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      Class 11 CHEMISTRY – JEE

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      • Chemistry
      • Class 11 CHEMISTRY – JEE
      CoursesClass 11ChemistryClass 11 CHEMISTRY – JEE
      • 1. Stoichiometry 1
        13
        • Lecture1.1
          Introduction & POAC 30 min
        • Lecture1.2
          Mole Stoichiometric relationship 29 min
        • Lecture1.3
          Successive reaction & Limiting reagent 25 min
        • Lecture1.4
          Gas Stoichiometry 29 min
        • Lecture1.5
          Important Types of Reactions 25 min
        • Lecture1.6
          Avogadro’s No.1 30 min
        • Lecture1.7
          Mole & Number 28 min
        • Lecture1.8
          Atomic, Molecular Wt 26 min
        • Lecture1.9
          Ionic wt, Avg. At. Wt. 15 min
        • Lecture1.10
          Molar wt. 27 min
        • Lecture1.11
          Molar Volume & Gas Analysis 30 min
        • Lecture1.12
          Gas Analysis 17 min
        • Lecture1.13
          Empirical Formula Determination 26 min
      • 2. Stoichiometry 2
        18
        • Lecture2.1
          Acid Base definition 23 min
        • Lecture2.2
          Acidity & Basicity 32 min
        • Lecture2.3
          Acidic Strength 30 min
        • Lecture2.4
          Acidic Strength 23 min
        • Lecture2.5
          Conjugate Acid-Base pair, Basic Strength 48 min
        • Lecture2.6
          Oxidation & Reduction 50 min
        • Lecture2.7
          Calculation of Oxidation Number 46 min
        • Lecture2.8
          O.A. & R.A., Balancing by Oxidation Number Method 01 hour
        • Lecture2.9
          Balancing by Ion Electron Method. 35 min
        • Lecture2.10
          Eq. Wt. 1 – n factor & Eq. Wt. Concept 47 min
        • Lecture2.11
          Eq. Wt. 2 – Eq. Concept 35 min
        • Lecture2.12
          Volumetric Analysis 43 min
        • Lecture2.13
          Volumetric analysis 44 min
        • Lecture2.14
          Titration – Acid Base Titration 49 min
        • Lecture2.15
          Titration – Acid Base Titration, Indicator 56 min
        • Lecture2.16
          Titration – Redox Titration-8 58 min
        • Lecture2.17
          Titration – Redox Titration, volume Strength of H2O2 50 min
        • Lecture2.18
          Titration – Redox Titration, Iodometry, Oleum, Bleaching Powder 49 min
      • 3. Thermodynamics & Thermochemistry
        19
        • Lecture3.1
          Zeroth Law 55 min
        • Lecture3.2
          1st law – System, Properties, State 40 min
        • Lecture3.3
          1st Law, Process, Internal energy, Work 43 min
        • Lecture3.4
          Work done in Irreversible process, Isobaric Process 49 min
        • Lecture3.5
          Isochoric Process & problems TD 42 min
        • Lecture3.6
          Isothermal irreversible Process, Problems on TD 46 min
        • Lecture3.7
          Adiabatic Process 49 min
        • Lecture3.8
          Problems on TD 44 min
        • Lecture3.9
          Thermochemistry & Enthalpy 38 min
        • Lecture3.10
          Hess’s Law, Kirchhoff’s Law 43 min
        • Lecture3.11
          Enthalpy of Formation, combustion 39 min
        • Lecture3.12
          Enthalpy of Hydrogenation, Hydration, dissolution, lattice energy 40 min
        • Lecture3.13
          Enthapy of Neutralisation, atomisation, Bond Energy 47 min
        • Lecture3.14
          Resonance energy & problems 45 min
        • Lecture3.15
          2nd Law, Entropy-positional 40 min
        • Lecture3.16
          TD Entropy, 3rd Law, Entropy change in a reaction 45 min
        • Lecture3.17
          Gibb’s free energy 43 min
        • Lecture3.18
          Efficiency, engine, pump & Carnot engine 39 min
        • Lecture3.19
          Chapter Notes – Thermodynamics & Thermochemistry
      • 4. Atomic Structure
        22
        • Lecture4.1
          Introduction, Cathode rays & Anode rays 41 min
        • Lecture4.2
          J.J. Thomson Model, Millikan Oil Drop Experiment 38 min
        • Lecture4.3
          Rutherford Experiment 51 min
        • Lecture4.4
