chapter24 quantum physics
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24. QUANTUM PHYSICS
Liew Sau Poh
Outline
24.1 Photons24.2 Wave-particle duality24.3 Atomic structure24.4 X-rays24.5 Nanoscience
Objectives
(a) describe important observations inphotoelectric emission experiments
(b) recognise features of photoelectric emissionthat cannot be explained by wave theory andexplain these features using the concept ofquantisation of light
(c) use the equation for a photon E = hf (d ) explain the meaning of work function and
threshold frequency
Objectives
(eeffect, hf =W + ½mv2
max
( f ) understand the meaning of stopping potentialand use eV s= ½mv2max
(h) use the relation = h/p to calculate deBroglie wavelength
(i) interpret the electron diffraction pattern as anevidence of the wave nature of electron
Objectives( j) explain the advantages of an electron
microscope as compared to an opticalmicroscope
(l) derive an expression for the radii of the orbits
(m) derive the formula
Objectives(n) explain the production of emission line
spectra with reference to the transitionsbetween energy levels
(o) explain the concepts of excitation energy andionisation energy
(p) interpret X-ray spectra obtained from X-raytubes
(q) explain the characteristic line spectrum and
continuous spectrum including min in X-rays
Objectives
(r) derive and use the equation min = hc / eV
(s) describe X-ray diffraction by two paralleladjacent atomic planes
d sin = m
(u) explain the basic concept of nanoscience(v) state the applications of nanoscience in
electronics devices
24.1 Photon
Photoelectric effect: When electromagnetic radiation is incident tothe surface of a metal, electrons are ejectedfrom the surface.
Photoelectrons:
The electrons emitted by this effect.UV
Metals Metals other than Alkali Metals Alkali Metals
Visible light
No photoelectronsPhotoelectrons Photoelectrons
Visible light
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Photon
A packet or bundle of energy is called aphoton.
Energy of a photon is
where h
f is the frequency of the radiation or photon,
c is the speed of light (e.m. wave) and
is the wavelength.
E = hf =hc
m =h
cEc2 =
p =hE
c =
Properties of photons
A photon travels at a speed of light c in vacuum.(i.e. 3 x 108 m/s)
It has zero rest mass. i.e. the photon can not existat rest.
The kinetic mass of a photon is,
The momentum of a photon is,
Photons travel in a straight line.Energy of a photon depends upon frequency of thephoton; so the energy of the photon does notchange when photon travels from one medium toanother.
Properties of photons
Wavelength of the photon changes indifferent media; so, velocity of a photon is
different in different media.Photons are electrically neutral.
Photons may show diffraction under givenconditions.
Photons are not deviated by magnetic andelectric fields.
Metals other than Alkali Metals
Visible lightNo photoelectrons
UV
Metals
Photoelectrons
Alkali Metals
PhotoelectronsVisible light
Photoelectric Effect
Photoelectric EffectThe phenomenon of emission of electrons from mainlymetal surfaces exposed to light energy (X rays,rays, UV rays, Visible light and even Infra Red rays) ofsuitable frequency is known as photoelectric effect.The electrons emitted by this effect are calledphotoelectrons.The current constituted by photoelectrons is known asphotoelectric current.Note: Non metals also show photoelectric effect.Liquids and gases also show this effect but to limitedextent.
Experimental (Photoelectric Effect)
UV light
K V
+A
+
C A
W
C Metallic cathode
A Metallic Anode
W Quartz Window
- Photoelectron
Experimental (Photoelectric Effect)
Glass transmits only visible and infra-red lightsbut not UV light.Quartz transmits UV light. When light of suitable frequency falls on themetallic cathode, photoelectrons are emitted.
These photoelectrons are attracted towards the+ve anode and hence photoelectric current isconstituted.
I A
Intensity (L)0
Experimental (Photoelectric Effect)
1) Effect of Intensity of Incident Light onPhotoelectric Current:For a fixed frequency, the photoelectric currentincreases linearly with increase in intensity ofincident light.
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0
SaturationCurrent
L1
L2
L2 > L1
IA
+Potential of A (V)VS
Experimental (Photoelectric Effect)
2) Effect of Potential onPhotoelectric Current:For a fixed frequency andintensity of incident light,the photoelectric currentincreases with increase in+ve potential applied to theanode.
When all thephotoelectrons reach theplate A, current becomesmaximum and is known assaturation current.
0
SaturationCurrent
L1
L2
L2 > L1
IA
+Potential of A (V)VS
Experimental (Photoelectric Effect)
2) Effect of Potential onPhotoelectric Current:
When the potential isdecreased, the currentdecreases but does notbecome zero at zeropotential.This shows that even in theabsence of accelerating
potential, a fewphotoelectrons manage toreach the plate on theirown due to their K.E.
0
SaturationCurrent
L1
L2
L2 > L1
I A
+Potential of A (V)VS
Experimental (Photoelectric Effect)
2) Effect of Potential onPhotoelectric Current:
When ve potential is
applied to the plate A w.r.t.C, photoelectric currentbecomes zero at aparticular value of vepotential called stoppingpotential or cut-offpotential.Intensity of incident lightdoes not affect the stoppingpotential.
IA
Potential of A (V)0VS1
+
Saturation Current
1
2
2 >
1
VS2
Experimental (Photoelectric Effect)
3) Effect of Frequency of IncidentLight on Photoelectric Current:For a fixed intensity of incidentlight, the photoelectric current
does not depend on thefrequency of the incident light.Because, the photoelectriccurrent simply depends on thenumber of photoelectronsemitted and in turn on thenumber of photons incidentand not on the energy ofphotons.
