Measurement and modeling of hydrogenic retention in molybdenum with the DIONISOS experiment
Chem 373- Orbitals of Hydrogenic Atom
Transcript of Chem 373- Orbitals of Hydrogenic Atom
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The orbitals for the hydrogenic atom are given by
(r, , ) R(r)nlYl,m( , ) ; n = 1, 2, 3 ...
l < n - 1; m = - l, - l+1, ....l - 1, l
and Rnl solution to
h
2
2{
2
Rnl(r)2r
2r
Rnl(r)r
) { Ze4 or
h
2
l(l 1)2 mr2
}Rnl(r) EnRnl(r)
Where
( , ) = Yl,m(( , ) =2l+1
4
(l | m! |
(l | m!|)
Pl|m| (cos ) exp[im ]
are eigenfunctions to L2 and Lz
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Hydrogen Levels
R1,0(r) 2Z
ao
3 / 2
e / 2
n 1, l = 0
n,l,m ( , ) = Rnl(r)Yl,m(( , )
R1,0(r) 2Z
ao
3 / 2
e / 2
No nodes. R1,0
(r) everywhere positive
For l = 0 we have m = 0;
Yo,o1
4
Value of Yoo is uniform over
sphere
1s orbital
O bi l f H d i A
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The balance of kinetic and potentialenergies that accounts for thestructure of the ground state ofh dro en (and similar atoms).
(a) The sharply curved but localizedorbital has high mean kinetic energy,but low mean potential energy
(b) the mean kinetic energy is low,but the potential energy is not very
favourable;
; (c) the compromise of moderatekinetic energy and moderatelyfavourable potential energy.
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R20 (r)1
2 2
Z
ao
3 / 2
(21
2)e / 4
n no, l = 0
n,l,m ( , ) = Rnl(r)Yl,m(( , )
R30 (r) 19 3
Zao
3 / 2
(6 2 19
2 )e / 6
One node at
(21
2) 0
with = 2Zr/ao; node : 2a
o
/ Z
two nodes at
(6 21
9
2
) 0
with = 2Zr/ao; nodes : 1.9ao / Z
and 7.1Zr/ao
For l = 0 we have m = 0;
Yo,o1
4
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n no, l = 0
no ,o,o( , ) = Rno ,o (r)Yo,o(( , )
Thus any two s - orbitals Rn'oYoo and RnoYoomust be orthorgonal
Rn'oYoo000
2Rn'oYoodv 0
Why has Rnl(r) n-1 nodes ?
We have seen previously that
any two independent solutions
to the Schrdinger equation must
be orthogonal :
i jdv ij
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Rn'oYoo000
2
Rn'oYoodv 0
Yoooo
2
Yoo sin d d Rn'oo
r
(r)Rno(r)r2dr 0
1 Rn'oo
r
(r)Rno(r)r2dr 0
Yoo normalized
The R1o function is positive
every where
R1,0(r) 2Z
ao
3 / 2
e / 2
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Thus for R2o to be orthogonal
to R1o
R1oo
r
(r)R 2o (r)r2dr 0
R20 must have positive and
negative regions
R20 (r)1
2 2
Z
ao
3 / 2
(21
2)e / 4
For R3o to be orthogonal to
R1o and R20 two nodes arerequired etc...
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The probability density
Pnlm(r, , ) = nlmr, , ) nlmr, , )
A constant-volume electron-sensitive
detector (the small cube) gives its greatest
reading at the nucleus, and a smallerreading elsewhere. The same reading is
obtained anywhere on a circle of given
radius: thes orbital is spherically
symmetrical.
P1,00 (r, . ) 2Z
ao
3 / 2
e / 2Yoo
2
Z
ao
3 / 2
e/ 2
Yoo1 Z
ao
3
e
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Representations of the1s and 2s hydrogenic
atomic orbitals in termsof their electron densities(as represented by thedensity of shading).
