Sodium
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Sodium | ||||||||||||||||||||||||||
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Appearance | silvery white metallic | |||||||||||||||||||||||||
Standard atomic weightAr°(Na) | ||||||||||||||||||||||||||
22.98976928(2)[1] | ||||||||||||||||||||||||||
Sodium in theperiodic table | ||||||||||||||||||||||||||
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Group | group 1: hydrogen andalkali metals | |||||||||||||||||||||||||
Period | period 3 | |||||||||||||||||||||||||
Block | s-block | |||||||||||||||||||||||||
Electron configuration | [Ne] 3s1 | |||||||||||||||||||||||||
Electrons per shell | 2, 8, 1 | |||||||||||||||||||||||||
Physical properties | ||||||||||||||||||||||||||
PhaseatSTP | solid | |||||||||||||||||||||||||
Melting point | 370.944K(97.794 °C, 208.029 °F) | |||||||||||||||||||||||||
Boiling point | 1156.090 K (882.940 °C, 1621.292 °F) | |||||||||||||||||||||||||
Density(nearr.t.) | 0.968 g/cm3 | |||||||||||||||||||||||||
when liquid (atm.p.) | 0.927 g/cm3 | |||||||||||||||||||||||||
Critical point | 2573 K, 35 MPa(extrapolated) | |||||||||||||||||||||||||
Heat of fusion | 2.60kJ/mol | |||||||||||||||||||||||||
Heat of vaporization | 97.42 kJ/mol | |||||||||||||||||||||||||
Molar heat capacity | 28.230 J/(mol·K) | |||||||||||||||||||||||||
Vapor pressure
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Atomic properties | ||||||||||||||||||||||||||
Oxidation states | −1, 0,[2]+1(a stronglybasicoxide) | |||||||||||||||||||||||||
Electronegativity | Pauling scale: 0.93 | |||||||||||||||||||||||||
Ionization energies |
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Atomic radius | empirical: 186pm | |||||||||||||||||||||||||
Covalent radius | 166±9 pm | |||||||||||||||||||||||||
Van der Waals radius | 227 pm | |||||||||||||||||||||||||
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Other properties | ||||||||||||||||||||||||||
Natural occurrence | primordial | |||||||||||||||||||||||||
Crystal structure | body-centered cubic(bcc) | |||||||||||||||||||||||||
Speed of soundthin rod | 3200 m/s (at 20 °C) | |||||||||||||||||||||||||
Thermal expansion | 71 µm/(m⋅K) (at 25 °C) | |||||||||||||||||||||||||
Thermal conductivity | 142 W/(m⋅K) | |||||||||||||||||||||||||
Electrical resistivity | 47.7 nΩ⋅m (at 20 °C) | |||||||||||||||||||||||||
Magnetic ordering | paramagnetic[3] | |||||||||||||||||||||||||
Molar magnetic susceptibility | +16.0·10−6cm3/mol (298 K)[4] | |||||||||||||||||||||||||
Young's modulus | 10 GPa | |||||||||||||||||||||||||
Shear modulus | 3.3 GPa | |||||||||||||||||||||||||
Bulk modulus | 6.3 GPa | |||||||||||||||||||||||||
Mohs hardness | 0.5 | |||||||||||||||||||||||||
Brinell hardness | 0.69 MPa | |||||||||||||||||||||||||
CAS Number | 7440-23-5 | |||||||||||||||||||||||||
History | ||||||||||||||||||||||||||
Discoveryand first isolation | Humphry Davy(1807) | |||||||||||||||||||||||||
Symbol | "Na": fromNew Latinnatrium,coined from GermanNatron,'natron' | |||||||||||||||||||||||||
Isotopes of sodium | ||||||||||||||||||||||||||
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![](https://upload.wikimedia.org/wikipedia/commons/thumb/8/8c/Sodium.jpg/220px-Sodium.jpg)
Sodiumis achemical elementwith anatomic numberof 11. Its symbol isNa(from its Latin namenatrium). It is analkali metal.Although sodium has manyisotopes,most decay in a short time. Because of this, all sodium in nature (mainly found inseawater) is of the isotope11Na23.Theatomic massof sodium is 22.9898.
Properties
[change|change source]Sodium is a light-weight,silver-coloredmetal.Sodium is soft. It can easily be cut with a knife. When someone cuts it, the exposed part will become white over time. It reacts with air to formsodium hydroxideandsodium carbonate.Sodium is a little lessdensethan water. It floats and reacts instantly with water, producinghydrogenandsodium hydroxide.This reaction has a lot of heat, usually causing the hydrogen to light on fire. When this happens, sodium melts because of its low melting point. Sodium is highly reactive because it has onevalence electron,which is easily removed.
Compared with otheralkali metals,sodium is less reactive thanpotassiumand more reactive thanlithium.[6]
Chemical compounds
[change|change source]These arechemical compoundsthat contain sodiumions.Sodium only exists in oneoxidation state:+1.
