COURSE STRUCTURE WITH CREDIT WEIGHTAGE OF CHEMISTRY …

COURSE STRUCTURE WITH CREDIT WEIGHTAGE OF CHEMISTRY FOR BACHELORS IN

SCIENCE (GENERAL) 2020 AND ONWARDS:

B.Sc. 1st SEMESTER

DISCIPLINE SPECIFIC COURSE (CORE)

CH120C: CHEMISTRY Max. Marks: 60

Course Weightage: 04 Credit (Theory) No. of Contact Hours: 60

Course Objectives:

To introduce students to basic concepts of chemical bonding, S-block elements, general organic chemistry and

states of matter.

Course outcomes: The students after learning the course will be able to:

1. Understand the nature and strength of forces between chemical constituents.

2. Understand the applications of different theories of chemical bonding.

3. Gain knowledge about the chemical reactivity of S-Block elements.

4. Understand stereochemical aspects of organic molecules.

5. Acquire knowledge of aromaticity and reaction intermediates.

6. Understand the structural and behavioral aspects of matter in solid, liquid and gaseous states.

UNIT-I: Chemical Bonding and Molecular Structure (15 Contact hours)

Ionic bond: Lattice energy and Born Haber Cycle. Factors affecting the structure of ionic solids;

Radius ratio effect; Coordination number and limitations of radius ratio rule. Solvation energy and

solubility of ionic solids.

Covalent bond: Formation of hydrogen molecule, Polarity in covalent bonds, Covalent-character of

ionic bond, Fajan’s rules, Percentage ionic character of a polar covalent bond. Dipole moment.

Valence bond theory: Directional characteristics of covalent bond and types of hybridizations.

Limitations of VB theory.

VSEPR theory: Assumptions; geometry of covalent molecules (BeF2, BF3, CH4, PCl5, SF6, SnCl2,

NH3, H2O, SF4, ClF3 and XeF2).

Molecular orbital theory: MO treatment of homo & hetero nuclear diatomic molecules (N2, O2, CO

& NO). Energy level diagrams, Bond order and applications.

UNIT II: S-Block Elements (15 Contact hours)

Electronegativity and electron affinity: Determination and applications. Effective nuclear charge,

slater rules and its applications.

Position of hydrogen in periodic table. Isotopes of hydrogen.

Chemical reactivity of s-block elements towards water, oxygen, nitrogen and halogens. Anomalous

behaviour and diagonal relationships (Lithium, Beryllium, Magnesium and Aluminum). Solubility of

alkali metals in ammonia, Ionic conductance.

Chemical characteristics of the compounds of alkali and alkaline earth metals; oxides and hydroxides,

carbonates, sulphates, halides. Hydrides and their classification.

SEM COURSE

CODE

COURSE TITLE COURSE

TYPE

CREDIT WEIGHTAGE

THEORY PRACTICAL

I CH120C CHEMISTRY DSC-1 4 2

II CH220C CHEMISTRY DSC-2 4 2

III CH320C CHEMISTRY DSC-3 4 2

IV CH420C CHEMISTRY DSC-4 4 2

V CH520DA NUCLEAR CHEMISTRY, HETEROATOMS

AND SOLUTION THERMODYNAMICS

DSE-5 4 2

V CH520DB CHEMISTRY OF BIO-MOLECULES DSE-6 4 2

VI CH620DA SPECTROSCOPY DSE-6 4 2

VI CH620DB ENVIRONMENTAL AND GREEN CHEMISTRY DSE-6 4 2

Unit III: General Organic Chemistry (15 Contact Hours)

Reactive intermediates: Structure, generation and stability of carbocations, carbanions, free-radicals,

carbenes, benzynes and nitrenes.

Aromaticity: Molecular orbital description of benzene. Requirements of aromaticity. Huckel’s rule and

its significance. Antiaromatics and non-aromatics. Aromaticity of non-benzenoid compounds like

pyrrole, thiophene, furan, pyridine and aromatic ions (3, 5 and 7-membered rings).

Stereochemistry: Chirality (up to 2 carbon atoms), Interconversion of Wedge formula, Newmann,

Sawhorse and Fischer representations, Conformers, Conformations with respect to ethane, butane and

cyclohexane.

Geometrical Isomerism: Cis-trans-nomenclature, E / Znomenclature (up to two C=C systems).

Optical isomerism: Enantiomerism, Diastereomerism and Meso compounds. D and L system. CIP

rules: R/ S (for up to 2 chiral carbon atoms). Threo and erythro isomers.

UNIT-IV: STATES OF MATTER (15 Contact hours)

Gaseous State: Deviation of gases from ideal behavior, van der Waal's equation of state.

Critical Phenomenon: PV isotherms of real gases, continuity of states, the isotherms of van derWaal's

equation. Relationship between critical constants and van der Waal's constants, the law of

corresponding states, reduced equation of state.

Molecular velocities: Qualitative discussion of the Maxwell's distribution of molecular velocities. root

mean square, average and most probable velocities; collision number, mean free path and collision

diameter.

Liquid State: Vapour pressure, Viscosity and Surface tension of liquids.

Solid State: Laws of crystallography: (i) Law of constancy of interfacial angles (ii) Law of rational

indices and (iii) Law of symmetry

Symmetry elements in crystals, lattice planes and miller indices. Bragg's equation and derivation.

Interplanar distances in terms of miller indices.

BOOKS RECOMMENDED:

1. Concise Inorganic Chemistry; J.D. Lee; 5thEdn., OUP/Wiley India Pvt. Limited, 2008

2. Chemistry of the Elements; N. N. Greenwood, A. Earnshaw; 2nd Edn, Elsevier India, 2010.

3. Principles of Inorganic Chemistry; B.R. Puri, L.R. Sharma and K.C. Kalia; 33rdEdn., Milestone

Publishers & Distributors/ Vishal Publishing Co., 2017

4. Advanced General Organic Chemistry: A Modern Approach; S.K. Ghosh; 3rd Revised Edn,

New Central, 2010.

5. Organic Chemistry; R.T. Morrison, R.N. Boyd, S. K. Bhattacharjee; 7thEdn, Pearson India,

2011.

6. Organic Chemistry; P.Y. Bruice; 8thEdn, Pearson Education, 2017.

7. Solomons Organic Chemistry; T. W. G. Solomons, C. B. Fryhle, Scott A. Snyder; Global Edn,

Wiley, 2017.

