Q UANTUM N UMBERS Addresses for electrons

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

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

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

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

pxpx pypy pzpz

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

ℓ Possible Value of m ℓ Number of Orbitals in this Subshell , 0, , -1, 0, +1, , -2, -1, 0, +1, +2, +3 7

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

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

Q UANTUM N UMBERS E XPLAINED !

C ONCLUSION NPossible Values of Electrons Shellmℓmℓ Numbe r of Orbital s Total Number of Orbitals in Shell 101s s 2p 0 -1, 0, s 3p 3d 0 -1, 0, +1 -2, -1, 0, +1, s 4p 4d 4f 0 -1, 0, +1 -2, -1, 0, +1, +2 -3, -2, -1, 0, +1, +2,