Periodic Table
Kelter, Carr, Scott, Chemistry A Wolrd of Choices 1999, page 74
Guiding Questions
Why is the periodic table so important?
Why is the periodic table shaped the way it's shaped?
Why do elements combine? Why do elements react?
What other patterns are there in the world and how do
they help us?
Table of Contents
‘Periodic Table’
How to Organize Elements
Mendeleev’s Periodic Table
Modern Periodic Table
Groups of Elements
Metals, Nonmetals,
Metalloids
Discovering Elements
Origin of Names of Elements
Selected Elements
Electron Filling Order
Diatomic Molecules
Size of Atoms – Trends
Ionization Energy
Summary of Periodic Trends
Essential Elements
Element Project
Atomic Structure and Periodicity
You should be able to
Identify characteristics of and perform calculations with frequency and
wavelength.
Know the relationship between types of electromagnetic radiation and
Energy; for example, gamma rays are the most damaging.
Know what exhibits continuous and line spectra.
Know what each of the four quantum numbers n, l, m, and ms represents.
Identify the four quantum numbers for an electron in an atom.
Write complete and shorthand electron configurations as well as orbital
diagrams for an atom or ion of an element.
Identify the number and location of the valence electrons in an atom.
Apply the trends in atomic properties such as atomic radii, ionization
energy, electronegativity, electron affinity, and ionic size.
Calcium atom = [Ar]4s2
Potassium atom = [Ar]4s1
p = 20
n = 20
e = 20
p = 19
n = 20
e = 19
Ca  2 e- + Ca2+
K  e- + K1+
Potassium ion = K1+ ≡ [Ar]
1s22s22p63s23p6
Calcium ion = Ca2+ ≡ [Ar] or
1s22s22p63s23p6
18e
19e19+
18e
20e-
>
20+
Oxygen atom = [He]2s22p4
Fluorine atom = [He] 2s22p5
p= 9
n = 10
e= 9
p= 8
n= 8
e= 8
F + e-  F1-
O + 2 e-  O2Oxideion
ion = O2- ≡ [Ne]
Oxygen
1s22s22p6
Fluorideion
ion = F1- ≡ [Ne]
Fluorine
1s22s22p6
8
6 e8+
8
7 e-
<
9+
Energy Level Diagram of a Many-Electron Atom
6s
6p
5d
4f
32
5s
5p
4d
18
4s
4p
3d
18
Arbitrary
Energy Scale
3s
3p
8
2s
2p
8
1s
2
NUCLEUS
O’Connor, Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 177
How to Organize Elements…
Periodic Table Designs
How to Organize…
Baseball Cards:
year, team, player, card number, value ($).
Elements:
when
they weremass,
discovered,
family, reactivity,
alphabetically,
value, density,
state
solid of
or matter,
liquid ormetal
gas vs. non-metal, atomic mass,
atomic number.
Which way is CORRECT to organize the elements?
Is it possible to organize the elements correctly in more than one way?
Interactive Periodic Table
e
Ir O N Mn
77
1
H
8
7
25
The Human Element
H
He
1
2
1
2
3
Li
Be
B
C
N
O
F
Ne
3
4
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
13
14
15
16
17
18
Na Mg
11
4
K
19
5
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
23
24
35
36
I
Xe
53
54
21
22
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
50
Hf
Ta
W
72
73
74
38
Cs Ba
55
7
Ca Sc
20
37
6
12
56
Fr Ra
87
88

