By using the data in Appendix E, determine whether each of the following substances is likely to serve as an oxidant or a reductant: (d) Zn(s)

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Identify the standard reduction potential for the half-reaction involving Zn(s) from Appendix E.

Recall that a substance with a more positive standard reduction potential is more likely to be reduced and act as an oxidant.

Conversely, a substance with a more negative standard reduction potential is more likely to be oxidized and act as a reductant.

Compare the standard reduction potential of Zn(s) with other substances to determine its tendency to act as an oxidant or reductant.

Conclude whether Zn(s) is more likely to serve as an oxidant or a reductant based on its standard reduction potential.

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Oxidation and Reduction

Oxidation and reduction are chemical processes that involve the transfer of electrons between substances. Oxidation refers to the loss of electrons, while reduction involves the gain of electrons. In redox reactions, one substance is oxidized and another is reduced, which is essential for understanding the roles of oxidants and reductants.

Standard Reduction Potentials

Standard reduction potentials are values that indicate the tendency of a chemical species to be reduced, measured under standard conditions. These potentials are used to predict the direction of redox reactions and determine whether a substance will act as an oxidant or reductant. A higher reduction potential means a greater likelihood of being reduced.

Electrochemical Series

The electrochemical series is a list of standard reduction potentials for various half-reactions, arranged from highest to lowest. This series helps in identifying which substances can act as oxidants or reductants in a reaction. By comparing the position of a substance like Zn(s) in this series, one can infer its behavior in redox reactions.