periodic table kelter, carr, scott, chemistry a wolrd of choices 1999, page 74
TRANSCRIPT
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 ElementsMendeleev’s Periodic TableModern Periodic TableGroups of ElementsMetals, Nonmetals,
MetalloidsDiscovering ElementsOrigin of Names of ElementsSelected Elements
Electron Filling OrderDiatomic MoleculesSize of Atoms – TrendsIonization EnergySummary of Periodic TrendsEssential ElementsElement Project
Atomic Structure and PeriodicityYou 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 orbitaldiagrams 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, ionizationenergy, electronegativity, electron affinity, and ionic size.
18e-18e- 20e-
19+ 20+
Potassium atom = [Ar]4s1 Calcium atom = [Ar]4s2
19e-
Potassium ion = K1+ ≡ [Ar] 1s22s22p63s23p6
Calcium ion = Ca2+ ≡ [Ar] or 1s22s22p63s23p6
p = 19n = 20e = 19
K e- + K1+
p = 20n = 20e = 20
Ca 2 e- + Ca2+
>
8 e- 8 e-7 e-6 e-
8+ 9+
Oxygen atom = [He]2s22p4 Fluorine atom = [He] 2s22p5
Oxygen ion = O2- ≡ [Ne] 1s22s22p6
Fluorine ion = F1- ≡ [Ne] 1s22s22p6
p = 8n = 8e = 8
O + 2 e- O2-
p = 9n = 10e = 9
F + e- F1-
<
Oxide ion Fluoride ion
Energy Level Diagram of a Many-Electron Atom
ArbitraryEnergy Scale
18
18
32
8
8
2
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
How to Organize Elements… Periodic Table Designs
How to Organize…
Baseball Cards:year, team, player, card number, value ($).
Elements:when they were discovered, family, reactivity, state of matter, metal vs. non-metal, atomic mass,atomic number.
alphabetically, mass, value, density, solid or liquid or gas
Which way is CORRECT to organize the elements?Which way is CORRECT to organize the elements?
Is it possible to organize the elements correctly in more than one way?Is it possible to organize the elements correctly in more than one way?
Li
3
H
1
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
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
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
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
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
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
La
57
Ac
89
1
2
3
4
5
6
7
∗
Ω
N7
C6
H1
S16
Ir77
O8
N7
Mn25
e
<
The Human ElementThe Human Element
Interactive Periodic Table
Aliens ActivityNautilus 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
Li
3
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
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
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
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
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
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
La
57
Ac
89
1
2
3
4
5
6
7
1A
2A
Alkali metals
Alkali earth metals
Transition metals
Boron group
Nonmetals
Noble gases
3B 5B 6B 7B 8B 1B 2B
3A 4A 5A 6A 7A
8A
4B
Lanthanoid Series
6
7Actinoid Series
C Solid
Br Liquid
H Gas
Dutch Periodic Table
106
107
108
109
110
111
112
113
114
115116
117 118
Strong, Journal of Chemical Education, Sept. 1989, page 743
Stowe’s Periodic Table
Benfey’s Periodic Table
Döbereiner’s Triads
NameAtomicMass Name
AtomicMass Name
AtomicMass
Calcium 40Barium 137
Average 88.5
Strontium 87.6
Chlorine 35.5Iodine 127
Average 81.3
Bromine 79.9
Sulfur 32Tellurium 127.5
Average 79.8
Selenium 79.2
Johann Döbereiner ~1817
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
Newlands Law of Octaves
1
LiNaK
John Newlands ~1863
Smoot, Price, Smith, Chemistry A Modern Course 1987, page 161
2
BeMg
3
BAl
4
CSi
5
NP
6
OS
7
FCl
Development of Periodic Table
Law of Triads
Law of Octaves
Elements could be classified into groups of three, or triads.Trends in physical properties such as density, melting point, and atomic mass were observed.
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.
J.W. Döbereiner (1829)
J.A.R. Newlands (1864)
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
GRUPPE I GRUPPE II GRUPPE III GRUPPE IV GRUPPE V GRUPPE VI GRUPPE VII GRUPPE VIII ___ ___ ___ ___
RH4 RH3 RH2 RH R2O RO R2O3 RO2 R2O5 RO3 R2O7 RO4 R
EIH
EN
1
2
3
4
5
6
7
8
9
10
11
12
From Annalen der Chemie und PharmacieAnnalen der Chemie und Pharmacie, VIII, Supplementary Volume for 1872, p. 151.
