Nitrogen dioxide

Not to be confused with nitric oxide (formula NO), nitrous oxide (N
2O), or generic nitrogen oxide pollutants NOx.

"NO2" redirects here. For other uses, see NO2 (disambiguation).

Nitrogen dioxide  | Skeletal formula of nitrogen dioxide with some measurementsEP | Spacefill model of nitrogen dioxide

|

NO2 converts to the colorless dinitrogen tetroxide (N2O4) at low temperatures and reverts to NO2 at higher temperatures.

Names
IUPAC name

Nitrogen dioxide

Other names

Nitrogen(IV) oxide,[1] deutoxide of nitrogen

Identifiers

CAS Number

* 10102-44-0 Y

3D model (JSmol)

* Interactive image
* Interactive image

ChEBI |

* CHEBI:33101 Y

ChemSpider |

* 2297499 Y

EC Number |

* 233-272-6

Gmelin Reference

| 976

PubChem CID

* 3032552

RTECS number |

* QW9800000

UNII |

* S7G510RUBH N

UN number | 1067

InChI

* InChI=1S/NO2/c2-1-3 Y

Key: JCXJVPUVTGWSNB-UHFFFAOYSA-N Y

* InChI=1/NO2/c2-1-3

Key: JCXJVPUVTGWSNB-UHFFFAOYAA

SMILES

* N(=O)[O]

* [N+](=O)[O-]

Properties

Chemical formula

| NO•2
Molar mass | 46.005 g·mol−1
Appearance  | Brown gas[2]
Odor | Chlorine-like
Density | 1.880 g/L[2]
Melting point |  −9.3 °C (15.3 °F; 263.8 K)[2]
Boiling point |  21.15 °C (70.07 °F; 294.30 K)[2]

Solubility in water

| Hydrolyses
Solubility | Soluble in CCl4, nitric acid,[3] chloroform
Vapor pressure | 98.80 kPa (at 20 °C)

Magnetic susceptibility (χ)

| +150.0·10−6 cm3/mol[4]

Refractive index (nD)

| 1.449 (at 20 °C)
Structure

Point group

| C2v

Molecular shape

| Bent
Thermochemistry[5]

Heat capacity (C)

| 37.2 J/(mol·K)

Std molar
entropy (S ~~o~~ 298)

| 240.1 J/(mol·K)

Std enthalpy of
formation (ΔfH⦵298)

| +33.2 kJ/mol
Hazards
Main hazards | Poison, oxidizer
Safety data sheet | ICSC 0930
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H270, H314, H330

GHS precautionary statements

| P220, P260, P280, P284, P305+351+338, P310
NFPA 704 (fire diamond)  |

Lethal dose or concentration (LD, LC):

LC50 (median concentration)

| 30 ppm (guinea pig, 1 h)
315 ppm (rabbit, 15 min)
68 ppm (rat, 4 h)
138 ppm (rat, 30 min)
1000 ppm (mouse, 10 min)[7]

LCLo (lowest published)

| 64 ppm (dog, 8 h)
64 ppm (monkey, 8 h)[7]
NIOSH (US health exposure limits):

PEL (Permissible)

| C 5 ppm (9 mg/m3)[6]

REL (Recommended)

| ST 1 ppm (1.8 mg/m3)[6]

IDLH (Immediate danger)

| 13 ppm[6]
Related compounds

Related nitrogen oxides

| Dinitrogen pentoxide

Dinitrogen tetroxide
Dinitrogen trioxide
Nitric oxide
Nitrous oxide

Related compounds

| Chlorine dioxide
Carbon dioxide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

Tracking categories (test):

* SizeSet

Nitrogen dioxide is a chemical compound with the formula NO
2. One of several nitrogen oxides, nitrogen dioxide is a reddish-brown gas. It is a paramagnetic, bent molecule with C2v point group symmetry. Industrially, NO
2 is an intermediate in the synthesis of nitric acid, millions of tons of which are produced each year, primarily for the production of fertilizers.

Nitrogen dioxide is poisonous and can be fatal if inhaled in large quantities.[8] Cooking with a gas stove produces nitrogen dioxide which causes poorer indoor air quality. Combustion of gas can lead to increased concentrations of nitrogen dioxide throughout the home environment which is linked to respiratory issues and diseases.[9][10] The LC50 (median lethal dose) for humans has been estimated to be 174 ppm for a 1-hour exposure.[11] It is also included in the NOx family of atmospheric pollutants.

