Physics the great Zone

The Electron

2010-02-14T15:29:00.016+05:30

When first investigated in the 18th and 19th centuries, electrical and magnetic

phenomena were generally construed in terms of lethereal fluids, as were those

associated with heat and light. These fluids were thought to comprise minute mutually

repelling particles. Thus, heat was either thought to be vibrations in the fluid caloric or

an accumulation of this fluid in the interstices of materials. Light was either a flux of

particles emitted at high speed from luminous bodies or the vibrations of a ubiquitous

fluid zether. Electric fluids-electricir)*-flowed readily through metals and other

conductors but did not penetrate insulators such as paper and glass. Opinion was

divided 8s to whether there was just one electric fluid or two-a positive fluid and a

negutive fluid.

The possibility that electricity might not be a continuous fluid was first raised in

the middle of the 19th century following Faraday’s quantitative researches on

electrolysis. These showed the existence of a systematic relationship between the

amount of electricity passed through an electrolytic cell and the quantity of material

that undergoes chemical reaction (electrolysis) in the cell. Thus, the passage of a

certain amount of electricity-96,500 coulombs in modem terms-always liberates a

gramequivalent of substance from the electrolyte, whether it is the metal released at

the negative cathode or the non-metal at the positive anode. Putting aside his

misgivings about atomism, Faraday recognised that this suggested electricity might be

atomic in nature and that a natural indivisible unit of electricity exists. In 1891 Stoney’

suggested that this natural unit of electricity be called an electron.

On this view, every ion carries an integer multiple of this natural unit. For

example, a silver ion, Agf, carries a single natural unit of positive charge; a typical

copper ion, Cu++, carries two such units. Given that a gramequivalent of monovalent

ions comprises a mole, the magnitude of the natural unit of electricity, e, can be

calculated by dividing the 96,500 coulombs by Avogadro’s number, 6.02. 10²³

^{The term electron is now used to designate the elementary particle that carries the}

^{natural unit of negative charge which was first identified towards the end of the 19th}

^{century in experiments on the conduction of electricity through gases at very low}

^{pressures. At atmospheric pressure, gases do not usually conduct electricity. However,}

^{at reduced pressures of O.5mmHg to lOmmHg and with applied potentials of several}

^{thousand volts, they can be made to pass a current. These greatly reduced gas pressures}

^{were first achieved at the end of the 19th century following the advances made at that}

^{time in vacuum pump technology. The gases were contained in narrow glass tubes,}

^{called dischaee tubes, into which suitabIe electrodes had been inserted. The passage}

^{of the current is eccompanied by the appearance of striking colours in the tubes (Fig}

^1.1).

^{At still lower pressures, -0.02mmHg, the colours disappear but the glass tube itself}

^{begins to glow with a green hue. An object placed in front of the cathode (the negative}

^{electrode) casts a shadow on the opposite wall of the discharge tube (Fig 1.2). Certain}

^{minerals, when placed in front of the cathode, fluoresce with brilliant colours. It}

^{appears that something is being emitted from the cathode; this emanation was given}

^{the name cathode rays.

^{^{^{In fbrther experiments it was found that the cathode rays were deflected by a
magnetic field as would a stream of negative charge (Fig 1.3a). Furthermore, a small
paddle wheel positioned between the electrodes rotated under their impact; switching
the polarity of the electrodes reversed the direction of th}}}^{^{^{e rotation (Fig 1.3b). These
two phenomena suggested the cathode rays mig}}}^{^{^{ht be negatively charged particles.}}}
^{^{^{Nevertheless, many physicists at the time still considered them to be of an Ethereal
rather than a material nature}}}
^{^{^.}}
^{^{^{Convinced that the cathode rays were in fact charged particles of matter,
J.J.Thomson set out in 1897 to measure their velocity, v, and the ratio, q/m,between
their charge, q, and their mass, m. In one of the experiments he conducted, a narrow
collimated beam of cathode rays was aimed along the length of a very low pressure
glass discharge tube. After emerging from the hole in the anode,}}}^{^{^{the beam passed}}}
^{^{^{through a thin slit, between a pair of vertical coils and, finally, between the horizontal
parallel plates of a condenser. The green spot that appeared on the glass at the far end}}}
^{^{^{of the tube indicated where the beam impinged upon it (Fig 1.4).}}}}

