Inorganic Nomenclature – Ch6 | Test Bank – 15e

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Package Title: Hein Test Bank

Course Title: Hein 14e

Chapter Number: 6

Question type: Multiple Choice

1) Which of the following exists in its natural state as a diatomic?

a) iron

b) bromine

c) boron

d) zirconium

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

2) Which of the following exist in its natural state as a diatomic?

a) helium

b) radium

c) iodine

d) boron

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

3) Which of the following does not exist in its natural state as a diatomic?

a) sodium

b) nitrogen

c) oxygen

d) chlorine

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

4) Which of the following is correct representation of the elemental sulfur?

a) S

b) S₂

c) S₄

d) S₈

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: 6.2

5) Which of the following is correct representation of the elemental selenium?

a) Se

b) Se₂

c) Se₄

d) Se₈

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: 6.2

6) Which is the correct name for Mg ⁺²?

a) magnesium

b) magnesium ion

c) manganide

d) magneside

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

7) What is the correct name for the Na ⁺ ion?

a) sodium(I)

b) sodium ion

c) sodium

d) sodide

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

8) What is the correct name for N^3-?

a) nitrogen(III) ion

b) nitrogen ion

c) nitride ion

d) Iodine (III)nitride(III) ion

Difficulty: medium

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

9) A silver atom is converted to a silver ion when the atom

a) gains one electron.

b) gains two electrons.

c) loses one electron.

d) loses two electrons.

Difficulty: medium

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

10) A potassium atom is converted to a potassium ion when the atom

a) gains one electron.

b) gains two electrons.

c) loses one electron.

d) loses two electrons.

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

11) A copper(II) ion forms when a copper atom

a) gains one electron.

b) gains two electrons.

c) loses one electron.

d) loses two electrons.

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

12) A manganese(III) ion forms when

a) a manganese ion gains three electrons.

b) a manganese ion loses three electrons.

c) a manganese atom gains three electrons.

d) a manganese atom loses three electrons.

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

13) A chloride ion forms when a chlorine atom

a) gains one electron.

b) gains two electrons.

c) loses one electron.

d) loses two electrons.

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

14) A sulfide ion forms when an sulfur atom

a) gains one electron.

b) gains two electrons.

c) loses one electron.

d) loses two electrons.

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

15) Which of the following is a cation?

a) chloride ion

b) chromate ion

c) nitrite ion

d) barium ion

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

16) Which of the following represents a tin(II) ion ?

a) Ti²⁺

b) Te²⁺

c) Sn²⁺

d) Tl²⁺

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

17) Which of the following is a cation?

a) vanadium(II) ion

b) fluoride ion

c) hydroxide ion

d) hydrogen carbonate ion

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Sections 6.2 and 6.5

18) Which of the following is a cation?

a) permanganate ion

b) oxide ion

c) copper(I) ion

d) bromide ion

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.2 and 6.5

19) Which of the following is a transition metal ion?

a) An arsenate ion

b) An ammonium ion

c) A chlorate ion

d) A zinc ion

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

20) CrO₄^2- is called a

a) dichromate ion.

b) chromium ion.

c) chromate ion.

d) chromium oxide ion.

Difficulty: easy

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: 6.5

21) Which of the following is an anion?

a) strontium ion

b) manganese(II) ion

c) sulfide ion

d) zinc ion

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

22) What is the formula for the bromite ion?

a) BrM^–

b) BrO^–

c) BrO₂^–

d) BrO₃^–

Difficulty: easy

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

23) The name of the ion OH^- ends with?

a) ide

b) ite

c) ate

d) None of the above

Difficulty: easy

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

24) Which of the following is an anion?

a) nitrate ion

b) potassium ion

c) magnesium ion

d) ammonium ion

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.2 and 6.5

25) Metals belonging to Group 3A(13) form ions with a charge of

a) +1.

b) +2.

c) +3.

d) –5.

Difficulty: medium

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

26) The alkaline earth metals belonging to Group 2A form ions with a charge of

a) +1.

b) +2.

c) –1.

d) –2.

Difficulty: medium

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

27) The elements in group 6A(16) form ions with a charge of

a) +6.

b) +2.

c) –6.

d) –2.

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

28) The halogens form ions with a charge of

a) +7.

b) +1.

c) –7.

d) –1.

