CHAPTER 9

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

D

31) Identify the compound with the largest dipole moment in the gas phase. A) Cl2 B) ClF C) HF D) LiF

D

32) Which molecule or compound below contains a polar covalent bond? A) C2H4 B) ZnS C) LiI D) NCl3 E) AgI

D

33) Identify the compound with the highest percent ionic character. A) HF B) IBr C) HCl D) LiF

D

36) Choose the bond below that is least polar. A) P-F B) C-Br C) C-F D) C-I E) C-Cl

D

37) The iodine atom in I2 would be expected to have a A) charge of 1-. B) partial charge δ-. C) partial charge δ+. D) charge of 0.

D

56) Which of the following resonance structures for OCN⁻ will contribute most to the correct structure of OCN⁻? A) O(2 lone pairs)=C=N (2 lone pairs) B) O(1 lone pair) ≡C—N(3 lone pairs) C) O(1 lone pair)=C(2 lp) N(1 lone pair) D) O(3 lone pairs)—C≡N(with 1 lone pair) E) They all contribute equally to the correct structure of OCN⁻.

D

75) Which of the following processes are exothermic? A) the second ionization energy of Mg B) the sublimation of Li C) the breaking the bond of I2 D) the formation of NaBr from its constituent elements in their standard state E) None of the above are exothermic

D

8) Use Lewis theory to determine the chemical formula for the compound formed between Ba and I. A) BaI B) Ba2I3 C) Ba3I2 D) BaI2 E) Ba2I

D

15) Identify the compound with the lowest magnitude of lattice energy. A) KCl B) KBr C) SrO D) BaO

B

22) Of the following elements, which has the highest electronegativity? A) Si B) P C) Ti D) Ge

B

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

B

34) Identify the compound with the smallest percent ionic character. A) HF B) IBr C) HCl D) LiF

B

4) Identify the compound with metallic bonding. A) NaBr B) Na C) H2O D) He E) S

B

42) Which of the following elements can form compounds with an expanded octet? A) O B) Br C) F D) Be E) None of the above can form compounds with an expanded octet.

B

54) Draw the Lewis structure for NO2⁻ including any valid resonance structures. Which of the following statements is TRUE? A) The nitrite ion contains one N—O single bond and one N=O double bond. B) The nitrite ion contains two N—O bonds that are equivalent to 1 bonds. C) The nitrite ion contains two N=O double bonds. D) The nitrite ion contains two N—O single bonds. E) None of the above are true.

B

55) Draw the Lewis structure for CO32- including any valid resonance structures. Which of the following statements is TRUE? A) The CO32- ion contains one C—O single bond and two C=O double bonds. B) The CO32- ion contains two C—O single bonds and one C=O double bond. C) The CO32- ion contains three C—O double bonds. D) The CO32- ion contains two C—O single bonds and one C≡O triple bond. E) None of the above are true.

B

6) Use Lewis theory to determine the chemical formula for the compound formed between Ba and N. A) BaN B) Ba3N2 C) BaN2 D) Ba2N E) Ba2N3

B

77) Which of the following processes are endothermic? A) the reaction associated with the lattice energy of LiCl. B) the reaction associated with the ionization energy of potassium. C) the reaction associated with the heat of formation of CaS. D) the formation of F2 from its elements in their standard states. E) None of the above are endothermic.

B

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

C

10) Use Lewis theory to determine the chemical formula for the compound formed between Li and Br. A) LiBr2 B) Li 2Br C) Li Br D) Li 2Br2

C

13) Which ionic compound would be expected to have the highest lattice energy? A) Rb2O B) SrO C) In2O3 D) CO2

C

21) Identify the number of bonding pairs and lone pairs of electrons in N2. A) 6 bonding pair and 1 lone pair B) 4 bonding pair and 2 lone pairs C) 3 bonding pairs and 2 lone pairs D) 2 bonding pairs and 1 lone pair E) 2 bonding pairs and 3 lone pairs

C

23) Of the following elements, which has the lowest electronegativity? A) Sr B) I C) Ba D) At

C

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

C

27) Identify the shortest bond. A) single covalent bond B) double covalent bond C) triple covalent bond D) all of the above bonds are the same length

C

29) Identify the strongest bond. A) single covalent bond B) double covalent bond C) triple covalent bond D) all of the above bonds are the same strength

