CHEMISTRY

  • Vision and Mission
  • Course Outcome
  • Laboratory
  • Faculty
  • Syllabus

PROFILE

Vision

  • The vision of the department is to make the students research-oriented and employable and enable them to become confident and competent with better comprehension and applications.

mission

  • Projects are introduced in the V and VI semesters of B.Sc. to motivate students towards research. The syllabus is industry-oriented. Certificate courses, seminars, PowerPoint presentations, discussions, etc. are an integral part of the curriculum to boost the student’s self-confidence.

Course Pattern and Scheme of Examination for I and II Semester SEP (2026)

Title and code of the paper Teaching hours Contact hours/Week Exam. hours IA Marks Total Marks Credits
First Semester

Chemistry-I CHE11T
45
3
3
20
80
100
3
First Semester

Chemistry Practical-I CHE11P
45
3
3
10
40
50
2
Second Semester

Chemistry-I1 CHE21T
45
3
3
20
80
100
3
Second Semester

Chemistry Practical-II CHE21P
45
3
3
10
40
50
2

PEOs, POs & PSOs

Program Education Objectives Program Outcomes Program Specific Outcomes
  • PEO 1 – Academic Excellence &  Application-Graduates will acquire comprehensive knowledge in Chemistry, Zoology, and Biotechnology and apply scientific principles to solve real-world problems in life sciences.

  • PEO 2 – Research, Innovation & Problem-Solving-Graduates will design and conduct experiments using chemical, biological, and molecular techniques to address interdisciplinary challenges.

  • PEO 3 – Lifelong Learning &  Professional Growth-Graduates will adapt to advancements in life sciences, chemical sciences and related industries through continuous learning and skill development.

  • PEO 4 – Ethics, Environment &  Social Responsibility-Graduates will practice professional ethics, environmental stewardship, and contribute to biodiversity conservation and societal well-being.
  • PO1 – Disciplinary Knowledge-Demonstrate comprehensive knowledge of concepts, theories, and experimental methods in Chemistry, Zoology, and Biotechnology.

  • PO2 – Critical Thinking & Problem Solving-Apply logical reasoning and evidence-based approaches to analyze complex scientific problems and develop viable solutions.

  • PO3 – Research-Related Skills-Design, conduct, and interpret experiments using appropriate tools and techniques, adhering to scientific methodology.

  • PO4 – Communication Skills-Present scientific ideas, findings, and arguments effectively through oral, written, and digital platforms for diverse audiences.

  • PO5 – Analytical & Quantitative Reasoning-Interpret data using quantitative methods, statistical tools, and scientific analysis for informed decision-making.

  • PO6 – Environment & Sustainability-Evaluate the impact of scientific activities on the environment and advocate for sustainable practices and biodiversity conservation.

  • PO7 – Ethics & Professional Integrity-Demonstrate ethical responsibility, integrity, and accountability in academic, research, and professional settings.

  • PO8 – Digital Literacy-Use modern tools, digital platforms, and information technology effectively for data analysis, research, and lifelong learning.

  • PO9 – Self-Directed Learning-Recognize learning needs, set goals, and acquire new knowledge and skills independently to keep pace with scientific and technological advancements

  • PO10 – Leadership & Teamwork-Work effectively as an individual and as a member or leader in multidisciplinary teams to achieve common goals.
  • PSO 1- Apply fundamental principles and techniques in organic, inorganic and physical chemistry.

  • PSO 2- Develop experimental skills for handling chemicals, instruments, and applying safety and good laboratory practices.

  • PSO 3- Develop research-oriented skills like ability to conduct research projects, critically analyse and interpret experimental data, utilize modern techniques to effectively communicate research findings.

  • PSO 4- Interpret mechanisms, stereochemistry, and synthetic routes for organic and inorganic molecules using modern analytical, spectroscopic, and retrosynthetic approaches.

