Exam

Name______

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

1) Which of the following is an ionic compound? 1) A) NO2 B) CF4 C) PCl3 D) SeBr2 E) LiCl

2) Which of the following is an ionic compound? 2) A) CH2O B) Cl2O C) PF5 D) Mg3(PO4)2 E) SCl2

3) Which of the following contains BOTH ionic and covalent bonds? 3) A) CaI2 B) CaSO4 C) COS D) SF6 E) None of the above contain both ionic and covalent bonds.

4) Which of the following is a molecular compound? 4) A) RbBr B) N2O4 C) NaNO3 D) SrSO3 E) CuCl2

5) Which of the following is a molecular compound? 5) A) P4O10 B) ZnS C) NaCN D) SrI2 E) LiOH

6) A covalent bond is best described as: 6) A) a bond between a metal and a polyatomic . B) a bond between a metal and a nonmetal. C) a bond between two polyatomic . D) the transfer of electrons. E) the sharing of electrons between atoms.

7) An ionic bond is best described as: 7) A) the attraction that holds the atoms together in a polyatomic ion. B) the transfer of electrons from one atom to another. C) the attraction between 2 nonmetal atoms. D) the attraction between 2 metal atoms. E) the sharing of electrons.

8) Which of the following is a molecular element? 8) A)S B)Ag C)Kr D)Mg E)Ti

9) Which of the following is a molecular element? 9) A) Xe B) I C) Li D) Mg E) Ar

1 10) Which of the following is an atomic element? 10) A) Mg B) Br C) O D) H E) N

11) What is the empirical formula for C4H10O2? 11) A) C2H4O B) CHO C) CHO2 D) CH2OE)C2H5O

12) What is the empirical formula for Hg2(NO3)2? 12) A) Hg2NO3 B) Hg(NO3)2 C) Hg4(NO3)4 D) HgNO3 E) Hg2(NO3)2

13) Write the formula for the compound formed between potassium and sulfur. 13) A) KS2 B) K2SC)KSD)K2SO3 E) K3S2

14) Write the formula for barium nitrite. 14) A) Ba3N2 B) Ba(NO2)2 C) B(NO2)3 D) BaNO3 E) BN

15) Write the formula for copper (II) sulfate pentahydrate. 15) A) CuS*5H2O B) CuSO4·5H2O C) (CuSO4)5 D) Cu2S*H2O E) Cu2SO3·H5

16) Write the formula for strontium nitride. 16) A) Sr3N2 B) Sr(NO3)2 C) Sr(NO2)2 D) Sr2N3 E) SrN

17) Determine the name for TiCO3. Remember that titanium forms several ions. 17) A) titanium carbonite B) titanium (II) carbonate C) titanium (II) carbonite D) titanium carbide E) titanium (I) carbonate

18) Write the name for Sn(SO4)2. Remember that Sn forms several ions. 18) A) tin (IV) sulfate B) tin (II) sulfite C) tin sulfide D) tin (I) sulfate E) tin (I) sulfite

2 19) Write the name for Ca3(PO4)2. 19) A) calcium (III) phosphite B) calcium phosphate C) tricalcium phosphorustetraoxide D) calcium phosphite E) calcium (II) phosphite

20) Determine the name for CoCl2·6H2O. Remember that Co forms several ions. 20) A) cobalt (I) chloride B) cobalt (II) chloride heptahydrate C) cobalt (I) chloride heptahydrate D) cobalt chloride hydrate E) cobalt (II) chloride hexahydrate

21) Determine the name for P4O10. 21) A) phophorus oxide B) diphosphorus pentaoxide C) phosphorus (IV) oxide D) phosphorus (II) oxide E) tetraphophorus decaoxide

22) Determine the name for N2O5. 22) A) nitrogen tetraoxide B) dinitrogen pentaoxide C) nitrogen (IV) oxide D) nitrogen oxide E) nitrogen (II) oxide

23) Determine the name for Cl2O. 23) A) chlorine oxide B) dichloro monoxide C) chlorate D) chlorine (II) oxide E) chlorine (I) oxide

24) Determine the name for H2CO3. 24) A) hydrocarbonic acid B) hydrocarbide acid C) carbonic acid D) dihydrogen carbonate E) carbonous acid

25) Determine the name for HClO3. 25) A) chlorate acid B) perchloric acid C) hydrochlorus acid D) chloric acid E) hydrochloric acid

3 26) Determine the name for aqueous HBr. 26) A) hydrobromic acid B) bromous acid C) hydrobromous acid D) bromic acid E) hydrogen bromate

