Transcript Periodic Patterns - Limestone District School Board

Periodic Table
Kelter, Carr, Scott, Chemistry A Wolrd of Choices 1999, page 74
Electron Configurations and the
Periodic Table
Periodic Patterns
• Period #
– energy level (subtract for d & f)
• A/B Group #
– total # of valence e-
• Column within sublevel block
– # of e- in sublevel
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Periodic Patterns
• Example - Hydrogen
1
2
3
4
5
6
7
1
1s
1st Period
1st column
of s-block
s-block
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Periodic Patterns
• Shorthand Configuration
– Core electrons:
• Go up one row and over to the Noble Gas.
– Valence electrons:
• On the next row, fill in the # of e- in each sublevel.
1
2
3
4
5
6
7
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32
Periodic Patterns
• Example - Germanium
1
2
3
4
5
6
7
[Ar]
2
4s
10
3d
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2
4p
Ge
72.61
Stability
• Full energy level
• Full sublevel (s, p, d, f)
• Half-full sublevel
1
2
3
4
5
6
7
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Stability
• Electron Configuration Exceptions
– Copper
EXPECT:
[Ar] 4s2 3d9
ACTUALLY:
[Ar] 4s1 3d10
– Copper gains stability with a full
d-sublevel.
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Stability
• Electron Configuration Exceptions
– Chromium
EXPECT:
[Ar] 4s2 3d4
ACTUALLY:
[Ar] 4s1 3d5
– Chromium gains stability with a half-full
d-sublevel.
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Stability
• Ion Formation
– Atoms gain or lose electrons to become more
stable.
– Isoelectronic with the Noble Gases.
1
2
3
4
5
6
7
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Stability
• Ion Electron Configuration
– Write the e- config for the closest Noble Gas
– EX: Oxygen ion  O2-  Ne
O2-
10e-
[He] 2s2 2p6
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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
Mendeleev’s Periodic Table
Group I
II
III
IV
V
VI
VII
VIII
F = 19
Period
1
H=1
2
Li = 7
Be= 9.4
B = 11
C = 12
N = 14
O = 16
F = 19
3
Na = 23
Mg = 24
Al = 27.3
Si = 28
P = 31
S = 32
C = 35.5
4
K = 39
Ca = 40
? = 44
Ti = 48
V = 51
Cr = 52
Mn = 55
5
Cu = 63
Zn = 65
? = 68
? = 72
As = 75
Se = 78
Br = 80
6
Rb = 85
Sr = 87
? Yt = 88
Zr = 90
Nb = 94
Mo = 96
? = 100
7
Ag = 108
Cd = 112
In = 113
Sn = 118
Sb = 122
Te = 125
J = 127
8
Cs = 133
Ba = 137
?Di = 138
?Ce = 140
?Er = 178
?La = 180
Ta = 182
W = 184
Tl = 204
Pb = 207
Bi = 208
Fe =56, Co = 59,
Ni = 59
Ru= 104, Rh = 104,
Pd = 106
9
10
11
12
Au = 199
Hg = 200
Th = 231
U = 240
Os = 195, Ir = 197,
Pt = 198
Mendeleev’s Early Periodic Table
REIHEN
TABELLE II
GRUPPE I
___
Li = 7
K = 39
11
12
Ca = 40
Rb = 85
RH3
R2O5
Cs = 133
__
GRUPPE VI
GRUPPE VII
RH2
RO3
? Yt = 88
Ba = 137
In = 113
? Di = 138
__
__
__
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
(Au = 199)
__
__ = 44
Sr = 87
( __ )
C = 12
Al = 27.3
Zn = 65
(Ag = 108)
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
Property
