[opuktun]

Hi, we often learn that orbital hybridization helps us in explaining the bond angle and bond length for simple molecules, e.g. CH4.

But why is it that s and p orbitals undergo hybridization? Is it because the resulting hybridized orbitals are more stable?

[savy2020]

Hybribisation of orbitals requires energy. Even then it occurs since the hybridised orbitals are more efficient tin bond formation more energy id released due to bond formation by overlap of hybridised orbitals

[opuktun]

Hybribisation of orbitals requires energy. Even then it occurs since the hybridised orbitals are more efficient tin bond formation more energy id released due to bond formation by overlap of hybridised orbitals

Thanks, this is a good answer. But how does it lead to "more efficient bond formation?"

[savy2020]

I don't have any reason for the formation of more efficient bond
But that is correct since the bond energies for binds between hybridised orbitals are more than that of the bonds between atomic non-hybridised orbitals
I just guess that there will be higher level overlap of the hybridised orbitals though I don't claim to have any proof for that.

[opuktun]

I just guess that there will be higher level overlap of the hybridised orbitals though I don't claim to have any proof for that.

That's a good point.

What do others think?

[cabaal]

If the carbon didn't hybridize in methane, it wouldn't be able to form more than 2 bonds.

[Borek]

This is not hybrydization (yet).