27) Which of the following is one possible form of pentane? 27) A) CH3CH2CH2CH2CH2CH3 B) CH3CH2CH2CH2CH2NH2 C) CH3CH2CH2CH2CH3 D) CH3CH=CHCH2CH3 E) CH3CH2-O-CH2CH2CH3

28) Which of the following compounds is ethanol? 28) A) C2H6 B) CH3CO2CH3 C) CH3CO2H D) C2H5OH E) CH3-O-CH3

29) Calculate the molar mass for Mg(ClO4)2. 29) A) 247.52 g/mol B) 119.52 g/mol C) 123.76 g/mol D) 223.21 g/mol E) 75.76 g/mol

30) Calculate the molar mass of Al(C2H3O2)3. 30) A) 139.99 g/mol B) 258.09 g/mol C) 86.03 g/mol D) 204.13 g/mol E) 56.00 g/mol

31) Calculate the molar mass of Ca3(PO4)2. 31) A) 87.05 g/mol B) 310.18 g/mol C) 215.21 g/mol D) 279.21 g/mol E) 246.18 g/mol

4 32) Write a balanced equation to show the reaction of sulfurous acid with hydroxide to form 32) water and lithium sulfite. A) HSO3 (aq) + LiOH (aq) → H2O (l) + LiSO3 (aq) B) H2S (aq) + 2 LiOH (aq) → 2 H2O (l) + Li2S (aq) C) HSO4 (aq) + LiOH (aq) → H2O (l) + LiSO4 (aq) D) H2SO3 (aq) + 2 LiOH (aq) → 2 H2O (l) + Li2SO3 (aq) E) H2SO4 (aq) + LiOH (aq) → H2O (l) + Li2SO4 (aq)

33) Write a balanced equation to show the reaction of gaseous ethane with gaseous oxygen to form 33) carbon monoxide gas and water vapor. A) 2 C2H6 (g) + 5 O2 (g) → 4 CO (g) + 6 H2O (g) B) 2 C2H6 (g) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (g) C) C2H6 (g) + 5 O (g) → 2 CO (g) + 3 H2O (g) D) 2 CH3 (g) + 5 O (g) → 2 CO (g) + 3 H2O (g) E) C2H6 (g) + 7 O (g) → 2 CO2 (g) + 3 H2O (g)

34) Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous 34) ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate. A) Al(CO3)2 (aq) + (NH3)2PO4 (aq) → AlPO4 (s) + 2 NH3CO3 (aq) B) Al(C2H3O2)2 (aq) + (NH4)2PO4 (aq) → AlPO4 (s) + 2 NH4C2H3O3 (aq) C) Al(CO2)3 (aq) + (NH4)3PO3 (aq) → AlPO3 (s) + 3 NH4CO2 (aq) D) Al(C2H3O2)2 (aq) + (NH3)2PO4 (aq) → AlPO4 (s) + 2 NH3C2H3O3 (aq) E) Al(C2H3O2)3 (aq) + (NH4)3PO4 (aq) → AlPO4 (s) + 3 NH4C2H3O3 (aq)

35) How many N2O4 molecules are contained in 76.3 g N2O4? The molar mass of N2O4 is 92.02 35) g/mol. A) 4.59 × 1025 N2O4 molecules B) 7.26 × 1023 N2O4 molecules C) 5.54 × 1025 N2O4 molecules D) 1.38 × 1024 N2O4 molecules E) 4.99 × 1023 N2O4 molecules

36) How many C2H4 molecules are contained in 45.8 mg of C2H4? The molar mass of C2H4 is 28.05 36) g/mol. A) 7.74 × 1026 C2H4 molecules B) 4.69 × 1023 C2H4 molecules C) 9.83 × 1020 C2H4 molecules D) 3.69 × 1023 C2H4 molecules E) 2.71× 1020 C2H4 molecules

37) What is the mass (in kg) of 6.89 × 1025 molecules of CO2? The molar mass of CO2 is 44.01 g/mol. 37) A) 3.85 kg B) 2.60 kg C) 5.04 kg D) 6.39 kg E) 3.03 kg

5 38) What is the mass of 9.44 × 1024 molecules of NO2? The molar mass of NO2 is 46.01 g/mol. 38) A) 341 g B) 685 g C) 294 g D) 205 g E) 721 g

39) Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass. 39) A) N2O3 B) NO3 C) N2OD)NOE)NO2

