Fall 2006 CH301 Worksheet 7 1. Predict the electronic geometry of the following molecules: (a) PCl5 (b) SeF4 (c) ICl2- 2. For the molecules in question #1, give the number of B and U electrons, and give their molecular geometry. 3. Give the bond angles in the following molecules: (a) SeCl6 (b) CH4 (d) BF3 4. Which of the following are polar molecules? H2O, CH2Cl2, XeF4, CH4, NH3 5. Draw the 3D VSEPR structure with dipoles for NO2-. IS NO2- a polar molecule? 6. Give the hybridization of the central atoms in the following molecules: (a) I3-, (b) CO2, (c) BCl3, (d) NCl3 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. 9. What was the immediate evidence that the carbon in methane formed hybridized orbitals? 10. Which of the following hybrid orbitals would you expect to be the lowest in energy? sp, sp2, sp3, dsp3, d2sp311. How many unpaired electrons does O2 have? Is it paramagnetic? 12. Is N2 more or less paramagnetic than O2? 13. Fill the molecular orbitals for C2. ____ _____ ____ ____ ____ ____ ____ ____ ____ ____ 14. What is the bond order in C2? 15. Is C2 paramagnetic? 16. List the following in terms of increasing bond length: Li2, N2, C2 17. List the following in terms of increasing bond energy: O2=, O2, O2+ 18. Fill the molecular orbitals for CO+. ____ ____ ____ ____ ____ ____ ____ ____ ____ ____ 19. What is the bond order for CO+? 20. Would you expect boron nitride (BN) to be paramagnetic? What would you expect the bond order to
View Full Document
Unlocking...