Chemical element · reference page

47Ag

Silver

Silver is element 47 (Ag), located in period 5, group 11 and the d block. At room temperature its reference phase is solid. Its electron configuration is [Kr] 4d10 5s1.

Atomic number47

Standard atomic weight107.8682(2)

Group11

Period5

Blockd

Electron configuration[Kr] 4d10 5s1

Electronic structure

What controls its chemistry

The d subshell participates in the chemistry of silver. Transition metals can use electrons of similar energies in bonding, which is why variable oxidation states, coordination compounds and catalytic behaviour are common across the d block.

Its electron configuration, [Kr] 4d10 5s1, should be read together with the oxidation state of the compound: removing electrons changes which d orbitals are occupied and can alter colour, magnetism, bonding and reactivity.

Chemical forms

Compounds, ions and materials

For silver, important chemical forms include metals and alloys, oxides, halides and coordination compounds. Variable oxidation states are common because s and d electrons have similar energies, and ligands around the metal ion can strongly alter colour, magnetism and reactivity.

Physical behaviour

State and phase changes

The reference phase at room temperature is solid. The listed density is 10.49 g/cm³. The melting point is 1 235 K (961.8 °C). The boiling point is 2 435 K (2 162 °C). Pressure, purity and crystal structure can shift measured physical properties.

Occurrence and applications

Where silver is found and used

In practice, silver is encountered in jewellery, electronics and solar cells.

In practice

Examples of real uses

Jewellery

Silver is used for colour, corrosion resistance, rarity, polish or mechanical properties in jewellery alloys.

Electronics

Silver is used in electronic components or materials where conductivity, semiconducting behaviour, optical response or chemical stability is useful.

Solar cells

Silver is used in photovoltaic absorbers, contacts, coatings or semiconductor layers that convert light into electrical energy.

Periodic position

What its neighbours tell us

Silver is in period 5 and group 11. In the neighbourhood shown here, it lies between palladium and cadmium in the same period; copper is above it and gold below it in the same group. These positions make it possible to compare atomic size, ionisation energy and bonding behaviour with nearby elements.

Reference data

Physical and atomic properties

Classificationtransition metal

Phase at room temperatureSolid

Electron shells2 · 8 · 18 · 18 · 1

Density10.49 g/cm³

Melting point1 235 K (961.8 °C)

Boiling point2 435 K (2 162 °C)

Pauling electronegativity1.93

First ionisation energy731 kJ/mol

Electron affinity125.9 kJ/mol

Values describe the element or neutral atom where applicable. Physical data can depend on allotrope, pressure and measurement conditions.

History

Discovery and identification

Silver was known before 5000 BC, with no single discoverer identified in this record. Its early use predates modern chemistry, so use of the material, chemical identification and the later atomic-number definition are separate stages.

Isotopes and atomic weight

How isotope composition changes the numbers

The standard atomic weight is 107.8682(2). This value refers to the isotopic composition of natural terrestrial material, not to the mass of one specific atom.

Silver has at least one stable isotope. Different isotopes have the same number of protons and therefore the same element identity, but different neutron numbers and atomic masses.

Safety

Handling and exposure

The hazards associated with silver depend on chemical form, dose and route of exposure. Pure silver, its ions and its compounds can have very different biological and environmental effects, so safety data should be checked for the actual substance being handled.