First of all, whenever somebody has any ambition or aim to do something, he or she should be confident to do that thing, means never lose HOPE.
FEW MANTRA TO CRACK ENTRANCE EXAM
FOR IIT-JEE: For the preparation of IIT-JEE, you have to clear & enhance your CONCEPTS. All you have to go through more and more CONCEPTS.
Whenever somebody prepares for IIT-JEE, just always be with THREE THINGS:
>First is: BUILDING THE CONCEPTS,
>Second is: PROPER APPLICATIONS OF CONCEPTS &
>Third is: PRACTICE.
Here remember, I stressed on the word 'PROPER'. In Physics, building CONCEPTS is not a tougher job but building RIGHT (PROPER) CONCEPTS is much tougher. Out of every 20 students, I guarantee, that there is only one or two students who know the RIGHT CONCEPT about a particular topic. So I would like to say that don't think Physics is a tougher subject. REMEMBER one more thing if I prefer even a single book, so it means you have to go through each & every line of that book starting from first page till you encounter the last page. There is no use of doing a lot of books only for one subject without getting any point. I saw a lot of students having their own library at their home. But as far PRACTICE is concerned, do whatever you get from anywhere. Whereas in case of Chemistry, just you need to put your efforts on PRACTICE in case of Inorganic Chemistry. In case of Organic part, just first build up your all BASIC Reactions, then start do PRACTICING. And for Physical Part, same thing you have to do as in case of Organic Part. For Maths (My favourite Subject), just use your brain as much as you can. Ultimately for preparation of any exam, remember some points:
1) Always start from BASICS because "without base, there will be no altitude" and "journey of a thousand miles begin with single step".
2) Always BUILD UP RIGHT & APPROPRIATE BASICS because "once the track of train is being changed, it will go on only that track". So always select the right track.
3) Never prefer solutions of questions before doing SELF-ATTEMPT at least five times till you get the right answer because "without fall you can not stand at once".
4) Never leave the question in between. And I saw a lot of students practicing this question without attempting it whole, and it's a very big fault for students and even it becomes their negative point sometimes. So please ignore this thing. Because "many of life's failure are people who did not realize how close they were to success when they gave up"
5) Always try a question with CONCEPTUAL APPROACH, not just read the question then start doing without getting the point that what question is saying.
6) Your study schedule should be such that you will even easily get the time for a little enjoyment daily.
7) Most important thing is that you should be having a time schedule as well as REGULARITY in study.
8) Also you will have to take appropriate sleep or rest of at least 6 hours a day if you are preparing for IIT-JEE otherwise your mind set-up for next day will not be in place.
9) Never cram the things, always TRY TO UNDERSTAND the problem or theory.
10) And BE CONFIDENT while you are preparing. NEVER LOSE CONFIDENCE.
11) Always keep contact with intelligent students of your class or at coaching centre.
12) For your brain storming, I always preferred MTG publications monthly magazine in maths part.
13) Always be AHEAD in exams like-OLYMPIAD, UNIFIED COUNCIL etc. Etc. (for more information-contact me)
14) Always keep the copy of latest syllabus for particular exam. Always check the syllabus before starting a new topic.
15) NEVER GET DEMORALIZED BY SOMEBODY but yes ALWAYS GET INSPIRED FROM SOMEBODY WHO IS YOUR SENIOR. (If you want, contact me)
16) I have a positive point i.e. once I set a goal, then I don't look at anything else, I just KEEP DETERMINATION in me until or unless I ACHIEVE THAT GOAL.
17) Whenever you complete any chapter or particular topic, first of all, go through that topic from NCERT. (It's very important).
18) There is one more thing, whenever you are studying just be CONCENTRATE on that thing so badly, so that you even don't know what is happening your nearby. Because studying 2 hours with DAMN GOOD CONCENTRATION is equals to studying 5-12 hours without any concentration.
19) Always study anything with GREAT INTEREST otherwise it will be of NO USE.
20) Even there are some students who think that they can nod prepare for IIT-JEE like EXAMS. So if they think so, then they are wrong. Because "ATTITUDE, NOT APTITUDE DETERMINES ALTITUDE".
