Difference between revisions of "Sodium azide"
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| − | '''Sodium azide''' is a sodium salt with the chemical formula NaN<sub>3</sub>. | + | {{Chembox |
| + | | Name = Sodium azide | ||
| + | | Reference = | ||
| + | | IUPACName = Sodium azide | ||
| + | | PIN = | ||
| + | | SystematicName = Sodium azide | ||
| + | | OtherNames = Azium<br>Sodium trinitride<br>Smite | ||
| + | <!-- Images --> | ||
| + | | ImageFile = Sodium azide bottle and sample.jpg | ||
| + | | ImageSize = 250 | ||
| + | | ImageAlt = | ||
| + | | ImageCaption = Sodium azide sample | ||
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| + | <!-- Sections --> | ||
| + | | Section1 = {{Chembox Identifiers | ||
| + | | 3DMet = | ||
| + | | Abbreviations = | ||
| + | | SMILES = [N-]=[N+]=[N-].[Na+] | ||
| + | }} | ||
| + | | Section2 = {{Chembox Properties | ||
| + | | AtmosphericOHRateConstant = | ||
| + | | Appearance = White solid | ||
| + | | BoilingPt = | ||
| + | | BoilingPtC = | ||
| + | | BoilingPt_ref = | ||
| + | | BoilingPt_notes = Violent decomposition | ||
| + | | Density = 1.846 g/cm<sup>3</sup> (20 °C) | ||
| + | | Formula = NaN<sub>3</sub> | ||
| + | | HenryConstant = | ||
| + | | LogP = | ||
| + | | MolarMass = 65.0099 g/mol | ||
| + | | MeltingPt = | ||
| + | | MeltingPtC = 275 | ||
| + | | MeltingPt_ref = | ||
| + | | MeltingPt_notes = (violent decomposition) | ||
| + | | Odor = Odorless | ||
| + | | pKa = 4.8 | ||
| + | | pKb = | ||
| + | | Solubility = 38.9 g/100 m; (0 °C)<br>40.8 g/100 m; (20 °C)<br>55.3 g/100 m; (100 °C) | ||
| + | | SolubleOther = Very soluble in anhydrous [[ammonia]]<br>Slightly soluble in [[benzene]]<br>Insoluble in [[acetone]], [[chloroform]], [[diethyl ether]], [[hexane]], [[toluene]] | ||
| + | | Solubility1 = 2.48 g/100 m; (25 °C) | ||
| + | | Solvent1 = methanol | ||
| + | | Solubility2 = 0.22 g/100 m; (0 °C) | ||
| + | | Solvent2 = ethanol | ||
| + | | Solvent = | ||
| + | | VaporPressure = ~0 mmHg | ||
| + | }} | ||
| + | | Section3 = {{Chembox Structure | ||
| + | | Coordination = | ||
| + | | CrystalStruct = Hexagonal | ||
| + | | MolShape = | ||
| + | }} | ||
| + | | Section4 = {{Chembox Thermochemistry | ||
| + | | DeltaGf = 99.4 kJ/mol | ||
| + | | DeltaHc = | ||
| + | | DeltaHf = 21.3 kJ/mol | ||
| + | | Entropy = 70.5 J·mol<sup>−1</sup>·K<sup>−1</sup> | ||
| + | | HeatCapacity = 76.6 J·mol<sup>−1</sup>·K<sup>−1</sup> | ||
| + | }} | ||
| + | | Section5 = {{Chembox Explosive | ||
| + | | ShockSens = | ||
| + | | FrictionSens = | ||
| + | | DetonationV = | ||
| + | | REFactor = | ||
| + | }} | ||
| + | | Section6 = {{Chembox Hazards | ||
| + | | AutoignitionPt = | ||
| + | | ExploLimits = | ||
| + | | ExternalMSDS = [http://www.sciencelab.com/msds.php?msdsId=9927588 ScienceLab] | ||
| + | | FlashPt = 300 °C | ||
| + | | LD50 = 27 mg/kg (oral, rats/mice) | ||
| + | | LC50 = | ||
| + | | MainHazards = Extremely toxic<br>Dangerous to environment | ||
| + | | NFPA-F = | ||
| + | | NFPA-H = | ||
| + | | NFPA-R = | ||
| + | | NFPA-S = | ||
| + | }} | ||
| + | | Section7 = {{Chembox Related | ||
| + | | OtherAnions = | ||
| + | | OtherCations = | ||
| + | | OtherFunction = | ||
| + | | OtherFunction_label = | ||
| + | | OtherCompounds = [[Lithium azide]]<br>[[Potassium azide]]<br>[[Rubidium azide]]<br>[[Caesium azide]] | ||
| + | }} | ||
| + | }} | ||
| + | '''Sodium azide''' is a sodium salt with the chemical formula '''NaN<sub>3</sub>'''. | ||
==Properties== | ==Properties== | ||
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Sodium azide will decompose at temperatures over 300°C to yield nitrogen gas. | Sodium azide will decompose at temperatures over 300°C to yield nitrogen gas. | ||
| − | :2 NaN<sub>3</sub> → | + | : 2 NaN<sub>3</sub> → 2 Na + 3 N<sub>2</sub> |
In contact with a strong acid will release [[hydrazoic acid]]. | In contact with a strong acid will release [[hydrazoic acid]]. | ||
| − | :NaN<sub>3</sub> + H<sup>+</sup> → HN<sub>3</sub> + Na<sup>+</sup> | + | : NaN<sub>3</sub> + H<sup>+</sup> → HN<sub>3</sub> + Na<sup>+</sup> |
