{"id":866473,"date":"2025-08-11T10:50:16","date_gmt":"2025-08-11T05:20:16","guid":{"rendered":"https:\/\/leverageedu.com\/discover\/?p=866473"},"modified":"2025-08-11T10:50:16","modified_gmt":"2025-08-11T05:20:16","slug":"ncert-notes-class-11-chemistry-part-ii-chapter-7-redox-reactions","status":"publish","type":"post","link":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-ii-chapter-7-redox-reactions\/","title":{"rendered":"NCERT Notes Class 11 Chemistry (Part-II) Chapter 7: Redox Reaction (Free PDF)"},"content":{"rendered":"\n<p>Chemistry studies the vast diversity of matter and the transformations that change one type of matter into another. These transformations occur through various kinds of chemical reactions, and among these, redox reactions form one of the most important categories. Redox reactions are processes in which oxidation and reduction occur simultaneously. Below, we have provided the NCERT Notes Class 11 Chemistry (Part-2) Chapter 7: Redox Reactions notes for your thorough exam prep.<\/p>\n\n\n\n\n\n\n<p><strong>Explore Notes of Class 11 Chemistry<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-background has-fixed-layout\" style=\"background-color:#f1c9d3\"><tbody><tr><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-1-some-basic-concepts-of-chemistry\/\">Chapter 1<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-2-structure-of-atom\/\">Chapter 2<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-3-classification-of-elements-and-periodicity-in-properties\/\">Chapter 3<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-class-11-chemistry-part-i-chapter-iv-chemical-bonding-and-molecular-structure\/\">Chapter 4<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics-free-pdf\/\">Chapter 5<\/a><\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-background has-fixed-layout\" style=\"background-color:#b5f6de\"><tbody><tr><td><a href=\"https:\/\/drive.google.com\/file\/d\/1XQ7KG9pcJPmyb9d_reebFkS_36JyCkHs\/view?usp=drive_link\"><strong>Download PDF of NCERT Notes Class 11 Chemistry (Part-II) Chapter-7: Redox Reaction<\/strong><\/a><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-introduction\">Introduction<\/h2>\n\n\n\n<p>Redox processes are widespread in both physical and biological systems.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>Physical Processes involving Redox Reactions:\n<ul class=\"wp-block-list\">\n<li>Combustion of fuels (e.g., coal, petrol, natural gas) for energy generation.<\/li>\n\n\n\n<li>Corrosion of metals.<\/li>\n\n\n\n<li>Electrochemical processes such as those in batteries.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Biological Processes:\n<ul class=\"wp-block-list\">\n<li>Cellular respiration.<\/li>\n\n\n\n<li>Photosynthesis.<\/li>\n\n\n\n<li>Metabolism of nutrients.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Industrial and Metallurgical Applications:\n<ul class=\"wp-block-list\">\n<li>Extraction of highly reactive metals (e.g., aluminium, sodium) and non-metals through electrochemical methods.<\/li>\n\n\n\n<li>Manufacture of important chemical compounds (e.g., caustic soda, chlorine).<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Agricultural Relevance:\n<ul class=\"wp-block-list\">\n<li>Redox principles are involved in the production of fertilisers and pesticides.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<p><strong>Everyday and Technological Importance<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Energy Production<\/strong>: Burning of fuels for domestic heating, transport, and industrial purposes is a redox process.<\/li>\n\n\n\n<li><strong>Electrochemical Applications<\/strong>: Dry cells, lead\u2013acid batteries, and fuel cells function via redox principles.<\/li>\n\n\n\n<li><strong>Metal Protection and Corrosion:<\/strong> Understanding corrosion as an electrochemical redox process allows the design of preventive measures.<\/li>\n\n\n\n<li><strong>Environmental Issues<\/strong>:\n<ul class=\"wp-block-list\">\n<li><strong>Hydrogen Economy<\/strong>: Proposes using liquid hydrogen as a clean fuel, based on redox concepts.<\/li>\n\n\n\n<li><strong>Ozone Layer Depletion<\/strong>: Involves redox changes in atmospheric chemistry leading to the \u2018ozone hole\u2019.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<p class=\"has-pale-ocean-gradient-background has-background\"><strong>Also Read: <\/strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-political-science-indian-constitution-at-work-chapter-6-judiciary\/\"><strong>NCERT Notes Class 11 Political Science Indian Constitution at Work Chapter 6: Judiciary (Free PDF)<\/strong><\/a><\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-classical-idea-of-redox-reactions-oxidation-and-reduction\">Classical Idea of Redox Reactions \u2013 Oxidation and Reduction<\/h2>\n\n\n\n<p>The classical idea of redox reactions- oxidation and reduction is discussed below.