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URL:https://www.learndesk.us/class/4795746681356288/lesson/0c4c2dc922a8a2efa501bd76c995a7b4?ref=outlook-calendar
SUMMARY:Unit 5
DTSTART;TZID=America/Los_Angeles:20260501T190000
DTEND;TZID=America/Los_Angeles:20260501T200000
LOCATION:https://www.learndesk.us/class/4795746681356288/lesson/0c4c2dc922a8a2efa501bd76c995a7b4?ref=outlook-calendar
DESCRIPTION: Electron configuration describes the electronic structure of an atom, an important principle to understand as it underlies chemical reactivity including bonding capabilities and magnetism amongst other chemical properties of the elements. There are a range of different orbitals with distinct energy levels, each holding a maximum of 2 electrons, with electrons occupying orbitals according to Hund’s rule, and the Aufbau and Pauli-Exclusion principles, such that atoms exist in the lowest possible energy state. In any one electron shell, an atom may fill up to one s orbital, three p orbitals, 5 d orbitals and 7 f orbitals. Each type of orbital is degenerate within any electron shell level, however not all of these orbital types exist in all of the electron shells. Hund’s rule: When electrons occupy degenerate orbitals, they must first occupy empty orbitals before doubly occupying any one of the degenerate orbitals. Aufbau principle: Electrons occupy orbitals in order of...

https://www.learndesk.us/class/4795746681356288/lesson/0c4c2dc922a8a2efa501bd76c995a7b4?ref=outlook-calendar
STATUS:CONFIRMED
SEQUENCE:3
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