Revised syllabus of FYBScChemistry SemI II CBCS Vide Item No 65R_1 Syllabus Mumbai University by munotes
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AC – 11/07/2022
ItemNo. 6.5 (R)
UNIVERSITYOF MUMBAI
Revised Syllabus for
F.Y.B.Sc.
(Chemistry)
Semester:I&I I
(CBCS)
(Witheffectfrom the academic year 2022 -23)
Page 4
Page 5
Proposed syllabus for CBCS
F. Y. B. Sc. Chemistry
For the subject of chemistry , there shall be two papers for 45 lectures each comprising of
three units of 15 L each.
Semester -I
1. Paper -I / II (General Chemistry) Unit -I will be for PhysicalChemistry
2. Paper -I / II Unit -II will be for Inorganic Chemistry
3. Paper - I / II Unit -III will be for OrganicChemistry.
Semester -II
1. Paper -I /II (General Chemistry) Unit -I will be for PhysicalChemistry
2. Paper -I / II Unit -II will be for Inorganic Chemistry
3. Paper -I / II Unit -III will be for OrganicChemistry
Page 6
Choice Based Credit System F.Y.B.Sc. Chemistry
Syllabus To be implemented from the
Academic year 2022 -2023
SEMESTER I
Course Code Unit Topic Credits L/per week
USCH101
I
Chemical Thermodynamics
2
1
Chemical calculations
II
Atomic structure
1
Periodic Table and periodicity
III
Basics of Organic Chemistry:
1
Bonding and Structure of organic
compounds
Fundamentals of organic reaction
Mechanism
USCH102
I
Chemical Kinetics
2 1
Liquid States
II
Comparative Chemistry of Main
Group elements 1
III
Stereochemistry I 1
USCHP1
Chemistry Practical 2 6
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SEMESTER II
Course Code Unit Topic Credits L/per week
USCH201
I
Gaseous State
2
1
Electrochemistry – I
Chemical Equilibria and
Thermodynamic Parameters
II
Concept of Qualitative Analysis
1
Acid Base Theories
III
Chemistry of Aliphatic Hydrocarbons
1
USCH202
I
Ionic Equilibria
2
1
Photochemistry
Molecular Spectroscopy
II
Chemical Bond and Reactivity
1
Oxidation Reduction Chemistry
III
Stereochemistry II
1
Aromatic Hydrocarbons
USCHP 2
Chemistry Practical
2
6
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Programme Outcomes
B.Sc. Chemistry
The student graduating with the Degree B.Sc Chemistry should be able to acquire ;
i) Core competency: Students will acquire core competency in the subject Chemistry, and in
allied subject areas.
ii) A systematic and coherent understanding of the fundamental concepts in Physical
chemistry, Organic Chemistry, Inorganic Chemistry, Analytical Chemistry , and all other
related allied chemistry subjects.
iii) Students will be able to use the evidence -based comparative chemistry approach to explain
chemical synthesis and analysis.
iv) Students will be able to characterize, identify and separate components of organic or
inorganic origin and will also be able to analyze them by making use of the modern
instrument al methods learned.
v) Students will be able to understand the basic principle of equipment and instruments used in
the chemistry laboratory.
vi) Students will be able to demonstrate the experimental techniques and methods of their area
of specialization in Che mistry
vii) The course curriculum also includes components that can be helpful to graduate students to
develop critical thinking ability by way of solving problems/numerical using basic
chemistry knowledge and concepts.
viii) Appreciate the central role of chemistr y in our society and use this as a basis for ethical
behavior in issues facing chemists including an understanding of safe handling of
chemicals, environmental issues , and key issues facing our society in terms of energy,
health , and medicine.
ix) Lifelong le arner: The course curriculum is designed to inculcate a habit of learning
continuously through the use of advanced ICT techniques and other available
techniques/books/journals for personal academic growth as well as for increasing
employability opportunity.
