1. The Periodic Table
PERIODS (or SERIES)
GROUPS
(or COLUMNS)

2. Metals, Nonmetals, Semimetals

3. Properties
Metals:
metallic luster, ductility, malleability, react with nonmetals, solid state, conduct heat, conduct electricity.
Located to the left of the “staircase”
Nonmetals:
dull, brittle, low melting point, nonconductors, react with metals and nonmetals
Located to the right of the “staircase”
Semimetals:
have properties of metals and nonmetals
Located on the “staircase”

4. Group 1: Alkali Metals Lower densities than other metals
One loosely bound valence electron
Highly reactive
React violently with water
Lithium (Li)
Sodium (Na)
Potassium (K)
Rubidium (Rb)
Cesium (Cs)
Francium (Fr)

5. Alkali Metals Sodium (Na) Density @ 293 K: 0.971 g/cm3 Color: silvery
Date of Discovery: 1807 by Sir Humphrey Davy Name Origin: soda (Na2CO3)
Symbol Origin: From the Latin word natrium (sodium) Uses: medicine, agriculture Obtained From: table salts and other foods

6. Alkali Metals Potassium (K) Density: 0.828g/cm3
Melting point: K (63.38 °C)
Boiling point: 1023K (759OC)
Date of Discovery: 1807 by Sir Humphrey Davy
“Kalium” is arabic for “calcined ash”
When in contact with water, hydrogen gas is produced. The hydrogen gas usually ignites.
Pure potassium is never found; it is isolated from compounds and frequently found in its ion form.

7. Alkali Metals Potassium (K) Potassium acts to
relax muscle contraction.
Assist regulation of heartbeat.
Help as a major component in Na+K+ Pump for action potentials.
Assist pH balance in blood and tissues.
Hypokalemia (potassium deficiency) can result in
Muscle weakness and spasms
Heart deterioration
RDA: 1875mg-5625mg
Some sources: bananas, orange juice, almonds, apples, dried figs

8. Group 2: Alkaline Earth Metals
Two electrons in the outer shell
reactive
Beryllium (Be)
Magnesium (Mg)
Calcium (Ca)
Strontium (Sr)
Barium (Ba)
Radium (Ra)

9. Alkaline Earth Metals Calcium (Ca) Density @ 293 K: 1.55 g/cm3
Melting point: 1115K (842 °C)
Boiling point: 1757K (1484 °C)
Color: Silvery
Date of Discovery: 1808 by Sir Humphrey Davy
Name Origin: From the latin word calcis (lime)
Uses: life forms for bones and shells Obtained From: chalk, limestone, marble. 3.5% of crust

10. Alkaline Earth Metals Calcium (Ca) Calcium acts to Contract muscles.
Promote health of bones.
Assist blood clotting.
Calcium carbonate –dietary supplement, antacid
Calcium citrate –dietary supplement, preservative (calcium is absorbed more readily compared to calcium carbonate but more must be taken)
RDA: 800 mg
Some good sources: sesame seeds, almonds, broccoli, dairy products

11. Groups 3-16 Transition Metals Other Metals Metalloids/Semimetals
Metals in Groups 3-12
Other Metals
(Aluminum (Al), Gallium (Ga), Indium (In), Thallium (Tl), Tin (Sn), Lead (Pb), Bismuth (Bi))
Metalloids/Semimetals
(Boron (B), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te), Polonium (Po), Astatine (At))
Nonmetals
(Carbon (C), Nitrogen (N), Phosphorus (P), Oxygen (O), Sulfur (S), Selenium (Se))

12. Group 17: Halogens
“Halogen” means “salt-former”-compounds containing halogens are salts.
Halogens have 7 valence electrons
At room temperature, halogens exist as all three states of matter:
Solid- Iodine (I), Astatine (At)
Liquid- Bromine (Br)
Gas- Fluorine (F), Chlorine (Cl)
Iodine:

13. Group 18: Noble Gases
Have the maximum number of valence electrons; they are stable, not on a quest to gain or lose electrons.
Do not readily form compounds
Helium (He)
Neon (Ne)
Argon (Ar)
Krypton (Kr)
Xenon (Xe)
Radon (Rn)

14. Inner Transition Elements
Lanthanides:
Silvery-white metals that tarnish when exposed to air, forming their oxides.
Relatively soft metals.
High melting points and boiling points.
Burn easily in air.
Actinides:
All are radioactive.
The metals tarnish readily in air.
very dense metals with distinctive structures.

15. Elements to Know H (hydrogen) Na (sodium) K (potassium) Mg (magnesium)
Ca (calcium)
C (carbon)
N (nitrogen)
P (phosphorus)
O (oxygen)
S (sulfur)
F (fluorine)
Cl (chlorine)
Br (bromine)
I (iodine)