## Homework Help: Problem 4.73

$sp, sp^{2}, sp^{3}, dsp^{3}, d^{2}sp^{3}$

John Huang 1G
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### Homework Help: Problem 4.73

4.73 (a) Draw a Lewis structure for each of the following species (b) Identify each as a radical or not. (c) Rank them in order of increasing HCH bond angles. Explain your choices.

How do I determine the bond angles of a molecule such as (CH3)-? The molecule results in having a central Carbon atom, with 3 Hydrogen single bonds, and ONE lone electron. Do I approach this molecule seeing it as a tetrahedral, or as a trigonal planar?

Eryn Wilkinson 3H
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Joined: Fri Sep 29, 2017 7:07 am

### Re: Homework Help: Problem 4.73

The shape would actually be approached as trigonal pyramidal, because the VSEPR formula is AX3E. This means that there is one lone pair on top, and 3 bonding pairs of electrons being repelled by it. The bond angles would be slightly less than 109.5 degrees, which is the usual bond angle for tetrahedral shape, because the lone pair has a greater repulsion strength than if it were a bonded pair.

104922499 1F
Posts: 53
Joined: Fri Sep 29, 2017 7:04 am

### Re: Homework Help: Problem 4.73

you should approach this problem as a trigonal pyramidal because with VSEPR formula is AX3E