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Chapter 8: Problem 62

Specify which of the following elements you would expect to have the greatest electron affinity and which would have the least: \(\mathrm{He}, \mathrm{K}, \mathrm{Co}, \mathrm{S}, \mathrm{Cl}\)

Short Answer

Expert verified
Among these elements, Chlorine (\( \mathrm{Cl} \)) would have the greatest electron affinity due to its position in Group 17 (Halogens), while Helium (\( \mathrm{He} \)), a noble gas, would have the least electron affinity despite being to the right of the.periodic table, due to its stable full-shell electron configuration.

Step by step solution

01

Determine the group for each element

Firstly, locate these elements in the periodic table. Hydrogen \( \mathrm{He} \) is a noble gas, Potassium \( \mathrm{K} \) belongs to group 1 (alkali metals), Cobalt \( \mathrm{Co} \) is a transition metal, Sulphur \( \mathrm{S} \) is in group 16 (oxygen group, chalcogens), and Chlorine \( \mathrm{Cl} \) is in group 17 (halogens).
02

Apply the periodic trends for electron affinity

Generally, across a period from left to right in the periodic table, atom size decreases and nuclear charge increases, which results in higher electron affinity (more energy is released when an electron is added). Therefore, halogens (\( \mathrm{Cl} \)) have the highest electron affinity. Through a group, the increase in atomic size results in a decrease in electron affinity. Therefore, alkali metals (\( \mathrm{K} \)) usually have the lowest electron affinity.
03

Consider the exceptions

But noble gases (\( \mathrm{He} \)) are the exception to this trend. With a complete outer electron shell, they do not usually accept additional electrons, so their electron affinity is actually lower than alkali metals.

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Most popular questions from this chapter

In general, ionization energy increases from left to right across a given period. Aluminum, however, has a lower ionization energy than magnesium. Explain.

On the basis of their positions in the periodic table, select the atom with the larger atomic radius in each of the following pairs: (a) \(\mathrm{Na}, \mathrm{Cs} ;\) (b) \(\mathrm{Be}, \mathrm{Ba} ;\) (c) \(\mathrm{N}\), \(\mathrm{Sb} ;(\mathrm{d}) \mathrm{F}, \mathrm{Br} ;(\mathrm{e}) \mathrm{Ne}, \mathrm{Xe}\)

List all the common ions of representative elements and transition metals that are isoelectronic with Ar.

Based on your knowledge of the chemistry of the alkali metals, predict some of the chemical properties of francium, the last member of the group.

Arrange the following in order of increasing first ionization energy: \(\mathrm{F}, \mathrm{K}, \mathrm{P}, \mathrm{Ca},\) and \(\mathrm{Ne} .\)
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