Element identity
Atomic number, symbol, relative atomic mass display and periodic position are established reference data.
Atomic / electronic model
Ground-state electron configuration and atomic reference values are compiled/evaluated data; orbital graphics are teaching probability models, not photographs.
Material / molecular structure
The displayed ordinary structure is based on established material or molecular science; simplified viewers are labelled as teaching schematics where exact crystallographic coordinates are not rendered.
Temperature / phase path
Transition values are reference/evaluated values for the stated teaching path; pressure, purity and allotropy can matter.
Geography
Real pins use reviewed place/dataset context. Conceptual layers are used when country pins would imply false occurrence, unsafe inventory or an incomplete global distribution.
The lens describes evidence status, not confidence theatre. “Unknown” is kept unknown, and teaching schematics are not presented as direct measurements.
Silver (Ag)
Silver is a Group 11 transition metal with a filled 4d subshell, one 5s electron, excellent electrical conduction, an FCC crystal and an unusual silvery-white metallic color.
Silver atomic number, mass, protons, electrons and electron configuration
Silver: quick answers
How many protons, neutrons and electrons does silver have?
Silver’s atomic number is 47, so every silver atom has 47 protons, and a neutral atom also has 47 electrons. Its most common natural isotope, silver-107, has 60 neutrons (other isotopes have different neutron counts).
What is the symbol for silver?
The chemical symbol for silver is Ag.
Is silver a solid, liquid or gas at room temperature?
Silver is a solid at room temperature (about 25 °C).
What family (group) is silver in?
Silver is a transition metal, in group 11, period 5 of the periodic table.
What is the electron configuration of silver?
The ground-state electron configuration of silver is [Kr] 4d¹⁰ 5s¹.
From atomic number to chemistry
Read these as a chain of causes, not as isolated facts. Each step links to the concept hub if you want the underlying idea explained.
Forty-seven protons define silver and neutral Ag contains 47 electrons.
A filled d subshell and outer s electron connect silver to Group 11.
Silver sits between copper and gold in the coinage-metal column.
Its solid electronic structure supports very high electrical conductivity and strong visible reflectance.
Silver group, period and position in the periodic table
Silver is the Period 5 member of Group 11, between copper and gold in the family sequence. Group membership gives a useful family comparison, but silver’s color, density, reactivity and electronic-band details remain its own.
Silver Visual Lab
Decode the Ag tile, rotate a true 3D ¹⁰⁷Ag teaching nucleus, inspect representative 5s and 4d orbital-shape models, explore the FCC crystal lattice and connect silver’s materials chemistry to the real world.
Seven facts packed into one square
Silver in one minute
Ag comes from argentum. The symbol comes from the Latin name for silver.
Silver is silvery-white. Its visible reflectance is shaped by interband transitions in the solid.
It conducts extremely well. That makes silver foundational to electrical systems.
It is FCC. The ordinary metallic crystal is face-centred cubic.
Two isotopes dominate nature. ¹⁰⁷Ag and ¹⁰⁹Ag are both stable.
2 · 8 · 18 · 18 · 1 electrons
Neutral silver has 47 electrons. The isolated ground-state atom is [Kr] 4d¹⁰ 5s¹: a filled 4d subshell plus one 5s electron.
A metal is an extended solid. The isolated-atom configuration is the starting point, but electrical conduction comes from delocalized electronic bands and scattering in the crystal.
Silver adopts an FCC crystal structure under ordinary conditions. Atoms occupy cube corners and face centres; those sites are shared among neighboring unit cells in the extended metal.
[Kr] 4d¹⁰ 5s¹
This is a qualitative isolated-atom learning model. It helps visualize orbital shape, while the properties of metallic silver require a solid-state band picture.
Why does silver appear everywhere electricity and heat move?
Its usefulness comes from a combination of conductivity, ductility, thermal performance, corrosion behavior and alloy chemistry.
Very high conductivity at critical interfaces
Silver is widely used where low electrical resistance and reliable contact performance justify its cost.
Why is silver such a bright, silvery reflector?
Silver reflects visible light very strongly across a broad wavelength range. Its electronic structure makes it look bright and silvery rather than strongly colored like copper or gold.
Start with a metal
Mobile electronic states give silver strong metallic reflection and electrical conduction.
Filled 4d states sit nearby
The filled 4d-derived bands lie close enough in energy to contribute important optical transitions.
Visible reflectance stays high
Silver has exceptionally strong visible reflectance, which is why polished silver is used in high-quality mirrors.
The surface looks bright and silvery-white
A broad, strong reflected spectrum gives the familiar bright metallic appearance.
