Four `Cl_(2)` molecules undergo a loss and gain of `6 "mole" ` of electrons to form two oxidation states of `Cl` in a auto redox change. What are the `+ve` and `-ve` oxidation state of `Cl` in the change?

Options

A. `Cl^(5+),Cl^(0)`
B. `Cl^(7+),Cl^(1-)`
C. `Cl^(3+), Cl^(0)`
D. `Cl^(3+),Cl^(1-)`

Answer

D

Explanation

`Cl_(2)` can show the gain of electron by
`2e+Cl_(2)rarr2Cl^(-)`
Since in all six electrons are used by four `Cl_(2)` molecules. Thus,
`{:(6e,+,3Cl_(2)rarr,6Cl^(-),),(,,Cl_(2)rarr,2Cl^(3+)+,6e):}`