IA
Potential of A (V)0VS1
+
Saturation Current
1
2
2 >
1
VS2
Experimental (Photoelectric Effect)4) Effect of Frequency of
Incident Light on StoppingPotential:For a fixed intensity ofincident light, thephotoelectric currentincreases and is saturated
with increase in +vepotential applied to theanode.However, the saturation
current is same fordifferent frequencies of theincident lights.
IA
Potential of A (V)0VS1
+
Saturation Current
1
2
2 >
1
VS2
Experimental (Photoelectric Effect)4) Effect of Frequency of
Incident Light on StoppingPotential:
When potential isdecreased and taken belowzero, photoelectric currentdecreases to zero but atdifferent stoppingpotentials for differentfrequencies.
Higher the frequency, higher the stopping potential. i.e. VS
VS (V)
0 0
5) Threshold Frequency
The graph between stoppingpotential and frequency does notpass through the origin.It shows that there is a minimum
value of frequency called thresholdfrequency below which photoelectric
emission is not possible howeverhigh the intensity of incident lightmay be.It depends on the nature of the metalemitting photoelectrons.
28.2 Concept of light quantisation
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Laws of Photoelectric Emission
For a given substance, there is a minimum value of frequency of incident light calledthreshold frequency below which nophotoelectric emission is possible, howsoever,the intensity of incident light may be.The number of photoelectrons emitted persecond (i.e. photoelectric current) is directly
proportional to the intensity of incident lightprovided the frequency is above the thresholdfrequency.
Laws of Photoelectric Emission
The maximum kinetic energy of the photoelectrons isdirectly proportional to the frequency provided thefrequency is above the threshold frequency.The maximum kinetic energy of the photoelectrons isindependent of the intensity of the incident light.The process of photoelectric emission isinstantaneous. i.e. as soon as the photon of suitablefrequency falls on the substance, it emitsphotoelectrons.The photoelectric emission is one-to-one. i.e. forevery photon of suitable frequency one electron isemitted.
the energy of the photon is absorbed by the electronand is used in two ways:
A part of energy is used to overcome the surfacebarrier and come out of the metal surface. This part work function 0).
The remaining part of the energy is used in giving a
to the maximum kinetic energy of the photoelectrons( ½ mv 2max
According to law of conservation of energy,
hf = + ½ mv2max
= hf 0 + ½ mv2max
½ mv2max = h ( f - f 0 )
Photon h
Metal
Photoelectron
½ mv2max
= h 0
½ mv2max = h ( - 0 )
Verification of Laws of Photoelectric Emission based
If < 0, then ½ mv 2max is negative, which isnot possible. Therefore, for photoelectricemission to take place > 0.Since one photon emits one electron, so thenumber photoelectrons emitted per second isdirectly proportional to the intensity ofincident light.
½ mv2max = h ( - 0 )
Verification of Laws of Photoelectric Emission based
It is clear that ½ mv 2max as h and 0 are constant.This shows that K.E. of the photoelectrons is directlyproportional to the frequency of the incident light.Photoelectric emission is due to collision between aphoton and an electron. As such there can not be anysignificant time lag between the incidence of photonand emission of photoelectron. i.e. the process is
instantaneous. The delay is only 10-8
seconds.
Application of Photoelectric Effect
Automatic fire alarm
Automatic burglar alarm
Scanners in Televisiontransmission
Reproduction of sound incinema film
In paper industry tomeasure the thickness ofpaper
To locate flaws or holes inthe finished goods
In astronomy
To determine opacity ofsolids and liquids
Automatic switching ofstreet lights
To control thetemperature of furnace
Photometry
Beauty meter Tomeasure the fair
complexion of skinLight meters used incinema industry to checkthe light
Photoelectric sorting
Photo counting
Meteorology
Photoelectric ThresholdBinding Energies
K: 100L: 50M: 20
Photon in
Photon energy: 15
Which shells arecandidates forphotoelectricinteractions?
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Photoelectric Threshold
Photon in
Photon energy: 15
NO
NO
NO
Binding EnergiesK: 100L: 50M: 20
Which shells arecandidates forphotoelectricinteractions?
Photoelectric Threshold
Photon in
Photon energy: 25
Binding EnergiesK: 100L: 50M: 20
Which shells arecandidates forphotoelectricinteractions?
Photoelectric Threshold
Photon in
Photon energy: 25
NO
NO
YES
Binding EnergiesK: 100
L: 50M: 20
Which shells arecandidates forphotoelectricinteractions?
Photoelectric Threshold
Photon in
Photon energy: 22
Which photon hasa greaterprobability forphotoelectricinteractions withthe m shell?
Photon energy: 25
A
B
1
P.E. ~ -----------energy3
Binding EnergiesK: 100
L: 50M: 20
Photoelectric Threshold
Photon in
Photon energy: 55
Which shells arecandidates forphotoelectricinteractions?
Binding EnergiesK: 100L: 50M: 20
Photoelectric Threshold
Photon in
Photon energy: 55
Which shells arecandidates forphotoelectricinteractions?
NO
YES
YES
Binding EnergiesK: 100L: 50M: 20
Photoelectric Threshold
Photon in
Photon energy: 105
Binding EnergiesK: 100L: 50M: 20
Which shells arecandidates forphotoelectricinteractions?
Photoelectric Threshold
Photon energy: 105
YES
YES
YES
Binding EnergiesK: 100L: 50M: 20
Which shells arecandidates forphotoelectricinteractions?
