Silver Element Properties
Complete reference for Silver (Ag, element 47): atomic data, electron configuration, isotopes, physical constants, oxidation states, and a property unit converter.
Silver
Transition Metal — Period 5, Group 11
Atomic Identity
Periodic Table Locator — Period 5 Neighborhood (d-block)
Silver (Z=47) sits between palladium (Z=46) and cadmium (Z=48) in Period 5. It is directly above gold (Z=79) and below copper (Z=29) in Group 11 — the three coinage metals sharing a filled inner d-subshell.
Electron Configuration
Full 4d¹⁰ stabilizes the atom — 5s has only 1 electron
Key Isotopes of Silver
| Isotope | Symbol | Protons | Neutrons | Mass (u) | Abundance | Stability |
|---|---|---|---|---|---|---|
| Silver-105 | ¹⁰⁵Ag | 47 | 58 | 104.906525 | Radioactive |
Unstable
EC/β⁺; t½ = 41.29 d — used in research |
| Silver-107 | ¹⁰⁷Ag | 47 | 60 | 106.905097 | 51.839% | Stable |
| Silver-109 | ¹⁰⁹Ag | 47 | 62 | 108.904752 | 48.161% | Stable |
| Silver-110m | ¹¹⁰ᵐAg | 47 | 63 | 109.906111 | Radioactive |
Unstable
IT/β⁻; t½ = 249.95 d — nuclear accident tracer |
| Silver-111 | ¹¹¹Ag | 47 | 64 | 110.905291 | Radioactive |
Unstable
β⁻; t½ = 7.45 d — cancer therapy radioisotope |
Silver has exactly two stable isotopes, Ag-107 and Ag-109, with nearly equal abundances — an unusual occurrence that places silver's standard atomic weight almost precisely between their masses. Ag-111 is under investigation as a therapeutic radioisotope for targeted cancer treatment, analogous to the clinically established Lu-177.
Physical Properties
Chemical Properties
Oxidation States of Silver
| State | Ion / Form | Example Compound | Notes |
|---|---|---|---|
| 0 | Ag⁰ | Ag metal, Ag nanoparticles | Native silver; colloidal silver antimicrobials |
| +1 | Ag⁺ (argentous) | AgNO₃, AgCl, AgBr, AgI, Ag₂O, Ag₂S | Dominant state; colorless in solution; most compounds are insoluble |
| +2 | Ag²⁺ (argentic) | AgF₂, AgO (mixed-valence oxide) | Strong oxidizer; AgO is actually Ag⁺Ag³⁺O₂ mixed-valence |
| +3 | Ag(III) | AgF₃, KAgF₄ | Rare; found only in strongly oxidizing fluoride compounds |
Ground State Quantum Numbers
Notable Emission Lines
Silver produces a pale blue-white flame in a flame test, faint because Ag⁺ has a high ionization energy relative to alkali metals. The resonance lines at 328.07 nm and 338.29 nm are primary lines used in atomic absorption spectroscopy (AAS) for silver determination in environmental and industrial samples.
Property Unit Converter
Convert common silver property values between units. Enter a value and select the conversion.
Common Silver Compounds
| Compound | Formula | Common Name | Key Uses |
|---|---|---|---|
| Silver(I) nitrate | AgNO₃ | Lunar caustic | Photography, lab reagent, antimicrobial wound care, silver plating |
| Silver(I) chloride | AgCl | Chlorargyrite | Photographic emulsions, electrodes, antiseptic dressings |
| Silver(I) bromide | AgBr | Bromargyrite | Primary photographic film and paper emulsion compound |
| Silver(I) iodide | AgI | Iodargyrite | Cloud seeding (nucleation agent), photography, antiseptic |
| Silver(I) oxide | Ag₂O | Silver monoxide | Oxidizing agent, silver button batteries (Ag₂O/Zn cells) |
| Silver(I) sulfide | Ag₂S | Acanthite / argentite | Main silver ore mineral; forms tarnish layer on silver metal |
| Silver(I) sulfate | Ag₂SO₄ | Silver sulfate | Organic chemistry oxidizer, wastewater treatment catalyst |
| Diaminosilver(I) nitrate | [Ag(NH₃)₂]NO₃ | Tollens' reagent | Aldehyde detection (silver mirror test), organic chemistry lab |
Key Facts About Silver
Best Electrical Conductor
Silver has the lowest electrical resistivity (15.87 nΩ·m) and highest thermal conductivity (429 W/(m·K)) of any element. These records stem from its filled 4d subshell and highly mobile single 5s conduction electron. Silver is used in high-performance electrical contacts, printed circuit boards, solar cell busbars, and superconducting magnet connections where copper is insufficient. Industrial demand for silver in electronics exceeds 250 million troy ounces per year.
