Solution Found!
Answer: Indicate which one of the two species in each of
Chapter 8, Problem 43P(choose chapter or problem)
Indicate which one of the two species in each of the following pairs is smaller:
(a) Cl or \(\mathrm{Cl}^{-}\)
(b) Na or \(\mathrm{Na}^{+}\)
(c) \(\mathrm{O}^{2-}\) or \(\mathrm{S}^{2-}\)
(d) \(\mathrm{Mg}^{2+}\) or \(\mathrm{Al}^{3+}\)
(e) \(\mathrm{Au}^{+}\) or \(\mathrm{Au}^{3+}\)
Questions & Answers
QUESTION:
Indicate which one of the two species in each of the following pairs is smaller:
(a) Cl or \(\mathrm{Cl}^{-}\)
(b) Na or \(\mathrm{Na}^{+}\)
(c) \(\mathrm{O}^{2-}\) or \(\mathrm{S}^{2-}\)
(d) \(\mathrm{Mg}^{2+}\) or \(\mathrm{Al}^{3+}\)
(e) \(\mathrm{Au}^{+}\) or \(\mathrm{Au}^{3+}\)
ANSWER:Step 1 of 6
The atomic size increases down the group due to the number of shells adding electrons to the outermost shell. On the other side, the atomic size decreases on moving from left to right across a period because of the increase in the effective nuclear charge as electrons are added to the same shell. For charged species, the higher is the positive charge lesser is the atomic size. For negatively charged species, higher is the