Question

Which of the following is the best reducing agent: \(\mathrm{F}_{2}, \mathrm{H}_{2}, \mathrm{Na}\), \(\mathrm{Na}^{+}, \mathrm{F}^{-}\) ? Explain. Order as many of these species as possible from the best to the worst oxidizing agent. Why can't you order all of them? From Table \(18.1\) choose the species that is the best oxidizing agent. Choose the best reducing agent. Explain.

Short answer

Among the given species, sodium \((\mathrm{Na})\) is the best reducing agent, and fluorine \((\mathrm{F}_{2})\) is the best oxidizing agent. This is because \(\mathrm{Na}\) has a higher tendency to lose electrons and get oxidized, while \(\mathrm{F}_{2}\) has a greater ability to gain electrons and get reduced due to its electronegativity. From Table 18.1, the strongest reducing agent is lithium \((\mathrm{Li})\), and the strongest oxidizing agent remains to be fluorine \((\mathrm{F}_{2})\).

Step-by-step solution

Identify the given species

The given species are: \(\mathrm{F}_{2}, \mathrm{H}_{2}, \mathrm{Na}, \mathrm{Na}^{+}, \mathrm{F}^{-}\).

Determine the best reducing agent

To determine the best reducing agent, we need to consider which species has the greatest tendency to lose electrons and get oxidized. Since metallic elements, such as sodium \((\mathrm{Na})\), are more likely to lose electrons and form cations, \(\mathrm{Na}\) can be considered the best reducing agent among the given species.

Order as oxidizing agents

Now, we need to order the given species based on their oxidizing ability. The order will be as follows: 1. \(\mathrm{F}_{2}\) 2. \(\mathrm{H}_{2}\) The \(\mathrm{F}_{2}\) is the strongest oxidizing agent among the given species, as it is the most electronegative element and thus has the highest tendency to gain electrons. The \(\mathrm{H}_{2}\) is second in the list of oxidizing agents, as it can gain electrons to form \(\mathrm{H}^-\) ions. We cannot order the other species because \(\mathrm{Na}\) is not an oxidizing agent and will not gain electrons, and the remaining ions \(\mathrm{Na}^{+}\) and \(\mathrm{F}^-\) are already in their oxidized and reduced forms, respectively.

Choose the best oxidizing agent and reducing agent from Table 18.1

From Table 18.1, we can determine the strongest reducing and oxidizing agents: Best oxidizing agent: \(\mathrm{F}_2\) Best reducing agent: \(\mathrm{Li}\) (lithium is at the top of the reactivity series) In summary, among the given species, \(\mathrm{Na}\) is the best reducing agent, while \(\mathrm{F}_{2}\) is the best oxidizing agent. From Table 18.1, the strongest reducing agent is \(\mathrm{Li}\), and the strongest oxidizing agent is still \(\mathrm{F}_{2}\).