Chromium nitrate

Chromium nitrate

Names
IUPAC name Chromium(III) nitrate
Other names Nitric acid, chromium(3+) salt
Identifiers
CAS Number	13548-38-4 7789-02-8 (nonahydrate)
3D model (Jmol)	Interactive image
ChemSpider	15285818
ECHA InfoCard	100.033.550
PubChem	24598
RTECS number	GB6300000
UNII	C6H0RE016B
UN number	2720
InChI InChI=1S/Cr.3NO3/c;3*2-1(3)4/q+2;3*-1 Key: BXWGVGRRIQRLLZ-UHFFFAOYSA-N InChI=1/Cr.3NO3/c;3*2-1(3)4/q+2;3*-1 Key: BXWGVGRRIQRLLZ-UHFFFAOYAO
SMILES [Cr+2].O=N([O-])=O.[O-]N(=O)=O.[O-]N(=O)=O
Properties
Chemical formula	Cr(NO3)3 [Cr(H2O)6](NO3)3•3H2O (nonahydrate)
Molar mass	238.011 g/mol (anhydrous) 400.21 g/mol (nonahydrate)
Appearance	Blue-violet crystals (anhydrous) Purple crystals (nonahydrate)
Density	1.85 g/cm^3 (nonahydrate)
Melting point	60.06 °C (140.11 °F; 333.21 K) nonahydrate
Boiling point	> 100 °C (212 °F; 373 K) (decomposes)
Solubility in water	81 g/100 mL (20 °C)
Hazards
Safety data sheet	Oxford MSDS
NFPA 704	0 3 1 OX
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	3250 mg/kg (rat, oral, nonahydrate) 110 mg/kg (mouse, oral)[1]
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

Chromium(III) nitrate describes several inorganic compounds consisting of chromium, nitrate and varying amounts of water. Most common is the dark violet hydrated solid, but an anhydrous green form is also known. Chromium(III) nitrate compounds are of a limited importance commercially, finding some applications in the dyeing industry.^[2] It is common in academic laboratories for the synthesis of chromium coordination complexes.

Structure

The relatively complicated formula - [Cr(H₂O)₆](NO₃)₃•3H₂O - highlights the complicated structure of this material. The chromium centers are bound to six water ligands, and the remaining volume of the solid is occupied by three nitrate anions and three molecules of water of crystallization. Such complicated formulas typify hydrated metal salts.

Properties and preparation

The anhydrous salt forms green crystals and very soluble in water (in contrast to anhydrous chromium(III) chloride which dissolves very slowly except under special conditions). At 100 °C it decomposes. The red-violet hydrate is highly soluble in water. Chromium nitrate is used in the production of alkali metal-free catalysts and in pickling.

Chromium nitrate can be prepared by dissolving chromium oxide in nitric acid.^[2]

References

1. "Chromium(III) compounds [as Cr(III)]". Immediately Dangerous to Life and Health. National Institute for Occupational Safety and Health (NIOSH).
2. Gerd Anger, Jost Halstenberg, Klaus Hochgeschwender, Christoph Scherhag, Ulrich Korallus, Herbert Knopf, Peter Schmidt, Manfred Ohlinger, "Chromium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005.

Salts and covalent derivatives of the Nitrate ion
HNO3																	He
LiNO3	Be(NO3)2											B(NO3)4^−	C	N	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	Xe(NO3)2
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 BiO(NO3)	Po	At	Rn
Fr	Ra		Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Nh	Fl	Mc	Lv	Ts	Og
		↓
		La	Ce(NO3)3, Ce(NO3)4	Pr	Nd	Pm	Sm	Eu	Gd(NO3)3	Tb	Dy	Ho	Er	Tm	Yb	Lu
		Ac	Th	Pa	UO2(NO3)2	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr