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So, I was wondering that how can a methane molecule form four $\mathrm{sp^3}$ hybrid orbitals, with each hybrid orbital containing one $\mathrm s$ and three $\mathrm p$ orbitals.
In four of such $\mathrm{sp^3}$ hybrid orbitals, it makes a total of four individual $\mathrm s$ orbitals and twelve individual $\mathrm p$ orbitals; whereas, we only have, numerically, one $\mathrm s$ orbital and three $\mathrm p$ orbitals available that constitute in hybridization.
As has been pointed out in the comments, an $\mathrm{sp}^3$ orbital is a linear combination not of one s orbital and three p orbitals, but rather of one part s orbital and three parts p orbital. Stated differently, the numbers in $sp^3$ denotes the ratio and not the number of orbitals we combine.
Oddities such as the $\mathrm{sp^5}$ orbitals in cyclopropane can therefore be rationalised. It does not mean that there are five p orbitals which form hybrids, which is obviously impossible. It simply means that that particular orbital has ~1/6 s orbital character and ~5/6 p orbital character.