Photography and Light Sensitivity
For over 150 years, silver halides (AgBr, AgCl, AgI) formed the backbone of photographic technology. Silver's unique photochemistry — the ability of photons to reduce Ag⁺ to atomic silver clusters at grain boundaries — enables latent image formation with extraordinary sensitivity (a single photon can trigger a detectable signal). Digital cameras have replaced silver-based photography for most uses, but silver halide media remain the archival gold standard for image permanence exceeding 500 years.
Tarnish: Silver Sulfide Chemistry
Silver tarnishes to form a black layer of silver sulfide (Ag₂S) when exposed to hydrogen sulfide (H₂S) or sulfur compounds in the air. Unlike copper's protective green patina, Ag₂S tarnish is purely cosmetic and does not protect the underlying metal. Silver can be cleaned by electrochemical reduction (aluminum foil + baking soda bath) that converts Ag₂S back to Ag without abrasion. Sterling silver (92.5% Ag, 7.5% Cu) tarnishes faster due to copper sulfide formation.
Antimicrobial Properties
Silver ions (Ag⁺) are potently antimicrobial, disrupting bacterial cell membranes, inactivating enzymes by binding sulfhydryl groups, and interfering with DNA replication. Silver nanoparticles release Ag⁺ ions continuously and are incorporated into wound dressings, medical device coatings, water purification filters, textiles, and food packaging. The EPA registers silver as an antimicrobial pesticide. Ancient civilizations stored water and wine in silver vessels precisely for this property.
Coinage and Monetary History
Silver's rarity, durability, divisibility, and attractive appearance made it the world's primary monetary metal for over 2,500 years. The Spanish dollar (peso de ocho, "piece of eight") mined from Potosi, Bolivia, funded global trade from 1550–1850 and became the model for the US dollar. The word "salary" derives from Latin salarium (salt money), but silver's role in salarium (silver payment) is equally ancient. Over 1.5 million tonnes of silver have been mined throughout history.
Solar Energy and Green Technology
Silver is an indispensable material in solar photovoltaics. Each silicon solar cell uses silver paste to form the front-side electrical contacts (busbars and fingers). A typical residential 6 kW solar installation contains approximately 20 grams of silver. Global solar panel production consumes roughly 100 million troy ounces of silver annually — about 10% of world silver supply — and this share is growing rapidly as the world transitions to renewable energy. Reduced silver loading per cell is a major research priority.
Summary
Complete reference for Silver (Ag, element 47): atomic data, electron configuration, isotopes, physical constants, oxidation states, and a property unit converter.
How it works
- Browse the atomic identity card for symbol, atomic number, and standard atomic weight.
- Check the electron configuration panel for the anomalous [Kr] 4d¹⁰ 5s¹ arrangement.
- Review the isotopes table for stable and notable radioactive isotopes with natural abundances.
- Consult the physical and chemical properties panels for melting point, density, ionization energies, and oxidation states.
- Use the interactive unit converter to convert silver property values between common units.
- Explore the key facts section for industrial context and interesting chemistry of silver.
Use cases
- Look up silver constants for chemistry homework, metallurgy, or materials science work.
- Verify atomic data when writing lab reports or research papers.
- Reference isotope data for radiochemistry or nuclear medicine research.
- Convert melting and boiling points between Celsius, Fahrenheit, and Kelvin.
- Study anomalous d-block electron configurations using silver as a canonical example.
- Confirm the dominant +1 oxidation state for writing ionic formulae or balancing redox equations.
- Research silver compounds for photography, antimicrobial applications, or electronics.
- Quick-reference conductivity and ionization energies for electrochemistry calculations.