-1 Oxidation
The Potassium (K) has an oxidation number of +1. The Bromine (Br) has an oxidation number of -1.
The oxidation number of K (Potassium) in KBr (Potassium Bromide) is +1. This is because alkali metals like Potassium typically have an oxidation number of +1 in compounds.
The oxidation number of bromine in HOBr is +1. This is because the oxidation number of oxygen is typically -2 and the overall compound is neutral, so the oxidation number of hydrogen is +1. This leaves bromine with an oxidation number of +1 to balance the compound.
The oxidation number of bromine in bromine trifluoride is +3. This is because each fluorine atom has an oxidation number of -1, and since there are three fluorine atoms in bromine trifluoride, the overall charge must balance out to zero.
Bromine has an oxidation number of negative one, except when with oxygen or flourine.
The Potassium (K) has an oxidation number of +1. The Bromine (Br) has an oxidation number of -1.
The oxidation number of K (Potassium) in KBr (Potassium Bromide) is +1. This is because alkali metals like Potassium typically have an oxidation number of +1 in compounds.
The oxidation number of bromine in HOBr is +1. This is because the oxidation number of oxygen is typically -2 and the overall compound is neutral, so the oxidation number of hydrogen is +1. This leaves bromine with an oxidation number of +1 to balance the compound.
The oxidation number of bromine in bromine trifluoride is +3. This is because each fluorine atom has an oxidation number of -1, and since there are three fluorine atoms in bromine trifluoride, the overall charge must balance out to zero.
Bromine has an oxidation number of negative one, except when with oxygen or flourine.
Actually there are a few KBrO3 or NaBrO3 etc - in the bromate ion, bromine is in oxidation state +7
Potassium bromide is composed of two elements: potassium (K) and bromine (Br). Potassium is a metal and bromine is a non-metal. The chemical formula for potassium bromide is KBr.
+1
The oxidation number of carbon in CBr4 is +4 because bromine is more electronegative than carbon and is assigned an oxidation number of -1 each. Since there are four bromine atoms in CBr4, the total oxidation number of bromine is -4. The sum of the oxidation numbers in a compound must equal zero, so the carbon must have an oxidation number of +4 to balance the negative oxidation numbers from the bromine atoms.
The oxidation number of Br- is -1. Bromine typically has an oxidation state of -1 when it forms an ion by gaining one electron.
The oxidation number of Cs (Cesium) is +1, and the oxidation number of Br (Bromine) is -1. In CsBr, Cesium donates one electron to Bromine, resulting in Cs having an oxidation number of +1 and Br having an oxidation number of -1 in the compound.
The oxidation number of bromine in aqueous HBrO (hypobromous acid) is +1. This is because in HBrO, oxygen is more electronegative than bromine and will have an oxidation number of -2, leaving bromine with a +1 oxidation state to balance the overall charge of the molecule.