Nitroxylic acid

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Nitroxylic acid
Hydrazine-1,1,2,2-tetrol.png
Names
IUPAC name
Hydrazine-1,1,2,2-tetrol
Identifiers
3D model (JSmol)
ChemSpider
PubChem CID
  • InChI=1S/H4N2O4/c3-1(4)2(5)6/h3-6H
    Key: HAEJYKGCOSKNFL-UHFFFAOYSA-N
  • N(N(O)O)(O)O
Properties
H4N2O4
Molar mass 96.042 g·mol−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Nitroxylic acid or hydronitrous acid is an unstable reduced oxonitrogen acid. It has formula H4N2O4 containing nitrogen in the +2 oxidation state. [1] It consists of a central pair of bonded nitrogen atoms with four hydroxyl groups around them, giving rise to hydrazine-1,1,2,2-tetrol as an alternate chemical name.

The corresponding anion called nitroxylate is N
2O4−
4; its empirical formula NO2−
2 is the basis for the original names of some of its salts.

The first clue that nitroxylic acid exists was when Edward Bedford Maxted electrolysed sodium nitrite dissolved in liquid ammonia. A bright yellow substance deposited on the cathode. He called this disodium nitrite. The disodium nitrite could also be made by mixing ammonia solutions of sodium and sodium nitrite in the complete absence of water. Disodium nitrite reacts with water to form sodium nitrite, sodium hydroxide and hydrogen. [2] Other ways to make the disodium nitrite include reacting sodium with ammonium nitrate or electrolysing sodium nitrate solution. The substance is called sodium nitroxylate by current systematic nomenclature rules.

Disodium nitrite is very unstable and experimenters often had their apparatus destroyed when making it. Disodium nitrite reacts with oxygen and carbon dioxide explosively. [3] Lithium sodium nitroxylate LiNaNO2 also exists and explodes at 130 °C. [4]

The parent compound, nitroxylic acid, might be produced when nitrous acid is reduced by the Eu2+ ion. [5]

Related Research Articles

<span class="mw-page-title-main">Nitrogen</span> Chemical element with atomic number 7 (N)

Nitrogen is a chemical element; it has symbol N and atomic number 7. Nitrogen is a nonmetal and the lightest member of group 15 of the periodic table, often called the pnictogens. It is a common element in the universe, estimated at seventh in total abundance in the Milky Way and the Solar System. At standard temperature and pressure, two atoms of the element bond to form N2, a colourless and odourless diatomic gas. N2 forms about 78% of Earth's atmosphere, making it the most abundant chemical species in air. Because of the volatility of nitrogen compounds, nitrogen is relatively rare in the solid parts of the Earth.

<span class="mw-page-title-main">Nitronium ion</span> Polyatomic ion

The nitronium ion, [NO2]+, is a cation. It is an onium ion because its nitrogen atom has +1 charge, similar to ammonium ion [NH4]+. It is created by the removal of an electron from the paramagnetic nitrogen dioxide molecule NO2, or the protonation of nitric acid HNO3.

<span class="mw-page-title-main">Ammonium</span> Chemical compound

Ammonium is a modified form of ammonia that has an extra hydrogen atom. It is a positively charged (cationic) molecular ion with the chemical formula NH+4 or [NH4]+. It is formed by the addition of a proton to ammonia. Ammonium is also a general name for positively charged (protonated) substituted amines and quaternary ammonium cations, where one or more hydrogen atoms are replaced by organic or other groups. Not only is ammonium a source of nitrogen and a key metabolite for many living organisms, but it is an integral part of the global nitrogen cycle. As such, human impact in recent years could have an effect on the biological communities that depend on it.

<span class="mw-page-title-main">Oxidizing agent</span> Chemical compound used to oxidize another substance in a chemical reaction

An oxidizing agent is a substance in a redox chemical reaction that gains or "accepts"/"receives" an electron from a reducing agent. In other words, an oxidizer is any substance that oxidizes another substance. The oxidation state, which describes the degree of loss of electrons, of the oxidizer decreases while that of the reductant increases; this is expressed by saying that oxidizers "undergo reduction" and "are reduced" while reducers "undergo oxidation" and "are oxidized". Common oxidizing agents are oxygen, hydrogen peroxide, and the halogens.

<span class="mw-page-title-main">Dinitrogen tetroxide</span> Chemical compound

Dinitrogen tetroxide, commonly referred to as nitrogen tetroxide (NTO), and occasionally (usually among ex-USSR/Russian rocket engineers) as amyl, is the chemical compound N2O4. It is a useful reagent in chemical synthesis. It forms an equilibrium mixture with nitrogen dioxide. Its molar mass is 92.011 g/mol.

<span class="mw-page-title-main">Nitrogen dioxide</span> Chemical compound with formula NO₂

Nitrogen dioxide is a chemical compound with the formula NO2. One of several nitrogen oxides, nitrogen dioxide is a reddish-brown gas. It is a paramagnetic, bent molecule with C2v point group symmetry. Industrially, NO2 is an intermediate in the synthesis of nitric acid, millions of tons of which are produced each year, primarily for the production of fertilizers.

The nitrite ion has the chemical formula NO−
2. Nitrite is widely used throughout chemical and pharmaceutical industries. 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.