## Contents

* 1 Properties
* 2 Preparation
* 3 Selected reactions
* 3.1 Thermal properties
* 3.2 As an oxidizer
* 3.3 Hydrolysis
* 3.4 Conversion to nitrates
* 3.5 With organic compounds
* 4 Uses
* 5 Environmental presence
* 5.1 Anthropogenic sources
* 6 Toxicity
* 6.1 Acute exposure
* 6.2 Long-term
* 7 Environmental effects
* 8 See also
* 9 References
* 10 Cited sources
* 11 External links

## Properties

Nitrogen dioxide is a reddish-brown gas with a pungent, acrid odor above 21.2 °C (70.2 °F; 294.3 K) and becomes a yellowish-brown liquid below 21.2 °C (70.2 °F; 294.3 K). It forms an equilibrium with its dimer, dinitrogen tetroxide (N

4), and converts almost entirely to N

4 below −11.2 °C (11.8 °F; 261.9 K).[6]

The bond length between the nitrogen atom and the oxygen atom is 119.7 pm. This bond length is consistent with a bond order between one and two.

Unlike ozone (O
3) the ground electronic state of nitrogen dioxide is a doublet state, since nitrogen has one unpaired electron,[12] which decreases the alpha effect compared with nitrite and creates a weak bonding interaction with the oxygen lone pairs. The lone electron in NO
2 also means that this compound is a free radical, so the formula for nitrogen dioxide is often written as •

The reddish-brown color is a consequence of preferential absorption of light in the blue region of the spectrum (400–500 nm), although the absorption extends throughout the visible (at shorter wavelengths) and into the infrared (at longer wavelengths). Absorption of light at wavelengths shorter than about 400 nm results in photolysis (to form NO + O, atomic oxygen); in the atmosphere the addition of the oxygen atom so formed to O
2 results in ozone.

## Preparation

See also: Chemistry:Ostwald process

Industrially, nitrogen dioxide is produced and transported as its cryogenic liquid dimer, dinitrogen tetroxide. It is produced industrially by the oxidation of ammonia, the Ostwald Process. This reaction is the first step in the production of nitric acid:[13]

4 NH
3 \+ 7 O
2 → 4 NO
2 \+ 6 H

It can also be produced by the oxidation of nitrosyl chloride:

2 NOCl + O
2 → 2NO
2 \+ Cl

Instead, most laboratory syntheses stabilize and then heat the nitric acid to accelerate the decomposition. For example, the thermal decomposition of some metal nitrates generates NO
2:[14]

Pb(NO

2 → PbO + 2 NO
2 + ​1⁄2 O

Alternatively, dehydration of nitric acid produces nitronium nitrate...

2 HNO
3 → N

5 \+ H

6 HNO
3 + ​1⁄2 P

10 → 3 N

5 \+ 2 H
3PO

...which subsequently undergoes thermal decomposition:

5 → 2 NO
2 + ​1⁄2 O

2 is generated by the reduction of concentrated nitric acid with a metal (such as copper):

4 HNO
3 \+ Cu → Cu(NO

2 \+ 2 NO
2 \+ 2 H

## Selected reactions

Nitric acid decomposes slowly to nitrogen dioxide by the overall reaction:

4 HNO
3 → 4 NO
2 \+ 2 H
2O \+ O

The nitrogen dioxide so formed confers the characteristic yellow color often exhibited by this acid. However, the reaction is too slow to be a practical source of NO

### Thermal properties

At low temperatures, NO
2 reversibly converts to the colourless gas dinitrogen tetroxide (N

4):

2 NO
2 ⇌ N

The exothermic equilibrium has enthalpy change ΔH = −57.23 kJ/mol.[15]

At 150 °C (302 °F; 423 K), NO
2 decomposes with release of oxygen via an endothermic process (ΔH = 14 kJ/mol):

2 NO2 →2 NO +  O

### As an oxidizer

As suggested by the weakness of the N–O bond, NO
2 is a good oxidizer. Consequently, it will combust, sometimes explosively, in the presence of hydrocarbons.[16]

### Hydrolysis

NO2 reacts with water to give nitric acid and nitrous acid:

3 NO
2 \+ H
2O → 2 HNO
3 \+ NO

This reaction is one of the steps in the Ostwald process for the industrial production of nitric acid from ammonia.[13] This reaction is negligibly slow at low concentrations of NO2 characteristic of the ambient atmosphere, although it does proceed upon NO2 uptake to surfaces. Such surface reaction is thought to produce gaseous HNO2 (often written as HONO) in outdoor and indoor environments.[17]

### Conversion to nitrates

2 is used to generate anhydrous metal nitrates from the oxides:[15]

MO + 3 NO
2 → M(NO

2 \+ NO

Alkyl and metal iodides give the corresponding nitrates:[12]

TiI
4 \+ 8 NO
2 → Ti(NO

4 \+ 4 NO + 2 I

### With organic compounds

The reactivity of nitrogen dioxide toward organic compounds has long been known.[18] For example, it reacts with amides to give N-nitroso derivatives.[19] It is used for nitrations under anhydrous conditions.[20]

## Uses

2 is used as an intermediate in the manufacturing of nitric acid, as a nitrating agent in the manufacturing of chemical explosives, as a polymerization inhibitor for acrylates, as a flour bleaching agent,[21]: 223 and as a room temperature sterilization agent.[22] It is also used as an oxidizer in rocket fuel, for example in red fuming nitric acid; it was used in the Titan rockets, to launch Project Gemini, in the maneuvering thrusters of the Space Shuttle, and in uncrewed space probes sent to various planets.[23]

## Environmental presence

Nitrogen dioxide tropospheric column density in 2011.

Nitrogen dioxide typically arises via the oxidation of nitric oxide by oxygen in air (e.g. as result of corona discharge):[15]

2 NO + O
2 → 2 NO

2 is introduced into the environment by natural causes, including entry from the stratosphere, bacterial respiration, volcanos, and lightning. These sources make NO
2 a trace gas in the atmosphere of Earth, where it plays a role in absorbing sunlight and regulating the chemistry of the troposphere, especially in determining ozone concentrations.[24]

### Anthropogenic sources

Nitrogen dioxide diffusion tube for air quality monitoring in the City of London.

Nitrogen dioxide also forms in most combustion processes. At elevated temperatures nitrogen combines with oxygen to form nitrogen dioxide:

2 \+ 2 O
2 → 2 NO

For the general public, the most prominent sources of NO
2 are internal combustion engines, as combustion temperatures are high enough to thermally combine some of the nitrogen and oxygen in the air to form NO
2.[8] Nitrogen dioxide accounts for a small fraction (generally well under 0.1) of NOx auto emissions.[25]

Outdoors, NO
2 can be a result of traffic from motor vehicles.[26] Indoors, exposure arises from cigarette smoke,[27] and butane and kerosene heaters and stoves.[28] Indoor exposure levels of NO
2 are, on average, at least three times higher in homes with gas stoves compared to electric stoves.[29][30]

A "fox tail" over Nizhniy Tagil Iron and Steel Works

Workers in industries where NO
2 is used are also exposed and are at risk for occupational lung diseases, and NIOSH has set exposure limits and safety standards.[6] Workers in high voltage areas especially those with spark or plasma creation are at risk.[citation needed] Agricultural workers can be exposed to NO
2 arising from grain decomposing in silos; chronic exposure can lead to lung damage in a condition called "silo-filler's disease".[31][32]

## Toxicity

Possible pathways implicated in long-term nitrogen dioxide exposure. Dotted lines indicate findings only supported by animal studies, while solid lines indicate findings from controlled human exposure studies. Dashed lines indicate speculative links to asthma exacerbation and respiratory tract infections. ELF = epithelial lining fluid.[33]: 4–62

Main article: Physics:Nitrogen dioxide poisoning

2 diffuses into the epithelial lining fluid (ELF) of the respiratory epithelium and dissolves. There, it chemically reacts with antioxidant and lipid molecules in the ELF. The health effects of NO
2 are caused by the reaction products or their metabolites, which are reactive nitrogen species and reactive oxygen species that can drive bronchoconstriction, inflammation, reduced immune response, and may have effects on the heart.[33]

### Acute exposure

Acute harm due to NO
2 exposure is rare. 100–200 ppm can cause mild irritation of the nose and throat, 250–500 ppm can cause edema, leading to bronchitis or pneumonia, and levels above 1000 ppm can cause death due to asphyxiation from fluid in the lungs. There are often no symptoms at the time of exposure other than transient cough, fatigue or nausea, but over hours inflammation in the lungs causes edema.[34][35]

