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{{distinguish|nitrourea}}
{{chembox
{{chembox
| Verifiedfields = changed
| Verifiedfields = changed
| Watchedfields = changed
| Watchedfields = changed
| verifiedrevid = 426796341
| verifiedrevid = 426796341
| Name =
| ImageFile = Urea nitrate.png
| ImageName = Structural formulae of the ions in urea nitrate
| ImageFile = Urea nitrate.png
| ImageName = Structural formulae of the ions in urea nitrate
| ImageFile1 = Urea-nitrate-3D-balls.png
| ImageFile1 = Urea-nitrate-3D-balls.png
| ImageSize1 = 220px
| ImageName1 = Ball-and-stick models of the ions in urea nitrate
| ImageSize1 = 220px
| ImageName1 = Ball-and-stick models of the ions in urea nitrate
| IUPACName =
| IUPACName =
| OtherNames =
| OtherNames =
| SystematicName =
|Section1={{Chembox Identifiers
| Section1 = {{Chembox Identifiers
| CASNo_Ref = {{cascite|changed|??}}
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo = 124-47-0
| CASNo = 124-47-0
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = DHJ35702MG
| PubChem = 31295
| PubChem = 31295
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
Line 24: Line 29:
| StdInChIKey = AYTGUZPQPXGYFS-UHFFFAOYSA-N
| StdInChIKey = AYTGUZPQPXGYFS-UHFFFAOYSA-N
}}
}}
|Section2={{Chembox Properties
| Section2 = {{Chembox Properties
| C=1 | H=5 | N=3 | O=4
| Formula = CH<sub>5</sub>N<sub>3</sub>O<sub>4</sub>
| MolarMass = 123.068 g/mol
| Appearance =
| Appearance =
| Density = 1.69&nbsp;g/cm<sup>3</sup>
| Density = 1.67±0.011&nbsp;g/cm<sup>3</sup><ref name="Characterization" />
| MeltingPtC = 163
| MeltingPtC = 157-159
| BoilingPt =
| BoilingPt =
| Solubility = 167.2±0.5 mg/mL<ref name="Characterization">{{cite journal | doi = 10.1002/prep.201200178 | title = Synthesis and Characterization of Urea Nitrate and Nitrourea | date = 2013 | last1 = Oxley | first1 = Jimmie C. | last2 = Smith | first2 = James L. | last3 = Vadlamannati | first3 = Sravanthi | last4 = Brown | first4 = Austin C. | last5 = Zhang | first5 = Guang | last6 = Swanson | first6 = Devon S. | last7 = Canino | first7 = Jonathan | journal = Propellants, Explosives, Pyrotechnics | volume = 38 | issue = 3 | pages = 335–344 }}</ref>
| Solubility = 15 g/100 g
|Solubility1 = 14.2±0.1 mg/mL<ref name="Characterization" />
| SolubleOther = soluble in alcohol<ref>http://cameochemicals.noaa.gov/chemical/12966</ref>}}
|Solvent1 = Ethanol
|Section3={{Chembox Hazards
|Solubility2 = 10.4±0.2 mg/mL<ref name="Characterization" />
| MainHazards =
| FlashPt =
|Solvent2 = Acetone
|Solubility3 = 54.8±0.9 mg/mL<ref name="Characterization" />
| AutoignitionPt =In the name of Allah the most beneficient
|Solvent3 = Methanol
the merciful.
| SolubleOther = }}