25
43
26
44
Re Os
75
76
27
28
29
47
30
32
46
Ir
Pt Au Hg
Tl
Pb
77
78
81
82
80
33
34
Sn Sb Te
45
79
48
31
51
52
Bi Po At Rn
83
84
85
86
Rf Db Sg Bh Hs Mt
104
105
106
107
108
109
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
57
58
59
Ac Th Pa
89
90
91
60
U
92
61
62
63
64
65
66
67
68
69
70
71
Np Pu Am Cm Bk Cf Es Fm Md No Lr
93
94
95
96
97
98
99
100
101
102
103
Aliens Activity
Nautilus shell has a repeating pattern.
Look carefully at the drawings of the ‘aliens’.
Organize all the aliens into a meaningful pattern.
Aliens Lab
Cards
Periodic Table
1
2
3
4
5
6
7
Alkali earth metals
H
1
8A
Alkali metals
1A
He
Transition metals
2A
Li
Be
3
4
Na
Mg
3A 4A 5A 6A 7A
Boron group
Nonmetals
B
C
N
O
F
Ne
5
6
7
8
9
10
Si
P
S
Cl
Ar
14
15
16
17
18
As Se Br
Kr
Noble gases
Al
8B
3B 4B 5B 6B 7B
1B 2B
11
12
K
Ca
Sc
Ti
V
Cr Mn Fe Co Ni Cu Zn
19
20
21
22
23
24
Rb
Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
37
38
39
40
41
42
49
50
Cs
Ba
Hf
Ta
W
55
56
72
73
74
Fr
Ra
87
88
25
26
43
27
44
Re Os
75
76
28
29
13
30
47
Ga Ge
31
48
Sn Sb
46
Ir
Pt Au Hg
Tl
Pb
77
78
81
82
80
33
32
45
79
51
34
35
36
Te
I
Xe
52
53
54
At
Rn
85
86
Bi Po
83
84
Rf Db Sg Bh Hs Mt
104
105
106
107
108
109
Lanthanoid Series
6
Br Liquid
H Gas
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
57
58
59
Actinoid Series
C Solid
7
Ac Th Pa
89
90
91
60
U
92
61
62
63
64
65
66
67
68
69
70
71
Np Pu Am Cm Bk Cf Es Fm Md No Lr
93
94
95
96
97
98
2
99
100
101
102
103
Dutch Periodic Table
117
116
115
114
113
112
111
110
109
108
107
106
Strong, Journal of Chemical Education, Sept. 1989, page 743
118
Stowe’s Periodic Table
Benfey’s Periodic Table
Döbereiner’s Triads
Johann Döbereiner
~1817
Name
Atomic
Mass
Name
Atomic
Mass
Calcium
Barium
40
137
Chlorine
Iodine
35.5
127
Sulfur
Tellurium
32
127.5
Average
88.5
Average
81.3
Average
79.8
Strontium
87.6
Bromine
79.9
Selenium
79.2
Name
Atomic
Mass
Döbereiner discovered groups of three related elements which he termed a triad.
Smoot, Price, Smith, Chemistry A Modern Course 1987, page 161
Newlands Law of Octaves
John Newlands
~1863
Newlands Law of Octaves
1
2
3
4
5
6
7
Li
Na
K
Be
Mg
B
Al
C
Si
N
P
O
S
F
Cl
Smoot, Price, Smith, Chemistry A Modern Course 1987, page 161
Development of Periodic Table
J.W. Döbereiner (1829)
Law of Triads
Elements could be classified into groups of three, or triads.
Trends in physical properties such as density, melting point,
and atomic mass were observed.
J.A.R. Newlands (1864)
Law of Octaves
Arranged the 62 known elements into groups of seven
according to increasing atomic mass.
He proposed that an eighth element would then repeat the
properties of the first element in the previous group.
Lothar Meyer (1830 – 1895)
Invented periodic table independently of Mendeleev
his work was not published until 1870 - one year after Mendeleev's
Dmitri Mendeleev
• Russian
• Invented periodic table
• Organized elements by
properties
• Arranged elements by atomic
mass
• Predicted existence of several
unknown elements
• Element 101
Dmitri Mendeleev
Dmitri Mendeléev
Mendeleev’s Periodic Table
Mendeleev’s Early Periodic Table
REIHEN
TABELLE II
GRUPPE I
___
Li = 7
K = 39
11
12
RH3
R2O5
Cs = 133
Sr = 87
GRUPPE VI
GRUPPE VII
RH2
RO3
In = 113
? Di = 138
__
__
(Au = 199)
__
? Yt = 88
Ba = 137
__
Si = 28
RH
R2O7
? Er = 178
Tl= 204
__
V = 51
Zr = 90
GRUPPE VIII
___
RO4
Cr = 52
Nb = 94
? Ce = 140
From Annalen der Chemie und Pharmacie, VIII, Supplementary Volume for 1872, p. 151.
__
W = 184
Pd = 106, Ag = 108
__ __ __ __
__
__
__
U = 240
Ni = 59, Cu = 63
Ru = 104, Rh = 104,
J = 127
__
Bi = 208
__
__ = 100
__
Ta = 182
Fe = 56, Co = 59,
Br = 80
Te = 125
__
Pb = 207
Mn = 55
Mo = 96
__
Cl = 35.5
Se = 78
Sb = 122
__
? La = 180
F = 19
S = 32
As = 75
Sn = 118
Th = 231
O = 16
P = 31
? = 72
__
__
Hg = 200
N = 14
Ti = 48
? = 68
__
Cd = 112
( __ )
__
Al = 27.3
Zn = 65
(Ag = 108)
C = 12
? = 44
__
Ca = 40
Rb = 85
9
10
GRUPPE V
RH4
RO2
B = 11
Mg = 24
(Cu = 63)
7
8
Be = 9.4
Na = 23
5
6
RO
R2O3
GRUPPE IV
H=1
3
4
GRUPPE III
___
R2O
1
2
GRUPPE II
___
Os = 195, Ir = 197,
__
__
Pt = 198, Au = 199
__ __ __ __
Elements Properties are Predicted
O’Connor Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 119,
Periodic Table of the Elements
1
2
3
H
He
1
2
Li
Be
B
C
N
O
F
Ne
3
4
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
13
14
15
16
17
18
Na Mg
11
4
K
19
5
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
23
24
35
36
I
Xe
53
54
21
22
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
50
Hf
Ta
W
72
73
74
38
Cs Ba
55
7
Ca Sc
20
37
6
12
56
Fr Ra
87
88

