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Sodium


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Atomic symbol: Na
Atomic number: 11
Atomic weight: 22.98977
Atomic volume: 23.7 cm3/mol
Density: 0.971 g/cm3
Period Number: 3
Group number: 1
Group name: Alkali Met.
Element classification: Metal


States


Phase at room temperature: Solid
Melting Point: 371.01 K
Boiling point: 1154.6 K
Heat of fusion: 2.598 kJ/mol
Heat of vaporization: 96.960 kJ/mol


Energies


Ionization Energy: 5.139 eV
1st ionization energy: 495.8 kJ/mole
2nd ionization energy: 4562.4 kJ/mole
3rd ionization energy: 6912.2 kJ/mole
Electronegativity: 0.93
Electron affinity: 52.868 kJ/mole
Specific heat: 1.23 J/gK
Heat atomization: 109 kJ/mole atoms


Oxidation & Electrons


Shells: 2,8,1
Electron Shell Configuration: [Ne] 3s1
Minimum oxidation number: -1
Maximum oxidation number: 1
Minimum common oxidation number: 0
Maximum common oxidation no: 1


Appearance & Characteristics


Structure:: bcc: body-centered cubic
Color: silvery
Hardness: 0.4 mohs
Toxicity: ?
Characteristics: soft
Uses: lamps, table salt


Reactions


Reaction with air: vigorous, =>Na2O2
Reaction with 6M HCl: vigorous, =>H2, NaCl
Reaction with 15M HNO3: vigorous, =>NaNO3, NOx
Reaction with 6M NaOH: vigorous, =>H2, NaOH


Other Forms


Number of isotopes: 1
Oxide(s): Na2O
Hydride(s): NaH
Chloride(s): NaCl


Radius


Atomic Radius: 186 pm
Ionic radius (1- ion): pm
Ionic radius (1+ ion): 116 pm
Ionic radius (2- ion): pm
Ionic radius (2+ ion): pm
Ionic radius (3+ ion): pm


Conductivity


Thermal conductivity: 142 J/m-sec-deg
Electrical conductivity: 209.6 1/mohm-cm
Polarizability: 23.6 A^3


Abundance


Source: Halite (misc)
Relative abundance solar system: 4.759 log
Abundance earth's crust: 4.4 log
Estimated crustal abundance: 2.36×104 milligrams per kilogram
Estimated oceanic abundance: 1.08×104 milligrams per liter
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 


History


(English, soda; Medieval Latin, sodanum: a headache remedy) Long recognized in compounds, sodium was first isolated by Davy in 1807 by electrolysis of caustic soda.


Sources


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.


Properties


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 1150C.


Compounds


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).


Uses


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


Thirteen isotopes of sodium are recognized.

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