Let tho oxidation number of Br=x.The oxidation no of H=+1 and that of o=-2. Thus adding all => 1 + x - 2 = 0 => x - 1 = 0 => x = 1
Thus x comes out to be x = 1.
The oxidation of oxygen is -2, hydrogen is +1, so bromine must be +1.
This is a little bit stong acid. Bromine shows +7 as the oxidation number.
+1 for H
+3 for Br
-2 for O
Br would have a 1+ oxidation #
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