Nitrite

The nitrite ion has the chemical formula NO−2. Nitrite (mostly sodium nitrite) is widely used throughout chemical and pharmaceutical industries.[1] The nitrite anion is a pervasive intermediate in the nitrogen cycle in nature. The name nitrite also refers to organic compounds having the –ONO group, which are esters of nitrous acid.

## Contents

* 1 Production
* 2 Structure
* 3 Reactions
* 3.1 Acid-base properties
* 3.2 Oxidation and reduction
* 3.3 Analysis of nitrite
* 3.4 Coordination complexes
* 4 Biochemistry
* 5 Uses
* 5.1 Chemical precursor
* 5.2 Nitrite in food preservation and biochemistry
* 5.2.1 Curing of meat
* 5.3 Antidote for cyanide poisoning
* 6 Organic nitrites
* 7 Safety
* 8 See also
* 9 References
* 10 External links

## Production

Sodium nitrite is made industrially by passing a mixture of nitrogen oxides into aqueous sodium hydroxide or sodium carbonate solution:[2][1]

NO + NO
2 \+ 2 NaOH → 2 NaNO
2 \+ H

NO + NO
2 \+ Na
2CO
3 → 2 NaNO
2 \+ CO

The product is purified by recrystallization. Alkali metal nitrites are thermally stable up to and beyond their melting point (441 °C for KNO2). Ammonium nitrite can be made from dinitrogen trioxide, N2O3, which is formally the anhydride of nitrous acid:

2 NH3 \+ H2O + N2O3 → 2 NH4NO2

## Structure

The two canonical structures of NO−2, which contribute to the resonance hybrid for the nitrite ion Dimensions of trans-HONO (from the microwave spectrum)

The nitrite ion has a symmetrical structure (C2v symmetry), with both N–O bonds having equal length and a bond angle of about 115°. In valence bond theory, it is described as a resonance hybrid with equal contributions from two canonical forms that are mirror images of each other. In molecular orbital theory, there is a sigma bond between each oxygen atom and the nitrogen atom, and a delocalized pi bond made from the p orbitals on nitrogen and oxygen atoms which is perpendicular to the plane of the molecule. The negative charge of the ion is equally distributed on the two oxygen atoms. Both nitrogen and oxygen atoms carry a lone pair of electrons. Therefore, the nitrite ion is a Lewis base.

In the gas phase it exists predominantly as a trans-planar molecule.

## Reactions

### Acid-base properties

Nitrite is the conjugate base of the weak acid nitrous acid:

HNO2 ⇌ H+ \+ NO−2; pKa ≈ 3.3 at 18 °C[3]

Nitrous acid is also highly unstable, tending to disproportionate:

3 HNO2 (aq) ⇌ H3O+ \+ NO−3 \+ 2 NO

This reaction is slow at 0 °C.[2] Addition of acid to a solution of a nitrite in the presence of a reducing agent, such as iron(II), is a way to make nitric oxide (NO) in the laboratory.

### Oxidation and reduction

The formal oxidation state of the nitrogen atom in nitrite is +3. This means that it can be either oxidized to oxidation states +4 and +5, or reduced to oxidation states as low as −3. Standard reduction potentials for reactions directly involving nitrous acid are shown in the table below:[4]

Half-reaction | E0 (V)

|

NO−3 \+ 3 H+ \+ 2 e− ⇌ HNO2 \+ H2O | +0.94
2 HNO2 \+ 4 H+ \+ 4 e− ⇌ H2N2O2 \+ 2 H2O | +0.86
N2O4 \+ 2 H+ \+ 2 e− ⇌ 2 HNO2 | +1.065
2 HNO2\+ 4 H+ \+ 4 e− ⇌ N2O + 3 H2O | +1.29

The data can be extended to include products in lower oxidation states. For example:

H2N2O2 \+ 2 H+ \+ 2 e− ⇌ N2 \+ 2 H2O; E0 = +2.65 V

Oxidation reactions usually result in the formation of the nitrate ion, with nitrogen in oxidation state +5. For example, oxidation with permanganate ion can be used for quantitative analysis of nitrite (by titration):

