Download Course: Chem-111F - Rajshahi University Alumni Association

Name of Examination
B.Sc (Hons) Part-I
B.Sc (Hons) Part-II
B.Sc (Hons) Part-III
B.Sc (Hons) Part-IV
Examination year
Session
2006
2007
2008
2009
20052006
20062007
20072008
20082009
The B. Sc (Hons) Examination in Chemistry shall consist of the
i)
DEPARTMENT OF CHEMISTRY
FACULTY OF SCIENCE
THE UNIVERSITY OF RAJSHAHI
B.Sc (Hons) Part - I Examination of 750 marks (9.5 units, 38 credits) at the
end of the 1st academic year;
ii) B.Sc (Hons) Part - II Examination of 750 marks (9.5 units, 38 credits) at the
end of the 2nd academic year;
ii) B.Sc (Hons) Part-III Examination of 850 marks (10.5 units, 42 credits) at
the end of the 3rd academic year;
iv) B.Sc (Hons) Part-IV Examination of 850 marks (10.5 units, 42 credits) at
the end of the 4th academic year.
Syllabus for the degree of Bachelor of Science with Honours
[B. Sc (Hons)] in Chemistry
Examination - 2009
For obtaining B. Sc (Hons) degree in Chemistry a student shall have to take
Chemistry courses of 2600 marks, Mathematics courses of 300 marks and
Physics or Applied Physics & Electronics courses of 300 marks, distributed in
four academic years. The Chemistry courses are represented by the prefix
‘Chem-’ followed by a 3 (three) digit number of which the central digit has the
following significance: 0 (general), 1 (Physical), 2 (Organic) and 3 (Inorganic)
Chemistry. The first and the last digits of the course number represent the
Honours year and the sectional course number; A, V and L at the end of the
course number represent the class assessment, the Viva-voce, and for the
laboratory courses, respectively. The letters F or H indicate a full or a half unit
course. The courses of Mathematics, Physics and Applied Physics & Electronics
are represented by the prefix ‘Math-’, ‘PH-’ and ‘APE’ respectively.
DEPARTMENT OF CHEMISTRY
B. Sc (Hons) Part – I Examination, 2006
Session: 20052006
The courses and distribution of marks are as follows:
Courses
Title
Units
Credits Marks
Course Chem-101AH (class assessment) includes tutorial, terminal, home
assignment and /or class examinations on theoretical courses by the relevant
course teacher(s) and attendance* of the students in the classes during the
academic year. Class assessment comprises (a) 80% marks in tutorial, terminal,
home assignment and /or class examinations and (b) 20% marks for attendance
in the class. The class teacher of each course shall submit the average
consolidated marks of class assessments and attendance in sealed envelope to
the Chairman of the relevant examination committee within three weeks from
the last class held. The relevant examination committee shall prepare the result
by taking the average marks of class assessments as submitted by the class
teachers of all the courses, and send a copy of the average consolidated marks to
the controller of examinations.
0.5
1.0
2
4
50
75
Chem-121F
General Chemistry – I
States of Matter, Thermodynamics
and Phase Equilibria
Organic Chemistry – I
1.0
4
75
Chem-131F
Chem-101AH
Inorganic Chemistry – I
Class Assessment-I
1.0
0.5
4
2
75
50
Chem-101VH
Chem-101L
Viva-voce in Chemistry-I
Practical Chemistry –I
0.5
1.0
2
4
50
75
Viva-voce examination (Chem-101VH) includes the assessment of the students
through oral examination (of all the courses) by the members of the relevant
examination committee. The examination committee shall send a copy of the
marks to the controller of examinations.
PH-111F
or
APE-111F
Mechanics, Properties of Matter &
Sound
or
Mechanics, Heats & Optics
Electricity & Magnetism
or
Electricity & Magnetism
Algebra, Trigonometry & Vector
Differential & Integral Calculus
1.0
4
75
* No student having less than 60% class attendance shall be allowed to sit for
the examination.
