Why is oxygen not sp2 hybrdized on the CO2 molecule and why does it remain primarily...

Why is oxygen not sp2 hybrdized on the CO2 molecule and why does it remain primarily unhybridized with only p orbitals sticking out?

Expert Solution

In ground state, the electron configuration of Carbon is 1s2 2s2 2p2. You can consider one of the 2s electrons to be excited to fill the other empty 2p orbital to give a configuration of 1s2 2s1 2p3. Each 2p orbital, 2px 2py and 2pz now holds one electron. The 2s and one of the 2porbitals, say the 2py can hybridize and form 2 sp hybrid orbitals.

Oxygen has the ground state electron configuration 1s2 2s2 2p4. Two of the 2p orbitals, say the 2px and the 2pz only hold one electron. The 2px can now overlap with one of the sp hybrids from the carbon to form a σ bond. The 2pz can now overlap with the unhybridized 2pz on the carbon to form a π bond.

The same thing can happen on the other side of the carbon forming another σ bond with Oxygen’s 2pz and a π bond with the 2py orbitals from each atom.It is because CO2 is linear in nature and hence the sp hybridization.

queen_honey_blossom answered 2 years ago

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