5 NO−2 \+ 2 MnO−4 \+ 6 H+ → 5 NO−3 \+ 2 Mn2+ \+ 3 H2O

The product of reduction reactions with nitrite ion are varied, depending on the reducing agent used and its strength. With sulfur dioxide, the products are NO and N2O; with tin(II) (Sn2+) the product is hyponitrous acid (H2N2O2); reduction all the way to ammonia (NH3) occurs with hydrogen sulfide. With the hydrazinium cation (N2H+5) the product of nitrite reduction is hydrazoic acid (HN3), an unstable and explosive compound:

HNO2 \+ N2H+5 → HN3 \+ H2O + H3O+

which can also further react with nitrite:

HNO2 \+ HN3 → N2O + N2 \+ H2O

This reaction is unusual in that it involves compounds with nitrogen in four different oxidation states.[2]

### Analysis of nitrite

See also: Chemistry:Nitrite test

Nitrite is detected and analyzed by the Griess Reaction, involving the formation of a deep red-colored azo dye upon treatment of a NO−2-containing sample with sulfanilic acid and naphthyl-1-amine in the presence of acid.[5]

### Coordination complexes

Main article: Chemistry:Transition metal nitrite complex

Nitrite is an ambidentate ligand and can form a wide variety of coordination complexes by binding to metal ions in several ways.[2] Two examples are the red nitrito complex [Co(NH3)5(ONO)]2+ is metastable, isomerizing to the yellow nitro complex [Co(NH3)5(NO2)]2+. Nitrite is processed by several enzymes, all of which utilize coordination complexes.

## Biochemistry

A schematic representation of the microbial nitrogen cycle.[6][7] ANAMMOX is anaerobic ammonium oxidation, DNRA is dissimilatory nitrate reduction to ammonium, and COMMAMOX is complete ammonium oxidation.

In nitrification, ammonium is converted to nitrite. Important species include Nitrosomonas. Other bacterial species such as Nitrobacter, are responsible for the oxidation of the nitrite into nitrate.

Nitrite can be reduced to nitric oxide or ammonia by many species of bacteria. Under hypoxic conditions, nitrite may release nitric oxide, which causes potent vasodilation. Several mechanisms for nitrite conversion to NO have been described, including enzymatic reduction by xanthine oxidoreductase, nitrite reductase, and NO synthase (NOS), as well as nonenzymatic acidic disproportionation reactions.

## Uses

### Chemical precursor

Azo dyes and other colorants are prepared by the process called diazotization, which requires nitrite.[1]

### Nitrite in food preservation and biochemistry

The addition of nitrites and nitrates to processed meats such as ham, bacon, and sausages speeds up the curing of meat and also impart an attractive colour.[8]

The academic and industrial consensus is that nitrites also reduces growth and toxin production of Clostridium botulinum.[9][10][11] On the other hand, a 2018 study (full text not available) by the British Meat Producers Association determined that legally permitted levels of nitrite do not affect the growth of C. botulinum.[12] In the U.S., meat cannot be labeled as "cured" without the addition of nitrite.[13][14][15] In some countries, cured-meat products are manufactured without nitrate or nitrite, and without nitrite from vegetable sources. Parma ham, produced without nitrite since 1993, was reported in 2018 to have caused no cases of botulism. This is because the interior of the muscle is sterile and the surface is exposed to oxygen.[8] Other manufacture processes do not assure these conditions, and reduction of nitrite results in toxin production.[16]

In mice, food rich in nitrites together with unsaturated fats can prevent hypertension by forming nitro fatty acids that inhibit soluble epoxide hydrolase, which is one explanation for the apparent health effect of the Mediterranean diet.[17] Adding nitrites to meat has been shown to generate known carcinogens; the World Health Organization (WHO) advises that eating 50 g (1.8 oz) of nitrite processed meat a day would raise the risk of getting bowel cancer by 18% over a lifetime.[8]

The recommended maximum limits by the World Health Organization in drinking water are 3 mg L−1 and 50 mg L−1 for nitrite and nitrate ions, respectively.[18] Ingesting too much nitrite and/or nitrate through well water is suspected to cause methemoglobinemia.[19]

