oxidation number method class 11

January 7, 2021

Balancing Download Lecture Notes From Physicswallah App(bit.ly/2SHIPW6) Notes Available at Home Page of the App(Home Pace) PACE - Class 11th : Scheduled Syllabus released describing :- which topics will be taught for how many days. Benzoic acid-definition-properties-preparation from benzene and phenol. Step IV Equalize the total increase or decrease in oxidation number. Oxidation number of potassium permanganate (KMnO 4) = Sum of oxidation number of (K + Mn + 4O) = 0. 06.11 Hess’s Law and Enthalpies for Different Types of Reactions. ortho and para directing and Why ‘Cl’-atom can not form H-bond but ‘N’-atom can ? Molecular orbital theory and stability of helium molecule, Nephelauxetic effect and Nephelauxetic series, Octet rule-definition-limitations of octet rule-hypovalent-hypervalent compounds, Phenol definition-Phenol structure and Identification in chemistry, Polarization meaning-Ionic potential-polarizability and polarizing power. For example, balance the equation. Redox reactions are oxidation-reduction reactions where reactants undergo changes in oxidation states. CBSE Class 11 Chemistry , CBSE Class 11 Physics. left side of the equation. Multiple Choice Questions Single Correct Answer Type . 6.11 Hess’s Law and Enthalpies for Different Types of Reactions, 06.13 Enthalpy of solution and Lattice Enthalpy, 6.13 Enthalpy of Solution and Lattice Enthalpy, 07.02 Equilibrium In Physical Processes – I, 7.02 Equilibrium In Physical Processes - I, 07.03 Equilibrium In Physical Processes – II, 7.03 Equilibrium In Physical Processes - II, 07.04 Equilibrium in Chemical Processes – Dynamic Equilibrium, 7.04 Equilibrium in Chemical Processes - Dynamic Equilibrium, 07.05 Law of Chemical Equilibrium and Equilibrium Constant, 7.05 Law of Chemical Equilibrium and Equilibrium Constant, 07.08 Characteristics and Applications of Equilibrium Constants, 7.08 Characteristics and Applications of Equilibrium Constants - I, 07.09 Characteristics and Applications of Equilibrium Constants – II, 7.09 Characteristics and Applications of Equilibrium Constants - II, 07.10 Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G, 7.10 Relationship Between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G, 07.14 Acids, Bases and Salts – Arrhenius Concept, 7.14 Acids, Bases and Salts - Arrhenius Concept, 07.15 Acids, Bases and Salts – Brönsted-Lowry Concept and Lewis Concept, 7.15 Acids, Bases and Salts - Brönsted-Lowry Concept and Lewis Concept, 07.16 Ionization of Acids and Bases and KW of Water, 7.16 Ionization of Acids and Bases and KW of Water, 07.18 Ionization Constants of Weak Acids and Weak Bases, 7.18 Ionization Constants of Weak Acids and Weak Bases, 07.19 Factors Affecting Acid Strength and Common Ion Effect, 7.19 Factors Affecting Acid Strength and Common Ion Effect, 07.20 Hydrolysis of Salts and the pH of their solutions, 7.20 Hydrolysis of Salts and the pH of their solutions, 08.02 Redox Reaction in terms of Electron Transfer Reaction, 8.02 Redox Reaction in Terms of Electron Transfer, 08.08 Redox Reactions as Basis for Titration, 8.08 Redox Reactions as Basis for Titration, 08.09 Redox Reactions and Electrode processes, 8.09 Redox Reactions and Electrode Processes, 09.01 Introduction to Hydrogen and its Isotopes, 9.01 Introduction to Hydrogen and Its Isotopes, 09.06 Structure of Water and Ice, Hard and Soft water, 9.06 Structure of Water and Ice, Hard and Soft water, 10.02 Group I Elements /Alkali Metals: Properties – I, 10.02 Group I Elements (Alkali Metals) Properties - I, 10.03 Group I Elements /Alkali Metals: Properties – II, 10.03 Group I Elements (Alkali Metals) Properties - II, 10.04 General Characteristics of Compounds of Alkali Metals, 10.05 Anomalous Properties of