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Welcome to Chem 1C with Terri Bentzinger

Welcome to Chem 1C with Terri Bentzinger. E-mail: benzene4president@gmail.com Website: http://clas.sa.ucsb.edu/staff/terri/ Drop-in: M/W 11-12, T 1-2, T/R 1-2 and 3-4, F 1-2 SRB Rm 3274. Bonding – ch. 13/14. 1. Arrange the following in order of relative electronegativity.

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Welcome to Chem 1C with Terri Bentzinger

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  1. Welcome to Chem 1C with Terri Bentzinger E-mail: benzene4president@gmail.com Website: http://clas.sa.ucsb.edu/staff/terri/ Drop-in: M/W 11-12, T 1-2, T/R 1-2 and 3-4, F 1-2 SRB Rm 3274

  2. Bonding – ch. 13/14 1. Arrange the following in order of relative electronegativity. N, P, F, Li, S, C

  3. Bonding – ch. 13/14 2. Predict the relative bond polarity C-O, C-N, C-H, C-Br

  4. Bonding – ch. 13/14 3. For each of the following draw the Lewis structure, determine the electronic and molecular geometries, predict the bond angle, state if polar or non polar and label the hybridization on the central atom. a. PCl3 g. XeI5+ b. SO3 h. ICl4- c. HCN i. SO2 d. H2CO j. NH4+ e. SF6 k. PCl5 f. BeF2 l. XeBr4

  5. Bonding – ch. 13/14 4. Which of the following shows these molecules in order from most polar to least polar? CH4 , CF2Cl2 , CF2H2 , CCl4 , CCl2H2 A) CH4 > CF2Cl2 > CF2H2 > CCl4 > CCl2H2 B) CH4 > CF2H2 > CF2Cl2 > CCl4 > CCl2H2 C) CF2Cl2 > CF2H2 > CCl2H2 > CH4 = CCl4 D) CF2H2 > CCl2H2 > CF2Cl2 > CH4 = CCl4 E) CF2Cl2 > CF2H2 > CCl4 > CCl2H2 > CH4

  6. Bonding – ch. 13/14 5. Draw the resonance structures for OCN- and determine the relative stability for the resonance contributors.

  7. Bonding – ch. 13/14 6. For the following structure: a. Fill in the missing bonds/electrons (if any) b. label the bonds as sigma (σ) or pi (π) c. label the hybridization for the carbons d. determine the bond angles

  8. Bonding – ch. 13/14 7. How many of the following molecules have all of their atoms in the same plane? F2O H2CO CO2 H2O2 NH3 BeCl2 H2C = CH2

  9. Bonding – ch. 13/14 8. Will all of the atoms in allene lie in the same plane?

  10. Bonding – ch. 13/14 9. Rank the following in order of increasing carbon-oxygen bond length. CO32- CO2 CO CH3OH

  11. Bonding – ch. 13/14 10. Fill in the following table:

  12. Bonding – ch. 13/14 MO diagram for homonuclear molecules in Groups 1-5 MO diagram for homonuclear molecules in Groups 6-8

  13. Bonding – ch. 13/14 Sigma vs. Pi P with P S with S

  14. Bonding – ch. 13/14 11. Label the following molecular orbitals. A. D. B. E. C.

  15. Bonding – ch. 13/14 12. Identify the element X if the ion X2- has the following valence electron configuration; (σ3s)2(σ3s*)2(π3p)4(σ3p)2(π3p*)1

  16. Bonding – ch. 13/14 13. Using the MO model predict the relative bond dissociation energy for the following F2 F2- F2+

  17. Bonding – ch. 13/14 – Answer Key 1. Arrange the following in order of relative electronegativity. N, P, F, Li, S, C Li<P<C<S<N<F 2. Predict the relative bond polarity C-O, C-N, C-H, C-Br C-H<C-Br<C-N<C-O

  18. Bonding – ch. 13/14 – Answer Key 3. For each of the following draw the Lewis structure, determine the electronic and molecular geometries, predict the bond angle, state if polar or non polar and label the hybridization on the central atom. a. PCl3=> EG-tetrahedral, MG-trigonal pyramid, <109º, polar, sp3 b. SO3 => EG/MG-trigonal planar, 120º, non-polar, sp2 c. HCN => EG/MG-linear, 180º, polar, sp d. H2CO => EG/MG-trigonal planar, 120º, polar, sp e. SF6 => EG/MG-octahedral, 90º, non-polar, d2sp3 or sp3d2 f. BeF2 => EG/MG-linear, 180º, non-polar, sp g. XeI5+ => EG-octahedral, MG-square pyramid, 90º, polar, d2sp3 or sp3d2 h. ICl4- => EG-octahedral, MG-square planar, 90º, non-polar, d2sp3 or sp3d2 i. SO2 => EG-trigonal planar, MG-bent, 120º, polar, sp2 j. NH4+ => EG/MG-tetrahedral, 109.5º, non-polar, sp3 k. PCl5 => EG/MG-trigonalbipyramid, 90º/120º, non-polar, dsp3 or sp3d l. XeBr4 => EG-octahedral, MG-square planar, 90º, d2sp3 or sp3d2

  19. Bonding – ch. 13/14 – Answer Key 4. Which of the following shows these molecules in order from most polar to least polar? A) CH4 > CF2Cl2 > CF2H2 > CCl4 > CCl2H2 B) CH4 > CF2H2 > CF2Cl2 > CCl4 > CCl2H2 C) CF2Cl2 > CF2H2 > CCl2H2 > CH4 = CCl4 D) CF2H2 > CCl2H2 > CF2Cl2 > CH4 = CCl4 E) CF2Cl2 > CF2H2 > CCl4 > CCl2H2 > CH4 5. Draw the resonance structures for OCN- and determine the relative stability for the resonance contributors. [O−C≡N]- <−> [O=C=N]- <−> [O ≡ C−N]- Most stable 2nd most stable least stable

  20. Bonding – ch. 13/14 – Answer Key 6. For the following structure: a. Fill in the missing bonds/electrons (if any) CO double bond and CN triple bond b. label the bonds as sigma (σ) or pi (π)single bonds= sigma, double=sigma and pi, triple=sigma and 2 pi c. label the hybridization for the carbons 3 carbons on the left are sp3, C with O is sp2 C with N is sp d. determine the bond angles sp3 has 109.5°, sp2 has 120° and sp has 180° 7. How many of the following molecules have all of their atoms in the same plane? H2C=CH2, H2CO, F2O, BeCl2, CO2 8. For each of the following structures determine the maximum number of atoms that lie in the same plane. allene has 5, acrylonitrile is all

  21. Bonding – ch. 13/14 – Answer Key 9. CH3OH > CO32- > CO2 > CO 10. 11. a. σ1s* orσ2s* b. σ2p c. π2p* d. σ1s orσ2s e. π2p 12. P 13. F2+ > F2> F2-

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