are elastic. (C) Molecules of gases are in constant motion. (A) atoms at standard conditions. (D) The molecules of a given gas are identical. (B) molecules at all conditions. (E) Molecules of gases are relatively far from each other. (C) molecules only at standard conditions. (D) atoms if conditions in both containers are the 17. Gases may be most easily liquefied by same. (E) molecules if conditions in both containers are the (A) raising the temperature and lowering the pressure. same. (B) raising the pressure and lowering the temperature. (C) lowering both the temperature and pressure. (D) raising both the temperature and pressure. 21. Which is STP? (E) lowering the temperature and keeping the presure unchanged. (A) 0 °C and 76 mmHg (B) 0 K and 76 mmHg 18. If the temperature and pressure are the same, one (C) 0 K and 760 mmHg gram of hydrogen has about the same number of atoms as

Atomic Molar Masses H 1.0 g·mol–1 O 16.0 g·mol–1 (A) 1 g of oxygen. . (B) 2 g of oxygen. .

(D) 100 °C and 76 cmHg

(E) 273 K and 760 mmHg

22. A student collects one liter samples of O , CO , and 2 2 CH at laboratory conditions. What quantity is the 4 same for all three samples? (C) 8 g of oxygen. (A) number of atoms divided by the number of molecules in each sample (D) 16 g of oxygen (B) number of molecules in each sample (E) 32 g of oxygen (C) number of atoms in each sample (D) mass of each sample 19. One liter of oxygen at STP contains approximately the same number of molecules as 23. Each of three identical containers holds a mole of (A) 2 L of He at STP. gas, all at the same temperature. 1/ (B) 3 L of O at STP. 3 (C) l L of CO at STP 2 1/ CH O SO (D) 5 L of CH at STP. 4 2 2 4 (E) (D) (E) 250 mL of NH at STP. 3 REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY (A) 1.5 1023 Which gas exerts the greatest pressure? Assume ideal 23 behavior. (B) 3.0 10 (C) 6.0 1023 (A) CH 23 4 (D) 2.4 10 (B) O 2 (C) SO 29. What is the mass of one mole of calcium nitrate, 2 Ca(NO ) ? (D) They all exert the the same pressure. 3 2

24. A weather balloon contains 12 L of hydrogen at 740 Atomic Molar Masses mmHg pressure. At what pressure in mmHg will the Ca 40. g·mol–1 volume become 20 L (temperature constant)? –1 N 14. g·mol –1 (A) 370 O 16. g·mol (B) 444 (C) 760 (A) 82 g (D) 1230 (B) 102 g (E) 1480 (C) 164 g (D) 204 g

30. The number of moles of water in 1,000 g of water is 25. A gas occupies a volume of 2.0 cubic feet at 13 atm. How many cubic feet does this gas occupy at 1.0 atm, Atomic Molar Masses temperature constant? –1 H 1.0 g·mol –1 (A) 6.5 O 16.0 g·mol (B) 13 (C) 15 (A) 18.0 (D) 26 (B) 55.5 (C) 180.0 (D) 1000.0 (E) 18,000.0 26. A sample of gas at 1.00 atm of pressure occupies a volume of 500 L. If the volume is decreased to 125 L 31. The molar mass of magnesium acetate, and the temperature is held constant, what is the new Mg(C H O ) , in g·mol–1 is pressure in atmospheres? 2 3 2 2

(A) 0.250 Atomic Molar Masses (B) 2.00 C 12. g·mol–1 (C) 1.25 –1 H 1. g·mol (D) 4.00 Mg 24. g·mol–1 27. For a given amount of dry gas at constant O 16. g·mol–1 temperature, when the pressure is doubled the volume is (A) 15 (B) 16 (A) halved. (C) 83 (B) unchanged. (D) 142 (C) doubled. (E) 166 (D) increased, but not doubled. 32. How many mole(s) of calcium carbonate, CaCO , is 28. Approximately how many molecules are in 11 g of 3 carbon dioxide, CO , gas? represented by 50 g of the compound? 2 Atomic Molar Masses Atomic Molar Masses –1 –1 Ca 40.1 g·mol C 12.0 g·mol –1 –1 C 12.0 g·mol O 16.0 g·mol –1 O 16.0 g·mol REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY (A) 1.0 –1 N 14.0 g·mol (B) 2.0 –1 (C) 0.20 O 16.0 g·mol (D) 4.0 (E) 0.50 (A) 6.02 g (B) 18.0 g 33. The molar mass of aluminum sulfate, Al (SO ) , is (C) 23.0 g 2 4 3 (D) 46.0 g

Atomic Molar Masses 23 –1 37. Calculate the mass of 12.0 10 molecules of Al 27 g·mol chlorine gas, Cl . 2 O 16 g·mol–1 –1 S 32 g·mol Atomic Molar Mass Cl 35.5 g·mol–1 (A) 150 g·mol–1 (B) 170 g·mol–1 (A) 35.5 g (C) 278 g·mol–1 (B) 71.0 g (C) 142 g (D) 342 g·mol–1 (D) 284 g (E) 450 g·mol–1 38. The correct formula for iron(III) sulfate is 34. The mass of one mole of ammonium carbonate, (NH ) CO , is approximately 4 2 3 (A) FeSO (D) Fe (SO ) 4 2 4 3 (B) Fe(SO ) (E) Fe (SO ) Atomic Molar Masses 4 2 3 4 2 (C) Fe SO C 12.0 g·mol–1 2 4 H 1.0 g·mol–1 39. The one correct formula among these is N 14.0 g·mol–1 –1 O 16.0 g·mol (A) Na OH (D) Zn(NO ) 2 3 3 (B) Cu(SO ) (E) BaNO (A) 43.0 g 4 2 3 (C) ZnCl (B) 72.0 g 2 (C) 78.0 g (D) 95.0 g 40. Which formula is incorrect?

