Fall 2006 CH301 Worksheet 7 1. Predict the electronic geometry of the following molecules: (a) PCl5 (b) SeF4 (c) ICl2- (a) trigonal bipyramidal (b) trigonal bipyramidal (c) trigonal bipyramidal 2. For the molecules in question #1, give the number of B and U electrons, and give their molecular geometry. (a) AB5, trigonal bipyramidal (b) AB4U, see-saw (c) AB2U3, linear 3. Give the bond angles in the following molecules: (a) SeCl6 (b) CH4 (d) BF3 (a) 90º, 180º (b) 109.5º (c) 120º 4. Which of the following are polar molecules? H2O, CH2Cl2, XeF4, CH4, NH3 H2O, CH2Cl2, NH3 5. Draw the 3D VSEPR structure with dipoles for NO2-. Is NO2- a polar molecule? NOOYes, it is polar. 6. Give the hybridization of the central atoms in the following molecules: (a) I3-, (b) CO2, (c) BCl3, (d) NCl3 (a) dsp3 (d) sp3 (b) sp (c) sp2 7. Draw the 3D structure of CH2COOH. List the types of bonds and the atomic orbits that form them. 8. Describe, in simple terms, the difference between a σ and a π bond. A sigma bond is formed from “head-on” overlap between orbitals, pi bonds are “side-to- side” overlap. 9. What was the immediate evidence that the carbon in methane formed hybridized orbitals? There is no separate peak on a spectrum for one lower-energy C-H bond. 10. Which of the following hybrid orbitals would you expect to be the lowest in energy? sp, sp2, sp3, dsp3, d2sp3 sp σ1s-sp2 σ1s-sp2 σsp2-sp2 σsp2-sp3 σsp2-sp3 σsp3-1s π2p-2pCCHOOHH11. How many unpaired electrons does O2 have? Is it paramagnetic? 2 12. Is N2 more or less paramagnetic than O2? less 13. Fill the molecular orbitals for C2. ____ _____ ____ ____ _↑↓_ _↑↓_ _↑↓_ _↑↓_ _↑↓_ _↑↓_ 14. What is the bond order in C2? 2 15. Is C2 paramagnetic? no 16. List the following in terms of increasing bond length: Li2, N2, C2 N2 < C2 < Li2 17. List the following in terms of increasing bond energy: O2-, O2, O2+ O2- < O2 < O2+ 18. Fill the molecular orbitals for CO+. ____ ____ ____ _↑↓_ _↑__ _↑↓_ _↑↓_ _↑↓_ _↑↓_ _↑↓_ 19. What is the bond order for CO+? 2.5 20. Would you expect boron nitride (BN) to be paramagnetic? What would you expect the bond order to be? no, bond order =
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