Ammonium nitrate

Ammonium nitrate
Structural formula
Ammonium nitrate crystal structure
Sample of white powder and spherules
Names
IUPAC name
Ammonium nitrate
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.026.680 Edit this at Wikidata
EC Number
  • 229-347-8
RTECS number
  • BR9050000
UNII
UN number 0222with > 0.2% combustible substances
1942with ≤ 0.2% combustible substances
2067fertilizers
2426liquid
  • InChI=1S/NO3.H3N/c2-1(3)4;/h;1H3/q-1;/p+1 checkY
    Key: DVARTQFDIMZBAA-UHFFFAOYSA-O checkY
  • InChI=1/NO3.H3N/c2-1(3)4;/h;1H3/q-1;/p+1
    Key: DVARTQFDIMZBAA-IKLDFBCSAH
  • [O-][N+]([O-])=O.[NH4+]
Properties
NH4NO3
Molar mass 80.043 g/mol
Appearance white crystalline solid
Density 1.725 g/cm3 (20 °C)
Melting point 169.6 °C (337.3 °F; 442.8 K)
Boiling point approx. 210 °C (410 °F; 483 K) decomposes
Endothermic
118 g/100 ml (0 °C)
150 g/100 ml (10 °C)
192 g/100 ml (20 °C)
297 g/100 ml (40 °C)
410 g/100 ml (60 °C)
576 g/100 ml (80 °C)
1024 g/100 ml (100 °C)[1]
−33.6×10−6 cm3/mol
Structure
orthorhombic[2]
Explosive data
Shock sensitivity very low
Friction sensitivity very low
Detonation velocity 2500 m/s
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Explosive, Oxidizer
GHS labelling:
GHS07: Exclamation mark GHS03: Oxidizing GHS01: Explosive
Danger
H201, H271, H319
P220, P221, P264, P271, P280, P372
NFPA 704 (fire diamond)
Lethal dose or concentration (LD, LC):
2085–5300 mg/kg (oral in rats, mice)[3]
Related compounds
Other anions
Ammonium nitrite
Other cations
Sodium nitrate
Potassium nitrate
Hydroxylammonium nitrate
Related compounds
Ammonium perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Ammonium nitrate is a chemical compound with the formula NH4NO3. It is a white crystalline salt consisting of ions of ammonium and nitrate. It is highly soluble in water and hygroscopic as a solid, although it does not form hydrates. It is predominantly used in agriculture as a high-nitrogen fertilizer.[5]

Its other major use is as a component of explosive mixtures used in mining, quarrying, and civil construction. It is the major constituent of ANFO, a popular industrial explosive which accounts for 80% of explosives used in North America; similar formulations have been used in improvised explosive devices.

Many countries are phasing out its use in consumer applications due to concerns over its potential for misuse.[6] Accidental ammonium nitrate explosions have killed thousands of people since the early 20th century.[6][7] Global production was estimated at 21.6 million tonnes in 2017.[8] By 2021, global production of ammonium nitrate was down to 16.7 million tonnes.[7]

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  2. ^ Kaniewski, Maciej; Huculak-Mączka, Marta; Zieliński, Jakub; Biegun, Marcin; Hoffmann, Krystyna; Hoffmann, Józef (2021). "Crystalline Phase Transitions and Reactivity of Ammonium Nitrate in Systems Containing Selected Carbonate Salts". Crystals. 11 (10): 1250. doi:10.3390/cryst11101250. ISSN 2073-4352.
  3. ^ Martel, B.; Cassidy, K. (2004). Chemical Risk Analysis: A Practical Handbook. Butterworth–Heinemann. p. 362. ISBN 1-903996-65-1.
  4. ^ "Hazard Rating Information for NFPA Fire Diamonds". Archived from the original on 17 February 2015. Retrieved 13 March 2015.
  5. ^ Zapp, Karl-Heinz (2012). "Ammonium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a02_243. ISBN 9783527303854.
  6. ^ a b Ammonium nitrate sold by ton as U.S. regulation is stymied. Archived 28 February 2018 at the Wayback MachineThe Dallas Morning News
  7. ^ a b "Ammonium nitrate production by country, 2023 - knoema.com". Knoema.
  8. ^ "Ammonium nitrate production by country, 2019". Knoema. Retrieved 14 August 2020.