Non-metals are usually less reactive but some of them are very reactive. That is why it is frequently used at extremely high temperatures. Its stability is due to the fine arrangements of metal ions and electrons in its structure. Key Point: Remember the common members of the activity series this way: Hydrogen gas is liberated when reactive metals come in contact with mineral acids. For example, reactive metals are added to the solution of less reactive metals for extraction purposes. Metals displacement reactionsĪctivity series of metals can be used to predict metal displacement. For example, at room temperature zinc does not react with water but above 50✬ it reacts, and hydrogen bubbles are witnessed. On going down the activity series, the tendency of metals to react decreases. The topmost metals react vigorously with water to liberate hydrogen gas. The reaction of metals with water can be predicted with activity series of metals. Applications and uses of activity series of metals 1. It also explains why aluminum forms a protective (insoluble) layer of aluminum oxide (Al 2O 3) and seems unreactive.Less reactive metals will not react even with hot water. Highly reactive metals can react with cold water.Hydrogen cannot reduce oxides of metals present above it in the series.Everything above hydrogen in the list can displace hydrogen from its acid.Some prominent outcomes of the activity series are given below: The activity series places metals in order of their tendency to participate in chemical reactions. The significant features of the activity series Therefore it can replace the copper from the CuSo 4 solution and become Zn 2+. It is important to note that this activity series is not absolute and can vary slightly depending on the specific conditions of the reaction.įor example, zinc is more reactive than copper. Moreover, this activity series describes the loss of electrons (oxidation potential), corrosive nature, and energy required for metal extraction processes from the ores. The more reactive metal will displace the less reactive metal from a compound. For example, if a metal higher in the activity series reacts with a compound containing a metal lower in the series, a single displacement reaction will occur. The activity series can help predict if a single displacement reaction will occur. The more reactive a metal is, the more likely it is to lose electrons and form a positive ion. The reactivity of these metals is usually determined by their ability to form positive ions. In the series, elements on the top are more reactive than those at the bottom. These reactions can be described using either word or symbol chemical equations close chemical equation A way of describing chemical reactions in words or symbols.Activity series or reactivity series of metals explain certain properties of metals, mainly the reactivity of metals. This method is called reduction with carbon. The more reactive element (carbon) is displacing the less reactive element (in this case a metal) from its compound.Ī chemical reaction where oxygen is removed from a compound is called a reduction close reduction A reaction involving the loss of oxygen from an element. This is a specific type of displacement reaction. The carbon makes an oxide - either carbon monoxide (CO) or carbon dioxide (CO₂). Elements cannot be broken down into simpler substances. Elements are listed on the periodic table. This leaves the metal as a pure element close element A pure substance that is made from only one type of atom. This means the carbon takes the oxygen away and displaces close displace When an element is displaced, it is pushed out of a compound by a more reactive element. Metal oxide + carbon → metal + carbon oxideĬarbon is more reactive than zinc, iron and copper. are the pure metal and either carbon monoxide or carbon dioxide. Products are written on the right of a chemical equation, after the arrow (→). The products close product A chemical which is made in a chemical reaction. Reactants appear on the left of a chemical equation, before the arrow →. The reactants close reactant The chemical present at the start of a reaction.
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