Construct the molecular orbital diagram for the carbon monoxide molecule. So Co Now here we're going to determine the right molecular orbital diagram. Carbon is less electronegative than oxygen, so we're going to use the molecular orbital diagram for carbon. So use this middle one here. Now remember that the more electronegative element has lower energy in terms of its atomic orbitals, so oxygen will represent this side and carbon will represent this side.
Now, in terms of number of valence electrons, we're going to say here that carbon is in Group fourane, so it has four valence electrons or valence electrons. So it'd be one, up, one down and then up up. Oxygen is in Group 6A, so it has six valence electrons, so one 2345 and then six. We now pull together our electrons in the atomic orbitals and put them into the molecular orbitals. So it'd be up, down, up, down.
Now we have a total of how many electrons here 6 electrons that we basically need to put into these remaining molecular orbitals. So it'd be up, up, down, down, and then we need two more up, down. So this will represent the filled in molecular orbital diagram. For carbon monoxide, we'd come down here and we'd fill it in. So we're going to say we have two of σ2S2 of σ2Sstar.
We see that we have 4-4 π2P and then finally we'd have two in the σ2P. So this would be all the electrons that we have to fill in this electron configuration for carbon monoxide. Now here these would have nothing in them, so you could in theory if you want just remove them from this because there D be 0 in here and zero in here. So we have our molecular orbital diagram above and this would be the completed electron configuration using that molecular orbital diagram for carbon monoxide.