25
43
26
44
Re Os
75
76
27
28
29
47
30
32
46
Ir
Pt Au Hg
Tl
Pb
77
78
81
82
80
33
34
Sn Sb Te
45
79
48
31
51
52
Bi Po At Rn
83
84
85
86
Rf Db Sg Bh Hs Mt
104
105
106
107
108
109
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
57
58
59
Ac Th Pa
89
90
91
60
U
92
61
62
63
64
65
66
67
68
69
70
71
Np Pu Am Cm Bk Cf Es Fm Md No Lr
93
94
95
96
97
98
99
100
101
102
103
Modern Periodic Table
• Henry G.J. Moseley
• Determined the atomic
numbers of elements
from their X-ray spectra
(1914)
• Arranged elements by
increasing atomic
number
• Killed in WW I at age 28
(Battle of Gallipoli in Turkey)
1887 - 1915
Introduction to the Periodic Table
• Elements are arranged in seven horizontal rows, in
order of increasing atomic number from left to right and
from top to bottom.
• Rows are called periods and are numbered from 1 to 7.
• Elements with similar chemical properties form vertical
columns, called groups, which are numbered from 1 to
18.
• Groups 1, 2, and 13 through 18 are the main group
elements.
• Groups 3 through 12 are in the middle of the periodic
table and are the transition elements.
• The two rows of 14 elements at the bottom of the
periodic are the lanthanides and actinides.
Copyright 2007 Pearson Benjamin Cummings. All rights reserved.
Groups of Elements
1A
1
H
1
2
3
Be
3
4
K
19
5
12
He
7A Halogens
3A Boron group
8A Noble gases
4A Carbon group
Hydrogen
3A 4A
Inner transition metals
8B
3B 4B 5B 6B 7B
Ca Sc
1B 2B
N
O
F
Ne
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
13
14
15
16
17
18
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
23
24
35
36
I
Xe
53
54
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
50
Hf
Ta
W
72
73
74
Cs Ba
56
Fr Ra
87

88
2
C
22
38
5A 6A 7A
B
21
55
7
6A Oxygen group
8A
20
37
6
2A Alkali earth metals
Na Mg
11
4
5A Nitrogen group
Transition metals
2A
Li
1A Alkali metals
25
43
26
44
Re Os
75
76
27
28
29
47
30
32
46
Ir
Pt Au Hg
Tl
Pb
77
78
81
82
80
33
34
Sn Sb Te
45
79
48
31
51
52
Bi Po At Rn
83
84
85
86
Rf Db Sg Bh Hs Mt
104
105
106
107
108
109
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
57

