Summary
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]
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| Names | |
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| IUPAC name
Mercury(I) nitrate
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| Other names
Mercurous nitrate
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| Identifiers | |
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3D model (JSmol)
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| ECHA InfoCard | 100.202.814 |
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PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| 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 | ? (anhydrous) decomposes at 70 °C (dihydrate) |
| slightly soluble, reacts | |
| −27.95·10−6 cm3/mol | |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Other anions
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Mercury(I) fluoride Mercury(I) chloride Mercury(I) bromide Mercury(I) iodide |
Other cations
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Mercury(II) nitrate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references
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Reactions Edit
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 nitrate reacts with elemental mercury to form mercurous nitrate.[citation needed]
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:[3]
- Hg2(NO3)2 ⇌ Hg + Hg(NO3)2
These reactions are reversible; the nitric acid formed can redissolve the basic salt.[citation needed]
References Edit
- ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, Florida: CRC Press, pp. 4–45, ISBN 0-8493-0594-2
- ^ D. Grdenić (1956). "The crystal Structure of Mercurous Nitrate Dihydrate". Journal of the Chemical Society: 1312. doi:10.1039/jr9560001312.
- ^ Patnaik, Pradyot (2003), Handbook of Inorganic Chemical Compounds, McGraw-Hill Professional, p. 573, ISBN 0-07-049439-8, retrieved 2009-07-20
| HNO3 | He | |||||||||||||||||
| LiNO3 | Be(NO3)2 | B(NO3)−4 | RONO2 | NO3- NH4NO3 |
HOONO2 | FNO3 +F |
Ne | |||||||||||
| NaNO3 | Mg(NO3)2 | Al(NO3)3 Al(NO3)−4 |
Si | P | S | ClONO2 +Cl |
Ar | |||||||||||
| KNO3 | Ca(NO3)2 | Sc(NO3)3 | Ti(NO3)4 | VO(NO3)3 | Cr(NO3)3 | Mn(NO3)2 | Fe(NO3)2 Fe(NO3)3 |
Co(NO3)2 Co(NO3)3 |
Ni(NO3)2 | CuNO3 Cu(NO3)2 |
Zn(NO3)2 | Ga(NO3)3 | Ge | As | Se | BrNO3 +Br |
Kr | |
| RbNO3 | Sr(NO3)2 | Y(NO3)3 | Zr(NO3)4 | NbO(NO3)3 | MoO2(NO3)2 | Tc | Ru(NO3)3 | Rh(NO3)3 | Pd(NO3)2 Pd(NO3)4 |
AgNO3 Ag(NO3)2 |
Cd(NO3)2 | In(NO3)3 | Sn(NO3)4 | Sb(NO3)3 | Te | INO3 +IO3 |
Xe(NO3)2 | |
| CsNO3 | Ba(NO3)2 | Lu(NO3)3 | Hf(NO3)4 | TaO(NO3)3 | WO2(NO3)2 | ReO3NO3 | Os | Ir3O(NO3)10 | Pt(NO3)2 Pt(NO3)4 |
Au(NO3)3 | Hg2(NO3)2 Hg(NO3)2 |
TlNO3 Tl(NO3)3 |
Pb(NO3)2 | Bi(NO3)3 BiO(NO3) |
Po(NO3)4 | At | Rn | |
| FrNO3 | Ra(NO3)2 | Lr | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
| ↓ | ||||||||||||||||||
| La(NO3)3 | Ce(NO3)3 Ce(NO3)4 |
Pr(NO3)3 | Nd(NO3)3 | Pm(NO3)3 | Sm(NO3)3 | Eu(NO3)3 | Gd(NO3)3 | Tb(NO3)3 | Dy(NO3)3 | Ho(NO3)3 | Er(NO3)3 | Tm(NO3)3 | Yb(NO3)3 | |||||
| Ac(NO3)3 | Th(NO3)4 | PaO2(NO3)3 | UO2(NO3)2 | Np(NO3)4 | Pu(NO3)4 | Am(NO3)3 | Cm(NO3)3 | Bk(NO3)3 | Cf(NO3)3 | Es | Fm | Md | No | |||||