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-original-definition-of-oxidation\">Original Definition of Oxidation<\/h3>\n\n\n\n<p>The original definition of oxidation is discussed below.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Oxidation<\/strong>: Addition of oxygen to an element or compound.<\/li>\n\n\n\n<li><strong>Reason<\/strong>: Presence of ~20% oxygen in the atmosphere; many elements occur naturally as oxides.<\/li>\n\n\n\n<li><strong>Examples<\/strong>:\n<ul class=\"wp-block-list\">\n<li>2Mg (s) + O\u2082 (g) \u2192 2MgO (s)<\/li>\n\n\n\n<li>S (s) + O\u2082 (g) \u2192 SO\u2082 (g)<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-extension-of-the-definition\">Extension of the Definition<\/h3>\n\n\n\n<p>The extension of the definition is given below.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Observation: In CH\u2084 oxidation, hydrogen is replaced by oxygen.<\/li>\n\n\n\n<li>Broader view: Oxidation includes the removal of hydrogen from a substance.<\/li>\n\n\n\n<li>Examples:\n<ul class=\"wp-block-list\">\n<li>CH\u2084 (g) + 2 O\u2082 (g) \u2192 CO\u2082 (g) + 2H\u2082O (l)<\/li>\n\n\n\n<li>2H\u2082S (g) + O\u2082 (g) \u2192 2 S (s) + 2H\u2082O (l)<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-further-extension\">Further Extension<\/h3>\n\n\n\n<p>The concept of oxidation can be further extended as follows<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxidation includes the addition of electronegative elements other than oxygen.<\/li>\n\n\n\n<li>Examples:\n<ul class=\"wp-block-list\">\n<li>Mg (s) + F\u2082 (g) \u2192 MgF\u2082 (s)<\/li>\n\n\n\n<li>Mg (s) + Cl\u2082 (g) \u2192 MgCl\u2082 (s)<\/li>\n\n\n\n<li>Mg (s) + S (s) \u2192 MgS (s)<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-removal-of-electropositive-elements-as-oxidation\">Removal of Electropositive Elements as Oxidation<\/h3>\n\n\n\n<p><strong>Example<\/strong>: 2K\u2084[Fe(CN)\u2086] (aq) + H\u2082O\u2082 (aq) \u2192 2K\u2083[Fe(CN)\u2086] (aq) + 2KOH (aq)<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-original-definition-of-reduction\">Original Definition of Reduction<\/h3>\n\n\n\n<p><strong>Reduction<\/strong>: Removal of oxygen from a compound.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-extended-definition-of-reduction\">Extended Definition of Reduction<\/h3>\n\n\n\n<p>Includes:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Removal of oxygen or any electronegative element.<\/li>\n\n\n\n<li>Addition of hydrogen or any electropositive element.<\/li>\n<\/ul>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Removal of oxygen:\n<ul class=\"wp-block-list\">\n<li>2HgO (s) \u2192 2Hg (l) + O\u2082 (g)<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Removal of electronegative element:\n<ul class=\"wp-block-list\">\n<li>2FeCl\u2083 (aq) + H\u2082 (g) \u2192 2FeCl\u2082 (aq) + 2HCl (aq)<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Addition of hydrogen:\n<ul class=\"wp-block-list\">\n<li>CH\u2082 = CH\u2082 (g) + H\u2082 (g) \u2192 C\u2082H\u2086 (g)<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Addition of an electron-positive element:\n<ul class=\"wp-block-list\">\n<li>2HgCl\u2082 (aq) + SnCl\u2082 (aq) \u2192 Hg\u2082Cl\u2082 (s) + SnCl\u2084 (aq)<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<p class=\"has-pale-ocean-gradient-background has-background\"><strong>Also Read<\/strong>: <strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-geography-fundamentals-of-geography-chapter-6-landforms-and-their-evolution\/\">NCERT Notes Class 11 Geography Fundamentals of Geography Chapter 6 Landforms and their Evolution (Free PDF<\/a>)<\/strong><\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-redox-reactions-in-terms-of-electron-transfer\">Redox Reactions in Terms of Electron Transfer<\/h2>\n\n\n\n<p>In this section, we have discussed the redox reactions in terms of electron transfer.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-examples-of-redox-as-electron-transfer\">Examples of Redox as Electron Transfer<\/h3>\n\n\n\n<p>The following are examples of redox reactions as electron transfer.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Reactions:\n<ul class=\"wp-block-list\">\n<li>2Na (s) + Cl\u2082 (g) \u2192 2NaCl (s)\u2003<\/li>\n\n\n\n<li>4Na (s) + O\u2082 (g) \u2192 2Na\u2082O (s)<\/li>\n\n\n\n<li>2Na (s) + S (s) \u2192 Na\u2082S (s)<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>In each reaction:\n<ul class=\"wp-block-list\">\n<li>Sodium is oxidised (addition of oxygen or a more electronegative element).<\/li>\n\n\n\n<li>Cl\u2082, O\u2082, and S are reduced (addition of electropositive sodium).<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Compounds formed are ionic: NaCl\u207b, (Na\u207a)\u2082O\u00b2\u207b, (Na\u207a)\u2082S\u00b2\u207b.