Bromine is in the seventh family on the Periodic Table. That means that it has seven valence electrons. It wants to have eight valence electrons to be stable, so it will gain an electron, making it negative. The oxidation number of Br is Br-1.
That depends on the substance it is part of.
In the element, the OS is zero.
In many compounds, such as metal bromides, it is -1.
It also forms compounds where its OS is +7, +5, +3 and +1.
Br = +1 oxidation state
O = -2 oxidation state
+5 oxidation state
-1
If Br had an oxidation number of +7, the net charge on the ion would be +1, and not -1. Thus, the oxidation number for Br in BrO3- should be 5+.
Oxidation number of Br in BrO3 is 6. BrO3 doesn't exist. It should actually be BrO3- ion with +5 oxidation number for Br.
Each Br atom has an oxidation number of zero.
The Potassium (K) has an oxidation number of +1. The Bromine (Br) has an oxidation number of -1.
dcn
If Br had an oxidation number of +7, the net charge on the ion would be +1, and not -1. Thus, the oxidation number for Br in BrO3- should be 5+.
Oxidation number of Br in BrO3 is 6. BrO3 doesn't exist. It should actually be BrO3- ion with +5 oxidation number for Br.
-2 for each O, +5 for Br
Each Br atom has an oxidation number of zero.
The Potassium (K) has an oxidation number of +1. The Bromine (Br) has an oxidation number of -1.
+1 for Na -1 for Br
Each Br atom has an oxidation number of zero.
dcn
The molecular formula should be CBr4. The oxidation numbers are -1 for each Br, +4 for C.
-1 in bromide (most common). It can exhibit oxidation numbers from -1 to +7 (in HBrO4)
-1 for Cl and +1 for Br
-1 for bromine in bromide