Sodium (Na)
alkali-metalSolid
Masse atomique relative standard
22,989769 uConfiguration électronique
[Ne] 3s1Point de fusion
97,8 °CPoint d’ébullition
882,85 °CMasse volumique
970 kg/m³États d’oxydation
−1, 0, +1Électronégativité (Pauling)
0,93Énergie d’ionisation (1re)
5,139077 eVAnnée de découverte
1807Rayon atomique
180 pmDétails
Sodium is a soft, highly reactive alkali metal in group 1. It has one valence electron and almost always forms Na⁺ in ordinary compounds. The element is abundant in seawater, evaporite deposits, and silicate minerals, but it is never found free in nature because it reacts readily with water, oxygen, and many nonmetals. Its salts are central to physiology, glassmaking, detergents, and bulk chemical manufacture.
Sodium, like every reactive element, is never found free in nature. Sodium is a soft, bright, silvery metal which floats on water. Decomposition in water results in the evolution of hydrogen and the formation of the hydroxide. It may or may not ignite spontaneously on water, depending on the amount of oxide and metal exposed to the water. It normally does not ignite in air at temperatures below 115°C.
The name derives from the English soda and Latin sodanum for "headache remedy". The symbol Na derives from the Latin natrium for "natron" (soda in English). Sodium was discovered in 1807 by the English chemist Humphry Davy from electrolysis of caustic soda (NaOH).
Although sodium is the sixth most abundant element on earth and comprises about 2.6% of the earth's crust, it is a very reactive element and is never found free in nature. Pure sodium was first isolated by Sir Humphry Davy in 1807 through the electrolysis of caustic soda (NaOH). Since sodium can ignite on contact with water, it must be stored in a moisture free environment.
From the English word, soda; Medieval Latin, sodanum: a headache remedy. Long recognized in compounds, sodium was first isolated by Davy in 1807 by electrolysis of caustic soda.
Pure sodium is a silvery, lustrous metal when freshly cut. It is soft enough to cut with a knife and quickly tarnishes in air as surface oxides, hydroxide, and carbonate form. At ordinary temperature it is a low-density solid with a relatively low melting point for a metal.
Metallic sodium is used mainly as a chemical reductant and heat-transfer medium where its high thermal conductivity and low neutron moderation are useful, notably in some fast-reactor designs. Sodium vapor lamps were historically important for efficient yellow street lighting. Sodium compounds have far larger uses: sodium chloride (NaCl) for food, deicing, and chlor-alkali feedstock; sodium carbonate (Na₂CO₃) for glass and detergents; and sodium hydroxide (NaOH) for pulp, alumina, soaps, and many chemical processes.
Sodium is used in the production of titanium, sodamide, sodium cyanide, sodium peroxide, and sodium hydride. Liquid sodium has been used as a coolant for nuclear reactors. Sodium vapor is used in streetlights and produces a brilliant yellow light.
Sodium also forms many useful compounds. Some of the most common are: table salt (NaCl), soda ash (Na2CO3), baking soda (NaHCO3), caustic soda (NaOH), Chile saltpeter (NaNO3) and borax (Na2B4O7·10H2O).
Metallic sodium is vital in the manufacture of esters and in the preparation of organic compounds. The metal may be used to improve the structure of certain alloys, descale metal, and purify molten metals.
An alloy of sodium with potassium, NaK, is an important heat transfer agent.
Isotopes in Biology
Both 22Na and 24Na have been used as radioactive tracers to study electrolytes in the human body [108] World Nuclear Association. Radioisotopes in Industry: Industrial Uses of Radioisotopes, World Nuclear Association (2014), Feb. 24; http://www.world-nuclear.org/info/inf56.html., [109] Australian Government, Australian Nuclear Science and Technology Organisation (Ansto). [Radioisotopes]:/their Role in Society Today/, Australian Government, Australian Nuclear Science and Technology Organisation (Ansto) (2014), Feb. 24; http://www.ansto.gov.au/__data/assets/pdf_file/0018/3564/Radioisotopes.pdf., [110] AUS-e-TUTE for Astute Science Students. Chemistry Tutorial: Summary of Radioactive Particles, Isotopes, Properties and Uses, AUS-e-TUTE for Astute Science Students (2014), Feb. 24; http://www.ausetute.com.au/nuclesum.html..