For skin or eye exposure, the affected area is flushed with saline. For inhalation, oxygen is administered, bronchodilators may be administered, and if there are signs of methemoglobinemia, a condition that arises when nitrogen-based compounds affect the hemoglobin in red blood cells, methylene blue may be administered.[36][37]

It is classified as an extremely hazardous substance in the United States as defined in Section 302 of the U.S. Emergency Planning and Community Right-to-Know Act (42 U.S.C. 11002), and it is subject to strict reporting requirements by facilities which produce, store, or use it in significant quantities.[38]

### Long-term

Exposure to low levels of NO
2 over time can cause changes in lung function.[39] Cooking with a gas stove is associated with poorer indoor air quality. Combustion of gas can lead to increased concentrations of nitrogen dioxide throughout the home environment which is linked to respiratory issues and diseases.[9][10] Children exposed to NO
2 are more likely to be admitted to hospital with asthma.[40]

In 2019, the Court of Justice of the EU, found that France did not comply with the limit values of the EU air quality standards applicable to the concentrations of nitrogen dioxide (NO2) in 12 air quality zones.[41]

## Environmental effects

Interaction of NO
2 and other NO
x with water, oxygen and other chemicals in the atmosphere can form acid rain which harms sensitive ecosystems such as lakes and forests.[42] Elevated levels of NO2 can also harm vegetation, decreasing growth, and reduce crop yields.[43]

## See also

* Dinitrogen tetroxide (N

* Nitric oxide (NO) – pollutant that is short lived because it converts to NO
2 in the presence of ozone
* Nitrite (NO−

* Nitrous oxide (N
2O) – "laughing gas", a linear molecule, isoelectronic with CO
2 but with a nonsymmetric arrangement of atoms (NNO)
* Nitryl

