HOLY CROSS COLLEGE (Autonomous) TIRUCHIRAPPALLI B.SC ...

HOLY CROSS COLLEGE (Autonomous) TIRUCHIRAPPALLI – 2

B.SC. DEGREE EXAMINATION, SEMESTER – I, NOVEMBER 2016

MAJOR CORE – 1: GENERAL CHEMISTRY – I

SPECIFIC OUTCOMES OF LEARNING (SOL)

Code: U15CH1MCT01

UNIT I:

The student

1.1 - Recalls about Rutherford’s nuclear model of atom.

- Understand’s the failure of Rutherford’s model.

- lists the postulates of planck’s quantum theory.

- understands the quantization of energy.

- explains photoelectric effect on the basis of quantum theory.

1.2 - lists the postulates of Bohr’s theory .

- explains Bohr’s model of an atom.

- Calculates Bohr’s radius and energy of electron for hydrogen atom.

- explains the origin of hydrogen spectrum based on Bohr’s theory.

- explains the fine structure in hydrogen atom using Sommerfield’s extension of

Bohr’s theory.

- argues the dual character matter.

1.3 - proposes particle and wave character for electron.

- relates various wave properties.

- derives de-Broglie equation.

- states Heisenberg’s uncertainty principle.

- predicts the probability of locating an electron.

1.4 - illustrates the uncertainty principle with Compton effect.

- formulates the postulates of quantum mechanics.

- derives Schrodinger wave equation.

- explains the significance of ψ and ψ2

.

- defines quantum numbers.

- draws the shapes of atomic orbitals.

UNIT II

2.1 - understands the long form of periodic table and the division of elements into s, p, d and f

blocks.

- recalls the cause of periodicity.

2.2 - states Slater’s rule.

- understands the applications and limitations of Slater’s rule.

- understands the filling of atomic orbitals based on Pauli’s exclusion principle.

- writes the electronic configuration of elements by applying Aufbau principle and Hund’s

rule.

2.3 - recognizes the periodic properties.

- defines atomic size, atomic volume, ionization potential, electron affinity, electronegativity

and metallic character.

- understands the variation of periodic properties along a group and a period.

UNIT III

3.1 - states Boyle’s law, Charles’s law and Avagadro’s law.

- deduces ideal gas equation.

- understands deviations from ideal behavior.

3.2 - relates the probability of molecular distribution of velocities and energies with Boltzmann

factor.

- interprets the graphs and draws conclusions.

- establishes the relationship between temperature and molecular velocities.

- predicts the effect of temperature on molecular velocities.

3.3 - defines most probable, root mean square and average velocity.

- establishes the relationship between the three types of velocities.

- applies the principles in problem solving.

- understands the terms collision number, collision diameter, collision frequency and mean

free path.

- understands transport phenomena in gases- viscosity, thermal conductivity and diffusion.

- derives Vanderwaal’s equation of state.

UNIT IV

4.1 - identifies the principles of chemical analysis.

- defines solubility product and understands the limitation of solubility product.

- applies solubility product principle in group analysis.

- applies complexation reaction in the identification of radical.

- illustrates oxidation reduction reactions in semi micro analysis.

- identifies the salts by visual test.

4.2 - formulates the reactions when the salts are treated with dil.H2SO4 and Con.H2SO4.

- outlines the preparation of soda extract.

- infers the reactions for the acid radicals like halides, phosphate, oxalate,

fluoride, arsenite, arsenate, borate, chromate and sulphate with soda extract.

- differentiates i. oxalate from carbonate ii. bromide from nitrate

4.3 - gives reasons for the interference of certain radicals like oxalate, fluoride,

borate, phosphate and arsenate.

- outlines a procedure for the removal of the above radicals.

- selects a suitable solvent for preparing the original solution for the separationof cations.

- classifies the cations into groups

4.4 - identifies acid radicals (simple & eliminating – CO32--

, S2--

, NO3--, Br

--, Cl

--. I

--.

SO4 2--

, Borate, oxalate, F--, and Phosphate) and basic radicals (group 1 to 6

including NH4+)

by their characteristic reactions.

UNIT V

5.1 - The students understands and applies the IUPAC system of nomenclature for aliphatic

compounds.

- applies the IUPAC system of nomenclature to write the structural formula from the given

IUPAC name.

5.2 - classifies the types of covalent bonds.

- illustrates σ and π bond.

- defines polarity of covalent bond.

- gives examples for heterolytic and hemolytic fission of bonds.

5.3 - classifies the organic reactions and illustrates substitution reaction, addition reaction,

elimination reaction, rearrangement and polymerization.

5.4 - formulates the reactions involved in the formation of free radicals, carbenes, carbanion,

carbocation.

- enumerates and explains the methods to detect the existence of free radicals.

- formulates the properties of free radicals, carbocation, carbanion, carbenes.

- identify the stable intermediates and give reasons for their stability.

*****



ALLIED – 1: ALLIED CHEMISTRY PAPER – I [BOTANY AND ZOOLOGY]


Code: U15CH1AOT01

UNIT I:

The student

1.1 - classifies the organic reactions and reagents.

- illustrates the classifications with suitable examples.

- differentiates electrophiles, nucleophiles & free radicals.

1.2 - defines inductive effect.

- recognizes the phenomenon of inductive effect.

- classifies +I and – I effect with example.

- illustrates the effect in various compounds and give reasons for the acidic and

basic nature.

- arrange the acids and bases in increasing or decreasing order.

- defines resonance.

- considers possibilities in writing resonating structures.

- relates resonance with resonance energy, bond length, stability and colour.

