Question #c0c79

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Question #c0c79

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Answer 1 · 2016-11-02T03:35:53

I disagree with the answer Methane is a classic example of $s p^{3}$ $sp^3$ hybridization.

Explanation:

In its ground state of $1 s^{2} 2 s^{2} 2 p^{2}$ $1s^2 2s^2 2 p^2$ only the unpaired set of two p electrons are able to bond. This would give rise to a formula of $C H_{2}$ $CH_2$ not $C H_{4}$ $CH_4$

Carbon monoxide is an example of Carbon bonding in the ground state not the $s p^{3}$ $sp^3$ hybridized state. CO has formed only two bonds. A double bond between the Carbon and the Oxygen The Lewis dot structure would look like this.
..
: C :: O:

Methane $C H_{4}$ $CH_4$ has formed four bonds requiring the the $s p^{3}$ $sp^3$ hybridization.

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Question #c0c79

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