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Application of The Reactivity Series of Metals in The Extraction of Metals The method that is used in the extraction of metal from its ore depends on the position of the metal in the reactivity series of metals. metals that are located lower than carbon in the reactivity series of metals can be extracted using … Read more
Position of Hydrogen in The Reactivity Series of Metals The position of hydrogen in the reactivity series of metal can also be determined based on its ability to displace oxygen from metal oxides. If hydrogen is more reactive than a metal, it can displace oxygen from metal oxide, and reduces the metal oxide to its … Read more
Position of Carbon in The Series of Reactivity of Metals The position of carbon in the series of reactivity of metals can be determined based on: the ability of metals to take away oxygen from carbon oxide, that is carbon dioxide. the ability of carbon to take away oxygen from metal oxides Experiment 1 If … Read more
When a metal reacts with oxygen to form a metal oxide, a redox reaction occurs.Metal + Oxygen → Metal oxide In this reaction, Metal is oxidised to metal ions. The oxidation number of the metal increases. Oxygen is reduced to the oxide ion. The oxidation number of oxygen decreases from 0 to -2. Metal acts … Read more
Controlling Rusting Steps to Control Rusting The use of a metal which is less electropositive The plating of iron with a thin layer of a metal which is less electropositive such as tin, silver or copper will prevent the iron underneath it to react with water and air, and so prevents the iron from rusting. … Read more
Corrosion of metal = metal loses its electrons to form positive ions.ExampleCorrosion of ironFe → Fe2+ + 2eCorrosion of MagnesiumMg → Mg2+ + 2e The higher the position of a metal in the electrochemical series, the more electropositive (reactive) the metal is. The metal has a greater tendency to give away electrons to form the metal ion, that … Read more
A redox reaction occurs when a solution of an oxidising agent is mixed with a solution of a reducing agent. If the solution of the oxidising agent and the solution of the reducing agent are separated by an electrolyte in a U-tube, the redox reaction will still take place but the transfer of electrons will … Read more
Displacement of Halogen From Halide Solution Halogens are elements in Group 17 of the Periodic Table of Elements. They are fluorine, chlorine, bromine, iodine, astatine. All halogens tend to accept one electron to form negative ions. For instance, The ions of halogen are called halide. The electronegativity of halogens decreases down the group, as shown … Read more
The electrochemical series is a series of arrangement of metals according to the order of the tendency of the metal to lose electrons to form positive ions. Elements which placed higher in the electrochemical series are more electropositive act as strong reducing agent can be oxidised easily The metal ions are weak oxidising agents because … Read more
Change of Iron(II) Ion to Iron(III) Ion Iron shows two oxidation numbers, that is +2 and +3. The aqueous solution of iron(II) ion Fe2+ is light green in colour. The aqueous solution of iron(III) ion Fe3+ is brown in colour. The change of iron(II) ion for iron(III) ion is an oxidation process. This can be … Read more