Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: ZanyCat on May 26, 2013, 05:30:06 AM
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I'll use CO2 as an example.
So the energy-level diagram for the carbon has: one 1s orbital, two 2sp orbitals and two 2p orbitals, listed from lowest to highest energy.
Ignoring the 1s, there are 4 valence electrons. In my way of thinking, the lowest energy shells should be filled first, so we would have :spinpaired: :spinpaired: in the sp hybridised orbitals, and 'empty' 2p orbitals.
But clearly, there's a pi bond, so in reality we have :spinup: :spinup: in the 2sp orbitals and :spinup: :spinup: in the 2p orbitals.
Where is my thinking going wrong? Thanks!
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You also have electrons from the oxygen atoms.