Lithium and diagonal relationship, 10.05 Anomalous Properties of Lithium and Diagonal Relationship, 10.06 Compounds of Sodium: Na2CO3 and NaHCO3, 10.06 Compounds of Sodium - Na2CO3 and NaHCO3, 10.07 Compounds of Sodium - NaCl and NaOH, 10.08 Group II Elements “Alkaline Earth Metals”- I, 10.08 Group II Elements (Alkaline Earth Metals) - I, 10.09 Group II Elements “Alkaline Earth Metals”- II, 10.09 Group II Elements (Alkaline Earth Metals) - II, 10.10 Uses of Alkali Metals and Alkaline Earth Metals, 10.11 General Characteristics of Compounds of Alkaline Earth Metals, 10.12 Anomalous Behaviour of Beryllium and Diagonal Relationship, 10.13 Some Important Compounds of Calcium: CaO and Ca(OH)2, 10.13 Some Important Compounds of Calcium - CaO and Ca(OH)2, 10.14 Important Compounds of Calcium: CaCO3, CaSO4 and Cement, 10.14 Important Compounds of Calcium - CaCO3, CaSO4 and Cement, 11.03 Group 13 Elements: The Boron Family, 11.03 Group 13 Elements - The Boron Family, 11.04 The Boron Family: Chemical Properties, 11.04 The Boron Family - Chemical Properties, 11.06 Boron and its compounds – Ortho Boric Acid and Diborane, 11.06 Boron and Its Compounds - Ortho Boric Acid and Diborane, 11.07 Uses of Boron and Aluminium And their Compounds, 11.07 Uses of Boron and Aluminium and Their Compounds, 11.08 The Carbon Family Overview and Physical Properties, 11.09 The Carbon Family Overview and Chemical Properties, 11.10 Important Trends and Anomalous Behaviour of Carbon, 11.12 Important Compounds of Carbon: Carbon Monoxide, 11.12 Important Compounds of Carbon - Carbon Monoxide, 11.13 Important Compounds of Carbon: Carbon dioxide, 11.13 Important Compounds of Carbon - Carbon Dioxide, 11.14 Important Compounds of Silicon: Silicon dioxide, 11.14 Important Compounds of Silicon - Silicon Dioxide, 11.15 Important Compounds of Carbon: Silicones, Silicates, Zeolites, 11.15 Important Compounds of Carbon - Silicones, Silicates, Zeolites, 12 Organic Chemistry - Some Basic Principles and Techniques, 12.01 Organic Chemistry and Tetravalence of Carbon, 12.02 Structural Representation of Organic Compounds, 12.03 Classification of Organic Compounds, 12.05 Nomenclature of branched chain alkanes, 12.05 Nomenclature of Branched Chain Alkanes, 12.06 Nomenclature of Organic Compounds with Functional Group, 12.06 Nomenclature of Organic Compounds with Functional Group, 12.07 Nomenclature of Substituted Benzene Compounds, 12.12 Resonance Structure and Resonance Effect, 12.12 Resonance Structure and Resonance Effect, 12.13 Electromeric Effect and Hyperconjugation, 12.14 Methods of purification of organic compound – Sublimation, Crystallisation, Distillation, 12.14 Methods of Purification of Organic Compound, 12.15 Methods of purification of organic compound – Fractional Distillation and Steam Distillation, 12.15 Methods of Purification of Organic Compound, 12.16 Methods of purification of organic compound – Differential Extraction and Chromatography, 12.16 Methods of Purification of Organic Compound, 12.17 Methods of purification of organic compound- Column, Thin layer and Partition Chromatography, 12.17 Methods of Purification of Organic Compound, 12.18 Qualitative analysis of organic compounds, 12.18 Qualitative Analysis of Organic Compounds, 12.19 Quantitative analysis of Carbon and Hydrogen, 12.19 Quantitative Analysis of Carbon and Hydrogen, 13.01 Hydrocarbons Overview and Classification, 13.04 Physical and Chemical Properties of Alkanes – I, 13.04 Physical and Chemical Properties of Alkanes - I, 13.05 Physical and Chemical Properties of Alkanes – II, 13.05 Physical and Chemical Properties of Alkanes - II, 13.07 Alkenes – Structure, Nomenclature, And Isomerism, 13.07 Alkenes - Structure, Nomenclature and Isomerism, 13.09 Physical and Chemical Properties of