MUEEE Chemistry Syllabus

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MUEEE 2021 Chemistry Syllabus

Section – A : Physical Chemistry Syllabus

Unit 1 : Some Basic Concepts in Chemistry

Matter and its nature, Dalton’s atomic theory; Concept of atom, molecule, element and compound; Physical quantities and their measurements in Chemistry, precision and accuracy, significant figures, S.I. Units, dimensional analysis; Laws of chemical combination; Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae; Chemical equations and stoichiometry.

Unit 2 : States of Matter

Classification of matter into solid, liquid and gaseous states.

a) Gaseous State

Measurable properties of gases; Gas laws – Boyle’s law, Charle’s law, Graham’s law of diffusion, Avogadro’s law, Dalton’s law of partial pressure; Concept of Absolute scale of temperature; Ideal gas equation, Kinetic theory of gases ( only postulates ); Concept of average, root mean square and most probable velocities; Real gases, deviation from Ideal behaviour, compressibility factor, vander Waals equation, liquefaction of gases, critical constants.

b) Liquid State

Properties of Liquids – vapour pressure, viscosity and surface tension and effect of temperature on them ( qualitative treatment only ).

c) Solid State

Classification of Solids : molecular, ionic, covalent and metallic solids, amorphous and crystalline solids ( elementary idea ); Bragg’s Law and its applications; Unit cell and lattices, packing in solids ( fcc, bcc and hcp lattices ), voids, calculations involving unit cell parameters, imperfection in solids; Electrical, magnetic and dielectric properties.

Unit 3 : Atomic Structure

Discovery of sub – atomic particles ( electron, proton and neutron ); Thomson and Rutherford atomic models and their limitations; Nature of electromagnetic radiation, photoelectric effect; Spectrum of hydrogen atom, Bohr model of hydrogen atom – its postulates, derivation of the relations for energy of the electron and radii of the different orbits, limitations of Bohr’s model; Dual nature of matter, de – Broglie’s relationship, Heisenberg uncertainty principle.

Elementary ideas of quantum mechanics, quantum mechanical model of atom, its important features, * and *2, concept of atomic orbitals as one electron wave functions; Variation of * and * 2 with r for 1s and 2s orbitals; various quantum numbers ( principal, angular momentum and magnetic quantum numbers ) and their significance; shapes of s, p and d – orbitals, electron spin and spin quantum number; Rules for filling electrons in orbitals – aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of elements, extra stability of half – filled and completely filled orbitals.

Unit 4 : Chemical Bonding and Molecular Structure

Kossel – Lewis approach to chemical bond formation, concept of ionic and covalent bonds.

a) Ionic Bonding :

Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy.

b) Covalent Bonding : Concept of electronegativity, Fajan’s rule, dipole moment; Valence Shell Electron Pair Repulsion ( VSEPR ) theory and shapes of simple molecules.

Quantum mechanical approach to covalent bonding : Valence bond theory – Its important features, concept of hybridization involving s, p and d orbitals; Resonance.

Molecular Orbital Theory : Its important features, LCAOs, types of molecular orbitals ( bonding, antibonding ), sigma and pi – bonds, molecular orbital electronic configurations of homo – nuclear diatomic molecules, concept of bond order, bond length and bond energy. Elementary idea of metallic bonding, Hydrogen bonding and its applications.

Unit 5 : Chemical Thermodynamics

Fundamentals of thermodynamics : System and surroundings, extensive and intensive properties, state functions, types of processes.

First law of thermo – dynamics : Concept of work, heat internal energy and enthalpy, heat capacity, molar heat capacity; Hess’s law of constant heat summation; Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization and solution.

Second law of thermo – dynamics : Spontaneity of processes; DS of the universe and DG of the system as criteria for spontaneity, DGo ( Standard Gibbs energy change ) and equilibrium constant.

Unit 6 : Solutions

Different methods for expressing concentration of solution – molality, molarity, mole fraction, percentage ( by volume and mass both ), vapour pressure of solutions and Raoult’s Law – Ideal and non – ideal solutions, vapour pressure – composition, plots for ideal and non – ideal solutions; Colligative properties of dilute solutions – relative lowering of vapour pressure, depression of freezing point, elevation of boiling point and osmotic pressure; Determination of molecular mass using colligative properties; Abnormal value of molar mass, Van’t Hoff factor and its significance.

Unit 7 : Equilibrium

Meaning of equilibrium, concept of dynamic equilibrium. Equilibria involving physical processes : Solid – liquid, liquid – gas and solid – gas equilibria, Henry’s law, general characterics of equilibrium involving physical processes.

Equilibria involving chemical processes : Law of chemical equilibrium, equilibrium constants ( Kp and Kc ) and their significance, significance of DG and DGo in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, effect of catalyst; Le Chatelier’s principle.

Ionic equilibrium : Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases ( Arrhenius, Br?nsted – Lowry and Lewis ) and their ionization, acid – base equilibria ( including multistage ionization ) and ionization constants, ionization of water, pH scale, common ion effect, hydrolysis of salts and pH of their solutions, solubility of sparingly soluble salts and solubility products, buffer solutions.

Unit 8 : Redox Reactions and Electrochemistry

Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, balancing of redox reactions.

Eectrolytic and metallic conduction, conductance in electrolytic solutions, specific and molar conductivities and their variation with concentration : Kohlrausch’s law and its applications.

Electro – chemical cells – Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half – cell and cell reactions, emf of a Galvanic cell and its measurement; Nernst equation and its applications; Relationship between cell potential and Gibbs’ energy change; Dry cell and lead accumulator; Fuel cells; Corrosion and its prevention.

