Silver (Ag)
transition-metalSolid
표준 원자량
107.8682 u전자 배치
[Kr] 5s1 4d10녹는점
961.78 °C끓는점
2161.85 °C밀도
1.0501e+4 kg/m³산화 상태
−2, −1, 0, +1, +2, +3전기 음성도(Pauling)
1.93제1 이온화 에너지
7.576234 eV발견 연도
해당 없음원자 반지름
160 pm상세 정보
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.
이미지
특성
물리적 특성
- 원자 반지름(경험값)
- 160 pm 모든 원소의 원자 반지름(경험값) 비교 →
- 공유 결합 반지름
- 145 pm 모든 원소의 공유 결합 반지름 비교 →
- 반데르발스 반지름
- 172 pm 모든 원소의 반데르발스 반지름 비교 →
- 금속 반지름
- 134 pm 모든 원소의 금속 반지름 비교 →
- 밀도
- 1.0501 × 104 kg/m³ 모든 원소의 밀도 비교 →
- 몰 부피
- 0.0103 L/mol
- STP에서의 상
- 고체 모든 원소의 STP에서의 상 비교 →
- 녹는점
- 961.78 °C 모든 원소의 녹는점 비교 →
- 끓는점
- 2161.85 °C 모든 원소의 끓는점 비교 →
- 열전도율
- 429 W/(m·K) 모든 원소의 열전도율 비교 →
- 비열
- 0.235 J/(g·K) 모든 원소의 비열 비교 →
- 몰 열용량
- 25.35 J/(mol·K) 모든 원소의 몰 열용량 비교 →
- 결정 구조
- 면심 입방 모든 원소의 결정 구조 비교 →
화학적 특성
- 전기 음성도(Pauling)
- 1.93 모든 원소의 전기 음성도(Pauling) 비교 →
- 전기 음성도(Allen)
- 1.87
- 전자 친화도
- 1.302 eV
- 제1 이온화 에너지
- 7.576234 eV 모든 원소의 제1 이온화 에너지 비교 →
- 제2 이온화 에너지
- 21.484474 eV 모든 원소의 제2 이온화 에너지 비교 →
- 제3 이온화 에너지
- 34.80012 eV 모든 원소의 제3 이온화 에너지 비교 →
- 제4 이온화 에너지
- 49.000169 eV 모든 원소의 제4 이온화 에너지 비교 →
- 제5 이온화 에너지
- 65.000224 eV 모든 원소의 제5 이온화 에너지 비교 →
- 산화 상태
- −2, −1, 0, +1, +2, +3 모든 원소의 산화 상태 비교 →
- 원자가 전자
- 11 모든 원소의 원자가 전자 비교 →
- 전자 배치
- [Kr] 5s1 4d10
열역학적 특성
- 임계점(온도)
- 6137 °C
- 융해열
- 0.11690936 eV 모든 원소의 융해열 비교 →
- 기화열
- 2.597295 eV 모든 원소의 기화열 비교 →
- 승화열
- 2.952791 eV
- 원자화열
- 2.952791 eV
- 원자화 엔탈피
- 2.952791 eV
핵 특성
- 양성자 수
- 47 모든 원소의 양성자 수 비교 →
- 중성자 수
- 60 모든 원소의 중성자 수 비교 →
- 알려진 동위원소 수
- 42 모든 원소의 알려진 동위원소 수 비교 →
- 안정 동위원소 수
- 2 모든 원소의 안정 동위원소 수 비교 →
- 가장 안정한 동위원소
- Ag-107
존재비
- 존재비(지각)
- 0.075 mg/kg 모든 원소의 존재비(지각) 비교 →
- 존재비(해양)
- 4 × 10−5 mg/L 모든 원소의 존재비(해양) 비교 →
결정 구조
- 격자 상수 a
- 409 pm
전자 구조
- 전자껍질별 전자 수
- 2, 8, 18, 18, 1 모든 원소의 전자껍질별 전자 수 비교 →
식별자
- CAS 등록 번호
- 7440-22-4 모든 원소의 CAS 등록 번호 비교 →
- 항 기호
- 2S1/2
- InChI
- InChI=1S/Ag
- InChI 키
- BQCADISMDOOEFD-UHFFFAOYSA-N
전자 배치 측정값
Ag: 4d¹⁰ 5s¹[Kr] 4d¹⁰ 5s¹1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s¹원자 모형
동위원소에 따라 중성자 수, 질량, 안정성은 달라지지만, 중성 원자의 전자 배치는 달라지지 않습니다.
개략적인 원자 모형이며 실제 비율과 다릅니다.
