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An explanation of electron configuration in the Quantum Mechanical Model of the Atom, using relatable analogies and diagrams. It covers the concept of energy levels, sublevels, orbitals, and the rules governing their occupation by electrons. The document also includes exercises for drawing orbital diagrams for specific elements.
What you will learn
Typology: Lecture notes
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Electrons are important because they
determine how elements will bond and react
with other elements.
Energy Levels –
give the general distance from the nucleus
1s
2s
3s
4s
1s
5s
6s
7s
2 p
3 p
4 p
5 p
6 p
7 p
3 d
4 d
5 d
6 d
4f
5f
Color YOUR Periodic Table!
Energy Level –
Principal Quantum #
(possibilities are 1-7)
Sublevel
(s, p, d, or f)
s: 1 or 2
p: 1-
d: 1-
f: 1-
If you add up all of the electrons, it should equal the atomic #
of the element
Example:
2
2
6
2
6
2
6
Highest energy electron
1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
6
1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
10
4p
6
5s
2
4d
10
5p
6
6s
2
4f
14
5d
10
6p
2
1s
2
2s
2
2p
4
Lewis Dot Structures – show only
the valence electrons.
Lewis Dot Structures – show only
the valence electrons.
C
-