Unit 9 : Chemical Kinetics

Rate of a chemical reaction, factors affecting the rate of reactions : concentration, temperature, pressure and catalyst; elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units, differential and integral forms of zero and first order reactions, their characteristics and half – lives, effect of temperature on rate of reactions – Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions ( no derivation ).

Unit 10 : Surface Chemistry

Adsorption : Physisorption and chemisorption and their characteristics, factors affecting adsorption of gases on solids – Freundlich and Langmuir adsorption isotherms, adsorption from solutions.

Catalysis : Homogeneous and heterogeneous, activity and selectivity of solid catalysts, enzyme catalysis and its mechanism.

Colloidal State : distinction among true solutions, colloids and suspensions, classification of colloids – lyophilic, lyophobic; multi – molecular, macromolecular and associated colloids ( micelles ),preparation and properties of colloids – Tyndall effect, Brownian movement, electrophoresis, dialysis, coagulation and flocculation; Emulsions and their characteristics.

Section – B : Inorganic Chemistry Syllabus

Unit 11 : Classification of Elements and Periodicity in Properties

Modern periodic law and present form of the periodic table, s, p, d and f block elements, periodic trends in properties of elements atomic and ionic radii, ionization enthalpy, electron gain enthalpy, valence, oxidation states and chemical reactivity.

Unit 12 : General Principles and Processes of Isolation of Metals

Modes of occurrence of elements in nature, minerals, ores; steps involved in the extraction of metals – concentration, reduction ( chemical and electrolytic methods ) and refining with special reference to the extraction of Al, Cu, Zn and Fe; Thermodynamic and electrochemical principles involved in the extraction of metals.

Unit 13 : Hydrogen

Position of hydrogen in periodic table, isotopes, preparation, properties and uses of hydrogen; Physical and chemical properties of water and heavy water; Structure, preparation, reactions and uses of hydrogen peroxide; Classification of hydrides – ionic, covalent and interstitial; Hydrogen as a fuel.

Unit 14 : S – Block Elements ( Alkali and Alkaline Earth Metals )

Group – 1 and 2 Elements

General introduction, electronic configuration and general trends in physical and chemical properties of elements, anomalous properties of the first element of each group, diagonal relationships. Preparation and properties of some important compounds – sodium carbonate, sodium chloride, sodium hydroxide and sodium hydrogen carbonate; Industrial uses of lime, limestone, Plaster of Paris and cement; Biological significance of Na, K, Mg and Ca.

Unit 15 : P – Block Elements

Unit 18 : Environmental Chemistry

General Introduction : Electronic configuration and general trends in physical and chemical properties of elements across the periods and down the groups; unique behaviour of the first element in each group.
Groupwise study of the p – block elements Group – 13 Preparation, properties and uses of boron and aluminium; Structure, properties and uses of borax, boric acid, diborane, boron trifluoride, aluminium chloride and alums.

Group – 14

Tendency for catenation; Structure, properties and uses of allotropes and oxides of carbon, silicon tetrachloride, silicates, zeolites and silicones. Group – 15 Properties and uses of nitrogen and phosphorus; Allotrophic forms of phosphorus; Preparation, properties, structure and uses of ammonia, 3 5 nitric acid, phosphine and phosphorus halides, ( PCl , PCl ); Structures of oxides and oxoacids of nitrogen and phosphorus.

Group – 16

Preparation, properties, structures and uses of dioxygen and ozone; Allotropic forms of sulphur; Preparation, properties, structures and uses of sulphur dioxide, sulphuric acid ( including its industrial preparation ); Structures of oxoacids of sulphur.

Group – 17

Preparation, properties and uses of chlorine and hydrochloric acid; Trends in the acidic nature of hydrogen halides; Structures of Interhalogen compounds and oxides and oxoacids of halogens.

Group – 18

Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon.

Unit 16 : d – and f – Block Elements

Transition Elements

General introduction, electronic configuration, occurrence and characteristics, general trends in properties of the first row transition elements – physical properties, ionization enthalpy, oxidation states, atomic radii, colour, catalytic behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation; Preparation, properties and uses of K Cr O and KMnO . 2 2 7 4Inner Transition Elements Lanthanoids – Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction. Actinoids – Electronic configuration and oxidation states.

Unit 17 : Co – Ordination Compounds

Introduction to co – ordination compounds, Werner’s theory; ligands, coordination number, denticity, chelation; IUPAC nomenclature of mononuclear co – ordination compounds, isomerism; Bonding – Valence bond approach and basic ideas of Crystal field theory, colour and magnetic properties; Importance of co – ordination compounds ( in qualitative analysis, extraction of metals and in biological systems ).

Unit 18 : Environmental Chemistry

Environmental Pollution : Atmospheric, water and soil.

Atmospheric Pollution : Tropospheric and Stratospheric.

Tropospheric Pollutants : Gaseous pollutants : Oxides of carbon, nitrogen and sulphur, hydrocarbons; their sources, harmful effects and prevention; Green house effect and Global warming; Acid rain.

Particulate Pollutants : Smoke, dust, smog, fumes, mist; their sources, harmful effects and prevention.

Stratospheric Pollution : Formation and breakdown of ozone, depletion of ozone layer – its mechanism and effects.

Water Pollution : Major pollutants such as pathogens, organic wastes and chemical pollutants; their harmful effects and prevention.

Soil Pollution : Major pollutants such as : Pesticides ( insecticides,. herbicides and fungicides ), their harmful effects and prevention.Strategies to control environmental pollution.

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