Models Of Chemical Bonding Chapter 9 Exam Questions

Chapter 9 Test Bank

Models of Chemical Bonding

1. Which of the following contains ionic bonding?

A. CO

B. SrF₂

C. Al

D. OCl₂

E. HCl

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

2. Which of the following is an ionic compound?

A. H₂S

B. NH₃

C. I₂

D. KI

E. CCl₄

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

3. Which of the following is a covalent compound?

A. Na₂O

B. CaCl₂

C. Cl₂O

D. CsCl

E. Al₂O₃

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

4. Which of the following contains covalent bonds?

A. BaO

B. IBr

C. Mg

D. LiBr

E. Cu

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

5. In which of these substances are the atoms held together by polar covalent bonding?

A. SrCl₂

B. CsCl

C. ClF

D. TiF₂

E. S₈

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

6. In which of these substances are the atoms held together by metallic bonding?

A. CO₂

B. Si

C. Br₂

D. S₈

E. Cr

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Metallic Bonding

Topic: Chemical Bonding

7. For which of the following elements (in their normal, stable, forms) would it be correct to describe the bonding as involving “electron pooling”?

A. hydrogen

B. helium

C. sulfur

D. iodine

E. aluminum

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Metallic Bonding

Topic: Chemical Bonding

8. Select the element whose Lewis symbol is correct.

A.

B.

C.

D.

E.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Lewis Dot Symbols

Topic: Chemical Bonding

9. Select the element whose Lewis symbol is correct.

A.

B.

C.

D.

E.

Bloom's: 3. Apply

Difficulty: Easy

Gradable: automatic

Subtopic: Lewis Dot Symbols

Topic: Chemical Bonding

10. Select the correct formula for a compound formed from calcium and chlorine.

A. CaCl

B. CaCl₂

C. Ca₂Cl

D. Ca₂Cl₂

E. CaCl₃

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

11. Select the correct formula for a compound formed from barium and nitrogen.

A. BaN

B. BaN₂

C. Ba₂N₃

D. Ba₂N

E. Ba₃N₂

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

12. The diameter of a chloride ion is 362 pm, and the diameter of a potassium ion is 276 pm. What is the distance between the nuclei of adjacent chloride and potassium ions in solid potassium chloride?

A. 1276 pm

B. 638 pm

C. 319 pm

D. 181 pm

E. 138 pm

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

13. The lattice energy for ionic crystals increases as the charge on the ions _____________ and the size of the ions __________________.

A. increases; increases

B. increases; decreases

C. decreases; increases

D. decreases; decreases

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

14. Select the compound with the highest lattice energy.

A. CaS(s)

B. BaO(s)

C. NaI(s)

D. LiBr(s)

E. MgO(s)

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

15. Select the compound with the lowest (i.e., least negative) lattice energy.

A. CsBr(s)

B. NaCl(s)

C. SrO(s)

D. CaO(s)

E. KBr(s)

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

16. Calculate the lattice energy of magnesium sulfide from the data given below.

Mg(s) → Mg(g) ΔH° = 148 kJ/mol

Mg(g) → Mg²+(g) + 2e– ΔH° = 2186 kJ/mol

S₈(s) → 8S(g) ΔH° = 2232 kJ/mol

S(g) + 2e– → S2–(g) ΔH° = 450 kJ/mol

8Mg(s) + S₈(s) → 8MgS(s) ΔH° = –2744 kJ/mol

Mg²+(g) + S²–(g) → MgS(s) ΔH°lattice = ?

