Question

# Hybridization of ${CH_3^ - }$ is:A.$s{p^3}$B.$s{p^2}$C.$sp$D.$ds{p^2}$

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Hint:To answer this question, you must recall the concept of hybridization. The concept of mixing of atomic orbitals in order to form new hybrid orbitals that possess different shapes and energies as compared to the original parent atomic orbitals is known as hybridisation.

$C:\left[ {He} \right]2{s^2}2{p^2}$
One electron is excited from the $2s$ orbital to $2p$ orbital to increase the covalency. The electronic configuration in this excited state is given as $C:\left[ {He} \right]2{s^1}2{p^3}$
Now we know that, since carbon forms three bonds, it has one free electron. The negative charge signifies another electron, thus resulting in a lone pair. Carbon has three bond pairs and one lone pair. It undergoes a hybridization of $s{p^3}$.