AP Inter 1st Year Zoology Study Material Pdf | Intermediate 1st Year Zoology Textbook Solutions

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Intermediate 1st Year Zoology Syllabus

TS AP Inter 1st Year Zoology Syllabus

Unit I Zoology – Diversity of Living World

  • 1.1 What is life?
  • 1.2 Nature, Scope & meaning of zoology
  • 1.3 Branches of Zoology
  • 1.4 Need for classification- Zoos as tools for the study of taxonomy
  • 1.5 Basic principles of Classification: Biological system of classification- (Phylogenetic classification only)
  • 1.6 Levels of Hierarchy of classification
  • 1.7 Nomenclature – Bi & Trinominal
  • 1.8 Species concept
  • 1.9 Kingdom Animalia
  • 1.10 Biodiversity – Meaning and distribution (Genetic diversity, Species diversity, Ecosystem diversity(alpha, beta, and gamma), other attributes of biodiversity, the role of biodiversity, threats to biodiversity, methods of conservation, IUCN Red data books, Conservation of wildlife in India – Legislation, Preservation, Organisations, Threatened species.

Unit II Structural Organization in Animals

  • 2.1 Levels of organization, Multicellularity: Diploblastic & Triploblastic conditions.
  • 2.2 Asymmetry, Symmetry: Radial symmetry, and Bilateral symmetry (Brief account giving one example for each type from the representative phyla)
  • 2.3 Acoelomates, Pseudocoelomates, and Eucoelomates: Schizo & Entero coelomates (Brief account of the formation of coelom)
  • 2.4 Tissues: Epithelial, Connective, Muscular, and Nervous tissues. (make it a little more elaborative)

Unit III Animal Diversity – I: Invertebrate Phyla
General Characters – Strictly restrict to 8 salient features only
Classification up to Classes with two or three examples – Brief account only

  • 3.1 Porifera
  • 3.2 Cnidaria
  • 3.3 Ctenophora
  • 3.4 Platyhelminthes
  • 3.5 Nematoda
  • 3.6 Annelida (Include Earthworm as a type study strictly adhering to NCERT textbook)
  • 3.7 Arthropoda
  • 3.8 Mollusca
  • 3.9 Echinodermata
  • 3.10 Hemichordata

Unit IV Animal Diversity – II: Phylum: Chordata
General Characters – Strictly restrict to 8 points only Classification up to Classes – Brief account only with two or three examples

  • 4.1 Sub phylum: Urochordata
  • 4.2 Sub phylum: Cephalochordata
  • 4.3 Sub phylum: Vertebrata
  • 4.4 Super Class: Agnatha
  • 4.4.1 Class Cyclostomata
  • 4.5 Super Class: Gnathostomata
  • 4.5.1 Super Class: Pisces
  • 4.5.2 Class: Chondrichthyes
  • 4.5.3 Class: Osteichthyes
  • 4.6 Tetrapoda
  • 4.6.1 Class: Amphibia (Include Frog as a type study strictly adhering to NCERT textbook)
  • 4.6.2 Class: Reptilia
  • 4.6.3 Class: Aves
  • 4.6.4 Class: Mammalia

Unit V Locomotion & Reproduction in Protozoa

  • 5.1 Locomotion: Definition, types of locomotor structures pseudopodia (basic idea of pseudopodia without going into different types), flagella & cilia (Brief account giving two examples each)
  • 5.2 Flagellar & Ciliary movement – Effective & Recovery strokes in Euglena, Synchronal & Metachronal movements in Paramecium
  • 5.3 Reproduction: Definition, types. Asexual Reproduction: Transverse binary fission in Paramecium & Longitudinal binary fission in Euglena. Multiple fission, Sexual Reproduction.

Unit VI Biology & Human Welfare

  • 6.1 Parasitism and parasitic adaptation
  • 6.2 Health and disease: introduction (follow NCERT) Life cycle, Pathogenicity, Treatment & Prevention (Brief account only)
    1. Entamoeba histolytica 2. Plasmodium vivax 3. Ascaris lumbricoides 4. Wuchereria bancrofti
  • 6.3 A brief account of pathogenicity, treatment & prevention of Typhoid, Pneumonia, Common cold, & Ringworm.
  • 6.4 Drugs and Alcohol abuse

Unit VII Type study of Periplaneta Americana

  • 7.1 Habitat and habits
  • 7.2 External features
  • 7.3 Locomotion
  • 7.4 Digestive system
  • 7.5 Respiratory system
  • 7.6 Circulatory system
  • 7.7 Excretory system
  • 7.8 Nervous system – sense organs, the structure of ommatidium.
  • 7.9 Reproductive system

Unit VIII Ecology & Environment

  • 8.1 Organisms and Environment: Ecology, population, communities, habitat, niche, biome, and ecosphere (definitions only)
  • 8.2 Ecosystem: Elementary aspects only Abiotic factors – Light, Temperature & Water (Biological effects only), Ecological adaptations
  • 8.3 Population interactions
  • 8.4 Ecosystems: Types, Components, Lake ecosystem
  • 8.5 Food chains, Food web, Productivity and Energy flow in Ecosystem, Ecological pyramids – Pyramids of numbers, biomass, and energy.
  • 8.6 Nutrition cycling – Carbon, Nitrogen, & Phosphorous cycles (Brief account)
  • 8.7 Population attributes Growth, Natality, and Mortality, Age distribution, and Population regulation.
  • 8.8 Environmental issues

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AP Inter 1st Year Botany Study Material Pdf | Intermediate 1st Year Botany Textbook Solutions

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Unit I Diversity in the Living World

Unit II Structural Organisation in Plants – Morphology

Unit III Reproduction in Plants

Unit IV Plant Systematics

Unit V Cell Structure and Function

Unit VI Internal Organisation of Plants

Unit VII Plant Ecology

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Intermediate 1st Year Botany Syllabus

TS AP Inter 1st Year Botany Syllabus

Unit I Diversity in the Living World (30 Periods)

Chapter 1 The Living World
What is living? Diversity in the living world; Taxonomic categories and taxonomical aids.

Chapter 2 Biological Classification
Five kingdom classifications – Monera, Protista, Fungi, Plantae and Animalia, Three domains of life (six kingdom classification), Viruses, Viroids, Prions & Lichens.

Chapter 3 Science of Plants – Botany
Origin, Development, Scope of Botany and Branches of Botany.

Chapter 4 Plant Kingdom
Sailent features, classification, and alternation of generations of the plants of the following groups – Algae, Bryophytes, Pteridophytes, Gymnosperms, and Angiosperms.

