1. Principles & Modern Applications
General Chemistry
Principles & Modern Applications
9th Edition
Petrucci/Harwood/Herring/Madura
Chapter 9
The Periodic Table and Some Atomic Properties
Dr. Travis D. Fridgen
Memorial University of Newfoundland
© 2007 Pearson Education

2. Which group has the elements listed in order of increasing atomic radius?
1. Al, P, Cl, Ar
2. Rb, Sr, Ca, Mg
3. N, P, S, Se
4. Ne, Ar, Cl, Br
5. H, He, Ne, Ar

3. Which group has the elements listed in order of increasing atomic radius?
1. Al, P, Cl, Ar
2. Rb, Sr, Ca, Mg
3. N, P, S, Se
4. Ne, Ar, Cl, Br
5. H, He, Ne, Ar

4. Which group in the periodic table is the element with the following ionization energies most likely be found.
1st IE = kJ mol-1
2nd IE = kJ mol-1
3rd IE = kJ mol-1
4th IE = kJ mol-1
5th IE = kJ mol-1
6th IE = kJ mol-1
1. Gr. 2
2. Gr. 13
3. Gr. 14
4. Gr. 16
5. Gr. 18

5. Which group in the periodic table is the element with the following ionization energies most likely be found.
1st IE = kJ mol-1
2nd IE = kJ mol-1
3rd IE = kJ mol-1
4th IE = kJ mol-1
5th IE = kJ mol-1
6th IE = kJ mol-1
1. Gr. 2
2. Gr. 13
3. Gr. 14
4. Gr. 16
5. Gr. 18

6. The most preferential oxidation state for tin and the ion’s electron configuration is,
1. I, [Kr]5s25p14d10
2. II, [Kr]5p24d10
3. II, [Kr]5s24d10
IV, [Kr]5s25p64d10
5. -I, [Kr]5s25p34d10

7. The most preferential oxidation state for tin and the ion’s electron configuration is,
1. I, [Kr]5s25p14d10
2. II, [Kr]5p24d10
3. II, [Kr]5s24d10
IV, [Kr]5s25p64d10
5. -I, [Kr]5s25p34d10

8. The most preferential oxidation state for gold and the ion’s electron configuration is,
1. I, [Xe]6s25d8
2. II, [Xe]5d9
3. I, [Xe]5d10
I, [Xe]6s25d10
I, [Xe]5d106p3

9. The most preferential oxidation state for gold and the ion’s electron configuration is,
1. I, [Xe]6s25d8
2. II, [Xe]5d9
3. I, [Xe]5d10
I, [Xe]6s25d10
I, [Xe]5d106p3

10. Which of the following has the smallest radius?
1. Li+
2. Li
3. O2-
4. Be2+
5. Ne

11. Which of the following has the smallest radius?
1. Li+
2. Li
3. O2-
4. Be2+
5. Ne

12. Which of the following lists has the species increasing in radius?
1. Kr, Ar, Cl-, S2-
2. Li+, Be2+, B3+
3. I-, Br-, Cl-, F-
4. F-, O2-, N3-, P3-
5. Cl-, S2-, P3-, Al3+

13. Which of the following lists has the species increasing in radius?
1. Kr, Ar, Cl-, S2-
2. Li+, Be2+, B3+
3. I-, Br-, Cl-, F-
4. F-, O2-, N3-, P3-
5. Cl-, S2-, P3-, Al3+

14. Which of the following species is most likely to accept another electron?
1. Ar
2. O
3. O-
4. N
5. C

15. Which of the following species is most likely to accept another electron?
1. Ar
2. O
3. O-
4. N
5. C

16. Below is an example of a charge exchange reaction between atomic oxygen and the krypton cation. These reactions are possible if they are exothermic. The ionization energies of Kr and O are 1350 and 1312 kJ mol-1, respectively. Is the charge exchange reaction shown below exothermic or endothermic? O Kr
Kr+ O+ + +
1. Exothermic
2. Endothermic
3. Not enough information given

