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Answer: Group 4A elements have much more negative electron

Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus ISBN: 9780321910417 77

Solution for problem 92AE Chapter 7

Chemistry: The Central Science | 13th Edition

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Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus

Chemistry: The Central Science | 13th Edition

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Problem 92AE

Group 4A elements have much more negative electron affinities than their neighbors in groups 3A and 5A (see Figure). Which of the following statements best explains this observation? (i) The group 4A elements have much higher first ionization energies than their neighbors in groups 3A and 5A. (ii) The addition of an electron to a group 4A element leads to a half-filled np3 outer electron configuration, (iii) The group 4A elements have unusually large atomic radii (iv) The group 4A elements are easier to vaporize than are the group 3A and 5A elements.

A Figure Electron affinity in kJ/mol for selected s- and p-block elements.

Why are the electron affinities of the Group 4A elements more negative than those of the Group 5A elements?

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13.4-13.5 Monday, January 25, 20168:10 AM Lectures Page 1 Lectures Page 2 Lectures Page 3 Lectures Page 4 Lectures Page 5 Lectures Page 6 Lectures Page 7 Lectures Page 8 Lectures Page 9 13.6-13.7 Wednesday, January 27, 20168:05 AM Lectures Page 1 Lectures Page 2 Lectures Page 3 Lectures Page 4 Lectures Page 5 Lectures Page 6 Lectures Page 7 Lectures Page 8

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Chapter 7, Problem 92AE is Solved
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Textbook: Chemistry: The Central Science
Edition: 13
Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
ISBN: 9780321910417

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Answer: Group 4A elements have much more negative electron