COURSE OUTCOME

Course Pattern and Scheme of Examination for I and II Semester SEP (2026)

Title and code of the paper Teaching hours Contact hours/Week Exam. hours IA Marks Total Marks Credits
First Semester

Chemistry-I CHE11T
45
3
3
20
80
100
3
First Semester

Chemistry Practical-I CHE11P
45
3
3
10
40
50
2
Second Semester

Chemistry-I1 CHE21T
45
3
3
20
80
100
3
Second Semester

Chemistry Practical-II CHE21P
45
3
3
10
40
50
2

PEOs, POs & PSOs

Program Education Objectives Program Outcomes Program Specific Outcomes
  • PEO 1 – Academic Excellence & Application-Graduates will acquire comprehensive
    knowledge in Chemistry, Zoology, and Biotechnology and apply scientific principles to solve
    real-world problems in life sciences.
  • PO1 – Disciplinary Knowledge-Demonstrate comprehensive knowledge of concepts,
    theories, and experimental methods in Chemistry, Zoology, and Biotechnology.
  • PSO 1- Apply fundamental principles and techniques in organic, inorganic and physical
    chemistry.
  • PEO 2 – Research, Innovation & Problem-Solving-Graduates will design and conduct
    experiments using chemical, biological, and molecular techniques to address interdisciplinary
    challenges.
  • PO2 – Critical Thinking & Problem Solving-Apply logical reasoning and evidence-based
    approaches to analyze complex scientific problems and develop viable solutions.
  • PSO 2- Develop experimental skills for handling chemicals, instruments, and applying
    safety and good laboratory practices.
  • PEO 3 – Lifelong Learning & Professional Growth-Graduates will adapt to advancements in
    life sciences, chemical sciences and related industries through continuous learning and skill
    development.
  • PO3 – Research-Related Skills-Design, conduct, and interpret experiments using
    appropriate tools and techniques, adhering to scientific methodology.
  • PSO 3- Develop research-oriented skills like ability to conduct research projects, critically
    analyse and interpret experimental data, utilize modern techniques to effectively
    communicate research findings.
  • PEO 4 – Ethics, Environment & Social Responsibility-Graduates will practice professional
    ethics, environmental stewardship, and contribute to biodiversity conservation and societal
    well-being.
  • PO4 – Communication Skills-Present scientific ideas, findings, and arguments effectively
    through oral, written, and digital platforms for diverse audiences.
  • PSO 4- Interpret mechanisms, stereochemistry, and synthetic routes for organic and
    inorganic molecules using modern analytical, spectroscopic, and retrosynthetic approaches.
  • PO4 – Communication Skills-Present scientific ideas, findings, and arguments effectively through oral, written, and digital platforms for diverse audiences.
  • PO5 – Analytical & Quantitative Reasoning-Interpret data using quantitative methods, statistical tools, and scientific analysis for informed decision-making.
  • PO6 – Environment & Sustainability-Evaluate the impact of scientific activities on the environment and advocate for sustainable practices and biodiversity conservation.
  • PO7 – Ethics & Professional Integrity-Demonstrate ethical responsibility, integrity, and
    accountability in academic, research, and professional settings.
  • PO8 – Digital Literacy-Use modern tools, digital platforms, and information technology
    effectively for data analysis, research, and lifelong learning.
  • PO9 – Self-Directed Learning-Recognize learning needs, set goals, and acquire new
    knowledge and skills independently to keep pace with scientific and technological
    advancements
  • PO10 – Leadership & Teamwork-Work effectively as an individual and as a member or leader in multidisciplinary teams to achieve common goals.

Program Duration:

The B.Sc. Programme with Chemistry is of three years duration. Each year is called an
academic year and is divided into two semesters. Thus, there will be a total of six semesters.

Assessment: Weightage for assessments (in percentage)

Type of Course Formative Assessment/IA Summative Assessment Marks/ESE
Theory
20
10
Practical
10
40

The curriculum will be delivered through various methods including chalk and talk,
power point presentations, audio, video tools, E-learning/E-content, virtual labs,
simulations, field trips/Industry visits, seminars (talks by experts), workshops, projects,
models and class discussions. The assessment broadly will comprise of Internal
Assessment (Continuous Evaluation) and End Semester Examination (ESE)

Scheme of Internal Assessment Marks: Theory

Sl no. Particulars IA Marks
1
Other IA
10
2
Mid Term Examination
10
Total Theory IA marks
20

Scheme of Internal Assessment Marks: Practical

Sl no. Particulars IA Marks
1
Other IA
5
2
Practical Test (Preparatory)
5
Total Practical IA marks
10

Scheme of Evaluation for Practical Examination

Sl no. Examination particulars Marks allotted
1
Experimental performance
25
2
Procedure writing
5
3
Record assessment
5
3
Viva-voce
5
Total
40