          Quantum Mechanics, BlackBody Radiation Experiment 41 min
        • Lecture4.5
          Wave 44 min
        • Lecture4.6
          Photoelectric Effect 46 min
        • Lecture4.7
          Problems on Photoelectric Effect 35 min
        • Lecture4.8
          Atomic Structure 44 min
        • Lecture4.9
          Bohr Theory 47 min
        • Lecture4.10
          H – Spectrum 49 min
        • Lecture4.11
          Problems on Bohr’s Theory 40 min
        • Lecture4.12
          Adv. Problems on Bohr Theory & Sommerfeld model 51 min
        • Lecture4.13
          Quantum Mechanical Model for Atomic Structure 47 min
        • Lecture4.14
          Schrodinger wave equation 54 min
        • Lecture4.15
          No. of Orbitals & Quantum no 45 min
        • Lecture4.16
          Orbital Curve, RPD curve, Definition of Node 46 min
        • Lecture4.17
          Calculation of Node, Orbital Picture 43 min
        • Lecture4.18
          Radial Probability curve, MPD, Avg. distance, Screening effect, Zeff 38 min
        • Lecture4.19
          Multielectron system, Electronic configuration 56 min
        • Lecture4.20
          Stability of Elec. Configuration 36 min
        • Lecture4.21
          Chapter Notes – Atomic Structure
        • Lecture4.22
          NCERT Solutions – Atomic Structure
      • 5. Chemical equilibrium
        9
        • Lecture5.1
          Introduction, Eqb constant & Eqb Position 51 min
        • Lecture5.2
          Types of Eqb Constant, Heterogeneous Eqb, Reaction Quotient 45 min
        • Lecture5.3
          Range of Eqb Constant 43 min
        • Lecture5.4
          Problems on Chemical Eqb 41 min
        • Lecture5.5
          Problems on Chemical Eqb 42 min
        • Lecture5.6
          Le-chatelier Principle 42 min
        • Lecture5.7
          Le-Chatelier Principle 35 min
        • Lecture5.8
          Eqb & 2nd Law of TD 26 min
        • Lecture5.9
          NCERT Solutions – equilibrium
      • 6. Ionic Equilibrium
        17
        • Lecture6.1
          Electrolyte, Dissociation of H2O, Nature of Solution 46 min
        • Lecture6.2
          PH scale, Log & Antilog 40 min
        • Lecture6.3
          PH of Strong Acid, Base Solution 51 min
        • Lecture6.4
          PH of Weak Acid, Base solution 41 min
        • Lecture6.5
          PH of mixture of Acids, Bases 46 min
        • Lecture6.6
          PH of Polybasic acids 40 min
        • Lecture6.7
          PH of Salt Solution 1 43 min
        • Lecture6.8
          PH of salt solution 2 52 min
        • Lecture6.9
          Common ion effect, Buffer solution 49 min
        • Lecture6.10
          Buffer Capacity 45 min
        • Lecture6.11
          Titration & PH Curve 1 40 min
        • Lecture6.12
          Titration & PH curve 2 46 min
        • Lecture6.13
          Acid Base indicator 35 min
        • Lecture6.14
          Solubility Equilibrium 47 min
        • Lecture6.15
          Precipitation of Solid, Qualitative analysis of cation 44 min
        • Lecture6.16
          Complex ion equilibrium 23 min
        • Lecture6.17
          Chapter Notes – Equilibrium
      • 7. Introduction & Development of Org. Chemistry
        3
        • Lecture7.1
          Introduction & Development Of Organic Chemistry 44 min
        • Lecture7.2
          Introduction & Syllabus 36 min
        • Lecture7.3
          NCERT Solutions – Org. Chemistry
      • 8. Nomenclature of Org. Compounds
        16
        • Lecture8.1
          Alkane 59 min
        • Lecture8.2
          Alkane 31 min
        • Lecture8.3
          Alkyl Group & Types Of Hydrogen 01 hour
        • Lecture8.4
          Alkene 54 min
        • Lecture8.5
          Alkenyl 32 min
        • Lecture8.6
          Alkyne & Alkenyl 47 min
        • Lecture8.7
          Cycloalkane 43 min
        • Lecture8.8
          Cycloalkene 35 min
        • Lecture8.9
          Bicycloalkane & Spirane 35 min
        • Lecture8.10
          Acid & Aldehyde 45 min
        • Lecture8.11
          Ester & Acid Halides 28 min
        • Lecture8.12
          Amide & Nitrile 28 min
        • Lecture8.13