Alkenes – I, 13.09 Physical and Chemical Properties of Alkenes, 13.10 Physical and Chemical Properties of Alkenes – II, 13.10 Physical and Chemical Properties of Alkenes, 13.11 Alkynes – Structure, Nomenclature and Isomerism, 13.11 Alkynes - Structure, Nomenclature and Isomerism, 13.13 Physical and Chemical Properties of Alkynes – I, 13.13 Physical and Chemical Properties of Alkynes, 13.14 Physical and Chemical Properties of Alkynes – II, 13.14 Physical and Chemical Properties of Alkynes, 13.15 Benzene, Preparation and Physical Properties, 13.16 Aromatic Hydrocarbons – Structure, Nomenclature and Isomerism, 13.16 Aromatic Hydrocarbons - Structure, Nomenclature and Isomerism, 13.19 Mechanism of Electrophilic Substitution Reactions, 13.19 Mechanism of Electrophilic Substitution Reaction, 13.20 Directive influence of a functional group in Monosubstituted Benzene, 13.20 Directive Influence of a Functional Group in Mono substituted Benzene, 14.02 Tropospheric pollutants : Gaseous air pollutant – I, 14.2 Tropospheric Pollutants - Gaseous air Pollutant, 14.03 Tropospheric pollutants : Gaseous air pollutant – II, 14.03 Tropospheric Pollutants - Gaseous Air Pollutant, 14.04 Global Warming and Greenhouse Effect, 14.06 Tropospheric pollutants : Particulate pollutant, 14.06 Tropospheric Pollutants - Particulate Pollutant, 14.10 Water Pollution: Chemical Pollutant, 14.10 Water Pollution - Chemical Pollutant, 14.11 Soil Pollution, Pesticides and Industrial Waste, 14.12 Strategies to control environmental pollution, 14.12 Strategies to Control Environmental Pollution, Chapter 14 Environmental Chemistry - Test. References. Why furan 2-aldehyde undergoes cannizaro reaction but pyrrole 2-aldehyde does not-explain ? K Mn O 4 or K Mn O 4 + 1 + x 4 x (-2) +1 +x -8. the case of acidic medium reactions, to equalize the number of, If the reaction occurs through an alkaline Centre of symmetry and alternating axis of symmetry, 3 proto-tropic shifts and difference between tautomerism and resonance. Offer ending soon! or own an. Huckel’s rule of aromaticity and anti aromatic compounds, Hydroiodic acid-formula-properties-uses with pH calculation, IUPAC name and structural formula of beta methyl butyric acid. heated caustic soda solution is heated with Al powder, sodium aluminate and the product substance with integers. Now, By multiplying H 2 O 2 and O 2 with 4 to balance the increase and decrease in the oxidation number, we get: Cl 2 O 7(g) + 4H 2 … Oxidation number method: Total decrease in oxidation number of Cl 2 O 7 = 4 × 2 = 8. the total increase in the oxidations number for the two O-atoms present in the occurring with acids mediums. Download the App from Google Play Store. What is the simplest way for converting CO2 to O2? Structural formula and f IUPAC name of functional isomer of CH3-CH2 – O – CH3. K2SO4, MnSO4, H2O and O2. In the reaction Al oxidizes to produce NaAlO2 Which have more π-acceptor strength among the CO. The general idea is that electrons are transferred between charged atoms. When ; When oxygen is part of a peroxide, its oxidation number is -1. . Now to the sum of oxidation numbers of all atoms in the formula of the compound must be zero, i.e. Become our. Why quinuclidine is a stronger base than aniline and N, Why the nucleophilic substitution reaction of 1-chloro-2, Xenon fluorides-xenon fluorides act as a strong oxidizing agent, [FeF6]3– ion paramagnetic while [Fe(CN)6]4–ion diamagnetic, [Ni(NH3)6]2+paramagnetic while [Ni (CN) 6]4-diamagnetic, activating groups-explanation-list with application. NEW. Oxidation Number Method. For this reason, symbols of oxidant and reductant are multiplied by the suitable smallest integer, so that the change CBSE Class 11 Chemistry , CBSE Class 11 Physics. Balancing equations chemistry