1. Understanding the Periodic Table: GROUPS

2. Look at your periodic table
Write 10 observations on your paper.
What are the 3 main groups we’ve learned about so far?

3. Metals 1. Ductile: conduct electricity very well.
2. Malleable: hammered, bent without breaking.
3. Shiny
Examples:
Silver (Ag)
Gold (Au)
Copper (Cu)
Aluminum (Al)

4. Nonmetals 1. Dull: not shiny 2. Brittle: breaks easily
3. Poor conductors of electricity and heat.
Examples:
Hydrogen (H)
Sulfur (S)
Chlorine (Cl)
Helium (He)

5. Semimetals or Metalloids
Have properties of both metals and nonmetals.
Only conduct electricity under certain conditions.
Examples:
Silicon (Si)
Boron (B)

6. Metals, Nonmetals, and Semi-metals on the Periodic Table
Color the metals, non-metals and semi-metals VERY LIGHTLY. There’s more……….

7. B A
Also called Families
18 Columns 8 Columns labeled A (colors)
10 Columns labeled B (gray)
Each group has unique properties
Elements in the same group have similar properties.

8. Group 1A – Alkali Metals
silvery white metal (except cesium, which is liquid golden)
Highly reactive.
Examples:
Sodium (Na)
Potassium (K)
Cesium (Cs)

9. Group 1A – Alkali Metals H  Li  Na  K 
Bohr Diagram
Lewis Dot Diagram
H 
Li 
Na 
K 
1 electron in each outer shell.
Energy levels increase by the period

10. Group 2A – Alkaline Earth Metals
Malleable and ductile metals.
Very reactive.
Examples:
Magnesium
Calcium (Ca)
Radium (Ra)

11. Group 2A – Alkaline Earth Metals
Be:
Mg:
Ca: 3 4
2 electrons in outer shell
Energy levels increase by the period

12. Groups 1B-8B: Transition Metals
Brightly colored, ductile metals.
Less reactive.
Different columns –different numbers of electrons in outer shell.
Examples:
Chromium (Cr)
Nickel (Ni)
Gold (Au)
Copper

13. Semimetals: Groups 3A-6A (along the zig zag line)
Properties of both metals and non-metals
Some are semi-conductors
Group number indicates how many electrons in the outer shell.
Examples:
Boron (B)
Silicon (Si)
Germanium (Ge)
Antimony (Sb)

14. Semimetals: Groups 3A-6A (along the zig zag line)
Boron (B)
Silicon (Si)
Germanium (Ge)
Astatine (As)
Antimony (Sb)…
Group number indicates the number of electrons in the outer shell. B Si Ge As Sb
Group 3
Group 4
Group 4
Group 5
Group 5

15. Group 7A: Halogens 7 electrons in the outer shell. Examples:
Nonmetals
Brittle, dull, poor conductors of electricity.
Very reactive ions Form salts with Group 1 elements
7 electrons in the outer shell.
Examples:
Chlorine (Cl)
Fluorine (F)
Bromine (Br)
Iodine (I)

16. Group 7A: Halogens F 7 electrons in the outer shell. Cl Br
As you look down the group the number of energy levels increases.

17. Group 8A: Inert Gases Also called Noble gases Inert means inactive
8 electrons in the outer shell, which makes them non-reactive
Examples:

18. Group 8A: Inert Gases He Ne
Bohr
Lewis He Ne
full outer shell, which makes them non-reactive
He only has the possibility of 2 electrons in outer energy level. All the others have 8. Ar Kr
Each next period brings another energy level.

19. Lanthanide, Actinide, TransUranium
Lanthanide also called Rare Earth Metals
Actinide and Transuranium are radioactive
All part of IIIB group
Examples:
Cesium
Uranium
Plutonium