The ionic radii of K+, Cl−, and S2− are 138, 181, and 184 pm, respectively. Which of the following statements best describes why these isoelectronic species have different radii? Select one: a. The radii of Cl− and S2− are sufficiently close that there is no suitable explanation to explain the variances in ionic radii. b. The effective nuclear charge of the ions determines the size of the radii. c. Alkali metals always have smaller radii that p-block elements. d. There is no explanation to explain why these species have different radii.
The ionic radii of K+, Cl−, and S2− are 138, 181, and 184 pm, respectively. Which of the following statements best describes why these isoelectronic species have different radii? Select one: a. The radii of Cl− and S2− are sufficiently close that there is no suitable explanation to explain the variances in ionic radii. b. The effective nuclear charge of the ions determines the size of the radii. c. Alkali metals always have smaller radii that p-block elements. d. There is no explanation to explain why these species have different radii.
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter11: Modern Atomic Theory
Section: Chapter Questions
Problem 75A
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The ionic radii of K+, Cl−, and S2− are 138, 181, and 184 pm, respectively. Which of the following statements best describes why these isoelectronic species have different radii?
Select one:
a.
The radii of Cl− and S2− are sufficiently close that there is no suitable explanation to explain the variances in ionic radii.
b.
The effective nuclear charge of the ions determines the size of the radii.
c.
Alkali metals always have smaller radii that p-block elements.
d.
There is no explanation to explain why these species have different radii.
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