Scheme for Summative Assessment : Theory Question paper pattern

Sl no. Question Paper Pattern Marks
1
Part A (10 out of 12 questions to be answered of, 2M each)
10 x 2 = 20
2
Part B (5 out of 7 questions to be answered of, 4M each)
5 x 4 = 20
3
Part C (5 out of 7 questions to be answered of, 8M each) (5+3) pattern
5 x 8= 40
Total
40

SEMESTER I

Chemistry-I: CHE11T

Title of the paper Chemistry-I (Theory) CHE11T
Total Contact hours/Sem
45 hours
Teaching Hours
3 hrs/Week
Internal Assessment marks
20
Summative Assessment Marks
80
No. of Credits
03

Objectives:

The objective of this course is to make the students aware of the SI Units, various analytical methods, types of errors in chemical analysis. It discusses the Periodicity in properties with reference to the s and p block, which is necessary in understanding their group chemistry, noble gases. The course is also infused with fundamentals of organic chemistry. To establish the applications on the concepts like alkanes, alkenes, alkynes and aromatic hydrocarbons are introduced. It emphasizes the concept of gases, liquids and solutions.

Course Outcomes:

By the end of the course, the students will be able to Understand the:

  • CO1: Apply principles of analytical chemistry and gaseous state to solve numerical and theoretical problems involving errors, statistical data treatment, titrimetric analysis, gas laws, critical constants, and liquefaction of gases.
  • CO2: Analyze periodic properties, noble gas chemistry, and compounds of nonmetals by explaining trends in the periodic table, comparing group properties, and describing preparation, structure, bonding, and applications of important inorganic compounds.
  • CO3: Demonstrate understanding of aliphatic hydrocarbons by explaining preparation methods, stereochemistry, conformations, mechanisms, and reactions of alkanes, cycloalkanes, alkenes, dienes, and alkynes.

Course Articulation Matrix:

Mapping of course outcome (COs) with PO and PSO

COs PO1 PO2 PO3 PO4 PO5 PO6 PO7 PO8 PO9 PO10 PSO1 PSO2 PSO3 PSO4
CO1
3
2
2
1
3
1
1
2
3
2
3
CO2
3
2
2
1
2
3
CO3
3
2
1
1
2
1
1
2
3
3
COs PO1 PO2 PO3 PO4 PO5 PO6 PO7 PO8 PO9 PO10 PSO1 PSO2 PSO3 PSO4
CO1 3 2 2 1 3 1 1 2 3 2 3
CO2 3 2 2 1 2 3
CO3 3 2 1 1 2 1 1 2 3 3

SEMESTER I

Chemistry-I: CHE11T

Contact Hours: 45

Teaching Hours: 3 Hours/Week

Course Outline

Unit I:
Analytical Chemistry (7 Hours)

Choice of analytical methods: accuracy, precision, sensitivity, selectivity. Errors: Determinate and determine errors, absolute error, relative error, minimization of errors. Statistical treatment of finite samples -mean, median, range, standard deviation and variance. Titrimetric analysis: Theory of acid-base indicators Ex: Phenolphthalein, methyl red. Titration curves for strong acid vs strong base, weak acid vs strong base and weak base vs strong acid titrations – titration curves. Quantitative applications – selecting and standardizing a titrant. Redox titrimetry: titration curves, Theory of redox indicators, Applications.

Gaseous state (8 Hours)

Introduction: Maxwell-Boltzmann distribution law. Explanation of velocity distribution curves based on this law (no derivation). Mean free path, collision frequency and collision number. Definition and expressions using SI units (no derivations). Derivation of expression for most probable speed from Maxwell-Boltzmann equation. Definitions and expressions for RMS velocity, average velocity and relationships between them. Numerical problems. Andrew’s isotherm on carbon dioxide and explanation of the curves (no experimental details). Derivation of critical constants Tc, Pc and Vc from vander Waal’s equation and their experimental determination by Cagniard de La Tour method for Tcand Pc. Amagat’s mean density method for Vc. Problems on the calculation of Tc, Pc and Vc, a and b. Law of corresponding states-statements, reduced equation of state and explanation, Joule- Thomson effect-explanation. Joule-Thomson co-efficient, inversion temperature-definition (no derivation). The application of Joule-Thomson effect to the liquefaction of air and hydrogen by Linde’s process.

