Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 7 - Periodic Properties of the Elements - Exercises: 7.18

Answer

For an electron in $n=3$, $$Z_{eff}(Mg)\lt Z_{eff}(P)\lt Z_{eff}(K)\lt Z_{eff}(Ti)\lt Z_{eff}(Rh)$$

Work Step by Step

We know that the effective nuclear charge $Z_{eff}$ for an electron would increase from left to right in a row in the periodic table, for the increase in nuclear charge. Therefore, - Row 3: $Z_{eff}(P)\gt Z_{eff}(Mg)$ - Row 4: $Z_{eff}(Ti)\gt Z_{eff}(K)$ Also, as we go down in the periodic table, the nuclear charge would dramatically increase, while the screening effect is almost the same for electrons in $n=3$, since the number of electrons in $n=1,2, 3$ stays the same. So, the effective nuclear charge would increase as we go down. Therefore, for an electron in $n=3$, $$Z_{eff}(Mg)\lt Z_{eff}(P)\lt Z_{eff}(K)\lt Z_{eff}(Ti)\lt Z_{eff}(Rh)$$
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