95% of the nitrite ingested in modern diets comes from bacterial conversion of nitrates naturally found in vegetables.[20] However, potentially cancer-causing nitroso compounds are not made in the pH-neutral colon. They are mostly made in the acidic stomach.[21][22]

#### Curing of meat

Nitrite reacts with the meat's myoglobin by attaching to the heme iron atom, forming reddish-brown nitrosomyoglobin and the characteristic pink "fresh" color of nitrosohemochrome or nitrosyl-heme upon cooking.[23] In the US, nitrite has been formally used since 1925. According to scientists working for the industry group American Meat Institute, this use of nitrite started in the Middle Ages.[24] Historians and epidemiologists argue that the widespread use of nitrite in meat-curing is closely linked to the development of industrial meat-processing.[25][26] French investigative journalist Guillaume Coudray [fr; fr] asserts that the meat industry chooses to cure its meats with nitrite even though it is established that this chemical gives rise to cancer-causing nitroso-compounds.[27] Some traditional and artisanal producers avoid nitrites. As many researches nowadays try to point out the hazardous generation of nitrosamines as nitrites link with free peptides in the gastrointestinal system, the EU published a regulation which obliges the reduction of nitrites on meat curing from 150 to 80 ppm (mg/kg).[28]

See also: Biology:Nitrosamine formation during digestion

Addition of ascorbic acid, erythorbic acid, or one of their salts enhance the binding of nitrite to the iron atom in myoglobin.[23] These chemicals also reduce the formation of nitrosamine in the stomach, but only when the fat content of a meal is less than 10%, beyond which they instead increase the formation of nitrosamine.[29][30]

### Antidote for cyanide poisoning

Nitrites in the form of sodium nitrite and amyl nitrite are components of many cyanide antidote kits.[31] Both of these compounds bind to hemoglobin and oxidize the Fe2+ ions to Fe3+ ions forming methemoglobin. Methemoglobin, in turn, binds to cyanide (CN), creating cyanmethemoglobin, effectively removing cyanide from the complex IV of the electron transport chain (ETC) in mitochondria, which is the primary site of disruption caused by cyanide. Another mechanism by which nitrites help treat cyanide toxicity is the generation of nitric oxide (NO). NO displaces the CN from the cytochrome c oxidase (ETC complex IV), making it available for methemoglobin to bind.[32]

## Organic nitrites

A nitrite ester

In organic chemistry, alkyl nitrites are esters of nitrous acid and contain the nitrosoxy functional group. Nitro compounds contain the C–NO2 group. Nitrites have the general formula RONO, where R is an aryl or alkyl group. Amyl nitrite and other alkyl nitrites have a vasodilating action and must be handled in the laboratory with caution. They are sometimes used in medicine for the treatment of heart diseases. A classic named reaction for the synthesis of alkyl nitrites is the Meyer synthesis[33][34] in which alkyl halides react with metallic nitrites to a mixture to nitroalkanes and nitrites.

## Safety

Nitrite salts can react with secondary amines to produce N-nitrosamines, which are suspected of causing stomach cancer. The World Health Organization (WHO) advises that each 50 g (1.8 oz) of processed meat eaten a day would raise the risk of getting bowel cancer by 18% over a lifetime; processed meat refers to meat that has been transformed through fermentation, nitrite curing, salting, smoking, or other processes to enhance flavor or improve preservation. The World Health Organization's review of more than 400 studies concluded in 2015 that there was sufficient evidence that processed meats caused cancer, particularly colon cancer; the WHO's International Agency for Research on Cancer (IARC) classified processed meats as carcinogenic to humans (Group 1).[8][35]

Nitrite (ingested) under conditions that result in endogenous nitrosation, specifically the production of nitrosamine, has been classified as Probably carcinogenic to humans (Group 2A) by the IARC.[36]

Large doses of nitrite causes acute poisoning in the form of methemoglobinemia, which can lead to death.[37]

