Lectures 3-4: One-electron atoms

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Lectures 3-4: One-electron atomsLectures 3-4: One-electron atoms

o Schrödinger equation for one-electron atom.

o Solving the Schrödinger equation.

o Wavefunctions and eigenvalues.

o Atomic orbitals.

o See Chapter 7 of Eisberg & Resnick.

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Ψ=Ψ(x,y,z, t)

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The Schrödinger equationThe Schrödinger equation

o One-electron atom is simplest bound system in nature.

o Consists of positive and negative particles moving in 3D Coulomb potential:

o Z =1 for atomic hydrogen, Z =2 for ionized helium, etc.

o Electron in orbit about proton treated using reduced mass:

o Total energy of system is therefore,

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μ =mM

m + M

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V = V (x,y,z) =−Ze2

4πε0 x 2 + y 2 + z2

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KE + PE = E

1

2μ( px

2 + py2 + pz

2) + V (x,y,z) = E

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o Using the Equivalence Principle, the classical dynamical quantities can be replaced with their associated differential operators:

o Substituting, we obtain the operator equation:

o Assuming electron can be described by a wavefunction of form,

can write

or

where, is the Laplacian operator.

€

px → −ih∂

∂x, py → −ih

∂

∂y, pz → −ih

∂

∂z

E → ih∂

∂t

€

−h2

2μ

∂ 2

∂x 2+

∂ 2

∂y 2+

∂ 2

∂z2

⎛

⎝ ⎜

⎞

⎠ ⎟+ V (x,y,z) = ih

∂

∂t

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Ψ=Ψ(x,y,z, t)

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−h2

2μ

∂ 2Ψ(x,y,z ,t)

∂x2+

∂ 2Ψ(x,y,z ,t)

∂y2+

∂ 2Ψ(x,y,z ,t)

∂z 2

⎛

⎝ ⎜

⎞

⎠ ⎟+V(x,y,z )Ψ(x,y,z ,t) = ih

∂Ψ(x,y,z ,t)

∂t

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−h2

2μ∇ 2Ψ + VΨ = ih

∂Ψ

∂t

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∇2 =∂ 2

∂x 2 +∂ 2

∂y 2 +∂ 2

∂z2

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o Since V(x,y,z) does not depend on time, is a solution to the Schrödinger equation and the eigenfunction is a solution of the time-independent Schrödinger equation:

o As V = V(r), convenient to use spherical polar coordinates.

where

o Can now use separation of variables to split the partial

differential equation into a set of ordinary differential equations.

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Ψ(x, y,z, t) =ψ (x, y,z)e−iEt / h

€

−h2

2μ∇ 2ψ (x,y,z) + Vψ (x, y,z) = Eψ (x,y,z)

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−h2

2μ∇ 2ψ (r,θ,φ) + V (r)ψ (r,θ,φ) = Eψ (r,θ,φ)

€

∇2 =1

r 2

∂

∂r(r 2 ∂

∂r)+

1

r 2 sinθ

∂

∂θ(sinθ

∂

∂θ)+

1

r 2 sin2θ

∂ 2

∂φ 2

(1)

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ψ(x, y,z)

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Separation of the Schrödinger equationSeparation of the Schrödinger equation

o Assuming the eigenfunction is separable:

o Using the Laplacian, and substituting (2) and (1):

o Carrying out the differentiations,

o Note total derivatives now used, as R is a function of r alone, etc.

o Now multiply through by and taking transpose,

(2)

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ψ(r,θ,φ) = R(r)Θ(θ)Φ(φ)

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−h2

2μ

1

r2

∂

∂rr2 ∂RΘΦ

∂r

⎛

⎝ ⎜

⎞

⎠ ⎟+

1

r2 sinθ

∂

∂θsinθ

∂RΘΦ

∂θ

⎛

⎝ ⎜

⎞

⎠ ⎟+

1

r2 sin2 θ

∂ 2RΘΦ

∂φ2

⎡

⎣ ⎢

⎤

⎦ ⎥+ V (r)RΘΦ = ERΘΦ

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−h2

2μ

ΘΦ

r2

∂

∂rr2 dR

dr

⎛

⎝ ⎜

⎞

⎠ ⎟+

RΦ

r2 sinθ

∂

∂θsinθ

dΘ

dθ

⎛

⎝ ⎜

⎞

⎠ ⎟+

RΘ

r2 sin2 θ

d2Φ

dφ2

⎡

⎣ ⎢

⎤

⎦ ⎥+ V (r)RΘΦ = ERΘΦ

€

−2μr2 sin2 θ /RΘΦh2

€

1

Φ

d2Φ

dφ2= −

sin2 θ

R

d

drr2 dR

dr

⎛

⎝ ⎜

⎞

⎠ ⎟−

sinθ

Θ

d

dθsinθ

dΘ

dθ

⎛

⎝ ⎜

⎞

⎠ ⎟−

2μ

h2r2 sin2 θ[E −V (r)] (3)