H = 1
Li = 7 Be = 9.4 B = 11 C = 12 N = 14 O = 16 F = 19
Na = 23 Mg = 24 Al = 27.3 Si = 28 P = 31 S = 32 Cl = 35.5
K = 39 Ca = 40 __ = 44 Ti = 48 V = 51 Cr = 52 Mn = 55 Fe = 56, Co = 59,
Ni = 59, Cu = 63(Cu = 63) Zn = 65 __ = 68 __ = 72 As = 75 Se = 78 Br = 80
Rb = 85 Sr = 87 ? Yt = 88 Zr = 90 Nb = 94 Mo = 96 __ = 100 Ru = 104, Rh = 104,
Pd = 106, Ag = 108 (Ag = 108) Cd = 112 In = 113 Sn = 118 Sb = 122 Te = 125 J = 127
Cs = 133 Ba = 137 ? Di = 138 ? Ce = 140 __ __ __ __ __ __ __
( __ ) __ __ __ __ __ __
__ __ ? Er = 178 ? La = 180 Ta = 182 W = 184 __ Os = 195, Ir = 197,
Pt = 198, Au = 199 (Au = 199) Hg = 200 Tl= 204 Pb = 207 Bi = 208 __ __
__ __ __ Th = 231 __ U = 240 __ __ __ __ __
TABELLE II
?
? ?
Elements Properties are Predicted
O’Connor Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 119,
Periodic Table of the Elements
Li
3
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
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
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
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
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
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
La
57
Ac
89
1
2
3
4
5
6
7
∗
Ω
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
1
2
3
4
5
6
7
∗
Ω
Ω
∗
Li
3
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
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
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
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
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
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
La
57
Ac
89
1
2
3
4
5
6
7
∗
Ω
1A
2A
1A
2A
3A
4A
5A
6A
7A
8A
Alkali metals
Alkali earth metals
Transition metals
Inner transition metals
Boron group
Carbon group
Nitrogen group
Oxygen group
Halogens
Noble gases
Hydrogen
3B 5B 6B 7B 8B 1B 2B
3A 4A 5A 6A 7A
8A
4B
Groups of Elements
Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 367
N
7
P
15
As
33
Sb
51
Bi
83
O
8
S
16
Se
34
Te
52
Po
84
F
9
Cl
17
Br
35
I
53
At
85
He
2
Ne
10
Ar
18
Kr
36
Xe
54
Rn
86
Li
3
Na
11
K
19
Rb
37
Cs
55
Fr
87
Be
4
Ca
20
Sr
38
Ba
56
Ra
88
Mg
12
1
2
1
2
15
16
17
18
Alkali metals
Alkaline earth metals
Nitrogen family
Oxygen family
Halogens
Noble gases
13 14 15 16 17
18
Diatomic ElementsH2
N2 O2 F2
Cl2
Br2
I2
Tl At
S
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Pb Bi Po
Al Si P
B C
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
Tl
Alkali Metals, Group 1H
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
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 2H
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
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 17H
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
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 18H
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
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 16H
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
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
Group 16, the Chalcogens – The chalcogens are oxygen, sulfur, selenium, tellurium, and
polonium.
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.
Chemistry of the Groups
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
O
8
S
16
Se
34
Te
52
Po
84
16
Pnicogens, Group 15H
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
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
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
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:
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
N
7
P
15
As
33
Sb
51
Bi
83
15
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 closed- shell electron configuration of the preceding noble gas
3. +2, in which the loss of two np2 electrons gives a filled ns2
subshell
Chemistry of the Groups
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
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.
Chemistry of the Groups
Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.
