AP Chemistry- Practice Bonding Questions for Exam - Quia

1 AP Chemistry- Practice Bonding Questions for Exam Multiple Choice Identify the choice that best completes the statement or answers the question. ____ 1. Which of the following is a correct lewis structure for oxygen? a. b. c. d. e. ____ 2. Which of the following is a correct lewis structure for C2H6O? a. b. c. d. Answers a and c are correct. e. Answers a, b, and c are correct. ____ 3. Which lewis structure is possible for N2O? a. b. c. d. e. ____ 4. Which of the following is not a correct lewis structure ? a. NO2 b. NO2- c. NO d. N2O e. All of the above are correct structures. ____ 5. What is the correct lewis structure of SF4? a. b. c. d. e. ____ 6. Which of the following are correct resonance structures of SO3? a. (1) and (5) b. (2) and (4) c. (1), (2), and (4) d.

2 (2), (3) and (4) e. (1), (2), (4), and (5) ____ 7. How many lone pairs of electrons are on the sulfur atom in sulfite ion, SO32-? a. 0 b. 1 c. 2 d. 3 e. 4 ____ 8. Formal charge is a. the absolute value of the charge on a polyatomic anion or cation. b. the difference between the number of lone pairs of electrons and shared pairs of electrons on any atom in a lewis structure . c. the difference between the number of valence electrons and the number of protons in any given atom. d. equal to the number of valence electrons in a free atom minus the number of shared in covalent bonds. e. the difference between the number of valence electrons in a free atom and the number of electrons assigned to the atom in a lewis structure . ____ 9. What is the formal charge on each atom in dichloromethane, CH2Cl2? a. C = 0, H = 0, Cl = 0 b.

3 C = 0, H = -1, Cl = +1 c. C = 0, H = +1, Cl = -1 d. C = -2, H = +1, Cl = +1 e. C = +4, H = -1, Cl = -1 ____ 10. Using formal charges and the octet rule, determine which lewis structure of OCN- is most stable. a. b. c. d. e. ____ 11. Use VSEPR theory to predict the molecular geometry of BH3. a. triangular planar b. triangular pyramidal c. linear d. tetrahedral e. triangular bipyramidal ____ 12. Use VSEPR theory to predict the molecular geometry of ICl3. a. triangular planar b. triangular pyramidal c. triangular bipyramidal d. t-shaped e. octahedral ____ 13. Which of the following species have the same molecular geometry: CO2, H2O, BeCl2, and N2O? a. CO2 and N2O only b. H2O and N2O only c. H2O and BeCl2 only d. CO2 and BeCl2 only e. CO2, BeCl2, and N2O ____ 14. What are the bond angles in SF6?

4 A. 90 and 180 b. c. 120 d. 90 and 120 e. 180 ____ 15. What is the hybridization of the carbon atoms in benzene, C6H6? a. sp b. sp2 c. sp3 d. sp3d e. sp3d2 ____ 16. What hybridization change does the carbon atom undergo in the combustion of methane? CH4(g) + 2O2(g) CO2(g) + 2H2O(g) a. sp sp2 b. sp2 sp3 c. sp3 sp d. sp2 sp e. none ____ 17. How many sigma and pi bonds are present in the following molecule? a. 8 sigma bonds and 1 pi bond b. 8 sigma bonds and 2 pi bonds c. 10 sigma bonds and 2 pi bonds d. 11 sigma bonds and 2 pi bonds e. 11 sigma bonds and 1 pi bond ____ 18. Which element is the most electronegative? a. phosphorus b. silicon c. carbon d. nitrogen e. oxygen ____ 19. Which of the following compounds is expected to have the strongest ionic bonds? a. RbF b.

5 NaF c. NaI d. CsBr e. CsI ____ 20. The central atom in XeF4 is surrounded by a. 3 single bonds, 1 double bond, and no lone pairs of electrons. b. 2 single bonds, 2 double bonds, and no lone pairs of electrons. c. 3 single bonds, 1 double bond, and 1 lone pair of electrons. d. 4 single bonds, no double bonds, and no lone pairs of electrons. e. 4 single bonds, no double bonds, and 2 lone pairs of electrons. ____ 21. Which one of the following molecules has a dipole moment? a. CI4 b. PF5 c. NCl3 d. SO3 e. O2 ____ 22. Label the hybridization at C#1, C#2, C#3, and C#4 in the molecule. C1 C2 C3 C4 a. sp sp sp3 sp3d b. sp sp sp2 sp3 c. sp sp2 sp2 sp2 d. sp2 sp2 sp3 sp3 e.

