CHM136H1 Lecture : Tutorial 1 Continued.pdf

• School: UTSG
• Department: Chemistry
• Course: CHM136H1
• Professor: C.Scott Browning

Document Summary

1. 11 describing chemical bonds: molecular orbital (mo) theory. Mo theory describes covalent bond formation as arising from a mathematical combination of atomic orbitals (wave functions) on different atoms to form molecular orbitals - so called because they belong to the entire molecule rather than the individual atom. A molecular orbital describes the region in a molecule where electrons are most likely to be found. A mo has a specific size, shape, and energy. Paramagnetic - unpaired electrons weakly attracted to a magnetic field. Diamagnetic - paired electrons even more weakly repelled from a magnetic field. Bond order = 1/2 (#e-s in bonding mo - # e-s in antibonding mo) In molecules with more than a 1s and 1s * the bond order for the non-valence e-s is 0. The filling of orbitals without stars is like constructive interference and the filling of orbitals with stars is like destructive interference.