Mercury(I) nitrate
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Template:Chembox image cellTemplate:Chembox AllOtherNamesTemplate:Chembox headerbarTemplate:Chembox IndexlistTemplate:Chembox JmolTemplate:Chembox ChEMBLTemplate:Chembox ECHATemplate:Chembox E numberTemplate:Chembox IUPHAR ligandTemplate:Chembox UNIITemplate:Chembox CompToxTemplate:Chembox headerbarTemplate:Chembox SolubilityInWaterTemplate:Chembox headerbarTemplate:Chembox GHS (set)Template:Chembox headerbarTemplate:Chembox Datapage checkTemplate:Chembox Footer| Template:Longitem | Template:Unbulleted list |
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| UN number | 1627 |
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| Template:Longitem | Hg2(NO3)2 (anhydrous) Hg2(NO3)2·2H2O (dihydrate) |
| Molar mass | 525.19 g/mol (anhydrous) 561.22 g/mol (dihydrate) |
| Appearance | white monoclinic crystals (anhydrous) colorless crystals (dihydrate) |
| Density | ? g/cm3 (anhydrous) 4.8 g/cm3 (dihydrate) |
| Melting point | Template:Chembox CalcTemperatures |
| Template:Longitem | −27.95·10−6 cm3/mol |
| NFPA 704 (fire diamond) | Template:NFPA 704 diamond |
| Template:Longitem | Mercury(I) fluoride Mercury(I) chloride Mercury(I) bromide Mercury(I) iodide |
| Template:Longitem | Mercury(II) nitrate |
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Mercury(I) nitrate is an inorganic compound, a salt of mercury and nitric acid with the formula Hg2(NO3)2. A yellow solid, the compound is used as a precursor to other Hg22+ complexes. The structure of the hydrate has been determined by X-ray crystallography. It consists of a [H2O-Hg-Hg-OH2]2+ center, with a Hg-Hg distance of 254 pm.[2]
It was first mentioned by Indian chemist Acharya Prafulla Chandra Ray in 1896.[3]
Reactions
Mercury(I) nitrate is formed when elemental mercury is combined with dilute nitric acid (concentrated nitric acid will yield mercury(II) nitrate). Mercury(I) nitrate is a reducing agent which is oxidized upon contact with air.
Mercuric(II) nitrate reacts with elemental mercury(0) to form mercurous(I) nitrate (comproportionation reaction):Script error: No such module "Unsubst".
Solutions of mercury(I) nitrate are acidic due to slow reaction with water:
- Hg2(NO3)2 + H2O ⇌ Hg2(NO3)(OH) + HNO3
Hg2(NO3)(OH) forms a yellow precipitate.
If the solution is boiled, or exposed to light, mercury(I) nitrate undergoes a disproportionation reaction yielding elemental mercury and mercury(II) nitrate:[4]
These reactions are reversible; the nitric acid formed can redissolve the basic salt.Script error: No such module "Unsubst".
References
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