Entrance | ENTRANCE INDIA

UPTU B.Tech TEE-303 Network Analysis & Synthesis Sem 3 2010-11

October 5, 2016September 19, 2016 by Soubhagya Ranjan Nath

JCECE – 2016 BIOLOGY FULL SYLLABUS

September 12, 2016 by [email protected]

BIOLOGY

1. Diversity in Living World

Diversity of living organisms Classification of the living organisms (five kingdom classification, major groups and principles of classificaton within each kingdom.) Systematics and binomial System of nomenclature Salient features of animal (non chordates up to phylum level and chordates up to class level) and plant (major groups; Angiospems up to subclass) classification. Botanical gardens, herbara, Zoological parks and museums

ll Structural Organisation in Animals and Plants

Tissues in animals and plants. Morphology, anatomy and functions of different parts of flowering plants: Root, stem, leaf, inflorescence, flower, fruit and seed. Morphology, anatormy and functions of differnt systems of an nnelid (earthworm), an insect (cockroach) and an amphibian (frog).

lll CELL : STRUCTURE AND FUNCTION

Cell: cell wall, cell membrance and cell organelles’ (plastids, mitochondria, endoplasmic reticulum, Golgi bodies/dictyosomes, ribosomes, lysosomes, vacuoles, Centrioles) and nuclear organization. Mitosis, meiosis, cell cycle. Basic chemical constituents of living bodies. Structure and functions of carbohydrates, proteins,
lipids and nucleic acids. Enzymes: types, properties and function.

IV Plant Physiology

Movement of water, food, nutrients and gasses, Plants and Water Mineral nutrition. Respiration, Photosynthesis, Plant growth and development.

V Human Physiology

Digestion and absorption. Dreathing and respiration. Body fluids and circulation. Excretory products and limination. Locomotion and movement. Control and coordination.

l SEXUAL REPRODUCTION

Pollination and fertilization in flowering plants. Development of seeds and fruits. Human reproduction: eproductive system in male and female, menstrual cycle. Production of gametes, fertilization, implantation, embryo development, pregnancy and prarturation. Reproductive health – birth control, contraception and sexually ransmitted diseases.

ll Genetics and evolution

Mendelian inheritancce. Chromosome theory of inheritance, deviations from Mendelian ratio (gene interaction – Incomplete dominance, co-dominance, complementary genes, multiple alleles). Sex determination in human beings : XX, XY Linkage and crossing over. Inherithnce pattern of harmophilia and blood groups in human beings. DNA: eplication, transcription, translation. Gene expression and regulation. Genome and Human Genome Project. DNA fingerprinting. Evolution: Theories and evidences.

III. BIOLOGY AND HUMAN WELFARE

Animal husbandry. Basic concepts of immunology, vaccines. Pathogens, Parasites. Plant breeding, tissue culture, food production.Microbes in household food processing, industrial production, sewage treatment and evergy eneration. Cancer and AIDS. Adolescence and drug/alcohol abuse.

IV. BIOTECHNOLOGY AND ITS APPLICATIONS

Recombinant DNA technology. Applications in Health, Agriculture and Industry Genetically modified (GM) organisms; biosafety issues. Insulin and Bt cotton

V. ECOLOGY & ENVIRONMENT

Ecosystems: components, types and energy flow. Species, population and community. Ecological adaptations. Centres of diversity and conservation of biodiversity, National parks and sanctuaries. Environmental issues.

Joint CSIR UGC NET Exam Question Papers & Answer Keys PDF Downloads

August 26, 2019September 8, 2016 by M Prakash

MH-CET– 2016 PHYSICS FULL SYLLABUS

September 8, 2016 by [email protected]

PHYSICS

Medical PG Prep AIPGMEE AIIMS JIPMER and Other PG Entrance Application

August 16, 2016August 16, 2016 by bn Mishra

EAMCET Mathematics Syllabus

June 21, 2016 by

1. ALGEBRA
“Functions : Types of functions – Definitions, Inverse functions and Theorems, Domain, Range, Inverse of real valued functions.
Mathematical Induction: Principle of Mathematical Induction & Theorems, Applications of Mathematical Induction, Problems on divisibility.
Matrices:Types of matrices, Scalar multiple of a matrix and multiplication of matrices, Transpose of a matrix, Determinants, Adjoint and Inverse of a matrix, Consistency and inconsistency of Equations- Rank of a matrix, Solution of simultaneous linear equations.
Complex Numbers: Complex number as an ordered pair of real numbers- fundamental operations – Representation of complex numbers in the form a+ib – Modulus and amplitude of complex numbers –Illustrations – Geometrical and Polar Representation of complex numbers in Argand plane- Argand diagram.
De Moivre’s Theorem: De Moivre’s theorem- Integral and Rational indices – nth roots of unity- Geometrical Interpretations – Illustrations.
Quadratic Expressions: Quadratic expressions, equations in one variable – Sign of quadratic expressions – Change in signs – Maximum and minimum values – Quadratic inequations.
Theory of Equations: The relation between the roots and coefficients in an equation – Solving the equations when two or more roots of it are connected by certain relation – Equation with real coefficients, occurrence of complex roots in conjugate pairs and its consequences – Transformation of equations – Reciprocal Equations.
Permutations and Combinations: Fundamental Principle of counting – linear and circular permutations – Permutations of ‘n’ dissimilar things taken ‘r’ at a time – Permutations when repetitions allowed – Circular permutations – Permutations with constraint repetitions – Combinations-definitions and certain theorems.
Binomial Theorem: Binomial theorem for positive integral index – Binomial theorem for rational Index (without proof) – Approximations using Binomial theorem.
Partial fractions: Partial fractions of f(x)/g(x) when g(x) contains non –repeated linear factors –
Partial fractions of f(x)/g(x) when g(x) contains repeated and/or non-repeated linear factors –
Partial fractions of f(x)/g(x) when g(x) contains irreducible factors.”
2. TRIGONOMETRY
“Trigonometric Ratios, variations, Graphs and Periodicity of Trigonometric functions – Trigonometric ratios and Compound angles – Trigonometric ratios of multiple and sub-multiple angles – Transformations – Sum and Product rules
Trigonometric Equations: General Solution of Trigonometric Equations – Simple Trigonometric Equations – Solutions
Inverse Trigonometric Functions: To reduce a Trigonometric Function into a bijection – Graphs of Inverse Trigonometric Functions – Properties of Inverse Trigonometric Functions
Hyperbolic Functions: Definition of Hyperbolic Function – Graphs – Definition of Inverse Hyperbolic Functions – Graphs – Addition formulas of Hyperbolic Functions
Properties of Triangles: Relation between sides and angles of a Triangle – Sine, Cosine, Tangent and Projection rules – Half angle formulae and areas of a triangle – In-circle and Ex-circle of a Triangle”
3. VECTOR ALGEBRA
“Addition of Vectors : Vectors as a triad of real numbers – Classification of vectors – Addition of vectors – Scalar multiplication – Angle between two non zero vectors – Linear combination of vectors – Component of a vector in three dimensions – Vector equations of line and plane including their Cartesian equivalent forms
Product of Vectors: Scalar Product – Geometrical Interpretations – orthogonal projections – Properties of dot product – Expression of dot product in i, j, k system – Angle between two vectors – Geometrical Vector methods – Vector equations of plane in normal form – Angle between two planes – Vector product of two vectors and properties – Vector product in i, j, k system – Vector Areas – Scalar Triple Product – Vector equations of plane in different forms, skew lines, shortest distance and their Cartesian equivalents. Plane through the line of intersection of two planes, condition for coplanarity of two lines, perpendicular distance of a point from a plane, Angle between line and a plane. Cartesian equivalents of all these results – Vector Triple Product – Results”
4. MEASURES OF DISPERSION
Range – Mean deviation – Variance and standard deviation of ungrouped/grouped data – Coefficient of variation and analysis of frequency distribution with equal means but different variances.
5. PROBABILITY:
“Random experiments and events – Classical definition of probability, Axiomatic approach and addition theorem of probability – Independent and dependent events conditional probability- multiplication theorem and Bayee’s theorem
Random Variables and Probability Distributions – Random Variables – Theoretical discrete distributions – Binomial and Poisson Distributions.”
6. COORDINATE GEOMETRY
“Locus : Definition of locus – Illustrations – To find equations of locus – Problems connected to it
Transformation of Axes : Transformation of axes – Rules, Derivations and Illustrations – Rotation of axes – Derivations – Illustrations
The Straight Line: Revision of fundamental results – Straight line – Normal form – Illustrations – Straight line – Symmetric form – Straight line – Reduction into various forms – Intersection of two Straight Lines – Family of straight lines – Concurrent lines – Condition for Concurrent lines – Angle between two lines – Length of perpendicular from a point to a Line – Distance between two parallel lines – Concurrent lines – properties related to a triangle
Pair of Straight lines: Equations of pair of lines passing through origin, angle between a pair of lines – condition for perpendicular and coincident lines – bisectors of angles – Pair of bisectors of angles – Pair of lines – second degree general equation – Conditions for parallel lines – distance between them, Point of intersection of pair of lines – Homogenizing a second degree equation with a first degree equation in X and Y.
Circle : Equation of circle -standard form-centre and radius of a circle with a given line segment as diameter & equation of circle through three non collinear points – parametric equations of a circle – Position of a point in the plane of a circle – power of a point-definition of tangent-length of tangent – Position of a straight line in the plane of a circle-conditions for a line to be tangent – chord joining two points on a circle – equation of the tangent at a point on the circle- point of contact-equation of normal – Chord of contact – pole and polar-conjugate points and conjugate lines – equation of chord with given middle point – Relative position of two circles- circles touching each other externally, internally common tangents –centers of similitude- equation of pair of tangents from an external point.
System of circles: Angle between two intersecting circles – Radical axis of two circles-properties – Common chord and common tangent of two circles – radical centre – Intersection of a line and a Circle.
Parabola: Conic sections –Parabola- equation of parabola in standard form-different forms of parabola- parametric equations – Equations of tangent and normal at a point on the parabola (Cartesian and parametric) – conditions for straight line to be a tangent.
Ellipse: Equation of ellipse in standard form – Parametric equations Equation of tangent and normal at a point on the ellipse (Cartesian and parametric)- condition for a straight line to be a tangent.
Hyperbola: Equation of hyperbola in standard form- Parametric equations – Equations of tangent and normal at a point on the hyperbola (Cartesian and parametric)- conditions for a straight line to be a tangent- Asymptotes.
Three Dimensional Coordinates: Coordinates – Section formulas – Centroid of a triangle and tetrahedron.
Direction Cosines and Direction Ratios: Direction Cosines – Direction Ratios
Plane : Cartesian equation of Plane – Simple Illustrations.”
7. CALCULUS
“Limits and Continuity: Intervals and neighborhoods – Limits – Standard Limits – Continuity
Differentiation: Derivative of a function – Elementary Properties – Trigonometric, Inverse Trigonometric, Hyperbolic, Inverse Hyperbolic Function – Derivatives – Methods of Differentiation – Second Order Derivatives
Applications of Derivatives: Errors and approximations – Geometrical Interpretation of a derivative – Equations of tangents and normals – Lengths of tangent, normal, sub tangent and sub normal – Angles between two curves and condition for orthogonality of curves – Derivative as Rate of change – Rolle’s Theorem and Lagrange’s Mean value theorem without proofs and their geometrical interpretation – Increasing and decreasing functions – Maxima and Minima.
Integration: Integration as the inverse process of differentiation- Standard forms – properties of integrals – Method of substitution- integration of Algebraic, exponential, logarithmic, trigonometric and inverse trigonometric functions. Integration by parts – Integration- Partial fractions method – Reduction formulae.
Definite Integrals: Definite Integral as the limit of sum – Interpretation of Definite Integral as an area – Fundamental theorem of Integral Calculus – Properties – Reduction formulae – Application of Definite integral to areas
Differential equations: Formation of differential equation-Degree and order of an ordinary differential equation – Solving differential equation by – a) Variables separable method – b) Homogeneous differential equation – c) Non – Homogeneous differential equation – d) Linear differential equations.”