Page 9
SEMESTER I
Paper I
UNIT I
1.1 Chemical Thermodynamics (10 L)
Thermodynamic terms; System, surrounding, boundaries, types of system, Intensive
and Extensive properties, State functions and path functions, Thermodynamic processes.
First law of thermodynamics: Concept of heat (q), work (w), internal energy (U),
enthalpy, heat capacity, relation between heat capacities, sign conventions, calculations
of heat, work, internal energy and enthalpy (H).
Thermochemistry: Heat of reactions, standard sta tes, enthalpy of formation of
molecules, enthalpy of combustion and its applications, calculations of bond energy,
bond dissociation energy and resonance energy from thermochemical data, Kirchhoff’s
equation
(Numerical problems expected wherever necessary )
1.2 Chemical Calculations: (5L)
Methods of expressing concentration of solutions: Normality, Molarity, Formality, Mole
fractions, Weight ratio, Volume ratio, Weight to volume ratio, ppm, ppb, millimoles,
milliequivalents, Preparation of solutions.
(Numeri cal problems expected wherever necessary)
UNIT II
2.1 Atomic structure:(8 L)
Historical perspectives of the atomic structure; J. J. Thomson Model, Rutherford’s
Atomic Model - alpha particle scattering experiment, Bohr’s theory, its limitations and
atomic spectrum of hydrogen atom. Structureof hydrogenatom.
Hydrogenicatoms:
1. Simple principles of quantummechanics
2. Atomicorbitals
i) Hydrogenic energylevels
ii) Shells, subshells and orbitals
iii) Electronspin
iv) Radial shapes oforbitals
v) Angular shapes oforbitals.
Aufbauprinciple, Hund's rule of maximum multiplicity and Pauli exclusion principle
2.2 Periodic Table and periodicity: (7 L)
Long form of Periodic Table; Classification for elements as main group, transition and
inner transition elements .
Periodicity in the following properties: Atomic and ionic size , electron gain enthalpy ,
ionization enthalpy, effective nuclear charge (Slater’s rule) , electronegativity,
Pauling and Mulliken methods. ( Numerical proble msexpected, wherever applicable.)
Unit III
3 Basics of Organic Chemistry
3.1 Classification and Nomenclature of Organic Compounds: (5L)
Nomenclature of mono and bi -functional aliphatic compounds on the basis of
priority order of the following classes of compounds : Alkanes, alkenes, alkynes,
haloalkanes, alcohols, ethers, aldehydes, ketones, carboxylic acids, carboxylic acid
Page 10
derivatives (acid halides, esters, anhydrides, amides), nitro co mpounds, nitriles and
amines and their cyclic analogues.
3.2 Bonding and Structure of organic compounds: (4L)
Hybridization : sp3, sp2, sp hybridization of carbon and nitrogen; sp3 and sp2
hybridizations of oxygen in Organic compounds (alcohol, ether, aldehyde, ketone,
carboxylic acid, ester, cyanide, amine and amide)
Overlap of atomic orbitals: Overlaps of atomic orbitals to form sigma and pi bonds,
shapes of organic molecules.
Shapes of molecules; Influence of hybridization on bond properties (as applicable to
ethane, ethene, ethyne).
3.3 Fundamentals of organic reaction mechanism: (6L)
Electronic Effects: Inductive, electromeric, reso nance and mesomeric effects,
hyperconjugation and their applications. Dipole moment ; Organic acids and bases; their
relative strengths.
Basic terms & concepts :: Homolytic and Heterolytic fission with suitable examples.
Electrophiles and Nucleophiles; Nucl eophilicity and basicity, Electrophilicity and
acidity.
Types (primary, secondary, tertiary, allyl, benzyl), shape and their relative stability
of the following reactive intermediates :
i. Carbocations ii. Carbanions and iii. Free radicals
Introduction to types of organic reactions: Addition, Elimination and Substitution
reaction. (With one example of each)
Semester - I
Paper – II
Unit – I
1.1 Chemical Kinetics: (8L)
Rate of reaction, rate constant, measurement of reaction rates, order and molecularity of
reaction, Integrated rate equation of first order and Second order reactions (with equal
initial concentration of reactants)
Determination of order of reaction by a) Integration method b) Graphical method c)
Ostwald’s isolation method d) Half time method,
Effect of temperature on the rate of reaction, Concept of activation energy and its
calculation from Arrhenius equation (derivation not expected).
