Periodic Table
Prof. Dr. Sabine Prys
14/10/2010
1
@designed by ps
2.1 BOHR‘s Atomic Theory
φ = 10-7 - 10-10 m
14/10/2010
Nucleus:
Protons
Neutrons
(+)
(n)
Electron Orbits:
Electrons
(-)
10
1
2.3 Electron Shell
2n2 Electrons per Shell
E
n = 4 N-Shell
n = 3 M-Shell
n = 2 L-Shell
n = 1 K-Shell
1 Z ⋅ e2 m ⋅ Z 2 ⋅ e4
E=− ⋅
=
2 r
2 ⋅ n2 ⋅ h2
Z
e
r
m
n
h
=
=
=
=
=
=
Atomic Number
Elementary Charge
Orbital Radius
Electron Mass
Shell Number
Planck‘s Constant
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An orbital represents2.3.6
the probability
Orbitals in space to meet an
electron
s orbital, p orbital
d orbital
orbitals were calculated as <Ψ|r|Ψ>
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2
2.3.9.1 Elektron Quantum Numbers
Quantum Number
Symbol
Values
Meaning
Nucleus Distance,
Energy, Shell
Angular Momentum,
principal quantum number
n
1,2,3,4,5,...
azimuthal quantum number
l
0,1,2, ... (n-1)
magnetic quantum number
m
0,±1,±2, ... ,± l
Subshell
Projection of angular
momentum, Energy Shift
spin projection
quantum number
s
±½
Intrinsic Angular Momentum,
The angular momentum corresponds to the orbital type (s,p,d,f..)
The projection of the angular momentum corresponds to the orbital position
(e.g. p: x,y,z, etc) an
2.4 Electron Shell Structure
Shells (K, L, M, N) are containing sub shells (s, p, d, f)
The filling of shells is restricted to rules
n=4
n=3
n=2
n=1
s
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p
d
f
28
3
2.4.1 Configuration of shells
Notation:
H
He
Li
Be
B
C
N
nlx
1 s1
1 s2
1 s2
1 s2
1 s2
1 s2
1 s2
n = shell Number
l = sub shell s,p,d,f..
x = number of e- per orbital
population number, no exponent !
2 s1
2 s2
2 s2
2 s2
2 s2
valence electrons
2p1
2p2
2p3
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2.4.1.1 Pauli‘s Rule
x
•
Within one atom electrons can not be equal in all 4 quantum
numbers
principal quantum number
azimuthal quantum number
magnetic quantum number
spin projection quantum number
4
2.4.1.2 HUND‘s Rule
•
Orbitals of the same energy within the one subshell were first
single occupied
2.4.2 Shell Configuration for N
PAULI‘s rule - HUND‘s rule
E
n=3
n=2
n=1
s
p
positive spin
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d
negative spin
32
5
2.4.3 Shell Configuration for K
Energy rule
E
n=4
n=3
4s
n=2
n=1
s
p
positive spin
d
negative spin
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2.4.4 Shell Configuration Rules
Energy rule
PAULI‘s rule
HUND‘s rule
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6
2.4.6 Shell Configuration for Na
30
11
Notation
Na
1s2
2s2 2p6 3s1
n=4
n=3
n=2
n=1
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2.4.7 Shell Configuration
for Ge , Sn
Ge (32)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
= [Ar] 4s2 3d10 4p2
Sn (50)
1s2
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2s2
2p6
3s2
3p6 4s2 3d10 4p6 5s2 4d10 5p2
= [Kr] 5s2 4d10 5p2
37
7
Test 1
[Ar]
Ar] 3d10 4s2 4p6 = ?
?
n=4
n=3
n=2
n=1
s
p
d
f
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Test 2
What is the shell configuration of silicon
?