Silver does not reflect visible light uniformly
Silvery metal: visible wavelengths are reflected more evenly.
Silver: broad high reflectance gives a bright silvery-white appearance.
Teaching diagram only — not a measured reflectance spectrum.
Color and conductivity are both band-structure properties
The isolated [Kr] 4d¹⁰ 5s¹ configuration is useful for introducing the atom, but a piece of silver is a solid with extended electronic bands. Classic optical measurements show an interband-transition threshold in the visible/near-visible region, while longer wavelengths behave more strongly like a free-electron metal.
That same solid-state viewpoint also explains why conductivity cannot be reduced to “the 5s electron moves around.” Mobile electronic states carry current; scattering from phonons, defects and impurities limits resistance.
Physical Review optical data · RSC/NIST contextWhy does silver conduct so well?
Use the cards to connect silver’s atomic and solid-state structure to the exceptional electrical and thermal conductivity that make the metal technologically important.
Electrical · mobile electronic states
Silver’s metallic band structure supports efficient charge transport. Resistivity still depends on temperature, purity and microstructure.
Silver physical, atomic, thermal and chemical properties
Reference data are grouped into tabs so detailed values do not flatten the page into a long generic grid.
| Atomic number | 47 | Number of protons. |
|---|---|---|
| Relative atomic mass | 107.8682 | Natural isotope-weighted reference value. |
| Electron configuration | [Kr] 4d¹⁰ 5s¹ | Ground-state shorthand. |
| Electronegativity | 1.90 | Pauling scale. |
| Non-bonded radius | 2.11 Å | Radius values depend on definition. |
| 1st ionization energy | 730.995 kJ/mol | Gaseous-atom reference. |
| Electron affinity | 125.624 kJ/mol | Gaseous-atom reference. |
| Appearance | Silvery-white metallic | Characteristic bulk silver color. |
|---|---|---|
| Density | 10.5 g/cm³ | Near room temperature. |
| Crystal structure | Face-centred cubic | FCC / cubic close-packed. |
| Group / period / block | 11 / 5 / d | Transition metal. |
| State | Solid | Near ordinary conditions. |
| Melting point | 1234.93 K | 961.78 °C. |
|---|---|---|
| Boiling point | 2435 K | Reference value used by this guide. |
| Temperature tool | Open the interactive state explorer ↓ | |
| Context | Phase boundaries and transport properties depend on pressure and material condition. | |
| Electrical behaviour | Excellent conductor | Mobile electronic states carry current efficiently. |
|---|---|---|
| Thermal behaviour | Excellent conductor | Important in heat exchangers and heat sinks. |
| Engineering note | Ductile | Can be drawn into wire and formed into complex parts. |
| Measurement note | Numerical conductivity depends on temperature, purity, work hardening and microstructure. | |
| Common oxidation states | +1, +2 | Ag(I) is by far the most common simple oxidation state; higher states occur in specialized chemistry. |
|---|---|---|
| Representative compounds | Ag₂O · AgNO₃ · AgCl · Ag₂S | Oxide, nitrate, chloride and sulfide examples. |
| Tarnish | Surface reaction products | Sulfur-containing environments can form dark silver-sulfide-rich tarnish layers. |
| ¹⁰⁷Ag | 51.839% | 47 p · 60 n · stable |
|---|---|---|
| ¹⁰⁹Ag | 48.161% | 47 p · 62 n · stable |
| Natural stable isotopes | 2 | Both contribute to relative atomic mass 107.8682. |
Silver makes more sense beside copper and gold
Copper, silver and gold share a filled d-subshell plus outer s-electron pattern, but family resemblance does not make their color, density or chemistry identical.
| Configuration | 3d¹⁰ 4s¹ |
|---|---|
| Electronegativity | 1.90 |
| Appearance | reddish |
| Configuration | 4d¹⁰ 5s¹ |
|---|---|
| Electronegativity | 1.93 |
| Appearance | silvery-white |
| Configuration | 5d¹⁰ 6s¹ |
|---|---|
| Electronegativity | 2.54 |
| Appearance | yellow |
Why compare Cu, Ag and Au?
All are conductive Group 11 metals with related isolated-atom configurations and a long history of coinage, electrical or decorative use.
Why silver still needs its own explanation
Silver is lighter and less noble than gold, has a distinctive silvery-white optical response, and its technical role is dominated by bulk electrical and thermal conduction.
Silver state at temperature: solid, liquid or gas
Use the slider or the three quick-state blocks to see how the tile color and state panel change across silver’s solid, liquid and gas regions.