## See also

* Curing (food preservation)
* Alkyl nitrites

## References

1. ↑ 1.0 1.1 1.2 Laue, Wolfgang; Thiemann, Michael; Scheibler, Erich; Wiegand, Karl Wilhelm (2006). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_265.
2. ↑ 2.0 2.1 2.2 2.3 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 461–464. ISBN 978-0-08-037941-8.
3. ↑ IUPAC SC-Database A comprehensive database of published data on equilibrium constants of metal complexes and ligands
4. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 431. ISBN 978-0-08-037941-8.
5. ↑ Ivanov, V. M. (2004-10-01). "The 125th Anniversary of the Griess Reagent" (in en). Journal of Analytical Chemistry 59 (10): 1002–1005. doi:10.1023/B:JANC.0000043920.77446.d7. ISSN 1608-3199.
6. ↑ Sparacino-Watkins, Courtney; Stolz, John F.; Basu, Partha (2013-12-16). "Nitrate and periplasmic nitrate reductases" (in en). Chem. Soc. Rev. 43 (2): 676–706. doi:10.1039/c3cs60249d. ISSN 1460-4744. PMID 24141308.
7. ↑ Simon, Jörg; Klotz, Martin G. (2013). "Diversity and evolution of bioenergetic systems involved in microbial nitrogen compound transformations" (in en). Biochimica et Biophysica Acta (BBA) - Bioenergetics 1827 (2): 114–135. doi:10.1016/j.bbabio.2012.07.005. PMID 22842521.
8. ↑ 8.0 8.1 8.2 8.3 Wilson, Bee (2018-03-01). "Yes, bacon really is killing us" (in en-GB). The Guardian (London). ISSN 0261-3077. https://www.theguardian.com/news/2018/mar/01/bacon-cancer-processed-meats-nitrates-nitrites-sausages. "In trade journals of the 1960s, the firms who sold nitrite powders to ham-makers spoke quite openly about how the main advantage was to increase profit margins by speeding up production."
9. ↑ "Effect of nitrite and nitrate on toxin production by Clostridium botulinum and on nitrosamine formation in perishable canned comminuted cured meat". Applied Microbiology 25 (3): 357–62. March 1973. doi:10.1128/AEM.25.3.357-362.1973. PMID 4572891.
10. ↑ Lee, Soomin; Lee, Heeyoung; Kim, Sejeong; Lee, Jeeyeon; Ha, Jimyeong; Choi, Yukyung; Oh, Hyemin; Choi, Kyoung-Hee et al. (August 2018). "Microbiological safety of processed meat products formulated with low nitrite concentration — A review". Asian-Australasian Journal of Animal Sciences 31 (8): 1073–1077. doi:10.5713/ajas.17.0675. ISSN 1011-2367. PMID 29531192.
11. ↑ Sindelar, Jeffrey J.; Milkowski, Andrew L. (May 2012). "Human safety controversies surrounding nitrate and nitrite in the diet". Nitric Oxide 26 (4): 259–266. doi:10.1016/j.niox.2012.03.011.
12. ↑ Doward, Jamie (2019-03-23). "Revealed: no need to add cancer-risk nitrites to ham". The Observer (London). https://www.theguardian.com/food/2019/mar/23/nitrites-ham-bacon-cancer-risk-additives-meat-industry-confidential--report. "The results show that there is no change in levels of inoculated C. botulinum over the curing process, which implies that the action of nitrite during curing is not toxic to C. botulinum spores at levels of 150ppm [parts per million] ingoing nitrite and below."
13. ↑ De Vries, John (1997). Food Safety and Toxicity. CRC Press. p. 70. ISBN 978-0-8493-9488-1.
14. ↑ sodium nitrite and nitrate facts Accessed 12 Dec 2014
15. ↑ Doyle, Michael P.; Sperber, William H. (23 September 2009). Compendium of the Microbiological Spoilage of Foods and Beverages. Springer. p. 78. ISBN 978-1-4419-0826-1. https://books.google.com/books?id=5IS2n8MBpf8C&pg=PA78.