8. March’s Advanced Organic Chemistry: Reactions, Mechanisms and Structure; M. B. Smith;

7th Edition, Wiley, 2013.

9. Principles of Physical Chemistry; B.R. Puri, L.R. Sharma and L.S. Pathania; 47thEdn, Vishal

Pubs & Co, 2017.

10. Atkins' Physical Chemistry; P. Atkins, J. de Paula, J. Keeler; 11thEdn. Oxford University Press,

2018.

11. Physical Chemistry; T. Engel, P. Reid, 3rdEdn, Pearson India, 2013.

12. A Textbook of Physical Chemistry, States of Matter and Ions In Solution (SI Units) - Vol. 1;

K.L Kapoor; 6thEdn, McGraw Hill Education, 2019.

CH120CLab: CHEMISTRY PRACTICAL Max. Marks: 30

Course Weightage: 02 Credits No. of Contact Hours: 60

Section A: Inorganic Chemistry - Volumetric Analysis

1. Preparation of primary standards (Acid, Base, Redox).

2. Titration and standardization of solutions (Acid-Base and Redox)

Section B: Organic Chemistry

1. Purification of organic compounds by crystallization (from water and alcohol) and sublimation.

2. Detection of N, S and halogens in organic compounds.

Section C: Physical Chemistry

1. Surface tension measurement (use of organic solvents excluded).

a. Determination of the surface tension of a liquid or a dilute solution using a

stalagmometer.

b. Study of the variation of surface tension of a detergent solution with concentration.

2. Viscosity measurement (use of organic solvents excluded).

a) Determination of relative viscosity of a liquid or dilute solution using an Ostwald’s

viscometer.

b) Study of the variation of viscosity of an aqueous solution with concentration of solute.

Books Recommended:

1. Vogel’s Qualitative Inorganic Analysis; G. Svehla; 7th Ed., Pearson Education. 2013,

2. Vogel’s Textbook of Quantitative Inorganic Analysis; Bassett, G. H. Jeffery, J. Basset, J.

Mendham, R. C. Denny, 6th ed., ELBS; 2007.

3. Advanced Practical Inorganic Chemistry; Gurdeep Raj; Krishna Prakashan Media (P) Ltd;

2013.

4. Vogel’s Textbook of Practical Organic Chemistry; B.S. Furniss, A.J. Hannaford, P.W.G.

Smith, & A.R., Tatchell; 5th Edn., Pearson India, 2003.

5. Practical Organic Chemistry; F.G. Mann, & B.C. Saunders; Orient-Longman, 1960.

6. Laboratory Manual in Organic Chemistry; R.K. Bansal; 5th Revised Edn, Nw Age International

Limited, 2008.

7. Comprehensive Practical Organic Chemistry: Qualitative analysis Ahluwalia, V.K. & Sunita

Dhingra; Universities Press, India, 2004.

8. Advanced Practical Organic Chemistry; N. K. Vishnoi; 3rdEdn; Vikas Publishing, 2009.

9. Advanced Practical Physical Chemistry; J.B. Yadav; Krishna Prakashan Media (P) Limited,

2015.

10. Advanced Physical Chemistry Experiments; J. N. Gurtu, A. Gurtu, PragatiPrakashan, 2008.

B.Sc. 2nd SEMESTER




Course Objectives:

To introduce students to basics of periodic table (P-block), hydrocarbons, organic reaction

mechanisms and reaction rates.

Course outcomes: The students after learning the course will be able to:

1. Understand the structure, bonding, synthesis, properties and use of the various compounds of

P-block elements.

2. Acquire knowledge about the chemical properties of aliphatic hydrocarbons.

3. Gather knowledge of aliphatic substitution, aromatic substitution and elimination reaction

mechanisms.

4. Understand the rates of second, third order reactions, the dependence of reaction rate on

temperature and comparative account of photochemical and thermal reactions.

UNIT I: P-Block elements (15 Contact hours)

Boron family: Boranes; classification, properties, Structure and bonding with special reference to

diborane. Empirical rules of bonding in higher boranes.

Carbon family: Silicates: Structure, bonding and classification

Nitrogen family: Allotropic forms of phosphorus. Structure and bonding of oxides and oxoacids of

nitrogen and phosphorus.

Oxygen family: Structure and bonding of fluorides and oxyacids of Sulphur. Hydrogen peroxide:

Preparation, properties and uses.

Halogens family: Structure and bonding of hydrogen halides, and oxoacids of halogens. Structure and

bonding of Interhalogens, polyhalides and pseudohalogens.

Noble gases: Fluorides, oxides and oxyfluorides of xenon: Structure and bonding.

UNIT II: Chemistry of saturated and unsaturated hydrocarbons (15 Contact hours)

Alkanes: Low-reactivity of alkanes-chlorination and bromination. The Reactivity-Selectivity

principle.

Alkenes: Structure of alkenes, Preparation of alkenes from alcohols and alkyl halides through

elimination reaction, Hoffmann and Satyzev’s rule, mechanistic and stereochemical implications.

Mechanistic details including regioselectivity and stereochemical implications of halogenation,

hydrohalogenation, hydroboration, epoxidation, hydroxylation and ozonolysis. 1, 2-addition of

isolated diene. 1, 2 and 1, 4-addition reactions of conjugated dienes. Thermodynamic vskinetic control.

Alkynes:Structure and acidic character of alkynes. Mechanisms of addition of halogens, hydrogen,

halides, hydration, hydroboration and catalytic and metal-ammonia reductions of alkynes.

UNIT-III: Organic Reaction Mechanisms (15 Contact hours)

Aliphatic Substitution and Elimination reactions: Mechanistic details of SN1 and SN2, E1 and E2

reactions. Effects of structure of alkyl halides, nature of nucleophiles, leaving groups, solvent and

stereochemical implications of SN reactions.

Aromatic Electrophilic Substitution reactions: General mechanism of aromatic electrophilic

substitution reactions. (Halogenation, Nitration, Sulfonation, Friedel-crafts alkylation and acylation

reactions of Benzene). The second substitution- Effect of substituents on reactivity and orientation.

Mechanisms of Gattermann, Houben-Houesch, Veils-Meir Haack and Riemer-Tieman reactions.

Aromatic Nucleophilic Substitution Reactions (Aryl halides):SNAr and Benzynemechanism

UNIT-IV: Chemical Kinetics (15 Contact hours)

Order of reaction, derivation of integrated rate equations for second (two reactants) and third order

reactions. Determination of order of reaction by differential rate, integration, half-life period and

isolation methods.