| Section3 =
Some Chemical Equations
| Section4 = {{Chembox Explosive
Introduction
| ShockSens = Low
Here are some equations:
| FrictionSens = Low
Equations
| DetonationV = 4700 m/s
eq. no Equations
| REFactor = }}
2H2+O2→2H2O
| Section5 = {{Chembox Hazards
C+O2→CO2
| GHSPictograms = {{GHS01}} {{GHS03}} {{GHS05}}
CuSO4+Fe→FeSO4+Cu
| GHSSignalWord = '''DANGER'''
AlCl3+Fe→FeCl3+Al
| HPhrases = {{H-phrases|201|271|301|304|314|332}}
CaCl2+Cl2+C→CCl4+Ca
| PPhrases = {{P-phrases|220|233|260|250|305+351+338}}
4Na+O2→2Na2O
| NFPA-F = 1
Fe+S→FeS
| NFPA-H = 2
2Fe+O2→2FeO
| NFPA-R = 3
2Zn+O2→2ZnO
CaO+CO2→CaCO3
H2+I2→2HI
H2+F2→2HF
H2+Cl2→2HCl
H2+Br2→2HBr
2Pb+O2→2PbO
SiO2+4Na→Na2O+Si
2H2+C→CH4
N2+3H­2→2NH3
2C+H2→C2H2
C2H5OH→H2O+C2H4­
CO2+SO2→2O2+C+S
Cs2(SO4)3+3H2→3H2SO4+2Cs
2NaOH+H2+Cl2→2NaCl+2H2O
H2S+Fe→FeS+H2
CaCl2+2Na→Ca+2NaCl
CaSO4+Cu→CuSO4+Ca
Reaction of Acid with metal oxide
Acids react with metal oxides to form salt and water. There are some of such equations:
27. FeO+H2SO4→FeSO4+H2O
28. ZnO+2HCl→ZnCl2+H2O
29. CuO+2HNO3→H2O+Cu(NO3)2
30. PbO+2HNO3→Pb(NO3)2+H2O
31. Na2O+2HNO3→H2O+2NaNO3
32. FeO+2HNO3→Fe(NO3)2+H2O
33. ZnO+2HNO3→H2O+Zn(NO3)2
34. FeO+2HCl→FeCl2+H2O
35. ZnO+H2SO4→ZnSO4+H2O
36. CuO+2HCl→CuCl2+H2O
37. PbO+2HCl→PbCl2+H2O
38. Na2O+2HCl→2NaCl+H2O
39. CaO+2HCl→CaCl2+H2O
40. MgO+2HCl→MgCl2+H2O
41. CuO+H2SO4→CuSO4
42. PbO+H2SO4→PbSO4+H2O
43. Na2O+H2SO4→Na2SO4+H2O
44. CaO+H2SO4→CaSO4+H2O
45. MgO+H2SO4→MgSO4+H2O
Reaction of Acid with metal
Acids react with metals to give salt and water. Some chemical equations are given below:
46. H2SO4+Cu→CuSO4+H2
47. H2SO4+Zn→ZnSO4+H2
48. 2HCl+Ca→CaCl2+H2
49. 2HCl+Mg→MgCl2+H2
50. Fe+2HNO3→Fe(NO3­)2+H2O
Reaction to prepare ozone artfically
Scientists tell us that the formula of ozone is O3. This layer protects the Earth from radioactive rays (which are alpha, beta and gamma rays). The equation to prepare ozone artifially:
2O2+O2→2O3
Reaction to estinguish fire
In the burning fire process it happens by reaction of oxygen gas (O2) and carbon/sulphur. To lit fire we first have to remove carbon/sulphur. Here is an equation to lit fire:
CO2+2H2→2H2O+C
Or
SO2+2Ca→2CaO+S
Redox reactions to remove greenhouse gases
Reactions in which oxidation state or oxidation number (a partial charge assigned to a substance) changes are called oxidation-reduction or redox reactions.
When rays of the Sun reach the Earth's atmosphere, some of them hit dust particles, and some are reflected by them. Some hit the clouds are absorbed by them. Some gases help the rays that not go back to space. The gases are called greenhouse gases. This whole process (excluding the definition of redox reactions) is called Greenhouse effect. Carbondioxide (CO2), Methane (CH4) and Nitrous oxide (N2O) are some important greenhouse gases. I will tell you how to make these gases useful. Here are equations to make these gases harmless:
N2O+2O2+H2O+2CaO→2CaNO3+H2+O2
CH4+C+3O2+CaO→2CaCO3+H2O
CO2+H2O+NaOH→H2O+NaHCO3
}}
}}
| Section6 =
}}
}}
[[File:Urea nitrate (IV).jpg|thumb|Crystals of urea nitrate]]
'''Urea nitrate''' is a fertilizer-based [[high explosive]] that has been used in [[improvised explosive device]]s in [[Afghanistan]], [[Pakistan]], [[Iraq]], and various other [[terrorism|terrorist]] acts elsewhere in the world, like the [[1993 World Trade Center bombings]].<ref name="wired">{{cite news|
'''Urea nitrate''' is a fertilizer-based [[high explosive]] that has been used in [[improvised explosive device]]s in [[Afghanistan]], [[Pakistan]], [[Iraq]], and various [[terrorism|terrorist]] acts elsewhere in the world such as in the [[1993 World Trade Center bombings]].<ref name="wired">{{cite news|
url=http://blog.wired.com/wiredscience/2007/09/spray-on-test-f.html|
url=http://blog.wired.com/wiredscience/2007/09/spray-on-test-f.html|
title=Chem Lab: Spray-On Test for Improvised Explosives|
title=Chem Lab: Spray-On Test for Improvised Explosives|
author=Aaron Rowe|
author=Aaron Rowe|
publisher=Wired
publisher=Wired
| date =18 September 2007}}</ref> It has a destructive power similar to better-known [[ammonium nitrate]] explosives, with a [[velocity of detonation]] between {{convert|11155|ft/s|m/s|abbr=on}} and {{convert|15420|ft/s|m/s|abbr=on}}.<ref name="globalsecurity">{{cite web|
| date =18 September 2007}}</ref> It has a destructive power similar to better-known [[ammonium nitrate]] explosives, with a [[velocity of detonation]] between {{convert|11155|ft/s|m/s|abbr=on|order=flip}} and {{convert|15420|ft/s|m/s|abbr=on|order=flip}}.<ref name="globalsecurity">{{cite web|
url=http://www.globalsecurity.org/military/systems/munitions/explosives-anfo.htm|
url=http://www.globalsecurity.org/military/systems/munitions/explosives-anfo.htm|
title=Explosives - ANFO (Ammonium Nitrate - Fuel Oil)|
title=Explosives - ANFO (Ammonium Nitrate - Fuel Oil)|
publisher=GlobalSecurity.org}}</ref>
publisher=GlobalSecurity.org}}</ref> It has chemical formula of {{chem2|CH5N3O4}} or {{chem2|(NH2)2COHNO3}}.


