Chem 1110 Chapter 4 Test Bank

B

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

C

1) Identify an ionic bond. A) Neutrons are pooled. B) Electrons are shared. C) Electrons are transferred. D) Protons are gained. E) Protons are lost.

D

10) Give the name for NaHSO₃. A) monosodium sulfite B) monosodium sulfate C) sodium bisulfate D) sodium bisulfite E) sodium bisulfide

D

11) Give the formula for calcium hydrogen sulfate. A) CaHSO₄ B) Ca₂(HSO₄)₂ C) Ca₂HSO₄ D) Ca(HSO₄)₂

D

12) Give the formula for calcium bisulfate. A) CaHSO₄ B) Ca₂(HSO₄)₂ C) Ca₂HSO₄ D) Ca(HSO₄)₂

C

13) Give the name for KMnO₄. A) potassium manganese tetraoxide B) potassium manganate C) potassium permanganate D) potassium permagnesium E) potassium magnesate

D

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

D

15) Give the correct formula for aluminum sulfate. A) Al₂SO₄ B) Al(SO₄)₃ C) Al₃(SO₄)₂ D) Al₂(SO₄)₃

E

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

C

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

A

18) Give the formula for sulfurous acid. A) H₂SO₃ B) HSO₃ C) H₂SO₄ D) HSO₄

A

19) Give the name for H₂SO₄. A) sulfuric acid B) persulfurous acid C) sulfurous acid D) hyposulfurous acid E) persulfuric acid

A

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

A

2) Which of the following ionic compounds would be expected to have the highest lattice energy? A) CsF B) CsCl C) CsBr D) CsI

A

20) Give the name for HNO₃. A) nitric acid B) nitrous acid C) hydrogen nitrate D) hydrogen nitrite E) hydrogen nitride

E

21) Determine the name for P₄O₁₀. A) phosphorus (IV) oxide B) diphosphorus pentoxide C) phosphorus oxide D) phosphorus (II) oxide E) tetraphosphorus decoxide

A

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

A

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

C

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

A

26) Calculate the molar mass of H₂CO₃. A) 62.03 g/mol B) 29.02 g/mol C) 61.02 g/mol D) 60.01 g/mol E) 74.04 g/mol

C

27) The molecular weight of urea ((NH₂)₂CO), a compound used as a nitrogen fertilizer, is ________ amu (rounded to one decimal place). A) 44.0 B) 43.0 C) 60.1 D) 8.0 E) 32.0

D

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

E

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

A

3) Which of the following ionic compounds would be expected to have the highest lattice energy? A) Li Br B) Na Br C) K Br D) Rb Br

E

30) How many moles of N₂O₄ are in 76.3 g N₂O₄? The molar mass of N₂O₄ is 92.02 g/mol. A) 7.02 × 103 moles B) 1.42 × 10-4 moles C) 1.00 mole D) 1.21 moles E) 0.829 moles

A

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

B

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

A

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

B

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

D

35) How many atoms of oxygen are contained in 47.6 g of Al₂(CO₃)₃? The molar mass of Al₂(CO₃)₃ is 233.99 g/mol. A) 1.23 × 10²³ O atoms B) 2.96 × 10²⁴O atoms C) 2.87 × 10²⁵ O atoms D) 1.10 × 10²⁴ O atoms E) 3.68 × 10²³ O atoms

E

36) How many atoms of carbon are contained in 47.6 g of Al₂(CO₃)₃? The molar mass of Al₂(CO₃)₃ is 233.99 g/mol. A) 1.23 × 10²³ C atoms B) 2.96 × 10²⁴ C atoms C) 2.87 × 10²⁵ C atoms D) 1.10 × 10²⁴ C atoms E) 3.68 × 10²³ C atoms

E

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

B

38) How many SO₃²⁻ ions are contained in 99.6 mg of Na₂SO₃? The molar mass of Na₂SO₃ is 126.05 g/mol. A) 1.52 × 10²⁷ SO₃²⁻ ions B) 4.76 × 10²⁰ SO₃²⁻ ions C) 2.10 × 10²¹ SO₃²⁻ ions D) 1.05 × 10²¹ SO₃²⁻ ions E) 9.52 × 10²⁰ SO₃²⁻ ions

E

39) Determine the volume of hexane that contains 5.33 × 10²² molecules of hexane. The density of hexane is 0.6548 g/mL and its molar mass is 86.17 g/mol. A) 8.59 mL B) 13.5 mL C) 7.40 mL D) 12.4 mL E) 11.6 mL

C

4) Which ionic compound would be expected to have the highest lattice energy? A) Na Cl B) Mg Cl₂ C) Al Cl₃ D) C Cl₄

