Name: Class: Date: 3. How many lone pairs of electrons are assigned to the carbon atom in carbon monoxide? a. 0 b. 1 c. 2 d. 3
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1 Class: Date: Midterm 3, Fall 2009 Record your name on the top of this exam and on the scantron form. Record the test ID letter in the top right box of the scantron form. Record all of your answers on the scantron form. Turn in both your answer sheet at the end of the period. You have 50 minutes. GOOD LUCK! 1. Which combination of atoms is most likely to produce a compound with covalent bonds? a. Na and Cl b. Al and O c. S and Br d. Pb and F 2. A sulfur atom has valence electrons. a. 2 b. 6 c. 16 d How many lone pairs of electrons are assigned to the carbon atom in carbon monoxide? a. 0 b. 1 c. 2 d What is the hybridization of each carbon atom in C 2 H 2? a. sp b. sp 2 c. sp 3 d. p 5. Which of the following are resonance structures for nitrite ion, NO 2? a. 1 and 2 b. 2 and 4 c. 3 and 4 d. 1, 2, and 3 6. Which of the following elements is most likely to form a molecular structure that disobeys the octet rule? a. B b. C c. O d. F 1
2 7. What is the correct Lewis structure for IF 3? a. c. b. d. 8. What is the formal charge on P in the phosphate resonance structure shown below? a. 0 b. +1 c. +3 d Use VESPR theory to predict the molecular geometry around either carbon atom in ethylene, C 2 H 4. a. linear b. bent c. trigonal-planar d. tetrahedral 10. What are the approximate F Br F bond angles in BrF 5? a. 90 and 180 b c. 90 and 120 d Place the following molecules in order from smallest to largest H N H bond angles: NH 4+, NH 3, and NH 2. a. NH + 4 < NH 3 < NH 2 b. NH + 4 < NH 2 < NH 3 c. NH 2 < NH 3 < NH + 4 d. NH 2 < NH + 4 < NH Which of the following compounds has polar covalent bonds: NaBr, Br 2, HBr, and CBr 4? a. HBr only b. Br 2 only c. NaBr only d. HBr and CBr 4 2
3 13. Choose which central atom in the following molecules is most electronegative. a. PH 3 b. CH 4 c. H 2 S d. H 2 O 14. Which of the following statements is/are correct? 1. The atom with the lowest electronegativity is usually the central atom in a molecule. 2. As the difference in electronegativity between two bonded atoms increases, the percent ionic character of the bond increases. 3. Electronegativity decreases down each group of the periodic table. c. 2 and 3 only d. 1, 2, and Three possible structures of C 2 H 2 Cl 2 are shown below. Which of these molecules are polar? c. 3 only d. 1 and In molecules, as bond order increases, a. bond length decreases and bond energy increases. b. bond length increases and bond energy is unchanged. c. bond length is unchanged and bond energy increases. d. both bond length and bond energy increase. 17. Use Lewis structures to predict the bond order for a carbon-oxygen bond in carbonate ion, CO 2 3. a. 1/2 b. 1 c. 4/3 d. 3/2 3
4 18. Calculate the enthalpy change (Δ r H) for the reaction below, Br 2 (g) + 3 F 2 (g) 2 BrF 3 (g) given the bond enthalpies of the reactants and products. a. 836 kj b. 89 kj c. +89 kj d. +99 kj Bond Enthalpy Bond (kj/mol rxn) Br Br 193 F F 155 Br F Which one of the statements concerning valence bond (VB) and molecular orbital (MO) bond theories is correct? a. MO theory predicts that electrons are localized between pairs of atoms. b. In VB theory, bonding electrons are delocalized over the molecule. c. MO theory can provide a quantitative picture of orbital energies and bonding. d. VB theory can provide a quantitative picture of orbital energies and bonding. 20. How many sigma (σ) bonds and pi (π) bonds are in the following molecule? a. seven σ and three π b. seven σ and two π c. five σ and five π d. five σ and three π 21. What is the hybridization of each carbon atom in benzene, C 6 H 6? Benzene contains a six-member carbon ring. a. sp b. sp 2 c. sp 3 d. sp 3 d 22. Which of the following characteristics apply to SO 2? 1. linear molecular shape 2. bent molecular shape 3. nonpolar molecule 4. polar molecule b. 1 and 3 c. 2 only d. 2 and 4 4
5 23. Dichloromethane, CH 2 Cl 2, is a common organic solvent. Which of the following statements concerning dichloromethane is/are CORRECT? 1. CH 2 Cl 2 has two isomers. 2. CH 2 Cl 2 is nonpolar. 3. The hybridization of the central carbon atom is sp 3. c. 3 only d. 1 and For which of the following compounds is it possible for cis and trans isomers to exist? c. 3 only d. 1 and Which of the underlined atoms (C 1, C 2, N, and O) has 109 degree bond angles? a. C 1 and C 2 b. C 1, N, and O c. N and O d. O and C What is the formal charge on each atom in the Lewis structure for CON - (below)? a. C = -1, O = +2, N = -2 c. C = +5, O = -2, N = -4 b. C = +1, O = 0, N = -2 d. C = -2, O = +1, N = 0 5
6 Midterm 3, Fall 2009 Answer Section MULTIPLE CHOICE 1. ANS: C PTS: 1 TOP: 8.1 Chemical Bond Formation 2. ANS: B PTS: 1 TOP: 8.2 Covalent Bonding and Lewis Structures 3. ANS: B PTS: 1 TOP: 8.2 Covalent Bonding and Lewis Structures 4. ANS: A PTS: 1 TOP: 8.2 Covalent Bonding and Lewis Structures 5. ANS: A PTS: 1 TOP: 8.4 Resonance 6. ANS: A PTS: 1 TOP: 8.5 Exceptions to the Octet Rule 7. ANS: A PTS: 1 TOP: 8.5 Exceptions to the Octet Rule 8. ANS: A PTS: 1 TOP: 8.6 Molecular Shapes 9. ANS: C PTS: 1 TOP: 8.6 Molecular Shapes 10. ANS: A PTS: 1 TOP: 8.6 Molecular Shapes 11. ANS: C PTS: 1 TOP: 8.6 Molecular Shapes 12. ANS: D PTS: 1 TOP: 8.7 Bond Polarity and Electronegativity 13. ANS: D PTS: 1 TOP: 8.7 Bond Polarity and Electronegativity 14. ANS: D PTS: 1 TOP: 8.7 Bond Polarity and Electronegativity 15. ANS: D PTS: 1 TOP: 8.8 Bond and Molecular Polarity 16. ANS: A PTS: 1 TOP: 8.9 Bond Properties: Order, Length, Energy 17. ANS: C PTS: 1 TOP: 8.9 Bond Properties: Order, Length, Energy 18. ANS: A PTS: 1 TOP: 8.9 Bond Properties: Order, Length, Energy 19. ANS: C PTS: 1 TOP: 9.1 Orbitals and Theories of Chemical Bonding 20. ANS: A PTS: 1 TOP: 9.2 Valence Bond Theory 21. ANS: B PTS: 1 TOP: 9.2 Valence Bond Theory 22. ANS: D PTS: 1 TOP: 9.2 Valence Bond Theory 23. ANS: C PTS: 1 TOP: 9.2 Valence Bond Theory 24. ANS: B PTS: 1 TOP: 9.2 Valence Bond Theory 25. ANS: C PTS: 1 TOP: 9.2 Valence Bond Theory 26. ANS: A PTS: 1 1
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