Consider the following substances: Fe(s), PbO2(s), H+(aq), Al(s), Ag(s), Cr2O72-(aq).(d) Which substances can be oxidized by Cu2+(aq)? Which can be reduced by H2O2(aq)?

Oxidation and reduction are chemical processes involving the transfer of electrons between substances. Oxidation refers to the loss of electrons, while reduction involves the gain of electrons. In redox reactions, one species is oxidized and another is reduced, which is essential for understanding how substances interact, particularly in the context of electrochemistry.

Standard reduction potentials are values that indicate the tendency of a species to gain electrons and be reduced. These potentials are measured under standard conditions and are used to predict the direction of redox reactions. A higher standard reduction potential means a greater likelihood of being reduced, which helps determine which substances can be oxidized or reduced in a reaction.

The reactivity of metals and nonmetals plays a crucial role in determining their ability to undergo oxidation or reduction. Metals, particularly those that are more electropositive, tend to lose electrons easily and can be oxidized, while nonmetals often gain electrons. Understanding the reactivity series helps predict which substances can be oxidized by Cu2+ or reduced by H2O2 in the given question.