(Numerical proble ms expected wherever necessary).
1.2 Liquid State : (7L)
Surface tension: Introduction, methods of determination of surface tension by drop
number method
Viscosity: Introduction, coefficient of viscosity, relative viscosity, specific viscosity,
reduced viscosity, determination of viscosity by Ostwald viscometer
Refractive index : Introduction, molar refraction and polarizability, determination of
refractive index by Abbe’s refractometer.
Liquid crystals : Introduction, Classification and structure of thermotropic phases
(Nematic, Smectic and Cholesteric phases), applications of liquid crystals.
(Numerical problems expected wherever necessary).
Unit II
2 Comparative chemistry of MainGroupElements:(15L)
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Metallic and non -metallic nature, oxidation states, electronegativity, anomalous behavior
of second period elements, allotropy, catenation, diagonal relationship.
Comparative chemistry of oxides and hydroxides of gr oup I and group II elements.
Some important compounds - NaHCO3, Na2CO3, CaO, CaCO3;
oxides of carbon, oxides of Sulphur and Nitrogen with respect to environmental aspects
like greenhouse effect, photochemical smog and acid rain.
Unit III
3 Stereochemistry I: (15L)
Projection formulae: Flying Wedge projection, Fischer Projection, Newman and
Sawhorse Projection formulae (of erythro, threo isomers of tartaric acid and 2,3 -
dichlorobutane) and their interconversions; Geometrical isomerism in alk ene and
cycloalkanes : cis–trans and syn -anti isomerism E/Z notations with C.I.P rules.
Optical Isomerism: Optical Activity, Specific Rotation, Chirality/Asymmetry,
Enantiomers, Molecules with two similar and dissimilar chiral -centres , Diastereoisomers,
meso structures, racemic mixture and resolution (methods of resolution not expected).
Relative and absolute configuration : D/L and R/S designations. Conformational
analysis of alkanes (ethane, propane and n -butane); Relative stability with energy
diagrams
Semester II
Paper I
Unit I
1.1 Gaseous State (6L)
Kinetic theory of gases, Maxwell -Boltzmann’s distribution of velocities (Qualitative
discussion), Ideal gas laws, Deviation from ideal gas laws, Ideal and real gases, Reasons
for deviation from ideal gas laws, Compressibility factor, Boyle’s temperature, van der
Waals equation of state, Critical phenomena, Relation between critical constants and van
der Waals constants.
( (Numerical problems expected wherever necessary)
1.2 Electrochemistry - I (4 L)
Conductance, specific conductance, equivalent conductance, molar conductance,
Variation of molar conductance with concentration of strong and weak electrolyte.
Reversible electrodes, Electrode potential, standard electrode potential, Galvanic cells,
Conventions to represent the galvanic cells, Concept of emf of cell.
(Numerical problems expected wherever necessary)
1.3 Chemical Equilibria and Thermodynamic Parameters (5L)
Second law of thermodynamics, concept of entropy, Physical significance of e ntropy,
Concept of free energy, Helmholtz and Gibbs free energy, Variation of free energy with
temperature and pressure, Spontaneity and Physical significance of free energy.
Re Reversible and irreversible reactions, equilibrium constants (Kc and Kp), rela tionship
between Kc and Kp. Thermodynamic derivation of equilibrium constant
(Numerical problems expected wherever necessary)
Unit II
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2 Concept of Qualitative Analysis:(8 L)
2.1 Testing of Gaseous Evolutes, Role of Papers impregnated with Reagents in qualitative
analysis (with reference to papers impregnated with starchiodide, potassium dichromate,
lead acetate, dimethylglyoxime and oxinereagents).
