Periodic Families

Alkali Metals (Group 1)

Elements: Li, Na, K, Rb, Cs, F

Valence Electrons: 1

Common charge: +1 (lose 1 electron)

Notes: Very reactive, never found uncombined in nature, react strongly with water.

Alkaline Earth Metals (Group 2)

Elements: Be, Mg, Ca, Sr, Ba, Ra

Valence Electrons: 2

Common Charge: +2 (lose 2 electrons)

Notes: Reactive, but less so than Group 1. Form basic (alkaline) solutions.

Transition Metals (Groups 3-12)

Elements: Includes Fe, Cu, Zn, Ag, Au, etc.

Valence Electrons: Usually 1–2 in outer shell, but can vary due to d-orbitals.

Common Charges: Variable (e.g., Fe²⁺, Fe³⁺, Cu⁺, Cu²⁺, etc.)

Notes: Often form colored compounds, multiple oxidation states.

Boron Group (Group 13)

Elements: B, Al, Ga, In, Tl

Valence Electrons: 3

Common Charge: +3 (lose 3 electrons)

Notes: Aluminum is the most common. Boron is a metalloid.

Carbon Group (Group 14)

Elements: C, Si, Ge, Sn, Pb

Valence Electrons: 4

Common Charges: +4 or -4 (can gain or lose 4 electrons)

Notes: Carbon is essential for life. Charge depends on bonding.

Nitrogen Group (Pnictogens, Group 15)

Elements: N, P, As, Sb, Bi

Valence Electrons: 5

Common Charge: -3 (gain 3 electrons)

Notes: Form covalent bonds often; nitrogen makes up ~78% of air.

Oxygen Group (Chalcogens, Group 16)

Elements: O, S, Se, Te, Po

Valence Electrons: 6

Common Charge: -2 (gain 2 electrons)

Notes: Oxygen is essential for respiration; sulfur is key in proteins.

Halogens (Group 17)

Elements: F, Cl, Br, I, At, Ts

Valence Electrons: 7

Common Charge: -1 (gain 1 electron)

Notes: Very reactive nonmetals, form salts with Group 1 metals.

Noble Gases (Group 18)

Elements: He, Ne, Ar, Kr, Xe, Rn, Og

Valence Electrons: 8 (except He with 2)

Common Charge: 0 (full valence shell, no charge)

Notes: Very stable, inert, rarely form compounds.