- defines hyper conjugation.

- relates hyper conjugation with bond length and stability.

- defines steric effect.

- give reasons for steric effect with suitable examples.

1.3 - recognizes the shape of ‘s’ and ‘p’ orbitals.

- differentiates sigma (σ) and Pi (Π) bond.

- defines the term hybridization.

- recognizes the phenomenon of hybridization.

- applies the concept to molecules like methane, ethylene and acetylene.

1.4 - defines the term isomerism.

- classifies the different types

- defines the structural and stereo isomerism.

- recalls the different types with an example.

UNIT II:

Carbohydrates and Heterocyclic compounds:

2.1 - defines and understands the term carbohydrates.

- classifies the different types.

- recalls the preparation and properties of glucose, fructose and sucrose.

- compares and differentiates the reactions of glucose with fructose.

- give reasons for reducing and non reducing action.

- understands mutarotation.

- identifies carbohydrates by the following tests

i. Tests with Con. H2SO4, Fehling’s solution and ammoniacal silver nitrate.

ii. Molisch Test.

iii. Furfural test.

- briefly explains starch and cellulose.

2.2 - defines heterocyclic compounds.

- explains the aromatic character.

- gives examples for heterocyclic compounds.

- recognizes the preparation, properties and uses of furan, pyrrole, thiphene and pyridine.

- compares pyrrole with pyridine.

- gives reasons for the basicity of pyrrole and pyridine.

- argues about the aromatic character of pyrrole and pyridine.

UNIT III:

Quantum Numbers:

3.1 - understands the principal, azimuthal, magnetic and spin quantum numbers.

- writes the electronic configuration of elements by applying Aufbau principle, Hund’s rule

and Pauli’s exclusion principle.

3.2 - understands long form of periodic table and the division of elements into s, p, d & f

blocks.

- recalls cause of periodicity.

3.3 - recognizes the periodic properties.

- defines atomic radius, ionization energy, electron affinity and electro negativity.

- Understands the variation of periodic properties along a group and a period.

UNIT IV

Chemical Kinetics and Catalysis:

4.1 Chemical Kinetics:

- recalls the definitions for rate, rate constant.

- relates the two by applying the law of mass action.

- defines order and molecularity with suitable examples.

- discriminates the order and molecularity.

- identifies pseudo unimolecular reaction.

- derives the rate constant and half life period for first order and second order

reactions (2A → products).

- determines order of reaction by various methods.

- solves numerical problems.

4.2 Catalysis:

- illustrates the following: Positive and negative catalysis, auto catalysis, induced

catalysis, enzyme catalysis, promoters, catalytic poisons.

- lists out the characteristics of catalysis.

- classifies catalysis.

- explains homogeneous catalysis using the intermediate compound formation theory.

- explains heterogeneous catalysis with the help of the adsorption theory.

UNIT V:

Chromatography & Osmosis:

5.1 - defines chromatography.

- identifies the different phases.

- classifies the different types.

- explains the method of separation of various constituents by

i. Column chromatography ii. Paper chromatography

iii. Thin layer chromatography

- interprets Rf value.

- concludes by listing the various applications.

- defines electrophoresis with an application.

5.2 - defines osmosis and osmotic pressure.

- determine the osmotic pressure by Berkeley and Hartley’s method.

- explains reverse osmosis and desalination.

----------

HOLY CROSS COLLEGE (AUTONOMOUS) TIRUCHIRAPPALLI – 2

B.SC. DEGREE EXAMINATION, SEMESTER III, NOVEMBER 2016

MAJOR CORE – 4 : GENERAL CHEMISTRY – III

SPECIFIC OUTCOMES OF LEARNING [SOL]

Code: U15CH3MCT04

UNIT I :

Second Law of Thermodynamics

1.1 - realizes the need for second law of thermodynamics to predict the direction of natural

processes.

- gives examples for spontaneous processes.

- states the different forms of II law.

- indicates the inability to convert heat completely into work.

- discusses the Carnot’s cycle and sees relationship between efficiency of a heat

engine and the temperature of the source and the sink.

- states and proves Carnot’s theorem.

- differentiates a heat engine from a refrigeration engine.

- solves numerical problems under efficiency.

- derives thermodynamic scale of temperature based on efficiency.

1.2 - defines entropy.

- expresses entropy changes in reversible and irreversible processes.

- concludes by stating II law in the form that all processes occurring in

nature are associated with a gain of entropy of the system and its surroundings.

- defines entropies of fusion, vaporization and transition.

- derives an expression for the entropy change of an ideal gas and finds ΔS at

constant temperature, pressure and volume.

- deduces an expression for entropy of mixing and proves that ΔSmix is always a

positive quantity.

- briefly discusses the physical significance of entropy.

1.3 - derives entropy relationships.

i. Variation of entropy with temperature.

ii. Variation of entropy with pressure and volume- Maxwell’s relations.

- combines the equations to obtain two thermodynamic equations of state.

1.4 - defines the work function and free energy.

- discriminate between the two by proving that

i. - ΔA = Wrev and ii. - ΔG = Wnet

- predicts the change in work function and free energy for an isothermal process.

- derives the various forms of Gibbs-Helmholtz equations.

- predicts the conditions of equilibrium in terms of entropy, work function and free

energy.

UNIT II:

Chemical Potential and Third Law of Thermodynamics :

2.1 - defines partial molar property and chemical potential (Partial molar free energy).

- derives Gibbs-Duhem equation.

- relates chemical potential with partial molar volume and partial molar entropy.

2.2 - derives expression for chemical potential of an ideal gas in a mixture in terms of

mole fraction, molar concentration and partial pressure.

