Question #caf58

1 Answer
David Drayer
Apr 16, 2017

In Carbon monoxide there is no hybridization.

Explanation:

Carbon number 6 has six total electrons this gives an electron configuration. of 1 s^2 2 s^2 2p^2

This leaves the valance configuration of 2^2 2p^2

The two s electrons are paired and are not used in bonding.

The two p electrons are in different p orbitals and able to be used for bonding. Therefore Carbon in it ground state configuration can form only two bonds.

Oxygen with a configuration of 1s^2 2s^2 2p^4 can also form only two bonds so the formation of CO requires no hybridization.

C=O

Related questions
See all questions in Orbital Hybridization
Impact of this question
2161 views around the world
You can reuse this answer
Creative Commons License