^{^{^{^{^{^{^{^{^{The cathode ray beam could be deflected vertically by two different means: (i)
magnetically; (ii) electrically:

(i) Magnetically-by passing a current through the coils. This induces a uniform
horizontal magnetic field, B, in the space between them which, in turn, exerts a
force, FB, on the cathode ray particles such that
FB = Bqv (1.2)}}}}}}
^{^{^{^{^{^{where v is the velocity of the particles. This force acts at right angles to the
direction of the particle's motion and so constitutes a centripetal force. Thus, as
they pass between the pair of coils, the cathode ray particles move in a circular
path-along the arc of a circle-such that}}}}}}}}^{^{^{^{^{^{^{^{where r is the radius of the arc.}}}}}}
^{^{^{^{^{^{(ii) Electrically-by connecting the condenser plates to a potential source; this
produces a vertical electric field, E, in the space between them that exerts a
vertical force, FE, on the cathode ray particles such that
FE = Eq (1.4)

Initially, Thomson applied just the magnetic field. This had the effect of moving
the green spot down from P to Q. He then activated the electric field and adjusted the}}}}}}
^{^{^{^{^{^{potential between the condenser plates until the field was just sufficient to return the
green spot from Q to P. At this point, the two forces, FB and FE, cancelled each other
out, such that:
FE = FB
or qE = Bqv =}}}}}}^{^{^{^{^{^mv2/r}}}}}}}^{^{^{^{^{^{^{^{From which, the particles' charge to mass ratio is given by}}}}}}}}}^{^{^{Thomson knew the value of the magnetic field, B, from the dimensions of the coils
and the current flowing through them, of the arc radius, r, from the dimensions of the
apparatus and the distance PQ and of the electric field, E, from the potential applied
between the condenser plates and the distance between them. Substituting these in
equation (1.6) gave a value, in modem SI units, of -2-10 power 11 C/kg for the charge to mass
ratio of the cathode ray particles. Thornson repeated the experiment using different
metal cathodes and with different gases in the low pressure tube, but in each case he
found approximately the same value for the ratio.The value found by Thomson for the
charge to mass ratio of the cathode ray
particles was three orders of magnitude greater than the largest previously known value
of this ratio, namely, that found for the aqueous hydrogen ion, H(aq). This could be
attributed either “to the smallness of m or the largeness of q, or a combination of these
two”. Thomson opted for the “smallness of m” and assumed that the magnitude of the
charge, q, carried by the cathode ray particles was equal to the smallest charge known
to be carried by any ion, i.e., q = -1.6-10 power -19 C. On this assumption, he calculated the
mass of the cathode ray particles and obtained the result, astonishing at the time, that
their mass was only Kg36 that of the hydrogen atom, itself the smallest of all atoms.*
In an attempt to verify Thomson’s assumption, direct measurements of the
magnitude of the charges carried by gaseous ions were made. Although these
experiments suffered initially from many sources of error, their results appeared to
confirm Thomson’s supposition. The issue was finally and unequivocally settled in
1906 when, in a series of accurate and careful experiments, Millikan8 measured the
magnitude of the electrical charges carried by both positively and negatively charged
oil droplets. In none of the hundreds of measurements he made, did he detect a droplet
that carried a charge whose magnitude was less than 1.6.1O power-l9 C , nor one that carried
a charge whose magnitude was a fractional multiple of this amount. In every case, the
magnitude of the charges was an integer multiple of e = 1.6.10power-19 C . The clear
inference was that electrical charge-positive or negative-always appears as an
integer multiple of the natural unit e.
The cathode ray particles Thomson had discovered are the elementary particles we
now call electrons; the electron was the first elementary particle to be discovered.
Electrons carry the natural unit, -e, of negative charge. They are the smallest of the
three constituent particles--protons, neutrons and electrons--of ordinary matter.
Though electrons have no discernible internal structure or dimensions, they
nevertheless possess an intrinsic angular momentum (spin) and an associated magnetic
moment.
Cathode rays were not the only emanations observed in discharge tubes. If the
cathode in the discharge tube was pierced, rays were seen to emerge from the hole in
the direction away from the anode (the positive electrode), i.e., in the opposite
direction to the cathode rays (Fig 1.5). These emanations were called canal rays; they
were found to be positively charged.
Having identified the cathode rays, Thomson proceeded to investigate the nature of
the canal rays. These too proved to be particles of matter. By measuring the ratio
between their charge and their mass he identified them as positive ions of the gas
present in the discharge tube. He construed that these positive ions were produced in
the space between the cathode and the anode from the bombardment of the gaseous
atoms by the cathode rays (electrons). Since they carried a positive charge, they were
attracted to and accelerated towards the negative cathode, passing through the hole that
had been pierced in it and emerging from the other side. In one notable experiment, in
which the gas in the discharge tube was a pure sample of the noble gas neon, Thomson
discovered two different species of positive ions in the canal rays whose masses
differed by about 10%. The ions could only be neon ions, the purity of the sample
ensured this. This discovery of different species of neon ions first demonstrated the
existence of atoms that share the same chemical identity but have different masses;
what we now refer to as isotopes.
In 1932, a particle was discovered that is identical to the electron in all its
properties except that it is positively and not negatively charged; it was designated the
unti-electron or positron. When a positron and electron collide, the pair of particles
self-destruct, releasing a burst of high frequency electromagnetic radiation- Y rays.}}}

