Chemistry:Bromine nitrate
From HandWiki
| |
| Names | |
|---|---|
| Other names
Bromine mononitrate, bromo nitrate
| |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
PubChem CID
|
|
| |
| |
| Properties | |
| BrNO3 | |
| Molar mass | 141.91 g/mol |
| Appearance | Yellow liquid |
| Melting point | −42 °C (−44 °F; 231 K) |
| Boiling point | 0 °C (32 °F; 273 K) |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Tracking categories (test):
Bromine mononitrate is an inorganic compound, derived from bromine and nitric acid with the chemical formula BrNO3. The compound is a yellow liquid, decomposes at temperatures above 0 °C.[1]
Synthesis
1. Reaction of silver nitrate on an alcoholic solution of bromine:
- Br
2 + AgNO
3 → BrNO
3 + AgBr
2. Reaction of bromine chloride with chlorine nitrate at low temperatures:
- BrCl + ClNO
3 → BrNO
3 + Cl
2
Physical properties
Bromine mononitrate forms an unstable yellow liquid that decomposes at temperatures above 0 °C.
The molecule has the structure BrONO2.[2][3]
The compound is easily soluble in trichlorofluoromethane and carbon tetrachloride.
Applications
Bromine nitrate plays a role in tropospheric chemistry as it reacts with sulfuric acid.[4][5]
References
- ↑ "Bromine nitrate properties - SpringerMaterials". materials.springer.com. https://materials.springer.com/substanceprofile/docs/smsid_zutgcekqnkjjrjlr.
- ↑ Colussi, Agustín J.; Grela, María A. (1998). "Thermochemical kinetics of bromine nitrate, bromine nitrite, halogen hydroperoxides, dichlorine pentoxide, peroxycarboxylic acids, and diacyl peroxides" (in en). International Journal of Chemical Kinetics 30 (1): 41–45. doi:10.1002/(SICI)1097-4601(1998)30:1<41::AID-KIN5>3.0.CO;2-U. ISSN 1097-4601. https://onlinelibrary.wiley.com/doi/abs/10.1002/%28SICI%291097-4601%281998%2930%3A1%3C41%3A%3AAID-KIN5%3E3.0.CO%3B2-U. Retrieved 31 October 2021.
- ↑ Parthiban, Srinivasan; Lee, Timothy J. (8 July 1998). "Ab initio investigation of the atmospheric molecule bromine nitrate: Equilibrium structure, vibrational spectrum, and heat of formation". The Journal of Chemical Physics 109 (2): 525–530. doi:10.1063/1.476589. ISSN 0021-9606. https://aip.scitation.org/doi/10.1063/1.476589. Retrieved 31 October 2021.
- ↑ Sander, R.; Rudich, Y.; Glasow, R. von; Crutzen, P. J. (1999). "The role of BrNO3 in marine tropospheric chemistry: A model study" (in en). Geophysical Research Letters 26 (18): 2857–2860. doi:10.1029/1999GL900478. ISSN 1944-8007. https://agupubs.onlinelibrary.wiley.com/doi/abs/10.1029/1999GL900478. Retrieved 31 October 2021.
- ↑ Spencer, John E.; Rowland, F. S. (1 January 1978). "Bromine nitrate and its stratospheric significance". The Journal of Physical Chemistry 82 (1): 7–10. doi:10.1021/j100490a002. ISSN 0022-3654. https://pubs.acs.org/doi/10.1021/j100490a002. Retrieved 31 October 2021.
Salts and covalent derivatives of the nitrate ion
| HNO3 | He | ||||||||||||||||
| LiNO3 | Be(NO3)2 | B(NO3)−4 | C | NO−3, 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, Fe(NO3)2 |
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(NO3)3 | Zr(NO3)4 | Nb | Mo | Tc | Ru | Rh | Pd(NO3)2 | AgNO3 | Cd(NO3)2 | In | Sn | Sb(NO3)3 | 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, TlNO3 |
Pb(NO3)2 | Bi(NO3)3 BiO(NO3) |
Po | At | Rn | |
| FrNO3 | Ra(NO3)2 | 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 | Nd(NO3)3 | Pm | Sm | Eu(NO3)3 | Gd(NO3)3 | Tb(NO3)3 | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac(NO3)3 | Th(NO3)4 | Pa | UO2(NO3)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||
 |  |