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

29) All chemical compounds must have a net charge of

a) 0

b) +1

c) +2

d) The charges of compounds can vary.

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

30) Which is the correct formula of potassium chlorate?

a) PCl

b) PClO₂

c) KClO₂

d) KClO₃

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

31) Metals combine with non-metals to form______compounds?

a) ionic

b) molecular

c) metallic

d) non-metallic

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

32) What is the formula of magnesium iodide?

a) MgI

b) MgI₂

c) Mg₂I

d) Mg₂I₂

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

33) What is the formula of barium oxide?

a) BaO

b) BaO₂

c) Ba₂O

d) Ba₂O₃

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

34) What is the formula of Sodium phosphite?

a) Na₃P

b) NaPO₃

c) Na(PO₃)₃

d) Na₃PO₃

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

35) What is the formula of aluminum sulfide?

a) AlSO₄

b) Al₂S₃

c) Al(SO₃)₃

d) Al₂(SO₄)₃

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

36) What is the formula of iron(III) oxide?

a) FeO

b) Fe₃O₂

c) Fe₂O₃

d) Fe₃O

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

37) PbO₂ is known as

a) lead oxide.

b) lead(II) oxide.

c) lead dioxide.

d) lead(IV) oxide.

Difficulty: medium

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

38) What is the formula of magnesium sulfate?

a) MgS

b) MgSO₃

c) MgSO₄

d) MgSO

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

39) What is the formula of calcium nitrate?

a) Ca₃N₂

b) Ca(NO₂)₃

c) Ca(NO₃)₂

d) Ca(NO₂)₂

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

40) Which is the formula of iron(II) nitrate?

a) Fe₃NO₃

b) FeNO₃

c) Fe(NO₃)₂

d) Fe₂NO₃

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

41) Which is the formula of aluminum chromate?

a) Al₂CrO₄

b) Al₃(CrO₄)₂

c) Al(CrO₄)₃

d) Al₂(CrO₄)₃

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

42) What is the formula of chromium(III) hydrogensulfate?

a) CrHSO₄

b) HCrSO₄

c) Cr(HSO₄)₃

d) Cr₃HSO₄

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

43) Which is a binary compound?

a) H₂

b) H₂O

c) CaSO₄

d) KClO

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

44) Which is a binary compound?

a) O₂

b) O₃

c) NaClO₃

d) NaCl

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

45) Which is a binary ionic compound?

a) Cl₂

b) MgSO₄

c) HCl

d) NaCl

Difficulty: medium

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

46) Which is a binary molecular compound?

a) Diphosphorus pentoxide

b) Phosphorous acid

c) Cesium carbonate

d) Ammonium perchlorate

Difficulty: hard

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

47) The total number ions per one aluminum sulfate is

a) 2

b) 3

c) 4

d) 5

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Sections 6.3 and 6.5

48) The total number of ions present in iron(II) carbonate is

a) 1

b) 2

c) 3

d) 4

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Sections 6.3 and 6.5

49) The total number of phosphate ions present in copper(II) phosphate is

a) 4

b) 3

c) 2

d) 1

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Sections 6.3 and 6.5

50) The total number of ions per one sodium phosphate is

a) 2

b) 3

c) 4

d) 5

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Sections 6.3 and 6.5

51) The Na₂O is named

a) sodium(II) oxide

b) disodium oxide

c) sodium(I) oxide

d) sodium oxide

e) Sodium peroxide

Difficulty: medium

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

52) Which of the following is the formula for carbon tetrachloride?

a) CCl

b) CCl₂

c) CCl₃

d) CCl₄

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

53) Which of the following is the formula for phosphorous pentachloride?

a) PCl₅

b) P₅Cl

c) P₂Cl₅

d) P₅Cl₂

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

54) Which of the following is the formula for dinitrogen tetroxide?

a) N₄O₂

b) NO₂

c) N₂O

d) N₂O₄

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

55) Which of the following is the formula for dinitrogen monoxide?

a) N₂O

b) NO₂

c) NO

d) N₂O₄

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

56) H₂S is called

a) sulfuric acid.

b) dihydrogen sulfuric acid.

c) hydrosulfuric acid.

d) hydrogen sulfite.

Difficulty: easy

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

57) Which of the following is the formula for hydrofluoric acid?

a) H₂F

b) HF₂

c) HFO₄

d) HF

Difficulty: easy

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

58) H₂SO₃ is named

a) hydrosulfuric acid.

b) sulfuric acid.

c) hydrosulfurous acid.

d) sulfurous acid.

