Instructor solution manual to accompany physical chemistry 7th ed by peter atkins chap13

13

Atomic structure and atomic spectra

Solutions to exercises
Discussion questions
E13.1(b)

(1) The principal quantum number, n, determines the energy of a hydrogenic atomic orbital through
eqn 13.13.
(2) The azimuthal quantum number, l, determines the magnitude of the angular momentum of a
hydrogenic atomic orbital through the relation {l(l + 1)}1/2 h
¯.
(3) The magnetic quantum number, ml , determines the z-component of the angular momentum of a
hydrogenic orbital through the relation ml h
¯.
(4) The spin quantum number, s, determines the magnitude of the spin angular momentum through
the relation {s(s + 1)}1/2 h
¯ . For a hydrogenic atomic orbitals, s can only be 1/2.
(5) The spin quantum number, ms , determines the z-component of the spin angular momentum
¯ . For hydrogenic atomic orbitals, ms can only be ±1/2.
through the relation ms h

E13.2(b)

(a) A boundary surface for a hydrogenic orbital is drawn so as to contain most (say 90%) of the
probability density of an electron in that orbital. Its shape varies from orbital to orbital because
the electron density distribution is different for different orbitals.
(b) The radial distribution function gives the probability that the electron will be found anywhere
within a shell of radius r around the nucleus. It gives a better picture of where the electron is
likely to be found with respect to the nucleus than the probability density which is the square of

the wavefunction.

E13.3(b)

The first ionization energies increase markedly from Li to Be, decrease slightly from Be to B, again
increase markedly from B to N, again decrease slightly from N to O, and finally increase markedly
from N to Ne. The general trend is an overall increase of I1 with atomic number across the period.
That is to be expected since the principal quantum number (electron shell) of the outer electron
remains the same, while its attraction to the nucleus increases. The slight decrease from Be to B is
a reflection of the outer electron being in a higher energy subshell (larger l value) in B than in Be.
The slight decrease from N to O is due to the half-filled subshell effect; half-filled sub-shells have
increased stability. O has one electron outside of the half-filled p subshell and that electron must pair
with another resulting in strong electron–electron repulsions between them.

E13.4(b)

An electron has a magnetic moment and magnetic field due to its orbital angular momentum. It also
has a magnetic moment and magnetic field due to its spin angular momentum. There is an interaction
energy between magnetic moments and magnetic fields. That between the spin magnetic moment
and the magnetic field generated by the orbital motion is called spin–orbit coupling. The energy of
interaction is proportional to the scalar product of the two vectors representing the spin and orbital
angular momenta and hence depends upon the orientation of the two vectors. See Fig. 13.29. The
total angular momentum of an electron in an atom is the vector sum of the orbital and spin angular
momenta as illustrated in Fig. 13.30 and expressed in eqn 13.46. The spin–orbit coupling results in
a splitting of the energy levels associated with atomic terms as shown in Figs 13.31 and 13.32. This
splitting shows up in atomic spectra as a fine structure as illustrated in Fig. 13.32.


INSTRUCTOR’S MANUAL

202

Numerical exercises
E13.5(b)

The energy of the photon that struck the Xe atom goes into liberating the bound electron and giving
it any kinetic energy it now possesses
Ephoton = I + Ekinetic

I = ionization energy

The energy of a photon is related to its frequency and wavelength
Ephoton = hν =

hc
λ

and the kinetic energy of an electron is related to its mass and speed
Ekinetic = 21 me s 2
So

hc
hc 1
− 2 me s 2
= I + 21 me s 2 ⇒ I =
λ
λ
I =

(6.626 × 10−34 J s) × (2.998 × 108 m s−1 )

58.4 × 10−9 m
− 21 (9.11 × 10−31 kg) × (1.79 × 106 m s−1 )2

= 1.94 × 10−18 J = 12.1 eV
E13.6(b)

The radial wavefunction is [Table 13.1]
2Zr
R3,0 = A 6 − 2ρ + 19 ρ 2 e−ρ/6 where ρ ≡
, and A is a collection of constants. Differentiating
a0
with respect to ρ yields
dR3,0
= 0 = A(6 − 2ρ + 19 ρ 2 ) × − 16 e−ρ/6 + −2 + 29 ρ Ae−ρ/6
dρ
= Ae−ρ/6 − ρ54 + 59 ρ − 3
2

This is a quadratic equation
0 = aρ 2 + bρ + c

where a = −

5
1
, b = , and c = −3.
54
9

The solution is

ρ=
so r =

√
−b ± (b2 − 4ac)1/2
= 15 ± 3 7
2a
15 3(71/2 )
±
2
2

a0
.
Z

Numerically, this works out to ρ = 7.65 and 2.35, so r = 11.5a0 /Z and 3.53a0 /Z . Substituting
Z = 1 and a0 = 5.292 × 10−11 m, r = 607 pm and 187 pm.
The other maximum in the wavefunction is at r = 0 . It is a physical maximum, but not a calculus
maximum: the first derivative of the wavefunction does not vanish there, so it cannot be found by
differentiation.