58
59
Ac Th Pa
89
90
91
60
U
92
61
62
63
64
65
66
67
68
69
70
71
Np Pu Am Cm Bk Cf Es Fm Md No Lr
93
94
95
96
97
98
99
100
101
102
103
Groups of Elements
1
18
He
2
13
14
15
16
17
2
Li
Be
N
O
F
Ne
3
4
7
8
9
10
Na
Mg
P
S
Cl
Ar
11
12
15
16
17
18
K
Ca
As
Se
Br
Kr
19
20
33
34
35
36
Rb
Sr
Sb
Te
I
Xe
37
38
51
52
53
54
Cs
Ba
Bi
Po
At
Rn
55
56
83
84
85
86
Fr
Ra
87
88
1
Alkali metals
16
Oxygen family
2
Alkaline earth metals
17
Halogens
18
Noble gases
15
Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 367
Nitrogen family
Diatomic Elements
H2
He
Li Be
B C N2 O2 F2 Ne
Na Mg
Al Si P S Cl2 Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br2 Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I2 Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac
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
Alkali Metals, Group 1
H
He
Li Be
B C N O F Ne
Na Mg
Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac
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
Alkaline Earth Metals, Group 2
H
He
Li Be
B C N O F Ne
Na Mg
Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac
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
Halogens, Group 17
H
He
Li Be
B C N O F Ne
Na Mg
Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac
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
Noble Gases, Group 18
H
He
Li Be
B C N O F Ne
Na Mg
Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac
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
Chalcogens, Group 16
H
He
Li Be
B C N O F Ne
Na Mg
Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac
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
Chemistry of the Groups
Group 16, the Chalcogens
– The chalcogens are oxygen, sulfur, selenium, tellurium, and
polonium.
16
O
8
S
16
Se
34
Te
52
Po
All of the chalcogens have ns2np4 valence-electron configurations.
Their chemistry is dominated by three oxidation states:
1. –2, in which two electrons are added to achieve the
closed-shell electron of the next noble gas.
2. +6, in which all six valence electrons are lost to give the
closed-shell electron configuration of the preceding noble
gas.
3. +4, in which only the four np electrons are lost to give a
filled ns2 subshell.
84
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
Pnicogens, Group 15
H
He
Li Be
B C N O F Ne
Na Mg
Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac
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
Chemistry of the Groups
Group 15, the Pnicogens
– The pnicogens are nitrogen, phosphorus, arsenic, antimony, and
bismuth.
– All the pnicogens have ns2np3 valence-electron configurations,
leading to three common oxidation states:
15
N
7
P
15
As
33
Sb
51
1. –3, in which three electrons are added to give the
closed-shell electron configuration of the next noble gas
2. +5, in which all five valence electrons are lost to give the
closed-shell electron configuration of the preceding noble
gas
3. +3, in which only the three np electrons are lost to give a
filled ns2 subshell
Bi
83
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
Chemistry of the Groups
Group 14
– Group 14 elements straddle the diagonal line that divides nonmetals from
metals.
– Carbon is a nonmetal, silicon and germanium are semimetals, and tin and
lead are metals.
– Group-14 elements have the ns2np2 valence-electron configuration.
– Group-14 elements have three oxidation states:
1. –4, in which four electrons are added to achieve the closed-shell
electron configuration of the next noble gas
2. +4, in which all four valence electrons are lost to give the closedshell electron configuration of the preceding noble gas
3. +2, in which the loss of two np2 electrons gives a filled ns2
subshell
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
Chemistry of the Groups
Group 13
– Of the Group-13 elements, only the lightest, boron, lies on the
diagonal line that separates nonmetals and metals, it is a
semimetal and possesses an unusual structure.
– The rest of Group 13 are metals (aluminum, gallium, indium, and
thallium) and are typical metallic solids.
– Elements of Group 13 are highly reactive and form stable
compounds with oxygen.
– Elements of Group 13 have ns2np1 valence-electron
configurations.
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
Lanthanide Series
H
He
Li Be
B C N O F Ne
Na Mg
Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac
La
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
Actinide Series
H
He
Li Be
B C N O F Ne
Na Mg
Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac
La
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
La
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
Chemistry of the Groups
1
1A
8A
H
He
1
2
3
2A
Li
Be
3
4
K
12
N
O
F
Ne
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
13
14
15
16
17
18
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
23
24
35
36
I
Xe
53
54
22
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
50
Hf
Ta
W
72
73
74
38
Cs Ba
56
Fr Ra
87

88
25
43
26
44
Re Os
75
76
27
28
29
47
30
32
46
Ir
Pt Au Hg
Tl
Pb
77
78
81
82
80
33
34
Sn Sb Te
45
79
48
31
51
52
Bi Po At Rn
83
84
85
86
Rf Db Sg Bh Hs Mt
104
105
106
107
108
109
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Lanthanides
57
Actinides
2
C
21
55
7
1B 2B
5A 6A 7A
B
20
37
6
8B
3B 4B 5B 6B 7B
Ca Sc
19
5
Transition Metals
Na Mg
11
4
3A 4A

58
59
Ac Th Pa
89
90
91
60
U
92
61
62
63
64
65
66
67
68
69
70
71
Np Pu Am Cm Bk Cf Es Fm Md No Lr
93
94
95
96
97
98
99
100
101
102
103
Metals and Nonmetals
1
2
3
H
He
1
2
Li
Be
B
C
3
4
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
13
14
15
16
17
18
Na Mg
11
4
K
19
5
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
23
24
35
36
I
Xe
53
54
21
22
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
50
Hf
Ta
W
72
73
74
38
Cs Ba
55
7
Ca Sc
20
37
6
12
56
Fr Ra
87
88