EAMCET 2016 Chemistry Syllabus

June 21, 2016 by

1. ATOMIC STRUCTURE:
Sub- atomic particles – Atomic models- Rutherford’s Nuclear model of atom – Developments to the Bohr’s model of atom – Nature of electromagnetic radiation – Particle nature of electromagnetic radiation- Planck’s quantum theory – Bohr’s model for Hydrogen atom – Explanation of line spectrum of hydrogen – Limitations of Bohr’s model – Quantum mechanical considerations of sub atomic particles – Dual behaviour of matter – Heisenberg’s uncertainty principle – Quantum mechanical model of an atom. Important features of Quantum mechanical model of atom – Orbitals and quantum numbers – Shapes of atomic orbitals – Energies of orbitals – Filling of orbitals in atoms – Aufbau Principle, Pauli’s exclusion Principle and Hund’s rule of maximum multiplicity – Electronic configurations of atoms – Stability of half filled and completely filled orbitals.
2. CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES:
Need to classify elements – Genesis of periodic classification – Modern periodic law and present form of the periodic table – Nomenclature of elements with atomic number greater than100 – Electronic configuration of elements and the periodic table – Electronic configuration and types of elements s,p,d and f blocks – Trends in physical properties- a) Atomic radius, b) Ionic radius, c) Variation of size in inner transition elements, d) Ionization enthalpy, e) Electron gain enthalpy, f) Electro negativity – Periodic trends in chemical properties: a) Valence or Oxidation states, b) Anomalous properties of second period elements – diagonal relationship – Periodic trends and chemical reactivity.
3. CHEMICAL BONDING AND MOLECULAR STRUCTURE:
Kossel – Lewis approach to chemical bonding – Octet rule – covalent bond, Lewis representation of simple molecules (Lewis Structures) – Formal Charge – Limitation of octet rule – Ionic or electrovalent bond – Factors favourable for the formation of ionic compounds-Crystal structure of sodium chloride-General properties of ionic compounds – Bond Parameters – bond length, bond angle, and bond enthalpy, bond order, resonance-Polarity of bonds dipole moment – Valence Shell Electron Pair Repulsion (VSEPR) theory. Predicting the geometry of simple molecules – Valence bond theory-Orbital overlap concept-Directional properties of bonds-overlapping of atomic orbitals – types of overlapping and nature of covalent bonds – strength of sigma and pi bonds-Factors favouring the formation of covalent bonds – Hybridisation-different types of hybridization involving s, p and d orbitals- shapes of simple covalent molecules – Coordinate bond – definition with examples – general properties of compounds containing coordinate bonds – Molecular orbital theory – Formation of molecular orbitals, Linear combination of atomic orbitals (LCAO)-conditions for combination of atomic orbitals – Types of molecular orbitals – Energy level diagrams for molecular orbitals –Electronic configuration and molecular behavior – Bonding in some homo nuclear diatomic molecules – H2 ,He2 ,Li2 ,B2 ,C2 ,N2 and O2 – Hydrogen bonding-cause of formation of hydrogen bond-Types of hydrogen bonds-inter and intra molecular-General properties of hydrogen bonds.
4. STATES OF MATTER: GASES AND LIQUIDS:
Intermolecular forces – Thermal Energy – Intermolecular forces Vs Thermal interactions – The Gaseous State – The Gas Laws – Ideal gas equation – Graham’s law of diffusion – Dalton’s Law of partial pressures – Kinetic molecular theory of gases – Kinetic gas equation of an ideal gas (No derivation) deduction of gas laws from Kinetic gas equation – Distribution of molecular speeds – rms, average and most probable speeds-Kinetic energy of gas molecules – Behaviour of real gases – Deviation from Ideal gas behaviour – Compressibility factor Vs Pressure diagrams of real gases – Liquefaction of gases – Liquid State – Properties of Liquids in terms of Inter molecular interactions – Vapour pressure, Viscosity and Surface tension (Qualitative idea only. No mathematical derivation).
5. STOICHIOMETRY:
Some Basic Concepts – Properties of matter – uncertainty in Measurement-significant figures, dimensional analysis. Laws of Chemical Combinations – Law of Conservation of Mass, Law of Definite Proportions, Law of Multiple Proportions, Gay Lussac’s Law of Gaseous Volumes, Dalton’s Atomic Theory, Avogadro Law, Principles, Examples – Atomic and molecular masses- mole concept and molar mass concept of equivalent weight – Percentage composition of compounds and calculations of empirical and molecular formulae of compounds – Stoichiometry and stoichiometric calculations – Methods of Expressing concentrations of solutions-mass percent, mole fraction, molarity, molality and normality – Redox reactions-classical idea of redox reactions, oxidation and reduction reactions-redox reactions in terms of electron transfer. Oxidation number concept – Types of Redox reactions-combination, decomposition, displacement and disproportionation reactions – Balancing of redox reactions – oxidation number method Half reaction (ion-electron) method – Redox reactions in Titrimetry.
6. THERMODYNAMICS:
Thermodynamic Terms – The system and the surroundings – Types of systems and surroundings – The state of the system – The Internal Energy as a State Function – (a) Work (b) Heat (c) The general case, the first law of Thermodynamics∆ – Applications – Work – Enthalpy, H- a useful new state function – Extensive and intensive ∆properties – Heat capacity – The relationship∆ between CP and Cv – Measurement of U and H: Calorimetry -Enthalpy change, r H of reactions – reaction Enthalpy (a) Standard enthalpy of reactions – (b) Enthalpy changes during phase transformations – (c) Standard enthalpy∆ of formation – (d) Thermo chemical∆ equations – (e) Hess’s law of∆ constant Heat summation – Enthalpies for different types of reactions – (a) Standard enthalpy of combustion ( c HO ) – (b) Enthalpy∆ of atomization ( a HO) – (c) Bond Enthalpy ( bond HO) – (d) Enthalpy of solution ( sol HO ) and dilution – lattice enthalpy – Spontaneity – (a) Is decrease in enthalpy a criterion for spontaneity? – (b) Entropy and spontaneity, the second law of thermodynamics – (c) Gibbs Energy and spontaneity – Gibbs Energy change and equilibrium – Absolute entropy and the third law of thermodynamics.
7. CHEMICAL EQUILIBRIUM AND ACIDS-BASES:
Equilibrium in Physical process – Equilibrium in chemical process – Dynamic Equilibrium – Law of chemical Equilibrium – Law of mass action and Equilibrium constant – Homogeneous Equilibria, Equilibrium constant in gaseous systems. Relationship between KP and Kc – Heterogeneous Equilibria – Applications of Equilibrium constant – Relationship between Equilibrium constant K, reaction quotient Q and Gibbs energy G – Factors affecting Equilibria-Le-chatelier principle application – to industrial synthesis of Ammonia and Sulphur trioxide – Ionic Equilibrium in solutions – Acids, bases and salts- Arrhenius, Bronsted-Lowry and Lewis concepts of acids and bases – Ionisation of Acids and Bases –Ionisation constant of water and it’s ionic product- pH scale-ionisation constants of weak acids-ionisation of weak bases-relation between Ka and Kb-Di and poly basic acids and di and 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 – Buffer solutions-designing of buffer solution-Preparation of Acidic buffer – Solubility Equilibria of sparingly soluble salts. Solubility – product constant Common ion effect on solubility of Ionic salts.
8. HYDROGEN AND ITS COMPOUNDS:
Position of hydrogen in the periodic table – Dihydrogen-Occurance and Isotopes – Preparation of Dihydrogen – Properties of Dihydrogen – Hydrides: Ionic, covalent, and non-stiochiometric hydrides – Water: Physical properties; structure of water, ice – Chemical properties of water; hard and soft water Temporary and permanent hardness of water – Hydrogen peroxide: Preparation; Physical properties; structure and chemical properties; storage and uses – Heavy Water – Hydrogen as a fuel.
9. THE s – BLOCK ELEMENTS:
(ALKALI AND ALKALINE EARTH METALS) – Group 1 Elements – Alkali metals; Electronic configurations; – Atomic and Ionic radii; Ionization enthalpy; Hydration enthalpy; Physical properties; Chemical properties; Uses – General characteristics of the compounds of the alkali metals: Oxides; Halides; Salts of Oxy Acids – Anomalous properties of Lithium: Differences and similarities with other alkali metals. Diagonal relationship; similarities between Lithium and Magnesium – Some important compounds of Sodium: Sodium Carbonate; Sodium Chloride; Sodium Hydroxide; Sodium hydrogen carbonate – Biological importance of Sodium and Potassium – Group 2 Elements: Alkaline earth elements; Electronic configuration – atomic and ionic radii – Ionization enthalpy; Hydration enthalpy; Physical properties, Chemical properties; Uses – General characteristics of compounds of the Alkaline Earth Metals: Oxides, hydroxides, halides, salts of Oxyacids – (Carbonates; Sulphates and Nitrates) – Anomalous behavior of Beryllium; its diagonal relationship with Aluminum – Some important compounds of calcium: Preparation and uses of Calcium Oxide ; Calcium Hydroxide; Calcium Carbonate;Plaster of Paris; Cement – Biological importance of Calcium and Magnesium.
10. P- BLOCK ELEMENTS GROUP – 13 ( BORON FAMILY):
General introduction – Electronic configuration, Atomic radii, Ionization enthalpy, Electro negativity; Physical & Chemical properties – Important trends and anomalous properties of boron – Some important compounds of boron – Borax, Ortho boric acid,diborane – Uses of boron, aluminium and their compounds.

