Iridium (Ir)
transition-metalSolid
Masse atomique relative standard
192,217 uConfiguration électronique
[Xe] 6s2 4f14 5d7Point de fusion
2445,85 °CPoint d’ébullition
4427,85 °CMasse volumique
2,25622e+4 kg/m³États d’oxydation
−3, −2, −1, +1, +2, +3, +4, +5, +6, +7, +8, +9Électronégativité (Pauling)
2,2Énergie d’ionisation (1re)
8,96702 eVAnnée de découverte
1803Rayon atomique
135 pmDétails
Iridium is a very dense platinum-group transition metal with exceptional resistance to corrosion and high-temperature attack. It occurs naturally mainly with platinum-group minerals and in nickel-copper sulfide ores. Chemically it forms robust complexes, especially in oxidation states +3 and +4, and it is notable for the global iridium anomaly associated with the Cretaceous-Paleogene boundary impact layer.
Iridium, a metal of the platinum family, is white (similar to platinum) but with a slight yellowish cast. Because iridium is very hard and brittle, it is hard to machine, form, or work.
It is the most corrosion-resistant metal known, and was used in making the standard meter bar of Paris, which is a 90 percent platinum and 10 percent iridium alloy. This meter bar was replaced in 1960 as a fundamental unit of length (see Krypton).
Iridium is not attacked by any of the acids nor by aqua regia, but is attacked by molten salts, such as NaCl and NaCN. The specific gravity of iridium is to osmium's specific gravity. Calculations of the densities of iridium and osmium from the space lattices give values of 22.65 and 22.61 g/cm^3, respectively. These values may be more reliable than actual physical measurements for determining which element is heavier.
The name derives from the Latin Iris, the Greek goddess of rainbows, because of the variety of colours in the element's salt solutions. Iridium and osmium were both discovered in a crude platinum ore in 1803 by the English chemist Smithson Tennant. Iridium was discovered independently by the French chemist H. V. Collet-Descotils, who actually published his paper one month before Tennant, but Tennant is given credit for the discovery, perhaps because he alone also found osmium in the ore.
Iridium and osmium were discovered at the same time by the British chemist Smithson Tennant in 1803. Iridium and osmium were identified in the black residue remaining after dissolving platinum ore with aqua regia, a mixture of 25% nitric acid (HNO3) and 75% hydrochloric acid (HCl). Today, iridium is still obtained from platinum ores and as a by-product of mining nickel.
From the Latin word iris meaning rainbow. Tennant discovered iridium in 1803 in the residue left when crude platinum is dissolved by aqua regia. The name iridium is appropriate because its salts are highly colored.
Pure iridium is a hard, brittle, silvery-white metal with a high luster. It remains bright in air under ordinary conditions and has an unusually high melting point. Bulk metal is difficult to machine because of its hardness and brittleness.
Iridium is used where chemical durability and high-temperature strength justify its cost. Major applications include crucibles for growing oxide crystals, spark-plug electrodes, electrical contacts, and wear-resistant alloys with platinum or osmium. Iridium coatings and components are used in some aerospace and industrial equipment. Radioisotope thermoelectric generators have used ¹⁹²Ir? No; ¹⁹²Ir is chiefly a gamma source for industrial radiography and some brachytherapy, not an energy source.
Pure iridium is very brittle and is nearly impossible to machine. It is primarily used as a hardening agent for platinum. Platinum-iridium alloys are used to make crucibles and other high temperature equipment. Iridium is also alloyed with osmium to make the tips of fountain pens and compass bearings.
Iridium is the most corrosive resistant metal known. For this reason, the standard meter bar was created from an alloy of 90% platinum and 10% iridium. This bar was replaced as the definition of the meter in 1960 when the meter was redefined in terms of the orange-red spectral line of krypton-86.
A thin, worldwide layer of iridium exists in a layer of sediment that was put down at the end of the Cretaceous period. Since meteors and asteroids contain a higher percentage of iridium than the earth's crust, this iridium enriched layer is seen as evidence that the earth was struck by a large meteor or asteroid at that time. Dust from the impact would have spread around the globe, depositing the iridium. The dust also would have blocked the sun for a time, resulting in the extinction of many plant and animal species, including the dinosaurs.