At last I prefer books for preparation of IIT-JEE subject-wise (according to me):
*MATHS: R.D.SHARMA (for theory and practice) and PURUSHOTTEM KUMAR-OBJECTIVE (it must be for practice)
*PHYSICAL CHEMISTRY: BHARTI BHAVAN PUBLICATIONS, R. C. MUKHERJEE (NUMERICAL CHEMISTRY), DR. P. BAHADUR,
*ORGANIC CHEMISTRY: NCERT (must), SOLOMONS, IIT CHEMISTRY
*INORGANIC CHEMISTRY: NCERT (must) (you need nothing else for preparing this part)
*NOTE: prefer MTG Publication monthly Magazine also &if are taking coaching from somewhere, then prefer that notes also.
*PHYSICS: H.C.VERMA (part 1 & 2 both)(for theory as well as practice), IIT GALAXY (VOL 1 TO 5),
At last I want to say one more thing for IIT-JEE that "DO PRACTICE AS MUCH AS YOU CAN WITH YOUR FULL EFFORT"
FOR AIEEE: There are lot of students who think that if they are preparing for IIT-JEE, then they are also preparing for AIEEE. It's wrong.
First of all, for preparation of AIEEE, they have to prepare tightly for CBSE EXAMS if the person is fresher otherwise dropper also have to prepare for CBSE, only then he can think of rank less than 20,000 in AIEEE.
If somebody is preparing for AIEEE (whether he is preparing for IIT-JEE or not), he or she has to keep THREE WORDS IN HIS OR HER MIND ALL THE TIME:
1) PRACTICE(as much as somebody can)
2) SPEED(for doing question with RIGHT APPROACH)
3) ACCURACY(the MOST IMPORTANT POINT to get the RIGHT ANSWER)
For AIEEE, you have to learn SMALL TRICKS and MAGIC to solve the question in possible time.
All other things are in same pattern as that of IIT-JEE.
<<<<>>>>
##CAN YOU TELL ME THE DIFFERENCE BETWEEN A GOOD TEACHER AND THE BEST TEACHER==? (Can u guess)???
If answer is NO, then READ THIS : THERE WILL BE NO DIFFERENCE HOW THEY ARE TEACHING THEIR STUDENTS,BUT THE ONLY DIFFERENCE IS THAT HOW ANY TEACHER IS CREATING INTEREST IN PARTICULAR SUBJECT AND HOW THAT TEACHER IS MOTIVATING AND INSPIRING THE STUDENTS TOWARDS ACHIEVING THEIR GOAL.
Somebody said right that: "ANYBODY CAN TEACH BUT EVERYBODY CAN NOT STUDY".
SO, there MUST be PROPER WAY TO TEACH SOMEBODY.
THERE ARE A LOT OF THINGS TO TELL BUT THIS IS ARTICLE!
THESE ALL BAD RANKS ARE DUE TO THE REASON THAT I DID NOT FOLLOW ALL THE POINTS I EXPLAINED ABOVE.
SO, DON'T YOU DO THE SAME MISTAKES ,IF YOU WANT TO BE IN TOP 500 HUNDRED RANKS OF IIT-JEE, BITSAT AND AIEEE!(guarantee)
Tuesday, November 4, 2008
AIEEE - 2008 SYLLABUS
SECTION: A
Physical Chemistry
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.
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, van der Waals equation, liquefaction of gases, critical constants.
Liquid State:
Properties of liquids - vapour pressure, viscosity and surface tension and effect of temperature on them (qualitative treatment only).
Cont...2
-2-
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, ψ and ψ2, concept of atomic orbitals as one electron wave functions; Variation of ψ and ψ2 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 STRUCURE
Kossel - Lewis approach to chemical bond formation, concept of ionic and covalent bonds.
Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy.
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.
Cont…..3
-3-
Molecular Orbital Theory - Its important features, LCAOs, types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, mo1ecular orbital electronic configurations of homonuclear 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 thermodynamics - 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, ioniz-ation and solution.
Second law of thermodynamics; Spontaneity of processes; ΔS of the universe and ΔG of the system as criteria for spontaneity, ΔGo (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 ΔG and ΔGo in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, effect of catalyst; Le
Chatelier’s principle.
