Periodic Properties Worksheet Key Page 2
ADVERTISEMENT
1
2
3
42
5. State which atom has a smaller first ionization energy according to periodic trends.
a) O, S
S
b) K, Na
K
c) Cd, Zn
Cd
d) Al, Ga
Ga
6. Explain the difference in ionization energy for each of the pairs in Problem 5.
The outer electrons of the atom with the smaller ionization are in a subshell further
away from the nucleus than the outer electrons of the atom with the larger ionization
energy.
7. State which atom has a larger ionization energy according to periodic trends.
a) Ba, Cs
Ba
b) Cl, S
Cl
c) Sc, Ti
Ti
d) Sb, Sn
Sb
8. Explain the difference in size for each of the pairs in Problem 8.
The outer electrons of both atoms are in the same subshell; however, the atom with
the larger ionization has a greater nuclear charge that attracts the electrons closer to
the nucleus making the electrons more difficult to remove.
9. Explain why the second ionization energy of rubidium is higher than the second ionization
energy of strontium.
The second electron removed from the rubidium atom is from the 4p subshell;
whereas, the second electron removed from strontium is from the 5s subshell. Since
the 4p subshell has a lower energy (a more negative energy) than the 5s subshell,
the second ionization energy of rubidium is much greater than the second ionization
energy of strontium.
ADVERTISEMENT
0 votes