Unit II Structural Organisation in Plants – Morphology (20 Periods)

Chapter 5 Morphology of flowering plants
Vegetative: Parts of a typical Angiosperimic plant; Vegetative morphology and modifications – Root, stem, and leaf – types; venation, Phyllotaxy.
Reproductive: Inflorescence – Racemose, Cymose, and special types (in brief).
Flower: Parts of a flower and their detailed description; Aestivation, Placentation.
Fruits: Types – True, False, and parthenocarpic fruits.

Unit III Reproduction in Plants (25 Periods)

Chapter 6 Modes of Reproduction
Asexual reproduction, binary fission, sporulation, budding, fragmentation, vegetative propagation in plants, sexual reproduction, in brief, Overview of the angiosperm life cycle.

Chapter 7 Sexual Reproduction in Flowering Plants
Stamen, Microsporangium/pollen grain, Pistil, megasporangium (ovule) and embryo sac; development of male and female gametophytes. Pollination types, agents, outbreeding devices, and pollen- pistil interaction Double Fertilization; Post fertilization events; Development of endosperm and embryo; development of seed, the structure of Dicotyledonous and Monocotyledonous seeds, Significance of fruit and seed Special modes Apomixis, parthenocarpy, polyembryony.

Unit IV Plant Systematics (10 Periods)

Chapter 8 Taxonomy of Angiosperms
Introduction. Types of Systems of classification (In brief). Semitechnical description of a typical flowering plant description of families: Fabaceae, Solanaceae, and Liliaceae.

Unit V Cell Structure and Function (35 Periods)

Chapter 9 Cell – The Unit of Life
Cell-Cell theory and cell as the basic unit of life-overview of the cell. Prokaryotic cells, Ultra Structure of Plant cell (structure in detail and functions in brief). Cell membrane, Cell wall, Cell organelles; Endoplasmic reticulum, Mitochondria, Plastids, Ribosomes, Golgi bodies, Vacuoles, Lysosomes, Microbodies, Centrosome and centriole, Cilia, Flagella, Cytoskeleton, and Nucleus. Chromosomes: Number, structural organization; Nucleosome.

Chapter 10 Biomolecules
Structure and function of Proteins, Carbohydrates, Lipids, and Nucletic acids.

Chapter 11 Cell Cycle and Cell Division
Cell Cycle, Mitosis, Meiosis – significance.

Unit VI Internal Organisation of Plants (25 Periods)

Chapter 12 Histology and Anatomy of Flowering Plants
Tissues – types, structure, and functions: Meristematic; Permanent tissues- Simple and Complex tissues. Tissue systems – Types, structure, and function: Epidermal, Ground, and Vascular tissue systems. Anatomy of Dicotyledonous and Monocotyledonous plant-Root, stem, and leaf. Secondary growth in Dicot stem and Dicot root.

Unit VII Plant Ecology (12 Periods)

Chapter 13 Ecological Adaptations, Succession, and Ecological Services
Introduction, Plant communities and Ecological adaptations: Hydrophytes, Mesophytes, and Xerophytes. Plant succession. Ecological services – Carbon fixation, Oxygen release, and pollination (In brief).

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AP Intermediate 1st Year Physics Important Questions with Answers Chapter Wise 2022

Intermediate 1st Year Physics Important Questions Chapter Wise 2022

  • Chapter 1 Physical World Important Questions
  • Chapter 2 Units and Measurements Important Questions
  • Chapter 3 Motion in a Straight Line Important Questions
  • Chapter 4 Motion in a Plane Important Questions
  • Chapter 5 Laws of Motion Important Questions
  • Chapter 6 Work, Energy and Power Important Questions
  • Chapter 7 Systems of Particles and Rotational Motion Important Questions
  • Chapter 8 Oscillations Important Questions
  • Chapter 9 Gravitation Important Questions
  • Chapter 10 Mechanical Properties of Solids Important Questions
  • Chapter 11 Mechanical Properties of Fluids Important Questions
  • Chapter 12 Thermal Properties of Matter Important Questions
  • Chapter 13 Thermodynamics Important Questions
  • Chapter 14 Kinetic Theory Important Questions

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Intermediate 1st Year Physics Syllabus

TS AP Inter 1st Year Physics Syllabus

Chapter 1 Physical World
What is Physics?, Scope and excitement of Physics, Physics, technology, and society, Fundamental forces in nature, Nature of Physical laws.

Chapter 2 Units and Measurements
Introduction, The international system of units, Measurement of length, Measurement of mass, Measurement of time, Accuracy, the precision of instruments, and errors in measurement, Significant figures, Dimensions of physical quantities, Dimensional formulae and dimensional equations, Dimensional analysis and its applications.

Chapter 3 Motion in a Straight Line
Introduction, Position, path length, and displacement, Average velocity and average speed, Instantaneous velocity and speed, Acceleration, Kinematic equations for uniformly accelerated motion, Relative velocity.

Chapter 4 Motion in a Plane
Introduction, Scalars and vectors, Multiplication of vectors by real numbers, Addition and subtraction of vectors, graphical method, Resolution of vectors, Vector addition, analytical method, Motion in a plane, Motion in a plane with constant acceleration, Relative velocity in two dimensions, Projectile motion, Uniform circular motion.

Chapter 5 Laws of Motion
Introduction, Aristotle’s fallacy, The law of inertia, Newton’s first law of motion, Newton’s second law of motion, Newton’s third law of motion, Conservation of momentum, Equilibrium of a particle, Common forces in mechanics, friction, Circular motion, Solving problems in mechanics.

Chapter 6 Work, Energy and Power
Introduction, Notions of work and kinetic energy: The work-energy theorem, Work, Kinetic energy, Work done by a variable force, The work-energy theorem for a variable force, The concept of potential energy, The conservation of mechanical energy, The potential energy of a spring, Various forms of energy: the law of conservation of energy, Power, Collisions.

Chapter 7 System of Particles and Rotational Motion
Introduction, Centre of mass, Centre of Gravity, The motion of centre of mass, Linear momentum of a system of particles, Vector product of two vectors, Angular velocity and its relation with linear velocity, Kinematics of rotational motion about a fixed axis, Torque and angular momentum, Equilibrium of a rigid body, Moment of inertia, Theorems of perpendicular and parallel axes, Dynamics of rotational motion about a fixed axis, Angular momentum in case of rotations about a fixed axis, Rolling motion.

Chapter 8 Oscillations
Introduction, Periodic and oscillatory motions, Simple harmonic motion, Simple harmonic motion and uniform circular motion, Velocity and acceleration in simple harmonic motion, Force law for Simple Harmonic Motion, Energy in simple harmonic motion, Some systems executing Simple Harmonic Motion, Damped simple harmonic motion, Forced oscillations and resonance.

