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Chapter 8: Problem 129

Why do elements that have high ionization energies also have more positive electron affinities? Which group of elements would be an exception to this generalization?

Short Answer

Expert verified
Elements with high ionization energies also tend to have positive electron affinities because both properties reflect the capability of an atom to hold onto and attract electrons. The exception to this rule is the noble gases, which have high ionization energies but not positive electron affinities due to their stable electron configuration.

Step by step solution

01

Understanding High Ionization Energies

High ionization energies imply that an element holds its electrons very tightly. This is because ionization energy is the energy required to remove an electron from a neutral atom in its gaseous phase. The stronger the hold an atom has on its electron, the more energy it requires to remove the electron, and thus, it has a higher ionization energy.
02

Understanding Positive Electron Affinities

Electron affinity is the amount of energy released when an electron is added to a neutral atom to form a negative ion. Therefore, if an element has positive electron affinity, it means the energy is released when an electron is added, i.e., the atom naturally tends to accept electrons.
03

Correlation Between High Ionization Energies and Positive Electron Affinities

Because atom's outermost electrons contribute to both ionization energy and electron affinity, elements that have high ionization energies tend to also have positive electron affinities. This is because both of these properties reflect the electron-holding capability and attraction force of an atom.
04

Identifying Exception

The noble gases, found in Group 18 of the Periodic Table, are an exception to this correlation. Their outermost electron layer is full, so they have high ionization energies because they hold their electrons tightly. However, because they already have a stable electron configuration, they do not naturally tend to accept electrons and thus do not have positive electron affinities.

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Most popular questions from this chapter

You are given four substances: a fuming red liquid, a dark metallic-looking solid, a pale-yellow gas, and a yellow-green gas that attacks glass. You are told that these substances are the first four members of Group 7A, the halogens. Name each one.

What is the electron affinity of the \(\mathrm{Na}^{+}\) ion?

Both \(\mathrm{H}^{-}\) and He contain two \(1 s\) electrons. Which species is larger? Explain your choice.

Which of the following species are isoelectronic with each other? \(\mathrm{C}, \mathrm{Cl}^{-}, \mathrm{Mn}^{2+}, \mathrm{B}^{-}, \mathrm{Ar}, \mathrm{Zn}, \mathrm{Fe}^{3+}, \mathrm{Ge}^{2+}\)

Group the species that are isoelectronic: \(\mathrm{Be}^{2+}, \mathrm{F}^{-}\) \(\mathrm{Fe}^{2+}, \mathrm{N}^{3-}, \mathrm{He}, \mathrm{S}^{2-}, \mathrm{Co}^{3+}, \mathrm{Ar}\)
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