Isotopes in Geochronology
22Na is a cosmogenic isotope with a half-life of 2.6 years that has been used to study the residence time of water in freshwater basins. It has been used for dating of young (up to a few decades old) surface water and groundwater (Fig. IUPAC.11.1) [111] D. G. Fleishman. J. Environ. Radioact.99, 1203 (2008)..
Isotopes in Medicine
22Na is used as a source to calibrate positron emission tomography (PET) imaging scanners to check that the instruments are functioning properly [112] T. Hasegawa, K. Oda, Y. Wada, Y. Sato, T. Yamada, M. Matsumoto, H. Murayama, T. Takeda, T. Sasaki, K. Kikuchi, Y. Abe, H. Miyatake, K. Miwa, K. Akimoto, K. Wagatsuma. “Application of novel calibration scheme based on traceable point-like 22Na sources to various types of PET scanners”, in Nuclear Science Symposium and Medical Imaging Conference (NSS/MIC), 2012 IEEE..
Sodium chemistry is dominated by the +1 oxidation state and ionic salts containing Na⁺. Sodium chloride (NaCl) is the most familiar salt and a major industrial feedstock. Sodium hydroxide (NaOH) is a strong base, sodium carbonate (Na₂CO₃) and sodium bicarbonate (NaHCO₃) are important alkaline carbonates, and sodium sulfate (Na₂SO₄) is used in detergents and glass. Sodium hydride (NaH) is a strong base and hydride donor in synthesis. Organosodium compounds exist but are generally more reactive and less commonly handled than organolithium reagents.
The most common compound is sodium chloride (table salt), but it occurs in many other minerals, such as soda niter, cryolite, amphibole, zeolite, etc.
Sodium compounds are important to the paper, glass, soap, textile, petroleum, chemical, and metal industries. Soap is generally a sodium salt of certain fatty acids. The importance of common salt to animal nutrition has been recognized since prehistoric times.
Among the many compounds that are of the greatest industrial importance are common salt (NaCl), soda ash (Na2CO3), baking soda (NaHCO3), caustic soda (NaOH), Chile saltpeter (NaNO3), di- and tri-sodium phosphates, sodium thiosulfate (hypo, Na2S2O3 • 5H2O), and borax (Na2B4O7 • 10H2O).
See more information at the Sodium compound page.
Metallic sodium reacts violently with water to form sodium hydroxide (NaOH) and hydrogen (H₂), which can ignite from the heat released. It is stored under dry mineral oil or inert gas and must be kept away from moisture, acids, and halogenated solvents. Concentrated sodium hydroxide and some other sodium compounds are corrosive. Sodium ions are essential in the body, but excessive dietary sodium is associated with adverse health effects in susceptible populations.
Sodium metal should be handled with great care. It cannot be maintained in an inert atmosphere and contact with water and other substances with which sodium reacts should be avoided.
Sodium is widely distributed in rocks, soils, natural brines, and oceans. Weathering releases Na⁺ from feldspars and other silicates, and rivers carry it to lakes and the sea, where it remains highly soluble. In arid regions it can accumulate in soils and impair plant growth by increasing salinity and altering soil structure. Road deicing salts can raise sodium and chloride levels in nearby waters and soils.
The main commercial sodium materials are salts rather than the metal. Sodium chloride is mined as rock salt, extracted from brines, and recovered by solar evaporation; it feeds chlor-alkali plants that make chlorine (Cl₂), hydrogen (H₂), and sodium hydroxide (NaOH). Sodium carbonate is produced from natural trona deposits or by synthetic processes such as the Solvay route. Metallic sodium is made by electrolysis of molten sodium chloride or related salt mixtures and has a much smaller, specialized market. Recycling is usually process-specific rather than a broad commodity loop.
