Silver (Ag)
transition-metalSolid
Standardatomgewicht
107,8682 uElektronenkonfiguration
[Kr] 5s1 4d10Schmelzpunkt
961,78 °CSiedepunkt
2161,85 °CDichte
1,0501e+4 kg/m³Oxidationszustände
−2, −1, 0, +1, +2, +3Elektronegativität (Pauling)
1,93Ionisierungsenergie (1.)
7,576234 eVEntdeckungsjahr
N/AAtomradius
160 pmDetails
Silver is a soft, dense transition metal in group 11, chemically related to copper and gold but more reactive than gold. It is the best elemental conductor of electricity and heat at ordinary temperatures and has exceptional optical reflectivity when freshly polished. In nature it occurs as native metal and in sulfide, sulfosalt, chloride, and telluride minerals, commonly associated with lead, zinc, copper, and gold ores.
Pure silver has a brilliant white metallic luster. It is a little harder than gold and is very ductile and malleable, being exceeded only by gold and perhaps palladium. Pure silver has the highest electrical and thermal conductivity of all metals, and possesses the lowest contact resistance. It is stable in pure air and water, but tarnishes when exposed to ozone, hydrogen sulfide, or air containing sulfur. The alloys of silver are important.
The name derives from the Anglo-Saxon seofor and siolfur, which is of unknown origin. The symbol Ag derives from the Latin argentum and Sanskrit argunas from "bright". Silver was known in prehistoric times.
Archaeological evidence suggests that people have been using silver for at least 5000 years. Silver can be obtained from pure deposits, from silver ores such as argentite (Ag2S) and horn silver (AgCl), and in conjunction with deposits of ores containing lead, gold or copper.
The Latin word for silver is argentum. Silver has been known since ancient times. It is mentioned in Genesis. Slag dumps in Asia Minor and on islands in the Aegean Sea indicate that man learned to separate silver from lead as early as 3000 B.C.
Pure silver is a bright white, highly lustrous metal with a clean metallic sheen. It is malleable and ductile, and it takes a very high polish. In air it does not oxidize rapidly, but exposed surfaces darken by tarnishing, mainly through reaction with sulfur compounds.
Silver is used in electrical contacts, conductive pastes, solders, brazing alloys, and high-reliability connectors because of its conductivity and workability. It remains important in jewelry, tableware, coinage, and decorative objects, usually as alloys to improve hardness. Silver mirrors and coatings serve optical applications. Silver halides were central to photographic film and paper, though that use has declined. Silver compounds and silver-containing surfaces are also used where controlled antimicrobial action is desired.
Silver and silver compounds have many uses. Pure silver is the best conductor of heat and electricity of all known metals, so it is sometimes used in making solder, electrical contacts and printed circuit boards. Silver is also the best reflector of visible light known, but silver mirrors must be given a protective coating to prevent them from tarnishing. Silver has also been used to create coins, although today other metals are typically used in its place. Sterling silver, an alloy containing 92.5% silver, is used to make silverware, jewelry and other decorative items. High capacity batteries can be made with silver and zinc and silver and cadmium. Silver nitrate (AgNO3) is light sensitive and is used to make photographic films and papers. Silver iodide (AgI) is used to seed clouds to produce rain.
Sterling silver is used for jewelry, silverware, etc. where appearance is paramount. This alloy contains 92.5% silver, the remainder being copper or some other metal. Silver is of the utmost importance in photography, about 30% of the U.S. industrial consumption going into this application. It is used for dental alloys. Silver is used in making solder and brazing alloys, electrical contacts, and high capacity silver-zinc and silver-cadmium batteries. Silver paints are used for making printed circuits. It is used in mirror production and may be deposited on glass or metals by chemical deposition, electrode position, or by evaporation. When freshly deposited, it is the best reflector of visible light known, but is rapidly tarnished and loses much of its reflectance. It is a poor reflector of ultraviolet. Silver fulminate, a powerful explosive, is sometimes formed during the silvering process. Silver iodide is used in seeding clouds to produce rain. Silver chloride has interesting optical properties as it can be made transparent; it also is a cement for glass. Silver nitrate, or lunar caustic, the most important silver compound, is used extensively in photography. Silver for centuries has been used traditionally for coinage by many countries of the world. In recent times, however, consumption of silver has greatly exceeded the output.
Isotopes in Earth/Planetary Science
The measurement of relative amounts of 107Ag and 109Ag is used to study the processes responsible for the isotopic fractionation of silver isotopes in ore deposits, which depends on the specific minerals and environmental conditions. This is currently an area of active research and it is thought that the relative amounts of the isotopes of silver are altered during the formation of the ore [351] Y. Luo, E. Dabek-Zlotorzynska, V. Celo, D. C. Muir, L. Yang. Anal. Chem.82, 3922 (2010)., [352] A. V. Chugaev, I. V. Chernyshev. Geochim. Cosmochim. Acta Suppl.73, A225 (2009)..