Cont….4
-4-
Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Bronsted - 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.
Electrochemical 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; Nemst 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.
Cont...5
-5-
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
UNIT -11:
Inorganic Chemistry
CLASSIFICATON OF ELEMENTS AND PERIODICITY IN PROPERTIES
Modem periodic law and present form of the periodic table, s, p, d and f block elements, periodic trends in properties of elementsatomic 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.
Cont….6
- 6-
UNIT - 15: p - BLOCK ELEMENTS
Group - 13 to Group 18 Elements
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 nitric acid, phosphine and phosphorus halides, (PCl3, PCl5); 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.
Cont...7
-7-
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 K2 Cr2 O7 and KMnO4.
Inner 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, co-ordination 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.
Cont…….8- 8 -
Soil pollution - Major pollutants such as: Pesticides (insecticides,. herbicides and fungicides), their harmful effects and prevention.
Strategies to control environmental pollution.
SECTION-C
Organic Chemistry
UNIT - 19: PURIFICATION AND CHARACTERISATION OF ORGANIC
COMPOUNDS
Purification - Crystallization, sublimation, distillation, differential extraction and chromatography - principles and their applications.
Qualitative analysis - Detection of nitrogen, sulphur, phosphorus and halogens.
Quantitative analysis (basic principles only) - Estimation of carbon, hydrogen, nitrogen, halogens, sulphur, phosphorus.
Calculations of empirical formulae and molecular formulae; Numerical problems in organic quantitative analysis.
UNIT - 20: SOME BASIC PRINCIPLES OF ORGANIC CHEMISTRY
Tetravalency of carbon; Shapes of simple molecules - hybridization (s and p); Classification of organic compounds based on functional groups: - C = C - , - C = C - and those containing halogens, oxygen, nitrogen and sulphur, Homologous series; Isomerism - structural and stereoisomerism.
Nomenclature (Trivial and IUPAC)
Covalent bond fission - Homolytic and heterolytic: free radicals, carbocations and carbanions; stability of carbocations and free radicals, electrophiles and nucleophiles.
Electronic displacement in a covalent bond - Inductive effect, electromeric effect, resonance and hyperconjugation.
Common types of organic reactions - Substitution, addition, elimination and rearrangement.
Cont…9
-9-
UNIT - 21: HYDROCARBONS
Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and reactions.
Alkanes - Conformations: Sawhorse and Newman projections (of ethane); Mechanism of halogenation of alkanes.
Alkenes - Geometrical isomerism; Mechanism of electrophilic addition: addition of hydrogen, halogens, water, hydrogen halides (Markownikoff's and peroxide effect); Ozonolysis, oxidation, and polymerization.
Alkynes - acidic character; addition of hydrogen, halogens, water and hydrogen halides; polymerization.
Aromatic hydrocarbons - Nomenclature, benzene - structure and aromaticity; Mechanism of electrophilic substitution: halogenation, nitration, Friedel – Craft’s alkylation and acylation, directive influence of functional group in mono-substituted benzene.
UNIT - 22: ORGANIC COMPOUNDS CONTAINING HALOGENS
General methods of preparation, properties and reactions; Nature of C-X bond; Mechanisms of substitution reactions.
Uses/environmental effects of chloroform, iodoform, freons and DDT.
UNIT - 23: ORGANIC COMPOUNDS CONTAINING OXYGEN
General methods of preparation, properties, reactions and uses. ALCOHOLS, PHENOLS AND ETHERS
Alcohols: Identification of primary, secondary and tertiary alcohols; mechanism of dehydration.
Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration and sulphonation, Reimer - Tiemann reaction.
Ethers:
Structure.
Cont….10
- 10
ALDEHYDE AND KETONES: Nature of carbonyl group;
Nucleophilic addition to >C=O group, relative reactivities of aldehydes and ketones; Important reactions such as - Nucleophilic addition reactions (addition of HCN, NH3 and its derivatives), Grignard reagent; oxidation; reduction (Wolff Kishner and Clemmensen); acidity of α - hydrogen, aldol condensation, Cannizzaro reaction, Haloform reaction; Chemical tests to distinguish between aldehydes and Ketones.
