Anhydrous nitric acid
|Molar mass||108.01 g/mol|
|Density||1.642 g/cm3 (18 °C)|
|Melting point||41 °C (106 °F; 314 K) |
|Boiling point||47 °C (117 °F; 320 K) sublimates|
|reacts to give HNO3|
|Solubility||soluble in chloroform
negligible in CCl4
|planar, C2v (approx. D2h)
N–O–N ≈ 180°
|178.2 J K−1 mol−1 (s)
355.6 J K−1 mol−1 (g)
Std enthalpy of
|−43.1 kJ/mol (s)
+11.3 kJ/mol (g)
Gibbs free energy (ΔfG˚)
|Main hazards||strong oxidizer, forms strong acid in contact with water|
|EU Index||Not listed|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is: / ?)(|
Dinitrogen pentoxide is the chemical compound with the formula N2O5. Also known as nitrogen pentoxide, N2O5 is one of the binary nitrogen oxides, a family of compounds that only contain nitrogen and oxygen. It is an unstable and potentially dangerous oxidizer that once was used as a reagent when dissolved in chloroform for nitrations but has largely been superseded by NO2BF4 (nitronium tetrafluoroborate).
N2O5 is a rare example of a compound that adopts two structures depending on the conditions: most commonly it is a salt, but under some conditions it is a polar molecule:
- N2O5 ⇌ [NO2+][NO3−]
Syntheses and properties
- P4O10 + 12 HNO3 → 4 H3PO4 + 6 N2O5
- N2O5 + H2O → 2 HNO3
Solid N2O5 is a salt, consisting of separated anions and cations. The cation is the linear nitronium ion NO2+ and the anion is the planar nitrate NO3− ion. Thus, the solid could be called nitronium nitrate. Both nitrogen centers have oxidation state +5.
The intact molecule O2N–O–NO2 exists in the gas phase (obtained by subliming N2O5) and when the solid is extracted into nonpolar solvents such as CCl4. In the gas phase, the O–N–O angle is 133° and the N–O–N angle is 114°. When gaseous N2O5 is cooled rapidly ("quenched"), one can obtain the metastable molecular form, which exothermically converts to the ionic form above −70 °C.
Reactions and applications
- N2O5 + Ar–H → HNO3 + Ar–NO2
where Ar represents an arene moiety.
In the atmosphere, dinitrogen pentoxide is an important reservoir of the NOx species that are responsible for ozone depletion: its formation provides a null cycle with which NO and NO2 are temporarily held in an unreactive state.
Replacement of the NO3− portion of N2O5 with BF4− gives nitronium tetrafluoroborate (NO2BF4, CAS#13826-86-3). This salt retains the high reactivity of NO2+, but it is thermally stable, decomposing at ca. 180 °C (into NO2F and BF3). NO2BF4 has been used to nitrate a variety of organic compounds, especially arenes and heterocycles. Interestingly, the reactivity of the NO2+ can be further enhanced with strong acids that generate the "super-electrophile" HNO22+.
- Emeleus (1 January 1964). Advances in Inorganic Chemistry. Academic Press. pp. 77–. ISBN 978-0-12-023606-0. Retrieved 20 September 2011.
- M.H. Deville (1849). "Note sur la production de l'acide nitrique anhydre". Compt. Rend. 28: 257–260.
- Jai Prakash Agrawal (19 April 2010). High Energy Materials: Propellants, Explosives and Pyrotechnics. Wiley-VCH. pp. 117–. ISBN 978-3-527-32610-5. Retrieved 20 September 2011.
- Holleman, A. F.; Wiberg, E. (2001), Inorganic Chemistry, San Diego: Academic Press, ISBN 0-12-352651-5
- Nitrogen(V) Oxide. Inorganic Syntheses 3. 1950. pp. 78–81.
- Talawar, M. B. et al. (2005). "Establishment of Process Technology for the Manufacture of Dinitrogen Pentoxide and its Utility for the Synthesis of Most Powerful Explosive of Today—CL-20". Journal of Hazardous Materials 124: 153–64. doi:10.1016/j.jhazmat.2005.04.021.