38. Draw Lewis structures, predict the geometry, and give the approximate bond angle for each of the following compounds.
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1 Screencast Draw Lewis structures, predict the geometry, and give the approximate bond angle for each of the following compounds. a. Sulfate ion b. Water c. Carbon dioxide 1
2 d. Ammonia e. Nitrate ion f. Carbonate ion g. Nitrogen trifluoride 2
3 h. Phosphorus trifluoride i. CH 4 j. CCl 2 F 2 3
4 k. OF 2 l. ICl 4 - m. IOF 5 n. I 3-4
5 o. BrF Explain why the bond angles in methane (CH 4 ) are o, while the bond angles in ammonia (NH 3 ) are o. 40. Explain why CH 4 has a tetrahedral geometry, while SF 4 has a see-saw shape. 5
6 41. In the following structures, identify: i. The shape around each carbon atom ii. The bond angles emerging from each carbon atom. Each atom is bonded to the carbon you are looking at is considered to be a terminal atom even other carbons. After finding the shape around the first carbon atom, move to the second and treat is as the central atom.) 6
7 Screencast Use the Lewis structures you drew in problem 1 to determine if the following are polar or nonpolar. Explain by discussing the shape, polarity of bonds and whether or not dipoles cancel. a. Sulfate ion b. Water c. Carbon dioxide d. Ammonia e. Nitrate ion f. Carbonate ion g. Nitrogen trifluoride h. Phosphorus trifluoride i. CH 4 j. CCl 2 F 2 k. OF 2 7
8 l. ICl 4 - m. IOF 5 n. I 3 - o. BrF 3 Screencast Describe what happens during the hybridization of the boron atom in BCl 3. Include orbital diagrams and details about the promotion of electrons. 44. Describe what happens during the hybridization of the bromine atom in BrF 3. Include orbital diagrams and details about the promotion of electrons. 45. Describe what happens during the hybridization of the sulfur atom in sulfur dichloride. Include orbital diagrams and details about the promotion of electrons. 8
9 46. Use the Lewis structures you drew in problem 1 to determine the type of hybridization (type of hybrid bonds) around the central atom in each of the structures listed below a. Sulfate ion b. Water c. Carbon dioxide d. Ammonia e. Nitrate ion f. Carbonate ion g. Nitrogen trifluoride h. Phosphorus trifluoride i. CH 4 j. CCl 2 F 2 9
10 k. OF 2 l. ICl 4 - m. IOF 5 n. I 3 - o. BrF 3 Screencast What is the difference between a sigma bond and a pi bond? 48. Use the structure below to answer the following questions. 10
11 a. What type of hybrid orbitals form around the first carbon? b. Describe what happens during the hybridization of the first carbon atom. Include details about the promotion of electrons. c. What type of hybrid orbitals from around the second carbon? d. Describe what happens during the hybridization of the second carbon atom. Include detains about the promotion of electrons e. How is the double bond between the first and second carbon formed? Reference types of orbitals involved in the bonds and the methods of bonding. 49. Use the structure below to answer the following question a. What type of hybrid orbitals form around the carbon? b. How many sigma bonds are there between the carbon and the nitrogen? 11
12 c. How many pi bonds are there between the carbon and the nitrogen? d. How many non-hybrid p-orbitals remain on the carbon atom in this compound? 50. Use the structure below to answer the following questions a. What type of hybrid orbitals form around the second carbon? b. What type of hybrid orbitals form around the third carbon? c. How many non-hybrid p-orbitals remain on the first carbon? d. How many sigma bonds exist in the entire structure? e. How many pi bonds exist in the entire structure? 12
13 Screencast
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