ATOMIC STRUCTURE AND ATOMIC SPECTRA

E13.7(b)

203

The radial wavefunction is [Table 13.1]

R3,1 = A 4 − 13 ρ ρe−ρ/6

where

ρ=

2Zr
a0

The radial nodes occur where the radial wavefunction vanishes. This occurs at
r=0

ρ = 0,
and when

4 − 13 ρ = 0,

ρ
= 4,
3

or

or

ρ = 12

ρa0
12a0
ρa0

=
=
= 6a0 = 3.18 × 10−10 m
2Z
2
2
Normalization requires
then r =

E13.8(b)

|ψ|2 dτ = 1 =
1 = N2

∞
0

∞
0

π
0

2π
0

[N (2 − r/a0 )e−r/2a0 ]2 dφ sin θ dθ r 2 dr

e−r/a0 (2 − r/a0 )2 r 2 dr

π
0

2π

sin θ dθ

dφ
0

Integrating over angles yields
∞

1 = 4πN 2

0
∞

= 4πN 2

0

e−r/a0 (2 − r/a0 )2 r 2 dr
e−r/a0 (4 − 4r/a0 + r 2 /a02 )r 2 dr = 4π N 2 (8a03 )
∞

In the last step, we used
0

So N =

E13.9(b)

e−r/k r 2 dr = 2k 3 ,

∞
0

e−r/k r 3 dr = 6k 4 , and

∞
0

e−r/k r 4 dr = 24k 5

1
4 2πa03

The average kinetic energy is
Eˆ K =

ψ ∗ Eˆ K ψ dτ

where ψ = N (2 − ρ)e
h
¯
∇2
Eˆ K = −
2m
2

−ρ/2

1
with N =
4

Z3
2π a03

1/2

and ρ ≡

Zr
a0

here

a 3 ρ 2 sin θ dρ dθ dφ
dτ = r 2 sin θ dr dθ dφ = 0
Z3

In spherical polar coordinates, three of the derivatives in ∇ 2 are derivatives with respect to angles, so
those parts of ∇ 2 ψ vanish. Thus
∇2ψ =

∂ 2ψ
2 ∂ψ
∂ 2ψ
+

=
r ∂r
∂r 2
∂ρ 2

∂ρ 2
2Z
+
2
ρa0
∂r

∂ψ
∂ρ

∂ρ
=
∂r

Z 2
×
a0

∂ 2ψ
2 ∂ψ
+
2
ρ ∂ρ
∂ρ

INSTRUCTOR’S MANUAL

204

∂ρ
= N (2 − ρ) × − 21 e−ρ/2 − N e−ρ/2 = N 21 ρ − 2 e−ρ/2
∂r
∂ 2ψ
= N 21 ρ − 2 × − 21 e−ρ/2 + 21 N e−ρ/2 = N 23 − 41 ρ e−ρ/2
∂ρ 2
Z 2
N e−ρ/2 (−4/ρ + 5/2 − ρ/4)
a0

∇2ψ =
and
Eˆ K =

π

∞

2π
0

0

0

Z 2
×
a0

N (2 − ρ)e−ρ/2

−¯h2
2m

a 3 dφ sin θ dθ ρ 2 dρ
× N e−ρ/2 (−4/ρ + 5/2 − ρ/4) 0
Z3
The integrals over angles give a factor of 4π , so
∞

a0
h
¯2
× −
Eˆ K = 4πN 2
Z
2m

0

(2 − ρ) × −4 + 25 ρ − 41 ρ 2 ρe−ρ dρ

The integral in this last expression works out to −2, using
Z3

Eˆ K = 4π

×

32πa03

a0
×
Z

h
¯2

0

e−ρ ρ n dρ = n! for n = 1, 2, and 3. So

h
¯ 2 Z2

=

m

∞

8ma02

The average potential energy is
V =

and V =

ψ ∗ V ψ dτ
∞

π

0

where V = −
2π

0

0

Z 2 e2
Ze2
=−
4π ε0 r
4π ε0 a0 ρ

N (2 − ρ)e−ρ/2 −

a 3 ρ 2 sin θ dρ dθ dφ
N (2 − ρ)e−ρ/2 0
Z3

Z 2 e2
4π ε0 a0 ρ

The integrals over angles give a factor of 4π , so
V = 4πN 2 −

Z 2 e2
4πε0 a0

×

∞

a03
Z3

0

(2 − ρ)2 ρe−ρ dρ
∞

The integral in this last expression works out to 2, using
0

V = 4π

Z3
32πa03

× −

Z 2 e2

4πε0 a0

×

a03
Z3

e−ρ ρ n dρ = n! for n = 1, 2, 3, and 4. So

× (2) = −

Z 2 e2
16π ε0 a0

E13.10(b) The radial distribution function is defined as
P = 4πr 2 ψ 2

so

P3s = 4πr 2 (Y0,0 R3,0 )2 ,

P3s = 4πr 2

1
4π

×

where ρ ≡

2Zr
2Zr
=
na0
3a0

1
243
here.

