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Redox Reactions
Rating: 5.0 out of 5(1 rating)
3 students

Redox Reactions

Oxidation and Reduction Reactions.
Created byVinay Arya
Last updated 10/2021
English

What you'll learn

  • The students will have a clear vision about the Oxidation Reactions.
  • The students will be able to differentiate between oxidizing agent and Reducing agent.
  • The students will be able to identify Reduction Reactions.
  • The learners will know about Balancing of Equations.

Course content

1 section • 16 lectures • 3h 28m total length

  • Contents of Redox Reactions12:12

    Explore the contents of redox reactions, introducing oxidation and reduction, electron transfer, and the concept of oxidation number, with examples like rusting and apples, plus balancing and electrochemical cells.

  • Oxidation and Reduction Reactions14:28

    Learn the fundamentals of oxidation and reduction, redox reactions, and oxidation states, with methane oxidation to carbon dioxide and water as examples.

  • Electron transfer reactions12:25

    Explore how oxidation and reduction drive electron transfer in redox reactions, illustrated by zinc displacing copper and zinc oxidation to Zn2+ while Cu2+ reduces to copper metal.

  • Redox reaction based on electron transfer14:00

    Explore redox reactions based on electron transfer, with oxidation and reduction explained through real-life and classroom examples like apple browning, magnesium oxidation, and oxidation numbers.

  • A reaction involving transfer of electrons.9:19

    Observe a redox reaction where iron displaces copper from copper(II) chloride, transferring electrons to form copper metal and ferrous ions, with a color change from blue to reddish-brown.

  • Redox reactions in aqueous solution11:26

    Explore redox reactions in aqueous solution, where metals like zinc, copper, and silver transfer electrons in displacement reactions, forming metal deposits and soluble salts while heat is released.

  • Oxidation Numbers11:34

    Explore oxidation numbers and redox concepts, learn to assign oxidation states using standard rules, and track electron transfer in reactions involving hydrogen, oxygen, chlorine, and metals.

  • Determining Oxidation Numbers of Elements11:19

    Learn how to determine oxidation numbers in compounds using standard rules, balancing formulas, and interpreting fixed and variable oxidation states, with worked examples like potassium, chromium, and oxygen in oxides.

  • Basic Rules12:41

    Identify oxidation numbers using basic rules: zero for elements in the elemental state, hydrogen plus one, fluorine minus one, and oxidation numbers in compounds and polyatomic ions.

  • Examples6:34

    Learn to calculate oxidation numbers using rules with examples for hydrogen, oxygen, sulfur (+6 in H2SO4), chromium, iron, and manganese, and note limitations like not being assignable to a species.

  • Paradox of fractional oxidation number15:21

    Explore the paradox of fractional oxidation numbers in redox chemistry, explaining how average oxidation states can be fractional while individual atoms remain integers, and identify oxidation and reduction roles.

  • Types of redox reactions12:13

    Explore the five main redox reaction types: combination, decomposition, displacement, disproportionation, and auto redox. Focus on how oxidation states change during these reactions.

  • Redox reactions as the basis for titrations6:38

    Explore redox reactions as the basis for titration, using permanganate with oxalic acid and iodine–starch indicators to mark end points, and review the metal activity series through displacement examples.

  • Balancing Redox Reactions31:40

    Explore how to balance redox reactions using the half-reaction method, assign oxidation states, split into oxidation and reduction steps, balance electrons, and combine half-reactions in acidic, basic, and neutral media.

  • Electrochemical Cells13:39

    Learn how electrochemical cells convert chemical energy to electrical energy through spontaneous redox reactions in galvanic cells, featuring two half-cells, electrodes, electrolytes, and a salt bridge.

  • Standard electrode potential13:13

    Understand standard electrode potentials and their role in electrochemical cells. Use the standard hydrogen electrode as reference to compare metal–ion effects and the electrochemical series.

Requirements

  • The students should have a idea about Electrolysis and Electrodes.

Description

Redox reactions are the chemical reactions in which reduction and oxidation occurs

simultaneously. In straight words addition of oxygen is oxidation and removal of

hydrogen is reduction.

ELECTRONIC CONCEPT OF OXIDATION AND REDUCTION

Oxidation is a process in which an atom or an ion loses one or more electrons.

Reduction is a process in which an atom or an ion gains one or more electrons.

REDOX REACTION

Redox reactions may be regarded as electron transfer reactions in which the electrons

are transferred from one reactant to the other. As the result substance which losses

electrons is called a reducing agent or reductant while another which accepts the

electrons is called an oxidizing agent or oxidant.

REDOX REACTIONS IN AQUEOUS SOLUTION

In aqueous solutions, the spontaneous redox reactions can be carried out directly

as well as indirectly.

Direct Redox Reactions: Redox reactions in which oxidation and reduction takes

place in the same vessel are called direct redox reactions. In such reactions, the

transfer of electrons from reductant to oxidant occurs over a very short distance

(within molecular diameters). For example, if a zinc rod is placed in a solution of

copper sulphate in a beaker, a spontaneous reaction occurs and following changes

will be observed.

Observations for redox reaction occurring in a beaker

Zinc rod starts dissolving and loses its mass gradually.

The blue color of the solution starts fading.

Copper metal either starts settling at the bottom of the beaker or depositing on the

zinc rod.

The reaction is exothermic i.e., it takes place with the evolution of heat.

The solution remains electrically neutral throughout.

The reaction will not continue indefinitely but stops after some time.

Who this course is for:

  • Biggane and eleventh standard students.

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