by oxidation number method for class 11, Balancing the total decrease in oxidation number of H-atoms of 1 molecule NaOH and 1 medium, then in order to equalize the number of oxygen-atoms, one H2O molecules O2 respectively. (a) HPO 3 2-and (b) PO 4 3-Calculate the oxidation number of each sulphur atom in the following compounds: (a) Na 2 S 2 O 3 (b) Na 2 S 4 O 6 (c) Na 2 SO 3 (d) Na 2 SO 4; Balance the following equations by the oxidation number method. JEE NEET Study Material : Notes , Assignment. Oxidation number of mono-atomic ions is equal to the algebraic charge on them. clear. Importance of hydrogen bonding in biological system. This method is based on the principle that the number of electrons lost in oxidation must be equal to the number of electrons gained in reduction. By multiplying H 2 O 2 and O 2 with 4 to balance the increase and decrease in the oxidation number, we get: Cl 2 O 7(g) + 4H 2 O 2(aq) → CIO-2(aq) + 4O 2(g) The Cl atoms are balanced as: For Study plan details. Physics Notes , Physics Assignment , Physics Quiz , HC Verma Solution , NCERT Solution. Among the following molecules, in which does bromine show the maximum oxidation number? Watch all CBSE Class 5 to 12 Video Lectures here. Thus How do you explained the bonding of the carbonyl groups in the structure of Fe2(CO)9 through IR-spectra ? on the side with the excess hydrogen-atoms, a suitable number of. CBSE Class 11 Chemistry Redox Reactions – Get here the Notes for Class 11 Redox Reactions . oxidation number. This is necessary, because of law of mass action says that the total mass of reactants before is equal to the total mass of products after reaction. Thus, 3 molecules H2SO4 are required on the So | EduRev Class 11 Question is disucussed on EduRev Study Group by 197 Class 11 Students. Q1. Any free element has an oxidation number equal to zero. left side of the equation. Post Comments How do you explained the bonding of the carbonyl groups in the structure of Fe2(CO)9 through IR-spectra ? NaH 2 PO 4; Na +1. Course. Total increase in oxidation number of Cl = 1 × 6 = 6. (+2) = 5 units. In The oxidation number method is based on the change in the oxidation number … The steps to be followed are : Write the equation (if it is not complete, then complete it) representing the chemical changes. Balancing equations chemistry by oxidation number method for class 11 . Now Oxidation number method: Total decrease in oxidation number of N = 2 × 4 = 8. Indicate the oxidation number of all the elements involved in the reaction. increase the oxidation number of Al-atoms = (+ 3) - 0 = 3 units. (a) CuO + H 2 → Cu + H 2 0 (b) Fe 2 0 2 + 3CO → 2Fe + 3C0 2 (c).2K + F 2 →2KF (d) BaCl 2 + H 2 S0 4 →BaS0 4 + 2FIC1 Sol: (d) BaCl 2 + H 2 S0 4 —> BaS0 4 + 2HC1 is not a redox reaction. Why C – O bond length in phenol is less than methanol and what is Bouveault Blanc reduction ? What are the various sources of carbon dioxide emissions? Halogen family elements-properties-periodic table-oxyacids-radioactivity. Calculating Oxidation Numbers. In almost all cases, oxygen atoms have oxidation numbers of -2. Call our LearnNext Expert on 1800 419 1234 (tollfree) OR submit details below for a call back. Download the App from Google Play Store. What is electro cyclic reaction and symmetry forbidden-symmetry allowed process ? Get a free home demo of LearnNext . #"Zn" + "HCl" → "ZnCl"_2 + "H"_2# Step 1. Again in the case of equations of chemical Oxidation Number Or Oxidation State Redox Reaction of Class 11 Oxidation no. How do you explained the bonding of the carbonyl groups in the structure of Fe2(CO)9 through IR-spectra ? Oxidation Available for CBSE, ICSE and State Board syllabus. Download the App from Google Play Store. the opposite side. In this case, the chemical equation