Difficulty: medium

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

59) HNO₃ is named

a) hydronitric acid.

b) nitric acid.

c) hydronitrous acid.

d) nitrous acid.

Difficulty: medium

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

60) What is the formula for the compound that forms between the elements sodium and bromine?

a) NaBr

b) NaBr₂

c) Na₂Br

d) SBr₂

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

61) What is the formula for the compound that forms between the elements calcium and fluorine?

a) CaF

b) CaF₂

c) Ca₂F

d) Ca₂F₂

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

62) What is the formula for the compound that forms between aluminum and oxygen?

a) AlO

b) AlO₂

c) Al₂O₃

d) Al₃O₂

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

63) What is the formula for the compound that forms between barium and oxygen?

a) BaO

b) Ba₂O

c) BaO₂

d) Ba₂O₃

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

64) Mn₂O₃ is name

a) manganese(III) oxide.

b) manganese(II) oxide.

c) manganese oxide(II).

d) manganese oxide(III).

e) Manganese trioxide

Difficulty: medium

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

65) CuCl₂ is name

a) copper(I) chloride.

b) copper(II) chloride.

c) copper chloride(I).

d) copper chloride(II).

Difficulty: medium

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

66) CO is called

a) monocarbon monoxide

b) carbon oxide

c) carbon monoxide

d) carbon (I) monoxide

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

67) Arsenic pentachloride is named

a) AsCl₅

b) As₅Cl

c) As₂Cl₅

d) AsCl

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

68) What is the formula for calcium permanganate?

a) CaMnO₄

b) Ca(MnO₄)₂

c) KMnO₄

d) Ca₂MnO₄

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: 6.3

69) HNO₂ is named

a) nitric acid.

b) nitrous acid.

c) hydronitric acid.

d) hydronitrous acid.

Difficulty: easy

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

70) Which compound’s name ends in -ite?

a) H₂SO₃

b) CaS

c) MgSO₃

d) HClO

Difficulty: hard

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Learning Objective 3: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Sections 6.3, 6.5, and 6.6

71) Which compound’s name ends in -ide?

a) H₂SO₄

b) HBr

c) KNO₂

d) KNO₃

Difficulty: hard

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Learning Objective 3: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Sections 6.3, 6.5, and 6.6

72) Which compound’s name ends in -ate?

a) KCl

b) KClO

c) KClO₂

d) KClO₃

Difficulty: hard

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Sections 6.3 and 6.5

73) Which of the following is the formula for sodium chlorite?

a) NaClO

b) NaClO₂

c) NaClO₃

d) NaClO₄

Difficulty: medium

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

74) Ca(ClO₃)₂ is named

a) calcium hypochlorite.

b) calcium chlorite.

c) calcium chlorate.

d) calcium perchlorate.

Difficulty: hard

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

75) Ni(HCO₃)₂ is named

a) Nickel (II) bicarbonate.

b) Nickel (I) bicarbonate.

c) Nickel bicarbonate.

d) Nickel (II) carbonate.

Difficulty: hard

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

76) AuH₂PO₄ is named

a) Gadolinium phosphoric acid.

b) Gold hydrogenphosphate.

c) Gadolinium(I) dihydrogenphosphate.

d) Gold(I) dihydrogenphosphate.

Difficulty: hard

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

77) HClO is named

a) hypochlorous acid.

b) chlorous acid.

c) chloric acid.

d) perchloric acid.

Difficulty: medium

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

78) What is the correct name for KMnO₄?

a) potassium(I) manganate.

b) potassium manganate.

c) potassium permanaganate.

d) potassium manganese oxide.

Difficulty: medium

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

79) What is the correct name for K₂Cr₂O₇?

a) dipotassium chromate.

b) potassium dichromate.

c) potassium(II) chromate.

d) dipotassium dichromate.

Difficulty: medium

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

80) The correct formula for periodic acid is

a) HI.

b) HIO.

c) HIO₃.

d) HIO₄.

Difficulty: hard

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

81) All the following ions carry a minus two charge except

a) sulfide.

b) carbonate.

c) sulfate.

d) nitrate.