×

Z 3
× (6 − 6ρ + ρ 2 )2 e−ρ
a0


ATOMIC STRUCTURE AND ATOMIC SPECTRA

205

But we want to find the most likely radius, so it would help to simplify the function by expressing it
in terms either of r or ρ, but not both. To find the most likely radius, we could set the derivative of
P3s equal to zero; therefore, we can collect all multiplicative constants together (including the factors
of a0 /Z needed to turn the initial r 2 into ρ 2 ) since they will eventually be divided into zero
P3s = C 2 ρ 2 (6 − 6ρ + ρ 2 )2 e−ρ
Note that not all the extrema of P are maxima; some are minima. But all the extrema of (P3s )1/2
correspond to maxima of P3s . So let us find the extrema of (P3s )1/2
d(P3s )1/2
d

=0=
Cρ(6 − 6ρ + ρ 2 )e−ρ/2
dρ
dρ
= C[ρ(6 − 6ρ + ρ 2 ) × (− 21 ) + (6 − 12ρ + 3ρ 2 )]e−ρ/2
0 = C(6 − 15ρ + 6ρ 2 − 21 ρ 3 )e−ρ/2

so

12 − 30ρ + 12ρ 2 − ρ 3 = 0

Numerical solution of this cubic equation yields
ρ = 0.49, 2.79, and 8.72
corresponding to
r = 0.74a0 /Z, 4.19a0 /Z, and 13.08a0 /Z
Comment. If numerical methods are to be used to locate the roots of the equation which locates
the extrema, then graphical/numerical methods might as well be used to locate the maxima directly.
That is, the student may simply have a spreadsheet compute P3s and examine or manipulate the
spreadsheet to locate the maxima.
E13.11(b) Orbital angular momentum is
¯ (l(l + 1))1/2
Lˆ 2 1/2 = h
There are l angular nodes and n − l − 1 radial nodes
(a) n = 4, l = 2, so Lˆ 2 1/2 = 61/2 h
¯ = 2.45 × 10−34 J s

2 angular nodes

1 radial node

(b) n = 2, l = 1, so Lˆ 2 1/2 = 21/2 h
¯ = 1.49 × 10−34 J s

1 angular node

0 radial nodes

(c) n = 3, l = 1, so Lˆ 2 1/2 = 21/2 h
¯ = 1.49 × 10−34 J s

1 angular node

1 radial node

E13.12(b) For l > 0, j = l ± 1/2, so
(a)

l = 1,

so

j = 1/2 or 3/2

(b)

l = 5,

so

j = 9/2 or 11/2

E13.13(b) Use the Clebsch–Gordan series in the form
J = j1 + j2 , j1 + j2 − 1, . . . , |j1 − j2 |
Then, with j1 = 5 and j2 = 3
J = 8, 7, 6, 5, 4, 3, 2


INSTRUCTOR’S MANUAL

206

E13.14(b) The degeneracy g of a hydrogenic atom with principal quantum number n is g = n2 . The energy E
of hydrogenic atoms is
E=−

hcZ 2 RH
hcZ 2 RH
=−
2
g
n

so the degeneracy is
g=−

hcZ 2 RH
E

(a)

g=−

(b)

g=−

(c)

g=−

hc(2)2 RH
= 1
−4hcRH
hc(4)2 RH
− 41 hcRH

= 64

hc(5)2 RH
= 25
−hcRH

E13.15(b) The letter F indicates that the total orbital angular momentum quantum number L is 3; the superscript
3 is the multiplicity of the term, 2S + 1, related to the spin quantum number S = 1; and the subscript
4 indicates the total angular momentum quantum number J .
E13.16(b) The radial distribution function varies as
4
P = 4πr 2 ψ 2 = 3 r 2 e−2r/a0
a0
The maximum value of P occurs at r = a0 since

dP
2r 2
∝ 2r −
a0
dr

e−2r/a0 = 0

at r = a0 and Pmax =

4 −2
e
a0

P falls to a fraction f of its maximum given by
f =

4r 2 −2r/a0
e
a03
4 −2
a0 e

r2
= 2 e2 e−2r/a0
a0

and hence we must solve for r in
f 1/2
r

= e−r/a0
e
a0
f = 0.50
r
0.260 = e−r/a0 solves to r = 2.08a0 = 110 pm and to r = 0.380a0 = 20.1 pm
a0
(b)
f = 0.75
r
0.319 = e−r/a0 solves to r = 1.63a0 = 86 pm and to r = 0.555a0 = 29.4 pm
a0
(a)

In each case the equation is solved numerically (or graphically) with readily available personal
computer software. The solutions above are easily checked by substitution into the equation for f .
The radial distribution function is readily plotted and is shown in Fig. 13.1.


ATOMIC STRUCTURE AND ATOMIC SPECTRA

207

0.15

0.10

0.05

0.00

0.0

0.5

1.0

1.5

2.0

2.5

Figure 13.1
E13.17(b) (a) 5d → 2s is not an allowed transition, for
(b) 5p → 3s is allowed , since
(c) 5p → 3f is not allowed, for

l = −2 ( l must equal ±1).

l = −1.
l = +2 ( l must equal ±1).

E13.18(b) For each l, there are 2l + 1 values of ml and hence 2l + 1 orbitals—each of which can be occupied
by two electrons, so maximum occupancy is 2(2l + 1)
(a) 2s: l = 0; maximum occupancy = 2
(b) 4d: l = 2; maximum occupancy = 10
(c) 6f : l = 3; maximum occupancy = 14
(d) 6h: l = 5; maximum occupancy = 22
E13.19(b) V2+ : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 3 = [Ar]3d 3
The only unpaired electrons are those in the 3d subshell. There are three. S = 23 and 23 − 1 = 21 .