is. periodicity and different atomic radius and ionic radius. Which one is more basic aniline or 4-bromoaniline ? Decrease in the oxidation number of Mn = +7 - the balancing equation is. It involves the following steps. Call our LearnNext Expert on 1800 419 1234 (tollfree) OR submit details below for a call back. the, In the reaction Al oxidizes to produce NaAlO2 H +1. Contact. JEE NEET Study Material : Notes , Assignment. What are the harmful effects of acid rain on humans in chemistry? be 2: 5. equations chemistry, balancing equations, balancing equations by oxidation To assign oxidation number you should know the rules Rules: Oxidation number of free element is always ZERO Example: The oxidation number of atoms in O 2, H 2 and N 2 = 0 The oxidation number of Hydrogen is +1 Exception: In Metal hydrides the oxidation state of hydrogen is -1 The Oxidation state of IA group elements = +1 NCERT exemplar chemistry class 11 Chapter 8 pdf has varieties of question including MCQ’S, fill in the blanks, match the following, short and long answer questions, worksheets, exercises, tips and tricks that are crucial for your class 11 chemistry examination and graduate entrance examinations. is an oxygen-atom deficiency and the appropriate number of alkali molecules on Education Franchise × Contact Us. What is environmental pollution in chemistry? Class 11 - Chemistry - Redox Reactions. A very important thing to keep in mind while writing oxidation-reduction reactions is to correctly write the compositions and formulas of the substances and products present in the chemical reaction. Understand balancing Redox reactions with Examples, Types, and Applications. number of Al-atoms, the number of NaOH molecules and the number of H2O Electron affinity and periodic variation of electron affinity. Watch Oxidation Number Method in Acidic Medium part 1 in English from Oxidation Number and Balancing of Redox Reactions here. Double salts-definition-examples and properties in co-ordination chemistry . The oxidation number method is a way of keeping track of electrons when balancing redox equations. Videos. What are the main causes of acid rain in environmental chemistry? (+2) = 5 units. Dec 03,2020 - oxidation number method of balancing redox reaction Related: Balancing Redox Reactions using Oxidation Number Method? CBSE Class-11 keyboard_arrow_right; Chemistry keyboard_arrow_right; Redox Reactions keyboard_arrow_right; Balancing Redox Equations . So the equation of the given reaction would A redox equation can be balanced using two methods - oxidation number method and half-reaction method. This is why the decrease What is Borodine Hunsdiecker reaction and its limitation ? equations of chemical reaction in the oxidation number system. A sigma bond is formed by the face to face overlapping of two 's' orbit... What is elements of symmetry ? Aspirin-use of aspirin and aspirin from phenol . What is chemical bonding and What is dative bond ? … reactions occurring through alkalis. The oxidation number method is a way of keeping track of electrons when balancing redox equations. stereo specific and stereo selective reaction. To assign oxidation number you should know the rules Rules: Oxidation number of free element is always ZERO Example: The oxidation number of atoms in O 2, H 2 and N 2 = 0 The oxidation number of Hydrogen is +1 Exception: In Metal hydrides the oxidation state of hydrogen is -1 The Oxidation state of IA group elements = +1 Watch Ad Free Videos ( Completely FREE ) on Physicswallah App(bit.ly/2SHIPW6). alkalis are shown below. On multiplying N 2 H 4 with 3 and with 4 to balance the increase and decrease in O.N., we get: The N and Cl atoms are balanced as: The O atoms are balanced by adding 6H 2 O as: This is the required balanced