Although its principal use is as a hardening agent for platinum, iridium is also used to make crucibles and devices requiring high temperatures. It is also used for electrical contacts.
The element forms an alloy with osmium which is used for tipping pens and compass bearings.
Isotopes in Industry
Metallic 192Ir (with a half-life of 74 days) is used as a radiation source in gamma cameras for non-destructive testing of products for manufacturing flaws, such as aircraft parts, boilers, and pipeline welds (Fig. IUPAC.77.1) [274] P. Hayward, D. Currie. “Radiography of welds using seleniuim 75, Ir 192 and x-rays”, in Asia-Pacific Conference on NDT, Auckland, New Zealand (2006)..
Isotopes in Medicine
Metallic 192Ir is used in brachytherapy [188] S. J. Adelstein, F. J. Manning. Isotopes for Medicine and the Life Sciences, pp. 20–25, National Academy Press, Washington DC (1995)., [521] A. Talamo, Y. Gohar. Radioactive Isotope Production for Medical Applications Using Kharkov Electron Driven Subcritical Assembly Facility, ANL-07/18, Argonne National Laboratory Argonne, Illinois (2007)., [522] S. A. Buzdar, M. A. Gadhi, M. A. Rao, N. A. Laghari, M. Anees. J. Pak. Med. Assoc.59, 113 (2009)., [523] T. Genkaa, S. Iwamotoa, E. Juitab, N. Takeuchia. Nucl. Inst. Methods Phys. Res. Section A: Accelerators, Spectrometers, Detectors and Associated Equipment.369, 709 (1996).. 191mIr (with a half-life of 5 s) is used for blood flow imaging (angiography), especially in pediatric populations [524] K. J. Kairemo, M. S. Kestilä, S. Savolainen, O. A. Korhola, J. V. Hiltunen, R. I. Svahn, E. T. Korppi Tommola, F. F. Knapp, C. Brihaye. J. Nucl. Biol. Med.38, 86 (1994)., [525] S. T. Treves, A. B. Packard, L. C. T. Fung. J. Nucl. Med.45, 508 (2004).. The m in the superscript 191mIr indicates a metastable state of the isotope.
Isotopes Used as a Source of Radioactive Isotope(s)
Iridium consists of two stable isotopes (191Ir and 193Ir) from which the radioactive isotopes 192Ir and 195mPt (with a half-life of 4 days) can be produced. Both are used in nuclear medicine. The m in the superscript 195mPt indicates a metastable state of the isotope.
Iridium chemistry is dominated by coordination compounds and oxides rather than simple salts. Common oxidation states are +3 and +4, while lower and higher states occur in organometallic or strongly oxidizing systems. Iridium(IV) oxide, IrO₂, is an electrically conducting oxide used in dimensionally stable anodes and electrochemical research. Hexachloroiridic acid, H₂IrCl₆, and related chloroiridate salts are important refining and precursor compounds. The complex [Ir(ppy)₃] is a representative phosphorescent organoiridium emitter.
See more information at the Iridium compound page.
Massive iridium metal is chemically inert and has low acute toxicity, but finely divided powder can present dust and fire hazards. Soluble iridium salts and organoiridium compounds should be treated as potentially toxic because biological effects are compound-specific and incompletely characterized. The radionuclide ¹⁹²Ir emits penetrating gamma radiation and requires strict shielding and source control.
Iridium is extremely scarce in the crust and is usually dispersed with other platinum-group elements. Natural mobility is low because the metal and many of its minerals are resistant to weathering, although complexing ligands and industrial processing can mobilize small amounts. The sharp enrichment of iridium in some boundary clays is widely used as evidence for extraterrestrial material mixed into sediment.
Iridium is recovered chiefly as a by-product of platinum-group metal refining from nickel-copper sulfide ores and platinum placers. Supply is constrained by the production of the host metals, complex separation chemistry, and limited primary deposits. Demand is small but specialized, so substitution is possible in some electrical and catalytic uses but difficult in high-temperature crucibles and certain corrosion-resistant components. Recycling from spent electrodes, crucibles, and industrial scrap is important because the metal is rare and costly to replace.