CARBOXYLIC ACIDS
Acidic strength and factors affecting it.
UNIT - 24: ORGANIC COMPOUNDS CONTAINING NITROGEN
General methods of preparation, properties, reactions and uses.
Amines: . Nomenclature, classification, structure basic character and identification of primary, secondary and tertiary amines and their basic character.
Diazonium Salts: Importance in synthetic organic chemistry.
UNIT - 25: POLYMERS
General introduction and classification of polymers, general methods of polymerization - addition and condensation, copolymerization; Natural and synthetic rubber and vulcanization; some important polymers with emphasis on their monomers and uses - polythene, nylon, polyester and bakelite.
UNIT - 26: BIOMOLECULES
General introduction and importance of biomolecules.
CARBOHYDRATES - Classification: aldoses and ketoses; monosaccharides (glucose and fructose), constituent monosaccharides of oligosacchorides (sucrose, lactose, maltose) and polysaccharides (starch, cellulose, glycogen).
Cont...11
- 11 -
/
PROTEINS - Elementary Idea of α - amino acids, peptide bond, . polypeptides; proteins: primary, secondary, tertiary and quaternary structure (qualitative idea only), denaturation of proteins, enzymes.
VITAMINS - Classification and functions.
NUCLEIC ACIDS - Chemical constitution of DNA and RNA.
Biological functions of Nucleic acids.
UNIT - 27: CHEMISTRY IN EVERYDAY LIFE
Chemicals in medicines - Analgesics, tranquilizers, antiseptics, disinfectants, antimicrobials, antifertility drugs, antibiotics, antacids, antihistamins - their meaning and common examples. .
Chemicals in food - Preservatives, artificial sweetening agents - common examples.
Cleansing agents - Soaps and detergents, cleansing action.
UNIT - 28: PRINCIPLES RELATED TO PRACTICAL CHEMISTRY
. Detection of extra elements (N,S, halogens) in organic compounds; Detection of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl and amino groups in organic compounds.
. Chemistry involved in the preparation of the following:
Inorganic compounds: Mohr's salt, potash alum.
Organic compounds: Acetanilide, p-nitroacetanilide, aniline yellow, iodoform.
. Chemistry involved in the titrimetric excercises - Acids bases and
the use of indicators, oxalic-acid vs KMnO4, Mohr's salt vs KMnO4.
. Chemical principles involved in the qualitative salt analysis:
Cont…12
-12-
Cations - Pb2+ , Cu2+, AI3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+ , Mg2+ ,
NH4+.
Anions – CO32-, S2-, SO42-, NO2- , NO3- , CI - , Br-, I- .
(Insoluble salts excluded).
. Chemical principles involved in the following experiments:
1. Enthalpy of solution of CuSO4
2. Enthalpy of neutralization of strong acid and strong
base. .
Preparation of lyophilic and lyophobic sols.
Kinetic study of reaction of iodide ion with hydrogen peroxide at room temperature.
3. 4.
Physical Chemistry
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.
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, van der Waals equation, liquefaction of gases, critical constants.
Liquid State:
Properties of liquids - vapour pressure, viscosity and surface tension and effect of temperature on them (qualitative treatment only).
Cont...2
-2-
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, ψ and ψ2, concept of atomic orbitals as one electron wave functions; Variation of ψ and ψ2 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 STRUCURE
Kossel - Lewis approach to chemical bond formation, concept of ionic and covalent bonds.
Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy.
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.
Cont…..3
-3-
Molecular Orbital Theory - Its important features, LCAOs, types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, mo1ecular orbital electronic configurations of homonuclear 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 thermodynamics - 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, ioniz-ation and solution.
Second law of thermodynamics; Spontaneity of processes; ΔS of the universe and ΔG of the system as criteria for spontaneity, ΔGo (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 ΔG and ΔGo in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, effect of catalyst; Le
Chatelier’s principle.
Cont….4
-4-
Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Bronsted - 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.
Electrochemical 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; Nemst 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.