6 Sp3 sp3 sp3 sp3 ____ 23. Which molecule is polar? a. BF3 b. H2Se c. N2 d. GeF4 e. CO2 ____ 24. London forces exist a. for all molecules. b. only for molecules with nonpolar bonds. c. only for molecules with polar bonds. d. only for molecules with metallic bonds. e. only for molecules with hydrogen Bonding . ____ 25. Which of the following interactions are present between CO2 molecules? I. London forces II. ion-dipole forces III. hydrogen Bonding IV. dipole-dipole attractions a. I only b. II and III c. II only d. III only e. I and IV ____ 26. How many sigma ( ) bonds and pi ( ) bonds are in the following molecule? a. five and two b. five and three c. five and five d. seven and two e. seven and three ____ 27. Which of the following characteristics apply to PCl3?

7 1. nonpolar molecule 2. polar bonds 3. trigonal-pyramidal molecular geometry 4. sp2 hybridized a. 1 and 2 b. 2 and 3 c. 3 and 4 d. 1, 2, and 3 e. 1, 2, 3, and 4 ____ 28. Which of the underlined atoms (C1, C2, N, and O) are sp2 hybridized? a. C1 and C2 b. C1, N, and O c. N and O d. O and C2 e. O only Molecular Orbital Theory The following molecular orbital diagram may be used for the following problems. For oxygen and fluorine, the 2p orbital should be lower in energy than the 2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules. ____ 29. According to molecular orbital theory, which of the following species is the most likely to exist? a. H22- b. He2 c. Li2 d. Li22- e. Be2 ____ 30. According to molecular orbital theory, what is the bond order of nitrogen, N2?

8 A. 1 b. 3/2 c. 2 d. 5/2 e. 3 ____ 31. Use molecular orbital theory to predict which species is paramagnetic. a. N2 b. O2 c. F2 d. Li2 e. H2 ____ 32. Refer to Molecular Orbital Theory. What is the molecular orbital configuration of N2? a. [core electrons] ( 2s)2 ( *2s)2 ( 2p)2 ( 2p)2 ( *2p)2 b. [core electrons] ( 2s)2 ( *2s)2 ( 2p)2 ( 2p)2 ( *2p)2 c. [core electrons] ( 2s)2 ( *2s)2 ( 2p)4 ( 2p)2 d. [core electrons] ( 2s)2 ( *2s)2 ( 2p)4 ( 2p)2 ( *2p)4 e. [core electrons] ( 2s)2 ( *2s)2 ( 2p)4 ( *2p)2 AP Chemistry- Practice Bonding Questions for Exam Answer Section MULTIPLE CHOICE 1. ANS: A PTS: 1 2. ANS: D PTS: 1 3. ANS: B PTS: 1 4. ANS: C PTS: 1 5. ANS: B PTS: 1 6. ANS: B PTS: 1 7. ANS: B PTS: 1 8. ANS: E PTS: 1 9. ANS: A PTS: 1 10. ANS: B PTS: 1 11.

9 ANS: A PTS: 1 12. ANS: D PTS: 1 13. ANS: E PTS: 1 14. ANS: A PTS: 1 15. ANS: B PTS: 1 16. ANS: C PTS: 1 17. ANS: E PTS: 1 18. ANS: E PTS: 1 OBJ: 08-7 Bond Properties: Bond polarity and Electronegativity 19. ANS: B PTS: 1 OBJ: Bonding in Ionic Compounds 20. ANS: E PTS: 1 OBJ: Exceptions to the Octet Rule 21. ANS: C PTS: 1 OBJ: Molecular polarity 22. ANS: B PTS: 1 OBJ: 09-3 Orbitals Consistent with Molecular Shapes: Hybridization 23. ANS: B PTS: 1 OBJ: 09-5 Molecular polarity 24. ANS: A PTS: 1 OBJ: 09-6 Noncovalent Interactions and Forces Between Molecules 25. ANS: A PTS: 1 OBJ: 09-6 Noncovalent Interactions and Forces Between Molecules 26. ANS: E PTS: 1 OBJ: Valence Bond Theory 27.

10 ANS: B PTS: 1 OBJ: Valence Bond Theory 28. ANS: A PTS: 1 OBJ: Valence Bond Theory 29. ANS: C PTS: 1 OBJ: Molecular Orbital Theory 30. ANS: E PTS: 1 OBJ: Molecular Orbital Theory 31. ANS: B PTS: 1 OBJ: Molecular Orbital Theory 32. ANS: C PTS: 1 OBJ: Molecular Orbital Theory