![]() This graphic places a selection of common metals into order of reactivity, as well as showing their reactions with air, water and steam. It’s also a useful tool in predicting the products of simple displacement reactions involving two different metals, as well as providing an insight into why different metals are extracted from their ores in different manners. The metal reactivity series is a commonly taught concept in chemistry, placing the metals, as its name suggests, in order of reactivity from most reactive to least reactive. The following chart summarizes the reactions discussed above. Iron will react with sulfuric acid to give hydrogen and iron (II) sulfate.įe (s) + H 2SO 4 (l) → FeSO 4 (aq.) + H 2 (g) Zinc (Zn) reacts with sulfuric acid (H 2SO 4) to produce zinc sulfate (ZnSO 4) while liberating hydrogen gas (H 2). ![]() Metals that lose electrons easily produce a fast and vigorous reaction.ġ. The reactivity of the metal determines the reaction rate. The amount of hydrogen produced depends on the starting mass of the metal and the acid’s strength. The electrons and protons combine to form a hydrogen atom. Each metal atom loses one or more electrons, and each acid molecule loses one or more protons. Highly reactive metals produce hydrogen when reacting with acid. Aluminum (Al) reacts vigorously with water to produce hydrogen gas.Ģ Al (s) + 6 H 2O (l) → 2 Al(OH) 3 (aq.) + 3 H 2 (g) 3. Sodium (Na) is highly reactive and displaces hydrogen (H 2) from water (H 2O).Ģ Na (s) + 2 H 2O (l) → 2 NaOH (aq.) + H 2 (g)Ģ. Highly reactive metals can react with cold water to form the corresponding hydroxide.ġ. Magnesium (Mg) can displace copper (Cu) in an aqueous solution of copper nitrate (Cu(NO 3) 2). ![]() Copper (Cu) can displace silver (Ag) in an aqueous solution of silver nitrate (AgNO 3).Ĭu (s) + 2 AgNO 3 (aq.) → Cu(NO 3) 2 (aq.) + 2 Ag (s/ppt.)Ģ. A characteristic of this reaction is that one cation trades places with another to form a new product.ġ. This reaction is known as a single-displacement reaction. Metals higher in the series tend to lose electrons and easily displace lower metals. Based on the importance of the reactivity series, let us look at the various chemical reactions that metals undergo. It helps us understand why different metals are extracted from their ores differently. Aside, it can predict the outcome of single-displacement reactions. It can predict the reactions between metals and water and metals and acids. The reactivity series is essential for several reasons. įrom this list, it is clear that potassium is the most reactive metal. ![]() The list below represents the order of the reactivity series from most reactive to least reactive.
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