CHEM422 Structure and Spectra: Electronic Vibrational and Microwave
Course Content:
*Unit 0: Matrix Algebra: Operations in matrices, diagonalization, solution to simultaneous equations, eigen values and eigen vectors
Unit I Theory of Normal Vibrations: Electromagnetic radiation, interaction of electromagnetic radiation with matter, quantum mechanical approach -transition probabilities: Einstein coefficients -pure vibrational and rotational spectra, selection rules, vibrational and rotational spectra of polyatomic molecules, Projection operators and normal modes, anharmonicity, selection rules -Raman effect: classical and quantum theory of Raman effect, rotational and vib-rotational Raman spectra
Unit II (Electronic spectroscopy): Transition moments, assignment of electronic transitions of N2, H2O and formaldehyde using group theory, fluorescence and phosphorescence, ESCA, PES, AUGER techniques
Unit III: Application to organic molecules: UV Visible Spectroscopy: Basic principles, application of UV Visible spectroscopy to organic structure elucidation, Woodward –Fisher rules, Octant rule, Application of ORD –CD to stereochemical assignments. IR –Spectroscopy –Basic principles, characteristic frequencies of common functional
Unit IV: Application to Inorganic Chemistry: Diatomic, triatomic, other geometry and compounds ofthe p-block elements –Application to Coordination Chemistry –Application to Organometallics –Application to Bio-Inorganic Chemistry
Unit V: Problem solving
CHEM312 Functional Group Transformations
Reactions of organic compounds and mechanism of reactions will be discussed.
CHEM414 Chemical Reactions and Energetics
CHEM111 Principles of General Chemistry I
Course outcome: On successful completion of this course learners will be able to:
- Comprehend the evolution of electronic structure of atom
- Use quantum numbers and atomic orbital wave function equations to visualize the shapes of orbitals
- Recognize the relationship between position of an element in periodic table and its atomic properties and the periodic trend in properties
- Explain the concept of chemical bonding
- Analyse the properties of gases, liquids, solids and solutions
Course Objectives
1. To develop conceptual knowledge about the electronic structure of atom, organization of periodic table and trend in atomic properties, properties of physical states of matter.
2. Apply the concepts to write electronic configuration of elements. Comprehend, analyse and predict type of chemical bonds and properties of matter.
Course Content:
Unit I Atomic structure
Blackbody emission and temperature, Photoelectric effect, Double slit experiment, Line spectrum of elements, Rutherford’s experiment, Bohr’s atomic model, Heisenberg’s Uncertainty, Quantum atomic model, hydrogen atomic orbitals and quantum numbers, atomic orbital equations (no derivation required), hybrid atomic orbitals, Electronic configuration of atoms, Madelung rule, atomic mass, synthetic elements, isotopes and stability of isotopes (qualitative description)
Unit II Periodic table and periodicity
Periodic trends in atomic properties, reactivity and compound formation, types of compounds, mole concept and composition, oxidation states - Chemical reactions, stoichiometry, chemical reactions in solutions, limiting reagent - Reactions in aqueous medium, precipitation, acid-base, redox, balancing redox reactions, oxidizing and reducing agents, stoichiometry and titration
Unit III Chemical bonding
Types of bonds, representation of electrons as dots, Lewis model of ionic, covalent structures, Electronegativity and bond polarity, Lewis structure of molecular compounds, resonance and formal charge, exception to octet rule, bond energies and bond lengths, bonding in metals - VSEPR theory, predicting molecular geometry, shapes and polarity - Valence Bond theory - Molecular orbital theory, electron delocalization
Unit IV Gases, Liquids, Solids and Solutions
Gas equations, van der Waals gas, virial gas equation, real gases, intermolecular forces - Properties of liquids, properties of solids, phase diagrams, nature of bonding in solids, crystal structures
Unit V Solutions
Types of solutions, solution concentration, solubilities of gases, vapour pressure, osmotic pressure, colligative properties of non-electrolyte solutions, electrolyte solutions, colloidal mixtures
Textbook:
Chemistry A Molecular approach, Nivaldo J Tro, 4ed, Pearson, 2017
Further Reading
Chemistry: The Central Science, Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten, Catherine J. Murphy, Patrick M. Woodward, Matthew W. Stoltzfus, 13ed, Pearson, 2015
CHEM313 Equilibrium Chemical Thermodynamics
Pre-requisite: A pass in higher secondary and working knowledge in basic calculus
Course Outline and Objective: By its origin, thermodynamics is closely related to the study of heat engines and thermodynamic processes. However, the science of thermodynamics should also be understood as the study of thermodynamic properties of substances. In this course, the point of view according to which thermodynamics is concerned with the study of macroscopic properties obtained from macroscopic laws. Students undergoing this course will be equipped to evaluate various thermochemical properties from different experimental variables. From solving problems, students may realise the connection between thermodynamics with biological systems and natural processes.
