Suggested problems Chapter 8
8.27
Two elements in period 5 are adjacent to one another in the periodic table. The ground-state atom of one has
only s electrons in its valence shell; the other has at least one d electron in an unfilled shell. Identify these
elements.
8.33
Given the following information, identify the group from the periodic table that contains elements that behave
like main-group element “E”.
(i) The electron affinity of E is greater than zero.
(ii) The ionization energy (IE) trend for element E is: first ionization energy < second ionization energy <<< third
ionization energy.
(iii) Samples of E are lustrous and are good electrical conductors.
8.35
Which of the following orbital diagrams are allowed by the Pauli exclusion principle? Explain how you arrived at
this decision. Give the electron configuration for the allowed ones.
a.
b.
1s
2s
2p
c.
2s
2p
1s
2s
2p
d.
1s
8.37
1s
2s
2p
Which of the following electron configurations are possible? Explain why the others are not.
a. 1s12s22p7
b. 1s22s22p63s33d7
c. 1s22s22p5
d. 1s22s22p63s23d8
8.39
Write all the possible orbital diagrams for the electron configuration 1s22p1. (There are six different diagrams).
8.41
Give the electron configuration of the ground state of iodine, using the building-up principle.
8.43
Use the building-up principle to obtain the electron configuration of the ground state of manganese.
8.45
Bromine is a Group VIIA element in Period 4. Deduce the valence-shell configuration bromine.
8.49
Thallium has the ground-state configuration [Xe]4f145d106s26p1. Give the group and period for this element.
Classify it as a main-group, a d-transition, or an f-transition element.
8.51
Write the orbital diagram for the ground state of cobalt. The electron configuration is [Ar]3d 74s2.
8.53
Write an orbital diagram for the ground state of the potassium atom. Is the atomic substance diamagnetic or
paramagnetic?
8.55
Order the following elements by increasing atomic radius according to what you expect from periodic trends: Se,
S, As.
8.57
Using periodic trends, arrange the following elements by increasing ionization energy: Ar, Na, Cl, Al.
8.63
Write the complete ground-state electron configuration of the strontium atom, Sr, using the building-up
principle.
8.71
Using the Figure below, predict the first ionization energy of francium (Z = 87).
8.73
Write the orbital diagram corresponding to the ground state of Nb, whose configuration is [Kr]4d45s1.
8.75
Match each set of characteristics on the left with an element in the column at the right.
a. A reactive nonmetal; the atom has a
large negative electron affinity
b. A soft metal; the atom has low
ionization energy
c. A metalloid that forms an oxide of
formula R2O3
d. A chemically unreactive gas
8.83
Sodium (Na)
Antimony (Sb)
Argon(Ar)
Chlorine (Cl2)
How much energy would be required to ionize 5.00 mg of Na(g) atoms to Na+(g) ions? The first ionization energy
of Na atoms is 496 kJ/mol.