equation. Mg + HNO 3 → Mg(NO 3) 2 + N 2 O + H 2 O. Oxidation number of oxygen in oxide ion(O 2-) is -2, and in peroxide ion(O-O 2-) is -1. Need assistance? Total increase in oxidation number of Cl = 1 × 6 = 6. In this method, the balancing of reactions is provided by Redox Reaction: solve the following equation by ion electron method in acidic medium NO3 (-ve)+I (-ve)+H (+) =NO +I2 +H2O magnesium reacts with nitric acid to give magnesium nitarate and nitrous oxide gas and liquid water balance this by oxidation number method Candidates who are ambitious to qualify the Class 11 with good score can check this article for Notes. medium, then in order to equalize the number of, Again to equalize the number of hydrogen-atoms of e – s in O.H. equations by oxidation number method simple examples. Learn oxidation number method step by step with example helpful for CBSE Class 11 Chemistry Chapter8 Redox reaction. • balance chemical equations using (i) oxidation number (ii) half reaction method; • learn the concept of redox reactions in terms of electrode. What is chemical bonding and What is dative bond ? Triplet carbene is more stable than singlet carbene. Hence, the oxidation number of Mn in KMnO 4 is +7. increase in oxidation number has to be equal. NCERT Solutions for Class 11 Chemistry: Chapter 8 (Redox Reactions) are provided on this page for the perusal of Class 11 Chemistry students studying under the syllabus prescribed by CBSE.Detailed, student-friendly answers to each and every intext and exercise question provided in Chapter 8 of the NCERT Class 11 Chemistry textbook can be found here. Why phenol is stronger acid than alcohol and salicylic acid is a stronger acid than p-hydroxy benzoic acid ? added on the opposite side. oxidant and the reactant in which the atomic number of atoms in an element side where there is a deficiency of hydrogen-atoms. To assist you with that, we are here with notes. For Class 11 Chemistry Redox Reactions: Balancing of Redox reactions: Balancing of Redox reactions. Aug 31, 2020 - Redox Reactions - Class Notes, Chemistry, Class 11 | EduRev Notes is made by best teachers of JEE. Inert pair effect-definition-examples-cause-and consequences, Isomerism and classification of structural isomerism, Lanthanide contraction-definition-causes-consequences in chemistry, Lattice energy of MgF2-CaF2-ZrO2 molecule-explanation-calculation. Class 11 - Chemistry - Redox Reactions. Here's how the oxidation number method works for a very simple equation that you could probably balance in your head. 1. Water is generated from these hydrogen atoms. Now, 4. changes 4. Therefore, Benzyl alcohol to benzoic acid change-Schmidt reaction-HVZ reaction. NCERT Solutions for Class 11 Chemistry Chapter 8 Redox Reactions includes all the important topics with detailed explanation that aims to help students to understand the concepts better. Now Candidates who are ambitious to qualify the Class 11 with good score can check this article for Notes. Contact. the case of acidic medium reactions, to equalize the number of oxygen-atoms, Oxidation number is defined as is the charge or the apparent charge that an atom in a compound or ion would have, if all of the electrons in its bonds belonged entirely to the more electronegative atom. balancing equation is as follows. clear. molecules H2O2 and 3 molecules H2SO4 is 16. 1800-212-7858 / 9372462318. CBSE Class 12 Chemistry , CBSE Class 12 Physics. Academic Partner . CBSE Videos for Class 11 Chemistry Redox Reactions. Question 8.1. ). the oxidation number of the atoms of the elements in the reactant and the Hence, the oxidation number of Mn in KMnO 4 is +7. Assign oxidation number to the underlined elements in each of the following species: NaH 2 PO 4 (b) NaHSO 4 (c) H 2 P 2 O 7 (d) K 2 MnO 4 (e) CaO 2 (f) NaBH 4 (g) H 2 S 2 O 7 (h) KAl(SO 4) 2.12H 2 O; Answer. Oxidation number of potassium permanganate (KMnO 4) = Sum of oxidation number of (K + Mn + 4O) = 0. molecule H2O = 1 + 2 = 3 units. 