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If a carbon atom is bonded to another atom/s with only single bonds, will it always have a hypridization of 2sp3? Since regions of e- density is equal to the number of hybrid orbital, as long as carbon is not bonded with a double or triple bond, it will always have 4 hybrid orbitals right?
Yes. Carbon typical forms 4 singles bonds. Each of these single bonds will have a hypridization of 2sp3. This is because we need a better way to explain how carbon can form 4 bonds if we usually see the valence electrons written as 2s2 2p2.
So if there's a double bond, and 2 single bonds on carbon, the hybridization would be sp2? How does that work in respect to valence electrons?
Each C will have three regions of electron density and will need three hybrid orbitals. Trigonal Planar makes each C sp2 hybridized. There will be 3 electrons in the 2sp2 region and 1 unpaired electron in 2p which is higher in energy than the hybridized region. The unhybridized 2p orbital on each C overlap side by side to form a pi bond. the double bond is one sigma and one pi bond.
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