Iridium occurs uncombined in nature with platinum and other metals of this family in alluvial deposits. It is recovered as a by-product from the nickel mining industry.
Iridium is a heavy r-process and s-process element made in late stellar evolution and explosive astrophysical environments. In the Solar System it is far more abundant in primitive meteorites than in Earth’s crust, because much of Earth’s original inventory partitioned into the core during differentiation. This siderophile behavior makes iridium a sensitive tracer of meteoritic input.
- Iridium is one of the densest elements, close to osmium in measured density.
- The name comes from Iris, reflecting the varied colors of some iridium salts.
- Iridium metal resists attack by aqua regia better than most noble metals.
- The Cretaceous-Paleogene boundary layer is enriched in iridium relative to ordinary crustal rocks.
- Iridium crucibles are used to grow some high-melting oxide crystals.
- Natural iridium consists mainly of the stable isotopes ¹⁹¹Ir and ¹⁹³Ir.
Images
Propriétés
Propriétés physiques
- Rayon atomique (empirique)
- 135 pm Comparer : Rayon atomique (empirique) de tous les éléments →
- Rayon covalent
- 141 pm Comparer : Rayon covalent de tous les éléments →
- Rayon de van der Waals
- 202 pm Comparer : Rayon de van der Waals de tous les éléments →
- Rayon métallique
- 127 pm Comparer : Rayon métallique de tous les éléments →
- Masse volumique
- 2,25622 × 104 kg/m³ Comparer : Masse volumique de tous les éléments →
- Volume molaire
- 0,00854 L/mol
- Phase aux CNTP
- Solide Comparer : Phase aux CNTP de tous les éléments →
- Point de fusion
- 2445,85 °C Comparer : Point de fusion de tous les éléments →
- Point d’ébullition
- 4427,85 °C Comparer : Point d’ébullition de tous les éléments →
- Conductivité thermique
- 147 W/(m·K) Comparer : Conductivité thermique de tous les éléments →
- Capacité thermique massique
- 0,131 J/(g·K) Comparer : Capacité thermique massique de tous les éléments →
- Capacité thermique molaire
- 25,1 J/(mol·K) Comparer : Capacité thermique molaire de tous les éléments →
- Structure cristalline
- Cubique à faces centrées Comparer : Structure cristalline de tous les éléments →
Propriétés chimiques
- Électronégativité (Pauling)
- 2,2 Comparer : Électronégativité (Pauling) de tous les éléments →
- Électronégativité (Allen)
- 1,68
- Affinité électronique
- 1,565 eV
- Énergie d’ionisation (1re)
- 8,96702 eV Comparer : Énergie d’ionisation (1re) de tous les éléments →
- Énergie d’ionisation (2e)
- 17,000059 eV Comparer : Énergie d’ionisation (2e) de tous les éléments →
- Énergie d’ionisation (3e)
- 28,000096 eV Comparer : Énergie d’ionisation (3e) de tous les éléments →
- Énergie d’ionisation (4e)
- 40,000138 eV Comparer : Énergie d’ionisation (4e) de tous les éléments →
- Énergie d’ionisation (5e)
- 57,000196 eV Comparer : Énergie d’ionisation (5e) de tous les éléments →
- États d’oxydation
- −3, −2, −1, +1, +2, +3, +4, +5, +6, +7, +8, +9 Comparer : États d’oxydation de tous les éléments →