- Sodium aluminum fluoride,used to make aluminum
- Sodium amide,very strong base
- Sodium arsenite,colorless solid, very toxic
- Sodium arsenate,oxidizing agent, very toxic
- Sodium azide,used in airbags
- Sodium bicarbonate,baking soda, used in cooking
- Sodium bismuthate,oxidizing agent, used to test for manganese
- Sodium bisulfate,acidic, used to lower pH
- Sodium bromate,oxidizing agent, used to dye hair
- Sodium bromide,rare, used in some medicine
- Sodium carbonate,used to make glass
- Sodium chlorate,used in some explosives
- Sodium chlorite,used in disinfectants
- Sodium chloride,table salt
- Sodium chromate,yellow,oxidizing agent,toxic
- Sodium dichromate,orange,oxidizing agent,toxic
- Sodium fluoride,used in toothpaste, bitter, toxic in large doses
- Sodium hydroxide,lye, used in soap, strongbase
- Sodium hypochlorite,bleach, disinfectant
- Sodium hypophosphite,reducing agent,poisonous
- Sodium iodate,oxidizing agent, prevents iodine deficiency
- Sodium iodide,a weak reducing agent, prevents iodine deficiency
- Sodium manganate,rare green solid
- Sodium nitrate,used in blasting powder
- Sodium nitrite,used in food preservation
- Sodium periodate,oxidizing agent
- Sodium permanganate,less common than potassium permanganate, oxidizing agent
- Sodium phosphate,various uses
- Sodium phosphide,catalyst,used to speed up chemical reactions
- Sodium phosphite,toxic, reducing agent
- Sodium selenate,strong oxidizing agent, other selenium compounds
- Sodium selenide,strong reducing agent, reactive
- Sodium selenite,weak oxidizing agent, vitamin supplement
- Sodium sulfate,bitter, laxative
- Sodium sulfite,a weak reducing agent, used to preserve dried food
- Sodium tellurate,strong oxidizing agent
- Sodium telluride,a strong reducing agent, reacts with air easily
- Sodium tellurite,main tellurite compound
Discovery and name origins
[change|change source]Sodium was discovered by Sir Humphrey Davy, an English scientist, in 1807. He created it byelectrolyzingsodium hydroxide. Davy named the element aftersoda,a name for sodium hydroxide orsodium carbonate.
Uses
[change|change source]Scientists can use it in the creation oforganic compounds.It is used in orangestreetlightsand lamps that emitultravioletlight.
Sodium compounds are used insoaps,toothpaste,baking,andantacids.
Thehuman bodyneeds sodiumions,taken in the form ofsodium chloride,to live. Too much of it can cause health problems. Many organisms in the ocean depend on theconcentrationof sodium ions in water to survive.
Occurrence and production
[change|change source]Sodium does not occur as an element in nature, because it is not stable enough. It exists only inchemical compounds.Sodiumionsare found in the ocean and in theEarth's crust.
Sodium is normally made byelectrolysisofsodium chloride,which is mined from the Earth's crust.
Related pages
[change|change source]- List of common elements
- Hyponatremia(a medical problem caused by not having enough sodium in the body)
References
[change|change source]- ↑"Standard Atomic Weights: Sodium".CIAAW.2005.
- ↑The compoundNaClhas been shown in experiments to exists in several unusualstoichiometriesunder high pressure, including Na3Cl in which contains a layer of sodium(0) atoms; seeZhang, W.; Oganov, A. R.; Goncharov, A. F.; Zhu, Q.; Boulfelfel, S. E.; Lyakhov, A. O.; Stavrou, E.; Somayazulu, M.; Prakapenka, V. B.; Konôpková, Z. (2013). "Unexpected Stable Stoichiometries of Sodium Chlorides".Science.342(6165): 1502–1505.arXiv:1310.7674.Bibcode:2013Sci...342.1502Z.doi:10.1126/science.1244989.PMID24357316.S2CID15298372.
- ↑Magnetic susceptibility of the elements and inorganic compounds,inLide, D. R., ed. (2005).CRC Handbook of Chemistry and Physics(86th ed.). Boca Raton (FL): CRC Press.ISBN0-8493-0486-5.
- ↑Weast, Robert (1984).CRC, Handbook of Chemistry and Physics.Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110.ISBN0-8493-0464-4.
- ↑Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021)."The NUBASE2020 evaluation of nuclear properties"(PDF).Chinese Physics C.45(3): 030001.doi:10.1088/1674-1137/abddae.
- ↑De Leon, N."Reactivity of Alkali Metals".Indiana University Northwest.Archived fromthe originalon 2018-10-16.Retrieved2007-12-07.
H | He | ||||||||||||||||||||||||||||||||||||||||
Li | Be | B | C | N | O | F | Ne | ||||||||||||||||||||||||||||||||||
Na | Mg | Al | Si | P | S | Cl | Ar | ||||||||||||||||||||||||||||||||||
K | Ca | Sc | Ti | V | Cr | Mn | Fe | Co | Ni | Cu | Zn | Ga | Ge | As | Se | Br | Kr | ||||||||||||||||||||||||
Rb | Sr | Y | Zr | Nb | Mo | Tc | Ru | Rh | Pd | Ag | Cd | In | Sn | Sb | Te | I | Xe | ||||||||||||||||||||||||
Cs | Ba | La | Ce | Pr | Nd | Pm | Sm | Eu | Gd | Tb | Dy | Ho | Er | Tm | Yb | Lu | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg | Tl | Pb | Bi | Po | At | Rn | ||||||||||
Fr | Ra | Ac | Th | Pa | U | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | ||||||||||
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