![]() ![]() The reducing power of metals weakens as you go through the series.Įlectropositivity of elements also decreases as one moves down the metal reactivity series.Īll metals above hydrogen in the activity range release hydrogen gas when reacted with dilute HCl or dilute H2SO4. These metals tarnish/corrode very easily. Metals at the top of the series of reactivity are strong reducing agents because they oxidize quickly. Metals at the top of the series are very reactive and, therefore, they do not occur free in nature, while the metals at the bottom of the series are least reactive and, therefore, they normally occur free in nature. The metals which are placed below hydrogen are less reactive than hydrogen and cannot displace hydrogen from its compounds like water and acids.Ī more reactive metal (placed higher in the reactivity series) can displace the less reactive metal from the solution of its salt. The metals which have been placed above hydrogen are more reactive than hydrogen and can displace hydrogen from its compounds like water and acids to liberate hydrogen gas. Lithium is the most reactive and platinum is the least reactive metal. The metal which is higher in the activity series is more reactive than the other. The reactivity series is very useful as it gives the following information: Reactivity Series of Metal chart are given below: Metals with high atomic numbers are more reactive because their electrons are far from the positively charged nucleus thus, they can be easily removed. Metals form positively charged ions because they tend to lose electrons. The reactivity of metals is due to their incomplete outer orbitals or their electron configuration. It is also known as a series of activities. ![]() Thus, a metal reactivity series can be defined as a series of metals in order of reactivity from highest to lowest. A reactivity series is a series of metals based on their reactivity from highest to lowest. 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 was 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. All metals above hydrogen liberate hydrogen gas (H 2) upon reacting with dilute hydrochloric acid (HCl) or dilute sulfuric acid (H 2SO 4).Metals at the bottom of the chart, gold, silver, and platinum, usually are unreactive and do not react with acid and water. ![]() The reducing ability of metals decreases as we go down the series.They are also strong reducing agents and oxidize quickly. Metals at the top of the list, such as lithium, sodium, and potassium, are highly reactive and result in a vigorous reaction.Metals higher in the series displace lower metals from their salts during single-displacement reactions. ![]()
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