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Photoelectric Threshold
Photoelectric interactions
decrease with increasing photonenergy
1P.E. ~ -----------
energy3
Photoelectric Threshold
Binding EnergiesK: 50L: 25
Photon energy: 49
NO
YES
Photon energy: 51
YES
YES
When photon energy just reaches bindingenergy of next (inner) shell, photoelectricinteraction now possible with that shell
shell offers new candidate target electrons
Photoelectric Threshold
When photon energies just reaches binding energy of
next (inner) shell, photoelectric interaction now
possible with that shell, where shell offers new
candidate target electrons
Photon Energy
InteractionProbability
K-shellinteractions possible
L-shellinteractions
possibleL-shellbindingenergy
K-shellbindingenergy
M-shellinteractions
possible
Photoelectric Threshold
causes step increases in interactionprobability as photon energy exceeds shell
binding energies
Photon Energy
InteractionProbability L-edge
K-edge
24.2 Wave-particle Duality
Dual Nature of Radiation and Matter Wave theory of electromagnetic radiationsexplained the phenomenon of interference,diffraction and polarization.On the other hand, quantum theory of e.m.radiations successfully explained thephotoelectric effect, Compton effect, blackbody radiations, X- ray spectra, etc.Thus, radiations have dual nature. i.e. waveand particle nature.
Dual Nature of Radiation and Matter
Louis de Broglie suggested that the particles likeelectrons, protons, neutrons, etc have also dual nature.i.e. they also can have particle as well as wave nature.Note: In no experiment, matter exists both as aparticle and as a wave simultaneously. It is either theone or the other aspect. i.e. The two aspects are
complementary to each other.His suggestion was based on:The nature loves symmetry.The universe is made of particles and radiations andboth entities must be symmetrical.
de Broglie wave
According to de Broglie, a moving materialparticle can be associated with a wave. i.e. a wave can guide the motion of the particle.The waves associated with the moving materialparticles are known as de Broglie waves or
matter waves.
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Expression for de Broglie wave
According to quantum theory, the energy of thephoton is
the photon is
If instead of a photon, we have a materialparticle of mass m moving with velocity v, thenthe equation becomes which is the expression for de Broglie wavelength.
E = h =hc
E = mc2
So = hmc
or =hp
where p = mcis momentum of a photon
= hmv
The Compton Effect
Let the light is made up of particles (photons),and that photons have momentum, with energyhf collides with a stationary electron.Some of the energy and momentum istransferred to the electron (this is known as theCompton effect), but both energy and
momentum are conserved (elastic collision). After the collision the photon has energy hf andthe electron has acquired a kinetic energy K .Conservation of energy: hf = hf + K
Conclusionde Broglie wavelength is inversely proportional to the
velocity of the particle. If the particle moves faster,then the wavelength will be smaller and vice versa.
If the particle is at rest, then the de Broglie wavelengthis infinite. Such a wave can not be visualized.de Broglie wavelength is inversely proportional to themass of the particle. The wavelength associated with aheavier particle is smaller than that with a lighterparticle.de Broglie wavelength is independent of the charge ofthe particle.
= hmv
Conclusion
Matter waves, similar to electromagnetic waves,can travel in vacuum and hence they are not
mechanical waves.Matter waves are not electromagnetic wavesbecause they are not produced by acceleratedcharges.Matter waves are probability waves, amplitudeof which gives the probability of existence ofthe particle at the point.
= hmv
Davisson and Germer Experiment A beam of electronsemitted by the electrongun is made to fall onNickel crystal cut alongcubical axis at aparticular angle.The scattered beam ofelectrons is received bythe detector which can berotated at any angle.
F
V
C
A
Nickel Crystal
Electron Gun
Crystal Lattice
Davisson and Germer ExperimentThe energy of theincident beam ofelectrons can be varied bychanging the applied
voltage to the electrongun.Intensity of scatteredbeam of electrons isfound to be maximum
when angle of scatteringis 50° and the
accelerating potential is54 V.
F
V
C
A
Nickel Crystal
Electron Gun
Crystal Lattice
Davisson and Germer Experiment
+ 50° + = 180°
i.e. = 65°
For Ni crystal, latticespacing d = 0.91 Å
For first principalmaximum, n = 1
Electron diffraction issimilar to X-raydiffraction.
F
V
CA
Nickel Crystal
Electron Gun
Crystal Lattice
2dsin = n gives = 1.65 Å
= 50
I n c i d e n t B e a m
Intensity of scattered beam at 54 V
I n c i d e n t B e a m
Intensity of scattered beam at 44 V
I n c i d e n t B e a m
Intensity of scattered beam at 48 V
I n c i d e n t B e a m
Intensity of scattered beam at 64 V
hypothesis, h=
2meV
de Broglie wavelength ofmoving electron at V = 54Volt is 1.67 Å which is inclose agreement with 1.65 Å.
12.27 Å=
Vor
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0 5 10 15 20 25
Diffraction
pattern after
100 electrons
Diffractionpattern after
3000 electrons
Diffraction
pattern after
70000 electrons
Intensity vsThe Electron Microscope
Using wave-nature and particle nature ofelectronElectron is accelerated through a high voltageBetter than optical microscope
Shorter Wavelength : (up to 10-10 ) vs (10-7)Higher resolving power: nanometer vs. micro
24.3 Atomic structure
SF027 66
atom
Early models of atom
In 1898, Joseph John Thomson suggested a model of an atom
that consists of homogenous positively charged spheres with tiny
negatively charged electrons embedded throughout the sphere
as shown in the Figure.
The electrons much likes currants in a plum pudding.
atom.
positively
charged
sphere
electron
In 1911, Ernest Rutherford performed a critical
correct and proposed his new atomic model known
shown in Figure
nucleuselectron
pictured as electrons orbiting around a central
nucleus which concentrated of positive charge.
The electrons are accelerating because their
directions are constantly changing as they circle the
nucleus.
nucleuselectron
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Based on the wave theory, an accelerating
charge emits energy.
Hence the electrons must emit the EM
radiation as they revolve around the nucleus.
