Mercury(I) nitrate

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Mercury(I) nitrate[1][2]
Mercury(I)-nitrate.png
Names
IUPAC name
Mercury(I) nitrate
Other names
Mercurous nitrate
Identifiers
10415-75-5 (anhydrous) YesY
7782-86-7 (dihydrate)
PubChem 25247
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
Hazards
NFPA 704
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g., canola oil Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazard OX: Oxidizer. E.g., potassium perchlorateNFPA 704 four-colored diamond
Related compounds
Other anions
Mercury(I) fluoride
Mercury(I) chloride
Mercury(I) bromide
Mercury(I) iodide
Other cations
Mercury(II) nitrate
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 YesY verify (what isYesY/N?)
Infobox references

Mercury(I) nitrate is a chemical compound with the formula Hg2(NO3)2. It is used in the preparation of other mercury(I) compounds, and, like all other mercury compounds, it is toxic.

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.

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:[2]

Hg2(NO3)2 → Hg + Hg(NO3)2

References[edit]

  1. ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4–45, ISBN 0-8493-0594-2 
  2. ^ a b Patnaik, Pradyot (2003), Handbook of Inorganic Chemical Compounds, McGraw-Hill Professional, p. 573, ISBN 0-07-049439-8, retrieved 2009-07-20 
Salts and the ester of the Nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)4 RONO2 NO3
NH4NO3
O FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)3 Co(NO3)2,
Co(NO3)3
Ni(NO3)2 Cu(NO3)2 Zn(NO3)2 Ga(NO3)3 Ge As Se Br Kr
RbNO3 Sr(NO3)2 Y Zr(NO3)4 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb Te I XeFNO3
CsNO3 Ba(NO3)2   Hf Ta W Re Os Ir Pt Au Hg2(NO3)2,
Hg(NO3)2
Tl(NO3)3 Pb(NO3)2 Bi(NO3)3 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv Uus Uuo
La Ce(NO3)x Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2(NO3)2 Np Pu Am Cm Bk Cf Es Fm Md No Lr