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-half-reaction-concept\">Half-Reaction Concept<\/h3>\n\n\n\n<p>The half-reaction concept is discussed below.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each redox process can be split into:\n<ul class=\"wp-block-list\">\n<li>Oxidation half: loss of electrons.<\/li>\n\n\n\n<li>Reduction half: gain of electrons.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Example (formation of NaCl):\n<ul class=\"wp-block-list\">\n<li>Oxidation: 2 Na (s) \u2192 2 Na\u207a (g) + 2 e\u207b<\/li>\n\n\n\n<li>Reduction: Cl\u2082 (g) + 2 e\u207b \u2192 2 Cl\u207b (g)<\/li>\n\n\n\n<li>Overall: 2 Na (s) + Cl\u2082 (g) \u2192 2 NaCl (s)<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-definitions-electron-transfer-concept\">Definitions (Electron Transfer Concept)<\/h3>\n\n\n\n<p>The following are the definitions of oxidation, reduction, oxidising, and reducing agent.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxidation: Loss of electron(s) by a species.<\/li>\n\n\n\n<li>Reduction: Gain of electron(s) by a species.<\/li>\n\n\n\n<li>Oxidising agent: Acceptor of electron(s).<\/li>\n\n\n\n<li>Reducing agent: Donor of electron(s).<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-oxidation-number\">Oxidation Number<\/h2>\n\n\n\n<p>Example: Formation of water- 2H\u2082 (g) + O\u2082 (g) \u2192 2H\u2082O (l)<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>H changes from 0 (in H\u2082) to +1 (in H\u2082O).<\/li>\n\n\n\n<li>O changes from 0 (in O\u2082) to \u20132 (in H\u2082O).<\/li>\n\n\n\n<li>Indicates electron shift from H to O (partial in covalent bonds).<\/li>\n\n\n\n<li>Oxidation number method:\n<ul class=\"wp-block-list\">\n<li>Assumes complete transfer of electrons from the less electronegative to the more electronegative atom.<\/li>\n\n\n\n<li>Used for bookkeeping in redox reactions.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-oxidation-number-representation\">Oxidation Number Representation<\/h3>\n\n\n\n<p><strong>Oxidation number<\/strong>: Oxidation state of an element in a compound, calculated assuming full electron transfer to the more electronegative element.<\/p>\n\n\n\n<p>Examples:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>2H\u2082 (0) + O\u2082 (0) \u2192 2H\u2082(+1)O(\u20132)<\/li>\n\n\n\n<li>H\u2082 (0) + Cl\u2082 (0) \u2192 2H(+1)Cl(\u20131)<\/li>\n\n\n\n<li>CH\u2084 (C\u20134H+1) + 4Cl\u2082 (0) \u2192 CCl\u2084 (C+4Cl\u20131) + 4H(+1)Cl(\u20131)<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-rules-for-determining-oxidation-number\">Rules for Determining Oxidation Number<\/h3>\n\n\n\n<p>Below, we have discussed the rules for determining oxidation number.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Elemental state<\/strong> \u2192 Oxidation number = 0 (e.g., H\u2082, O\u2082, Cl\u2082, Na).<\/li>\n\n\n\n<li><strong>Monatomic ions<\/strong> \u2192 Equal to charge (Na\u207a = +1, Cl\u207b = \u20131).\n<ul class=\"wp-block-list\">\n<li>Alkali metals: always +1.<\/li>\n\n\n\n<li>Alkaline earth metals: always +2.<\/li>\n\n\n\n<li>Al in compounds: +3.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Oxygen<\/strong>: Usually \u20132.\n<ul class=\"wp-block-list\">\n<li>In peroxides: \u20131.<\/li>\n\n\n\n<li>In superoxides: \u2013\u00bd.<\/li>\n\n\n\n<li>In compounds with fluorine: positive (+2 in OF\u2082, +1 in O\u2082F\u2082).<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Hydrogen<\/strong>: +1 (except in metal hydrides: \u20131).<\/li>\n\n\n\n<li><strong>Fluorine<\/strong>: \u20131 in all compounds.\n<ul class=\"wp-block-list\">\n<li>Other halogens: \u20131 unless combined with oxygen.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Sum Rule<\/strong>:\n<ul class=\"wp-block-list\">\n<li>Neutral compound \u2192 Sum = 0.<\/li>\n\n\n\n<li>Polyatomic ion \u2192 Sum = ion charge.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-oxidation-reduction-definitions-oxidation-number-concept\">Oxidation-Reduction Definitions (Oxidation Number Concept)<\/h3>\n\n\n\n<p>The oxidation and reduction reactions are defined on the basis of oxidation number concepts.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Oxidation<\/strong>: Increase in oxidation number.<\/li>\n\n\n\n<li><strong>Reduction<\/strong>: Decrease in oxidation number.<\/li>\n\n\n\n<li><strong>Oxidising agent<\/strong>: Increases the oxidation number of other species (gets reduced).<\/li>\n\n\n\n<li><strong>Reducing agent<\/strong>: Decreases the oxidation number of other species (gets oxidised).<\/li>\n\n\n\n<li><strong>Redox reaction<\/strong>: Involves a change in the oxidation number of species.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-pale-ocean-gradient-background has-background\"><strong>Also Read<\/strong>: <a href=\"https:\/\/leverageedu.com\/discover\/indian-exams\/exam-prep-best-books-for-upsc-optional-psychology\/\"><strong>Best Books for UPSC Optional Psychology<\/strong><\/a><\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-types-of-redox-reactions\">Types of Redox Reactions<\/h2>\n\n\n\n<p>The types of redox reactions are discussed below.