40) Determine the empirical formula for a compound that is found to contain 10.15 mg P and 34.85 mg 40) Cl. A) PCl3 B) PCl C) P3Cl D) P2Cl3 E) PCl2

41) Determine the empirical formula for a compound that contains C, H and O. It contains 52.14% C 41) and 34.73% O by mass. A) CH3OB)C2H6O C) CHO D) C4H13O2 E) CH4O3

42) Determine the molecular formula of a compound that has a molar mass of 183.2 g/mol and an 42) empirical formula of C2H5O2. A) C6H15O6 B) C8H20O8 C) C3H7O3 D) C2H5O2 E) C4H10O4

43) Determine the molecular formula of a compound that has a molar mass of 92.0 g/mol and an 43) empirical formula of NO2. A) N3O6 B) N2O5 C) N2O4 D) NO2 E) N2O3

44) How many atoms of oxygen are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3 44) is 233.99 g/mol. A) 1.10 × 1024 O atoms B) 2.87 × 1025 O atoms C) 2.96 × 1024 O atoms D) 1.23 × 1023 O atoms E) 3.19 × 1024 O atoms

45) How many sodium ions are contained in 99.6 mg of Na2SO3? The molar mass of Na2SO3 is 45) 126.05 g/mol. A) 4.76 × 1020 sodium ions B) 1.52 × 1027 sodium ions C) 9.52 × 1020 sodium ions D) 2.10 × 1021 sodium ions E) 1.05 × 1021 sodium ions

46) How many moles of N2O3 contain 2.55 × 1024 oxygen atoms? 46) A) 7.87 moles N2O3 B) 4.23 moles N2O3 C) 1.41 moles N2O3 D) 2.82 moles N2O3 E) 12.7 moles N2O3

6 47) How many moles of PCl3 contain 3.68 × 1025 chlorine atoms? 47) A) 20.4 moles PCl3 B) 16.4 moles PCl3 C) 54.5 moles PCl3 D) 61.1 moles PCl3 E) 49.1 moles PCl3

48) How many moles of C3H8 contain 4.95 × 1024 hydrogen atoms? 48) A) 9.73 moles C3H8 B) 6.58 moles C3H8 C) 1.03 moles C3H8 D) 3.09 moles C3H8 E) 8.22 moles C3H8

49) How many millimoles of Ca(NO3)2 contain 4.78 × 1022 formula units of Ca(NO3)2? The molar 49) mass of Ca(NO3)2 is 164.10 g/mol. A) 57.0 mmol Ca(NO3)2 B) 12.6 mmol Ca(NO3)2 C) 20.7 mmol Ca(NO3)2 D) 13.0 mmol Ca(NO3)2 E) 79.4 mmol Ca(NO3)2

50) How many moles of C3H8 contain 9.25 × 1024 molecules of C3H8? 50) A) 15.4 moles C3H8 B) 65.1 moles C3H8 C) 46.2 moles C3H8 D) 34.9 moles C3H8 E) 28.6 moles C3H8

51) Calculate the mass percent composition of sulfur in Al2(SO4)3. 51) A) 28.12 % B) 42.73 % C) 35.97 % D) 9.372 % E) 21.38 %

52) Calculate the mass percent composition of lithium in Li3PO4. 52) A) 26.75 % B) 30.72 % C) 17.98 % D) 55.27 % E) 20.82 %

53) Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO 2 53) and 59.38 mg of H2O. What is the empirical formula for the compound? A) C5H2OB)C6HO3 C) CHO D) C3H7OE)C3H6O

7 54) How many molecules of ethane are contained in 25.0 mL of butane? The density of butane is 54) 0.6011 g/mL and the molar mass is 58.12 g/mol. A) 7.14 × 1025 molecules butane B) 2.59 × 1023 molecules butane C) 1.56 × 1023 molecules butane D) 6.87 × 1023 molecules butane E) 1.46 × 1027 molecules butane

55) Determine the volume of hexane that contains 5.33 × 1022 molecules of hexane. The density of 55) hexane is 0.6548 g/mL and its molar mass is 86.17 g/mol. A) 12.4 mL B) 7.40 mL C) 8.59 mL D) 13.5 mL E) 11.7 mL

MATCHING. Choose the item in column 2 that best matches each item in column 1.

Match the following.

56) oxygen A) O (g) 2 56)

57) chlorine B) Ca2 (g) 57)

58) neon C) Ca (s) 58)

59) calcium D) I2(s) 59)

60) iodine E) Cl2(g) 60)

F) Ne2 (g)

G) Cl(g)

H) O (g)

I) I (g)

J)Ne (g)

SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question.

