1. Mendeleev’s Periodic Table
Dmitri Mendeleev

2. Modern Russian Table

3. Stowe Periodic Table

4. A Spiral Periodic Table

5. “Mayan” Periodic Table

6. Period
The Periodic Table
Group or Family
Group or family
Period

7. Properties of Metals
Metals are good conductors of heat and electricity
Metals are malleable
Metals are ductile
Metals have high tensile strength
Metals have luster

8. Examples of Metals
Potassium, K reacts with water and must be stored in kerosene
Copper, Cu, is a relatively soft metal, and a very good electrical conductor.
Zinc, Zn, is more stable than potassium
Mercury, Hg, is the only metal that exists as a liquid at room temperature

9. Properties of Nonmetals
Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element.
Nonmetals are poor conductors of heat and
electricity
Nonmetals tend to be brittle
Many nonmetals are gases at room temperature

10. Examples of Nonmetals
Microspheres of phosphorus, P, a reactive nonmetal
Sulfur, S, was once known as “brimstone”
Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure

11. Properties of Metalloids
Metalloids straddle the border between metals and nonmetals on the periodic table.
They have properties of both metals and nonmetals.
Metalloids are more brittle than metals, less brittle than most nonmetallic solids
Metalloids are semiconductors of electricity
Some metalloids possess metallic luster

12. Silicon, Si – A Metalloid
Silicon has metallic luster
Silicon is brittle like a nonmetal
Silicon is a semiconductor of electricity
Other metalloids include:
Boron, B
Germanium, Ge
Arsenic, As
Antimony, Sb
Tellurium, Te

13. The Properties of a Group: the Alkali Metals
  Easily lose valence electron (Reducing agents) +1
 Soft enough to cut with a knife
React violently with water
 Stored in Oil
React with halogens to form salts

14. The Properties of a Group IIA: Alkaline Earth Metals
2 e- in outer shell
Will lose 2 e- : +2
Alkaline Earth Metals – Group IIA

15. Group IIIA: The Boron Family
3 e- in the outer shell
B- metalloid, All other elements are metals, will form then 3+ ions
Al- 3rd most abundant element in earth’s crust, very strong in alloys, doesn’t corrode easily

16. Group IVA: Carbon Family
4 e- in outer shell
Si: 2nd most abundant in Earth’s crust
SiO2 is in sand, semi conductor, silica=glass
Ge: electronic devices
Sn: coats steel for “tin cans”
Pb: In batteries and computer, used to be in paint and gas

17. Group VA: Nitrogen Family
5 e- in outer shell
N & P: Nonmetals
As & Sb are metalloids
Bi: Metal
N: 79% of earth’s atmosphere, colorless, odorless and diatomic (N2 )
P: in your bones; in fertilizers, detergents, soft drinks

18. Group VIA: Oxygen Family
6 e- in outer (normally will gain 2e-; 2- charge then)
O, S, Se: Nonmetals
Te: metalloid
Po: metal (metalloid)
O: most abundant element on earth, colorless, odorless, diatomic (O2); extremely reactive, O3
S: unpleasant odor; added to natural gas to detect leaks; skunks, rotten eggs

19. The Properties of Group VIIA: The Halogens
Contain 7 e- in outer shell
Easily gain valence electron
(Oxidizing agents) -1
Can be prepared from their “salt”
NaCl  Cl2
NaF  F2
 KBr  Br2

20. Group VIIIA: Noble Gases Inert Elements
Filled Outer Energy (filled s and p’s)
8e- in outer shell; chemically inactive

22. Half of the distance between nucli in
Determination of Atomic Radius:
Half of the distance between nucli in
covalently bonded diatomic molecule
"covalent atomic radii"
Periodic Trends in Atomic Radius
  Radius decreases across a period
Increased effective nuclear charge due
to decreased shielding
  Radius increases down a group
Addition of principal quantum levels

23. Table of Atomic Radii

24. Increases for successive electrons taken from the same atom
Ionization Energy - the energy required to remove an electron from an atom
  Increases for successive electrons taken from
the same atom
  Tends to increase across a period
Electrons in the same quantum level do
not shield as effectively as electrons in
inner levels
    Irregularities at half filled and filled
sublevels due to extra repulsion of
electrons paired in orbitals, making them
easier to remove
  Tends to decrease down a group
Outer electrons are farther from the
nucleus

25. Table of 1st Ionization Energies

26. Ionization of Magnesium
Mg kJ  Mg+ + e-
Mg kJ  Mg e-
Mg kJ  Mg e-

27. Another Way to Look at Ionization Energy

28. Electronegativity
The ability of an atom in a molecule to attract shared electrons to itself.
Linus Pauling

29. Table of Electronegativities

30. Electronegativity A measure of the ability of an atom in a chemical
compound to attract electrons
  Electronegativities tend to increase across
a period
  Electronegativities tend to decrease down a
group or remain the same

31. Periodic Table of Electronegativities

32. Ionic Radii Cations Anions Positively charged ions formed when
an atom of a metal loses one or
more electrons
Cations
  Smaller than the corresponding
atom
Negatively charged ions formed
when nonmetallic atoms gain one
or more electrons
Anions
Larger than the corresponding
atom

33. Table of Ion Sizes

34. Summation of Periodic Trends