5. Which of the following is the correct Lewis structure for SOCl 2

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1 Unit C Practice Problems Chapter 8 1. Draw the lewis structures for the following molecules: a. BeF 2 b. SO 3 c. CNS 1- d. NO 2. The correct Lewis symbol for ground state carbon is a) b) c) d) e) 3. Which of the atoms below is least likely to violate the octet rule? a) Be b) P c) S d) B e) F 4. What is the bond order of the C O bond in acetone? O CH 3 C CH 3 a) 4 b) 1.5 c) 0.5 d) 1 e) 2 5. Which of the following is the correct Lewis structure for SOCl 2? (Consider formal charge) a) d) b) e) c) 6. Which of the following bonds is most polar? a) N Cl d) Br Br b) C N e) S O c) S S

2 7. The molecule BrF 3 has how many lone pairs of electrons on the central atom? a) 0 b) 1 c) 2 d) 3 8. Classify the following bonds as either metallic, ionic, covalent, or covalent network: a. Francium Fluoride b. Diamond c. Gold d. Water Chapter 9 1. Use VSEPR theory to predict the shapes of the following molecules: a. BrF 5 b. HCN c. BF 3 d. SO 2 e. SCl 2 2. What type of hybridized orbital is used by the central atom of each of the molecules in problem 1? 3. CCl 4 is a perfect tetrahedron, but AsCl 4 is a distorted tetrahedron. Explain. 4. BeCl 2 and TeCl 2 are both covalent molecules, yet BeCl 2 is linear while TeCl 2 is nonlinear (bent). Explain. 5. What types of hybridized orbitals can be formed by elements of the third period that cannot be formed by elements in the second period?

3 6. Which molecule should have the larger dipole moment, HBr or HI? 7. Which of the following molecules has a dipole moment? a. CCl 4 b. H 2 S c. CO 2 d. BCl 3 e. Cl 2 8. Choose the best answer. For the water molecule: a. The bonds are polar, and the molecule is nonpolar. b. The bonds are nonpolar, and the molecule is polar. c. The bonds are polar, and the molecule is polar. d. The bonds are nonpolar and the molecule is nonpolar. 9. NF 3 has a trigonal pyramidal geometry. How many electron pairs are in the valence shell of the central atom? 10. Predict whether the following molecules are polar or nonpolar: SO 2, NF 3, CS Determine the total number of sigma and pi bonds in the molecules CCl 2 O and CH 3 CHCHCN. 12. Predict which will exhibit delocalized pi bonding (resonance structures): (SO 3 ) 2-, (NH 4 ) +, NO 2, (NCS) -, (OCN) -, (I 3 ) -

4 13. Identify the hybridization of the central atom in the following compounds and ions: CF 4, SF 4, (PO 2 F 2 ) -, (SF 3 ) +, (I 3 ) -, (SO 4 ) 2-, (BH 4 ) -, (SF 5 ) -, OSF 4, ClF 3, BCl 3, (XeO 6 ) Describe the bonding in XeF 4 using hybrid orbitals. Remember to consider first the Lewis structure, then the structural pair geometry and molecular shape. 15. Describe the hybridization of each carbon and oxygen atom in acetic acid, CH 3 CO 2 H

5 Chapter 25 Name the following:

6 5. 6. CH 3 CH=CHCH 2 CH 3 7. CH 3 (CH 2 ) 4 CH(CH 3 ) 2 8. (CH 3 ) 2 CHC CCH 3 9. The following structures all have the same molecular formula: C 6 H 14. Which of these structures represent the same molecule? Draw the following molecules: 1. 2-methylbutane

7 2. 2,3,3,3-tetramethylpentane 3. 5-methyl-1-hexyne 4. 2,3-dimethyl-2-butene 5. 3-ethyl-2,3-dimethyloctane

8 Unit C Practice Problems Answers Chapter 8 1. a: b: c: d: 2. a 3. e 4. e 5. b 6. a 7. c 8. a: ionic; b: covalent network; c: metallic; d: covalent

9 Chapter 9 1. a. Square pyramidal, b. Linear, c. Trigonal Planar, d. Bent, e. Bent 2. a. sp 3 d 2, b. sp, c. sp 2, d. sp 2, e. sp 3 3. CCl 4 has four electron pairs about the central C atom, while AsCl 4 has 5 pairs about the As atom with only 4 Cl atoms attached. The extra pair of unshared electrons in AsCl 4 prevents it from forming a tetrahedron. 4. There are two electron pairs in the valence shell of Be in BeCl 2, but there are four pairs in the valence shell of Te in TeCl 2. These four pairs are at the corners of a tetrahedron. When two Cl atoms bond to a Te atom via two of the pairs, the Cl-Te-Cl bond angle is degrees. 5. sp 3 d and sp 3 d 2 6. HBr because of the bond polarity. Br is more electronegative than I is. 7. b only 8. c 9. Four 10. Polar, Polar, Nonpolar 11. CCl 2 O - 3 sigma, 1 pi; CH 3 CHCHCN - 9 sigma, 3 pi 12. No, No, Yes, Yes, Yes, No 13. sp 3 (tetrahedral) sp 3 d (trigonal bipyramidal) sp 3 (tetrahedral) sp 3 (tetrahedral) sp 3 d (trigonal bipyramidal) sp 3 (tetrahedral) sp 3 (tetrahedral) sp 3 d 2 (octahedral) sp 3 d (trigonal bipyramidal) sp 3 d (trigonal bipyramidal) sp 2 (trigonal planar) sp 3 d 2 (octahedral) 14. Xe atom uses sp 3 d 2 hybridization (octahedral, square planar) 15. single-bonded C is sp 3 (tetrahedral), double-bonded C is sp 2 (trigonal planar) single-bonded O is sp 3 (tetrahedral, bent), double-bonded O is sp 2 (trigonal planar)

10 Chapter 25 Name the following molecules: 1. 3,5-dimethyl 2-hexene 2. 2,2,3-triimethylpentane 3. 4-methyloctane 4. 6-ethyl-2,5,6-trimethyloctane 5. 5-ethyl-2-methyl-3-heptyne 6. 2-pentene 7. 2-methylheptane 8. 4-methyl-2-pentyne 9. A&B Draw the following molecules: 1. 2-methylbutane 2. 2,3,3,3-tetramethylpentane

11 3. 5-methyl-1-hexyne 4. 2,3-dimethyl-2-butene 5. 3-ethyl-2,3-dimethyloctane

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