A. –3406 kJ/mol

B. –2720. kJ/mol

C. 2720. kJ/mol

D. 3406 kJ/mol

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

17. The lattice energy of CaF₂ is the energy change for which one, if any, of the following processes?

A. Ca²⁺(s) + 2F^–(g) → CaF₂(g)

B. CaF₂(g) → CaF₂(s)

C. Ca(g) + 2F(g) → CaF₂(s)

D. CaF₂(aq) → CaF₂(s)

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

18. The lattice energy of MgCl² is the energy change for which one of the following processes?

A. Mg(s) + Cl₂(g) → MgCl₂(s)

B. Mg(g) + 2Cl(g) → MgCl₂(s)

C. Mg²⁺(s) + 2Cl^–(g) → MgCl₂(g)

D. Mg²⁺(g) + 2Cl^–(g) → MgCl₂(s)

E. MgCl₂(aq) → MgCl₂(s)

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

19. A Born-Haber cycle applied to the formation reaction of an ionic solid

A. is normally used to calculate ionization energy.

B. is normally used to calculate electron affinity.

C. is normally used to calculate bond energy.

D. is normally used to determine the overall enthalpy change.

E. is an application of Hess's Law.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

20. Analysis of an unknown substance showed that it has a high boiling point and is brittle. It is an insulator as a solid but conducts electricity when melted. Which of the following substances would have those characteristics?

A. HCl

B. Al

C. KBr

D. SiF₄

E. I₂

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

21. Which one of the following properties is least characteristic of typical ionic compounds?

A. high melting point

B. high boiling point

C. brittleness

D. poor electrical conductor when solid

E. poor electrical conductor when molten

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

22. When two atoms form a covalently-bonded diatomic molecule, the distance between the nuclei

at which the potential energy is at a minimum is called

A. the bond energy.

B. the bond length.

C. the molecular diameter.

D. the covalent radius.

E. the covalent diameter.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

23. Arrange the following bonds in order of increasing bond strength.

A. C–I < C–Br < C–Cl < C–F

B. C–F < C–Cl < C–Br < C–I

C. C–Br < C–I < C–Cl < C–F

D. C–I < C–Br < C–F< C–Cl

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

24. Select the strongest bond in the following group.

A. C–S

B. C–O

C. C=C

D. C≡N

E. C–F

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

25. Which one of the following properties is least characteristic of substances composed of small, covalently-bonded molecules?

A. low melting point

B. low boiling point

C. weak bonds

D. poor electrical conductor when solid

E. poor electrical conductor when molten

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

26. Quartz (SiO₂) is a solid with a melting point of 1550 °C. The bonding in quartz is best described as

A. lattice energy.

B. network attractions.

C. ionic bonding.

D. covalent bonding.

E. metallic bonding.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Easy

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

27. Nitrogen and hydrogen combine to form ammonia in the Haber process. Calculate (in kJ) the standard enthalpy change ΔH° for the reaction written below, using the bond energies given.

N₂(g) + 3H₂(g) → 2NH₃(g)

Bond: N≡N H–H N–H

Bond energy(kJ/mol): 945 432 391

A. –969 kJ

B. –204 kJ

C. –105 kJ

D. 204 kJ

E. 595 kJ

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Bond Energies and ΔHorxn

Topic: Chemical Bonding

28. Hydrogenation of double and triple bonds is an important industrial process. Calculate (in kJ) the standard enthalpy change ΔH° for the hydrogenation of ethyne (acetylene) to ethane.

H–C≡C–H(g) + 2H₂(g) → H₃C–CH₃(g)

Bond: C–C C≡C C–H H–H

Bond energy (kJ/mol): 347 839 413 432

A. –296 kJ

B. –51 kJ

C. 51 kJ

D. 296 kJ

E. 381 kJ

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Bond Energies and ΔHorxn

Topic: Chemical Bonding

29. Acetone can be easily converted to isopropyl alcohol by addition of hydrogen to the carbon–oxygen double bond. Calculate the enthalpy of reaction using the bond energies given.