Chem-101H
Chem-111F
PH-112F
or
APE-112F
Math-112F
Math-115F
Total
11 Courses
1.0
4
75
Course : Chem-101H
General Chemistry - I
Examination - 3 hours
1.0
1.0
4
4
75
75
(Full Marks : 50 (0.5 unit, 2 credit)
50 lectures, two lectures per week, total 25 weeks
9.5
38
750
1.
Chemical calculations (7 Lectures): Units, dimensions and standards; SI
units, conversion of units, uncertainties in measurements, significant
figures and rounding off numbers with some calculations, scientific
notation, plotting of data, slope and intercept of a linear plot. Gram
atomic and gram molecular weights, gram equivalent weight of an acid,
base and salt. Concentration units: normal, molar, and formal solutions,
molality and mole fraction, percentage and ppm, practice exercises of
molar unit.
2.
The gaseous state and the kinetic molecular theory (5 Lectures):
Characteristics of gases, the gas laws, the ideal gas equation, evaluation
of R. Partial pressure, pressure of gases collected over water, the kinetic
theory of gases, different kind of velocity mean free path. Diffusion and
effusion of gases, gas density and molecular weight, heat capacity of
gases and the principle of equipartition of energy.
3.
Chemical equilibrium (5 Lectures): Reversible reactions, law of mass
action, different forms of equilibrium constants, Le-Chatelier’s principle,
effect of pressure, temperature, concentration and addition of inert gas on
the position of equilibrium, some industrial applications of the principle.
Of the four PH and APE courses, students are required to take either two PH or
two APE courses.
Examination of the theory courses of 75 marks (1.0 unit, 4 credit) shall be of 4
(Four) hours duration, of 50 marks (0.5 unit, 2 credit) 3 (three) hours duration
and of the practical course of 75 marks (1.0 unit, 4 credit) shall be of 18
(eighteen) hours duration (3 days). Marks of the practical course (Chem-101LF)
include 25 marks for continuous Lab. assessment. The students are required to
submit a report after each practical class to the class teacher(s) for evaluation.
After evaluation the report shall be returned to the students. The class teacher(s)
shall submit the average marks of all Lab. evaluation in sealed envelopes to the
chairman of the relevant examination committee within three weeks from the
last class held. The examination committee shall send a copy of each of the
consolidated practical and
lab. Evaluation marks
to the controller of
examinations.
4.
Bonding and energy changes (6 Lectures): Covalent bond ( and 
bond), bond length, bond energy, hybridisation of orbitals; sp, sp 2 and sp3
orbitals, heat of reaction, heat of hydrogenation, heat of combustion,
energy changes during a reaction, energy of activation, progress of
reaction, transition state and intermediates.
5.
Detection of elements and functional groups (5 Lectures): Criteria of
purity and calculation of formula of organic compounds, determination of
degree of unsaturation, detection of elements and functional group
analysis of organic compounds and their reactions.
6.
Isomerism (5 Lectures): Classification, optical isomerism due to one/two
chiral centres. Enantiomers, diastereomers and meso compounds, cistrans isomerism and their nomenclature.
7.
Principles of qualitative inorganic analysis (7 Lectures): Solubility and
solubility product, common ion effect and their application in the
precipitation reactions, analytical group classification of metal ions.
Principles and reactions involved in the detection of acid radicals,
interfering radicals and their separation.
8.
Theories of acids and bases (5 Lectures): Arrhenius, protonic, Lewis
and Usanovich concepts of acids and bases, pH and buffer solution,
hydrolysis of salts, indicators.
9.
Chemical hazards (5 Lectures): Hazardous materials, disposal of
hazardous materials with special reference to H2S gas, HCl fume, HNO3
fume, lead, arsenic, benzene and carbon tetrachloride.