35. The number of molecules present in 22.0 g of carbon (A) BaHCO (B) Ca(OH) (C) Al O (D) K SO dioxide at STP is 3 2 2 3 2 4

(E) ZnCO Atomic Molar Masses 3 C 12.0 g·mol–1 41. Which formula is incorrect? O 16.0 g·mol–1 (A) Al (SO ) (D) NH HSO 12 2 4 3 4 4 (A) 2.01 10 (B) BaHCO (E) LiH (B) 6.03 1012 3 (C) Ca(OH) (C) 2.06 1022 2 (D) 3.01 1023 42. What is the formula for aluminum sulfate? (E) 6.02 1023 (A) AlSO 4 36. What mass of nitrogen dioxide, NO , has the same 2 (B) Al SO 2 4 number of molecules as 18.0 g of water, H O? 2 (C) Al SO 3 4 (D) Al (SO ) Atomic Molar Masses 3 4 2 (E) Al (SO ) H 1.0 g·mol–1 2 4 3 REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY 43. What is the formula for chromium(III) oxide? (B) iron(III) sulfate (D) iron(II) sulfate(III)

(A) CrO (B) Cr O (C) Cr O (D) Cr O 53. What is the correct name for Fe(NO ) ? 2 3 2 3 3 2 (A) iron(II) nitrate (C) iron(III) nitrate (B) iron(II) nitrite (D) iron(III) nitrite 44. What is the formula for strontium sulfide? 54. The formula for hydrogen bromate is HBrO , and the (A) SrS (B) Sr S (C) SrS (D) SrS 3 2 2 3 formula for dysprosium oxide is Dy O . What is the 2 3 45. What is the formula for copper(II) hydroxide? formula for dysprosium bromate?

(A) CuOH (B) Cu(OH) (C) Cu OH (D) CuOH (A) Dy BrO (C) Dy(BrO ) 2 2 2 2 3 3 3 (B) Dy BrO (D) Dy (BrO ) 3 3 2 3 3 46. Which is the formula for ammonium nitrate? 55. The formula for ytterbium sulfate is Yb (SO ) . (A) NH N (B) NH N (C) NH NO 2 4 3 3 4 4 2 What is the formula for ytterbium chloride? (D) NH NO 4 3 (A) YbCl (B) Yb Cl (C) Yb Cl (D) YbCl 2 2 3 2 2 3 47. What is the formula for sodium carbonate? 56. In which pair of anions do both names end in ‘–ate’? (A) NaHCO (C) So CO 3 2 3 (B) NaCO (D) Na CO (A) Cl–, ClO – (C) NO –, NO – 3 2 3 3 2 3 (B) ClO –, NO – (D) HS–, HSO – 48. What is the formula for chromium(III) sulfate? 3 3 4

(A) Cr (SO ) (C) Cr (SO ) 57. Barium perrhenate has this formula: Ba(ReO ) . The 2 4 3 2 3 3 4 2 (B) Cr (SO ) (D) Cr SO perrhenate ion is 3 4 2 3 4

(A) ReO – (B) ReO 2– (C) ReO 3– (D) ReO 4– 49. Which formula is followed by its correct name? 4 4 4 4

(A) FeCl , iron(III) chloride 3 58. What is the total number of oxygen atoms represented by the formula KAl(SO ) ·12H O? (B) FeS, iron(II) sulfite 4 2 2 (C) Mg N , magnesium nitrite 3 2 (A) 9 (D) KNO , potassium nitrate (B) 16 2 (C) 20 (E) HClO, hydrochloric oxide (D) 48 (E) 96 50. The compound not properly named is 59. Which is the number of atoms of hydrogen in one (A) Fe O , iron(III) oxide. 2 3 molecule of glycerine, C H (OH) ? 3 5 3 (B) Pb O , lead(III) tetraoxide. 3 4 (C) CuCl , copper(II) chloride. (A) 14 (B) 8 (C) 6 (D) 5 2 (D) Pb (PO ) , lead(III) phosphate. 3 4 2 60. The total number of atoms represented by the (E) P S , diphosphorus pentasulfide. formula K Fe(CN) is 2 5 3 6

51. What is the name of the compound having the (A) 4 formula CaH ? 2 (B) 10 (C) 11 (A) calcium amide (C) calcium hydrate (D) 16 (B) calcium hydride (D) calcium hydroxide (E) 36 61. The total number of atoms represented by 52. What is the name of the compound Fe (SO ) ? 5Al(C H O ) is 2 4 3 2 3 2 3

(A) iron(II) sulfate (C) iron(II) trisulfate (A) 22 REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY (B) 60 ? Sb + ? Cl ? SbCl 2 3 (C) 71 (D) 84 is correctly balanced, the sum of the coefficients is (E) 110 (A) 2 (B) 3 (C) 6 (D) 7 62. The number of atoms of oxygen indicated by the formula Ca (PO ) is 3 4 2 (E) 9

(A) 12 70. Which expression is correctly balanced? (B) 8 (C) 7 (A) Na O + 2H O 2NaOH + O 2 2 2 2 (D) 4 (B) 2Na O + 2H O 4NaOH + 2O (E) 3 2 2 2 2 (C) 4Na O + 3H O 4NaOH + 2O 2 2 2 2 63. How many atoms are in one molecule of acetone, (D) 2Na O + 2H O 4NaOH + O CH COCH ? 2 2 2 2 3 3 (E) 3Na O + 2H O 6NaOH + O 2 2 2 2 (A) 1 (B) 6 (C) 3 (D) 10 71. Which set of coefficients balances this equation? 64. Using only these formulas, ? CH (g) ? C H (g) + ? H (g) 4 3 8 2 XY X Z QZ 2 2 (A) 3, 1, 1 (B) 3, 2, 1 (C) 3, 1, 2 (D) 6, 2, 2

what formula would you expect for a compound of (E) 6, 2, 6 elements Q and Y? 72. Consider the unbalanced expression: (A) QY (B) QY (C) Q Y (D) QY 2 2 4 ? CH CH CHO(l) + ? O (g) ? CO (g) + ? H O(g) 3 2 2 2 2 65. Which set consists only of compounds? Which set of coefficients balances the equation? (A) Na, Ca, He (C) NaCl, CH , Br 4 2 (B) H O+, Cl–, I – (D) H S, CuCl , KI (A) 2, 8, 3, 6 (D) 1, 8, 3, 3 3 3 2 2 (B) 3, 8, 6, 6 (E) 1, 4, 3, 3 (C) 1, 4, 3, 2 66. Which substance contains only one kind of atom? 73. Consider the unbalanced expression: (A) water (C) aluminum (B) ethanol (D) carbon dioxide – + ? Cu(s) + ? NO (aq) + ? H (aq) 3 BALANCE EQUATIONS (REG, IONIC, NET IONIC 2+ ? Cu (aq) + ? NO(g) + ? H O(l) 2 67. Which property is always conserved during a chemical reaction? Which set of coefficients correctly balances the equation?