Isotopes in Forensic Science and Anthropology
Silver isotope-amount ratiosn(107Ag)/n(109Ag) along with isotope-amount ratios of copper n(65Cu)/n(63Cu), and isotope-amount ratios of lead (n(206Pb)/n(204Pb), n(207Pb)/n(204Pb) and n(208Pb)/n(204Pb)) have been used to determine origins of European coins and information on the flow of goods in the world market over time (Fig. IUPAC.47.1). Metals from Peru and Mexico and those from European mining have distinct isotopic signatures that enable the origin of the metal to be determined by examining the isotopic compositions of silver, copper, and lead in the coins. Abundant silver sources, mined in Mexico and Peru in the 16 th century, were used to mint coins, but they were not a major influence in the European coin market until the 18 th century (Fig. IUPAC.47.1) [237] A. M. Desaulty, P. Telouk, E. Albalat, F. Albarede. Proc. Natl. Acad. Sci.108, 9002 (2011)..
Isotopes in Geochronology
The amount ratio n(107Pd)/n(107Ag) is used in geochronology to date major events in the Solar System [344] W. R. Kelly, G. J. Wasserburg. Geophys. Res. Lett.5 1079 (1978)., [345] G. J. Wasserburg, D. A. Papanastassiou. Some Short-Lived Nuclides in the Early Solar-System – A Connection with the Placental ISM, in Essays in Nuclear Astrophysics, C. A. Barnes, D. D. Clayton, and D. N. Schramm. Cambridge University Press, Cambridge, UK (1982)., [346] J. H. Chen, G. J. Wasserburg. Live 107Pd in the Early Solar System and Implications on Planetary Evolution, in Earth Processes: Reading the Isotopic Code, Geophysical Monograph 95, A. Basu and S. Hart. Amer. Geophys. U., Washington (1996)., [347] J. H. Chen, G. J. Wasserburg. Geochim. Cosmochim. Acta54, 1729 (1990)., [348] A. P. Dicken. Radiogenic Isotope Geology, Cambridge University Press, New York (1995)., [353] G. J. Wasserburg. “Short-lived nuclei in the early solar-system”, in Protostars and Planets, D. C. Black, M. S. Matthews (Eds.), Univ. Arizona Press, Tucson, Arizona, USA (1985).. Although 107Ag is naturally occurring, it is also the daughter product by beta decay of 107Pd. If both excess 107Ag and 107Pd are present in a sample of extraterrestrial origin, then the material would have formed sometime after 107Pd decayed (i.e. sometime after the 6.5-million-year half-life of 107Pd). The n(107Pd)/n(107Ag) amount ratio can be measured to help determine when the 107Pd decay process began and determine how much time has elapsed since the material was formed.
Isotopes in Industry
107Ag is being studied as a possible target for cyclotron production of 103Pd (with a half-life of 17 days) via the 107Ag (p, α n) 103Pd reaction. 103Pd releases X-rays and Auger electrons at the rate of about 80 X-rays and 186 Auger electrons per 100 decays of 103Pd, which makes this isotope an ideal candidate for internal radiotherapy for the treatment of cancers. The production of this isotope in a no-carrier form (not formed in another solution) is important for its medical uses. By using neutrons, photons, and charged particles to force reactions with isotopes of a higher mass number than 103, 103Pd will occur in a fraction of those reactions. The most common methods of 103Pd production use targets of rhodium or other isotopes of palladium. However, 107Ag has also been studied as a feasible option [349] M. Hussain, S. Sudar, M. N. Aslam, H. A. Shah, R. Ahmad, A. A. Malik, S. M. Qaim. Appl. Radiat. Isot.67, 1842 (2009)., [354] F. G. Perey. Phys. Rev. Lett.131, 745 (1963).. 109Ag is used to produce the gamma reference source 110mAg to help calibrate gamma detectors [349] M. Hussain, S. Sudar, M. N. Aslam, H. A. Shah, R. Ahmad, A. A. Malik, S. M. Qaim. Appl. Radiat. Isot.67, 1842 (2009)., [354] F. G. Perey. Phys. Rev. Lett.131, 745 (1963)..