N O F Ne
Nonmetals
25
26
27
28
29
METALS
43
44
Re Os
75
76
47
30
32
46
Ir
Pt Au Hg
Tl
Pb
77
78
81
82
80
33
34
Sn Sb Te
45
79
48
31
51
52
Bi Po At Rn
83
84
85
86
Rf Db Sg Bh Hs Mt
104
105
106
107
108
Metalloids
109
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
57
58
59
Ac Th Pa
89
90
91
60
U
92
61
62
63
64
65
66
67
68
69
70
71
Np Pu Am Cm Bk Cf Es Fm Md No Lr
93
94
95
96
97
98
99
100
101
102
103
Metals, Nonmetals, & Metalloids
1
2
Nonmetals
3
4
5
Metals
6
7
Metalloids
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 349
Properties of Metals, Nonmetals,
and Metalloids
METALS
malleable, lustrous, ductile, good conductors of heat
and electricity
NONMETALS
gases or brittle solids at room temperature, poor
conductors of heat and electricity (insulators)
METALLOIDS (Semi-metals)
dull, brittle, semi-conductors (used in computer chips)
Discovering the Periodic Table
H
Ancient Times
1894-1918
Midd. -1700
1923-1961
1735-1843
1965-
He
1843-1886
Li
Be
B
C
N
O
F
Ne
Na Mg
Al
Si
P
S
Cl
Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
K
Ca Sc
Rb Sr
Y
Cs Ba La
Ti
V
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
Sn Sb Te
Hf
Tl
Pb
Ta
W
Re Os
Ir
Pt Au Hg
Bi
I
Xe
Po At Rn
Fr Ra Ac Rf Db Sg Bh Hs Mt
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Timeline of Elements Discovery
Journal of Chemical Education, Sept. 1989
Th Pa
U
Np Pu Am Cm Bk Cf Es Fm Md No Lr
Discovering the Periodic Table
H
Ancient Times
1894-1918
Midd. -1700
1923-1961
1735-1843
1965-
He
1843-1886
Li
Be
B
C
N
O
F
Ne
Na Mg
Al
Si
P
S
Cl
Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
K
Ca Sc
Rb Sr
Y
Cs Ba La
Ti
V
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
Sn Sb Te
Hf
Tl
Pb
Ta
W
Re Os
Ir
Pt Au Hg
Bi
I
Xe
Po At Rn
Fr Ra Ac Rf Db Sg Bh Hs Mt
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa
Journal of Chemical Education, Sept. 1989
U
Np Pu Am Cm Bk Cf Es Fm Md No Lr
Discovering the Periodic Table
H
Ancient Times
1894-1918
Midd. -1700
1923-1961
1735-1843
1965-
He
1843-1886
Li
Be
B
C
N
O
F
Ne
Na Mg
Al
Si
P
S
Cl
Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
K
Ca Sc
Rb Sr
Y
Cs Ba La
Ti
V
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
Sn Sb Te
Hf
Tl
Pb
Ta
W
Re Os
Ir
Pt Au Hg
Bi
I
Xe
Po At Rn
Fr Ra Ac Rf Db Sg Bh Hs Mt
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa
Journal of Chemical Education, Sept. 1989
U
Np Pu Am Cm Bk Cf Es Fm Md No Lr
Symbols are Useful
The use of symbols is not unique to chemistry.
Symbols can be quite helpful - when you know what they mean.
Arithmetic
+ - x ..
Money
$
Music
c
A Swedish chemist who invented modern chemical symbols.
Discovered the elements:
silicon, selenium, cerium, and thorium.
Jons Jakob Berzelius
(1799 - 1848)
Discovering the Elements
Metal
gold
silver
iron
mercury
tin
Sun
Moon
Mars
Mercury
Jupiter
Solie
Lunae
Martis
Mercurii
Jovis
lundi
mardi
mercredi
jeudi
Monday
Tuesday
Wednesday Thursday
copper lead
Symbol
Celestial body
Venus
Saturn
Day
Latin (dies)
French
dimanche
English
Sunday
Ringnes, Journal of Chemical Education, Sept. 1989, page 731
Veneris Saturni
vendredi
samedi
Friday
Saturday
Chemical Symbols
Gold
Sun
Silver
Moon
Iron
Mars
Copper
Venus
Lead
Saturn
Tin
Jupiter
Mercury
Mercury
Symbols
Ancient
used
Astronomical
in the 16th and
Symbols
17th Century
Fire
Air
Earth
Alchemical Symbols used in the 15th Century
Brownlee, Fuller, Hancock, Sohon, Whitsit, First Principles of Chemistry, 1931, page 74
Water
Chemical Symbols
Antimony
Water
Copper
Sulfur
Sulfuric acid
Symbols used in the 18th Century
Oxygen
Nitrogen
Copper
Hydrogen
Sulfur
Mercury
Carbon
Silver
Water
S
Carbon dioxide
Lead
C
Potassa
L
Alcohol
Symbols used by John Dalton
Brownlee, Fuller, Hancock, Sohon, Whitsit, First Principles of Chemistry, 1931, page 74
Soda
Gold
G
Origin of the Names of Elements
Title
Pre-chemical Names
Names from celestial bodies
Names from mythology / superstition
Names from minerals / ores,
other than geographical names
Names from colors
Names from properties other than color
Geographical names from the domicile or
workplace of the discoverer(s)
Geographical names from minerals / ores
Constructed names
Names from persons
Ringnes, Journal of Chemical Education, Sept. 1989, page 731
Number of Elements
10
8
10
13
9
8
13
10
16
10
Map of Elements Discovered
Ringnes, Journal of Chemical Education, Sept. 1989, page 732
Several Synthetic Elements
Synthetic
•
•
•
•
Man-made
Bk = Berkelium
Cf = Californium
Am = Americium
–
All made by nuclear bombardment
at Berkeley, California, U.S.A.
Einsteinium (Es)
Albert Einstein
– Relativity
– E = mc2
– Offered Presidency of Israel
– Element 99
– Photoelectric effect
• Solar calculator
Curium (Cm)
• Madame Curie
– Pioneer in radioactivity
• (Ra = radium)
– 25 pounds of pitchblende ore
yields 1/1000 of a gram of
radium
– Emits 2 millions times as
much radiation as uranium
• (Rn = radon gas)
– Discovered 5 elements
– Nobel Prize (5 in Curie family)
– Born in Poland
• (Po = polonium)
Marie Curie (1876–1934)
Radium (Ra)
Radium was used as a fluorescent paint on watch dials. It was
applied with thin brushes that workers would lick to keep a fine tip.
Many people died from the exposure to radium.
Radon Gas
Zone 1 counties have a predicted average indoor radon screening
level greater than 4 pCi/L (pico curies per liter) (red zones)
Zone 2 counties have a predicted average indoor radon screening
level between 2 and 4 pCi/L (orange zones)
Zone 3 counties have a predicted average indoor radon screening
level less than 2 pCi/L (yellow zones)
Radon gas occurs naturally
from the radioactive decay
of radium. Radium is found
in small amounts in rock.
Ra  Rn + radiation
Predicted fraction of homes over 4 picocuries/liter radon
http://www.epa.gov/radon/zonemap.html
Nobelium (No)
Element 102
Inventor:
dynamite (TNT)
blasting gelatin
Trinitrotoluene
Nobel Prize
Alfred Nobel
“Merchant of Death”
Seaborgium (Sg)
Glenn Seaborg
– Separated f-block from rest of periodic table
– Worked on Manhattan Project
(Atomic bomb)
– Classified until after WW II
– Element 106
• Only living person to have an element named for
them
Silicon vs. Silicone
• Silicon (Si) element
• Silicone (…Si – O – Si…) polymer
– Sealant (caulk) prevents leaks
– Breast augmentation
No cause-and-effect relationship exists between
breast enlargement and breast cancer. Only one
researcher found a causal link.
12
Mg
24.305
Magnesium
Atomic Mass 24 amu
melting point = 650oC
silver gray metal
(1202oF)
used in flash bulbs, bombs,and flares
8th most abundant element (2.2% of Earth’s crust)
lack of Mg produces same biological effect
as alcoholism (delirium tremens)
Potassium Metal in Water
Newmark, CHEMISTRY, 1993, page 25
Noble
gases
The Periodic Table
1
Alkaline
earth metals
Halogens
18
H
1
He
2
Li
Be
3
4
Na Mg
Alkali metals
11
K
19
3
4
5
6
7
8
9
Transition metals
10
11
12
12
Ca Sc
13
14
15
B
C
N
O
F
Ne
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
13
14
15
16
17
18
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
23
24
35
36
I
Xe
53
54
22
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
50
Hf
Ta
W
72
73
74
Cs Ba
55
56
Fr Ra
87