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-combination-reactions\">Combination Reactions<\/h3>\n\n\n\n<p>The combination reactions are discussed as follows.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>General: A + B \u2192 C<\/li>\n\n\n\n<li>Either\/both reactants in elemental form.<\/li>\n\n\n\n<li>Examples:\n<ul class=\"wp-block-list\">\n<li>C (0) + O\u2082 (0) \u2192 CO\u2082 (C+4O\u20132)\u2003<\/li>\n\n\n\n<li>3Mg (0) + N\u2082 (0) \u2192 Mg\u2083N\u2082 (Mg+2N\u20133)\u2003<\/li>\n\n\n\n<li>CH\u2084 (C\u20134) + 2O\u2082 (0) \u2192 CO\u2082 (C+4) + 2H\u2082O (H+1O\u20132)<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-decomposition-reactions\">Decomposition Reactions<\/h3>\n\n\n\n<p>The decomposition reactions are discussed as follows.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Opposite of combination: one compound \u2192 2+ components, at least one elemental.<\/li>\n\n\n\n<li>Examples:\n<ul class=\"wp-block-list\">\n<li>2H\u2082O (H+1O\u20132) \u2192 2H\u2082 (0) + O\u2082 (0)<\/li>\n\n\n\n<li>2NaH (Na+1H\u20131) \u2192 2Na (0) + H\u2082 (0)<\/li>\n\n\n\n<li>2KClO\u2083 (K+1Cl+5O\u20132) \u2192 2KCl (K+1Cl\u20131) + 3O\u2082 (0)<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-displacement-reactions\">Displacement Reactions<\/h3>\n\n\n\n<p>The displacement reactions are discussed as follows.<\/p>\n\n\n\n<p><strong>a) Metal Displacement<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>More reactive metal displaces less reactive metal from compound.<\/li>\n\n\n\n<li>Examples:\n<ul class=\"wp-block-list\">\n<li>CuSO\u2084 + Zn \u2192 ZnSO\u2084 + Cu<\/li>\n\n\n\n<li>V\u2082O\u2085 + 5Ca \u2192 2V + 5CaO<\/li>\n\n\n\n<li>TiCl\u2084 + 2Mg \u2192 Ti + 2MgCl\u2082<\/li>\n\n\n\n<li>Cr\u2082O\u2083 + 2Al \u2192 Al\u2082O\u2083 + 2Cr<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<p><strong>b) Non-Metal Displacement<\/strong><\/p>\n\n\n\n<p>(i) <strong>Hydrogen Displacement<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Active metals (alkali, alkaline earth) from water:\n<ul class=\"wp-block-list\">\n<li>2Na + 2H\u2082O \u2192 2NaOH + H\u2082\u2003<\/li>\n\n\n\n<li>Ca + 2H\u2082O \u2192 Ca(OH)\u2082 + H\u2082\u2003<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Less active metals with steam:\n<ul class=\"wp-block-list\">\n<li>Mg + 2H\u2082O \u2192 Mg(OH)\u2082 + H\u2082\u2003<\/li>\n\n\n\n<li>2Fe + 3H\u2082O \u2192 Fe\u2082O\u2083 + 3H\u2082\u2003<\/li>\n\n\n\n<li>Metals with acids:<\/li>\n\n\n\n<li>Zn + 2HCl \u2192 ZnCl\u2082 + H\u2082\u2003<\/li>\n\n\n\n<li>Mg + 2HCl \u2192 MgCl\u2082 + H\u2082\u2003<\/li>\n\n\n\n<li>Fe + 2HCl \u2192 FeCl\u2082 + H\u2082\u2003<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<p>(ii) <strong>Halogen Displacement<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Reactivity order: F\u2082 &gt; Cl\u2082 &gt; Br\u2082 &gt; I\u2082.<\/li>\n\n\n\n<li>Examples:\n<ul class=\"wp-block-list\">\n<li>2H\u2082O + 2F\u2082 \u2192 4HF + O\u2082\u2003<\/li>\n\n\n\n<li>Cl\u2082 + 2KBr \u2192 2KCl + Br\u2082\u2003<\/li>\n\n\n\n<li>Cl\u2082 + 2KI \u2192 2KCl + I\u2082\u2003<\/li>\n\n\n\n<li>Br\u2082 + 2I\u207b \u2192 2Br\u207b + I\u2082\u2003<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-disproportionation-reactions\">Disproportionation Reactions<\/h3>\n\n\n\n<p>The disproportionation reactions are discussed as follows.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>An element in one oxidation state is simultaneously oxidised and reduced.<\/li>\n\n\n\n<li>Condition: Element can exist in \u22653 oxidation states.<\/li>\n\n\n\n<li>Examples:\n<ul class=\"wp-block-list\">\n<li>2H\u2082O\u2082 \u2192 2H\u2082O + O\u2082\u2003(O: \u20131 \u2192 \u20132 and 0)\u2003<\/li>\n\n\n\n<li>P\u2084 + 3OH\u207b + 3H\u2082O \u2192 PH\u2083 + 3H\u2082PO\u2082\u207b\u2003(P: 0 \u2192 \u20133 and +1)\u2003<\/li>\n\n\n\n<li>S\u2088 + 12OH\u207b \u2192 4S\u00b2\u207b + 2S\u2082O\u2083\u00b2\u207b + 6H\u2082O\u2003(S: 0 \u2192 \u20132 and +2)\u2003<\/li>\n\n\n\n<li>Cl\u2082 + 2OH\u207b \u2192 ClO\u207b + Cl\u207b + H\u2082O\u2003(Cl: 0 \u2192 +1 and \u20131)\u2003<\/li>\n\n\n\n<li>Fluorine exception: Cannot disproportionate (most electronegative, no positive oxidation state).<\/li>\n\n\n\n<li>2F\u2082 + 2OH\u207b \u2192 2F\u207b + OF\u2082 + H\u2082O<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-balancing-of-redox-reactions\">Balancing of Redox Reactions<\/h2>\n\n\n\n<p>Two main methods are used to balance redox equations:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-oxidation-number-method\">Oxidation Number Method<\/h3>\n\n\n\n<p>The steps of the oxidation number method are:<\/p>\n\n\n\n<p><strong>Steps:<\/strong><\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>Write correct formulas for all reactants and products.