Chapter 9 Gravitation
Introduction, Kepler’s laws, The universal law of gravitation, The gravitational constant, Acceleration due to the gravity of the earth, Acceleration due to gravity below and above the surface of the earth, Gravitational potential energy, Escape speed, Earth satellite, The energy of an orbiting satellite, Geostationary and polar satellites, Weightlessness.

Chapter 10 Mechanical Properties of Solids
Introduction, Elastic behaviour of solids, Stress and strain, Hooke’s law, Stress-strain curve, Elastic moduli, Applications of elastic behaviour of materials.

Chapter 11 Mechanical Properties of Fluids
Introduction, Pressure, Streamline flow, Bernoulli’s principle, Viscosity, Reynolds number, Surface tension.

Chapter 12 Thermal Properties of Matter
Introduction, Temperature and heat, Measurement of temperature, Ideal-gas equation and absolute temperature, Thermal expansion, Specific heat capacity, Calorimetry, Change of state, Heat transfer, Newton’s law of cooling.

Chapter 13 Thermodynamics
Introduction, Thermal equilibrium, Zeroth law of thermodynamics, Heat, internal energy, and work, The first law of thermodynamics, Specific heat capacity, Thermodynamic state variables and equation of State, Thermodynamic processes, Heat engines, Refrigerators and heat pumps, The second law of thermodynamics, Reversible and irreversible processes, Carnot engine, Carnot’s theorem.

Chapter 14 Kinetic Theory
Introduction, Molecular nature of matter, Behaviour of gases, Kinetic theory of an ideal gas, Law of equipartition of energy, Specific heat capacity, Mean free path.

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AP Intermediate 1st Year Chemistry Important Questions with Answers Chapter Wise 2022

Intermediate 1st Year Chemistry Important Questions Chapter Wise 2022

  • Chapter 1 Atomic Structure Important Questions
  • Chapter 2 Classification of Elements and Periodicity in Properties Important Questions
  • Chapter 3 Chemical Bonding and Molecular Structure Important Questions
  • Chapter 4 States of Matter: Gases and Liquids Important Questions
  • Chapter 5 Stoichiometry Important Questions
  • Chapter 6 Thermodynamics Important Questions
  • Chapter 7 Chemical Equilibrium and Acids-Bases Important Questions
  • Chapter 8 Hydrogen and its Compounds Important Questions
  • Chapter 9 The s-Block Elements Important Questions
  • Chapter 10 The p-Block Elements – Group 13 Important Questions
  • Chapter 11 The p-Block Elements – Group 14 Important Questions
  • Chapter 12 Environmental Chemistry Important Questions
  • Chapter 13 Organic Chemistry-Some Basic Principles and Techniques Important Questions

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Intermediate 1st Year Chemistry Syllabus

TS AP Inter 1st Year Chemistry Syllabus

Chapter 1 Atomic Structure (20 Periods)

  • 1.1 Sub-atomic particles
  • 1.2 Atomic models-Rutherford’s Nuclear model of the atom
  • 1.3 Developments to Bohr’s model of the atom.
    • 1.3.1 Nature of electromagnetic radiation
    • 1.3.2 Particle nature of electromagnetic radiation-Planck’s quantum theory
  • 1.4 Bohr’s model for the hydrogen atom
    • 1.4.1 Explanation of line spectrum of hydrogen
    • 1.4.2 Limitations of Bohr’s model
  • 1.5 Quantum mechanical considerations of sub-atomic particles
    • 1.5.1 Dual behaviour of matter
    • 1.5.2 Heisenberg’s uncertainty principle
  • 1.6 Quantum mechanical model of an atom. Important features of the Quantum mechanical model of the atom.
    • 1.6.1 Orbitals and quantum numbers
    • 1.6.2 Shapes of atomic orbitais
    • 1.6.3 Energies of orbitals
    • 1.6.4 Filling of orbitals in atoms, Aufbau principle, Pauli’s exclusion principle, and Hund’s rule of maximum multiplicity
    • 1.6.5 Electronic configurations of atoms
    • 1.6.6 Stability of half-filled and completely filled orbitals.

Chapter 2 Classification of Elements and Periodicity in Properties (20 Periods)

  • 2.1 Need to classify elements
  • 2.2 Genesis of periodic classification
  • 2.3 Modem periodic law and present form of the periodic table
  • 2.4 Nomenclature of elements with atomic number greater than 100
  • 2.5 Electronic configuration of elements and the periodic table
  • 2.6 Electronic configuration and types of elements s.p.d. and f blocks
  • 2.7 Trends in physical properties:
    • 2.7.1 (a) Atomic radius, (b) Ionic radius, (c) Variation of size in inner transition elements, (d) Ionization enthalpy, (e) Electron gain enthalpy, (f) Electro negativity
    • 2.7.2 Periodic trends in chemical properties: (a) Valence or Oxidation states, (b) Anomalous properties of second-period elements – diagonal relationship.
    • 2.7.3 Periodic trends and chemical reactivity.

Chapter 3 Chemical Bonding and Molecular Structure (20 Periods)

  • 3.1 Kossel – Lewis approach to chemical bonding
  • 3.2 Ionic or electrovalent bond – Factors favourable for the formation of the ionic compounds-Crystal structure of Sodium chloride – General Properties of ionic compounds.
  • 3.3 Bond Parameters – bond length, bond angle, bond enthalpy, bond order, and resonance – Polarity of bonds dipole moment.
  • 3.4 Valence Shell Electron Pair Repulsion (VSEPR) theories. Predicting the geometry of simple molecules.
  • 3.5 Valence bond theory – Orbital overlap concept-Directional properties of bonds-overlapping of atomic orbitals strength of sigma and pi bonds-Factors favouring the formation of covalent bonds.
  • 3.6 Hybridisation-different types of hybridization involving s, p, and d orbitals -shapes of simple covalent molecules.
  • 3.7 Coordinate bond – definition with examples.
  • 3.8 Molecular orbital theory – Formation of molecular orbitals. Linear combination of atomic orbitals (LCAO)- conditions for a combination of atomic orbitals – Energy level diagrams for molecular orbitals – Bonding in some homo nuclear diatomic molecules – H2, He2, Li2, B2, C2, N2 and O2
  • 3.9 Hydrogen bonding-cause of formation of hydrogen bond-Types of hydrogen bonds-inter and intra molecular – General properties of hydrogen bonds.