Recommended Books:
1. Darrell D. Ebbing
2. H. Anderson
3. D.A. Mc Quarrie & P.A. Rock
4. Paul Ander & A.J. Sonnessa
5. P.W. Atkins
6. R.T. Morison and R.N. Boyd
7. I.L. Finar
8. A. I. Vogel
9. O.D. Tyagi & M. Mehra
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General Chemistry
Chemical Calculations
General Chemistry
General Chemistry
Elements of Physical Chemistry
Organic Chemistry
Organic Chemistry, Vol. 1
Inorganic Qualitative Analysis
A Textbook of Environmental Chemistry
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Course: Chem-111F
States of Matter, Thermodynamics and Phase Equilibria
Examination - 4 hours
Full Marks: 75 (1 unit, 4 credit)
(60 lectures, 3 lectures per week, total 20 weeks)
1.
The gaseous state (real gases) (14 Lectures): Ideal gas equation and its
presure-volume behaviour, pressure-volume behaviour of real gases and
the causes of deviation from the ideal gas equation. van der Waals’
equation and its limitations, other equations of state, virial equation.
Behaviour of gases near liquefaction temperature, critical phenomena,
continuity of state, law of corresponding state and the reduced equation of
states, liquefaction of gases.
2.
The liquid state (16 Lectures): Liquid vs. gases and solids, liquid-vapour
equilibrium, molecular interpretation of vapour pressure. Boiling point,
critical temperature and the heat of vaporization (Trouton’s law), Craft’s
rule, surface tension of liquids and molecular interpretation of surface
free energy, temperature dependence of surface tension and parachor,
determination of surface tension, wetting characteristics of liquids.
Viscosity and viscosity coefficient, flow of liquid through a narrow tube,
measurement of viscosity coefficient, effect of temperature and pressure
on viscosity, molecular interpretation of viscosity and rheochor, factors
affecting the viscosity of a liquid, viscosity of liquid mixtures, refractive
index, optical activity.
3.
Thermodynamics and thermochemistry (20 Lectures): Scope and
limitations of thermodynamics, state, system and surrounding, properties
of thermodynamic functions, IUPAC convention for sign of work and
heat, the first law of thermodynamics, reversible and irreversible
processes, isothermal and adiabatic changes, enthalpy and its temperature
dependence, Joule-Thompson effect. Thermochemistry: Thermochemical
laws and thermochemical calculations, different types of heat of reaction,
Kirchhoff’s equation, bond enthalpy.
4.
The phase equilibria (10 Lectures): Phase, components and degrees of
freedom, conditions of equilibrium in a heterogeneous system, phase rule
and phase diagram. One component system: water, CO 2 and sulphur
systems, enantiotropy and monotropy, phosphorous system.
Recommended Books:
1. Darrell D. Ebbing
2. P.W. Atkins
3. N. Kundu and S.K. Jain
4. Klotz and Rossenberg
5. B.H. Mahan
6. P.W. Atkins
7. K.L. Kapoor
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General Chemistry
Physical Chemistry
Physical Chemistry
Chemical Thermodynamics
Elementary Chemical Thermodynamics
Elements of Physical Chemistry
Physical Chemistry Vol. I
Course : Chem-121F
Organic Chemistry-I
Examination - 4 hours
Full Marks : 75 (1 unit, 4 credit, 60 lectures)
1.
Aliphatic Hydrocarbons:
(i) The alkanes (paraffins) (6 Lectures): Structure, conformation of ethane
and butane, nomenclature, preparations and reactions, photo-chemical
halogenation with mechanism (free radical mechanism).
Recommended Books:
1.
2.
3.
4.
5.
6.
7.
(iv)
The cycloalkanes (alicyclic compounds) (8 Lectures):
Nomenclature, preparations, reactions. Baeyer strain theory; SachseMohr modification, conformation of alicyclic compounds, angle strain,
torsional strain, Vander Waals strain.
2.
Aromatic Hydrocarbons (10 Lectures): Nomenclature, structure of
benzene (Kekule structure, resonance structure, M.O. structure),
aromaticity (Huckel rule), mechanism of electrophilic aromatic
substitution:
halogenation,nitration,
sulphonation,
Friedel-Crafts
alkylation and acylation. Orientation in benzene ring in its derivatives,
activation and deactivation in aromatic di-substitution.
3.