(A) mass (B) volume (C) pressure (D) solubility (A) 4, 5, 3, 8, 2, 3 (D) 3, l, 8, 7, 4, 2 (B) 2, 4, 3, 8, 3, 3 (E) 3, 2, 8, 3, 2, 4 68. The equation (C) 3, 2, 8, 7, 2, 4

Cu + 4HNO Cu(NO ) + 2H O + ? 74. The expression for pentane, C H , burning in 3 3 2 2 5 12 oxygen is would be completed and balanced by using ? C H (g) + ? O (g) ? CO (g) + ? H O(g) 5 12 2 2 2 (A) NO (B) 2NO (C) 3NO (D) 4NO 2 2 2 2 What set of coefficients balances the equation? (E) 2NO (A) 1, 8, 5, 6 (C) 1, 8, 5, 12 69. When the equation (B) 2, 8, 10, 6 (D) 1, 11, 5, 12 REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY 75. Which set of coefficients correctly balances the equation?

+ 3+ ? Al(s) + ? H (aq) ? Al (aq) + ? H (g) 2

(A) 1, 2, 1, 2 (C) 3, 2, 3, 2 (B) 2, 6, 2, 3 (D) 2, 3, 2, 3 81. The overall equation for the reaction between KCl and AgNO is 3 76. Which equation represents the complete combustion + – + – of acetylene in an excess of air? K (aq) + Cl (aq) + Ag (aq) + NO (aq) + – 3 K (aq) + NO (aq) + AgCl(s) (A) C H + 2O 2CO + H 3 2 2 2 2 2 (B) C H + O 2CO + H What is the net ionic equation? 2 2 2 2 (C) C H + O 2C + H O + – 2 2 2 (A) Ag (aq) + Cl (aq) AgCl(s) + – (D) C H + O 2C + H O (B) K (aq) + Cl (aq) KCl(s) 2 2 2 2 2 + – (C) K (aq) + NO (aq) KNO (s) (E) 2C H + 5O 4CO + 2H O + –3 + 3 – 2 2 2 2 2 (D) K (aq) + Cl (aq) + Ag (aq) + NO (aq) 3 + + – – Ag (aq) + K (aq) + Cl (aq) + NO (aq) 77. Dysprosium oxide, Dy O , reacts with hydrochloric 3 2 3 acid to produce only water and a salt. The salt is 82. Complete the equation for the reaction between solutions of lead nitrate, Pb(NO ) , and ammonium (A) Dy Cl (B) DyCl (C) DyCl (D) DyCl 3 2 2 3 2 3 6 sulfide, (NH ) S. 4 2 78. Which equation represents the dissolving of sodium 2+ – + 2– sulfate, Na SO , in water? Pb (aq) + 2NO (aq) + 2NH (aq) + S (aq) 2 4 3 4

2+ 2– 2+ 2– (A) Na SO (s) Na (aq) + SO (aq) (A) 2NH NO (s) + Pb (aq) + S (aq) 2 4 4 4 3 + 2– + 2– (B) Na SO (s) 2Na (aq) + SO (aq) (B) Pb(NO ) (s) + 2 NH (aq) + S (aq) 2 4 4 3 2 4 2+ 2– 2– 2+ – (C) Na SO (s) Na (aq) + S (aq) + 4O (aq) (C) (NH ) S(s) + Pb (aq) + 2NO (aq) 2 4 2 4 2 3 2+ 2– 2– + – (D) Na SO (s) 2Na (aq) + S (aq) + O (aq) (D) PbS(s) + 2NH (aq) + 2NO (aq) 2 4 4 3

83. Which is the balanced net ionic equation for the 79. What is the net ionic equation for the reaction formation of the precipitate silver chromate, between solutions of sodium chloride, NaCl, and Ag CrO ? silver nitrate, AgNO ? 2 4 3 + 2– + – 1/ 3/ (A) 2Ag (aq) + CrO (aq) Ag CrO (s) (A) Na (aq) + NO (aq) Na(s) + 2N (g) + 2O (g) 4 2 4 3 2 2 + 2– + – 1/ (B) Ag (aq) + CrO (aq) Ag CrO (s) (B) Ag (aq) + Cl (aq) Ag(s) + 2Cl (g) 4 2 4 2 0 2– + – + – (C) Ag (aq) + CrO (aq) Ag CrO (s) (C) Ag (aq) + Cl (aq) Ag (aq) + Cl (aq) 4 2 4 + – + 2– (D) Ag (aq) + Cl (aq) AgCl(s) (D) Ag CrO (s) 2Ag (aq) + CrO (aq) 2 4 4 80. Which equation represents the dissolving (dissociation) of aluminum sulfate, Al (SO ) , in 84. Which two ions do not participate in the reaction 2 4 3 between solutions of silver nitrate, AgNO , and water? 3 potassium chloride, KCl? 3+ 6+ 2– (A) Al (SO ) (s) 2Al (aq) + 3S (aq) + 4O (aq) 2 4 3 (A) K+ and Ag+ (C) K+ and Cl– 3+ 2– (B) Al (SO ) (s) 2Al (aq) + 3SO (aq) (B) K+ and NO – (D) Ag+ and Cl– 2 4 3 4 3 2+ 3– (C) Al (SO ) (s) 2Al (aq) + 3SO (aq) 2 4 3 4 85. In the equation: 3+ 3– (D) Al (SO ) (s) Al (aq) + SO (aq) 2 4 3 4 BaCl (aq) + Na SO (aq) BaSO (s) +2NaCl (aq) 2 2 4 4 REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY 90. What volume is occupied by 2.00 g of a substance What is the net ionic equation for this reaction? having a density of 5.00 g·cm–3?

– + (A) Cl (aq) + Na (aq) NaCl (aq) (A) 0.400 cm3 (C) 7.00 cm3 2– 2+ (B) Cl (aq) + Na (aq) 2NaCl (aq) 3 3 2 2 (B) 2.50 cm (D) 10.0 cm 2+ 2– (C) Ba (aq) + SO (aq) BaSO (s) 4 4 91. If 50 mL of a 200 mL sample of 0.10 M sodium (D) BaCl (s) + Na SO (s) 2 2 4 chloride solution is spilled, what is the concentration 2+ – + 2– Ba (aq) + 2Cl (aq) + 2Na (aq) + SO (aq) of the remaining solution? 4 (A) 0.20 M (B) 0.10 M (C) 0.075 M (D) 0.025 M

86. Which is the net ionic equation for the reaction of lead(II) nitrate and sodium chromate?

2+ 2– (A) Pb (aq) + CrO (aq) PbCrO (s) 4 4 92. In the reaction (B) Pb(NO ) (aq) + Na CrO (aq) 3 2 2 4 PbCrO (s) + 2NaNO (aq) 4Al + 3O 2Al O 4 3 2 2 3 + 2– (C) 2Na (aq) + CrO (aq) Na CrO (aq) 4 2 4 how many moles of aluminum oxide, Al O , are 2+ – + 2– 2 3 (D) Pb (aq) + NO (aq) + Na (aq) + CrO (aq) 3 4 produced from one mole of aluminum, Al? + – PbCrO (s) + Na (aq) + NO (aq) 4 3 (A) 0.5 (B) 2 (C) 3 (D) 4 87. What is the net ionic equation for the reaction between lead(II) nitrate and potassium sulfide? 93. Given the equation