11. p-BLOCK ELEMENTS – GROUP – 14 ( CARBON FAMILY):
General introduction – Electronic configuration, Atomic radii, Ionization enthalpy, Electro negativity; Physical & Chemical properties – Important trends and anomalous properties of carbon – Allotropes of carbon – Uses of carbon – Some important compounds of carbon and silicon – carbonmonoxide, carbon dioxide,Silica, silicones, silicates and zeolites.
12. ENVIRONMENTAL CHEMISTRY:
Definition of terms: Air, Water and Soil Pollutions – Environmental Pollution – Atmospheric pollution; Tropospheric Pollution; Gaseous Air Pollutants (Oxides of Sulphur; Oxides of Nitrogen; Hydro Carbons; Oxides of Carbon (CO; CO2) – Global warming and Green house effect – Acid Rain- Particulate Pollutants- Smog – Stratospheric Pollution: Formation and breakdown of Ozone- Ozone hole- effects of depletion of the Ozone layer – Water Pollution: Causes of Water Pollution; International standards for drinking water – Soil Pollution: Pesticides, Industrial Wastes. Strategies to control environmental pollution- waste Management- collection and disposal – Green Chemistry: Green chemistry in day-to-day life; Dry cleaning of clothes; Bleaching of paper; Synthesis of chemicals.
13. ORGANIC CHEMISTRY-SOME BASIC PRINCIPLES AND TECHNIQUES AND HYDROCARBONS:
General introduction – Tetravalency of Carbon: shapes of organic compounds – Structural representations of organic compounds – Classification of organic compounds – Nomenclature of organic compounds – Isomerism – Fundamental concepts in organic reaction mechanisms – Fission of covalent bond – Nucleophiles and electrophiles – Electron movements in organic reactions – Electron displacement effects in covalent bonds-Types of Organic reactions – Methods of purification of organic compounds – Qualitative elemental analysis of organic compounds – Quantitative elemental analysis of organic compounds – HYDROCARBONS: Classification of Hydrocarbons – Alkanes – Nomenclature, isomerism (structural and conformations of ethane only) – Preparation of alkanes – Properties – Physical properties and chemical Reactivity, Substitution reactions – Halogenation(free radical mechanism), Combustion, Controlled – Oxidation, Isomerisation, Aromatization, reaction with steam and Pyrolysis – Alkenes- Nomenclature, structure of ethene, Isomerism(structural and geometrical) – Methods of preparation Properties- Physical and chemical reactions: Addition of Hydrogen, halogen, water, sulphuric acid, Hydrogen halides (Mechanism- ionic and peroxide effect, Markovnikov’s , antiMarkovnikov’s or Kharasch effect). Oxidation, Ozonolysis and Polymerization – Alkynes – Nomenclature and isomerism, structure of acetylene. Methods of preparation of acetylene – Physical properties, Chemical reactions- acidic character of acetylene, addition reactions- of hydrogen, Halogen, Hydrogen halides and water. Polymerization – Aromatic Hydrocarbons – Nomenclature and isomerism. Structure of benzene, Resonance and aromaticity – Preparation of benzene. Physical properties. Chemical properties: Mechanism of electrophilic substitution. Electrophilic substitution reactions- Nitration, Sulphonation, Halogenation, Friedel-Craft’ alkylation and acylation – Directive influence of functional groups in mono substituted benzene, Carcinogenicity and toxicity.
14. SOLID STATE:
General characteristics of solid state – Amorphous and crystalline solids – Classification of crystalline solids based on different binding forces (molecular, ionic, metallic and covalent solids ) – Probing the structure of solids: X-ray crystallography – Crystal lattices and unit cells .Bravais lattices primitive and centred unit cells – Number of atoms in a unit cell (primitive, body centred and face centred cubic unit cell) – Close packed structures: Close packing in one dimension, in two dimensions and in three dimensions- tetrahedral and octahedral voids- formula of a compound and number of voids filled- locating tetrahedral and octahedral voids – Packing efficiency in simple cubic, bcc and in hcp, ccp lattice. – Calculations involving unit cell dimensions – density of the unit cell – Imperfections in solids-types of point defects-stoichiometric and non-stoichiometric defects – Electrical properties-conduction of electricity in metals, semiconductors and insulators- band theory of metals – Magnetic properties.
15. SOLUTIONS:
Types of solutions – Expressing concentration of solutions-mass percentage, volume percentage, mass by volume percentage, parts per million, mole fraction, molarity and molality – Solubility: Solubility of a solid in a liquid, solubility of a gas in a liquid,Henry’s law – Vapour pressure of liquid solutions: vapour pressure of liquid- liquid solutions. Raoult’s law as a special case of Henry’s law -vapour pressure of solutions of solids in liquids – Ideal and non-ideal solutions – Colligative properties and determination of molar mass-relative lowering of vapour pressure-elevation of boiling point-depression of freezing point-osmosis and osmotic pressure-reverse osmosis and water purification – Abnormal molar masses-van’t Hoff factor.
16. ELECTROCHEMISTRY AND CHEMICAL KINETICS: ELECTROCHEMISTRY:
Electrochemical cells – Galvanic cells :measurement of electrode potentials – Nernst equation-equilibrium constant from Nernst equation- electrochemical cell and Gibbs energy of the cell reaction – Conductance of electrolytic solutions- measurement of the conductivity of ionic solutions-variation of conductivity and molar conductivity with concentration-strong electrolytes and weak electrolytes-applications of Kohlrausch’s law – Electrolytic cells and electrolysis: Faraday’s laws of electrolysis-products of electrolysis – Batteries: primary batteries and secondary batteries – Fuel cells – Corrosion of metals-Hydrogen economy – CHEMICAL KINETICS – Rate of a chemical reaction – Factors influencing rate of a reaction: dependance of rate on concentration- rate expression and rate constant- order of a reaction, molecularity of a reaction – Integrated rate equations-zero order reactions-first order reactions-half life of a reaction – Pseudo first order reaction – Temperature dependence of the rate of a reaction -effect of catalyst – Collision theory of chemical reaction rates.
17. SURFACE CHEMISTRY:
Adsorption and absorption: Distinction between adsorption and absorption- mechanism of adsorption-types of adsorption- characteristics of physisorption-characteristics of chemisorptions-adsorption isotherms- adsorption from solution phase – applications of adsorption – Catalysis: Catalysts, promoters and poisons-auto catalysis- homogeneous and heterogeneous catalysis – adsorption theory of heterogeneous catalysis – important features of solid catalysts: (a)activity (b)selectivity-shape-selective catalysis by zeolites- enzyme catalysis-characteristics and mechanism- catalysts in industry – Colloids – Classification of colloids: Classification based on physical state of dispersed phase and dispersion medium- classification based on nature of interaction between dispersed phase and dispersion medium- classification based on type of particles of the dispersed phase- multi molecular, macromolecular and associated colloids- cleansing action of soaps-preparation of colloids-purification of colloidal solutions- properties of colloidal solutions: Tyndal effect, colour,Brownian movement-charge on colloidal particles, electrophoresis – Emulsions – Colloids Around us- application of colloids.
18. GENERAL PRINCIPLES OF METALLURGY:
Occurrence of metals – Concentration of ores – levigation, magnetic separation, froth floatation, leaching – Extraction of crude metal from concentrated ore-conversion to oxide, reduction of oxide to the metal – Thermodynamic Principles of metallurgy-Ellingham diagram-limitations-applications-extraction of iron, copper and zinc from their oxides- Electrochemical principles of metallurgy – Oxidation and reduction – Refining of crude metal-distillation, liquation poling, electrolysis, zone refining and vapour phase refining -Uses of aluminium, copper, zinc and iron.

