Redox reaction class 11 notes

Subtopics of Class 11 Chemistry Chapter 8 Redox Reactions • Classical Idea Of Redox Reactions – Oxidation And Reduction Reactions • Redox Reactions In Terms Of Electron Transfer Reactions • Competitive Electron Transfer Reactions • Oxidation Number • Types Of Redox Reactions • Balancing Of Redox Reactions • Redox Reactions As The Basis For Titrations • Limitations Of Concept Of Oxidation Number • Redox Reactions And Electrode Processes. Redox Reactions Class 11 Notes Chemistry Chapter 8 • Oxidation Oxidation is defined as the addition of oxygen/electronegative element to a substance or rememoval of hydrogen/ electropositive element from a susbtance. For example, • Reduction Reduction is defined as the memoval of oxygen/electronegative element from a substance or addition of hydrogen or electropositive element to a substance. For example, • Redox Reaction in Terms of Electron Transfer Reaction A few examples of redox reaction on the basis of electronic concept are given below: According to electronic concept every redox reaction consists of two steps known as half reactions. (i) Oxidation reaction: Half reactions that involve loss of electrons are called oxidation reactions. (ii) Reduction reaction: Half reactions that involve gain of electrons are called reduction reactions. Oxidising agent: Acceptor of electrons. Reducing agent: Donar of electrons. • Competitive Electron Transfer Reactions To understand this concept let us do an experiment. Place a strip of metallic zinc ...

Please refer toRedox Reactions Class11ChemistryRedox Reactions Notes and Questions Oxidation number denotes the oxidation state of an element in a compoundascertained according to a set of rules formulated on the basis that electron in acovalent bond belongs entirely to more electronegative element. Calculation of oxidation number- 1. O. S. of all the elements in their elemental form (in standard state) is taken aszero O. S. of elements in Cl 2, F 2, O 2, P 4, O 3, Fe(s), H 2, N 2, C(graphite) is zero. 2. Common O. S. of elements of group one (1st) is one. Common O. S. ofelements of group two (2nd) is two. 3. For ions composed of only one atom, the oxidation number is equal to thecharge on the ion. 4. The oxidation number of oxygen in most compounds is –2 .While in peroxides(e.g., H 2O 2, Na 2O 2), each oxygen atom is assigned an oxidation number of –1,in super oxides (e.g., KO 2,Rb O 2) each oxygen atom is assigned an oxidation number of – (½). 5. In oxygen difluoride (OF 2) and dioxygen difluoride (O 2F 2), the oxygen isassigned an oxidation number of +2 and +1,respectively. 6. The oxidation number of hydrogen is +1 but in metal hydride its oxidation no.is –1. 7. In all its compounds, fluorine has an oxidation number of –1. 8. The algebraic sum of the oxidation number of all the atoms in a compoundmust be zero. 9. In polyatomic ion, the algebraic sum of all the oxidation numbers of atomsof the ion must equal the charge on the ion. Stock notation: the oxidation number is ...

Chapter 8 Redox Reactions Class 11 Notes are prepared by our panel of highly experienced teachers strictly according to the latest Syllabus on the guidelines by CBSE. Redox Reactions Class 11 Notes Chemistry Chapter 8 Redox Reaction Class 11 Notes • Oxidation Oxidation is defined as the addition of oxygen/electronegative element to a substance or rememoval of hydrogen/ electropositive element from a susbtance. For example, • Reduction Reduction is defined as the memoval of oxygen/electronegative element from a substance or addition of hydrogen or electropositive element to a substance. For example, • Redox Reaction in Terms of Electron Transfer Reaction A few examples of redox reaction on the basis of electronic concept are given below: According to electronic concept every redox reaction consists of two steps known as half reactions. (i) Oxidation reaction: Half reactions that involve loss of electrons are called oxidation reactions. (ii) Reduction reaction: Half reactions that involve gain of electrons are called reduction reactions. Oxidising agent: Acceptor of electrons. Reducing agent: Donar of electrons. Redox Reactions Class 11 Notes • Competitive Electron Transfer Reactions To understand this concept let us do an experiment. Place a strip of metallic zinc in an aqueous solution of copper nitrate as shown in Fig. After one hour following changes will be noticed. (i) Strips becomes coated with reddish metallic copper. (ii) Blue colour of the solution disappears. (iii...