## References

1. ↑ "nitrogen dioxide (CHEBI:33101)". Chemical Entities of Biological Interest (ChEBI). UK: European Bioinformatics Institute. 13 January 2008. Main. https://www.ebi.ac.uk/chebi/searchId.do?chebiId=33101.
2. ↑ 2.0 2.1 2.2 2.3 Haynes, 4.79.
3. ↑ Mendiara, S. N.; Sagedahl, A.; Perissinotti, L. J. (2001). "An electron paramagnetic resonance study of nitrogen dioxide dissolved in water, carbon tetrachloride and some organic compounds". Applied Magnetic Resonance 20 (1–2): 275–287. doi:10.1007/BF03162326.
4. ↑ Haynes, 4.134.
5. ↑ Haynes, 5.16.
6. ↑ 6.0 6.1 6.2 6.3 6.4 NIOSH Pocket Guide to Chemical Hazards. "#0454". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0454.html.
7. ↑ 7.0 7.1 "Nitrogen dioxide". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/10102440.html.
8. ↑ 8.0 8.1 Template:EPA content
9. ↑ 9.0 9.1 "Clearing the Air: Gas Cooking and Pollution in European Homes" (in en). 8 November 2023. https://www.clasp.ngo/research/all/cooking-with-gas-findings-from-a-pan-european-indoor-air-quality-field-study/.
10. ↑ 10.0 10.1 Seals, Brady; Krasner, Andee. "Gas Stoves: Health and Air Quality Impacts and Solutions" (in en-US). https://rmi.org/insight/gas-stoves-pollution-health/.
11. ↑ "Immediately Dangerous to Life or Health Concentrations (IDLH): Nitrogen dioxide". The National Institute for Occupational Safety and Health (NIOSH). May 1994. https://www.cdc.gov/niosh/idlh/10102440.html.
12. ↑ 12.0 12.1 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 455-7. ISBN 978-0-08-037941-8.
13. ↑ 13.0 13.1 Thiemann, Michael; Scheibler, Erich; Wiegand, Karl Wilhelm (2005). Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_293. ISBN 978-3-527-30673-2.
14. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 456. ISBN 978-0-08-037941-8.
15. ↑ 15.0 15.1 15.2 Holleman, A. F.; Wiberg, E. (2001) Inorganic Chemistry. Academic Press: San Diego. ISBN 0-12-352651-5.
16. ↑ Chan, Wai-To; Heck, Simone M.; Pritchard, Huw O. (2001). "Reaction of nitrogen dioxide with hydrocarbons and its influence on spontaneous ignition. A computational study". Physical Chemistry Chemical Physics 3 (1): 56–62. doi:10.1039/b006088g. Bibcode: 2001PCCP....3...56C.
17. ↑ Finlayson-Pitts, B. J.; Wingen, L. M.; Sumner, A. L.; Syomin, D.; Ramazan, K. A. (2002-12-16). "The heterogeneous hydrolysis of NO2 in laboratory systems and in outdoor and indoor atmospheres: An integrated mechanism" (in en). Physical Chemistry Chemical Physics 5 (2): 223–242. doi:10.1039/B208564J. https://escholarship.org/content/qt8wx9v8h9/qt8wx9v8h9.pdf?t=njz4b2.
18. ↑ Riebsomer, J. L. (1945). "The Reactions of Nitrogen Tetroxide with Organic Compounds". Chemical Reviews 36 (2): 157–233. doi:10.1021/cr60114a002.
19. ↑ Emil White (1967). "Deamination of Amines. 2-Phenylethyl Benzoate Via the Nitrosoamide Decomposition". Organic Syntheses 47: 44. doi:10.15227/orgsyn.047.0044.
20. ↑ Smith, Michael B.; March, Jerry (2007), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (6th ed.), New York: Wiley-Interscience, p. 687, ISBN 978-0-471-72091-1, https://books.google.com/books?id=JDR-nZpojeEC&printsec=frontcover
21. ↑ Subcommittee on Emergency and Continuous Exposure Guidance Levels for Selected Submarine Contaminants; Committee on Toxicology; Board on Environmental Studies and Toxicology; Division on Earth and Life Studies; National Research Council. Chapter 12: Nitrogen Dioxide in Emergency and Continuous Exposure Guidance Levels for Selected Submarine Contaminants. National Academies Press, 2007. ISBN 978-0-309-09225-8
22. ↑ "Mechanism Overview, June 2012". noxilizer.com. Noxilizer, Inc.. http://noxilizer.com/pdf/news/WhitePaper-Mechanism_Overview_6_14_12.pdf.
23. ↑ Cotton, Simon (21 March 2013) Nitrogen dioxide. RSC Chemistry World.
24. ↑ WHO Air Quality Guidelines – Second Edition. Chapter 7.1 Nitrogen Dioxide.
25. ↑ Wild, Robert J.; Dubé, William P.; Aikin, Kenneth C.; Eilerman, Scott J.; Neuman, J. Andrew; Peischl, Jeff; Ryerson, Thomas B.; Brown, Steven S. (2017). "On-road measurements of vehicle NO2/NOx emission ratios in Denver, Colorado, USA". Atmospheric Environment 148: 182–189. doi:10.1016/j.atmosenv.2016.10.039. https://www.sciencedirect.com/science/article/abs/pii/S1352231016308469. Retrieved 2025-02-25.
26. ↑ "Air quality guidelines – global update 2005". https://www.who.int/phe/health_topics/outdoorair/outdoorair_aqg/en/.
27. ↑ US Dept. of Health and Human Services, Public Health Service, Agency for Toxic Substances and Disease Registry, Division of Toxicology. April 2002 ATSDR Nitrous Oxides.
28. ↑ "The Impact of Unvented Gas Heating Appliances on Indoor Nitrogen Dioxide Levels in 'TIGHT' Homes". ahrinet.org. 2013-03-21. http://www.ahrinet.org/App_Content/ahri/files/Product Section/Vent-Free NO2 Modeling Study Final Summary March 21 2013.pdf.
29. ↑ Garrett, Maria H.; Hooper, Martin A.; Hooper, Beverley M.; Abramson, Michael J. (1998-09-01). "Respiratory Symptoms in Children and Indoor Exposure to Nitrogen Dioxide and Gas Stoves". American Journal of Respiratory and Critical Care Medicine 158 (3): 891–895. doi:10.1164/ajrccm.158.3.9701084. PMID 9731022. https://research.monash.edu/files/304219582/304218990_oa.pdf.
30. ↑ Template:EPA content
31. ↑ Chan-Yeung, M.; Ashley, M. J.; Grzybowski, S. (1978). "Grain dust and the lungs". Canadian Medical Association Journal 118 (10): 1271–4. PMID 348288.
32. ↑ Gurney, J. W.; Unger, J. M.; Dorby, C. A.; Mitby, J. K.; von Essen, S. G. (1991). "Agricultural disorders of the lung". Radiographics 11 (4): 625–34. doi:10.1148/radiographics.11.4.1887117. PMID 1887117.
33. ↑ 33.0 33.1 U.S. EPA. Integrated Science Assessment for Oxides of Nitrogen – Health Criteria (2016 Final Report). U.S. Environmental Protection Agency, Washington, DC, EPA/600/R-15/068, 2016. Federal Register Notice Jan 28, 2016 Free download available at Report page at EPA website.
34. ↑ Toxnet Nitrogen dioxide: Human Health Effects Page accessed March 28, 2016.
35. ↑ CDC NIOSH International Chemical Safety Cards (ICSC): Nitrogen Dioxide Page last reviewed: July 22, 2015; Page last updated: July 1, 2014.
36. ↑ Agency for Toxic Substances and Disease Registry via the CDC Medical Management Guidelines for Nitrogen Oxides Page last reviewed: October 21, 2014; Page last updated: October 21, 2014
37. ↑ University of Kansas Hospital, Poison Control Center Poison Facts: Medium Chemicals: Nitrogen Dioxide page accessed March 28, 2016
38. ↑ "40 C.F.R.: Appendix A to Part 355—The List of Extremely Hazardous Substances and Their Threshold Planning Quantities". Government Printing Office. http://edocket.access.gpo.gov/cfr_2008/julqtr/pdf/40cfr355AppA.pdf.
39. ↑ Int Panis, L (2017). "Short-term air pollution exposure decreases lung function: a repeated measures study in healthy adults". Environmental Health 16 (1). doi:10.1186/s12940-017-0271-z. PMID 28615020. Bibcode: 2017EnvHe..16...60I.
40. ↑ Wang, Weiyi; Gulliver, John; Beevers, Sean; Freni Sterrantino, Anna; Davies, Bethan; Atkinson, Richard W.; Fecht, Daniela (2024). "Short-Term Nitrogen Dioxide Exposure and Emergency Hospital Admissions for Asthma in Children: A Case-Crossover Analysis in England". Journal of Asthma and Allergy 17: 349–359. doi:10.2147/JAA.S448600. ISSN 1178-6965. PMID 38623450.
41. ↑ "Air quality: Commission decides to refer France to the Court over failure to meet its obligation to protect citizens against poor air quality". 2020-10-30. https://ec.europa.eu/commission/presscorner/detail/en/ip_20_1880.
42. ↑ US EPA, OAR (2016-07-06). "Basic Information about NO2" (in en). https://www.epa.gov/no2-pollution/basic-information-about-no2.
43. ↑ "Nitrogen oxides" (in en). https://www.qld.gov.au/environment/pollution/monitoring/air/air-pollution/pollutants/nitrogen-oxides.

