Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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### VSEPR Theory and Molecular Geometry

#### Example Molecule: Methane (CH<sub>4</sub>)

The table below demonstrates the application of the Valence Shell Electron Pair Repulsion (VSEPR) theory to determine the molecular geometry of methane.

| Molecule or Molecular Ion | Lewis Structure | Valence Shell Electron Pairs | Bonding Electron Pairs | Nonbonding Electron Pairs | VSEPR Formula | Approx. Bond Angle | Geometric Shape |
|---------------------------|-----------------|-----------------------------|------------------------|--------------------------|---------------|--------------------|-----------------|
| 1. CH<sub>4</sub>       | H<br>:<sub>H</sub>C<sub>H</sub>:<br>H  | 4                           | 4                      | 0                      | AX<sub>4</sub>          | 109.5°            | tetrahedral      |

### Additional Exercises
For practice, complete the VSEPR table for the following molecules without strict adherence to the Lewis octet rule. Refer to your laboratory instructor for further guidance.

1. **SnF<sub>2</sub>**
2. **SnF<sub>4</sub>**

Remember to determine the number of valence shell electron pairs, the number of bonding and nonbonding electron pairs, the VSEPR formula, approximate bond angles, and the geometric shape in a similar manner to the table above.

This exercise aims to solidify the understanding of molecular shapes and bond angles using VSEPR theory, crucial for predicting molecular geometry and bonding properties.
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Transcribed Image Text:### VSEPR Theory and Molecular Geometry #### Example Molecule: Methane (CH<sub>4</sub>) The table below demonstrates the application of the Valence Shell Electron Pair Repulsion (VSEPR) theory to determine the molecular geometry of methane. | Molecule or Molecular Ion | Lewis Structure | Valence Shell Electron Pairs | Bonding Electron Pairs | Nonbonding Electron Pairs | VSEPR Formula | Approx. Bond Angle | Geometric Shape | |---------------------------|-----------------|-----------------------------|------------------------|--------------------------|---------------|--------------------|-----------------| | 1. CH<sub>4</sub> | H<br>:<sub>H</sub>C<sub>H</sub>:<br>H | 4 | 4 | 0 | AX<sub>4</sub> | 109.5° | tetrahedral | ### Additional Exercises For practice, complete the VSEPR table for the following molecules without strict adherence to the Lewis octet rule. Refer to your laboratory instructor for further guidance. 1. **SnF<sub>2</sub>** 2. **SnF<sub>4</sub>** Remember to determine the number of valence shell electron pairs, the number of bonding and nonbonding electron pairs, the VSEPR formula, approximate bond angles, and the geometric shape in a similar manner to the table above. This exercise aims to solidify the understanding of molecular shapes and bond angles using VSEPR theory, crucial for predicting molecular geometry and bonding properties.
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