          Alcohol & Sulphonic Acid 37 min
        • Lecture8.14
          Isonitrile, Amine, Nitroalkane, Halo Compounds 39 min
        • Lecture8.15
          Ketone, Anhydride & Ether 34 min
        • Lecture8.16
          Polyfunctional Group Compounds 41 min
      • 9. GOC 1- Hybridisation, Resonance, Aromaticity
        16
        • Lecture9.1
          Concept Of Hybridisation 42 min
        • Lecture9.2
          Sp3, Sp2 Hybridisation 44 min
        • Lecture9.3
          Sp Hybridisation, Relative Study Of Sp3, Sp2, Sp Orbitals 46 min
        • Lecture9.4
          Effect Of Hybridisation On Bond Length, Planar Nature 59 min
        • Lecture9.5
          Concept Of Resonance 39 min
        • Lecture9.6
          Doing Resonance 18 min
        • Lecture9.7
          Resonance Hybrid, Cannonical St. , Resonance Energy 44 min
        • Lecture9.8
          Condition Of Resonance 40 min
        • Lecture9.9
          Writing Cannonical St. 39 min
        • Lecture9.10
          Relative Stability Of Cannonical St. 37 min
        • Lecture9.11
          Resonance Energy 45 min
        • Lecture9.12
          Effect Of Resonance On Bond Length, Enthalpy Of Hydrogenation 43 min
        • Lecture9.13
          Introduction To Aromaticity 43 min
        • Lecture9.14
          Introduction To Aromaticity 39 min
        • Lecture9.15
          Unsaturation Factor 31 min
        • Lecture9.16
          Chapter Notes – GOC General Organic chemistry
      • 10. GOC 2 - Substituent effect
        5
        • Lecture10.1
          Substituent Effect, Hyperconjugation 48 min
        • Lecture10.2
          Substituent Effect, Hyperconjugation 43 min
        • Lecture10.3
          Substituent Effect, Mesomeric Effect 47 min
        • Lecture10.4
          Substituent Effect, Inductive Effect 46 min
        • Lecture10.5
          Substituent Effect, Electromeric Effect, Staric Effect, Relative M & I Effect 41 min
      • 11. GOC 2 - Reactive Intermediate
        6
        • Lecture11.1
          Reactive Intermediate, Carbocation 45 min
        • Lecture11.2
          Reactive Intermediate, Carbocation, Carbonium Ion Rearrangement 42 min
        • Lecture11.3
          Reactive Intermediate, Carbonium Ion Rearrangement 41 min
        • Lecture11.4
          Reactive Intermediate, Carbanion 36 min
        • Lecture11.5
          Reactive Intermediate, Free Radical 47 min
        • Lecture11.6
          Reactive Intermediate, Carbene & Nitrene 42 min
      • 12. GOC 2 - Acid, base, Electrophile, Nucleophile
        3
        • Lecture12.1
          Acid Base, Electrophile Nucleophile 50 min
        • Lecture12.2
          Acid Base, Electrophile Nucleophile 47 min
        • Lecture12.3
          Hard Acid Base, Electrophilic Nucleophilic Strength 40 min
      • 13. Isomerism
        20
        • Lecture13.1
          Structural Isomers 39 min
        • Lecture13.2
          Tautomerism 37 min
        • Lecture13.3
          Stability Of Tautomers 43 min
        • Lecture13.4
          Factors Affecting Stability, Catalysis In Tautomerism 39 min
        • Lecture13.5
          Geometrical Isomerism 41 min
        • Lecture13.6
          E-z Nomenclature, Properties Of G.i. 43 min
        • Lecture13.7
          No. Of G.i., Interconversion Of G.i. 48 min
        • Lecture13.8
          Optical Isomerism & Its Conditions 50 min
        • Lecture13.9
          Different Types Of Projections, R-s Configuration 57 min
        • Lecture13.10
          Relationship Between Optical Isomers 45 min
        • Lecture13.11
          Dissymmetry In A Molecule 44 min
        • Lecture13.12
          Enantiomers, Mesomers, Diastereomers 39 min
        • Lecture13.13
          Special Case Of Optical Isomerism 47 min
        • Lecture13.14
          No. Of Optical Isomers, Stereoisomers 45 min
        • Lecture13.15
          D,l Configuration, Retention & Inversion 36 min
        • Lecture13.16
          Measurement Of Optical Activity 45 min
        • Lecture13.17
          No. Of Isomers 35 min
        • Lecture13.18
          Resolution Of Optical Isomers, Syn, Anti Addition, Elimination. 28 min