61) Describe the difference between ionic and molecular compounds. Give an example of 61) each.

62) How can one compound contain both ionic and covalent bonds? Give an example. 62)

63) Why arenʹt prefixes used in naming ionic compounds? 63)

64) Describe the difference between a molecular formula and an empirical formula. Give an 64) example.

8 65) Can you predict the for a covalent compound between nitrogen and 65) oxygen? Explain your answer.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

66) According to the following balanced reaction, how many moles of NO are formed from 8.44 moles 66) of NO2 if there is plenty of water present?

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

A) 25.3 moles NO B) 1.83 moles NO C) 2.81 moles NO D) 5.50 moles NO E) 8.44 moles NO

67) Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles 67) of water? Assume that there is excess C3H7SH present.

C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O (g)

A) 2.33 moles O2 B) 3.50 moles O2 C) 4.14 moles O2 D) 1.55 moles O2 E) 6.21 moles O2

68) According to the following balanced reaction, how many moles of KO are required to exactly react 68) with 5.44 moles of H2O?

4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)

A) 10.9 moles H2O B) 16.7 moles H2O C) 4.87 moles H2O D) 8.33 moles H2O E) 2.72 moles H2O

9 69) Consider the following balanced reaction. How many grams of water are required to form 75.9 g 69) of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol.

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

A) 38.0 g H2O B) 43.4 g H2O C) 10.9 g H2O D) 21.7 g H2O E) 26.5 g H2O

70) Consider the following balanced reaction. What mass (in g) of CO 2 can be formed from 288 mg of 70) O2? Assume that there is excess C3H7SH present.

C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O (g)

A) 0.126 g CO2 B) 0.209 g CO2 C) 0.198 g CO2 D) 0.396 g CO2 E) 0.792 g CO2

71) According to the following reaction, how many grams of sulfur are formed when 37.4 g of water 71) are formed? 2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l)

A) 66.6 g S B) 14.0 g S C) 44.4 g S D) 56.1 g S E) 99.8 g S

72) How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen. 72)

6 Li(s) + N2(g) → 2 Li3N(s)

A) 61.0 g Li3N B) 20.3 g Li3N C) 58.3 g Li3N D) 18.3 g Li3N E) 15.1 g Li3N

73) How many grams of oxygen are formed when 6.21 moles of KOH are formed? 73)

4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)

A) 4.97 g O2 B) 3.59 g O2 C) 11.7 g O2 D) 19.9 g O2 E) 27.9 g O2

10 74) How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the 74) following reaction? The molar mass of KNO3 is 101.11 g/mol.

4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

A) 0.580 mol O2 B) 23.2 mol O2 C) 18.5 mol O2 D) 1.73 mol O2 E) 0.724 mol O2

75) How many molecules of HCl are formed when 50.0 g of water reacts according to the following 75) balanced reaction? Assume excess ICl3.

2 ICl3 + 3 H2O → ICl + HIO3 + 5 HCl

A) 3.65 × 1024 molecules HCl B) 2.78 × 1024 molecules HCl C) 6.09 × 1025 molecules HCl D) 1.67 × 1024 molecules HCl E) 5.02 × 1025 molecules HCl

76) How many molecules of H2S are required to form 79.0 g of sulfur according to the following 76) reaction? Assume excess SO2.

2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l)

A) 5.06 × 1025 molecules H2S B) 2.44 × 1023 molecules H2S C) 3.17 × 1025 molecules H2S D) 1.48 × 1024 molecules H2S E) 9.89 × 1023 molecules H2S

77) Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g 77) N2O4 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol.

N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g)

A) LR = N2H4, 59.0 g N2 formed B) LR = N2H4, 13.3 g N2 formed C) No LR, 45.0 g N2 formed D) LR = N2O4, 105 g N2 formed E) LR = N2O4, 45.7 g N2 formed

11 78) Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to 78) the following balanced reaction. A possibly useful molar mass is BCl3 = 117.16 g/mol.

BCl3(g) + 3 H2O(l) → H3BO3(s) + 3 HCl(g)

A) 75.9 g HCl B) 132 g HCl C) 187 g HCl D) 25.3 g HCl E) 56.0 g HCl

79) Determine the theoretical yield of H2S (in moles) if 4.0 mol Al2S3 and 4.0 mol H2O are reacted 79) according to the following balanced reaction. A possibly useful molar mass is Al2S3 = 150.17 g/mol.