Sodium is present in fair abundance in the sun and stars. The D lines of sodium are among the most prominent in the solar spectrum. Sodium is the fourth most abundant element on earth, comprising about 2.6% of the earth's crust; it is the most abundant of the alkali group of metals.
It is now obtained commercially by the electrolysis of absolutely dry fused sodium chloride. This method is much cheaper than that of electrolyzing sodium hydroxide, as was used several years ago.
Sodium is a moderately abundant light element produced chiefly by stellar nucleosynthesis involving carbon and neon burning and by related neutron-capture reactions in stars. Its yellow D spectral lines are strong and easily observed in stellar atmospheres, comets, planetary exospheres, and interstellar gas. On rocky planets it is commonly incorporated into silicates and soluble salts rather than existing as metal.
- Sodium’s chemical symbol comes from natrium, a Latinized name related to soda minerals.
- The yellow sodium D lines near 589 nm are among the most recognizable atomic emission features.
- Liquid sodium has been used as a coolant because it stays liquid over a broad temperature range.
- Fresh sodium surfaces can look mirror-bright before tarnishing within seconds in moist air.
- Common table salt usually contains additives, so it is not pure sodium chloride.
Images
Propriétés
Propriétés physiques
- Rayon atomique (empirique)
- 180 pm Comparer : Rayon atomique (empirique) de tous les éléments →
- Rayon covalent
- 166 pm Comparer : Rayon covalent de tous les éléments →
- Rayon de van der Waals
- 227 pm Comparer : Rayon de van der Waals de tous les éléments →
- Rayon métallique
- 157 pm Comparer : Rayon métallique de tous les éléments →
- Masse volumique
- 970 kg/m³ Comparer : Masse volumique de tous les éléments →
- Volume molaire
- 0,0237 L/mol
- Phase aux CNTP
- Solide Comparer : Phase aux CNTP de tous les éléments →
- Point de fusion
- 97,8 °C Comparer : Point de fusion de tous les éléments →
- Point d’ébullition
- 882,85 °C Comparer : Point d’ébullition de tous les éléments →
- Conductivité thermique
- 142 W/(m·K) Comparer : Conductivité thermique de tous les éléments →
- Capacité thermique massique
- 1,228 J/(g·K) Comparer : Capacité thermique massique de tous les éléments →
- Capacité thermique molaire
- 28,23 J/(mol·K) Comparer : Capacité thermique molaire de tous les éléments →
- Structure cristalline
- Cubique centré Comparer : Structure cristalline de tous les éléments →
Propriétés chimiques
- Électronégativité (Pauling)
- 0,93 Comparer : Électronégativité (Pauling) de tous les éléments →
- Électronégativité (Allen)
- 0,869
- Affinité électronique
- 0,5479 eV
- Énergie d’ionisation (1re)
- 5,139077 eV Comparer : Énergie d’ionisation (1re) de tous les éléments →
- Énergie d’ionisation (2e)
- 47,286523 eV Comparer : Énergie d’ionisation (2e) de tous les éléments →
- Énergie d’ionisation (3e)
- 71,620247 eV Comparer : Énergie d’ionisation (3e) de tous les éléments →
- Énergie d’ionisation (4e)
- 98,936341 eV Comparer : Énergie d’ionisation (4e) de tous les éléments →
- Énergie d’ionisation (5e)
- 138,404476 eV Comparer : Énergie d’ionisation (5e) de tous les éléments →
- États d’oxydation
- −1, 0, +1 Comparer : États d’oxydation de tous les éléments →