For S = 23 , MS = ± 21 and ± 23
for S = 21 , MS = ± 21
E13.20(b) (a) Possible values of S for four electrons in different orbitals are 2, 1, and 0 ; the multiplicity is
2S + 1, so multiplicities are 5, 3, and 1 respectively.
(b) Possible values of S for five electrons in different orbitals are 5/2, 3/2, and 1/2 ; the multiplicity
is 2S + 1, so multiplicities are 6, 4, and 2 respectively.
E13.21(b) The coupling of a p electron (l = 1) and a d electron (l = 2) gives rise to L = 3 (F), 2 (D), and 1 (P)
terms. Possible values of S include 0 and 1. Possible values of J (using Russell–Saunders coupling)
are 3, 2, and 1 (S = 0) and 4, 3, 2, 1, and 0 (S = 1). The term symbols are
1

F3 ; 3 F4 , 3 F3 , 3 F2 ; 1 D2 ; 3 D3 , 3 D2 , 3 D1 ; 1 P1 ; 3 P2 , 3 P1 , 3 P0 .

Hund’s rules state that the lowest energy level has maximum multiplicity. Consideration of spin–orbit
coupling says the lowest energy level has the lowest value of J (J + 1) − L(L + 1) − S(S + 1). So
the lowest energy level is 3 F2


INSTRUCTOR’S MANUAL

208

E13.22(b) (a) 3 D has S = 1 and L = 2, so J = 3, 2, and 1 are present. J = 3 has 7 states, with MJ = 0,
±1, ±2, or ±3; J = 2 has 5 states, with MJ = 0, ±1, or ±2; J = 1 has 3 states, with
MJ = 0, or ±1.
(b) 4 D has S = 3/2 and L = 2, so J = 7/2, 5/2, 3/2, and 1/2 are present. J = 7/2 has 8
possible states, with MJ = ±7/2, ±5/2, ±3/2 or ±1/2; J = 5/2 has 6 possible states, with
MJ = ±5/2 ±3/2 or ±1/2; J = 3/2 has 4 possible states, with MJ = ±3/2 or ±1/2;
J = 1/2 has 2 possible states, with MJ = ±1/2.
(c) 2 G has S = 1/2 and L = 4, so J = 9/2 and 7/2 are present. J = 9/2 had 10 possible

states, with MJ = ±9/2, ±7/2, ±5/2, ±3/2 or ±1/2; J = 7/2 has 8 possible states, with
MJ = ±7/2, ±5/2, ±3/2 or ±1/2.
E13.23(b) Closed shells and subshells do not contribute to either L or S and thus are ignored in what follows.
(a) Sc[Ar]3d 1 4s 2 : S = 21 , L = 2; J = 25 , 23 , so the terms are 2 D5/2 and 2 D3/2
(b) Br[Ar]3d 10 4s 2 4p 5 . We treat the missing electron in the 4p subshell as equivalent to a single
“electron” with l = 1, s = 21 . Hence L = 1, S = 21 , and J = 23 , 21 , so the terms are
2
P3/2 and 2 P1/2

Solutions to problems
Solutions to numerical problems
P13.2

All lines in the hydrogen spectrum fit the Rydberg formula
1
= RH
λ

1
n21

1
− 2
n2

13.1, with ν˜ =

1
λ

RH = 109 677 cm−1

Find n1 from the value of λmax , which arises from the transition n1 + 1 → n1
1
1
1
2n1 + 1
= 2−
= 2
2
λmax RH
(n
+
1)
n1
n1 (n1 + 1)2
1
n2 (n1 + 1)2
= (656.46 × 10−9 m) × (109 677 × 102 m−1 ) = 7.20
λmax RH = 1
2n1 + 1
and hence n1 = 2, as determined by trial and error substitution. Therefore, the transitions are given by
ν˜ =

1
= (109 677 cm−1 ) ×
λ

1
1

− 2
4 n2

,

n2 = 3, 4, 5, 6

The next line has n2 = 7, and occurs at
ν˜ =

1
= (109 677 cm−1 ) ×
λ

1
1
−
4 49

= 397.13 nm

The energy required to ionize the atom is obtained by letting n2 → ∞. Then
ν˜ ∞ =

1
= (109 677 cm−1 ) ×
λ∞

1
− 0 = 27 419 cm−1 ,

4

or

3.40 eV


ATOMIC STRUCTURE AND ATOMIC SPECTRA

209

(The answer, 3.40 eV, is the ionization energy of an H atom that is already in an excited state, with
n = 2.)
Comment. The series with n1 = 2 is the Balmer series.

610 nm

I

460 nm

413 nm

The lowest possible value of n in 1s 2 nd 1 is 3; thus the series of 2 D terms correspond to 1s 2 3d, 1s 2 4d,
etc. Figure 13.2 is a description consistent with the data in the problem statement.

670 nm

P13.4

Figure 13.2
If we assume that the energies of the d orbitals are hydrogenic we may write
E(1s 2 nd 1 , 2 D) = −

hcR
n2

[n = 3, 4, 5, . . .]

