2. History of the Periodic Table
Mrs. Hardeman

3. Russian chemist Dimitri Mendeleev proposed arranging elements by atomic weights and properties!!
A few elements seemed to be out of place!!!!

4. Soon after Rutherford’s discovery of the nucleus, I subjected the known elements to x-rays. I was able to derive the relationship between x-ray frequency and the # of protons(the Atomic Number).
Moseley arranged a new Periodic Table according to Atomic # and many of the “mistakes” with Mendeleev’s table were corrected!!!
Henry Moseley

6. Who developed the 1st Periodic Table?
Mendeleev
Moseley
Eidson
Hatfield

7. Whose Periodic Table was arranged in order of increasing Atomic #?
Mendeleev
Moseley
Eidson
Hatfield

8. Metals Most are solids. Metals are opaque, lustrous elements.
Are good conductors of heat and electricity.
Most metals are malleable and ductile.
Most are, in general, denser than the other elemental substances.

9. Nonmetals Great insulators
Poor conductors of heat and electricity when compared to metals.
Great insulators
Most are gases.
In solid form, they are dull and brittle.
Usually have lower densities than metals
They have significantly lower melting points and boiling points than metals
Nonmetals usually have little or no luster.

10. Metalloids Have properties of both metals and non-metals.
Ex.) Will conduct heat better than non-metals, but not as good as metals.
Some are considered semi-conductors of electricity which makes them useful for computers.

11. Which of the following elements is a metal?
Carbon
Silicon
Sodium
Chlorine

12. Which of the following elements is a nonmetal?
Carbon
Silicon
Sodium
Lithium

13. Which of the following elements is a metalloid?
Carbon
Silicon
Sodium
Chlorine

14. Periods—horizontal rows on the table(7)
Family(groups)—vertical columns on the table(18)

15. Valence Electrons
The valence electrons are the electrons in the last shell or energy level of an atom. They do show a repeating or periodic pattern. The valence electrons increase in number as you go across a period. Then when you start the new period, the number drops back down to one and starts increasing again.
“We can check this with a few drawings! ”

16. Draw Hydrogen
How many valence electrons? 1

17. Draw Lithium
How many valence electrons? 1

18. Draw Sodium
How many valence electrons? 1

19. Draw Berylium
How many valence electrons? 2

20. Draw Magnesium
How many valence electrons? 2

21. Do you notice the Trend?

22. Valence Electrons(cont)
We could actually draw any of the families and we would see that the # of valence electrons is the same throughout any of the families!!

23. Valence Electrons

24. How many valance electrons does Oxygen have?3 4 6 8

25. How many valance electrons does Krypton have?3 4 6 8

26. How many valance electrons does Magnesium have?1 2 3 4

27. Chemical Families

28. Alkali Metals Group 1 Except Hydrogen.
Composed of highly reactive(active) metals.
1 valence electron
Tend to lose 1 electron to form compounds(+1)
React vigorously with water.
In nature, they are never found in their pure state.
React with halogens to form salts.

29. Alkaline Earth Metals Composed of reactive metals. 2 valence electrons
Tend to lose 2 electrons to form compounds(+2).
Compounds of alkaline earth metals comprise many common minerals.
Many are used in fireworks.

30. Transition Metals They are usually have high melting points.
They have several oxidation states.
Typically, +2 or +3

31. Boron Family 3 valence electrons
Tend to lose three electrons and form positive ions(+3).

32. Carbon Family
The elements of the Carbon Family show great versatility.
Carbon is the basis for organic chemistry and forms more compounds than any other element except hydrogen.
4 valence electrons
Gain, lose, share(+/- 4)

33. Nitrogen Family 5 valence electrons. Typically gains 3 electrons(-3)
Nitrogen is the principal constituent of the air.
Many are used in fertilizers.

34. Oxygen Family 6 valence electrons Typically gains 2 electrons(-2)
Oxygen makes up nearly half of the Earth's crust by mass.
Oxygen produced by plants sustains life.

35. Halogens 7 valence electrons Typically gain 1 electron(-1)
Most active non-metals.
Halogen means "salt formers".
They lack only one electron to form a complete shell.
Tend to gain an electron to form compounds.

36. Nobel Gases 8 valence electrons(except He has 2)
Will not gain or lose electrons(0)
Gases which have closed shells
Are unreactive chemically.
“Neon” lights.

37. A NG AE
Family Names H TM

38. Sodium(Na) belongs to which chemical family?
Alkali Metals
Alkaline Earth Metals
Halogens
Nobel Gases

39. Chlorine(Cl) belongs to which chemical family?
Alkali
Alkaline Earth
Halogens
Nobel Gases

40. Calcium(Ca) belongs to which chemical family?
Alkali
Alkaline Earth
Halogens
Nobel Gases

41. Xenon(Xe) belongs to which chemical family?
Alkali
Alkaline Earth
Halogens
Nobel Gases

43. Attention: New Additions to Periodic Table
WOMANIUM (Wo) Physical properties: Generally soft and round in form. Boils at nothing and may freeze any time. Very bitter if not used well. Chemical properties: Very active and highly unstable. Possesses strong affinity with gold, silver, platinum, and precious stones. Violent when left alone. Turns slightly green when placed next to a better specimen. Usage: An extremely good catalyst for dispersion of wealth. Caution: Highly explosive in inexperienced hands!
MANIUM (Xy) Physical properties: Solid at room temperature but gets bent out of shape easily. Difficult to find a pure sample. Due to rust, aging samples are unable to conduct electricity as easily as young samples. Chemical properties: Attempts to bond with WO any chance it can get. Also tends to form strong bonds with itself. Becomes explosive when mixed with Childrium for prolonged period of time. Usage: Possibly good methane source. Caution: In the absence of Wo, this element rapidly decomposes and begins to smell.

44. Color your Periodic Table:
Label # of valence electrons with a color.
Label Family Names and color each with a different color.
Draw a “box” around Hydrogen and Label “NM”.
Place a big “M” over the metals, a “NM” over the nonmetals and circle the metalloids.