REDOX REACTIONS in 60 Minutes || Full Chapter Revision || Class 11th JEE
JEE Wallah・2 minutes read
Redox reactions involve oxidation and reduction processes, with oxidation defined as loss of electrons and reduction as gain of electrons. Balancing redox reactions involves adjusting atoms, charges, and electrons separately before combining them to obtain the balanced chemical reaction.
Insights
- Redox reactions involve simultaneous oxidation and reduction processes, with oxidation defined as the addition of oxygen or electronegative elements, and reduction as the removal of oxygen or electronegative elements. Oxidants supply oxygen, while reducing agents supply hydrogen or remove it, showcasing a fundamental interplay of elements in chemical reactions.
- The n factor in redox reactions is crucial for determining the number of moles of electrons gained or lost by a substance, affecting its behavior as an oxidant or reducing agent. This factor plays a key role in titration processes, where the Law of Equivalence ensures that reactants and products' gram equivalents are equal, allowing for precise determination of unknown solutions' normality through careful calculations and observations at the equivalence point.
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What are redox reactions?
Redox reactions involve oxidation and reduction processes.
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Summary
00:00
Understanding Redox Reactions and Oxidation Numbers
- Redox reactions involve simultaneous oxidation and reduction processes.
- Three concepts of oxidation and reduction are classical, electronic, and oxidation number.
- The classical concept defines oxidation as addition of oxygen or electronegative elements.
- Reduction is the opposite of oxidation, involving removal of oxygen or electronegative elements.
- Oxidant supplies oxygen, while reducing agent supplies hydrogen or removes it.
- The substance being oxidized is the substance itself.
- The electronic concept explains oxidation as loss of electrons and reduction as gain of electrons.
- Oxidation number is the charge on an atom when all attached elements are removed.
- Rules for calculating oxidation numbers include zero for elements in their natural state.
- Maximum oxidation numbers are determined by group numbers, with exceptions for chromium and manganese.
13:54
Understanding Redox Reactions and Reactivity Order
- An element in its maximum oxidation state behaves as an oxidant, unable to act as a reducing agent due to its inability to further oxidize.
- When an element's oxidation state decreases, it indicates reduction, making the element itself an oxidant.
- Conversely, an element in its minimum oxidation state can only behave as a reducing agent, with its oxidation number increasing.
- Intermediate oxidation states, like nitrogen in HNO2 at +3, can exhibit characteristics of both oxidants and reducing agents.
- Redox reactions can be classified into types, with the NCRT classification highlighting combination and decomposition reactions.
- Combination reactions involve elements combining to form compounds, while decomposition reactions entail compounds breaking down into simpler substances.
- Displacement reactions occur when a more reactive element displaces a less reactive one, as seen in the example of zinc displacing copper in CuSO4.
- The reactivity order of halogens dictates displacement reactions, with fluorine being the most reactive.
- Dysprosium reactions involve simultaneous oxidation and reduction of a single element, exemplified by Br2 becoming Br3-.
- Normality, a concentration term, is calculated using gram equivalents of solute divided by the volume of the solution in liters, with formulas for dilution and mixing substances provided.
28:14
Determining n Factors in Redox Reactions
- The basicity of a substance is determined by the number of replaceable H+ ions it can provide.
- Exceptions to the standard n factors include H3PO3 having an n factor of 2, H3P2 with an n factor of 1, and H3BO3 also considered to have an n factor of 1.
- The n factor of a base is equivalent to its acidity, which is the number of replaceable -OH ions it can provide.
- The n factor varies depending on the substance, with examples like NaOH having an n factor of 1 and Mg(OH)2 having an n factor of 2.
- In redox reactions, the n factor is calculated based on the number of moles of electrons gained or lost by a substance.
- The n factor in redox reactions is determined by the number of moles of electrons gained or lost by a substance.
- The n factor calculation in redox reactions involves considering the change in oxidation state of elements.
- The n factor in redox reactions is calculated based on the total moles of electrons gained or lost by a substance.
- The Law of Equivalence states that the number of gram equivalents of all reactants and products in a chemical reaction are equal.
- Titration involves using a burette to add a standard solution to an unknown solution until a color change indicator signals the endpoint, allowing for the determination of the unknown solution's normality.
42:01
"Titration and Redox Reactions: A Guide"
- During a titration process, the color of the solution changes with each drop added, indicating the equivalence point where the equivalents of the substances are equal.
- The formula n1 v1 = n2 v2 is used to calculate the volume of the solution that has reacted based on the equivalence point.
- Titration is a method to determine the concentration of a solution with unknown concentration by using a solution with a known concentration.
- Acid-base titration involves equating the equivalents of acid and base to reach the equivalence point where the color changes.
- Redox titration involves the equivalents of a reducing agent and an oxidant being equated at the equivalence point.
- Acid-base titration can be simple, back, or double titration, with back titration involving titrating an excess substance with another after the first titration.
- Double titration includes using two indicators to determine the equivalence point, as seen in an example involving a mixture of bases.
- Balancing redox reactions can be done using the ion-electron method, where oxidation and reduction reactions are balanced separately before combining them.
- An example of balancing a redox reaction involving potassium dichromate and sulfite ions is provided, showcasing the steps to balance the reaction.
- The process involves balancing the atoms, charges, and electrons in the oxidation and reduction reactions before combining them to obtain the balanced redox reaction.
55:47
Balancing Chemical Reactions in Acidic and Basic Mediums
- Balance the reactions by making the electrons the same in both reactions, then combine them to get the final balanced reaction in acidic medium.
- In basic medium, balance the reduction first by adjusting the number of hydrogen and oxygen atoms, ensuring the charges are equal on both sides by adding the same amount of O- ions.
- To balance the charge, calculate the difference in charge on both sides and adjust by adding the necessary number of electrons, ensuring the number of electron transfers is the same in both reactions before combining them for the final balanced chemical reaction.
