1. Unlocking the Periodic Table of Elements

2. Regular, repeating pattern

3. Unlocking the Periodic Table of Elements
Dmitri Mendeleev (Russian Chemist)
Credited with 1st Periodic Table
Classified elements by:
Name
Atomic Mass
Properties

4. Henry Moseley (British Physicist)
Credited with Modern Periodic Table
Used  atomic # instead of mass
Classified and arranged by :
Atomic #
Arrangement of electrons in valence shell

5. Parts of the Periodic Table:
Periods 
7 Horizontal rows
Elements 57 – 71 fit into period 6
Elements 89 – 103 fit into period 7
No similarities among the elements in a period
Moves from Metals (left) to Nonmetals (right)
Valence shells fill up as elements move from left to right

6. 2 8 8

7. Groups  Vertical columns Elements have similar properties
Due to same valence shell electron configuration
Also known as “Families”
Numbered 1 – 18 from left to right

8. Metalloids touch the zig-zag line on the right
Nonmetal
right of zig-zag line
Metalloid
Poor Metals
Metals Large area left of the zig-zag line
Metal

9. So … what exactly is a metal?????
What makes something a metal????
What do you think of when you hear the word “metal”

10. Properties of metals Most are silver or grey
Luster – reflects light when polished
Conducts heat & electricity
Usually high () melting point (MP)
Malleable – can be flattened, bent & shaped without breaking e.g. aluminum foil
Ductile – can be pulled into thin wire e.g. copper
Exceptions: Pure gold and silver (soft metals)
Gallium- MP just above room temp
Mercury – liquid at room temp

11. They can give up or lose these electrons easily
***Remember, properties come from the electrons in the valence shell of the atoms***
Most metals have 1 to 3 electrons in their valence shell
They can give up or lose these electrons easily
They also hold their electrons loosely and can share them with other metal atoms (metallic bonds we will talk about later)
Loose sharing of electrons gives rise to the properties of metals such as being malleable, conductive & ductile

12. Most gold or silver coins and jewelry are alloys.= +
Brass (alloy)
Zinc (metal)
Copper (metal)
Carbon (nonmetal) = +
Steel (alloy)
Iron (metal)

13. (Lithium, Sodium, Potassium, Ribidium, Cesium, Francium)
Group 1 Alkali Metals
6 elements (Li, Na, K, Rb, Cs, Fr)
(Lithium, Sodium, Potassium, Ribidium, Cesium, Francium)
1 valence electron (easily lost)
Very reactive, combine easily
 Exist in nature only as positive ions that will form ionic bonds with negative ions e.g. NaCl

14. (Beryllium, Magnesium, Calcium, Strontium, Barium, Radium)
Group Alkaline Earth Metals
6 elements (Be, Mg, Ca, Sr, Ba, Ra)
(Beryllium, Magnesium, Calcium, Strontium, Barium, Radium)
Reactive, but not as reactive as alkali metals
2 valence electrons
Occur as ions, or combined with other elements
e.g. Ca2+ or CaCl2

15. Transition Metals Shiny MP Good conductors
Less reactive, but will combine with other elements
Some magnetic (Iron, Cobalt, Nickel)
Found in ores (minerals containing large amounts of metal compounds) (remember the alloys)

16. Rare Earth Metals 2 separate rows at the bottom of the periodic table
Lanthanide Series (follows Lanthanum in period 6)
*Except for # 61, all occur in nature in small amounts in the earth’s crust
Actinide Series (follows Actinium in period 7)
*Most synthetic
Transuranium Elements – Atomic # > 92, synthetic, radioactive

17. Properties of Nonmetals
Do not have luster
Poor conductors of heat and electricity
Usually dull and brittle
Not malleable and not ductile
Many are gases at room temperature
The CHONSP elements are very important to life. Carbon is the backbone of macromolecules containing the other nonmetal elements that life depends on.

18. Group 13 the Boron Group Aluminum = poor metal 3 valence electrons
Boron = metalloid
Most abundant metal in Earth’s crust

19. Group 14 the Carbon Group Carbon= nonmetal Silicon = metalloid
Germanium = poor metal
4 valence electrons

20. Group 15 the Nitrogen Group
5 valence electrons
Nitrogen = 79% of air we breathe
Phosphorus found in DNA, teeth, and bones

21. Group 16 the Oxygen Group 6 valence electrons
Oxygen = Most abundant element in Earth’s crust
Sulfur = Proteins, vulcanizing rubber
Selenium = light meters, solar cells, photocopiers

22. Group 17 the Halogen Group
Halogen = “salt former”
Fluorine = most reactive
7 valence electrons, negative -1 anion
Combine with alkali metals to form salt e.g. NaCl

23. Group 18 the Noble Gases Colorless gases Inert
All found in Earth’s atmosphere
Glow with color when electrical current passed through gas
Neon lights

24. Hydrogen 1 valence electron Gas
Properties of both metals and nonmetals

25. Sci Kap
You CAN Science!

26. References
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[Transition metals]. (n.d.). Retrieved November 16, 2016, from
[Zinc]. (n.d.). Retrieved November 16, 2016, from