        • Lecture13.19
          Conformational Isomers 51 min
        • Lecture13.20
          Conformers Of Propane, Butane, Cyclohexane & Problems 44 min
      • 14. Reaction Mechanism
        21
        • Lecture14.1
          Introduction, Types Of Organic Reactions 35 min
        • Lecture14.2
          Nucleophilic Substitution Reaction 40 min
        • Lecture14.3
          Sn1 & Sn2 Reaction, Sni Pathway 53 min
        • Lecture14.4
          Reactivity In Sn1 & Sn2 Path 42 min
        • Lecture14.5
          Reactivity In Sn1 & Sn2 Path 36 min
        • Lecture14.6
          Reactivity In Sn1 & Sn2 Path 30 min
        • Lecture14.7
          Reactivity In Sn1 & Sn2 Path 41 min
        • Lecture14.8
          Elimination Reaction 53 min
        • Lecture14.9
          E1 & E2 Reaction, Isotopic Effect 46 min
        • Lecture14.10
          Orientation In Elimination Reaction 45 min
        • Lecture14.11
          Problems On Elimination Reaction 48 min
        • Lecture14.12
          Elimination Vs Substitution 34 min
        • Lecture14.13
          Addition Reaction 51 min
        • Lecture14.14
          Problems On Addition Reaction 46 min
        • Lecture14.15
          Electrophilic Aromatic Substitution Reaction 49 min
        • Lecture14.16
          Orientation In Electrophilic Aromatic Substitution 53 min
        • Lecture14.17
          Reactivity In Electrophilic Aromatic Substitution Reaction 30 min
        • Lecture14.18
          Examples Of Electrophilic Aromatic Substitution Reaction 37 min
        • Lecture14.19
          Examples Of Electrophilic Aromatic Substitution Reaction 37 min
        • Lecture14.20
          Nucleophilic Aromatic Substitution 44 min
        • Lecture14.21
          Benzyne Pathway 27 min
      • 15. Alkane
        7
        • Lecture15.1
          Alkane Preparation 49 min
        • Lecture15.2
          Alkane Preparation & Selective Hydrogenation 31 min
        • Lecture15.3
          Alkane Preparation 40 min
        • Lecture15.4
          Alkane Preparation 38 min
        • Lecture15.5
          Alkane Preparation 32 min
        • Lecture15.6
          Alkane Properties 55 min
        • Lecture15.7
          Alkane Properties & Problems 39 min
      • 16. Alkene
        7
        • Lecture16.1
          Alkene Preparation 45 min
        • Lecture16.2
          Alkene Preparation 36 min
        • Lecture16.3
          Alkene Properties 53 min
        • Lecture16.4
          Alkene Properties 40 min
        • Lecture16.5
          Alkene Properties 42 min
        • Lecture16.6
          Alkene Properties & Ozonolysis 41 min
        • Lecture16.7
          Alkene Properties, Oxidation, Substitution 38 min
      • 17. Alkyl Halides
        4
        • Lecture17.1
          Preparation 38 min
        • Lecture17.2
          Properties 49 min
        • Lecture17.3
          Haloform Reaction 28 min
        • Lecture17.4
          Grignard Reagent 29 min
      • 18. Chemical Bonding
        32
        • Lecture18.1
          Introduction, definition, Concept & Type of Bonding 53 min
        • Lecture18.2
          Ionic Bonding, covalent bonding 50 min
        • Lecture18.3
          Ionic Character in Covalent Bonding, Electronegativity 34 min
        • Lecture18.4
          Dipole Moment 42 min
        • Lecture18.5
          Fajan’s Rule 34 min
        • Lecture18.6
          Model for Covalent Compound, V.B.T. – Lewis St. Model 56 min
        • Lecture18.7
          Lewis Structure Model 45 min
        • Lecture18.8
          Formal Charge 46 min
        • Lecture18.9
          Formal Charge Rule 44 min
        • Lecture18.10
          Resonance 43 min
        • Lecture18.11
          Merits & Demerits of Lewis St. Model 44 min
        • Lecture18.12
          Drawing Lewis St. 30 min
        • Lecture18.13
          VSEPR 1 49 min
        • Lecture18.14
          VSEPR 2 51 min
        • Lecture18.15
          VSEPR 3 51 min
        • Lecture18.16
          VSEPR 4 33 min
        • Lecture18.17
          BackBonding 38 min
        • Lecture18.18
          Bond Angle determination 47 min
