Transcript The Periodic Table and Periodicity

The Periodic Table
and Periodicity
Arrangement

In order of increasing atomic number in
specific columns and rows.
Groups- vertical columns of the PT
The Periodic Table
1
1
2
3
4
5
6
7
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
Periods- horizontal row on the PT
The Periodic Table
1
1
2
3
4
5
6
7
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
Groups are important on the PT

Why?
 The
elements in a group have similar
chemical and physical properties!
Alkali Metals – Group 1
1
1
H
2
Li
3
Na
4
K
5
Rb
6
Cs
7
Fr
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
Alkaline Earth Metals – Group 2
1
2
1
2
Be
3
Mg
4
Ca
5
Sr
6
Ba
7
Ra
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
Halogens – Group 17
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
1
2
F
3
Cl
4
Br
5
I
6
At
7
18
Noble Gases – Group 18
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
1
He
2
Ne
3
Ar
4
Kr
5
Xe
6
Rn
7
Uuo
Transition Metals – Groups 3 - 12
1
1
2
3
4
5
6
7
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
Inner Transition Metals
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
1
2
3
4
5
6
7
La
Yb
Ac
No
17
18
Metals Lustrous
 Good conductors of heat & electricity
 Malleable – can be pounded into thin
sheets
 Ductile – can be drawn into thin wire

Metals on the PT
1
1
2
3
4
5
6
7
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
Nonmetals - Lack properties of
metals
1
1
2
3
4
5
6
7
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
Metalloids (semi-metals)- have a
mixture of metallic and nonmetallic
properties
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
1
2
3
Si
4
Ge
5
6
7
As
Sb
Te
Po
At
18
Diatomic Elements


Most elements can be
isolated to atomic
elements – individual
atoms
7 elements are too
reactive to exist as
individual atoms, instead,
they are found as
molecular elements – 2
atoms bonded together







Hydrogen, H2
Oxygen, O2
Nitrogen, N2
Chlorine, Cl2
Bromine, Br2
Iodine, I2
Fluorine, F2
Periodicity

Atomic radius – defined as ½ the distance
between the nuclei of two adjacent atoms
of an element.
Periodicity

First Ionization Energy – energy needed to
remove an electron from an atom.

Electronegativity – ability of an atom to
attract electrons to itself