Sodium azide can be destroyed by reacting it with [[nitrous acid]] | Sodium azide can be destroyed by reacting it with [[nitrous acid]] | ||
| − | :2 NaN<sub>3</sub> + 2 HNO<sub>2</sub> → 3 N<sub>2</sub> + 2 NO + 2 NaOH | + | : 2 NaN<sub>3</sub> + 2 HNO<sub>2</sub> → 3 N<sub>2</sub> + 2 NO + 2 NaOH |
===Physical=== | ===Physical=== | ||
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==Preparation== | ==Preparation== | ||
| − | Industrially sodium azide is prepared via "Wislicenus process", by reacting [[sodium amide]] with [[nitrous oxide]]. Sodium amide is prepared by reacting metallic sodium with anhydrous [[ammonia]]. | + | Industrially sodium azide is prepared via "Wislicenus process", by reacting [[sodium amide]] with [[nitrous oxide]]. Sodium amide is prepared by reacting metallic sodium with anhydrous [[ammonia]], in inert atmosphere. |
| − | :2 Na + 2 NH<sub>3</sub> → 2 NaNH<sub>2</sub> + H<sub>2</sub> | + | : 2 Na + 2 NH<sub>3</sub> → 2 NaNH<sub>2</sub> + H<sub>2</sub> |
| − | :2 NaNH<sub>2</sub> + N<sub>2</sub>O → NaN<sub>3</sub> + NaOH + NH<sub>3</sub> | + | : 2 NaNH<sub>2</sub> + N<sub>2</sub>O → NaN<sub>3</sub> + NaOH + NH<sub>3</sub> |
| − | As this method uses metallic sodium and inert conditions it is expensive for the amateur chemist. | + | As this method uses metallic sodium and inert conditions, it is expensive for the amateur chemist, though not impossible. Here's [https://www.youtube.com/watch?v=M-Ezs224YU8 one person] who managed to make it work. |
A less complex synthesis involves the reaction of a nitrite ester with hydrazine: | A less complex synthesis involves the reaction of a nitrite ester with hydrazine: | ||
| − | :R-ONO + N<sub>2</sub>H<sub>4</sub> + NaOH → NaN<sub>3</sub> + R-OH + 2 H<sub>2</sub>O | + | : R-ONO + N<sub>2</sub>H<sub>4</sub> + NaOH → NaN<sub>3</sub> + R-OH + 2 H<sub>2</sub>O |
Another method discussed involves the reaction of [[sodium nitrite]] with [[urea]] under controlled conditions. | Another method discussed involves the reaction of [[sodium nitrite]] with [[urea]] under controlled conditions. | ||
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===Disposal=== | ===Disposal=== | ||
| − | When disposed of, it must never be poured down the drain, as it will react to either copper or lead plumbing to yield hydrazoic acid. Hydrolysis can also occur in aqueous solutions, at certain pH. Sodium azide must be treated with nitrous acid before being discarded.<ref>http://www.bt.cdc.gov/agent/sodiumazide/basics/facts.asp</ref> | + | When disposed of, it must never be poured down the drain, as it will react to either copper or lead plumbing to yield hydrazoic acid. Hydrolysis can also occur in aqueous solutions, at certain pH. Sodium azide must be treated with [[nitrous acid]] before being discarded.<ref>http://www.bt.cdc.gov/agent/sodiumazide/basics/facts.asp</ref> Acidified sodium nitrite can also be used. |
| + | |||
| + | [[Sodium hypochlorite]] diluted solution (aka bleach) can also be used.<ref>https://www.ncbi.nlm.nih.gov/m/pubmed/20667654/</ref> | ||
==References== | ==References== | ||
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=253 Sodium Azide] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=253 Sodium Azide] | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=7553 Sodium nitrate/urea complex] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=7553 Sodium nitrate/urea complex] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=79308 Sodium azide toxicity] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=81633 Sodium Azide contact with metal] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=154258 How to verify/identify sodium azide?] | ||
[[Category:Chemical compounds]] | [[Category:Chemical compounds]] | ||
[[Category:Inorganic compounds]] | [[Category:Inorganic compounds]] | ||
[[Category:Sodium compounds]] | [[Category:Sodium compounds]] | ||
| + | [[Category:Nitrogen compounds]] | ||
[[Category:Azides]] | [[Category:Azides]] | ||
[[Category:Energetic materials]] | [[Category:Energetic materials]] | ||
[[Category:Things that can kill you very quickly]] | [[Category:Things that can kill you very quickly]] | ||
| + | [[Category:Blood agents]] | ||