The probability densityPnlm(r, , ) = nlmr, , ) nlmr, , )
P1,00 (r)1 Z
ao
3
e
P2o0 (r)1
32
Z
ao
3
(21
2)2 e / 2
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e1
e2
e3
e4
e5
Orbitals of Hydrogenic Atom An asideHow do we plot Ylm ?
Consider a unit sphere
withradius 1. Draw a large
number ofunit vectors fromthe origin ofthe sphere in
different directions
(e.i. different , )re1 ,
re2,
re3,
re4 ...ren
Calculate the value of Ylm( , )
at the position of eachren
(e.i for each n, n). Constructthe vectors : R1 , R2, R3,..Rn
where :rRn
renYlm( , )
Draw Rn
R2
R3
1R
R4
R5
O bi l f H d i A A id
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Orbitals of Hydrogenic Atom An aside
R2
R
31
R
R4
R5
Draw a surface through the
endpoints of all rRn .
This surface represents Ylm( , )
O bit l f H d i At An aside
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Orbitals of Hydrogenic Atom An aside
For Yoo( , ) we have
rRn
1
2
ren for all n
We have that Yoo( , ) is spherical
e.u. the same for all n, n
THus Yoo representing the angular
part of a ns function is representedby a sphere
ns - orbital
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The boundary surface of an s orbital,within which there is a 90 per cent
probability of finding the electron.
Orbitals of Hydrogenic Atom M di
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The variation of the mean radius of a
hydrogenic atom with the principal and
orbital angular momentum quantum
numbers. Note that the mean radius lies inthe order d p sfor a given value ofn.
Mean radius
The mean radius is given as the
espectation value
r nlmr nlmdv
For the hydrogenic atom
< r >nl n2 1
1
2(1
l(l 1)
n2aoZ
O bit l f H d i At
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A constant-volume electron-sensitive
detector (the small cube) gives its greatest
reading at the nucleus, and a smaller
reading elsewhere. The same reading is
obtained anywhere on a circle of given
radius: the s orbital is spherically
symmetrical.
P1,00 (r, . ) 2Z
ao
3 / 2
e / 2Yoo
2 Z
ao
3 / 2e / 2Yoo
1 Z
ao
3e
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The radial distribution function
P gives the probability that the electron
will be found anywhere
in a shell of radiusr. For a 1s
electron in hydrogen,P is a
maximum whenr is equal to
the Bohr radiusa0. The value
ofP is equivalent to the readingthat a detector shaped like a
spherical shell would give as
its radius was varied.
Orbitals of Hydrogenic Atom Radial probability density
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The probability of finding the electron
between r and r + dr is :
Pnl(r)dr Pnlm(r, , )dvoo
2
P
nlm
(r, , )rsin d d r2droo
2
|Rnl((r) |2 Ylm( , ) |
2 sin d d r2droo
2
1 |Rnl
((r) |2 r2dr
Thus the radial probability density is
Pnl(r) | Rnl((r)|
2
r
2
Radial probability density
Orbitals of Hydrogenic Atom Radial probability density
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The radial probability density is
Pnl(r) | Rnl((r)|2 r2
The most probable radius corrsponds
to the maxima for Pnl(r).