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8
3.0 Periodic Table of Elements
(PT)
Main Groups
Periods
I
II
III
IIII
V
VI
1
1H
2
3 Li
4
3
11 Na
12Mg
13Al
14Si
15P
16
4
19 K
20Ca
31Ga
32Ge
33As
5
37 Rb 38Sr
49 In
50 Sn
6
55 Cs
56Ba
81Tl
82 Pb
7
87 Fr
88Ra
VII
VIII
2 He
Be
5
B
6
113
C
7
N
8
O
9
10Ne
17Cl
18
34Se
35Br
36Kr
51Sb
52 Te
53I
54 Xe
83Bi
84Po
85At
86Rn
114
115
S
F
116
117
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Ar
118
41
3.1 Main Group Elements (s,p)
I
Alkali metal elements
Li, Na, K, Rb, Cs, Fr
very reactive metals
II
Alkaline earth elements
Be, Mg, Ca, Ba, Sr, Ra
less very reactive metals
III Earth elements
B, Al, Ga, In, Tl
light metals
Nitrogen group
N, P, As, Sb, Bi
increasing metallic properties
VI Chalcogens
O, S, Se, Te, Po
ore-former
VII Halogens
F, Cl, Br, I, At
salt-former
IIII Carbon group
C, Si, Ge, Sn, Pb
increasing metallic properties
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V
VIII Noble gases
He, Ne, Ar, Kr,Xe, Rn
inert elements
valence electrons: s, p
42
9
3.1.1 Examples: CaF2 Fluorite
Chemical Formula:
CaF2
Molecular Weight:
78.07 g/m
Calcium
51.33 % Ca
Fluorine
48.67 % F
Synonym:
Fluorite Spar
Locality:
common world wide
Environment:
low temperature vein deposits
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3.2 Transition Metal Elements
(s,d)
s2p6d1
Scandium-Group IIIb Sc
Sc
Y
La
Ac
1s2
1s2
1s2
1s2
2s2 p6
2s2 p6
2s2 p6
2s2 p6
3s2 p6 d1
3s2 p6 d10
3s2 p6 d10
3s2 p6 d10
4s2
4s2 p6 d1
4s2 p6 d10
4s2 p6 d10
5s2
5s2 p6 d1
5s2 p6 d10
6s2
6s2 p6 d1 7s2
valence electrons: s, d
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10
3.2.2 Examples: Iron Minerals
FeO
Hematite
Fe2O3
Fe2O3
Magnetite:
Fe3O4
Fe3O4 (magnetic)
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3.2.3 Examples: Pyrite
FeS2
Chemical Formula:
FeS2
Molecular Weight
119.98 g/m
Iron
46.55 % Fe
Sulphur
53.45 % S
Synonym:
Fool's Gold
Locality:
Common world wide
Environment:
sedimentary magmatic,
metamorphic, and hydrothermal.
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11
3.3 Lanthanoids und Actinoids
(f)
57La
Xe 5d1 6s2
89Ac
Rn 6d1 7s2
58Ce
Xe
4f2
6s2
90Th
Rn
6d2 7s2
59Pr
Xe
4f3
6s2
91Pa
Rn
5f2
6d1 7s2
60Nd
Xe
4f4
6s2
92U
Rn
5f3
6d1 7s2
valence electrons: s, d, f
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3.3.1 Webelements (1)
http://www.webelements.com
12
3.3.2 Webelements (2)
http://www.webelements.com
4.0 Periodic Properties
atomic diameter
I
II
III
IIII
V
VI
VII
1
1
2
3 Li
4
3
11 Na
12Mg
13Al
14Si
15P
16
4
19 K
20Ca
31Ga
32Ge
33As
34Se
5
37 Rb
38Sr
49
51Sb
52
6
55 Cs
56Ba
81Tl
83Bi
84Po
7
87 Fr
88Ra
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H
VIII
2 He
Be
5
B
In
113
6
C
50
Sn
82 Pb
114
7
N
115
8
O
S
Te
116
9
F
10Ne
17Cl
18
35Br
36Kr
53I
54
85At
86Rn
117
Ar
Xe
118
52
13
4.1 Ionisation Energy
∆EI
∆EI
Na+ + eCat ion
Na
= ionisation energy = 8,3 . 10-19 J (per atom)
increases with Z
decreases with increasing rAtom
decreases: s>p>d>f
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4.1.1 Ionisation Energy Curve
He
Ne
Ar
Kr
F
H
Li Na K
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10
Xe
Br
Zn
Cl
20
Rb
30
Hg Rn
Cd
40
Cs
50
60
70
Atomic Number
54
14
4.1.2 PT Ionisation Energy
I
II
III
IIII
V
VI
VII
1
1 H
2
3 Li
4
3
11 Na
12Mg
13Al
14Si
15P
16
4
19 K
20Ca
31Ga
32Ge
33As
34Se
5
37 Rb
38Sr
49
51Sb
52
6
55 Cs
56Ba
81Tl
83Bi
84Po
7
87 Fr
88Ra
VIII
2 He
Be
5
B
In
113
6
C
50
Sn
82 Pb
114
7
N
115
8
O
S
Te
116
9
F
10Ne
17Cl
18
35Br
36Kr
53I
54
85At
86Rn
117
Ar
Xe
118
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4.1.3 Higher Ionisation
Energies
Z
Ionization Energy of Elements Z = 1, ..12
Element ionization energy in eV for removel of electron x
1
2
3
4
5
6
7
1
2
3
4
5
6
7
8
9
10
11
12
H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
13,6
24,6
5,4
9,3
8,3
11,3
14,5
13,6
17,4
21,6
5,1
7,6
54,4
75,6
18,2
25,1
24,4
29,6
35,2
35,0
41,0
47,3
15,0
122,4
153,9
37,9
47,9
47,4
54,9
62,6
64,0
71,6
80,1
217,7
259,3
64,5
77,5
77,4
87,2
97,1
98,9
109,3
340,1
391,9
97,9
113,9
114,2
126,4
138,6
141,2
489,8
551,9
138,1
157,1
157,9
172,4
186,7
666,8
739,1
185,1
207,0
208,4
225,3
15
4.2 Electron Affinity
∆EE
Cl.