C

3) Identify the compound with covalent bonding. A) NaBr B) Na C) H2O D) He E) S

C

30) Identify the number of bonding pairs and lone pairs of electrons in water. A) 1 bonding pair and 1 lone pair B) 1 bonding pair and 2 lone pairs C) 2 bonding pairs and 2 lone pairs D) 2 bonding pairs and 1 lone pair E) 3 bonding pairs and 2 lone pairs

C

31) Which molecule or compound below contains a pure covalent bond? A) Li2CO3 B) SCl6 C) Br2 D) PCl3 E) NaCl

C

34) The electronegativity is 2.1 for H and 1.9 for Pb. Based on these electronegativities PbH4 would be expected to A) be ionic and contain H- ions. B) be ionic and contain H+ ions. C) have polar covalent bonds with a partial negative charges on the H atoms. D) have polar covalent bonds with a partial positive charges on the H atoms.

C

35) Choose the bond below that is most polar. A) H-I B) H-Br C) H-F D) H-Cl E) C-H

C

35) The compound ClF contains A) ionic bonds. B) nonpolar covalent bonds. C) polar covalent bonds with partial negative charges on the F atoms. D) polar covalent bonds with partial negative charges on the Cl atoms.

C

64) Identify the compound with atoms that have an incomplete octet. A) ICl5 B) CO2 C) BF3 D) Cl2 E) CO

C

66) Which compound has the shortest carbon-carbon bond length? A) CH3CH3 B) CH2CH2 C) HCCH D) all bond lengths are the same

C

67) Which compound has the highest carbon-carbon bond strength? A) CH3CH3 B) CH2CH2 C) HCCH D) all bond strengths are the same

C

7) Use Lewis theory to determine the chemical formula for the compound formed between Na and O. A) NaO B) NaO2 C) Na2O D) Na2O3 E) Na3O2

C

76) Which of the following processes are endothermic? A) K⁺(g) + I⁻(g) → KI(s) B) 2 Br(g) → Br2(g) C) Ca(s) → Ca(g) D) 2 Na(s) + O2(g) → Na2O(s) E) None of the above are endothermic.

C

36) The phosphorus atom in PCl3 would be expected to have a A) partial positive (δ+) charge. B) partial negative (δ-) charge. C) 3+ charge. D) 3- charge.

A

41) Which of the following elements can form compounds with an expanded octet? A) Se B) C C) Li D) F E) All of the above elements can form compounds with an expanded octet.

A

5) Identify the substance that conducts electricity. A) NaCl dissolved in water B) solid NaCl C) ethanol D) solid sugar E) sugar dissolved in water.

A

57) Using Lewis structures and formal charge, which of the following ions is most stable? OCN⁻ ONC⁻ NOC⁻ A) OCN⁻ B) ONC⁻ C) NOC⁻ D) None of these ions are stable according to Lewis theory. E) All of these compounds are equally stable according to Lewis theory.

A

65) Which compound has the longest carbon-carbon bond length? A) CH3CH3 B) CH2CH2 C) HCCH D) all bond lengths are the same

A

32) Identify the compound with the smallest dipole moment in the gas phase. A) Cl2 B) ClF C) HF D) LiF

A

11) Which of the following ionic compounds would be expected to have the highest lattice energy? A) LiF B) LiCl C) LiBr D) LiI

A

11) 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.

A

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

A

14) Identify the compound with the highest magnitude of lattice energy. A) MgCl2 B) BaCl2 C) SrCl2 D) CsCl2

A

2) Identify the compound with ionic bonding. A) NaBr B) Na C) H2O D) He E) S

A

28) Identify the weakest bond. A) single covalent bond B) double covalent bond C) triple covalent bond D) all of the above bonds are the same strength

A

1) Which of the following statements is TRUE? A) A covalent bond is formed through the transfer of electrons from one atom to another. B) A pair of electrons involved in a covalent bond are sometimes referred to as "lone pairs." C) It is not possible for two atoms to share more than two electrons. D) Single bonds are shorter than double bonds. E) A covalent bond has a lower potential energy than the two separate atoms.

E

33) Which molecule or compound below contains an ionic bond? A) CO2 B) C2Br4 C) SiF4 D) OCl2 E) NH4NO3

E

9) Use Lewis theory to determine the chemical formula for the compound formed between Al and Cl. A) Al3Cl2 B) Al2Cl3 C) AlCl2 D) AlCl E) AlCl3

E