Electron Configuration Chart - Clark College

2
CHEM& 141 F08 3
Filling in Electrons
The Rules:
Aufbau Principle: Electrons fill in electrons by order
of energy, from low high.
Not all orbitals are available for all energy (n) levels.
Pauli Exclusion Principle: Each individual orbital
takes 2 electrons only!
There is one s orbital = 2 electrons.
There are three p orbitals = 6 electrons.
There are five d orbitals = 10 electrons.
There are seven f orbitals = 14 electrons.
Hund’s Rule: If there are multiple orbitals at the
same energy, they fill singly first, before electrons
pair.
CHEM& 141 F08 4
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!
Page 2/16
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