+ Ze e
energy loss
As a result of the continuous loss of energy, the radii
of the electron orbits will be decreased steadily.
This would lead the electrons spiral and falls into the
nucleus, hence the atom would collapse as shown in
Figure.
+ Ze
e
energy loss
1. Only certain discrete orbits (stationary states) are
allowed for the electron
2. Electron in a stationary state does not radiate
3. Classical mechanics apply to electron in a stationary
state (not between states)
4. When an electron moves from one SS to another, a
change in energy occurs involving the emission (or
absorption) of a single photon of frequency v = E/h
5. Permitted orbits (SS) are those in which angular
momentum can take on only the discrete values
nh/2
force as the centripetal force he obtained
22
21
20
4 11
)4(4 nnh
mev e
+e
e
v
r
e F
In 1913, Neils Bohr proposed a
new atomic model based on
hydrogen atom.
assumes that each electron
moves in a circular orbit which is
centred on the nucleus, the
necessary centripetal force being
provided by the electrostatic force
of attraction between the
positively charged nucleus andthe negatively charged electron.
On this basis he was able to show that the energy ofan orbiting electron depends on the radius of its orbit.
This model has several features which are describedby the postulates (assumptions) stated below :
1. The electrons move only in certain circular orbits,called STATIONARY STATES or ENERGY LEVELS.When it is in one of these orbits, it does not radiateenergy.
2. The only permissible orbits are those in the discreteset for which the angular momentum of the electron L
equals an integer times h/ 2 . Mathematically,
2
nh L
2
nhmvr (11.1)
and m v r L
where
orbittheof radius:r electrontheof mass:m
,... , ,n 321numberquantum principal:
3. Emission or absorption of radiation occurs onlywhen an electron makes a transition from oneorbit to another .The frequency f of the emitted (absorbed) radiationis given by
if E E h f E
where
constantsPlanck':h
stateenergyfinal:f E
energyof change: E
stateenergyinitial:i E
If E f > E iIf E f < E i Emission of EM radiation
Absorption of EM radiation
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Energy level of hydrogen atom
Consider one electron of charge e and mass m moves in a
circular orbit of radius r around a positively charged nucleus with
a velocity v.
The electrostatic force between electron and nucleus contributes
the centripetal force as write in the relation below:
ce F F centripetal force electrostatic force
r
m v
r
QQ 2
2
21
04
1and eQQ 21
r
emv
0
22
4(11.3)
+e
e v
r
e F
By taking square of both side of the equation, we get
By dividing the eqs. (11.4) and (11.3), thus
2
nhmvr
(11.4)2
22222
4
hnr vm
r
e
hn
mv
r vm
0
2
2
22
2
222
4
4
2
022
me
hnr and
k 4
10
electrostaticconstant
which r n is radii of the permissible orbits for the
where a0 is called the of hydrogenatom.
k m e
hnr
4
12
22
(11.5).. .3,2,1;4 22
22
nm ke
hnr n
02anr n
22
2
04 mke
ha
(11.6)
and
the radius of themost stable (lowest) orbit or ground state (n=1) inthe hydrogen atom and its value is
Unit conversion:
The radii of the orbits associated with allowed orbitsor states n are 4a0 ,9a0 , thus theradii are quantized.
2199312
234
0
1060.11000.91011.94
1063.6a
m1031.5 1 10a OR 0.531 Å (angstrom)
1 Å = 1.00 10 10 m
Energy level in hydrogen atom
is defined as a fixed energy corresponding to theorbits in which its electrons move around thenucleus.
The energy levels of atoms are quantized.
The total energy level E of the hydrogen atom isgiven by
K U E (11.7)
Kinetic energy of the electron Potential energy of the electron
Energy level in hydrogen atom
Potential energy U of the electron is given
by
r
QkQU 21 eQeQ 21 ;where
02 anr and
02
2
an
keU (11.8)
nucleus electron
Kinetic energy K of the electron is given by
Therefore the eq. (11.7) can be written as
2
2
1mv K
(11.9)
butr
emv
0
22
4
r
e K
0
2
42
1where k
04
1
02
2
2
1
an
ke K
02
2
02
2
2
1
an
ke
an
ke E n
and0
2 anr
20
21
2 na
ke E n (11.10)
In general, the total energy level E for the atom is
Using numerical value of k , e and a0, thus the eq. (11.10) can be
written as
2
2
0
2
2 n
Z
a
ke E n (11.11)
211
2199 1
1031.52
1060.11000.9
n E n
219
181
eV
1060.1
1017.2
n
1,2,3,...eV;6.13
2 n
n E n (11.12)
Note:
Eqs. (11.10) and (11.12) are valid for energy level of thehydrogen atom.
where n u m b e r a t o m ic: Z
where (orbi t)stateo f l eve lene rgy: t hn E n
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The negative sign in the eq. (11.12) indicates that work has tobe done to remove the electron from the bound of the atom toinfinity, where it is considered to have zero energy.
The energy levels of the hydrogen atom are when
n=1, the ground state (the state of the lowest energy level) ;
n=2, the first excited state;
n=3, the second excited state;
n=4, the third excited state;
n= , the energy level is
eV613eV1
6.1321 . E
eV403eV2
6.1322 . E
0eV6.132
E
eV511eV3
6.13
23 . E
eV850eV4
6.1324 . E
electron is completelyremoved from the atom.
Figure 11.4 shows diagrammatically the various energy levels in thehydrogen atom.
excited state
is defined as helowest stableenergy state ofan atom.
is defined as he energy
levels that
higher thanhe ground
state.
(eV E nn
0.0
5 54.04 85.0
3 51.1
2 40.3
1 6.13
Excitation energyis defined as the energyrequired by an electron thatraises it to an excited statefrom its ground state.