D

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

B

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

C

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

D

43) Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass. A) NO B) N₂O C) NO₂ D) N₂O₃ E) NO₃

E

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

A

45) Determine the empirical formula for a compound that contains C, H and O. It contains 52.14% C and 34.73% O by mass. A) C₂H₆O B) CHO C) C₄H₁₃O₂ D) CH₄O₃ E) CH₃O

A

46) Determine the molecular formula for a compound that is 70.79% carbon, 8.91% hydrogen, 4.59% nitrogen, and 15.72% oxygen. A) C₁₈H₂₇NO₃ B) C₁₈H₂₇NO₂ C) C₁₇H₂₇NO₃ D) C₁₇H₂₆NO₃

C

47) Determine the molecular formula of a compound that is 49.48% carbon, 5.19% hydrogen, 28.85% nitrogen, and 16.48% oxygen. The molecular weight is 194.19 g/mol. A) C₈H₁₂N₄O₂ B) C₄H₅N₂O C) C₈H₁₀N₄O₂ D) C₈H₁₀N₂O

C

48) Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO2 and 59.38 mg of H₂O. What is the empirical formula for the compound? A) C₅H₂O B) CHO C) C₃H₆O D) C₃H₇O E) C₆HO₃

A

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

B

5) Give the name for SnO. A) tin (I) oxide B) tin (II) oxide C) tin (III) oxide D) tin (IV) oxide

A

5) Identify the compound with the highest magnitude of lattice energy. A) Mg Br₂ B) Ba Br₂ C) Sr Br₂ D) Ca Br₂

B

50) Which of the following compounds is ethanol? A) C₂H₆ B) C₂H₅OH C) CH₃CO₂H D) CH₃CO₃CH₃ E) CH₃OCH₃

A

51) Which of the following compounds is nail polish remover? A) (CH₃)₂C=O B) C₂H₅OH C) CH₃CO₂H D) CH₃CO₂CH₃ E) CH₃OCH₃

A

58) Which of the following statements is TRUE? A) An ionic bond is much stronger than most covalent bonds. B) An ionic bond is formed through the sharing of electrons. C) Ionic compounds at room temperature typically conduct electricity. D) Once dissolved in water, ionic compounds rarely conduct electricity. E) None of the above are true.

B

59) Use Lewis theory to determine the chemical formula for the compound formed between Al and O. A) Al₃O₂ B) Al₂O₃ C) AlO₂ D) Al₂O E) AlO

A

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

B

6) Identify the compound with the lowest magnitude of lattice energy. A) KCl B) KBr C) Mg S D) Ba S

C

60) Which of the following reactions is associated with the lattice energy of Li2O (ΔH°latt)? A) Li₂O(s) → 2 Li⁺(g) + O²⁻(g) B) 2 Li⁺(aq) + O²⁻(aq) → Li₂O(s) C) 2 Li⁺(g) + O²⁻(g) → Li₂O(s) D) Li₂O(s) → 2 Li⁺(aq) + O²⁻(aq) E) 2 Li(s) +(1/2) O₂(g) → Li₂O(s)

D

61) Which of the following reactions is associated with the lattice energy of CaS (ΔH°latt)? A) Ca(s) + S(s) → CaS(s) B) CaS(s) → Ca(s) + S(s) C) Ca²⁺(aq) + S²⁻(aq) → CaS(s) D) Ca²⁺(g) + S²⁻(g) → CaS(s) E) CaS(s) → Ca2⁺(aq) + S²⁻(aq)

E

62) Which of the following reactions is associated with the lattice energy of RbI (ΔH°latt)? A) Rb(s) +(¹/₂) I₂(g) → RbI(s) B) RbI(s) → Rb⁺(g) + I⁻(g) C) RbI(s) → Rb(s) + (¹/₂) I₂(g) D) RbI(s) → Rb⁺(aq) + I⁻(aq) E) Rb⁺(g) + I⁻(g) → RbI(s)

A

63) Place the following in order of decreasing magnitude of lattice energy. K₂O Rb₂S Li₂O A) Li₂O > K₂O > Rb₂S B) Li₂O > Rb₂S > K₂O C) Rb₂S > K₂O > Li₂O D) Rb₂S > Li₂O > K₂O E) K₂O > Li₂O > Rb₂S

B

64) Place the following in order of decreasing magnitude of lattice energy. NaF RbBr KCl A) RbBr > NaF > KCl B) NaF > KCl > RbBr C) KCl > NaF > RbBr D) NaF > RbBr > KCl E) RbBr > KCl > NaF

C

65) Place the following in order of increasing magnitude of lattice energy. CaO MgO SrS A) MgO < CaO < SrS B) SrS < MgO < CaO C) SrS < CaO < MgO D) CaO < MgO < SrS E) CaO < SrS < MgO

