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Spin pairing and overlapping theory cannot explain the equal bond length as well as equal bond angles in CH₄ molecule. To explain the above facts we are in need of hybridization theory. Hybridization is the mixing of atomic orbitals of comparable energy and the number of atomic orbitals involved Is equal to the number of hybrid orbitals formed of equal energy.
Increasing order of the energy of hybrid orbitals is:

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$s p^{3} < s p^{2} < s p$

$s p^{2} < s p^{3} < s p$

$s p < s p^{3} < s p^{2}$

$s p < s p^{2} < s p^{3}$

answer is D.

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Detailed Solution

The sp orbital is closer to nucleus, so has lower energy. So, Increasing order of the energy of hybrid orbitals is,

$s p < s p^{2} < s p^{3}$

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