2+ 2– N + 3H 2NH (A) Pb (aq) + S (aq) PbS(s) 2 2 3 + – (B) K (aq) + NO (aq) KNO (aq) 3 3 Theoretically, the number of moles of ammonia produced (C) Pb(NO ) (aq) + K S(aq) PbS(s) + 2KNO (aq) from 2 mol of nitrogen is 3 2 2 3 2+ – + 2– (D) Pb (aq) + 2NO (aq) + 2K (aq) + S (aq) (A) 1 (B) 2 (C) 3 (D) 4 3 + – PbS(s) + 2K (aq) + 2NO (aq) 3 (E) 5

STOICHIOMETRY W/LIMITING REACTANTS 94. In an experiment, 0.0041 mol of maleic acid, C H O , reacted with 0.0082 mol of sodium 88. 50.0 g of water is heated from 22.0 °C to 36.0 °C. 4 4 4 How much heat is absorbed? hydroxide, NaOH. Which equation describes the reaction? Specific Heat Capacity for Water (A) C H O + NaOH NaC H O + H O 4.18 J·°C–1·g–1 4 4 4 4' 3 4 2 (B) C H O + 2NaOH Na C H O + 2H O 4 4 4 2 4 2 4 2 (A) 1510 J (B) 2930 J (C) 4520 J (D) 4600 J (C) C H O + 3NaOH Na C HO + 3H O 4 4 4 3 4 4 2 (D) C H O + 4NaOH Na C O + 4H O (E) 7520 J 4 4 4 4 4 4 2

89. How much heat is required to raise the temperature of 95. In neutralizing 0.015 mol of H PO , 0.030 mol of 3 3 25.0 g of iron from 10.0 °C to 40.0 °C? NaOH was consumed. Which equation describes this reaction? Specific Heat Capacity of Iron 0.444 J·g–1·°C–1 (A) H PO + NaOH NaPO + H O 3 3 3 2 (B) H PO + NaOH NaH PO + H O (A) 750 J (B) 444 J (C) 333 J (D) 313 J 3 3 2 3 2 (C) H PO + 3NaOH NaPO + 3H O 3 3 3 2 REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY (D) H PO + 2NaOH Na HPO + 2H O 100.The volume of pure oxygen needed to burn 3 3 2 3 2 completely 800 mL of acetylene (C H ) gas is 2 2 96. Silica, SiO , reacts with hydrofluoric acid, HF, 2 according to this equation (A) 800 mL (D) 10000 mL (B) 1600 mL (E) 20000 mL SiO + 4HF 2H O + SiF (C) 2000 mL 2 2 4 101.A mixture of 2.0 g of hydrogen and 32 g of oxygen is Which reagent is completely consumed when 2 mol of exploded and produces water. What mass of gas SiO is added to 6 mol of HF? 2 remains uncombined?

(A) SiF (B) H O (C) HF (D) SiO Atomic Molar Masses 4 2 2 H 1.0 g·mol–1 O 16.0 g·mol–1

(A) 1.0 g of hydrogen (D) 16 g of oxygen (B) 1.0 g of oxygen (E) 24 g of oxygen (C) 8.0 g of oxygen

97. How many grams of calcium carbonate, CaCO , 3 102.The equation for the complete combustion of butane gas, C H , is would be needed to produce 44.8 L of carbon dioxide 4 10 gas, CO , measured at STP? 2 2C H + 13O 8CO + 10H O 4 10 2 2 2 Atomic Molar Masses Ca 40.1 g·mol–1 How many liters of carbon dioxide is produced when a –1 mixture of 1.00 L of butane gas and 13.0 L of oxygen is C 12.0 g·mol burned? (measured under the same conditions) O 16.0 g·mol–1 (A) 1.00 L (B) l. 63 L (C) 8.00 L (D) 4.00 L CaCO + 2HCl CaCl + H O + CO 3 2 2 2 (E) 13.0 L

(A) 50.0 (B) 100 (C) 111 (D) 200 103.The mass of potassium chloride formed by the complete decomposition of 490 g of potassium 98. What volume of oxygen, O , at STP can be prepared 2 chlorate is by the complete decomposition of 0.100 mol of potassium chlorate, KClO ? 3 Atomic Molar Masses Cl 35.5 g·mol–1 2KClO 2KCl + 3O –1 3 2 K 39.1 g·mol O 16.0 g·mol–1 (A) 1.49 L (B) 3.36 L (C) 4.80 L (D) 6.72 L (A) 96 g (B) 122.5 g (C) 149 g (D) 298 g 99. The equilibrium equation for the Haber process at 500 °C is (E) 490 g N + 3H 2NH + heat 2 2 3 104.In the reaction

When one liter of nitrogen combines with three liters of 2Al + 3H SO 3H + Al (SO ) hydrogen the maximum volume of ammonia produced is 2 4 2 2 4 3

(A) 1 L (B) 2 L (C) 3 L (D) 4 L the mass of aluminum that reacts with 1 mol of hydrogen ions is approximately (E) 6 L REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY (A) 3.0 g (B) 9.0 g (C) 13.5 g (D) 27.0 g –1 H 1.0 g·mol –1 (E) 81.0 g O 16.0 g·mol

CaO + H O Ca(OH) 105.What is the maximum mass of tungsten (W) obtained 2 2 from the use of 18 g of hydrogen according to the equation (A) 18.7 g (B) 24.7 g (C) 56.1 g (D) 74.1 g WO + 3H W + 3H O 3 2 2 109.Consider the equation:

2Al(OH) Al O + 3H O Atomic Molar Masses 3 2 3 2 H 1. g·mol–1 –1 When 15.0 g of aluminum hydroxide, Al(OH) is W 184. g·mol 3 decomposed, how many grams of water will be formed? (A) 1 184 g (D) 18 184 g (B) 3 184 g (E) 184 g + 3 16 g Atomic Molar Masses (C) 9 184 g Al 27.0 g·mol–1 H 1.0 g·mol–1 O 16.0 g·mol–1

(A) 3.86 g (B) 5.19 g (C) 4.20 g (D) 22.5 g

106.In the reaction represented by the equation

COCl + 2NaI 2NaCl + CO + I 2 2 110.What mass of water is produced by complete combustion of 126 g of propene, C H ? what is the maximum mass of iodine that can be liberated 3 6 from 60.0 g of sodium iodide? 2C H + 9O 6H O + 6CO 3 6 2 2 2 Molar Masses –1 NaI 150. g·mol Atomic Molar Masses –1 I 254. g·mol C 12.0 g·mol–1 2 H 1.0 g·mol–1 (A) 5.00 g (B) 25.4 g (C) 50.8 g (D) 127 g O 16.0 g·mol–1