Cont...5
-5-
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
UNIT -11:
Inorganic Chemistry
CLASSIFICATON OF ELEMENTS AND PERIODICITY IN PROPERTIES
Modem periodic law and present form of the periodic table, s, p, d and f block elements, periodic trends in properties of elementsatomic 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.
Cont….6
- 6-
UNIT - 15: p - BLOCK ELEMENTS
Group - 13 to Group 18 Elements
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 nitric acid, phosphine and phosphorus halides, (PCl3, PCl5); 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.
Cont...7
-7-
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 K2 Cr2 O7 and KMnO4.
Inner 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, co-ordination 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.
Cont…….8- 8 -
Soil pollution - Major pollutants such as: Pesticides (insecticides,. herbicides and fungicides), their harmful effects and prevention.
Strategies to control environmental pollution.
SECTION-C
Organic Chemistry
UNIT - 19: PURIFICATION AND CHARACTERISATION OF ORGANIC
COMPOUNDS
Purification - Crystallization, sublimation, distillation, differential extraction and chromatography - principles and their applications.
Qualitative analysis - Detection of nitrogen, sulphur, phosphorus and halogens.
Quantitative analysis (basic principles only) - Estimation of carbon, hydrogen, nitrogen, halogens, sulphur, phosphorus.
Calculations of empirical formulae and molecular formulae; Numerical problems in organic quantitative analysis.
UNIT - 20: SOME BASIC PRINCIPLES OF ORGANIC CHEMISTRY
Tetravalency of carbon; Shapes of simple molecules - hybridization (s and p); Classification of organic compounds based on functional groups: - C = C - , - C = C - and those containing halogens, oxygen, nitrogen and sulphur, Homologous series; Isomerism - structural and stereoisomerism.
Nomenclature (Trivial and IUPAC)
Covalent bond fission - Homolytic and heterolytic: free radicals, carbocations and carbanions; stability of carbocations and free radicals, electrophiles and nucleophiles.
Electronic displacement in a covalent bond - Inductive effect, electromeric effect, resonance and hyperconjugation.
Common types of organic reactions - Substitution, addition, elimination and rearrangement.
Cont…9
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UNIT - 21: HYDROCARBONS
Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and reactions.
Alkanes - Conformations: Sawhorse and Newman projections (of ethane); Mechanism of halogenation of alkanes.
Alkenes - Geometrical isomerism; Mechanism of electrophilic addition: addition of hydrogen, halogens, water, hydrogen halides (Markownikoff's and peroxide effect); Ozonolysis, oxidation, and polymerization.
Alkynes - acidic character; addition of hydrogen, halogens, water and hydrogen halides; polymerization.
Aromatic hydrocarbons - Nomenclature, benzene - structure and aromaticity; Mechanism of electrophilic substitution: halogenation, nitration, Friedel – Craft’s alkylation and acylation, directive influence of functional group in mono-substituted benzene.
UNIT - 22: ORGANIC COMPOUNDS CONTAINING HALOGENS
General methods of preparation, properties and reactions; Nature of C-X bond; Mechanisms of substitution reactions.
Uses/environmental effects of chloroform, iodoform, freons and DDT.
UNIT - 23: ORGANIC COMPOUNDS CONTAINING OXYGEN
General methods of preparation, properties, reactions and uses. ALCOHOLS, PHENOLS AND ETHERS
Alcohols: Identification of primary, secondary and tertiary alcohols; mechanism of dehydration.
Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration and sulphonation, Reimer - Tiemann reaction.
Ethers:
Structure.
Cont….10
- 10
ALDEHYDE AND KETONES: Nature of carbonyl group;
Nucleophilic addition to >C=O group, relative reactivities of aldehydes and ketones; Important reactions such as - Nucleophilic addition reactions (addition of HCN, NH3 and its derivatives), Grignard reagent; oxidation; reduction (Wolff Kishner and Clemmensen); acidity of α - hydrogen, aldol condensation, Cannizzaro reaction, Haloform reaction; Chemical tests to distinguish between aldehydes and Ketones.
CARBOXYLIC ACIDS
Acidic strength and factors affecting it.