Halides (8 Lectures): Nomenclature, preparation, halide exchange. SN2
and SN1 mechanism; reactions, general SN2 reactions of halides, the
Grignard reagent, quat. ions.
4.
Alcohols and Phenols (10 Lectures): Nomenclature, classification
(1°/2°/3° and mono-di-trihydric), preparations, reactions, association
(hydrogen bonding) of alcohols, test of alcohols, distinction between
different types of alcohol, preparation and reactions of phenols.
5.
Ethers and Epoxides (4 Lectures): Nomenclature, preparation and
reaction. Sulfur analogues of ethers, sulfides, crown ethers, host-guest
interaction.
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Organic Chemistry
Organic Chemistry, Vol. I
Organic Chemistry
A Textbook of Organic Chemistry
Organic chemistry, Vol. I
: A Textbook of Organic Chemistry
: Organic Chemistry
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(ii) The alkenes (olefins) (10 Lectures): Structure, nomenclature,
preparations, reactions, mechanism of addition to double bonds.
Regioselective reactions: E1 & E2 reactions, Markownikoff and antiMarkownikoff addition; the peroxide effect; oxidation and reduction of
olefins.
(iii) The alkynes (acetylenes) (4 Lectures): Structure, nomenclature,
preparations, reactions, and mechanisms, acidity of alkynes.
R. T. Morrison and R.N. Boyd
I.L. Finar
J.D. Roberts and M.C. Casserio
B.S. Bahl and Arun Bahl
S.M. Mukherjee, S.P. Singh &
R.P. Kapoor
Raj K. Bansal
R.J. Fessenden & J.S. Fessenden
Course : Chem-131F
Inorganic Chemistry-I
Examination - 4 hours
Full Marks : 75 (1 unit, 4 credit, 60 lectures)
1.
Atomic Structure (8 Lectures): Fundamental particles, nuclear charge,
atomic spectra, Bohr atomic model, four quantum numbers, distribution of
electrons in atoms, Pauli exclusion principle, Hund’s rule of maximum
multiplicity.
2.
Atomic Spectra (9 Lectures): Spectroscopic levels in multielectronic
system, term multiplicities, Russel-Saunder's coupling, spectra of higher
elements, fine structure of spectral lines.
3.
Basic Quantum Mechanics (9 Lectures): Dual nature of electromagnetic
radiation, black body radiation, photoelectric effect and compton effect,
particle and wave nature of electron; de Broglie relation; Heisenberg
uncertainty principle; preliminary idea about orbitals; physical significance
of s,p and d orbitals.
4.
Chemical Bonding (12 Lectures): Covalent bond; formation of hydrogen
molecule, potential energy diagram and its interpretation; sigma- and pibonds; bond energy, bond length and bond angle; ionic characteristics of
covalent bond; polarity of bonds and electric dipole moments; the concept
of hybridization of bond orbitals. Fundamental ideas of the Molecular
Orbital Theory (MOT); electronic configurations of simple molecules in
terms of MO concept -- such as He2, N2, O2, F2, HF, CO and NO.
5.
Periodic Table (12 Lectures): Periodic law, classification of elements,
modern periodic table in the light of electronic configurations of
elements, different types of elements, periodic properties, atomic,
covalent and ionic radii, ionization potential, electronegativity, electron
affinity, effective nuclear charge.
6.
Oxidation-reduction Reactions (10 Lectures): Combination,
decomposition, displacement and complicated types of reactions,
oxidation number, method of balancing redox reactions, ionic
representation of the equations of redox reaction, redox potential,
electrochemical series and its application in oxidation-reduction
reactions.
Recommended Books:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
F.A. Cotton and G.Wilkinson
J.E. Huheey
: Basic Inorganic Chemistry
: Inorganic Chemistry:
Principles of Structure and
Reactivity
H.V. Anderson
: Chemical Calculations
D.K. Sabera
: Electronic Structure and
Chemical Bonding.
