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Chapter 2: Problem 10

Choose the best response for the following. The ionization energy for the chlorine atom is equal in magnitude to the electron affinity for a. the Cl atom. b. the \(\mathrm{Cl}^{-}\) ion. c. the \(\mathrm{Cl}^{+}\) ion. d. the \(F\) atom. e. none of these.

Short Answer

Expert verified
The correct answer is b. The ionization energy for the chlorine atom is equal in magnitude to the electron affinity for the \(\mathrm{Cl}^{-}\) ion.

Step by step solution

01

Option a: The Cl atom

Since chlorine has a high electron affinity, adding an electron to a Cl atom will release a significant amount of energy. However, removing an electron from the Cl atom would require even more energy, as it has a high ionization energy. So, ionization energy for the chlorine atom is not equal to the electron affinity for the Cl atom.
02

Option b: The \(\mathrm{Cl}^{-}\) ion

The chlorine atom gains an electron to become the \(\mathrm{Cl}^-\) ion, which corresponds to its electron affinity. On the other hand, the ionization energy of the \(\mathrm{Cl}^-\) ion corresponds to the requirement of removing an electron from the \(\mathrm{Cl}^-\) ion, returning it to its neutral state (Cl atom). In this case, the ionization energy of \(\mathrm{Cl}^-\) is equal to the electron affinity of the Cl atom.
03

Option c: The \(\mathrm{Cl}^{+}\) ion

Removing an electron from the Cl atom will result in the formation of \(\mathrm{Cl}^+\) ion, which refers to its ionization energy. However, the electron affinity of \(\mathrm{Cl}^+\) is not equal to the ionization energy of the Cl atom since adding an electron to a \(\mathrm{Cl}^+\) ion yields a Cl atom, which has a higher electron affinity than the ionization energy for the \(\mathrm{Cl}^+\) ion.
04

Option d: The \(F\) atom

Fluorine has a higher electron affinity compared to chlorine and an even higher ionization energy than chlorine. Therefore, ionization energy of chlorine is not equal to the electron affinity of the \(F\) atom.
05

Option e: None of these

Only one answer should be correct, so option e could not be that answer since an earlier option is the correct response. Based on the analysis, the correct answer is: b. The \(\mathrm{Cl}^-\) ion.

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Most popular questions from this chapter

Identify the following elements. a. An excited state of this element has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{5} 3 s^{1}\). b. The ground-state electron configuration is \([\mathrm{Ne}] 3 s^{2} 3 p^{4}\). c. An excited state of this element has the electron configuration \([\mathrm{Kr}] 5 s^{2} 4 d^{6} 5 p^{2} 6 s^{1}\). d. The ground-state electron configuration contains three unpaired \(6 p\) electrons.

For each of the following pairs of elements $$ (\mathrm{C} \text { and } \mathrm{N}) \quad(\mathrm{Ar} \text { and } \mathrm{Br}) $$ pick the atom with a. more favorable (more negative) electron affinity. b. higher ionization energy. c. larger size.

In the second row of the periodic table, \(\mathrm{Be}, \mathrm{N},\) and \(\mathrm{Ne}\) all have positive (unfavorable) electron affinities, whereas the other second-row elements have negative (favorable) electron affinities. Rationalize why Be, \(N,\) and Ne have unfavorable electron affinities.

How many orbitals in an atom can have the designation \(5 p,\) \(3 d_{z}, 4 d, n=5, n=4 ?\)

As the weapons officer aboard the Starship Chemistry, it is your duty to configure a photon torpedo to remove an electron from the outer hull of an enemy vessel. You know that the work function (the binding energy of the electron) of the hull of the enemy ship is \(7.52 \times 10^{-19} \mathrm{J}\) a. What wavelength does your photon torpedo need to be to eject an electron? b. You find an extra photon torpedo with a wavelength of \(259 \mathrm{nm}\) and fire it at the enemy vessel. Does this photon torpedo do any damage to the ship (does it eject an electron)? c. If the hull of the enemy vessel is made of the element with an electron configuration of \([\mathrm{Ar}] 4 s^{1} 3 d^{10},\) what metal is this?
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