Actually there are a few KBrO3 or NaBrO3 etc - in the bromate ion, bromine is in oxidation state +7
Bromine typically exists in the -1 oxidation state in ionic compounds. In elemental form or as part of a molecule, bromine can have various oxidation states ranging from -1 to +7.
Bromine has an oxidation number of negative one, except when with oxygen or flourine.
The oxidation states of halogens can range from -1 to +7. Fluorine typically has an oxidation state of -1, while the other halogens (chlorine, bromine, iodine) can have oxidation states from -1 to +7 depending on the compound and bonding.
-1 in bromide (most common). It can exhibit oxidation numbers from -1 to +7 (in HBrO4)
The oxidation state of Cl in HClO4 is +7. In HClO4, since the oxidation state of H is +1 and that of O is -2, the sum of the oxidation states in the compound must equal 0. Therefore, the oxidation state of Cl in this case is +7.
-1 = in Bromides 0 = in Br2 +1 = in Hypobromites +3 = in Bromine trichloride +5 = in Bromates +7 = in Perbromates
The most common oxidation state of chlorine is -1, where it gains one electron to achieve a full valence shell. However, chlorine can also exhibit oxidation states of +1, +3, +5, and +7 depending on the compound it is a part of.
7
HIO4.2H2O O.S. of H = +1 O.S. of I = +7 O.S. of O = -2
O.S of Mn = 3+ O.S. of Cl = 7+ O.S. of O = 2-
Technetium oxidation states are between -1 and +7; the most usual valences are +3, +4 and +7.