<\/li>\n\n\n\n<li>Assign oxidation numbers to all elements and identify the atoms whose oxidation numbers change.<\/li>\n\n\n\n<li>Calculate the change in oxidation number per atom and for the entire molecule\/ion. Multiply by suitable numbers to make total increases equal total decreases.<\/li>\n\n\n\n<li>Adjust charges:\n<ul class=\"wp-block-list\">\n<li>If in an acidic medium, add H\u207a ions.<\/li>\n\n\n\n<li>If in basic medium, add OH\u207b ions.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Balance hydrogen atoms by adding H\u2082O molecules, then check and balance oxygen atoms.<\/li>\n\n\n\n<li>Ensure the equation is balanced for both atoms and charges.<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-half-reaction-method\">Half Reaction Method<\/h3>\n\n\n\n<p><strong>Steps (Example: Oxidation of Fe\u00b2\u207a to Fe\u00b3\u207a by Cr\u2082O\u2087\u00b2\u207b in acidic medium):<\/strong><\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>Write the unbalanced ionic equation:<br>Fe\u00b2\u207a + Cr\u2082O\u2087\u00b2\u207b \u2192 Fe\u00b3\u207a + Cr\u00b3\u207a<\/li>\n\n\n\n<li>Split into half reactions:\n<ul class=\"wp-block-list\">\n<li>Oxidation: Fe\u00b2\u207a \u2192 Fe\u00b3\u207a<\/li>\n\n\n\n<li>Reduction: Cr\u2082O\u2087\u00b2\u207b \u2192 Cr\u00b3\u207a<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Balance atoms other than O and H:<br>Cr\u2082O\u2087\u00b2\u207b \u2192 2Cr\u00b3\u207a<br><\/li>\n\n\n\n<li>Balance oxygen by adding H\u2082O and balance hydrogen by adding H\u207a:<br>Cr\u2082O\u2087\u00b2\u207b + 14H\u207a \u2192 2Cr\u00b3\u207a + 7H\u2082O<\/li>\n\n\n\n<li>Balance charges by adding electrons:\n<ul class=\"wp-block-list\">\n<li>Oxidation: Fe\u00b2\u207a \u2192 Fe\u00b3\u207a + e\u207b<\/li>\n\n\n\n<li>Reduction: Cr\u2082O\u2087\u00b2\u207b + 14H\u207a + 6e\u207b \u2192 2Cr\u00b3\u207a + 7H\u2082O<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Multiply oxidation half reaction by 6 to equalise electrons:<br>6Fe\u00b2\u207a \u2192 6Fe\u00b3\u207a + 6e\u207b<\/li>\n\n\n\n<li>Add half reactions and cancel electrons:<br>6Fe\u00b2\u207a + Cr\u2082O\u2087\u00b2\u207b + 14H\u207a \u2192 6Fe\u00b3\u207a + 2Cr\u00b3\u207a + 7H\u2082O<\/li>\n\n\n\n<li>Verify the balance of atoms and charges.<\/li>\n\n\n\n<li>For basic medium, first balance as acidic, then add OH\u207b ions equal to H\u207a ions on both sides, combining OH\u207b and H\u207a to form H\u2082O.<\/li>\n<\/ol>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-redox-reactions-as-the-basis-for-titrations\">Redox Reactions as the Basis for Titrations<\/h2>\n\n\n\n<p>Redox titrations are used to determine the strength of a reductant or oxidant using a redox-sensitive indicator.<\/p>\n\n\n\n<p><strong>Types of Indicators<\/strong>:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>Self-indicator reagents:\n<ul class=\"wp-block-list\">\n<li>Example: KMnO\u2084 (MnO\u2084\u207b) \u2013 acts as its own indicator.<\/li>\n\n\n\n<li>Endpoint: appearance of a faint pink colour when all reductant is consumed.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>External indicators:\n<ul class=\"wp-block-list\">\n<li>Example: K\u2082Cr\u2082O\u2087 with diphenylamine indicator.<\/li>\n\n\n\n<li>Diphenylamine turns blue just after the equivalence point.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Iodometric method:\n<ul class=\"wp-block-list\">\n<li>Oxidant liberates iodine from iodide ions:<br>2Cu\u00b2\u207a + 4I\u207b \u2192 Cu\u2082I\u2082 + I\u2082<\/li>\n\n\n\n<li>I\u2082 reacts with starch to give an intense blue colour.<\/li>\n\n\n\n<li>I\u2082 is titrated with sodium thiosulfate:<br>I\u2082 + 2S\u2082O\u2083\u00b2\u207b \u2192 2I\u207b + S\u2084O\u2086\u00b2\u207b<\/li>\n\n\n\n<li>Blue colour disappears at the endpoint.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-limitations-of-the-concept-of-oxidation-number\">Limitations of the Concept of Oxidation Number<\/h3>\n\n\n\n<p>The oxidation number approach assumes complete electron transfer, which is not always the case in covalent compounds (electron shift is often partial).<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The modern view:\n<ul class=\"wp-block-list\">\n<li><strong>Oxidation<\/strong> = decrease in electron density around the atom.<\/li>\n\n\n\n<li><strong>Reduction<\/strong> = increase in electron density around the atom.<br><\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>This reflects the gradual shift in understanding redox processes beyond simple integer oxidation states.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-redox-reactions-and-electrode-processes\">Redox Reactions and Electrode Processes<\/h2>\n\n\n\n<p>The redox reactions and electrode processes are discussed below.<\/p>\n\n\n\n<p><strong>Direct vs. Indirect Electron Transfer<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Example: Zn rod in CuSO\u2084 solution.