lecture3 pol mechnism
TRANSCRIPT
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Electronic polarization
343
V RT!
For calculating the effect of electronic polarization,
We consider an idealized atomwith perfect spherical
symmetry. I
t has a point likecharge + ze in the nucleus, andThe exact opposite charge zehomogeneously distributed inthe volume of the atom, whichis
with R= radius of the atom
Ques: Density of electrons?
Ques: Lorentz force = coulomb force =?
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The density of electrons (Charge/Volume of atom) is then
In the presence of an electric field E;
Lorentz force: F1=-zeE acts on charges.
The positive charge in the nucleus and the center of thenegative charges from the electron "cloud" will thusexperience forces in different direction and will become
separated.We have the idealized situation shown in theimage in last slide.
33
4
z e
RV
T!
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The attractive force (between opposite charges)
F2 is given by
2 2
0
2
30
3 3
3 3
(charge of nucleus)(negative charge encolesd in sphere of radius d)
4
( )
4
negative charge encolesd in sphere of radius d
4 3 d= ze
4 3 R
Fd
ze
dR
zed
R
TI
TI
T
T
!
!
!
Q
* Q= charge density x volume
--
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Equating F1 and F2 we have equilibrium distance dE as
Therefore the induced dipole moment is
As polarization is dipole moment per unit volume so
And Electronic Polarizability:
3
0
3
0
4 and
P4
P NR E
NR
E
TI
G T
I
!
!
3
04
Ezed R EQ TI! !
304
E
R Ed
ze
TI!
3
04
.
R
E
e
TIE
EQ
!
! Where e is defined byElectronic polarizability.Ques: What is the Dimension
of Polarizability?
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P = NEeE = Io(Ir-1)E
This gives
Io(Ir-1) = NEe
Here N is the number of dipoles per unit volume.
There are a number of interesting points about the
last result:1. We have justified the "law" of a linear relationship
between E and P for the electronic polarizationmechanism (sometimes also called inducedpolarization).
2. We can easily extend the result to a mixture of different atoms: All we have to do is to sum over therelative densities of each kind of atom.
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3
0
3
0
4 and
= 4
P NR E
NRE
TI
TI
!
!
We can easily get an order of magnitude for .
Taking a typical density ofN
x 10
25
m
3
andR6 x 10 12 m, we obtain G8.14 x 105,
and r=1. 000 0814
Note:
1. The values ofmolecular dipole moments are usually
expressed in Debye units(3.3 x10-30 Cm). The Debye unit,
abbreviated as D, equals 10-18 electrostatic units (e.s.u.).
2. The permanent dipole moments of non-symmetricalmolecules generally lie between 0.5 and 5D.
3. In the case ofpolymers and biopolymers one can meet
much higher values ofdipole moments ~ hundreds or
even thousands of Debye units.
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2.Ionic polarization
Consider a simple ioniccrystal, e.g. NaCl.
Each Na+ - Cl pair is a naturaldipole, no matter how you pair up two atoms.
The polarization of a givenvolume, however, is exactlyzero because for every dipolemoment there is a neighboring
one with exactly the samemagnitude, but opposite sign.
Note that the dipoles can notrotate; their direction is fixed.
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In an electric field, theions feel forces in
opposite directions.
For a field acting asshown, the lattice distortsa little bit (hugelyexaggerated in thedrawing)
The Na+ ions moved a bitto the right, the Cl ionsto the left.
The dipole momentsbetween adjacent NaCl -
pairs in field direction arenow different and there isa net dipole moment ina finite volume now.
Ques: How large is d?
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How large is d?
The force F1 increasing the distance is given by
F1 = q E
with q = net charge of the ion.
The restoring force F2: ford
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Other relations
2
0
2
0
r
and
NqP .
Find out and
q EYd
E
Yd
Q
I
!
Exercise:
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Summary: Ionic polarization
0
qEd
Yd!
2
02
0
r
and
q= .
ind out and
q E
Yd
E
Yd
Q
I
!
Net Displacement:
In the presence of E:
Dipole moment:
Polarization:
00
2
0 Yd
Nq
E
P
IIG !!
And r= (G+1)
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Orientation Polarization In the case of Orientation polarization (sometime called Dipolar
polarization) we have a material with built-in dipoles that areindependent of each other, i.e. they can rotate freely- in sharp contrastto ionic polarization.
The prime example is liquid water, where every water molecule is a little dipole that can have any orientation
with respect to the other molecules.