+
e-
ClAnion
∆EE = Electron Affinity = - 6,0 . 10-19 J (per atom)
H
F
Cl
Br
I
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(kJ / mol)
- 72
-333
-364
-342
-295
57
Test 3
Which are the corresponding energies ?
Cl+
Cl.
Cl.
Cl-
+ e
+ e
Cl+
Cl.
Cl.
Cl+ e+ e-
?
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16
4.3 Electronegativity
number:
Atom 1
EN
binding electrons
Atom 2
attraction to binding electrons
Mulliken, 1966:
EN ~
EN
2,1
0,7
4,0
3,0
2,8
2,4
H
Fr
F
Cl
Br
I
1
[∆EE + ∆EI ]
2
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4.3.1 Electronegativity in the PT
I
II
III
IIII
V
VI
VII
1
1
2
3 Li
4
3
11 Na
12Mg
13Al
14Si
15P
16
4
19 K
20Ca
31Ga
32Ge
33As
34Se
5
37 Rb
38Sr
49
51Sb
52
6
55 Cs
56Ba
81Tl
83Bi
84Po
7
87 Fr
88Ra
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H
VIII
2 He
Be
5
B
In
113
6
C
50
Sn
82 Pb
114
7
N
115
8
O
S
Te
116
9
F
10Ne
17Cl
18
35Br
36Kr
53I
54
85At
86Rn
117
Ar
Xe
118
60
17
4.3.2 Electronegativity Curve
F
Electro negativity
Elektronegativität
4,5
4
3,5
3
2,5
2
1,5
1
0,5
0
Cl
Br
I
1
51
101
Atomic Number
Ordnungszahl
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4.3.2.1 Electronegativity Examples
H
2,1
Li
1,0
Na
0,9
Mg
1,2
K Ca
0,8 1,0
Rb Sr
0,8 1,0
Be
1,5
Al
1,5
Sc
1,3
B
2,0
Si
1,8
C
2,5
P
2,1
Ti Ge As
1,6 1,7 2,0
Y Zr Sn Sb Te
1,3 1,6 1,7 1,8 2,1
N
3,0
S
2,5
Se
2,4
O
3,5
F
4,0
Cl
3,0
Br
2,8
I
2,4
Cs Ba
0,7 0,9
1
EN
2
3
4
18
4.3.3 Metal Properties
electrical
conductor
~
plastic
deformations
large
atomic radii
1/T
atomic lattice
thermal
conductor
low ionisation
energies
supra
conductivity
metal
shining
4.4 Metal Behaviour
metal behaviour
I
non metal behaviour
II
III
IIII
V
VI
VII
H
1
1
2
3 Li
4
3
11 Na
12Mg
13Al
14Si
15P
16
4
19 K
20Ca
31Ga
32Ge
33As
34Se
5
37 Rb
38Sr
49
51Sb
52
6
55 Cs
56Ba
81Tl
83Bi
84Po
7
87 Fr
88Ra
Metals
14/10/2010
VIII
2
Be
5
B
In
113
6
C
50
Sn
82 Pb
7
N
114
Semi-metals
115
8
O
9
S
Te
116
F
He
10Ne
17Cl
18
35Br
36Kr
53I
54
85At
86Rn
117
Ar
Xe
118
Non-metals
64
19
4.4.1 Metal Classifications
Density
light metals
ρ < 4 - 5 g/cm3
heavy metals
ρ > 4 - 5 g/cm3
e.g. Al,
e.g. Pb,
Mg
Cd
Galvanic Corrosion Potential Chart
K, Na, Mg, Al, Zn, Fe, Pb, Cu, Ag, Au
Cathodic  Anodic
least noble
corroded metals
most noble
protected metals
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4.5 Semi-Metals
I
II
III
IIII
V
VI
VII
H
1
1
2
3 Li
4
3
11 Na
12Mg
13Al
14Si
15P
16
4
19 K
20Ca
31Ga
32Ge
33As
34Se
5
37 Rb
38Sr
49
51Sb
52
6
55 Cs
56Ba
81Tl
83Bi
84Po
7
87 Fr
88Ra
VIII
2
Be
5
B
In
113
6
C
50
Sn
82 Pb
114
7
N
115
8
O
S
Te
116
9
F
He
10Ne
17Cl
18
35Br
36Kr
53I
54
85At
86Rn
117
Ar
Xe
118
conductivity increases with temperature, various modifications, e.g.