<\/li>\n\n\n\n<li>Direct reaction:\n<ul class=\"wp-block-list\">\n<li>Zn is oxidised to Zn\u00b2\u207a.<\/li>\n\n\n\n<li>Cu\u00b2\u207a is reduced to Cu metal.<\/li>\n\n\n\n<li>Electrons transfer directly from Zn to Cu\u00b2\u207a.<\/li>\n\n\n\n<li>Heat is evolved.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Modification for indirect electron transfer:\n<ul class=\"wp-block-list\">\n<li>Separate the two half reactions into different containers.<\/li>\n\n\n\n<li>Use zinc sulphate solution with Zn rod and copper sulphate solution with Cu rod in separate beakers.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-redox-couples\">Redox Couples<\/h3>\n\n\n\n<p>A Pair consisting of oxidised and reduced forms of a species taking part in a half reaction. Oxidised form \/ Reduced form (vertical line represents phase\/interface). Examples in this experiment<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Zn\u00b2\u207a\/Zn<\/li>\n\n\n\n<li>Cu\u00b2\u207a\/Cu<\/li>\n\n\n\n<li>The oxidised form is always written first.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-daniell-cell-setup\">Daniell Cell Setup<\/h3>\n\n\n\n<p>The Daniell cell setup is discussed as follows.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Beaker 1: Zn rod in ZnSO\u2084 solution.<\/li>\n\n\n\n<li>Beaker 2: Cu rod in CuSO\u2084 solution.<\/li>\n\n\n\n<li>Connected by:<\/li>\n\n\n\n<li><strong>Salt bridge<\/strong> (U-tube with KCl or NH\u2084NO\u2083 gelled with agar-agar).\n<ul class=\"wp-block-list\">\n<li>Maintains electrical neutrality.<\/li>\n\n\n\n<li>Allows ion migration without mixing solutions.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Metallic wire<\/strong> between rods (with ammeter and switch).<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-observations-when-the-switch-is-on\">Observations When the Switch is ON<\/h3>\n\n\n\n<p>The following are the observations when the switch is on.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>Electrons flow through the metallic wire from Zn to Cu.<\/li>\n\n\n\n<li>Ionic current between solutions flows via the salt bridge.<\/li>\n\n\n\n<li>The flow of current is possible due to a potential difference between the electrodes.<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-electrode-potential\">Electrode Potential<\/h3>\n\n\n\n<p>Potential associated with an electrode is called electrode potential. Standard conditions for Standard Electrode Potential (E\u00b0):<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>All species have unit concentration (1 mol dm\u207b\u00b3).<\/li>\n\n\n\n<li>Gases at 1 atm pressure (if present).<\/li>\n\n\n\n<li>Temperature: 298 K.<\/li>\n\n\n\n<li>Reference electrode: Standard Hydrogen Electrode (SHE) has E\u00b0 = 0.00 V (by convention)<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"h-interpretation-of-e-values\">Interpretation of E\u00b0 values<\/h3>\n\n\n\n<p>The interpretation of E\u00b0 values is given below.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Negative E\u00b0<\/strong>: The Redox couple is a stronger reducing agent than H\u207a\/H\u2082.<\/li>\n\n\n\n<li><strong>Positive E\u00b0<\/strong>: The Redox couple is a weaker reducing agent than H\u207a\/H\u2082.<\/li>\n\n\n\n<li>E\u00b0 values indicate the relative tendency of species to exist in oxidised or reduced form.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-important-formulas-in-ncert-notes-class-11-chemistry-part-ii-chapter-7-redox-reactions\">Important Formulas in NCERT Notes Class 11 Chemistry (Part-II) Chapter 7: Redox Reactions<\/h2>\n\n\n\n<p>Here are the important formulas and equations from NCERT Notes Class 11 Chemistry (Part-2) Chapter 7: Redox Reactions&nbsp;<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxidation Number = (Charge on atom in free state) or as per rules of electronegativity<\/li>\n\n\n\n<li><strong>Oxidation<\/strong>: Increase in oxidation number of an element.<\/li>\n\n\n\n<li><strong>Reduction<\/strong>: Decrease in oxidation number of an element.<\/li>\n\n\n\n<li><strong>Redox reaction<\/strong>: A Change in oxidation number of interacting species indicates a redox reaction.