Chapter 4 States of Matter: Gases and Liquids (15 Periods)

  • 4.1 Intermolecular forces
  • 4.2 Thermal Energy
  • 4.3 Intermolecular forces Vs Thermal interactions
  • 4.4 The Gaseous State
  • 4.5 The Gas Laws
  • 4.6 Ideal gas equation
  • 4.7 Graham’s law of diffusion – Dalton’s Law of partial pressures
  • 4.8 Kinetic molecular theory of gases
  • 4.9 Kinetic gas equation of an ideal gas(No derivation)- Deduction of gas laws from Kinetic gas equation.
  • 4. 10 Distribution of molecular speeds – rms, average and most probable speeds -Kinetic energy of gas molecules.
  • 4.11 Behaviour of real gases – Deviation from Ideal gas behaviour – Compressibility factor Vs Pressure diagrams of real gases.
  • 4.12 Liquefaction of gases
  • 4.13 Liquid State – Properties of Liquids in terms of intermolecular interactions – Vapour pressure, Viscosity, and Surface tension (Qualitative idea only. No mathematical derivation).

Chapter 5 Stoichiometry (15 Periods)

  • 5.1 Some Basic Concepts – Properties of matter – uncertainty in Measurement – significant figures, dimensional analysis
  • 5.2 Laws of Chemical Combinations – Law of Conservation of mass, the law of definite proportions, the law of multiple proportions, Gay Lussac’s law of gaseous volumes, Dalton’s atomic theory, Avogadro law, principles, and examples.
  • 5.3 Atomic and molecular masses- mole concept and molar mass concept of equivalent weight.
  • 5.4 Percentage composition of compounds and calculations of empirical and molecular formulae of compounds.
  • 5.5 Stoichiometry and stoichiometric calculations.
  • 5.6 Methods of expressing concentrations of solutions-mass percent, mole fraction, molarity, and normality.
  • 5.7 Redox reactions-classical idea of redox reactions, oxidation, and reduction reactions-redox reactions in terms of electron transfer.
  • 5.8 Oxidation number concept.
  • 5.9 Types of Redox reactions-combination, decomposition, displacement, and disproportionation reactions.
  • 5.10 Balancing of redox reactions- oxidation number method, half-reaction(ion-electron) method.
  • 5.11 Redox reactions in titrimetry

Chapter 6 Thermodynamics (10 Periods)

  • 6.1 Thermodynamic terms
    • 6.1.1 The system and the surroundings
    • 6.1.2 Types of systems and surroundings
    • 6.1.3 The state of the system
    • 6.1.4 The Internal Energy as a state function, (a) Work (b) Heat (c) The general case, the first law of Thermodynamics
  • 6.2 Applications
    • 6.2.1 Work
    • 6.2.2 Enthalpy. H- a useful new state function
    • 6.2.3 Extensive and intensive properties.
    • 6.2.4 Heat capacity
    • 6.2.5 The relationship between Cp and Cv
  • 6.3 Measurement of “U and H”: calorimetry.
  • 6.4 Enthalpy change, ‘rH’of reactions-reaction Enthalpy, (a) Standard enthalpy of reactions, (b) Enthalpy changes during transformations, (c) Standard enthalpy of formation, (d) Thermo chemical equations, (e) Hess’s law of constant heat summation.
  • 6.5 Enthalpies for different types of reactions, (a) Standard enthalpy of combustion (“cH°) (b) Enthalpy of atomization (“a Ho). Phase transition, sublimation, and ionization, (c) Bond Enthalpy (“bond H6) (d) Enthalpy of solution (“sol Ho), and dilution.
  • 6.6 Spontaneity, (a) Is a decrease in enthalpy a criterion for spontaneity? (b) Entropy and spontaneity are the second law of thermodynamics, (c) Gibbs Energy and spontaneity.
  • 6.7 Gibbs Energy change and equilibrium.
  • 6.8 Absolute entropy and the third law of thermodynamics.

Chapter 7 Chemical Equilibrium and Acids-Bases (15 Periods)

  • 7.1 Equilibrium in a physical process
  • 7.2 Equilibrium in chemical process – dynamic equilibrium.
  • 7.3 Law of chemical equilibrium- Law of mass action and equilibrium constant.
  • 7.4 Homogeneous equilibria, the equilibrium constant in the gaseous system, Relationship between K and Kc.
  • 7.5 Heterogeneous equilibria.
  • 7.6 Applications of equilibrium constant.
  • 7.7 Relationship between equilibrium constant K reaction quotient Q arid Gibbs energy G.
  • 7.8 Factors affecting equilibrium Le-chatelier’s principle applies to the industrial synthesis of ammonia and sulphur trioxide.
  • 7.9 Ionic Equilibrium in solutions.
  • 7.10 Acids, bases, and salts – Arrhenius, Bronsted- Lowry, and Lewis concepts of acids and bases.
  • 7.11, Ionisation of acids and bases – Ionisation constant of water and ifs ionic product- pH scale -ionisation constants of weak acids-ionization of weak bases-relation between Ka and Kb -di and polybasic acids and di poly acidic bases-factors affecting acid strength-common ion effect in the ionization of acids and bases-hydrolysis of salts and pH of their solutions.
  • 7.12 Buffer solutions-designing of buffer solution-preparation of the acidic buffer.
  • 7.13 Solubility equilibria of sparingly soluble salts, solubility product constant common ion effect solubility of Ionic salts.

Chapter 8 Hydrogen and its Compounds (8 Periods)

  • 8.1 Position of hydrogen in the periodic table.
  • 8.2 Dihydrogen-occurrence and isotopes.
  • 8.3 Preparation of dihydrogen
  • 8.4 Properties of dihydrogen
  • 8.5 Hydrides:ionic. covalent, and non-stiochiometrichydrides
  • 8.6 Water-physical properties; structure of water, ice. Chemical properties of water; hard and soft water temporary and permanent hardness of water
  • 8.7 Hydrogen peroxide: Preparation; physical properties; structure and chemical properties; storage and uses
  • 8.8 Heavy water
  • 8.9 Hydrogen as a fuel

Chapter 9 s-Block Elements (Alkali and Alkaline Earth Metals) (8 Periods)
Group 1 Elements:

  • 9.1 Alkali metals; electronic configurations; atomic and ionic radii; ionization enthalpy hydration enthalpy; physical properties; chemical properties; uses.
  • 9.2 General characteristics of the compounds of the alkali metals; oxides; halides; salts of oxy acids.
  • 9.3 Anomalous properties of lithium: differences and similarities with other alkali metals, diagonal relationship; similarities between lithium and magnesium.
  • 9.4 Some important compounds of sodium- Sodium Carbonate; Sodium Chloride; Sodium Hydroxide; Sodium Hydrogen Carbonate.
  • 9.5 Biological importance of Sodium and Potassium.