Temperature dependence of reaction rates: Arrhenius equation, concept of activation energy.

Theories of chemical kinetics: Simple collision theory based on hard sphere model for atomic

reactions, limitations.

Steady state and equilibrium approximation Kinetics of thermal and photochemical reactions: Decomposition of hydrogen iodide and hydrogen-

bromine.

Books Recommended:





4. Organic Chemistry; R.T. Morrison, R.N. Boyd, S. K. Bhattacharjee; 7thEdn, Pearson India,

2011.

5. Organic Reactions and Their Mechanisms; P.S. Kalsi; 4thEdn, New Age Int. Pvt. Ltd., 2017.

6. Organic Reaction Mechanisms; V.K. Ahluwalia, R.K. Parashar; 4thEdn, Narosa Publishing

House, 2010.

7. Advanced Organic Chemistry; J. Singh, L.D.S Yadav; 14thEdn, PragatiPrakashan, 2017.

8. Organic Chemistry; P.Y. Bruice; 8thEdn. Pearson Education, 2017.


Pubs & Co, 2017.


2018.

11. Physical Chemistry; T. Engel, P. Reid; 3rdEdn, Pearson India, 2013.

CH220C: PRACTICALS Max. Marks: 30

Course Weightage: 02 Credit No. of Contact Hours: 60

Section A: Physical Chemistry

1. Chemical Kinetics and Polarimetry:

a) To determine the specific reaction rate of the hydrolysis of methyl acetate /ethyl

acetate catalyzed by hydrogen ions at room temperature.

b) To determine the angle of rotation and hence specific rotation of an optically active-

compound.

c) To study the kinetics of inversion of cane sugar.

Section B: Organic Chemistry

1. Functional Group Identification: Aromatic hydrocarbons, unsaturation, carboxylic acids,

carbonyl compounds, phenols, alcohols, amines, amides, nitro compounds.

2. Preparation, recrystallization, percent yield and identification (melting point) of the following

reactions products (Any two).

(a) Bromination of Phenol/Aniline

(b) Benzoylation of Aniline/Phenol

(c) 2, 4-dinitrophenylhydrazone formation of aldehyde/Ketones.

Section C: Inorganic Chemistry

1. Determination of acetic acid concentrations in commercial vinegar using NaOH.

2. Determination of calcium content in chalk as calcium oxalate by permanganometry.

3. Determination of ferrous ions by dichromate method.

Books Recommended:

1. Vogel’s Qualitative Inorganic Analysis; G. Svehla; 7th Ed., Pearson Education. 2013.




2013.

4. Vogel’s Textbook of Practical Organic Chemistry; B.S. Furniss, A.J. Hannaford, P.W.G. Smith,

& A.R., Tatchell; 5th Edn., Pearson India, 2003.


6. Laboratory Manual in Organic Chemistry; R.K. Bansal; 5th Revised Edn., New Age International

Limited, 2008.

7. Comprehensive Practical Organic Chemistry: Preparation and Quantitative Analysis;V. K.

Ahluwalia, R. Aggarwaal; Universities Press, India, 2000.



2015.


11. Inorganic Chemistry Practical; D. Pant, Bookrix, 2010.

B.Sc. 3rd SEMESTER




Course Objectives:

To introduce students to basic concepts of periodic table (d-block), chemistry of alcohols, phenol,

ethers, thermodynamics and its applications to equilibria.

Course outcomes: The students after learning the course will be able to understand:

1. The trends in the chemical and physical properties of transition and inner transition elements

along with their compounds.

2. The preparation and chemical reactions of alcohols, phenols and ethers.

3. Laws of thermodynamics and their application to chemical and phase equilibria.

UNIT I: Transition and Inner Transition Elements (15 Contact hours)

Transition elements: Variable-oxidation states. Standard electrode Potentials of M2+/M and M3+/

M2+systems.

Ionic / Covalent and Acidic / Basic character of transition metal oxides in various oxidation states.

Stabilization of unusual oxidation states.

Spectral and magnetic Properties; Calculation and uses of magnetic moment value.

Interstitial hydrides and oxides of first transition series: Preparation, properties &uses.

Inner-Transition elements: Electronic configuration, oxidation states, Magnetic properties and

complexing behaviour of inner-transition elements.

Cause and consequences of Lanthanoid/Actinoid Contractions.

Separation of lanthanoids: Fractional crystallization, Ion–exchange and solvent extraction-methods.

UNIT II: Chemistry of Oxygen Bearing Compounds-I (15 Contact hours)

Alcohols: Classification, relative reactivity of 1o, 2o, 3o alcohols involving cleavage of C-O and O-H

bonds. Reactions of alcohols: Esterfication, alkylation, acetylation, dehydration, oxidation, reaction

with thionyl chloride and Bouvaelt-Blanc-Reduction, Vicinal Diols: Oxidation by per-iodic acid and

lead tetraacetate. Pinacol-Pinacolone rearrangement.

Phenol: Preparation of phenol from cumene. Acidity of phenol and effect of substituents on acidity.

Mechanism of bromination of phenol, Kolbe-Schmidt reaction.

Ethers: Williamson’s ether synthesis. Cleavage of ethers.

Epoxides: Preparation of epoxides. Mechanism of acid/base catalyzed ring openings of epoxides.

Reactions of Grignard and organolithium reagents with epoxides.

UNIT-III: Chemical Thermodynamics (15 Contact hours)

Thermodynamic functions: State and path functions and their differentials. Heat capacity, heat

capacities at constant volume and constant pressure and their relationship, Joule-Thomson effect,

Calculation of w, q, ΔU & ΔH for the expansion of ideal gases under isothermal and adiabatic

conditions. Kirchhoff’s equation.

Second law of thermodynamics: Different statements of the law. Carnot cycle and its efficiency,

Carnot theorem. Concept of entropy, entropy as a function of V&T, and as a function of P&T.

Clausius inequality; entropy as criteria for spontaneity and equilibrium. Entropy change in physical

processes, ideal gas expansion and entropy of mixing of ideal gases. Third law of thermodynamics: Gibbs function (G) and Helmholtz function (A) and spontaneity,

Gibbs-Helmholtz equation, Variation of G and A with P, V and T. Nernst heat theorem, third law of

thermodynamics.

