CHEM 214 Lecture Notes - Lecture 27: Diatomic Molecule, Sigma Bond, Pi Bond

• School: McGill University
• Department: Chemistry
• Course: CHEM 214
• Professor: Anthony Mittermaier

Document Summary

2s orbitals combined to form a sigma bond, in comparison with the 1s combination, we can observe one radial type node: symmetric. These are all the mo"s you can get from 2nd row of homonuclear diatomics: Here they are simplified, with their energy ordering as per o2 and f2 (final exam): Early triumph of qm, people understood ionic bonds for a lot time. Not a good theory to explain why homonuclear diatomic would form (why oxygen is paramagnetic). Schrodinger equation was defined, it explained electron configuration and bond strength of 2nd row. Important thing is that there is difference in configurations for f2 and o2 in terms of the ordering of 3sg (pz) and 1pu (px and py). In o2 or f2, 3sg is lower in energy than 1pu. In contrast, for n2, 3sg is higher in energy than 1pu. F2: memorize ordering (final exam), overall bond order is 1 (single bond).