- derives Clausius-Clapeyron equation and applies it to solid-liquid (fusion) and

liquid-vapour (vaporization) equilibria.

- applies Clausius-Clapeyron equation to solve problems.

2.3 - recalls Nernst Heat theorem.

- states the III law of thermodynamics.

- Interprets the variation of entropy with temperature.

- Determines the absolute entropies of solids, liquids and gases.

- Finds exceptions to III law.

- Lists a few applications of III law.

2.4 - states the law of Mass Action.

- applies the law to a general reversible reaction and derives an expression

for the equilibrium constant.

- differentiates between Kp and Kc.

- derives Van’t Hoff reaction isotherm.

- derives thermodynamically the law of chemical equilibrium.

- defines standard free energy of reaction.

- derives the Van’t Hoff’s equation which gives the temperature dependence of

equilibrium constant.

- applies Van’t Hoff equation to solve problems.

UNIT III :

S-block elements:

3.1 - identifies s-block elements.

- gives an account of the physical properties such as atomic and ionic radii, ionization

energy, reducing properties, the electropositive characters, hydration of ions, oxidation

potentials, flame colouration, lattice energy and chemical properties.

3.2 - studies the trends in physical and chemical properties of compound

- compares Li with other elements of group I and Be with other elements of group II.

- defines diagonal relationship.

- enumerates the similarities between Li and Mg, Al and Be.

- discusses the biological importance of Na, K, Ca and Mg ions.

3.3 - discusses the preparation, properties and uses of some specific compounds such

as LiAlH4, NaNH2, NaCN, Beryllium acetate, CaC2, CaCN2, Plaster of Paris, Epsom

Salt.

UNIT IV:

p – block elements:

4.1 - identifies the p-block elements

- gives an account of the physical properties such as electronic configuration, atomic

radii, ionic radii, ionization potential, electron affinity, electro negativity, metallic and

non- metallic properties, oxidation states, inert pair effect, allotropy, catenation and

flame colouration.

4.2 - discusses the preparation, properties and structure of diborane, Borazole

and Borax.

- compares borazole with benzene.

- describes the unique character of carbon in catenation.

- discusses the structure of graphite and diamond.

- explains the use of liquid NH3 as non aqueous solvent.

4.3 - explains the anomalous behavior of oxygen.

- classifies oxides based on their chemical behaviour as acidic oxides, basic oxides,

amphoteric oxides and neutral oxides with examples.

4.4 - describes the unique character of fluorine.

- discusses the properties of pseudo halogens, positive nature of iodine by giving suitable

evidences.

- explains the applications and hazards of chlorofluoro carbons.

- discusses the biological functions and toxicity of iodine.

UNIT V

Aromatic Hydrocarbons:

5.1 - able to give names to the aromatic hydrocarbon and their derivatives.

- explain the structure of benzene using Molecular orbital picture.

- reasons out the stability of benzene ring using the concept resonance.

- defines aromaticity

- states Huckel’s rule and applies to various compounds.

5.2 - identifies the activating and deactivating groups.

- predicts the formation of products and gives reasons for the orientation.

- writes Hammett equation.

- gives the significance and importance of σ and ρ.

5.3 - Proposes the mechanism for electrophilic substitution reaction.

- illustrates the mechanism of nitration, sulphonation, halogenations, Friedel Crafts

acylation and alkylation reaction.

- formulates the other reactions of benzene ring.

- illustrates the nucleophilic substitution reactions in benzene using benzyne mechanism.

5.4 - formulates the synthesis of naphthalene, anthracene, phenanthrene.

- enumerates the properties of these hydrocarbons.

- lists out the uses of these compounds.

****

HOLY CROSS COLLEGE (AUTONOMOUS) TIRUCHIRAPALLI-2

B.SC. DEGREE EXAMINATION, SEMESTER III, NOVEMBER 2016

ALLIED – 4: ALLIED CHEMISTRY PAPER – I [FOR PHYSICS]


CODE: U15CH3AOT01

UNIT I: Fundamental concept:

The student

- classifies the organic reactions and reagents to different groups.

- illustrates this classification.

- defines inductive effect.

- recognizes the phenomenon of inductive effect.

- classifies it into +I and – I effect with examples.

- illustrates the effect in various compounds and gives reasons for the acidic

and basic nature.

- arranges the acids and bases in increasing or decreasing order.

- defines and illustrates resonance.

- considers possibilities in writing resonating structures.

- relates resonance with resonance energy, bond length, stability and colour.

- defines hyperconjucation.

- relates hyperconjucation with bond length and stability.

- defines steric effect.

- gives reasons for steric effect with suitable example.

- relates steric effect with resonance.

Aromatic Compounds:

Benzene:

- recalls the large scale preparation of Benzene from coal tar and petroleum products,

preparation of benzene from acetylene.

- emphasizes the mechanistic aspect of electrophilic substitution reactions such as nitration,

sulphonation, halogenations and Freidel-crafts alkylation and acetylation.

- recalls the equations for the addition of H2 and Cl2 with benzene under difference conditions.

Phenol:

- recollects the preparation of phenol from coal tar and from chlorobenzene.

-gives reason for the acidic behavior of phenol based on resonance.

-writes the equations for the formation of salts, esters and ethers from phenol.

-identifies the product formed when phenol reacts with FeCl3, Zn dust, Benzene – di azonium

chloride and pthalic anhydride.

- recognizes the reactions such as Reimer-Teimen reaction, Kolbes reaction and formulates the

reactions.

Benzaldehyde:

- Learns the preparation of Benzaldehyde from toluene by Rosenmund reduction and

Gattermann – Koch synthesis.

