Asked by Natash
what is the appropriate hybridization for the carbon atom in CO2?
the explanation I was given is 2 electron groups around the center atom carbon suggest sp hybridization. the 2 unhibridized p orbitals on carbon form the 2 pi bonds.
My question is why pi bonds? Isn't it supposed to be sigma ?
the explanation I was given is 2 electron groups around the center atom carbon suggest sp hybridization. the 2 unhibridized p orbitals on carbon form the 2 pi bonds.
My question is why pi bonds? Isn't it supposed to be sigma ?
Answers
Answered by
DrBob222
The CO2 molecule is
O=C=O
In a double bond, one bond is the sigma and the other is a pi. In triple bonds, one sigma and two pi bonds.
O=C=O
In a double bond, one bond is the sigma and the other is a pi. In triple bonds, one sigma and two pi bonds.