Then for the 2 D → 2 P transitions
ν˜ =

1
|E(1s 2 2p 1 , 2 P)| R
− 2
=
hc
λ
n

E = hν =

hc
E
= hcν˜ , ν˜ =
λ
hc

from which we can write


R
1


+


−7
9

610.36 × 10 cm


|E(1s 2 2p 1 , 2 P)|
1 R
1
R
= + 2 =
+

hc
λ
n
16
460.29 × 10−7 cm





1
R


+
25
413.23 × 10−7 cm

(b) − (a) solves to R = 109 886 cm−1
Then (a) − (c) solves to R = 109 910 cm−1 Mean = 109 920 cm−1

(b) − (c) solves to R = 109 963 cm−1
The binding energies are therefore
R
= −12 213 cm−1
9
1
− 12 213 cm−1 = −28 597 cm−1
E(1s 2 2p, 2 P) = −
610.36 × 10−7 cm
1
− 28 597 cm−1 = −43 505 cm−1
E(1s 2 2s 1 , 2 S) = −
670.78 × 10−7 cm

E(1s 2 3d 1 , 2 D) =

(a)
(b)
(c)

INSTRUCTOR’S MANUAL

210

Therefore, the ionization energy is
I (1s 2 2s 1 ,2 S) = 43 505 cm−1 ,
P13.5

or

5.39 eV

The 7p configuration has just one electron outside a closed subshell. That electron has l = 1, s = 1/2,
and j = 1/2 or 3/2, so the atom has L = 1, S = 1/2, and J = 1/2 or 3/2. The term symbols are
P1/2 and 2 P3/2 , of which the former has the lower energy. The 6d configuration also has just one
electron outside a closed subshell; that electron has l = 2, s = 1/2, and j = 3/2 or 5/2, so the atom
2

has L = 2, S = 1/2, and J = 3/2 or 5/2. The term symbols are 2 D3/2 and 2 D5/2 , of which the
former has the lower energy. According to the simple treatment of spin–orbit coupling, the energy is
given by
El,s,j = 21 hcA[j (j + 1) − l(l + 1) − s(s + 1)]
where A is the spin–orbit coupling constant. So
E(2 P1/2 ) = 21 hcA[ 21 (1/2 + 1) − 1(1 + 1) − 21 (1/2 + 1)] = −hcA
and E(2 D3/2 ) = 21 hcA[ 23 (3/2 + 1) − 2(2 + 1) − 21 (1/2 + 1)] = − 23 hcA
This approach would predict the ground state to be 2 D3/2
Comment. The computational study cited above finds the 2 P1/2 level to be lowest, but the authors
caution that the error of similar calculations on Y and Lu is comparable to the computed difference

between levels.
P13.7

RH = kµH ,

RD = kµD ,

R = kµ [18]

where R corresponds to an infinitely heavy nucleus, with µ = me .
me mN
[N = p or d]
Since µ =
me + m N
RH = kµH =

kme
R
me =
me
1+ m
1
+
mp
p

R
me where mp is the mass of the proton and md the mass of the deuteron. The
1+ m
d

two lines in question lie at

Likewise, RD =

1
= RH 1 − 41 = 43 RH
λH

1
= RD 1 − 41 = 43 RD
λD

and hence
λD
ν˜ H
RH
=
=
RD
λH
ν˜ D
Then, since
1+
RH
=
RD
1+

me
md

me
mp

,

md =

me
1+

me
mp

RH
RD

−1


ATOMIC STRUCTURE AND ATOMIC SPECTRA

211

and we can calculate md from
me

md =

me
1+ m

p

λD
λH

−1

=

me
me
1+ m
p

ν˜ H
ν˜ D

−1

9.10939 × 10−31 kg

=

1+

9.10939×10−31 kg
1.67262×10−27 kg

×

82 259.098 cm−1
82 281.476 cm−1

−1

= 3.3429 × 10−27 kg

Since I = Rhc,
ID
RD
ν˜ D
82 281.476 cm−1
=
=
=
= 1.000 272
IH
RH
ν˜ H
82 259.098 cm−1
P13.10

If we assume that the innermost electron is a hydrogen-like 1s orbital we may write
r∗ =

52.92 pm
a0
[Example 13.3] =
= 0.420 pm
Z

126

Solutions to theoretical problems
P13.12

Consider ψ2pz = ψ2,1,0 which extends along the z-axis. The most probable point along the z-axis
is where the radial function has its maximum value (for ψ 2 is also a maximum at that point). From
Table 13.1 we know that
R21 ∝ ρe−ρ/4
dR
= 1 − 41 ρ e−ρ/4 = 0 when ρ = 4.
dρ
2a0
2a0
Therefore, r ∗ =
, and the point of maximum probability lies at z = ±
= ±106 pm
Z
Z
Comment. Since the radial portion of a 2p function is the same, the same result would have been
obtained for all of them. The direction of the most probable point would, however, be different.
and so

P13.13

In each case we need to show that

all space

ψ1∗ ψ2 dτ = 0

∞

π

2π

(a)
0

0

0

?