- Identifies the products formed when benzaldehyde undergoes addition reaction with HCN,

Grignard reagent, NH2OH, NH2NHC6H5.

- Recalls the products formed when benzaldehyde reacts with LiAlCl4 and Zn/HCl and with

oxidizing agents.

- Understands and formulates the reactions such as cannizaro reaction, Benzoin condensation,

perkin’s reaction.

Acetophenone:

- learn the preparation of acetophenone by Freidel Crafts – acetylation and catalytic air

oxidation method.

- understands and identifies the product formed on the addition reaction with HCN, Grignard

reagent, NH2OH, NH2NHC6H5 with acetophenone.

- Writes the equation for the reaction of acetophenone with K2Cr2O7 or KMnO4 and reduction

reaction [Clemenson reduction]

- Understand the reactions such as Iodoform reduction, Mannich reaction.

- predicts the product formed.

- identifies the isomers formed based on the orientation of activating and deactivating groups

present in benzene nucleus.

UNIT II:

The student

- defines quantum numbers.

- Understands principal, Azimuthal, magnetic and spin quantum numbers.

- Understand the terms Aufbau’s principle and Hund’s rule.

- States and illustrates Pauli’s Exclusion principle.

- Understands the long form of the periodic table.

- Classifies the elements as s, p, d, f block elements.

- Explains the cause of periodicity.

- Argues about the trends of periodic properties like atomic radius, ionic radius ionization

energy, electron affinity and electronegativity along the groups and periods.

UNIT III

Chemical Bonding:

The student

- defines ionic bonding.

- Explains the factors influencing the formation of ionic bonding.

- Understands the variable electrovalency with examples.

- Lists the properties of ionic compounds.

- Defines covalent bonding.

- Explains orbital overlap concept of molecules like H2, F2, O2 and HF.

- Explains variable covalency.

- list the properties of covalent compounds.

- understands polarity in covalent bonds.

- illustrates Fajan’s rules.

- defines polarization.

- understands the effects of polarization and percent ionic character.

UNIT IV

Electrical and Magnetic properties of molecules

- defines dipolemoment.

- differentiates between polar and non polar molecules.

- understands induced polarization, polarizability, polarization of a

molecule in an electric field.

- identifies Mosotti-Clausius and Debye equations.

- applies dipolemoment measurements to the structure of molecules – CO2,

BCl3, NH3,CCl4 and H2O.

- understands magnetic permeability, magnetic susceptibility and magnetic

moment.

- explains diamagnetism and paramagnetism.

UNIT V:

Solutions and Colligative properties:

The student

- States and explains Raoult’s law.

- Catagorises the solutions as ideal and non ideal solutions.

- defines ideal solution.

- Identifies the non-ideal solutions as Type I, Type II and Type III.(Vapour pressure –

composition curves only)

- Defines the colligative properties, the lowering of vapour pressure and osmotic pressure.

- Relates them to molecular weight of a non-volatile solute.

- Determines the above properties by a suitable method for each.

- Deduces the laws of osmotic pressure.

- Defines reverse osmosis and isotonic solutions.

Phase Rule:

The student

- defines phase, component, degree of freedom.

- States Phase rule.

- Defines one component system.

- Explains the phase diagram of water system.

- Defines two component system.

- Recognizes simple eutectic system.

- Elaborates the phase diagram of Pb-Ag system.

*****



SKILL-BASED ELECTIVE – 3 : INDUSTRIAL CHEMISTRY


Code: U15CH3SBT03

The students

UNIT I:

1.1 - Explains the various processes involved in the Pharmaceutical industry

- Formulates the preparation of p-acetamol, asprin and brufen.

1.2 - Identifies the special varieties of soaps.

- Illustrates the cleansing action of soaps.

- Defines and recognizes the composition of synthetic detergents.

UNIT II

2.1 - Defines dyes, relates the colour with the constitution of dyes by Otto-Witt theory and

Valence

Bond Theory.

2.2 - Classifies the dyes according to application and according to structure.

2.3 - formulates the preparation and list the uses of dyes Malachite green, Methyl orange,

Bismarck brown. Phenolphthalein, Fluorescein, alizarin, Indigo, Anillin yellow,

crystal violet.

UNIT III

3.1 - Understands the occurance of addition and condensation polymers.

- formulates the mechanism of ionic and free radical polymerization.

- Illustrate Ziegler-Natta polymerization.

3.2 - Defines, classifies and give examples for Silicones

- Recalls the stereochemistry of polymers

- Defines plasticity and identifies the types of plastics

- Defines and gives examples for natural and synthetic rubbers.

UNIT IV

4.1 - Identifies the raw materials for the manufacture of glass.

- Explains the steps involved in the manufacture of glass.

- Recognizes the different varieties of glass.

4.2 - Identifies the raw materials for the manufacture of Portland cement

- formulates the reaction involved in the setting of Portland cement.

- Define the term ‘Concrete’

4.3 - illustrates the steps involved in the manufacture of white lead and red lead.

UNIT V

5.1 - List out the functions of essential nutrients

- identifies the types of manures

- recalls N.P.K. fertilizers.

5.2 - Knows the various raw materials used in the paper industry

- Understands the steps involved in the manufacture of paper

*****

HOLY CROSS COLLEGE (AUTONOMOUS) TIRUCHIRAPPALLI-2

B.SC. DEGREE EXAMINATION, SEMESTER V, NOVEMBER 2016

MAJOR CORE – 8: ORGANIC CHEMISTRY

SPECIFIC OUCOMES OF LEARNING (SOL)

Code: U08CH5MCT08

UNIT : I

1.1 - studies the preparation of aliphatic and aromatic monocarboxylic acids.