Moreover, the orientation changes all the time because the molecules
moves! (O
rientation polarization for dielectric dipoles thus is pretty muchlimited to liquids)
It is like a snapshot (2D) with a very, very short exposure time. A fewnanoseconds later the same piece of water may look totally different indetail, but pretty much the same in general.
In a three-dimensional piece of water the blue and green circles would nothave to be in the same plane; but that is easy to imagine and is difficult to
draw
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Orientation polarization: visualize it
in water Water molecules that form natural dipoles.
because the negatively charged oxygen atom and the two positivelycharged H - atoms have different centers of charge.
Each molecule carries a dipole moment which can be drawn as a vectorof constant length.
If we only draw a vector denoting the dipole moment, we get - in two
dimensions - a picture like this:
The sum of all dipole moments will be zero, if the dipoles arerandomly oriented.
If we now introduce a field E, the dipoles would have a tendency toturn into the field because that would lower their energy.
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The dipoles are not sitting still, but moving around and rotating allthe time - because they contain thermalenergy and thus also someentropy.
The electrical field induces average orientation in field direction. Most of the time an individual dipole points in all kinds of directions.
The "real" picture (in the sense of a snapshot with a very short exposuretime) looks like this:
The orientation of all dipoles is just a little bit shifted so that anaverage orientation in field direction results. In the picture, the effectis even exaggerated!
With out FieldW
ithF
ield
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Energy of a dipole in Electric field:
Consider a Polar moleculewhich caries a permanent
dipole moment (qd, like
water molecule) is placed in an
electric field E.
The Potential energy is givenby;
U= -.E=- Ecos()
E
+q(1)
(2)-q
d
cos( )EUkT kT
e e
Q U
!
In thermal equilibrium the relative number of molecules with the potentialenergy Uis proportional to (Boltzmann statistics)
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Number ofdipoles in a solid angle:
Let n() be the number of dipoles per unit solid angle at
, we have
The number of dipoles in a solid angle d;
co s ( )
0( ) .
E
k Tn n eQ U
U !
0
cosexp( )2 sin
En d
kT
Q UT U U
Note:Where d;! r.dS/r3
Can be calculated
as follows:
********************************************************************************************
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Average Dipole Moment The average dipole moment in an electric field is the net moment
of the assembly divided by the total numberof dipoles
Therefore,
00
00
exp( cos / )2 sin ( cos )
exp( cos / )2 sin
n E kT d
n E kT d
T
T
Q U T U Q U UQ
Q U T U U "!
cosE xk
Q U !where and E akQ !
L(a)L(a)is calledLangeven functionLangeven function
cos
0
cos
0
1cos sin
2 1
1sin
2[ ]1 1 1
cot ( ),[ ]
aE
xk
a
aE
xk
a
x x a a a
a
x a a a
a
e d e xdx
ae d e dx
xe e e eanha L a
a e e e a a
T Q U
T Q U
U U UQ
QU U
"! ! !
! ! ! !
Coth(a)
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....453
1
)(
3
!
aa
aaCoth
kT
Ea
where
aPP
aNN
a
so
vv
.
)(.
)(..
)(.
Q
QQ
QQ
!
!
!
!Where Ps is saturation polarization and
Po is orientation Polarization.
y=1/3a
0 1 2 4 5 6 7 80.0
0.2
0.4
0.6
0.8
1.0 y=1
y=L(a)
a
y
Langevin
In Fig. the angeven unction L(a)L(a) is
plotted against aa.
L(a)L(a) has a limiting value 11, which was to
be expected since this is the maximum o
coscosUU..
Case I: when a is very high : at Low Temp;
a>>1 L(a)=1, Po = Ps
Case II: when a is very ow: at high Temp;
a
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TkT
Hence
ENP
and
kT
ENP
oo
voo
v
o
1
3
3
2
2
w!
!
!
EQ
E
E
QOrientation Polarization
Orientation Polarizability
OrDipolar Polarizability
Note: Derivation shows that tendency o the extended ield toalign the dipoles is contracted by thermal motion resulting in a
decreasing value o Po with increasing T
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Total Polarizability of Polyatomic Gas:
P = Pe+ Pi + Po
P = NEe + NEi + NEo= 0 (r - 1) E
Hence
(r - 1) = =N./ 0
Where is called Total Polarizabilty
kie
3
2
QEEE !
Is knownas Langevin- DebyeEquation