CHEM 1A Lecture Notes - Lecture 7: Pauli Exclusion Principle, Noble Gas, Unpaired Electron
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2 peaks that are separated with none going down the middle. 2 states that the electron seems to be in. Electron 4 qns: n, l, m_l, m_s. No two electrons can have the same set of quantum numbers. Hund"s rule: if we have more than one electron and more than one degenerate orbitals, electrons will spread out. Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin. Li has a new unpaired electron in the 2s orbital. 2s energy is less than 2p energy. Each time you make a more complicated shell, pushes up in energy. Principal energy levels overlap as they get larger. N = 1 only has one orbital. Start to spread out parallel according to hund"s rule. Look for nearest noble gas and add valence to it. How many electrons does each element have.
