Redox Reactions – Other Ionic Reactions

by Adam Le Gresley, PhD

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    00:01 Right. Let’s move on to a practical application of some of the ionic chemistry that we discussed in the previous module. RedOx reactions are by far the most important types of reactions that you’ll come across. They involve the transfer of electrons from one species to another. Oxidation is defined as the loss of electrons. So, this would be, for example, let’s say, sodium, which is in group 1 as an element, would be oxidised when it lost its single outer shell electron.

    00:36 A reduction is defined as a gain of electrons. Let us take fluorine. When it, in order to complete its outer shell, takes on a single electron, it would be considered to be reduced.

    00:49 Sometimes an easy way to remember this is by the mnemonic, oil rig. Oxidation is loss, reduction is gain. Oxidation and reduction must occur simultaneously since, of course, the electrons must go somewhere; you don’t lose them, there is conservation of matter. So, let’s have a look at one example - the reaction of iron with a solution of copper sulphate. It is an example of an oxidation reduction reaction or a RedOx reaction. The equation for this is given below on our board.

    01:21 Iron, as a solid, reacts with a solution of copper sulphate. Note, aq means it is in water.

    01:29 And this results in the formation of a solution of iron sulphate and solid copper is then precipitated out. Let’s look at this in more detail. What do we actually mean? The net ionic equation, if we isolate it, shows that we are losing two electrons from the iron which we’re going to add to the copper ion, 2+, to form solid copper. So, in this scenario, iron or Fe is lost of two electrons or deprived of two electrons which results in the formation of Fe2+ cation.

    02:10 The copper cation, which is already in solution, is reduced, gain in two electrons and can be converted from its 2+ cation to its oxidation state zero element.

    02:24 And of course, this would… reaction would be visible because copper, as an element, is insoluble in water and would precipitate out.

    About the Lecture

    The lecture Redox Reactions – Other Ionic Reactions by Adam Le Gresley, PhD is from the course Ionic Chemistry.

    Included Quiz Questions

    1. N₂, O₂ and Cl₂ get easily oxidized in the presence of non-metals
    2. Oxidation process involves the gain of oxygen or the loss of electrons or hydrogen
    3. Reduction process includes the loss of oxygen or the gain of electrons or hydrogen
    4. All metals readily donate electrons due to their low electronegativities
    5. Non-metals readily accept electron due to high electronegativities
    1. Corrosion of gold and platinum jewelry in the dark
    2. Combustion of petroleum
    3. Corrosion of exposed metal
    4. Decaying process of wood
    5. Electron transport chain in the living cells
    1. A metal atom in a compound form or solution form does not get displaced by an atom of another metal
    2. The addition of magnesium metal to copper sulfate solution leads to the disappearance of blue color
    3. With an addition of an iron nail, the blue color of CuSO₄ solution turns to light green with the formation of reddish brown deposits of copper metal on the iron nail
    4. The reactivity series of metals says: K > Na > Ca > Mg > Al > Zn > Fe > Cu > Ag > Au
    5. The least reactive metals like gold and platinum, exist in their pure elemental forms in nature

    Author of lecture Redox Reactions – Other Ionic Reactions

     Adam Le Gresley, PhD

    Adam Le Gresley, PhD

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