Interactive Periodic Table

Organization

The periodic table arranges all 118 known chemical elements by increasing atomic number. Elements in the same column (group) share similar chemical properties and valence electron counts. Rows (periods) correspond to the number of electron shells.

Element Categories

• Alkali Metals: Soft, highly reactive metals in Group 1 (Li, Na, K, Rb, Cs, Fr)
• Alkaline Earth Metals: Reactive metals in Group 2 (Be, Mg, Ca, Sr, Ba, Ra)
• Transition Metals: Groups 3-12, known for variable oxidation states and colored compounds
• Post-transition Metals: Softer metals near the metalloid boundary (Al, Ga, In, Sn, Tl, Pb, Bi, Nh, Fl, Mc, Lv)
• Metalloids: Properties between metals and nonmetals (B, Si, Ge, As, Sb, Te, Po)
• Nonmetals: Poor conductors, diverse properties (C, N, O, P, S, Se)
• Halogens: Highly reactive nonmetals in Group 17 (F, Cl, Br, I, At, Ts)
• Noble Gases: Stable, unreactive gases in Group 18 (He, Ne, Ar, Kr, Xe, Rn, Og)
• Lanthanides: Rare earth elements 57-71
• Actinides: Radioactive elements 89-103

Electron Configuration

Electrons occupy orbitals in order of increasing energy. The notation uses principal quantum numbers and subshell letters (s, p, d, f) with superscripts showing electron count. Noble gas core notation abbreviates inner shells — for example, sodium is written [Ne] 3s¹ instead of 1s² 2s² 2p⁶ 3s¹.

Key Properties

• Atomic Number: Proton count, defines the element
• Atomic Mass: Weighted average of naturally occurring isotopes (in amu)
• Electronegativity: Pauling scale measure of electron-attracting tendency in bonds
• Density: Mass per unit volume at standard conditions
• Melting/Boiling Point: Phase transition temperatures at 1 atm pressure
• Oxidation States: Common charges when forming compounds

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