        • Lecture18.19
          Concept of Hybridisation 44 min
        • Lecture18.20
          Sp3, Sp2 Hybridisation 44 min
        • Lecture18.21
          SP hybridisation, Relative study of SP, SP2, SP3 Hybridisation 46 min
        • Lecture18.22
          Hybridsation involving D-orbitals 39 min
        • Lecture18.23
          Hybridsation with D-orbitals, Limitation of Hybridisation 41 min
        • Lecture18.24
          Calculation of Hybridisation of Central Atom, Problems 43 min
        • Lecture18.25
          Merits & demerits of VBT, Introduction to MOT 33 min
        • Lecture18.26
          MO formation, Bond Order 43 min
        • Lecture18.27
          MO with P-orbitals, B2, Magnetic Character 43 min
        • Lecture18.28
          MO of Diatomic Species, Hetroatomic Species 51 min
        • Lecture18.29
          Secondary Bondings 39 min
        • Lecture18.30
          H Bonding 37 min
        • Lecture18.31
          Metallic Bonding 52 min
        • Lecture18.32
          Chapter Notes – Chemical Bonding
      • 19. Periodic Table
        10
        • Lecture19.1
          Development of P.T. 43 min
        • Lecture19.2
          Mandeelev P.T. & Mosley, Modern P.T. 43 min
        • Lecture19.3
          Modern P.T. & Periodic Properties 27 min
        • Lecture19.4
          Atomic Volume & Radius 49 min
        • Lecture19.5
          Atomic Radius, Ionisation Energy 28 min
        • Lecture19.6
          Ionisation Energy 48 min
        • Lecture19.7
          Electron Affinity, Hydration Energy 52 min
        • Lecture19.8
          Electronegativity, Lattice Energy 46 min
        • Lecture19.9
          Oxidising & Reducing Power, Nature of oxides 38 min
        • Lecture19.10
          M.P. & B.P., Density, Bond Energy, Diagonal relationship, Inert Pair Effect 25 min
      • 20. Metallurgy
        7
        • Lecture20.1
          Introduction, Concentration of ore 49 min
        • Lecture20.2
          Roasting, Calcination, smelting 41 min
        • Lecture20.3
          Refining of metal 29 min
        • Lecture20.4
          Pyrometallurgy, electrometallurgy, Hydrometallurgy 32 min
        • Lecture20.5
          Ellingham Diagram 43 min
        • Lecture20.6
          Extraction of Cu & Fe 22 min
        • Lecture20.7
          Extraction of Al & Zn 26 min
      • 21. Hydrogen and its Compounds
        7
        • Lecture21.1
          preparation, properties & Type of Hydrogen 57 min
        • Lecture21.2
          Compounds of Hydrogen, Hydrides, Water, Hydrates 56 min
        • Lecture21.3
          Hardness of Water, H2O2 56 min
        • Lecture21.4
          Problems 48 min
        • Lecture21.5
          Problems 28 min
        • Lecture21.6
          Chapter Notes – Hydrogen and its Compounds
        • Lecture21.7
          NCERT Solutions – Hydrogen
      • 22. S block metals
        8
        • Lecture22.1
          IA 1 – elemental Properties of Alkali metals& its Compounds 57 min
        • Lecture22.2
          IA 2 – Na & its compounds 01 hour
        • Lecture22.3
          IA 3 – Na & its Compounds, Use of Na & K 27 min
        • Lecture22.4
          IIA 1 – Elemental Properties 41 min
        • Lecture22.5
          IIA 2 – Compounds of IIA Metals 53 min
        • Lecture22.6
          IIA 3 – Compounds of Ca 48 min
        • Lecture22.7
          Chapter Notes – S block metals
        • Lecture22.8
          NCERT Solutions – S block metals
      • 23. p block elements
        8
        • Lecture23.1
          Introduction to P – Block & IIIA – elemental properties 51 min
        • Lecture23.2
          IIIA – General properties of compounds & B-compounds 40 min
        • Lecture23.3
          IIIA – Boron compounds, Use of B and Al 35 min
        • Lecture23.4
          IVA – Elemental Properties of C family 46 min
        • Lecture23.5
          IVA – Allotropes of C & compounds of C 01 hour
        • Lecture23.6
          IVA – Compounds of Si 48 min
        • Lecture23.7
          Chapter Notes – p block elements
        • Lecture23.8
          NCERT Solutions – p block elements