Precipitation equilibria, Formation of precipitates likeAgCl, AgBr, AgI and BaSO 4
effect of common ions, uncommon ions, oxidationstates, buffer action, complexing
agents on precipitation of ionic compounds. (Balanced chemical equations)
2.2 Acid Base Theories: (7L)
Arrhenius, Lowry - Bronsted, Lewis, Solvent – Solute concept of acids and bases,
Usanovich concept, Hard and Soft acids and bases, Applications of HSAB.
Unit III
3 Chemistry of Aliphatic Hydrocarbons
3.1 Carbon - Carbon sigma bonds: (3L)
Chemistry of alkanes: Formation of alkanes, Wurtz Reaction, Wurtz -Fittig reaction, free
radical substitutions: Halogenation - relative reactivity and selectivity
3.2 Carbon - Carbon pi bonds (12L):
Formation of alkenes and alkynes by elimination reactions : Mechanism of E1, E2,
E1cb reaction. Saytzeff and Hofmann eliminations
Reactions of alkenes : Electrophilic additions with mechanisms
(Markownikoff / AntiMarkownikoff addition),
Mechanism of oxymercuration - demercuration, hydroboration - oxidation, ozonolysis,
reduction (catalytic and chemical), syn - and anti -dihydroxylati on (oxidation), 1, 2 - and
1, 4-addition reactions in conjugated dienes, Diels -Alder reaction.
Reaction of alkynes : Acidity, Electrophilic and Nucleophilic additions with
mechanisms. Hydration to form carbonyl compounds, Alkylation of terminal alkynes
Semester II
Paper II
Unit I
1.1 Ionic Equilibria: (7L)
Strong and weak electrolytes, degree of ionization, factors affecting degree of
ionization,Ionization constant and ionic product of water, Ionization of weak acids and
bases, Dissociation constants of mono -, di-, and tri -protic acids.
P pH scale, Buffer solutions, types of buffers, Derivation of Henderson equation for acidic
and basic buffers, Buffer action, buffer capacity
(Numerical problems expected, wherever necessary)
1.2 Photochemistry (4L)
Laws of photochemistry, Quantum yield or efficiency, experimental determination of
quantum yield, Reasons for low and high quantum yield, Primary and secondary
processes.
Photochemical reactions (with suitable examples), Photosensitizers and photosensitized
reactions, Fluorescence, Phosphorescence and Chemiluminescence.
(Numerical problems expected, wherever necessary)
1.3 Molecular Spectroscopy: (4L)
E Electromagnetic radiation, electromagnetic spectrum, Planck’s equat ion, Interaction of
electromagnetic radiation with matter; Absorption, Emission, Scattering, Electronic,
Vibrational and Rotational transitions, Beer -Lamberts law.
Page 13
(Numerical problems expected, wherever necessary)
Unit II
2.1 Chemical Bond and Reactivity:( 10 L)
Types of chemical bond, comparison between ionic and covalent bonds, polarizability
(Fajan’s Rule), shapes of molecules, Lewis dot structure, Sidgwick Powell Theory, basic
VSEPR theory for AB n type molecules with and without lone pair of electrons,
isoelectronic principles, applications and limitations of VSEPR theory.
2.2 Oxidation Reduction Chemistry: (5L)
Reductionpotentials,
Redox potentials: half reactions ; balancing redoxequations.
Applications of redoxchemistry ; Redox reagents in Volumetric analysis ;
a) I2
b)KMnO4
Unit III
3.1 Stereochemistry II: (5L)
Cycloalkanes and Conformational Analysis: (5L)
Types of cycloalkanes and their relative stability, Baeyer strain theory, Conformational
analysis of cyclohexane: Chair, Boat and Twist boat forms; Relative stability with
energy diagram .
3.2 Aromatic Hydrocarbons: (10L)
Aromaticity: Hückel’s rule, anti -aromaticity, aromatic character of arenes, cyclic
carbocations/carbanions and heterocyclic compounds with suitable examples.
