More poison but where is triple bond?
Carbon monoxide, none of the five pairs of orbits \(n=5\), stands out to be counted as part of triple bond.
Unfortunately,
This is not valid for carbon dioxide, \(CO_2\). As the molecule is linear, but in that case, the center \(C\) does not have a valid Quantum Number. There is however another solution,
Carbon has an \(n=2\). Two Oxygen atoms are bonded to the Carbon orbits that are perpendicular to each other. But being free to rotate, one of the orbits rotates by \(90^o\), still rotating in a plane perpendicular to the other orbit pair and spreads the two oxygen atoms furthest apart. The molecule is then linear.
Hew!