<\/li>\n\n\n\n<li><strong>Balancing via Oxidation Number Method<\/strong>: Increase in ON = Decrease in ON (per atom basis \u00d7 number of atoms)<\/li>\n\n\n\n<li><strong>Oxidation Half Reaction<\/strong>: Fe\u00b2\u207a \u2192 Fe\u00b3\u207a + e\u207b<\/li>\n\n\n\n<li><strong>Reduction Half Reaction<\/strong>: Cr\u2082O\u2087\u00b2\u207b + 14H\u207a + 6e\u207b \u2192 2Cr\u00b3\u207a + 7H\u2082O<\/li>\n\n\n\n<li><strong>Overall Redox Reaction<\/strong>: 6Fe\u00b2\u207a + Cr\u2082O\u2087\u00b2\u207b + 14H\u207a \u2192 6Fe\u00b3\u207a + 2Cr\u00b3\u207a + 7H\u2082O<\/li>\n\n\n\n<li><strong>Electrode Potential<\/strong>: E\u00b0cell = E\u00b0cathode \u2212 E\u00b0anode<\/li>\n\n\n\n<li><strong>Nernst Equation<\/strong>: Ecell = E\u00b0cell \u2212 (0.0591 \/ n) log Q<\/li>\n<\/ul>\n\n\n\n<p><strong>Explore Notes of Class 11 Chemistry<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-background has-fixed-layout\" style=\"background-color:#f1c9d3\"><tbody><tr><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-1-some-basic-concepts-of-chemistry\/\">Chapter 1<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-2-structure-of-atom\/\">Chapter 2<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-3-classification-of-elements-and-periodicity-in-properties\/\">Chapter 3<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-class-11-chemistry-part-i-chapter-iv-chemical-bonding-and-molecular-structure\/\">Chapter 4<\/a><\/strong><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-i-chapter-5-thermodynamics-free-pdf\/\">Chapter 5<\/a><\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p><strong>Download the Solutions of Other Chapters of Class 11 Chemistry<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-background has-fixed-layout\" style=\"background-color:#d0a0f9\"><tbody><tr><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-chemistry-part-1-chapter-1-some-basic-concepts-of-chemistry\/\"><strong>Chapter 1<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-chemistry-part-i-chapter-2-structure-of-atom-free-pdf\/\"><strong>Chapter 2<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-chemistry-part-1-chapter-3-classification-of-elements-and-periodicity-in-properties\/\"><strong>Chapter 3<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-chemistry-part-1-chapter-iv-chemical-bonding-molecular-structure\/\"><strong>Chapter 4<\/strong><\/a><\/td><td><strong>Chapter 5<\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p><strong>Related Reads<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table is-style-stripes\"><table class=\"has-pale-ocean-gradient-background has-background has-fixed-layout\"><tbody><tr><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-psychology-chapter-8-motivation-and-emotion\/\"><strong>NCERT Solutions Class 11 Psychology Chapter 8: Motivation and Emotion (Free PDF)<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-psychology-chapter-8-motivation-and-emotion\/\"><strong>NCERT Notes Class 11 Psychology Chapter 8: Motivation and Emotion (Free PDF)<\/strong><\/a><\/td><\/tr><tr><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-psychology-chapter-7-thinking\/\"><strong>NCERT Solutions Class 11 Psychology Chapter 7: Thinking (Free PDF)<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-psychology-chapter-7-thinking\/\"><strong>NCERT Notes Class 11 Psychology Chapter 7: Thinking (Free PDF)<\/strong><\/a><\/td><\/tr><tr><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-psychology-chapter-6-memory\/\"><strong>NCERT Notes Class 11 Psychology Chapter 6: Memory (Free PDF)<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-solutions-class-11-psychology-chapter-6-memory\/\"><strong>NCERT Solutions Class 11 Psychology Chapter 6: Memory (Free PDF)<\/strong><\/a><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<figure class=\"wp-block-embed is-type-video is-provider-youtube wp-block-embed-youtube wp-embed-aspect-16-9 wp-has-aspect-ratio\"><div class=\"wp-block-embed__wrapper\">\n<iframe loading=\"lazy\" title=\"Redox Reactions Class 11 One Shot | NCERT Chemistry Complete Chapter-7 Revision | CBSE 2025-26\" width=\"1200\" height=\"675\" src=\"https:\/\/www.youtube.com\/embed\/X86UraGJtNk?feature=oembed\" frameborder=\"0\" allow=\"accelerometer; autoplay; clipboard-write; encrypted-media; gyroscope; picture-in-picture; web-share\" referrerpolicy=\"strict-origin-when-cross-origin\" allowfullscreen><\/iframe>\n<\/div><\/figure>\n\n\n\n<p>Source- Next Toppers: 11th Science<\/p>\n\n\n\n<p><strong>Explore notes on other subjects in the NCERT Class 11<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-background has-fixed-layout\" style=\"background-color:#ffc7c7\"><tbody><tr><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-and-solutions-class-11-english\/\"><strong>English<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-and-solutions-class-11-sociology\/\"><strong>Sociology<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-and-solutions-class-11-geography\/\"><strong>Geography<\/strong><\/a><\/td><td><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-and-solutions-class-11-political-science\/\"><strong>Political Science<\/strong><\/a><\/td><td><strong><a href=\"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-and-solutions-class-11-psychology\/\">Psychology<\/a><\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"h-faqs\">FAQs<\/h2>\n\n\n\n<div class=\"schema-faq wp-block-yoast-faq-block\"><div class=\"schema-faq-section\" id=\"faq-question-1754881449008\"><strong class=\"schema-faq-question\"><strong>Q1. What is meant by oxidation number?