- Explains Hammett equation and gives the significance of the terms involved in it.

- compares acid strengths of substituted benzoic acids, haloacids. Gives reasons

for the acidity of carboxylic acid.

1.2 - recalls the preparation and properties of aromatic sulphonic acids.

- illustrates the action of heat on dicarboxylic acids and states Blanc’s rule.

- illustrate the action of heat on α, β and γ- hydroxy acids.

- formulates the mechanism of acyl substitution.

1.3 - recollects the characteristics of reactive methylene groups.

- repeats the synthetic applications of malonic and acetoacetic ester, predicts the products.

UNIT II

2.1 - predicts the preparation and properties of aliphatic nitro compounds.

- identifies the conversion of nitrobenzene to o, m and p- dinitrobenzene.

- identifies and recognizes the structures and preparation and uses of T.N.T.

- predicts the products of reduction of nitrobenzene in alkaline, acidic and neutral media.

2.2 - compares the basic characters of aliphatic and aromatic amines.

- studies the methods of separating aliphatic amines.

- predicts the preparation and properties of phenylene diamines.

2.3 - writes the reaction, mechanism of diazotization and gives the applications.

2.4 - recognizes the preparation and synthetic uses of diazomethane and

diazoacetic ester and resonance structure of diazomethane and diazoacetic ester.

UNIT III

3.1 - classifies the amino acids.

- understands and give examples for essential and non-essential amino acids.

- recollects preparation and reactions of amino acids.

- defines zwitter ion and isoelectric point.

3.2 - recalls the definition of polypeptides.

- formulates the synthesis of peptides.

- elucidates the structure of poly peptide by end group ananlysis.

3.3 - categorizes proteins on the basis of physical and chemical properties and studies

physiological functions.

- summarises the primary and secondary structures of proteins.

3.4 - repeats the type of nucleic acids.

- recollects the names of the bases of nucleic acids.

- enumerates the biological functions of DNA and RNA.

UNIT IV:

Molecular Rearrangement:

- defines the term rearrangement, classifies the rearrangement as inter and

intra molecular rearrangement.

- illustrates and formulate the mechanism for the following rearrangements such as

Pinacol-pinacolone, Beckmann, Benzidine, Curtius, Schmidt, Claisen, Fries, Benzilic

acid and Cope rearrangements.

- give reasons for the greater migratory aptitude of certain groups.

UNIT V:

5.1 - classifies the carbohydrates.

- recalls the reactions of glucose and fructose.

- rewrites the inter conversions.

- recollects the ascending and descending series.

5.2 - elaborates the constitution of glucose and fructose.

- illustrates mutarotation with the mechanism.

- illustrates epimerization.

5.3 - formulates the reactions of maltose, lactose and sucrose.

- draws the structures of maltose, lactose and sucrose.

5.4 - enumerates the properties and uses of starch and cellulose.

*******


B.SC. DEGREE EXAMINATION, SEMESTER – V, NOVEMBER 2016

MAJOR CORE - 9 : PHYSICAL CHEMISTRY – I


Code: UO8CH5MCT09

UNIT I:

The student

- defines specific conductance, equivalent conductance and molar conductance.

- Derive the relationship between Κ & Λ.

- Establishes the variation of the Κ & Λ with dilution.

- Defines cell constant and determines the conductance of an electrolyte experimentally.

- Defines ionic mobility and determine it.

- Sees relationship between mobility of ions and discharge of ions at the respective electrodes.

- Understands the determination of transport number of a cation and an anion of an electrolyte

(AgNO3) by Hittorf’s method.

- Determines the transport number by moving boundary method.

- Calculate transport numbers of ions.

- Establishes the effect of concentration on transport number.

UNIT II:

- States Kohlrausch’s law and applies it to calculate Λm of weak electrolyte and ionic

conductances.

- Applies conductance measurements to

i. determine α of a weak electrolyte.

ii. determine ionic product of water.

iii. determine solubility of sparingly soluble salt.

iv. conductometric titration:

a. strong acid Vs strong base.

b. weak acid Vs strong base.

c. mixture of strong acid and weak acid Vs strong base.

d. strong acid Vs weak base.

e. weak acid Vs weak base.

f. KCl Vs AgNO3.

- arrives at the theory of strong electrolyte (Debye Huckel theory) in terms

of interionic forces, asymmetry effect and electrophoretic effect.

- formulates Debye Huckel Onsager equation and estabilishes its significance.

- Discusses Debye Falkenhagen effect and Wien effect.

UNIT III:

- defines electrochemical cell.

- Recalls the construction of Daniel cell.

- Understands the relative tendencies of electrodes to liberate electrons.

- Classifies the reversible electrodes into various types, metal/metal ion, gas/ion,

metal/insoluble salt/anion and redox electrodes.

- Defines and identifies the sign of single electrode potentials.

- Calculates the electrode potentials.

- Elaborates the construction and working

i. standard hydrogen electrode

ii. calomel electrode and

iii. silver-silver chloride electrode

- defines a reversible cell.

- Establishes the relationship between

i. Free energy and electrical energy.

ii. Electrical energy and heat of cell reaction.

- derives Nernst equation.

- Applies it to calculate electrode potential and cell potential.

- Defines the E.M.F. of a cell and determines it potentiometrically.

- Designs Weston Cadmium cell.

- Defines standard electrode potential.