Ionization energyis defined as theenergy requiredby an electron inthe ground stateto escapecompletely fromthe attraction ofthe nucleus.
An atom
becomes ion. Ground state
1st excited state
2nd excited state
3rd excited state4th excited state
Free electronFigure 11.4
Line spectrum
The emission lines correspond to the photonsof discrete energies that are emitted whenexcited atomic states in the gas make
transitions back to lower energy levels.
Line spectrum
Figure below shows line spectra produced by
emission in the visible range for hydrogen
(H), mercury (Hg) and neon (Ne).
Figure 11.5
Hydrogen Spectrum
= 656, 486, 434, 410 & 397 nm, what is the pattern?
Hydrogen emission line spectrum
Emission processes in hydrogen give rise to series,which are sequences of lines corresponding toatomic transitions.
The series in the hydrogen emission line spectrumare
Lyman series involves electron transitions that end at the ground state of hydrogen atom. It isin the ultraviolet (UV) range.
Balmer series involves electron transitions thatend at the 1st excited state of hydrogen atom. It
is in the visible light range.
Hydrogen emission line spectrum
The series in the hydrogen emission linespectrum are
Paschen series involves electron transitions that end at the 2nd excited state of hydrogen atom. Itis in the infrared (IR) range.
Brackett series involves electron transitions that
end at the 3rd excited state of hydrogen atom. It isin the IR range.
Pfund series involves electron transitions that endat the 4th excited state of hydrogen atom. It is inthe IR range.
Figure below shows diagrammatically the
series of hydrogen emission line spectrum.
)eV(n E 0.0
54.085.0
51.1
39.3
6.13
n
4
3
2
1
5
Ground state
1st excited state
2nd excited state
3rd excited state4th excited state
Free electron
Lyman series
Balmer series
Paschen series
Brackett seriesPfund series
Stimulation 11.1
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in the Bohr model of a hydrogen atom.
Wavelength of hydrogen emission line
spectrum
If an electron makes a transition from an outer orbit oflevel ni to an inner orbit of level nf , thus the energy isradiated.The energy radiated in form of EM radiation(photon) where the wavelength is given by
hc E
hc
E 1
Wavelength of hydrogen emission line
spectrum
rd postulate, the eq. (11.13)
can be written as
hc E
hc
E 1
if
11nn E E
hcwhere
2
f 0
21
2f na
ke E n
and2
i0
21
2ina
ke E n
2
i0
2
2
f 0
21
2
1
2
11
na
ke
na
ke
hc
2i
2f 0
2 11
2
1
nna
ke
hc
2
i
2
f 0
211
2 nnhca
keand H R
hca
ke
0
2
2
2
i
2
f
111
nn R H
(11.14)
where17 m10097.1constantsRydberd': H R
nn of valuefinal:f
nn of valueinitial:i
Note: For the hydrogen line spectrum,
Lyman series( nf =1 )
Balmer series( nf =2 )
Paschen series( nf =3 )
Brackett series( nf =4 )
Pfund series( nf =5 )
To calculate the shortest wavelength in any series , take ni= .
2
i
2
1
1
11
n R H
2
i
2
1
2
11
n R H
2
i
2
1
3
11
n R H
2
i
2
1
4
11
n R H
2
i
2
1
5
11
n
R H
predicts successfully the energy levels of thehydrogen atom but fails to explain the energylevels of more complex atoms.
can explain the spectrum for hydrogen atom butsome details of the spectrum cannot be explainedespecially when the atom is placed in a magneticfield.
Magnetic field
Transitions
No magnetic field
1
2
Energy Levels
Spectra Figure 11.7
cannot explain the Zeeman effect
Zeeman effect is defined as the splittingof spectral lines when the radiatingatoms are placed in a magnetic field.
Magnetic field
Transitions
No magnetic field
1
2
Energy Levels
Spectra
24.4 X-ray
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Review: Atoms
Smallest particle of matter that has theproperties of an element.
Contains a small, dense, positively chargedcenter (nucleus).
Nucleus surrounded by a negative cloud ofelectrons.
Electrons revolve in fixed, well-defined orbits(energy levels).
Review: Atoms
3 Fundamental Particles of an Atom
Electron
Proton
Neutron
Atoms
Electrons can only existin certain shells thatrepresent electronbinding energies
K, L, M shells (K isclosest to the nucleus)
The closer an electronis to the nucleus, thehigher the bindingenergy (strength ofattachment to thenucleus).
AtomsIn their normal state, atoms are electrically
neutral
If an atom has an extra electron or has had an
electron removed, it has been ionized.
How X-rays are CreatedTo produce x-rays, you need 3 things:
1. A source of electrons
2. A force to move them rapidly
3. Something to stop them rapidly
*All 3 conditions met in an x-ray tube
Early X-ray Tube Early X-ray Tube
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The X-Ray tube is the single most important component of theradiographic system. It is the part that produces the X-rays
Wilhelm Conrad Röntgen (1845-1923)
A modern radiograph of a hand
History of X-ray and XRD
Wilhelm Conrad Röntgen discovered X-Rays in1895.1901 Nobel prize in Physics
Early use of X-Rays
Within few months of
their discovery, X-rays
were being put to
practical use.
This is an X-ray of bird
shot embedded in a
hand.
Unfortunately, much of
the early use of X-rays
was far too aggressive,
resulting in later cancer.
Section 9.4
History of X-ray and XRD
Radiographs like theones in the last slide are
simply shadowgrams.The X-rays either passstraight through or arestopped by the object.The diagram on theupper left illustrates theprinciple and shows aperfect shadow.
History of X-ray and XRDIn reality, a large fractionof the X-rays are notsimply absorbed ortransmitted by the objectbut are scattered. Thediagram on the bottomleft illustrates this effectand illustrates the fuzzyedge of the object that is
produced in the image bythe scattered X-rays.