UNIT IV: Chemical and Phase Equilibria (15 Contact hours)

Equilibrium: Relationship between equilibrium constant and free energy change. Thermodynamic

derivation of law of mass action. Clausius-Clapeyron equation, applications.

Phase Equilibria: Meaning of the terms: phase, component and degree of freedom, Phase rule.

Phase diagrams of one component system – water and Sulphur systems. Phase equilibria of two component system: Solid-liquid equilibria, simple eutectic system (Pb-Ag), desilverisation of lead. Partially miscible liquids: Lower and upper consolute temperatures, (examples of phenol-water,

trimethylamine-water, nicotine-water systems). Nernst distribution law and its applications

Books Recommended:


2. Inorganic Chemistry: Principles of Structure and Reactivity; J. E. Huheey, E. A. Keiter, R. L.

Keiter, O. K. Medhi; 4thEdn., Pearson Education India, 2006




5. Reaction Mechanism In Organic Chemistry (Revised Edition); Mukherji and Singh; 3rdEdn,

Macmillan, 2007.

6. Organic Reactions and Their Mechanisms; P.S. Kalsi; 4thEdn, New Age Int. Pvt Ltd., 2017.

7. Advanced Organic Chemistry; J. Singh, L.D.S Yadav; 14thEdn, PragatiPrakashan, 2017.



Pubs & Co, 2017.


2018.

11. Physical Chemistry; T. Engel, P. Reid; 3rdEdn, Pearson India, 2013.

12. A Textbook of Physical Chemistry, Thermodynamics and Chemical Equilibrium (SI Units) -

Vol. 2; K.L Kapoor; 6th Edn, McGraw Hill Education, 2019.



Section A: Inorganic Chemistry

1. Qualitative Analysis: To identify the given Inorganic mixture containing three acidic and

three basic radicals (excluding insoluble and interfering radicals) by Macro Scale. Analysis (06

known and 06 unknown mixtures).

2. Paper Chromatography: Separation and identification of metal ions from mixtures containing

two cations through ascending and radial methods. (03 exercises)

Section B: Physical Chemistry

1. Determination of water equivalent of Calorimeter.

2. Determination of enthalpy of neutralization of hydrochloric acid with sodium hydroxide.

3. Determination of enthalpy of hydration of copper sulphate.

Section C: Organic Chemistry

1. Separation and Identification of binary mixtures of Organic Compounds using H2O, NaHCO3

or NaOH.

2. Organic Synthesis a) Aspirin via Acetylation of Salicylic acid

b) Iodoform from acetone.

c) p-bromoacetanilide from acetanilide.

Books Recommended:





2013.




6. Laboratory Manual in Organic Chemistry; R.K. Bansal; 5th Revised Edn., New Age

International Limited, 2008.

7. Comprehensive Practical Organic Chemistry: Qualitative analysis Ahluwalia, V.K.

&SunitaDhingra; Universities Press, India, 2004.





2015.

11. Senior Practical Physical Chemistry PB; B. D. Khosla; V. C. Garg; A. R. Gulati; R. Chand &

Co, 2008.



B.Sc. 4th SEMESTER




Course Objectives:

To introduce students to coordination chemistry, carbonyl group chemistry and electrochemistry and

introductory quantum chemistry.

Course outcomes: The students after learning the course will be able to understand;

1. The structure, bonding and isomerism in various types of complexes.

2. The preparation and chemical reactions of carbonyl compounds.

3. The electrochemistry of electrodes and cells.

4. The limitation of classical mechanics and importance of quantum mechanics.

UNIT I: Coordination Chemistry (15 Contact hours)

Introduction, experimental verification of Werner’s theory. Effective atomic number: Stability of

coordination compounds (Thermodynamic and Kinetic) and the factors affecting stability. Chelate and

macrocyclic effects.

Stereochemistry of coordination compounds with coordination numbers 2-6; Optical and

Geometrical isomerism.

Bonding in coordination compounds: Valence bond theory, Limitations, Crystal Field theory, crystal

field splitting in tetrahedral, square planar and octahedral systems. Calculation of CFSE, Factors

affecting magnitude of CFSE; pairing energy and CFSE under weak and strong field ligands.

Spectrochemical series. Magnetic and electronic properties of transition metal complexes. Limitations

of crystal field theory.

UNIT II: Chemistry of Oxygen Bearing Compounds-II (15 Contact hours)

Aldehydes and ketones: Structure and reactivity of carbonyl group. Synthesis of aldehydes starting

from acid chlorides and those of ketones from nitriles, carboxylic acids and 1, 3-dithianes. Reactions

of carbonyl compounds with HCN, ROH, NaHSO3, NH2 -G derivatives. Mechanisms involved in

Benzoin, Aldol/Cross Aldol, Perkin, Knoevenagel and Cannizzaro. Condensations / reactions.

Clemmenson and Wolf-Kishner reductions, and Baeyer–Villegar oxidation.

Carboxylic acids and their derivatives: Mechanistic details of preparation of carboxylic acids using

Grignard reagent, hydrolysis of nitriles andoxidation of alkyl benzenes. Factors affecting acid strength

of carboxylic acids. Mechanisms involved in the HVZ reaction, conversion of acids to its derivatives.

Relative stabilities and interconversion of acid derivatives into one another.

UNIT III: Electrochemistry (15 Contact hours)

Arrhenius theory of electrolyte dissociation and its limitations. Kohlrausch’s law. Debye-Huckel-

Onsager's equation for strong electrolytes (elementary treatment without derivation). Transport

number, definition and determination by Hittorf’s and moving boundary methods. Application of

conductivity measurements: determination of degree of dissociation and dissociation constants of

acids, solubility product of a sparingly soluble salt, conductometric titrations. Electrochemical reaction and electrode potential. Nernst equation and its use for estimation of

equilibrium electrode potential. Types of reversible electrodes (half-cells): metal-metal ion, gas-metal-

ion, metal-insoluble salt-anion and redox electrodes. Glass electrode. Standard hydrogen electrode,

Secondary reference electrodes (calomel, Ag/AgCl). Electrochemical series and its significance.

Application of EMF measurements: determination of thermodynamic functions of cell reactions (∆G,

∆H and K.), pH,pKa and solubility product. Concentration cells and its types.

UNIT IV: An introduction to Quantum Chemistry (15 Contact hours)

Limitation of Classical mechanics: Black-body radiation and Planck's radiation law, photoelectric

effect, heat capacity of solids and atomic spectra.

