Chapter 3 2 In which set do all elements tend to form cations in binary

23) In which set do all elements tend to form cations in binary ionic compounds?

A) K, Ga, O

B) Sr, Ni, Hg

C) N, P, Bi

D) O, Br, I

24) What is the charge on the Sc ions in Sc2O3?

A) 3-

B) 1+

C) 2+

D) 3+

25) Write the formula for the compound formed between potassium and sulfur.

A) KS

B) KS2

C) K2S

D) K2SO3

E) K3S2

26) Write the formula for barium nitrite.

A) Ba3N2

B) BaNO3

C) BaN

D) Ba(NO2)2

E) Ba(NO2)3

27) Write the formula for barium nitride.

A) Ba3N2

B) Ba(NO3)2

C) BaN

D) Ba2N3

E) Ba(NO2)2

28) Give the structure for cesium chlorate.

A) CsClO

B) CsClO2

C) CsClO3

D) CsClO4

29) Give the structure for lithium hypochlorite.

A) LIClO

B) LIClO2

C) LIClO3

D) LIClO4

30) Write the name for Sr3(PO4)2.

A) strontium (III) phosphite

B) strontium (II) phosphite

C) strontium phosphate

D) tristrontium phosphorustetraoxide

E) strontium phosphite

31) Write the name for PbS.

A) lead (I) sulfate

B) lead (I) sulfide

C) lead (II) sulfide

D) lead (II) sulfate

E) lead sulfide

32) Write the name for CoS.

A) cobaltous sulfate

B) cobaltous sulfide

C) cobaltic sulfide

D) cobaltic sulfate

E) cobalt sulfide

33) Give the formula for stannous nitrate

A) Sn(NO2)3

B) Sn(NO3)3

C) Sn(NO3)2

D) Sn(NO2)2

E) Sn2(NO2)

34) The solid compound, K2SO4, contains

A) K+, S6+, and O2- ions.

B) K+ and SO4 -2 ions.

C) K2+ and SO4 -2 ions.

D) K2SO4 molecules.

35) What is the chemical formula for iron(III) sulfate?

A) Fe3S

B) Fe3SO4

C) Fe2S3

D) Fe2(SO4)3

36) Rb2S is named

A) rubidium disulfide.

B) rubidium sulfide.

C) rubidium(II) sulfide.

D) rubidium sulfur.

37) What is the chemical formula for calcium hydroxide?

A) CaH2

B) CaOH

C) CaOH2

D) Ca(OH)2

38) What is the chemical formula for magnesium hydride?

A) MgH2

B) MgOH

C) MgOH2

D) Mg(OH)2

39) The chemical formula for lithium peroxide is

A) LiOH.

B) LiO2.

C) Li2O.

D) Li2O2.

40) The compound, Cu(IO3), is named

A) copper iodate(II).

B) copper(I) iodate.

C) copper(I) iodate(II).

D) copper(II) iodate.

41) The chemical formula for calcium nitride is

A) Ca(NO3)2.

B) Ca(NO2)2.

C) Ca3N2.

D) CaN2.

42) The chemical formula for the sulfite ion is

A) S–.

B) S 2-.

C) SO32-.

D) SO42-.

43) The ion, IO2–, is named

A) iodate ion.

B) iodite ion.

C) iodine dioxide ion.

D) iodine(II) oxide ion.

44) The compound, NO2, is named

A) nitrate.

B) nitrite.

C) nitrogen dioxide.

D) nitrogen (IV) oxide.

45) An aqueous solution of H2S is named

A) hydrosulfuric acid.

B) hydrosulfurous acid.

C) sulfuric acid.

D) sulfurous acid.

46) The chemical formula for nitrous acid is

A) H3N(aq).

B) H NO2(aq).

C) H NO3(aq).

D) H2N2O6(aq).

47) Determine the name for aqueous HF.

A) fluoric acid

B) fluorous acid

C) hydrofluorous acid

D) hydrogen fluorate

E) hydrofluoric acid

48) Determine the name for Cl2O.

A) chlorine oxide

B) dichlorine monoxide

C) chlorine (I) oxide

D) chlorine (II) oxide

E) chlorate

49) Give the name for PBr3.

A) phosphorus tribromide

B) potassium tribromide

C) phosphorus (III) bromide

D) phosphorus (II) bromide

E) phosphorus bromide

50) Determine the name for HBrO3.

A) hydrobromic acid

B) hydrobromus acid

C) bromate acid

D) bromic acid

E) perbromic acid

51) What is the molar mass of nitrogen gas?

A) 14.0 g/mol

B) 28.0 g/mol

C) 6.02 × 1023 g/mol

D) 1.20 × 1023 g/mol

52) What is the mass of a single fluorine molecule, F2?