16. ↑ Lebrun, S.; Van Nieuwenhuysen, T.; Crèvecoeur, S.; Vanleyssem, R.; Thimister, J.; Denayer, S.; Jeuge, S.; Daube, G. et al. (December 2020). "Influence of reduced levels or suppression of sodium nitrite on the outgrowth and toxinogenesis of psychrotrophic Clostridium botulinum Group II type B in cooked ham". International Journal of Food Microbiology 334. doi:10.1016/j.ijfoodmicro.2020.108853.
17. ↑ Charles, R. L.; Rudyk, O.; Prysyazhna, O.; Kamynina, A.; Yang, J.; Morisseau, C.; Hammock, B. D.; Freeman, B. A. et al. (2014). "Protection from hypertension in mice by the Mediterranean diet is mediated by nitro fatty acid inhibition of soluble epoxide hydrolase". Proceedings of the National Academy of Sciences 111 (22): 8167–72. doi:10.1073/pnas.1402965111. PMID 24843165. Bibcode: 2014PNAS..111.8167C.
18. ↑ Bagheri, H.; Hajian, A.; Rezaei, M.; Shirzadmehr, A. (2017). "Composite of Cu metal nanoparticles—multiwall carbon nanotubes—reduced graphene oxide as a novel and high performance platform of the electrochemical sensor for simultaneous determination of nitrite and nitrate". Journal of Hazardous Materials 324 (Pt B): 762–772. doi:10.1016/j.jhazmat.2016.11.055. PMID 27894754. Bibcode: 2017JHzM..324..762B.
19. ↑ "When does nitrate become a risk for humans?". Journal of Environmental Quality 37 (2): 291–295. 2008. doi:10.2134/jeq2007.0177. PMID 18268290. Bibcode: 2008JEnvQ..37..291P. https://digitalcommons.unl.edu/agronomyfacpub/102.
20. ↑ "Is celery juice a viable alternative to nitrites in cured meats?" (in en). https://www.mcgill.ca/oss/article/food/celery-juice-viable-alternative-nitrites-cured-meats.
21. ↑ Lee, L; Archer, MC; Bruce, WR (October 1981). "Absence of volatile nitrosamines in human feces". Cancer Res. 41 (10): 3992–4. PMID 7285009.
22. ↑ Kuhnle, GG et al. (October 2007). "Diet-induced endogenous formation of nitroso compounds in the GI tract". Free Radic. Biol. Med. 43 (7): 1040–7. doi:10.1016/j.freeradbiomed.2007.03.011. PMID 17761300.
23. ↑ 23.0 23.1 Pappenberger, Günter; Hohmann, Hans-Peter (2013). "Industrial Production of l-Ascorbic Acid (Vitamin C) and d-Isoascorbic Acid". Biotechnology of Food and Feed Additives. Advances in Biochemical Engineering/Biotechnology 143: 143–188. doi:10.1007/10_2013_243. ISBN 978-3-662-43760-5. PMID 24258144.
24. ↑ Binkerd, E. F.; Kolari, O. E. (1975-01-01). "The history and use of nitrate and nitrite in the curing of meat". Food and Cosmetics Toxicology 13 (6): 655–661. doi:10.1016/0015-6264(75)90157-1. ISSN 0015-6264. PMID 1107192.
25. ↑ Coudray, Guillaume (2017) (in fr). Cochonneries: Comment la charcuterie est devenue un poison. Paris: La Découverte. pp. 40–70. ISBN 978-2-7071-9358-2.
26. ↑ Lauer, Klaus (1991-01-01). "The history of nitrite in human nutrition: A contribution from German cookery books" (in en). Journal of Clinical Epidemiology 44 (3): 261–264. doi:10.1016/0895-4356(91)90037-A. ISSN 0895-4356. PMID 1999685. https://www.jclinepi.com/article/0895-4356(91)90037-A/abstract.
27. ↑ "Guillaume Coudray on the Nitro Meat Cancer Connection". 14 April 2021. https://www.corporatecrimereporter.com/news/200/guillaume-coudray-on-the-nitro-meat-cancer-connection/.
28. ↑ "COMMISSION DECISION (EU) 2024/1225 of 30 April 2024 concerning national provisions notified by Denmark on the addition of nitrite to certain meat products". https://eur-lex.europa.eu/legal-content/EN/TXT/PDF/?uri=OJ:L_202401225.