D

7) Give the structure for sodium perchlorate. A) NaClO B) NaClO₂ C) NaClO₃ D) NaClO₄

B

7) Place the following in order of increasing magnitude of lattice energy. MgO KI Ba O A) Ba O < MgO < KI B) KI < Ba O < MgO C) MgO < Ba O < KI D) KI < MgO < Ba O E) MgO < KI < Ba O

D

71) When drawing out Lewis structures, how many electrons surround the most stable element? A) 1 B) 3 C) 6 D) 8 E) 10

A

72) The energy associated with formation of a crystalline structure from gaseous ions is know as the A) ionization energy. B) lattice energy. C) precipitation energy. D) electron affinity. E) potential energy.

C

73) What is the formula for zinc chloride? A) ZnC B) Zn₂Cl₂ C) ZnCl₂ D) Zn₂Cl E) ZnCl₃

D

74) What is the formula for calcium phosphate? A) CaP B) Ca₂P₃ C) Ca₂(PO₄)₃ D) Ca₃(PO₄)₂ E) CaPO₄

B

75) What is the chemical name for P₂I₄? A) phosphorous (IV) iodine B) diphosphorous tetraiodine C) phosphorous tetraiodine D) phosphorous (II) iodine E) diphosphorous iodine

A

76) A compound was isolated and found to contain 72.2% magnesium and the rest nitrogen. What is the empirical formula of this compound? A) Mg₃N₂ B) MgN₃ C) MgN D) Mg₂N₃ E) Mg₃N

D

77) Dioxybenzone is a compound found in sunscreen, and only contains carbon, oxygen, and hydrogen. Analysis of the compound found that it contains 4.92% hydrogen and 26.18% oxygen. The molar mass of the compound is 244.25 g/mol. What is the molecular formula? A) C₁₂H₁₀O₃ B) C₁₀H₈O₄ C) C₈H₁₁O₅ D) C₁₄H₁₂O₄ E) C₁₆H₁₀O₆

C

78) What is the empirical formula for a compound that undergoes combustion analysis and produces 12.32g of CO2 and 6.71g of H₂O? A) C₃H₄ B) C₄H₇ C) C₃H₈ D) CH₄ E) C₂H₃

B

79) A single covalent bond contains ________ of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs E) 4 pairs

B

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

C

80) A double covalent bond contains ________ of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs E) 4 pairs

D

81) A triple covalent bond contains ________ of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs E) 4 pairs

A

82) What is the chemical formula for barium oxide? A) BaO B) BaO₂ C) Ba₂O₂ D) Ba₂O E) Ba₂O³

B

83) How many Fe(II) ions are there in 10.0 g of FeSO₄? A) 1.93 × 10⁻²⁵ iron(II) ions B) 3.96 × 10²² iron(II) ions C) 9.15 × 10²⁴ iron(II) ions D) 9.14 × 10²⁶ iron(II) ions

D

83) What is the chemical name for S₂O? A) sulfur dioxide B) sulfur oxide C) disulfur oxide D) disulfur monoxide E) sulfur monoxide

B

84) What is the empirical formula for a species that is composed of sulfur and oxygen with 57.19% of the mass coming from sulfur? A) SO B) S₂O₃ C) S₃O₂ D) SO₂ E) S₂O

E

85) What is the empirical formula for a compound that is composed of 62.04% carbon. 27.55% oxygen, and 10.41% hydrogen? A) CHO B) C₄H₉O₂ C) C₂H₄O₃ D) CH₂O₂ E) C₃H₆O

B

86) What is the empirical formula for a compound that is composed of 53.91% carbon. 35.91% oxygen, and 10.17% hydrogen? A) CHO B) C₄H₉O₂ C) C₂H₄O₃ D) CH₂O₂ E) C₃H₆O

B

87) Calculate the mass percent composition of magnesium in Mg(NO₃)₂. A) 32.6% B) 16.4 % C) 8.92 % D) 27.5 % E) 83.6 %

D

88) Calculate the molar mass of Ba(C₂O₄)₂. A) 128.53 g/mol B) 328.01 g/mol C) 294.77 g/mol D) 225.34 g/mol E) 301.90 g/mol

A

89) An unknown compound contains only carbon and hydrogen. When it undergoes combustion analysis, it produces 3.767 g of CO₂ and 0.616 g of H₂O. What is the empirical formula? A) C₅H₄ B) C₇H₁₄ C) C₂H₃ D) CH E) CH₄

D

9) Give the name for NaHSO₃. A) sodium sulfite B) sodium sulfate C) sodium hydrogen sulfate D) sodium hydrogen sulfite E) sodium sulfide

B

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