(b) Which of the following reactions would you expect to occur according to the activity series you established in part (a)?

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Identify the metals or elements involved in the reactions provided.

Refer to the activity series you established in part (a) to determine the reactivity order of these metals or elements.

Compare the reactivity of the elements in each reaction: a more reactive element can displace a less reactive element from its compound.

For each reaction, check if the element that is supposed to displace another is higher in the activity series.

Conclude which reactions are feasible based on whether the displacing element is more reactive than the element it is trying to displace.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Activity Series

The activity series is a list of metals ranked by their reactivity from highest to lowest. It helps predict whether a metal will displace another in a chemical reaction. More reactive metals can replace less reactive ones in compounds, which is crucial for understanding single displacement reactions.

Single Displacement Reactions

Single displacement reactions occur when one element replaces another in a compound. The general form is A + BC → AC + B, where A is a more reactive element displacing B from the compound BC. Understanding this type of reaction is essential for applying the activity series to predict reaction outcomes.

Reactivity of Metals

The reactivity of metals is influenced by their ability to lose electrons and form positive ions. Factors such as atomic size, ionization energy, and electronegativity play a role in determining a metal's reactivity. This concept is vital for interpreting the activity series and predicting which reactions will occur.

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