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Bromine monofluoride is a quite unstable interhalogen compound with the chemical formula BrF. It can be produced through the reaction of bromine trifluoride (or bromine pentafluoride) and bromine. Due to its lability, the compound can be detected but not isolated: [2] BrF 3 + Br 2 → 3 BrF BrF 5 + 2 Br 2 → 5 BrF Br 2(l) + F 2(g) → 2 BrF (g)
The well-characterized heavier halogens (chlorine, bromine, and iodine) all form mono-, tri-, and pentafluorides: XF, XF 3, and XF 5. Of the neutral +7 species, only iodine heptafluoride is known. [93] While chlorine and bromine heptafluorides are not known, the corresponding cations ClF + 6 and BrF + 6, extremely strong oxidizers, are. [94]
Chlorine monofluoride (ClF) is the lightest interhalogen compound. ClF is a colorless gas with a normal boiling point of −100 °C. Bromine monofluoride (BrF) has not been obtained as a pure compound — it dissociates into the trifluoride and free bromine. It is created according to the following equation: Br 2 (l) + F 2 (g) → 2 BrF(g)
Carbon monofluoride (CF, CF x, or (CF) x), also called polycarbon monofluoride; Chlorine monofluoride, a volatile interhalogen compound with formula ClF; Iodine monofluoride, a chocolate-brown solid compound with formula IF; Hydrogen fluoride, a liquid or gas with boiling point at about 20 °C, HF; Nitrogen monofluoride, a metastable compound ...
Bond energies to bromine tend to be lower than those to chlorine but higher than those to iodine, and bromine is a weaker oxidising agent than chlorine but a stronger one than iodine. This can be seen from the standard electrode potentials of the X 2 /X − couples (F, +2.866 V; Cl, +1.395 V; Br, +1.087 V; I, +0.615 V; At, approximately +0.3 V ...
Bromine fluoride may refer to several compounds with the elements bromine and fluorine: Bromine monofluoride, BrF;
Bromine was discovered independently by two chemists, Carl Jacob Löwig [13] and Antoine Balard, [14] [15] in 1825 and 1826, respectively. [16] Löwig isolated bromine from a mineral water spring from his hometown Bad Kreuznach in 1825. Löwig used a solution of the mineral salt saturated with chlorine and extracted the bromine with diethyl ...
The compound forms a colorless volatile liquid that decomposes at temperatures above 10 °C. It is highly reactive and unstable, [ 4 ] and corrodes glass at room temperature. Chemical properties