Approximately standard-pressure teaching model. Real phase behavior also depends on pressure and experimental conditions.
Where on Earth is silver mined and where are major reserves?
Natural occurrence and modern production are different questions. The default map shows 2025 estimated mine output from USGS; the reserve mode uses the same USGS 2026 reporting framework.
How silver is produced: the high-level process
Processing depends on ore type. Silver is commonly recovered from polymetallic ores and by-product streams, so routes depend strongly on the host ore, so this is a high-level map rather than a one-size-fits-all recipe.
Mine and characterize
Geology and mineralogy determine whether silver occurs in lead-zinc, copper, gold or dedicated silver-bearing ores.
Concentrate or leach
Ore concentration and leaching choices depend on mineralogy and co-products.
Recover silver
Smelting, leaching, electrorefining and by-product recovery can concentrate silver depending on the feed stream.
Refine + fabricate
Refined silver becomes bullion, electrical materials, powders, pastes, coatings and alloy feedstock.
Silver was worked before written chemistry
Native silver
Native silver was one of the first metals people could work directly.
Coinage + ornaments
Silver became important for ornaments, exchange and coinage in many societies.
From argentum
The symbol Ag comes from the Latin word argentum.
Electronics + optics
Silver is important in contacts, conductive pastes, mirrors, solar technology and specialized chemistry.
What is silver used for?
Electrical contacts
Silver’s very high conductivity makes it valuable where low contact resistance matters.
Conductive pastes
Silver pastes and inks are used in electronics and photovoltaic contacts.
Mirrors
High visible reflectance makes silver important in optical coatings and mirrors.
Photography history
Light-sensitive silver halides were foundational to photographic film and paper.
Jewelry + silverware
Silver alloys combine luster and workability with improved practical durability.
Antimicrobial surfaces
Silver ions and compounds are used in selected antimicrobial materials and medical products.
Representative silver compounds and oxidation states
Silver(I) oxide · Ag₂O
A brown-black Ag(I) oxide illustrating the +1 oxidation state.
Silver nitrate
A soluble Ag(I) compound widely used as a laboratory and industrial silver source.
Silver chloride
A light-sensitive Ag(I) halide central to classic photographic chemistry.
Silver sulfide
A dark silver compound associated with common tarnish on silver surfaces.
Natural silver: ¹⁰⁷Ag and ¹⁰⁹Ag
Three-question Silver check
What is silver’s ground-state electron configuration shorthand?
Why is silver useful for wiring?
Which two isotopes make up natural silver?
Silver questions: quick answers first, then the mechanism
Open a question for a fast answer followed by the deeper materials or electronic explanation.
Why does silver tarnish?
Short answer: Silver darkens mainly because sulfur-containing substances in the environment form a thin silver-sulfide-rich surface layer.
This is tarnish, not iron rust. The rate depends on sulfur-containing gases, humidity, pollutants and the alloy or surface condition. The black appearance is associated primarily with Ag₂S-rich corrosion products rather than a simple layer of silver oxide.
The underlying metal can remain an excellent electrical conductor even while a thin surface film changes appearance and contact behavior.
Key point: Silver tarnish is sulfur chemistry at the surface, not “silver rust.”
Why is silver the best electrical conductor among common elemental metals?
Short answer: At ordinary temperatures, pure silver has exceptionally low electrical resistivity because its metallic electronic structure provides highly mobile carriers with comparatively low scattering.
“Best conductor” needs conditions: conductivity changes with temperature, purity, defects and frequency. For bulk elemental metals near room temperature, silver is the benchmark, but copper is often preferred in wiring because it combines excellent conductivity with lower cost and practical mechanical properties.
As with copper, conductivity belongs to the metallic solid and its band structure; it is not explained by treating one valence electron as a classical free particle detached from the crystal.
Key point: Silver’s conductivity is exceptional under defined material conditions; engineering choice also depends on cost, strength and environment.
How is silver different from gold if both are Group 11?
Short answer: They share a filled d-shell plus outer s-electron pattern, but their energies, colors, chemical reactivity, density and relativistic effects differ.
Group position gives family resemblance, not identity. Silver is lighter and silvery-white, gold is much denser and yellow, and gold’s heavy-atom relativistic effects are substantially stronger.
Scientific sources for Silver
Core atomic data, isotopic composition, physical properties, optical interpretation and changing mining figures are tied to scientific or government sources. Production/reserve figures are labeled by source year.
Questions to ask next about Silver
A good element lesson should lead to the next useful question, not end after a list of facts.
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