Terms
The arrangement of electrons in the energy levels, sublevels and orbitals of atoms.
Electron Configuration
regions within the energy levels; corresponds to the block grouping s,p,d,f on the Periodic Table
Sublevels
name the element 1s²2s²2p³
Nitrogen
name the element [Ne]3s²3p¹
Aluminum
8
Oxygen
an electron in the highest occupied energy level of an atom
Valence Electron
3 mutually perpendicular dumbbell shaped orbitals; second to fill from 2nd energy level on up; can hold max of 6 electrons
P orbitals
name the element 1s²2s²2p⁶3s²3p¹
Aluminum
name the element [He]2s²2p³
Nitrogen
29
Copper
a region around the nucleus of an atom where electrons are likely to be found
Electron Cloud
spherical orbitals; first to fill for any energy level; can only hold 2 electrons
S orbitals
name the element 1s²2s²2p⁶3s²
Magnesium
name the element [Ar]4s²
Calcium
20
Calcium
maximum of two electrons may occupy an atomic orbital, but only if they have opposite spins
Pauli Exclusion Principle
can hold a total of 14 electrons in 7 sub-shells; in the fourth and fifth energy levels
F orbitals
name the element 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d⁷
Rhodium
name the element [Ne]3s²3p⁵
Chlorine
10
Neon
an electron in a temporarily higher energy level than in its ground state
Excited state
5 orbitals of cloverleaf shape; third to fill for any energy level; beginning in the third shell, can hold a total of 10 electrons.
D orbitals
name the element 1s²2s²2p⁶3s²3p²
Silicon
name the element [Ar]4s²3d¹⁰4p³
Arsenic
19
Potassium