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

2. Energy Level #1 (N = 1) –1–1 sublevel  s 2 electrons Energy Level #2 (N = 2) –2–2 sublevels  s & p 2 + 6 = 8 electrons Energy Level #3 (N = 3) –3–3 sublevels  s, p, & d 2 + 6 + 10 = 18 electrons Energy Level #4 (N = 4) –4–4 subleverls  s, p, d, & f 2 + 6 + 10 + 14 = 32 electrons

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