Electron Configurations
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Transcript Electron Configurations
Electron
Configurations
“Any one who is not shocked
by Quantum theory does
not understand it.”
Niels Bohr
Electron Configurations
The quantum mechanical model of the atom
predicts energy levels for electrons; it is
concerned with probability, or likelihood, of
finding electrons in a certain position.
Electron Configurations
Regions where electrons are likely to be
found are called orbitals. EACH ORBITAL
CAN HOLD UP TO 2 ELECTRONS!
Electron Configurations
In quantum theory, each electron is assigned
a set of quantum numbers
analogy: like the mailing address of an
electron
Principal Quantum Number (n)
Describes the energy level that the electron occupies
n=1, 2, 3, 4
n=1
n=2
n=3
n=4
The larger the value of n, the farther away from the
nucleus and the higher the energy of the electron.
**Electrons always start filling in the lowest
possible energy level available (AUFBAU
PRINCIPLE)
Sublevels (l)
The number of sublevels in each energy level is
EQUAL to the quantum number, n, for that energy
level.
Sublevels are labeled with a number that is the
principal quantum #, and a letter: s, p, d, f (ex: 2 p
is the p sublevel in the 2nd energy level)
***REMEMBER THIS… let’s start filling in the chart
Sublevels (l)
Principal Energy Level
Sublevels
Orbitals
n=1
1s
2s
2p
one (1s)
one (2s)
three (2p)
n=3
3s
3p
3d
one (3s)
three (3p)
five (3d)
n=4
4s
4p
4d
4f
one (4s)
three (4p)
five (4d)
seven (4f)
n=2
Sublevels (l)
Sublevel
# of orbitals
Max # of electrons
s
1
2
p
3
6
d
5
10
f
7
14
ONLY 2 electrons per 1
orbital!!!!!
Electron Configurations
NOTICE!!!!!! 3d is on the 4th
energy level (d block is n-1)
Complete electron configurations
helium
1s2
boron
1s22s22p1
neon
1s22s22p6
aluminum
1s22s22p63s23p1
Uranium
(follow your
periodic table)
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f4
Abbreviated electron diagrams
helium
boron
(AKA: noble gas config.)
1s2
[He]2s22p1
N3-
= [Ne]
aluminum [Ne]3s23p1
cobalt
[Ar]4s23d7
uranium
[Rn]7s25f4
[He]2s22p6
Se2-
Mg2+
= same # of
electrons as a Kr
atom: [Ar]
4s23d104p6
= same # of
electrons as a
Ne atom: [He]
2s22p6
Spin quantum number (ms)
Labels the orientation of the electron
Electrons in an orbital spin in
opposite directions; these
directions are designated as
+½ and -½
Pauli Exclusion Principle
States that no 2 electrons have an
identical set of four quantum #’s to
ensure that no more than 2 electrons
can be found within a particular
orbital.
Hund’s Rule
Orbitals of equal energy are each occupied by
one electron before any pairing occurs.
Repulsion between electrons in a single orbital is
minimized
(ex: you want your own bedroom before you would
have to share a bedroom with a sibling)
All electrons in singly occupied orbitals must have
the same spin (such as in the p sublevel).
When 2 electrons occupy the same orbital they must
have opposite spins
(want to be a little different. You wouldn’t want to
wear the exact same clothes as your brother or
sister, right?!)
Orbital Diagrams
Each orbital is represented by a box.
Each electron is represented by an arrow.
Orbital Diagrams
hydrogen
1s
helium
1s
carbon
1s
2s
2p