원자 지문
방출 / 흡수 스펙트럼
동위원소 분포
| 질량수 | 원자 질량(u) | 천연 존재비 | 반감기 |
|---|---|---|---|
| 107 안정 | 106.9050916 ± 0.0000026 | 51.8390% | 안정 |
| 109 안정 | 108.9047553 ± 0.0000014 | 48.1610% | 안정 |
상 / 상태
이유: 녹는점(961.78 °C)보다 936.8 °C 낮음
개략도이며 실제 비율과 다름
상전이점
전이 에너지
녹는점에서 1 mol을 녹이는 데 필요한 에너지
끓는점에서 1 mol을 기화시키는 데 필요한 에너지
승화점에서 1 mol을 승화시키는 데 필요한 에너지
밀도
표준 조건에서
표준 조건에서
심화
원자 스펙트럼
전체 47개 중 10개를 표시합니다. 이온 전하순으로 정렬되었습니다(오름차순).
보유 스펙트럼선 데이터 ?
| 이온 | 전하 | 총 스펙트럼선 수 | 전이 확률 | 준위 표기 |
|---|---|---|---|---|
| Ag I | 0 | 103 | 7 | 97 |
| Ag II | +1 | 455 | 237 | 455 |
| Ag III | +2 | 140 | 0 | 0 |
보유 에너지 준위 데이터 ?
| 이온 | 전하 | 준위 |
|---|---|---|
| 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 |
이온 반지름
전체 11개 중 10개를 표시합니다.
| 전하 | 배위 | 스핀 | 반지름 |
|---|---|---|---|
| +1 | 2 | 해당 없음 | 67 pm |
| +1 | 4 | 해당 없음 | 100 pm |
| +1 | 4 | 해당 없음 | 102 pm |
| +1 | 5 | 해당 없음 | 109.00000000000001 pm |
| +1 | 6 | 해당 없음 | 114.99999999999999 pm |
| +1 | 7 | 해당 없음 | 122 pm |
| +1 | 8 | 해당 없음 | 128 pm |
| +2 | 4 | 해당 없음 | 79 pm |
| +2 | 6 | 해당 없음 | 94 pm |
| +3 | 4 | 해당 없음 | 67 pm |
화합물
동위원소 (2)
| 질량수 | 원자 질량(u) | 천연 존재비 | 반감기 | 붕괴 방식 | |
|---|---|---|---|---|---|
| 107 안정 | 106.9050916 ± 0.0000026 | 51.8390% ± 0.0080% | 안정 | stable | |
| 109 안정 | 108.9047553 ± 0.0000014 | 48.1610% ± 0.0080% | 안정 | stable |
스펙트럼선
전체 125개 중 50개를 표시합니다. 기본적으로 세기가 측정된 스펙트럼선만 표시됩니다.
| 파장(nm) | 세기 | 이온화 단계 | 유형 | 전이 | 정확도 | 출처 | |
|---|---|---|---|---|---|---|---|
| 562.2482 nm | 21000 | Ag II | emission | 4d9.(2D<5/2>).5d 2[7/2] → 4d9.(2D<5/2>).4f 2[9/2]* | 측정값 | NIST | |
| 540.01037 nm | 20000 | Ag II | emission | 4d9.(2D<5/2>).5d 2[9/2] → 4d9.(2D<5/2>).4f 2[11/2]* | 측정값 | NIST | |
| 540.31323 nm | 15000 | Ag II | emission | 4d9.(2D<5/2>).5d 2[9/2] → 4d9.(2D<5/2>).4f 2[11/2]* | 측정값 | NIST | |
| 555.19264 nm | 12000 | Ag II | emission | 4d9.(2D<5/2>).5d 2[7/2] → 4d9.(2D<5/2>).4f 2[9/2]* | 측정값 | NIST | |
| 548.81562 nm | 8300 | Ag II | emission | 4d9.(2D<5/2>).5d 2[5/2] → 4d9.(2D<5/2>).4f 2[7/2]* | 측정값 | NIST | |
| 558.97829 nm | 4200 | Ag II | emission | 4d9.(2D<5/2>).5d 2[5/2] → 4d9.(2D<5/2>).4f 2[7/2]* | 측정값 | NIST | |
| 534.00267 nm | 2900 | Ag II | emission | 4d9.(2D<5/2>).5d 2[9/2] → 4d9.(2D<5/2>).4f 2[9/2]* | 측정값 | NIST | |
| 554.32121 nm | 2700 | Ag II | emission | 4d9.(2D<5/2>).5d 2[5/2] → 4d8.(3F).5s.5p.(3P*) 1F* | 측정값 | NIST | |
| 557.96782 nm | 2400 | Ag II | emission | 4d9.(2D<5/2>).5d 2[7/2] → 4d9.(2D<5/2>).4f 2[7/2]* | 측정값 | NIST | |
| 549.38302 nm | 2300 | Ag II | emission | 4d9.(2D<5/2>).5d 2[5/2] → 4d9.(2D<5/2>).4f 2[7/2]* | 측정값 | NIST | |
| 555.81412 nm | 2300 | Ag II | emission | 4d9.(2D<5/2>).5d 2[5/2] → 4d9.(2D<5/2>).4f 2[3/2]* | 측정값 | NIST | |
| 557.38257 nm | 2300 | Ag II | emission | 4d9.(2D<5/2>).5d 2[7/2] → 4d9.(2D<5/2>).4f 2[7/2]* | 측정값 | NIST | |