Bond: C=O H–H C–H O–H C–C C–O

Bond energy (kJ/mol): 745 432 413 467 347 358

A. –484 kJ

B. –366 kJ

C. –61 kJ

D. +61 kJ

E. +366 kJ

Bloom's: 3. Apply

Difficulty: Hard

Gradable: automatic

Subtopic: Bond Energies and ΔHorxn

Topic: Chemical Bonding

30. Using the bond energies provided below, calculate ΔH° for the reaction

CH₄(g) + 4Cl₂(g) → CCl₄(g) + 4HCl(g)

Bond energies: C–H = 413 kJ/mol, Cl–Cl = 243 kJ/mol, C–Cl = 339 kJ/mol, H–Cl = 427 kJ/mol

A. 1422 kJ

B. 440 kJ

C. 110 kJ

D. –110 kJ

E. – 440 kJ

Accessibility: Keyboard Navigation

Bloom's: 3. Apply

Difficulty: Medium

Gradable: automatic

Subtopic: Bond Energies and ΔHorxn

Topic: Chemical Bonding

31. Combustion of a fat will release more energy than combustion of an equal mass of carbohydrate because

A. fats contain more bonds to oxygen than carbohydrates.

B. fats contain fewer bonds to oxygen than carbohydrates.

C. the total energy of the carbon-carbon and carbon-hydrogen bonds in fats is greater than the energy content of the carbon-oxygen and oxygen-hydrogen bonds in the reaction products (carbon dioxide and water).

D. the total energy of the carbon-carbon and carbon-hydrogen bonds in fats is greater than the energy content of the bonds in carbohydrates.

E. fats have higher molar masses than carbohydrates.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Bond Energies and ΔHorxn

Topic: Chemical Bonding

32. When one mole of each of the following liquids is burned, which will produce the most heat energy?

A. C₆H₁₄

B. C₅H₁₂

C. C₆H₁₄O

D. C₆H₁₂O

E. C₆H₁₀O₃

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Bond Energies and ΔHorxn

Topic: Chemical Bonding

33. Electronegativity is a measure of

A. the energy needed to remove an electron from an atom.

B. the energy released when an electron is added to an atom.

C. the magnitude of the negative charge on an electron.

D. the attraction by an atom for electrons in a chemical bond.

E. the magnitude of the negative charge on a molecule.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Electronegativity

Topic: Chemical Bonding

34. Which of the following elements is the most electronegative?

A. S

B. Ru

C. Si

D. Te

E. Cs

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Electronegativity

Topic: Chemical Bonding

35. Which of the following elements is the least electronegative?

A. Si

B. Se

C. S

D. Sc

E. Sr

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Electronegativity

Topic: Chemical Bonding

36. Which of the following elements is the most electronegative?

A. Ne

B. Rb

C. P

D. I

E. Cl

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Electronegativity

Topic: Chemical Bonding

37. Arrange aluminum, boron, nitrogen, and phosphorous in order of increasing electronegativity.

A. Al<B<P<N

B. B<Al<N<P

C. Al<N<P<B

D. N<P<B<Al

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Electronegativity

Topic: Chemical Bonding

38. Arrange calcium, rubidium, sulfur, and arsenic in order of decreasing electronegativity.

A. S > As > Rb > Ca

B. S > As > Ca > Rb

C. As > S > Rb > Ca

D. As > S > Ca > Rb

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Electronegativity

Topic: Chemical Bonding

39. Arrange oxygen, sulfur, calcium, rubidium, and potassium in order of decreasing electronegativity.

A. O > S > Ca > K > Rb

B. O > S > Ca > Rb > K

C. O > S > Rb > K > Ca

D. O > S > Rb > Ca > K

E. None of these choices are correct.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Electronegativity

Topic: Chemical Bonding

40. Based on electronegativity trends in the periodic table, predict which of the following compounds will have the greatest % ionic character in its bonds.

A. H₂O

B. LiI

C. CaO

D. RbF

E. HCl

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Bond Polarity

Topic: Chemical Bonding

41. Which of the following period 3 chlorides would be expected to have the highest melting point?

A. MgCl₂

B. AlCl₃

C. SiCl₄

D. PCl₃

E. SCl₂

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

42. Select the most polar bond amongst the following.

A. C–O

B. Si–F

C. Cl–F

D. C–F

E. C–I

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Bond Polarity

Topic: Chemical Bonding

43. Which of the following compounds displays the greatest ionic character in its bonds?

A. NO₂

B. CO₂

C. H₂O

D. HF

E. NH₃

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Bond Polarity

Topic: Chemical Bonding

44. Analysis of an unknown substance showed that it has a moderate melting point and is a good conductor of heat and electricity in the solid phase. Which of the following substances would have those characteristics?

