Chem Atomic Theory

Paschen Series

n—>3, lower energy than visible, in infrared region of EM spectrum

Balmer’s series

n—>2, visible region of EM spectrum

Lyman series

n—>1, too large to be visible, in UV region of EM spectrum

orbital

region in space where the chance of finding an electron is high (90%)

s-orbital

max electrons = 2

p-orbital

3 types (x,y,z) with 2 each (6 total)

d-orbital

5 types, 2 electrons each, 10 total

energy level configuration order

principal quantum number (n)

indicates general energy of orbital (n² = total orbital #)

angular/orbital quantum # (l)

determines type of orbital (s, p, d, f)

magnetic quantum # (ml)

determines type of sub-orbital (Px, Py, Pz, etc)

electron “spin” (intrinsic angular momentum) (ms)

• charge allows electrons to develop a magnetic field as it moves

• depending on direction of spin, they generate the field in a certain orientation

• can spin up (+1/2) or down (-1/2)

Pauli exclusion principle

• no 2 electrons in the same atom can have the same 4 quantum numbers (n, l, ml, ms)

• must be filled lowest energy orbitals to highest

draw an orbital diagram for any element

yay!