APTITUDE TEST B.ARCH./B.PLANNIN

2010-02-14T14:15:00.001+05:30

Part I

Awareness of persons, places, Buildings, Materials.) Objects, Texture related to Architecture and build~environment. Visualising three dimensional objects from two dimensional drawings. Visualising. different sides of three dimensional objects. Analytical Reasoning Mental Ability (Visual, Numerical and Verbal).

Part II

Three dimensional - perception: Understanding and appreciation of scale and proportion of objects, building forms and elements, colour texture, harmony and contrast. Design and drawing of geometrical or abstract shapes and patterns in pencil. Transformation of forms both 2 D and 3 D union, substraction, rotation, development of surfaces and volumes, Generation of Plan, elevations and 3 D views of objects. Creating two dimensional and three dimensional compositions using given shapes and forms. Sketching of scenes and activities from memory of urbanscape (public space, market, festivals, street scenes, monuments, recreational spaces etc.), landscape (river fronts, jungles. gardens, tre es, plants etc.) and rural life.

CHEMISTRY

2010-02-14T13:36:00.003+05:30

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).
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.
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.
Molecular Orbital Theory - Its important features, LCAOs, types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, molecular 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, ionization and solution.
Second law of thermodynamics- 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.
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; 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

Unit 11: 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 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

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.

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 K₂Cr₂O₇ 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.
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

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.
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 ? - 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: BIO MOLECULES
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).
PROTEINS - Elementary Idea of ? - 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:
Cations - Pb²⁺ , Cu²⁺, AI³⁺, Fe³⁺, Zn²⁺, Ni²⁺, Ca²⁺, Ba²⁺, Mg²⁺, NH⁴⁺.
Anions- CO₃^2-, S^2-, SO₄^2-, NO^2-, NO^3-, 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. .
3. Preparation of lyophilic and lyophobic sols.
4. Kinetic study of reaction of iodide ion with hydrogen peroxide at room temperature.

PHYSICS

2010-02-14T13:02:00.002+05:30

The syllabus contains two Sections - A and B. Section - A pertains to the Theory Part having 80% weightage, while Section - B contains Practical Component (Experimental Skills) having 20% weightage.

SECTION A

Unit 1: PHYSICS AND MEASUREMENT
Physics, technology and society, S I units, Fundamental and derived units. Least count, accuracy and precision of measuring instruments, Errors in measurement, Significant figures. Dimensions of Physical quantities, dimensional analysis and its applications

Unit 2: KINEMATICS

Frame of reference. Motion in a straight line: Position-time graph, speed and velocity. Uniform and non-uniform motion, average speed and instantaneous velocity Uniformly accelerated motion, velocity-time, position- time graphs, relations for uniformly accelerated motion. Scalars and Vectors, Vector addition and Subtraction, Zero Vector, Scalar and Vector products, Unit Vector, Resolution of a Vector. Relative Velocity, Motion in a plane, Projectile Motion, Uniform Circular Motion.