Silver chemistry is dominated by the +1 oxidation state, with Ag⁺ forming many salts and coordination complexes. Silver nitrate (AgNO₃) is a common soluble reagent and precursor for other silver compounds. Silver chloride (AgCl), silver bromide (AgBr), and silver iodide (AgI) are sparingly soluble, light-sensitive halides that underpinned traditional photography. Silver sulfide (Ag₂S) is the principal tarnish product and an important natural mineral. Higher oxidation states such as +2 and +3 exist in specialized compounds, usually with strong oxidizing ligands or solid-state structures.
See more information at the Silver compound page.
Massive metallic silver has low acute toxicity, but dusts, soluble salts, and fine particles require careful handling. Chronic intake of bioavailable silver compounds can cause argyria, a persistent gray-blue discoloration of skin and other tissues. Silver nitrate (AgNO₃) is corrosive and stains skin and organic materials. Some silver compounds are toxic to aquatic organisms. Molten silver presents ordinary burn and metal-fume hazards in foundry or refining work.
While silver itself is not considered to be toxic, most of its salts are poisonous. Exposure to silver (metal and soluble compounds, as Ag) in air should not exceed 0.01 mg/m3, (8-hour time-weighted average - 40 hour week). Silver compounds can be absorbed in the circulatory system and reduced silver deposited in the various tissues of the body. A condition, known as argyria, results with a grayish pigmentation of the skin and mucous membranes. Silver has germicidal effects and kills many lower organisms effectively without harm to higher animals.
Silver is a trace element in soils, sediments, natural waters, and living organisms, with no established essential biological role in humans. In the environment Ag⁺ is strongly complexed or immobilized by sulfide, chloride, organic matter, and mineral surfaces. Mining, smelting, photography wastes, electronics, and some antimicrobial products can add silver to waste streams. In anoxic sediments, formation of silver sulfide (Ag₂S) greatly reduces mobility and bioavailability.
Silver is produced both from primary silver mines and, very often, as a by-product of lead, zinc, copper, and gold mining. Supply therefore depends partly on the economics of other base and precious metals. Demand is split among industrial uses, jewelry and silverware, investment products, and smaller specialty applications. Recycling is important from photographic materials, jewelry, electronics, and industrial scrap, but recovery is uneven when silver is widely dispersed in small devices or coatings. Its price is volatile because it is both an industrial metal and a precious metal.
Silver occurs natively and in ores such as argentite (Ag2S) and horn silver (AgCl); lead, lead-zinc, copper, gold, and copper-nickel ores are principal sources. Mexico, Canada, Peru, and the U.S. are the principal silver producers in the western hemisphere.
Silver is far less abundant cosmically than lighter metals such as iron or magnesium. Its stable isotopes, ¹⁰⁷Ag and ¹⁰⁹Ag, are made mainly by neutron-capture processes in earlier generations of stars, including slow and rapid neutron-capture pathways. In planetary materials it behaves as a chalcophile and moderately siderophile element, concentrating in sulfide phases and metallic portions more than in silicate minerals.
- Silver has the highest electrical conductivity of any element.
- Sterling silver is usually 92.5% silver, with copper as the main hardening metal.
- Fresh silver mirrors reflect visible light very well but tarnish in sulfur-rich air.
- Silver halides darken because light can reduce Ag⁺ to metallic silver.
- Most mined silver is not obtained from mines worked only for silver.
- Native silver can form wires, plates, and dendritic crystals in some deposits.
Bilder
Eigenschaften
Physikalisch
- Atomradius (empirisch)
- 160 pm Vergleiche Atomradius (empirisch) aller Elemente →
- Kovalenzradius
- 145 pm Vergleiche Kovalenzradius aller Elemente →
- Van-der-Waals-Radius
- 172 pm Vergleiche Van-der-Waals-Radius aller Elemente →
- Metallradius
- 134 pm Vergleiche Metallradius aller Elemente →
- Dichte
- 1,0501 × 104 kg/m³ Vergleiche Dichte aller Elemente →
- Molares Volumen
- 0,0103 L/mol
- Aggregatzustand bei Standardbedingungen
- Fest Vergleiche Aggregatzustand bei Standardbedingungen aller Elemente →
- Schmelzpunkt
- 961,78 °C Vergleiche Schmelzpunkt aller Elemente →
- Siedepunkt
- 2161,85 °C Vergleiche Siedepunkt aller Elemente →
- Wärmeleitfähigkeit
- 429 W/(m·K) Vergleiche Wärmeleitfähigkeit aller Elemente →
- Spezifische Wärmekapazität
- 0,235 J/(g·K) Vergleiche Spezifische Wärmekapazität aller Elemente →
- Molare Wärmekapazität
- 25,35 J/(mol·K) Vergleiche Molare Wärmekapazität aller Elemente →
- Kristallstruktur
- Flächenzentriert kubisch Vergleiche Kristallstruktur aller Elemente →
Chemisch
- Elektronegativität (Pauling)
- 1,93 Vergleiche Elektronegativität (Pauling) aller Elemente →
- Elektronegativität (Allen)
- 1,87
- Elektronenaffinität
- 1,302 eV
- Ionisierungsenergie (1.)
