Ammonium dinitramide

{{chembox

| Verifiedfields = changed

| verifiedrevid = 477366559

| ImageFile = Ammonium dinitramide.png

| ImageSize = 220px

| IUPACName = Azanium dinitroazanide

| OtherNames = {{ubl|Ammonium dinitroazanide{{Cite web |title=Ammonium dinitramide |url=https://pubchem.ncbi.nlm.nih.gov/compound/10219428 |access-date=2024-07-18 |website=pubchem.ncbi.nlm.nih.gov}}|Ammonium dinitramide}}

|Section1={{Chembox Identifiers

| CASNo_Ref = {{cascite|correct|PubChem}}

| CASNo = 140456-78-6

| EC_number = 604-184-9

| MeSHName =

| PubChem = 10219428

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| ChemSpiderID = 8394920

| UNII = 8JCB80Q5K1

| SMILES = [NH4+].[N-]([N+](=O)[O-])[N+](=O)[O-]

| InChI = 1/N3O4.H3N/c4-2(5)1-3(6)7;/h;1H3/q-1;/p+1

| InChIKey = BRUFJXUJQKYQHA-IKLDFBCSAM

| StdInChI_Ref = {{stdinchicite|correct|chemspider}}

| StdInChI = 1S/N3O4.H3N/c4-2(5)1-3(6)7;/h;1H3/q-1;/p+1

| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

| StdInChIKey = BRUFJXUJQKYQHA-UHFFFAOYSA-O

}}

|Section2={{Chembox Properties

| Formula = {{chem2|[NH4][N(NO2)2]}}

| H=4 | N=4 | O=4

| MolarMass = 124.06 g/mol

| Appearance =

| Density = 1.81 g/cm³

| MeltingPtC = 93

| BoilingPt = decomposes at {{convert|127|C|F K|abbr=on}}

| Solubility =

}}

| Section3 = {{Chembox Structure

| Structure_ref =

| CrystalStruct =

| SpaceGroup =

| PointGroup =

| LattConst_a = 6.914 Å

| LattConst_b = 11.787 Å

| LattConst_c = 5.614 Å

| LattConst_alpha = 90.00

| LattConst_beta = 100.40

| LattConst_gamma = 90.00

| UnitCellFormulas = 4

}}

| Section4 = {{Chembox Thermochemistry

| DeltaGf = −150.6 kJ/mol

| DeltaHf= −148 kJ/mol

}}

|Section6={{Chembox Explosive

| ShockSens = Low{{cite journal |last1=Östmark |first1=H. |last2=Bemm |first2=U. |last3=Langlet |first3=A. |last4=Sandén |first4=R. |last5=Wingborg |first5=N. |title=The properties of ammonium dinitramide (ADN): Part 1, basic properties and spectroscopic data |journal=Journal of Energetic Materials |date=1 June 2000 |volume=18 |issue=2–3 |pages=123–138 |doi=10.1080/07370650008216116 |bibcode=2000JEnM...18..123O |s2cid=94304770 |url=https://www.tandfonline.com/doi/abs/10.1080/07370650008216116 |issn=0737-0652|url-access=subscription }}

| FrictionSens = Low

| DetonationV =

| REFactor = }}

|Section7={{Chembox Hazards

| GHSPictograms = {{GHS01}}{{GHS02}}{{GHS07}}{{GHS08}}

| GHSSignalWord = Danger

| HPhrases = {{H-phrases|201|228|302|371}}

| PPhrases = {{P-phrases|210|230|240|241|250|260|264|270|280|301+312|309+311|330|370+378|370+380|372|373|401|405|501}}

| MainHazards =

| FlashPt =

| AutoignitionPt =

| NIOSH_id = 7175

}}

|Section8= {{Chembox Related

| OtherAnions =

| OtherCations = Guanylurea dinitramide

| OtherFunction =

| OtherFunction_label =

| OtherCompounds =

}}

Ammonium dinitramide (ADN) is an inorganic compound with the chemical formula {{chem2|[NH4][N(NO2)2]|auto=1}}. It is the ammonium salt of dinitraminic acid {{chem2|HN(NO2)2}}. It consists of ammonium cations {{chem2|[NH4]+}} and dinitramide anions {{chem2|−N(NO2)2}}. ADN decomposes under heat to leave only nitrogen, oxygen, and water.

It makes an excellent solid rocket oxidizer with a slightly higher specific impulse than ammonium perchlorate and, more importantly, does not leave corrosive hydrogen chloride fumes. This property is also of military interest because halogen-free smoke is harder to detect. It decomposes into low-molecular-mass gases, which contributes to higher performance without creating excessive temperatures if used in gun or rocket propellants. However, the dinitramide salt is more prone to detonation under high temperatures and shock compared with the perchlorate.