ψ1s ψ2s r 2 dr sin θ dθ dφ = 0

1 1/2
ψ1s = R1,0 Y0,0
Y0,0 =
[Table 12.3]
ψ2s = R2,0 Y0,0
4π
Since Y0,0 is a constant, the integral over the radial functions determines the orthogonality of
the functions.
∞
0

R1,0 R2,0 r 2 dr

R1,0 ∝ e−ρ/2 = e−Zr/a0

ρ=

R2,0 ∝ (2 − ρ/2)e−ρ/4 = 2 −

2Zr
a0
Zr
a0

e−Zr/2a0

ρ=

2Zr
a0


INSTRUCTOR’S MANUAL

212

∞
0

R1,0 R2,0 r 2 dr ∝
=
=

∞
0
∞
0

e−Zr/a0 2 −

Zr
a0

e−Zr/2a0 r 2 dr

2e−(3/2)Zr/a0 r 2 dr −

2 × 2!
3 Z
2 a0

3

Z
a0

−

×

∞
0

3!
3 Z
2 a0

4

Z −(3/2)Zr/a0 3
e
r dr
a0

= 0

Hence, the functions are orthogonal.
(b) We use the px and py orbitals in the form given in Section 13.2(f ), eqn 25
px ∝ x,

py ∝ y

Thus

all space

px py dx dy dz ∝

+∞
−∞

+∞

+∞

−∞

−∞

xy dx dy dz

This is an integral of an odd function of x and y over the entire range of variable from −∞ to
+∞, therefore, the integral is zero . More explicitly we may perform the integration using the
orbitals in the form (Section 13.2(f ), eqn 13.25)
px = f (r) sin θ cos φ
all space

py = f (r) sin θ sin φ
∞

px py r 2 dr sin θ dθ dφ =

0

f (r)2 r 2 dr

π
0

sin2 θ dθ

2π

0

cos φ sin φ dφ

π
.
2
The third factor is zero. Therefore, the product of the integrals is zero and the functions are
orthogonal.
The first factor is nonzero since the radial functions are normalized. The second factor is

P13.14

−

h
¯2
2µ

2 d
d2
+
2
r dr
dr

+ Veff R = ER [13.11]

(1)

l(l + 1)¯h2
l(l + 1)¯h2
Ze2
Z¯h2
+
+
=−
2
4πε0 r
µa0 r
2µr
2µr 2
Using ρ = Zr/a0 , the derivative term of the Hamiltonian can be written in the form

where Veff = −

d2
2 d
=
+
r dr
dr 2

d2
2 d
Z 2
×
+
a0
ρ dρ

dρ 2

≡ Dop

(2)

To determine E2s and E2p , we will evaluate the left side of (1) and compare the result to the right side.
2s orbital.

R2s = N2s (2 − ρ)e−ρ/2

where ρ ≡ Zr/a0 here

dR2s
= N2s −1 − 21 (2 − ρ) e−ρ/2 = N2s
dρ

ρ−4
2

e−ρ/2 =

ρ−4
R2s
2(2 − ρ)

d2 R2s
ρ −ρ/2
6−ρ
e

R2s
= N2s 21 − 41 (ρ − 4) e−ρ/2 = N2s 23 −
=
2
4
4(2
− ρ)
dρ


ATOMIC STRUCTURE AND ATOMIC SPECTRA

−

h
¯2
h
¯2
Dop R2s = −
2µ
2µ
= −

Veff R2s = −
−

h
¯2
2µ

213

h
¯2
Dop + Veff R2s =
2µ
=−

2p orbital.

ρ−8
4ρ

×

×

Z¯h2
Z 2
R2s = −
×
µa0 r
a0

Therefore E2s = − 41

Z 2
R2s
a0

ρ−4
6−ρ
+
×
4(2 − ρ) ρ(2 − ρ)
Z 2
R2s
a0

h
¯2
µ

1
R2s
ρ

Z 2
h
¯2
× −
a0
2µ
¯2
Z2h

×

ρ−8
2

+
R2s
4ρ
ρ

1
R2s
4

2µa02

Z2h
¯2

(3)

2µa02

R2p = N2p ρe−ρ/2

where ρ ≡ Zr/a0 here

dR2p
ρ −ρ/2
2−ρ
= N2p 1 −
e
R2p
=
dρ

2
2ρ
d2 R2p
ρ
= N2p − 21 − 21 1 −
2
dρ 2
−

h
¯2
h
¯2
Dop R2p = −
2µ
2µ
=−

Veff R2p = −
=
−

h
¯2
2µ

ρ−4
R2p
4ρ

e−ρ/2 =

ρ − 4 4 − 2ρ
+
4ρ
2ρ 2
ρ 2 − 8ρ + 8
4ρ 2

×

×

Z 2
R2p
a0

Z 2
R2p
a0

Z¯h2
Z 2
h
¯2
×
+ 2 R2p = −
µa0 r
a0
µr

Z 2
h
¯2
× −
a0
2µ

h
¯2
Dop + Veff R2p =
2µ
=−

Therefore E2p = − 41

×

2µa02

1
+
ρ

Z 2
×
a0

h
¯2

µ

1
R2p
ρ2

2(ρ − 1)
R2p
ρ2

Z 2
h
¯2
× −
a0
2µ
¯2
Z2h

h
¯2
µ

ρ2
4ρ 2

×

ρ 2 − 8ρ + 8 2(ρ − 1)
R2p

+
4ρ 2
ρ2

R2p = −

Z2h
¯2
2µa02

Comparison of eqns (3) and (4) reveals that E2s = E2p .