- 7,576234 eV Vergleiche Ionisierungsenergie (1.) aller Elemente →
- Ionisierungsenergie (2.)
- 21,484474 eV Vergleiche Ionisierungsenergie (2.) aller Elemente →
- Ionisierungsenergie (3.)
- 34,80012 eV Vergleiche Ionisierungsenergie (3.) aller Elemente →
- Ionisierungsenergie (4.)
- 49,000169 eV Vergleiche Ionisierungsenergie (4.) aller Elemente →
- Ionisierungsenergie (5.)
- 65,000224 eV Vergleiche Ionisierungsenergie (5.) aller Elemente →
- Oxidationszustände
- −2, −1, 0, +1, +2, +3 Vergleiche Oxidationszustände aller Elemente →
- Valenzelektronen
- 11 Vergleiche Valenzelektronen aller Elemente →
- Elektronenkonfiguration
- [Kr] 5s1 4d10
Thermodynamisch
- Kritischer Punkt (Temperatur)
- 6137 °C
- Schmelzwärme
- 0,11690936 eV Vergleiche Schmelzwärme aller Elemente →
- Verdampfungswärme
- 2,597295 eV Vergleiche Verdampfungswärme aller Elemente →
- Sublimationswärme
- 2,952791 eV
- Atomisierungswärme
- 2,952791 eV
- Atomisierungsenthalpie
- 2,952791 eV
Nuklear
- Protonen
- 47 Vergleiche Protonen aller Elemente →
- Neutronen
- 60 Vergleiche Neutronen aller Elemente →
- Bekannte Isotope
- 42 Vergleiche Bekannte Isotope aller Elemente →
- Stabile Isotope
- 2 Vergleiche Stabile Isotope aller Elemente →
- Stabilstes Isotop
- Ag-107
Häufigkeit
- Häufigkeit (Erdkruste)
- 0,075 mg/kg Vergleiche Häufigkeit (Erdkruste) aller Elemente →
- Häufigkeit (Ozean)
- 4 × 10−5 mg/L Vergleiche Häufigkeit (Ozean) aller Elemente →
Kristallstruktur
- Gitterkonstante a
- 409 pm
Elektronische Struktur
- Elektronen pro Schale
- 2, 8, 18, 18, 1 Vergleiche Elektronen pro Schale aller Elemente →
Identifikatoren
- CAS-Nummer
- 7440-22-4 Vergleiche CAS-Nummer aller Elemente →
- Termsymbol
- 2S1/2
- InChI
- InChI=1S/Ag
- InChI-Key
- BQCADISMDOOEFD-UHFFFAOYSA-N
Elektronenkonfiguration Gemessen
Ag: 4d¹⁰ 5s¹[Kr] 4d¹⁰ 5s¹1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s¹Atommodell
Isotope ändern die Neutronenzahl, Masse und Stabilität — nicht die Elektronenkonfiguration eines neutralen Atoms.
Schematisches Atommodell, nicht maßstabsgetreu.
Atomarer Fingerabdruck
Emissions- / Absorptionsspektrum
Isotopenverteilung
| Massenzahl | Atommasse (u) | Natürliche Häufigkeit | Halbwertszeit |
|---|---|---|---|
| 107 Stabil | 106,9050916 ± 0,0000026 | 51,8390% | Stabil |
| 109 Stabil | 108,9047553 ± 0,0000014 | 48,1610% | Stabil |
Phase / Zustand
Grund: 936,8 °C unter Schmelzpunkt (961,78 °C)
Schematisch, nicht maßstabsgetreu
Phasenübergangspunkte
Übergangsenergien
Energie benötigt, um 1 mol am Schmelzpunkt zu schmelzen
Energie benötigt, um 1 mol am Siedepunkt zu verdampfen
Energie benötigt, um 1 mol am Sublimationspunkt zu sublimieren
Dichte
Bei Standardbedingungen
Bei Standardbedingungen
Erweitert
Atomspektren
10 von 47 angezeigt. Sortiert nach Ionenladung (aufsteigend).
