Tin(IV) nitrate

Names
Other names
Identifiers

3D model (JSmol)

ChemSpider
ECHA InfoCard 100.222.600
EC Number

PubChem CID

Properties
Sn(NO3)4
Molar mass 366.73 g/mol
Appearance Silky Crystals
Density 2.65 g/cm3
Melting point 91 °C (196 °F; 364 K)
Boiling point 98 °C (208 °F; 371 K) (decomposes)
Reacts
Solubility Soluble in carbon tetrachloride, chloroform
Structure[3]
Monoclinic
P21/c

a = 7.80 Å, b = 13.85 Å, c = 10.23 Å

Hazards
GHS labelling:

Danger
H272, H314
P220, P280, P305+P351+P338, P310

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Tin(IV) nitrate is a salt of tin with nitric acid. It is a volatile white solid, subliming at 40 °C under a vacuum. Unlike other nitrates, it reacts with water to produce nitrogen dioxide.

Structure[edit]

It is structurally very similar to titanium(IV) nitrate, with the only major difference being the Sn–O bond(2.161 Å) being slightly longer than the Ti–O bond(2.068 Å).[3]

Production[edit]

It was first prepared in the 1960s. Tin(IV) chloride was added to dinitrogen pentoxide at -78 °C, which produced tin(IV) nitrate and nitryl chloride:[4]

SnCl4 + 4 N2O5 → Sn(NO3)4 + 4 NO2Cl

Attempts to prepare this compound by reacting tin(II) oxide and nitric acid resulted in a formation of tin(II) nitrate hydroxide.[5]

Reactions[edit]

This compound is sensitive to water, it hydrolyzes into tin(IV) oxide and nitrogen dioxide. Tin(IV) nitrate reacts with trifloroacetic acid anhydride to yield (NO2+)2[Sn(OOCCF3)62−] which is a nitronium salt. With trifluoroacetic acid a similar compound solvated with trifluoroacetic acid is produced.[6]

It also reacts with acetic anhydride or acetic acid to produce tin(IV) acetate and with nitric oxide to produce tin(IV) oxynitrate.

The reaction of tin(IV) nitrate with triphenylphosphine and triphenylarsine yields dinitratotin(IV)bis(diphenylphosphonate) and dinitratotin(IV)bis(diphenylarsonate).[6]

References[edit]

  1. ^ “Tin(IV) Nitrate”. American Elements. American Elements. Retrieved 16 February 2021.
  2. ^ “Tin(IV) nitrate”. Sigma-Aldrich. Sigma-Aldrich. Retrieved 16 February 2021.
  3. ^ a b C. D. Garner; D. Sutton; S. C. Wallwork (1967). “The crystal structures of anhydrous nitrates and their complexes. Part IV. Tin(IV) nitrate”. Journal of the Chemical Society A: Inorganic, Physical, Theoretical: 1949–1954. doi:10.1039/J19670001949.
  4. ^ C. C. Addison; W. B. Simpson (1965). “Tin(IV) nitrate: the relation between structure and reactivity of metal nitrates”. Journal of the Chemical Society: 598–602. doi:10.1039/JR9650000598.
  5. ^ J. D. Donaldson; W. Moser (1961). “Basic tin(II) nitrate”. Journal of the Chemical Society (Resumed). 381: 1996–2000. doi:10.1039/JR9610001996.
  6. ^ a b Harrison, Philip G.; Khalil, Mutassim I.; Logan, Norman (January 1978). “A contribution to the chemistry of tin(IV) nitrate”. Inorganica Chimica Acta. 30: 165–170. doi:10.1016/S0020-1693(00)89031-3.
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

+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 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 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

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