The Periodic Table
Chap. 6
I. Early Attempts at
Organizing the Elements
I. Early Attempts at
Organizing the Elements
A. Lavoisier’s list: 23 elements
I. Early Attempts at
Organizing the Elements
A. Lavoisier’s list: 23 elements
B. 1870’s : 70 known elements
I. Early Attempts at
Organizing the Elements
A. Lavoisier’s list: 23 elements
B. 1870’s : 70 known elements
C. Dobereiner’s triads
Halogen Triad
Cl
Br
mass
35.5 u
density .00321
M.P.
B.P.
I
79.9 u
3.12
127 u
4.93
-101oC
-7oC
114oC
oC
o
59 C
o
185 C
-34
Self Check – Ex. 1
Ca
mass
40 u
1.55
Sr
Ba
88 u
137 u
3.62
M.P.
842oC
?
?
B.P.
o
1500 C
o
1412 C
density
727oC
1845
oC
Self Check – Ex. 1
Ca
Sr
Ba
40 u
1.55
88 u
2.6
137 u
3.62
M.P.
842oC
7770C
727oC
B.P.
o
1500 C
o
1412 C
mass
density
1845
oC
I. Early Attempts at
Organizing the Elements
A.
B.
C.
D.
Lavoisier’s list: 23 elements
1870’s : 70 known elements
Dobereiner’s triads
Newlands: Law of Octaves
I. Early Attempts at
Organizing the Elements
E. Mendeleev’s Table
I. Early Attempts at
Organizing the Elements
E. Mendeleev’s Table
1. produced simultaneously
with Meyer
I. Early Attempts at
Organizing the Elements
E. Mendeleev’s Table
1. produced simultaneously
with Meyer
2. organized elements by
increasing mass
I. Early Attempts at
Organizing the Elements
E. Mendeleev’s Table
3. rearranged a few elements
to match properties
I. Early Attempts at
Organizing the Elements
E. Mendeleev’s Table
3. rearranged a few elements
to match properties
4. left gaps for undiscovered
elements
I. Early Attempts at
Organizing the Elements
E. Mendeleev’s Table
3. rearranged a few elements
to match properties
4. left gaps for undiscovered
elements
5. described periodic law
Periodic Law
When arranged according to
increasing atomic number,
there is a repeating pattern of
an element’s properties
II.The Modern Periodic Table
II.The Modern Periodic Table
A. Periods
II.The Modern Periodic Table
A. Periods
B. Groups/Families
II.The Modern Periodic Table
A. Periods
B. Groups/Families
C. Metals/Non-Metals/Semimetals
II.The Modern Periodic Table
A.
B.
C.
D.
Periods
Groups/Families
Metals/Non-Metals/Semimetals
Transition Metals/Inner
Transition Metals/
Representative Elements
II.The Modern Periodic Table
A.
B.
C.
D.
Periods
Groups/Families
Metals/Non-Metals/Semimetals
Transition Metals/Inner
Transition Metals/
Representative Elements
E. Physical States
II.The Modern Periodic Table
A.
B.
C.
D.
Periods
Groups/Families
Metals/Non-Metals/Semimetals
Transition Metals/Inner
Transition Metals/
Representative Elements
E. Physical States
F. Naturally occurring elements
III. Periodic Trends
III. Periodic Trends
A. Valence Electrons
III. Periodic Trends
A. Valence Electrons
1. as you go down a group, the
number of valence electrons
__________
III. Periodic Trends
A. Valence Electrons
1. as you go down a group, the
number of valence electrons
__________
2. as you go across a period, the
number of valence electrons
__________
III. Periodic Trends
B. Atomic Radius
Atomic radius
Distance between the nucleus
and the outermost electron.
III. Periodic Trends
B. Atomic Radius
1. as you go down a group, the
atomic radius __________
III. Periodic Trends
B. Atomic Radius
1. as you go down a group, the
atomic radius __________
2. as you go across a period, the
atomic radius __________
Atomic Radius
250
Atomic Radius (pm)
19
20
200
11
12
3
150
13
14
4
100
5
50
1
6
7
8
9
15
16
17
18
10
2
0
0
2
4
6
8
10
12
Atomic Number
14
16
18
20
Self Check – Ex. 2
Put the following atoms in
order from smallest to
largest radius
P Mg O Ca
III. Periodic Trends
C. Ionic Radius
Ion
An atom that has gained or
lost an electron
III. Periodic Trends
C. Ionic Radius
1. as you remove an electron,
the radius __________
III. Periodic Trends
C. Ionic Radius
1. as you remove an electron,
the radius __________
2. as you add an electron, the
radius __________
III. Periodic Trends
C. Ionic Radius
1. as you remove an electron,
the radius __________
2. as you add an electron, the
radius __________
3. the isoelectronic atoms that
are the smallest have the most
_______
Isoelectronic atoms
Atoms that have the same
number of electrons.
Self Check – Ex. 3
Put the following in order
of increasing radius
Cl
2+
Ca
Ar
+
K
III. Periodic Trends
D. 1st Ionization Energy
Ionization Energy
The energy required to
remove an electron.
III. Periodic Trends
D. 1st Ionization Energy
1. as you go down a group the
ionization energy ________
III. Periodic Trends
D. 1st Ionization Energy
1. as you go down a group the
ionization energy ________
2. as you go across a period the
ionization energy ________
First Ionization Energy of Elements
Ionization Energy (kJ/mol)
2500
2
10
2000
9
18
1500
7
1
8
17
6
1000
4
15
5
14
12
3
500
16
20
13
11
19
0
0
2
4
6
8
10
12
Atomic Number
14
16
18
20
III. Periodic Trends
D. 1st Ionization Energy
1. as you go down a group the
ionization energy ________
2. as you go across a period the
ionization energy ________
3. as you remove each
additional electron the
ionization energy ________
Successive Ionization Energy
Name
1st IE
(kJ/mol)
2nd IE
(kJ/mol)
3rd IE
(kJ/mol)
4th IE
(kJ/mol)
Boron
800
2430
3660 25020
Self Check – Ex. 4
For what ionization will a
large jump in ionization
energy be observed with
aluminum?
III. Periodic Trends
E. Electronegativity
Electronegativity
The ability of an atom to
attract electrons in a
chemical bond.
III. Periodic Trends
E. Electronegativity
1. electronegativity values are
only reported for elements
that bond.
III. Periodic Trends
E. Electronegativity
1. electronegativity values are
only reported for elements
that bond.
2. as you go down a group the
electronegativity ________.
III. Periodic Trends
E. Electronegativity
1. electronegativity values are
only reported for elements
that bond.
2. as you go down a group the
electronegativity ________.
3. as you go across a period the
electronegativity ________.
Self Check – Ex. 5
Put these in order of
decreasing electronegativity.
Sr O B Mg F
The End