(E) 254 g (A) 18.0 g (B) 54.0 g (C) 126 g (D) 162 g

107.What mass of iron oxide, Fe O , is produced from 3 4 111.If 10.0 g of iron, Fe, and 10.0 g of sulfur, S, are 2.00 mol of iron, Fe? heated together, how many grams of iron(II) sulfide, FeS, could be formed? 3Fe(s) + 4H O(g) Fe O (s) + 4H (g) 2 3 4 2 Atomic Molar Masses –1 Molar Mass Fe 55.8 g·mol –1 Fe O 231. g·mol–1 S 32.1 g·mol 3 4 Fe + S FeS (A) 154 g (B) 231 g (C) 462 g (D) 693 g (A) 10.0 (B) 15.7 (C) 27.6 (D) 88.0 108.What mass of calcium hydroxide, Ca(OH) , is 2 obtained from 18.7 g of calcium oxide, CaO? 112.The equation for the complete combustion of propane, C H , is 3 8 Atomic Molar Masses –1 C H (g) + 5O (g) 3CO (g) + 4H (g) Ca 40.1 g·mol 3 8 2 2 2 REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY 116.A compound contains 85.71% carbon and 14.29% What is the maximum mass of carbon dioxide produced hydrogen by mass. Its simplest formula is when a mixture of 0.500 mol of propane and 3.00 mol of oxygen is ignited? Atomic Molar Masses C 12 g·mol–1 Atomic Molar Masses H 1 g·mol–1 C 12.0 g·mol–1 –1 O 16.0 g·mol (A) CH (B) CH (C) C H (D) C H 2 2 2 2 (E) C H (A) 22.0 g (B) 29.3 g (C) 44.0 g (D) 66.0 g 2 4 (E) 132. g 117.Decomposition of 12 g of a compound containing 113.Consider the equation: only carbon and hydrogen yields 9 g of carbon and 3 g of hydrogen. What is the simplest formula of the CH (g) + 2O (g) CO (g) + 2H O(l) compound? 4 2 2 2

How many moles of reactant are in excess when 2.0 mol Atomic Molar Masses –1 of CH (g) are ignited in 2.0 mol of O (g)? C 12.0 g·mol 4 2 H 1.0 g·mol–1 (A) l.0 mol CH (C) 0.5 mol CH 4 4 (A) CH (B) CH (C) C H (D) C H (B) 2.0 mol O (D) no excess of either 2 4 2 5 3 7 2 reactant (E) C H 3 9

114.How many grams of water, H O, can be prepared 2 when 2.00 mol of hydrogen, H , and 2.00 mol of 2 118.A sample of a compound contains 3.21 g of sulfur, S, oxygen, O , are mixed and reacted in this process? 2 and 11.4 g of fluorine, F. Find the empirical formula of the compound. 2H + O 2H O 2 2 2 Atomic Molar Masses –1 Atomic Molar Masses F 19.0 g·mol –1 H 1.0 g·mol–1 S 32.0 g·mol O 16.0 g·mol–1 (A) SF (B) SF (C) SF (D) SF 2 3 6 (A) 18.0 g (B) 36.0 g (C) 68.0 g (D) 72.0 g 119.A compound has the empirical formula CH O and 2 EMPIRICAL FORMULAS –1 the molecular mass 180 g·mol . What is its molecular formula? 115.Upon analysis a compound is found to contain 22.8% sodium, 21.8% boron, and 55.4% oxygen. Its (A) CH O (C) C H O simplest formula is 8 10 12 4 2 (B) C H O (D) C H O 6 12 6 12 24 12 Atomic Molar Masses B 11 g·mol–1 120.A substance has an empirical (simplest) formula of –1 CH and a molar mass of 30 g·mol–1. The molecular Na 23 g·mol 3 O 16 g·mol–1 (true) formula is

(A) Na B O (D) Na B O Atomic Molar Masses 2 4 7 3 4 –1 (B) NaBO (E) Na BO C 12.0 g·mol 3 4 –1 (C) NaB O H 1.0 g·mol 2 5 (A) (CH ) (B) (CH ) (C) (CH ) (D) (CH ) 3 1 3 2 3 3 3 4 REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY

121.A compound whose empirical formula is CH has a 129.An ion has 13 electrons, 12 protons, and 14 neutrons. 2 What is the mass of the ion? molar mass of 28 g·mol–1. What is the molecular formula? (A) 14 u (B) 25 u (C) 26 u (D) 27 u (E) 39 u Atomic Molar Masses C 12.0 g·mol–1 130.The symbol that represents 11 protons, 12 neutrons, and 10 electrons would be: H 1.0 g·mol–1 + 2+ (A) CH (B) C H (C) C H (D) CH (A) Na (B) Na (C) Mg (D) Mg 2 2 4 2 2 4 131.The atomic number of an element is determined by 122.A gaseous compound contains a ratio of one atom of the number of sulfur to one atom of fluorine. A mole of this gas has a mass of approximately 102 g. What is the (A) protons in each of its atoms. molecular formula? (B) neutrons in each of its atoms. (C) particles in each of its atoms. Atomic Molar Masses (D) protons plus neutrons in each of its atoms. F 19. g·mol–1 (E) protons plus electrons in each of its atoms. –1 S 32. g·mol 132.All positive ions differ from their corresponding atoms by having (A) SF (B) S F (C) S F (D) SF 2 2 3 3 4 (A) larger diameters. UNIT 7 PERIOD TABLE/TRENDS (B) fewer electrons. (C) a charge of +1. 123.A calcium ion is a calcium atom that has (D) greater atomic masses. (E) stronger metallic properties (A) lost one electron. (D) lost two electrons. 133.Which group represents particles that contain the (B) gained one electron. (E) gained two electrons. same number of electrons? (C) gained one ion. 124.An atom that loses or gains an electron becomes (A) F, Ne, Na (D) O2–, S2–, Se2– (B) Mg, Al, Si (E) Ca2+, Fe2+, Zn2+ (A) an ion. (D) a molecule. – + (B) a radical. (E) an electrolyte. (C) Cl , Ar, K (C) an isotope. 134.Note the chart of interactions of equal volumes of 125.Metallic atoms become ions by various 0.100 M aqueous solutions. (Symbols of elements or ions have been replaced by capital letters, (A) losing protons. (C) gaining protons. and soluble products are indicated by “S”) What is (B) losing electrons. (D) gaining electrons. the formula of the precipitate?