19. p-BLOCK ELEMENTS:
GROUP-15 ELEMENTS – Occurance- electronic configuration, atomic and ionic radii, ionisation energy,electronegativity, physical and chemical properties – Dinitrogen-preparation, properties and uses – Compounds of nitrogen-preparation and properties of ammonia – Oxides of nitrogen – Preparation and properties of nitric acid – Phosphorous-allotropic forms – Phosphine-preparation and properties – Phosphorous halides – Oxoacids of phosphorous – GROUP-16 ELEMENTS – Occurance-electronic configuration, atomic and ionic radii, ionisation enthalpy,electron gain enthalpy, electronegativity,physical and chemical properties – Dioxygen-preparation, properties and uses – Simple oxides – Ozone-preparation,properties, structure and uses – Sulphur-allotropic forms – Sulphur dioxide-preparation, properties and uses – Oxoacids of sulphur – Sulphuric acid-industrial process of manufacture, properties and uses – GROUP-17 ELEMENTS – Occurance, electronic configuration, atomic and ionic radii, ionisation enthalpy, electron gain enthalpy, electronegativity ,physical and chemical properties – Chlorine-preparation, properties and uses – Hydrogen chloride- preparation, properties and uses – Oxoacids of halogens – Interhalogen compounds – GROUP-18 ELEMENTS – Occurance, electronic configuration, ionisation enthalpy,atomic radii electron gain enthalpy, physical and chemical properties (a) Xenon-fluorine compounds-XeF2,XeF4 and XeF6 –preparation, hydrolysis and formation of fluoro anions-structures of XeF2, XeF4 and XeF6 (b) Xenon-oxygen compounds XeO3 and XeOF4 – their formation and structures.
20. d AND f BLOCK ELEMENTS & COORDINATION COMPOUNDS
“d AND f BLOCK ELEMENTS: Position in the periodic table – Electronic configuration of the d-block elements – General properties of the transition elements (d-block) -physical properties, variation in atomic and ionic sizes of transition series, ionisation enthalpies, oxidation states,trends in the M²+/M and M³+/M²+ standard_electrode_ potentials, trends in stability of higher oxidation states, chemical reactivity and values, magnetic properties, formation of coloured ions, formation of complex compounds, catalytic properties, formation of interstitial compounds, alloy formation – Some important compounds of transition elements-oxides and oxoanions of metals – preparation and properties of potassium dichromate and potassium permanganate-structures of chromate, dichromate, manganate and permanganate ions – Inner transition elements (f-block) -lanthanoids- electronic configuration-atomic and ionic sizes-oxidation states- general characteristics – Actinoids-electronic configuration atomic and ionic sizes, oxidation states, general characteristics and comparision with lanthanoids – Some applications of d and f block elements.
COORDINATION COMPOUNDS : Werner’s theory of coordination compounds – Definitions of some terms used in coordination compounds – Nomenclature of coordination compounds – IUPAC nomenclature – Isomerism in coordination compounds – (a) Stereo isomerism-Geometrical and optical isomerism (b) Structural isomerism-linkage, coordination, ionisation and solvate isomerism – Bonding in coordination compounds. (a)Valence bond theory – magnetic properties of coordination compounds-limitations of valence bond theory
(b) Crystal field theory (i) Crystal field splitting in octahedral and tetrahedral coordination entities (ii) Colour in coordination compounds – limitations of crystal field theory – Bonding in metal carbonyls – Stability of coordination compounds – Importance and applications of coordination compounds.”
21. POLYMERS:
Classification of Polymers – Classification based on source, structure, mode of polymerization, molecular forces and growth polymerization – Types of polymerization reactions – addition polymerization or chain growth polymerization – ionic polymerization, free radical mechanism-preparation of addition polymers-polythene, teflon and polyacrylonitrile – condensation polymerization or step growth polymerization-polyamides – preparation of Nylon 6,6 and nylon 6-poly esters- terylene – bakelite, melamine, formaldehyde polymer – copolymerization-Rubber-natural rubber-vulcanisation of rubber-Synthetic rubbers-preparation of neoprene and buna-N – Molecular mass of polymers-number average and weight average molecular masses- poly dispersity index(PDI) – Biodegradable polymers-PHBV, Nylon 2-nylon 6 – Polymers of commercial importance- poly propene, poly styrene, poly vinyl chloride (PVC), urea – formaldehyde resin, glyptal, bakelite- their monomers, structures and uses.
22. BIOMOLECULES:
Carbohydrates – Classification of carbohydrates – Monosaccharides: preparation of glucose from sucrose and starch – Properties and structure of glucose- D,L configurations of glucose – Structure of fructose Disaccharides: Sucrose – preparation, structure-Invert sugar- Structures of maltose and lactose-Polysaccharides: Structures of starch cellulose and glycogen- Importance of carbohydrates – Aminoacids: Natural aminoacids-classification of aminoacids – structures and D and L forms – Zwitter ions Proteins: Structures, classification, fibrous and globular – primary, secondary, tertiary and quarternary structures of proteins – Denaturation of proteins – Enzymes: Enzymes, mechanism of enzyme action – Vitamins: Vitamin-names- classification of vitamins – sources of vitamins-deficiency diseases of different types of vitamins -Nucleic acids: chemical composition of nucleic acids, structures of nucleic acids, DNA finger printing biological functions of nucleic acids – Hormones.
23. CHEMISTRY IN EVERYDAY LIFE:
Drugs and their classification: (a) Classification of drugs on the basis of pharmocological effect (b) Classification of drugs on the basis of drug action (c) Classification of drugs on the basis of chemical structure (d) Classification of drugs on the basis of molecular targets – Drug-Target interaction-Enzymes as drug targets (a) Catalytic action of enzymes (b) Drug-enzyme interaction Receptors as drug targets – Therapeutic action of different classes of drugs: antacids, antihistamines, neurologically active drugs: tranquilizers, analgesics–non- narcotic, narcotic analgesics, antimicrobials-antibiotics, antiseptics and disinfectants – antifertility drugs – Chemicals in food- artificial sweetening agents, food preservatives, antioxidants in food – Cleansing agents-soaps and synthetic detergents.
24. HALOALKANES AND HALOARENES:
Classification and nomenclature – Nature of C-X bond – Methods of preparation: Alkyl halides and aryl halides-from alcohols, from hydrocarbons (a)by free radical halogenation (b) by electrophilic substitution (c) by replacement of diazonium group (Sand-Meyer reaction) (d) by the addition of hydrogen halides and halogens to alkenes – by halogen exchange – Physical properties – melting and boiling points, density and solubility – Chemical reactions: Reactions of haloalkanes (i)Nucleophilic substitution reactions (a) SN² mechanism (b) SN¹ mechanism (c) stereochemical aspects of nucleophilic substitution reactions -optical activity (ii) Elimination reactions (iii) Reaction with metals – Reactions of haloarenes: (i)Nucleophilic substitution (ii)Electrophilic substitution and (iii) Reaction with metals – Polyhalogen compounds: Uses and environmental effects of dichloro methane, trichloromethane, triiodomethane, tetrachloro methane, freons and DDT.
25. ORGANIC COMPOUNDS CONTAINING C, H AND O:
(Alcohols, Aldehydes, Phenols, Ethers, Ketones and arboxylic acids) – ALCOHOLS, PHENOLS AND ETHERS – Alcohols, phenols and ethers – classification – Nomenclature: (a)Alcohols, (b)phenols and (c)ethers – Structures of hydroxy and ether functional groups -Methods of preparation: Alcohols from alkenes and carbonyl compounds- Phenols from haloarenes, benzene sulphonic acid, diazonium salts, cumene – Physical propertics of alcohols and phenols – Chemical reactions of alcohols and phenols (i) Reactions involving cleavage of O-H bond-Acidity of alcohols and phenols, esterification (ii) Reactions involving cleavage of C-O bond- reactions with HX, PX3, dehydration and oxidation (iii) Reactions of phenols- electrophilic aromatic substitution, Kolbe’s reaction, Reimer – Tiemann reaction, reaction with zinc dust, oxidation – Commercially important alcohols (methanol,ethanol) – Ethers–Methods of preparation: By dehydration of alcohols, Williamson synthesis- Physical properties-Chemical reactions: Cleavage of C-O bond and electrophilic substitution of aromatic ethers – ALDEHYDES AND KETONES – Nomenclature and structure of carbonyl group – Preparation of aldehydes and ketones (1) by oxidation of alcohols (2) by dehydrogenation of alcohols (3) from hydrocarbons –Preparation of aldehydes (1) from acyl chlorides (2) from nitriles and esters (3) from hydrocarbons-Preparation of ketones (1) from acyl chlorides (2) from nitriles (3) from benzene or substituted benzenes – Physical properties of aldehydes and ketones – Chemical reactions of aldehydes and ketones-nucleophilic addition, reduction, oxidation, reactions due to – Hydrogen and other reactions (Cannizzaro reaction, electrophilic substitution reaction) – Uses of aldehydes and ketones – CARBOXYLIC ACIDS – Nomenclature and structure of carboxyl group – Methods of preparation of carboxylic acids- (1)from primary alcohols and aldehydes (2) from alkylbenzenes (3)from nitriles and amides (4)from Grignard reagents (5) from acyl halides and anhydrides (6) from esters – Physical properties – Chemical reactions: (i) Reactions involving cleavage of O-H bond-acidity, reactions with metals and alkalies (ii) Reactions involving cleavage of C-OH bond-formation of anhydride, reactions with PCl5, PCl3, SOCl2, esterification and reaction with ammonia (iii) Reactions involving -COOH group-reduction, decarboxylation (iv) Substitution reactions in the hydrocarbon part – halogenation and ring substitution – Uses of carboxylic acids.
26. ORGANIC COMPOUNDS:
“CONTAINING NITROGEN – I. AMINES – Structure of amines – Classification – Nomenclature – Preparation of amines: reduction of nitro compounds, ammonolysis of alkyl halides, reduction of nitriles, reduction of amides, Gabriel phthalimide synthesis and Hoffmann bromamide degradation reaction – Physical properties – Chemical reactions: basic character of amines, alkylation, acylation, carbyl amine reaction, reaction with nitrous acid, reaction with aryl sulphonyl chloride, electrophilic substitution of aromatic amines-bromination, nitration and sulphonation – II. DIAZONIUM SALTS – Methods of preparation of diazonium salts (by diazotization) Physical properties – Chemical reactions. Reactions involving displacement of Nitrogen; Sandmeyer reaction, Gatterman reaction, replacement by i) iodiode and fluoride ions ii) hydrogen, hydroxyl and Nitro groups; Reactions involving retention of diazo group; coupling reactions; Importance of diazonium salts in synthesis of aromatic compounds.
III. CYANIDES AND ISOCYANIDES – Structure and nomenclature of cyanides and isocyanides – Preparation, physical properties and chemical reactions of cyanides and isocyanides and uses.”

