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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
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 energy is released when an electron is added to the neutral atom, which contributes to the stability of the anion. The larger the negative electron affinity value, the more stable the anion of that element is compared to the neutral atom.

Step by step solution

01

Define Electron Affinity

Electron affinity is the amount of energy released or absorbed when an electron is added to an isolated gaseous atom to form a negatively charged ion or anion. It is expressed in units of kilojoules per mole (kJ/mol).
02

Explain Negative and Positive Electron Affinities

If the electron affinity of an element is negative, it means that energy is released when the electron is added to the neutral atom, making the anion more stable. On the other hand, if the electron affinity is positive, it means that energy is absorbed when the electron is attached to the atom, making the formed anion less stable than the neutral atom.
03

Relate Electron Affinity to Stability of Anions

The larger the negative electron affinity value of an element, the more energy is released when the electron is attached to the neutral atom, and hence, the more stable is the anion of that element. This indicates that the anion is more stable than the neutral atom.
04

Answering the Exercise

So, if the electron affinity for an element is a negative number, it means that the anion of the element is indeed more stable than the neutral atom because energy is released in the process of the anion formation. This energy release contributes to the stability of the anion compared to the neutral atom.

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Most popular questions from this chapter

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Lithium is added to water. (b) Calcium is added to water. (c) Potassium reacts with chlorine gas. (d) Rubidium reacts with oxygen.

Detailed calculations show that the value of \(Z_{\text {eff }}\) for the outermost electrons in \(\mathrm{Si}\) and \(\mathrm{Cl}\) atoms is \(4.29+\) and \(6.12+,\) respectively. (a) What value do you estimate for \(Z_{\text {eff }}\) experienced by the outermost electron in both Si and Cl by assuming core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant? (b) What values do you estimate for \(Z_{\text {eff }}\) using Slater's rules? (c) Which approach gives a more accurate estimate of \(Z_{\text {eff }} ?\) (d) Which method of approximation more accurately accounts for the steady increase in \(Z_{\text {eff }}\) that occurs upon moving left to right across a period? (e) Predict \(Z_{\text {eff }}\) for a valence electron in P, phosphorus, based on the calculations for \(\mathrm{Si}\) and \(\mathrm{Cl}\).

Using only the periodic table, arrange each set of atoms in order from largest to smallest: \((\mathbf{a}) \mathrm{Ar},\) As, \(\mathrm{Kr} ;\) (b) $\mathrm{Cd}, \mathrm{Rb}, \mathrm{Te} ;(\mathbf{c})$ \(\mathrm{C}, \mathrm{Cl}, \mathrm{Cu}\).

What is the relationship between the ionization energy of an anion with a 1 - charge such as \(\mathrm{F}^{-}\) and the electron affinity of the neutral atom, \(\mathrm{F}\) ?

Which neutral atom is isoelectronic with each of the following ions? \(\mathrm{H}^{-}, \mathrm{Ca}^{2+}, \mathrm{In}^{3+}, \mathrm{Ge}^{2+}\)
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