Upload
others
View
14
Download
0
Embed Size (px)
Citation preview
• 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
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
• s is the first and
simplest sublevelShape of
“s”
sublevel
• p is the second sublevelShape of
“p”
sublevel
Shape of “d” sublevel
Shape of “f” sublevel
All electrons follow three rules when filling energy levels and sublevels. They are:
• Aufbau Principle
• Pauli Exclusion Principle
• Hund’s Rule
1s2s2p3s3p
Orbital
Diagrams
• An e- occupies the
lowest energy orbital
that can receive it.
• Start at the bottom
Aufbau
Principle
The Hotel Californium
1st floor
2nd floor
5th floor
n = 1
n =2
n = 5
= electron
Aufbau
Principle
• 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
• 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
Hund’s
Rule
• 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
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
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
• 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
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
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 ↓)
• Determine the orbital
diagram for the
following:
▪ Cobalt (Co)
▪ Germanium (Ge)
1s2s2p3s3p4s3d
Cobalt – 27 e- Germanium – 32 e-
1s2s2p3s3p4s3d
4p
7p
6d
5f
7s
6p
5d
4f
6s
5p
4d
5s
4p
3d
4s
3p
3s
2p
2s
1s