Preparation Tips for LAW Graduates

July 14, 2016June 17, 2016 by Rohit

TIPS FOR LAW GRADUATES

Law is set of rules that enforced in the society to create a fear in them to not make any mistake or any crime. Law has been mainly developed in the society to create an awareness in the people to follow various rules and regulations in them Many of the citizen who have aim to take this a their profession a they have a passion in this field. The interested people need not be good in their speech. While in the course of time during their education, practice and by their hard work they can develop their skills in this field. The main skill of the lawyer is to create questions about the situations around them. Preparation Tips for LAW Graduates

The qualification of a lawyer is he/she must have a LLB degree. The private and government law colleges prevail in the country. There are about 1500 law colleges. These colleges must be recognized by the Bar Council of India. Students can option two types of streams which are 3 years and 5 years course period. Five years course period is for candidates who option law after completing their 10^th/12^th. Three years course period are referred for candidates who option after completing any Bachelor’s degree. At present there are 17 specialized Law Universities which conduct a common admission test for their candidates for an admission at their respective Universities.

Law graduates can opt different careers for them. The lawyers can be at courts for solving the disputes or litigation of the public. A legal lawyer can be hired by an organization for their confidential and legal problem. When a lawyer higher studies or research in their studies, they can pursue their career as a professor/Lecturer in various law colleges which are more wanted currently.

The students who are willing to join Law colleges who are in Economically Weaker Sections can select government aided colleges for their financial support. The National Law colleges are more expensive. The fees may be between 30,000 to 1,20,000 per annum excluding their boarding, transportation and other charges.

The great leaders in the society were lawyers. The lawyers must have confidence to solve any problem. The skill developed by them must be helpful to the society. Lawyers can build a society with less crime rate.

National Institute of Technology (NIT) Durgapur – Admissions, Courses

July 4, 2016June 17, 2016 by Rohit

ADMISSIONS OPEN AT NIT, DURGAPUR

National Institute of Technology, Durgapur which is one of the ancient institutions in India. The main mission of the institution is to bring engineering education in India. The institution consists of Undergraduate, Post Graduate and Doctor of Philosophy courses. The admission for the Post Graduate and PhD course has been started. The last date for application is June 24.

Admissions

The Admissions for Master degree and PhD courses in the NIT, Durgapur is a dream for many students. The institution has released its official notification regarding the above.

Eligibility Criteria

Master’s Degree Courses

The candidate who likes to pursue Post graduate course in this institution must have the completed a Undergraduate course in its relevant area from a recognized University/Institution and must have aggregate of 6.5 out of 10

PhD Courses

The candidate interested in pursuing PhD courses must have a Bachelor’s degree and Master’s Degree in Engineering/Architecture/Pharmacy/Technology from a recognized University/Institution. The CGPA (Cumulative Grade Point Average) for the candidate must be 7.5 or 70% based on the institution recognized marks

Selection Procedure

Written Test will be conducted for screening the candidates. The selected candidates from the screening test are called for the interview process. The selection process is strictly based on the marks scored by the candidates in the written test

Application fees

The candidate must pay application fee for the admission process
Master’s degree -1000
PhD -1500

How to Apply

Log onto the official website nitdgp.ac.in
Read the instruction provided to fill the form
Fill the online application form with mandatory fields
Upload the photo and signature of the candidate
Pay the fees using online or offline modes
Online mode of transaction involves Net Banking, Credit/Debit Cards
Offline mode of transaction involves DD, E-challan
Submit the application
Take the printout for future reference

Remember the dates

Last date to submit the application: June 24
Last date to take the printed version: June 31
Written Test and Viva Voce conducted for M.Tech courses: July 11 to 13
Written Test and Viva Voce conducted for PhD courses: July 14 to 15

Reform of Syllabus by ICSE

July 4, 2016June 17, 2016 by Rohit

Reform of Syllabus by ICSE

The Central Board of Secondary Education is one of the Board of Education which mainly empowers best education to all the public and private schools. The Central Board of Secondary Education consists of excellent syllabus which is mainly governed by Union Government of India. The CBSE conducts different entrance exams like JEE Main which is an IIT entrance Test, All India Pre Medical Test for medical entrance and National Eligibility Test for Lecturers.

The exams are mainly based on its syllabus. Due to these reasons, many students who are interested in these areas move from their Board of Education to CBSE. Following these reasons, the ICSE has decided to reform its syllabus and to conduct a competitive exam.

The JEE Main exam is one of the toughest exam to overcome the exam, many students are attending coaching classes which increases their stress and less their study hours. The Council of Indian School Certificate Examination has determined to forward a letter to government to be a neutral body and CBSE alone cannot conduct any examination.

The streams of both the boards are same which are Mathematics, Physics, Chemistry and Biology. The merging of the subjects has been stopped while the students selecting the streams after their 10^th exams, the decision will be a main drawback for them.

The volume of the books will be reduced and the reference for the syllabus shall be NCERT books. The each subjects contain two volume of books which will make a fear in the mind of students about their education pattern. By these kind of activities pupil enlighten their mind with these activities to build a confidence in them. When these education pattern changes, the students will not consider studies as stress but as strength.

NCERT Solution to Class XI Mathematics

August 19, 2019May 25, 2016 by M Prakash

Sets Solutions

Relations and Functions Solutions

Trigonometric Functions Solutions

Principle of Mathematical Induction Solutions

Complex Numbers and Quadratic Equations Solutions

Linear Inequalities Solutions

15th Annual Convocation of VTU on 5th May 2016

April 7, 2016 by bn Mishra

Visvesvaraya Technological University has announced 15th Annual Convocation of the University to be held on 5th May 2016 at VTU Belagavi, Karnataka.