Lanthanide SeriesH
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
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
La
Actinide SeriesH
N O F
Cl
Br
I
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At
Al Si P S
B C
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
La
La
Chemistry of the Groups
1
2
3
4
5
6
7
∗
Ω
Ω
∗
Li
3
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
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
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
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
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
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
La
57
Ac
89
1
2
3
4
5
6
7
∗
Ω
1A
2A
3B 5B 6B 7B 8B 1B 2B
3A 4A 5A 6A 7A
8A
4B
Transition Metals
Actinides
Lanthanides
Metals and Nonmetals
Li
3
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
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
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
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
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
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
La
57
Ac
89
1
2
3
4
5
6
7
∗
Ω
METALS
Nonmetals
Metalloids
Metals, Nonmetals, & Metalloids1
2
3
4
5
6
7
Metals
Metalloids
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 349
Nonmetals
Properties of Metals, Nonmetals, and Metalloids
METALSMETALS
NONMETALSNONMETALS
METALLOIDSMETALLOIDS
malleable, lustrous, ductile, good conductors of heat and electricity
gases or brittle solids at room temperature, poor conductors of heat and electricity (insulators)
(Semi-metals)dull, brittle, semi-conductors (used in computer chips)
Cr Mn
Li
K
N O F
Na
BBe
H
Al Si Cl
Ca Ti V Co Ni Se Br
Sr Y Zr Nb Mo Rh Pd Cd Te I
Ba Ta W Os Ir
Mg
Ce Tb Er
Th U
P
Zn As
Sb
Pt Bi
Midd. -1700
1735-1843
Discovering the Periodic Table
C
S
Fe Cu
Ag Sn
Au Hg Pb
Ancient Times
He
Sc Ga Ge
Rb Ru In
Cs Tl
Pr Nd Sm Gd Dy Ho Tm Yb
La
1843-1886
Ne
Ar
Kr
Xe
Po Rn
Ra
Eu Lu
Pa
Ac
1894-1918
Tc
Hf Re At
Fr
Pm
Np Pu Am Cm Bk Cf Es Fm Md No Lr
1923-1961
Rf Db Sg Bh Hs Mt
1965-
Journal of Chemical Education, Sept. 1989Timeline of Elements Discovery
Cr Mn
Li
K
N O F
Na
BBe
H
Al Si Cl
Ca Ti V Co Ni Se Br
Sr Y Zr Nb Mo Rh Pd Cd Te I
Ba Ta W Os Ir
Mg
Ce Tb Er
Th U
P
Zn As
Sb
Pt Bi
Midd. -1700
1735-1843
Discovering the Periodic Table
C
S
Fe Cu
Ag Sn
Au Hg Pb
Ancient Times
He
Sc Ga Ge
Rb Ru In
Cs Tl
Pr Nd Sm Gd Dy Ho Tm Yb
La
1843-1886
Ne
Ar
Kr
Xe
Po Rn
Ra
Eu Lu
Pa
Ac
1894-1918
Tc
Hf Re At
Fr
Pm
Np Pu Am Cm Bk Cf Es Fm Md No Lr
1923-1961
Rf Db Sg Bh Hs Mt
1965-
Journal of Chemical Education, Sept. 1989
P
Zn As
Sb
Pt Bi
Midd. -1700
Cr Mn
Li
K
N O F
Na
BBe
H
Al Si Cl
Ca Ti V Co Ni Se Br
Sr Y Zr Nb Mo Rh Pd Cd Te I
Ba Ta W Os Ir
Mg
Ce Tb Er
Th U
1735-1843
Discovering the Periodic Table
C
S
Fe Cu
Ag Sn
Au Hg Pb
Ancient Times
He
Sc Ga Ge
Rb Ru In
Cs Tl
Pr Nd Sm Gd Dy Ho Tm Yb
La
1843-1886
Ne
Ar
Kr
Xe
Po Rn
Ra
Eu Lu
Pa
Ac
1894-1918
Tc
Hf Re At
Fr
Pm
Np Pu Am Cm Bk Cf Es Fm Md No Lr
1923-1961
Rf Db Sg Bh Hs Mt
1965-
Journal of Chemical Education, Sept. 1989
Symbols are UsefulThe use of symbols is not unique to chemistry.Symbols can be quite helpful - when you know what they mean.
Arithmetic Money Music
$ + - x .. c
Jons Jakob Berzelius (1799 - 1848)
A Swedish chemist who invented modern chemical symbols.
Discovered the elements: silicon, selenium, cerium, and thorium.
