Consider the following substances: Fe2+(aq), Sn2+(aq), I-(aq). Identify the strongest reducing agent and the weakest reducing agent.

Verified step by step guidance

1. Identify the standard reduction potentials for each species from a standard reduction potential table.
2. Recall that a reducing agent is a substance that donates electrons and is oxidized in the process.
3. The strength of a reducing agent is inversely related to its reduction potential; the lower (more negative) the reduction potential, the stronger the reducing agent.
4. Compare the standard reduction potentials of Fe^{2+}, Sn^{2+}, and I^{-} to determine which has the lowest and highest values.
5. Identify the species with the lowest reduction potential as the strongest reducing agent and the one with the highest reduction potential as the weakest reducing agent.

Key Concepts

Reducing Agents

A reducing agent is a substance that donates electrons in a chemical reaction, thereby reducing another substance. The strength of a reducing agent is determined by its ability to lose electrons easily. Stronger reducing agents have a greater tendency to be oxidized, while weaker reducing agents are less likely to lose electrons.

Standard Reduction Potentials

Standard reduction potentials (E°) are measured values that indicate the tendency of a species to gain electrons and be reduced. A more negative E° value corresponds to a stronger reducing agent, as it indicates a greater likelihood of oxidation. By comparing the E° values of the given ions, one can determine which is the strongest and weakest reducing agent.

Electrochemical Series

The electrochemical series is a list of standard reduction potentials for various half-reactions, arranged from strongest to weakest oxidizing agents. This series helps predict the direction of redox reactions and the relative strength of reducing agents. By consulting this series, one can identify which of the given ions (Fe2+, Sn2+, I-) is the strongest and weakest reducing agent.