Unit 3: LAWS OF MOTION

Force and Inertia, Newton’s First Law of motion; Momentum, Newton’s Second Law of motion; Impulse; Newton’s Third Law of motion. Law of conservation of linear momentum and its applications, Equilibrium of concurrent forces.
Static and Kinetic friction, laws of friction, rolling friction.
Dynamics of uniform circular motion: Centripetal force and its applications.

Unit 4: WORK, ENERGY AND POWER

Work done by a constant force and a variable force; kinetic and potential energies, workenergy theorem, power. Potential energy of a spring, conservation of mechanical energy, conservative and nonconservative forces; Elastic and inelastic collisions in one and two dimensions

Unit 5: ROTATIONAL MOTION

Centre of mass of a two-particle system, Centre of mass of a rigid body; Basic concepts of rotational motion; moment of a force, torque, angular momentum, conservation of angular momentum and its applications; moment of inertia, radius of gyration. Values of moments of inertia for simple geometrical objects, parallel and perpendicular axes theorems and their applications. Rigid body rotation, equations of rotational motion.

Unit 6: GRAVITATION

The universal law of gravitation. Acceleration due to gravity and its variation with altitude and depth. Kepler’s laws of planetary motion. Gravitational potential energy; gravitational potential. Escape velocity. Orbital velocity of a satellite. Geo-stationary satellites.

Unit7: PROPERTIES OF SOLIDS AND LIQUIDS

Elastic behaviour, Stress-strain relationship, Hooke’s Law, Young’s modulus, bulk modulus, modulus of rigidity. Pressure due to a fluid column; Pascal’s law and its applications. Viscosity, Stokes’ law, terminal velocity, streamline and turbulent flow, Reynolds number. Bernoulli’s principle and its applications. Surface energy and surface tension, angle of contact, application of surface tension - drops, bubbles and capillary rise. Heat, temperature, thermal expansion; specific heat capacity, calorimetry; change of state, latent heat. Heat transfer- conduction, convection and radiation, Newton’s law of cooling.

Unit 8: THERMODYNAMICS

Thermal equilibrium, zeroth law of thermodynamics, concept of temperature. Heat, work and internal energy. First law of thermodynamics. Second law of thermodynamics: reversible and irreversible processes. Carnot engine and its efficiency.

Unit 9: KINETIC THEORY OF GASES

Equation of state of a perfect gas, work doneon compressing a gas.Kinetic theory of gases - assumptions, concept of pressure. Kinetic energy and temperature: rms speed of gas molecules; Degrees of freedom, Law of equipartition of energy,applications to specific heat capacities of gases; Mean free path, Avogadro’s number.

Unit 10: OSCILLATIONS AND WAVES

Periodic motion - period, frequency, displacement as a function of time. Periodic functions. Simple harmonic motion (S.H.M.) and its equation; phase; oscillations of a spring -restoring force and force constant; energy in S.H.M. - kinetic and potential energies; Simple pendulum - derivation of expression for its time period; Free, forced and damped oscillations, resonance.

Wave motion. Longitudinal and transverse waves, speed of a wave. Displacement relation for a progressive wave. Principle of superposition of waves, reflection of waves, Standing waves in strings and organ pipes, fundamental mode and harmonics, Beats, Doppler effect in sound

Unit 11: ELECTROSTATICS

Electric charges: Conservation of charge, Coulomb’s law-forces between two point charges, forces between multiple charges; superposition principle and continuous charge distribution.
Electric field: Electric field due to a point charge, Electric field lines, Electric dipole, Electric field due to a dipole, Torque on a dipole in a uniform electric field.