Discovering the Elements
Celestial body Sun Moon Mars Mercury Jupiter Venus Saturn
DayLatin (Latin (diesdies) ) Solie Lunae Martis Mercurii Jovis Veneris Saturni
French French dimanche lundi mardi mercredi jeudi vendredi samedi
English English Sunday Monday Tuesday Wednesday Thursday Friday Saturday
Metal gold silver iron mercury tin copper lead
Symbol
Ringnes, Journal of Chemical Education, Sept. 1989, page 731
Chemical Symbols
Ancient Astronomical Symbols
Sun Moon Mars Venus Saturn Jupiter Mercury
Symbols used in the 16th and 17th Century
Gold Silver Iron Copper Lead Tin Mercury
Alchemical Symbols used in the 15th CenturyFire Air Earth Water
Brownlee, Fuller, Hancock, Sohon, Whitsit, First Principles of Chemistry, 1931, page 74
Chemical Symbols
Symbols used in the 18th Century
Antimony Water Sulfuric acidCopper Sulfur
Symbols used by John Dalton
Carbon
Hydrogen
Oxygen
Silver
Sulfur
Nitrogen
S Lead
Mercury
Copper C
L Gold
Potassa
Soda
G
Water Carbon dioxide Alcohol
Brownlee, Fuller, Hancock, Sohon, Whitsit, First Principles of Chemistry, 1931, page 74
Origin of the Names of Elements
Title Number of Elements
Pre-chemical Names 10Names from celestial bodies 8Names from mythology / superstition 10Names from minerals / ores,
other than geographical names 13Names from colors 9Names from properties other than color 8Geographical names from the domicile or
workplace of the discoverer(s) 13Geographical names from minerals / ores 10Constructed names 16Names from persons 10
Ringnes, Journal of Chemical Education, Sept. 1989, page 731
Map of Elements Discovered
Ringnes, Journal of Chemical Education, Sept. 1989, page 732
Several Synthetic Elements
• Man-made• Bk = Berkelium• Cf = Californium• Am = Americium
Synthetic
– 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 wasapplied with thin brushes that workers would lick to keep a fine tip. Many people died from the exposure to radium.
Radon Gas
Radon gas occurs naturallyfrom the radioactive decayof radium. Radium is found in small amounts in rock.
Ra Rn + radiation
Predicted fraction of homes over 4 picocuries/liter radon
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)
http://www.epa.gov/radon/zonemap.html
Nobelium (No)Element 102
Alfred Nobel
Nobel PrizeInventor: dynamite (TNT) blasting gelatin
“Merchant of Death”
Trinitrotoluene
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 oneresearcher found a causal link.
Magnesium
Atomic Mass 24 amumelting point = 650oC (1202oF)
silver gray metal
used in flash bulbs, bombs,and flares8th most abundant element (2.2% of Earth’s crust)
lack of Mg produces same biological effect as alcoholism (delirium tremens)
Mg24.305
12
The Periodic Table
Li
3
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