<span class="mw-page-title-main">Dinitrogen pentoxide</span> Chemical compound

Dinitrogen pentoxide is the chemical compound with the formula N2O5. It is one of the binary nitrogen oxides, a family of compounds that contain only nitrogen and oxygen. It exists as colourless crystals that sublime slightly above room temperature, yielding a colorless gas.

<span class="mw-page-title-main">Sodium azide</span> Chemical compound

Sodium azide is an inorganic compound with the formula NaN3. This colorless salt is the gas-forming component in some car airbag systems. It is used for the preparation of other azide compounds. It is an ionic substance, is highly soluble in water, and is acutely poisonous.

<span class="mw-page-title-main">Devarda's alloy</span> Chemical compound

Devarda's alloy is an alloy of aluminium (44% – 46%), copper (49% – 51%) and zinc (4% – 6%).

<span class="mw-page-title-main">Methyl nitrite</span> Chemical compound

Methyl nitrite is an organic compound with the chemical formula CH
3ONO. It is a gas, and is the simplest alkyl nitrite.

<span class="mw-page-title-main">Sulfamic acid</span> Chemical compound

Sulfamic acid, also known as amidosulfonic acid, amidosulfuric acid, aminosulfonic acid, sulphamic acid and sulfamidic acid, is a molecular compound with the formula H3NSO3. This colourless, water-soluble compound finds many applications. Sulfamic acid melts at 205 °C before decomposing at higher temperatures to water, sulfur trioxide, sulfur dioxide and nitrogen.

<span class="mw-page-title-main">Ammonium nitrite</span> Chemical compound

Ammonium nitrite is a chemical compound with the chemical formula [NH4]NO2. It is the ammonium salt of nitrous acid. It is composed of ammonium cations [NH4]+ and nitrite anions NO−2. It is not used in pure isolated form since it is highly unstable and decomposes into water and nitrogen, even at room temperature.

<span class="mw-page-title-main">Potassium nitrite</span> Chemical compound

Potassium nitrite (distinct from potassium nitrate) is the inorganic compound with the chemical formula KNO2. It is an ionic salt of potassium ions K+ and nitrite ions NO2−, which forms a white or slightly yellow, hygroscopic crystalline powder that is soluble in water.

A nitrate test is a chemical test used to determine the presence of nitrate ion in solution. Testing for the presence of nitrate via wet chemistry is generally difficult compared with testing for other anions, as almost all nitrates are soluble in water. In contrast, many common ions give insoluble salts, e.g. halides precipitate with silver, and sulfate precipitate with barium.

<span class="mw-page-title-main">Alkyl nitrite</span> Organic compounds of the form R–O–N=O

In organic chemistry, alkyl nitrites are a group of organic compounds based upon the molecular structure R−O−N=O, where R represents an alkyl group. Formally they are alkyl esters of nitrous acid. They are distinct from nitro compounds.

The chemical element nitrogen is one of the most abundant elements in the universe and can form many compounds. It can take several oxidation states; but the most common oxidation states are -3 and +3. Nitrogen can form nitride and nitrate ions. It also forms a part of nitric acid and nitrate salts. Nitrogen compounds also have an important role in organic chemistry, as nitrogen is part of proteins, amino acids and adenosine triphosphate.

<span class="mw-page-title-main">Dinitrogen trioxide</span> Chemical compound

Dinitrogen trioxide is the inorganic compound with the formula N2O3. It is a nitrogen oxide. It forms upon mixing equal parts of nitric oxide and nitrogen dioxide and cooling the mixture below −21 °C (−6 °F):

Calcium nitrite is an inorganic compound with the chemical formula Ca(NO
2)
2. In this compound, as in all nitrites, nitrogen is in a +3 oxidation state. It has many applications such as antifreeze, rust inhibitor of steel and wash heavy oil.

<span class="mw-page-title-main">Sodium hyponitrite</span> Chemical compound

Sodium hyponitrite is a solid ionic compound with formula Na
2N
2O
2 or (Na+
)2[ON=NO]2−.

References

  1. ↑ Sahoo, Balaram; Nayak, Nimai Charan; Samantaray, Asutosh; Pujapanda, Prafulla Kumar (2012). Inorganic Chemistry. PHI Learning Pvt. Ltd. p. 353. ISBN   9788120343085.
  2. ↑ Maxted, Edward Bradford (1917). "LXXXVII.—Disodium nitrite, an additive compound of sodium nitrite and sodium". J. Chem. Soc., Trans. 111: 1016–1019. doi:10.1039/CT9171101016.
  3. ↑ Suekichi, ABE; Taijiro, OKABE (10 February 1953). On the Electrolysis of Liquid Ammonia Solution of Alkali Nitrates. The Chemical Research Institute of Non-Aqueous Solutions (Thesis). pp. 189–201. hdl:10097/26573.
  4. ↑ Bretherick, L. (27 October 2016). Bretherick's Handbook of Reactive Chemical Hazards. Elsevier. p. 1318. ISBN   9781483162508.
  5. ↑ Fraser, R. T. M.; Lee, R. N.; Hayden, K. (1967). "The europium(II) ion reduction of nitrite and nitropenta-amminecobalt(III) ions". Journal of the Chemical Society A: Inorganic, Physical, Theoretical: 741. doi:10.1039/J19670000741.
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