<\/strong><\/strong> <p class=\"schema-faq-answer\">Ans: Oxidation number denotes the oxidation state of an element in a compound, determined according to rules based on the assumption that the electron pair in a covalent bond belongs entirely to the more electronegative element.<\/p> <\/div> <div class=\"schema-faq-section\" id=\"faq-question-1754881466378\"><strong class=\"schema-faq-question\"><strong>Q2. What is a redox couple?<\/strong><\/strong> <p class=\"schema-faq-answer\">Ans: A redox couple consists of the oxidised and reduced forms of a substance taking part in an oxidation or reduction half-reaction, represented as oxidised form\/reduced form (e.g., Zn\u00b2\u207a\/Zn, Cu\u00b2\u207a\/Cu).<\/p> <\/div> <div class=\"schema-faq-section\" id=\"faq-question-1754881491588\"><strong class=\"schema-faq-question\"><strong>Q3. What is the difference between oxidation and reduction in terms of oxidation number?<\/strong><\/strong> <p class=\"schema-faq-answer\">Ans: Oxidation is an increase in the oxidation number of an element in a given substance, whereas reduction is a decrease in the oxidation number of an element in a given substance.<\/p> <\/div> <\/div>\n\n\n\n<p>For more topics, follow LeverageEdu <a href=\"https:\/\/leverageedu.com\/discover\/category\/school-education\/ncert-study-material\/\"><strong>NCERT Study Material<\/strong><\/a> today!&nbsp;<\/p>\n","protected":false},"excerpt":{"rendered":"Chemistry studies the vast diversity of matter and the transformations that change one type of matter into another.&hellip;\n","protected":false},"author":133,"featured_media":866481,"comment_status":"open","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"editor_notices":[],"footnotes":""},"categories":[477,389],"tags":[],"class_list":{"0":"post-866473","1":"post","2":"type-post","3":"status-publish","4":"format-standard","5":"has-post-thumbnail","7":"category-ncert-study-material","8":"category-school-education"},"yoast_head":"<!-- This site is optimized with the Yoast SEO Premium plugin v27.3 (Yoast SEO v27.3) - https:\/\/yoast.com\/product\/yoast-seo-premium-wordpress\/ -->\n<title>NCERT Notes Class 11 Chemistry (Part-II) Chapter 7: Redox Reaction (Free PDF) - Leverage Edu Discover<\/title>\n<meta name=\"description\" content=\"NCERT Notes for Class 11 Chemistry (Part-II) Chapter 7: Redox Reactions. 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What is meant by oxidation number?","answerCount":1,"acceptedAnswer":{"@type":"Answer","text":"Ans: Oxidation number denotes the oxidation state of an element in a compound, determined according to rules based on the assumption that the electron pair in a covalent bond belongs entirely to the more electronegative element.","inLanguage":"en-US"},"inLanguage":"en-US"},{"@type":"Question","@id":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-ii-chapter-7-redox-reactions\/#faq-question-1754881466378","position":2,"url":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-ii-chapter-7-redox-reactions\/#faq-question-1754881466378","name":"Q2. What is a redox couple?","answerCount":1,"acceptedAnswer":{"@type":"Answer","text":"Ans: A redox couple consists of the oxidised and reduced forms of a substance taking part in an oxidation or reduction half-reaction, represented as oxidised form\/reduced form (e.g., Zn\u00b2\u207a\/Zn, Cu\u00b2\u207a\/Cu).","inLanguage":"en-US"},"inLanguage":"en-US"},{"@type":"Question","@id":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-ii-chapter-7-redox-reactions\/#faq-question-1754881491588","position":3,"url":"https:\/\/leverageedu.com\/discover\/school-education\/ncert-notes-class-11-chemistry-part-ii-chapter-7-redox-reactions\/#faq-question-1754881491588","name":"Q3. What is the difference between oxidation and reduction in terms of oxidation number?","answerCount":1,"acceptedAnswer":{"@type":"Answer","text":"Ans: Oxidation is an increase in the oxidation number of an element in a given substance, whereas reduction is a decrease in the oxidation number of an element in a given substance.","inLanguage":"en-US"},"inLanguage":"en-US"}]}},"acf":[],"_links":{"self":[{"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/posts\/866473","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/users\/133"}],"replies":[{"embeddable":true,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/comments?post=866473"}],"version-history":[{"count":0,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/posts\/866473\/revisions"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/media\/866481"}],"wp:attachment":[{"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/media?parent=866473"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/categories?post=866473"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/leverageedu.com\/discover\/wp-json\/wp\/v2\/tags?post=866473"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}