Syllabus for BITSAT Chemistry 2016

January 23, 2016 by

Part II: Chemistry

1. States of Matter

1.1   Measurement: Physical quantities and SI units, Dimensional analysis, Precision, Significant figures.
1.2   Chemical reactions: Laws of chemical combination, Dalton’s atomic theory; Mole concept; Atomic, molecular and molar masses; Percentage composition empirical & molecular formula; Balanced chemical equations & stoichiometry
1.3   Three states of matter, intermolecular interactions, types of bonding, melting and boiling points
Gaseous state: Gas Laws, ideal behavior, ideal gas equation, empirical derivation of gas equation, Avogadro number, Kinetic theory – Maxwell distribution of velocities, Average, root mean square and most probable velocities and relation to temperature, Diffusion; Deviation from ideal behaviour – Critical temperature, Liquefaction of gases, van der Waals equation.
1.4   Liquid state: Vapour pressure, surface tension, viscosity.
1.5   Solid state: Classification; Space lattices & crystal systems; Unit cell in two dimensional and three dimensional lattices, calculation of density of unit cell – Cubic & hexagonal systems; Close packing; Crystal structures: Simple AB and AB2 type ionic crystals, covalent crystals – diamond & graphite, metals. Voids, number of atoms per unit cell in a cubic unit cell, Imperfections- Point defects, non-stoichiometric crystals; Electrical, magnetic and dielectric properties; Amorphous solids – qualitative description. Band theory of metals, conductors, semiconductors and insulators, and n- and p- type semiconductors.

2. Atomic Structure

2.1 Introduction: Radioactivity, Subatomic particles; Atomic number, isotopes and isobars, Thompson’s model and its limitations, Rutherford’s picture of atom and its limitations; Hydrogen atom spectrum and Bohr model and its limitations.
2.2 Quantum mechanics: Wave-particle duality – de Broglie relation, Uncertainty principle; Hydrogen atom: Quantum numbers and wavefunctions, atomic orbitals and their shapes (s, p, and d), Spin quantum number.
2.3 Many electron atoms: Pauli exclusion principle; Aufbau principle and the electronic configuration of atoms, Hund’s rule.
2.4 Periodicity: Brief history of the development of periodic tables Periodic law and the modern periodic table; Types of elements: s, p, d, and f blocks; Periodic trends: ionization energy, atomic, and ionic radii, inter gas radii, electron affinity, electro negativity and valency. Nomenclature of elements with atomic number greater than 100.

3. Chemical Bonding & Molecular Structure

3.1 Valence electrons, Ionic Bond: Lattice Energy and Born-Haber cycle; Covalent character of ionic bonds and polar character of covalent bond, bond parameters
3.2 Molecular Structure: Lewis picture & resonance structures, VSEPR model & molecular shapes
3.3 Covalent Bond: Valence Bond Theory- Orbital overlap, Directionality of bonds & hybridization (s, p & d orbitals only), Resonance; Molecular orbital theory- Methodology, Orbital energy level diagram, Bond order, Magnetic properties for homonuclear diatomic species (qualitative idea only).
3.4 Metallic Bond: Qualitative description.
3.5 Intermolecular Forces: Polarity; Dipole moments; Hydrogen Bond.

4. Thermodynamics

4.1 Basic Concepts: Systems and surroundings; State functions; Intensive & Extensive Properties; Zeroth Law and Temperature
4.2 First Law of Thermodynamics: Work, internal energy, heat, enthalpy, heat capacities and specific heats, measurements of ΔU and ΔH, Enthalpies of formation, phase transformation, ionization, electron gain; Thermochemistry; Hess’s Law, Enthalpy of bond dissociation, combustion, atomization, sublimation, solution and dilution
4.3 Second Law: Spontaneous and reversible processes; entropy; Gibbs free energy related to spontaneity and non-spontaneity, non-mechanical work; Standard free energies of formation, free energy change and chemical equilibrium
4.4 Third Law: Introduction

5. Physical and Chemical Equilibria

5.1 Concentration Units: Mole Fraction, Molarity, and Molality
5.2 Solutions: Solubility of solids and gases in liquids, Vapour Pressure, Raoult’s law, Relative lowering of vapour pressure, depression in freezing point; elevation in boiling point; osmotic pressure, determination of molecular mass; solid solutions, abnormal molecular mass, van’t Hoff factor. Equilibrium: Dynamic nature of equilibrium, law of mass action
5.3 Physical Equilibrium: Equilibria involving physical changes (solid-liquid, liquid-gas, solid-gas), Surface chemistry, Adsorption, Physical and Chemical adsorption, Langmuir Isotherm, Colloids and emulsion, classification, preparation, uses.
5.4 Chemical Equilibria: Equilibrium constants (KP, KC), Factors affecting equilibrium, Le-Chatelier’s principle.
5.5 Ionic Equilibria: Strong and Weak electrolytes, Acids and Bases (Arrhenius, Lewis, Lowry and Bronsted) and their dissociation; degree of ionization, Ionization of Water; ionization of polybasic acids, pH; Buffer solutions; Henderson equation, Acid-base titrations; Hydrolysis; Solubility Product of Sparingly Soluble Salts; Common Ion Effect.
5.6 Factors Affecting Equilibria: Concentration, Temperature, Pressure, Catalysts, Significance of G and G0 in Chemical Equilibria.

6. Electrochemistry

6.1 Redox Reactions: Oxidation-reduction reactions (electron transfer concept); Oxidation number; Balancing of redox reactions; Electrochemical cells and cell reactions; Standard electrode potentials; EMF of Galvanic cells; Nernst equation; Factors affecting the electrode potential; Gibbs energy change and cell potential; Secondary cells; dry cells, Fuel cells; Corrosion and its prevention.
6.2 Electrolytic Conduction: Electrolytic Conductance; Specific and molar conductivities; variations of conductivity with concentration , Kolhrausch’s Law and its application, Electrolysis, Faraday’s laws of electrolysis; Coulometer; Electrode potential and electrolysis, Commercial production of the chemicals, NaOH, Na, Al, Cl2 & F2.

7. Chemical Kinetics

7.1 Aspects of Kinetics: Rate and Rate expression of a reaction; Rate constant; Order and molecularity of the reaction; Integrated rate expressions and half life for zero and first order reactions.
7.2 Factor Affecting the Rate of the Reactions: Concentration of the reactants, catalyst; size of particles, Temperature dependence of rate constant concept of collision theory (elementary idea, no mathematical treatment); Activation energy; Catalysis, Surface catalysis, enzymes, zeolites; Factors affecting rate of collisions between molecules.
7.3 Mechanism of Reaction: Elementary reactions; Complex reactions; Reactions involving two/three steps only.
7.4 Surface Chemistry: Adsorption – physisorption and chemisorption; factors affecting adsorption of gasses on solids; catalysis: homogeneous and heterogeneous, activity and selectivity: enzyme catalysis, colloidal state: distinction between true solutions, colloids and suspensions; lyophillic, lyophobic multi molecular and macromolecular colloids; properties of colloids; Tyndall effect, Brownian movement, electrophoresis, coagulations; emulsions – types of emulsions.

8. Hydrogen and s-block elements

8.1   Hydrogen: Element: unique position in periodic table, occurrence, isotopes; Dihydrogen: preparation, properties, reactions, and uses; Molecular, saline, ionic, covalent, interstitial hydrides; Water: Properties; Structure and aggregation of water molecules; Heavy water; Hydrogen peroxide: preparation, reaction, structure & use, Hydrogen as a fuel.
8.2   s-block elements: Abundance and occurrence; Anomalous properties of the first elements in each group; diagonal relationships; trends in the variation of properties (ionization energy, atomic & ionic radii).
8.3   Alkali metals: Lithium, sodium and potassium: occurrence, extraction, reactivity, and electrode potentials; Biological importance; Reactions with oxygen, hydrogen, halogens water and liquid ammonia; Basic nature of oxides and hydroxides; Halides; Properties and uses of compounds such as NaCl, Na2CO3, NaHCO3, NaOH, KCl, and KOH.
8.4   Alkaline earth metals: Magnesium and calcium: Occurrence, extraction, reactivity and electrode potentials; Reactions with O2, H2O, H2 and halogens; Solubility and thermal stability of oxo salts; Biological importance of Ca and Mg; Preparation, properties and uses of important compounds such as CaO, Ca(OH)2, plaster of Paris, MgSO4, MgCl2, CaCO3, and CaSO4; Lime and limestone, cement.

