![Silver element card: symbol Ag, atomic number 47, atomic mass 107.87, electron configuration [Kr] 4d¹⁰ 5s¹, oxidation states +1, Transition metal, group 11, period 5, solid at room temperature.](https://stage.chemistry-dictionary.com/wp-content/uploads/2026/09/silver-chemical-element.webp)
Silver sits in group 11 of the periodic table alongside copper and gold. It is a ductile metal, meaning you can easily stretch it into thin wires. It naturally exists in the Earth’s crust as a completely pure, uncombined element.
Miners also frequently extract it from natural mineral deposits like argentite and chlorargyrite. A single electron in its outermost shell moves freely through the solid metallic lattice. This highly mobile electron gives silver its unparalleled electrical and thermal conduction properties.
Silver strongly resists general chemical corrosion in clean air and pure water. This chemical stability ensures it lasts a very long time in most physical environments. However, silver noticeably tarnishes when exposed to normal ambient air over long periods.
The metal reacts continuously with trace amounts of hydrogen sulfide gas in the atmosphere. This slow chemical reaction forms a characteristic dark surface layer of silver sulfide (Ag2S). The metal readily forms many diverse chemical compounds in the +1 oxidation state.
Silver nitrate (AgNO3) serves as a highly versatile starting chemical for other chemical reactions. Chemists use it frequently to synthesize a wide variety of useful silver-based materials. Furthermore, specific chemical compounds called silver halides are extremely sensitive to visible light.
Light alters their atomic structure almost instantly upon any direct physical exposure. This unique chemical property formed the fundamental basis of traditional photographic film and medical imaging.