Electric flux, Gauss’s law and its applications to find field due to infinitely long uniformly charged straight wire, uniformly charged infinite plane sheet and uniformly charged thin spherical shell. Electric potential and its calculation for a point charge, electric dipole and system of charges; Equipotential surfaces, Electrical potential energy of a system of two point charges in an electrostatic field.

Conductors and insulators, Dielectrics and electric polarization, capacitor, combination of capacitors in series and in parallel, capacitance of a parallel plate capacitor with and without dielectric medium between the plates, Energy stored in a capacitor.

Unit 12: CURRENT ELECTRICITY

Electric current, Drift velocity, Ohm’s law, Electrical resistance, Resistances of different materials, V-I characteristics of Ohmic and nonohmic conductors, Electrical energy and power, Electrical resistivity, Colour code for resistors; Series and parallel combinations of resistors; Temperature dependence of resistance.

Electric Cell and its Internal resistance, potential difference and emf of a cell, combination of cells in series and in parallel. Kirchhoff’s laws and their applications. Wheatstone bridge, Metre bridge. Potentiometer - principle and its applications.

Unit 13: MAGNETIC EFFECTS OF CURRENT AND MAGNETISM

Biot - Savart law and its application to current carrying circular loop. Ampere’s law and its applications to infinitely long current carrying straight wire and solenoid. Force on a moving charge in uniform magnetic and electric fields. Cyclotron.

Force on a current-carrying conductor in a uniform magnetic field. Force between two parallel current-carrying conductors-definition of ampere. Torque experienced by a current loop in uniform magnetic field; Moving coil galvanometer, its current sensitivity and conversion to ammeter and voltmeter.

Current loop as a magnetic dipole and its magnetic dipole moment. Bar magnet as an equivalent solenoid, magnetic field lines; Earth’s magnetic field and magnetic elements. Para-, dia- and ferro- magnetic substances.

Magnetic susceptibility and permeability, Hysteresis, Electromagnets and permanent magnets.

Unit 14: ELECTROMAGNETIC INDUCTION AND ALTERNATING CURRENTS

Electromagnetic induction; Faraday’s law, induced emf and current; Lenz’s Law, Eddy currents. Self and mutual inductance. Alternating currents, peak and rms value of alternating current/ voltage; reactance and impedance; LCR series circuit, resonance; Quality factor, power in AC circuits, wattless current. AC generator and transformer.

Unit 15: ELECTROMAGNETIC WAVES

Electromagnetic waves and their characteristics. Transverse nature of electromagnetic waves.

Electromagnetic spectrum (radio waves, microwaves, infrared, visible, ultraviolet, Xrays, gamma rays). Applications of e.m. waves.

Unit 16: OPTICS

Reflection and refraction of light at plane and spherical surfaces, mirror formula, Total internal reflection and its applications, Deviation and Dispersion of light by a prism, Lens Formula, Magnification, Power of a Lens, Combination of thin lenses in contact, Microscope and Astronomical Telescope (reflecting and refracting) and their magnifyingpowers.

Wave optics: wavefront and Huygens’ principle, Laws of reflection and refraction using Huygen’s principle. Interference, Young’s double slit experiment and expression for fringe width, coherent sources and sustained interference of light. Diffraction due to a single slit, width of central maximum. Resolving power of microscopes and astronomical telescopes, Polarisation, plane polarized light; Brewster’s law, uses of plane polarized light and Polaroids.

Unit 17: DUAL NATURE OF MATTER AND RADIATION

Dual nature of radiation. Photoelectric effect, Hertz and Lenard’s observations; Einstein’s photoelectric equation; particle nature of light. Matter waves-wave nature of particle, de Broglie relation. Davisson-Germer experiment.

Unit 18: ATOMS AND NUCLEI

Alpha-particle scattering experiment; Rutherford’s model of atom; Bohr model, energy levels, hydrogen spectrum. Composition and size of nucleus, atomic masses, isotopes, isobars; isotones. Radioactivity-alpha, beta and gamma particles/rays and their properties; radioactive decay law. Mass-energy relation, mass defect; binding energy per nucleon and its variation with mass number, nuclear fission and fusion.

