1. Energy Level Diagrams E
Hund’s rule – e- half-fill each orbital in a sublevel before pairing up 6s
Pictorial representation of electron distribution in orbitals 5p 4d
Aufbau principle – e- occupy the lowest energy orbital available
p. 188 in text 5s 4p
Pauli exclusion principle – max 2 e- per orbital (spin up and spin down) 3d E 4s 3p 3s 2p 2s
n = 1 l = 0 ml = 0 ms = -½ 1s

2. Orbitals Being Filled Groups 1 8 2 1s 1 3 4 5 6 7 1s 2s 2 2p 3 3s 3p 1s 2s 2 2p 3 3s 3p
Periods 4s 3d 4p 4 4d 5p 5 5s La 5d 6p 6 6s Ac 6d 7 7s 4f
Lanthanide series 5f
Actinide series
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 345

3. Anions - Add e- to lowest energy sublevel available.
Energy Level Diagrams 6s 5p 4d 5s 4p 3d E 4s 3p 3s
Cl- 2p 2s
Anions - Add e- to lowest energy sublevel available. 1s

4. Cations - Remove e- from sublevel with highest value of n.
Energy Level Diagrams 6s 5p 4d 5s 4p
Cations - Remove e- from sublevel with highest value of n. 3d E 4s 3p 3s
Sr2+ 2p 2s 1s

5. Cations - Remove e- from sublevel with highest value of n.
Energy Level Diagrams 6s 5p 4d 5s 4p
Cations - Remove e- from sublevel with highest value of n. 3d E 4s 3p 3s
Fe2+ and Fe3+ 2p 2s 1s

6. Energy Level Diagram of a Many-Electron Atom
6s p d f
5s p d
4s p d
Arbitrary
Energy Scale
3s p
2s p 1s
NUCLEUS
O’Connor, Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 177

7. Orbital Diagrams for Nickel 28 1s 2s 2p 3s 3p 4s 3d 2s 2p 3s 3p 4s 3d 1s
Excited State 2s 2p 3s 3p 4s 3d 1s
Pauli Exclusion 2s 2p 3s 3p 4s 3d 1s
Hund’s Rule

8. Homework
p. 191 #3alt,4
p. 197 #5

9. The Periodic Table * Y * Lanthanides Y Actinides Alkaline H He Li Be B
Noble
gases
Alkaline
earth metals
Halogens 1 18 H 1 He 2 2 13 14 15 16 17 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 Na 11 Mg 12 3 4 5 6 7 8 9 10 11 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18
Transition metals K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36
Alkali metals Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 * Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 Fr 87 Ra 88 Y Rf
104 Db
105 Sg
106 Bh
107 Hs
108 Mt
109
Uun
110
Uuu
111
Uub
112
Uuq
113
Uuh
116
Uuo
118
* Lanthanides La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71
Y Actinides Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm
100 Md
101 No
102 Lr
103

11. Electron Configuration
H 1s1
Ca 1s22s22p63s23p64s2
Pb 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p2
Cl- 1s22s22p63s23p6
Fe2+ 1s22s22p63s23p63d6
Fe3+ 1s22s22p63s23p63d5
Ca [Ar]4s2
Cl- [Ar]
Fe2+ [Ar]3d6
Shorthand: [noble gas]

12. Electron Filling in Periodic Tables s p 1 2 d 3 K
4s1 Ca
4s2 Sc
3d1 Ti
3d2 V
3d3 Cr
3d5 Cr
3d4 Cu
3d9 Mn
3d5 Fe
3d6 Co
3d7 Ni
3d8 Cu
3d10 Zn
3d10 Ga
4p1 Ge
4p2 As
4p3 Se
4p4 Br
4p5 Kr
4p6 4 Cr
4s13d5 Cu
4s13d10 4f 4d
n = 4 4p 3d Cr
4s13d5 4s
n = 3 3p
Energy 3s 4s 3d 2p
n = 2 2s Cu
4s13d10
n = 1 1s 4s 3d

13. Homework
p. 194 #6-11
p. 197 #1,2,6-10,13

14. Anomalous e- Configurations

15. 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

16. Paramagnetism – substances exhibit a weak magnetic attraction
 believed to be caused by the presence of unpaired electrons
Q: Which substances containing calcium, zinc, copper (II) and manganese(II) ions are paramagnetic? CaSO4(s) ZnSO4(s) CuSO4(s) MnSO4(s)

17. Quantum Challenge
The 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-1 ml = 0,1…+l ms = ½,-½

18. Task: Design the periodic table for the first 30 elements.
Label the s,p and d block elements.
Shade or colour the noble gas-like elements.
Show your work!!