## Cited sources

* Haynes, William M., ed (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. ISBN 978-1-4398-5511-9.

## External links

* International Chemical Safety Card 0930
* National Pollutant Inventory – Oxides of nitrogen fact sheet
* NIOSH Pocket Guide to Chemical Hazards
* WHO-Europe reports: Health Aspects of Air Pollution (2003) (PDF) and "Answer to follow-up questions from CAFE (2004) (PDF)
* Nitrogen Dioxide Air Pollution
* Current global map of nitrogen dioxide distribution
* A review of the acute and long term impacts of exposure to nitrogen dioxide in the United Kingdom IOM Research Report TM/04/03
* Reaction of nitrogen dioxide with hydrocarbons and its influence on spontaneous ignition

* 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

* v
* t
* e

Oxides

Mixed oxidation states|

* Antimony tetroxide (Sb2O4)
* Cobalt(II,III) oxide (Co3O4)
* Europium(II,III) oxide (Eu3O4)
* Iron(II,III) oxide (Fe<sub>3O4)
* Lead(II,IV) oxide (Pb3O4)
* Manganese(II,III) oxide (Mn3O4)
* Silver(I,III) oxide (Ag2O2)
* Triuranium octoxide (U3O8)
* Carbon suboxide (C3O2)
* Mellitic anhydride (C12O9)
* [[Chemistry:Praseodymium(III,IV) Praseodymium(III,IV) oxide]] (Pr6O11)
* Terbium(III,IV) oxide (Tb4O7)

