CHEM 1E03 Lecture Notes - Fall 2018 Lecture 8 - Ion, Molecular orbital theory, Triple bond

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1E03
• Professor: Randall Dumont; Linda Davis

Document Summary

Electronic structure of a set of covalently bonded atoms. Orbitals - electrons go in in pairs. Group 1 atom one val e. They tell us which atom is central least en. H only form one bond (terminal, non central atom) Exceptions: be, b, al (in gas phase), atoms in group 2, 13: we form multiple bonds to fulfill the octet rules for atoms missing required electrons, not always. Not all molecules have octets - some have more, some have less. No 2 less en n has 7e - s in val shell: When es are paired up, stable states, transitions b/w excited and ground states requires uv light. No2 excited states are lower in energy, closer, transition involves blue light. The lewis structure of o2 doesnt give the right explanation of the electronic structure. Molecular orbital theory explains electronic structure of o 2 - its a diradical.