29. ↑ Combet, E.; Paterson, S; Iijima, K; Winter, J; Mullen, W; Crozier, A; Preston, T; McColl, K. E. (2007). "Fat transforms ascorbic acid from inhibiting to promoting acid-catalysed N-nitrosation". Gut 56 (12): 1678–1684. doi:10.1136/gut.2007.128587. PMID 17785370.
30. ↑ Combet, E; El Mesmari, A; Preston, T; Crozier, A; McColl, K. E. (2010). "Dietary phenolic acids and ascorbic acid: Influence on acid-catalyzed nitrosative chemistry in the presence and absence of lipids". Free Radical Biology and Medicine 48 (6): 763–771. doi:10.1016/j.freeradbiomed.2009.12.011. PMID 20026204.
31. ↑ Meillier, Andrew; Heller, Cara (2015). "Acute Cyanide Poisoning: Hydroxocobalamin and Sodium Thiosulfate Treatments with Two Outcomes following One Exposure Event". Case Reports in Medicine 2015. doi:10.1155/2015/217951. ISSN 1687-9627. PMID 26543483.
32. ↑ Bebarta, Vikhyat S.; Brittain, Matthew; Chan, Adriano; Garrett, Norma; Yoon, David; Burney, Tanya; Mukai, David; Babin, Michael et al. (June 2017). "Sodium Nitrite and Sodium Thiosulfate Are Effective Against Acute Cyanide Poisoning when Administered by Intramuscular Injection". Annals of Emergency Medicine 69 (6): 718–725.e4. doi:10.1016/j.annemergmed.2016.09.034. ISSN 0196-0644. PMID 28041825.
33. ↑ Victor Meyer (1872). "Ueber die Nitroverbindungen der Fettreihe". Justus Liebig's Annalen der Chemie 171 (1): 1–56. https://zenodo.org/record/1427331. ; Victor Meyer, J. Locher (1876). "Ueber die Pseudonitrole, die Isomeren der Nitrolsäuren". Justus Liebig's Annalen der Chemie 180 (1–2): 133–55. doi:10.1002/jlac.18761800113. https://zenodo.org/record/1427351. ; V. Meyer and Stüber (1872). "Vorläufige Mittheilung". Chemische Berichte 5: 203–05. doi:10.1002/cber.18720050165. https://zenodo.org/record/1425020. ; Victor Meyer, O. Stüber (1872). "Ueber die Nitroverbindungen der Fettreihe". Chemische Berichte 5: 399–406. doi:10.1002/cber.187200501121. https://zenodo.org/record/1427331. ; Victor Meyer, A. Rilliet (1872). "Ueber die Nitroverbindungen der Fettreiche. Dritte Mittheilung". Chemische Berichte 5 (2): 1029–34. doi:10.1002/cber.187200502133. https://zenodo.org/record/1425028. ; Victor Meyer, C. Chojnacki (1872). "Ueber die Nitroverbindungen der Fettreihe. Vierte Mittheilung". Chemische Berichte 5 (2): 1034–38. doi:10.1002/cber.187200502134. https://zenodo.org/record/1425030.
34. ↑ Robert B. Reynolds, Homer Adkins (1929). "The Relationship of the Constitution of Certain Alky Halides to the Formation of Nitroparaffins and Alkyl Nitrites". Journal of the American Chemical Society 51 (1): 279–87. doi:10.1021/ja01376a037. Bibcode: 1929JAChS..51..279R.
35. ↑ "Carcinogenicity of consumption of red and processed meat". The Lancet Oncology 16 (16): 1599–1600. December 2015. doi:10.1016/S1470-2045(15)00444-1. PMID 26514947. https://www.thelancet.com/journals/lanonc/article/PIIS1470-2045(15)00444-1/fulltext. Retrieved 2024-10-13.
36. ↑ "Carcinogenicity of nitrate, nitrite, and cyanobacterial peptide toxins". The Lancet Oncology 7 (8): 628–629. August 2006. doi:10.1016/S1470-2045(06)70789-6. PMID 16900606. https://www.thelancet.com/journals/lanonc/article/PIIS1470-2045(06)70789-6/fulltext. Retrieved 2024-10-13.
37. ↑ "Severe Methemoglobinemia due to Sodium Nitrite Poisoning". Case Reports in Emergency Medicine 2016. 3 August 2016. doi:10.1155/2016/9013816. PMID 27563472.