Group 2 Elements:

  • 9.6 Alkaline earth elements; electronic configuration; ionization enthalpy; hydration enthalpy; physical properties; chemical properties; uses.
  • 9.7 General. characteristics of compounds of the alkaline earth metals: oxides, hydroxides, halides, salts of oxyacids (carbonates; sulphates, and nitrates).
  • 9.8 Anomalous behavior of beryllium; its diagonal relationship with aluminium.
  • 9.9 Some important compounds of calcium: Preparation and uses of calcium oxide; calcium hydroxide; calcium carbonate; plaster of Paris; cement.
  • 9.10 Biological importance of calcium and magnesium.

Chapter 10 p-Block Elements Group 13 (8 Periods)
Boron Family

  • 10.1 General introduction – electronic configuration, atomic radii, ionization enthalpy, electronegativity; physical & chemical properties.
  • 10.2 Important trends and anomalous properties of boron.
  • 10.3 Some important compounds of boron-borax, orthoboric acid, and diborane.
  • 10.4 Use of boron, aluminium, and their compounds.

Chapter 11 p-Block Elements Group 14 (8 Periods)
Carbon Family

  • 11.1 General introduction – electronic configuration, atomic radii, ionization enthalpy, electronegativity; physical & chemical properties.
  • 11.2 Important trends and anomalous properties of carbon.
  • 11.3 Allotropes of carbon
  • 11.4 Uses of carbon
  • 11.5 Some important compounds of carbon and silicon-carbon monoxide, carbon dioxide, Silica, silicones, silicates, and zeolites.

Chapter 12 Environmental Chemistry (8 Periods)

  • 12.1 Definition of terms: Air, Water, and Soil Pollutions
  • 12.2 Environmental pollution
  • 12.3 Atmospheric pollution; tropospheric pollution; gaseous air pollutants (oxides of sulphur; oxides of nitrogen; hydrocarbons; oxides of carbon (CO; CO2), Global warming and greenhouse effect.
  • 12.4 Acid Rain-particulate pollutants-smog.
  • 12.5 Stratospheric Pollution: formation and breakdown of ozone-ozone hole-effects of depletion of the ozone layer.
  • 12.6 Water Pollution: causes of water pollution; international standards for drinking water.
  • 12.7 Soil Pollution: pesticides, industrial wastes.
  • 12.8 Strategies to control environmental pollution – waste management- collection and disposal
  • 12.9 Green chemistry: green chemistry in day-to-day life; dry cleaning of clothes; bleaching of paper; synthesis of chemicals.

Chapter 13 Organic Chemistry-Some Basic Principles and Techniques and Hydrocarbons (25 Periods)

  • 13.1 General introduction
  • 13.2 Tetravalency of carbon: shapes of organic compounds
  • 13.3 Structural representations of organic compounds
  • 13.4 Classification of organic compounds
  • 13.5 Nomenclature of organic compounds
  • 13.6 Isomerism
  • 13.7 Fundamental concepts in organic reaction mechanisms
    • 13.7.1 Fission of covalent bond
    • 13.7.2 Nucleophiles and electrophiles
    • 13.7.3 Electron movements in organic reactions
    • 13.7.4 Electron displacement effects in covalent bonds
    • 13.7.5 Types of Organic reactions
  • 13.8 Methods of purification of organic compounds
  • 13.9 Qualitative elemental analysis of organic compounds
  • 13.10 Quantitative elemental analysis of organic compounds

Hydrocarbons

  • 13.11 Classification of Hydrocarbons.
  • 13.12 Alkanes- nomenclature, isomerism (structural and conformations of ethane only)
    • 13.12.1 Preparation of alkanes
    • 13.12.2 Properties-physical properties and chemical reactivity, substitution reactions- halogenation (a free radical mechanism), combustion, controlled oxidation, isomerization, aromatization, reaction with steam, and Pyrolysis.
  • 13.13 Alkenes- Nomenclature, the structure of ethane, Isomerism (structural and geometrical).
    • 13.13.1 Methods of preparation.
    • 13.13.2 Properties: Physical and chemical reactions, the addition of hydrogen, halogen, water, sulphuric acid, Hydrogen halides Mechanism-ionic and peroxide effect, Markovnikov’s anti-Markovnikov’s or Kharasch effect). Oxidation, ozonolysis, and polymerization.
  • 13.14 Alkynes- nomenclature and isomerism, the structure of acetylene. Methods of preparation of acetylene.
    • 13.14.1 Physical properties, chemical reactions- the acidic character of acetylene, addition reactions of hydrogen, halogen, hydrogen halides, and water. Polymerization.
  • 13.15 Aromatic hydrocarbons: Nomenclature and isomerism. Structure of benzene, resonance, and aromaticity.
    • 13.15.1 Preparation of benzene, Physical properties, Chemical properties: Mechanism of electrophilic substitution. Electrophilic substitution reactions- nitration, sulphonation, halogenation, Friedel-Craft’s alkylation, and acylation.
    • 13.15.2 Directive influence of functional groups in mono substituted benzene, Carcinogenicity and toxicity.

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AP Inter 2nd Year Chemistry Important Questions Chapter 6(d) Group-18 Elements

Students get through AP Inter 2nd Year Chemistry Important Questions Lesson 6(d) Group-18 Elements which are most likely to be asked in the exam.

AP Inter 2nd Year Chemistry Important Questions Lesson 6(d) Group-18 Elements

Very Short Answer Questions

Question 1.
List out the uses of Neon.
Answer:
Uses of Ne:

  1. Ne is used in discharge tubes and fluorescent bulbs for advertisement display purposes.
  2. ‘Ne’ – bulbs are used in botanical gardens and in greenhouses.

Question 2.
Write any two uses of argon.
Answer:
Uses of Ar:

  1. ‘Ar’ is used to create inert atmosphere in high temperature metallurgical process.
  2. ‘Ar’ is used in filling electric bulbs.

AP Inter 2nd Year Chemistry Important Questions Chapter 6(d) Group-18 Elements

Question 3.
In modern diving apparatus, a mixture of He ánd O2 is used – Why? (IPE 2016 (AP))
Answer:
In modem diving apparatus, a mixture of He and O2 is used because He is very low soluble in blood.

Question 4.
Helium is heavier than hydrogen. Yet helium is used (instead of H2) in filling balloons for meteorological observations – Why?
Answer:
‘He’ is a non—inflammable and light gas. Hence it is used in filling balloons for meterological observations.