Al2S3 (s) + 6 H2O(l) → 2 Al(OH)3 (s) + 3 H2S(g)

A) 6.0 mol H2S B) 18 mol H2S C) 12 mol H2S D) 2.0 mol H2S E) 4.0 mol H2S

80) Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe 2O3 react 80) with excess Al according to the following reaction.

Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)

A) 61.03 % B) 20.02 % C) 57.30 % D) 28.65 % E) 81.93 %

81) Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 81) 750.0 mL of solution. A) 2.30 M B) 1.50 M C) 1.18 M D) 0.768 M E) 0.130 M

82) Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to 82) yield 50.0 mL of solution. A) 0.0107 M B) 0.0936 M C) 0.0337 M D) 0.0651 M E) 0.0297 M

83) How many milliliters of a 0.184 M NaNO3 solution contain 0.113 moles of NaNO3? 83) A) 326 mL B) 543 mL C) 614 mL D) 163 mL E) 885 mL

84) How many liters of a 0.0550 M KCl solution contain 0.163 moles of KCl? 84) A) 2.96 L B) 8.97 L C) 3.37 L D) 1.48 L E) 1.12 L

85) How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution? 85) A) 7.65 × 10-3 mol B) 1.31 × 10-3 mol C) 8.74 × 10-3 mol D) 1.14 × 10-3 mol E) 3.67 × 10-3 mol

12 86) How many moles of CH3CH2OH are contained in 548 mL of 0.0788 M CH3CH2OH solution? 86) A) 4.32 × 10-2 mol B) 1.44 × 10-2 mol C) 2.32 × 10-2 mol D) 5.26 × 10-2 mol E) 6.95 × 10-2 mol

87) How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3 87) mL of 0.140 M sucrose solution? A) 1.21 × 1021 molecules C12H22O11 B) 1.63 × 1023 molecules C12H22O11 C) 5.90 × 1024 molecules C12H22O11 D) 8.29 × 1022 molecules C12H22O11 E) 6.15 × 1022 molecules C12H22O11

88) How many chloride ions are present in 65.5 mL of 0.210 M AlCl3 solution? 88) A) 5.79 × 1024 chloride ions B) 4.02 × 1023 chloride ions C) 1.21 × 1022 chloride ions D) 2.49 × 1022 chloride ions E) 8.28 × 1021 chloride ions

89) What is the concentration of nitrate ions in a 0.125 M Mg(NO 3)2 solution? 89) A) 0.125 M B) 0.250 M C) 0.375 M D) 0.0625 M E) 0.160 M

90) Which of the following solutions will have the highest concentration of chloride ions? 90) A) 0.10 M NaCl B) 0.10 MAlCl3 C) 0.05 M CaCl2 D) 0.10 M MgCl2 E) All of these solutions have the same concentration of chloride ions.

91) Which of the following solutions will have the highest electrical conductivity? 91) A) 0.045 M Al2(SO4)3 B) 0.10 M KF C) 0.10 M NaI D) 0.10 M LiBr E) 0.050 M (NH4)2CO3

92) How many milliliters of a 0.266 M LiNO3 solution are required to make 150.0 mL of 0.075 M 92) LiNO3 solution? A) 18.8 mL B) 42.3 mL C) 35.1 mL D) 23.6 mL E) 53.2 mL

13 93) What volume (in L) of 0.0887 M MgF2 solution is needed to make 275.0 mL of 0.0224 M MgF2 93) solution? A) 14.4 mL B) 72.3 mL C) 10.9 mL D) 69.4 mL E) 91.8 mL

94) Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M 94) Ca(NO3)2 solution to 150.0 mL. A) 0.0199 M B) 1.13 M C) 0.0501 M D) 0.0887 M E) 0.0313 M

95) Which of the following is NOT a strong electrolyte? 95) A) MgCO3 B) LiOH C) Li2SO4 D) NaC2H3O2 E) CaCl2

96) Which of the following is considered a STRONG electrolyte? 96) A) PbCl2 B) HC2H3O2 C) C12H22O11 D) NH4NO3 E) CH3OH

97) According to the following reaction, what volume of 0.244 M KCl solution is required to react 97) exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution?

2 KCl(aq) + Pb(NO3)2 (aq) → PbCl2(s) + 2 KNO3(aq)

A) 97.4 mL B) 43.0 mL C) 116 mL D) 58.1 mL E) 86.1 mL

98) What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 98) solution? Hint: you will want to write a balanced reaction. A) 345 mL B) 139 mL C) 581 mL D) 278 mL E) 173 mL

99) What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution 99) with 55.0 mL of 0.109 M MgCl2 solution?