88
Lanthanides
25
43
26
44
Re Os
75
76
27
28
29
47
30
104
La
Ac
89
105
106
107
108
32
46
Ir
Pt Au Hg
Tl
Pb
77
78
81
82
80
109
110
111
112
33
34
Sn Sb Te
45
79
48
31
Rf Db Sg Bh Hs Mt Uun Uuu Uub
57
 Actinides
2
V
21
38
17
Ti
20
37
16
51
52
Bi Po At Rn
83
84
85
86
Uuq
Uuh
Uuo
113
116
118
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
58
59
Th Pa
90
91
60
U
92
61
62
63
64
65
66
67
68
69
70
71
Np Pu Am Cm Bk Cf Es Fm Md No Lr
93
94
95
96
97
98
99
100
101
102
103
Orbitals Being Filled
1
Periods
1
1s
8
Groups
2
3
4
5
2
2s
2p
3
3s
3p
4
4s
3d
4p
5
5s
4d
5p
6
6s
La
5d
6p
7
7s
Ac
6d
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 345
6
7 1s
4f
Lanthanide series
5f
Actinide series
Electron Filling in Periodic Table
s
p
1
2
d
3
4
5
6
7

f

s
Electron Filling in Periodic Table
metallic character increases
nonmetallic character increases
metallic character increases
nonmetallic character increases
Periodic Table
s
1
s
H
p
H
He
1
2
1
2
3
Li
Be
B
C
N
O
F
Ne
3
4
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
13
14
15
16
17
18
Na Mg
11
4
K
19
5
Ca Sc
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
23
24
35
36
I
Xe
53
54
21
22
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
50
Hf
Ta
W
72
73
74
38
Cs Ba
55
7
12
20
37
6
d
56
Fr Ra
87

