Electron Configuration Chart - Clark College
3
CHEM& 141 F08 5
Filling in Electrons
n = 1 → 1s orbital → 2 electrons
n = 2 → 2s orbital → 2 electrons
→ 2p orbital → 6 electrons
n = 3 → 3s orbital → 2 electrons
→ 3p orbital → 6 electrons
→ 3d orbital → 10 electrons
n = 4 → 4s orbital → 2 electrons
→ 4p orbital → 6 electrons
→ 4d orbital →10 electrons
→ 4f orbital → 14 electrons
Beyond n = 4, all
levels have s, p, d
and f orbitals.
Lower energy rows
have fewer orbitals
available, therefore
there are fewer
elements there!
CHEM& 141 F08 6
Filling in Electrons
Electrons get filled into orbitals individually:
s:
p:
orbital with
1 electron
unoccupied
orbital
orbital with
2 electrons
One electron Two electrons Three electrons
Four electrons Five electrons Six electrons
The Pauli
Exclusion
Principle!
Hund’s Rule: fill orbitals singly first, then start pairing!
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