Question 5.
How is XeO3 prepared? (IPE May – 2015(AP), 2014)
Answer:
XeF6 on hydrolysis produce XeO3.
XeF6 + 3H2O → XeO3 + 6HF

Question 6.
Give the preparation of
a) XeOF4 and
b) XeO2F2. (TS Mar. 17; IPE 2014)
Answer:
Partial hydrolysis of XeF6 gives oxy fluorides XeOF4 and XeO2F2
XeF6 + H2O → XeOF4 + 2HF
XeF6 + 2H2O → XeO2F2 + 4HF

Question 7.
Explain the structure of XeO3. (TS Mar. 17; IPE 16, 15’ 14 (TS))
Answer:
Structure of XeO3:

  1. Central atom is Xe’.
  2. ‘Xe undergoes sp3 hybridisation in 3rd excited state.
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 1
  3. ‘Xe’ forms 3σ-bonds and 3π-bonds with three oxygens.
  4. Shape of molecule is pyramidal with bond angle 103°.
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 2

AP Inter 2nd Year Chemistry Important Questions Chapter 6(d) Group-18 Elements

Question 8.
Explain the shape of XeF4 on the basis of VSEPR theory.
Answer:
Shape of XeF4:

  1. Central atom in XeF4 is
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 3
  2. Xe undergoes sp3d2 hybridisation in its 2nd excited state.
  3. Shape of the molecule is squãre planar with bond angle 90° and bond length 1.95A
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 4
  4. Xe – forms four σ-bonds by the overlap of sp3d2 – 2pz(F) orbitals.

Question 9.
Which noble gas is radio active ? How is it formed?
Answer:
Radon (Rn) is radio active noble gas. Radon is obtained as decay product of 86R226.
86Ra226 → 86Rn222 + 2He4

Question 10.
How are XeF2, XeF4, XeF6 prepared? Give equation.
Answer:
AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 5

Question 11.
Noble gases are inert – explain.
Answer:
Noble gases are chemically inert:

  1. Noble gases have stable electronic configuration octet configuration except He.
  2. Noble gases have high Ionisation energy values and have large positive values of electron gain enthalpy.

Question 12.
Write the name and formula of the first noble gas compound prepared by Bertlett.
Answer:
The first noble gas compound prepared by Bertlett is XePtF6. Name of the compound is xenon hexa fluoro platinate.

Question 13.
Why do noble gases form compounds with fluorine and oxygen only?
Answer:
Noble gases form compounds with flourine and oxygen only.
Reason: Oxygen and Fluorine are most electronegative elements.

AP Inter 2nd Year Chemistry Important Questions Chapter 6(d) Group-18 Elements

Short Answer Questions

Question 1.
Explain the structures of
a) XeF2 and
b) XeF4. (AP Mar. ‘17, IPE 16, 15, ‘14 (TS)) (TS Mar. ’14)
Answer:
Xenon forms the binary fluorides XeF2, XeF4, XeF6 as follows. These are formed by direct combination of Xe and F2.
AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 6

Structure of XeF2:

  1. In XeF2 central atom is ‘Xe’.
  2. ‘Xe’ undergoes sp3d hybridisation in its 1st excited state.
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 7
  3. Shape of molecule is linear.
  4. Xe form two σ-bonds with two fluorines.
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 8

b) Structure of XeF4:

  1. Central atom in XeF4 is ‘Xe’.
  2. Xe undergoes sp3d2 hybridisation in it’s 2nd excited state.
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 9
  3. Shape of the molecule is square planar with bond angle 90° and bond length 1.95A
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 10
  4. Xe forms four σ-bonds by the overlap of sp3d2 – 2pz (F) orbitals.

Question 2.
Explain the structures of
a) XeF6 and
b) XeOF4 (IPE Mar & May – 2015, 14)
Answer:
Structure òf XeF6 is ‘Xe’.

  1. Central atom in XeF6 is ‘Xe’.
  2. Xe undergoes sp3d3 hybridisation in it’s 3rd excited state.
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 11
  3. Shape of molecule is distorted octahedral.
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 12

b) Structure of XeOF4:

  1. In XeOF4 molecule ‘Xe’ undergoes sp3d2 hybridisation.
  2. Shape of the molecule is square pyramid.
  3. There is one Xe-O double bond containing.
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 13
    pπ = dπ overlapping.
    Partial hydrolysis of XeF6 gives XeOF4
    XeF6 + H2O → XeOF4 + 2HF
    XeOF4 is a colourless volatile liquid. It has a square pyramidal shape.

AP Inter 2nd Year Chemistry Important Questions Chapter 6(d) Group-18 Elements

Question 3.
Explain the structure of
a) XeO3 and
b) XeO4 (T.S. Mar. ‘16)
Answer:
a) Structure of XeO3:

  1. Central atom is ‘Xe’
  2. ‘Xe’ undergoes sp3 hybridisation in 3rd excited state.
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 14
  3. ‘Xe forms 3σ-bonds and 3π-bonds with three oxygens.
  4. Shape of molecule is pyramidal with bond angle 103°.
    AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 15

b) Structure of XeO4:
Xe is in sp3 hybridisation four singma bonds and four dπ – pπ bonds. Shape of XeO4 is tetrahedral.
AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 16

Question 4.
Write the preparations of Xenon flourides.
Answer:
Xenon flourides : Xenon forms three binary fluorides, Xe F2, XeF4, and XeF6 by the direct reaction of Xenon with fluorine under suitable conditions.
AP Inter 2nd Year Chemistry Important Questions Chapter 6(c) Group-17 Elements 17
XeF6 can also be prepared by the interaction of XeF4 and O2F2 at 143 K.
XeF4 + O2F2 → XeF6 + O2

Question 5.
Write the preparations of Xenon Oxides.
Answer:
Xenon Oxides: Xenon forms two oxides XeO3 and XeO4 with oxygen.
These oxides are formed by the hydrolysis of xenon fluorides.
6XeF4 + 12 H2O → 4 Xe + 2 XeO3 + 24 HF + 3O2
XeF6 + 3 H2O → XeO3 + 6 HF

Question 6.
Give the formulae and describe the structures of a noble gas species, isostructural with
a) [latex]\mathrm{ICl}_4^{-}[/latex]
b) [latex]\mathbf{I B r}_2^{-}[/latex]
c) [latex]\mathrm{BrO}_3^{-}[/latex]
Answer:
a) [latex]\mathrm{ICl}_4^{-}[/latex] is also structural with XeF4 and it has square planar shape.
b) [latex]\mathbf{I B r}_2^{-}[/latex] is also structural with XeF2 and it has linear shape.
c) [latex]\mathrm{BrO}_3^{-}[/latex] is iso-structural with XeO4 and it has tetrahedral šhape.

