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.
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter6: The Periodic Table And Periodic Law
Section: Chapter Questions
Problem 66A
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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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