        NCERT Solutions – Hydrogen

        9.1. Justify the position of hydrogen in the periodic table on the basis of its electronic configuration.

        Answer:

        Hydrogen has been placed at the top of the alkali metal in group, but it is not a member of the group.

        Its position is not justified properly because of its electronic configuration as (1s1). It can be placed with alkali metals because it also has similar configuration (ns1) as alkali metals.
        However, it can also be placed along with halogen in group 17 since just like halogen it can acquire inert gas configuration by accepting one electron.

        9.2. Write the names of isotopes of hydrogen. What is the mass ratio of these isotopes?

        Answer:

        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-1

         

        9.3. Why does hydrogen occur in a diatomic form rather than in a monoatomic form under normal conditions?

        Answer:

        In diatomic form, the K-shell of hydrogen is complete (1s2) and so it is quite stable.

        9.4. How can the production of dihydrogen obtained from ‘Coal gasification’ be increased?

        Answer:

        The production of dihydrogen in coal gasification can be increased by reacting CO(y) present in syngas with steam in the presence of iron chromate catalysts.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-2
        With the removal of C02 the reaction shifts in the forward direction and thus, the production of dihydrogen will be increased.

        9.5. Describe the bulk preparation of dihydrogen by electrolytic method. What is the role of an electrolyte in this process?

        Answer:

        In bulk, hydrogen can be produced by electrolysis of acidified water using Pt electrodes.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-3
        Electrolyte is added to increase the dissociation of water.

        9.6. Complete the following reactions.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-4

        Answer:

        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-5

        9.7. Discuss the consequences of high enthalpy of H-H bond, in terms of chemical reactivity of dihydrogen.

        Answer: 

        This is due to its small atomic size and also small bond length (74 pm) of H-H bond.

        9.8. What do you understand by (i) Electron-deficient (ii) Electron-precise (iii) Electron-rich compounds of hydrogen? Provide justification with suitable examples.

        Answer: 

        (i) Electron deficient hydrides: Compounds in which central atom has incomplete octet, are called electron deficient hydrides. For example, BeH2, BH3 are electron deficient hydrides.
        (ii) Electron precise hydrides: Those compounds in which exact number of electrons are present in central atom or the central atom contains complete octet are called precise hydrides e.g., CH4, SiH4, GeH4 etc. are precise hydrides.
        (iii) Electron rich hydrides: Those compounds in which central atom has one or more lone pair of excess electrons are called electron rich hydrides, e.g.,NH3, H2O.

        9.9. What characteristics do you expect from an electron-deficient hydride with respect to its structure and chemical reaction?

        Answer:

        It is expected to be a Lewis acid. They are likely to accept electrons to become stable. They can form coordinate bond with electron rich compound.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-6

        9.10. Do you expect the carbon hydride of type Cn H2n+2 to act as ‘Lewis’ acid or base? Justify your answer.

        Answer:

        Carbon hydrides of the type Cn H2n+2 are electron precise hydrides. Because they have atom with exact number of electrons to form covalent bonds. Thus, they do not behave as Lewis acid or base. Since they have no tendency to accept or lose electrons.

        9.11. What do you understand by the term ‘non-stoichiometric hydrides’? Do you expect this type of hydrides to be formed by alkali metals? Justify your answer.

        Answer:

        Those hydrides which do not have fix composition are called non-stoichiometric hydrides, and the composition varies with temperature and pressure. This type of hydrides are formed by d and /block elements. They cannot be formed by alkali metals because alkali metal hydrides form ionic hydrides.

        9.12. How do you expect the metallic hydrides to be useful for hydrogen storage? Explain.

        Answer:

        In metallic hydrides, hydrogen is adsorbed as H-atoms. Due to the adsorption of H atoms the metal Lattice expands and become unstable. Thus, when metallic hydride is heated, it decomposes to form hydrogen and finely divided metal. The hydrogen evolved can be used as fuel.

        9.13. How does the atomic hydrogen or oxy-hydrogen torch function for cutting and welding purposes ? Explain.

        Answer:

        When hydrogen is burnt in oxygen the reaction is highly exothermic, it produces very high temperature nearly 4000°C which is used for cutting and welding purposes.

        9.14.  Among NH3 H2O and HE, which would you expect to have highest magnitude of hydrogen bonding and why?

        Answer:

        HF is expected to have highest magnitude of hydrogen bonding since, ‘F’ is most electronegative. Therefore, HF is the most polar.

        9.15. Saline hydrides are known to react with water violently producing fire. Can C02, a well known fire extinguisher, be used in this case? Explain.

        Answer:

        No. Because if saline hydrides react with water the reaction will be highly exothermic thus the hydrogen evolved in this case can catch fire. C02 cannot be used as fire extinguisher because C02 will get absorbed in alkali metal hydroxides.

        9.16. Arrange the following:
        (i) CaH2, BeH2 and TiH2 in order of increasing electrical conductance.
        (ii) LiH, NaH and CsH in order of increasing ionic character.
        (iii) H-H, D—D and F—F in order of increasing bond dissociation enthalpy.
        (iv) NaH, MgH2 and H2O in order of increasing reducing property.