- Électrons de valence
- 1 Comparer : Électrons de valence de tous les éléments →
- Configuration électronique
- [Ne] 3s1
Propriétés thermodynamiques
- Point critique (température)
- 2300 °C
- Point critique (pression)
- 3,5e+7 Pa
- Enthalpie de fusion
- 0,02694719 eV Comparer : Enthalpie de fusion de tous les éléments →
- Enthalpie de vaporisation
- 1,012593 eV Comparer : Enthalpie de vaporisation de tous les éléments →
- Enthalpie de sublimation
- 1,11209 eV
- Enthalpie d’atomisation
- 1,11209 eV
- Enthalpie d’atomisation
- 1,114163 eV
Propriétés nucléaires
- Protons
- 11 Comparer : Protons de tous les éléments →
- Neutrons
- 12 Comparer : Neutrons de tous les éléments →
- Isotopes connus
- 23 Comparer : Isotopes connus de tous les éléments →
- Isotopes stables
- 1 Comparer : Isotopes stables de tous les éléments →
- Isotope le plus stable
- Na-23
- Année de découverte
- 1807
Abondance
- Abondance (croûte terrestre)
- 2,36e+4 mg/kg Comparer : Abondance (croûte terrestre) de tous les éléments →
- Abondance (océan)
- 1,08 × 104 mg/L Comparer : Abondance (océan) de tous les éléments →
Structure cristalline
- Paramètre de maille a
- 423 pm
Structure électronique
- Électrons par couche
- 2, 8, 1 Comparer : Électrons par couche de tous les éléments →
Identifiants
- Numéro CAS
- 7440-23-5 Comparer : Numéro CAS de tous les éléments →
- Symbole de terme
- 2S1/2
- InChI
- InChI=1S/Na
- Clé InChI
- KEAYESYHFKHZAL-UHFFFAOYSA-N
Configuration électronique Mesuré
Na: 3s¹[Ne] 3s¹1s² 2s² 2p⁶ 3s¹Modèle 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 |
|---|---|---|---|
| 23 Stable | 22,989769282 ± 0,0000000019 | 100,0000% | Stable |
Phase / État
Explication: 72,8 °C en dessous du point de fusion (97,8 °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
Données avancées
Spectres atomiques
Affichage de 10 sur 11. Tri par charge ionique croissante.
Raies répertoriées ?
| Ion | Charge | Nombre total de raies | Probabilités de transition | Désignations des niveaux |
|---|---|---|---|---|
| Na I | 0 | 869 | 523 | 858 |
| Na II | +1 | 1345 | 176 | 605 |
| Na III | +2 | 560 | 417 | 560 |
| Na IV | +3 | 687 | 671 | 687 |
| Na V | +4 | 529 | 503 | 527 |
| Na VI | +5 | 657 | 594 | 641 |
| Na VII | +6 | 1374 | 1369 | 1374 |
| Na VIII | +7 | 464 | 456 | 464 |
| Na IX | +8 | 172 | 138 | 172 |
| Na X | +9 | 594 | 586 | 594 |
Niveaux répertoriés ?
| Ion | Charge | Niveaux |
|---|---|---|
| Na I | 0 | 430 |
| Na II | +1 | 165 |
| Na III | +2 | 120 |
| Na IV | +3 | 104 |
| Na V | +4 | 102 |
| Na VI | +5 | 116 |
| Na VII | +6 | 142 |
| Na VIII | +7 | 89 |
| Na IX | +8 | 46 |
| Na X | +9 | 111 |
Rayons ioniques
| Charge | Coordinence | Spin | Rayon |
|---|---|---|---|
| +1 | 4 | N/D | 99 pm |
| +1 | 5 | N/D | 100 pm |
| +1 | 6 | N/D | 102 pm |
| +1 | 7 | N/D | 112.00000000000001 pm |
| +1 | 8 | N/D | 118 pm |
| +1 | 9 | N/D | 124 pm |
| +1 | 12 | N/D | 139 pm |
Composés
Isotopes (1)
Thirteen isotopes of sodium are recognized.
| Nombre de masse | Masse atomique (u) | Abondance naturelle | Demi-vie | Mode de désintégration | |
|---|---|---|---|---|---|
| 23 Stable | 22,989769282 ± 0,0000000019 | 100,0000% | Stable | stable |
Raies spectrales
Affichage de 50 sur 480. Seules les raies spectrales dont l’intensité a été mesurée sont affichées par défaut.
