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CHEM 6A Lecture Notes - Lecture 9: Paramagnetism, Bohr Model, Pauli Exclusion Principle

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29 Oct 2015

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CHEM 6A Full Course Notes

CHEM 6A Full Course Notes

Document Summary

Describes 3d regions of space called orbitals where electrons are likely to be found. Instead of locating electrons, talk about regions with high probability of finding an electron. Ml: magnetic quantum number l: angular quantum number: quantum number in schrodinger"s model, 1) principal quantum number. Describes size of orbital and energy of orbital indirectly. As n increases, so does size of orbital: 2) angular quantum number. Describes shape of orbital (s, p d, f: 3) magnetic quantum number. Describes the orientation of an orbital shells, subshells, and orbitals: space outside nucleus in an atom is called the electron cloud. D contains 5 orbitals f contains 7 orbitals. Aufbau principle: electrons fill orbitals starting with the lowest energy level and moving upwards. Pauli exclusion principle: can be no more than 2 electrons in any orbital and those electrons must have different spins. For a negative ion: add electron to next available orbital.

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Related Questions

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