AP Chemistry- Practice Bonding Questions for Exam

Size: px

Start display at page:

Download "AP Chemistry- Practice Bonding Questions for Exam"

Maximilian Weaver
6 years ago
Views:

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? d. e. 2. Which of the following is a correct Lewis structure for C 2 H 6 O? d. Answers a and c are correct. e. Answers a, b, and c are correct. 3. Which Lewis structure is possible for N 2 O? d. e.

2 4. Which of the following is not a correct Lewis structure? NO 2 NO 2 - NO d. N 2 O e. All of the above are correct structures. 5. What is the correct Lewis structure of SF 4? d. e. 6. Which of the following are correct resonance structures of SO 3?

3 (1) and (5) (2) and (4) (1), (2), and (4) d. (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, SO 3 2-? d. 3 e Formal charge is the absolute value of the charge on a polyatomic anion or cation. the difference between the number of lone pairs of electrons and shared pairs of electrons on any atom in a Lewis structure. 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, CH 2 Cl 2? C = 0, H = 0, Cl = 0 C = 0, H = -1, Cl = +1 C = 0, H = +1, Cl = -1 d. C = -2, H = +1, Cl = +1 e. C = +4, H = -1, Cl = Using formal charges and the octet rule, determine which Lewis structure of OCN - is most stable. d. e.

4 11. Use VSEPR theory to predict the molecular geometry of BH 3. triangular planar triangular pyramidal linear d. tetrahedral e. triangular bipyramidal 12. Use VSEPR theory to predict the molecular geometry of ICl 3. triangular planar triangular pyramidal triangular bipyramidal d. t-shaped e. octahedral 13. Which of the following species have the same molecular geometry: CO 2, H 2 O, BeCl 2, and N 2 O? CO 2 and N 2 O only H 2 O and N 2 O only H 2 O and BeCl 2 only d. CO 2 and BeCl 2 only e. CO 2, BeCl 2, and N 2 O 14. What are the bond angles in SF 6? 90º and 180º 109.5º 120º d. 90º and 120º e. 180º 15. What is the hybridization of the carbon atoms in benzene, C 6 H 6? sp sp 2 sp 3 d. sp 3 d e. sp 3 d What hybridization change does the carbon atom undergo in the combustion of methane? CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(g) sp sp 2 sp 2 sp 3 sp 3 sp d. sp 2 sp e. none 17. How many sigma and pi bonds are present in the following molecule?

5 8 sigma bonds and 1 pi bond 8 sigma bonds and 2 pi bonds 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? phosphorus silicon carbon d. nitrogen e. oxygen 19. Which of the following compounds is expected to have the strongest ionic bonds? RbF NaF NaI d. CsBr e. CsI 20. The central atom in XeF 4 is surrounded by 3 single bonds, 1 double bond, and no lone pairs of electrons. 2 single bonds, 2 double bonds, and no lone pairs of electrons. 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? CI 4 PF 5 NCl 3 d. SO 3 e. O Label the hybridization at C#1, C#2, C#3, and C#4 in the molecule. C1 C2 C3 C4 sp sp sp 3 sp 3 d sp sp sp 2 sp 3 sp sp 2 sp 2 sp 2 d. sp 2 sp 2 sp 3 sp 3 e. sp 3 sp 3 sp 3 sp Which molecule is polar? BF 3 H 2 Se N 2 d. GeF 4

6 e. CO London forces exist for all molecules. only for molecules with nonpolar bonds. 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 CO 2 molecules? I. London forces II. ion-dipole forces III. hydrogen bonding IV. dipole-dipole attractions I only II and III II only d. III only e. I and IV 26. How many sigma (σ) bonds and pi (π) bonds are in the following molecule? five σ and two π five σ and three π five σ and five π d. seven σ and two π e. seven σ and three π 27. Which of the following characteristics apply to PCl 3? 1. nonpolar molecule 2. polar bonds 3. trigonal-pyramidal molecular geometry 4. sp 2 hybridized 1 and 2 2 and 3 3 and 4 d. 1, 2, and 3 e. 1, 2, 3, and Which of the underlined atoms (C 1, C 2, N, and O) are sp 2 hybridized?

7 C 1 and C 2 C 1, N, and O N and O d. O and C 2 e. O only Molecular Orbital Theory The following molecular orbital diagram may be used for the following problems. For oxygen and fluorine, the σ 2p orbital should be lower in energy than the π 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? H 2 2- He 2 Li 2 d. Li 2 2- e. Be According to molecular orbital theory, what is the bond order of nitrogen, N 2? 1 3/2 2 d. 5/2 e. 3

8 31. Use molecular orbital theory to predict which species is paramagneti N 2 O 2 F 2 d. Li 2 e. H Refer to Molecular Orbital Theory. What is the molecular orbital configuration of N 2? [core electrons] (σ 2s ) 2 (σ* 2s ) 2 (π 2p ) 2 (σ 2p ) 2 (σ* 2p ) 2 [core electrons] (σ 2s ) 2 (σ* 2s ) 2 (π 2p ) 2 (σ 2p ) 2 (π* 2p ) 2 [core electrons] (σ 2s ) 2 (σ* 2s ) 2 (π 2p ) 4 (σ 2p ) 2 d. [core electrons] (σ 2s ) 2 (σ* 2s ) 2 (π 2p ) 4 (σ 2p ) 2 (π* 2p ) 4 e. [core electrons] (σ 2s ) 2 (σ* 2s ) 2 (π 2p ) 4 (π* 2p ) 2

9 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: ANS: B PTS: ANS: A PTS: ANS: D PTS: ANS: E PTS: ANS: A PTS: ANS: B PTS: ANS: C PTS: ANS: E PTS: ANS: E PTS: 1 OBJ: 08-7 Bond Properties: Bond Polarity and Electronegativity 19. ANS: B PTS: 1 OBJ: 9.3 Bonding in Ionic Compounds 20. ANS: E PTS: 1 OBJ: 9.6 Exceptions to the Octet Rule 21. ANS: C PTS: 1 OBJ: 9.9 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: 10.2 Valence Bond Theory 27. ANS: B PTS: 1 OBJ: 10.2 Valence Bond Theory 28. ANS: A PTS: 1 OBJ: 10.2 Valence Bond Theory 29. ANS: C PTS: 1 OBJ: 10.3 Molecular Orbital Theory 30. ANS: E PTS: 1 OBJ: 10.3 Molecular Orbital Theory 31. ANS: B PTS: 1 OBJ: 10.3 Molecular Orbital Theory 32. ANS: C PTS: 1 OBJ: 10.3 Molecular Orbital Theory

1) Based on the octet rule, magnesium most likely forms a ion. A) Mg- B) Mg6+ C) Mg2+ D) Mg6- E) Mg2-

1) Based on the octet rule, magnesium most likely forms a ion. A) Mg- B) Mg6+ C) Mg2+ D) Mg6- E) Mg2- 1) ased on the octet rule, magnesium most likely forms a ion. ) Mg- ) Mg6+ ) Mg2+ ) Mg6- E) Mg2-2) ased on the octet rule, phosphorus most likely forms a ion. ) P5- ) P5+ ) P+ ) P3- E) P3+ 3) Which ion