Electrophilic aromatic substitution: halogenation, nitration, sulphonation and Friedel -
Crafts alkylation/acylation with their mechanism, Directing effects of the groups
Reference Books:
Unit – I
1) Concise Graduate Chemistry – I, II, III & IV , University Text Book of Chemistry , University
of Mumbai.
2)
3) Atkins, P. W. & Paula, J. de Atkin’s Physical Chemistry 10th Ed., Oxford
University Press (2014).
4) Castellan, G. W. Physical Chemistry 4th Ed. Narosa (2004).
5) Keith J. Laidler& John H. Meiser, Physical Chemistry, 2nd Ed. (2004)
6) Puri B. R., Sharma L. R. &Pathania M. S. Principles of Physical Chemistry, Vishal
Publishing Company, 2008
7) Ball, D. W. Physical Chemistry Thomson Press, India (2007).
8) Mortimer, R. G. Physical Chemistry 3rd Ed. Elsevier: NOIDA, UP (2009).
9) Engel, T. & Reid, P. Physical Chemistry3rd Ed., Prentice -Hall (2012).
10) McQuarrie, D. A. & Simon, J. D . Molecular Thermodynamics Viva Books Pvt.
Ltd.: New Delhi (2004).
11) Levine, I .N. Physical Chemistry 6th Ed.,Tata Mc Graw Hill (2010).
Page 14
Unit II
1. Concise Graduate Chemistry – I, II, III & IV, University Text Book of Chemistry, University
of Mumbai.
2. Lee, J.D. Concise Inorganic Chemistry ELBS, 1991.
3. Douglas, B.E. and McDaniel, D.H. Concepts & Models of Inorganic Chemistry , Oxford, 1970
4. Atkins, P.W. & Paula, J. Physical Chemistry, 10th Ed., Oxford University Press, 2014.
Day, M.C. and Selbin, J. Theoretical Inorganic Chemistry, ACS Publications, 1962.
5. Rodger, G.E. Inorganic and Solid State Chemistry, Cengage Learning India
Unit III
1. Concise Graduate Chemistry – I, II, III & IV, University Text Book of Chemistry,
University of Mumbai.
2. Morrison, R. T. and Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt Ltd.
(Pearson Education).2012
3. Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt Ltd. (Pearson
Education).
4. Finar, I. L. Organic Chemistry (Volume 2: Stereochemistr y and the Chemistry of Natural
Products), Dorling Kindersley (India) Pvt Ltd. (Pearson Education).
5. Eliel, E. L. and Wilen, S. H. Stereochemistry of Organic Compounds, Wiley: London, 1994
6. Kalsi, P. S. Stereochemistry Conformation and Mechanism, New Age Inte rnational, 2005.
7. Mc Murry, J.E. Fundamentals of Organic Chemistry, 7th Ed. Cengage Learning India
Edition, 2013
8. Paula Y Bruice, Organic Chemistry, 7th Ed, Pearson education, Asia.2014
9. Graham Solomon, Fryhle, Dnyder, Organic Chemistry, Wiley publication. 12 th Ed,2016
10. Bahl and Bahl, Advanced Organic chemistry by S. Chand publication.2010
11. Peter Sykes. Guidebook to the mechanism in Organic chemistry ,6thedition
12. D. Nasipuri.Stereochemistry of Organic Compounds,Principles and Applications, Second
Edition
Chemistry lab.
Semester – I
Unit – I: Physical Chemistry
1) To prepare 0.1 N succinic acid and standardize the NaOH solution of different concentrations.
2) To determine the rate constant for the hydrolysis of ester using HCl as catalyst.
3) To determine enthalp y of dissolution of salt (KNO 3)
4) Determination of viscosity of aqueous solutions of (i) polymer (ii) ethanol and (iii) sugar at
room temperature (Any two solutions).
Unit II: Inorganic Chemistry
1) Commercial analysis of (anytwo)
a) Mineralacid
b) Organicacid
c) Salt of weak acid and strongbase.