Classical wave equation, concept of quantization in standing waves, de- Broglie equation, Schrodinger

wave equation and its importance. Eigen value equation- Eigen function and Eigen values. Wave

Function and its physical interpretation.

Introduction to operators, Algebra, Rules for setting operators (position and linear momentum),

Hamiltonian operator. Linear and Hermitian operators, commutation of operators. Operator method

for derivation of Schrodinger equation. Postulates of quantum mechanics,

Quantum mechanical treatment of particle in a one-dimensional box.

Books Recommended:

1. Coordination Chemistry; D Banerjee; 3rdEdn., Asian Books, 2009.



3. Advanced Inorganic Chemistry; S. Prakash, G.D. Tuli, S.K. Basu, R.D. Madan; 18th Revised

edition, S Chand, 2000.

4. Advanced Organic Chemistry; J. Singh, L.D.S Yadav; 14thEdn., PragatiPrakashan, 2017.


6. Organic Reactions and Their Mechanisms; P.S. Kalsi; 4thEdn., New Age Int. Pvt. Ltd., 2017.

7. Advanced Organic Chemistry; J. Singh, L.D.S Yadav; 14thEdn., PragatiPrakashan, 2017.

8. Principles of Physical Chemistry; B.R. Puri, L.R. Sharma and L.S. Pathania; 47thEdn.,Vishal

Pubs & Co, 2017.


2018.

10. Physical Chemistry; T. Engel, P. Reid,;3rdEdn., Pearson India, 2013.

11. Quantum Chemistry; D. A. McQuarrie; viva Student Edn., Viva Books, 2016.

12. Quantum Chemistry; R.K. Prasad; 4th revised Edn., New Age International, 2010.



Section A: Organic Chemistry:

Organic Preparations:

a) Dibenzal acetone from benzaldehyde.

b) Adipic acid by chromic acid oxidation of cyclohexanol.

c) Phenol formaldehyde resin.

d) Cinnamic acid by Knoevenagelcondenation.

Section B: Inorganic Chemistry:

Preparation of following coordination compounds of transition metals (Any Three)

a) Potassium trisoxalatoferrate (III)-K3[Fe(C2O4)3].

b) Tetraamine Copper Sulphate [Cu(NH3)4]SO4.

c) Potassium trisoxalatochromate (III).

d) Tristhiourea copper (I) sulphate monohydrate

Section C: Physical Chemistry

a) Construction of the phase diagram of a binary system (simple eutectic) using cooling

curves.

b) Determination of the critical solution temperature and composition of the phenol water

system and study the effect of impurities on it.

Books Recommended:





2013.

4. The Synthesis and Characterization of Inorganic compounds W. A Jolly, 3rdEdn.; 1990.

5. Synthesis and Technique in Inorganic chemistry, G. S. Girlomi; R. J. Angleci; University

Science Books. 3rdEdn.; 1999.




8. Laboratory Manual in Organic Chemistry; R.K. Bansal; 5th Revised Edn., Nw Age






2015.


B.Sc. 5th SEMESTER

DISCIPLINE SPECIFIC ELECTIVES (DSEs)

OPTION-I

CH520DA: CHEMISTRY: NUCLEAR CHEMISTRY, HETEROATOMS AND

SOLUTION THERMODYNAMICS

Max. Marks: 60


Course Objectives:

To introduce students to nuclear chemistry, heteroatom (nitrogen) chemistry and applications of

thermodynamics to solutions.


1. The nuclear structure, radioactivity and its applications.

2. The preparation and chemical reactivity of nitro-compounds, amines and aromatic heterocycles.

3. The applications of thermodynamic principles to solutions.

UNIT I: Nuclear Chemistry (15 Contact hours)

The nucleus: Subatomic particles, nuclear forces (Meson theory), nuclear size and density. Stability

of nucleus: n/p ratio, binding energy, packing fraction, structure of nucleus- Shell model and Liquid

drop model.

Radioactivity: Natural and induced. Radioactive decay-α-decay, β-decay, γ-decay; neutron, emission,

positron emission and electron capture. Group displacement law and radioactive series. Measurement

of radioactivity: ionization chamber, geiger counters, scintillation counters. Applications: Carbon

dating, neutron activation and isotope dilution analyses

Radiation chemistry: Units of radiation; LET and G-Value. Dosimetry, radiation chemistry of oxygen.

UNIT II: Nitrogen bearing compounds (15 Contact hours)

Nitro-compounds: Classification, general properties and preparation (nitration).

Reactions: Reaction with nitrous acid, reduction of nitro compounds by chemical and electrolytic

methods. Di- substitution of aromatic nitro compounds: synthesis of o-, m-, p-dinitrobenzenes.

Amines: Classification and preparation via ammonolysis of halides, reductive amination, reduction of

nitriles, Gabriel-Phthalamide reaction and Hofmann Bromamide reaction.

Basicity of amines, factors affecting basicity. Carbylamine reaction, Hinsberg Test, Schotten–

Baumann Reaction.

Electrophilic substitutions in aniline: Nitration, bromination, sulphonation. Diazonium salts:

Preparation and reactions; Sandmeyer Reaction, Gattermann reaction. Synthesis of phenols and

carboxylic acids from diazonium salts. Coupling of diazonium salts.

UNIT III: Heterocyclic compounds (15 Contact hours)

Naming monocyclic compounds with one and more than one heteroatom, handling the extra hydrogen.

Structural features of pyrrolidine, pyrrole, furan, thiophene, pyridine, piperidine. Comparison of

basicity of pyrrolidine, pyrrole, piperidine and pyridine. Pall-Knorr synthesis of pyrrole, furan and

thiophene. Electrophilic substitution reactions of pyrrole, furan and thiophene and their relativity

reactivity. Mechanistic details in the preparations of indole and quinoline using Fischer-Indole and

Bishlier-Napierlaski synthesis.

UNIT IV: Thermodynamics of solutions (15 Contact hours)

Thermodynamics of ideal solution: Free energy change of mixing, Enthalpy, Volume and Entropy

change of mixing, Non-ideal solutions,Concept of activity and activity coefficient, Chemical potential

and its variation with pressure and temperature, Gibbs Duhem equation

Thermodynamics of colligative properties: Elevation of boiling point and depression of freezing point.

Excess thermodynamic functions of non-ideal solutions.

Books Recommended:

1. Principles of Inorganic Chemistry; B.R. Puri, L.R. Sharma and K.C. Kalia; 33rd Edn. Milestone

Publishers & Distributors/ Vishal Publishing Co., 2017.

