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| Identifiers | |
|---|---|
| |
3D model (JSmol) | |
| ChemSpider |
|
| ECHA InfoCard | 100.004.276 |
| UNII | |
| |
| |
| Properties | |
| CH5N3O4 | |
| Molar mass | 123.068 g·mol−1 |
| Density | 1.67±0.011 g/cm3[1] |
| Melting point | 157–159 °C (315–318 °F; 430–432 K) |
| 167.2±0.5 mg/mL[1] | |
| Solubility inEthanol | 14.2±0.1 mg/mL[1] |
| Solubility inAcetone | 10.4±0.2 mg/mL[1] |
| Solubility inMethanol | 54.8±0.9 mg/mL[1] |
| Explosive data | |
| Shock sensitivity | Low |
| Friction sensitivity | Low |
| Detonation velocity | 4700 m/s |
| Hazards | |
| GHS labelling: | |
   | |
| Danger | |
| H201,H271,H301,H304,H314,H332 | |
| P220,P233,P250,P260,P305+P351+P338 | |
| NFPA 704 (fire diamond) | |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
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Urea nitrate is a fertilizer-basedhigh explosive that has been used inimprovised explosive devices inAfghanistan,Pakistan,Iraq, and variousterrorist acts elsewhere in the world such as in the1993 World Trade Center bombings.[2] It has a destructive power similar to better-knownammonium nitrate explosives, with avelocity of detonation between 3,400 m/s (11,155 ft/s) and 4,700 m/s (15,420 ft/s).[3] It has chemical formula ofCH5N3O4 or(NH2)2COHNO3.
Urea nitrate is produced in one step by reaction ofurea withnitric acid. This is anexothermic reaction, so steps must be taken to control the temperature.
It was discovered in 1797 byWilliam Cruickshank,[4] inventor of theChloralkali process.
Urea nitrate explosions may be initiated using ablasting cap.[3]
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Urea contains acarbonyl group. The more electronegative oxygen atom pulls electrons away from the carbon atom, forming a polar bond with greater electron density around the oxygen atom, giving it a partial negative charge. In a simplistic sense, nitric acid dissociates in aqueous solution into protons (hydrogen cations) and nitrate anions. The electrophilic proton contributed by the acid is attracted to the negatively charged oxygen atom on the urea molecule and the two form a covalent bond. The formed O-H bond is stabilized into a hydroxyl group when the oxygen abstracts an electron pair away from the central carbon atom, which leads to bond resonance between it and the two amino groups. As such, the urea cation can be thought of as a amidinium species. Paired with the spectator nitrate counteranion, it forms urea nitrate.
The compound is favored by many amateur explosive enthusiasts as a principal explosive for use in larger charges. In this role it acts as a substitute for ammonium nitrate based explosives. This is due to the ease of acquiring the materials necessary to synthesize it, and its greater sensitivity to initiation compared to ammonium nitrate based explosives.[5]
Media related toUrea nitrate at Wikimedia Commons
