In the compound FeBr2, the oxidation state of iron (Fe) and bromine (Br) can be determined as follows:
Let's assign the oxidation state of bromine as x.
Since FeBr2 is a neutral compound, the sum of the oxidation states of its elements must add up to zero. Therefore, we can set up the equation:
2(-1) + x = 0
Simplifying the equation, we get:
-2 + x = 0
Adding 2 to both sides, we find:
x = 2
So, the oxidation state of bromine (Br) in FeBr2 is -1.
To determine the oxidation state of iron (Fe), we can use the fact that the sum of the oxidation states of all the elements in a compound must add up to zero. In this case, we have one iron atom and two bromine atoms:
Fe + 2(-1) = 0
Simplifying the equation, we find:
Fe - 2 = 0
Adding 2 to both sides, we get:
Fe = 2
Therefore, the oxidation state of iron (Fe) in FeBr2 is +2.