126.How many electrons are in a chromium(III) ion, Cr3+? AY BX CY DX ppt S S (A) 52 (B) 27 (C) 24 (D) 21 CY S S 127.The number of neutrons in the nucleus of an atom of BX ppt Be is

(A) 36 (B) 13 (C) 9 (D) 5 (A) DY (B) BY (C) AX (D) CX (E) 4 135.An odorless, colorless, tasteless gas is suspected to be 128.Which symbol represents an atom that contains the oxygen. Which result would support this hypothesis? largest number of neutrons? (A) The gas would extinguish a flame. (A) U (B) U (C) Np (D) Pu (B) The gas would turn limewater milky. (C) The gas would burn in air producing only water. (E) Pa (D) A glowing splint would burst into flame in the gas. REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY (A) MCl (B) MCl (C) MCl (D) MCl 2 3 4 136.The chemical properties of atoms depend principally upon (E) M Cl 2 (A) their atomic masses. (B) the masses of the nuclei involved. 144.What is the most probable formula for a compound of (C) the number of neutrons in their nuclei. silicon, Si, and hydrogen, H? (D) the ratio in which the atoms combine with other (A) SiH (B) SiH (C) SiH (D) SiH atoms. 2 6 4 (E) the number of electrons in their outermost shells. 145.A hypothetical element, Z, forms a chloride with the 137.The similar chemical behavior of the elements in a formula ZCl . What is the most probable formula for given family in the periodic table is best accounted 5 for by the fact that atoms of these elements have its oxide?

(A) ZO (B) ZO (C) Z O (D) Z O (A) the same number of electrons in the outermost shell. 2 5 2 5 5 2 (B) the same number of electrons. (C) the same number of protons. 146.Based on the position of the elements in the periodic (D) similar nuclear structures. chart, the most likely formula for strontium nitride is (E) a common origin (A) Sr N (B) Sr N (C) Sr N (D) Sr N 138.The best explanation of the extreme activity of 2 5 5 2 2 3 3 2 fluorine as compared to other halogens is that the fluorine atom 147.Which family of elements always forms ions with an oxidation number of +2 in compounds? (A) has the smallest atomic radius. (B) has the smallest nuclear charge. (A) halogens (C) transition metals (C) has seven valence electrons. (B) alkali metals (D) alkaline–earth metals (D) is the strongest reducing agent. (E) needs one electron to complete its outermost shell. 148.Which element is the most electronegative? 139.In the modern periodic table the elements are (A) Be (B) Mg (C) Ca (D) Sr arranged in the order of increasing (E) Ba 149.Since sodium and potassium are both members of (A) atomic masses. (C) atomic numbers. Group 1A in the periodic table, a sodium and a (B) atomic radii. (D) atomic volumes. potassium atom have the same

140. In which set are the three elements in the same (A) atomic mass. family? (B) number of protons in their nuclei. (C) atomic number and the same nuclear charge. (A) B, C, N (C) Hg, Ga, Sr (D) characteristic of losing one electron per atom to form (B) N, O, F (D) Zn, Cd, Hg an ion. (E) total number of electrons around the nucleus. 141.Which scientist is given credit for developing the periodic table? 150.The element requiring the least amount of energy to remove one electron from an atom is (A) Rutherford (C) Dalton (B) Mendeleev (D) Planck

142.lf XO is the correct formula for an oxide, the (A) Na (B) Be (C) O (D) Cl 2 formula for the chloride of X is (E) Ar (A) XCl (B) XCl (C) XCl (D) X Cl 2 4 2 3 151.In which part of the periodic table are the most electronegative elements found? (E) XCl 3

143.M represents a metallic element, the oxide of which has the formula M O. The formula of the chloride of 2 M is (A) upper left (C) upper right (B) lower left (D) lower right REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY (A) protons. (C) isotopes. (B) neutrons. (D) electrons.

157.The molar mass of a compound is 75 g·mol–1. A student reported an experimental value of 78 g·mol–1. The percent error is

(A) (D) 100

(B) 100 (E) 100

(C) 100

158.A student reads a balance as 38.81 g. The correct reading is 38.41 g. What is the percent error?

152.Consider a plot of a property of the alkaline earth (A) 0.0104% (C) 0.400% metals. (B) 0.104% (D) 1.04% 159.The number of protons in the atom whose atomic mass is 89 and atomic number is 39, is

(A) 39 (B) 50 (C) 51 (D) 89

Which property is plotted on this graph? (E) 128

(A) first ionization energy 160.The particles present in the orbitals of an atom are (B) atomic radius (C) atomic mass (A) mesons. (D) positrons. (D) number of valence electrons (B) protons. (E) electrons. (C) neutrons. 153.As the atomic numbers of the elements in a family increase, the 161.A neutral atom whose outermost electron shell contains eight electrons (A) atomic radii decrease. (B) atomic masses decrease. (A) is very active. (C) ionization energies decrease. (B) has a combining number of one (D) elements become less metallic. (C) is classified as a metal. (E) number of electrons in the outermost energy level (D) is chemically inert. increases. (E) is more active than hydrogen.

154.Which of these atoms has the smallest radius? 162.When the halogens form ions, the result is

(A) K (B) Cl (C) Br (D) Cs (A) colored ions. (B) positive ions. 155.Which characteristic of fluorine causes it to be the (C) diatomic molecules. most active member of the halogen family, Group (D) covalent compounds. 7A? (E) a completed outer shell of electrons.

(A) It forms diatomic molecules. 163.The correct electronic configuration for the sodium (B) It has the smallest atomic radius. atom, Na, is (C) It has no naturally occuring isotopes. (D) It has seven electrons in its outer shell. (A) 1s22s22p6 2 2 6 1 UNIT 11-13 ATOMIC STRUCTURE/DIAGRAMMING (B) 1s 2s 2p 3s ELECTRONS (C) 1s22s22p43s23p1 (D) 1s22s22p82d103s1 156.The chemical activity of an atom is most closely 2 2 6 10 2 1 related to the number and arrangement of its (E) 1s 2s 2p 2d 3s 3p REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY (A) 1 (B) 2 (C) 3 (D) 6

(E) 10 164.Which element has the electron configuration 2 2 6 2 6 1 5 1s 2s 2p 3s 3p 4s 3d ? 172.What neutral atom has the electron configuration 1s22s22p63s23p64s1? (A) zinc (D) chromium (B) copper (E) potassium (A) Na (B) K (C) Ca (D) Ba (C) nickel 173.Which sublevel becomes filled when a chloride ion, 165.The electron arrangement that represents the most – active metallic element in this list is Cl , is formed?

