1. PERIODIC TABLE
Where it all is

2. What do you know?
What stuff do you already know about the periodic table?

3. Mendelev’s Table
Mendeleev’s table as published in 1869, with many gaps and uncertainties mg

4. How is it Arranged
Based on increasing atomic number and on electron configurations
Repeating chemical and physical properties.
Groups or Families
Columns that go up and down.
Periods
Rows that go across

5. Classification of Elements
Metals
On the left side
Make up ¾ of all elements
Malleable, Ductile, Conduct electricity, form positive ions.
NonMetals
On the Right side
Dull, Brittle, Insulators, form negative ions
Metalloids (Semimetals)
Found along the staircase between metals and nonmetals, have properties of both.

7. Group 1 – Alkali Metals Highly reactive All have 1 valence electron
Forms +1 ions

8. Group 2 – Alkaline Metals
Very reactive
Have 2 Valence electrons
All are s2 – forms +2 ions

9. Transitional Metals Groups 3 to 12
These are the common metals.
D orbital metals.
Forms various positive ions. You will be told their oxidation state.

10. Boron Family – Group 13 Have 3 Valence electrons
Boron which forms a –3 ion
One is a metalloid (Boron)
The post transition metals form various cations

11. Carbon Family – Group 14 Carbon family has 4 valence electrons
Carbon and silicon form a -4 charge
Composed of:
one non-metal (Carbon)
Two metaloids (Silicon and Germanium

12. Group 15 – Nitrogen Family
All have 5 valence electrons
Nitrogen, phosphorus and arsenic form a -3 charge.
Composed of:
two nonmetals - Nitrogen and Phosphorous
Two metalloids – Arsenic and Antimony

13. Group 16 – Oxygen Family All have 6 valence electrons Composed of:
Oxygen, sulfur, selenium, and tellurium form -2 charges
Composed of:
3 nonmetals – Oxygen, Sulfur, Selenium
1 metalloid – Tellurium

14. Group 17 - Halogens
All have 7 valence electrons (all form a -1 charge)
All are nonmetals
Highly reactive
Never found in nature as single atoms
When pure will form F2, Cl2, Br2, I2

15. Group 18 – Noble Gases All have 8 valence electrons Rarely form bonds
Never form ions
Helium, Neon, Argon have never been found in a natural compound

16. Actiticides and Lanthicides
Called Rare Earths
They are rare on earth - Most are manmade
All are radioactive
All elements greater then Uranium (92) are manmade
Some are used in medical research

18. TRENDS Atomic Radius – The size of the atom.
Smaller Up and Right
Negative Ions Larger
Positive Ions Smaller
Ionization Energy – The energy required to remove electrons
Greater Up and Right
Fluorine the highest
Francium the lowest

19. More on Trends
Electronegativity – The ability of atoms to attract electrons during bonding
Greater Up and Right
Fluorine the Greatest Electronegivity
Francium the Lowest
Octet Rule – Atoms Tend to gain, lose or share electrons to have a full (s2, p6) valence shell.

20. Summarize what you learned
What are the major trends of the periodic table?
What are groups? What are periods?
Summarize in your own words.