- Tabulates the standard electrode potentials of various electrodes (electrochemical series)

- Applies electrochemical series to

i. calculate Eo Cell.

ii. Predict the spontaneity of the cell reaction.

iii. Calculate ΔGo and K (equilibrium constant) of a reaction.

iv. Predict reactions of metals with acids to liberate hydrogen.

UNIT IV:

- defines a concentration cell.

- Classifies them.

- Derives an expression for the E.M.F. of two types of concentration cells.

- Identifies liquid junction potential in concentration cells with transference and derives an

expression for the same.

- Applies E.M.F. measurements to

i. Calculate transport number.

ii. determine the valency of ions in doubtful cases.

iii. calculate the solubility of a sparingly soluble salt.

iv. determine pH of a solutions using

a. hydrogen electrode.

b. quinhydrone electrode and

c. glass electrode.

v. potentiometric titrations.

- defines over-voltage.

- determines hydrogen over-voltage.

- applies over-voltage to electroplating.

- explains corrosion with the help of electrochemical theory.

- lists out the methods for the prevention of corrosion.

UNIT V: Photochemistry:

- compare photochemical reactions with thermal reactions.

- states and derives – Lambert – Beer’s law.

- States Grothuss-Draper law and Stark-Einstein’s law of photochemical equivalence.

- Defines quantum yield.

- Determines quantum yield using chemical actinometer.

- Classifies photochemical reactions based on quantum yield.

- Gives reasons for high and low quantum yield reactions.

- Solves numerical problems.

- Discusses the kinetics of photochemical combination of hydrogen and bromine.

- Explains photosensitized reactions with examples.

- Discusses fluorescence, phosphorescence and chemiluminescence.

******


B.SC. DEGREE EXAMINATION, SEMESTER – V, NOVEMBER 2016

MAJOR ELECTIVE – 2: CHEMISTRY OF BIOMOLECULES


Code: UO8CH5MET03

UNIT I:

The Student

1.1 - briefly explain the digestion and absorption of carbohydrates.

- restates the fate of glucose after absorption.

1.2 - defines glycogenesis, glycogenolysis, glycolysis, gluconeogenesis.

- gives equations for the biochemical reactions taking place through intermediary

metabolism of carbohydrates.

- explains the 4 steps mentioned above.

1.3 - explains the regulation of blood sugar by kidney and liver.

(metabolic processes)

- defines G.T. test.

- differentiates glycosuria and diabetes mellitus.

UNIT II:

2.1 - defines lipids, gives examples. Enumerates the lipids present in blood.

2.2 - gives an account of oxidation of fatty acid through β-oxidation cycle of

saturated fatty acids with equations.

2.3 - illustrates ketogenesis, ketosis and ketolysis.

- lists out the role of liver in fat metabolism.

2.4 - gives reasons for the formation of fatty liver.

- enumerates the factors influencing absorption of chloresterol.

- defines atherosclerosis and hypercholesterolemia.

UNIT III:

3.1 - briefly explains the absorption of end products of protein digestion.

- recognizes the term metabolic pool.

- gives a general scheme of metabolic pathway of protein metabolism.

- assesses the overall metabolism of protein in terms of N2 present in protein.

3.2 - gives an account of anabolism of protein in terms of protein turnover and

biosynthesis of protein.

- defines – transcription, translation.

3.3 - illustrates the changes undergone by amino acids in the body.

- formulates the reactions.

3.4 - identifies the inborn errors of phenylalanine metabolism.

- recalls the changes in the metabolisms when food is completely withdrawn.

UNIT IV:

4.1 - defines enzymes.

- lists out the properties of enzymes.

- classifies enzymes.

- gives an account of enzyme action.

- enumerates the factors influencing enzyme action.

- defines, classifies enzyme inhibitors.

4.2 - recalls the digestion of food in the mouth, stomach and pancreas and intestine.

- identifies the composition of intestinal juice, pancreatic juice, salivary secretion and gastric

secretion.

4.3 - identifies the beneficial products formed by the action of intestinal bacteria.

- illustrates the terms `fermentation’ and `putrefaction’.

4.4 - identifies the circulating thyroid hormone.

- discusses the metabolic effects of thyroxin.

- recognizes the chemical agents interfering the synthesis of thyroid.

- identifies the diseases associated the abnormal metabolism of thyroxine.

UNIT V:

Identifies the constituents of blood:

5.1 - lists out the functions of plasma protein.

- identifies the blood groups and Rh factors.

- explains the mechanism of blood coagulation.

5.2 - draws the structure of Hb.

- enumerates the properties of Hb.

- gives an account of the metabolism of Hb.

5.3 - gives examples of bile pigments.

- lists out the properties of pigments.

- discusses the disease Jaundice.

******

HOLY CROSS COLLEGE (Autonomous) TIRUCHIRAPPALI-2

B.A./B.SC./B.COM/B.R.SC. DEGREE EXAMINATION – SEMESTER V- NOV. 2016

NON MAJOR ELECTIVE – 1 : HOME CARE


CODE: UO8CH5NMT01

UNIT I:

The student

- identifies a balanced diet.

- Understands the essential nutrients.

- Understands the sources of various essential nutrients.

- Categorizes the composition of a balanced diet for different age groups – infants,

preschool, adolescents, adults and aged.

- Understands the specific functions of nutrients.

- Interprets the effects of cooking on various nutrients.

UNIT II:

Marriage and Family:

- divides the family life cycle into different stages – independence, marriage, parenting,

launching, adult children and retirement.

- Lists and defines types of marriages as polygamy, polygyny, polyandry, monogamy and

group marriages.

- Defines single parenthood.

- Classifies Indian families as modern nuclear family and joint family.

