Chapter 4 Periodic Table of Elements.ppt

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1. Chapter 6:
The Periodic Table

2. Organizing the Elements
Demitri Mendeleeve(Russian –1869)
Published the 1
st
periodic table
Based on atomic mass

3. The Periodic Law
Modern Periodic Table
Organized according to atomic number
Periods = rows 1-7
equal to the principal energy level
Groups= columns 1-18
elements have similar properties
Law:Properties of elements repeat as you
move from Left→ Rightacross a period

4. Period → Group ↓

5. Metallic Character
Approx. 2/3 of the elements are metals
Metallic Properties
Luster
Conductivity
Malleability
Ductility
Tend to lose electrons
Nonmetallic Properties
Dull luster
Poor conductors
Brittle
Tend to gain electrons
Metalloids (semimetals)
Some properties characteristic of metals and other
properties characteristic of nonmetals

6. 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
He
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
*
W
METALS
Nonmetals
Metalloids

7. Reference Table
•Periodic Table
Trends:
1. Across a period, metallic character →
Why?
More electrons in outer shells
Less tendency to lose electrons
2. Down a group, metallic character →
Why?
Less electrons in outer shells
Greater tendency to lose electrons
decreases
increases

8. Metallic Review
Identify each element as a metal,
nonmetal or metalloid
a)Gold -
b)Silicon -
c)Sulfur -
d)Barium -
Metal
Metalloid
Nonmetal
Metal

9. Which of these sets of elements have
similar physical and chemical properties?
a)oxygen, nitrogen, carbon,
b)strontium, magnesium, calcium, beryllium
c)nitrogen, neon, , fluorine
Name 2 elements that have properties
similar to those of the element sodium.
Any other Group 1 element:
Lithium, Potassium, Rubidium, Cesium, Francium
boron
nickel

10. Identify each property below as more
characteristic of a metal or a nonmetal
a)Brittle -
b)Malleable -
c)Poor conductor of electricity -
d)Shiny -
e)Tend to gain electrons -
In which pair of elements are the chemical
properties of the elements most similar?
a)sodium and chlorine
b)nitrogen and phosphorus
c)boron and oxygen
Nonmetal
Metal
Nonmetal
Metal
Nonmetal

11. Classifying the Elements
Alkali Metals–
Alkaline Earth Metals–
Halogens–
Noble Gases–
Representative Elements–
Transition Elements–
Group 1 (1A)
Group 2 (2A)
Group 17 (7a)
Group 18 (8A) Inert gases
Groups 1A –7A
All Group B

12. 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
He
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
*
W
Label your Reference PeriodicTable…
1
2 1314151617
18
3456789101112

13. Classifying Review
Which of the following are symbols for
representative elements
Na, Mg, , Cl?
Which of these metals is nota transition
metal?
a)Aluminum
b)Silver
c)Iron
d)Zirconium
Fe, Ni

14. Atomic Radius
Atoms are roughly spherical
Sphere size can be determined using the radius
Problem:
Solution:
Atomic Radii–half the
distance between the
nuclei of identical atoms
that are bonded together
Edges of orbitals are fuzzy and
difficult to measure…

15. Reference Table:
•Table S
Trends:
1. Across a period, the atomic radius →
Why?
Nuclei have larger positive charges
Electrons are pulled in closer
2. Down a group, the atomic radius →
Why?
Greater number of energy shells
Valence electrons are further away from the nucleus
decreases
increases

17. Atomic Radius Review
Which element in each pair has a larger
atomic radius?
a) & lithium
b) & bromine
c)carbon &
d) & neon
Arrange these elements in order of
decreasing atomic size: sulfur, chlorine,
aluminum, and sodium.
Sodium → Aluminum → Sulfur → Chlorine
sodium
calcium
germanium
fluorine

18. Ionization Energy
What is an ion?
An electrically charged atom
Atoms may either gainor loseelectrons
Loss of electrons = (+) charge →
Gain of electrons = (-) charge →
Ionization energy=
cation
anion
the amount of energy requiredto
remove the most loosely bound
electron
A + energyA
+
+ e
-

19. Reference Table
•Table S
Trends:
1. Across a period, the ionization energy →
Why?
Electrons are held closer to the nucleus
Electrons are more difficult to remove
2. Down a group, the ionization energy →
Why?
Electrons are further away from the nucleus
Electrons are easier to remove
Relate Back:
increases
decreases
What type of relationship exists between
ionization energy and atomic radii?Inverse

21. Ionization Review
Which element in each pair has a greater
ionization energy?
a)lithium,
b)magnesium,
c)cesium,
Arrange the following groups in order of
increasing ionization energy
a)Be, Mg, Sr
b)Bi, Cs, Ba
c)Na, Al, S
boron
strontium
aluminum
Be → Mg → Sr
Bi → Ba → Cs
Na → Al → S

22. Ionic Size
Cationsfrom when
atoms loosee
-
The cation is
smaller
Anionsfrom when
atoms gain e
-
The anion is larger

23. Reference Table
•No true table
Trends:
1. Across a period, ionic size →
Why?
When e
-
are lost, the attraction between the remaining
e
-
increases
e
-
are drawn closer to the nucleus
2. Down a group, ionic size →
Why?
Increased atomic radius
e
-
are further away from the nucleus
increases
decreases

25. Ion Size Review
Which particle has the larger radius in
each atom/ion pair?
a)Na,
b)S,
c)I,
d)Al,
The ions Na
+
and Mg
2+
each have 10e
-
.
Which ion would you expect to have a
smaller ionic radius?
Mg
2+
atomic radius is smaller & e
-
are
pulled in closer
Na
+
S
2-
I
-
Al
3+

26. Electronegativity
A measure of the ability of an atom to attract a
pair of electrons when bonded to another atom
Ability to ‘pull’ electrons from another atom
Electrons pulled closer: Electrons pulled away:

27. Reference Table
•Table S
Trends:
1. Across a period, the electronegativity →
Why?
Atoms are very close to a stable octet
‘Pull’ electrons from other atoms
2. Down a group, the electronegativity →
Why?
Top atoms have few electrons, and hold them tightly
Bottom atoms have numerous electrons and little desire
to acquire more
increases
decreases

29. Electronegativity Review
Which element in each pair has a higher
electronegativity value?
a)Cl,
b)C,
c)Mg,
d)As,
Which element in each pair has a greater
attraction for electrons?
a)Ca or
b)O or
c)S
F
N
Ne
Ca
O
F
or K

30. DecreasesIncreasesElectronegativity
IncreasesDecreasesIon Size
DecreasesIncreasesIonization
Energy
IncreasesDecreasesAtomic Radius
IncreasesDecreasesMetallic
Character
Variation down
a Group
Variation across
a Period
Periodic
Property
Summary