17. Below is an example of a charge exchange reaction between atomic oxygen and the krypton cation. These reactions are possible if they are exothermic. The ionization energies of Kr and O are 1350 and 1312 kJ mol-1, respectively. Is the charge exchange reaction shown below exothermic or endothermic? O Kr
Kr+ O+ + +
1. Exothermic
2. Endothermic
3. Not enough information given

18. In general the ionization energy increases going across a period
In general the ionization energy increases going across a period. However, as seen to the right, the ionization energy of Al is considerably smaller than that of Mg. The best explanation for this is
1. Al is a smaller atom than Mg.
2. s electrons penetrate closer to the nucleus and therefore shield p electrons more effectively.
the electrons in Mg are farther from the nucleus than in Al.
4. Al is a larger atom than Mg since its electrons are less tightly held to the nucleus.

19. In general the ionization energy increases going across a period
In general the ionization energy increases going across a period. However, as seen to the right, the ionization energy of Al is considerably smaller than that of Mg. The best explanation for this is
1. Al is a smaller atom than Mg.
2. s electrons penetrate closer to the nucleus and therefore shield p electrons more effectively.
the electrons in Mg are farther from the nucleus than in Al.
4. Al is a larger atom than Mg since its electrons are less tightly held to the nucleus.

20. P2 P3 P4
Generally, the ionization energies increase going across a period as shown to the right. The best explanation is
The charge on the nucleus increases so the electrons are more attracted to the nucleus.
2. The atoms’ radii increase as you go across the periodic table.
3. The atoms’ radii decrease as you go across the periodic table.
4. Electrons in the same shell do not shield each other completely so the effective nuclear charge is felt by each additional electron is greater.

21. P2 P3 P4
Generally, the ionization energies increase going across a period as shown to the right. The best explanation is
The charge on the nucleus increases so the electrons are more attracted to the nucleus.
2. The atoms’ radii increase as you go across the periodic table.
3. The atoms’ radii decrease as you go across the periodic table.
4. Electrons in the same shell do not shield each other completely so the effective nuclear charge is felt by each additional electron is greater.

22. The ionization energy decreases as you go down any group in the periodic table as shown for the rare gases and chalcogens to the right. The best explanation for this trend is…
As you go down the periodic table metallic character of the elements increases.
Atomic radius decreases as you go down the periodic table.
The electrons in the outer shell are further from the nucleus and are effectively shielded by the core electrons.
The charge on the nucleus increases so the electrons are more attracted to the nucleus.

23. The ionization energy decreases as you go down any group in the periodic table as shown for the rare gases and chalcogens to the right. The best explanation for this trend is
As you go down the periodic table metallic character of the elements increases.
Atomic radius decreases as you go down the periodic table.
The electrons in the outer shell are further from the nucleus and are effectively shielded by the core electrons.
The charge on the nucleus increases so the electrons are more attracted to the nucleus.

24. Which of the following atoms would you expect to be diamagnetic?18 Ar
39.948 20 Ca
40.078 30 Zn
65.39 35 Br
79.904
1. Ar, Ca and Zn only
4. Ar only
2. Ar and Br only
5. All are diamagnetic
3. Zn and Ca only

25. Which of the following atoms would you expect to be diamagnetic?18 Ar
39.948 20 Ca
40.078 30 Zn
65.39 35 Br
79.904
1. Ar, Ca and Zn only
4. Ar only
2. Ar and Br only
5. All are diamagnetic
3. Zn and Ca only

26. Both Mn2+ and Fe3+ are the same and more paramagnetic than Mn
Which of the following species would you expect to be most paramagnetic?
1. Mn 25 Mn
2. Mn2+
3. Fe3+ 26 Fe
55.847
Both Mn2+ and Fe3+ are the same and more paramagnetic than Mn
5. All have the same paramagnetism.

27. Both Mn2+ and Fe3+ are the same and more paramagnetic than Mn
Which of the following species would you expect to be most paramagnetic?
1. Mn 25 Mn
2. Mn2+
3. Fe3+ 26 Fe
55.847
Both Mn2+ and Fe3+ are the same and more paramagnetic than Mn
5. All have the same paramagnetism.

28. Which of the following reactions would you expect to be the most vigorous?

29. Which of the following reactions would you expect to be the most vigorous?