Urea nitrate is produced in one step by reaction of [[urea]] with [[nitric acid]]. This is an [[exothermic reaction]], so steps must be taken to control the temperature.
Urea nitrate is produced in one step by reaction of [[urea]] with [[nitric acid]]. This is an [[exothermic reaction]], so steps must be taken to control the temperature.


Urea nitrate explosions may be initiated using a blasting cap.<ref name="globalsecurity" />
Urea nitrate explosions may be initiated using a [[blasting cap]].<ref name="globalsecurity" />


==Chemistry==
==Chemistry==
Urea contains a [[Carbonyl|carbonyl group]]. The more electronegative oxygen atom pulls electrons away from the carbon forming a greater electron density around the oxygen, giving the oxygen a partial negative charge and forming a polar bond. When nitric acid is presented, it ionizes. A hydrogen cation contributed by the acid is attracted to the oxygen and forms a covalent bond [electrophile H<sup>+</sup>]. The electronegative NO<sub>3</sub><sup>−</sup> ion then is attracted to the positive hydrogen ion. This forms an ionic bond and hence the compound urea nitrate.
Urea contains a [[Carbonyl|carbonyl 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.


:{{chem2 | (NH2)2CO (aq) + HNO3 (aq) -> [(NH2)2COH]+[NO3]− (s) }}
(NH<sub>2</sub>)<sub>2</sub>CO (aq) + HNO<sub>3</sub> (aq) → (NH<sub>2</sub>)<sub>2</sub>COHNO<sub>3</sub> (s)


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.
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.
Line 139: Line 86:


==Further reading==
==Further reading==
* {{cite journal |vauthors=Almog J, Burda G, Shloosh Y, Abramovich-Bar S, Wolf E, Tamiri T |title=Recovery and detection of urea nitrate in traces |journal=J. Forensic Sci. |volume=52 |issue=6 |pages=1284–90 |date=November 2007 |pmid=17868267 |doi=10.1111/j.1556-4029.2007.00551.x |url=}}
*{{cite journal |vauthors=Almog J, Burda G, Shloosh Y, Abramovich-Bar S, Wolf E, Tamiri T |title=Recovery and detection of urea nitrate in traces |journal=J. Forensic Sci. |volume=52 |issue=6 |pages=1284–90 |date=November 2007 |pmid=17868267 |doi=10.1111/j.1556-4029.2007.00551.x |s2cid=10228717 }}
* {{cite journal |author=Mr.X |title=Improvised Urea Nitrate |journal=aware eZine Gamma |date=July 2008 |url=http://www.awarenetwork.org/etc/gamma/?x=5}}
*{{cite journal |author=Mr.X |title=Improvised Urea Nitrate |journal=Aware EZine Gamma |date=July 2008 |url=http://www.awarenetwork.org/etc/gamma/?x=5 |access-date=2008-11-11 |archive-url=https://web.archive.org/web/20080920082234/http://www.awarenetwork.org/etc/gamma/?x=5 |archive-date=2008-09-20 |url-status=dead }}


==External links==
[[File:Urea nitrate (IV).jpg|thumb|Urea nitrate]]
*{{Commonscatinline}}


[[Category:Explosive chemicals]]
[[Category:Explosive chemicals]]
[[Category:Nitrates]]
[[Category:Nitrates]]
[[Category:Ureas]]
[[Category:Ureas]]


{{explosive-stub}}

Latest revision as of 18:13, 3 April 2024

Not to be confused with nitrourea.
Urea nitrate
Structural formulae of the ions in urea nitrate
Ball-and-stick models of the ions in urea nitrate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.004.276 Edit this at Wikidata
UNII
  • InChI=1S/CH4N2O.HNO3/c2*2-1(3)4/h(H4,2,3,4);(H,2,3,4) ☒N
    Key: AYTGUZPQPXGYFS-UHFFFAOYSA-N ☒N
  • InChI=1/CH4N2O.HNO3/c2*2-1(3)4/h(H4,2,3,4);(H,2,3,4)
    Key: AYTGUZPQPXGYFS-UHFFFAOYAL
  • C(=O)(N)N.[N+](=O)(O)[O-]
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 in Ethanol 14.2±0.1 mg/mL[1]
Solubility in Acetone 10.4±0.2 mg/mL[1]
Solubility in Methanol 54.8±0.9 mg/mL[1]
Explosive data
Shock sensitivity Low
Friction sensitivity Low
Detonation velocity 4700 m/s
Hazards
GHS labelling:
GHS01: Explosive GHS03: Oxidizing GHS05: Corrosive
Danger
H201, H271, H301, H304, H314, H332
P220, P233, P250, P260, P305+P351+P338
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g. hydrogen peroxideSpecial hazards (white): no code
2
1
3
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)
Crystals of urea nitrate

Urea nitrate is a fertilizer-based high explosive that has been used in improvised explosive devices in Afghanistan, Pakistan, Iraq, and various terrorist acts elsewhere in the world such as in the 1993 World Trade Center bombings.[2] It has a destructive power similar to better-known ammonium nitrate explosives, with a velocity 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 of CH5N3O4 or (NH2)2COHNO3.

Urea nitrate is produced in one step by reaction of urea with nitric acid. This is an exothermic reaction, so steps must be taken to control the temperature.

Urea nitrate explosions may be initiated using a blasting cap.[3]

Chemistry

[edit]

Urea contains a carbonyl 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.

(NH2)2CO (aq) + HNO3 (aq) → [(NH2)2COH]+[NO3]− (s)

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.

References

[edit]
  1. ^ a b c d e Oxley, Jimmie C.; Smith, James L.; Vadlamannati, Sravanthi; Brown, Austin C.; Zhang, Guang; Swanson, Devon S.; Canino, Jonathan (2013). "Synthesis and Characterization of Urea Nitrate and Nitrourea". Propellants, Explosives, Pyrotechnics. 38 (3): 335–344. doi:10.1002/prep.201200178.
  2. ^ Aaron Rowe (18 September 2007). "Chem Lab: Spray-On Test for Improvised Explosives". Wired.
  3. ^ a b "Explosives - ANFO (Ammonium Nitrate - Fuel Oil)". GlobalSecurity.org.

Further reading

[edit]
[edit]
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