Why do some metals react with acids while others don't?

Some metals react with acids due to their position in the reactivity series, while others don't due to their lower reactivity.

The reactivity of metals with acids is primarily determined by their position in the reactivity series. The reactivity series is a list of metals ranked in order of decreasing reactivity. Metals that are high up in the reactivity series, such as potassium, sodium, and calcium, react vigorously with acids. They can displace hydrogen from the acid, resulting in the formation of a salt and hydrogen gas. This is an exothermic reaction, meaning it releases energy in the form of heat.

On the other hand, metals that are lower down in the reactivity series, such as copper, silver, and gold, do not react with acids under normal conditions. These metals are less reactive and cannot displace hydrogen from the acid. Therefore, no reaction occurs. For example, if you were to put a piece of copper in hydrochloric acid, you would observe no change because copper is less reactive than hydrogen.

However, it's important to note that not all acids react with metals in the same way. For instance, nitric acid behaves differently because it's a strong oxidising agent. Even metals lower in the reactivity series, like copper and silver, can react with concentrated nitric acid.

In summary, whether a metal reacts with an acid or not depends on two main factors: the reactivity of the metal (as determined by its position in the reactivity series) and the type of acid used. Understanding these factors and how they interact is key to predicting and explaining the outcomes of reactions between metals and acids.