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I am trying to understand hybridisation. In methane carbon has $\mathrm{sp^3}$ hybridisation, but what is the hybridisation of hydrogen? Is it $\mathrm{sp^3}$? If yes then why?

Wildcat
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Matix
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    What orbitals does hydrogen have available for bonding? – bon Jun 26 '16 at 09:27
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    Orbitals of hydrogen atoms aren't hybridised in $\ce{CH4}$ at all: 1$\mathrm{s}$ orbital of each hydrogen atom forms a $\sigma$-bond with one of the four $\mathrm{sp^3}$-hybridised orbitals of the carbon atom. – Wildcat Jun 26 '16 at 09:28
  • Also, per calculations and experimental data, you could also argue for an unhybridised carbon since there are two different energies of the binding MOs. – Jan Jun 26 '16 at 16:56
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    You should answer your own question so that it may be useful to future users. – bon Jul 12 '16 at 10:21

2 Answers2

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Hydrogen does not hybridise, as it only has one filled $s$ orbital. Hybridisation is the "mixing of $s$ and $p$ orbitals; here is a good explanation (for ethane, but it explains the general theory as well).

Marcel
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it is always possible to find the hybridization of the central atom i.e., Carbon. The atomic orbital of hydrogen does not undergo hybridization.

Preethika Sampath Kumar
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