A. NaCl

B. Si

C. CCl₄

D. I₂

E. Ga

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Metallic Bonding

Topic: Chemical Bonding

45. Which one of the following properties is least characteristic of typical metals?

A. moderately high melting point

B. high boiling point

C. brittleness

D. good electrical conductor when solid

E. good electrical conductor when molten

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Metallic Bonding

Topic: Chemical Bonding

46. The melting points of metals are only moderately high because

A. metallic bonding is weak.

B. metals have fewer bonding electrons than nonmetals.

C. metals also have relatively low boiling points.

D. the melting process does not break the metallic bonds.

E. metals prefer to be bonded to nonmetals.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Metallic Bonding

Topic: Chemical Bonding

47. The majority of elements are good electrical conductors when in solid form.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Metallic Bonding

Topic: Chemical Bonding

48. A single covalent bond consists of a single delocalized electron pair.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

49. The lattice energy is the energy released when separated ions in the gas phase combine to form ionic molecules in the gas phase.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

50. The lattice energy of large ions is greater in magnitude than that of small ions of the same charge.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

51. The electrostatic energy of two charged particles is inversely proportional to the square of the distance between them.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

52. The electrostatic energy of two charged particles is inversely proportional to the distance between them.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

53. In covalent bond formation, the potential energy reaches a maximum when the internuclear distance is equal to the bond length.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

54. Bond energy increases as bond order increases, for bonding between a given pair of atoms.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

55. Covalently bonded substances do not necessarily exist as separate molecules.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Covalent Bonding

Topic: Chemical Bonding

56. The more C–O and O–H bonds there are in a substance, the greater will be the amount of heat released when a fixed mass of the substance is burned.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Bond Energies and ΔHo

Topic: Chemical Bonding

57. The stronger the bonds in a fuel, the more energy it will yield.

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Bond Energies and ΔHo

Topic: Chemical Bonding

58. Electronegativities on Pauling's scale are calculated from ionization energies and electron affinities.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Electronegativity

Topic: Chemical Bonding

59. No real bonds are 100% ionic in character.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Easy

Gradable: automatic

Subtopic: Bond Polarity

Topic: Chemical Bonding

60. As a measure of the strength of metallic bonding, the boiling point of a metal is a better indicator than its melting point.

Accessibility: Keyboard Navigation

Bloom's: 1. Remember

Difficulty: Medium

Gradable: automatic

Subtopic: Metallic Bonding

Topic: Chemical Bonding

61. In which of the following processes does the enthalpy change (ΔH) directly represent the magnitude of the lattice energy of KCl(s)?

A. Cl₂(g) + 2K(s) → 2KC (s)

B. KCl(s) → K⁺(aq) + Cl^- (aq)

C. KCl(s) → K⁺(g) + Cl^-(g)

D. KCl(s) → K(s) + Cl^-(g)

E. KCl(s) → K(s) + Cl(g)

Accessibility: Keyboard Navigation

Bloom's: 2. Understand

Difficulty: Medium

Gradable: automatic

Subtopic: Ionic Bonding and Lattice Energy

Topic: Chemical Bonding

Category # of Questions

Accessibility: Keyboard Navigation 58

Bloom's: 1. Remember 17

Bloom's: 2. Understand 35

Bloom's: 3. Apply 9

Difficulty: Easy 16

Difficulty: Hard 4

Difficulty: Medium 35

Difficulty: Easy 3

Difficulty: Medium 3

Gradable: automatic 61

Subtopic: Bond Energies and ΔHo 2

Subtopic: Bond Energies and ΔHorxn 6

Subtopic: Bond Polarity 4

Subtopic: Covalent Bonding 12

Subtopic: Electronegativity 8

Subtopic: Ionic Bonding and Lattice Energy 20

Subtopic: Lewis Dot Symbols 2

Subtopic: Metallic Bonding 7

Topic: Chemical Bonding 6

Topic: Chemical Bonding 55