Max von Laue (1897-1960)
History of X-ray and XRDThe first kind of scatter process to berecognised was discovered by Maxvon Laue who was awarded the Nobelprize for physics in 1914 "for hisdiscovery of the diffraction of X-raysby crystals". His collaborators WalterFriedrich and Paul Knipping took thepicture on the bottom left in 1912. Itshows how a beam of X-rays isscattered into a characteristic pattern
by a crystal. In this case it is coppersulphate.
Max von Laue (1897-1960)
History of X-ray and XRD
The X-ray diffraction pattern ofa pure substance is like afingerprint of the substance.The powder diffraction methodis thus ideally suited for
characterization andidentification of polycrystallinephases.
What are X-rays?
Beams of electromagnetic radiation
Short wavelength, high energy
Wave (sinusoidal, oscillating electric field with, at rightangles to it, a magnetic field)
wavelengthfrequency
Particle (photon)
Photon energy E E = h (h -34 Js)
Interacts
with
electrons!
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Properties of a wave
Wave = c / (c=300.000 km/s)
Electromagnetic radiation
Å (Ångström) is non-SI unit of length X-rays: 10-8 to 10-11 m1 Å = 10-10 m = 0.1 to 100 Å
0.1 nm dimension of atoms, bonds, unit-
X-Rays
Electromagnetic radiation with short
wavelengths
Wavelengths less than for ultravioletWavelengths are typically about 0.1 nm
X-rays have the ability to penetrate most
materials with relative ease
High energy photons which can break
chemical bonds danger to tissue
Discovered and named by Roentgen in 1895
X-Rays
X-rays (discovered and named
by Roentgen): electromagnetic
radiation with short typicallyabout 0.1 nm wavelengths
X-rays have the ability to
penetrate most materials with
relative ease
X-rays are produced when
high-speed electrons are
suddenly slowed down
Wilhelm Conrad Röntgen
1845 1923
How are X-rays generated? A. Radioactive materials undergo decay (too many
nuclear particles or too high neutron/proton ratio)
1532P -> 16
32S + X-ray
How are X-rays generated? A. Machines
X-ray tube (accelerates electrons which
interact with electrons of target)
Particle accelerator
e-
X-ray tube
1. W filament isheated, electrons
2. Electrons are
accelerated inelectric field
3. Electrons interactwith target (anode), producing X-rays
TungstenFilament
Target (Co, Cu)
Electron beam
X-rays
Two types of X-radiation are produced:
Bremsstrahlung radiation), produces a continuous spectrum of X-ray wavelengths
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Two types of X-radiation are produced:
2. Characteristic Radiation (X-rays of distinctwavelengths, unique for each element)
a) Incoming electronknocks inner shellelectron out of its
place b) Empty site is filled by
an electron from ahigher shell
Two types of X-radiation are produced:
2. Characteristic Radiation (X-rays of distinctwavelengths, unique for each element)
a) The difference in binding energy between inner andouter shell electrons
is released as X-rayof characteristicwavelength
Typical X-ray spectrum
Continuous radiation
= Bremsstrahlung
radiation
Characteristic radiation is
used in XRD, which
requires monochromatic
radiation
(eg. CuK = 1.5418 Å)
Production of X-rays
X-rays are produced
when high-speed
electrons are suddenly
slowed down
Can be caused by the
electron striking a
metal target
A current in the
filament causes
electrons to be emitted
Production of X-raysThese freed electrons
are accelerated toward
a dense metal target
The target is held at a
higher potential than the
filament
Production of X-rays (Bremsstrahlung) An electron passes near a
target nucleus and is
deflected from its path by its
attraction to the nucleus
This produces an acceleration
of the electron and hence
emission of electromagnetic
radiation
Production of X-rays (Bremsstrahlung)
If the electron loses all of its
energy in the collision, the
initial energy of the electron
is completely transformed
into a photon
The wavelength then is
max
min
hc e V h
min
hc
e V
Production of X-rays (Bremsstrahlung)
Not all radiation produced
is at this wavelength
Many electrons undergo
more than one collision
before being stopped
This results in the
continuous spectrum
produced
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Characteristic X-Rays
When a metal target is
bombarded by high-energy
electrons, x-rays are
emitted
The x-ray spectrum
typically consists of a broad
continuous spectrum and a
series of sharp linesThe lines are dependent
on the metal of the target
The lines are called
characteristic x-rays
Characteristic X-Rays
The details of atomic structure can be used to explaincharacteristic x-rays
A bombarding electron collides with an electron in thetarget metal that is in an inner shell
If there is sufficient energy, the electron is removedfrom the target atom
The vacancy created by the lost electron is filled by anelectron falling to the vacancy from a higher energy
levelThe transition is accompanied by the emission of aphoton whose energy is equal to the differencebetween the two levels
X-ray Spectrum
The x-ray spectrum has
two distinct components
1) Bremsstrahlung: a
continuous broad
spectrum, which depends
on voltage applied to the
tube
2) The sharp, intense lines,
which depend on the
nature of the target material
Production of Characteristic Radiation
The X-ray Production X-rays are emitted when high energy electrons or any
other charged particles bombard a metal target.
The X-ray spectrum typically consists of a broad
continuous band containing a series of sharp lines.
The continuous spectrum is a result of collision
between incoming electrons and the target atoms.
The sharp lines are a result of the removal of inner
shell electrons of the target atoms.
Possible Interaction Between Electron Beam
and the Target
The X-ray Spectrum Some Features of the Spectrum
The energy of Bremsstrahlung radiation range from
zero to a maximum value which depends on the
potential difference applied on the tube.
