Chemistry Reference
In-Depth Information
4.26
Which of the following sets of quantum numbers is (are)
not
permitted?
(a)
(b)
(c)
(d)
4.27 Make a chart showing all possible values of
4.36 Explain why the helium atom is stable with only two
electrons in its outermost shell, but beryllium is not.
4.37
How many electrons are present in each of the following
atoms? Assuming that each is a neutral atom, identify the
element.
(a)
(b)
(c)
4.38
How many electrons are permitted (a) in a
d
orbital and
(b) in a
d
subshell?
4.39
Write detailed electronic configurations for Li, C, and
Mg.
4.40
(a) How many orbitals are in the 2
p
subshell?
(b) How many orbitals are in the 3
p
subshell?
(c) How many orbitals are in the 4
p
subshell?
(d) What is the maximum number of electrons permit-
ted in a 5
p
subshell?
4.41 In a given atom, what is the maximum number of
electrons that can have the following quantum numbers?
(a)
(b)
(c)
(d) and
4.42 (a) What is the letter designation for
(b) How many different values are possible for an
electron in a subshell for which
(c) How many different orbitals are in an subshell?
(d) What is the maximum number of electrons in an
subshell?
4.43 (a) How many 2
p
orbitals are present in any atom?
(b) What is the maximum number of electrons in the
2
p
subshell?
(c) How many electrons are present in the 2
p
subshell of
a fluorine atom?
(d) Explain why the subshell is not full in the fluorine
atom.
1
2
n
3,
/
0,
m
/
1,
m
s
n
3,
/
2,
m
/
1,
m
s
1
1
2
n
3,
/
2,
m
/
0,
m
s
1
s
2
2
s
2
2
p
6
3
s
2
3
p
1
1
2
n
3,
/
3,
m
/
2,
m
s
1
s
2
2
s
2
2
p
6
3
s
2
3
p
6
4
s
2
3
d
1
/
,
m
/
,
and
1
s
2
2
s
2
2
p
6
3
s
2
3
p
6
4
s
2
3
d
10
4
p
6
m
s
for an electron with
n
2
and another with
n
3.
4.4 Relative Energies of Electrons
4.28
(a) What values of
m
/
are permitted for an electron with
/
5?
(b) How many different values of
m
/
are permitted for
an electron with
4.29
Arrange the following electrons, identified only by their
n
and quantum numbers, in order of increasing energy
from lowest to highest.
(a) (b)
(c) (d)
4.30 Arrange the following electrons in order of increasing
energy:
(a) (b)
(c) (d)
4.31
Arrange the following electrons in order of increasing
energy:
(a)
(b)
(c)
(d)
4.32 Compare the energies of the following electrons, identi-
fied by their quantum numbers only:
(a)
(b)
(c)
4.33 Arrange the following four electrons in order of increas-
ing energy:
(a)
(b)
(c)
(d)
/
5?
/
n
6,
/
3
n
6,
/
2
n
5,
/
3
n
5,
/
2
n
5,
4,
/
2
n
n
3,
/
3
n
5,
/
1
n
4,
/
2
/
0
n
4,
/
3
n
6,
/
0
n
4,
/
1,
m
/
1
/
3?
m
/
1
2
n
5,
/
1,
m
/
1,
m
s
/
3?
1
2
n
5,
/
1,
m
/
0,
m
s
/
3
1
2
n
5,
/
1,
m
/
1,
m
s
1
2
n
5,
/
1,
m
/
0,
m
s
/
3
1
2
n
3,
/
2,
m
/
1,
m
s
1
2
n
3,
/
2,
m
/
1,
m
s
1
2
n
3,
/
2,
m
/
0,
m
s
1
2
n
4,
/
0,
m
/
0,
m
s
4.6 Shapes of Orbitals
1
2
n
3,
/
1,
m
/
1,
m
s
1
2
n
3,
/
2,
m
/
0,
m
s
4.44
According to Figure 4.8(c), which two 3
d
orbitals cannot
have an electron in the
xz
-plane?
4.45 According to Figure 4.8(b), which 2
p
orbital cannot have
an electron in the
xz
-plane?
4.46 How many
d
orbitals are pictured in Figure 4.8?
4.47
(a) How many of the
p
orbitals pictured in Fig-
ure 4.8(b) are oriented along an axis? (b) How many
of the
d
orbitals pictured in Figure 4.8(c) are oriented
along axes?
1
2
n
4,
/
1,
m
/
1,
m
s
4.5 Shells, Subshells, and Orbitals
4.34
What does the number of values permitted for a given
n
value have to do with the number of subshells in a shell?
4.35 What does the number of
/
value have to do with the number of orbitals in a subshell?
/
m
/
values permitted for a given