- Électrons de valence
- 9 Comparer : Électrons de valence de tous les éléments →
- Configuration électronique
- [Xe] 6s2 4f14 5d7
Propriétés thermodynamiques
- Enthalpie de fusion
- 0,27050837 eV Comparer : Enthalpie de fusion de tous les éléments →
- Enthalpie de vaporisation
- 6,26004 eV Comparer : Enthalpie de vaporisation de tous les éléments →
- Enthalpie de sublimation
- 6,944085 eV
- Enthalpie d’atomisation
- 6,944085 eV
- Enthalpie d’atomisation
- 6,93372 eV
Propriétés nucléaires
- Protons
- 77 Comparer : Protons de tous les éléments →
- Neutrons
- 116 Comparer : Neutrons de tous les éléments →
- Isotopes connus
- 43 Comparer : Isotopes connus de tous les éléments →
- Isotopes stables
- 2 Comparer : Isotopes stables de tous les éléments →
- Isotope le plus stable
- Ir-193
- Année de découverte
- 1803
Abondance
- Abondance (croûte terrestre)
- 0,001 mg/kg Comparer : Abondance (croûte terrestre) de tous les éléments →
Structure cristalline
- Paramètre de maille a
- 384 pm
Structure électronique
- Électrons par couche
- 2, 8, 18, 32, 15, 2 Comparer : Électrons par couche de tous les éléments →
Identifiants
- Numéro CAS
- 7439-88-5 Comparer : Numéro CAS de tous les éléments →
- Symbole de terme
- 4F9/2
- InChI
- InChI=1S/Ir
- Clé InChI
- GKOZUEZYRPOHIO-UHFFFAOYSA-N
Configuration électronique Mesuré
Ir: 4f¹⁴ 5d⁷ 6s²[Xe] 4f¹⁴ 5d⁷ 6s²1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d⁷ 6s²Modèle atomique
Les isotopes diffèrent par leur nombre de neutrons, leur masse et leur stabilité — pas par la configuration électronique de l’atome neutre.
Modèle atomique schématique, non à l’échelle.
Empreinte atomique
Spectre d’émission / d’absorption
Distribution isotopique
| Nombre de masse | Masse atomique (u) | Abondance naturelle | Demi-vie |
|---|---|---|---|
| 191 Stable | 190,9605893 ± 0,0000021 | 37,3000% | Stable |
| 193 Stable | 192,9629216 ± 0,0000021 | 62,7000% | Stable |
Phase / État
Explication: 2420,8 °C en dessous du point de fusion (2445,85 °C)
Schématique, non à l’échelle
Points de transition de phase
Énergies de transition
Énergie nécessaire pour faire fondre 1 mol au point de fusion
Énergie nécessaire pour vaporiser 1 mol au point d’ébullition
Énergie nécessaire pour sublimer 1 mol au point de sublimation
Masse volumique
Dans les conditions standard
Dans les conditions standard
Spectres atomiques
Affichage de 10 sur 77. Tri par charge ionique croissante.
Raies répertoriées ?
| Ion | Charge | Nombre total de raies | Probabilités de transition | Désignations des niveaux |
|---|---|---|---|---|
| Ir I | 0 | 402 | 70 | 398 |
| Ir II | +1 | 473 | 129 | 473 |
| Ir IV | +3 | 1374 | 1374 | 1374 |
Niveaux répertoriés ?
| Ion | Charge | Niveaux |
|---|---|---|
| Ir I | 0 | 231 |
| Ir II | +1 | 76 |
| Ir III | +2 | 2 |
| Ir IV | +3 | 224 |
| Ir V | +4 | 2 |
| Ir VI | +5 | 2 |
| Ir VII | +6 | 2 |
| Ir VIII | +7 | 2 |
| Ir IX | +8 | 2 |
| Ir X | +9 | 2 |
Rayons ioniques
| Charge | Coordinence | Spin | Rayon |
|---|---|---|---|
| +3 | 6 | N/D | 68 pm |