## External links

* Material Safety Data Sheet, sodium nitrite (archive)
* ATSDR – Case Studies in Environmental Medicine – Nitrate/Nitrite Toxicity (archive) – US Department of Health and Human Services (public domain)
* Article about Toxicity of Nitrite

* v
* t
* e

Nitrogen species

* Hydrides:
* NH3
* NH4+
* NH2− MNH2
* N3−
* NH2OH
* N2H4
* N3–
* Organic:
* -NH2
* -CHR=NHR
* -CONHR2
* HCN
* CN−
* C2N2
* H2NCN
* CH2N2
* Oxides:
* N2O
* NO
* NO2
* N2O3
* N2O4
* N2O5
* H2N2O2
* H4N2O4
* HNO2
* HNO3
* HONO3
* HN2O2−
* N2O22−
* NO2−
* ONOO−
* NO3−
* NO43−
* O2NOO−
* NO+
* NO2+
* Halides:
* NF3
* NCl3
* NBr3
* NI3
* FN3
* ClN3
* BrN3
* NH2Cl
* NHCl2

Chemical formulas

Template:Nitrites

* v
* t
* e

Nitric oxide signaling modulators

Forms|

* Nitroxyl anion (NO−; oxonitrate(1-), hyponitrite anion)
* Nitric oxide (NO⋅; nitrogen monoxide)
* Nitrosonium (NO+; nitrosyl cation)

Targets|

| sGC|

* Activators/stimulators: Ataciguat
* BAY 41-2272
* BAY 41-8543
* BAY 60-4552
* BI-703704
* Cinaciguat (BAY 58-2667)
* GSK-2181236A
* Praliciguat
* Riociguat (BAY 63-2521)
* Vericiguat

* Inhibitors: ODQ

|

NO donors
(prodrugs)|

* Nitrates: Diethylene glycol dinitrate (DEGDN)
* Erythritol tetranitrate (ETN)
* Ethylene glycol dinitrate (EGDN; nitroglycol)
* Isosorbide mononitrate (ISMN)
* Isosorbide dinitrate (ISDN)
* Itramin tosilate
* Mannitol hexanitrate
* Naproxcinod (nitronaproxen; AZD-3582, HCT-3012)
* NCX-466
* NCX-2216
* NCX-4016
* NCX 4040
* NCX-4215
* Nicorandil
* Nipradilol (K-351)
* Nitrate (NO−3)
* Nitroatorvastatin (NCX-6560)
* Nitroflurbiprofen (HCT-1026)
* Nitrofluvastatin
* Nitroglycerin (glyceryl trinitrate (GTN))
* Nitropravastatin (NCX-6550)
* Pentaerithrityl tetranitrate (PETN)
* Propatylnitrate
* Propylene glycol dinitrate (PGDN)
* Sodium trioxodinitrate (Angeli's salt)
* Tenitramine
* Trolnitrate

* Nitroso compounds/nitrites: Nitrite (NO−2); O-Nitroso compounds (alkyl nitrites): Amyl nitrite (isoamyl nitrite, isopentyl nitrite)
* Cyclohexyl nitrite
* Ethyl nitrite
* Hexyl nitrite
* Isobutyl nitrite (2-methylpropyl nitrite)
* Isopropyl nitrite
* Methyl nitrite
* n-Butyl nitrite
* Pentyl nitrite
* tert-Butyl nitrite; S-Nitroso compounds (thionitrites): LA810
* S-Nitrosoalbumin (SNALB)
* S-Nitrosated AR545C
* S-Nitroso-N-acetylcysteine (SNAC)
* S-Nitroso-N-acetylpenicillamine (SNAP)
* S-Nitroso-N-valerylpenicillamine (SNVP)
* S-Nitrosocaptopril (SNO-Cap)
* S-Nitrosocysteine (SNC, CysNO, SNO-Cys)
* S-Nitrosodiclofenac
* S-Nitrosoglutathione (GSNO, SNOG)
* SNO-t-PA
* SNO-vWF; N-Nitroso compounds (e.g., nitrosamines): SIN-1A

