1. Periodic Trends

2. Arrangement Elements are arranged according to atomic number
Number of protons
Not atomic mass

3. Group/Family Vertical column in the periodic table 18 groups
Elements in same group
Same physical and chemical properties
Same number of electrons in last energy level
Example:
Group 18
All gases
All unreactive

4. Valence electrons Electrons in the last energy level of an atom
Involved in chemical reactions and bonding
Coincides with the unit’s place on the group number except for Groups
Group 1: 1 valence electron
Group 2: 2 v.e.
Group 18: 8 v.e. except for He

5. Lewis Dot Diagram
Shows the number of valence electrons in a neutral atom
Each dot represents 1 valence electron

6. Lewis Structure Practice
Carbon Hydrogen Calcium Oxygen

8. Metals Left and middle of periodic table except H Properties:
Ductile: drawn into a wire
Malleable: hammered into thin sheets
Good conductors of heat/electricity
Luster: shine
Solid at room temperature (except for Hg)

9. Nonmetals Far right side of periodic table Properties
Brittle: break when hammered
Lack luster
Poor conductors
Solid or gas at room temperature (except Br)

10. Metalloids (Semi-metals)
Along the black line that divides metals and nonmetals
Have properties of both metals and nonmetals

11. 3 states of matter Liquid: Gas: Solid: Hg and Br
all the noble gases (group 18)
and O, F, N, H, Cl
Solid:
rest of the elements in the periodic table

13. Ions Charged elements Metals Nonmetals
Positive ions (lose electrons) to have a complete valence shell
Magnesium  Mg2+
Nonmetals
Negative ions (gain electrons) to fill valence shell
Nitrogen  N3-

14. Relationship between charge and group

15. State the charge of the following elements as ions
Fluorine Phosphorus Beryllium Aluminum