UNIT - 24: ORGANIC COMPOUNDS CONTAINING NITROGEN
General methods of preparation, properties, reactions and uses.
Amines: . Nomenclature, classification, structure basic character and identification of primary, secondary and tertiary amines and their basic character.
Diazonium Salts: Importance in synthetic organic chemistry.
UNIT - 25: POLYMERS
General introduction and classification of polymers, general methods of polymerization - addition and condensation, copolymerization; Natural and synthetic rubber and vulcanization; some important polymers with emphasis on their monomers and uses - polythene, nylon, polyester and bakelite.
UNIT - 26: BIOMOLECULES
General introduction and importance of biomolecules.
CARBOHYDRATES - Classification: aldoses and ketoses; monosaccharides (glucose and fructose), constituent monosaccharides of oligosacchorides (sucrose, lactose, maltose) and polysaccharides (starch, cellulose, glycogen).
Cont...11
- 11 -
/
PROTEINS - Elementary Idea of α - amino acids, peptide bond, . polypeptides; proteins: primary, secondary, tertiary and quaternary structure (qualitative idea only), denaturation of proteins, enzymes.
VITAMINS - Classification and functions.
NUCLEIC ACIDS - Chemical constitution of DNA and RNA.
Biological functions of Nucleic acids.
UNIT - 27: CHEMISTRY IN EVERYDAY LIFE
Chemicals in medicines - Analgesics, tranquilizers, antiseptics, disinfectants, antimicrobials, antifertility drugs, antibiotics, antacids, antihistamins - their meaning and common examples. .
Chemicals in food - Preservatives, artificial sweetening agents - common examples.
Cleansing agents - Soaps and detergents, cleansing action.
UNIT - 28: PRINCIPLES RELATED TO PRACTICAL CHEMISTRY
. Detection of extra elements (N,S, halogens) in organic compounds; Detection of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl and amino groups in organic compounds.
. Chemistry involved in the preparation of the following:
Inorganic compounds: Mohr's salt, potash alum.
Organic compounds: Acetanilide, p-nitroacetanilide, aniline yellow, iodoform.
. Chemistry involved in the titrimetric excercises - Acids bases and
the use of indicators, oxalic-acid vs KMnO4, Mohr's salt vs KMnO4.
. Chemical principles involved in the qualitative salt analysis:
Cont…12
-12-
Cations - Pb2+ , Cu2+, AI3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+ , Mg2+ ,
NH4+.
Anions – CO32-, S2-, SO42-, NO2- , NO3- , CI - , Br-, I- .
(Insoluble salts excluded).
. Chemical principles involved in the following experiments:
1. Enthalpy of solution of CuSO4
2. Enthalpy of neutralization of strong acid and strong
base. .
Preparation of lyophilic and lyophobic sols.
Kinetic study of reaction of iodide ion with hydrogen peroxide at room temperature.
3. 4.
BIO MOLECULES -
CARBOHYDRATES - Classification: aldoses and ketoses; monosaccharides (glucose and fructose), constituent monosaccharides of oligosacchorides (sucrose, lactose, maltose) and polysaccharides (starch, cellulose, glycogen).
Carbohydrates are classified as:
Monosaccharides
Oligosaccharides
Polysaccharides
Monohydrates may be represented as follows
H
!
C=O
!
(H-C-OH)-n
!
CH-2OH
A polyhdroxy aldehyde
CH-2OH
!
C=O
!
(H-C-OH)-n
!
CH-2OH
A polyhdroxy ketone
Monosaccharides are named as follows.
1. The calss name of monosaccharides begins with the prefix 'aldo' for polyhydroxy aldehydes and "keto' for polyhydroxy ketones.
2. the name ends with suffix 'ose".
3. In between prefix and suffix, the number of carbon atoms (i.e. di, tri, tetr etc.) is inserted.
Examples
H
|
C=O
|
(H-C-OH)
|
CH-2OH
Aldotriose - (A polyhdroxy aldehyde)
CH-2OH
|
C=O
|
CH-2OH
Ketotriose - (A polyhdroxy ketone )
Reducing and Nonreducing Sugars
Reducing sugars are easily oxidized to give carboxylic acid.