| +4 | 6 | N/D | 62.5 pm |
| +5 | 6 | N/D | 56.99999999999999 pm |
Composés
Isotopes (2)
| Nombre de masse | Masse atomique (u) | Abondance naturelle | Demi-vie | Mode de désintégration | |
|---|---|---|---|---|---|
| 191 Stable | 190,9605893 ± 0,0000021 | 37,3000% ± 0,2000% | Stable | stable | |
| 193 Stable | 192,9629216 ± 0,0000021 | 62,7000% ± 0,2000% | Stable | stable |
Raies spectrales
| Longueur d’onde (nm) | Intensité | Degré d’ionisation | Type | Transition | Précision | Source | |
|---|---|---|---|---|---|---|---|
| 382.7577 nm | 58 | Ir II | emission | 5d7.(2D2).6s 3D → 5d7.(4F<5/2>).6p (5/2,1/2)* | Mesurée | NIST | |
| 384.593 nm | N/D | Ir II | emission | 5d7.(2G).6s 1G → 5d7.(4F<9/2>).6p (9/2,3/2)* | Mesurée | NIST | |
| 387.3624 nm | 9 | Ir II | emission | 5d6.6s2 5D → 5d7.(4P<5/2>).6p (5/2,1/2)* | Mesurée | NIST | |
| 389.558 nm | N/D | Ir II | emission | 5d6.6s2 5D → 5d7.(4F<7/2>).6p (7/2,1/2)* | Mesurée | NIST | |
| 395.1973 nm | N/D | Ir II | emission | 5d6.6s2 5D → 5d7.(4F<9/2>).6p (9/2,1/2)* | Mesurée | NIST | |
| 395.2882 nm | 8 | Ir II | emission | 5d7.(2H).6s 3H → 5d6.6s.(6D<9/2>).6p (9/2,1/2)* | Mesurée | NIST | |
| 397.882 nm | 6 | Ir II | emission | 5d7.(2F).6s 3F → 5664* | Mesurée | NIST | |
| 398.6377 nm | 5 | Ir II | emission | 5d6.6s2 5D → 5d7.(4F<3/2>).6p (3/2,1/2)* | Mesurée | NIST | |
| 399.0389 nm | 6 | Ir II | emission | 5d6.6s2 3H → 6197* | Mesurée | NIST | |
| 400.1961 nm | 12 | Ir II | emission | 5d7.(2D2).6s 3D → 5d7.(4P<5/2>).6p (5/2,1/2)* | Mesurée | NIST | |
| 402.5321 nm | 4 | Ir II | emission | 5d7.(2F).6s 3F → 5d6.6s.(6D<5/2>).6p (5/2,1/2)* | Mesurée | NIST | |
| 402.5399 nm | 29 | Ir II | emission | 5d7.(2D2).6s 3D → 5d7.(4F<7/2>).6p (7/2,1/2)* | Mesurée | NIST | |
| 404.1381 nm | 45 | Ir II | emission | 5d7.(2H).6s 3H → 5d7.(4F<9/2>).6p (9/2,1/2)* | Mesurée | NIST | |
| 404.4911 nm | 7 | Ir II | emission | 5d7.(2F).6s 3F → 5d7.(4F<9/2>).6p (9/2,3/2)* | Mesurée | NIST | |
| 410.8315 nm | 48 | Ir II | emission | 5d7.(2F).6s 3F → 5d7.(4F<5/2>).6p (5/2,1/2)* | Mesurée | NIST | |
| 411.7209 nm | 3 | Ir II | emission | 5d7.(2G).6s 3G → 5d7.(4F<9/2>).6p (9/2,1/2)* | Mesurée | NIST | |
| 412.8911 nm | 17 | Ir II | emission | 5d7.(2P).6s 3P → 5d7.(4P<1/2>).6p (1/2,1/2)* | Mesurée | NIST | |
| 413.91 nm | 21 | Ir II | emission | 5d7.(2P).6s 3P → 5d7.(4F<9/2>).6p (9/2,3/2)* | Mesurée | NIST | |
| 439.0196 nm | 4 | Ir II | emission | 5d6.6s2 5D → 5d7.(4P<5/2>).6p (5/2,1/2)* | Mesurée | NIST | |
| 443.3888 nm | N/D | Ir II | emission | 5d7.(2F).6s 3F → 5d6.6s.(6D<7/2>).6p (7/2,1/2)* | Mesurée | NIST | |
| 454.5672 nm | N/D | Ir II | emission | 5d7.(2H).6s 3H → 5d7.(4F<9/2>).6p (9/2,1/2)* | Mesurée | NIST | |
| 461.1752 nm | N/D | Ir II | emission | 5d7.(2F).6s 3F → 5d7.(4P<5/2>).6p (5/2,1/2)* | Mesurée | NIST | |
| 467.5844 nm | 5 | Ir II | emission | 5d7.(2G).6s 3G → 5d7.(4F<9/2>).6p (9/2,1/2)* | Mesurée | NIST | |
| 479.5262 nm | N/D | Ir II | emission | 5d6.6s2 5D → 5d7.(4F<9/2>).6p (9/2,1/2)* | Mesurée | NIST |
Propriétés étendues