| Longueur d’onde (nm) | Intensité | Degré d’ionisation | Type | Transition | Précision | Source | |
|---|---|---|---|---|---|---|---|
| 588.995094 nm | 80000 | Na I | emission | 2p6.3s 2S → 2p6.3p 2P* | Mesurée | NIST | |
| 589.592424 nm | 40000 | Na I | emission | 2p6.3s 2S → 2p6.3p 2P* | Mesurée | NIST | |
| 388.181 nm | 420 | Na I | emission | 2p5.(2P*).3s.3p.(3P*) 4D → 2p5.3s.(3P*).3d 4F* | Mesurée | NIST | |
| 443.234 nm | 310 | Na I | emission | 2p5.(2P*).3s.3p.(3P*) 4S → 2p5.3s.(3P*).4s 4P* | Mesurée | NIST | |
| 411.3703 nm | 300 | Na II | emission | 2s2.2p5.3p 1S → 2s2.2p5.(2P*<1/2>).3d 2[3/2]* | Mesurée | NIST | |
| 507.12 nm | 270 | Na I | emission | 2p5.(2P*).3s.3p.(3P*) 4D → 2p5.3s.(3P*).4s 4P* | Mesurée | NIST | |
| 412.3069 nm | 250 | Na II | emission | 2s2.2p5.3p 1S → 2s2.2p5.(2P*<1/2>).4s 2[1/2]* | Mesurée | NIST | |
| 423.335 nm | 250 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[5/2]* → 2s2.2p5.(2P*<1/2>).4f 2[7/2] | Mesurée | NIST | |
| 424.09 nm | 250 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[5/2]* → 2s2.2p5.(2P*<1/2>).4f 2[7/2] | Mesurée | NIST | |
| 429.249 nm | 250 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[1/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 429.287 nm | 250 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[1/2]* → 2s2.2p5.(2P*<3/2>).4f 2[3/2] | Mesurée | NIST | |
| 430.882 nm | 250 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[1/2]* → 2s2.2p5.(2P*<3/2>).4f 2[3/2] | Mesurée | NIST | |
| 430.904 nm | 250 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[1/2]* → 2s2.2p5.(2P*<3/2>).4f 2[3/2] | Mesurée | NIST | |
| 432.091 nm | 250 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[3/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 433.729 nm | 250 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[3/2]* → 2s2.2p5.(2P*<3/2>).4f 2[3/2] | Mesurée | NIST | |
| 434.412 nm | 250 | Na II | emission | 2s2.2p5.3p 1S → 2s2.2p5.(2P*<3/2>).4s 2[3/2]* | Mesurée | NIST | |
| 439.281 nm | 250 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[7/2]* → 2s2.2p5.(2P*<3/2>).4f 2[9/2] | Mesurée | NIST | |
| 408.1372 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[3/2]* → 2s2.2p5.(2P*<1/2>).4f 2[5/2] | Mesurée | NIST | |
| 436.859 nm | 200 | Na II | emission | 2s2.2p5.3p 1S → 2s2.2p5.(2P*<3/2>).3d 2[3/2]* | Mesurée | NIST | |
| 437.522 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[7/2]* → 2s2.2p5.(2P*<3/2>).4f 2[7/2] | Mesurée | NIST | |
| 438.748 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[7/2]* → 2s2.2p5.(2P*<3/2>).4f 2[7/2] | Mesurée | NIST | |
| 440.512 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[7/2]* → 2s2.2p5.(2P*<3/2>).4f 2[9/2] | Mesurée | NIST | |
| 444.669 nm | 200 | Na II | emission | 2s2.2p5.(2P*<1/2>).3d 2[5/2]* → 2s2.2p5.(2P*<1/2>).4f 2[5/2] | Mesurée | NIST | |
| 444.741 nm | 200 | Na II | emission | 2s2.2p5.(2P*<1/2>).3d 2[5/2]* → 2s2.2p5.(2P*<1/2>).4f 2[7/2] | Mesurée | NIST | |
| 445.473 nm | 200 | Na II | emission | 2s2.2p5.(2P*<1/2>).3d 2[5/2]* → 2s2.2p5.(2P*<1/2>).4f 2[5/2] | Mesurée | NIST | |
| 445.523 nm | 200 | Na II | emission | 2s2.2p5.(2P*<1/2>).3d 2[5/2]* → 2s2.2p5.(2P*<1/2>).4f 2[7/2] | Mesurée | NIST | |