The intensity of the low energy photons within the
spectrum is reduced because the absorption of the
target material.
The average energy of the X-ray beam is about one
third of the maximum.
The sharp lines, K,L,M etc stay at the same positions.
The line X-ray can be produced only when the
incoming electrons exceed some values.
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31.2 X-ray diffraction
A modern Diffractometer
X-ray tube sample Detector
The X-ray diffractometer
Powder diffractometer with Bragg-Brentano geometry.
Analyst controls (choice of target in X-ray tube)
(positions of X-ray tube / sample / detector
n = 2 d sin
Experiment of Laue 1912
X-ray diffraction by a single crystal
What is X-ray diffraction?Scattering phenomenon, X-rays passing through
crystal
A tool for the characterisation of solid materials
based on their crystal structure
Used by
Earth Scientists
Chemists
Physicists
Material Scientists
Archaeologists
Rosalind E. Franklin 1952
What is XRD used for?Identification of minerals
Quantification of minerals
Determination of crystal structure
Unit-cell dimensions, symmetry, atom
Determination of grain sizes, strain
Typical samples
Minerals, rocks, corals, shells
What is X-ray diffraction?
XRD complements other analytical methods Visual
Need large crystals! cm
Optical microscopy (colour, birefringence,
µm to mm
SEM (composition: wt.% SiO2 What about polymorphs? (Calcite, Aragonite= CaCO3)
> 3 µm
XRF (composition: wt.% SiO2
What about polymorphs? (Calcite, Aragonite= CaCO3)
Interaction of X-rays with crystal structures
Crystal structure:
three-dimensional, periodic arrangement
of atoms in space.
Many different layers of atoms exist in a crystal
structure.
Each set of layers has a distinct interplanar distance
(d-spacing).
Unit-cell of NaCl
Cl Na
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Interaction of X-rays with crystal structures
X-rays (electromagnetic wave) interact with the electrons
of the atoms in the crystal
Coherent Scatter : elastic collision between a photon (X-
ray) and and electron (in crystal)
- outgoing photons (X-ray) have same wavelength,
frequency and energy as incoming photons [XRD!]
Incoherent Scatter (= Compton scatter): inelastic collision
between photon and electron
- outgoing photons have lower energy
Interaction of X-rays with a scattering center
Every electron/atom in structure acts as a
scattering center, and is a source of spherical
waves of the same wavelength and frequency as
the incoming wave.
Incoming wave
+
+
-
-
Interference
Positive Negative
Interference Interference
Crests and troughs add up and
form a wave with twice the
amplitude.
Crests and troughs are offset
and cancel each other out.
This happens to most X-rays
scattered in crystals due to the
large number of scattering
centers ...
X-rays passing through a crystal lattice
X-rays
out of phase!
Diffraction
some X-rays to experience positive (or
constructive) interference in crystals. This is
called diffraction.
radiation coherently, the concerted
constructive interference at specific angles is
called diffraction
Diffraction in crystalline materials is best
described with= 2 dhkl sin
X-rays
in phase!
dhkl
For positive interference to occur, the path-difference must be equal to one wavelength ( or multiple wavelengths
(n .
n = 2 dhkl
sin
hkl
Diffraction of X-rays by Crystals
For diffraction to occur,the spacing between thegrooves must beapproximately equal tothe wavelength of theradiation to be measured
For X-rays, the regulararray of atoms in a crystalcan act as a three-dimensional grating fordiffracting X-rays
Schematic for X-ray Diffraction
A beam of X-rays with acontinuous range ofwavelengths is incident on thecrystal
The diffracted radiation is veryintense in certain directions
These directionscorrespond to constructive
interference from wavesreflected from the layers ofthe crystal
The diffraction pattern isdetected by photographic film
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Photo of X-ray Diffraction Pattern
The array of spots is called a
Laue pattern
The crystal structure is
determined by analyzing the
positions and intensities of the
various spots
This is for NaCl
The beam reflected from thelower surface travels fartherthan the one reflected fromthe upper surface
If the path difference equalssome integral multiple of thewavelength, constructiveinterference occurs
gives theconditions for constructiveinterference
Constructive interference: 2dsin m
d 0.5nm in NaCl
For =.017nm
X-ray
d
1st maximum will be at 100
X-Ray Diffraction
Crystal solid such
as sodiumdsin
Bragg Equation
sin = (n )/2d
= angle of incidence
= wavelength
d = interplane distance of crystal
Bragg Equation
Incident angle
Reflected angle
Wavelength of X-ray
Total Diffracted
Angle
2
2
When the X-rays strike a layer of a crystal, some of
them will be reflected. We are interested in X-rays
that are in-phase with one another. X-rays that add
together constructively in x-ray diffraction analysis
in-phase before they are reflected and after they
reflected.
The line CE isequivalent
to the distancebetween the twolayers (d)
Bragg EquationThese two x-ray beams travel slightly different
distances. The difference in the distances traveled is
related to the distance between the adjacent layers.
Connecting the two beams with perpendicular lines
shows the difference between the top and the
bottom beams.
sin E d
sin EF d
The length DE is the same as EF, so the totaldistance traveled by the bottom wave is expressedby:
Constructive interference of the radiation fromsuccessive planes occurs when the path differenceis an integral number of wavelenghts. This is theBragg Law.
sin DE d
2 sin DE EF d
2 sinn d
Bragg Equation
nd sin2
where, d is the spacing of the planes and n is theorder of diffraction.
Bragg reflection can only occur for wavelength
This is why we cannot use visible light. No diffractionoccurs when the above condition is not satisfied .