Unit I: Behaviour of gases and liquids: Real gases, virial equation of state, gas liquid phases - molecular structure of liquids
Unit II First and second laws: First law of thermodynamics, Internal energy, work and heat, enthalpy, effect of enthalpy with temperature, thermochemistry – state functions and exact differentials – Joule Thomson effect – adiabatic changes – Entropy: definitions, Carnot cycle, Clausius inequality, entropy changes in physical processes, measurement of entropy - Third law: Nernst theorem and third law entropy
Unit III System properties and consequences: Helmholtz and Gibbs energies, spontaneous process, maximum work, Standard Gibbs energies – Maxwell relations, temperature, pressure effects on internal, Helmholtz, Gibbs energies, fugacity
Unit IV Physical transformations: Phase stability and phase diagrams, phase rule, thermodynamics of phase transitions – simple mixtures: Partial molar quantities, thermodynamics of mixing, ideal solutions, ideal dilute solutions, excess functions, colligative properties – Phase diagrams: non reacting and reacting binary systems, azeotropes, eutectics, ternary systems
Unit V Equilibrium systems: Activities – solute activity, mean activity coefficients, Debye-Huckel limiting law and theory, activity coefficient – Gibbs energy minimum and equilibrium: effect of temperature and pressure on Gibbs energy change and equilibrium constant Ionic equilibrium: Half-cell reactions and electrodes, types of cells, liquid junction potential, Nernst equation, thermodynamics of cells, determination of standard potentials, activity coefficients, equilibrium constants
Textbook:
Physical Chemistry Thermodynamics, Structure, and Change, Peter W Atkins, Julio de Paula, 10ed, W H Freeman, 2014
Further Readings:
Physical Chemistry, Robert G Mortimer, 3ed, Elsevier, 2008
Physical Chemistry, Thomas Engel and Philip Reid, 3ed, Pearson, 2013
CHEM311 Basic Inorganic Chemistry II
Pre-requisite: A pass in higher secondary
Course Outline and Outcome: Course describes the nature of coordination compounds and their structures, electronic properties. Students undergoing this course will have working knowledge on synthetic and analysis of coordination compounds and their involvement in biological systems.
Course Content:
Unit I (Coordination Compounds I) Introduction, physical and chemical properties of transition elements; Introduction to coordination compounds; coordination numbers and geometries in transition metal complexes; nomenclature; isomerism in transition metal complexes – structural, geometrical and optical isomerism.
Unit II (Coordination Compounds II) Double salts and coordination compounds; Werner’s work; effective atomic number; bonding in transition metal complexes Valence bond theory, crystal field theory (octahedral and tetrahedral complexes); magnetism.
Unit III (Early Transition Elements) Introduction and the chemistry of Scandium group, Titanium group, Vanadium group, Chromium group and Manganese group,
Unit IV (Late Transition Elements) Introduction and the chemistry of Iron group, Cobalt group, Nickel group, Copper group and Zinc group.
Unit V (Inner Transition Elements) Lanthanides: Introduction, occurrence, separation, oxidation states and general chemistry. Actinides: Introduction, isolation and general chemistry
Text Book:
1. D. F. Shriver, P. W. Atkins, C. H. Langford, Inorganic Chemistry, ELBS. 1990.
Further Reading:
1. A. G. Sharpe, Inorganic Chemistry, 3ed, Addison-Wesley, 1999.
2. J. D. Lee, A New Concise Inorganic Chemistry, 3ed, ELBS, 1987.
3. B. Douglas, D. McDaniel, J. Alexander, Concepts and Models of Inorganic Chemistry, 3ed, John Wiley, 2001.
CHEM110 GENERAL CHEMISTRY LABORATORY I
Introductory Chemistry Laboratory. The following are tentative list of experiments:
1.
EVNS 467 Fundamental of Geographic Information System
EVNS 413 Advanced Sustainable development
ECOL485 Ecology of Urban Environment
ECOL462 Landscape Ecology and Planning
ECOL472 Environmental Informatics and Modeling
database management systems, spatial data structure, how to extract information from different
data sources such as airborne data, space-borne data, climate data, GPS, topographical maps, and how to convert them into digital form. It also teaches the students how to integrate and
analyze the trend and patterns. It also introduces the students to the concept of weightage, and how to assign class weightage and layer weightage. The fundamentals of spatial modeling and how to perform modeling to identify the suitability and vulnerability. It also introduces the components of an information system and remote sensing. This course also demonstrates data collection using GPS, Map reading, DBMS, 2D analysis, and 3D analysis