| 445.72 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 447.463 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<3/2>).4f 2[3/2] | Mesurée | NIST | |
| 447.88 nm | 200 | Na II | emission | 2s2.2p5.(2P*<1/2>).3d 2[3/2]* → 2s2.2p5.(2P*<1/2>).4f 2[5/2] | Mesurée | NIST | |
| 448.167 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[5/2]* → 2s2.2p5.(2P*<3/2>).4f 2[7/2] | Mesurée | NIST | |
| 449.015 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[5/2]* → 2s2.2p5.(2P*<3/2>).4f 2[7/2] | Mesurée | NIST | |
| 449.088 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[5/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 449.961 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[5/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 450.697 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[3/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 451.92 nm | 200 | Na II | emission | 2s2.2p5.(2P*<1/2>).3d 2[3/2]* → 2s2.2p5.(2P*<1/2>).4f 2[5/2] | Mesurée | NIST | |
| 452.497 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[3/2]* → 2s2.2p5.(2P*<3/2>).4f 2[3/2] | Mesurée | NIST | |
| 453.331 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 455.152 nm | 200 | Na II | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<3/2>).4f 2[3/2] | Mesurée | NIST | |
| 391.803 nm | 160 | Na I | emission | 2p5.(2P*).3s.3p.(3P*) 4D → 2p5.3s.(3P*).3d 4F* | Mesurée | NIST | |
| 438.42 nm | 160 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[7/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 439.63 nm | 160 | Na II | emission | 2s2.2p5.(2P*<3/2>).3d 2[7/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 459.094 nm | 160 | Na II | emission | 2s2.2p5.3p 1S → 2s2.2p5.(2P*<3/2>).3d 2[1/2]* | Mesurée | NIST | |
| 472.23 nm | 160 | Na II | emission | 2s2.2p5.(2P*<1/2>).3d 2[5/2]* → 2s2.2p5.(2P*<3/2>).4f 2[7/2] | Mesurée | NIST | |
| 473.113 nm | 160 | Na II | emission | 2s2.2p5.(2P*<1/2>).3d 2[5/2]* → 2s2.2p5.(2P*<3/2>).4f 2[7/2] | Mesurée | NIST | |
| 474.163 nm | 160 | Na II | emission | 2s2.2p5.(2P*<1/2>).3d 2[5/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 476.892 nm | 160 | Na II | emission | 2s2.2p5.(2P*<1/2>).3d 2[3/2]* → 2s2.2p5.(2P*<3/2>).4f 2[5/2] | Mesurée | NIST | |
| 418.546 nm | 150 | Na I | emission | 2p5.(2P*).3s.3p.(3P*) 4P → 2p5.3s.(3P*).3d 4D* | Mesurée | NIST | |
| 386.543 nm | 130 | Na I | emission | 2p5.(2P*).3s.3p.(3P*) 4D → 2p5.3s.(3P*).3d 4F* | Mesurée | NIST | |
| 408.7593 nm | 130 | Na II | emission | 2s2.2p5.3s 1P* → 2s2.2p5.3p 3S | Mesurée | NIST | |
| 420.2759 nm | 130 | Na II | emission | 2s2.2p5.(2P*<3/2>).4s 2[3/2]* → 2s2.2p5.(2P*<1/2>).4f 2[5/2] | Mesurée | NIST |
Propriétés étendues
Rayons covalents (données étendues)
- Rayon covalent (Pyykkö)
- 155 pm
- Rayon covalent (Pyykkö, liaison double)
- 160 pm
- Rayon covalent (Bragg)
- 177 pm
Rayons de van der Waals
- Bondi
- 227 pm
- Batsanov
- 240 pm
- Alvarez
- 250 pm
- UFF
- 298,3 pm
- MM3
- 270 pm
Rayons atomiques et métalliques
- Rayon atomique (Rahm)
- 225 pm
- Rayon métallique (C12)
- 190 pm
Échelles de numérotation
- Mendeleev
- 2
- Pettifor
- 11
- Glawe
- 11
Échelles d’électronégativité
- Ghosh
- 0
- Miedema
- 3
- Gunnarsson–Lundqvist
- 3
- Robles–Bartolotti
- 2
Polarisabilité et dispersion
- Polarisabilité dipolaire
- 162,7 a.u.