A) 3.155 × 10-23 g

B) 6.310 × 10-23 g

C) 19.00 g

D) 38.00 g

53) What is the mass of 0.500 mol of dichlorodifluoromethane, CCl2F2?

A) 4.14 × 10-3 g

B) 60.5 g

C) 121 g

D) 242 g

54) How many moles are there in 3.00 g of ethanol, CH3CH2OH?

A) 0.00725 mol

B) 0.0652 mol

C) 15.3 mol

D) 138 mol

55) How many moles of C8H18 contain 9.25 × 1024 molecules of C8H18 ?

A) 65.1 moles C8H18

B) 28.6 moles C8H18

C) 34.9 moles C8H18

D) 46.2 moles C8H18

E) 15.4 moles C8H18

56) What is the mass of 8.50 x 1022 molecules of NH3?

A) 0.00829 g

B) 0.417 g

C) 2.40 g

D) 121 g

57) What is the mass of 3.91 × 1024 molecules of SeO2? The molar mass of SeO2 is 110.96 g/mol.

A) 205 g

B) 294 g

C) 721 g

D) 341 g

E) 685 g

58) What is the molar mass of 1-butene if 5.38 × 1016 molecules of 1-butene weigh 5.00 μg?

A) 56.0 g/mol

B) 178 g/mol

C) 224 g/mol

D) 447 g/mol

59) What mass of carbon dioxide, C O2, contains the same number of molecules as 3.00 g of

trichlorofluoromethane, CCl3F?

A) 0.106 g

B) 0.961 g

C) 1.04 g

D) 9.37 g

60) What mass of phosphorus pentafluoride, PF5, has the same number of fluorine atoms as 25.0 g of

oxygen difluoride, OF2?

A) 0.933 g

B) 10.0 g

C) 23.3 g

D) 146 g

61) How many anions are there in 2.50 g of MgBr2?

A) 8.18 × 1021 anions

B) 1.64 × 1022 anions

C) 4.43 × 1025 anions

D) 8.87 × 1025 anions

62) Which of the following has the greatest mass?

A) 3.88 × 1022 molecules of O2

B) 1.00 g of O2

C) 0.0312 mol of O2

D) All of the above have the same mass.

63) Which of the following has the smallest mass?

A) 3.50 × 1023 molecules of I2

B) 85.0 g of Cl2

C) 2.50 mol of F2

D) 0.050 kg of Br2

64) Give the mass percent of oxygen in C14H19NO2.

A) 13.72%

B) 72.07%

C) 8.21%

D) 6.00%

65) How many moles of NCl3 contain 2.55 × 1024 chlorine atoms?

A) 1.41 moles NCl3

B) 4.23 moles NCl3

C) 12.7 moles NCl3

D) 7.87 moles NCl3

E) 2.82 moles NCl3

66) How many moles of PBr3 contain 3.68 × 1025 bromine atoms?

A) 61.1 moles PBr3

B) 20.4 moles PBr3

C) 16.4 moles PBr3

D) 54.5 moles PBr3

E) 49.1 moles PBr3

67) How many moles of C3H8 contain 4.95 × 1024 hydrogen atoms?

A) 8.22 moles C3H8

B) 6.58 moles C3H8

C) 1.03 moles C3H8

D) 9.73 moles C3H8

E) 3.09 moles C3H8

68) A sample of pure lithium nitrate contains 10.1% lithium by mass. What is the % lithium by mass in a

sample of pure lithium carbonate that has twice the mass of the first sample?

A) 5.05%

B) 10.1%

C) 20.2%

D) 40.4%

69) How many Fe(II) ions are there in 20.0 g of FeSO4?

A) 2.19 × 10-25 iron(II) ions

B) 7.92 × 1022 iron(II) ions

C) 4.57 × 1024 iron(II) ions

D) 1.82 × 1027 iron(II) ions

70) A sample of pure calcium fluoride with a mass of 15.0 g contains 7.70 g of calcium. How much

calcium is contained in 40.0 g of calcium fluoride?

A) 2.27 g

B) 7.70 g

C) 15.0 g

D) 20.5 g

71) Which one of the following contains 39% carbon by mass?

A) C2H2

B) CH4

C) CH3NH2

D) CO2

72) Determine the mass percent (to the hundredths place) of H in sodium bicarbonate (NaHCO3).

73) How many oxygen atoms are there in 7.00 g of sodium dichromate, Na2Cr2O7?

A) 0.187 oxygen atoms

B) 2.30 × 1021 oxygen atoms

C) 1.60 × 1022 oxygen atoms

D) 1.13 × 1023 oxygen atoms

74) How many chloride ions are there in 4.50 mol of aluminum chloride?

