1. Periodic Table SWBAT: Identify properties of metals and nonmetals
SWBAT: Identify specific groups of elements and their properties from the periodic table

2. 1. Periodic Table Periods
a. Periods are the horizontal rows in the periodic table b. Used to help identify energy levels of atoms of different elements

3. 2. Periodic Table Groups
a. Groups or Families of elements are the vertical columns in the periodic table b. Elements in the same group have similar chemical properties

4. 3. Metals a. Located to the left of the stairs b. Properties
Solid at room temp
High melting points
High densities
Malleable (bend, shape, hit with hammer and not break)
Ductile (make wires)
Conduct electricity
Conduct heat

5. 4. Nonmetals a. Located to the right of the stairs b. Properties
Liquids and gases at room temp
Poor conductors of heat
Poor conductors of electricity
brittle

6. 5. Metalloids a. Found on and under the stairs b. Properties
Similar to both metals and nonmetals
Reactivity depends on the other elements
Often make good semiconductors

7. 6. Alkali Metals
a. Group 1A b. Have 1 valence electron c. Highly reactive d. React with water e. Francium is so reactive it will react with air

8. 7. Alkaline Earth Metals
a. Group 2A b. Have 2 valence electrons c. 2nd most reactive group d. Used to make base solutions e. Many elements are used in fireworks, batteries, flashbulbs f. Radioactive Radium was used in glow in the dark paint

9. 8. Transition Metals a. Transition metals – d block
b. Inner transition metals – f block
c. Lanthanide series – found naturally on earth
d. Actinide series – All radioactive, most man made

10. 9. Halogens
a. Group 7A b. Have 7 valence electrons c. Very reactive with alkali and alkaline earth metals d. Fluorine is most reactive

11. 10. Noble Gases
a. Group 8A b. Have 8 valence electrons c. Don’t bond with other elements (unless forced to) d. Neon – advertising signs e. Argon – light bulbs f. Helium – balloons g. Xenon - headlights

13. Periodic Table and electron configuration
The rows going across will represent energy levels
The blocks will represent the type of atomic orbital
Each element will represent an electron

14. Periodic Table
The periodic table holds the key….

15. Electron Configuration
Li – O – Al – Cl – F – Si – Br – Rb – Ag -

16. Electron Configuration
Li - 1s22s1 O - 1s22s22p4 Al - 1s22s22p63s23p1 Cl - 1s22s22p63s23p5 F - 1s22s22p5 Si - 1s22s22p63s23p2 Br - 1s22s22p63s23p64s23d104p5 Rb - 1s22s22p63s23p64s23d104p65s1 Ag - 1s22s22p63s23p64s23d104p65s24d9

17. Valence Electrons
1) The electrons in the outermost shell (energy level) of an atom are the valence electrons. 2) They are the electrons on an atom that can be gained or lost in a chemical reaction. 3) Since d and f subshells are formed under s and p, they are seldom used in bonding. Thus, valence electrons will be represented by the s and p orbitals.