4.9 – NOTES Electron Configurations

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Presentation transcript:

4.9 – NOTES Electron Configurations

III. Electron Configurations A. Ground-state electron configurations 1. The aufbau principle electrons start at the lowest level possible;

2. Pauli Exclusion principle - no 2 electrons can have the same 4 quantum #s; - even # of electrons – element can be paramagnetic or diamagnetic - odd # of electrons – element must be paramagnetic - if e- spin same way  should be paramagnetic (attracted by magnets); spin opposite way  diamagnetic (slightly repelled by magnet; ex – He)

3. Hund’s rule - most stable arrangement of e- in subshells, one w/ greatest # of parallel spins; result electrons will NOT pair (due to repulsion) until forced to do so.

B. Orbital diagrams and electron configuration notations There are 2 representations of electron configurations: orbital notation and electron configuration notation. We will start with hydrogen and work our way through the periodic table, writing both configurations. Orbital e- configs Hydrogen:

Helium: Lithium:

Beryllium: Boron:

Carbon: Nitrogen:

Oxygen: Fluorine:

Neon: