Neither strontium (Sr) nor antimony (Sb) is shown in the activity series of Table 4.5. Based on their positions in the periodic table, which would you expect to be the better reducing agent? Will the following reaction occur? Explain.

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 often determined by its position in the activity series, where metals higher in the series are generally better at losing electrons. Understanding the properties of strontium and antimony, including their electron configurations and reactivity, is essential for determining which is the better reducing agent.

Activity Series

The activity series is a list of metals ranked by their ability to displace other metals from compounds in solution. Metals higher in the series are more reactive and can act as reducing agents more effectively. Since strontium is an alkaline earth metal and typically more reactive than antimony, which is a metalloid, this series helps predict the likelihood of a reaction occurring between these elements.

Periodic Trends

Periodic trends refer to the predictable patterns in elemental properties across the periodic table, such as electronegativity, ionization energy, and atomic radius. These trends influence the reactivity of elements; for instance, as you move down a group, metallic character increases, making elements more likely to act as reducing agents. Analyzing the positions of strontium and antimony in the periodic table provides insight into their relative reactivity and potential to participate in redox reactions.