UNIT III:

Fire prevention and Protection:

- identifies the major causes of fire in homes.

- Understands how to prevent fire and fire fighting in homes.

- Classifies the methods of extinguishing fires.

- Defines starvation, cooling and smothering.

- Lists the simple extinguishing agents.

- Recognizes the chemical fire extinguishers.

- Understands the characteristics and functions of CO2 extinguishers.

UNIT IV:

Care of household metals:

- Identifies the ingredients in metal polishes.

- Lists the functions of metal polishes.

- Recollects the composition of metal polishes.

- Lists the general rules for cleaning and polishing.

- Understands the methods of cleaning and polishing of aluminium utensils, silverware,

copper and Brassware, gold and Teflon.

UNIT V:

Safe use of pesticides:

- Understands the need of pesticides at home.

- Identifies common insects at home.

- Understands the pesticides used for each type of insects like mosquitoes, flies, ants,

cockroaches, termites and head louse.

- Lists the precautions in the application of various pesticides at home.

HOLY CROSS COLLEGE (Autonomous) TIRUCHIRAPPALI-2

B.A./B.SC./B.COM/B.R.SC. DEGREE EXAMINATION – SEMESTER V - NOV. 2016

NON MAJOR ELECTIVE – 1: COSMETOLOGY


CODE: UO8CH5NMT02

UNIT I:

The student

- To know the different types of skin.

- To understand the six main functions of skin.

- To list out the important diet for skin.

- To list out the effect of natural sources wind and rain on skin .

- Effects on skin during summer and winter.

- Enumerates the threats to he skin.

- To identify the different skin diseases namely acne, warts.

UNIT II:

- Knows the structure, texture and types of hair.

- Understands the problems of hair such as hair falling, baldness, graying of hair, problems

of lice, dandruff.

- Learns the treatment for above problems.

- Studies the need of hair care – conditioning.

UNIT III

- to define and understand the term facial.

- To study the different types of facial.

- To know about the manual massage.

- To list out the various advantages and disadvantages of massage.

- To define mask treatment and elaborates setting and non-setting masks.

- Lists the uses of setting and non-setting masks.

UNIT IV:

- Classifies the important cosmetics.

- Identifies the types of ingredients in various cosmetics.

- Understands the formulation, preparation, methods and effects of the cosmetics like face

cream, cold cream, vanishing cream.

- Elaborates the characteristics of toilet powders.

- Knows the meaning of dentifrices.

- Lists the ingredients of dentifrices.

UNIT V:

- to understand the meaning of cleansing, toning, moisturizing, exfoliation.

- To know the preparation of cleansing milk, cleansing cream, cleansing lotion.

- To relate the applications of astringents, skin bracers and skin fresheners in toning.

- To understand the importance of moisturizers.

- To know the method of cleansing.

- To classify the types of Exfoliation.

- Lists the types of possible hazards on different types of cosmetics.

********



CHEMISTRY MAIN CORE – 7: INORGANIC CHEMISTRY


Code: U08CH5MCT07

UNIT I:

The student

- Differentiates double salts and co-ordination compounds.

- Defines the terms complex ion, co-ordination number and ligands.

- Classifies the ligands as positive, negative and neutral ligands.

- Illustrates monodentate and polydentate ligands.

- Defines chelates with examples.

- Recalls the physical methods in the study of complexes.

- Formulates and name the mononuclear complexes according to IUPAC system.

- Recalls the postulates of Werner’s theory.

- Explains Sidgwick theory.

- Defines EAN rule.

- Identifies the different types of structural isomerism.

- Explains the geometrical and optical isomerism in 4 and 6 co-ordinated complexes.

UNIT II:

- Understands the postulates of VBT .

- Explains the formation of inner sphere and outersphere complexes.

- Justifies the magnetic properties and geometry of complexes on the basis of VBT.

- Identifies the defects of VBT.

- Draws the shapes of d orbitals.

- Recalls the splitting of d-orbitals.

- Explains the splitting of d-orbitals in octahedral, tetrahedral and square planar

complexes.

- Defines crystal field stabilization energy.

- Explains the factors affecting the magnitude of Δo.

- Applies CFT to explain colour, magnetic properties and spin states (high spin, low

spin) of the complexes.

- Explains John-Teller theorem.

- Identifies the defects of CFT.

- Differentiates labile and inert complexes.

- Recollects the definition of stepwise stability constant and overall stability constant.

- Derives the relationship between stepwise stability constant and overall stability

constant.

- Recalls the factors affecting the stability of complexes.

- Determines the stability constant by Job’s method and Bjerrum method.

UNIT III:

- explains the mechanism of unimolecular and bimolecular substitution in square planar

and octahedral complexes.

- Illustrates trans effect.

- applies trans effect in the preparation of cis and trans isomers.

- discusses the theories of trans effect.

- defines electron transfer reaction.

- classifies electron transfer reaction.

- identifies the mono, binuclear and polynuclear carbonyls of Ni, Cr, Fe and Co.

- formulates the reactions. - draws the structures of the carbonyls.

- gives examples of heteronuclear carbonyls.

UNIT IV:

Nuclear Chemistry:

The student

- Identifies the subatomic particles and stable and unstable particles.

- Enumerates the properties of nuclear particles.

- Explain the nuclear forces and meson theory.

- Illustrates magic number.

- Elaborates the nuclear shell structure and liquid drop model.

- Defines mass defect and nuclear binding energy.

- Calculate the mass defect and binding energy per nucleon.

- Gives reasons for the stability of nucleus based on n/p ratio.

- Illustrates the whole number rule and defines packing fraction.