They reduce
(i) Tollens reagent (an ammoniacal solution of silver nitrate) to shiny silver mirror.
(ii) Fehling's solution (an acqueous solution of cupric iron and tartrate salts) to red precipitate of cuprous oxide, and
(iii) Benedict's reagent (an alkaline solution containing a cupric citrate complex) to red precipitate of curous oxide)
All aldoses are reducing sugars, but some ketoses are reducing sugars as well. For example, fructose (a ketose) reduces Tollens reagent. This occurs because fructose is readily isomerized to an aldose in basic solution.
amino acids are organic compounds containing both an amino group (NH2) and carboxylic group (COOH). They are represented by the general formula:
R
|
C-COOH
|
NH2
Essential amino acids
These amino acids are required by the body but are not made by our bodies. hence they must be supplied in diets.
Valine
Leucine
Isoleucine
Phenylalanine
Methionine
Trptophan
threonine
Lysine
Agrinine
L-Family of Amino Acids
With the exception of glycine, all other α amino acids have chiral carbon atom and have two optically active isomers.
However all naturally occurring amino acids belong to L series which have -NH2 group on the left.
Structure of Amino acids
amino acids exist as dipolar ion called a zwitter ion.
i) when an acid is added to an amino acid-COO- accepts this proton and therefore the basic character is due to -COO-group.
ii) When an alkali is added to amino acid -NH3+ group releases the proton and therefore acidic character is due to -NH3+ group.
Peptide
peptides are compounds formed by the condensation of two or more same or different α amino acids. The condensation occurs between amino acids with the elimination of water. In this case,the carboxyl group of one amino acid and amine group of another amino acid gets condensed with the elimination of water molecule. The resulting C-N linkage is called peptide linkage. The bond of C with O becomes a double bond.
The formation of peptide can be between two amino acid molecules or the number can go on until a single molecule containing several hundred thousands of aminoacids is formed.
Proteins
Structurally, proteins are long polymers of amino acids linked by peptide bonds
Monday, November 3, 2008
CHEMISTRY ONLINE - AIEEE CHEMISTRY
EXPERIMENTAL SECTION - (ACCORDING TO NEW SYALLUBUS)
Preparation of Ferrous ammonium sulphate (Mohr’s salt)
Ferrous ammonium sulphate (Mohr’s salt)
It is a double salt. A double salt is a substance obtained by the combination of two different salts which crystallize together as a single substance but ionize as two distinct salts when dissolved in water.
Mohr’s salt is prepared by dissolving an equimolar mixture of hydrated ferrous sulphate and ammonium sulphate in water containing a little of sulphuric acid and the crystallization from the solution.
On crystallization light green crystals of ferrous ammonium sulphate separate out.
Ferrous sulphate FeSO4.7H2O
Ammonium sulphate (NH4)2SO4
Mohr’s salt FeSO4.(NH4)2SO4.6H2O
Apparatus and materials required
Two beakers, china-dish, funnel, funnel-stand, glass rod, wash bottle, tripod stand, wire-gauze,
Ferrous sulphate crystals, ammonium sulphate crystals, dilute sulphuric acid, and ethyl alcohol.
Preparation of Ferrous ammonium sulphate (Mohr’s salt)
Ferrous ammonium sulphate (Mohr’s salt)
It is a double salt. A double salt is a substance obtained by the combination of two different salts which crystallize together as a single substance but ionize as two distinct salts when dissolved in water.
Mohr’s salt is prepared by dissolving an equimolar mixture of hydrated ferrous sulphate and ammonium sulphate in water containing a little of sulphuric acid and the crystallization from the solution.
On crystallization light green crystals of ferrous ammonium sulphate separate out.
Ferrous sulphate FeSO4.7H2O
Ammonium sulphate (NH4)2SO4
Mohr’s salt FeSO4.(NH4)2SO4.6H2O
Apparatus and materials required
Two beakers, china-dish, funnel, funnel-stand, glass rod, wash bottle, tripod stand, wire-gauze,
Ferrous sulphate crystals, ammonium sulphate crystals, dilute sulphuric acid, and ethyl alcohol.
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