The Eurenco Bofors company produced LMP-103S as a 1-to-1 substitute for hydrazine by dissolving 65% ammonium dinitramide, {{chem2|[NH4]N(NO2)2}}, in 35% water solution of methanol and ammonia. LMP-103S has 6% higher specific impulse and 30% higher impulse density than hydrazine monopropellant. Additionally, hydrazine is highly toxic and carcinogenic, while LMP-103S is only moderately toxic. LMP-103S is UN Class 1.4S, allowing for transport on commercial aircraft, and was demonstrated on the Prisma satellite in 2010. Special handling is not required. LMP-103S could replace hydrazine as the most commonly used monopropellant.{{Cite web |title=Green propellant LMP 103S |url=https://www.ecaps.se/rocket-fuel-1 |access-date=2024-04-25 |website=ecaps.se}}{{Cite journal |last1=Persson |first1=Mathias |last2=Anflo |first2=Kjell |last3=Friedhoff |first3=Pete |date=2019 |title=Flight Heritage of Ammonium Dinitramide (ADN) Based High Performance Green Propulsion (HPGP) Systems |url=https://onlinelibrary.wiley.com/doi/10.1002/prep.201900248 |journal=Propellants, Explosives, Pyrotechnics |volume=44 |issue=9 |pages=1073–1079 |doi=10.1002/prep.201900248 |issn=0721-3115|url-access=subscription }}

The ADN-based monopropellant FLP-106 is reported to have improved properties relative to LMP-103S, including higher performance (ISP of 259 s vs. 252 s) and density (1.362 g/cm³ vs. 1.240 g/cm³).{{Cite book |last1=Larsson |first1=Anders |url=http://www.intechopen.com/books/advances-in-spacecraft-technologies |title=Advances in Spacecraft Technologies |last2=Wingborg |first2=Niklas |date=2011-02-14 |publisher=InTech |isbn=978-953-307-551-8 |editor-last=Hall |editor-first=Jason |chapter=Green Propellants Based on Ammonium Dinitramide (ADN) |doi=10.5772/13640 |chapter-url=https://cdn.intechopen.com/pdfs/13473/InTech-Green_propellants_based_on_ammonium_dinitramide_adn_.pdf |doi-access=free}}

History

Ammonium dinitramide was invented in 1971 at the Zelinsky Institute of Organic Chemistry in the USSR. Initially all information related to this compound was classified because of its use as a rocket propellant, particularly in Topol-M intercontinental ballistic missiles. In 1989 ammonium dinitramide was independently synthesized at SRI International.{{cite web |url=http://www.sri.com/psd/research/adn.html |title=Dinitramide Salts: ADN Plus Other Salts |publisher=SRI International |accessdate=2012-04-15 |url-status=dead |archiveurl=https://web.archive.org/web/20120526005446/http://www.sri.com/psd/research/adn.html |archivedate=2012-05-26}} SRI obtained US and international patents for ADN in the mid-1990s, at which time scientists from the former Soviet Union revealed that they had discovered ADN 18 years earlier.

Propellant mixtures

ADN can be mixed with conventional propellants such as nitrocellulose to improve its oxygen balance.{{Cite journal |last1=Wang |first1=Qiong |last2=Wang |first2=Xiao-Hong |last3=Pan |first3=Qing |last4=Chang |first4=Hai |last5=Yu |first5=Hong-Jian |last6=Pang |first6=Wei-Qiang |date=3 March 2023 |title=Thermal Behaviors and Interaction Mechanism of Ammonium Dinitramide with Nitrocellulose |journal=Molecules |volume=28 |issue=5 |page=2346 |doi=10.3390/molecules28052346 |doi-access=free |pmid=36903591 |pmc=10005589 }} One of the challenges of using ADN is its hygroscopicity. Hu et al. have investigated the possibility of reducing the hygroscopicity of ADN by co-crystallization with 3,4-diaminofurazan.{{Cite journal |last1=Hu |first1=Dongdong |last2=Wang |first2=Yinglei |last3=Xiao |first3=Chuan |last4=Hu |first4=Yifei |last5=Zhou |first5=Zhiyong |last6=Ren |first6=Zhongqi |date=September 2023 |title=Studies on ammonium dinitramide and 3,4-diaminofurazan cocrystal for tuning the hygroscopicity |url=https://doi.org/10.1016/j.cjche.2023.01.006 |journal=Chinese Journal of Chemical Engineering |volume=61 |pages=157–164 |doi=10.1016/j.cjche.2023.01.006 |url-access=subscription }}