Mendeleev’s Predictions in 1871
Observed Properties
Scandium (Discovered in 1877)
Molar Mass
Oxide formula
Density of oxide
Solubility of oxide
44 g
M2O3
3.5 g / ml
Dissolves in acids
43.7 g
Sc2O3
3.86 g / ml
Dissolves in acids
Gallium (Discovered in 1875)
Molar mass
Density of metal
Melting temperature
Oxide formula
Solubility of oxide
68 g
6.0 g / ml
Low
M2O3
Dissolves in ammonia solution
69.4 g
5.96 g / ml
30 0C
Ga2O3
Dissolves in ammonia
Germanium (Discovered in 1886)
Molar mass
Density of metal
Color of metal
Melting temperature
Oxide formula
Density of oxide
Chloride formula
Density of chloride
Boiling temperature
of chloride
72 g
5.5 g / ml
Dark gray
High
MO2
4.7 g / ml
MCl4
1.9 g / ml
Below 100 oC
O’Connor Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 119,
71.9 g
5.47 g / ml
Grayish, white
900 0C
GeO2
4.70 g / ml
GeCl4
1.89 g / ml
86 0C
Modern Periodic Table
• H.G.J. Moseley
• Arranged elements by
increasing atomic
number
• Killed in WW I at age
28
(Battle of Gallipoli)
1887 - 1915
Groups of Elements
1A
1
H
1
2
3
Be
3
4
7
2A
Alkali earth metals
6A
Oxygen group
Transition metals
7A
Halogens
3A
Boron group
8A
Noble gases
4A
Carbon group
8A
He
3A 4A
B C
5A 6A 7A 2
N O F Ne
Hydrogen
Inner transition metals
5
6
7
8
9
10
Al
Si
P
S
Cl
Ar
8B
K
3B 4B 5B 6B 7B
1B 2B 13 14 15 16 17
Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
12
20
21
22
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
Hf
Ta
W
72
73
74
37
6
Nitrogen group
Na Mg
19
5
5A
2A
Li
11
4
1A Alkali metals
38
Cs Ba
55
56
Fr
Ra
87
88
*
W
25
43
26
44
Re Os
75
76
27
28
29
47
30
45
46
Ir
Pt Au Hg
Tl
77
78
81
79
48
31
80
32
33
34
Sn Sb Te
50
51
Pb Bi
82
83
52
35
36
I
Xe
53
54
Po At Rn
84
85
86
105
106
107
108
109
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
57
W
24
Kr
Rf Db Sg Bh Hs Mt
104
*
23
18
58
59
Ac Th Pa
89
90
91
60
U
92
61
62
63
64
65
66
Np Pu Am Cm Bk Cf
93
94
95
96
97
98
67
68
69
70
71
Es Fm Md No Lr
99
100
101
102
103
Groups of Elements
Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 367
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
Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 367
1
Alkali metals
2
Alkali earth metals 17 Halogens
15
Nitrogen family
16
18
Oxygen family
Noble gases
Metals and Nonmetals
1
2
3
H
He
1
2
Li
Be
B
C
3
4
5
Na Mg
11
4
K
19
5
7
Ca Sc
O
F
Ne
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
20
21
22
Rb Sr
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
39
40
41
42
49
Hf
Ta
W
72
73
74
37
6
12
N
38
Cs Ba
55
56
Fr
Ra
87
88
*
W
Nonmetals
25
26
27
28
29
30
METALS
43
44
Re Os
75
76
47
45
46
Ir
Pt Au Hg
Tl
77
78
81
79
48
31
80
32
33
34
Sn Sb Te
50
51
Pb Bi
82
83
52
Po At Rn
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
Np Pu Am Cm Bk Cf
93
94
95
96
97
98
67
68
69
70
71
Es Fm Md No Lr
99
100
101
102
103
Metals, Nonmetals, & Metalloids
1
Nonmetals
2
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
Li
Ancient Times
1894-1918
Midd. -1700
1923-1961
1735-1843
1965-
1843-1886
Be
B
C
N
O
F
Ne
Al
Si
P
S
