1. Periodic Properties of the Elements
Chemistry: The Central Science, 10th edition
Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten
Chapter 7
Periodic Properties of the Elements
Todd Austell, The University of North Carolina
 2006, Pearson Prentice Hall

2. The order of atomic masses on the periodic table is in no way related to atomic numbers.
The atomic number depends on the number of protons in the nucleus, while the atomic weight depends (mainly) on the number of both protons and neutrons in the nucleus.
Atomic masses are a function of group numbers on the periodic table and do not increase linearly with atomic number.
For certain midperiodic table elements, the effective mass of each proton in the nucleus varies.

3. The order of atomic masses on the periodic table is in no way related to atomic numbers.
The atomic number depends on the number of protons in the nucleus, while the atomic weight depends (mainly) on the number of both protons and neutrons in the nucleus.
Atomic masses are a function of group numbers on the periodic table and do not increase linearly with atomic number.
For certain midperiodic table elements, the effective mass of each proton in the nucleus varies.

4. The 2p electron of a Ne atom.
This cannot be determined without knowing the charge of the atom.
Both the 2s electron and 2p electron experience the same effective nuclear charge.
The 2s electron of a Na atom.

5. The 2p electron of a Ne atom.
This cannot be determined without knowing the charge of the atom.
Both the 2s electron and 2p electron experience the same effective nuclear charge.
The 2s electron of a Na atom.

6. Yes No

7. Yes No

8. the uncertainty principle the Pauli exclusion principle Hund’s rule
the photoelectric effect
Au – do students need Equations 7.3 and 7.4 to answer this question?

9. the uncertainty principle
the Pauli exclusion principle
Hund’s rule
the photoelectric effect

10. I1 for the boron atom is equal to I2 for the carbon atom.
I2 for the carbon atom is greater.
I1 for the boron atom is greater.

11. I1 for the boron atom is equal to I2 for the carbon atom.
I2 for the carbon atom is greater.
I1 for the boron atom is greater.

12. They have the same electron configuration: [Ar]3d3.
They have different electron configurations.

13. They have the same electron configuration: [Ar]3d3.
They have different electron configurations.

14. EA for Cl is significantly more endothermic than IE1 for Cl.
IE1 for Cl– is significantly more exothermic than EA for Cl.
They are equal in magnitude and opposite in sign.
They are equal in magnitude and sign.

15. EA for Cl is significantly more endothermic than IE1 for Cl.
IE1 for Cl– is significantly more exothermic than EA for Cl.
They are equal in magnitude and opposite in sign.
They are equal in magnitude and sign.

16. There is no correlation between ionization energy and metallic character.
Increasing ionization energy correlates with decreasing metallic character.
Increasing ionization energy correlates with increasing metallic character.
Decreasing ionization energy correlates with decreasing metallic character.

17. There is no correlation between ionization energy and metallic character.
Increasing ionization energy correlates with decreasing metallic character.
Increasing ionization energy correlates with increasing metallic character.
Decreasing ionization energy correlates with decreasing metallic character.

18. molecular
ionic

19. molecular
ionic

20. Sc P

21. Sc P

22. Cs has the lowest ionization energy of the alkali metals.
Cs has the greatest density of the alkali metals.
Cs is the most conductive of the alkali metals.
Cs has the most electrons of the alkali metals.

23. Cs has the lowest ionization energy of the alkali metals.
Cs has the greatest density of the alkali metals.
Cs is the most conductive of the alkali metals.
Cs has the most electrons of the alkali metals.

24. CaCO3 is a very poor source of calcium due to its poor solubility in water.
The dissolution reaction of metal carbonates is catalyzed by enzymes in the intestines.
Metal carbonates are soluble in the acidic environment of the stomach.
Metal carbonate solids can be directly passed into the skeletal system from the stomach.

25. CaCO3 is a very poor source of calcium due to its poor solubility in water.
The dissolution reaction of metal carbonates is catalyzed by enzymes in the intestines.
Metal carbonates are soluble in the acidic environment of the stomach.
Metal carbonate solids can be directly passed into the skeletal system from the stomach.

26. It is not possible to use the data in Table 7
It is not possible to use the data in Table 7.7 to determine the characteristics of astatine.
Yes, by extrapolating from the other data, we can estimate that the atomic radius is approximately 1.10 angstroms and I1 must be approximately 1000 kJ/mol.
Yes, by extrapolating from the other data, we can estimate that the atomic radius is approximately 1.5 angstroms and I1 must be approximately 900 kJ/mol.

27. It is not possible to use the data in Table 7
It is not possible to use the data in Table 7.7 to determine the characteristics of astatine.
Yes, by extrapolating from the other data, we can estimate that the atomic radius is approximately 1.10 angstroms and I1 must be approximately 1000 kJ/mol.
Yes, by extrapolating from the other data, we can estimate that the atomic radius is approximately 1.5 angstroms and I1 must be approximately 900 kJ/mol.