Silberberg Ch' 8

1
Summary of Quantum Numbers of Electrons in Atoms
Name Symbol Permitted Values
Property
Principal n Positive integers
(1,2,3, etc.) Orbital energy

(size) Angular
l Integers from 0 to n - 1
Orbital shape (the l momentum

values 0, 1, 2, and 3

correspond to the s,

p, d, and f orbitals) Magnetic
ml Integers from -l to 0 to l
Orbital orientation Spin ms
1/2 or -1/2
Direction of e- spin


Table 8.2
2
Fig. 8.4
3
Order of Electron Filling
4
Fig. 8.10
5
Electron Configuration - I

• H 1s 1
• He 1s 2
  He
• Li 1s2 2s 1
  He 2s 1
• Be 1s2 2s 2 He 2s 2
• B 1s2 2s 2 2p 1 He 2s 2 2p
  1
• C 1s 2 2s 2 2p 2 He 2s 2 2p
  2
• N 1s 2 2s 2 2p 3 He 2s 2 2p
  3
• O 1s 2 2s 2 2p 4 He 2s 2 2p
  4
• F 1s 2 2s 2 2p 5 He 2s 2
  2p 5
• Ne 1s 2 2s 2 2p 6 He 2s 2 2p6
  Ne

6
The Periodic Table of the Elements
Electronic Structure
He
H
Ne
F
O
N
C
B
Li
Be
Ar
Cl
S
P
Si
Al
Na
Mg
Kr
Zn
Cu
Ni
Co
Fe
Mn
Cr
V
Ti
Sc
Br
Se
As
Ge
Ga
K
Ca
Xe
Cd
Ag
Pd
Rh
Ru
Tc
Mo
Nb
Zr
Y
I
Te
Sb
Sn
In
Rb
Sr
Rn
Hg
Au
Pt
Ir
Os
Re
W
Ta
Hf
La
At
Po
Bi
Pb
Tl
Cs
Ba
Ac
Rf
Ha
Fr
Ra
Sg
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
S Orbitals
P Orbitals f Orbitals
d Orbitals
7
Mendeleevs Predicted vs Actual Properties
of Element 32 - Germanium
Property Predicted
Properties Actual Properties
Atomic Mass 72
72.59
Appearance Gray Metal
Gray Metal
Density 5.5
g/cm3 5.35 g/cm3
Molar volume 13 cm3 /mol
13.22 cm3/mol
Specific heat capacity 0.31 J/g K
0.32 J/g K
Oxide density 4.7 g/cm3
4.23 g/cm3
Sulfide formula and ES2 insoluble
in GeS2 insoluble in
solubility H2O soluble in
H2O soluble in
aqueous (NH4)S
aqueous (NH4)S
Chloride formula ECl4
GeCl4
(boiling point) lt 100oC
84oC
Chloride density 1.9 g/cm3
1.844 g/cm3
Element preparation reduction of
K2EF6 Reduction of
with sodium
K2GeF6 with sodium
8
Magnetic Properties

• Paramagnetic - An atom or ion which has unpaired
  electrons, which add up to give a spin vector.
  They are thereby attracted by a magnetic field.
• Diamagnetic - An atom or ion with all electrons
  paired and with no net spin.

9
Apparatus for Measuring the Magnetic Behavior of
a Sample
Fig. 8.25
10
Orbital Box Diagrams - I H Be
Element Symbol Electron
Orbital Box Diagrams
Configuration
Hydrogen H 1s1
Helium He 1s2 Lithium
Li 1s22s1 Beryllium
Be 1s22s2
1s
2s
1s
2s
2s
1s
1s
2s
11
Fig. 8.5
12
Hunds Rule

• For an atom in its ground-state configuration,
  all unpaired electrons have the same spin
  orientation.
• Therefore electrons tend to occupy all free
  orbitals and not pair up, so that their spins all
  add up to produce a general vector for the atom.

13
Electronic Configuration Ions

• Na 1s 2 2s 2 2p 6 3s 1 Na 1s 2
  2s 2 2p 6
• Mg 1s 2 2s 2 2p 6 3s 2 Mg2 1s 2 2s
  2 2p6
• Al 1s 2 2s 2 2p 6 3s 2 3p 1 Al3 1s 2
  2s 2 2p 6
• O 1s 2 2s 2 2p 4 O- 2 1s
  2 2s 2 2p 6
• F 1s 2 2s 2 2p 5 F- 1
  1s 2 2s 2 2p 6
• N 1s 2 2s 2 2p 3
  N- 3 1s 2 2s 2 2p 6

14
Isoelectronic Atoms and Ions

• H- 1 He Li Be2
• N- 3 O- 2 F- Ne Na Mg2
  Al3
• P- 3 S- 2 Cl- Ar K Ca2
  Sc3 Ti4
• As- 3 Se- 2 Br- Kr Rb Sr2
  Y3 Zr4
• Sb- 3 Te- 2 I- Xe Cs Ba2
  La3 Hf4

15
Fig. 8.11
16
Atomic Radii of the Main-Group and Transition
Elements
Fig. 8.12
17
Fig. 8.13
18
Periodicity of First Ionization Energy (IE1)
Fig. 8.14
19
Fig. 8.15
20
Fig. 8.16
21
Successive Ionization Energies
Valence Z Element
Electrons IE1 IE2 IE3 IE4 IE5
IE6 IE7
3 Li 1 0.52 7.30
11.81 4 Be 2
0.92 1.76 14.85 21.01 5 B
3 0.80 2.43 3.66 25.02
32.82 6 C 4
1.09 2.35 4.62 6.22 37.83 47.28 7
N 5 1.40 2.86 4.58
7.48 9.44 53.27 64.36 8 O
6 1.31 3.39 5.30 7.47
10.98 13.33 71.33 9 F
7 1.68 3.37 6.05 8.41 11.02
15.16 17.87
22
Electron Affinities of the Main-Group Elements
Fig. 8.17
23
Trends in Three Atomic Properties
Fig 8.18
24
Trends in Metallic Behavior
Fig. 8.19
25
The Trends in Acid-Base Behavior of Elemental
Oxides
Fig. 8.22
26
Fig. 8.27