Rayons covalents (données étendues)
- Rayon covalent (Pyykkö)
- 122 pm
- Rayon covalent (Pyykkö, liaison double)
- 115 pm
- Rayon covalent (Pyykkö, liaison triple)
- 107 pm
Rayons de van der Waals
- Batsanov
- 200 pm
- Alvarez
- 241 pm
- UFF
- 284 pm
- MM3
- 236 pm
Rayons atomiques et métalliques
- Rayon atomique (Rahm)
- 240 pm
- Rayon métallique (C12)
- 136 pm
Échelles de numérotation
- Mendeleev
- 65
- Pettifor
- 65
- Glawe
- 62
Échelles d’électronégativité
- Ghosh
- 0
- Miedema
- 6
- Gunnarsson–Lundqvist
- 6
- Robles–Bartolotti
- 6
Polarisabilité et dispersion
- Polarisabilité dipolaire
- 54 a.u.
- Polarisabilité dipolaire (incertitude)
- 7 a.u.
- C₆ (Gould–Bučko)
- 522 Ha·Bohr6
Paramètres de Miedema
- Volume molaire de Miedema
- 8,52 cm3/mol
- Densité électronique de Miedema
- 6
Risque d’approvisionnement et économie
- Concentration de la production
- 60
- Risque relatif d’approvisionnement
- 8
- Répartition des réserves
- 95
- Stabilité politique (principal producteur)
- 44
- Stabilité politique (principal détenteur de réserves)
- 44
Transitions de phase et allotropes
| Point de fusion | 2719,15 K |
| Point d’ébullition | 4701,15 K |
Catégories d’états d’oxydation
Données de référence avancées
Constantes d’écran (14)
| n | Orbitale | σ |
|---|---|---|
| 1 | s | 1,4881 |
| 2 | p | 4,4624 |
| 2 | s | 20,1102 |
| 3 | d | 13,514 |
| 3 | p | 21,9311 |
| 3 | s | 22,7942 |
| 4 | d | 37,2628 |
| 4 | f | 38,6552 |
| 4 | p | 35,086 |
| 4 | s | 34,152 |
Détail des rayons cristallins (3)
| Charge | CN | Spin | rcrystal (pm) | Origine |
|---|---|---|---|---|
| 3 | VI | 82 | estimated, | |
| 4 | VI | 76,5 | from r^3 vs V plots, | |
| 5 | VI | 71 | estimated, from metallic oxides, |
Modes de désintégration des isotopes (64)
| Isotope | Mode | Intensité |
|---|---|---|
| 163 | p | — |
| 164 | p | — |
| 164 | A | — |
| 164 | B+ | — |
| 165 | p | — |
| 165 | A | — |
| 166 | A | 93% |
| 166 | p | 7% |
| 167 | A | 43,5% |
| 167 | p | 38,6% |
Facteurs de diffusion des rayons X (515)
| Énergie (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 2,22753 |
| 10,1617 | — | 2,30683 |
| 10,3261 | — | 2,38895 |
| 10,4931 | — | 2,474 |
| 10,6628 | — | 2,56207 |
| 10,8353 | — | 2,65417 |
| 11,0106 | — | 2,75003 |
| 11,1886 | — | 2,84935 |
| 11,3696 | — | 2,94781 |
| 11,5535 | — | 3,0118 |
Données complémentaires
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
1×10-3 milligrams per kilogram
Références (1)
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
Not Applicable
Références (1)
Sources
Sources of this element.
Iridium occurs uncombined in nature with platinum and other metals of this family in alluvial deposits. It is recovered as a by-product from the nickel mining industry.
Références (1)
- [6] Iridium https://periodic.lanl.gov/77.shtml
Références
(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.
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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 Iridium.
The element property data was retrieved from publications.