- Polarisabilité dipolaire (incertitude)
- 0,5 a.u.
- C₆
- 1518 Ha·Bohr6
- C₆ (Gould–Bučko)
- 1570 Ha·Bohr6
Paramètres de Miedema
- Volume molaire de Miedema
- 23,78 cm3/mol
- Densité électronique de Miedema
- 1
Risque d’approvisionnement et économie
- Concentration de la production
- 24
- Risque relatif d’approvisionnement
- 4
- Stabilité politique (principal producteur)
- 24
Transitions de phase et allotropes
| Point de fusion | 370,94 K |
| Point d’ébullition | 1156,09 K |
| Point critique (température) | 2573,15 K |
| Point critique (pression) | 35 MPa |
Catégories d’états d’oxydation
Données de référence avancées
Constantes d’écran (4)
| n | Orbitale | σ |
|---|---|---|
| 1 | s | 0,3741 |
| 2 | p | 4,1982 |
| 2 | s | 4,4286 |
| 3 | s | 8,4926 |
Détail des rayons cristallins (7)
| Charge | CN | Spin | rcrystal (pm) | Origine |
|---|---|---|---|---|
| 1 | IV | 113 | ||
| 1 | V | 114 | ||
| 1 | VI | 116 | ||
| 1 | VII | 126 | ||
| 1 | VIII | 132 | ||
| 1 | IX | 138 | calculated, | |
| 1 | XII | 153 |
Modes de désintégration des isotopes (47)
| Isotope | Mode | Intensité |
|---|---|---|
| 17 | p | 100% |
| 18 | p | — |
| 19 | p | 100% |
| 20 | B+ | 100% |
| 20 | B+A | 25% |
| 21 | B+ | 100% |
| 22 | B+ | 100% |
| 22 | e+ | 90,6% |
| 22 | EC | 9,4% |
| 24 | B- | 100% |
Facteurs de diffusion des rayons X (504)
| Énergie (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 0,01475 |
| 10,1617 | — | 0,01517 |
| 10,3261 | — | 0,01559 |
| 10,4931 | — | 0,01603 |
| 10,6628 | — | 0,01648 |
| 10,8353 | — | 0,01695 |
| 11,0106 | — | 0,01743 |
| 11,1886 | — | 0,01792 |
| 11,3696 | — | 0,01842 |
| 11,5535 | — | 0,01894 |
Données complémentaires
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
2.36×104 milligrams per kilogram
Références (1)
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
1.08×104 milligrams per liter
Références (1)
Sources
Sources of this element.
Sodium is present in fair abundance in the sun and stars. The D lines of sodium are among the most prominent in the solar spectrum. Sodium is the fourth most abundant element on earth, comprising about 2.6% of the earth's crust; it is the most abundant of the alkali group of metals.
It is now obtained commercially by the electrolysis of absolutely dry fused sodium chloride. This method is much cheaper than that of electrolyzing sodium hydroxide, as was used several years ago.
Références (1)
- [6] Sodium https://periodic.lanl.gov/11.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.
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 Sodium.
The element property data was retrieved from publications.