AP Inter 2nd Year Chemistry Important Questions Chapter 6(d) Group-18 Elements

Question 7.
Write any two uses of Helium.
Answer:
Uses of Helium:

  1. It is non inflammable and very light gas. Hence it is used in the balloons of Meteorological observations.
  2. It is used in gas cooled nuclear reactors and used as cryogenic agent.
  3. It is used as diluent for oxygen in modern diving apparatus.

AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen

Students get through AP Inter 2nd Year Chemistry Important Questions 13th Lesson Organic Compounds Containing Nitrogen which are most likely to be asked in the exam.

AP Inter 2nd Year Chemistry Important Questions 13th Lesson Organic Compounds Containing Nitrogen

Very Short Answer Questions

Question 1.
Gabriel Phthalimide synthesis exclusively forms primary amines only. Explain.
Answer:
Gabriel Phthalimide synthesis exclusively forms primary amines only.
Reason: In this reaction primary amines are formed without the traces of 2° (or) 3° amines.

Questions 2.
Write equations for carbylamine reaction of any one aliphatic amine.
Answer:
When Ethyl amine (1° – amine) reacts with chloroform in presence of alkali to form ethyl isocyanide.
CH3 – CH2 – NH2 + CHCl3 + 3KOH A AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 1 CH3 – CH2 – NC + 3KCl + 3H2O

AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen

Question 3.
Why aniline does not undergo Friedel — Crafts reaction?
Answer:
Aniline is a lewis base and AlCl3 is a Lewis acid. In Friedel.Craft’s reaction both of these combined to form a complex.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 2
Due to formation of complex the electrophilic substitution tendency decreases in aniline and it does not undergo this reaction.

Question 4.
Give structures of A, B and C in the following reactIons. [T.S. Mar. 17] [A.P. & T.S. Mar. 16]
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 3
Answer:
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 4
A – Phenyl Cyanide B – Benzoic acid C – Benzarnide

Question 5.
Why cannot aromatic primary amines be prepared by Gabriel phthalimide synthesis?
Answer:
Aromatic 1° – amines cannot be prepared by Gabriel phthalinide synthesis because aryl halides do not undergo nucleophilic substitution with an ion formed by phthalinide.

Question 6.
Accomplish the following conversions. [Mar. 14]
i) Benzolc acid to benzamide
ii) Aniline to p – bromoanlline.
Ans:
Conversion of benzoic acid to benzamide
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 5
ii) Conversion of Aniline to p – bromoanlline.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 6

Question 7.
How are Amines prepared by Hoffmann bromamide degradation method.
Answer:
Hoffmann bromamide degradation method: In this method amides are directly converted into amines. When amides are treated with Br5 in NaOH gives amine.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 7

AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen

Question 8.
What is Diazotisation reaction ? Give equation. [IPE 16, 14 (T.S.)]
Answer:
Diazotisation reaction: Aromatic primary amines react with nitrous acid at low temperatures to form diazonium salts.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 8

Question 9.
What is sulphonation ? Give equation.
Answer:
Sulphonation : Aniline reacts with cone H2SO4 and forms anilinium hydrogen sulphate which on heating gives P – amino benzene sulphonic acid (sulphanilic acid) which exists as Zwitter ion.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 9
Aniline does not undergo Friedel crafts reactiondue to salt formation with AlCl3.

Question 10.
Arrange the following bases in increasing order of their basic strength. Aniline, P – nitroaniline and P – toluidine.
Answer:
The increasing order of basic strength of given compounds is
P – nitroaniline < aniline < P – toluidine
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 10

AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen

Question 11.
How is benz ene diazonium chloride prepared? Give equation.
Answer:
Preparation: Benzene diazomum chloride is prepared by the reaction of aniline with nitrous acid at 273 – 278K. The conversion of primary aromatic amine into diazonium chloride is called Diazotisation.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 11

Question 12.
Arrange the following bases in decreasing order of pHb, values. C2H5NH2, C6H5NHCH3, (C2H5)2 NH and C6H5NH2.
Answer:
The decreasing order of pKb values of given amines is
C6H5NH2 > C6H5NHCH3 > C6H5NH2 > (C2H5)2 NH

Question 13.
What is a coupling reaction ? Give equation. .
Answer:
Coupling reactions : The azoproducts obtained when diazonium slats react with aromatic compounds have extended conjugated system through N = N. This reaction is called coupling reaction and the prodocuts formed are coloured.
a) Reaction with Phenol
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 12

Question 14.
How do you convert aniline to parabromo aniline. [IPE 2014]
Answer:
Aniline is first acylated to give acetaniiyde which on bromination gives parabromo derivative. This bromo derivative on hydrolysis gives parabromo aniline.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 13

Question 15.
How is Aniline prepared. [IPE 2016 (TS)]
Answer:
Aniline is prepared by reduction of nitro benzene in acid medium.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 14

AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen

Question 16.
Explain why ethylamine is more soluble in water where as aniline is not soluble.
Answer:
Ethyl amine is a primary amine, due to intermolecular hydrogen bonding with water molecules it is soluble in water. Though Aniline has – NH2 group, due to hydrophobic aryl group it is not soluble in water.

Short Answer Questions

Question 1.
Explain with a suitable example how benzene sulphonylchloride can distinguish primary, secondary and tertiary amines.
Answer:
Benzene sulphonyl chloride is called Hinsberg’s reagent. This is used to distinguish the 1°, 2°, 3° – amines.

  • with 1° – amine : Benzene sulphonyl chloride reacts with 1° – amine and produce N – Alkyl benzene sulphonamide which is soluble in alkali.
  • with 2° – amine : Benzene sulphonyl chloride reacts with 2° – amine and produce N, N – Dialkyl benzene sulphonamide which is insoluble in alkali.
    AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 15
  • with 2° – amine: Benzene suiphonyl chloride reacts with 2° – amine and produce N, N – Dialkyl benzene sulphonamide which is insoluble in alkali.
    AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 16
  • with 3° – amine : Benzene sulphonyl chloride does not react with benzene sulphonyl chloride.