| 542.40509 nm | 2200 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[3/2]* | 측정값 | NIST | |
| 541.08117 nm | 1800 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[3/2]* | 측정값 | NIST | |
| 514.28157 nm | 1700 | Ag II | emission | 4d9.(2D<5/2>).5d 2[1/2] → 4d9.(2D<5/2>).4f 2[1/2]* | 측정값 | NIST | |
| 558.84183 nm | 1700 | Ag II | emission | 4d9.(2D<5/2>).5d 2[7/2] → 4d9.(2D<5/2>).4f 2[9/2]* | 측정값 | NIST | |
| 536.27883 nm | 1600 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[7/2]* | 측정값 | NIST | |
| 539.24682 nm | 1500 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[5/2]* | 측정값 | NIST | |
| 547.86589 nm | 1500 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[1/2]* | 측정값 | NIST | |
| 533.25049 nm | 1300 | Ag II | emission | 4d9.(2D<5/2>).5d 2[9/2] → 4d9.(2D<5/2>).4f 2[7/2]* | 측정값 | NIST | |
| 531.24574 nm | 1200 | Ag II | emission | 4d9.(2D<5/2>).5d 2[9/2] → 4d9.(2D<5/2>).4f 2[9/2]* | 측정값 | NIST | |
| 520.9078 nm | 1000 | Ag I | emission | 4d10.5p 2P* → 4d10.5d 2D | 측정값 | NIST | |
| 546.54853 nm | 1000 | Ag I | emission | 4d10.5p 2P* → 4d10.5d 2D | 측정값 | NIST | |
| 441.196 nm | 830 | Ag II | emission | 4d9.(2D<5/2>).6p 2[7/2]* → 4d9.(2D<5/2>).8s 2[5/2] | 측정값 | NIST | |
| 541.19338 nm | 740 | Ag II | emission | 4d9.(2D<5/2>).5d 2[3/2] → 4d9.(2D<5/2>).4f 2[3/2]* | 측정값 | NIST | |
| 513.72469 nm | 720 | Ag II | emission | 4d9.(2D<5/2>).5d 2[1/2] → 4d8.(3F).5s.5p.(3P*) 1D* | 측정값 | NIST | |
| 421.09542 nm | 700 | Ag I | emission | 4d10.5p 2P* → 4d10.6d 2D | 측정값 | NIST | |
| 431.959 nm | 630 | Ag II | emission | 4d9.(2D<5/2>).6p 2[7/2]* → 4d9.(2D<5/2>).8s 2[5/2] | 측정값 | NIST | |
| 443.063 nm | 580 | Ag II | emission | 4d9.(2D<3/2>).6p 2[5/2]* → 4d9.(2D<3/2>).8s 2[3/2] | 측정값 | NIST | |
| 408.59155 nm | 470 | Ag II | emission | 4d9.(2D<3/2>).5p 2[5/2]* → 4d8.5s2 1G | 측정값 | NIST | |
| 449.492 nm | 410 | Ag II | emission | 4d9.(2D<5/2>).6p 2[5/2]* → 4d9.(2D<5/2>).8s 2[5/2] | 측정값 | NIST | |
| 453.041 nm | 410 | Ag II | emission | 4d9.(2D<5/2>).6p 2[5/2]* → 4d9.(2D<5/2>).8s 2[5/2] | 측정값 | NIST | |
| 405.5475 nm | 400 | Ag I | emission | 4d10.5p 2P* → 4d10.6d 2D | 측정값 | NIST | |
| 431.354 nm | 290 | Ag II | emission | 4d9.(2D<3/2>).6p 2[5/2]* → 4d9.(2D<3/2>).8s 2[3/2] | 측정값 | NIST | |
| 436.409 nm | 290 | Ag II | emission | 4d9.(2D<3/2>).6p 2[1/2]* → 4d9.(2D<3/2>).8s 2[3/2] | 측정값 | NIST | |
| 444.917 nm | 290 | Ag II | emission | 4d9.(2D<3/2>).6p 2[3/2]* → 4d9.(2D<3/2>).8s 2[3/2] | 측정값 | NIST | |
| 478.83966 nm | 260 | Ag II | emission | 4d9.(2D<3/2>).5p 2[3/2]* → 4d8.5s2 1D | 측정값 | NIST | |
| 418.547499 nm | 250 | Ag II | emission | 4d9.(2D<3/2>).5p 2[5/2]* → 4d8.5s2 1D | 측정값 | NIST | |
| 723.9381 nm | 250 | Ag II | emission | 4d9.(2D<5/2>).6s 2[5/2] → 4d8.(3F).5s.5p.(3P*) 5G* | 측정값 | NIST | |