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
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
88Ψ
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
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
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
La
57
Ac
89
1
2
3 4 5 6 7
∗ Lanthanides
Ψ Actinides
Noblegases
Halogens
Transition metals
Alkalineearth metals
Alk
ali
meta
ls
8 9 10 11 12
13 14 15 16 17
18
Uun
110
Uuu
111
Uub
112
Uuq
113
Uuh
116
Uuo
118
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
Electron Filling in Periodic Table
1
2
3
4
5
6
7
s
d
p
s
f
∗
Ω
Ω
∗
Electron Filling in Periodic Tablemetallic character increases
nonmetallic character increases
met
allic
cha
ract
er in
crea
ses
non
met
allic
cha
ract
er in
crea
ses
1
2
3
4
5
6
7
s
d
p
s
f
∗
Ω
Ω
∗
Li
3
H
1
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
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
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
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
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
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
La
57
Ac
89
1
2
3
4
5
6
7
∗
Ω
Periodic Table
1
2
3
4
5
6
Li
180.5
He
-269.7
C
4100
N
-210.1
O
-218.8
F
-219.6
Ne
-248.6
Na
98
B
2027
Be
1283
H
-259.2
Al
660
Si
1423
P
44.2
S
119
Cl
-101
Ar
-189.6
K
63.2
Ca
850
Sc
1423
Ti
1677
V
1917
Cr
1900
Mn
1244
Fe
1539
Co
1495
Ni
1455
Cu
1083
Zn
420
Ga
29.78
Ge
960
As
817
Se
217.4
Br
-7.2
Kr
-157.2
Rb
38.8
Sr
770
Y
1500
Zr
1852
Nb
2487
Mo
2610
Tc
2127
Ru
2427
Rh
1966
Pd
1550
Ag
961
Cd
321
In
156.2
Sn
231.9
Sb
630.5
Te
450
I
113.6
Xe
-111.9
Cs
28.6
Ba
710
Hf
2222
Ta
2997
W
3380
Re
3180
Os
2727
Ir
2454
Pt
1769
Au
1063
Hg
-38.9
Tl
303.6
Pb
327.4
Bi
271.3
Po
254At
Rn
-71
Mg
650
Mg
650
1
2
3
4
5
6
Melting PointsSymbolMelting point oC
> 3000 oC 2000 - 3000 oC
La
920
He
0.126
Ralph A. Burns, Fundamentals of Chemistry , 1999, page 1999
Elements with Highest Densities
Year DensityElement Discovered (g/cm3)
Osmium 1804 22.59Iridium 1804 22.56Platinum 1784 21.45Rhenium 1925 21.01Neptunium 1940 20.47Plutonium 1940 20.26Gold prehistoric 19.32Tungsten 1783 19.26Uranium 1789 19.05Tantalum 1802 16.67
1
2
3
4
5
6
Ω
Li
0.53
He
0.126
C
2.26
N
0.81
O
1.14
F
1.11
Ne
1.204
Na
0.97
B
2.5
Be
1.8
H
0.071
Al
2.70
Si
2.4
P
1.82w
S
2.07
Cl
1.557
Ar
1.402
K
0.86
Ca
1.55
Sc
(2.5)
Ti
4.5
V
5.96
Cr
7.1
Mn
7.4
Fe
7.86
Co
8.9
Ni
8.90
Cu
8.92
Zn
7.14
Ga
5.91
Ge
5.36
As
5,7
Se
4.7
Br
3.119
Kr
2.6
Rb
1.53
Sr
2.6
Y
5.51
Zr
6.4
Nb
8.4
Mo
10.2
Tc
11.5
Ru
12.5
Rh
12.5
Pd
12.0
Ag
10.5
Cd
8.6
In
7.3
Sn
7.3
Sb
6.7
Te
6.1
I
4.93
Xe
3.06
Cs
1.90
Ba
3.5
Hf
13.1
Ta
16.6
W
19.3
Re
21.4
Os
22.48
Ir
22.4
Pt
21.45
Au
19.3
Hg
13.55
Tl
11.85
Pb
11.34
Bi
9.8
Po
9.4
At
---
Rn
4.4
Mg
1.74
1
2
3
4
5
6
Densities of Elements
Mg
1.74