Liniendaten ?
| Ion | Ladung | Gesamtlinien | Übergangswahrscheinlichkeiten | Niveau-Bezeichnungen |
|---|---|---|---|---|
| Ag I | 0 | 103 | 7 | 97 |
| Ag II | +1 | 455 | 237 | 455 |
| Ag III | +2 | 140 | 0 | 0 |
Niveaudaten ?
| Ion | Ladung | Niveaus |
|---|---|---|
| Ag I | 0 | 107 |
| Ag II | +1 | 100 |
| Ag III | +2 | 64 |
| Ag IV | +3 | 2 |
| Ag V | +4 | 2 |
| Ag VI | +5 | 2 |
| Ag VII | +6 | 2 |
| Ag VIII | +7 | 2 |
| Ag IX | +8 | 2 |
| Ag X | +9 | 2 |
Ionenradien
10 von 11 angezeigt.
| Ladung | Koordination | Spin | Radius |
|---|---|---|---|
| +1 | 2 | N/A | 67 pm |
| +1 | 4 | N/A | 100 pm |
| +1 | 4 | N/A | 102 pm |
| +1 | 5 | N/A | 109.00000000000001 pm |
| +1 | 6 | N/A | 114.99999999999999 pm |
| +1 | 7 | N/A | 122 pm |
| +1 | 8 | N/A | 128 pm |
| +2 | 4 | N/A | 79 pm |
| +2 | 6 | N/A | 94 pm |
| +3 | 4 | N/A | 67 pm |
Verbindungen
Isotope (2)
| Massenzahl | Atommasse (u) | Natürliche Häufigkeit | Halbwertszeit | Zerfallsart | |
|---|---|---|---|---|---|
| 107 Stabil | 106,9050916 ± 0,0000026 | 51,8390% ± 0,0080% | Stabil | stable | |
| 109 Stabil | 108,9047553 ± 0,0000014 | 48,1610% ± 0,0080% | Stabil | stable |
Spektrallinien
50 von 125 angezeigt. Standardmäßig werden nur Spektrallinien mit gemessener Intensität angezeigt.
| Wellenlänge (nm) | Intensität | Ionenstufe | Typ | Übergang | Genauigkeit | Quelle | |
|---|---|---|---|---|---|---|---|
| 562.2482 nm | 21000 | Ag II | emission | 4d9.(2D<5/2>).5d 2[7/2] → 4d9.(2D<5/2>).4f 2[9/2]* | Gemessen | NIST | |
| 540.01037 nm | 20000 | Ag II | emission | 4d9.(2D<5/2>).5d 2[9/2] → 4d9.(2D<5/2>).4f 2[11/2]* | Gemessen | NIST | |
| 540.31323 nm | 15000 | Ag II | emission | 4d9.(2D<5/2>).5d 2[9/2] → 4d9.(2D<5/2>).4f 2[11/2]* | Gemessen | NIST | |
| 555.19264 nm | 12000 | Ag II | emission | 4d9.(2D<5/2>).5d 2[7/2] → 4d9.(2D<5/2>).4f 2[9/2]* | Gemessen | NIST | |
| 548.81562 nm | 8300 | Ag II | emission | 4d9.(2D<5/2>).5d 2[5/2] → 4d9.(2D<5/2>).4f 2[7/2]* | Gemessen | NIST | |
| 558.97829 nm | 4200 | Ag II | emission | 4d9.(2D<5/2>).5d 2[5/2] → 4d9.(2D<5/2>).4f 2[7/2]* | Gemessen | NIST | |
| 534.00267 nm | 2900 | Ag II | emission | 4d9.(2D<5/2>).5d 2[9/2] → 4d9.(2D<5/2>).4f 2[9/2]* | Gemessen | NIST | |
| 554.32121 nm | 2700 | Ag II | emission | 4d9.(2D<5/2>).5d 2[5/2] → 4d8.(3F).5s.5p.(3P*) 1F* | Gemessen | NIST | |
| 557.96782 nm | 2400 | Ag II | emission | 4d9.(2D<5/2>).5d 2[7/2] → 4d9.(2D<5/2>).4f 2[7/2]* | Gemessen | NIST | |
| 549.38302 nm | 2300 | Ag II | emission | 4d9.(2D<5/2>).5d 2[5/2] → 4d9.(2D<5/2>).4f 2[7/2]* | Gemessen | NIST | |
| 555.81412 nm | 2300 | Ag II | emission | 4d9.(2D<5/2>).5d 2[5/2] → 4d9.(2D<5/2>).4f 2[3/2]* | Gemessen | NIST | |
| 557.38257 nm | 2300 | Ag II | emission | 4d9.(2D<5/2>).5d 2[7/2] → 4d9.(2D<5/2>).4f 2[7/2]* | Gemessen | NIST | |
| 542.40509 nm | 2200 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[3/2]* | Gemessen | NIST | |
| 541.08117 nm | 1800 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[3/2]* | Gemessen | NIST | |
| 514.28157 nm | 1700 | Ag II | emission | 4d9.(2D<5/2>).5d 2[1/2] → 4d9.(2D<5/2>).4f 2[1/2]* | Gemessen | NIST | |
