Provide an example of the reactivity of metals in the activity series.

The reactivity of metals in the activity series increases as you move down the list.

The activity series is a list of metals arranged in order of their reactivity, with the most reactive metal at the top and the least reactive metal at the bottom. The reactivity of metals is determined by their ability to lose electrons and form positive ions. Metals at the top of the activity series, such as potassium and sodium, are highly reactive and readily lose electrons to form positive ions. Metals at the bottom of the activity series, such as gold and platinum, are much less reactive and do not readily lose electrons.

The reactivity of metals in the activity series is important in many chemical reactions, including the reactions of metals with acids and the displacement reactions of metals in aqueous solutions. For example, when a more reactive metal, such as magnesium, is added to a solution of a less reactive metal, such as copper, the magnesium will displace the copper from the solution and form a solid copper metal. This is because magnesium is more reactive than copper and can readily lose electrons to form positive ions.

Overall, the activity series is a useful tool for predicting the outcomes of chemical reactions involving metals and for understanding the reactivity of different metals.

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