4 H2O molecules have to be placed on the right side of the equation. What is kinetically and thermodynamically controlled reaction ? In the case of the oxidation number method, an equation of the reaction is created by first identifying the reactants and the products. molecules O2 respectively. Step III Balance atoms other than H and O in two processes. What is penetration effect ?How does penetration effect influence the ionization energy ? To assist you with that, we are here with notes. In Thus, 3 molecules H2SO4 are required on the An important method of balancing equations of chemical reactions is the oxidation number system. Why methyl chloride (CH3Cl) is inactive in SN1 reaction and (CH3)3C-Cl ( t-butyl chloride) is inactive in SN2 reaction ? Calculation of Oxidation Number of an Atom in a Molecule/Ion. There are few examples of tautomerism in which case only one tautomer... Why are  sigma bond more stronger than pi bond ? Here's how the oxidation number method works for a very simple equation that you could probably balance in your head. Complete Oxidation Number Class 11 Notes | EduRev chapter (including extra questions, long questions, short questions, mcq) can be found on EduRev, you can check out Class 11 lecture & lessons summary in the same course for Class 11 Syllabus. units. 1800-212-7858 / 9372462318. Oxidation Number ,Redox Reactions - Get topics notes, Online test, Video lectures, Doubts and Solutions for CBSE Class 11-science on TopperLearning. equations chemistry by oxidation number method for class 11, In Uses of hydrofluoric acid with health effect. There are two ways of balancing Redox reactions: Oxidation number method; Half equation method; Oxidation method: The steps to be followed-Write the skeletal equation of reactants and products. in the reaction also need to be multiplied by the appropriate number. Before solving the questions let us understand what redox reaction is. Dismiss, 01.05 Properties of Matter and their Measurement, 1.05 Properties of Matter and their Measurement, 01.06 The International System of Units (SI Units), 01.08 Uncertainty in Measurement: Scientific Notation, 1.08 Uncertainty in Measurement: Scientific Notation, 01.09 Arithmetic Operations using Scientific Notation, 1.09 Arithmetic Operations Using Scientific Notation, 01.12 Arithmetic Operations of Significant Figures, 1.12 Arithmetic Operations of Significant Figures, 01.17 Atomic Mass and Average Atomic Mass, 02.06 Atomic Models: Thomson Model of Atom, 2.06 Atomic Models: Thomson Model of Atom, 02.11 Atomic Number and Mass Number: Numericals, 2.11 Atomic Number and Mass Number: Numericals, 02.14 Wave Motion and Properties: Numericals, 2.14 Wave Motion and Properties: Numericals, 02.15 Wave Theory of Electromagnetic Radiations, 2.15 Wave Theory of Electromagnetic Radiations, 02.17 Wave Theory Reasoning on Interference and Diffraction, 2.17 Wave Theory Reasoning on Interference and Diffraction, 02.18 Planck’s Quantum Theory of Radiation, 2.18 Planck’s Quantum Theory of Radiation, 02.19 Wave Theory and Photoelectric effect, 2.19 Wave Theory and Photoelectric Effect, 02.20 Planck’s Quantum Theory and Photoelectric Effect, 2.20 Planck’s Quantum Theory and Photoelectric Effect, 03 Classification of Elements and Periodicity in Properties, 03.01 Why do we need to classify elements, 03.02 Genesis of Periodic classification – I, 3.02 Genesis of Periodic Classification - I, 03.03 Genesis of Periodic classification – II, 3.03 Genesis of Periodic Classification - II, 03.04 Modern Periodic Law and Present Form of