| 558.84183 nm | 1700 | Ag II | emission | 4d9.(2D<5/2>).5d 2[7/2] → 4d9.(2D<5/2>).4f 2[9/2]* | Gemessen | NIST | |
| 536.27883 nm | 1600 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[7/2]* | Gemessen | NIST | |
| 539.24682 nm | 1500 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[5/2]* | Gemessen | NIST | |
| 547.86589 nm | 1500 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[1/2]* | Gemessen | NIST | |
| 533.25049 nm | 1300 | Ag II | emission | 4d9.(2D<5/2>).5d 2[9/2] → 4d9.(2D<5/2>).4f 2[7/2]* | Gemessen | NIST | |
| 531.24574 nm | 1200 | Ag II | emission | 4d9.(2D<5/2>).5d 2[9/2] → 4d9.(2D<5/2>).4f 2[9/2]* | Gemessen | NIST | |
| 520.9078 nm | 1000 | Ag I | emission | 4d10.5p 2P* → 4d10.5d 2D | Gemessen | NIST | |
| 546.54853 nm | 1000 | Ag I | emission | 4d10.5p 2P* → 4d10.5d 2D | Gemessen | NIST | |
| 441.196 nm | 830 | Ag II | emission | 4d9.(2D<5/2>).6p 2[7/2]* → 4d9.(2D<5/2>).8s 2[5/2] | Gemessen | NIST | |
| 541.19338 nm | 740 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[3/2]* | Gemessen | NIST | |
| 513.72469 nm | 720 | Ag II | emission | 4d9.(2D<5/2>).5d 2[1/2] → 4d8.(3F).5s.5p.(3P*) 1D* | Gemessen | NIST | |
| 421.09542 nm | 700 | Ag I | emission | 4d10.5p 2P* → 4d10.6d 2D | Gemessen | NIST | |
| 431.959 nm | 630 | Ag II | emission | 4d9.(2D<5/2>).6p 2[7/2]* → 4d9.(2D<5/2>).8s 2[5/2] | Gemessen | NIST | |
| 443.063 nm | 580 | Ag II | emission | 4d9.(2D<3/2>).6p 2[5/2]* → 4d9.(2D<3/2>).8s 2[3/2] | Gemessen | NIST | |
| 408.59155 nm | 470 | Ag II | emission | 4d9.(2D<3/2>).5p 2[5/2]* → 4d8.5s2 1G | Gemessen | NIST | |
| 449.492 nm | 410 | Ag II | emission | 4d9.(2D<5/2>).6p 2[5/2]* → 4d9.(2D<5/2>).8s 2[5/2] | Gemessen | NIST | |
| 453.041 nm | 410 | Ag II | emission | 4d9.(2D<5/2>).6p 2[5/2]* → 4d9.(2D<5/2>).8s 2[5/2] | Gemessen | NIST | |
| 405.5475 nm | 400 | Ag I | emission | 4d10.5p 2P* → 4d10.6d 2D | Gemessen | NIST | |
| 431.354 nm | 290 | Ag II | emission | 4d9.(2D<3/2>).6p 2[5/2]* → 4d9.(2D<3/2>).8s 2[3/2] | Gemessen | NIST | |
| 436.409 nm | 290 | Ag II | emission | 4d9.(2D<3/2>).6p 2[1/2]* → 4d9.(2D<3/2>).8s 2[3/2] | Gemessen | NIST | |
| 444.917 nm | 290 | Ag II | emission | 4d9.(2D<3/2>).6p 2[3/2]* → 4d9.(2D<3/2>).8s 2[3/2] | Gemessen | NIST | |
| 478.83966 nm | 260 | Ag II | emission | 4d9.(2D<3/2>).5p 2[3/2]* → 4d8.5s2 1D | Gemessen | NIST | |
| 418.547499 nm | 250 | Ag II | emission | 4d9.(2D<3/2>).5p 2[5/2]* → 4d8.5s2 1D | Gemessen | NIST | |
| 723.9381 nm | 250 | Ag II | emission | 4d9.(2D<5/2>).6s 2[5/2] → 4d8.(3F).5s.5p.(3P*) 5G* | Gemessen | NIST | |
| 398.51904 nm | 220 | Ag II | emission | 4d9.(2D<5/2>).5p 2[3/2]* → 4d8.5s2 3P | Gemessen | NIST | |
| 433.316 nm | 210 | Ag II | emission | 4d9.(2D<5/2>).6p 2[7/2]* → 4d9.(2D<5/2>).8s 2[5/2] | Gemessen | NIST | |
| 447.909 nm | 210 | Ag II | emission | 4d9.(2D<5/2>).6p 2[3/2]* → 4d9.(2D<5/2>).8s 2[5/2] | Gemessen | NIST | |
| 451.558 nm | 210 | Ag II | emission | 4d9.(2D<5/2>).6p 2[5/2]* → 4d9.(2D<5/2>).8s 2[5/2] | Gemessen | NIST | |
| 381.09396 nm | 200 | Ag I | emission | 4d10.5p 2P* → 4d10.7d 2D | Gemessen | NIST | |
| 699.906 nm | 200 | Ag II | emission | 4d8.(3F).5s.5p.(3P*) 5D* → 4d9.(2D<3/2>).7s 2[3/2] | Gemessen | NIST | |
