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Chapter 7: Problem 50

If the electron affinity for an element is a negative number, does it mean that the anion of the element is more stable than the neutral atom? Explain.

Short Answer

Expert verified
Yes, if the electron affinity for an element is a negative number, it means that the anion of the element is more stable than the neutral atom. This is because a negative electron affinity value indicates that energy is released during the formation of the anion, which corresponds to the stabilization of the anionic species.

Step by step solution

01

Understand electron affinity

Electron affinity is the energy change that occurs when an electron is added to a neutral atom to form a negative ion. In other words, it's the amount of energy released (exothermic process) or absorbed (endothermic process) when an electron is added to an atom. Electron affinity is usually expressed in units of kJ/mol.
02

Identify the meaning of negative electron affinity

When an element has a negative electron affinity, it means that energy is released when an electron is added to the neutral atom, making the process exothermic. A negative electron affinity indicates that the negatively charged ion (anion) formed after the addition of an electron is more stable than the neutral atom because it involves a release of energy, which is associated with the formation of more stable species.
03

Explain the relationship between electron affinity and anion stability

An anion is more stable than the neutral atom if its formation is accompanied by the release of energy, resulting in a negative electron affinity value for the element. This is because the electron being added to the atom can stabilize the anion by lowering its overall energy, and this stabilization is achieved through the release of energy (which corresponds to a negative electron affinity value). In conclusion, if an element has a negative electron affinity, it means that the anion of the element is indeed more stable than the neutral atom. The negative electron affinity value indicates that energy is released during the formation of the anion, and this energy release is associated with the stabilization of the anionic species.

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Most popular questions from this chapter

Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. If such an atom does not exist, explain why. (a) \(\mathrm{Cl}^{-}\), (b) \(\mathrm{Sc}^{3+}\), (c) \(\mathrm{Fe}^{2+}\), (d) \(\mathrm{Zn}^{2+}\), (e) \(\mathrm{Sn}^{4+}\).

(a) Why is calcium generally more reactive than magnesium? (b) Why is calcium generally less reactive than potassium?

In the chemical process called electron transfer, an electron is transferred from one atom or molecule to another. (We will talk about electron transfer extensively in Chapter 20.) A simple electron transfer reaction is $$ \mathrm{A}(g)+\mathrm{A}(g) \longrightarrow \mathrm{A}^{+}(g)+\mathrm{A}^{-}(g) $$ In terms of the ionization energy and electron affinity of atom A, what is the energy change for this reaction? For a representative nonmetal such as chlorine, is this process exothermic? For a representative metal such as sodium, is this process exothermic?

Which of the following chemical equations is connected to the definitions of (a) the first ionization energy of oxygen, (b) the second ionization energy of oxygen, and (c) the electron affinity of oxygen? (i) \(\mathrm{O}(g)+\mathrm{e}^{-} \longrightarrow \mathrm{O}^{-}(g)\) (ii) \(\mathrm{O}(g) \longrightarrow \mathrm{O}^{+}(g)+\mathrm{e}^{-}\) (iii) \(\mathrm{O}(g)+2 \mathrm{e}^{-} \longrightarrow \mathrm{O}^{2-}(g)\) (iv) \(\mathrm{O}(g) \longrightarrow \mathrm{O}^{2+}(g)+2 \mathrm{e}^{-}\) (v) \(\mathrm{O}^{+}(g) \longrightarrow \mathrm{O}^{2+}(g)+\mathrm{e}^{-}\)

Chlorine reacts with oxygen to form \(\mathrm{Cl}_{2} \mathrm{O}_{7}\). (a) What is the name of this product (see Table \(2.6\) )? (b) Write a balanced equation for the formation of \(\mathrm{Cl}_{2} \mathrm{O}_{7}(l)\) from the elements. (c) Under usual conditions, \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is a colorless liquid with a boiling point of \(81^{\circ} \mathrm{C}\). Is this boiling point expected or surprising? (d) Would you expect \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) to be more reactive toward \(\mathrm{H}^{+}(a q)\) or \(\mathrm{OH}^{-}(a q)\) ? (e) If the oxygen in \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is considered to have the \(-2\) oxidation state, what is the oxidation state of the \(\mathrm{Cl}\) ? What is the electron configuration of \(\mathrm{Cl}\) in this oxidation state?
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