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Chemistry involves a lot of conceptual clarity to answer all kinds of questions in the CBSE exams . That is why it becomes essential for Class 11 students to get Chemistry Class 11 Notes prepared by experienced teachers. The subject matter experts at Vedantu have designed these Notes of Chemistry Class 11 by putting in hours of research on the latest CBSE curriculum . These notes are extremely beneficial for students from an exam point of view. Students can also download the revision notes so that preparing for exams becomes much easier. Download CBSE Class 11 Chemistry Revision Notes 2023-24 PDF Also, check CBSE Class 11 Chemistry revision notes for other chapters: CBSE Class 11 Chemistry Revision Notes CBSE Class 11 Chemistry Chapter 1 Revision Notes CBSE Class 11 Chemistry Chapter 8 Revision Notes CBSE Class 11 Chemistry Chapter 2 Revision Notes CBSE Class 11 Chemistry Chapter 9 Revision Notes CBSE Class 11 Chemistry Chapter 3 Revision Notes CBSE Class 11 Chemistry Chapter 10 Revision Notes CBSE Class 11 Chemistry Chapter 4 Revision Notes CBSE Class 11 Chemistry Chapter 11 Revision Notes CBSE Class 11 Chemistry Chapter 5 Revision Notes CBSE Class 11 Chemistry Chapter 12 Revision Notes CBSE Class 11 Chemistry Chapter 6 Revision Notes CBSE Class 11 Chemistry Chapter 13 Revision Notes CBSE Class 11 Chemistry Chapter 7 Revision Notes CBSE Class 11 Chemistry Chapter 14 Revision Notes Class 11th Chemistry is a stepping stone for students to hone their knowledge in Chemistry f...

Introduction Redox reaction is related to gain or loss of electrons. Reaction in which oxidation and reduction takes place simultaneously is called redox reaction. This chapter deals with problems based on redox reactions, oxidation number and balancing of redox reactions by ion, electron method and oxidation number method. Oxidation Reactions Oxidation is defined as the addition of oxygen/electronegative element to a substance or rememoval of hydrogen/ electropositive element from a susbtance. 2Mg(s) + O 2(g) ⟶ 2MgO(s) Mg(s) + Cl 2(g) ⟶ MgCl 2(s) Reduction Reactions Reduction is defined as the memoval of oxygen/electronegative element from a substance or addition of hydrogen or electropositive element to a substance. 2FeCl 3(aq) + H 2(g) ⟶ 2FeCl 2(aq) + 2HCl(aq) 2HgO(s) ⟶ 2Hg(l) + O 2(g) Redox Reactions Reaction in which oxidation and reduction takes place simultaneously is called redox reaction. Oxidation and reduction are complementary to each other, one cannot take place alone. So both oxidation and reduction will occur simultaneously. It is obvious that if a substance takes electrons there must be another substance to give up these electrons. 2FeCl 3 + SnCl 2⟶ 2Fecl 2 + SnCl 4 Oxidation Number or Oxidation State Oxidation number for an element is the arbitrary charge present on one atom when all other atoms bonded to it are removed. For example, if we consider a molecule of HCl, the Cl atom is more electronegative than H-atom, therefore, the bonded electrons will go w...

Oxidation Reduction 1.Addition of oxygen 1.Addition of hydrogen 2.Removal of hydrogen 2.Removal of oxygen 3.Addition of electronegative element 3.Addition of electropositive element 4.Removal of electropositive element 4.Removal of electronegative element 5.Loss of electron by an element 5.Gain of electrons by an element