Energy Level Diagrams

1s

3s

2s2p

4s3p

3d4p

5s4d

5p6s

E

Pictorial representation of electron distribution

in orbitalsAufbau principle – e- occupy the lowest energy orbital available

p. 188 in text

Hund’s rule – e- half-fill each orbital in a sublevel

before pairing up

Pauli exclusion principle – max 2 e- per orbital (spin up and spin down)

n = 1 l = 0 ml = 0 ms = -½

Orbitals Being Filled

1s

2s

3s

4s

5s

6s

7s

3d

4d

5d

6d

2p

3p

4p

5p

6p

1s

La

Ac

1

3 4 5 6 7

4f

5f

Lanthanide series

Actinide series

Groups 8

Per

iods

1 2

2

3

4

5

6

7

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 345

Energy Level Diagrams

1s

3s

2s2p

4s3p

3d4p

5s4d

5p6s

E

Anions - Add e- to lowest energy sublevel available.

Cations - Remove e- from sublevel with highest

value of n.

Energy Level Diagrams

1s

3s

2s2p

4s3p

3d4p

5s4d

5p6s

E

Cations - Remove e- from sublevel with highest

value of n.

Energy Level Diagrams

1s

3s

2s2p

4s3p

3d4p

5s4d

5p6s

E

Energy Level Diagram of a Many-Electron Atom

ArbitraryEnergy Scale

1s

2s 2p

3s 3p

4s 4p 3d

5s 5p 4d

6s 6p 5d 4f

NUCLEUS

O’Connor, Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 177

Orbital Diagrams for Nickel

2s 2p 3s 3p 4s 3d1s

2s 2p 3s 3p 4s 3d1s

2s 2p 3s 3p 4s 3d1s

2s 2p 3s 3p 4s 3d1s

Excited State

Pauli Exclusion

Hund’s Rule

Ni58.6934

28

2 2 6 2 6 2 8

2 2 6 2 6 1 9

Homework

• p. 191 #3alt,4• p. 197 #5

Electron Configuration• H 1s1

• Ca 1s22s22p63s23p64s2

• Pb1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p2

• Cl- 1s22s22p63s23p6

• Fe2+ 1s22s22p63s23p63d6

• Fe3+ 1s22s22p63s23p63d5

• Ca [Ar]4s2

• Cl- [Ar]• Fe2+ [Ar]3d6

Shorthand: [noble gas]

Electron Filling in Periodic Table

K4s1

Ca4s2

Sc3d1

Ti3d2

V3d3

Mn3d5

Fe3d6

Co3d7

Ni3d8

Cr3d4

Cu3d9

Zn3d10

Ga4p1

Ge4p2

As4p3

Se4p4

Br4p5

Kr4p6

1

2

3

4

s

d

p

s

Cr4s13d5

Cu4s13d10

4f

4d

4p

4s

n = 4

3d

3p

3s

n = 3

2p

2sn = 2

1sn = 1

Ene

rgy

4s 3d

Cr4s13d5

4s 3d

Cu4s13d10

Cr3d5

Cu3d10

Homework

• p. 194 #6-11• p. 197 #1,2,6-10,13

Anomalous e- Configurations

Ferromagnetic – Fe, Co and Ni are smaller, closely packed atoms able to orient themselves in a magnetic field (group of these atoms oriented in the same direction – domain theory) , explains full magnetism

Q: Which substances containing calcium, zinc, copper (II) and manganese(II) ions are paramagnetic?

CaSO4(s)

ZnSO4(s)

CuSO4(s)

MnSO4(s)

Paramagnetism – substances exhibit a weak magnetic attraction believed to be caused by the presence of unpaired electrons

Quantum ChallengeThe arrangement of elements in the periodic table is a direct consequence of the allowed values for the four quantum numbers. If the laws of physics allowed these numbers to have different values, the appearance of the periodic table would change.Suppose, in a different universe, the quantum number ml has the allowed values of ml = 0,1,…+l. All other allowed values are unchanged so the set of allowed values is:n = 1,2,3…l = 0,1,2…n-1ml = 0,1…+l

ms = ½,-½

Task:

1. Design the periodic table for the first 30 elements.

2. Label the s,p and d block elements.3. Shade or colour the noble gas-like elements.

Show your work!!