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CH107 – Physical Chemistry
• Atomic and molecular structure• Intermolecular forces & dynamics• Driving forces for equilibrium
Instructor (D3): Prof. Arindam Chowdhury, Chemistry, Room 215 Phone: x-7154; 9969437094
CH107/ D3 Course InformationCH107/ D3 Course Information
Instructor: Arindam ChowdhuryInstructor: Arindam Chowdhury
Room No. 215; Department of Chemistry [email protected] (022)2576 7154
Course Secretary: Ms. Charine AstridCentral Facility, Chemistry Department
Email: [email protected]
Phone: (022)2576 4159
Attendance, marks change and course related issues:
CH107 / D3 CH107 / D3
23 lectures and 7 tutorials (23 lectures and 7 tutorials (Attendance is mandetoryAttendance is mandetory))
Lectures at Hall 1 Lectures at Hall 1
MondaysMondays 9.30, 9.30, Tuesdays Tuesdays 10.30 and 10.30 and Thursdays Thursdays 11.30 am11.30 am
17/0917/09 19/09 19/09 23/0923/09 24/0924/09 26/09 26/09 01/1001/10 03/10 03/10 07/1007/10 08/1008/10 10/10 10/10 14/1014/10 15/1015/10 17/10 17/10 21/1021/10 22/1022/10 24/10 24/10 28/1028/10 29/1029/10 31/10 31/1004/11 07/11 04/11 07/11 11/11 11/11 12/1112/11
Tutorials at Tutorials at LCT (31, 32, 33, 22, 23) LCT (31, 32, 33, 22, 23) on on MondaysMondays 23 pm 23 pm
23/0923/0907/10 14/10 21/10 28/1007/10 14/10 21/10 28/1004/11 11/1104/11 11/11
CH107/D3 CH107/D3
Tutorial venue and Teaching AssistantsTutorial venue and Teaching Assistants
D3/T1D3/T1 LCT31LCT31 Shekhar HansdaShekhar Hansda
D3/T2D3/T2 LCT32LCT32 Arindam ChowdhuryArindam Chowdhury
D3/T3D3/T3 LCT33LCT33 Tuhin KhanTuhin Khan
D3/T4D3/T4 LCT22LCT22 Avinash Kumar SinghAvinash Kumar Singh
D3/T5D3/T5 LCT23LCT23 Sandip KarSandip Kar
Emails and phone numbers to be providedEmails and phone numbers to be provided
Office hours : 2 hrs/week and mutually convenient timeOffice hours : 2 hrs/week and mutually convenient time
CH107 CH107
Time TableTime Table
Duration Duration Halfsemester (~8 weeks)Halfsemester (~8 weeks)
Quiz Quiz 19 October 201319 October 2013
EndSemester ExamEndSemester Exam Anywhere between 1829 Anywhere between 1829 November 2013November 2013
TotalTotal 50 Marks50 Marks
Quiz Quiz 20 Marks20 Marks
EndSemester ExamEndSemester Exam 30 Marks30 Marks
Passing MarksPassing Marks 15 (To be followed strictly)15 (To be followed strictly)
Evaluation SchemeEvaluation Scheme
Course Code CH 103 – SEM1SEM1
Course Name Chemistry
Total Grades Given are
416
Out of Which
AA+AB 44
BB 96
BC 95
CC 90
CD 49
DD 23
FR 19
Coursewise Statistics
Course Code CH 103 – SEM2SEM2
Course Name Chemistry
Total Grades Given are
452
Out of Which
AA +AB 22
BB 49
BC 71
CC 105
CD 89
DD 53
FR 63
GRADING STASTICSCoursewise Statistics
Course Code CH 103 – SEM-SEM-11
Course Name Chemistry
Total Grades Given are
424Out of Which
AA+AB 57
AP 1
BB 72
BC 83
CC 64
CD 64
DD 36
FR 47
Coursewise Statistics
Course Code CH 103 – SEM-SEM-22
Course Name Chemistry
Total Grades Given are
462Out of Which
AA + AB 38
BB 49
BC 69
CC 82
CD 89
DD 48
FR 87
Coursewise StatisticsGRADING STASTICS
Why should you study Chemistry?Is there a role of Chemistry inreshaping the modern world?
All of Science and Engineering is moving towards interdisciplinary fields of cuttingedge research!!!
Knowing only one subject often not good enough!
