CHM135H1 Lecture Notes - Lecture 1: Valence Bond Theory, Pauli Exclusion Principle, Octet Rule
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CHM135H1 Full Course Notes
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Document Summary
Atomic mass: average weighted mass (of different isotopes) Tetravalent- 4 bonds: 4 valence electrons available for bonding, most stable configuration. Quantum mechanics: describes electron energies & locations with wave functions. Psy2: where electrons are most likely to be found. Electron cloud has no specific boundary- only most probable areas. 4 different orbitals- s, p, d, f. Orbitals grouped in shells of increasing size & energy: s- spherical, p- dumbbell, d- cloverleaf. Atomic structure: electron configurations: aufbau"s principle: lowest-energy orbitals fill first, pauli exclusion principle: only 2 electrons in each shell & have opposite, hund"s rule: fill empty shells w/ 1 electron first. Possible to promote an electron from lower energy shell to higher. Covalent bonds: bonding through sharing electrons between two atoms: dashed bond- into the paper, wedged bond- out of the paper, line bond- in the plane of the page. Kekule structures: line b/w atoms indicating electron sharing.