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Separation of the Schrödinger equationSeparation of the Schrödinger equation

o As the LHS of Eqn 3 does nor depend on r or and RHS does not depend on their common value cannot depend on any of these variables.

o Setting the LHS of Eqn 3 to a constant:

and RHS becomes

o Both sides must equal a constant, which we choose as l(l+1):

o We have now separated the time-independent Schrödinger equation into three ordinary differential equations, which each only depend on one of (4), (5) and R(6). .

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1

Φ

d2Φ

dφ2= −ml

2 =>d2Φ

dφ2= −ml

2Φ (4)

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−1

R

d

drr2 dR

dr

⎛

⎝ ⎜

⎞

⎠ ⎟−

1

Θsinθ

d

dθsinθ

dΘ

dθ

⎛

⎝ ⎜

⎞

⎠ ⎟−

2μ

h2r2[E −V (r)] = −

ml2

sin2 θ

€

=>1

R

d

drr2 dR

dr

⎛

⎝ ⎜

⎞

⎠ ⎟+

2μr2

h2[E −V (r)] =

ml2

sin2 θ−

1

Θsinθ

d

dθsinθ

dΘ

dθ

⎛

⎝ ⎜

⎞

⎠ ⎟

€

− 1

sinθ

d

dθsinθ

dΘ

dθ

⎛

⎝ ⎜

⎞

⎠ ⎟+

ml2Θ

sin2 θ= l(l +1)Θ

1

r2

d

drr2 dR

dr

⎛

⎝ ⎜

⎞

⎠ ⎟+

2μr2

h2[E −V (r)]R = l(l +1)

R

r2

(5)

(6)

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Summary of separation of Schrödinger equationSummary of separation of Schrödinger equation

o Express electron wavefunction as product of three functions:

o As V ≠ V(t), attempt to solve time-independent Schrodinger equation.

o Separate into three ordinary differential equations for and .

o Eqn. 4 for () only has acceptable solutions for certain value of ml.

o Using these values for ml in Eqn. 5, () only has acceptable values for certain values of l.

o With these values for l in Eqn. 6, R(r) only has acceptable solutions for certain values of En.

o Schrödinger equation produces three quantum numbers!

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ψ(r,θ,φ) = R(r)Θ(θ)Φ(φ)

€

R(r),Θ(θ)

€

(φ)

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Azimuthal solutions (Azimuthal solutions ((())))

o A particular solution of (4) is

o As the einegfunctions must be single valued, i.e., =>

and using Euler’s formula,

o This is only satisfied if ml = 0, ±1, ±2, ...

o Therefore, acceptable solutions to (4) only exist when ml can only have certain integer values, i.e. it is a quantum number.

o ml is called the magnetic quantum number in spectroscopy.

o Called magnetic quantum number because plays role when atom interacts with magnetic fields.

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(φ) = e im lφ

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e iml 0 = e iml 2π

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1= cosml 2π + isin ml 2π

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Polar solutions (Polar solutions ((())))

o Making change of variables (z = rcos, Eqn. 5 transformed into an associated Legendre equation:

o Solutions to Eqn. 7 are of form

where are associated Legendre polynomial functions.

remains finite when = 0, 1, 2, 3, ...

ml = -l, -l+1, .., 0, .., l-1, l

o Can write the associated Legendre functions using quantum number subscripts:

00 = 1

10 = cos 1±1 = (1-cos2)1/2

20 = 1-3cos2 2±1 = (1-cos2)1/2cos 2±2 = 1-cos2

€

d

dz(1- 2z )

dΘ

dz

⎡ ⎣ ⎢

⎤ ⎦ ⎥+ l(l +1) -

2lm

1- 2z

⎡

⎣ ⎢

⎤

⎦ ⎥Θ = 0

(7)

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lml(θ) = sin|m l | θFl |m l |(cosθ)

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Fl |m l |(cosθ)

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Spherical harmonic solutionsSpherical harmonic solutions

i.e., product of trigonometric and polynomial

functions.

o First few spherical harmonics are:

Y00= 1

Y10= cosY1

±1= (1-cos2)1/2 e±i

Y 2

0= 1-3cos2Y2±1= (1-cos2)1/2cos e±i

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lmlY (θ ,φ ) = l lmΘ (θ )

lmΦ (φ )

QuickTime™ and aTIFF (Uncompressed) decompressor

are needed to see this picture.

o Customary to multiply () and () to form so called spherical harmonic functions

which can be written as:

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Radial solutions (R( r ))Radial solutions (R( r ))

o What is the ground state of hydrogen (Z=1)? Assuming that the ground state has n = 1, l = 0 Eqn. 6 can be written

o Taking the derivative

(7)

o Try solution , where A and a0 are constants. Sub into Eqn. 7:

o To satisfy this Eqn. for any r, both expressions in brackets must equal zero. Setting the second expression to zero =>

o Setting first term to zero =>

€

1

r2

d

drr2 dR

dr

⎛

⎝ ⎜

⎞

⎠ ⎟+

2μ

h2E +

e2

4πε0r

⎡

⎣ ⎢

⎤

⎦ ⎥R = 0

€

a0 =4πε0h

2

μe2

€

d2R

dr2+

2

r

dR

dr+

2μ

h2E +

e2

4πε0r

⎡

⎣ ⎢

⎤

⎦ ⎥R = 0

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R = Ae−r / a0

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E = −h2

2μa02

= −13.6 eVSame as Bohr’s results

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o Radial wave equation

has many solutions, one for each positive integer of n.

o Solutions are of the form (see Appendix N of Eisberg & Resnick):

where a0 is the Bohr radius. Bound-state solutions are only acceptable if

where n is the principal quantum number, defined by n = l +1, l +2, l +3, …

o En only depends on n: all l states for a given n are degenerate (i.e. have the same energy).

€

d2R

dr2+

2

r

dR

dr+

2μ

h2E +

e2

4πε0r

⎡

⎣ ⎢

⎤

⎦ ⎥R = 0

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Rnl (r) = e−Zr / na0Zr

a0

⎛

⎝ ⎜

⎞

⎠ ⎟

l

Gnl

Zr

a0

⎛

⎝ ⎜

⎞

⎠ ⎟

€

En = −Z 2μe4

(4πε0)22h2n2

= −13.6Z 2

n2 eV

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o Gnl(Zr/a0) are called associated Laguerre polynomials, which depend on n and l.

o Several resultant radial wavefunctions (Rnl( r )) for the hydrogen atom are given below

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o The radial probability function Pnl(r ), is the probability that the electron is found between r and r + dr:

o Some representative radial probability functions are given at right:

o Some points to note:

o The r2 factor makes the radial probability density vanish at the origin, even for l = 0 states.

o For each state (given n and l), there are n - l - 1nodes in the distribution.

o The distribution for states with l = 0, have n maxima, which increase in amplitude with distance from origin.

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Pnl (r)dr = Rnl (r)Ylm l(θ,φ)

2r2dV∫

= 4πr2 Rnl

2r2dr

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o Radial probability distributions for an electron in several of the low energy orbitals of hydrogen.

o The abscissa is the radius

in units of a0. s orbitals

p orbitals

d orbitals

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Hydrogen eigenfunctionsHydrogen eigenfunctions

o Eigenfunctions for the state described by the quantum numbers (n, l, ml) are therefore of form:

and depend on quantum numbers:

n = 1, 2, 3, …

l = 0, 1, 2, …, n-1

ml = -l, -l+1, …, 0, …, l-1, l

o Energy of state on dependent on n:

o Usually more than one state has same

energy, i.e., are degenerate.

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ψnlm l(r,θ,φ) = Rnl (r)Θ lm l

(θ)Φm l(φ)

€

En = −13.6Z 2

n2

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Born interpretation of the wavefunctionBorn interpretation of the wavefunction

o Principle of QM: the wavefunction contains all the dynamical information about the system it describes.

o Born interpretation of the wavefunction: The probability (P(x,t)) of finding a particle at a position between x and x+dx is proportional to |Ψ(x,t)|2dx:

P(x,t) = Ψ*(x,t) Ψ(x,t) = |Ψ(x,t)|2

o P(x,t) is the probability density.

o Immediately implies that sign of wavefunction has no

direct physical significance.