¯2
Z2h
2µa02

1
R2p
4

(4)


INSTRUCTOR’S MANUAL

214

P13.15

|ψ3px |2 dτ = 1. The integrations are most easily performed in spherical

(a) We must show that
coordinate (Fig. 11).

2π π ∞

ψ3px

2

dτ =

ψ3px

2 2

r sin(θ ) dr dθ dφ

0 0 0
2π π ∞

=

2

Y1−1 − Y11
√
2

R31 (ρ)

0 0 0

r 2 sin(θ ) dr dθ dφ (Table 13.1, eqn 13.25)

where ρ = 2r/a0 , r = ρa0 /2, dr = (a0 /2) dρ.
=

1
2

2π π ∞

a0 3
2

1 3/2
1
4 − ρ ρe−ρ/6
a0
3

1
27(6)1/2

0 0 0

2
3 1/2
2 sin(θ ) cos(φ)
ρ 2 sin(θ ) dρ dθ dφ

8π

×

1
=
46 656π

2π π ∞

2
1
4 − ρ ρe−ρ/6 sin(θ ) cos(φ) ρ 2 sin(θ ) dρ dθ dφ
3

0 0 0

1
=
46 656π

π

2π
2

cos (φ) dφ
0

∞

3

sin (θ ) dθ
0

0

π

=1

1 2
4 − ρ ρ 4 e−ρ/3 dρ
3

4/3

34992

Thus, ψ3px is normalized to 1.

We must also show that

ψ3px ψ3dxy dτ = 0

Using Tables 12.3 and 13.1, we find that
ψ3px =

1
54(2π)1/2

ψ3dxy = R32
=

1 3/2
1
4 − ρ ρe−ρ/6 sin(θ ) cos(φ)
a0
3

Y22 − Y2−2
√
2i

1
32(2π)1/2

1 3/2 2 −ρ/6 2
ρ e
sin (θ ) sin(2φ)
a0

where ρ = 2r/a0 , r = ρa0 /2, dr = (a0 /2)dρ.
∞

ψ3px ψ3dxy dτ = constant ×

ρ e
0

π

2π
5 −ρ/3

dρ

sin4 (θ )dθ

cos(φ) sin(2φ)dφ
0

0
0

Since the integral equals zero, ψ3px and ψ3dxy are orthogonal.


ATOMIC STRUCTURE AND ATOMIC SPECTRA

215

(b) Radial nodes are determined by finding the ρ values (ρ = 2r/a0 ) for which the radial wavefunction equals zero. These values are the roots of the polynomial portion of the wavefunction.
√
√
For the 3s orbital 6 − 6ρ + ρ 2 = 0 when ρnode = 3 + 3 and ρnode = 3 − 3 .
The 3s orbital has these two spherically symmetrical modes. There is no node at ρ = 0 so we
conclude that there is a finite probability of finding a 3s electron at the nucleus.
For the 3px orbital (4 − ρ)(ρ) = 0 when ρnode = 0 and ρnode = 4 .
There is a zero probability of finding a 3px electron at the nucleus.

For the 3dxy orbital ρnode = 0 is the only radial node.
(c)

|R10 Y00 |2 r dτ =

r 3s =
∞

2π π
2 3
R10
r dr

=

a0
3 888

|Y00 |2 sin(θ ) dθ dφ
0 0

0

=

|R10 Y00 |2 r 3 sin(θ ) dr dθ dφ

1

∞

6 − 2ρ + ρ 2 /9

2

ρ 3 e−ρ/3 dρ

0
52488

r 3s =

27a0
2

(d)

Radial distribution functions of atomic hydrogen
0.12

3px

3dxy
0.1

3s

r 2R2a0

0.08

0.06

0.04

0.02

0
0

5

10

15
r /a0

20

25

30

Figure 13.3(a)

The plot shows that the 3s orbital has larger values of the radial distribution function for r <
a0 . This penetration of inner core electrons of multi-electron atoms means that a 3s electron


INSTRUCTOR’S MANUAL

216

experiences a larger effective nuclear charge and, consequently, has a lower energy than either a
3px or 3dxy electron. This reasoning also lead us to conclude that a 3px electron has less energy
than a 3dxy electron.
E3s < E3px < E3dxy .
(e) Polar plots with θ = 90◦
The s Orbital
90
120

60

150

30

180

0
00.20.40.60.8

210

330
300

240
270

The p Orbital
90
120

60

30

150

180

0
0 0.2 0.4 0.6 0.8

210

330

300

240
270

The d Orbital
90
120

60

30

150

180

0
0

0.2

0.4

210

330

300

240
270

Figure 13.3(b)


ATOMIC STRUCTURE AND ATOMIC SPECTRA

217

Boundary surface plots
s - Orbital boundary surface

p - Orbital boundary surface

d - Orbital boundary surface

f - Orbital boundary surface

Figure 13.3(c)
P13.20

Ze2 1
·
4π ε0 r 2
(angular momentum)2
(n¯h)2
The repulsive centrifugal force =
=
[postulated]
me r 3
me r 3
The two forces balance when

