1. (2.2) The Periodic Table (p118-121)

2. Periodic Table of the Elements (p450)

3. Table Characteristics
Metals (LEFT), non-metals (RIGHT) and metalloids (STAIRCASE LINE)
Periods (or rows)
Groups / Families (or columns)

4. Common Chemical Groups
There are 18 chemical groups on the periodic table, however four of these groups are of particular interest
Alkali metals (group 1)
Alkaline earth metals (group 2)
Halogens (group 17)
Noble gases (group 18)

5. Alkali Metals
Group 1
Soft, silver-grey metals that react easily with water and with oxygen
NOTE: H is not an alkali metal.
alkali metals in water

6. Alkaline Earth Metals Group 2
Silver-grey metals that are harder than group 1 metals.
Reactive atoms (less reactive than group 1 metals) that combine easily with other atoms.

7. Halogens Group 17 Coloured non-metals that are VERY reactive
Can be a solid, a liquid or a gas

8. Noble Gases Group 18 Non-metals that are colourless, odourless gases.
Unreactive (inert) atoms that do not combine easily with other atoms.

9. Ion Charge
Reactive elements can become stable (full valence shell) by gaining or losing electrons.
An atom that gains electrons becomes a negatively charged ion called an anion.
Non-metals gain electrons.
An atom that loses electrons becomes a positively charged ion called a cation.
Metals lose electrons.

10. Magnesium Ion Mg Mg2+ Magnesium atom loses 2 valence electrons
Mg2+ has a full valence shell and is stable

11. Nitride Ion N N3- Nitrogen atom gains 3 valence electrons
The nitride ion has a full valence shell, so it is stable

12. What will the charge be?

13. CLASS WORK
“Periodic Table Assignment”