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

pdf

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-

pdf

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