BrO3 is an anion of minus one (-1) charge.
BrO3^-1
Using oxygen as the standard at '-2'
Then the oxygen moiety is 3 X -2 = -6
So doing a 'little' sum
-6 + Br = -1
Add '6' to both sides
Br = 5 (The oxidation number of Br).
NB Using '-2' for oxygen is a good standard for most molecules/ions. However, oxygen's oxidation number does vary , but not in very many molecules/ions.
In the bromate anion, BrO3- Br has the oxidation number of 5. To work this out remove each O from the ion as O2- this leaves Br with a notional charge of +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.
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+.
Each Oxygen has -2 number.Bromines oxidation number is +5.
LiBrO3 this decomposes to Li^(+) & BrO3^(-) The bromate anion has a charge of '-1' Use the standard for oxygen at '-2' Since there are 3 oxygens then the oxygen moiety is 3 X -2 = -6 Creating a little sum Br + -6( oxygen moiety) = -1( anion charge) Br - 6 = -1 Add '6 'to both sides Br = (+)5 The oxidation state of bromine.
-1 for each Br, +5 for P
Oxidation number of Br in BrO3 is 6. BrO3 doesn't exist. It should actually be BrO3- ion with +5 oxidation number for Br.
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+.
-2 for each O, +5 for Br
In the bromate ion (BrO3-) bromine is in the 5+ oxidation stae while the oxygen atoms are in the 2- oxidation state.
Each Oxygen has -2 number.Bromines oxidation number is +5.
-2 for each O, +5 for Br
LiBrO3 this decomposes to Li^(+) & BrO3^(-) The bromate anion has a charge of '-1' Use the standard for oxygen at '-2' Since there are 3 oxygens then the oxygen moiety is 3 X -2 = -6 Creating a little sum Br + -6( oxygen moiety) = -1( anion charge) Br - 6 = -1 Add '6 'to both sides Br = (+)5 The oxidation state of bromine.
-1 for each Br, +5 for P
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.
In the formula NaBrO3, Oxygen will always have a -2 oxidation number. In this case the total number for oxygen in -6 because there are three oxygen atoms. Sodium will always have a +1 oxidation number therefore its total oxidation number is +1. The entire charge has to equal zero so taking what we have now: -6 and +1 we have a -5 left over. Therefore, Bromine must have a +5 oxidation number.
+1 for Na -2 for each O +5 for Br
The oxidation number of Sb in Sb2O5 is +5.