2. Essentials of Nuclear Chemistry; H. J. Arnikar; 4th ed.; New Age; 2002

3. Introduction to Nuclear Chemistry; D. J. Carswell; Elsevier; 1967.

4. Fundamentals of Heterocyclic Chemistry by Louis D. Quin and John A. Tyrell.

5. March’s Advanced Organic Chemistry: Reactions, Mechanisms and Structure; M. B. Smith;

7th Edition, Wiley, 2013.


Pubs & Co, 2017.


2018.

8. Physical Chemistry; T. Engel, P. Reid,; 3rdEdn., Pearson India, 2013.

9. A Textbook of Physical Chemistry, Thermodynamics and Chemical Equilibrium (SI Units) -

Vol. 2; K.L Kapoor; 6thEdn, McGraw Hill Education, 2019.

B.Sc. 5th SEMESTER-CHEMISTRY

OPTION-I (LAB COURSE)

CH520DA: PRACTICALS Max. Marks: 30


1. Conductometry

a. To determine the strength of the given acid conductometrically using standard

alkali solutions.

b. To determine the solubility and solubility product of a sparingly soluble electrolyte

conductometrically.

2. pH metry

a. To determine the concentration of a strong acid solution by titration with a strong base.

b. To determine pKa of a weak acid by pH metry.

c. Estimation of acid content of soft drinks by pH metric titrations.

3. Gravimetry (Any Three) a. Estimation of Copper as CuSCN.

b. Estimation of Nickel as [Ni(dmg)2].

c. Estimation of Silver as AgCl.

d. Estimation of Barium as BaSO4.

4. Chromatography and Synthesis

a. Separation of mixture of dyes by TLC / Column chromatography.

b. Preparation of nitro and m-dinitrobenzene from Benzene.

Books Recommended:


2015.


Co, 2008.




2013.






9. Laboratory Manual in Organic Chemistry; R.K. Bansal; 5th Revised Edn, New Age


10. Comprehensive Practical Organic Chemistry: Preparation and Quantitative Analysis; V. K.

Ahluwalia, R. Aggarwal; Universities Press, India, 2000.

B.Sc. 5th SEMESTER


OPTION-II

CH520DB: CHEMISTRY: CHEMISTRY OF BIOMOLECULES

Max. Marks: 60


Course Objectives:

To impart knowledge about biomolecules and their role in bio-systems


1. The structure and properties of biomolecules (carbohydrates, amino acids, proteins, lipids, DNA,

RNA) and their role in bio-systems.

2. The importance of metal ions in bio-systems.

3. The application of thermodynamics to bio-systems.

UNIT 1: Bio-organic chemistry-I (15 Contact hours)

Carbohydrates: Classification of carbohydrates, D and L-Notation, Configuration of aldoses and

ketoses, Reactions of monosaccharides in basic solutions, Oxidation, reduction reactions of

monosaccharides, Chain lengthening: Fischer Kiliani synthesis, Chain shortening: Wohldegration,

Stereochemistry of glucose (Fischer proof). Open chain and cyclic structure of glucose and fructose,

Anomers and mutarotation, Formation of glycosides, Anomeric effect, Reducing and non-reducing

sugars, Structural features of disacharrides (sucrose, maltose, lactose) and polysacharrides (starch and

cellulose).

UNIT II: Bio-organic chemistry -II (15 Contact hours)

Amino Acids: Classification of amino Acids, Essential amino acids, configuration of amino acids,

Acid-base properties of amino acids andIso-electric point.

Peptide and disulfide bonds, Synthesis of simple peptides (upto dipeptides) by N-protection (t-

butyloxycarbonyl and phthaloyl) & C-activating groups and Merrifield solid phase synthesis.

Overview of primary, secondary, tertiary and quaternary structure of proteins. Determination of

primary structure of polypeptides/proteins, End group analysis. Denaturation of Proteins.

Classification of lipids, oils and fats, common fatty acids present in oils and fats. Saponification value,

Iodine number.

Components of nucleic-acids: Adenine, guanine, thymine and cytosine (structure only), other

components of nucleic acids, nucleosides and nucleotides (nomenclature), Structure of

polynucleotides; DNA, RNA.

UNIT III: Bio-inorganic chemistry 15 Contact hours

Concept of essentiality, criteria and classification of essential elements as per their role in living

systems, bulk metals and trace metals, Role of alkali and alkaline earth metals in bio-systems with

special reference to Na+, K+ and Mg2+ ions: Na+/K+ pump; Role of Mg2+ ions in energy production

and chlorophyll. Role of Ca2+ in blood clotting, stabilization of protein structures and structural role

(bones).Application of radioactive elements for biosystems.

Dioxygen transport (haemocyanin and hemoerythrin), Structure and physiological role of hemoglobin

and myoglobin, Bohr effect and cooperativity.

UNIT IV: Biophysical chemistry (15 Contact hours)

Standard free energy, entropy and chemical potential change in biochemical reactions, effect of

temperature and pH on ΔG˚. Methods of determination of free energy changes. Relationship between

Keq and ΔG˚. Oxidation-reduction reactions in biological systems. Free energy changes of oxidation-

reduction changes. High energy compounds: ATP, structure and hydrolysis.

Buffer solutions, buffer in tissues, buffer action, buffer capacity. Coupled reactions and their

significance in biological systems.

Mechanism of membrane transport: Transport through cell membrane, active and passive transport

systems.

Books Recommended:

1. Lehninger’s Principles of Biochemistry, Nelson, D. L. & Cox, M. M. 7th Ed., W. H.Freeman,

2017.

2. Bruice, P.Y. Organic Chemistry, 8th Edition, 2016.

3. Principles of Biochemistry; Voet, voet and Pratt, Wiley and Sons, 2016.

4. Biological Chemistry by James. P. Allen, Wiley Blackwell, 2008.

5. Bio inorganic Chemistry ; K. Hussain Reddy; New Age International (P) Ltd; 2005

6. Metal -Ions in Biochemistry; P. K. Bhattacharya; Narosa Publishing House; 2005.

7. Biophysical Chemistry-J.L. Gurth and A. GurthPragatiPrakashan 2009, 3rd Edition


OPTION-II (LAB COURSE)

CH520DB: PRACTICALS Max. Marks: 30


1. Separation of a given mixture of sugars by paper Chromatography (2 exercises).

2. Separation of a given mixture of amino acids by paper Chromatography (2 exercises).

3. To determine the saponification value of an oil/fat.

4. To determine the iodine value of an oil/fat.

5. Differentiate between a reducing/non-reducing sugars.

6. To find the pKa of a given amino acid.

7. To study the titration curve of glycine.

8. To determine the concentration of glycine solution by formylation method.

Books Recommended:




3. Laboratory Manual in Organic Chemistry; R.K. Bansal; 5th Revised Edn, Nw Age International

Limited, 2008.



