lectures 1-2 - University of California, Santa Cruz · Lectures 1-2 40 Solvay Conference 1927 The...
Transcript of lectures 1-2 - University of California, Santa Cruz · Lectures 1-2 40 Solvay Conference 1927 The...
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Chemistry 1B-01, Fall 2012 Lectures 1-2
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Chemistry 1B
Fall 2012
lectures 1-2(ch 12 pp 522-536)6th
[ch 12 pp 522-537]7th
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• Why? To understand the behavior of electronsin atoms an molecules
goals of lectures 1-2
• The “laws of nature” in 1900 (successful for describing large objects)
describe particles AND describe waves
• Experiments that contradicted these laws(when applied on the scale of atomic dimensions)
Ultraviolet Catastrophe and Photoelectric Effect Spectrum of Hydrogen Atom Davisson-Germer and Compton Experiments
• particles BEHAVE AS waves
waves BEHAVE AS particles
• obtain and use observed quantitative relationships (HW #1)
• Why? To understand the behavior of electronsin atoms an molecules
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Chemistry 1B-01, Fall 2012 Lectures 1-2
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physics and chemistry in 1900
• fundamental particles and chargeelectron: - charge, me= 9.109 10-31 kgproton: + charge, mp= 1.672 10-27 kgneutron: 0 charge, mn= 1.675 10-27 kg
[back page]
• particles in general
• electromagnetic waves
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light waves
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Chemistry 1B-01, Fall 2012 Lectures 1-2
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properties of electromagnetic radiation (light WAVES)
• electromagnetic wavefig 12.1~ fig 12.2fig 12.3spectrum of visible light
• wave phenomena• refraction• dispersion• diffraction • interference and Fig. 12.7
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Planck’s Formula
• Blackbody radiation- Fig 12.4
• Ultraviolet catastrophe (p. 525)
• E=h (energy per photon)
(HW#1 PROB 12.21)
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some comments about “energy” ( sec 9.1, pp. 359-360)
• kinetic energy
• potential energy
• conservation of energy
• momentum (p. 158)
• units and conversions
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photoelectric effect (pp 514-515)
• apparatus Sil Fig. 7.7
• what’s observed
• interpretation (HW#1 12.27)
photoemissive
material
anode collector
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Chemistry 1B-01, Fall 2012 Lectures 1-2
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−
photoelectric effect : electron in a “potential well” (CLASSICAL: small amplitude, long wavelength)
ener
gy
low amplitudewave
(long l)
no electron ejected
attraction of metal
for election
is work function (value depends on the metal being irradiated)
low amplitudewave
(long l)
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−
photoelectric effect : electron in a “potential well” (CLASSICAL: large amplitude, long wavelength)
ener
gy
no electron ejected
attraction of metal
for election
is work function (value depends on the metal being irradiated)
large amplitudewave
(long l)
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−
photoelectric effect : electron in a “potential well” (= long)
ener
gy
low energyphoton
no electron ejected
attraction of metal
for election
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−
photoelectric effect : electron in a “potential well” ( = medium)
ener
gy
medium energy
photon
no extra energy for KE
attraction of metal
for election
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Chemistry 1B-01, Fall 2012 Lectures 1-2
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−
photoelectric effect : electron in a “potential well” ( = short)
ener
gy
high energy
photon
mucho extra energy for KE
attraction of metal
for election
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summary of observations
KE
of
ejec
ted
ele
ctro
ns
frequency of light ( )
cesium sodium
0=Cs
h0= Na
h
> 0 more intense light more electrons, but of same kinetic energy
0= 4.60 1014 sec-1
l0= 652.6 10-9 m = 652.6 nm
0= 5.95 1014 sec-1
l0= 504 10-9 m = 504 nm
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conservation of energy (p 527)
if a individual photon that has sufficient energy to ‘kick’ electron out of the potential well of metal:
if an individual photon does not have sufficient energyto ‘kick’ electron out of the potential well of metal:
NO ELECTRONS EJECTED !!
energy of photon= energy to get out of well + kinetic energy of electron
20 metal electron
0 metal
1 2
metal
1hν = hν + K.E.= Φ + m v
2K.E.=hν -hν hν-Φ
2v = hν -Φ
photon e
photon
electron photonem
0 metal hν Φ work function of metalDEFINITION :
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spectrum of atomic hydrogen
• classical prediction (death spiral)
• observation of atomic spectrafig. 12.8
• Bohr model (HW#1 12.35a,d, 12.36, *12.39)
fig. 12.10, Silberberg 7.10
1 12 22 21 2
7 1
1 1 1and are integers with
1.096776 10 R is the Rydberg constant
R n n n nn n
R m
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Davisson-Germer experiment
X-ray diffractionof Al foil
Electron diffractionof Al foil
mind blowing
diffraction by slits and crystals
constructive int
destructive int
remember: WAVES showed
x-rays electrons ??