* Nitrosyl compounds: Metal nitrosyl complexes: Roussin's black salt
* Roussin's red salt
* Sodium nitroprusside (SNP)

* NONOates (diazeniumdiolates): Diethylamine/NO (DEA/NO)
* Diethylenetriamine/NO (DETA/NO)
* GLO/NO
* JS-K
* Methylamine hexamethylene methylamine/NO (MAHMA/NO)
* PROLI/NO
* Spermine/NO (SPER/NO)
* V-PYRRO/NO

* Heterocyclic compounds: Furoxans: Furoxan
* REC15/2739; Sydnonimines: Feprosidnine
* Linsidomine (SIN-1)
* Molsidomine (SIN-10)
* Sydnonimine

* Unsorted: Cimlanod
* FK-409
* FR144220
* FR146881
* N-Acetyl-N-acetoxy-4-chlorobenzenesulfonamide

Enzyme
(inhibitors)|

| NOS|

| nNOS|

* 3-Bromo-7-nitroindazole
* 3-Chloroindazole
* 3-Chloro-5-nitroindazole
* 5-Nitroindazole
* 6-Nitroindazole
* 7-Nitroindazole
* A-84643
* Aminoguanidine (pimagedine)
* ARL-17477
* Indazole
* N5-(1-Iminoethyl)-L-ornithine (L-NIO)
* Nω-Methyl-L-arginine (L-NMA)
* Nω-Propyl-L-arginine (L-NPA)
* Nitroarginine (NNA, NOARG)
* Pentamidine isethionate
* TRIM

|

iNOS|

* 1-Amino-2-hydroxyguanidine
* 2-Ethylaminoguanidine
* 2-Iminopiperidine
* 1400W
* AEITU
* Aminoguanidine (pimagedine)
* AMT
* AR-C 102222
* BYK-191023
* Canavanine
* Cindunistat (SD-6010)
* EITU
* IPTU
* MITU
* N5-(1-Iminoethyl)-L-ornithine (L-NIO)
* N6-(1-Iminoethyl)-L-lysine (L-NIL)
* Nω-Methyl-L-arginine (L-NMA)
* Ronopterin (VAS-203)
* TRIM

eNOS|

* Aminoguanidine (pimagedine)
* N5-(1-Iminoethyl)-L-ornithine (L-NIO)
* Nω-Methyl-L-arginine (L-NMA)
* Nitroarginine (NNA, NOARG)

Unsorted|

* Asymmetric dimethylarginine (ADMA)
* CKD-712
* Guanidinoethyldisulfide (GED)
* GW-273629
* Indospicine
* KD-7040
* Nitroarginine methyl ester (NAME)
* NCX-456
* NXN-462
* ONO-1714
* VAS-2381

Arginase|

* ABH
* Nω-Hydroxy-L-arginine (NOHA)
* chlorogenic acid
* ginseng
* epicatechin
* ornithine
* norvaline
* lysine
* alpha aminoacids

CAMK|

* Calmidazolium
* W-7

Others|

* Precursors: L-Arginine
* Nω-Hydroxy-L-arginine (NOHA)

* Cofactors: NADPH
* FAD
* FMN
* Heme
* BH4
* CaM
* O2
* Ca2+

* Indirect/downstream NO modulators: ACE inhibitors/AT-II receptor antagonists (e.g., captopril, losartan)
* ETB receptor antagonists (e.g., bosentan)
* L-Type calcium channel blockers (e.g., dihydropyridines: nifedipine)
* Nebivolol (beta blocker)
* PDE5 inhibitors (e.g., sildenafil)
* Statins (e.g., simvastatin)

See also: Receptor/signaling modulators

0.00

(0 votes)

Original source: https://en.wikipedia.org/wiki/Nitrite. Read more

|

Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Nitrite&oldid=4036823"
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template