The diffracted beams (reflections) from any set oflattice planes can only occur at particular anglespradicted by the Bragg law.
d n 2
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Arthur Holly Compton
1892 1962
Discovered the Comptoneffect
Worked with cosmic rays
Director of the lab at U ofChicago
Shared Nobel Prize in 1927
The Compton Effect
Compton directed a beam of x-rays toward a block ofgraphite
He found that the scattered x-rays had a slightlylonger wavelength that the incident x-rays
This means they also had less energy
The amount of energy reduction depended on theangle at which the x-rays were scattered
The change in wavelength is called the Compton shift
Compton Scattering
Compton assumed the photons acted like otherparticles in collisions
Energy and momentum were conserved
The shift in wavelength is
(1 cos )o
e
h
m c
Compton Scattering
The quantity h/mec is called the Compton wavelength
Compton wavelength = 0.002 43 nm
Very small compared to visible light
The Compton shift depends on the scattering angleand not on the wavelength
Experiments confirm the results of Comptonscattering and strongly support the photon concept
Three-Dimensional Conformal Radiation
Therapy (3D-CRT)
Tumors usually have an irregularshape
Three-dimensional conformalradiation therapy (3D-CRT) usessophisticated computers and CTscans and/or MRI scans to createdetailed 3-D representations ofthe tumor and surroundingorgans
Three-Dimensional Conformal Radiation
Therapy (3D-CRT)
Radiation beams are thenshaped exactly to the size andshape of the tumor
Because the radiation beams are very precisely directed, nearbynormal tissue receives lessradiation exposure
Sample
We are choosing incoming angle =
outgoing angle.
Therefore only diffraction from
atomic planes in the crystal
structure that are parallel to the flat
sample surface are detected
For example, if we analysed this
single muscovite crystal with XRD,
lying flat on the sample holder with
its 001 plane, only (001) planes
would diffract.
muscovite
(001)
sample
Powder X-ray Diffraction
Sample
However, we want ALL
crystallographic planes to
contribute to the XRD pattern.
All samples need to be ground
up very finely (ideally 1-10 µm
grain size), and the grainsoriented randomly in the
sample holder.muscovite
(001)
sample
Powder X-ray Diffraction
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24.5 Nanoscience
Nanoscience refers to the ability to manipulateindividual atoms and molecules, making itpossible to build machines on the scale ofhuman cells.
Nanotechnology
Nanotechnology is the understanding andcontrol of matter at dimensions of roughly 1 to100 nanometers.Nanotechnology involves imaging, measuring,modeling, and manipulating matter at thislength scale.
Nanoscale
At the nanoscale, the physical, chemical, andbiological properties of materials differ infundamental and valuable ways from the
properties of individual atoms and molecules orbulk matter.Nanotechnology R&D is directed towardunderstanding and creating improvedmaterials, devices, and systems that exploitthese new properties
Facts
A nanometer is one billionth of a meter.In 2005 the US government spent an estimated$1,081 million
While difficult to measure accurately, somehave estimated that worldwide governmentfunding has increased to about five times whatit was in 1997, exceeding $2 billion in 2002.
CMOS TECHNOLOGY
Introduction178
(released March 2004):
150 million transistors
90 nm design rules
3.4 GHz clock frequency
DRAM chips:
4 Gb chips demonstrated
(~ 109 transistors/cm2)
- 130 nm) processor
Now chips based on thedesign rules of 22 nm are onthe way.
In 2004 we were already inside nanotechnology!
One area of nanotechnology R&D is medicine.Medical researchers work at the micro- andnano-scales to develop new drug deliverymethods, therapeutics and pharmaceuticals.For a bit of perspective, the diameter of DNA,our genetic material, is in the 2.5 nanometer
range, while red blood cells are approximately2.5 micrometers.
Applications/Products
-
limited), nanoparticles are being used in anumber of industries. Nanoscale materials areused in electronic, magnetic andoptoelectronic, biomedical, pharmaceutical,
cosmetic, energy, catalytic and materialsapplications. Areas producing the greatestrevenue for nanoparticles reportedly arechemical-mechanical polishing, magneticrecording tapes, sunscreens, automotivecatalyst supports, biolabeling,
Nanotechnology has thepotential to profoundlychange our economy and toimprove our standard ofliving, in a manner not unlikethe impact made by advances
over the past two decades byinformation technology. It isquite possibly the next step intechnology that will lead togreat innovations. If thecapabilities of nanoscience arefully harnessed, anythingcould be possible.
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Numerous products featuring the uniqueproperties of nanoscale materials are availableto consumers and industry today. Mostcomputer hard drives, for instance, containgiant magnetoresistance (GMR) heads that,through nano-thin layers of magneticmaterials, allow for a significant increase in
storage capacity. Other electronic applicationsinclude non-volatile magnetic memory,automotive sensors, landmine detectors andsolid-state compasses
Nanomaterials
Examples are nanoscale particles, tubes androds.
Nanotube
Nanoparticles
Nanorods
Some other uses
Burn and wounddressings Water filtration
Catalysis A dental-bondingagentStep assists on vans.Coatings for easiercleaning glassBumpers andcatalytic converterson cars
Protective and glare-reducing coatings foreyeglasses and cars
Sunscreens andcosmetics.Longer-lasting tennisballs.Light-weight,stronger tennisracquets.Stain-free clothingand mattresses.Ink.
Medical uses
The pharmaceutical and chemical industries arebeing impacted greatly by nanotechnology, as well. New commercial applications ofnanotechnology that are expected in two to five years in these industries include:advanced drug delivery systems, includingimplantable devices that automaticallyadminister drugs and sensor drug levels andmedical diagnostic tools, such as cancer taggingmechanisms.
Bibliographyhttp://www.nsf.gov/news/overviews/nano/index.jsp http://www.nanoscience.com/education/index.html http://www.nsf.gov/discoveries/index.jsp?prio_area=10