Question

Read the following redox reaction and determine which reactant is reduced and which is oxidized.

F2 + Zn --> ZnF2

Which is reduced & which is oxidized? Thanks!

Answer 1

Im gping to help you like this: In ZnF2 , you have a lattice of Zn2+ ions and F− ions. So you can re-write your equation as: Zn→Zn2++2e− F2+2e−→2F−
I think with this you may know how to proceed. May this help you a lot

Answer 2

Answer :
`F_2` reactant is reduced and
`Zn` reactant is oxidized.

Explanation :

Redox reaction : It is a type of reaction in which an oxidation and reduction reaction takes palace simultaneously.

Oxidation : The loss of electrons or increase in the oxidation number is an oxidation.

Reduction : The gain of electrons or decrease in the oxidation number is a reduction.

The given balanced redox reaction is,

`F_2+Zn\rightarrow ZnF_2`

The oxidation number of
`F_2` = 0

The oxidation number of
`Zn` = 0

The oxidation number of Zn in
`ZnF_2`

x + 2(-1) = 0

x = +2

The oxidation number of
`F_2` in
`ZnF_2` = -1

That means
`F_2` is reduced due to decrease in the oxidation number from 0 to (-1) and 'Zn' is oxidized due to increase in the oxidation number from 0 to (+2).

Therefore,
`F_2` reactant is reduced and
`Zn` reactant is oxidized.