e learning resources for Semester I BSc Chemistry Core and Chemistry General Elective Courses

Dear Students,

                  Welcome to the Department of Chemistry,A.S.College, Deoghar with courses in Chemistry Core and Chemistry General Elective.Our country is fast progressing with NATIONAL MISSION ON EDUCATION THROUGH ICT in providing online e learning platforms like SWAYAM ,Swayam Prabha,e PG and NPTEL  offering MOOCs courses.Now, onwards 24x7 learning is possible at one's ease anywhere and anytime .With special thanks  to  our visionaries and Ministry of Human Resources ,Government of India, I invite you all to participate, learn ,skill ,employ and serve our motherland .Following is the brief introduction of Swayam Prabha Channels. 

The SWAYAM PRABHA is a group of 32 DTH channels devoted to telecasting of high-quality educational programmes on 24X7 basis using the GSAT-15 satellite. Every day, there will be new content for at least (4) hours which would be repeated 5 more times in a day, allowing the students to choose the time of their convenience. The channels are uplinked from BISAG, Gandhinagar. The contents are provided by NPTEL, IITs, UGC, CEC, IGNOU, NCERT and NIOS. The INFLIBNET Centre maintains the web portal.

CORE COURSE (HONOURS IN CHEMISTRY)

Semester I

Paper:101- INORGANIC CHEMISTRY-I

Atomic Structure:

Bohr’s theory, its limitations and atomic spectrum of hydrogen atom. Wave mechanics: de Broglie equation, Heisenberg’s Uncertainty Principle and its significance, Schrödinger’s wave equation, significance of ψ and ψ2.

Quantum numbers and their significance. Normalized and orthogonal wave functions. Sign of wave functions. Radial and angular wave functions for hydrogen atom. Radial and angular distribution curves. Shapes of s, p, d and f orbitals. Contour boundary and probability diagrams. Pauli’s Exclusion Principle, Hund’s rule of maximum multiplicity, aufbau’s principle and its limitations, Variation of orbital energy with atomic number.

(14 Lectures)

Please click below for Revision Lectures and Resources on Structure of Atom on Swayam Prabha by MHRD,Government of India .

1. STRUCTURE OF THE ATOM 1
2. STRUCTURE OF THE ATOM 2
3. STRUCTURE OF THE ATOM 3
4. STRUCTURE OF THE ATOM 4
5. STRUCTURE OF THE ATOM 5
6. STRUCTURE OF THE ATOM 6
7. STRUCTURE OF THE ATOM 7

PLEASE CLICK BELOW e-Resources and links ON ATOMIC STRUCTURE:

1. Atomic structure-1
2. Atomic structure-2
3. Atomic structure-3
4. Atomic structure-4

Periodicity of Elements:

s, p, d, f block elements, the long form of periodic table. Detailed discussion of the following properties of the elements, with reference to s & p-block.

(a) Effective nuclear charge, shielding or screening effect, Slater rules,

variation of effective nuclear charge in periodic table.

(b) Atomic radii (van der Waals)

(c) Ionic and crystal radii.

(d) Covalent radii (octahedral and tetrahedral)

(e) Ionization enthalpy, Successive ionization enthalpies and factors

affecting ionization energy. Applications of ionization enthalpy.

 (f) Electron gain enthalpy, trends of electron gain enthalpy.

(g) Electronegativity, Pauling’s/ Mulliken’s/ Allred Rachow’s/ and

Mulliken-Jaffé’s electronegativity scales. Variation of electronegativity with bond order, partial charge, hybridization, group electronegativity. Sanderson’s electron density ratio. (16 Lectures)

PLEASE CLICK BELOW e-Resources and links ON PERIODIC PROPERTIES:

1. Periodic properties-1
2. Periodic properties-2
3. Periodic properties-3
4. Periodic properties-4
5. Periodic properties-5

Chemical Bonding:

(i) lonic bond: General characteristics, types of ions, size effects, radius ratio rule and its limitations. Packing of ions in crystals. Born-Landé equation with derivation and importance of Kapustinskii expression for lattice energy. Madelung constant, Born-Haber cycle and its application, Solvation energy.

(ii) Covalent bond: Lewis structure, Valence Bond theory (Heitler- London approach). Energetics of hybridization, equivalent and non-equivalent hybrid orbitals. Bent’s rule, Resonance and resonance energy, Molecular orbital theory. Molecular orbital diagrams of diatomic and simple polyatomic molecules N2, O2, C2, B2, F2, CO, NO, and their ions; HCl,BeF2, CO2, (idea of s-p mixing and orbital interaction to be given). Formal charge, Valence shell electron pair repulsion theory (VSEPR), shapes of simple molecules and ions containing lone pairs and σ bond and π bond electrons, and bond multiple bonding (bond lengths). Covalent character in ionic compounds, polarizing power and polarizability. Fajan’s rules and consequences of polarization. Ionic character in covalent compounds: Bond moment and dipole moment. Percentage ionic character from dipole moment and electronegativity difference.

(iii) Weak Chemical Forces: van der Waals forces, ion-dipole forces, dipole-dipole interactions, induced dipole interactions, Instantaneous dipole-induced dipole interactions. Repulsive forces, Hydrogen bonding (theories of hydrogen bonding, valence bond treatment) Effects of chemical force, melting and boiling points, solubility energetics of dissolution process. Principles involved in volumetric analysis to be carried out in class. (30 Lectures)

Please click below for Revision Lectures and Resources on Chemical Bonding on Swayam Prabha by MHRD,Government of India .

1. CHEMICAL BONDING & MOLECULAR STRUCTURE 1
2. CHEMICAL BONDING & MOLECULAR STRUCTURE 2
3. CHEMICAL BONDING & MOLECULAR STRUCTURE 3
4. CHEMICAL BONDING & MOLECULAR STRUCTURE 4
5. CHEMICAL BONDING & MOLECULAR STRUCTURE 5
6. CHEMICAL BONDING & MOLECULAR STRUCTURE 6
7. CHEMICAL BONDING & MOLECULAR STRUCTURE 7

PLEASE CLICK BELOW e-Resources and links ON CHEMICAL BONDING:

1. Chemical Bonding-1
2. Chemical Bonding-2
3. Chemical Bonding-3
4. Chemical Bonding-4
5. Chemical Bonding-5
6. Chemical Bonding-6
7. Chemical Bonding-7
8. Chemical Bonding-8
9. Chemical Bonding-9
10. Chemical Bonding-10
11. Chemical Bonding-11
12. Chemical Bonding-12
13. Chemical Bonding-13
14. Chemical Bonding-14

Reference Books:

1. Lee, J.D. Concise Inorganic Chemistry, ELBS, 1991.
2. Multistage equilibria in polyelectrolyte systems; hydrolysis and hydrolysis constants.
3. Reference Books:
4. Atkins, P. W. & Paula, J. de Atkin’s Physical Chemistry Ed., Oxford University Press  (2006).
5. Ball, D. W. Physical Chemistry Thomson Press, India (2007).
6. Castellan, G. W. Physical Chemistry 4th Ed. Narosa (2004).
7. Mortimer, R. G. Physical Chemistry 3rd Ed. Elsevier: NOIDA, UP (2009).

SEMESTER-I

Paper 102, PHYSICAL CHEMISTRY

Gaseous state:

Please Click to open Pre Lecture Revision Notes on Gaseous State (Strictly for Self Study)

Kinetic molecular model of a gas: postulates and derivation of the kinetic gas equation; collision frequency; collision diameter; mean free path and viscosity of gases, including their temperature and pressure dependence, relation between mean free path and coefficient of viscosity,σfromη;variation calculation 0f viscosity of with temperature and pressure. Maxwell distribution and its use in evaluating molecular velocities (average, root mean square and most probable) and average kinetic energy,law of equipartition of energy, degrees of freedom and molecular basis ofheat capacities. Behaviour of real gases: Deviations from ideal gas behaviour,compressibility factor, Z, and its variation with pressure for different gases.

Causes of deviation from ideal behaviour. Van der Waals equation of state, its derivation and application in explaining real gas behaviour, mention of other equations of state (Berthelot, Dietrici); virial equation of state; vander Waals equation expressed in virial form and calculation of Boyle temperature. Isotherms of real gases and their comparison with vander Waals isotherms, continuity of states, critical state, relation between critical constants and vander Waals constants, law of corresponding states.(25 Lectures)

Please click below for Revision Lectures and Resources for Undergraduate Chemistry Core Paper 102 on Swayam Prabha by MHRD,Government of India .

1. STATES OF MATTER: GASES AND LIQUIDS 1
2. STATES OF MATTER: GASES AND LIQUIDS 2
3. STATES OF MATTER: GASES AND LIQUIDS 3
4. STATES OF MATTER: GASES AND LIQUIDS 4
5. STATES OF MATTER: GASES AND LIQUIDS 5
6. STATES OF MATTER: GASES AND LIQUIDS 6
7. STATES OF MATTER: GASES AND LIQUIDS 7
8. STATES OF MATTER: GASES AND LIQUIDS 8

PLEASE CLICK BELOW e-Resources and links ON GASEOUS STATE on Swayam Prabha by MHRD,Government of India . :

1. GASEOUS STATE-1
2. GASEOUS STATE-2
3. GASEOUS STATE-3
4. GASEOUS STATE-4
5. GASEOUS STATE-5
6. GASEOUS STATE-6
7. GASEOUS STATE-7
8. GASEOUS STATE-8
9. GASEOUS STATE-9

Ionic equilibria:

Strong, moderate and weak electrolytes, degree of ionization, factors

affecting degree of ionization, ionization constant and ionic product of water. Ionization of weak acids and bases, pH scale, common ion effect; dissociation constants of mono- , di-and triprotic acids (exact treatment). Salt hydrolysis-calculation of hydrolysis constant, degree of hydrolysis and pH for different salts. Buffer solutions; derivation of Henderson equation and its applications; buffer capacity, buffer range, buffer action and applications of buffers in analytical chemistry and biochemical processes in the human body.

Solubility and solubility product of sparingly soluble salts – applications of solubility product principle. Qualitative treatment of acid – base titration curves (calculation of pH at various stages). Theory of acid–base indicators; selection of indicators and their limitations. Multistage equilibria in polyelectrolyte systems; hydrolysis and hydrolysis constants.(35 Lectures)

Please click below for Revision Lectures and Resources for Undergraduate Chemistry Core Paper 102 on Swayam Prabha by MHRD,Government of India .

1. EQUILIBRIUM 1
2. EQUILIBRIUM 2
3. EQUILIBRIUM 3
4. EQUILIBRIUM 4
5. EQUILIBRIUM 5
6. EQUILIBRIUM 6
7. EQUILIBRIUM 7
8. EQUILIBRIUM 8
9. EQUILIBRIUM 9
10. EQUILIBRIUM 10

PLEASE CLICK BELOW e-Resources and links ON CHEMICAL AND  IONIC EQUILIBRIUM:

1. Chemical Equilibrium-1
2. Chemical Equilibrium-2

Reference Books:

1. Atkins, P. W. & Paula, J. de Atkin’s Physical Chemistry Ed., Oxford University Press (2006).
2. Ball, D. W. Physical Chemistry Thomson Press, India (2007).
3. Castellan, G. W. Physical Chemistry 4th Ed. Narosa (2004).
4. Mortimer, R. G. Physical Chemistry 3rd Ed. Elsevier: NOIDA, UP (2009).

CHEMISTRY PRACTICAL-I (4) 60 Lectures

Before you begin Study and Experimentation,Please Watch the Lectures at links given below for Fundamentals of Analytical Chemistry A e-PG Course by the MHRD, Government of India)

1. Neatness and cleanliness in laboratory
2. Types of instrumental methods
3. Common apparatus and basic techniques
4. Laboratory procedures and good laboratory practices
5. Calibration of glasswares and instrument
6. Chemical Equilibrium
7. Stoichiometric calculations
8. Extraction methods
9. Ion exchange methods
10. Gravimetric methods
11. Chromatographic methods- II
12. Molecular spectroscopy
13. Atomic absorption spectroscopy
14. Acids, bases and their salts and complexes (Monoprotic systems)
15. Polyprotic systems
16. Comlexometric titration
17. Precipitation Titration
18. Redox Titration
19. Clinical chemistry
20. Thermoanalytical method- II

Group-A

(A) Titrimetric Analysis 
(i) Calibration and use of apparatus 
(ii) Preparation of solutions of different Molarity/Normality of titrants

(B) Acid-BaseTitrations

(i) Estimation of carbonate and hydroxide present together in mixture.

(ii) Estimation of carbonate and bicarbonate present together in a mixture.

(iii) Estimation of freealkali present in different soaps/detergents

(C) Oxidation-Reduction Titrimetry

(i) Estimation of Fe(II)and oxalic acid using standardized KMnO4 solution.

(ii) Estimation of oxalic acid and sodium oxalate in a given mixture.

(iii)Estimation of Fe(II) with K2Cr2O7 using internal (diphenylamine, anthranilic acid) and external indicator.

Group-B

1. Surface tension measurements.

a. Determine the surface tension by (i) drop number (ii) drop weight method.

b. Study the variation of surface tension of detergent solutions with concentration.

2. Viscosity measurement using Ostwald’s viscometer.

a. Determination of viscosity of aqueous solutions of (i) polymer (ii) ethanol and (iii) sugar at room temperature.

b. Study the variation of viscosity of sucrose solution with the concentration of solute.

Reference text:

1. Vogel, A.I. A Textbook of Quantitative Inorganic Analysis, ELBS.

2. Khosla, B. D.; Garg, V. C. & Gulati, A. Senior Practical Physical Chemistry, S. Chand & Co.: New Delhi (2011).

3. Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experiments in Physical Chemistry 8 th Ed.; McGraw-Hill: New York (2003).

4. Halpern, A. M. & McBane, G. C. Experimental Physical Chemistry 3rdEd.; W.H. Freeman & Co.: New York (2003).