Predicting and identifying reactions and products Study Guide

The reactivity of a metal is directly linked to its tendency to lose electrons and form positive ions. Metals react by losing one or more outer shell electrons to achieve a stable electron configuration, typically forming a positive ion (cation). More reactive metals have a greater tendency to lose these electrons, meaning they readily oxidise. This tendency is observable in their reactions with other substances, such as water or dilute acids. In these reactions, the metal atoms lose electrons to hydrogen ions (from water or acid), which then combine to form hydrogen gas. A more reactive metal will lose electrons more easily, leading to a more vigorous reaction. For instance, when a reactive metal like potassium reacts with water, it rapidly loses an electron to form a potassium ion, K+, and the reaction is very vigorous, producing hydrogen gas explosively. In contrast, a less reactive metal like copper does not readily lose electrons and therefore does not react with dilute acids or water. The position of a metal in the reactivity series directly reflects its ease of electron loss and subsequent formation of positive ions. Metals higher in the series lose electrons more easily and are thus more reactive, forming their positive ions more readily than metals lower in the series. This fundamental principle underpins the displacement reactions where a more reactive metal will displace a less reactive metal from its compound.