1. One way of organizing the periodic table

2. Another way of organizing the periodic table….
Metals vs Nonmetals

4. Characteristics of Metals?
Good conductors of heat and electricity
Shiny (have luster)
Malleable (bendable)
Ductile (can be pulled into a wire)

5. Characteristic of Nonmetals
Poor (bad) conductors of heat and electricity
Solids are brittle (break instead of bend)
Generally the opposite of metals

7. The metalloid elements are…Po

8. What are metalloids? Sometimes they have characteristics of metals
Sometimes they have characteristics of nonmetals

9. Another way of organization…

10. Groups or Families: up and down columns on the periodic table
Periods: side to side rows on the periodic table

11. Groups have special names…
1A – Alkali Metals
2A – Alkaline Earth Metals
7A – Halogens
8A – Noble Gases

13. Two rows on the bottom are…
Inner Transition Metals

15. PNICOGENS
CHALCOGENS

16. What are the representative elements?
Representative elements: elements in groups 1A – 7A
* Wide range of physical and chemical properties

17. Electrons are the Key!
The reason elements in the same family have the same chemical and physical properties is because they have the same number of electrons in their outer shell

18. The group number equals the number of electrons in its outermost energy level
(this will be more important later on…)
So all Group 1A elements have 1 electron in the outer shell

19. Atoms can gain or lose electrons

20. Cations Positive ions = cations
Formed when a metallic atom LOSES electrons.
Examples: Sodium  Na+1 Magnesium  Mg+2
You can determine how many electrons are lost based on location on the periodic table.
These must be memorized.

21. Anions Negative ions = anions Non-metals gain electrons become anions.
Examples: Bromine  Br -1 Oxygen  O-2
You need to MEMORIZE the common charges of the anions to be successful for the rest of the school year…

22. Group 1A = +1
Group 2A = +2
Group 3A = +3
Group 4A = + or – 4
Group 5 A = -3
Group 6A = -2
Group 7A = -1
Group 8A = 0
Aluminum, Zinc, and Silver (Special Charges)
Now onto PERIODIC TRENDS…..

23. Atomic Radii and Size
Periodic: Atomic Radii and size decrease as you go L to R across the table.
Same principle energy level
Add p+ and e-, increase nuclear charge, pulls in orbitals closer to the nucleus
Group: Atomic Radii and size increase as you go down a group
Electrons being added to outer orbital (increasing principle energy level)

25. Ion Size Cations are smaller in size than the neutral element.
Anions are larger in size than the neutral element.

26. Ionization Energy
Ionization Energy (IE): The energy required to remove and electron from a gaseous atom.
Remove 1st electron = 1st IE
Remove 2nd electron = 2nd IE

27. Trends in Ionization Energy
Periodic: IE generally increases as you move L to R across the period.
Harder to remove an electron as you go L to R because of greater attraction to nucleus
Shielding effect -
Group: 1st IE generally decreases as you go down a group.
Atom gets bigger, outermost e- farthest from nucleus, easy to be removed.

29. Electronegativity
Electronegativity: The tendency for atoms to attract electrons when they are chemically combined.
Do they share electrons equally?

30. Electronegativity Trends
Periodic: Electronegativity increases as you go L to R across the period
Elements want to be like noble gases!
Group: Electronegativity decreases as you go down a group.
The most electronegative element is Fluorine.

32. Summary of Trends Decreasing Atomic Radius
Increasing Ionization Energy
Increasing Electronegativty
Decreasing Ionization Energy
Decreasing Electronegativity
Increasing Atomic Radius