Chemistry: An Introduction to General, Organic, and Biological Chemistry (12th Edition)

Published by Prentice Hall
ISBN 10: 0321908449
ISBN 13: 978-0-32190-844-5

Chapter 7 - Section 7.5 - Oxidation-Reduction Reactions - Questions and Problems - Page 235: 7.42a

Answer

$Li$ is oxidized and $F$ is reduced.

Work Step by Step

1. Rewrite the equation to show the ions and the atoms: $2Li(s) + F_2(g) --\gt 2Li^+(s) + 2F^-(s)$ 2. Analyze what happens to each atom/ion during the reaction. During this process, These are the charge increases/decreases: $Li^0 --\gt Li^+$: The increase in charge indicates that $Li$ is oxidized. $F^0 --\gt F^-$: The decrease in charge indicates that $F$ is reduced.
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