Periodic Table
Periodic Table Family Notes
1. Alkali Metals (Group 1)
Elements: Li, Na, K, Rb, Cs, Fr
Detailed Characteristics
● Have 1 valence electron in their outer energy level.
● Easily lose this electron, forming +1 ions.
● The most reactive metals on the periodic table.
● React vigorously with water, producing hydrogen gas and heat.
● Soft enough that some can be cut with a knife.
● Silver-colored and shiny when freshly cut.
● Become more reactive as you move down the group.
Where They Are Found
● Never found alone in nature because they react quickly with other elements.
● Usually found in compounds such as salts and minerals.
Real-World Uses
● Lithium: rechargeable batteries.
● Sodium: table salt, street lamps.
● Potassium: fertilizers and plant growth.
2. Alkaline Earth Metals (Group 2)
Elements: Be, Mg, Ca, Sr, Ba, Ra
Detailed Characteristics
● Have 2 valence electrons.
● Form +2 ions by losing both electrons.
● Reactive metals, but less reactive than alkali metals.
● Harder, denser, and stronger than alkali metals.
● Good conductors of heat and electricity.
● Shiny, silver-white appearance.
Biological Importance
● Calcium is necessary for healthy bones and teeth.
● Magnesium is important for muscle and nerve function.
Real-World Uses
● Magnesium: fireworks and lightweight alloys.
● Calcium: cement, chalk, and bones.
● Barium: medical imaging and fireworks.
3. Transition Metals (Groups 3-12)
Detailed Characteristics
● Include most familiar metals.
● Excellent conductors of electricity and heat.
● Strong, dense, and have high melting points.
● Less reactive than Groups 1 and 2.
● Many can form ions with different charges.
● Often produce colorful compounds.
Special Features
● Some act as catalysts that speed up chemical reactions.
● Many are magnetic.
Real-World Uses
● Iron: buildings, bridges, vehicles.
● Copper: electrical wiring.
● Titanium: aircraft and medical implants.
● Gold and Silver: jewelry and electronics.
4. Boron Family (Group 13)
Elements: B, Al, Ga, In, Tl
Detailed Characteristics
● Have 3 valence electrons.
● Usually form +3 ions.
● Contains one metalloid (boron) and several metals.
● Less reactive than Groups 1 and 2.
Interesting Facts
● Gallium melts at about room temperature and can melt in your hand.
● Aluminum is the most abundant metal in Earth's crust.
Real-World Uses
● Aluminum: cans, airplanes, foil.
● Boron: glass, detergents, and fiberglass.
5. Carbon Family (Group 14)
Elements: C, Si, Ge, Sn, Pb
Detailed Characteristics
● Have 4 valence electrons.
● Can gain, lose, or share electrons.
● Includes nonmetals, metalloids, and metals.
● Forms many complex compounds.
Biological Importance
● Carbon is the basis of all living things.
● Every living organism contains carbon compounds.
Real-World Uses
● Carbon: fuels, plastics, living organisms.
● Silicon: computer chips and solar panels.
● Tin: food cans and solder.
6. Nitrogen Family (Group 15)
Elements: N, P, As, Sb, Bi
Detailed Characteristics
● Have 5 valence electrons.
● Need three more electrons for a full outer shell.
● Can form many different compounds.
● Includes nonmetals, metalloids, and metals.
Biological Importance
● Nitrogen is essential for proteins and DNA.
● Phosphorus is important for bones, teeth, and energy transfer in cells.
Real-World Uses
● Nitrogen: fertilizers and food preservation.
● Phosphorus: fertilizers and matches.
● Bismuth: medicines and cosmetics.
7. Oxygen Family (Chalcogens, Group 16)
Elements: O, S, Se, Te, Po
Detailed Characteristics
● Have 6 valence electrons.
● Usually gain 2 electrons to form −2 ions.
● Includes nonmetals, metalloids, and metals.
● Very important in both living and nonliving systems.
Biological Importance
● Oxygen is needed for cellular respiration.
● Sulfur is found in proteins and amino acids.
Real-World Uses
● Oxygen: breathing and medical treatments.
● Sulfur: fertilizer and sulfuric acid production.
● Selenium: solar panels and electronics.
8. Halogens (Group 17)
Elements: F, Cl, Br, I, At
Detailed Characteristics
● Have 7 valence electrons.
● Need just one more electron to become stable.
● Extremely reactive nonmetals.
● React readily with metals to form salts.
● Never found free in nature.
Physical Properties
● Fluorine and chlorine are gases.
● Bromine is a liquid.
● Iodine and astatine are solids.
Real-World Uses
● Fluoride: toothpaste.
● Chlorine: disinfecting water.
● Iodine: antiseptics and nutrition.
9. Noble Gases (Group 18)
Elements: He, Ne, Ar, Kr, Xe, Rn
Detailed Characteristics
● Have complete outer electron shells.
● Extremely stable and unreactive.
● Colorless, odorless gases.
● Rarely combined with other elements.
Why They Are Special
● Their full electron shells make them very stable.
● They almost never participate in chemical reactions.
Real-World Uses
● Helium: balloons and MRI machines.
● Neon: advertising signs.
● Argon: welding and light bulbs.
● Xenon: flash lamps and spacecraft engines.
10. Lanthanides
Elements: La-Lu
Detailed Characteristics
● Known as the Rare Earth Elements.
● Soft, shiny, silver-colored metals.
● Good conductors of electricity.
● They often react with oxygen in the air.
Importance
● Essential for many modern technologies.
● Difficult and expensive to separate from ores.
Real-World Uses
● Powerful magnets.
● Smartphones.
● Electric vehicles.
● Wind turbines.
● Laser systems.
11. Actinides
Elements: Ac-Lr
Detailed Characteristics
● Radioactive elements.
● Many are human-made.
● Heavy metals with unstable nuclei.
● Release energy through radioactive decay.
Importance
● Important in nuclear science and medicine.
● Some can be used as fuel in nuclear reactors.
Real-World Uses
● Uranium: nuclear power plants.
● Plutonium: nuclear fuel.
● Americium: smoke detectors.
● Certain actinides: cancer treatments and scientific research.
Family Comparison
Easy Memory Trick
Group 1 loses 1, Group 2 loses 2, Group 17 gains 1, Group 18 has none to gain or
lose.
This pattern helps students understand why alkali metals, halogens, and noble gases
behave so differently.