constructive int
destructive int
constructive and destructive interference
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wave-particle duality
• diffraction of electrons-(Davisson-Germer Experiment; p. 530)
• De Broglie relationship (p. 528) (HW#1 12.30,12.33)
• What is “meaning” of electron wave?? (http://phys.educ.ksu.edu/vqm/html/doubleslit/index.html)(http://www.youtube.com/watch?v=DfPeprQ7oGc)
• Wavelengths of “ordinary” objects (p. 528, example 12.2) Silberberg Table 7.1 (HW#1 prob S2)
• Compton Experiment
• Heisenberg uncertainty principle (p. 539) boing!! (HW#1 12.45)
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Chemistry 1B-01, Fall 2012 Lectures 1-2
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goals of lectures 1-2
• The “laws of nature” in 1900 (successful for describing large objects)
describe particles AND describe waves
• Experiments that contradicted these laws(when applied on the scale of atomic dimensions)
Davisson-Germer and Compton Experiments
Ultraviolet Catastrophe and Photoelectric Effect
Spectrum of Hydrogen Atom
• particles BEHAVE AS waves
waves BEHAVE AS particles
• Ensuing quantitative relationships
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What to do ??
invent quantum mechanics !!!
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Solvay Conference 1927
The mid-1920's saw the development of the quantum theory, which had a profound effect on chemistry. Many theories in science are first presented at international meetings. This photograph of well-known scientists was taken at the international Solvay Conference in 1927. Among those present are many whose names are still known today. Front row, left to right: I. Langmuir, M. Planck, M. Curie, H. A. Lorentz, A. Einstein, P. Langevin, C. E. Guye, C. T. R. Wilson, O. W. Richardson. Second row, left to right: P. Debye, M. Knudsen, W. L. Bragg, H. A.Kramers, P. A. M. Dirac, A. H. Compton, L. V. de Broglie, M. Born, N. Bohr. Standing, left to right: A. Piccard, E. Henriot, P. Ehrenfest, E. Herzen, T. De Donder, E. Schroedinger, E. Verschaffelt, W. Pauli, W. Heisenberg, R. H. Fowler, L. Brillouin.
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‘fuel’ for quantum mechanicians
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quantum mechanics: WEIRD
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end of lectures 1-2
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figure 12.1 Zumdahl
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figure ~12.2
=cHW PROBS #12.22, 12.28
wave amplitude
wavelength (l) and frequency (n )
c=speed of light2.996 â 108 m s-1
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Silberberg figure 7.2
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Zumdahl figure 12.3
HW PROBS #12.21, #12.26
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R O Y G B I V
ROY G BIV
wavelength and color
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Silberberg figure 7.5 and Zumdahl 12.7
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Zumdahl figure 12.3 and Silberberg figure 7.6
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Ultraviolet catastrophe
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Silberberg figure 7.7
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classical “decay and death of hydrogen atom”
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Zumdahl figure 12.8
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Silberberg figure 7.10 (emission: H-electron loses energy)
2 1 1 2
2 1
218
2
18 22 21 2
2 178 10
1 12 178 10
2 17
2 1 2 1
Z=1 for H atom, n=1, 2, 3, ...
energy lost (emitted) by H atom, n n (n >n )
energy of photon em
-
itted
.
.
.
n
n n n n
photon n n
photon
ZE J
n
E E E J Zn n
E E
h
18 22 21 2
18 22 21 2
182 7 1 2
2 2 2 21 2 1 2
1 18 10
1 12 178 10
1 2 178 10 1 1 1 11 0967 10
.
..
photon
J Zn n
hcJ Z
n n
JZ m Z
hc n n n n
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Silberberg figure 7.10 (absorption, H-electron gains energy)
1 2 2 1
1 2
218
2
18 22 22 1
2 178 10
1 12 178 10
.
.
1 2 2 1
Z=1 for H atom, n=1, 2, 3, ...
energy gained (absorbed) by H atom, n n (n >n )
energy of photon abs
+
orbed
n
n n n n
photon n n
photon
ZE J
n
E E E J Zn n
E E
h 18 21 22 2
1 2
18 22 21 2
182 7 1 2
2 2 2 21 2 1 2
1 12 178 10
1 12 178 10
1 2 178 10 1 1 1 11 0967 10
.
.
..
(note loss of - and switch of n ,n )
photon
J Zn n
hcJ Z
n n
JZ m Z
hc n n n n
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Zumdahl figure 12.10
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Silberberg figure 7.5 and Zumdahl 12.7
constructive=high intensity
destructive=low intensity
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from http://phys.educ.ksu.edu/vqm/html/doubleslit/index.html
photons l= 402 nm
electrons v=3.06 106 m sec-1photons l= 594 nm
[slit 10-5 m] [slit 5 10-9 m]
electrons v= 4.6 106 m sec-1
ve e
h
m
l increases x 1.5 v decreases x 1.5l increases
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Silberberg Table 7.1
note mass in g, need to use kg for mvl=h(l correct in table)
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waves: x vs v
xx
y
Vx Vx
x larger x smaller
vx smaller vx larger
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Uncertainty and measurement
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particles in classical physics
• particles have mass (m) , definite positions (x) and velocities (v)
• particles have kinetic energyand momentum p=mv
• particles obey Newton’s laws of physics F=ma
21KE= mv
2