+1 oxidation state|

* Copper(I) oxide (Cu<sub>2O)
* Caesium oxide (Cs2O)
* Dicarbon monoxide (C2O)
* Dichlorine monoxide (Cl2O)
* Gallium(I) oxide (Ga2O)
* Lithium oxide (Li2O)
* Potassium oxide (K2O)
* Rubidium oxide (Rb2O)
* Silver oxide (Ag2O)
* Thallium(I) oxide (Tl2O)
* Sodium oxide (Na2O)
* Water (hydrogen oxide) (H2O)

+2 oxidation state|

* Aluminium(II) oxide (AlO)
* Barium oxide (BaO)
* Beryllium oxide (BeO)
* Cadmium oxide (CdO)
* Calcium oxide (CaO)
* Carbon monoxide (CO)
* Chromium(II) oxide (CrO)
* Cobalt(II) oxide (CoO)
* Copper(II) oxide (CuO)
* Europium(II) oxide (EuO)
* Germanium monoxide (GeO))
* Iron(II) oxide (FeO)
* Lead(II) oxide (PbO)
* Magnesium oxide (MgO)
* Manganese(II) oxide (MnO)
* Mercury(II) oxide (HgO)
* Nickel(II) oxide (NiO)
* Nitric oxide (NO)
* Palladium(II) oxide (PdO)
* Silicon monoxide (SiO)
* Strontium oxide (SrO)
* Sulfur monoxide (SO)
* Disulfur dioxide (S2O2)
* Thorium monoxide (ThO)
* Tin(II) oxide (SnO)
* Titanium(II) oxide (TiO)
* Vanadium(II) oxide (VO)
* Zinc oxide (ZnO)

+3 oxidation state|

* Aluminium oxide (Al<sub>2O3)
* Antimony trioxide (Sb2O3)
* Arsenic trioxide (As2O3)
* Bismuth(III) oxide (Bi2O3)
* Boron trioxide (B2O3)
* Cerium(III) oxide (Ce2O3)
* Dibromine trioxide (Br2O3)
* Chromium(III) oxide (Cr2O3)
* Dinitrogen trioxide (N2O3)
* Dysprosium(III) oxide (Dy2O3)
* Erbium(III) oxide (Er2O3)
* Europium(III) oxide (Eu2O3)
* Gadolinium(III) oxide (Gd2O3)
* Gallium(III) oxide (Ga2O3)
* Holmium(III) oxide (Ho2O3)
* Indium(III) oxide (In<sub>2O3)
* Iron(III) oxide (Fe2O3)
* Lanthanum oxide (La2O3)
* Lutetium(III) oxide (Lu2O3)
* Manganese(III) oxide (Mn2O3)
* Neodymium(III) oxide (Nd2O3)
* Nickel(III) oxide (Ni2O3)
* Phosphorus trioxide (P4O6)
* Praseodymium(III) oxide (Pr2O3)
* Promethium(III) oxide (Pm2O3)
* Rhodium(III) oxide (Rh2O3)
* [[Chemistry:Samarium(III) Samarium(III) oxide]] (Sm2O3)
* Scandium oxide (Sc2O3)
* Terbium(III) oxide (Tb2O3)
* Thallium(III) oxide (Tl2O3)
* Thulium(III) oxide (Tm2O3)
* Titanium(III) oxide (Ti2O3)
* Tungsten(III) oxide (W2O3)
* Vanadium(III) oxide (V2O3)
* Ytterbium(III) oxide (Yb2O3)
* Yttrium(III) oxide (Y2O3)

+4 oxidation state|

* Americium dioxide (AmO2)
* Carbon dioxide (CO2)
* Carbon trioxide (CO3)
* Cerium(IV) oxide (CeO2)
* Chlorine dioxide (ClO2)
* Chromium(IV) oxide (CrO<sub>2)
* Dinitrogen tetroxide (N2O4)
* Germanium dioxide (GeO<sub>2)
* [[Chemistry:Hafnium(IV) Hafnium(IV) oxide]] (HfO2)
* Lead dioxide (PbO2)
* Manganese dioxide (MnO2)
* Neptunium(IV) oxide (NpO2)
* Nitrogen dioxide (NO2)
* Osmium dioxide (OsO2)
* Plutonium(IV) oxide (PuO2)
* Praseodymium(IV) oxide (PrO2)
* Protactinium(IV) oxide (PaO2)
* Rhodium(IV) oxide (RhO2)
* Ruthenium(IV) oxide (RuO<sub>2)
* Selenium dioxide (SeO2)
* Silicon dioxide (SiO2)
* Sulfur dioxide (SO2)
* Tellurium dioxide (TeO<sub>2)
* [[Chemistry:Terbium(IV) Terbium(IV) oxide]] (TbO2)
* Thorium dioxide (ThO2)
* Tin dioxide (SnO2)
* Titanium dioxide (TiO<sub>2)
* Tungsten(IV) oxide (WO2)
* Uranium dioxide (UO2)
* Vanadium(IV) oxide (VO2)
* Zirconium dioxide (ZrO2)