The attractive Coulomb force =

Ze2
¯2
1
n2 h

× 2 =
,
4πε0
r
me r 3
The total energy is
E = EK + V =
=

n2 h
¯2
2me

×

implying that

r=

¯ 2 ε0
4π n2 h
Ze2 me

Ze2
n2 h
¯2
(angular momentum)2
1
Ze2
−

[postulated]
× =
−
2
2I
4π ε0
r
4π ε0 r
2me r
2

Ze2 me
4πn2 h
¯ 2ε

−
0

Ze2
4π ε0

×

Ze2 me
4π n2 h
¯ 2ε

= −
0

Z 2 e 4 me
¯2
32π 2 ε02 h

1
× 2
n


INSTRUCTOR’S MANUAL

218

P13.21

(a) The trajectory is defined, which is not allowed according to quantum mechanics.
¯ , not by n¯h. In
(b) The angular momentum of a three-dimensional system is given by {l(l + 1)}1/2 h
the Bohr model, the ground state possesses orbital angular momentum (n¯h, with n = 1), but
the actual ground state has no angular momentum (l = 0). Moreover, the distribution of the
electron is quite different in the two cases. The two models can be distinguished experimentally
by (a) showing that there is zero orbital angular momentum in the ground state (by examining
its magnetic properties) and (b) examining the electron distribution (such as by showing that the
electron and the nucleus do come into contact, Chapter 18).

P13.25

Justification 13.5 noted that the transition dipole moment, µfi had to be non-zero for a transition to
be allowed. The Justification examined conditions that allowed the z component of this quantity to
be non-zero; now examine the x and y components.

f ∗ x i dτ

µx,fi = −e

µy,fi = −e

and

f ∗ y i dτ

As in the Justification, express the relevant Cartesian variables in terms of the spherical harmonics,
Yl,m . Start by expressing them in spherical polar coordinates:
x = r sin θ cos φ

and y = r sin θ sin φ.

Note that Y1,1 and Y1,−1 have factors of sin θ . They also contain complex exponentials that can be
related to the sine and cosine of φ through the identities (eqns FI1.20 and FI1.21)
cos φ = 1/2(eiφ + e−iφ )

and

sin φ =1/2i(eiφ −e−iφ ).

These relations motivate us to try linear combinations Y1,1 +Y1,−1 and Y1,1 +Y1,−1 (form Table 12.3;
note c here corresponds to the normalization constant in the table):
Y1,1 + Y1,−1 = −c sin θ (eiφ + e−iφ ) = −2c sin θ cos φ = −2cx/r,
so x = −(Y1,1 + Y1,−1 )r/2c;
Y1,1 − Y1,−1 = c sin θ (eiφ − e−iφ ) = 2ic sin θ sin φ = 2icy/r,
so y = (Y1,1 − Y1,−1 )r/2ic.

Now we can express the integrals in terms of radial wavefunctions Rn,l and spherical harmonics Yl,ml
e
µx,fi =
2c

∞

π 2π

Y ∗ lf ,mlf (Y1,1 + Y1,−1 )Yli ,mli sin θ dθ dφ.

2

Rnf ,lf rRni ,li r dr
0

0 0

The angular integral can be broken into two, one of which contains Y1,1 and the other Y1,−1 . According
to the “triple integral” relation below Table 12.3, the integral
π 2π

Y ∗ lf ,mlf Y1,1 Yli ,mli sin θ dθ dφ
0 0

vanishes unless lf = li ± 1 and mf = mi ± 1. The integral that contains Y1,−1 introduces no further
constraints; it vanishes unless lf = li ± 1 and mlf = mli ± 1. Similarly, the y component introduces
no further constraints, for it involves the same spherical harmonics as the x component. The whole
set of selection rules, then, is that transitions are allowed only if
l = ±1 and

ml = 0 or ± 1 .


ATOMIC STRUCTURE AND ATOMIC SPECTRA

P13.26

219

(a) The speed distribution in the molecular beam is related to the speed distribution within the
chamber by a factor of v cos θ as shown in Fig. 13.4. Since an integration over all possible θ
must be performed, the cos θ factor may be absorbed into the constant of proportionality.
fbeam (v) = Cvfchamber (v)

where C is to be determined

Molecular beam
Chamber

Figure 13.4
By normalization over the possible beam speeds (0 < vbeam < ∞)
2
fbeam = Cv v 2 e−(mv /2kT )
2
= Cv 3 e−(mv /2kT )

∞

fbeam dv = 1 = C

v=0

∞
v=0

2
v 3 e−(mv /2kT ) dv = C

1
2(m/2kT )2

2

C = 2(m/2kT )
v2 =

∞
v=0

v 2 fbeam (v) dv = C

2
v 5 e−(mv /2kT ) dv

1
(m/2kT )2
=
2
(m/2kT )3

(m/2kT )3
4kT
=
m
m 2
m 4kT
v =
= 2kT
EK =
2
2
m
=C

x=

(b)
or

2µB L2
4EK

dB
dz

dB
4EK x
4(2kT ) x
=
=

2
dz
2µB L
2µB L2
=
=

4kT x
µ B L2
4(1.3807 × 10−23 J K−1 ) × (1000 K) × (1.00 × 10−3 m)
(9.27402 × 10−24 J T−1 ) × (50 × 10−2 m)2

dB
= 23.8 T m−1
dz