SymbolDensity in g/cm3C, for gases, in g/L
8.0 – 11.9 g/cm3 12.0 – 17.9 g/cm3 > 18.0 g/cm3
La
6.7
4f
4d
4p
4s
n = 4
3d
3p
3s
n = 3
2p
2s
n = 2
1sn = 1
En
erg
y
Sublevels
Li
3
H
1
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
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
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
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
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
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
La
57
Ac
89
1
2
3
4
5
6
7
∗
Ω
1
2
3
4
5
6
7
s
d
p
s
f
∗
Ω
Ω
∗
Electron Filling in Periodic Table
Li
2s1
H
1s1
He
1s2
C
2p2
N
2p3
O
2p4
F
2p5
Ne
2p6
Na
3s1
B
2p1
Be
2s2
H
1s1
Al
3p1
Si
3p2
P
3p3
S
3p4
Cl
3p5
Ar
3p6
K
4s1
Ca
4s2
Sc
3d1
Ti
3d2
V
3d3
Cr
3d5
Mn
3d5
Fe
3d6
Co
3d7
Ni
3d8
Cu
3d10
Zn
3d10
Ga
4p1
Ge
4p2
As
4p3
Se
4p4
Br
4p5
Kr
4p6
Rb
5s1
Sr
5s2
Y
4d1
Zr
4d2
Nb
4d4
Mo
4d5
Tc
4d6
Ru
4d7
Rh
4d8
Pd
4d10
Ag
4d10
Cd
4p1
In
5p1
Sn
5p2
Sb
5p3
Te
5p4
I
5p5
Xe
5p6
Cs
6s1
Ba
6s2
Hf
5d2
Ta
5d3
W
5d4
Re
5d5
Os
5d6
Ir
5d7
Pt
5d9
Au
5d10
Hg
5d10
Tl
6p1
Pb
6p2
Bi
6p3
Po
6p4
At
6p5
Rn
6p6
Fr
7s1
Ra
7s2
Rf
6d2
Db
6d3
Sg
6d4
Bh
6d5
Hs
6d6
Mt
6d7
Mg
3s2
Ce
4f2
Pr
4f3
Nd
4f4
Pm
4f5
Sm
4f6
Eu
4f7
Gd
4f7
Tb
4f9
Dy
4f10
Ho
4f11
Er
4f12
Tm
4f13
Yb
4f14
Lu
4f114
Th
6d2
Pa
5f2
U
5f3
Np
5f4
Pu
5f6
Am
5f7
Cm
5f7
Bk
5f8
Cf
5f10
Es
5f11
Fm
5f14
Md
5f13
No
5f14
Lr
5f14
La
5d1
Ac
6d1
1
2
3
4
5
6
7
s
d
p
s
f
∗
Ω
Ω
∗
Names and Symbols of Selected Elements
Name* Symbol Name* Symbol
Aluminum Al Lead (plumbum) PbArgon Ar Lithium LiBarium Ba Magnesium MgBoron B Mercury (hydrargyrum) HgBromine Br Neon NeCadmium Cd Nickel NiCalcium Ca Nitrogen NCarbon C Oxygen OChlorine Cl Phosphorus PCobalt Co Potassium (kalium) KCopper (cuprum) Cu Silicon SiFluorine F Silver (argentum) AgGold (aurum) Au Sodium (natrum) NaHelium He Strontium SrHydrogen H Sulfur SIodine I Tin (stannum) SnIron (ferrum) Fe Zinc 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 anatom in a molecule to attract sharedelectrons to itself.
Linus Pauling1901 - 1994
1
2
3
4
5
6
1
2
3
4
5
6
Electronegativities
7
Be
1.5
Al
1.5
Si
1.8
Ti
1.5
V
1.6
Cr
1.6
Mn
1.5
Fe
1.8
Co
1.8
Ni
1.8
Cu
1.9
Zn
1.7
Ga
1.6
Ge
1.8
Nb
1.6
Mo
1.8
Tc
1.9
Ag
1.9
Cd
1.7
In
1.7
Sn
1.8
Sb
1.9
Ta
1.5
W
1.7
Re
1.9
Hg
1.9
Tl
1.8
Pb
1.8
Bi
1.9
1.5 - 1.9
N
3.0
O
3.5
F
4.0
Cl
3.0
3.0 - 4.0
C
2.5
S
2.5
Br
2.8
I
2.5
2.5 - 2.9
Na
0.9
K
0.8
Rb
0.8
Cs
0.7
Ba
0.9
Fr
0.7
Ra
0.9
Below 1.0
H
2.1
B
2.0
P
2.1
As
2.0
Se
2.4
Ru
2.2
Rh
2.2
Pd
2.2
Te
2.1
Os
2.2
Ir
2.2
Pt
2.2
Au
2.4
Po
2.0
At
2.2
2.0 - 2.4
Per
iod
Actinides: 1.3 - 1.5
Li
1.0
Ca
1.0
Sc
1.3
Sr
1.0
Y
1.2
Zr
1.4
Hf
1.3
Mg
1.2
La
1.1
Ac
1.1
1.0 - 1.4
Lanthanides: 1.1 - 1.3
∗
∗ψ
ψ
1A
2A
3B 4B 5B 6B 7B 1B 2B
3A 4A 5A 6A 7A
8A
Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 373
8B