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Redox Reaction

Redox reactions involve simultaneous oxidation and reduction processes, where oxidizing agents gain electrons and reducing agents lose electrons. Examples include the addition or removal of oxygen (e.g., zinc oxide and carbon), the transfer of electrons (e.g., silver and chlorine), and the gain or loss of hydrogen (e.g., H2S and Cl2). Additionally, color changes in solutions, such as the transition of potassium manganate(VII) from purple to colorless, can indicate redox reactions.

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10 views3 pages

Redox Reaction

Redox reactions involve simultaneous oxidation and reduction processes, where oxidizing agents gain electrons and reducing agents lose electrons. Examples include the addition or removal of oxygen (e.g., zinc oxide and carbon), the transfer of electrons (e.g., silver and chlorine), and the gain or loss of hydrogen (e.g., H2S and Cl2). Additionally, color changes in solutions, such as the transition of potassium manganate(VII) from purple to colorless, can indicate redox reactions.

Uploaded by

ayesha khan
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© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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What is redox reaction

Oxidising agent and reducing agent

Redox reaction in terms of oxygen+ examples

Redox reaction in terms of electrons+ examples

Redox reaction in terms of Hydrogen+ examples

Redox reaction in terms of color change


What is redox reaction

 Redox reactions
 Redox reactions are reactions where both oxidation and reduction are taking place.
Displacement reactions are examples of redox reactions
 Oxidising agent and reducing agent
 An oxidizing agent is a substance that undergoes reduction but causes oxidation by accepting
electrons.
 A reducing agent is a substance that undergoes oxidation but causes reduction to take plaace

Redox reaction in terms of oxygen+ examples

 Oxidation is a reaction in which oxygen is added to an element or a compound


 Reduction is a reaction in which oxygen is removed from an element or compound
 Example: Identifying the loss and gain of oxygen in an equation
 zinc oxide + carbon → zinc + carbon monoxide
 ZnO + C → Zn + CO

 In this reaction, the zinc oxide has been reduced since it has lost oxygen
 The carbon atom has been oxidised since it has gained oxygen
 Zinc oxide is acting as Oxidant
 Carbon is acting as a reductant

Redox reaction in terms of electrons+ examples

 Oxidation is a reaction in which an element, ion or compound loses electrons


o This can be shown in a half equation, e.g. when silver reacts with chlorine, silver
is oxidised to silver ions:
 Ag → Ag+ + e-
 Reduction is a reaction in which an element, ion or compound gains electrons
o This can be shown in a half equation, e.g. when oxygen reacts with magnesium,
oxygen is reduced to oxide ions:
 O2 + 4e- → 2O2-
Oxidation is the loss of hydrogen

o H2S+Cl2→S+2HCl
o In the above reaction, H2S is changing into S. That is, Hydrogen is being removed from
Hydrogen sulphide.
o Now by definition, the removal of hydrogen from a compound is called oxidation,

Reduction is the gain of hydrogen

o 2NH3 + 3Br2 = N2 + 6HBr


o Here, Br2 is changing into HBr. That is, hydrogen is being added to bromine. By definition,
the addition of hydrogen to a substance is called reduction.

 The tests for redox reactions involve the observation of a colour change in the solution being
analysed
 Two common examples are acidified potassium manganate(VII), and potassium iodide
 Potassium manganate(VII), KMnO4, is an oxidising agent which is often used to test for the
presence of reducing agents
 When acidified potassium manganate(VII) is added to a reducing agent its colour changes from
purple to colourless

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