Download CH101 Chemistry

CH101
Chemistry
Dr Sumana Dutta
Room No. CHF101,
Department of Chemistry
[email protected]
258 2322
CH101
Chemistry
(3-1-0-8)
Physical Chemistry
Structure and Bonding; Origin of quantum theory, postulates of quantum mechanics;
Schrodinger wave equation: operators and observables, superposition theorem and expectation values, solutions for particle in a
box, harmonic oscillator, rigid rotator, hydrogen atom; Selection rules of microwave and vibrationalspectroscopy; Spectroscopic
term symbol; Molecular orbitals: LCAO-MO; Huckel theory of conjugated systems; Rotational, vibrational and electronic
spectroscopy; Chemical Thermodynamics: The zeroth and first law, Work, heat, energy and enthalpies; The relation between C¬¬v
and Cp; Second law: entropy, free energy (the Helmholtz and Gibbs) and chemical potential; Third law; Chemical equilibrium;
Chemical kinetics: The rate of reaction, elementary reaction and chain reaction; Surface: The properties of liquid surface,
surfactants, colloidal systems, solid surfaces, physisorption and chemisorption;
Inorganic Chemistry
The periodic table of elements; Shapes of inorganic compounds; Chemistry of materials;
Coordination compounds: ligand, nomenclature, isomerism, stereochemistry, valence bond, crystal field and molecular orbital
theories; Bioinorganic chemistry and organometallic chemistry;
Organic Chemistry
Stereo and regio-chemistry of organic compounds, conformers; Pericyclic reactions; Organic
photochemistry; Bioorganic chemistry: Amino acids, peptides, proteins, enzymes, carbohydrates, nucleic acids and lipids;
Macromolecules (polymers); Modern techniques in structural elucidation of compounds (UV-vis, IR, NMR); Solid phase synthesis
and combinatorial chemistry; Green chemical processes.
Texts:
1. P. W. Atkins, Physical Chemistry, 5th Ed., ELBS, 1994.
2. C. N. Banwell, and E. M. McCash, Fundamentals of Molecular Spectroscopy, 4th Ed., Tata McGraw-Hill, 1962.
3. F. A. Cotton, and G. Wilkinson, Advanced Inorganic Chemistry, 3rd Ed., Wiley Eastern Ltd., New Delhi, 1972, reprint in 1988.
4. D. J. Shriver, P. W. Atkins, and C. H. Langford, Inorganic Chemistry, 2nd Ed., ELBS ,1994.
5. S. H. Pine, Organic Chemistry, McGraw-Hill, 5th Ed., 1987
References:
1. I. A. Levine, Physical Chemistry, 4th Ed., McGraw-Hill, 1995.
2. I. A. Levine, Quantum Chemistry, EE Ed., prentice Hall, 1994.
3. G. M. Barrow, Introduction to Molecular Spectroscopy, International Edition, McGraw-Hill, 1962
4. J. E. Huheey, E. A. Keiter and R. L. Keiter, Inorganic Chemistry:Principle,structure and reactivity, 4th Ed,Harper Collins,1993
5. L. G. Wade (Jr.), Organic Chemistry, Prentice Hall, 1987.
General Instructions
• Slot: B and B1
• Venue: Lecture Hall – L1 (Div I & III)
L2 (Div II & IV)
• Divisions – Div I : 159 students (ME & CE)
Div II : 166 students (ECE, EEE, BT)
Div III:172 students (CSE, EPH,M&C)
Div IV: 159 students(CL, CST, DD)
• Division - I & II: Classes in the morning (9 am - 12 noon)
• Division - III & IV: Classes in the afternoon (2 pm – 5 pm)
Evaluation and grading
2 Quizes: 2 x 10 = 20 % weightage (40 min each)
Midsem exam: 30 % weightage (2 h)
Endsem exam: 50 % weightage (3 h)
Grades
AA:> 90%
AB: >80%
BB: >70%
BC: >60%
CC: >50%
CD: >40%
DD: >30%
F: <30%
Extraordinarily bright students have a chance to secure AS grade!
Rules
• Students are expected to attend all classes. A
student will be debarred from appearing in an
end- semester examination if his/her attendance
falls below 75 percent and will be awarded an
“F”grade in that course.
• You should attend all the Tutorials.. they are not
the same as previous years!
• No examination/quiz/tutorial will be repeated.
Physical Chemistry
Chemical Thermodynamics
Gases: a review. The zeroth and first law, Work, heat, energy and enthalpies; The relation between Cv and Cp;
Second law: entropy, free energy (the Helmholtz and Gibbs) and chemical potential; Third law;
Chemical equilibrium
TEXT: P. W. Atkins, Physical Chemistry, 5th Ed., ELBS, 1994. (or any other editions, e.g. 9th Ed.)
Chemical Kinetics
The rate of reaction, elementary reaction and chain reaction
TEXT: P. W. Atkins, Physical Chemistry, 5th Ed., ELBS, 1994. (or any other editions, e.g. 9th Ed.)
G. W. Castellan, Physical Chemistry, 3rd Ed., Narosa Publishing House, 1985. (or later editions)
Or any basic Physical Chemistry text
Quantum Mechanics:
Structure and Bonding; Origin of quantum theory, postulates of quantum mechanics; Schrodinger wave
equation: operators and observables, superposition theorem and expectation values, solutions for particle in a
box, harmonic oscillator, rigid rotator, hydrogen atom; Selection rules of microwave and
vibrationalspectroscopy; Spectroscopic term symbol; Molecular orbitals: LCAO-MO; Huckel theory of
conjugated systems; Rotational, vibrational and electronic spectroscopy
TEXT: P. W. Atkins, Physical Chemistry, 5th Ed., ELBS, 1994. (or any other editions, e.g. 9th Ed.)
Surface:
Properties of liquid surface, surfactants, colloidal systems, solid surfaces, physisorption and chemisorption
Websites:
http://www.iitg.ernet.in/sumana/CH101.html
http://echem1a.cchem.berkeley.edu/
http://ocw.mit.edu/courses/#chemistry
Very important instruction
Magnitude of a physical quantity written
without units is incomplete and incorrect. (In an
examination it will be treated as wrong answer and not granted any
marks). Use SI units.
Gases: A quick review
Properties:
Gases expand to fill any container: random motion, no attraction
Gases are fluids (like liquids): no attraction
Gases have very low densities: almost no volume = lots of empty
space
Gases can be compressed: almost no volume = lots of empty space
Gases undergo diffusion & effusion: random motion
Physical Measures
V: volume of gas
p: pressure exerted by the gas on the walls of the container
T: Temperature of the gas
n: amount (mass) of gas
Boyle’s Law
n,T constant
p
V
Charles’ Law
V
n,p constant
T
Gay-Lussac’s Law
n,V constant
p
T
Combined Gas Law
p1 V1 p2 V2
=
T1
T2
n constant
Avogadro’s Hypothesis
Equal volumes of gases at the same T
and P have the same number of
molecules
V∝n
V
p,T constant
n
Ideal gas Law
pV ∝ nT
=>
pV = nRT
R: universal gas constant
R = 8.314 JK-1mol-1
Partial Pressure
In a mixture of gases
ni RT nt RT
෍ pi = ෍
=
=p
V
V
pi is the partial pressure of ith gas
Ideal gas
Properties of molecules/atoms of an ideal gas
Has no volume
Undergo elastic collisions
Are in constant, random, straight-line motion
Do not attract or repel each other
Have an average KE directly related to Kelvin temperature
Real Gases
Properties of the molecules/atoms in a real gas
Have their own volume
Attract each other
van der Waals equation of state
ഥ − bሻ ቀp +
ሺV
a
ቁ = RT
2
ഥ
V
a and b are vd Waals constants
0
N·b