140 CHAPTER 5. IDENTICAL PARTICLES
Problem 5.13
(a) Orthohelium should have lower energy than parahelium, for corresponding states (which is true).
(b) Hund’s first rule says S = 1 for the ground state of carbon. But this (the triplet) is symmetric, so the
orbital state will have to be antisymmetric. Hund’s second rule favors L = 2, but this is symmetric, as
you can see most easily by going to the “top of the ladder”: |22 = |11
1
||11
2
. So the ground state of
carbon will be S =1,L= 1. This leaves three possibilities:
3
P
2
,
3
P
1
, and
3
P
0
.
(c) For boron there is only one electron in the 2p subshell (which can accommodate a total of 6), so Hund’s
third rule says the ground state will have J = |L − S|. We found in Problem 5.12(b) that L = 1 and
S =1/2, so J =1/2, and the configuration is
2
P
1/2
.
(d) For carbon we know that S = 1 and L = 1, and there are only two electrons in the outer subshell, so
Hund’s third rule says J = 0, and the ground state configuration must be
3
P
0
.
For nitrogen Hund’s first rule says S =3/2, which is symmetric (the top of the ladder is |
3
2
3
2
=
|
1
2
1
2
1
|
1
2
1
2
2
|
1
2
1
2
3
). Hund’s second rule favors L = 3, but this is also symmetric. In fact, the only
antisymmetric orbital configuration here is L = 0. [You can check this directly by working out the
Clebsch-Gordan coefficients, but it’s easier to reason as follows: Suppose the three outer electrons are in
the “top of the ladder” spin state, so each one has spin up (|
1
2
1
2
); then (since the spin states are all the
same) the orbital states have to be different: |11, |10, and |1−1. In particular, the total z-component of
orbital angular momentum has to be zero. But the only configuration that restricts L
z
to zero is L = 0.]
The outer subshell is exactly half filled (three electrons with n =2,l = 1), so Hund’s third rule says
J = |L − S| = |0 −
3
2
| =3/2. Conclusion: The ground state of nitrogen is
4
S
3/2
. (Table 5.1 confirms
this.)
Problem 5.14
S =2;L =6;J =8. (1s)
2
(2s)
2
(2p)
6
(3s)
2
(3p)
6
(3d)
10
(4s)
2
(4p)
6
definite
(36 electrons)
(4d)
10
(5s)
2
(5p)
6
(4f)
10
(6s)
2
likely
(30 electrons)
.
Problem 5.15
Divide Eq. 5.45 by Eq. 5.43, using Eq. 5.42:
E
tot
/N q
E
F
=
2
(3π
2
Nq)
5/3
10π
2
mV
2/3
1
Nq
2m
2
(3π
2
Nq/V )
2/3
=
3
5
.
Problem 5.16
(a) E
F
=
2
2m
(3ρπ
2
)
2/3
.ρ=
Nq
V
=
N
V
=
atoms
mole
×
moles
gm
×
gm
volume
=
N
A
M
· d, where N
A
is Avogadro’s
number (6.02 ×10
23
), M = atomic mass = 63.5 gm/mol, d = density = 8.96 gm/cm
3
.
ρ =
(6.02 × 10
23
)(8.96 gm/cm
3
)
(63.5gm)
=8.49 × 10
22
/cm
3
=8.49 × 10
28
/m
3
.
E
F
=
(1.055 × 10
−34
J · s)(6.58 × 10
−16
eV · s)
(2)(9.109 × 10
−31
kg)
(3π
2
8.49 × 10
28
/m
3
)
2/3
= 7.04 eV.
c
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