(A) 2)7 (B) 2)8)1 (C) 2)8)2 (D) 2)8)3 (A) 2p (B) 3p (C) 4p (D) 3s

(E) 2)8)6 174.Which electron configuration represents a noble gas?

166.What is the electronic configuration of an aluminum (A) ls22s22p63s23p5 (C) 1s22s22p63s23p64s1 atom, Al? (B) ls22s22p63s23p6 (D) ls22s22p63s23p64s2

2 2 6 3 (A) ls 2s2 p 3d 175.When an electron shifts from one energy level to a (B) 1s22s22p63s23p1 higher level in the same atom, energy is absorbed. Which of the electron transitions represented below (C) ls22s22p62d13s2 absorbs (that is, requires) the most energy? (D) 1s22s22p62d103s23p5 (E) 1s22s22p63s23p63d74s2

167.Which atom contains a partially filled 3p orbital?

(A) iron (D) calcium (A) A (B) B (C) C (D) D (B) argon (E) aluminum (C) boron 176.A single burst of light is released from an atom. Which statement explains what happens in the atom? 168.Which element has the electron configuration 1s22s22p63s2? (A) An electron is changed from a particle to a wave. (B) An electron moved from a higher to a lower energy (A) aluminum (C) magnesium level. (B) calcium (D) sodium (C) An electron pulled a proton out of the nucleus. (D) An electron pulled a neutron out of the nucleus. 169.Which electron configuration represents an atom in an excited state? 177.Neon atoms produce characteristic spectral lines when their electrons 2 2 6 (A) 1s 2s 2p (A) return to lower energy levels. 2 2 6 2 (B) 1s 2s 2p 3s (B) orbit the nucleus in a single energy level. (C) 1s22s22p63s23p64s23d1 (C) remain in their normal energy levels and move faster. (D) remain in their normal energy levels and move (D) 1s22s22p63s23p64s24p1 slower.

170.When two electrons occupy the same orbital, they must have

(A) opposite spins. 178.Which electron configuration represents a transition (B) mutual attraction. element? (C) four identical quantum numbers. (D) different magnetic quantum numbers. 2 2 6 2 (A) 1s 2s 2p 3s (E) different principal quantum numbers. (B) 1s22s22p63s23p6 171.What is the maximum number of electrons allowed in (C) 1s22s22p63s23p64s1 an orbital? (D) 1s22s22p63s23p63d3 4s2 REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY

BONDING 187.The type of bond formed when two atoms share a pair of electrons is called 179.In which pair do both compounds exhibit ionic bonding? (A) ionic. (D) bivalent. (B) double. (E) electrovalent. (A) SO , HCl (D) KCl, CO 2 2 (C) covalent (B) KNO , CH (E) NaCl, H O 3 4 2 (C) NaF, KBr 188.A pure substance melts at 113 °C and does not conduct electricity in either the solid or liquid state. 180.A chemical bond is considered to be predominantly The bonding in this substance is primarily ionic if (A) ionic. (C) metallic. (A) atoms of the same element combine. (B) network. (D) covalent (molecular). (B) the reaction forming the bond is endothermic. (C) atoms of an active metal combine with the atoms of 189.Which pair of atoms forms a covalent bond? an active nonmetal. (D) the bond is between atoms of elements which are of (A) Li and Br (C) K and Br the same family. (B) Na and Br (D) H and Br (E) atoms of one metal combine with atoms of another 190.When a chlorine molecule, Cl , is formed, the orbital metal. 2 overlap may be represented by the designation 181.Which bond has the least ionic character? (A) p – p (B) s – p (C) s – s (D) s – d (A) P—Cl (B) H—Cl (C) Br—Cl (D) S—Cl (E) p – d (E) Cl—Cl POLARITY OF MOLECULES 182.Which type of bonding predominates in solid potassium chloride, KCl? 191.Which represents a polar molecule?

(A) ionic (C) hydrogen (A) F (B) O (C) CH (D) CO (B) metallic (D) covalent (molecular) 2 2 4 2 (E) HCl 183.Which pair of elements react to form a compound that has the greatest ionic character? 192.Which molecule is essentially nonpolar? (A) xenon and fluorine (C) cesium and chlorine (A) CH (B) HCl (C) HBr (D) H O (B) carbon and oxygen (D) iron and sulfur 4 2

(E) NH 184.Which compound contains both ionic and covalent 3 bonds? 193.The compounds H S, H Se, and H Te boil below 0 (A) CO (B) KNO (C) NaCl (D) CCl F 2 2 2 2 3 2 2 °C at standard pressure. Water (H O) boils at 100 °C. 2 185.The electronegativity of francium is 0.7 and that of This abnormally high boiling point of water is a fluorine is 4.0. The difference in electronegativity consequence of the suggests that the predominant bonding between Fr and F is (A) low molar mass of water. (B) low electrical conductivity of water. (A) ionic. (B) metallic. (C) covalent. (C) covalent bonds in the water molecule. (D) very weak. (E) coordinate covalent (D) stability of the bonds in the water molecules. (E) hydrogen bonds between the water molecules 186.A solid has no electrical conductivity at room temperature. It is heated to 600 °C, melts, and then 194.The graph below shows the boiling points of four has electrical conductivity. The solid has which type hydrogen compounds. of bonding?

(A) ionic bonding (C) metallic bonding (B) covalent bonding (D) van der Waals forces REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY 200.Which formula represents a nonpolar molecule? What type of bonding explains the large difference between the boiling points of H O and the other hydrogen (A) HCl (B) CF (C) NH (D) H S 2 4 3 2 compounds? 201.Which is an example of a nonpolar molecule that (A) ionic bonding (C) hydrogen bonding contains polar covalent bonds? (B) covalent bonding (D) van der Waals attractions (A) CCl (B) N (C) H O (D) NH 4 2 2 3 195.An explanation of the heat of vaporization of water being much higher than the heat of vaporization of 202.Which molecule is nonpolar? ethane (C H ) is that 2 6 (A) H O (B) HF (C) NF (D) CF 2 3 4 (A) ethane has dipolar molecules. 203.The shape of a chloroform molecule, CHCl , is (B) water is more dense than liquid ethane. 3 (C) water has a higher boiling point than ethane. (D) water molecules are lighter than ethane molecules. (A) linear. (D) tetrahedral. (E) energy is needed to break the hydrogen bonding (B) cubical. (E) planar triangular. between water molecules. (C) octahedral.

