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Chapter 7: Problem 127

Order the atoms in each of the following sets from the least exothermic electron affinity to the most. a. S, Se b. F, Cl, Br, I

Short Answer

Expert verified
a. The order of least exothermic electron affinity to most for S and Se is: Se < S. b. The order for F, Cl, Br, and I is: I < Br < Cl < F.

Step by step solution

01

Identify the position of S and Se in the periodic table

S (Sulfur) and Se (Selenium) are located in Group 16 of the periodic table. Sulfur is in the 3rd period while Selenium is in the 4th period.
02

Determine the trend in electron affinity for S and Se

Since Sulfur and Selenium are in the same group (Group 16), we use the trend that electron affinity decreases as we move down a group. Therefore, Sulfur should have a higher electron affinity than Selenium.
03

Order the atoms from least to most exothermic electron affinity

Based on the trend, the order from least exothermic electron affinity to most exothermic electron affinity should be Se < S. b. Ordering F, Cl, Br, and I based on their electron affinity
04

Identify the position of F, Cl, Br, and I in the periodic table

F (Fluorine), Cl (Chlorine), Br (Bromine), and I (Iodine) are located in Group 17 of the periodic table. They are in the 2nd, 3rd, 4th, and 5th periods, respectively.
05

Determine the trend in electron affinity for F, Cl, Br, and I

Since these atoms are in the same group (Group 17), we can use the trend that electron affinity decreases as we move down a group. As we move down from Fluorine (F) to Iodine (I), the electron affinity should decrease.
06

Order the atoms from least to most exothermic electron affinities

Based on the trend, the order from least exothermic electron affinity to most exothermic electron affinity should be I < Br < Cl < F.

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Most popular questions from this chapter

Write the expected ground-state electron configuration for the following: a. the element with one unpaired 5\(p\) electron that forms a covalent with compound fluorine b. the (as yet undiscovered) alkaline earth metal after radium c. the noble gas with electrons occupying 4f orbitals d. the first-row transition metal with the most unpaired electrons

Valence electrons are those electrons in the outermost principal quantum level (highest n level) of an atom in its ground state. Groups 1A to 8A have from 1 to 8 valence electrons. For each group of the representative elements (1A–8A), give the number of valence electrons, the general valence electron configuration, a sample element in that group, and the specific valence electron configuration for that element.

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