1. Q UANTUM N UMBERS Addresses for electrons

2. P RINCIPAL Q UANTUM N UMBER ( N ) Energy level Size of the orbital n 2 = # of orbitals in the energy level Bigger n = higher energy and bigger orbital

3. A NGULAR M OMENTUM N UMBER, ℓ Describes the overall shape of the orbital Energy sublevel ℓ Subshell Name 0s 1p 2d 3f s p d f

4. n=# of sublevels per level n 2 =# of orbitals per level

5. MAGNETIC QUANTUM NUMBER, M ℓ Orientation of orbitals within a subshell Specifies the exact orbital within each sublevel

6. pxpx pypy pzpz

7. Orbitals combine to form a spherical shape. 2s 2p z 2p y 2p x

8. ℓ Possible Value of m ℓ Number of Orbitals in this Subshell 001 1-1, 0, +13 2-2, -1, 0, +1, +2 5 3-3, -2, -1, 0, +1, +2, +3 7

9. S PIN M AGNETIC N UMBER, M S An orbital can hold 2 electrons that spin in opposite directions. Spin quantum number can have values of +1/2 or -1/2

11. P AULI E XCLUSION P RINCIPLE AND Q UANTUM N UMBERS No two electrons in an atom can have the same 4 quantum numbers. Each electron has a unique “address”. 1. Principal #  energy level 2. Angular Momentum #  sublevel (s,p,d,f) 3. Magnetic #  orbital 4. Spin #  electron

12. Q UANTUM N UMBERS E XPLAINED !

13. C ONCLUSION NPossible Values of Electrons Shellmℓmℓ Numbe r of Orbital s Total Number of Orbitals in Shell 101s011 20101 2s 2p 0 -1, 0, +1 1313 4 3012012 3s 3p 3d 0 -1, 0, +1 -2, -1, 0, +1, +2 135135 9 401230123 4s 4p 4d 4f 0 -1, 0, +1 -2, -1, 0, +1, +2 -3, -2, -1, 0, +1, +2, +3 13571357 16