crystalline, amorphous, semiconductor behaviour, electron conductivity,
defect electron conductivity
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20
Test 4
Explain the semiconductor‘s energy bands
?
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4.5.2 Dopants
I
II
III
IIII
V
VI
VII
H
1
1
2
3 Li
4
3
11 Na
12Mg
13Al
14Si
15P
16
4
19 K
20Ca
31Ga
32Ge
33As
34Se
5
37 Rb
38Sr
49
51Sb
52
6
55 Cs
56Ba
81Tl
83Bi
84Po
7
87 Fr
88Ra
2
Be
p-type dopants
acceptor atoms
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VIII
5
B
In
113
6
C
50
Sn
82 Pb
114
7
N
115
8
O
9
S
Te
116
F
He
10Ne
17Cl
18
35Br
36Kr
53I
54
85At
86Rn
117
Ar
Xe
118
n-type dopants
donator atoms
68
21
4.5.3 Semiconductor Materials 1
• Group IV elemental semiconductors
– Diamond (C)
– Silicon (Si)
– Germanium (Ge)
• Group IV compound semiconductors
– Silicon carbide (SiC)
– Silicon germanide (SiGe)
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4.5.4 Semiconductor Materials 2
• III-V semiconductors
– Aluminium antimonide
(AlSb)
– Aluminium arsenide
(AlAs)
– Aluminium nitride (AlN)
– Aluminium phosphide
(AlP)
– Boron nitride (BN)
– Boron phosphide (BP)
– Boron arsenide (BAs)
– phosphide (InP)
– Gallium antimonide
(GaSb)
– Gallium arsenide (GaAs)
– Gallium nitride (GaN)
– Gallium phosphide (GaP)
– Indium antimonide (InSb)
– Indium arsenide (InAs)
– Indium nitride (InN)
70
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4.5.5 Semiconductor Materials 3
• III-V ternary semiconductor alloys
14/10/2010
–
–
–
–
–
–
–
–
–
–
–
–
Aluminium gallium arsenide (AlGaAs, AlxGa1-xAs)
Indium gallium arsenide (InGaAs, InxGa1-xAs)
Indium gallium phosphide (InGaP)
Aluminium indium arsenide (AlInAs)
Aluminium indium antimonide (AlInSb)
Gallium arsenide nitride (GaAsN)
Gallium arsenide phosphide (GaAsP)
Aluminium gallium nitride (AlGaN)
Aluminium gallium phosphide (AlGaP)
Indium gallium nitride (InGaN)
Indium arsenide antimonide (InAsSb)
Indium gallium antimonide (InGaSb)
71
4.5.6 Semiconductor Materials 4
• III-V quaternary semiconductor alloys
– Aluminium gallium indium phosphide (AlGaInP, also
InAlGaP, InGaAlP, AlInGaP)
– Aluminium gallium arsenide phosphide (AlGaAsP)
– Indium gallium arsenide phosphide (InGaAsP)
– Aluminium indium arsenide phosphide (AlInAsP)
– Aluminium gallium arsenide nitride (AlGaAsN)
– Indium gallium arsenide nitride (InGaAsN)
– Indium aluminium arsenide nitride (InAlAsN)
– Gallium arsenide antimonide nitride (GaAsSbN)
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23
4.5.7 Semiconductor Materials 5
• III-V quinary semiconductor alloys
– Gallium indium nitride arsenide antimonide (GaInNAsSb)
– Gallium indium arsenide antimonide phosphide
(GaInAsSbP)
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4.5.8 Semiconductor Materials 6
• II-VI semiconductors
–
–
–
–
–
–
–
14/10/2010
Cadmium selenide (CdSe)
Cadmium sulfide (CdS)
Cadmium telluride (CdTe)
Zinc oxide (ZnO)
Zinc selenide (ZnSe)
Zinc sulfide (ZnS)