2) Titration using double indicator: analysis of solution of Na2CO3andNaHCO3
Page 15
3) Gravimetric analysis
a) To determine the percent purity of sample of BaSO4containingNH4Cl
b) To determine the percent purity of ZnO containingZnCO3.
Unit III Organic Chemistry
1. Purification of organic compounds by recrystallization selecting suitable solvent (minimum 2
organic compounds to be given)
(Learners are expected to report a) Solvent for recrystallization. b) Percentage Yield and the
melting points of the purified compound.)
2. Basic principles of Organic compound characterization (minimum 4 Solid organic
compounds)
(Learners should perform Preliminary Tests, Solubility Test, obtain melting point and
recrystallize the compound with given solvent)
Minimum 80 percent of practical must be completed in each term
Chemistry lab:
Semester - II
Unit – I: Physical Chemistry
1) To determine the amount of strong acid in the given solution by titrating against strong base
conductometrically.
2) To determine the dissociation constant of weak acid (Ka) using Henderson’s equation and the
method of incomplete titration pH metrically.
3) To verify Beer -Lamberts law using KMnO 4 solution by colorimetric method.
4) To standardize commerci al sample of HCl using borax and to write material safety data of the
chemicals involved.
Unit II Inorganic Chemistry
1) Qualitative analysis: ( 5 mixtures to beanalyzed)
Semi -micro inorganic qualitative analysis of a sample containing two cations and
two anions(from amongst):
Cations (from amongst): Pb2+, Ba2+, Ca2+, Sr2+, Cu2+, Cd2+, Fe2+, Ni2+, Mn2+, Mg2+, Al3+, Cr3+,
K+,NH 4+
Anions ( from amongst): CO32-, S2-, SO 2-, NO2-, NO3-, Cl-, Br-, I-, SO42-, PO4
(Scheme of analysis should avoid use of sulphide ion in any form for precipitation/
separation of cations.)
2) Redox Titration: To determine the percentage of copper(II) present in agiven sample by
titration against a standard aqueous solution of sodium thiosulfate (iodometrytitration)
Page 16
Unit III Organic Chemistry
1) Characterization of organic compounds containing C, H, (O), N, S, X elements
(6 solid/liquid Organic compounds)
(Preliminary Tests, Solubility/Miscibility Test, Detection of Elements, Detection of
Functional group and determination of Physical constant)
Minimum 80 percent of practicals must be completed in each term
Reference Books
Unit I :Physical Chemistry
1) Laboratory Experiments in Chemistry I & II, University Practical Book of Chemistry,
University of Mumbai.
2) Athawale, V. D. & Mathur, P. Experimental Physical Chemistry New Age International: New
Delhi (2001).
3) Khosla, B. D.; Garg, V. C. & Gulati, A. Senior Practical Physical Chemistry, R. Chand &
Co.: New Delhi (2011).
4) Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experiments in Physical Chemistry8th Ed.;
McGraw -Hill: New York (2003).
5) Halpern, A. M. &McBane, G. C. Experimental Physical Chemistry3rd Ed.; W.H. Freeman &
Co.: New York (2003).
Unit II: Inorganic Chemistry
1) Laboratory Experiments in Chemistry I & II, University Practical Book of Chemistry,
University of Mumbai.
2) Mendham, J., A. I. Vogel’s Quantitative Chemical Analysis 6thEd., Pearson, 2009.
Unit III: Organic Chemistry
1) Laboratory Experiments in Chemistry I & II, University Practical Book of Chemistry,
University of Mumbai.
2) Mann, F.G. & Saunders, B.C. Practical Organic Chemistry, Pearson Education (2009).
3) Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical Organic Chemistry, 5th
Ed., Pearson (2012).
4) Vogel, A.I., Tatchell, A.R., Furnis, B.S., Hannaford, A.J. & Smith, P.W.G., Textbook of
Practical Organic Chemistry, Prentice -Hall, 5th edition, 1996.