Erwin Schrodinger...
Transcript of Erwin Schrodinger...
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• Erwin Schrodinger proved
Bohr’s idea wrong
• Said electrons do not move
around in fixed orbits around
the nucleus
• But rather proved that
electrons move in 3D areas
around the nucleus
• Showed the probability of
where an e- may be in the
atom
Today’s
Atom
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Energy
Levels,
Sublevels
and
Orbitals
• Within the energy levels
are 3D areas called
sublevels that have their
own significant shape
• Inside sublevels there are
orbitals, where e- are
arranged
Sublevel
name
# of
orbitals# of e-
s 1 2
p 3 6
d 5 10
f 7 14
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• s is the first and
simplest sublevelShape of
“s”
sublevel
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• p is the second sublevelShape of
“p”
sublevel
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Shape of “d” sublevel
Shape of “f” sublevel
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All electrons follow three rules when filling energy levels and sublevels. They are:
• Aufbau Principle
• Pauli Exclusion Principle
• Hund’s Rule
1s2s2p3s3p
Orbital
Diagrams
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• An e- occupies the
lowest energy orbital
that can receive it.
• Start at the bottom
Aufbau
Principle
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The Hotel Californium
1st floor
2nd floor
5th floor
n = 1
n =2
n = 5
= electron
Aufbau
Principle
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• A maximum of two
electrons may occupy a
single orbital, but only
if the electrons have
opposite spins
• Two e- per orbital, one
up, one down
Pauli
Exclusion
Principle
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• Orbitals of equal energy
are each occupied by
one e- before any orbital
is occupied by a second
e- and all e-s in singly
occupied orbitals must
have the same spin
state.
• Split them up before you
pair them up
Hund’s
Rule
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Hund’s
Rule
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• Includes a line for each
of the atom’s orbitals
• Lines are filled with
arrows representing
electrons
▪ Up and down facing
arrows to show opposite
spins
Orbital
Diagrams
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Sublevel
name
# of
orbitals
Amt. of
Electrons
s 1 2
p 3 6
d 5 10
f 7 14
sublevel # of lines # of arrows in
sublevel
Sublevels,
orbitals &
# of
electrons
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Orbital Diagrams
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d 6f
7s 7p 7d 7f
1s2s2p3s3p4s3d
Incr
easi
ng e
ner
gy
Start on bottom of first arrow,
go up the arrow, then go to
bottom of the next arrow, go up
the arrow and repeat
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• Remember the rules
electrons follow when
filling energy levels,
sublevels and orbitals
▪ Aufbau Principle
▪ Pauli Exclusion Principle
▪ Hund’s Rule
• Let’s determine the
orbital diagram for
Phosphorus
▪ 15 electrons
Orbital
Diagrams
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1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d 6f
7s 7p 7d 7f
7p
6d
5f
7s
6p
5d
4f
6s
5p
4d
5s
4p
3d
4s
3p
3s
2p
2s
1s
Orbital diagram
for 118 electrons
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Filling in Orbital Diagrams:
• The first 2 e- go into 1s orbital
(line )
• only 13 more to go...
• Next e- go into 2s orbital
• only 11 more…
• Next e- go into 2p orbital
• Up, up, up then down, down, down
• only 5 more…
• Next e- go into 3s orbital
• only 3 more…
• Last e- go into 3p orbital
• e- by themselves before being
paired
• 3 unpaired e-
1s2s2p3s3p4s3d
Notice the opposite
spins (one ↑, one ↓)
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• Determine the orbital
diagram for the
following:
▪ Cobalt (Co)
▪ Germanium (Ge)
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1s2s2p3s3p4s3d
Cobalt – 27 e- Germanium – 32 e-
1s2s2p3s3p4s3d
4p
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7p
6d
5f
7s
6p
5d
4f
6s
5p
4d
5s
4p
3d
4s
3p
3s
2p
2s
1s