| 392.01238 nm | 180 | Ag II | emission | 4d9.(2D<5/2>).5p 2[3/2]* → 4d8.5s2 3P | Gemessen | NIST | |
| 462.00355 nm | 170 | Ag II | emission | 4d9.(2D<3/2>).5p 2[5/2]* → 4d8.5s2 1D | Gemessen | NIST | |
| 394.9435 nm | 160 | Ag II | emission | 4d9.(2D<5/2>).5p 2[3/2]* → 4d8.5s2 3P | Gemessen | NIST | |
| 502.73432 nm | 160 | Ag II | emission | 4d9.(2D<3/2>).5p 2[3/2]* → 4d8.5s2 1D | Gemessen | NIST | |
| 390.930327 nm | 140 | Ag II | emission | 4d9.(2D<5/2>).5p 2[5/2]* → 4d8.5s2 1D | Gemessen | NIST |
Erweiterte Eigenschaften
Kovalente Radien (Erweitert)
- Kovalenzradius (Pyykkö)
- 128 pm
- Kovalenzradius (Pyykkö, doppelt)
- 139 pm
- Kovalenzradius (Pyykkö, dreifach)
- 137 pm
- Kovalenzradius (Bragg)
- 177 pm
Van-der-Waals-Radien
- Batsanov
- 210 pm
- Alvarez
- 253 pm
- UFF
- 314,8 pm
- MM3
- 243 pm
Atom- & Metallische Radien
- Atomradius (Rahm)
- 225 pm
- Metallradius (C12)
- 144 pm
Nummerierungsskalen
- Mendeleev
- 72
- Pettifor
- 71
- Glawe
- 67
Elektronegativitätsskalen
- Ghosh
- 0
- Miedema
- 4
- Gunnarsson–Lundqvist
- 4
- Robles–Bartolotti
- 3
Polarisierbarkeit & Dispersion
- Dipolpolarisierbarkeit
- 55 a.u.
- Dipolpolarisierbarkeit (Uns.)
- 8 a.u.
- C₆ (Gould–Bučko)
- 341 Ha·Bohr6
Miedema-Parameter
- Miedema-Molvolumen
- 10,25 cm3/mol
- Miedema-Elektronendichte
- 3
Lieferrisiko & Wirtschaftlichkeit
- Produktionskonzentration
- 19
- Relatives Lieferrisiko
- 6
- Reservenverteilung
- 23
- Politische Stabilität (Top-Produzent)
- 23
- Politische Stabilität (Top-Reserven)
- 20
Phasenübergänge & Allotrope
| Schmelzpunkt | 1234,93 K |
| Siedepunkt | 2435,15 K |
| Kritischer Punkt (Temperatur) | 6410,15 K |
Oxidationszustands-Kategorien
Erweiterte Referenzdaten
Abschirmkonstanten (10)
| n | Orbital | σ |
|---|---|---|
| 1 | s | 0,9577 |
| 2 | p | 4,0806 |
| 2 | s | 12,3658 |
| 3 | d | 14,4602 |
| 3 | p | 17,1914 |
| 3 | s | 16,9688 |
| 4 | d | 32,2372 |
| 4 | p | 28,4376 |
| 4 | s | 27,1352 |
| 5 | s | 40,2445 |
Kristallradien-Details (11)
| Ladung | CN | Spin | rcrystal (pm) | Herkunft |
|---|---|---|---|---|
| 1 | II | 81 | ||
| 1 | IV | 114 | calculated, | |
| 1 | IVSQ | 116 | ||
| 1 | V | 123 | calculated, | |
| 1 | VI | 129 | calculated, | |
| 1 | VII | 136 | ||
| 1 | VIII | 142 | ||
| 2 | IVSQ | 93 | ||
| 2 | VI | 108 | ||
| 3 | IVSQ | 81 |
Isotopenzerfallsarten (68)
| Isotop | Modus | Intensität |
|---|---|---|
| 92 | B+ | — |
| 92 | p | — |
| 93 | p | — |
| 93 | B+ | — |
| 93 | B+p | — |
| 94 | B+ | 100% |
| 94 | B+p | 0,2% |
| 95 | B+ | 100% |
| 95 | B+p | 2,3% |
| 96 | B+ | 100% |
Röntgenstreufaktoren (508)
| Energie (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 1,18566 |
| 10,1617 | — | 1,22941 |
| 10,3261 | — | 1,27478 |
| 10,4931 | — | 1,32182 |
| 10,6628 | — | 1,38215 |
| 10,8353 | — | 1,45541 |
| 11,0106 | — | 1,53256 |
| 11,1886 | — | 1,61379 |
| 11,3696 | — | 1,69933 |
| 11,5535 | — | 1,78755 |
Zusätzliche Daten
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
7.5×10-2 milligrams per kilogram
Referenzen (1)
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
4×10-5 milligrams per liter
Referenzen (1)
Sources
Sources of this element.