9. p- d- and f-block elements

9.1   General: Abundance, distribution, physical and chemical properties, isolation and uses of elements; Trends in chemical reactivity of elements of a group; electronic configuration, oxidation states; anomalous properties of first element of each group.
9.2   Group 13 elements: Boron; Properties and uses of borax, boric acid, boron hydrides & halides. Reaction of aluminum with acids and alkalis;
9.3   Group 14 elements: Carbon: carbon catenation, physical & chemical properties, uses, allotropes (graphite, diamond, fullerenes), oxides, halides and sulphides, carbides; Silicon: Silica, silicates, silicone, silicon tetrachloride, Zeolites, and their uses
9.4   Group 15 elements: Dinitrogen; Preparation, reactivity and uses of nitrogen; Industrial and biological nitrogen fixation; Compound of nitrogen; Ammonia: Haber’s process, properties and reactions; Oxides of nitrogen and their structures; Properties and Ostwald’s process of nitric acid production; Fertilizers – NPK type; Production of phosphorus; Allotropes of phosphorus; Preparation, structure and properties of hydrides, oxides, oxoacids (elementary idea only) and halides of phosphorus, phosphine.
9.5   Group 16 elements: Isolation and chemical reactivity of dioxygen; Acidic, basic and amphoteric oxides; Preparation, structure and properties of ozone; Allotropes of sulphur; Preparation/production properties and uses of sulphur dioxide and sulphuric acid; Structure and properties of oxides, oxoacids (structures only), hydrides and halides of sulphur.
9.6   Group 17 and group 18 elements: Structure and properties of hydrides, oxides, oxoacids of halogens (structures only); preparation, properties & uses of chlorine & HCl; Inter halogen compounds; Bleaching Powder; Uses of Group 18 elements, Preparation, structure and reactions of xenon fluorides, oxides, and oxoacids.
9.7   d-Block elements: General trends in the chemistry of first row transition elements; Metallic character; Oxidation state; ionization enthalpy; Ionic radii; Color; Catalytic properties; Magnetic properties; Interstitial compounds; Occurrence and extraction of iron, copper, silver, zinc, and mercury; Alloy formation; Steel and some important alloys; preparation and properties of CuSO4, K2Cr2O7, KMnO4, Mercury halides; Silver nitrate and silver halides; Photography.
9.8   f-Block elements: Lanthanoids and actinoids; Oxidation states and chemical reactivity of lanthanoids compounds; Lanthanide contraction and its consequences, Comparison of actinoids and lanthanoids.
9.9   Coordination Compounds: Coordination number; Ligands; Werner’s coordination theory; IUPAC nomenclature; Application and importance of coordination compounds (in qualitative analysis, extraction of metals and biological systems e.g. chlorophyll, vitamin B12, and hemoglobin); Bonding: Valence-bond approach, Crystal field theory (qualitative); Stability constants; Shapes, color and magnetic properties; Isomerism including stereoisomerisms; Organometallic compounds.

10. Principles of Organic Chemistry and Hydrocarbons

10.1   Classification: General Introduction, classification based on functional groups, trivial and IUPAC nomenclature. Methods of purification: qualitative and quantitative,
10.2   Electronic displacement in a covalent bond: Inductive, resonance effects, and hyperconjugation; free radicals; carbocations, carbanions, nucleophiles and electrophiles; types of organic reactions, free radial halogenations.
10.3   Alkanes and cycloalkanes: Structural isomerism, general properties and chemical reactions, free redical helogenation, combustion and pyrolysis.
10.4   Alkenes and alkynes: General methods of preparation and reactions, physical properties, electrophilic and free radical additions, acidic character of alkynes and (1,2 and 1,4) addition to dienes.
10.5   Aromatic hydrocarbons: Sources; properties; isomerism; resonance delocalization; aromaticity; polynuclear hydrocarbons; IUPAC nomenclature; mechanism of electrophilic substitution reaction, directive influence and effect of substituents on reactivity; carcinogenicity and toxicity.
10.6   Haloalkanes and haloarenes: Physical properties, nomenclature, optical rotation, chemical reactions and mechanism of substitution reaction. Uses and environmental effects; di, tri, tetrachloromethanes, iodoform, freon and DDT.
10.7   Petroleum: Composition and refining, uses of petrochemicals.

11. Stereochemistry

11.1   Introduction: Chiral molecules; optical activity; polarimetry; R,S and D,L configurations; Fischer projections; enantiomerism; racemates; diastereomerism and meso structures.
11.2   Conformations: Ethane conformations; Newman and Sawhorse projections.
11.3   Geometrical isomerism in alkenes

12. Organic Compounds with Functional Groups Containing Oxygen and Nitrogen

12.1 General: Nomenclature, electronic structure, important methods of preparation, identification, important reactions, physical and chemical properties, uses of alcohols, phenols, ethers, aldehydes, ketones, carboxylic acids, nitro compounds, amines, diazonium salts, cyanides and isocyanides.
12.2 Specific: Reactivity of -hydrogen in carbonyl compounds, effect of substituents on alpha-carbon on acid strength, comparative reactivity of acid derivatives, mechanism of nucleophilic addition and dehydration, basic character of amines, methods of preparation, and their separation, importance of diazonium salts in synthetic organic chemistry.

13. Biological , Industrial and Environmental chemistry

13.1   The Cell: Concept of cell and energy cycle.
13.2   Carbohydrates: Classification; Monosaccharides; Structures of pentoses and hexoses; Anomeric carbon; Mutarotation; Simple chemical reactions of glucose, Disaccharides: reducing and non-reducing sugars – sucrose, maltose and lactose; Polysaccharides: elementary idea of structures of starch, cellulose and glycogen.
13.3   Proteins: Amino acids; Peptide bond; Polypeptides; Primary structure of proteins; Simple idea of secondary , tertiary and quarternary structures of proteins; Denaturation of proteins and enzymes.
13.4   Nucleic Acids: Types of nucleic acids; Primary building blocks of nucleic acids (chemical composition of DNA & RNA); Primary structure of DNA and its double helix; Replication; Transcription and protein synthesis; Genetic code.
13.5   Vitamins: Classification, structure, functions in biosystems; Hormones
13.6   Polymers: Classification of polymers; General methods of polymerization; Molecular mass of polymers; Biopolymers and biodegradable polymers; methods of polymerization (free radical, cationic and anionic addition polymerizations); Copolymerization: Natural rubber; Vulcanization of rubber; Synthetic rubbers. Condensation polymers.
13.7   Pollution: Environmental pollutants; soil, water and air pollution; Chemical reactions in atmosphere; Smog; Major atmospheric pollutants; Acid rain; Ozone and its reactions; Depletion of ozone layer and its effects; Industrial air pollution; Green house effect and global warming; Green Chemistry, study for control of environmental pollution.
13.8 Chemicals in medicine, health-care and food: Analgesics, Tranquilizers, antiseptics, disinfectants, anti-microbials, anti-fertility drugs, antihistamines, antibiotics, antacids; Preservatives, artificial sweetening agents, antioxidants, soaps and detergents.

14. Theoretical Principles of Experimental Chemistry

14.1   Volumetric Analysis: Principles; Standard solutions of sodium carbonate and oxalic acid; Acid-base titrations; Redox reactions involving KI, H2SO4, Na2SO3, Na2S2O3 and H2S; Potassium permanganate in acidic, basic and neutral media; Titrations of oxalic acid, ferrous ammonium sulphate with KMnO4, K2 Cr2O7/Na2S2O3, Cu(II)/Na2S2O3.
14.2   Qualitative analysis of Inorganic Salts: Principles in the determination of the cations Pb2+, Cu2+, As3+, Mn2+, Al3+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+, Fe3+, Ni2+ and the anions CO32-, S2-, SO42-, SO32-, NO2-, NO3-, Cl-, Br-, I-, PO43-, CH3COO-, C2O42-.
14.3   Physical Chemistry Experiments: preparation and crystallization of alum, copper sulphate. Benzoic acid ferrous sulphate, double salt of alum and ferrous sulphate, potassium ferric sulphate; Temperature vs. solubility; Study of pH charges by common ion effect in case of weak acids and weak bases; pH measurements of some solutions obtained from fruit juices, solutions of known and varied concentrations of acids, bases and salts using pH paper or universal indicator; Lyophilic and lyophobic sols; Dialysis; Role of emulsifying agents in emulsification. Equilibrium studies involving ferric and thiocyanate ions (ii) [Co(H2O)6]2+ and chloride ions; Enthalpy determination for strong acid vs. strong base neutralization reaction (ii) hydrogen bonding interaction between acetone and chloroform; Rates of the reaction between (i) sodium thiosulphate and hydrochloric acid, (ii) potassium iodate and sodium sulphite (iii) iodide vs. hydrogen peroxide, concentration and temperature effects in these reactions.
14.4 Purification Methods: Filtration, crystallization, sublimation, distillation, differential extraction, and chromatography. Principles of melting point and boiling point determination; principles of paper chromatographic separation – Rf values.
14.5   Qualitative Analysis of Organic Compounds: Detection of nitrogen, sulphur, phosphorous and halogens; Detection of carbohydrates, fats and proteins in foodstuff; Detection of alcoholic, phenolic, aldehydic, ketonic, carboxylic, amino groups and unsaturation.
14.6   Quantitative Analysis of Organic Compounds: Basic principles for the quantitative estimation of carbon, hydrogen, nitrogen, halogen, sulphur and phosphorous; Molecular mass determination by silver salt and chloroplatinate salt methods; Calculations of empirical and molecular formulae.
14.7   Principles of Organic Chemistry Experiments: Preparation of iodoform, acetanilide, p-nitro acetanilide, di-benzayl acetone, aniline yellow, beta-naphthol; Preparation of acetylene and study of its acidic character.
14.8   Basic Laboratory Technique: Cutting glass tube and glass rod, bending a glass tube, drawing out a glass jet, boring of cork.

