electron arrangement what do we know?. electron arrangement what do we know? e- are in the e- cloud
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Electron ArrangementWhat do we know?
Electron ArrangementWhat do we know?
• e- are in the e- cloud
Electron ArrangementWhat do we know?
• e- are in the e- cloud
• e- are responsible for the volume of the atom
Bohr Model
Bohr Model
• e- move certain distances from the nucleus
Bohr Model
• e- move certain distances from the nucleus–close to nucleus have less E–E increases as e- move away from
nucleus
• e- move with certain speeds due to E
• e- move with certain speeds due to E–give off E only when they move to
a lower E level
• e- move with certain speeds due to E–give off E only when they move to
a lower E level
• outer most e- are called valence e- and have the most E
• e- move with certain speeds due to E–give off E only when they move to
a lower E level
• outer most e- are called valence e- and have the most E–valence e- determine behavior of
atoms and are involved in bonding
Energy state of an e- is described by a set of 4 numbers called
quantum numbers
Energy state of an e- is described by a set of 4 numbers called
quantum numbers QN - describe the most probable
location of e- in terms of:
Energy state of an e- is described by a set of 4 numbers called
quantum numbers QN - describe the most probable
location of e- in terms of:1. distance from the nucleus
Energy state of an e- is described by a set of 4 numbers called
quantum numbers QN - describe the most probable
location of e- in terms of:1. distance from the nucleus2. shape of the orbital
Energy state of an e- is described by a set of 4 numbers called
quantum numbers QN - describe the most probable
location of e- in terms of:1. distance from the nucleus2. shape of the orbital3. position of orbital in 3 axis of space
Energy state of an e- is described by a set of 4 numbers called
quantum numbers QN - describe the most probable
location of e- in terms of:1. distance from the nucleus2. shape of the orbital3. position of orbital in 3 axis of space4. direction of spin of e-
I. Principal Quantum Number
I. Principal Quantum Number
• indicates the most probable distance of an e- from the nucleus
I. Principal Quantum Number
• indicates the most probable distance of an e- from the nucleus
Energy Level Shell Total # of e-
I. Principal Quantum Number
• indicates the most probable distance of an e- from the nucleus
Energy Level Shell Total # of e-
1
2
3
4
5
6
7
I. Principal Quantum Number
• indicates the most probable distance of an e- from the nucleus
Energy Level Shell Total # of e-
1 K
2 L
3 M
4 N
5 O
6 P
7 Q
I. Principal Quantum Number
• indicates the most probable distance of an e- from the nucleus
Energy Level Shell Total # of e-
1 K 2
2 L
3 M
4 N
5 O
6 P
7 Q
I. Principal Quantum Number
• indicates the most probable distance of an e- from the nucleus
Energy Level Shell Total # of e-
1 K 2
2 L 8
3 M
4 N
5 O
6 P
7 Q
I. Principal Quantum Number
• indicates the most probable distance of an e- from the nucleus
Energy Level Shell Total # of e-
1 K 2
2 L 8
3 M 18
4 N
5 O
6 P
7 Q
I. Principal Quantum Number
• indicates the most probable distance of an e- from the nucleus
Energy Level Shell Total # of e-
1 K 2
2 L 8
3 M 18
4 N 32
5 O
6 P
7 Q
I. Principal Quantum Number
• indicates the most probable distance of an e- from the nucleus
Energy Level Shell Total # of e-
1 K 2
2 L 8
3 M 18
4 N 32
5 O 32
6 P …
7 Q …
I. Principal Quantum Number
• can be determined from the period/series number on the periodic table
II. Orbital Quantum Number
II. Orbital Quantum Number
• indicates shape of the orbital cloud
II. Orbital Quantum Number
• indicates shape of the orbital cloud
• 4 orbital shapes, represented by letters
II. Orbital Quantum Number
s lowest E
II. Orbital Quantum Number
s lowest E
pdf highest E
II. Orbital Quantum Numbermax # e-
s 2p 6d 10f 14
II. Orbital Quantum Number
# of orbital shapes is = to the principal QN
Principal QN
# orbital shapes
types of orbitals
1
2
3
4
Principal QN
# orbital shapes
types of orbitals
1 1
2
3
4
Principal QN
# orbital shapes
types of orbitals
1 1 s2
3
4
Principal QN
# orbital shapes
types of orbitals
1 1 s2 2
3 3
4 4
Principal QN
# orbital shapes
types of orbitals
1 1 s2 2 s, p3 3
4 4
Principal QN
# orbital shapes
types of orbitals
1 1 s2 2 s, p3 3 s, p, d4 4
Principal QN
# orbital shapes
types of orbitals
1 1 s2 2 s, p3 3 s, p, d4 4 s, p, d, f
III. Magnetic Quantum Number
III. Magnetic Quantum Number
• describes the orbital positions with respect to the 3 axis of space
III. Magnetic Quantum Number
III. Magnetic Quantum Number
• describes the orbital positions with respect to the 3 axis of space
• each position, regardless of type can only hold a maximum of 2 e-
s orbital/sublevel
s orbital/sublevel
• 1 orbital position for “s”
s orbital/sublevel
• 1 orbital position for “s”
• spherical shape
s orbital/sublevel
• 1 orbital position for “s”
• spherical shape
• lowest possible energy sub-level
s orbital/sublevel
• 1 orbital position for “s”
• spherical shape
• lowest possible energy sub-level
• all energy levels have an s orbital1s, 2s, 3s, 4s…
p orbital/sublevel
p orbital/sublevel
• second energy sublevel… more E
p orbital/sublevel
• second energy sublevel… more E
• 3 possible “p” orbitals per E Level
p orbital/sublevel
• second energy sublevel… more E
• 3 possible “p” orbitals per E Level
• 6 total e- possible in “p” sub-group
p orbital/sublevel
• second energy sublevel… more E
• 3 possible “p” orbitals per E Level
• 6 total e- possible in “p” sub-group
• 2p, 3p, 4p, 5p…
d orbital/sublevel
d orbital/sublevel
• 5 possible “d” orbitals per E Level
d orbital/sublevel
• 5 possible “d” orbitals per E Level
• 10 total e- possible in “d” sub-group
d orbital/sublevel
• 5 possible “d” orbitals per E Level
• 10 total e- possible in “d” sub-group
• 3d, 4d, 5d…
f orbital/sublevel
f orbital/sublevel
• 7 possible “f” orbitals per E Level
f orbital/sublevel
• 7 possible “f” orbitals per E Level
• 14 total e- possible in “f” sub-group
f orbital/sublevel
• 7 possible “f” orbitals per E Level
• 14 total e- possible in “f” sub-group• 4f, 5f
Quantum number summaryOrbitals Positions electrons
ADD these to your e- in Atoms Questions
13) What is the Octet rule?14) Describe what happens to e- when atoms absorb energy?15) How does quantum mechanics differ from classical mechanics?