Silver occurs natively and in ores such as argentite (Ag2S) and horn silver (AgCl); lead, lead-zinc, copper, gold, and copper-nickel ores are principal sources. Mexico, Canada, Peru, and the U.S. are the principal silver producers in the western hemisphere.
Referenzen (1)
- [6] Silver https://periodic.lanl.gov/47.shtml
Production
Production of this element (from raw materials or other compounds containing the element).
Silver is also recovered during electrolytic refining of copper. Commercial fine silver contains at least 99.9% silver. Purities of 99.999+% are available commercially.
Referenzen (1)
- [6] Silver https://periodic.lanl.gov/47.shtml
Isotopes in Forensic Science and Anthropology
Information on the use of this element's isotopes in forensic science and anthropology.
Silver isotope-amount ratiosn(107Ag)/n(109Ag) along with isotope-amount ratios of copper n(65Cu)/n(63Cu), and isotope-amount ratios of lead (n(206Pb)/n(204Pb), n(207Pb)/n(204Pb) and n(208Pb)/n(204Pb)) have been used to determine origins of European coins and information on the flow of goods in the world market over time (Fig. IUPAC.47.1). Metals from Peru and Mexico and those from European mining have distinct isotopic signatures that enable the origin of the metal to be determined by examining the isotopic compositions of silver, copper, and lead in the coins. Abundant silver sources, mined in Mexico and Peru in the 16 th century, were used to mint coins, but they were not a major influence in the European coin market until the 18 th century (Fig. IUPAC.47.1) [237] A. M. Desaulty, P. Telouk, E. Albalat, F. Albarede. Proc. Natl. Acad. Sci.108, 9002 (2011)..
Referenzen (2)
- [237] A. M. Desaulty, P. Telouk, E. Albalat, F. Albarede. Proc. Natl. Acad. Sci.108, 9002 (2011).
- [4] IUPAC Periodic Table of the Elements and Isotopes (IPTEI) https://doi.org/10.1515/pac-2015-0703
Referenzen
(9)
Data deposited in or computed by PubChem
The half-life and atomic mass data was provided by the Atomic Mass Data Center at the International Atomic Energy Agency.
Element data are cited from the Atomic weights of the elements (an IUPAC Technical Report). The IUPAC periodic table of elements can be found at https://iupac.org/what-we-do/periodic-table-of-elements/. Additional information can be found within IUPAC publication doi:10.1515/pac-2015-0703 Copyright © 2020 International Union of Pure and Applied Chemistry.
The information are cited from Pure Appl. Chem. 2018; 90(12): 1833-2092, https://doi.org/10.1515/pac-2015-0703.
Thomas Jefferson National Accelerator Facility (Jefferson Lab) is one of 17 national laboratories funded by the U.S. Department of Energy. The lab's primary mission is to conduct basic research of the atom's nucleus using the lab's unique particle accelerator, known as the Continuous Electron Beam Accelerator Facility (CEBAF). For more information visit https://www.jlab.org/
The periodic table at the LANL (Los Alamos National Laboratory) contains basic element information together with the history, source, properties, use, handling and more. The provenance data may be found from the link under the source name.
The periodic table contains NIST's critically-evaluated data on atomic properties of the elements. The provenance data that include data for atomic spectroscopy, X-ray and gamma ray, radiation dosimetry, nuclear physics, and condensed matter physics may be found from the link under the source name. Ref: https://www.nist.gov/pml/atomic-spectra-database
This section provides all form of data related to element Silver.
The element property data was retrieved from publications.