What describes the change in oxidation states of the following reaction? 2Cl- + F2 > 2F- + Cl2 a. Cl– reduces to Cl and F oxidizes to F–. b. Cl– oxidizes to Cl and F reduces to F–. d. Cl is the reducing agent and F– is the oxidizing agent.

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What describes the change in oxidation states of the following reaction? 2Cl- + F2 > 2F- + Cl2 a. Cl– reduces to Cl and F oxidizes to F–. b. Cl– oxidizes to Cl and F reduces to F–. d. Cl is the reducing agent and F– is the oxidizing agent.

Chemistry
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At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.

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@warpedkitten diatomic elements like F2 and Cl2 have an oxidation state of 0 so remember if your oxidation state goes up that means that electrons are lost oxidation. if your oxidation state goes down that means you've gained electrons and that's reduction
I agree with u @Photon336 So as we can see cl - goes to 0 oxidation state thus it is oxidising. And F2 goes from 0 to -1 state ttus reducing so the answer will be b

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