A) 3.00 chloride ions

B) 13.5 chloride ions

C) 2.71 × 1024 chloride ions

D) 8.13 × 1024 chloride ions

75) How many cations are there in 10.0 g of sodium phosphate?

A) 3.67 × 1022 cations

B) 1.10 × 1023 cations

C) 9.87 × 1024 cations

D) 2.96 × 1025 cations

76) What is the empirical formula of a compound that is 62.0% C, 10.4% H, and 27.5% O by mass?

A) C3HO

B) C6HO3

C) C6H12O2

D) C5H10O2

E) C3H6O

77) What is the empirical formula of a substance that contains 2.64 g of C, 0.444 g of H, and 3.52 g of

O?

A) C H2O

B) C2H4O2

C) C2H4O3

D) C3H4O4

78) Which one of the following is not an empirical formula?

A) CHO

B) CH2O

C) C2H4O

D) C2H4O2

79) Methane and oxygen react to form carbon dioxide and water. What mass of water is formed if 0.80 g

of methane reacts with 3.2 g of oxygen to produce 2.2 g of carbon dioxide?

A) 1.8 g

B) 2.2 g

C) 3.7 g

D) 4.0 g

80) Combustion analysis of an unknown compound containing only carbon and hydrogen produced

0.2845 g of CO2 and 0.1451 g of H2O. What is the empirical formula of the compound?

A) CH2

B) C2H5

C) C4H10

D) C5H2

81) Combustion analysis of 1.200 g of an unknown compound containing carbon, hydrogen, and oxygen

produced 2.086 g of CO2 and 1.134 g of H2O. What is the empirical formula of the compound?

A) C2H5O

B) C2H5O2

C) C2H10O3

D) C3H8O2

82) A certain alcohol contains only three elements, carbon, hydrogen, and oxygen. Combustion of a

50.00 gram sample of the alcohol produced 95.50 grams of CO2 and 58.70 grams of H2O. What is the

empirical formula of the alcohol?

83) What is the stoichiometric coefficient for oxygen when the following equation is balanced using the

lowest, whole-number coefficients?

_____ C2H6O (l) + _____ O2(g) → _____ CO2(g) + _____ H2O(l)

A) 9

B) 7

C) 5

D) 3

84) Aluminum metal reacts with aqueous iron(II) chloride to form aqueous aluminum chloride and iron

metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced

using the lowest, whole-number stoichiometric coefficients?

A) 1

B) 2

C) 3

D) 4

85) Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid. What is

the coefficient for sulfuric acid when the equation is balanced using the lowest, whole-numbered

coefficients?

A) 1

B) 2

C) 3

D) none of these

86) Identify an amine.

A) CH3CH2OCH2CH3

B) CH3CH2OH

C) CH3CH2NH2

D) CH3CH2CH2CH3

E) CH3COOH

87) Identify an ether.

A) CH3CH2OCH2CH3

B) CH3CH2I

C) CH3CH2NH2

D) CH3CH2CH2CH3

E) CH3COOH

88) Identify a carboxylic acid.

A) CH3CH2SCH2CH3

B) CH3CH2Br

C) CH3CH2NH2

D) CH3CH2CH2CH3

E) CH3COOH

89) Identify a hydrocarbon.

A) CH3CH2SCH2CH3

B) CH3CH2I

C) CH3CH2PH2

D) CH3CH2CH2CH3

E) CH3COOH

90) Which of the following compounds is vinegar?

A) C2H6

B) C2H5Br

C) CH3CO2H

D) CH3CO2CH3

E) CH3NHCH3

Matching Questions

Match the following.

A) H2(g)

B) Ne2(g)

C) Ca(s)

D) H(g)

E) Ca2(s)

F) I2(s)

G) Cl2(g)

H) Cl(g)

I) Ne(g)

J) O(g)

K) I(s)

L) O2(g)

1) oxygen

Diff: 1 Page Ref: 3.4

2) chlorine

Diff: 1 Page Ref: 3.4

3) neon

Diff: 1 Page Ref: 3.4

4) calcium

Diff: 1 Page Ref: 3.4

5) iodine

Diff: 1 Page Ref: 3.4

6) hydrogen

Diff: 1 Page Ref: 3.4

Short Answer Questions

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

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

3) Define empirical formula.

4) What is the structure of the covalent compound formed by nitrogen and oxygen? Is this the only

possibility? Explain.

5) Describe a structural formula

6) Describe the difference between an atomic element and a molecular element.

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

8) Why aren’t prefixes used in naming ionic compounds?

9) Give the name for HNO2.

10) Calculate the mass percent composition of oxygen in Al2(SO4)3.

11) Balance the following equation.

_____ C10H12 + _____ O2 → _____ H2O + _____ CO2

12) Balance the following equation.

_____ C9H20 + _____ O2 → _____ H2O + _____ CO2