Bromine

Bromine, Br₂, does not react with oxygen, O₂, or nitrogen, N₂.

Bromine does react with ozone, O₃, at -78 °C, forming bromine(IV) oxide, BrO₂.

Br₂(l) + 2 O₃(g) 2 BrO₂(s) + O₂(g)


Bromine react with carbon monoxide, CO, forming COBr₂ [4].

Br₂(l) + CO(g) COBr₂(l)

Bromine, Br₂, react with hot aqueous alkali, forming bromate, BrO₃⁻. Only one sixth of the total bromine is converted in this reaction.

3 Br₂(g) + 6 OH⁻(aq) BrO₃⁻(aq) + 5 Br⁻(aq) + 3 H₂O(l)

Bromine, Br₂, reacts with fluorine, F₂, in gas phase, forming BrF. The product is difficult to obtain pure as BrF react with itself, forming Br₂, BrF₃ and BrF₅.

Br₂(g) + F₂(g) 2 BrF(g)
3 BrF(g) Br₂(l) + BrF₃(l)
5 BrF(g) 2 Br₂(l) + BrF₅(l)

Using excess fluorine at 150 °C, bromine will react with fluorine forming BrF₅.

Br₂(l) + 5 F₂(g) 2 BrF₅(l)


Chlorine, Cl₂, reacts with bromine, Br₂, in gas phase, forming the unstable bromine(I) chloride, ClBr.

Cl₂(g) + Br₂(g) 2 ClBr(g)


Bromine, Br₂, reacts with iodine, I₂, at room temperature, forming bromine(I) iodide, BrI.

Br₂(l) + I₂(s) 2 IBr(s)

Hydrogen reacts with Br₂ forming hydrogen bromide. The reaction is slow at room temperature, and increases in speed with increasing temperatures [4].

H₂(g) + Br₂(g) 2 HBr(g)

Cd reacts directly with Br₂ in aqueous solution and Br₂(g) at 450 °C [5].

Cd(s) + Br₂(aq) Cd²⁺(aq) + 2 Br⁻(aq)
Cd(s) + Br₂(g) CdBr₂(s) [pale yellow]


Mn(II)-ions are readily oxidized to MnO₂ by brome under alkaline conditions

Mn²⁺(aq) + Br₂(aq) + 2 OH⁻(aq) MnO₂(s) [brown-black] + 2 HBr(aq)

Manganese with oxidation steps >2 will be reduced to Mn(II) by Br⁻ under acidic conditions under the formation of Br₂, e.g.

MnO₂(s) + 2 Br⁻(aq) + 4 H⁺(aq) Mn²⁺(aq) + Br₂(aq) + 2 H₂O(l)


Nickel(II) can be oxidized to nickel(III) using Br₂ under alkaline conditions

2 Ni(OH)₂(s) + Br₂(aq) + 2 OH⁻(aq) 2 Ni(OH)₃(s) + 2 Br⁻(aq)

Phosphorous reacts with excess Br₂ forming phosphorous(V)chloride [4].

2 P(s) + 5 Br₂(l) 2 PBr₅(s)

with excess phosphorous [4], the reaction is

2 P(s) + 3 Br₂(l) 2 PBr₃(s)
PBr₃(s) + Br₂(l) PBr₅(s)

Sulfur reacts with excess bromine forming sulfur(I)bromide or sulfur(II)bromide [4]:

2 S(s) + Br₂(g) S₂Br₂(s)
S(s) + Br₂(g) SBr₂(s)


Bromine reacts with H₂S forming HBr [4]:

H₂S(g) + Br₂(l) 2 HBr(g) + S(s)

Bromine, Br₂, react with water, forming hypobromite, BrO⁻ [4].

Br₂(l) + H₂O(l) BrO⁻(aq) + 2 H⁺(aq) + Br⁻(aq)