Orbital Filling Chart
Order for filling orbitals1s 2s 2p 3s 3p 4s 3d 4p 5s 4d . . .
Aufbau Principle – e- occupy orbitals of lowest E 1st
* 4s is lower E than 3d
Order for filling orbitals
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d . . .
e- configuration
Quantum Number Rewind
Orbital Filling Chart
e- configuration
Write the e- configuration for the following:
1. beryllium2. carbon3. sodium4. magnesium
5. aluminum6. potassium
**EC: bromine
Quantum Numbers
Principle
Principle
[E level] (n)
Principle
[E level] (n)
Orbital
Principle
[E level] (n)
Orbital
[shape](l)
Principle
[E level] (n)
Orbital
[shape](l)
Magnetic
Principle
[E level] (n)
Orbital
[shape](l)
Magnetic[positions
per orbital]
(m)
Principle
[E level] (n)
Orbital
[shape](l)
Magnetic[positions
per orbital]
Number of e- per orbital
Principle
[E level] (n)
Orbital
[shape](l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Principle
[E level] (n)
Orbital
[shape](l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
Principle
[E level] (n)
Orbital
[shape](l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1
2
3
4
Principle
[E level] (n)
Orbital
[shape](l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s
2
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1
2
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e-
2
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1
2
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2sp
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1
p
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1
p 3
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
p 3 6e-
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4p 3 6e-
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3sp
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3spd
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s 1 2e-
pd
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s 1 2e-
p 3 6e-
d
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s 1 2e-
p 3 6e-
d 5 10e-
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s 1 2e-
9p 3 6e-
d 5 10e-
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s 1 2e-
9 18p 3 6e-
d 5 10e-
4
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s 1 2e-
9 18p 3 6e-
d 5 10e-
4
spd
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s 1 2e-
9 18p 3 6e-
d 5 10e-
4
spdf
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s 1 2e-
9 18p 3 6e-
d 5 10e-
4
s 1 2e-
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s 1 2e-
9 18p 3 6e-
d 5 10e-
4
s 1 2e-
p 3 6e-
df
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3
s 1 2e-
9 18p 3 6e-
d 5 10e-
4
s 1 2e-
p 3 6e-
d 5 10e-
f
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3
s 1 2e-
9 18p 3 6e-
d 5 10e-
4
s 1 2e-
p 3 6e-
d 5 10e-
f 7 14e-
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3s 1 2e-
9 18p 3 6e-
d 5 10e-
4
s 1 2e-
16p 3 6e-
d 5 10e-
f 7 14e-
Principle[E level]
(n)
Orbital [shape]
(l)
Magnetic[positions
per orbital]
Number of e- per orbital
Number of orbitals
per sublevel
(n2)
Maximum number of electrons
(2n2)
1 s 1 2e- 1 2
2s 1 2e-
4 8p 3 6e-
3
s 1 2e-
9 18p 3 6e-
d 5 10e-
4
s 1 2e-
16 32p 3 6e-
d 5 10e-
f 7 14e-
Write the e- configuration for the following:
1. beryllium2. carbon3. sodium4. magnesium
5. aluminum6. potassium
**EC: bromine
e- configuration
1. Oxygen2. fluorine3. Silicon4. Copper5. ArsenicEC: krypton
IV. Spin Quantum Number
IV. Spin Quantum Number
• indicates the spin of e- (clockwise & counterclockwise)
IV. Spin Quantum Number
• indicates the spin of e- (clockwise & counterclockwise)
• Pauli Exclusion Principle – no more than 2 e- per orbital, which must be of opposite spin
• Hund’s Rule – an e- can not enter a half filled orbital if an empty orbital of the same E is available
• Hund’s Rule – an e- can not enter a half filled orbital if an empty orbital of the same E is available
• place 1 e- into each p, d or f orbital before pairing them
• Pauli Exclusion Principle – no more than 2 e- per orbital, which must be of opposite spin
Orbital Notation• uses all 4 QN to represent e- arrangement
Orbital Notation Practice1. Fluorine
2. Magnesium
3. Phosphorus
4. Argon
5. Manganese
6. Arsenic
**EC: mercury
Write e- configuration and orbital diagrams for the following
1) Boron2) Sulfur3) Chlorine4) Potassium
5) Cobalt6) Copper7) Iodine8) barium