Unit II:
Periodic Properties: (6 Hours)

Atomic and ionic radii, ionization energy, electron affinity and electronegativity- trends in the periodic table and application in predicting and explaining chemical behavior. Comparative studies of groups 1, 2, 16 and 17 with respect to electronic configuration, atomic and ionic radii, and ionization energy and electro negativity. Comparative study of compounds-halides, oxides and carbonates of groups 1 and 2: hydrides of groups 16 and 17. Diagonal relationship between Li and Mg.

Noble gases: (5 Hours)

Introduction to noble gases, general characteristics including occurrence and applications.
Preparation, properties, structures and nature of bonding of fluorides & oxides of Xenon (XeF2,
XeF4, XeF6, XeO3, XeO4).

Compounds of nonmetals: (4 Hours)

Synthesis, structure and applications of compounds of the following elements;

  • Boron-boranes (classification), diborane, borazole.
  •  Nitrogen-Hydrazine, hydroxylamine.
  • Sulphur-thionyl chloride.

Unit III:
Aliphatic Hydrocarbons: (15 Hours)

Alkanes (4 Hours): Preparation of symmetrical and unsymmetrical alkanes, Corey-House synthesis, Wurtz reaction and Wurtz-Fittig reaction- their merits and demerits. Difference between conformation and configuration. Conformations of ethane and butane, explanation of stability based on energy profile diagrams. Conformation and stability of 1,2- dichloroethane.

Cycloalkanes (4 Hours): Nomenclature. Method of formation, Baeyer’s strain theory and its limitation, Sachse – Mohr theory of strain-less rings; cyclopropane ring – banana bonds. Conformations of cyclohexane and stability. Geometrical isomerism with examples, cis and trans isomerism in 1,2- dimethyl cyclohexane.

Alkenes (3 Hours): Preparation of alkenes by Wittig reaction. Addition of HX to unsymmetrical alkene – Markownikov’s rule and Antimarkownikov’s rule with mechanism.
Reactions: Hydroboration- oxidation, reduction, oxymercuration- demercuration, epoxidation, Ozonolysis, oxidation with KMnO4 and OsO4.

Diens (2 Hours): Classification- isolated, conjugated, cumulated. Structure of allene and butadiene.1,2 addition and 1,4 addition reactions. Diels Alder reaction-1,3-butadiene with maleic anhydride.

Alkynes (2 Hours): Preparation- Acetylene from CaC 2 dehydrohalogenation of vicinal-dihalides. Reactions: alkylation of terminal alkynes and conversion to higher alkynes, ozonolysis and oxidation with alkaline hot. KMnO4.

Reference books:

  1. Analytical Chemistry: Basic Concepts, Priti Malhotra, Ane Books Pv tLtd,2021.
  2. Advanced Inorganic Chemistry,6 th Edition, F.A.Cotton, G.Wilkinson, C.A.Murillo and M.Bochmann-JohnWiley&Sons,1999.
  3. Inorganic Chemistry, ELBS 2 nd Edition, D. F. Shriver, P. W. Atkins and C. H. Langford, Oxford Univ. Press 2002.
  4. Organic Chemistry, Morrison,R.T.& Boyd, R.N.Pearson, 2010.
  5. Physical Chemistry, Castellan, G.W.4 th Ed.Narosa,2004.
  6. Advanced Organic Chemistry, Bahl, A.& Bahl,B .S,S.Chand,2010.
  7. Organic Chemistry, Graham Solomon, T.W., Fryhle,C.B.& Dnyder,S.A.JohnWiley& Sons, 2014.
  8. Inorganic Chemistry,4 th Edition,J.E.Huhee,E.A.Keiter and R.I.Keiter,Pearson Education Asia, 2000
  9. Analytical Chemistry,Gary D.Christian,6 th Edition,Wiley,2007
  10. Physical Chemistry,Barrow,G.M.Tata McGraw‐Hill,2007.

SEMESTER I

Chemistry Practical I: CHE11P

Title of the paper Chemistry-I
(Practical) CHE11P
Duration of the Examination
03 hours
Teaching Hours
3 hrs/Week
Internal Assessment marks
10
Summative Assessment Marks
40
No. of Credits
02

Course Learning Outcomes:

By the end of the course, the students will be able to Understand the:

  • CO1: Demonstrate proficiency in basic laboratory techniques, including preparation of solutions, titration, filtration, and crystallization.
  • CO2: Demonstrate the ability to prepare standard solutions and perform titrimetric estimations involving redox, acid-base, and precipitation reactions.
  • CO3: Apply standard analytical procedures to determine the composition of industrial and natural samples such as ores, bleaching powder, and detergents.
  • CO4: Maintain proper laboratory records, analyse experimental data, and present results effectively.
  • CO5: Analyze and interpret experimental data quantitatively, calculate concentrations, and determine the percentage purity of chemical substances.