Unit 19: ELECTRONIC DEVICES

Semiconductors; semiconductor diode: I-V characteristics in forward and reverse bias; diode as a rectifier; I-V characteristics of LED, photodiode, solar cell and Zener diode; Zener diode as a voltage regulator. Junction transistor, transistor action, characteristics of a transistor; transistor as an amplifier (common emitter configuration) and oscillator. Logic gates (OR, AND, NOT, NAND and NOR). Transistor as a switch.

Unit 20: COMMUNICATION SYSTEMS

Propagation of electromagnetic waves in the atmosphere; Sky and space wave propagation, Need for modulation, Amplitude and Frequency Modulation, Bandwidth of signals, Bandwidth of Transmission medium, Basic Elements of a Communication System (Block Diagram only)

SECTION-B

Unit 21: EXPERIMENTAL SKILLS

Familiarity with the basic approach and observations of the experiments and activities:
1. Vernier callipers-its use to measure internal and external diameter and depth of a vessel.
2. Screw gauge-its use to determine thickness/diameter of thin sheet/wire.
3. Simple Pendulum-dissipation of energy by plotting a graph between square of amplitude and time.
4. Metre Scale - mass of a given object by principle of moments.
5. Young’s modulus of elasticity of the material of a metallic wire.
6. Surface tension of water by capillary rise and effect of detergents.
7. Co-efficient of Viscosity of a given viscous liquid by measuring terminal velocity of a given spherical body.
8. Plotting a cooling curve for the relationship between the temperature of a hot body and time.
9. Speed of sound in air at room temperature using a resonance tube. 10. Specific heat capacity of a given
(i) solid and
(ii) liquid by method of mixtures.
11. Resistivity of the material of a given wire using metre bridge.
12. Resistance of a given wire using Ohm’s law.
13. Potentiometer –
(i) Comparison of emf of two primary cells.
(ii) Determination of internal resistance of a cell.
14. Resistance and figure of merit of a galvanometer by half deflection method.
15. Focal length of:
(i) Convex mirror
(ii) Concave mirror, and
(iii) Convex lens using parallax method.
16. Plot of angle of deviation vs angle of incidence for a triangular prism.
17. Refractive index of a glass slab using a travelling microscope.
18. Characteristic curves of a p-n junction diode in forward and reverse bias.
19. Characteristic curves of a Zener diode and finding reverse break down voltage.
20. Characteristic curves of a transistor and finding current gain and voltage gain.
21. Identification of Diode, LED, Transistor, IC, Resistor, Capacitor from mixed collection of such items.
22. Using multimeter to:
(i) Identify base of a transistor
(ii) Distinguish between npn and pnp type transistor
(iii) See the unidirectional flow of current in case of a diode and an LED.
(iv) Check the correctness or otherwise of a given electronic component (diode, transistor or IC).

AIEEE Examination

2010-02-14T12:16:00.008+05:30

All India Engineering/Architecture Entrance Examination 2010

Scheme of Examination
Entrance examination would consist of two papers i.e. 1st paper consisting of three parts of Physics, Chemistry and Mathematics of equal weightage with objective type questions for BE/B.Tech courses and 2nd paper – consisting of Mathematics,Aptitude Test and Drawing for B. Architecture and B. Planning. The Aptitude Test is designed to evaluate candidate’s perception, imagination, observation, creativity and architectural awareness.

Scoring and Negative Marking
There will be objective type questions with four options having single correct answer. For each incorrect response one fourth (1/4) of the total marks allotted to the question would be deducted. No deduction from the total score will, however, be made if no response is indicated for an item in the answer sheet. The candidates are advised not to attempt such item in the answer sheet if they are not sure of the correct response. More than one answer indicated against a question will be deemed as incorrect response and will be negatively marked. All objective type questions are required to be answered on specially designed machine gradable answer sheets. Answers are to be marked using ball point pen (black/blue) only. For the purpose of evaluation, Test Booklet Code as printed in the Answer Sheet on Side-2 will be accepted as final. Subject combination for each paper & type of questions in each paper are given in the table below :

Requirement of papers for different courses is given in the table below:

Schedule of Examination
AIEEE will be conducted on the following dates as per schedule given below:

For those unable to appear in AIEEE on scheduled date of examination for any reason, including loss of application form/admit card in transit, no re-examination shall be held under any circumstances. The schedule will remain unaltered even if the date is declared as a public holiday.
Students may move to the venue of examination for refreshment etc. if they have applied for BE/B.Tech and B. Arch/B. Planning together.

