University:
York University
Course:
CHEM 1000 | Chemical Structure
Academic year:

2021
Views:

54

Pages:

3
Author:

Niklas

Lecture 1 (01/12/21) Electron Config. (amt of e) Quantum #s principal (n) azimuthal (s, p, d, f) Spin (+1/2, -1/2) *up/down ex: CARBON 1s²2s²2p² 4 valence e Consider: Methane CH₄ H | H-C-H | H tetrahedral 4 covalent C-H Bonds Non-polar Gas Unreactive Carbon: 1s²2s²2p² Hydrogen: 1s¹ Lewis Theory of Chemical Bonding: Atoms share val. e to boost the # count of others & themselves. Complete or Fill val. shell C/N/O/Halogens val. e = (octet rule) H val. e = 1 Boron doesn't always follow octet rule. Formal Charge Formal Charge = #Ve - #B - #NBe Cf = #Ve - #B - #NBe (#LP x 2) ex: Nitrate Anion NO₃⁻ O || O-N-O | O Nomenclature: Heteroatom: Any atom which is not C/H/metal. (B/Si/N/O/S/Halogens) R- "Substituent" (generic group) "more or less a place holder" Me/CH₃/Methyl = R-C ex: trimethylamine Me | Me-N-Me | Me Cf(N) = 5 - 3 - 2 = 0 Cheat Sheet: Oxygen (-): 1B 3LP (-): 2B 2LP (-): 3B 1LP (0): 3B 1LP (0): 4B 0LP (0): 5B 0LP Nitrogen (-): 2B 3LP (-): 3B 2LP (-): 4B 1LP (0): 4B 1LP (0): 5B 0LP (0): 6B 0LP Carbon (-): 3B 1LP (0): 4B 0LP (0): 5B 0LP