        Answer:

        (i) BeH2< TiH2 < CaH2
        (ii) LiH < NaH < CsH
        (iii) F—F < H—H < D—D
        (iv) H2O < MgH2 < NaH

        9.17. Compare the structures of H2O and H2O2

        Answer:

        In water, O is sp3 hybridized. Due to stronger lone pair-lone pair repulsions than bond pair-bond pair repulsions, the HOH bond angle decreases from 109.5° to 104.5°. Thus water molecule has a bent structure.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-7
        H2O2 has a non-planar structure. The O—H bonds are in different planes. Thus, the structure of H2O2 is like an open book.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-8

        9.18. What do you understand by the term ‘auto-protolysis’ of water? what is its significance?

        Answer: 

        Auto-protolysis means self-ionisation of water. It may be represented as
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-9
        Due to auto-protalysis water is amphoteric in nature, i.e., it can act as an acid as well as base.

        9.19. Consider the reaction of water with F2 and suggest, in terms of oxidation and reduction, which species are oxidised/reduced ?

        Answer:  

        2F2(ag) + 2H20(l)—————> O2(g) + 4H+(aq) + 4F(aq)
        In this reaction water acts as a reducing agent and itself gets oxidised to O2 while F2 acts as an oxidising agent and hence itself reduced to F– ions.

        9.20. Complete the following chemical reactions.
        (i) PbS(s) + H2O2 (aq) ————->
        (ii) MnO4– (aq) + H2O2 (aq) ————->
        (iii) CaO(s) + H2O(g) ————->
        (iv) AlCl3(g) + H2O(l)————->
        (v) Ca3N2(S) + H2O(l) ————->
        Classify the above into (a) hydrolysis, (b) redox and (c) hydration reactions.

        Answer:

        (i) PbS(s) +4H2O2(aq) ————-> PbSO4(s) + 4H2O(l)
        (ii) 2MnO4– (aq) +H2O2(aq) + 6H+(aq) ————-> 2Mn (aq) + 8H2O(l) + 5O2(g)
        (iii) CaO(s) + H2O(g) ————->Ca(OH)2(aq)
        (iv) AlCl3(aq) + 3H2O(l) ————-> Al(OH)3(S) + 3HCl (aq)
        (v) Ca3N2(s) + H2O(l) ————->3Ca(OH)2(aq) + 2NH3(aq)
        (a) Hydrolysis reactions, (iii) (iv) and (v)
        (b) Redox reactions (i) and (ii)

        9.21. Describe the structure of common form of ice.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-10

        Answer: 

        Ice crystallizes in the normal hexagonal form. However, at very low temperatures it condenses in cubic form. In the normal hexagonal ice each oxygen atom is tetrahedrally surrounded by four other hydrogen atoms.

        9.22. What causes the temporary and permanent hardness of water?

        Answer:

        Temporary hardness of water is due to the presence of bicarbonates of calcium and magnesium in water i.e., Ca(HCO3)2 and Mg(HCO3) in water. Permanent hardness of water is due to the presence of soluble chlorides and sulphates of calcium and magnesium i.e., CaCl2, CaS04, MgCl2 and MgS04.

        9.23. Discuss the principle and method of softening of hard water by synthetic ion-exchange resins.

        Answer:

        Cation exchange resins have large organic molecule with S03H group which are insoluble in water. Ion exchange resin (RS03H) is changed to RNa on treatment with NaCl. The resin exchange Na+ ions with Ca2+ and Mg2+ ions present in hard water and make it soft.
        2RNa(s) + M2+(aq) ——> R2M(s) + 2Na+(aq)
        where, M = Mg, Ca.
        The resins can be regenerated by adding aqueous NaCl solution.

        9.24. Write chemical reaction to show the amphoteric nature of water.

        Answer: 

        Water is amphoteric in nature because it acts as an acid
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-11

        9.25. Write chemical reactions to justify that hydrogen peroxide can function as an oxidising as well as reducing agent.

        Answer: 

        As an oxidising agent
        2Fe2+  (aq) + 2H+(aq) +H2O2(aq) ———–> 2Fe3+  (aq) + 2 H2O(l)
        As a reducing agent
        I2(s) + H2O2 (aq) + 2OH– (aq) ———> 2I– (aq) + 2 H2O(l) + O2(g)

        9.26. What is meant by ‘demineralised water’ and how can it be obtained?

        Answer: 

        Demineralised water is free from all soluble mineral salts which is obtained by passing water successively through a cation exchange (in the form of H+) and an anion exchange in the form of OH– resins.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-12
        H+ exchanges for Na+, Ca2+, Mg2+ and other cations present in water. This process results in release of proton which makes the water acidic.
        OH– exchanges, for anions like Cl–, HCO3–,SO42-etc.
        OH– ions thus liberated neutralize the H+ ions set free in the cation exchange process. H+(aq) + OH–(aq) ——-> H2O(l)

        9.27. Is demineralised or distilled water useful for drinking purposes? If not, how can it be made useful ?

        Answer: 

        No, demineralised water is not fit for drinking purposes. It can be made useful by adding required amount of ions which are useful for our body.

