Metal Reactivity and Reactions

Overview

This lecture covers the reactivity series of metals, metal reactions with acids and water, and how to predict outcomes in displacement reactions.

The reactivity series ranks metals by how easily they form positive ions by losing outer shell electrons.
Group 1 metals are the most reactive, followed by Group 2 metals; transition metals are generally the least reactive.
Carbon and hydrogen are included in the series for comparison, even though they are not metals.

Metals reacting with acids produce a salt and hydrogen gas.
Highly reactive metals like potassium react explosively with acids, while less reactive metals show milder reactions.
Magnesium reacts with acids to produce bubbles; zinc and iron produce fewer bubbles; copper shows no reaction.
Temperature changes in reactions can indicate the degree of reactivity.
Fair testing requires equal mass, surface area, and consistent acid type and concentration for all samples.

Only the most reactive metals react with water to form metal hydroxides and hydrogen gas.
Lithium reacts with water, but zinc, iron, and copper do not; magnesium reacts only very slightly.

More reactive metals can displace less reactive metals from their compounds.
Magnesium will displace iron from iron sulfate solution, forming magnesium sulfate and iron.
Copper will not displace iron from iron sulfate, as copper is less reactive.

Reactivity Series — an ordered list of metals based on how easily they lose electrons to form positive ions.
Displacement Reaction — a reaction where a more reactive metal replaces a less reactive metal from its compound.
Transition Metals — metals found in the center of the periodic table, generally less reactive.
Positive Ion — an atom that has lost one or more electrons.

Review the reactivity series and memorize the order of common metals.
Practice predicting products of acid, water, and displacement reactions using the series.