| + | [[Category:Solids]] | ||
Latest revision as of 00:44, 31 December 2021
 Sodium azide sample
| |
| Names | |
|---|---|
| IUPAC name
Sodium azide
| |
| Systematic IUPAC name
Sodium azide | |
| Other names
Azium
Sodium trinitride Smite | |
| Identifiers | |
| Jmol-3D images | Image |
| |
| Properties | |
| NaN3 | |
| Molar mass | 65.0099 g/mol |
| Appearance | White solid |
| Odor | Odorless |
| Density | 1.846 g/cm3 (20 °C) |
| Melting point | 275 °C (527 °F; 548 K) (violent decomposition) |
| Boiling point | Violent decomposition |
| 38.9 g/100 m; (0 °C) 40.8 g/100 m; (20 °C) 55.3 g/100 m; (100 °C) | |
| Solubility | Very soluble in anhydrous ammonia Slightly soluble in benzene Insoluble in acetone, chloroform, diethyl ether, hexane, toluene |
| Solubility in methanol | 2.48 g/100 m; (25 °C) |
| Solubility in ethanol | 0.22 g/100 m; (0 °C) |
| Vapor pressure | ~0 mmHg |
| Acidity (pKa) | 4.8 |
| Thermochemistry | |
| Std molar
entropy (S |
70.5 J·mol−1·K−1 |
| Std enthalpy of
formation (ΔfH |
21.3 kJ/mol |
| Hazards | |
| Safety data sheet | ScienceLab |
| Flash point | 300 °C |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
27 mg/kg (oral, rats/mice) |
| Related compounds | |
| Related compounds
|
Lithium azide Potassium azide Rubidium azide Caesium azide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sodium azide is a sodium salt with the chemical formula NaN3.
Contents
Properties
Chemical
Sodium azide will decompose at temperatures over 300°C to yield nitrogen gas.
- 2 NaN3 → 2 Na + 3 N2
In contact with a strong acid will release hydrazoic acid.
- NaN3 + H+ → HN3 + Na+
Sodium azide can be destroyed by reacting it with nitrous acid
- 2 NaN3 + 2 HNO2 → 3 N2 + 2 NO + 2 NaOH
Physical
Sodium azide is a white odorless salt. Sodium azide is soluble in water (40.8 g/100 mL at 20 °C) and ammonia, but insoluble in acetone, ether, chloroform and hexane.
Availability
Sodium azide was used in the first car airbags, as the gas generator. It is usually mixed with either silica and iron(III) oxide so purification is required.
Preparation
Industrially sodium azide is prepared via "Wislicenus process", by reacting sodium amide with nitrous oxide. Sodium amide is prepared by reacting metallic sodium with anhydrous ammonia, in inert atmosphere.
- 2 Na + 2 NH3 → 2 NaNH2 + H2
- 2 NaNH2 + N2O → NaN3 + NaOH + NH3
As this method uses metallic sodium and inert conditions, it is expensive for the amateur chemist, though not impossible. Here's one person who managed to make it work.
A less complex synthesis involves the reaction of a nitrite ester with hydrazine:
- R-ONO + N2H4 + NaOH → NaN3 + R-OH + 2 H2O
Another method discussed involves the reaction of sodium nitrite with urea under controlled conditions.
Projects
- Generating pure nitrogen gas
- Preparation of pure sodium
Handling
Safety
Sodium azide is extremely toxic. The toxicity of azides is similar that of cyanides, the lethal dose for an adult human is around 0.7 g.
Storage
Sodium azide should be stored in spark-free containers, away from moisture or any acidic vapors.
Disposal
When disposed of, it must never be poured down the drain, as it will react to either copper or lead plumbing to yield hydrazoic acid. Hydrolysis can also occur in aqueous solutions, at certain pH. Sodium azide must be treated with nitrous acid before being discarded.[1] Acidified sodium nitrite can also be used.
Sodium hypochlorite diluted solution (aka bleach) can also be used.[2]
References
- ↑ http://www.bt.cdc.gov/agent/sodiumazide/basics/facts.asp
- ↑ https://www.ncbi.nlm.nih.gov/m/pubmed/20667654/
Relevant Sciencemadness threads
Categories:
- Chemical pages without CAS Registry Number
- Articles without EBI source
- Chemical pages without ChemSpiderID
- Chemical pages without DrugBank identifier
- Articles without KEGG source
- Articles without InChI source
- Articles without UNII source
- Articles containing unverified chemical infoboxes
- Chemical compounds
- Inorganic compounds
- Sodium compounds
- Nitrogen compounds
- Azides
- Energetic materials
- Things that can kill you very quickly
- Blood agents
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