![]() Note that all of the p bonds have C 2 antisymmetry about the internuclear axis. Note that all of the s bonds have cylindrical symmetry (or a C-infinity rotation element) about the internuclear axis. Based on the above reasoning, we would predict that the molecular orbital energy level diagram for diatomic N 2 would look something like this: We can show one of the p molecular orbitals in the plane of the page we picture the other one tilted to indicate that it is perpendicular to the plane of the page. They do not show as dramatic an energy difference from the nitrogen atomic orbitals because side-on overlap is not as good as head-on overlap. This generates the 2p p and 2p p * molecular orbitals. Each nitrogen also has two p orbitals perpendicular to the internuclear axis that have side-on, or p, overlap with the corresponding p orbitals on the other nitrogen atom. This generates the 2p s and 2p s * molecular orbitals. Each nitrogen atom has one p orbital lying along the internuclear axis that has head-on, or s, overlap with the corresponding p orbital on the other nitrogen atom. Note that the p orbitals of the two nitrogen atoms interact in two ways. The atomic electrons shown on the sides go into the molecular orbitals in the middle when the two nitrogen atoms interact. ![]() The molecular s and p bonding and antibonding orbitals are shown in the middle of the diagram. These atomic electrons are shown on either side of the molecular orbital diagram. Each nitrogen atom has the electron configuration 1s 22s 22p 3. This handout is in response to questions about the energy level ordering for homonuclear diatomics. ![]()
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