88
25
43
26
44
Re Os
75
76
27
28
29
30
47
48
31
32
46
Ir
Pt Au Hg
Tl
Pb
77
78
81
82
80
34
Sn Sb Te
45
79
33
51
52
Bi Po At Rn
83
84
85
86
Rf Db Sg Bh Hs Mt
104
105
106
107
108
109
f
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
57

58
59
Ac Th Pa
89
90
91
60
U
92
61
62
63
64
65
66
67
68
69
70
71
Np Pu Am Cm Bk Cf Es Fm Md No Lr
93
94
95
96
97
98
99
100
101
102
103
Melting Points
1
H
Mg
-259.2
2
3
4
Li
Be
180.5
1283
98
650
K
Ca Sc
850
Rb Sr
38.8
6
> 3000 oC
Na Mg
63.2
5
650
770
710
-269.7
B
V
Y
Al
1500 1852 2487 2610 2127 2427 1966 1550
920
Ta
N
O
Si
P
1423 44.2
S
119
420 29.78 960
W
Re Os
Ir
961
Ne
Cl
In
Ar
-101 -189.6
Kr
817 217.4 -7.2 -157.2
Sn Sb Te
I
Xe
321 156.2 231.9 630.5 450 113.6 -111.9
Pt Au Hg
Tl
Pb Bi
Po
2222 2997 3380 3180 2727 2454 1769 1063 -38.9 303.6 327.4 271.3 254
Ralph A. Burns, Fundamentals of Chemistry , 1999, page 1999
F
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Zr Nb Mo Tc Ru Rh Pd Ag Cd
Hf
C
2027 4100 -210.1 -218.8 -219.6 -248.6
2000 - 3000 oC
1423 1677 1917 1900 1244 1539 1495 1455 1083
Cs Ba La
28.6
He
0.126
Symbol
Melting point oC
660
Ti
He
At
Rn
-71
Elements with Highest Densities
Element
Osmium
Iridium
Platinum
Rhenium
Neptunium
Plutonium
Gold
Tungsten
Uranium
Tantalum
Year
Discovered
1804
1804
1784
1925
1940
1940
prehistoric
1783
1789
1802
Density
(g/cm3)
22.59
22.56
21.45
21.01
20.47
20.26
19.32
19.26
19.05
16.67
1
Densities of
Elements
H
He
0.071
2
3
4
Li
Be
B
C
N
O
0.53
1.8
2.5
2.26
0.81
1.14
Na Mg
Al
Si
P
S
0.97
2.70
2.4 1.82w 2.07 1.557 1.402
K
0.86
5
1.74
Ca Sc
Ti
V
1.55
4.5
5.96
Rb Sr
(2.5)
Ne
1.11 1.204
Cl
Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
7.1
3.119
2.6
I
Xe
4.93
3.06
7.4
7.86
8.9
8.90
8.92
7.14
5.91
5.36
5,7
4.7
In
Sn Sb Te
5.51
6.4
8.4
10.2
8.6
7.3
7.3
6.7
Cs Ba La
Hf
Ta
W
Pt Au Hg
Tl
Pb
Bi Po At Rn
1.90
13.1
16.6
19.3
2.6
3.5
Y
F
Zr Nb Mo Tc Ru Rh Pd Ag Cd
1.53
6
0.126
6.7
8.0 – 11.9 g/cm3
Mg
1.74

11.5
12.5
Re Os
12.5
Ir
12.0
10.5
21.4 22.48 22.4 21.45 19.3 13.55 11.85 11.34
12.0 – 17.9 g/cm3
9.8
6.1
9.4
> 18.0 g/cm3
Symbol
Density in g/cm3C, for gases, in g/L
---
4.4
4f
Sublevels
4d
Energy
n=4
n=3
4p
3d
4s
3p
3s
2p
n=2
2s
n=1
1s
1
H
H
He
1
2
1
2
3
Li
Be
B
C
N
O
F
Ne
3
4
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
13
14
15
16
17
18
Na Mg
11
4
K
19
5
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
23
24
35
36
I
Xe
53
54
21
22
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
50
Hf
Ta
W
72
73
74
38
Cs Ba
55
7
Ca Sc
20
37
6
12
56
Fr Ra
87
88