CBSE Class 8 Science Syllabus

December 23, 2015 by Rohit

CBSE Class 8 Science:

This is a syllabus of elementary standard 8^th in CBSE. This covers various topics such as

Food
Materials
The world of living
Moving things, people and ideas
How things work?
Natural Phenomena

Food:

This covers various topics under “Food” such as crop production, basic practices in crop production, preparation of soil for cultivation, selection of seeds and sowing techniques, importance of manures and fertilizers, process of irrigation, weeding, harvesting and its importance, methods of storage of water for irrigation, food from animals, microorganisms, etc.

Generally, Agriculture is the cultivation of crops to provide food for all life forms. For such cultivation, soil must be replenished with the nourished manures and fertilizers which can help the seeds to germinate and grow into saplings. Also, enough amounts of other nutrients and water must be supplied at the regular intervals.

Irrigation:

The proper water supply to the plants according to its type and the season is called as irrigation. There are two types of irrigation such as Traditional irrigation and modern irrigation. Traditional irrigation is the standard method which is done with the help of human labors and animals. This is one of the cheapest irrigation methods which are done with the help of chain pump, moat and rahat. Modern irrigation method is a modern method of supplying water to the crops at the regular interval. This requires solar power or bio gas to automatically sprinkle water to the crops without any wastage.

How to protect the crop?

Crops are prone to the attacks of pests and insects. Thus, it is necessary to take required steps to protect the crop at the right time. Insects are the six leg organisms which cause heavy loss to the crops whereas pests are the organisms which cause diseases in crop plants. These can be controlled by spraying insecticides and pesticides which can prevent crops from such pests and insects.

Weeding:

The process of removing waste plants is called as weeding. Weeds If present always compete with the healthy crops in obtaining water, sunlight and nutrients. Thus, it is necessary to remove the weeds or unnecessary crops. Weeding can either be done manually by using harrow before they produce flowers and seeds or it can be tilled along with the soil to kill them. Weeds can also be destroyed by using weedicides which are poisonous to the human beings.

Harvesting:

The process of cutting the mature crop to gather the grains is called as harvesting. This can either be done manually by using a sickle or using a harvestor.

Threshing:

It is the process of separating the grains from the straw and chaff. A machine called thresher is used for this purpose.

Winnowing:

It is the process of natural wind to flow through the grains so that the lighter substances fly away allowing heavier substance falling to the ground.

Animal Husbandry:

Breeding and rearing living organisms like cow, goat for the food and other products from them. For example dairy products, poultry farming, pisiculture, sericulture, piggery, etc.,

Examples:

Give two examples for each type of crops:

Kharif crop:
Rabi crop:

Answer:

Maize and paddy
Wheat and pea

Name the microorganism which can fix the atmospheric nitrogen in the soil.

Answer: Rhizobium, azatobactor, Blue green algae, etc.

Materials:

This covers various topics such as Synthetic fibers and plastics, metals and non metals, coal and petroleum, combustion and flame, etc.

Synthetic fibers and plastics:

There are different types of fibers available such natural and synthetic fibers. Cotton is a natural fiber which is obtained from the cotton plant whereas synthetic fibers are the man-made fibers which are prepared by the many raw materials such as petrochemicals. Synthetic fibers are made up of many small units which combine to form large unit called as a polymer. Plastics are the polymers which consist of very long molecules each composed of carbon atoms linked in chains.

Metals and non-metals:

Metals are hard, strong and durable which is made used in many machineries, trains, automobiles, aeroplanes, water boiler, etc., However not all metals are hard and strong. Sodium and potassium are soft metals which can be cut with a knife whereas mercury is a liquid. Metals are very good conductors of heat. Non metals exist in three states such as solids, liquids and gas. Non metals do not conduct electricity and heat except graphite.

Coal and petroleum:

Animals and plants are drifted down to the earth after their death and decomposed to form peat. Coal was formed due to the compression of peat at high temperature and pressure. Coal is the world’s most abundant fossil fuel. Petroleum is formed from the compressed organic matter which is a dark and oily liquid with an unpleasant odour. As petroleum is lighter than that of water, the deposits of petroleum occur above the water level.

Combustion and flame:

Combustion is a chemical process which gives off heat when reacting with oxygen. Such substances are called as combustible substances. Example of such substances are LPG, Kerosene, petrol, etc. There are three types of combustion such as rapid combustion, spontaneous combustion and explosion. The substances which vaporizes while burning produced flames. Kerosene oil and molten wax are the substances that give flame while burning. There are two types of flames such as luminous flames and non-luminous flames.

Examples:

Name the petroleum product which can surface the road.

Answer: Bitumen

List the conditions under which combustion can take place?

Answer: Inflammable substance, ignition temperature and Air

The world of living:

These covers the topics such as conservation of plants and animals, cell structure and functions, reproduction in animals, etc.

Conservation of plants and animals:

Conservation of forest refers to the prevention and maintenance of animals and plants species and protecting them from various threats. Forest can be conserved by maintaining biosphere reserves, wild life sanctuaries, national and zoological parks and botanical gardens.

Cell structure and function:

Cell is a structural and functional unit of all living organisms. Every cell in the body is meant to have some basic function. For example, alveolar is an example of single cell. A group of cells which combine to perform similar function is said to be a tissue. A structure of the cell is made up of cell wall, cell membrane, cytoplasm, and the cell organelles.

Cell wall:

This is present in the structure of a plant cell which gives basic strength and rigidity to the plant body and stands erect during all environmental conditions.

Cell membrane:

This is a biological membrane which separates interior of the cells from the outside environment.

Cytoplasm:

It is a jelly like fluid which is present between the nucleus and cell membrane. Cytoplasm is a site of protein synthesis. Almost all metabolic reactions take place in cytoplasm.

Cell organelles:

These are the living structures which float in the cytoplasm of a cell.

Reproduction in animals:

This chapter widely covers the topics such as sexual and asexual reproduction in animals, Oviparous and viviparous animals.

Sexual and asexual reproduction in animals:

Reproduction is a process of developing own species. This can take place in all living organisms such as humans, animals and plants. There are two types of reproduction. They are sexual and asexual reproduction.

Sexual reproduction:

This type of reproduction involves two organisms such as male and female. Reproductive organs of female produces egg (ovum) whereas the male reproductive organs produce sperm. A zygote is the future individual formed by the fusion of egg and sperm.

Asexual Reproduction:

This is a type of reproduction where single parent gives rise to the offspring. Animals reproduce asexually by different process such as binary fission, budding, regeneration, cloning and fragmentation.

Oviparous and viviparous animals:

Oviparous animals are the animals which can lay eggs. For example: Hen, Frog, Fish, etc., These types of animals undergo external fertilization.

Viviparous animals are the animals which give birth to the young ones. For example, Lion, cat and humans. These types of animals undergo internal fertilization.

Examples:

A place where animals are protected in their natural habitats is called as ________

Answer: Wild life sanctuary

Where does the internal fertilization occur in humans?

Answer: Female body

Moving things, ideas and people:

This chapter covers various topics such as force, pressure, friction and sound. Let’s check one by one.

Force:

An interaction of one object with the other object results in force between two objects. Force has both magnitude and direction. The SI unit of force is Newton.

Pressure:

Thrust which is a force acted on an object (perpendicular to its surface) acting per unit surface area is called as pressure. The SI unit of pressure is Newton per square meter. (N/m²).

Friction:

Friction is a type of force which opposes the relative motion between two surfaces of objects in contact.

Sound:

Sound is a form of energy which causes sensation of hearing. Sound can be heard from all possible objects around us. They are produced from the vibrations caused in the object.

Examples:

Give an example of a situation in which applied force causes a change in the shape of an object.

Answer: Inflated balloon

Sound can travel through _______

Answer: Air, liquids and solids

How things work?

This chapter covers topics such as conductivity of liquids and chemical effect of electric current.

Conductivity of liquids:

Materials through which electric current can pass is called as conductors. Those materials which pass electric current through them are called as good conductors of electricity whereas those materials which do not allow electric current to pass through them are called as bad conductor of electricity.

Pure water or distilled water is a poor conductor of electricity but if any impurities present in the water, it turns to good conductor of electricity.

Chemical effect of electric current:

When an electric current is passed through a conducting solution chemical reactions are formed. This is known as chemical effect of electric current. Examples of chemical effects of electric current are:

Formation of bubbles of gas on the electrodes
Change in the color of solutions
Deposition of metals in electrodes

Examples:

When the free ends of the tester are dipped into the solution, the magnetic needle shows the deflection. Why is it so?

Answer: It is because the solution conducts electricity and the solution plays the rule of the cell.

Which of the following cannot be easily charged by friction?

A plastic scale
A woolen cloth
An inflated balloon
A Copper rod

Answer: A copper rod

Natural Phenomena:

This covers the topic such as Lighting, protection from lightning, earthquakes, etc.,

Lightning:

Lightning is occurred when friction occurs between water and droplets found in the atmosphere. In other words, lightning is cause due to the heavy electric discharge from the clouds to the earth.

Earthquakes:

A sudden violent shaking of the ground which causes great disaster to the earth.

Examples:

Which of the following is not a green gas?

Carbon dioxide
Sulphur dioxide
Nitrogen
Methane

Answer: Sulphur dioxide

State the laws of reflection?

Answer: The angle of incident is equal to the angle of reflection. The ray of incidence, the ray of reflection and the normal point of incidence lie in the same plane.

Thus, the above are the topics which are covered under the CBSE Class 8 Science.