Course Articulation Matrix:

Mapping of course outcomes (COs) with programme outcomes

COs PO1 PO2 PO3 PO4 PO5 PO6 PO7 PO8 PO9 PO10 PSO1 PSO2 PSO3 PSO4
CO1
3
3
1
1
1
2
2
1
1
2
CO2
3
3
2
2
3
1
2
3
2
1
1
CO3
3
3
1
2
1
1
1
1
3
1
2
CO4
3
3
2
2
2
1
2
1
1
2
CO5
3
2
3
3
2
1
3
2
2
COs PO1 PO2 PO3 PO4 PO5 PO6 PO7 PO8 PO9 PO10 PSO1 PSO2 PSO3 PSO4
CO1 3 3 1 1 1 2 2 1 1 2
CO2 3 3 2 2 3 1 2 3 2 1 1
CO3 3 3 1 2 1 1 1 1 3 1 2
CO4 3 3 2 2 2 1 2 1 1 2
CO5 3 2 3 3 2 1 3 2 2
 

List of experiments to be conducted

  1. Calibration of glasswares: pipette, burette and volumetric flask and preparation of solutions.
  2. Estimation of potassium permanganate using standard sodium oxalate solution.
  3. Determination of percentage of manganese dioxide from pyrolusite ore.
  4. Estimation of ferrous ammonium sulphate using standard potassium dichromate solution using internal indicator.
  5. Estimation of ferrous ammonium sulphate using standard potassium dichromate solution using external indicator.
  6. Estimation of sodium thiosulphate using standard potassium dichromate solution.
  7. Determination of the percentage of available chlorine in the given sample of commercial bleaching powder.
  8. Estimation of the amount of alkali present in soaps/detergents.
  9. Estimation of nitrogen in an ammonium salt using sodium hydroxide solution and standard oxalic acid.
  10. Estimation of the amount of carbonate and bicarbonate in the given mixture.
  11. Estimation of chloride by Mohr’s method.

SEMESTER II

Chemistry-II: CHE21T

Title of the paper Chemistry-II (Theory)
CHE21T
Total Contact hours/ Sem
45 hours
Teaching Hours
3 hrs/Week
Internal Assessment marks
20
Summative Assessment Marks
80
No. of Credits
3

Objectives:

The course reviews the structure of the atom, which is a necessary pre-requisite in understanding the nature of chemical bonding in compounds. It provides basic knowledge about ionic, covalent and metallic bonding. To establish applications of aromatic hydrocarbons, alkyl and aryl halides. Solve the conceptual questions using the knowledge gained by studying the quantum mechanical model of the atom, quantum numbers, radial and angular distribution curves, shapes of s, p, and d orbitals. The constitution of the course strongly focuses on the colligative properties of the solutions. It helps in understanding the photophysical and photochemical processes. This course helps the students to relate the structure of an organic compound to its physical and chemical properties.

Course Outcomes:

By the end of the course, the students will be able to Understand the:

  • CO1: Understand the concepts of ionic, covalent, weak, and metallic bonding, including molecular structure, bonding theories, and intermolecular interactions.
  • CO2: Explain the structure, aromaticity, preparation, and reaction mechanisms of aromatic hydrocarbons and organic halogen compounds.
  • CO3: Apply the principles of quantum mechanics and photochemistry to analyze atomic structure, energy transitions, and photochemical processes.