25
43
26
44
Re Os
75
76
27
28
29
47
30
32
46
Ir
Pt Au Hg
Tl
Pb
77
78
81
82
80
33
34
Sn Sb Te
45
79
48
31
51
52
Bi Po At Rn
83
84
85
86
Rf Db Sg Bh Hs Mt
104
105
106
107
108
109
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
57
58
59
Ac Th Pa
89
90
91
60
U
92
61
62
63
64
65
66
67
68
69
70
71
Np Pu Am Cm Bk Cf Es Fm Md No Lr
93
94
95
96
97
98
99
100
101
102
103
Electron Filling in Periodic Table
s
s
1
2
3
4
5
6
7
H
p
H
He
1s1
1s2
1s1
Li
Be
B
C
N
O
F
Ne
2s1
2s2
2p1
Al
2p2
Si
2p3
P
2p4
S
2p5
Cl
Ar
3s1
K
Ca Sc
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
3p1
3p2
3p3
3p4
3p5
Kr
Na Mg
d
3s2
2p6
3p6
Rb Sr
4s1
4s2
3d1
Y
3d2
Zr Nb Mo Tc Ru Rh Pd Ag Cd
3d3
3d5
3d5
3d6
3d7
3d8
3d10
3d10
4p1
In
Sn Sb Te
4p2
4p3
4p4
4p5
I
Xe
5s1
5s2
4d1
4d2
Hf
Ta
4d4
4d5
W
Re Os
4d6
4d7
4d8
Ir
4d10
Pt Au Hg
4d10
4p1
5p1
Tl
Pb
5p2
5p3
5p4
5p5
5p6
6s1
6s2
5d2
5d3
5d4
5d5
5d6
5d7
5d9
5d10
5d10
6p1
6p2
6p3
6p4
6p5
6p6
6d2
6d3
6d4
6d5
6d6
6d7
Cs Ba
Fr Ra
7s1

7s2
Rf Db Sg Bh Hs Mt
4p6
Bi Po At Rn
f
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu

Ac Th Pa
5d1
4f2
4f3
4f4
6d1
6d2
5f2
5f3
U
4f5
4f6
4f7
4f7
4f9
4f10
4f11
4f12
4f13
4f14
4f114
5f4
5f6
5f7
5f7
5f8
5f10
5f11
5f14
5f13
5f14
5f14
Np Pu Am Cm Bk Cf Es Fm Md No Lr
Names and Symbols of
Selected Elements
Name*
Aluminum
Argon
Barium
Boron
Bromine
Cadmium
Calcium
Carbon
Chlorine
Cobalt
Copper (cuprum)
Fluorine
Gold (aurum)
Helium
Hydrogen
Iodine
Iron (ferrum)
Symbol
Name*
Al
Ar
Ba
B
Br
Cd
Ca
C
Cl
Co
Cu
F
Au
He
H
I
Fe
Symbol
Lead (plumbum)
Lithium
Magnesium
Mercury (hydrargyrum)
Neon
Nickel
Nitrogen
Oxygen
Phosphorus
Potassium (kalium)
Silicon
Silver (argentum)
Sodium (natrum)
Strontium
Sulfur
Tin (stannum)
Zinc
Pb
Li
Mg
Hg
Ne
Ni
N
O
P
K
Si
Ag
Na
Sr
S
Sn
Zn
*Names given in parentheses are ancient Latin or Greek words from which the symbols are derived.
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
Electronegativity
The ability of an
atom in a molecule
to attract shared
electrons to itself.
Linus Pauling
1901 - 1994
Electronegativities
1A
1
H
2.1
2
Period
3
4
5
6
7
8A
2A
3A
4A
5A
6A
7A
Li
Be
B
C
N
O
F
1.0
1.5
2.0
2.5
3.0
3.5
4.0
Al
Si
P
S
Cl
1.5
1.8
2.1
2.5
3.0
Na Mg
4B
5B
Ca Sc
Ti
V
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
1.0
1.3
1.5
1.6
1.6
1.7
1.6
1.8
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
Sn Sb Te
0.8
1.2
1.4
1.6
1.8
1.9
2.2
2.2
2.2
1.7
1.7
1.8
Cs Ba La
Hf
Ta
W
Re Os
Ir
Pt Au Hg
Tl
Pb Bi Po At
0.7
0.9
1.3
1.5
1.7
1.9
2.2
2.2
1.8
1.8
Fr
Ra Ac
0.9
1.2
K
0.8
1.0
3B
1.1

0.9
1.1
8B
7B
1.5
1.8
2.2
1.8
1B
1.8
1.9
1.9
2.4
1.9
2.0
1.9
1.9
2.4
2.1
2.0
Lanthanides: 1.1 - 1.3

0.7
6B
2B
Actinides: 1.3 - 1.5
Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 373
Below 1.0
2.0 - 2.4
1.0 - 1.4
2.5 - 2.9
1.5 - 1.9
3.0 - 4.0
2.8
I
2.5
2.2