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Lecture 1 (8/27/01)
1.The flame test revisited. We all should know the common flame colors
observed for Na,Li,K,Ca ,Sr, Ba,B and Cu.
2.Be able to describe the appearance of the line spectrum of excited hydrogen
atoms viewed through a diffraction grating.
3.The Balmer equation and the Rydberg constant.Be able to calculate the
frequencies of the four visible lines in the Balmer spectrum.
4.We should all be able to write down equations for Newton's second law
and Coulomb's equation for the force between charges.Thus we can obtain
the Newton -Coulomb expression from classical physics.
5.Know the Bohr quantum postulate: i.e. the quantisation of the angular
momentum of the electron.
l=pr=mvr=nh/2p.
Demonstrations
1.The Flame test .
2.Discharge tube of Hydrogen .
Recitation 1 (8/28/01)
1.Be able to derive the equation for the centripetal acceleration i.e
a = [v2/r ].
2.Be able to rearrange the Newton- Coulomb equation to make "v"
or "r" the subject.
3.Write down equations for v, p, l, n0, w, K, U , E , 1/l and n in terms
of "r".[note p=mv].
Demonstration
1.Lead and aluminum balls on strings are used to Illustrate the equation
for the centripetal acceleration , namely : a = m [ v 2 / r ].
Lecture 2 (8/29/01)
1.Show that Bohr's theory, which starts by assuming " l " [
i.e. l=mvr] is quantised, predicts the quantisation of "r" ,
"v", p, w, n0 , K, U and E.
2.Show how the Bohr theory yields a value for the Rydberg constant.
3.Calculation of the energy required to promote an electron from n1=1
to the n1=2 state.
4.Be able to calculate the Ionization Energy [IE ] for a H atom by using
the Rydberg Equation.
5.Be able to state Bohr's Correspondence Principle.
6.Know the principal characteristics of waves.
Demonstrations.
1.Laser and various gratings.
Lecture 3 (8/31/01)
1.Describe two achievements and one failing of the Bohr model.
2.Actual example of the Correspondence principle.
3.Know how the de Broglie equation justifies Bohr's quantum postulate..
4.Show how De Broglie derived the equation h=pl from the Einstein equations.
5.Know who was responsible in 1926 for the appearance of three new equivalent
versions of Quantum Theory. I.e. Heisenburg, Schrodinger and Dirac.
Demonstrations.
1.Jig-saw to show waves on a taut string.
2.Waves on a circular metal wire.
3.Water waves used to show diffraction and interference.
Recitation 2 (9/4/01)
1.Decide what types of questions , derived from the first three lectures
, could appear on Friday Quiz 1?
2.Card problems were distributed for small group discussion. Topics included
a.Schrodinger wave equation for a particle in a one dimensional box.
b.Heisenberg uncertainty of velocity of first orbit electron in hydrogen
c.Calculation of IE for Hydrogen using Rydberg equation
d.Explaining the trends in IE seen as we go from H to C.
e.Sketching the main valence bond contributors for simple molecules.
f. Review of Concepts of Formal Charge and Oxidation States.
Lecture 4 (9/5/01)
1.Describe the Schrodinger Wave equation and it's solutions.
2.Show how the three quantum numbers can generate the "long version
of Periodic Table.
3.Discuss the "drumskin " orbitals.
4.The Aufbau Principle , Hund's rule and the Pauli Exclusion Principle.
5.The Slater -Zener rules according to Purcell and Kotz for the calculation
of "Screening" constants.
6.Use E = - (1312 ) Z*2/ n2 in order to obtain the energy of each electron
in an atom or ion.
7.Be able to calculate IE(1) and EA(1) for He through Ne.
Lecture 5 (9/7/01)
1.Obtain Mulliken electronegativity [cM] from IE(!) and EA(1).
2.Be able to convert Xm to Xp. by use of the equation : Xp = 0.34 Xm -
0.2
3.Be able to "guesstimate" the Xp for any element in the first
two periods i.e. Li through Cl.
4.Approximate solutions of the Schrodinger Wave Equation i.e. VB and MO
applied to diatomics such as O2, N2, and CO
Demonstration
1.Liquefaction of Oxygen to show its reactivity, color and paramagnetism.
