Question

give the oxidation number of bromine in the following:

part 1 of 4
write the oxidation number of bromine in \\(\text{brf}_5\\).

part 2 of 4
write the oxidation number of bromine in \\(\text{br}_2\\).

part 3 of 4
write the oxidation number of bromine in \\(\text{brf}\\).

part 4 of 4
write the oxidation number of bromine in \\(\text{libr}\\).

Explanation:

Determine oxidation state in BrF5

Fluorine is the most electronegative element and always has an oxidation state of \(-1\) in its compounds.
Let \(x\) be the oxidation state of bromine in \(\text{BrF}_5\):

$$ x + 5(-1) = 0 \implies x = +5 $$

Determine oxidation state in Br2

Elemental bromine \(\text{Br}_2\) is a pure homonuclear diatomic molecule.
By definition, the oxidation state of any element in its free, uncombined elemental form is \(0\):

$$ 2x = 0 \implies x = 0 $$

Determine oxidation state in BrF

Fluorine is more electronegative than bromine and takes an oxidation state of \(-1\).
Let \(x\) be the oxidation state of bromine in \(\text{BrF}\):

$$ x + 1(-1) = 0 \implies x = +1 $$

Determine oxidation state in LiBr

Lithium is an alkali metal (Group 1) and always has an oxidation state of \(+1\) in ionic compounds.
Let \(x\) be the oxidation state of bromine in \(\text{LiBr}\):

$$ +1 + x = 0 \implies x = -1 $$

Answer:

Question 1

The oxidation number of bromine in \(\text{BrF}_5\) is <blank>+5</blank>.

Question 2

The oxidation number of bromine in \(\text{Br}_2\) is <blank>0</blank>.

Question 3

The oxidation number of bromine in \(\text{BrF}\) is <blank>+1</blank>.

Question 4

The oxidation number of bromine in \(\text{LiBr}\) is <blank>-1</blank>.