W.L. Jolly
: Principle of Inorganic hemistry
B.R. Puri and L.R. Sharma
: Principles of Inorganic
Chemistry
S.Z. Haider
: Modern Inorganic Chemistry
M.C. Day and J. Selbin
: Theoretical Inorganic
Chemistry
Satya Prakash, Tuli, Basu and Madan : Advanced Inorganic
Chemistry
Manas Chanda
: Atomic Structure and
Chemical Bond
Course : PH-111F
Mechanics, Properties of matter and Sound
Examination - 4 hours
Full Marks: 75 (1 unit, 4 credit, 60 lectures)
(Three lectures per week; total: 20 weeks)
4.
Oscillatory Motions: Hooke’s law and vibration; simple harmonic
motion; combination of harmonic motions; damped harmonic motion;
forced oscillation and resonance.
5.
Gravitation: Center of gravity of extended bodies; gravitational field,
potential and their calculations; escape velocity.
6.
Surface Tension: Surface tension as a molecular phenomenon; surface
tension and surface energy; capillary rise or fall of liquids; pressure on a
curved membrane due to surface tension.
7.
Elasticity: Moduli of elasticity, Poisson’s ratios; relations between elastic
constants and their determination; cantilever.
8.
Fluid Dynamics: Viscosity and coefficient of viscosity, Poiseuille’s
equation; Bernoulli’s theorem and its applications, Torricell’s theorem;
venturimeter.
Recommended Books:
1.
2.
3.
4.
5.
6.
7.
8.
9.
Vector Analysis: Vectors and scalars; addition and multiplication of
vectors; triple scalar and vector products; derivatives of vectors; gradient,
divergence, and curl and their physical significance.
2.
Conservation of Energy and Linear Momentum: Conservative and
non-conservative forces and systems; conservation of energy and
momentum; center of mass.
3
Rotational Motions: Rotational variable; rotation with constant angular
acceleration; relation between linear and angular kinematics; torque on a
particle; angular momentum of a particle; kinetic energy of rotation and
moment of inertia; combined translational and rotational motion of a rigid
body; conservation of angular momentum.
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Mechanics and Properties of Matter
Theoretical Physics (part I)
General Properties of Matter
Physics ( I and II)
General Physics
Elements of Properties of Matter
General Properties of Matter
Vector Analysis
Mechanics
Group B : Sound (Marks : 25)
1.
Wave in Elastic Media: Mechanical waves; types of waves,
superposition principle, wave velocity; power and intensity in wave
motion; interference of waves; complex waves; standing waves and
resonance.
2.
Sound Waves: Audible, ultrasonic, and infrasonic waves; propagation
and speed of longitudinal waves; vibrating systems and sources of sound;
beats; Doppler Effect.
Group A : Mechanics & properties of Matters (Marks: 50)
1.
Ahmed and Nath
Constant
Emran, et al
Halliday and Resnick
Haque
Mathur
Newman and Searle
Spiegel
Symon
Recommended books:
1.
2.
3.
4.
5.
Halliday and Resnick
Emran
Coulson
Saha
Wood
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Physics (I and II)
Textbook of Sound
Waves
Textbook of Sound
Textbook of Sound
Course : PH-112F
Electricity and Magnetism
Examination - 4 hours
Course : Math-112F
(Algebra, Trigonometry & Vector)
Examination - 4 hours
Full Marks : 75 (1 unit, 4 credit, 60 lectures)
(Three lectures per week. Total : 20 weeks)
Full Marks : 75 (1 unit, 4 credit, 60 lectures)
(Three lectures per week; Total : 20 weeks)
1.
Electrostatistics: Electric dipole: electric field due to a dipole, dipole on
external electric field, Gauss’s law and its applications.
1.
2.
Capacitors: Parallel plate capacitors with dielectrics, dielectrics and
Gauss’s law, susceptibility, permittivity and dielectric constant, energy
stored in an electric field.
2.
3.
Electric Current: Electron theory of conductivity, conductor,
semiconductors and insulators, superconductors, current and current
density, Kirchhoff’s law and its applications.
4.
Magnetism: Magnetic dipole, field due to a dipole, mutual potential
energy of two small magnets, magnetic shell, energy in a magnetic field,
magnetometers.
