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The Periodic Table and Periodicity. Arrangement. In order of increasing atomic number in specific columns and rows. Groups- vertical columns of the PT. Periods- horizontal row on the PT. Groups are important on the PT. Why? - PowerPoint PPT Presentation
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The Periodic Table and Periodicity
Arrangement
In order of increasing atomic number in specific columns and rows.
Groups- vertical columns of the PTThe Periodic Table
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1
2
3
4
5
6
7
Periods- horizontal row on the PTThe Periodic Table
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1
2
3
4
5
6
7
Groups are important on the PT
Why? The elements in a group have similar
chemical and physical properties!
Alkali Metals – Group 1
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1 H
2 Li
3 Na
4 K
5 Rb
6 Cs
7 Fr
Alkaline Earth Metals – Group 2
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1
2 Be
3 Mg
4 Ca
5 Sr
6 Ba
7 Ra
Halogens – Group 17
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1
2 F
3 Cl
4 Br
5 I
6 At
7
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 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1
2
3
4
5
6
7
Inner Transition Metals
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1
2
3
4
5
6
7
La Yb
Ac No
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 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1
2
3
4
5
6
7
Nonmetals - Lack properties of metals
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1
2
3
4
5
6
7
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 18
1
2
3 Si
4 Ge As
5 Sb Te
6 Po At
7
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