Difficulty: easy

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

82) Which of the following is the formula for sodium oxalate?

a) NaO

b) NaCO

c) NaC₂O₄

d) Na₂C₂O₄

Difficulty: medium

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

83) Which of the following compounds is most likely to be ionic?

a) BaSO₄

b) SO₃

c) H₂O

d) PCl₃

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

84) Which of the following compounds is most likely to be ionic?

a) HNO₂

b) SbF₅

c) I₂O₄

d) Cd(MnO₄)₂

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

85) V₂O₅ is called

a) divanadium pentaoxide.

b) vanadium(II) oxide.

c) vanadium(V) oxide.

d) divanadium(V) pentaoxide.

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: 6.4

86) Which of the following compounds is most likely to be molecular?

a) CH₄

b) NaCl

c) Ca(NO₃)₂

d) Hg

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

87) Which of the following elements will most likely form ions with a –2 charge?

a) Cr

b) Sr

c) Se

d) N

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

88) The formula of an ionic compound is X₂Y₃. Which pair of atoms is most likely to be X and Y, respectively?

a) Na and S

b) Al and O

c) Ca and P

d) Cr and Cl

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

89) The formula of an ionic compound is XY. Which pair of atoms is most likely to be X and Y, respectively?

a) Na and K

b) Li and S

c) K and N

d) Ca and O

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

90) Based on the following picture, the correct name for this compound is

blue = carbon; yellow = sulfur

a) disulfur carbide.

b) carbon disulfide.

c) carbon(II) sulfide.

d) carbon disulfite.

Difficulty: medium

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

91) Based on the following picture, the correct name for this compound is

red = bromine; green = chlorine

a) monobromine tetrachlorine.

b) bromine pentachloride.

c) bromine(V) chloride.

d) bromine tetrachloride.

Difficulty: medium

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

92) A compound has the formula Na₂Y. Which of the following ions is most likely to be Y?

a)

b)

c)

d)

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Sections 6.3 and 6.5

93) A compound has the formula Sr₃Y₂. Which of the following ions is most likely to be Y?

a)

b)

c)

d)

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Sections 6.3 and 6.5

94) The formula for the hydrogen carbonate anion is . The formula for the hydrogen phosphate anion must be

a)

b)

c)

d)

Difficulty: medium

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Sectin 6.5

95) Which of the following alternatives represents an incorrect name-formula match?

a) potassium dichromate = K₂Cr₂O₇

b) tin(II) hydroxide = Sn(OH)₂

c) barium nitrite = BaNO₂

d) calcium chlorate = Ca(ClO₃)₂

Difficulty: hard

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

96) Which of the following alternatives represents an incorrect name-formula match?

a) calcium chlorate = Ca(ClO₄)₂

b) tin(II) nitrate = Sn(NO₃)₂

c) sodium carbonate = Na₂CO₃

d) silver sulfate = Ag₂SO₄

Difficulty: hard

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

97) Based on the following figure, the name of the compound shown is

green = chlorine; red = oxygen; white = hydrogen

a) hydrogen chlorate.

b) perchloric acid.

c) hydrogen chlorine tetroxide.

d) chlorine trioxygen hydroxide.

Difficulty: hard

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

98) Which ions combine to form the compound PbO?

a) Pb²⁺ and O^–

b) Pb²⁺ and O^2–

c) Pb⁺ and O^2–

d) Pb⁴⁺ and O^2–

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

Question type: True/False

99) Calcium sulfide is CaSO₃.

Difficulty: medium

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

100) ZnBr₂ is a binary compound.

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

101) An ion is a positively or negatively charged atom or group of atoms.

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

102) The formula of copper(II) sulfate is Cu₂S.

Difficulty: medium

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

103) H₂SO₄ is hydrosulfuric acid.

Difficulty: medium

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

104) When a chemical formula is written, the more metallic element is placed first.

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

105) NO₃ ^– is the nitrite ion.

Difficulty: easy

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

106) The formulas of the compounds magnesium oxide, calcium oxide, and barium oxide all contain the same number of ions.

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

107) The prefix “tetra” means four.

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

108) All chemical compounds have a charge of zero.

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

109) Molecular compounds are always binary.

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

110) All ions have a charge of zero.

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

111) Two metals combine together to form an ionic compound.

Difficulty: easy

Learning Objective 1: Discuss the formation, charge, and naming of simple ions

Section Reference 1: Section 6.2

112) The prefix “hepta” means six.

