CHEM 11200 Lecture Notes - Lecture 9: Diamagnetism, Noble Gas
19 Jul 2020
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Electron configuration: aufbau principle: electrons occupy the lowest energy orbitals available, hund"s rule: electrons occupy each subshell singly before pairing up, pauli exclusion rule: only two electrons per orbital, one of each spin state. Diamagnetic: atom that has all of its electrons spin paired. Paramagnetic: atom that does not have all of its electrons spin paired. Count the number of electrons in the element. Place electrons in each subshell (following the rules) in the following order. 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p (go left to right) Stop when you hit the proper number of electrons. Since the noble gases have all their electrons filled (complete octet), we can use the closest noble gas and pick up from the next subshell. In some instances, atoms achieve a lower energy state (more desired) by having a filled or half filled d subshell and therefore electrons will be moved from the s subshell before it into the d subshell.
