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Chapter 7: Problem 38

The changes in electron affinity as one goes down a group in the periodic table are not nearly as large as the variations in ionization energies. Why?

Short Answer

Expert verified
The changes in electron affinity down a group in the periodic table are not as large as the variations in ionization energies because electron affinity is less affected by the shielding effect and the atomic radius. Although both ionization energy and electron affinity decrease down a group due to increased shielding and atomic radius, electron affinity experiences smaller variations since the added electrons enter the same outer orbital, leading to similar affinities for elements within the group. On the other hand, ionization energy experiences more prominent variations due to the greater impact of increased distance and shielding effect on electron removal.

Step by step solution

01

Definition of Electron Affinity and Ionization Energy

Electron affinity is the amount of energy released when an electron is added to a neutral atom to form a negatively charged ion, while ionization energy is the energy required to remove an electron from a neutral atom to form a positively charged ion. Both of these properties are determined by the effective nuclear charge and the distance between the electrons and the nucleus.
02

Factors Affecting Electron Affinity and Ionization Energy

As we move down a group in the periodic table, the number of electron shells (energy levels) increases. This increases the shielding effect, which is the ability of the inner shell electrons to shield the outer shell electrons from the attraction of the nucleus. Additionally, the atomic radius (distance between the nucleus and the outermost electron) increases, causing a decrease in the effective nuclear charge experienced by the outer electrons.
03

Variation in Ionization Energy Down a Group

The increase in the shielding effect and the atomic radius down a group results in a decrease in the ionization energy. The outermost electrons become less tightly held by the nucleus, making it easier to remove them from the atom. Therefore, ionization energy generally decreases down a group in the periodic table.
04

Variation in Electron Affinity Down a Group

Electron affinity is affected by the shielding effect and the atomic radius in a similar manner. As we go down a group, the increase in the shielding effect and the atomic radius causes electron affinity to decrease. However, some elements in the same group share a similar electron affinity because the added electron enters the same outer orbital. This decreases the impact of those variations down the group.
05

Comparison of Variations in Ionization Energy and Electron Affinity

The variations in ionization energy are more prominent due to the increased distance between the outermost electron and the nucleus and the stronger shielding effect as we move down the group. However, electron affinity is less affected by these factors as the added electrons are entering the same outer orbital, causing smaller variations within the group. This is why changes in electron affinity down a group are not as large as variations in ionization energies.

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Most popular questions from this chapter

An unknown element is a nonmetal and has a valence electron configuration of \(n s^{2} n p^{4} .\) a. How many valence electrons does this element have? b. What are some possible identities for this element? c. What is the formula of the compound this element would form with potassium? d. Would this element have a larger or smaller radius than barium? e. Would this element have a greater or smaller ionization energy than fluorine?

The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize these values in terms of electron configurations.

Write equations corresponding to the following. a. the fourth ionization energy of Se b. the electron affinity of \(\mathrm{S}^{-}\) c. the electron affinity of \(\mathrm{Fe}^{3+}\) d. the ionization energy of Mg

The ionization energy for a 1\(s\) electron in a silver atom is $2.462 \times 10^{6} \mathrm{kJ} / \mathrm{mol} .$ a. Determine an approximate value for \(Z_{\text { eff }}\) for the \(A g 1 s\) electron. Assume the Bohr model applies to the 1 s electron. \(Z_{\mathrm{eff}}\) is the apparent nuclear charge experienced by the electrons. b. How does \(Z_{\text { eff }}\) from part a compare to \(Z\) for Ag? Rationalize the relative numbers.

What is the physical significance of the value of \(\psi^{2}\) at a particular point in an atomic orbital?
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