There is also interest in using ADN to make liquid monopropellants. When ADN is co-crystalized with a crown ether (18C6), the hygroscopicity is greatly reduced, but so is its performance as an explosive.{{Cite journal |last1=Qiao |first1=Shen |last2=Li |first2=Hong-zhen |last3=Yang |first3=Zong-wei |date=June 2022 |title=Decreasing the hygroscopicity of ammonium dinitramide (ADN) through cocrystallization |journal=Energetic Materials Frontiers |volume=3 |issue=2 |pages=84–89 |doi=10.1016/j.enmf.2022.03.001 |doi-access=free }} ADN was mixed with amine nitrates in order to lower its melting point for use as a liquid monopropellant. The onset temperature for ADN was essentially unchanged, but some cross-reaction with the amine nitrates was observed.{{Cite journal |last1=Matsunaga |first1=Haroki |last2=Katoh |first2=Katsumi |last3=Habu |first3=Hiroto |last4=Noda |first4=Masaru |last5=Miyake |first5=Atsumi |date=November 2018 |title=Thermal behavior of ammonium dinitramide and amine nitrate mixtures |journal=Journal of Thermal Analysis and Calorimetry |volume=135 |issue=5 |pages=2677–2685 |doi=10.1007/s10973-018-7875-6 }} Kim et al. have also examined mixtures of ADN with hydrogen peroxide as a potential liquid monopropellant.{{Cite journal |last1=Kim |first1=Ju Won |last2=Bhosale |first2=Vikas Khandu |last3=Kim |first3=Kyu-Seop |last4=Lee |first4=Seung Ho |last5=Kwon |first5=Sejin |date=February 2, 2022 |title=Room-temperature catalytically reactive ammonium dinitramide–H2O2 monopropellant for microsatellites |url=https://doi.org/10.1016/j.asr.2021.11.022 |journal=Advances in Space Research |volume=69 |issue=3 |pages=1631–1644 |doi=10.1016/j.asr.2021.11.022 |url-access=subscription }}

Preparation

There are at least 20 different synthesis routes that produce ammonium dinitramide. In the laboratory ammonium dinitramide can be prepared by nitration of sulfamic acid or its salts (here potassium sulfamate) at low temperatures:

: {{chem2|KSO3NH2 + 2 HNO3 → KHSO4 + [NH4]N(NO2)2 + H2O}}

The process is performed under red light, since the compound is decomposed by higher-energy photons. The details of the synthesis remain classified.

Other sources{{who?|date=February 2019}} report ammonium synthesis from ammonium nitrate, anhydrous nitric acid, and fuming sulfuric acid (oleum) containing 20% free sulfur trioxide. A base other than ammonia must be added before the acid dinitramide decomposes. The final product is obtained by fractional crystallization.

Another synthesis known as the urethane synthesis method requires four synthesis steps and results in a yield of up to 60%.{{cite patent |country=US |number=5714714 |pubdate=1998-02-03 |title=Process for preparing ammonium dinitramide |assign1=USA, Secretary of the Navy |inventor1-last=Stern |inventor1-first=Alfred G. |inventor2-last=Koppes |inventor2-first=William M. |inventor3-last=Sitzmann |inventor3-first=Michael E. |inventor4=Lori A. Nock; Donna M. Cason-Smith}} Ethyl carbamate is nitrated with nitric acid:

: {{chem2|CH3CH2\sO\sC(\dO)\sNH2 + HNO3 → CH3CH2\sO\sC(\dO)\sNH\sNO2 + H2O}}

and then reacted with ammonia to form the ammonium salt of N-nitrourethane:

: {{chem2|CH3CH2\sO\sC(\dO)\sNH\sNO2 + NH3 → [CH3CH2\sO\sC(\dO)\sN−\sNO2][NH4+]}}

This is nitrated again with nitrogen pentoxide to form ethyl dinitrocarbamate and ammonium nitrate:

: {{chem2|[CH3CH2\sO\sC(\dO)\sN−\sNO2][NH4+] + O(NO2)2 → CH3CH2\sO\sC(\dO)\sN(NO2)2 + [NH4]+NO3−}}

Finally, treatment with ammonia again splits off the desired ammonium dinitramide and regenerates the urethane starting material:

: {{chem2|CH3CH2\sO\sC(\dO)\sN(NO2)2 + 2 NH3 → CH3CH2\sO\sC(\dO)\sNH2 + [NH4+][−N(NO2)2]}}

Ammonium dinitramide

History

Propellant mixtures

Preparation

References

Further reading