Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons. (b) For the reaction \(\mathrm{Fe}^{3+}(a q)+\mathrm{Co}^{2+}(a q) \longrightarrow \mathrm{Fe}^{2+}(a q)+\) \(\mathrm{Co}^{3+}(a q), \mathrm{Fe}^{3+}(a q)\) is the reducing agent and \(\mathrm{Co}^{2+}(a q)\) is the oxidizing agent. (c) If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction.

Is "If something is oxidized, it is formally losing electrons" true or false? In a redox reaction, when a reactant is oxidized, it formally loses electrons as it has an increase in its oxidation state. Therefore, this statement is true.

Is "For the reaction \(\mathrm{Fe}^{3+}(a q)+\mathrm{Co}^{2+}(a q)\longrightarrow \mathrm{Fe}^{2+}(a q)+\mathrm{Co}^{3+}(a q), \mathrm{Fe}^{3+}(a q)\) is the reducing agent and \(\mathrm{Co}^{2+}(a q)\) is the oxidizing agent" true or false? First, identify which elements are being oxidized and which are being reduced: - \(\mathrm{Fe}^{3+}(a q)\) is reduced to \(\mathrm{Fe}^{2+}(a q)\) because its oxidation state decreases from +3 to +2. - \(\mathrm{Co}^{2+}(a q)\) is oxidized to \(\mathrm{Co}^{3+}(a q)\) because its oxidation state increases from +2 to +3. A reducing agent is a substance that causes the reduction of another substance, meaning it provides electrons to the other species. In this case, \(\mathrm{Fe}^{3+}(a q)\) is the species being reduced, and \(\mathrm{Co}^{2+}(a q)\) is the species that is providing the electrons for this reduction to happen, so \(\mathrm{Co}^{2+}(a q)\) is the reducing agent. An oxidizing agent is a substance that causes the oxidation of another substance, meaning it takes electrons from the other species. In this case, \(\mathrm{Co}^{2+}(a q)\) is the species being oxidized, and \(\mathrm{Fe}^{3+}(a q)\) is the species taking electrons from Cobalt, so \(\mathrm{Fe}^{3+}(a q)\) is the oxidizing agent. Therefore, this statement is false because it incorrectly states the roles of \(\mathrm{Fe}^{3+}(a q)\) and \(\mathrm{Co}^{2+}(a q)\).

Is "If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction" true or false? In a redox reaction, there is always a change in the oxidation state of at least one element in the reactants and products, since the exchange of electrons is occurring in the reaction. If there are no changes in the oxidation states of the elements in a reaction, then it cannot be a redox reaction. Therefore, this statement is true.