Course Articulation Matrix:

Mapping of course outcomes (COs) with programme outcomes

COs PO1 PO2 PO3 PO4 PO5 PO6 PO7 PO8 PO9 PO10 PSO1 PSO2 PSO3 PSO4
CO1
3
2
1
1
3
1
1
1
1
3
1
1
1
CO2
3
3
2
1
2
1
1
1
1
3
2
1
3
CO3
3
3
1
1
3
2
2
3
1
COs PO1 PO2 PO3 PO4 PO5 PO6 PO7 PO8 PO9 PO10 PSO1 PSO2 PSO3 PSO4
CO1 3 2 1 1 3 1 1 1 1 3 1 1 1
CO2 3 3 2 1 2 1 1 1 1 3 2 1 3
CO3 3 3 1 1 3 2 2 3 1
 

SEMESTER I

Chemistry-II: CHE21T

Contact Hours: 45

Credit Points: 3

Teaching Hours: 3 Hours/Week

Course Outline

Unit I:
Chemical Bonding: (15 Hours)

Ionic bond: Lattice energy, Born-Haber cycle, Born-Lande equation (No derivation), problems on it. Calculation of lattice energies of NaCl and MgO, effect of lattice energy on solubility of ionic compounds.

Covalent bond: hybridization and directional characteristics of sp, sp 2 , sp 3 , sp 3 d, sp 3 d 2 . Shapes of BeCl 2 , BF 3 ,SiCl 4 , PCl 5 and SF 6 .
Polarization concept, Fajan’s rule, polarity and polarizability of ions.
VSEPR theory: Shapes of NH 3 , H 2 O, BrF 3 and ICl 2 –
Molecular orbital theory: H 2 ,He 2 + ,Be 2 ,N 2 ,O 2 , CO and NO (bond order, stability and magnetic properties to be discussed). Bond length, bond angle and bond energy.
Weak interactions: i) Hydrogen bonding: Intramolecular and Intermolecular types, anomalous properties of HF, H 2 O, NH 3 ,alcohols, carboxylic acids, nitrophenols and biomolecules. ii) van der Waals forces: Dipole-dipole, dipole- induced dipole interactions and temporarily dipole- induced dipole interactions.

Metallic bond: Band theory, electrical properties of metals, semiconductors and insulators.

Unit II:
Aromatic hydrocarbons (9 Hours):

Structure of benzene using molecular orbital theory. Huckel’s aromaticity rule with respect to benzenoids (ex: Benzene, naphthalene, anthracene & phenanthrene) and non-benzenoids (Ex: cyclopentadienyl anion and cycloheptadienyl cation), Antiaromaticity. Aromatic electrophilic substitution-mechanisms of halogenation, nitration, sulphonation, & Friedel-Craft’s reactions; orienting influence of substituents in toluene, chlorobenzene, nitrobenzene & phenol. Hyper conjugation & resonance effects of these groups. Hydrogenation of aromatic compounds- Birch reduction, side chain oxidation of toluene to benzaldehyde and benzoic acid, oxidation of naphthalene, anthracene & phenanthrene.

Organic halogen compounds (6 Hours):

Alkyl halides: Methods of preparation-halogenation of alkanes.
Nucleophilic substitution reactions – SN1 and SN2 mechanisms with energy profile diagram; Effect of nature of alkyl groups, nature of leaving groups, nucleophiles and solvents on SN1 and SN2 mechanisms.
Elimination reactions – E1 and E2 mechanisms, Saytzeff and Hofmann Eliminations.
Aryl halides: Preparation by halogenations, Sandmeyer reaction. Relative reactivity of alkyl, allyl, vinyl and aryl halides towards substitution.

Unit III:
Quantum Mechanics: (7 Hours)

Derivation of expressions for radius, energy and ionization energies of hydrogen like atoms. Numerical Problems. Limitations of classical mechanics. Wave particle duality, Uncertainty principle. Hamiltonian operator, eigen values and eigen functions,

Schrödinger wave equation for particle in a one-dimensional box, particle in a 3- dimensional box and concept of degeneracy. Schrödinger wave equation for H-atom & its separation into three equations (no derivation), significance of ψ and ψ 2

Postulates of quantum mechanics. quantum numbers, radial & angular wave functions & probability distribution curves, shapes of s, p & d orbitals, Pauli’s exclusion principle, Hund’s multiplicity rule, Aufbau principle,

Photochemistry: (8 Hours): Introduction to photochemical reactions, Laws of photochemistry-Grotthus-Draper law, Stark- Einstein law. Differences between photophysical and photochemical processes with examples. Comparison of photochemical and thermal reactions. Quantum yield of photochemical combination of (i)H2 and Cl2 (ii)H2 and Br2 (iii) dissociation of HI (iv) dimerization of anthracene. Reasons for the high and low quantum yield. Problems based on quantum efficiency. Photosensitization and photo stationary equilibrium. Singlet and triplet states. Fluorescence, phosphorescence, luminescence, bioluminescence and chemical sensors. Jablonski diagram. Explanation of internal conversion, inter-system crossing Beer-Lambert’s law and its applications. Numerical problems on absorption coefficient and molar extinction coefficient.