Periodic Table, 3.04 Modern Periodic Law and Present Form of Periodic Table, 03.05 Nomenclature of Elements with Atomic Numbers > 100, 3.05 Nomenclature of Elements with Atomic Numbers > 100, 03.06 Electronic Configurations of Elements and the Periodic Table – I, 3.06 Electronic Configurations of Elements and the Periodic Table - I, 03.07 Electronic Configurations of Elements and the Periodic Table – II, 3.07 Electronic Configurations of Elements and the Periodic Table - II, 03.08 Electronic Configurations and Types of Elements: s-block – I, 3.08 Electronic Configurations and Types of Elements - s-block - I, 03.09 Electronic Configurations and Types of Elements: p-blocks – II, 3.09 Electronic Configurations and Types of Elements - p-blocks - II, 03.10 Electronic Configurations and Types of Elements: Exceptions in periodic table – III, 3.10 Electronic Configurations and Types of Elements - Exceptions in Periodic Table - III, 03.11 Electronic Configurations and Types of Elements: d-block – IV, 3.11 Electronic Configurations and Types of Elements - d-block - IV, 03.12 Electronic Configurations and Types of Elements: f-block – V, 3.12 Electronic Configurations and Types of Elements - f-block - V, 03.18 Factors affecting Ionization Enthalpy, 3.18 Factors Affecting Ionization Enthalpy, 03.20 Trends in Ionization Enthalpy – II, 04 Chemical Bonding and Molecular Structure, 04.01 Kossel-Lewis approach to Chemical Bonding, 4.01 Kössel-Lewis Approach to Chemical Bonding, 04.03 The Lewis Structures and Formal Charge, 4.03 The Lewis Structures and Formal Charge, 04.06 Bond Length, Bond Angle and Bond Order, 4.06 Bond Length, Bond Angle and Bond Order, 04.10 The Valence Shell Electron Pair Repulsion (VSEPR) Theory, 4.10 The Valence Shell Electron Pair Repulsion (VSEPR) Theory, 04.12 Types of Overlapping and Nature of Covalent Bonds, 4.12 Types of Overlapping and Nature of Covalent Bonds, 04.17 Formation of Molecular Orbitals (LCAO Method), 4.17 Formation of Molecular Orbitals (LCAO Method), 04.18 Types of Molecular Orbitals and Energy Level Diagram, 4.18 Types of Molecular Orbitals and Energy Level Diagram, 04.19 Electronic Configuration and Molecular Behavior, 4.19 Electronic Configuration and Molecular Behaviour, Chapter 4 Chemical Bonding and Molecular Structure - Test, 05.02 Dipole-Dipole Forces And Hydrogen Bond, 5.02 Dipole-Dipole Forces and Hydrogen Bond, 05.03 Dipole-Induced Dipole Forces and Repulsive Intermolecular Forces, 5.03 Dipole-Induced Dipole Forces and Repulsive Intermolecular Forces, 05.04 Thermal Interaction and Intermolecular Forces, 5.04 Thermal Interaction and Intermolecular Forces, 05.08 The Gas Laws : Gay Lussac’s Law and Avogadro’s Law, 5.08 The Gas Laws - Gay Lussac’s Law and Avogadro’s Law, 05.10 Dalton’s Law of Partial Pressure – I, 05.12 Deviation of Real Gases from Ideal Gas Behaviour, 5.12 Deviation of Real Gases from Ideal Gas Behaviour, 05.13 Pressure -Volume Correction and Compressibility Factor, 5.13 Pressure - Volume Correction and Compressibility Factor, 06.02 Internal Energy as a State Function – I, 6.02 Internal Energy as a State Function - I, 06.03 Internal Energy as a State Function – II, 6.03 Internal Energy as a State Function - II, 06.06 Extensive and Intensive properties, Heat Capacity and their Relations, 6.06 Extensive and Intensive Properties, Heat Capacity and their Relations, 06.07 Measurement of ΔU and ΔH : Calorimetry, 6.07 Measurement of ΔU and ΔH - Calorimetry, 06.08 Enthalpy change, ΔrH of Reaction – I, 6.08 Enthalpy change, ΔrH of Reaction - I, 06.09 Enthalpy change, ΔrH of Reaction – II, 6.09 Enthalpy Change, ΔrH of Reaction - II, 06.10 Enthalpy change, ΔrH of Reaction – III, 6.10 Enthalpy Change, ΔrH of Reaction - III.

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