| 398.51904 nm | 220 | Ag II | emission | 4d9.(2D<5/2>).5p 2[3/2]* → 4d8.5s2 3P | 측정값 | NIST | |
| 433.316 nm | 210 | Ag II | emission | 4d9.(2D<5/2>).6p 2[7/2]* → 4d9.(2D<5/2>).8s 2[5/2] | 측정값 | NIST | |
| 447.909 nm | 210 | Ag II | emission | 4d9.(2D<5/2>).6p 2[3/2]* → 4d9.(2D<5/2>).8s 2[5/2] | 측정값 | NIST | |
| 451.558 nm | 210 | Ag II | emission | 4d9.(2D<5/2>).6p 2[5/2]* → 4d9.(2D<5/2>).8s 2[5/2] | 측정값 | NIST | |
| 381.09396 nm | 200 | Ag I | emission | 4d10.5p 2P* → 4d10.7d 2D | 측정값 | NIST | |
| 699.906 nm | 200 | Ag II | emission | 4d8.(3F).5s.5p.(3P*) 5D* → 4d9.(2D<3/2>).7s 2[3/2] | 측정값 | NIST | |
| 392.01238 nm | 180 | Ag II | emission | 4d9.(2D<5/2>).5p 2[3/2]* → 4d8.5s2 3P | 측정값 | NIST | |
| 462.00355 nm | 170 | Ag II | emission | 4d9.(2D<3/2>).5p 2[5/2]* → 4d8.5s2 1D | 측정값 | NIST | |
| 394.9435 nm | 160 | Ag II | emission | 4d9.(2D<5/2>).5p 2[3/2]* → 4d8.5s2 3P | 측정값 | NIST | |
| 502.73432 nm | 160 | Ag II | emission | 4d9.(2D<3/2>).5p 2[3/2]* → 4d8.5s2 1D | 측정값 | NIST | |
| 390.930327 nm | 140 | Ag II | emission | 4d9.(2D<5/2>).5p 2[5/2]* → 4d8.5s2 1D | 측정값 | NIST |
확장 특성
공유 결합 반지름(확장)
- 공유 결합 반지름(Pyykkö)
- 128 pm
- 공유 결합 반지름(Pyykkö, 이중 결합)
- 139 pm
- 공유 결합 반지름(Pyykkö, 삼중 결합)
- 137 pm
- 공유 결합 반지름(Bragg)
- 177 pm
반데르발스 반지름
- Batsanov
- 210 pm
- Alvarez
- 253 pm
- UFF
- 314.8 pm
- MM3
- 243 pm
원자 및 금속 반지름
- 원자 반지름(Rahm)
- 225 pm
- 금속 반지름(C12)
- 144 pm
번호 척도
- Mendeleev
- 72
- Pettifor
- 71
- Glawe
- 67
전기 음성도 척도
- Ghosh
- 0
- Miedema
- 4
- Gunnarsson–Lundqvist
- 4
- Robles–Bartolotti
- 3
분극률 및 분산
- 쌍극자 분극률
- 55 a.u.
- 쌍극자 분극률(불확도)
- 8 a.u.
- C₆ (Gould–Bučko)
- 341 Ha·Bohr6
미데마 매개변수
- 미데마 몰 부피
- 10.25 cm3/mol
- 미데마 전자 밀도
- 3
공급 위험 및 경제성
- 생산 집중도
- 19
- 상대적 공급 위험
- 6
- 매장량 분포
- 23
- 정치적 안정성(최대 생산국)
- 23
- 정치적 안정성(최대 매장국)
- 20
상전이 및 동소체
| 녹는점 | 1234.93 K |
| 끓는점 | 2435.15 K |
| 임계점(온도) | 6410.15 K |
산화 상태 분류
심화 참고 데이터
차폐 상수 (10)
| n | 오비탈 | 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 |
결정 반지름 상세 정보 (11)
| 전하 | CN | 스핀 | rcrystal (pm) | 기원 |
|---|---|---|---|---|
| 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 |
동위원소 붕괴 방식 (68)
| 동위원소 | 모드 | 세기 |
|---|---|---|
| 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% |
X선 산란 인자 (508)
| 에너지 (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 |
추가 데이터
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
7.5×10-2 milligrams per kilogram
참고 문헌 (1)
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
4×10-5 milligrams per liter
참고 문헌 (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.
참고 문헌 (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.
참고 문헌 (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)..
참고 문헌 (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
참고 문헌
(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.