Ψ(x,t) P(x,t)

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o In H-atom, ground state orbital has the same sign everywhere => sign of orbital must be all positive or all negative.

o Other orbitals vary in sign. Where orbital changes sign, Ψ = 0 (called a node) => probability of finding electron is zero.

o Consider first excited state of hydrogen: sign of

wavefunction is insignificant (P = Ψ2 = (-Ψ)2).

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o Next excited state of H-atom is asymmetric about origin. Wavefunction has opposite sign on opposite sides of nucleus.

o The square of the wavefunction is identical on

opposite sides, representing equal distribution

of electron density on both side of nucleus.

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Atomic orbitalsAtomic orbitals

o Quantum mechanical equivalent of orbits in Bohr model.





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s orbitalss orbitals

o Named from “sharp” spectroscopic lines.

o l = 0, ml = 0

ψn,0,m = Rn,0 (r ) Y0,m (, )

o Angular solution:

o Value of Y0,0 is constant over sphere.

o For n = 0, l = 0, ml = 0 => 1s orbital

o The probability density is

-0.20

0.2

-0.20

0.2

-0.2

0

0.2

-0.2

0

0.2

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Y0,0 =1

4π

€

ψ1,0,0 =1

π

Z

a0

⎛

⎝ ⎜

⎞

⎠ ⎟

3 / 2

e−Zr / a0

€

Pnlml(r,θ,φ) =ψ nlm l

(r,θ,φ)*ψ nlml(r,θ,φ)

€

=>P1,0,0(r,θ,φ) =1

π

Z

a0

⎛

⎝ ⎜

⎞

⎠ ⎟

3

e−2Zr / a0

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p orbitalsp orbitals

o Named from “principal” spectroscopic lines.

o l = 1, ml = -1, 0, +1 (n must therefore be >1)

ψn,1,m = Rn1 (r ) Y1,m (, )

o Angular solution:

o A node passes through the nucleus and separates the two lobes of each orbital.

o Dark/light areas denote opposite sign of the wavefunction.

o Three p-orbitals denoted px, py , pz €

ψ2,1,0(r,θ,φ) = R2,1(r)3

4π

⎛

⎝ ⎜

⎞

⎠ ⎟

1/ 2

cosθ = 2 pz

€

Y1,0 =3

4πcosθ

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d orbitalsd orbitals

o Named from “diffuse” spectroscopic lines.

o l = 2, ml = -2, -1, 0, +1, +2 (n must therefore be >2)

ψn,2,m = Rn1 (r ) Y2,m (, )

o Angular solution:

o There are five d-orbitals, denoted

o m = 0 is z2. Two orbitals of m = -1 and +1 are xz and yz. Two orbitals with m = -2 and +2 are designated xy and x2-y2.

-1-0.500.5

1-1 -0.5 0 0.5

1

-2

-1

0

1

2

-1-0.500.5

1

-2

-1

0

1

2

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Y2,0 =5

4π

1

2(3cos2 θ −1)

€

dz 2 ,dxz,dyz,dxy,dx 2 −y 2

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Quantum numbers and spectroscopic notationQuantum numbers and spectroscopic notation

o Principal quantum number: o n = 1 (K shell)o n = 2 (L shell)o n = 3 (M shell)o …

o If n = 1 and l = 0 = > the state is designated 1s. n = 3, l = 2 => 3d state.

o Three quantum numbers arise because time-independent Schrödinger equation contains three independent variables, one for each space coordinate.

o The eigenvalues of the one-electron atom depend only on n, by the eigenfunctions depend on n, l and ml, since they are the product of Rnl(r ), lml () and ml().

o For given n, there are generally several values of l and ml => degenerate eigenfunctions.

o Angular momentum quantum number:o l = 0 (s subshell)o l = 1 (p subshell)o l = 2 (d subshell)o l = 3 (f subshell)o …

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Orbital transitions for hydrogenOrbital transitions for hydrogen

o Transition between different energy levels of the hydrogenic atom must follow the following selection rules:

l = ±1

m = 0, ±1

o A Grotrian diagram or a term diagram shows the allowed transitions.

o The thicker the line at right, the more probable and hence more intense the transitions.

o The intensity of emission/absorption lines could not be explained via Bohr model.

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Schrödinger vs. Bohr modelsSchrödinger vs. Bohr models

o Schrodinger’s QM treatment had a number of advantages over semi-classical Bohr model:

1. Probability density orbitals do not violate the Heisenberg Uncertainty Principle.

1. Orbital angular momentum correctly accounted for.

1. Electron spin can be properly treaded.

1. Electron transition rates can be explained.

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Lectures 3-4: One-electron atoms