Question 2.
How do you prepare Ethyl cyanide and Ethyl isocyanide from a common alkylhalide ? [IPE 2014]
Answer:
Preparation of ethyl cyanide : Ethyl chloride reacts with aq. Ethanolic KCN to form Ethyl cyanide as a major product.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 17
Preparation of Ethyl isocyanide : Ethyl chloride reacts with aq. Ethanolic AgCN to form Ethyl iso cyanide as a major product.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 18

Question 3.
How do you distinguish cyanides and isocyanides by hydrolysis and reducation.
Answer:
i) Hydrolysis : Cyanides on hydrolysis give carboxylic acids and ammmonia where as isocynanides on hydrolysis give primary amines and formic acid:
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 19
ii) Reduction: Reducation of nitriles give primary amines where as reduction of isocyanides yield secondary amines.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 20

AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen

Question 4.
How do you carryout the following conversions? .
i) N – Ethylamine to N, N – Diethyl propanamine
ii) Aniline to Benzene suiphonamide
Answer:
Conversion of
i) N – Ethyl amine to N, N – Diethyl propanamine : Ethyl amine reads with ethyl chloride and propyl chloride to from N, N – Di ethyl propanamine.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 21

ii) Conversion of Aniline to Benzene sulphonamide : Aniline reacts with benzene sulphonyl chloride to form N – Phenyl benzene sulphonamide.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 22

Question 5.
Explain the basic character of different Amines.
Answer:
Basic Character of Amines : Aniline reacts with acid and form salts.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 23
Structure qnd Basicity : Alkyl amines are more basic than ammonia. The alkyl group pushes the electrons towards nitrogen by + I effect. Thus line pair of electrons on nitrogen are more available for sharing with the proton of acid. Hence the basic nature of alkylamines increases with increase in number of alkyl groups. Thus in gaseous phase the basicity order of amines is in the order 36 amine > 2° amine >1° amine > ammonia.

In the aqueous phase the substituted ammonium cations get stabilised by +1 effect and also by solvation with water molecules. Greater the size of the ion, lesser will be the solvation and less stabilised is the ion. The order of stability is.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 24
Greater the stability of the ammonium cation, stronger is the basic nature of amine. The order of basicity of aliphatic amines is primary > secondary > tertiary. The – CH3 group Creates less steric hindrance to hydrogen bortding than C2H5 group, thus the change of alkyl group changes the basic strength. The basic strength of methyl substituted and ethly substituted amines in aqueous soltuion is in the order.
(C2H5)2 NH > (C2H5)3 N > C2H5 – NH2 > NH3
(CH3 NH)2 > CH3 – NH2 > (CH3)3N >NH3
Aromatic amines are less basic than ammonia. The lone pair of electrons on nitrogen is in conjugation with benzene ring.

AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen

Question 6.
Write two methods each for the preparation of alkyl cyanide and alkyl isocyanide.
Answer:
Preparation
a) From Alkyl Halides : Alkyl halides with ethanolic potassium cyanide gives cyanides where as with silver cyanide gives alkyl isocyanide.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 25
b) From amides and aldoximes : The dehydration of amides (or) oximes with dehydrating agents like P2O5 (or) with benzene suiphonyl chloride yeild cyanides.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 26
c) Isocyanides from amines: (Carbyl amine reaction)
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 27

AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen

Question 7.
Give one chemical test to distinguish between the following pairs of compounds.
i) Methylamine and dimethylamine
ii) Aniline and N.Methylanhline
iii) Ethylamine and aniline
Answer:
i) Methyl amine (1° – amine) and dimethyl amine (2° – amine) are distinguished by iso cyanide test (or) Carbylamine test. Methyl amine responds to carbylamine reaction to produce methyl isocyanide where as dimethyl amine does not respond to the iso cyanide test.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 28
ii) Anjiine (1° – amine) and N.methyl (2° – amine) aniline are distinguished by carbylamine test (or) isocyanide test. Aniline responds to carbyl amine test to give foul smelling phenyl iso cyanide where as N – methyl aniline does not responds to carbyl amine Test.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 29
iü) Ethyl amine (1° – aliphatic amine) and aniline (1° – aromatic amine) are distinguished by Diazotisation reaction. Aniline undergo diazotisafion reaction to form benzene diazonium salt where as ethyl amine form highly unstable alkyl diazonium salt.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 30

Long Answer Questions

Question 1.
Explain the following name reactions: [T.S. Mar. 17] [IPE -2015, B.M.P 2016 (TS), (AP)]
i) Sandmeyer reaction
ii) Gatterman reaction
Answer:
i) Sandmeyer reaction: Formation of chiorobenzene, Bromo benzene (or) cyano benzene from benzene diazonium salts with reagents Cu2Cl2/HCl, Cu2Br2/HBr, CuCN/KCN is called sandmyeres reaction.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 31
ii) Gatterman reaction : Formation of chioro benzene, Bromobenzene from benzene diazonium salts with reagents Cu/HCl, Cu/HBr is referred as gatterman reaction.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 32

Question 2.
Complete the following conversions.
i) CH3NC + HgO →
ii) ? + 2H2O → CH2NH2 + HCOOH
iii) CH3CN + C2H5MgBr → ? AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 33
iv) CH3CH2NH2 + CHCl3 + KOH AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 34
v) AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 35
Answer:
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 36

AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen

Question 3.
Explain why aniline in strong acidic medium gives a mixture Of Nitro anilines and what steps need to be taken to prepare selectively P – nitro aniline.
Answer:
In strong acidic medium anline undergo nitration to form mixture of nitro anilines. In strongly acidic medium aniline is protonated to form the anilinium ion which is metadirecting. So besides the ortho and para derivatives meta derivative also formed. .
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 37
By protecting – NH2 group by acetylation reaction with acetic anhydride the nitration reaction can be controlled and the – P nitro derivative can be formed as major product.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 38

Question 4.
Complete the following conversions : Aniline to
i) Fluorobenzene
ii) Cyanobenzene
iii) Benzene and
iv) Phenol
Answer:
i) Aniline to Fluorobenzene
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 39
iv) Aniline to phenol
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 40

AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen

Question 5.
i) Account for the stability of aromatic diazonium ions when compared to aliphatic diazonium ions.
ii) Write the equations showing the conversion of aniline diazoniumchloride to
a) chlorobenzene,
b) Iodobenzene and
c) Bromobenzene
Answer:
i) Aliphatic diazonium salts which are formed from 1° -aliphatic amines are highly unstable and liberate nitrogen gas and alcohols.

Aromatic diazonium salts formed from 1° – aromatic amines are stable for a short time in solution at low temperatures (0 – 5°C). The stability of arene diazonium ion is explained on the basis of resonance.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 41

Question 6.
Write the steps involved in the coupling of Benzene diazonium chloride with aniline and phenol.
Answer:
Benzene diazonium chloride reacts with phenol in which the phenol molecule at its para position is coupled with the diazonium salt to form P-hydroxyazobenzene. This type of reactions is known as coupling reactions. Similarly the reaction o£ diazonium salt with aniline yields P – amino azobenzene.
AP Inter 2nd Year Chemistry Important Questions Chapter 13 Organic Compounds Containing Nitrogen 42