chemistry...?

Question

Which statements are true about the reaction shown below?

CrO2- + ClO- →CrO42- + Cl-


A. Cr is an oxidizing agent.
B. Cl is oxidized.
C. O is oxidized.
D. Cl is an oxidizing agent.
E. Cr is oxidized.

more than one answer possible

Answer 1

D, E

Cr went from +5 to +10, it lost electrons so it was oxidized
Cl went from +3 to -1, it gained electrons so it was reduced, and therefore it is an oxidizing agent.

Answer 2

First, go through the equation and assign oxidation numbers to each element on both sides of the equation.

You'll find that the oxidation numbers of Cl and of Cr change--one of them increases and one decreases.

The element whose oxidation number increases was oxidized, and the one whose oxidation number decreases was reduced. An oxidizing agent becomes reduced in a redox reaction.

I think that two of the answers are correct, but you should be able to figure that out...

Answer 3

CrO2- + 2ClO- →CrO42- + 2Cl-

CrO2- the oxidation state of chromium is +3

In CrO42-, the oxidation state of chromium is +6


Cr has been oxidised and lost three electrons and therefore acting as a reducing agent

In ClO-, the oxidation state of chlorine is +1

In Cl-. the oxidation state of chlorine is -1

Chlorine has been reduced and gained two electrons, abd therefore acting as an oxidising agent.

A) is false
B) is false
C) is false
D) is true
E) is true.

Answer 4

E. Cr is oxidized, therefore Cl is the oxidizing agent, D is also true.