1. Ch. 4 Arrangement of Electrons in Atoms
TABLE 4 – 2 (pg. 104)
Principal Quantum Number
Main Energy Level (1-7)
Orbital Quantum Number
Sublevels  S, P, D, F
S = 1 orbitals  2 electrons
P = 3 orbitals  6 electrons
D = 5 orbitals  10 electrons
F = 7 orbitals  14 electrons

2. Energy Level #1 (N = 1)
1 sublevel  s
2 electrons
Energy Level #2 (N = 2)
2 sublevels  s & p
2 + 6 = 8 electrons
Energy Level #3 (N = 3)
3 sublevels  s, p, & d
= 18 electrons
Energy Level #4 (N = 4)
4 subleverls  s, p, d, & f
= 32 electrons

3. Orbital Notation – uses symbols to represent the number of electrons in each sublevel.
Arrows represent the electrons.
Electron–configuration Notation – uses superscripts to represent the number of electrons in each sublevel orbital
No superscript represents no electrons present in the sublevel.
Long hand vs. Short hand
Electron–dot Notation – shows the elctrons in the outer most or highest energy level.