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

113) AgCl is a molecular compound.

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

114) CO is a molecular compound.

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

115) is a molecular compound.

Difficulty: easy

Learning Objective 1: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.5

116) H₂C₂O₄ is an acid.

Difficulty: medium

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

Question type: Essay

117) Translate the following sentences into chemical equations:
a) Silver nitrate and potassium chloride yield potassium nitrate and silver chloride.
b) Zinc chromate and lead(II) nitrate yield zinc nitrate and lead(II) chromate.
c) Copper (II) nitrate and sodium hydroxide yield copper (II) hydroxide and sodium nitrate.

Difficulty: hard

Learning Objective 1: Name binary ionic and nonionic compounds.

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.4 and 6.5

Solution: a) AgNO₃ + KCl → KNO₃ + AgCl; b) ZnCrO₄ + Pb(NO₃)₂ → Zn(NO₃)₂ + PbCrO₄; c) CuNO₃ + NaOH → CuOH + NaNO₃

118) Translate the following sentences into chemical equations:
a) Calcium chloride decomposes to form calcium and chlorine.
b) Carbon and oxygen combine to form carbon dioxide.
c) Magnesium and copper(II) nitrate react to produce copper and magnesium nitrate.

Difficulty: hard

Learning Objective 1: Name binary ionic and nonionic compounds.

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Section 6.4 and 6.5

Solution: a) CaCl₂ → Ca + Cl₂; b) C + O₂ → CO₂; c)Mg + Cu(NO₃)₂ → Cu + Mg(NO₃)₂

119) Write the formulas for the compounds that would form from the combination of these ions:
a) Q ⁺² and Z^-3
b) A ⁺³ and B ^-1
c) X ⁺² and Y ^-2

Difficulty: easy

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

Solution: a) Q₃Z₂; b) AB₃; c) XY

120) Write the formulas for the compounds that would form from the combination of these polyatomic ions:
a) AB ⁺³ and YZ ^–2
b) CD ⁺¹ and WX ^–3
c) EF ⁺² and UV ^–1

Difficulty: medium

Learning Objective 1: Write the chemical formula for an ionic compound from the name of the compound

Section Reference 1: Section 6.3

Solution: a) (AB)₂(YZ)₃; b) (CD)₃WX; c) EF(UV)₂

121) Identify four elements that can form more than one cation.

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

Solution: Many transition elements form more than one cation. List any four of the following. Some examples are: titanium, vanadium, chromium, manganese, iron, cobalt, nickel, copper,

gold, and others.

122) Nitrogen and oxygen combine in a number of ways. In these compounds the oxygen atom always carries a –2 charge. What is the charge of the nitrogen atom in each of the following compounds?
a) NO
b) NO2
c) N2O
d) N2O4

Difficulty: hard

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

Solution: a) +2; b) +4; c) +1; d) +4

123) Name the following compounds formed between nitrogen and oxygen.
a) NO
b) NO2
c) N2O
d) N2O4

Difficulty: easy

Learning Objective 1: Name binary ionic and nonionic compounds.

Section Reference 1: Section 6.4

Solution: a) nitrogen monoxide; b) nitrogen dioxide; c) dinitrogen monoxide; d) dinitrogen tetroxide

124) Write the correct formula for each of the following acids.
a) hydrochloric acid
b) hydrosulfuric acid
c) nitric acid
d) acetic acid
e) sulfuric acid

Difficulty: hard

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

Solution: a) HCl; b) H₂S; c) HNO₃; d) HC₂H₃O₂; e) H₂SO₄

125) Write the correct formula for each of the following acids.
a) nitrous acid
b) sulfurous acid
c) hydrobromic acid
d) phosphoric acid
e) chloric acid

Difficulty: hard

Learning Objective 1: Use the rules to name an acid from its formula and to write the formula for an acid from its name.

Section Reference 1: Section 6.6

Solution: a) HNO₂; b) H₂SO₃; c) HBr; d) H₃PO₄; e) HClO₃

126) Complete the following table:

Difficulty: hard

Learning Objective 1: Name binary ionic and nonionic compounds.

Learning Objective 2: Recognize names, formulas and charges of common polyatomic ions, name compounds containing polyatomic ions and write formulas from names of compounds containing polyatomic ions.

Section Reference 1: Sections 6.4 and 6.5