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Electron Config

Electron Configuration the arrangement of electrons in the energy levels, sublevels and orbitals of atoms
S orbitals spherical orbitals; first to fill for any energy level; can only hold 2 electrons
P orbitals 3 mutually perpendicular dumbbell shaped orbitals; second to fill from 2nd energy level on up; can hold max of 6 electrons
D orbitals 5 orbitals of cloverleaf shape; third to fill for any energy level; beginning in the third shell, can hold a total of 10 electrons.
F orbitals their shapes are even more complex than s, p, or d orbitals; can hold a total of 14 electrons in 7 sub-shells; in the fourth and fifth energy levels
Aufbau Principle states that each electron occupies the lowest energy orbital available
Pauli Exclusion Principle maximum of two electrons may occupy an atomic orbital, but only if they have opposite spins
Hund's Rule electrons occupy equal energy orbitals so as to maximize the number of unpaired electrons
Principle Energy Level main energy level or distance of an electron from the nucleus; (n); correspond to the rows 1-7 on the Periodic Table
Sublevels regions within the energy levels; corresponds to the block grouping s,p,d,f on the Periodic Table
spherical s sublevel
dumbbell p sublevel
clover d sublevel
double clover f sublevel
Orbital Notation Uses circles to represent atomic orbitals with a label underneath to indicate sublevel and energy level
Noble Gas located in group 18 on the Periodic Table.
Isoelectronic two atoms that have the same number of electrons
Valence Electrons Electrons located in the outermost energy level
n Principle quantum number
l Angular momentum quantum number
ml Magnetic quantum number
ms Electron spin quantum number
Created by: Curt