• Nanoelectronics/Nanotechnology: Molecular Electronics• Energy Science – “Solar Energy” conversion• BioTechnology – Disease cure, health, medicine• Atmospheric Science – Go Green “Save the World”
Plastic Electronics and DisplaysConductingpolymers are replacing l iquid crystals
Micro & Nanoelectronics
1947, Transistor, Bell LabsSilicon Transistor, TI 1954 Intel, 1990s, hundreds of
Transistors in a single chip
Transistors, Intel, 2006, 45 nm separationNext Generation: Molecular Chips
Mechanics of Electrons and Atoms
Nano-scienceAnd Nanotechnology
Mult-electron Atoms(Periodic Table)
Electron Microscopy
Intermolecular ForcesAnd Interactions
Multi-atomicBonding, Molecular
Structure
Biology, Materials Science
Condensed Matter Physics
Chemical ReactionsMolecular Dynamics
Atomic/MolecularSpectroscopy
Contents of PartI (14 Lectures ) • Origin of Quantization: Lecture 14
Need of a new theory for electrons, atoms and moleculesPostulates of Quantum MechanicsEnergy Quantization: Particle in a Potential Well
•Electronic Structure in Atoms: Lecture 58Hydrogen Atom and Quantum NumbersAtomic Orbitals and Electron DensitiesMultielectronic atoms and the implications of “Spin”
• Chemical Bonding: Lectures 912Molecular Orbital Theory – Linear Combination of Atomic OrbitalsEnergetic and electronic structure of diatomic molecules
• MolecularElectronic structure Lecture 1314 Bonding in polyatomics using hybridization
Contents of PartII (9 Lectures )
• Intermolecular Forces and PE Surfaces
Lecture 1516
• Reaction Dynamics and Kinetic theories
Lecture 1719
• Driving Forces for Chemical reactions
Lecture 2021
• Chemical Potential and Equilibrium
Lecture 2223
Recommended Text• Physical Chemistry – I.N. Levine, 5th Ed.• Physical Chemistry – P.W. Atkins 2nd Ed.• Physical Chemistry: Molecular Approach
McQuarrie and Simon
Important Websites:CH107 Course Material for 2013And previous year’s powerpoint slides:www.chem.iitb.ac.in/academics/menu.php
and will be regularly updated in IITB Moodlehttp://moodle.iitb.ac.in
Classical EM theory can not explain Blackbody Radiation
Theories based on classical physics unable to explain temperaturedependence of emitted radiation (radiant energy density)
Sun, stars…hot iron rod
All classical theories led to the so called “Ultraviolet Catastrophe”
23
8( ) ; bk T cT d d
cνπρ ν ν ν ν
λ= =
Max Planck assumed energies of osci l lators are discontinuous
3
/( )
1v bv taT d
eνρ ν =
−
Assumption: Energy of electronic oscillators were discrete;Assumption: Energy of electronic oscillators were discrete;Proportional to integral multiple of frequenciesProportional to integral multiple of frequencies
E = Energy of electronic oscillatorsv = frequency of electronic oscillatorsh = Planck’s constant = 6.626 x e34 joulesecNote: h came in as a fitting parameter
OscE nhν=
1858-1947
Planck never believed his theory was right, since he was a classical physicist
3
3 /
8( )1B
vh k T
h dT dc e νπ ν νρ ν
÷
=−
Photoelectr ic Effect
1. Increasing intensity of light increases number of photoelectrons, but not their max. kinetic energy (KEMAX)!
2. Light below a certain wavelength will not cause ejection of electrons, no matter how high it’s intensity!
3. Extremely weak violet light ejects few electrons! But their KEMax >> KEMax of electrons ejected by intense light of longer wavelength
0
20
( )
Wave Energy related
to
of
E E Sin kx t
Intensity E
Independent
ω
ω
= −
µ
Photodetectors, Photovoltaics, Elevator sensor, smoke detectors
Experimental Observations
Einstein: l ight behaves l ike partic les
2
0
Energy to remove e' from surface
1
2
0
P M
M
E hv KE mv
KE hv
φ φ
φφ
=
= = + = +
= − ≥
Borrowing Planck’s idea that ∆E=hv, Einstein further proposed radiation itself existed as small packets of energy (Quanta), known as PHOTONS
P
P
E
E h
νν
µ=
1879-1955; Nobel prizeFor explanation of Photoelectric effect
Energy of photon isfrequency dependent(self contradictory! )
Line Spectra of Atoms
Rydberg’s formula:
1 22 21 2
1 1 1; HR n n
c n n
ννλ
= = = − > ÷
RH = 109677.57 cm-1
1854-1919
Bohr’s Phenomenological Model(RutherfordPlanckEinsteinBohr Model)
• Electrons rotate in circular orbits around a central massive nucleus (+ve), and obey laws of classical
mechanics.
• Allowed orbits are those for which the electron’s angular momentum mevr = n h/2π, n=1,2,3,4,…… • Only certain discrete energy values: “Stationary States”
Atom in such a state does not emit EM radiation (light)
• Transition from a stationary state (Ea) to another (Eb), atom emits or absorbs
EM radiation (light)
1885-1962
Explanation of atomic spectra n=1,2,3,...
2(2 )
nhmvr
r nπ
π λ
=
=
4
2 2 2 2
1 1 , 1, 2,3,...
8e
i fi f
m eE h n n
h n nν
ε
∆ = − = = ÷ ÷
Spectral Transitions: ∆E=hc/λ
Explains Rydberg’s Formula
4
2 2 20
1.
8e
n
m eE
h nε= −
Quantization of Angular momentum