5.
Electromagnetic Induction: Faraday’s experiment, Faraday’s laws,
Ampere’s law, motional e.m.f., self-and mutual inductance,
galvanometers - moving cell ballistic and deadbeat types.
6.
Thermoelectricity: Thermal e.m.f., Seebeck, Peltier and Thomson
effects, laws of addition of thermal e.m.f., thermoelectric power.
7.
DC and AC circuits: DC circuits with LR, RC, LC and LCR in series,
AC circuits with LR, RC, LC and LCR in series.
8.
AC and DC meters: Ammeter, voltmeter, ohmmeter, watt meter,
frequency meter, AC/DC bridge, digital voltmeter.
Recommended Books:
1. Acharyya
2. Admas and Page
3. Constant
4. Din
5. Emran et al.
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6.
7.
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Halliday and Resnick
Kip
Electricity and Magnetism
Principles of Electricity
Theoretical Physics
Electricity and Magnetism
Textbook of Magnetism,
Electricity and Modern Physics
Physics (I & II)
Fundamentals of Electricity and Magnetism
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3.
4.
5.
6.
7.
(a) Algebra of sets: De Morgan’s rule, relation & function.
(b) Determinants: Properties and Cramer’s rule.
Theory of equations: (a) Theorems and relation between roots and
coefficients.
(a) De Moiver’s theorem; (b) Deduction from De Moiver’s theorem.
(a) Functions of complex arguments ; (b) Gregory’s series.
(a) Summation of series.
(b) Hyperbolic functions.
Vector addition, multiplication & differentiation.
Vector differential operator - grad., div. and curl.
Recommended Books:
1.
2.
3.
4.
5.
6.
7.
Barnside and Panton
Bernard and Child
Hall and Knight
Das and Mukherjee
M.A. Sattar
M.R. Spiezel
M.A. Sattar
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Theory of Equations
Higher Algebra
Higher Algebra
Higher Trigonometry
Higher Trigonometry
Vector Analysis
Vector Analysis
Course : Math -115F
Differential & Integral Calculus
Examination - 4 hours
Full Marks : 75 (1 unit, 4 credit, 60 lectures)
(Three lectures per week, Total : 20 weeks)
1.
2.
3.
Functions: Domain, range, inverse function and graphs of functions; limits,
continuity and indeterminate form.
Ordinary differentiation: Differntiability, differentiation, successive
differentiation and Leibnitz theorem.
(a) Expansions of functions: Rolle’s theorem, mean value theorem,
Taylor’s and Maclaurin’s formulae.
(b) Maximum and minimum of functions of one variable.
4.
5.
6.
7.
(a) Partial differentiation: Euler’s theorem, tangents and normals ; (b)
Asymptotes.
Indefinite Integrals: Method of substitution, integration by parts, special
trigonometric functions and rational fractions.
Definite Integrals: Fundamental theorem, general properties, evaluation of
definite integrals and reduction formulae.
Multiple Integrals: Determination of length, areas and volumes.
The total marks for the practical course shall be obtained by adding the above
two marks (i) & (ii). The examination committee shall send a copy of the
consolidated marks to the controller of examinations.
Section A : Physical Chemistry Practical
1.
Recommended books:
1.
2.
3.
4.
5.
6.
7.
Ayres
Das and Mukherjee
Das and Mukherjee
Edwards
Williamson
Muhammad and Bhattacherjee
Muhammad and Bhattacherjee
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Calculus
Differential Calculus
Integral Calculus
Differential Calculus
Integral Calculus
Differential Calculus
Integral Calculus
2.
3.
4.
5.
------------6.
Course : Chem-101L
(Chemistry Practical-I)
Examination - 18 hours (63)
Full Marks : 75 (1 unit, 4 credit)
Section A: Physical Chemistry Practical
Section B: Organic Chemistry Practical
Section C: Inorganic Chemistry Practical
(i) Experiment: 50* (Section : A+B+C), (ii) Continuous Lab. Assessment:
25** (Section : A+B+C)
* The examiners in all the three sections shall assess the experiment(s) out of 50
marks and submit them to the chairman of the relevant examination committee.
