# How does an hybridised orbital become unhybridised after bond cleavage?

In $\ce{CH4}$, $1 s$ and $3 p$ orbitals are hybridised into four $sp^3$ orbitals. But on homolytic bond cleavage an unpaired electron remains in an unhybridised $p$ orbital?

Similarly in heterolytic bond cleavage of $\ce{CH4}$, the methyl carbocation has an unhybridised empty $p$ orbital?

• We have had this confusion many times before. See here for some detail. Hybridisation is simply a mathematical quirk to make valence bond theory work better. It doesn't exist in the real world. In methane, the atomic orbitals overlap to form a set of molecular orbitals. $sp^3$ orbitals do not come into the final bonding description of methane (at least in the MO theory version). – bon Jun 28 '15 at 16:04