+5 oxidation state|

* Antimony pentoxide (Sb2O5)
* Arsenic pentoxide (As2O5)
* Dinitrogen pentoxide (N2O5)
* Niobium pentoxide (Nb2O5)
* Phosphorus pentoxide (P2O5)
* Protactinium(V) oxide (Pa2O5)
* Tantalum pentoxide (Ta2O5)
* Vanadium(V) oxide (V2O5)

+6 oxidation state|

* Chromium trioxide (CrO3)
* Molybdenum trioxide (MoO3)
* Rhenium trioxide (ReO3)
* Selenium trioxide (SeO3)
* Sulfur trioxide (SO3)
* Tellurium trioxide (TeO3)
* Tungsten trioxide (WO3)
* Uranium trioxide (UO3)
* Xenon trioxide (XeO3)
* Iridium trioxide (IrO3)

+7 oxidation state|

* Dichlorine heptoxide (Cl2O7)
* Manganese heptoxide (Mn2O7)
* [[Chemistry:Rhenium(VII) Rhenium(VII) oxide]] (Re2O7)
* Technetium(VII) oxide (Tc2O7)

+8 oxidation state|

* Osmium tetroxide (OsO4)
* Ruthenium tetroxide (RuO4)
* Xenon tetroxide (XeO4)
* Iridium tetroxide (IrO4)
* Hassium tetroxide (HsO4)

Related|

* Oxocarbon
* Suboxide
* Oxyanion
* Ozonide
* Peroxide
* Superoxide

Oxides are sorted by oxidation state. Category:Oxides

* v
* t
* e

Oxygen compounds

* AgO
* Al2O3
* AmO2
* Am2O3
* As2O3
* As2O5
* Au2O3
* B2O3
* BaO
* BeO
* Bi2O3
* BiO2
* Bi2O5
* BrO2
* Br2O3
* Br2O5
* CO
* CO2
* C2O3
* CaO
* CaO2
* CdO
* CeO2
* Ce3O4
* Ce2O3
* ClO2
* Cl2O
* Cl2O3
* Cl2O4
* Cl2O6
* Cl2O7
* CoO
* Co2O3
* Co3O4
* CrO3
* Cr2O3
* Cr2O5
* Cr5O12
* CsO2
* Cs2O3
* CuO
* D2O
* Dy2O3
* Er2O3
* Eu2O3
* FeO
* Fe2O3
* Fe3O4
* Ga2O
* Ga2O3
* GeO
* GeO2
* H2O
* H218O
* H2O2
* HfO2
* HgO
* Hg2O
* Ho2O3
* I2O4
* I2O5
* I2O6
* I4O9
* In2O3
* IrO2
* KO2
* K2O2
* La2O3
* Li2O
* Li2O2
* Lu2O3
* MgO
* Mg2O3
* MnO
* MnO2
* Mn2O3
* Mn2O7
* MoO2
* MoO3
* Mo2O3
* NO
* NO2
* N2O
* N2O3
* N2O4
* N2O5
* NaO2
* Na2O
* Na2O2
* NbO
* NbO2
* Nd2O3
* OF2
* O2F2
* O3F2
* O4F2
* O2PtF6

Chemical formulas

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

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Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Nitrogen_dioxide&oldid=4177475"
*[CID]: Compound ID
*[H270]: May cause or intensify fire: oxidizer
*[H314]: Causes severe skin burns and eye damage
*[H330]: Fatal if inhaled
*[P220]: Keep/Store away from clothing/…/combustible materials
*[P260]: Do not breathe dust/fume/gas/mist/vapours/spray
*[P280]: Wear protective gloves/protective clothing/eye protection/face protection
*[P284]: Wear respiratory protection
*[P305+351+338]: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do – continue rinsing
*[P310]: Immediately call a POISON CENTER or doctor/physician
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