In the reaction Se₂Cl₂ → A + B . The oxidation state of A and B are

Se₂Cl₂ is a neutral molecule, so the sum of the oxidation states of Se and Cl must be zero.

Let x be the oxidation state of Se and y be the oxidation state of Cl.

Then we have: 2x + 2y = 0

Simplifying this equation gives:

x + y = 0

Since Cl has a fixed oxidation state of -1 in most of its compounds, we can substitute -1 for y in the equation above to get:

x + (-1) = 0

x = +1

Therefore, the oxidation state of Se in Se₂Cl₂ is +1.

Now let's look at the products A and B.

Since Se is being oxidized in this reaction, at least one of the products A or B must have a higher oxidation state than +1.

We cannot determine the exact oxidation states of A and B without more information about the reaction and the nature of the products.