Lecture 6 (9/10/01)
1.Use of the Bohr radius formula modified by Slater rules to calculate
covalent radii and ionic radii.
2.The Domain method for obtaining the Shapes of Molecules
3.Polar versus non – polar molecules.
4.Dipole Moments.
5.Origin of Pauling Electro negativity Scale.
Demonstration
1.Use of colored balloons to construct an MO diagram for the diatomics.
Recitation 3 (9/11/01)
1.Obtain signature and printed name for photographs.
2.Card problems to be distributed to small groups.Topics that will be
included:
a.Calculation of IE and EA using Bohr-Slater equation.
b.Calculation of the radius of an atom or ion.
c.Construction of an MO diagram for dioxygen and Carbon monoxide..
d.Use of VSEPR or Domain theory to drawer molecular shapes.
Lecture 7 (9/12/01)
1.Review VSEPR Rules.Examples discussed XeF4,IF3,IF52-,IF7
2.QCD 666? Give out hand out on Fundamental Particles.
3.What holds nucleons together?
4.What holds neutrons together?
4.Gellman’s Standard Model discussed.
Lecture 8 (9/14/01)
1.The stable isotopes.
2.Types of radioactivity.
3.Binding energy and mass defect.
4.The majic numbers and the Mayer-Jensen shell model of the nucleus.
5.Nuclear spins..
6. Applications of Radioisotopes namely : tracers, dating and NMR
Lecture 9 (9/17/01)
1.Symmetry Operations and Elements of symmetry.
2.An assortment of molecular models were used to illustrate the latter.
3.Showed all symmetry elements of benzene.Point group D6h.
4.Use of flow chart to determine point group.
Recitation 4 (9/18/01)
1.IR frequency of C13-O16 compared to C12-O16.
2.Intro to multinuclear NMR Spectroscopy
3.Predicting nmr spectra.
4.The 2nI +1 formula.
5.Pascals Triangle.
6.Practice determining point groups of molecules.
e.g. CH4,BF3,NH3,H2O, and allene.
Lecture 10 (9/19/01)
1.Successive operations
2.A multiplication table for the C2h point group.
3.Special features of special point groups.
4.Character Tables
5.Vibrational modes.
Lecture 11 (9/21/01)
1.The fifty minute quiz was given.
2.The take-home quiz was distributed.
3.Later on the day scores were distributed by e-mail to each student.
Lecture 12 (9/24/01)
1.Vibrational Analysis.
2.Character Tables discussed.
3.LGO’s or ligand group orbitals were discussed.
3.The molecular orbital diagram for water was generated.
4.Comparison of VB and MO for the case of water.
Recitation 5 (9/25/01)
1.A set of nine models of molecules and various objects were inspected
i.e “hands-On”activity .
2.Point group assignments were made to each of the nine..
3.Decisions on the presence or absence of chiral centers was discussed.
Lecture 13 (9/26/01)
1.Demonstration on bond energies involving the combustion of Hydrogen
gas. A propane torch attached to a stick was used to explode balloons
of hydrogen gas.
2.Using balloons to show the formation of hybrids.
3.Identifying possible types of hybridisation from the domain number.
4.Identifying LGO’s for methane.
5.Construction of an MO diagram for methane.
6.MO diagram for SF6.
Lecture 14 (9/28/01)
1.Completing the MO diagram for SF6.
2.ccp and hcp
3.Unit cells of ccp and hcp.
4.Holes in ccp and hcp.
5.sc and bcc
6.Phase diagram of iron
7.Tennis balls and ping-pong balls were used to illustrate ccp, hcp and
both tetrahedral and octahedral holes.
8.Take home exam 1 was collected in.
9.No volunteers registered for filling lungs with SF6.
Lecture 15 (10/1/01)
1.Models of Seven crystal systems.
2.Models of Fourteen Bravois lattices.
3.Examination of a set of real crystals
4.Introduction of Band theory of metals.
5.Insulators ,conductors and semi-conductors discussed.
6.Examples of C,Si,Ge,Sn and Pb discussed.
7.Notion of the Fermi level.
8.Doping.
Recitation 6 (10/2/01)
1.Collection of Homework 3.
2.How to find a total reducible representaton ( GR ) for H2O and decompose
it into translations, rotations and vibrations .
3.Determination of the number of IR and Raman bands for H2O.