- Defines and illustrates isotopes, isobars, isotones and isomers.

- Illustrates nuclear transformation based on Bohr’s theory.

- Classifies nuclear reactions.

- Explains the energetic of nuclear reactions.

- Formulates the nuclear reaction induced by charged projectiles and neutron.

- defines and differentiates nuclear fission and nuclear fusion.

- Identifies stellar energy, controlled nuclear fission.

- Explains artificial transmutation and induced radio activity.

- Enumerates the applications of radio isotopes in medicine, agriculture and industry.

- Illustrates carbon dating.

UNIT V:

Bio-Inorganic Chemistry:

- Recalls the structure of porphyrin ring system.

- Draws the structure of myoglobin and cytochrome-C.

- Recognizes the functions of myoglobin and cytochrome-C.

- Draws the structure of plastocyanin (Blue copper proteins) and ferridoxin.

- Recognizes the functions of blue copper proteins and ferridoxin.

Inner Transition elements:

- Writes electronic configuration of Lanthanides.

- recognizes the properties of Lanthanides.

- recognizes magnetic properties, sizes of atoms and ions, colour, solubility,

oxidation states, basic character and chemical reactivity.

- suggests methods for the separation of lanthanides.

- recalls the preparation of Transuranic elements.

- writes electronic configuration of actinides.

- gives reasons for the different oxidation state of actinides.

- enumerates the general properties.

*********



CHEMISTRY MAIN CORE – 7: INORGANIC CHEMISTRY


Code: U08CH5MCT07

UNIT I:

The student

- Differentiates double salts and co-ordination compounds.

- Defines the terms complex ion, co-ordination number and ligands.

- Classifies the ligands as positive, negative and neutral ligands.

- Illustrates monodentate and polydentate ligands.

- Defines chelates with examples.

- Recalls the physical methods in the study of complexes.

- Formulates and name the mononuclear complexes according to IUPAC system.

- Recalls the postulates of Werner’s theory.

- Explains Sidgwick theory.

- Defines EAN rule.

- Identifies the different types of structural isomerism.

- Explains the geometrical and optical isomerism in 4 and 6 co-ordinated complexes.

UNIT II:

- Understands the postulates of VBT .

- Explains the formation of inner sphere and outersphere complexes.

- Justifies the magnetic properties and geometry of complexes on the basis of VBT.

- Identifies the defects of VBT.

- Draws the shapes of d orbitals.

- Recalls the splitting of d-orbitals.

- Explains the splitting of d-orbitals in octahedral, tetrahedral and square planar

complexes.

- Defines crystal field stabilization energy.

- Explains the factors affecting the magnitude of Δo.

- Applies CFT to explain colour, magnetic properties and spin states (high spin, low

spin) of the complexes.

- Explains John-Teller theorem.

- Identifies the defects of CFT.

- Differentiates labile and inert complexes.

- Recollects the definition of stepwise stability constant and overall stability constant.

- Derives the relationship between stepwise stability constant and overall stability

constant.

- Recalls the factors affecting the stability of complexes.

- Determines the stability constant by Job’s method and Bjerrum method.

UNIT III:

- explains the mechanism of unimolecular and bimolecular substitution in square planar

and octahedral complexes.

- Illustrates trans effect.

- applies trans effect in the preparation of cis and trans isomers.

- discusses the theories of trans effect.

- defines electron transfer reaction.

- classifies electron transfer reaction.

- identifies the mono, binuclear and polynuclear carbonyls of Ni, Cr, Fe and Co.

- formulates the reactions. - draws the structures of the carbonyls.

- gives examples of heteronuclear carbonyls.

UNIT IV:

Nuclear Chemistry:

The student

- Identifies the subatomic particles and stable and unstable particles.

- Enumerates the properties of nuclear particles.

- Explain the nuclear forces and meson theory.

- Illustrates magic number.

- Elaborates the nuclear shell structure and liquid drop model.

- Defines mass defect and nuclear binding energy.

- Calculate the mass defect and binding energy per nucleon.

- Gives reasons for the stability of nucleus based on n/p ratio.

- Illustrates the whole number rule and defines packing fraction.

- Defines and illustrates isotopes, isobars, isotones and isomers.

- Illustrates nuclear transformation based on Bohr’s theory.

- Classifies nuclear reactions.

- Explains the energetic of nuclear reactions.

- Formulates the nuclear reaction induced by charged projectiles and neutron.

- defines and differentiates nuclear fission and nuclear fusion.

- Identifies stellar energy, controlled nuclear fission.

- Explains artificial transmutation and induced radio activity.

- Enumerates the applications of radio isotopes in medicine, agriculture and industry.

- Illustrates carbon dating.

UNIT V:

Bio-Inorganic Chemistry:

- Recalls the structure of porphyrin ring system.

- Draws the structure of myoglobin and cytochrome-C.

- Recognizes the functions of myoglobin and cytochrome-C.

- Draws the structure of plastocyanin (Blue copper proteins) and ferridoxin.

- Recognizes the functions of blue copper proteins and ferridoxin.

Inner Transition elements:

- Writes electronic configuration of Lanthanides.

- recognizes the properties of Lanthanides.

- recognizes magnetic properties, sizes of atoms and ions, colour, solubility,

oxidation states, basic character and chemical reactivity.

- suggests methods for the separation of lanthanides.

- recalls the preparation of Transuranic elements.

- writes electronic configuration of actinides.

- gives reasons for the different oxidation state of actinides.

- enumerates the general properties.

******

HOLY CROSS COLLEGE (Autonomous) TIRUCHIRAPPALLI B.SC ...

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