5. Comprehensive Practical Organic Chemistry: Qualitative analysis Ahluwalia, V.K. & Sunita

Dhingra; Universities Press, India, 2004.

B.Sc. 6th SEMESTER


OPTION-I

CH620DA: CHEMISTRY: SPECTROSCOPY

Max. Marks: 60


Course Objectives:

To provide basic knowledge of spectroscopy and its applications.


1. The regions of electromagnetic spectrum and its interactions with matter.

2. The underlying principles involved in transitions (rotational, vibrational, electronic NMR),

interpretation of the corresponding spectra and applications

THEORY: 4 CREDITS

Unit- I Spectroscopy-I (15 Contact hours)

Spectroscopy: Electromagnetic radiation, regions of the spectrum, Representation of molecular spectrum, Peak position, intensity and width. Types of peak broadening. Statement of Born-Oppenheimer approximation. Rotational spectrum: Moment of inertia, classification of molecules on the basis of moment of inertia.

Energy of a rigid diatomic rotor, selection rules for rotational transition and associated spectrum,

relative population of rotational levels and spectral intensity, determination of bond length in diatomic

molecules.

Unit-II Spectroscopy-II (15 Contact hours)

Vibrational Spectrum: Classical and quantum mechanical (qualitative) treatment of simple harmonic

oscillator, selection rules for vibrational transition, pure vibrational spectrum of a diatomic molecule,

determination and relation of force constant with bond length and bond energy.

Molecular vibrations, IR transitions and selection rules. Group frequency and fingerprint regions and

its significance. Effect of resonance, inductive effect and H-bonding on infrared absorptions.

Characteristic absorptions of alkanes, alkenes, alkynes, alcohols, ethers, carbonyl compounds, amines

and carboxylic acids and their derivatives.

Unit- III Spectroscopy-III (15 Contact hours)

Photochemistry: Laws of photochemistry. Grothus-Drapper law, Stark-Einstein law. Beer-Lambert

law, molar absorptivity. Jablonski diagram-fluorescence, phosphorescence, non-radiative processes

(internal conversion, intersystem crossing) quantum yield.

Ultraviolet-visible spectroscopy: Presentation and analysis of electronic spectra. Types of electronic

excitations. Chromophores and auxochromes. Bathochromic and hypsochromic shifts. Effects of

conjugation and solvents on absorption bands. Ultraviolet spectra of enes and enones. Prediction of

maxima of enes using Woodward’s rules.

Unit- IV Spectroscopy-IV (15 Contact hours)

Nuclear Magnetic Resonance Spectroscopy: Basic principles of NMR spectroscopy. Shielding and

deshielding of protons. The chemical shift. Equivalent and non-equivalent protons. Spin-spin splitting,

coupling constants for vicinal, geminal and long-range couplings. Characteristic functional group

NMR absorptions. The 1HNMR spectra of ethyl bromide, ethanol, acetaldehyde, ethyl acetate, methyl

propionate, toluene and acetophenone.

Books Recommended:

1. Fundamentals of Molecular Spectroscopy; C. N. Banwell, E.M. McCash; 4thEdn. (Indian Edn.),

Tata McGraw-Hill, 2017.

2. Principles of Physical Chemistry; B.R. Puri, L.R. Sharma and L.S. Pathania; 47thEdn. Vishal

Pubs & Co, 2017.

3. Spectroscopy of Organic Compounds; P.S. Kalsi; 7thEdn, New Age International Pvt. Ltd.,

2016.

4. Introduction to Spectroscopy; D.L. Pavia, G.M. Lampman, G.S. Kriz, J.R Vyvyan;5thEdn.,

Cengage Learning India Pvt. Ltd., 2015.

5. Organic Spectroscopy; L.D.S. Yadav; 1st Edn, Springer Netherlands, 2005.

6. Organic Spectroscopy; W. Kemp; 3rdEdn, Palgrave Macmillan, 2008.

7. Kakkar, R. Atomic & Molecular Spectroscopy: Concepts & Applications, Cambridge

University Press; 2015.

8. John R. Dyer: Applications of Absorption Spectroscopy of Organic Compounds, Prentice Hall.

9. Spectrometric Identification of Organic Compounds; R. M. Silverstein, F. X. Webster, D. J.

Kiemle, D. L. Bryce; 8thEdn., John Wiley & Sons, 2014.


LAB COURSE (OPTION-I)

CH620DA: PRACTICALS Max. Marks: 30


Part 1: Spectrophotometry

1. To determine the λmax of KMnO4 and K2Cr2O7 and calculate the energies of two absorption

bands in these molecules in different units.

2. Verify Lambert-Beer’s law

3. Determination of unknown concentration of CuSO4/KMnO4/K2Cr2O7 in a solution using

spectrophotometer.

4. Spectrophotometric determination of Fe (II), using 1, 10-Phenanthroline.

Part 11: Refractometry

1. To determine refractive index of a liquid by using Abbe’s refractometer. 2. To determine percentage composition of a mixture of two liquids by refractometry

(Glycerol and water). Books Recommended:


2015.


Co, 2008.




5. Experimental Physical Chemistry; A. M. Halpern, & G. C. Mc Bane; 3rd Ed.; W.H. Freeman

& Co; 2006.

6. Experiments in Physical Chemistry; C. W.; Garland, J. W. Nibler, & D. P. Shoemaker, 8th Ed.;

McGraw-Hill: New York, 2003.

7. Principles of Instrumental Analysis; D.A. Skoog, F.J. Holler & T.A. Nieman Cengage Learning

India Ed.

B.Sc. 6th SEMESTER


OPTION-II

CH620DB: CHEMISTRY: ENVIRONMENTAL AND GREEN CHEMISTRY

Max. Marks: 60


Course Objectives:

To sensitize students about importance of environment and ways to keep it pollution free.