Syllabus
The question papers for the Examination shall be based on a common minimum syllabus drawn from syllabi taught in different State Boards.

Syllabus Of Mathematics

Syllabus Of Physics

Syllabus Of Chemistry

SYLLABUS FOR APTITUDE TEST B.ARCH./B.PLANNING

Language of the Question Papers
Candidates can opt for question papers either in English or in Hindi. The option has to be exercised while filling Application Form. It cannot be changed later.

Eligibility Criteria : Candidates are, however, required to appear in the papers as per Scheme of Examination for AIEEE specified in para 2.4 of this Bulletin.

The minimum academic qualification for admission through AIEEE 2010 is a pass in the final examination of 10+2 (Class XII) or its equivalent referred to as the qualifying examination

LIST OF QUALIFYING EXAMINATIONS

Those appearing in 10+2 (Class XII) final or equivalent examination may also appear in AIEEE 2010 for consideration of provisional admission. Those appearing in 10+2 (Class 12) in 2011 are not eligible to appear in AIEEE-2010.

Subject combinations required in the qualifying examination for admission to B.E./B.Tech. and B. Arch./B. Planning Courses shall be as under:

*This is as per decision of the All India Council for Technical Education (AICTE).

**Provisionally as per the orders of the Hon'ble High Court of Delhi and directive recieved from the Ministry of Human Resource Development, Govt. of India.

The number of attempts which a candidate can avail at All India Engineering/Architecture Entrance Examination shall be limited to 03(three) uniformly for all the candidates in consecutive years. The candidates passed +2 to exam in 2008, 2009 or appearing in +2 in 2010 are only eligible to appear in AIEEE-2010. Candidates passed +2 in 2007 or before or appearing in 2011 are not eligible to appear in AIEEE-2010.

Date of Birth

Only those candidates whose date of birth falls on or after October 01, 1985 are eligible. However, in the case of Scheduled Caste (SC), Scheduled Tribe (ST) and Physically Handicapped (PH) candidates, upper age limit is relaxed by 5 years, i.e. SC, ST and PH candidates who were born on or after October 01, 1980 are eligible. Date of birth as recorded in the Secondary Education Board/University certificate only will be taken as authentic.

Examination Centres Cities

List of cities where the examination will be conducted is given in Appendix VI. Candidates are required to give four options convenient to them. While every effort will be made to allot a Centre in one of the places opted by the candidate, the Board reserves its discretion to allot a Centre other than that of candidate’s choice any where in India. Under no circumstances, the Centre once allotted shall be changed by the Board.

Admit Card

The Admit Card will be sent by post "Under Certificate of Posting (UPC)" to the candidates (including those who made application online) about four weeks before the conduct of the examination, however, the Board will not be responsible for any consequences that may arise due to loss of admit card in transit. It will be the responsiblity of the candidate to contact/write to the Board in case he/she is not in receipt of the Admit Cards by 6th April 2010. Such requests be sent to Assistant Secretary (AIEEE), Central Board of Secondary Education, PS 1-2 Institutional Area, IP Extension, Patparganj, Delhi-110 092 with 2 photographs (as pasted on the Application Form), one should be attested by Principal of the institution where candidate is studying/passed XII or by the gazetted officer. Photocopy of the Application Form, proof regarding remittance of fee (photocopy of the Demand Draft/Challan) in respect of those candidates who have made application online, and the original postal receipt issued by the Post Office for having dispatched the Application Form by Registered/Speed Post in order to get a duplicate Admit Card. Such request for issue of duplicate admit card should accompany with a Demand Draft in favour of Secretary,CBSE payable at Delhi/New Delhi amounting Rs.50/- as fee and additional Rs.30/- as postal charges for outstation candidates.Request for the issue of admit card after the examination will not be entertained.
In no case the duplicate Admit Card would be issued at the Examination Centres.