For 1s
rraoZ
Radial probability density
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Orbitals with increasing l are called
n1m Rn1(r)Y1m ( , ) p - orbitals m = -1,0,1
n2m Rn2(r)Y2m( , ) d - orbitals m = - 2, -1, 0,1,2
n3m Rn3(r)Y3m( , ) f - orbitals m = - 3, -2, -1,0,1, 2, 3
Orbitals of Hydrogenic Atom
Structure of Hydrogenic Atoms
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Orbitals of Hydrogenic AtomStructure of Hydrogenic Atoms
Rnl is a solution to
h2
2
{2Rnl(r)
2
r
2
r
Rnl(r)
r
) {Ze
4 or
h2l(l 1)
2 mr2
}Rnl(r) ERnl(r)
Veff
As l increases the ve centrigugal termh
2l(l 1)
2 mr2
becomes more repulsive near nucleus at small r.Hence Rnl(r) tend to zero as r o with increasing
spead as l becomes larger
Structure of Hydrogenic Atoms
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Structure of Hydrogenic Atoms
R1,0(r) 2Z
ao
3 / 2
e Zr/r
R21(r)1
2 6
Z
ao
5 / 2
reZr / 2ao
R3,2 (r)4
81 30
Z
ao
7 / 2
r2eZr / 4ao
for r o ; 1s 2Z
ao
3 / 2
for r o ; 2p r
for r o ; 3p r2
The asymptotic behaviour of the radial s,p, and d functions
differ as a result of the centrifugal term in the radial Schrdinger
equation
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Close to the nucleus,p orbitals are proportional to r,d orbitals are proportional to r2,and f orbitals are proportional to r3.Electrons are progressively excludedfrom the neighbourhood of the nucleusas l increases. An s orbital has a
finite, nonzero value at the nucleus.
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nlm(r, , ) R(r)
nlY
l,m( , )
n = 2 , l = 1
211(r, , ) R(r)21Y1,1( , ) = -R(r)213
8
1/ 2
sin ei
m 1,0,1
210(r, , ) R(r)21Y1,0( , ) = R(r)213
4
1/ 2
cos
21 1(r, , ) R(r)21Y1,-1( , ) = R(r)213
8
1/2
sin e i
Let us now look at the angular part of the p- functions
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211(r, , ) -R(r)213
8
1/ 2
sin ei
Orbitals of Hydrogenic Atom
x
y
z
L2
h2l(l 1)
Lz hml
x
yz
r v
vL
vr
vv
l = 1 , m = 1
The electron has an angular momentumrL
such that L L = h2l(l 1)
The z - component ofsL is Lz h
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210(r, , ) = R(r)213
4
1/ 2
cos l = 1 , m = 0
x
y
z
L2
h2l(l 1)
Lz hml
m=0
The electron has an angular momentum rL
such that L L = h2l(l 1)
The z - component ofsL is Lz o
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21 1(r, , ) = R(r)213
8
1/ 2
sin e i l = 1, m = -1
x
yz
L
2
h
2
l(l 1)
Lz hml
m=-1
The electron has an angular momentum rL
such that L L = h2l(l 1)
The z - component ofsL is Lz h
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Plotting angular part of
210(r, , ) = R(r)213
4
1/ 2
cos 2pz
R k cos
+
-
Draw vectorrR of length
kcos through each point
( , ) on sphere
Draw surface through allvectors R
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211(r, , ) -R(r)213
8
1/2
sin [cos isin ]
21 1(r, , ) = R(r)213
8
1/ 2
sin [cos isin ]
The remaining two orbitals are complex
However by linear combinations we can get the real orbitals
2pyi
2{ 211 + 21 1} = R(r)21
3
8
1/2
sin sin
2px1
2{ 211 - 21 1} = R(r)21
3
8
1/ 2
sin cos
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2pyi
2{ 211 + 21 1} = R(r)21
3
8
1/2
sin sin
2px1
2{ 211 - 21 1} = R(r)21
3
8
1/ 2
sin cos
The orbitals 2px and 2py have the same energies and eigenvalues to
L2 as 211 and 21-1 . However only the latter are eigenfunctions of Lz
+
-
x
z
+-
y
2py 2px
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The boundary surfacesof p orbitals. A nodalplane passes throughthe nucleus and
separates the two lobesof each orbital.The dark and light areas denoteregions of opposite sign
of the wavefunction.
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A Grotrian diagram that summarizes the
appearance and analysis of the spectrum of
atomic hydrogen. The thicker the line, the
more intense the transition.
In transitions between
different energy levels of
the hydrogenic atomthe following selection
rules apply
l = 1m = o, 1