1. The harmful impacts of chemicals on the environment.

2. The design of a green process/reaction in lab.

3. The synthesis of industrially important chemicals using green approach.

UNIT I: Environmental Chemistry-I (15 contact hours)

Physical characteristics of atmosphere, Stratification of atmosphere, Energy and mass transfer in the

atmosphere, Chemical and photochemical reactions in the atmosphere, Acid-base reactions in the

atmosphere, Organic and inorganic particulate matter in the atmosphere, Atmospheric pollutant gases,

Acid rain, formation of acid rain and its effects, Photochemical smog: Formation and effects, Green-

house gases and global warming, Ozone layer depletion.

Soil: Nature and composition of soil, Inorganic and organic matter of soil, soil humus, Soil solution,

Acid-base and ion exchange reactions in soils, Macronutrients in soil, N, P, K in soil, Micronutrients

in soil.

UNIT II: Environmental Chemistry-II (15 contact hours)

Wastes and pollutants in soil, soil pH, acidity, alkalinity, Influence of pH on soils, redox potential and

reduction processes in soils, chemical reactions in soil (reactions in soil solution, ion-exchange, ligand

exchange, complexation and precipitation).

Introduction to aquatic chemistry: Gases in water, Nature and types of pollutants in water, Elemental

pollutants, Heavy metals, metalloids, Inorganic pollutants, Algal nutrients and eutrophication, acidity,

alkalinity and salinity, BOD, organic pollutants (sewage, soaps and detergents), pesticides in water,

water disinfection, water reuse and recycle.

UNIT 1II: Green Chemistry-I (15 Contact hours)

Need for green chemistry and role of chemists. Green chemistry and its 12 basic principles (detailed

overview of principles along with examples). Planning a green synthesis in a laboratory (choice of

starting materials, reagents, catalysts, solvents, reaction-conditions like energy sources).

Green solvents: Water, ionic liquids, supercritical water and carbon dioxide.

Green catalysts: Acid, base and oxidation catalysts, biocatalysts, phase transfer catalysis

UNIT IV: Green Chemistry-II (15 Contact hours)

Green reactions in Solid phase/Ionic liquids: Aldol condensation, Cannizaro, Claisen-Schmidt and

Grignard reactions.

Phase-Transfer Catalysis: Michael-addition and Williamson’s ether synthesis.

Enzymatic Transformations: Benzoin condensation, Reduction of aldehydes/ketones using Baker’s

yeast/Daucus carota.

Green processes of Industrial importance: Synthesis of styrene, adipic acid, catechol, urethane,

caprolactam, paracetamol, ibuprofen, slidenafilcitrate, (S)-metachlor, citral, vanillin, menthol and

bioethanol using green route and comparision with their conventional synthetic routes.

Books Recommended:

1. New Trends in Green Chemistry, V. K. Ahluwalia, M. Kidwai: Anamaya Publishers: New

Delhi: Ist Edition: 2004.

2. Green Chemistry-Environment Friendly Alternatives, RashmiSanghi& M. M. Srivastava:

Narosa: 2007.

3. Green Chemistry-An Introductory Text; IInd Edition: Mike Lancaster: RSC: 2010.

4. Green Chemistry-Theory and Practice; P.T. Anastas and J. C. Warner; Oxford; 2000

5. Green Chemistry-Environmentally Benign Reactions, V.K. Ahluwalia, Anne Books Pvt.

Limited; 2012.

6. Green Chemistry: Fundamentals and applications, S.C. Ameta, R.Ameta, Apple academic

press, 2013.

7. Green Chemistry and Processes: MukeshDoble, Anil Kumar Kruthiventi; Academic Press-

Elsevier 2007.

8. Principles of Environmental Chemistry, R. M. Harrison: RSC Publishing, 2007.

9. Environmental Chemistry, S. E. Manahan, CRC Press LLC, 2000.

10. Environmental Chemistry; A. K. De, 7th Edn; New Age International Pvt Ltd; 2010.

11. Environmental Chemistry Fundamentals, J.G. Ibanez, M.H. Esparza, C.D. Serrano, A.F.

Infante, M. M Singh, Springer Publishers, 2007.


OPTION-II (LAB COURSE)

CH620DB: PRACTICALS Max. Marks: 30

Course Weightage: 02 Credit No. of Contact hours: 60

Part 1: Green Chemistry

1. Micelle assisted reduction of aromatic carbonyl compound in water using NaBH4 (Aqueous

phase reaction)

2. Photoreduction of benzophenone to benzopinacol in presence of sunlight (Photochemical

reaction).

3. Reduction of acetophenone using Daucuscarrotaroot (Enzymatic transformations).

4. Aldol condensation in solid phase between an aromatic aldehyde and acetophenone(Solid

phase reaction).

5. Solid phase synthesis of hydrazone from an aromatic aldehyde/ketone and phenyl hydrazine.

Part-II: Environmental Chemistry

1. Determination of pH of soil sample using pH meter.

2. Determination of pH, acidity and alkalinity of a water sample.

3. Determination of total soluble salts in soil using conductance measurements.

4. Determination of carbonate and bicarbonates in soil.

5. Estimation of total hardness of water by EDTA method.

6. Determination of calcium, magnesium and iron in soil.

7. Determination of dissolved oxygen (DO) of a water sample.

8. To determine the total residual chlorine in a water sample.

9. To determine chloride ion in a given water supply by argentometric method.

Books Recommended:

1. Green Chemistry: Environmentally Benign Reactions, V.K. Ahluwalia 2nd Edition,Ane

Books Pvt. Ltd, 2012.

2. Green Chemistry Experiment: A monograph International Publishing House Pvt Ltd. New

Delhi. Bangalore Sharma, R.K.; Sidhwani, I.T. &Chaudhari, M.K. I.K. (2013).

3. Solvent Free Organic Synthesis, Koichi Tanaka; Wiley VCH VerlagGmbHand Co.

KGaWienhiem Germany.

4. Introduction to Organic Laboratory Techniques: A Microscale and Macro Scale Approach,

Pavia, D.L., Lampman, G.M., Kriz, G.S. & Engel, R.G. 1995.

5. A Laboratory Manual for Environmental Chemistry, R. Gopalan, R. W. Sugumar, I K

International Publishing house Pvt. Ltd; 2008.

6. Experiments in Environmental Chemistry: A laboratory Manual, D. W. Connell and P.D.

Vowles, IstEdn., Pergamon International Library, 1980. 7. Quantitative Chemical Analysis, D. C. Harris, 8thEdn. W. H. Freeman. And Co, 2010.

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