#sp^3# hybridization - can somebody explain what my book is trying to say?

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This is for #CH_4#. I understand that the electron configuration for #C# contradicts what actually happens in bonding, but I don't understand what #2 is trying to say.

1 Answer
Truong-Son N.
Dec 20, 2017

All it is saying is that invoking hybridization, i.e. mixing of pure, differing atomic orbitals to form new, identical orbitals that are not rigidly #90^@# apart from each other, allows more flexibility in bonding.

Recall that the four valence atomic orbitals (i.e. pure orbitals) of carbon are the #2s# and the #2p_x#, #2p_y#, and #2p_z#.

The #2s# is spherical, with no directionality, while the #2p# orbitals are each aligned along their coordinate axes. The #2p# orbitals DO have directionality, but only along their axes.

http://www.chemtube3d.com/

Since the #2p# orbitals are mutually orthogonal---that is, they are all #90^@# from each other, they cannot form bond angles other than #90^@#, and that is just not what is shown by experiment.

We did not observe

but we did observe

The pure #p# orbitals cannot rotate off their cartesian axes. If they did, they would not exist.

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