Reference Books:

  1. Concise Inorganic Chemistry,5 th Edition, J.D.Lee, Blackwell Science,2001.
  2. Principles of Inorganic Chemistry, B. R. Puri and L. R. Sharma, Jauhar S. P-S. N. Chand & Co., 1998.
  3. Basic Inorganic Chemistry,3 rd Edition, F.A.Cotton, G.Wilkinson , P.L.Gaus-John Wiley & Sons, 1995.
  4. Fundamentals of Organic Chemistry, McMurry, J.E.,7 th Edition, Cengage Learning India Edition, 2013.
  5. Text Book of Physical Chemistry, K.L.Kapoor, McGraw Hill Education Private Limited, 2022.
  6. Introduction to Quantum Theory and Atomic Structure, P.A.Cox, Oxford Chemistry Primers, 1996.
  7. Text Book of Physical Chemistry, Soni P.L.,Dharmarha OP,Dash UN,Sultan Chand & Sons, 2023.
  8. Organic Chemistry, Finar, I.L.Vol.1,6thEdition, Pearson,2002.
  9. Physical Chemistry, Puri, Sharma, Pathania,48thEdition

SEMESTER II

Chemistry Practical II: CHE21P

Title of the paper Chemistry-II (Practical)
Duration of the Examination
03 hours
Teaching Hours
3 hrs/Week
Internal Assessment marks
10
Summative Assessment Marks
40
No. of Credits
2

Course Learning Outcomes:

By the end of the course, the students will be able to Understand the:

  • CO1: Develop laboratory skills in handling physical chemistry instruments and techniques such as viscometry, stalagmometry, colorimetry, and thermometric measurements.
  • CO2: Apply experimental methods to determine physical properties including density, viscosity, surface tension, molar mass, transition temperature, distribution coefficient, and critical solution temperature.
  • CO3: Analyze experimental data to evaluate molecular behavior, reaction kinetics, electrolyte dissociation, and physicochemical properties of solutions and mixtures.

Course Articulation Matrix:

Mapping of course outcomes (COs) with programme outcomes

COs PO1 PO2 PO3 PO4 PO5 PO6 PO7 PO8 PO9 PO10 PSO1 PSO2 PSO3 PSO4
CO1
3
3
3
3
2
2
3
3
CO2
3
3
3
2
3
2
2
3
3
2
CO3
3
3
3
2
3
2
2
2
3
3

COsPO1PO2PO3PO4PO5PO6PO7PO8PO9PO10PSO1PSO2PSO3PSO4
CO1333 3 2 2 33  
CO233323 22  332 
CO333323  2223 3 

 

List of experiments to be conducted

  1. Determination of the density using specific gravity bottle and viscosity of a liquid using Ostwald’s viscometer.
  2. Determination of the density using specific gravity bottle and surface tension of a liquid using Stalagmometer.
  3. Determination of molar mass of an non -electrolyte by Walker-Lumsden method.
  4. Determination of percentage composition of a binary mixture by viscosity method
  5. Determination of molar mass of polymer by viscosity method.
  6. Determination of transition temperature of a salt hydrate by thermometric method.
  7. Determination of degree of dissociation of electrolyte by Walker-Lumsden method.
  8. Determination of critical solution temperature of phenol water system.
  9. Determination of distribution coefficient of benzoic acid between water and toluene.
  10. Study of kinetics of their action between KI and K2S2O8 by colorimetric method.

LABORATORY

FACULTY

Mrs. Shilpa P

Assistant Professor

M.Sc., M.Phil
Shilpap.nmkrv@rvei.edu.in

Mrs. Suparna K

Assistant Professor

MSc NET
suparnak.nmkrv@rvei.edu.in

Dr. Santhosh A S

Assistant Professor

M.Sc., B.Ed., Ph.D.
santhoshas.nmkrv@rvei.edu.in

Dr. Shruthi C D

Assistant Professor

M.Sc., Ph.D.
shruthicd.nmkrv@rvei.edu.in

Dr. Shridevi Salagare

Assistant Professor

M.Sc., B.Ed., Ph.D.

Ms Savitha N

Assistant Professor