Chapter 8- home assignments-periodic properties
7. The electron configuration of a copper(I) ion is
8. The cobalt(III) ion, Co3+, has how many 3d electrons?
9. Which of the atoms listed below has the largest radius?
10. For which of the following reactions is the enthalpy change equal to the second ionization
energy of nitrogen?
A. N2+(g) → N3+(g) + e–
B. N2+(g) + e– →N+(g)
C. N(g) →N2+(g) + 2e–
D. N–(g) + e– → N2–(g)
E. N+(g) →N2+(g) + e–
11. Which of the elements listed below has the highest first ionization energy?
16. Which of the following elements has the greatest metallic character?
17. Which of the following is a basic oxide?
19. Which, if any, is the ground-state electron configuration for S2–?
A. [Ne] or 1s22s22p63s23p6
B. [Ar] or 1s22s22p63s23p6
D. [Ar] or 1s22s22p63s23p4
E. None of the above
20. Which, if any, is the ground-state electron configuration for Mg2+?
A. [Ne] or 1s22s22p6
B. [Ar] or 1s22s22p6
D. [Ne]3s23p2 or 1s22s22p63s23p2
E. None of the above
21. The following successive ionization energies correspond to an element in the third row of the
periodic table: I1 = 786.3 kJ/mol, I2 =1,580 kJ/mol, I3= 3,230 kJ/mol, I4 = 4,360 kJ/mol, I5 =
16,000, and I6 = 20,000 kJ/mol. Based on this pattern of ionization energies, identify the
E. None of the above
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