        9.28. Describe the usefulness of water in biosphere and biological systems.

        Answer: 

        (i) Major part of all living system is made of water.
        (ii) It constitutes about 65 – 70% of body weights of animals and plants.
        (iii) Some properties of water like high specific heat, thermal conductivity, surface tension, high polarity allow water to play a major role in biosphere.
        (iv) Because of high heat of vaporisation it is responsible ro regulate temperature of living beings.
        (v) It is an excellent fluid for the transportation of minerals and nutrients in plants.
        (vi) It is also required for photosynthesis in plants.

        9.29. What properties of water make it useful as a solvent? What types of compound can it (i) dissolve (ii) hydrolyse?

        Answer: 

        Water is highly polar in nature thats why it has high dielectric constant and high dipole moment. Because of these properties, water is a universal solvent.
        It can hydrolyse many oxides metallic or non-metallic, hydrides, carbides, nitrides etc.

        9.30. Knowing the properties of H2O and D2O, do you think D2O can be used for drinking purpose.

        Answer: 

        No, D2O is injurious to human beings, plants and animals.

        9.31. What is the difference between the terms ‘hydrolysis’ and ‘hydration’?

        Answer: 

        Hydrolysis is a chemical reaction in which a substance reacts with water under neutral, acidic or alkaline conditions.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-14

        9.32. How can saline hydrides remove traces of water from organic compounds?

        Answer: 

        Saline hydrides (i.e, CaH2 NaH etc.) react with water and form the corresponding metal hydroxide with the liberation of H2 gas. Thus, these hydrides can be used to remove traces of water from the organic compounds.
        NaH(s) + H2O(l) ———–> NaOH(aq) + H2(g)
        CaH2(s) + 2H2O(l) ———> Ca(OH)2(aq) + H2(g)

        9.33. What do you expect the nature of hydrides is, if formed by elements of atomic numbers 15,19, 23 and 44 with dihydrogen? Compare their behaviour towards water.

        Answer: 

        Atomic No. 15 is of phosphorus. The hydride is PH3 and its nature is covalent. Atomic No. (Z = 19) is of potassium. The hydride is KH and it is ionic in nature. Atomic No. (Z = 23) is of vanadium. The hydride is VH. It is interstitial or metallic. Atomic No. 44 is of ruthenium, its hydride is interstitial or metallic.

        9.34. Do you expect different products in solution when aluminium (III) chloride and potassium chloride treated separately with (i) normal water (ii) acidified water (iii) alkaline water? Write equation wherever necessary.

        Answer:

        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-15

        9.35. How does H2O2 behave as a bleaching agent?

        Answer: 

        Bleaching action of H2O2 is due to the oxidation of colouring matter by nascent oxygen.
        H2O2(Z) ———> H2O(Z) + O(g)

        9.36. What do you understand by the terms:
        (i) Hydrogen economy (ii) hydrogenation (iii) syngas (iv) water-gas shift reaction (v) fuel-cell?

        Answer: 

        (i) Hydrogen economy: The basic principle of hydrogen economy is the storage and transportation of energy in the form of liquid or gaseous dihydrogen.
        (ii) Hydrogenation: Hydrogenation means addition of hydrogen across double and triple bonds in presence of catalyst to form saturated compounds.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-16
        (iii) Syngas: The mixture of CO and H2 are called synthesis or syngas. It can be produced by the reaction of steam on hydrocarbon or coke at high temperature in the presence of nickel catalyst
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-17
        (iv) Water-gas shift reaction: The amount of hydrogen in the syngas can be increased by the action of CO of syngas mixture with steam in the presence of iron chromate as catalyst.This is called water-gas shift reaction.
        cbse-class-11th-chemistry-solutions-chapter-9-hydrogen-18
        (v) Fuel-Cell: It is a cell which converts chemical energy of fuel directly into electrical energy.

        Prev Chapter Notes – Hydrogen and its Compounds
        Next IA 1 – elemental Properties of Alkali metals& its Compounds

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