# Mercury(II) fulminate

Names Identifiers ${\displaystyle {\ce {{}^{-}O-{\overset {+}{N}}#C-Hg-C#{\overset {+}{N}}-O^{-}}}}$ Other names Fulminated Mercury CAS Number 628-86-4 3D model (JSmol) Interactive image ChEBI CHEBI:39152 ChemSpider 9197626 ECHA InfoCard 100.010.053 PubChem CID 11022444 InChI InChI=1S/2CNO.Hg/c2*1-2-3; Key: MHWLNQBTOIYJJP-UHFFFAOYSA-N InChI=1/2CNO.Hg/c2*1-2-3;/rC2HgN2O2/c6-4-1-3-2-5-7Key: MHWLNQBTOIYJJP-HZIBCBEIAJ SMILES [O-][N+]#C[Hg]C#[N+][O-] Chemical formula C2N2O2Hg Molar mass 284.624 g/mol Appearance Grey, Pale Brown, or White Crystalline solid Density 4.42 g/cm3 Melting point 160 °C (320 °F; 433 K) Boiling point 356.6 °C (673.9 °F; 629.8 K) Solubility in water slightly soluble Solubility soluble in ethanol, ammonia Shock sensitivity High Friction sensitivity High Detonation velocity 4250 m/s Main hazards Highly Toxic, Shock Sensitive Explosive NFPA 704 (fire diamond) Autoignitiontemperature 170 °C (338 °F; 443 K) Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is  ?) Infobox references

Mercury(II) fulminate, or Hg(CNO)2, is a primary explosive. It is highly sensitive to friction, heat and shock and is mainly used as a trigger for other explosives in percussion caps and blasting caps. Mercury(II) cyanate, though its empirical formula is identical, has a different atomic arrangement; the cyanate and fulminate anions are isomers.

First used as a priming composition in small copper caps beginning in the 1820s, mercury fulminate quickly replaced flints as a means to ignite black powder charges in muzzle-loading firearms. Later, during the late 19th century and most of the 20th century, mercury fulminate or potassium chlorate became widely used in primers for self-contained rifle and pistol ammunition. Mercury fulminate has the distinct advantage over potassium chlorate of being non-corrosive, but it is known to weaken with time, by decomposing into its constituent elements. The reduced mercury which results forms amalgams with cartridge brass, weakening it, as well. Today, mercury fulminate has been replaced in primers by more efficient chemical substances. These are non-corrosive, less toxic and more stable over time; they include lead azide, lead styphnate and tetrazene derivatives. In addition, none of these compounds require mercury for manufacture, supplies of which can be unreliable in wartime.

## Preparation

Mercury(II) fulminate is prepared by dissolving mercury in nitric acid and adding ethanol to the solution. It was first prepared by Edward Charles Howard in 1800.[1] The crystal structure of this compound was only determined in 2007.[2]

Silver fulminate can be prepared in a similar way, but this salt is even more unstable than mercury fulminate; it can even explode under water and is impossible to accumulate in large amounts because it detonates under its own weight.

## Decomposition

The thermal decomposition of mercury(II) fulminate can begin at temperatures as low as 100 °C, though it proceeds at a much higher rate with increasing temperature.[3]

A possible reaction for the decomposition of mercury(II) fulminate yields carbon dioxide gas, nitrogen gas, and a combination of relatively stable mercury salts.

4 Hg(CNO)2 → 2 CO2 + N2 + HgO + 3 Hg(OCN)CN
Hg(CNO)2 → 2 CO + N2 + Hg
Hg(CNO)2 → :Hg(OCN)2 (cyanate or / and isocyanate)
2 Hg(CNO)2 → 2 CO2 + N2 + Hg + Hg(CN)2 (mercury(II) cyanide)

## In popular culture

In the 1955 comedy film "Mister Roberts ", Ensign Frank Pulver test fires a fulminate of mercury firecracker and blows up the ship's laundry spreading soap suds across three decks.

In the episode of Breaking Bad titled "Crazy Handful of Nothin'", Walter White used mercury (II) fulminate to blow up Tuco Salamanca's headquarters.