196.The higher boiling point of HF compared with HCl, 204.Which molecule is nonpolar? HBr, and HI is caused by (A) H O (B) HF (C) NF (D) CF (A) covalently bonded molecules. 2 3 4 (B) the size of the molecules. 205.The arrangement of atoms in a water molecule, H O, (C) the shape of the molecules. 2 (D) hydrogen bonding between molecules. is best described as (E) weak van der Waals forces between HF molecules. (A) ring. (B) bent. (C) linear. (D) spherical. MOLECULAR SHAPES 206.What is the shape of the ammonia, NH , molecule? 3 197.Compounds that have the same molecular formula but different structural formulas are known as (A) bent (C) planar (B) linear (D) pyramidal (A) isomers. (C) isotopes. (B) polymers. (D) allotropes. 207.The shape of the CH molecule is most similar to the 4 shape of a molecule of

(A) H O (B) N H (C) SiH (D) C H 198.A molecule is said to be polar if it 2 2 4 4 2 4

(A) has a north and south pole. 208.Which molecule has all of its atoms in one plane? (B) has a symmetrical electron distribution. (C) exhibits a polar spin under certain conditions. (A) H SO (B) CH (C) BF (D) NH (D) may exhibit a positive or negative charge. 2 4 4 3 3 (E) exhibits a partial positive charge at one end and a 209. Which term best describes the shape of the ammonia, NH , molecule? partial negative charge at the other. 3

199.Which represents a polar molecule? (A) linear (C) tetrahedral (B) pyramidal (D) trigonal planar (A) H–Cl (D) H–H UNIT 8 RADIOACTIVITY/MOLECULAR STRUCTURE Cl Cl C Cl 210.Rutherford’s alpha–particle bombardment of gold foil Cl helped develop our current model of the atom by (B) O=C=O (E) (C) NN (A) finding the mass of the electron. (B) showing the existence of the neutron. (C) showing that the electron carries a negative charge. REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY (D) showing that the atom has a concentrated central charge 218.A radioactive element having atomic number 82 and atomic mass 214 loses a beta particle, . The 211.The symbol Zn indicates this isotope contains resulting element has

(A) 30 protons and 35 neutrons. Atomic No. Atomic Mass (B) 35 protons and 30 neutrons. (C) 35 protons and 35 neutrons. (A) 80 210 u (D) 65 protons and 30 neutrons. (B) 81 213 u (E) 95 protons and 30 electrons. (C) 81 214 u (D) 82 213 u 212.Isotopes differ in (E) 83 214 u

(A) atomic number. (D) number of neutrons. 219.If the radioactive atom U emits an alpha particle, the (B) nuclear charge. (E) number of electrons. atom remaining is represented by (C) number of protons (A) U (B) Th (C) U (D) Th 213.A hypothetical element X has three isotopes: 40X, (E) Pa 41X, and 42X. Their abundances are 72.0%, 9.00%, and 19.0% respectively. What is the atomic mass of 220.Which particle completes the equation? X? O + n C + ? (A) 40.5 u (B) 40.8 u (C) 41.0 u (D) 41.5 u (A) beta (B) alpha (C) proton (D) neutron 214.Copper has an atomic molar mass of 63.5 g·mol–1. Why is the atomic molar mass not a whole number? (E) deuteron

(A) All copper atoms have identical chemical properties. 221.Which nuclide is produced when a radioactive (B) The fractional number results from the fact that carbon–14 atom emits an electron? protons and neutrons have different masses. (C) There are at least two naturally occurring isotopes of C ? + e copper. 14 (D) Every copper atom has an atomic mass of 63.5 u. (A) C (B) 7N (C) C (D) B

215.The difference between the atomic number of an atom and its mass number gives the number of

(A) protons. (D) orhitals. (B) neutrons. (E) electrons. 222.Given the nuclear reaction (C) energy levels. Th Pa + X What is X?

(A) A proton, p (C) A positron, e 216.Two kinds of emission from radioactive substances (B) A neutron, n (D) A beta particle, e that are considered to be particles of matter are 223.The half–life of radium is 1600 years. If a given (A) alpha and beta emission. sample contains one gram of radium, how much (B) alpha and gamma emission. radium remains after 4800 years?

(C) beta and gamma emission. 1/ 1/ 1/ (A) l g (B) 2 g (C) 3 g (D) 8 g (D) gamma emission and X–radiation. (E) alpha emission and X–radiation. 1/ (E) 16 g 217.What type of reaction is illustrated by this equation? 224.Strontium–90 has a half–life of 28 years. What H + H He + energy fraction of a sample remains as strontium–90 after 84 years? (A) a chemical reaction (C) a fission reaction 1/ 1/ 1/ 1/ (B) radioactive decay (D) a fusion reaction (A) 28 (B) 8 (C) 4 (D) 3 REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY 8 LAB TECHNIQUES/PROCEDURES

225.A barometer is used to measure the 7 (A) pressure of the air at 0 °C only. (B) mass of a column of mercury. (C) temperature of the air at standard pressure. 6 (D) density of mercury. (E) pressure of the air.

226.Which apparatus delivers 50.00 mL of liquid most accurately? (A) 6.20 mL (B) 6.25 mL (C) 6.40 mL (D) 7.80 mL

(A) 50–mL buret 231.Which device should be used to measure 22.5 mL of (B) 50–mL beaker an aqueous solution? (C) 50–mL test tube (D) 50–mL graduated cylinder

25 227.Most student thermometers have an uncertainty of 20 0.2 Celsius degrees. Which is the proper reading of 15 30 30 the thermometer shown in the illustration? 10 5 20 20 10 10 25 m L 17 A B C D 16 15 14 (A) A (B) B (C) C (D) D

(A) l6. °C (B) 16.4 °C(C) 16.40 °C (D)16.45 °C

228.A narrow–necked, glass–stoppered bottle contains sulfuric acid. When the acid is being poured, the stopper should be 232.In the laboratory, never dip a stirring rod into a (A) placed on the lab table. reagent bottle because (B) put into the reaction vessel. (C) held in the palm of the hand. (A) the bottle may tip. (D) held inverted between the index and middle fingers. (B) the rod might break. (C) the rod may puncture the bottle. 229.Which device is commonly used to measure liquid (D) the contents of the bottle may become contaminated. volumes most precisely? (E) the amount of liquid remaining on the rod is too small to be used. (A) graduated cylinder (C) balance (B) graduated beaker (D) buret 233.The purpose of filtration is to

230.This drawing shows the surface of water in a 10 mL (A) form precipitates. graduated cylinder. How much water is in the (B) remove water from solutions. cylinder? (C) separate dissolved ions from the solvent. (D) separate insoluble substances from a solution. REVIEW SHEET 1ST SEMESTER HONORS CHEMISTRY