Scandium nitrate

Scandium(III) nitrate, Sc(NO3)3, is an ionic compound. It is an oxidizer, as all nitrates are. The salt is applied in optical coatings, catalysts, electronic ceramics and the laser industry.

Scandium(III) nitrate
Scandium(III) nitrate
Names
IUPAC name
scandium(3+) trinitrate
Identifiers
3D model (JSmol)
ECHA InfoCard 100.033.350
EC Number
  • 236-701-5
UNII
  • InChI=1S/3NO3.Sc/c3*2-1(3)4;/q3*-1;+3
    Key: DFCYEXJMCFQPPA-UHFFFAOYSA-N
  • [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Sc+3]
Properties
Sc(NO3)3
Molar mass 230.97 g/mol
Appearance off-white crystals
Solubility in other solvents water and strong mineral acids
Related compounds
Related compounds
 Scandium(III) chloride
Scandium(III) fluoride
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

Preparation

Scandium nitrate can be prepared by the reaction between scandium metal with dinitrogen tetroxide.[1]

Sc + 3 N2O4 → Sc(NO3)3 + 3 NO

The anhydrous form can also be obtained by the reaction between scandium chloride and dinitrogen pentoxide.[2] The tetrahydrate can be obtained from the reaction between scandium hydroxide and nitric acid.[3]

Properties

Scandium nitrate is a white solid which dissolves in water and ethanol.[4] It has multiple hydrated forms, including the dihydrate, trihydrate, and tetrahydrate. The tri- and tetrahydrate exist in the monoclinic crystal system. Upon heating in air to 50 °C, the tetrahydrate transforms into the dihydrate, which at 60 °C further converts to Sc4O3(NO3)3·6.5H2O. At 140–220 °C, Sc4O5(NO3)3 is formed.[2]

References
  1. Brauer, Georg (1975). Handbuch der präparativen anorganischen Chemie (3rd ed.). Stuttgart: Enke. p. 1109. ISBN 3-432-02328-6. OCLC 310719485.
  2. Scandium : its occurrence, chemistry, physics, metallurgy, biology, and technology. Chaim T. Horovitz. Academic Press. 2012. p. 119. ISBN 0323144519. OCLC 768016723.{{cite book}}: CS1 maint: others (link)
  3. Riedel, Erwin (2011). Anorganische Chemie. Christoph Janiak (8th ed.). Berlin: De Gruyter. p. 773. ISBN 978-3-11-022567-9. OCLC 753966312.
  4. William M., Haynes (2012). CRC Handbook of Chemistry and Physics. William M. Haynes (93rd ed.). Boca Raton, FL: CRC. p. 86. ISBN 978-1-4398-8049-4. OCLC 793213751.
Salts and covalent derivatives of the nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)−4 RONO2 NO−3
NH4NO3		 HOONO2 FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3
Al(NO3)−4		 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)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 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 Xe(NO3)2
CsNO3 Ba(NO3)2   Lu(NO3)3 Hf(NO3)4 TaO(NO3)3 W Re Os Ir 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 Es Fm Md No
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