2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq)

A) 1.70 g B) 2.56 g C) 0.839 g D) 0.859 g E) 1.72 g

100) According to the following reaction, what mass of PbCl2 can form from 235 mL of 0.110 M KCl 100) solution? Assume that there is excess Pb(NO3)2.

2 KCl(aq) + Pb(NO3)2 (aq) → PbCl2(s) + 2 KNO3(aq)

A) 5.94 g B) 3.59 g C) 1.80 g D) 1.30 g E) 7.19 g

14 101) According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 mL of 0.227 101) M LiOH solution? Assume that there is excess FeCl2.

FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq)

A) 3.97 × 10-2 moles B) 6.49 × 10-2 moles C) 2.52 × 10-2 moles D) 1.99 × 10-2 moles E) 5.03 × 10-2 moles

102) How many of the following compounds are soluble in water? 102)

Cu(OH)2 LiNO3 NH4Br K2S

A) 0 B) 3 C) 1 D) 4 E) 2

103) Which of the following compounds is soluble in water? 103) A) MgCO3 B) CaS C) PbCl2 D) BaSO4 E) None of these compounds is soluble in water.

104) How many of the following compounds are insoluble in water? 104)

KC2H3O2 CaSO4 SrS AlPO4

A) 3 B) 0 C) 1 D) 2 E) 4

105) Which of the following compounds is insoluble in water? 105) A) Hg2I2 B) MgSO4 C) BaS D) (NH4)2CO3 E) All of these compounds are soluble in water.

106) Which of the following pairs of aqueous solutions will react when mixed? 106) A) NaCl + Li3PO4 B) AgC2H3O2 + Cu(NO3)2 C) Hg2(NO3)2 + LiI D) NH4NO3 + Li2CO3 E) None of the above solution pairs will produce a reaction.

15 107) Which of the following pairs of aqueous solutions will react when mixed? 107) A) Sr(C2H3O2)2 + Na2SO4 B) KNO3 + NaOH C) LiOH + Na2S D) (NH4)2SO4 + LiCl E) None of the above solution pairs will produce a reaction.

108) Which of the following pairs of aqueous solutions will react when mixed? 108) A) K2CO3 + HNO3 B) Li2S + HCl C) HCl + LiOH D) MgCl2 + KOH E) All of these solution pairs will produce reactions.

109) Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of 109) lithium sulfide and copper (II) nitrate are mixed. (the superscripts below arenʹt really acceptable on most of the ions, I donʹt know how to make it any better) A) Li+ (aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq) B) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s) C) Li+ (aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq) D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq) E) No reaction occurs.

110) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and 110) Fe(NO3)2 are mixed. A) Fe2+(aq) + S2-(aq) → FeS(s) B) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq) C) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s) D) K+(aq) + NO3-(aq) → KNO3(s) E) No reaction occurs.

111) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 111) and KOH are mixed. A) H+(aq) + OH-(aq) → H2O(l) B) H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + K2SO4(s) C) 2 K+(aq) + SO42-(aq) → K2SO4(s) D) H22+(aq) + OH-(aq) → H2(OH)2(l) E) No reaction occurs.

16 112) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of 112) Al(C2H3O2)3 and LiNO3 are mixed. A) Al3+(aq) + 3 NO3-(aq) → Al(NO3)3(s) B) Al3+(aq) + 3 NO3-(aq) + Li+(aq) + C2H3O2-(aq) → Al(NO3)3(aq) + LiC2H3O2(s) C) 3 Li+(aq) + (C2H3O2)33-(aq) → Li3(C2H3O2)3 (s) D) Li+(aq) + C2H3O2-(aq) → LiC2H3O2(s) E) No reaction occurs.

113) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of 113) Na2CO3 and HCl are mixed. A) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g) B) 2 H+(aq) + CO32-(aq) → H2CO3(s) C) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq) D) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq) E) No reaction occurs.

114) Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of 114) MgSO3 and HI are mixed. A) 2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g) B) 2 H+(aq) + SO32-(aq) + Mg2+(aq) + 2 I-(aq)→ H2SO3(s) + MgI2(aq) C) Mg2+(aq) + 2 I-(aq) → MgI2(s) D) 2 H+(aq) + SO32-(aq) → H2SO3(s) E) No reaction occurs.

115) Identify the spectator ions in the following molecular equation. 115)

KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)

A) Ag+ & Br- B) Ag+ & NO3- C) K+ & Br- D) K+ & NO3- E) There are no spectator ions in this reaction.

116) Choose the statement below that is TRUE. 116) A) The term ʺweak electrolyteʺ means that the substance is inert. B) A strong acid solution consists of only partially ionized acid molecules. C) The term ʺstrong electrolyteʺ means that the substance is extremely reactive. D) A weak acid solution consists of mostly nonionized acid molecules. E) A molecular compound that does not ionize in solution is considered a strong electrolyte.

17 117) Which of the following is an acid base reaction? 117) A) MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s) B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq) C) C(s) + O2(g) → CO2(g) D) Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq) E) None of the above are acid base reactions.

118) Which of the following is a precipitation reaction? 118) A) 2 LiI(aq) + Hg2(NO3)2(aq) → Hg2I2(s) + 2 LiNO3(aq) B) NaCl(aq) + LiI(aq) → NaI(aq) + LiCl(aq) C) HCl(aq) + KOH(aq) → KCl(aq) + H2O(l) D) Zn(s) + 2 AgNO3(aq) → 2 Ag(s) + Zn(NO3)2(aq) E) None of the above are precipitation reactions.

119) Which of the following is a gas-evolution reaction? 119) A) 2 C2H6(l) + 7 O2(g) → 4 CO2(g) + 6 H2O(g) B) LiCl(aq) + NaNO3(aq) → LiNO3(aq) + NaCl(g) C) NH4Cl(aq) + KOH(aq) → KCl(aq) + NH3(g) + H2O(l) D) 2 H2(g) + O2(g) → 2 H2O(g) E) None of the above are gas-evolution reactions.

120) Which of the following is an oxidation-reduction reaction? 120) A) NaI(aq) + AgNO3(aq) → AgI(s) + NaNO3(aq) B) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) C) HCl(aq) + LiOH(aq) → LiCl(aq) + H2O(l) D) Pb(C2H3O2)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2 NaC2H3O2(aq) E) All of the above are oxidation-reduction reactions.

121) Determine the oxidation state of P in PO33-. 121) A) 0 B) +6 C) +2 D) +3 E) -3

122) Determine the oxidation state of Sn in Sn(SO4)2. 122) A) +4 B) +2 C) -2D)+6E)0

123) What element is undergoing oxidation (if any) in the following reaction? 123)

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)

A) H B) C C) O D) both C and H E) None of the elements is undergoing oxidation.

18 124) What element is undergoing reduction (if any) in the following reaction? 124)

Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)

A) Ag B) Zn C) O D) N E) This is not an oxidation-reduction reaction.

125) Determine the reducing agent in the following reaction. 125)

2 Li(s) + Fe(C2H3O2)2(aq) → 2 LiC2H3O2(aq) + Fe(s)

A) Fe B) Li C) C D) O E) H

126) Determine the oxidizing agent in the following reaction. 126)

Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s)

A) Cl B) O C) Ni D) Ag E) This is not an oxidation-reduction reaction.

127) The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M 127) LiOH solution. What is the concentration of the H2SO4 solution (in M)? A) 0.10 M B) 0.25 M C) 0.20 M D) 0.36 M E) 0.40 M

128) The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M 128) KOH solution. What is the concentration of the H3PO4 solution (in M)? A) 0.138 M B) 1.03 M C) 0.343 M D) 0.0461 M E) 0.114 M

129) Chose the reaction that represents the combustion of C6H12O2. 129) A) C6H12O2(l) + 9 O2(g) → 6 CO2(g) + 6 H2O(g) B) C6H12O2(l) → 6 C(s) + 6 H2(g) + O2(g) C) Mg(s) + C6H12O2(l) → MgC6H12O2(aq) D) 6 C(s) + 6 H2(g) + O2(g) → C6H12O2(l) E) None of the above represent the combustion of C6H12O2.

130) Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts with 130) 3.41 x 1023 atoms of Fe according to the following reaction.

2 HCl(aq) + Fe(s) → H2(g) + FeCl2(aq)

A) 1.51 g B) 1.33 g C) 0.187 g D) 0.374 g E) 1.14 g

19 131) According to the following reaction, what amount of Al2O3 remains when 20.00 g of Al2O3 and 131) 2.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 = 150.17 g/mol, H2O = 18.02 g/mol.

Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g)

A) 14.00 g B) 19.78 g C) 28.33 g D) 11.67 g E) 8.33 g

SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question.

