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7440-23-5

Basic Information
CAS No.: 7440-23-5
Name: Sodium
Article Data: 592
Cas Database
Molecular Structure:
Molecular Structure of 7440-23-5 (Sodium)
Formula: Na
Molecular Weight: 22.9898
Synonyms: Atomicsodium;Natrium;Sodium atom;Sodium metal;Sodium-23;
EINECS: 231-132-9
Density: 1.04 g/mL at 20 °C
Melting Point: 97.8 °C(lit.)
Boiling Point: 883 °C(lit.)
Flash Point: 128°F
Solubility: soluble in water
Appearance: light, soft silver metal
Hazard Symbols: CorrosiveC,FlammableF,ToxicT
Risk Codes: 34-14/15-45
Safety: 26-8-6A-45-43D-43-53
Transport Information: N/A
PSA: 0.00000
LogP: 0.11250
Synthetic route

sodium azide

7440-23-5

sodium

Conditions
ConditionsYield
In neat (no solvent) heating NaN3 to 275°C;;100%
In neat (no solvent) heating NaN3 to 275°C;;100%
In neat (no solvent) carbon support was impregnated with NaN3 following with drying procedureunder UHV and at 450°C; carbon support was used;
497-19-8

sodium carbonate

7440-23-5

sodium

Conditions
ConditionsYield
With pyrographite; calcium oxide In neat (no solvent) 110°C, 1-2 Torr;;94%
With coal; CaO In neat (no solvent) 110°C, 1-2 Torr;;94%
With pyrographite In neat (no solvent) 110°C, 1-2 Torr;;92%
7647-14-5

sodium chloride

7440-23-5

sodium

Conditions
ConditionsYield
With calcium carbide In neat (no solvent) byproducts: CaCl2, C; at 900°C, diminshed yield with increase of pressure (1-10 Torr);;92%
With calcium carbide; sodium fluoride In neat (no solvent) byproducts: CaCl2, C; powdered and pressed, 0.5 Torr, 6% NaF, 875°C;;82%
With calcium carbide In neat (no solvent) reduction at 900°C;;63%
7757-82-6

sodium sulfate

7440-23-5

sodium

Conditions
ConditionsYield
With pyrographite In neat (no solvent) 110°C, 1-2 Torr;;54%
With coal In neat (no solvent) 110°C, 1-2 Torr;;54%
With pyrographite; calcium oxide In neat (no solvent) 110°C, 1-2 Torr;;83-95
16940-66-2

sodium tetrahydroborate

A

boron

B

1333-74-0

hydrogen

C

7440-23-5

sodium

Conditions
ConditionsYield
decompn. at 500°C, heating in N2- or H2-atm.;A n/a
B 45%
C n/a
decompn. at 500°C, heating in N2- or H2-atm.;A n/a
B 45%
C n/a
7647-15-6

sodium bromide

A

7726-95-6

bromine

B

7440-23-5

sodium

Conditions
ConditionsYield
Electrolysis;

dolomite

7647-14-5

sodium chloride

A

7440-23-5

sodium

B

7439-95-4

magnesium

Conditions
ConditionsYield
In neat (no solvent) 1200°C;; simultaneous preparation of Na and Mg;;

borax

7439-95-4

magnesium

A

magnesium diboride

B

7440-23-5

sodium

Conditions
ConditionsYield
In gaseous matrix slow reaction with small amounts; vigorous reaction with greater amounts and at a certain temperature;;
In gaseous matrix slow reaction with small amounts; vigorous reaction with greater amounts and at a certain temperature;;

iron acetylide

1310-73-2

sodium hydroxide

7440-23-5

sodium

Conditions
ConditionsYield
In neat (no solvent) byproducts: iron, carbon dioxide, carbon monoxide; reaction of FeC2 (70 parts metal, 30 parts carbon) with 3 parts NaOH in a cast iron crucible; passing in of CO is of advantage; further byproduct: hydrogene;;

sodium monoxide

7440-23-5

sodium

Conditions
ConditionsYield
In gas Kinetics; byproducts: O2; carrier gas (He); fast flow reactor; not isolated, detected by fluorescence;
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  • Sodium CAS NO.7440-23-5

  • Casno:

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    Sodium CAS NO.7440-23-5

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History

In medieval Europe a compound of Sodium (CAS NO.7440-23-5) with the Latin name of sodanum was used as a headache remedy. The name sodium probably originates from the Arabic word suda meaning headache as the headache-alleviating properties of sodium carbonate or soda were well known in early times.
 Sodium's chemical abbreviation Na was first published by J?ns Jakob Berzelius in his system of atomic symbols (Thomas Thomson, Annals of Philosophy) and is a contraction of the element's new Latin name natrium which refers to the Egyptian natron, the word for a natural mineral salt whose primary ingredient is hydrated sodium carbonate. Hydrated sodium carbonate historically had several important industrial and household uses later eclipsed by soda ash, baking soda and other sodium compounds.
Although Sodium (sometimes called "soda" in English) has long been recognized in compounds, it was not isolated until 1807 by Sir Humphry Davy through the electrolysis of caustic soda.
 Sodium imparts an intense yellow color to flames. As early as 1860, Kirchhoff and Bunsen noted the high sensitivity that a flame test for sodium could give.

Specification

The Sodium is an organic compound with the formula Na. The IUPAC name of this chemical is sodium. With the CAS registry number 7440-23-5, it is also named as Sodium metal. The product's categories are Inorganics; ACS Grade Synthetic Reagents; Essential Chemicals; Routine Reagents; Alkali Metals Metal and Ceramic Science; Metals; Reduction; Synthetic Reagents. Besides, it is light, soft silver metal.It is  an element that is a member of the alkali group of metals. It has the atomic symbol Na, atomic number 11, and atomic weight 23. With a valence of 1, it has a strong affinity for oxygen and other nonmetallic elements. Sodium provides the chief cation of the extracellular body fluids. Its salts are the most widely used in medicine. (From Dorland, 27th ed) Physiologically the sodium ion plays a major role in blood pressure regulation, maintenance of fluid volume, and electrolyte balance.

Preparation of Sodium:
this chemical was first produced commercially in 1855 by thermal reduction of sodium carbonate with carbon at 1100 °C, in what is known as the Deville process.
Na2CO3 (l) + 2 C (s) → 2 Na (g) + 3 CO (g)

Uses of Sodium:
Sodium in its metallic form can be used to refine some reactive metals, such as zirconium and potassium, from their compounds. In certain alloys to improve their structure. It is used to descale metal (make its surface smooth) and purify molten metals. In sodium vapor lamps, an efficient means of producing light from electricity, often used for street lighting in cities. Low-pressure sodium lamps give a distinctive yellow-orange light which consists primarily of the twin sodium D lines. High-pressure sodium lamps give a more natural peach-colored light, composed of wavelengths spread much more widely across the spectrum. It is used as a heat transfer fluid in some types of nuclear reactors and inside the hollow valves of high-performance internal combustion engines. In organic synthesis, sodium is used as a reducing agent, for example in the Birch reduction. In chemistry, sodium is often used either alone or with potassium in an alloy, NaK as a desiccant for drying solvents. Used with benzophenone, it forms an intense blue coloration when the solvent is dry and oxygen-free. The sodium fusion test uses sodium's high reactivity, low melting point, and the near-universal solubility of its compounds, to qualitatively analyze compounds.

When you are using Sodium, please be cautious about it as the following:
It reacts violently with water, liberating extremely flammable gases. Please keep container tightly closed. In case of contact with eyes, rinse immediately with plenty of water and seek medical advice. Besides, this chemical can cause burns and may cause cancer. When you are using it, avoid exposure - obtain special instructions before use. In case of accident or if you feel unwell seek medical advice immediately (show the label where possible).

You can still convert the following datas into molecular structure:
(1)SMILES: [Na]
(2)InChI: InChI=1/Na CopyCopied
(3)InChIKey: KEAYESYHFKHZAL-UHFFFAOYAO
(4)Std. InChI: InChI=1S/Na
(5)Std. InChIKey: KEAYESYHFKHZAL-UHFFFAOYSA-N

The toxicity data of Sodium is as follows:

Organism Test Type Route Reported Dose (Normalized Dose) Effect Source
mouse LD50 intraperitoneal 4gm/kg (4000mg/kg)   "Structure et Activite Pharmacodyanmique des Medicaments du Systeme Nerveux Vegetatif," Bovet, D., and F. Bovet-Nitti, New York, S. Karger, 1948Vol. -, Pg. 704, 1948.