4.Determination of the number of IR and Raman bands for PF5.
5.Physical explanation of IR and Raman illustrated using tuning fork boxes
and Walky-talky radio sets.
.
Lecture 16 (10/3/01)
1.Use of character tables to determine potential orbitals used in Hybrid
schemes for BeH2, BF3, CH4, PF5, and SF6.
2.Examination of a set of common crystal structures using models.
Lecture 17 (10/5/01)
1.Band theory of metals.
Lecture 18 (10/8/01)
1.The radius ratio rules.
2.Examples dealt with : MgO and BeF2.
3.Finding the number of formula units in unit cells of NaCl,CsCl,TiO2,CaTiO3
and hexagonal ZnS.
Recitation 7 (10/9/01)
1.Predicting the number of IR and Raman bands for IF7.
2.Discussion of finding a reducible representation for the 12 xyz vectors
on the Cl atoms in PtCl4 (2-).
Lecture 19 (10/10/01)
1.Review for exam 2.
2.Practice nodal analysis.
Lecture 20 (10/12/01)
1.Exam postponed
2.Further review
3.Hand out Take home quiz.
Lecture 21 (10/15/01)
1.Lecture Quiz 2
Recitation 8 (10/16/01)
1.Lattice Energy discussed
2.MO diagram for square planar H4 and cubic H8.
3.MO diagram for square planar MH4.
Lecture 22 (10/17/01)
1.Volume of a unit cell: V=abcv(1-cos2a-cos2b-cos2g+2cosa cosb cosg)
2.Volume of cubic unit cell: V=a3.
3.Calculate the theoretical density of Po.
4.Calculate the Madelung constant for a one-dimensional crystal.
5.Derive energy of Avogadro’s number of ion pairs of NaCl.
6.Derive the Coulombic expression for the lattice energy of NaCl.
Recitation 9 (10/23/01)
1.Calculate the theoretical density of Sodium ( a bcc lattice)
2.Calculate the theoretical density of Zinc ( a hcp lattice)
3.The MO diagram derived from Character table for BF3 including both p
and s contributions.
Lecture 23 (10/24/01)
1.Coulombic Equation for Energy of 1.0 moles of diatomics.
2.Madelung Equation.
3.Born Lande Equation.
4.Lattice Energy Calculated for NaCl.
5.Theoretical Lattice Energy of CaF2. Calculated from the Born Lande Equation.
6.Experimental determination of Lattice Energy of CaF2 from Born Haber
Cycle.
Lecture 24 (10/26/01)
1.Relative strengths of various types of acids and bases.
2.Use of Proton Level diagrams in solving Acid-Base problems.
3.Amhoterism.
4.Acidity of Aquated cations..
5.Which is the stronger acid? Al(H2O)63+ or Na(H2O)6+.
6.Which is the stronger base? OH- or CH3-.
Lecture 25 (10/29/01)
1.Discussion of the solubility of salts.
Recitation 10 (10/30/01)
1.Coordination Complexes.
Lecture 26 (10/31/01)
1.Stability of Complexes.
2.How to read Latimer Diagrams.
3.Ellingham Diagrams.
Lecture 27 (11/02/01)
1.Demonstrations of acid base reactions included……..
2.Distribute topic list for exam 3.
3.Practice in balancing half and full equations.
4.The Nova film “Kaboom”.
Lecture 28 (11/05/01)
1.Give back take home 2.
2.Practice on balancing redox.
3.Practice on Latimer diagrams.
4.Theory of Ellingham diagrams.
Recitation 11 (11/06/01)
1.MO diagram for an octahedral complex.
Lecture 29 (11/07/01)
1.The Silver one pot demonstration.Starting with AgNO3 a series of precipitations
interspersed with the formation of soluble complex ions are performed.
2.The Solubility Rules for various salts in aqueous solutions ,given in
Oxtoby , Gillis
or any Freshman text are re-visited .
Lecture 30 (11/09/01)
1.Friday Quiz 3
2.Distribute Take-home exam 3.
Lecture 31 (11/12/01)
1.Presentation by Larry Lewis from GE entitled “From Sand to Silicones
“.
Recitation 12 (11/13/01)
1.Discovery Film by the poet Roger McGough entitled “Elements”.
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