Cl
Ar
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Kr
Na Mg
K
Ca Sc
Rb Sr
Y
Cs Ba La
Fr
Ti
V
He
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
Sn Sb Te
Hf
Tl
Pb Bi
Ta
W
Re Os
Ir
Pt Au Hg
I
Xe
Po At Rn
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
Electron Filling in Periodic Table
metallic character increases
nonmetallic character increases
metallic character increases
nonmetallic character increases
Melting Points
He
1
H
Mg
-259.2
2
3
4
Li
Be
180.5
1283
650
K
Ca Sc
Rb Sr
38.8
6
> 3000
98
850
770
710
B
oC
2000 - 3000
oC
Al
660
Ti
V
C
N
O
F
Y
1500 1852 2487 2610 2127 2427 1966 1550
920
Ta
P
1423 44.2
420 29.78 960
Zr Nb Mo Tc Ru Rh Pd Ag Cd
Hf
Si
S
119
Ne
W
Re Os
Ir
961
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 At Rn
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
Cl
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
1423 1677 1917 1900 1244 1539 1495 1455 1083
Cs Ba La
28.6
-269.7
2027 4100 -210.1 -218.8 -219.6 -248.6
Na Mg
63.2
5
650
He
0.126
Symbol
Melting point oC
-71
Densities of
Elements
1
2
3
4
H
He
0.071
0.126
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
Ca Sc
Ti
V
1.55
4.5
5.96
Rb Sr
(2.5)
2.6
I
Xe
4.93
3.06
7.86
8.9
8.90
8.92
7.14
5.91
5.36
5,7
4.7
6.4
8.4
10.2
8.6
7.3
7.3
Cs Ba La
Hf
Ta
W
Pt Au Hg
Tl
Pb Bi
1.90
13.1
16.6
19.3
8.0 – 11.9 g/cm3
Mg
1.74
W
Ralph A. Burns, Fundamentals of Chemistry , 1999, page 200
Ar
3.119
7.4
5.51
6.7
Cl
7.1
Sn Sb Te
3.5
1.11 1.204
Kr
In
2.6
Y
Ne
Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br
Zr Nb Mo Tc Ru Rh Pd Ag Cd
1.53
6
1.74
F
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
6.7
9.8
6.1
Po At Rn
9.4
> 18.0 g/cm3
Symbol
Density in g/cm3C, for gases, in g/L
---
4.4
Periodic Trends in Atomic Radii
LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 175
Relative Size of Atoms
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 350
Shielding Effect
Valence
+
nucleus
-
Kernel electrons block
the attractive force of
the nucleus from the
valence electrons
-
Electron
Shield
“kernel”
electrons
Electrons
Atomic Radii
Atomic
Radii
vs.
Ionic
Radii
First Ionization Energy Plot
First Ionization
Energy Plot
5s
5p
4d
18
4s
4p
3d
18
3s
3p
8
2s
2p
8
1s
2
NUCLEUS
First Ionization
Energy Plot
5s
5p
4d
18
4s
4p
3d
18
3s
3p
8
2s
2p
8
1s
2
NUCLEUS
Formation of Cation
sodium atom
Na
sodium ion
Na+
ee-
e-
e-
e-
e-
ee-
e-
11p+
ee-
loss of
one valence
electron
e-
e-
11p+
e-
e-
e-
e-
e-
e-
e-
e-
Formation of Anion
chlorine atom
Cl
e-
egain of
one valence
electron
ee-
e-
e-
chloride ion
Cl1e-
eee-
e-
e-
e-
ee-
e-
17p+
17p+
e-
e-
e-
e-
ee-
e-
e-
ee-
e-
e-
e-
e-
e-
ee-
e-
Nuclear charge increases
Shielding increases
Atomic radius increases
Ionic size increases
Ionization energy decreases
Electronegativity decreases
Summary of Periodic Trends
Shielding is constant
Atomic radius decreases
Ionization energy increases
Electronegativity increases
Nuclear charge increases
1A
0
2A
Ionic size (cations)
decreases
3A 4A 5A 6A 7A
Ionic size (anions)
decreases