Average marks shall be computed by dividing the total marks of three sections
by three.
** The relevant teachers of the three sections shall evaluate continuously the
Lab. classes out of 25 marks and submit the average marks of Lab. evaluation in
sealed envelopes to the Chairman of the relevant examination committee within
three weeks from the last Lab. held. The average marks shall be computed by
the examination committee.
7.
8.
9.
10.
11.
12.
13.
(a) Laboratory procedures, safety regulations, scientific notations, plotting
of data and finding of slope and intercept.
(b) Significant figures, rounding off numbers and practice exercises for the
use of calculator.
Determination of formula and composition of a suitable hydrate. (CuSO 4,
5H2O; NiSO4, 7H2O; CoCl2, 6H2O).
Studies on the (i) stoichiometry of the lead nitrate and potassium chromate
system, (ii) decomposition of the metal halate (KClO3).
Determination of empirical formula of copper sulphide.
Determination of the molecular weight of a suitable (a) monobasic and (b)
dibasic salt of organic acids by chemical method.
Mass and density measurements:
(a) Determination of the density of a solid by (i) dimensional and (ii)
water displacement (Archimedes’ principle) method.
(b) Determination of the density of a liquid / solution by (i) Finagles,
(ii) density bottle / pycnometer method.
(c) Measurement of density of solution at different molar
concentration and determination of the unknown concentration of
a solution.
Calibration of volumetric apparatus, viz. pipette, burette, measuring flask,
etc.
Determination of molar volume of hydrogen gas at S.T.P.
Determination of the molar gas constant R
Determination of the molar masses of hexane and cyclohexane by Dumas
method / Victor Mayers’s method.
Determination of the coefficient of viscosity of a liquid/solution by
Ostwald’s viscometer method.
Measurement of the coefficient of viscosity of Urea solution at different
concentrations and determination of the unknown concentration of a given
solution.
Thermochemistry :
(a) Determination of the heat capacity of a supplied calorimeter and
measurement of the heat of solution of inorganic salts in water
(NaOH / KNO3 in H2O)
(b)
Determination of the heat capacity of a supplied calorimeter and
measurement of the heat of neutralization of an aq. strong acid
with an aq. strong base. (aq. HCl+aq. NaOH)
(c) Determination of the heat capacity of a supplied calorimeter and
measurement of the heat of neutralization of an aq. strong acid
with solid strong base. (HCl aq. + NaOHs) and verification of the
Hess’s law.
(d) Determination of the heat of formation of magnesium oxide.
NB:
A few more experiments, relevant to the theoretical courses may be
done, subject to the availability of the Lab. facilities.
Section B: Organic Chemistry Practical
Systematic identification of organic compounds:
i) Determination of melting point of solid and boiling point of liquid
organic compounds.
ii) Detection of N, S and halogens in organic compounds.
iii) Solubility test and classification of the compound.
iv) Identification of functional groups : primary amine, secondary amine,
substituted amide, nitro, simple amide and imide, carboxylic,
phenolic, carbonyl, aromatic hydrocarbon. etc.; preparation of
derivative, conclusion, naming of the compound / structure of
compound. Identification of the compound under investigation should
be systematic.
Section C: Inorganic Chemistry Practical
Inorganic qualitative analysis (semi-micro/macro method of analysis) :
Systematic qualitative analysis of a mixture of compounds containing not more
than four radicals, of which there shall not be more than three basic radicals and
more than two acid radicals.
i)
Basic radicals: Silver, lead, mercury, bismuth, copper, cadmium, tin,
arsenic, antimony, iron, aluminium, chromium, manganese, zinc,
cobalt, nickel, calcium, barium, strontium, magnesium, potassium,
sodium and ammonium.
ii) Acid radicals: Carbonate, sulphite, sulfide, sulphate, nitrate, nitrite,
chloride, bromide, iodide, phosphate and borate.
Recommended Books:
1. D.P. Shoemaker et al
2. G.S. Weiss et al
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