Procedure for Conduct of Examination and Use of Answer Sheet

Procedure for conduct of examination and instructions for use of the Test Booklet and Answer Sheet are given in Appendix VII. Candidates are advised to go through carefully before going for the Examination.

Evaluation and Declaration of Results

On the basis of performance in AIEEE, separate rank lists will be prepared for B.E./B.Tech. and B.Arch/B.Planning. Score Card indicating All India Rank and State Rank with total marks and marks in each subject shall be sent to all candidates appearing in AIEEE.

Candidates scoring above a certain cut off percentage of marks (being different for General, OBC, SC/ST/PH category candidates) to be called for counselling shall be determined at the time of declaration of AIEEE results.All India/State Rank and marks shall also be released on AIEEE website. The results of AIEEE-2010 is likely to be declared on or before 7th June, 2010.The All India/State Rank to be called for Central counselling will be decided by Central Counselling Board which will be constituted by the Ministry of Human Resource Development, Govt. of India and decision of seat matrix etc. will be taken by Central Counselling Board. The required information will be displayed at apropriate time on website www.ccb.nic.in .
The score cards will be dispatched to the candidates from 12.06.2010 to 27.06.2010 under Certificate of Posting (UPC). The Board will not be responsible for any consequences that may arise due to loss of score card in transit.In case of non-receipt of the score card within the stipulated period candidate may apply for duplicate score card on payment of Rs. 50/- (plus postal charges of Rs. 30/- for outstation candidates) in the form of Demand Draft in favour of Secretary, CBSE, payable at Delhi/New Delhi between 09.07.2010 to 31.08.2010. No request for issue of duplicate score card will be entertained thereafter.

As per the notified cut off score and the candidates declared eligible up to the notified Rank shall be called to appear for counselling.

In case of two or more candidates obtaining equal marks, inter-se merit of such candidates shall be determined as follows:

B.E/B.Tech - By marks obtained in Mathematics and then in Physics in the AIEEE and then by age (preference to older candidates).

B.Arch/B.Planning - By marks obtained in Aptitude Test and then in Mathematics in the AIEEE and then by age (preference to older candidates).

Rules For Rechecking/Re-Evaluation of Answer Sheets

Since the AIEEE answer sheets are machine graded with extreme care and repeatedly scrutinized, there is no provision for rechecking/re-evaluation of answer sheets. No correspondence in this regard will be entertained.

Counselling, Seat Allocation, Document Verification and Admissions

Final list of institutions admitting students (with intake in each discipline and category as per reservation) through AIEEE-2010, including counselling procedure, counselling schedule and counselling centres would be displayed on the CCB website in May/June 2010. The decision for the above will be taken by the CCB.

The Central Counselling Board shall send by post the Information Brochure for Counselling only to the candidates eligible for counselling. The counselling will be made on line Offcampus and Depending upon the requirement and facilities.

Verification of documents would be done at the time of counselling/admission. The purpose would be to verify different records regarding identification, age, qualifying examination, state of eligibility and category of the candidate. On failing to establish of any of the documents, the candidates will not be considered for admission.

SC, ST, OBC and PH candidates will be required to produce original certificate issued by the competent authority at the time of counselling, failing which they will not be considered for admission.

All correspondence regarding counselling and refund of the amount paid to the Central Counselling Board (CCB) or any of the participating institution should be made with the concerned authorities. No correspondence in this regard be made to CBSE. Legal Jurisdiction

All disputes pertaining to the conduct of AIEEE shall fall within the jurisdiction of Delhi only. The Secretary of the Board shall be the legal person in whose name the Board may sue or may be sued. If any person or officer dealing with the conduct of AIEEE engages himself/herself in act(s) that would result in the leakage of the question paper(s) or attempt to use or help in the use of unfair means in this examination, he/she shall be liable to prosecution under the Indian Penal Code.

Rules Of Reservation

Reservation for SC/ST/OBC and Physically Handicapped candidates will be applicable as per Govt. of India/State concerned existing rules or amended from time to time.