132) Describe the difference between complete ionic and net ionic equations. 132)

133) Explain the difference between a strong and weak electrolyte. Give an example of each. 133)

134) What causes a precipitation reaction to occur between two soluble compounds? 134)

135) How can you tell if a reaction is an oxidation-reduction reaction? 135)

136) How would the concentration change if a1.0 L flask of 1.0 M NaCl were left uncapped on a 136) laboratory bench for several days. Why?

MATCHING. Choose the item in column 2 that best matches each item in column 1.

Match the following.

137) CH (g) + 2 O (g) → CO (g) + 2 A) Oxidation Reduction 4 2 2 137) H2O(g) B) Combustion 138) H SO (aq) + 2 LiOH(aq) → 2 H O(l) + 2 4 2 138) C) Acid Base Li2SO4(aq)

D) Gas Evolution 139) Mg(s) + Cu(NO ) (aq) → 3 2 139) Mg(NO3)2(aq) + Cu(s) E) Precipitation

140) HCl(aq) + (NH ) S(aq) → H S(g) + 4 2 2 140) 2NH4Cl(aq)

141) NaCl(aq) + AgNO (aq) → AgCl(s) + 3 141) NaNO3(aq)

20 Answer Key Testname: UNTITLED3

1) E 2) D 3) B 4) D 5) A 6) E 7) B 8) A 9) B 10) A 11) E 12) D 13) B 14) B 15) B 16) A 17) B 18) A 19) B 20) E 21) E 22) B 23) B 24) C 25) D 26) A 27) C 28) D 29) D 30) D 31) B 32) D 33) A 34) E 35) E 36) C 37) C 38) E 39) A 40) A 41) B 42) A 43) C 44) A 45) C 46) C 47) A 48) C 49) E 50) A 21 Answer Key Testname: UNTITLED3

51) A 52) C 53) E 54) C 55) E 56) A 57) E 58) J 59) C 60) D 61) An ionic compound is formed between a metal and a nonmetal (or polyatomic ions) and is held together through the attraction of opposite charges. An example is NaCl. A molecular compound is usually formed between 2 or more nonmetals and is held together through the sharing of electrons between atoms. An example is CO2. 62) An ionic compound that contains a polyatomic ion, such as NaNO3, has both ionic bonds (that hold the sodium and nitrate ions together) as well as covalent bonds (that hold the atoms within the nitrate ion together). 63) The charges on the ions dictate how many must be present to form a neutral unit. Molecular compounds do not have such constraints and therefore must use prefixes to denote the number of atoms present. 64) A molecular formula is the exact number of each type of atom necessary to build a specific molecule. An empirical formula is simply the smallest whole number ratio between atoms in a compound. For example, C2H4 is the molecular formula for ethene. The empirical formula for ethene is CH2, the smallest whole number ratio between the elements. 65) No, since nitrogen and oxygen are both nonmetals, they combine by sharing electrons. This can be done in multiple different ways. Some possible compounds are N2O, N2O3, NO2.

66) C 67) B 68) A 69) C 70) C 71) E 72) B 73) A 74) E 75) B 76) E 77) E 78) E 79) D 80) E 81) B 82) C 83) C 84) A 85) A 86) A 87) A 88) D 89) B 90) B 22 Answer Key Testname: UNTITLED3

91) A 92) B 93) D 94) E 95) A 96) D 97) E 98) D 99) C 100) B 101) D 102) B 103) B 104) D 105) A 106) C 107) A 108) E 109) D 110) A 111) A 112) E 113) A 114) A 115) D 116) D 117) B 118) A 119) C 120) B 121) D 122) A 123) B 124) A 125) B 126) D 127) C 128) E 129) A 130) C 131) D 132) A complete ionic equation shows all of the substances present in the reaction mixture. A net ionic equation only shows the substances that are participating in the reaction. The spectator ions are absent in the net ionic equation. 133) A strong electrolyte is either an ionic compound that is soluble in water or a molecular compound that ionizes completely in water. Possible examples are NaCl or HCl. A weak electrolyte is only slightly soluble or does not ionize to any great extent in water. Possible examples are AgCl or HC2H3O2. 134) A precipitate, or insoluble compound, forms from a pair of the ions present. This ʺtrapsʺ some of the ions into a newly formed compound causing reaction. 135) At least one species is losing electrons while at least one other species is gaining electrons. This can be evaluated by assigning oxidation numbers to each element present and looking to see if these change from reactant to product. 23 Answer Key Testname: UNTITLED3

136) The concentration would slowly increase as water from the solution evaporated. This is because the amount of NaCl in the flask would remain constant while the amount of water decreases. 137) B 138) C 139) A 140) D 141) E

24