Redox Equilibrium

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

Oxidising Agents and Reduction Agents In a redox reaction, a compound that is reduced is the oxidizing agent. An oxidising agent is a substance which oxidises something else. Inversely, a compound that is oxidised is the reducing agent. A reducing agent reduces something else. Example: In this reaction, iron(III) oxide is reduced. Therefore it is … Read more

Oxidation and Reduction in Terms of Electron Transfer Oxidation occurs when a reactant loses electron. Reduction occurs when a reactant gain of electron. Example: CuO + Mg → Cu + MgOIn this reaction, copper (II) ion in copper(II) oxide gains 2 electrons to form copper metal.Half equation:Cu2+ + 2e → Cu This is a reduction process. Magnesium metal … Read more

Oxidation and Reduction in Term of Changes of Oxidation State Oxidation involves an increase in oxidation stateReduction involves a decrease in oxidation state Another way to determine oxidation and reduction is to see the change of the oxidation state after a reaction. An atom is said to be oxidised when its oxidation state increases. An … Read more

Using the Oxidation States in Naming Compounds You will have come across names like iron(II) sulphate and iron(III) chloride. The (II) and (III) are the oxidation states of the iron in the two compounds: +2 and +3 respectively. That tells you that they contain Fe2+ and Fe3+ ions. Example Formula Name of the compound FeCl2 … Read more

Oxidation States (Oxidation Numbers) Oxidation state shows the total number of electrons which have been removed from an element (a positive oxidation state) or added to an element (a negative oxidation state) to get to its present state. Oxidation State of Some Elements 1. The oxidation state of an element is zero.Example Element Oxidation State … Read more