Zinc telluride (ZnTe)
74
24
4.5.9 Semiconductor Materials 7
• II-VI ternary alloy semiconductors
–
–
–
–
Cadmium zinc telluride (CdZnTe, CZT)
Mercury cadmium telluride (HgCdTe)
Mercury zinc telluride (HgZnTe)
Mercury zinc selenide (HgZnSe)
• I-VII semiconductors
– Cuprous chloride (CuCl)
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4.5.10 Semiconductor Materials 8
• IV-VI semiconductors
–
–
–
–
–
Lead selenide (PbSe)
Lead sulfide (PbS)
Lead telluride (PbTe)
Tin sulfide (SnS)
Tin telluride (SnTe)
• IV-VI ternary semiconductors
– lead tin telluride (PbSnTe)
– Thallium tin telluride (Tl2SnTe5)
– Thallium germanium telluride (Tl2GeTe5)
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25
4.5.11 Semiconductor Materials 9
• V-VI semiconductors
– Bismuth telluride (Bi2Te3)
• II-V semiconductors
–
–
–
–
–
–
Cadmium phosphide (Cd3P2)
Cadmium arsenide (Cd3As2)
Cadmium antimonide (Cd3Sb2)
Zinc phosphide (Zn3P2)
Zinc arsenide (Zn3As2)
Zinc antimonide (Zn3Sb2)
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4.5.12 Semiconductor Materials
10
• Layered semiconductors
–
–
–
–
–
Lead(II) iodide (PbI2)
Molybdenum disulfide (MoS2)
Gallium Selenide (GaSe)
Tin sulfide (SnS)
Bismuth Sulfide (Bi2S3)
• Others
14/10/2010
–
–
–
–
–
Copper indium gallium selenide (CIGS)
Platinum silicide (PtSi)
Bismuth(III) iodide (BiI3)
Mercury(II) iodide (HgI2)
Thallium(I) bromide (TlBr)
78
26
4.5.13 Semiconductor Materials
11
• Miscellaneous oxides
–
–
–
–
–
Titanium dioxide: anatase (TiO2)
Copper(I) oxide (Cu2O)
Copper(II) oxide (CuO)
Uranium dioxide (UO2)
Uranium trioxide (UO3)
• Organic semiconductors
• Magnetic semiconductors
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Exercises
1.
2.
3.
4.
5.
6.
Explain the different quantum numbers ?
What was the conclusion of the RUTHERFORD experiment ?
How many electrons can be found in the L-shell ?
List some Lanthanoids ?
What does HUND’s rule say ? What does PAULI’s rule
Which orbitals are valence orbitals in (a) main group elements
(b) in transition group group elements (c) in Lanthanoids?
7. What is the meaning of electronegativity ?
8. How many oxygen atoms can be bond by silicon ?
9. What are ore-former ?
10. What is the galvanic corrosion potential chart ?
11. What is a heavy metal ?
12. Where are the semi-metals located in the periodic table ?
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27
Literature
E. Lindner; Chemie für Ingenieure; M. Lindner Verlag, 1993
P.W. Atkins & J.A. Beran; Chemie einfach alles; VCH, 1996
W. Schröter et. al; Taschenbuch der Chemie; Verlag Harry Deutsch, 1990
Römpp; Chemie Lexikon, 9. Auflage; Thieme Verlag, 1990
Linus Pauling; Grundlagen der Chemie; Verlag Chemie, 1973
B. Bröcker; DTV-Atlas zur Atomphysik; DTV Verlag 1993
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Web-Links
•
•
•
14/10/2010
http://www.chemtutor.com/
http://library.thinkquest.org/2923/
http://www.chemfinder.com
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