Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 14

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 Cl \(^{-}\) ion. c. the Cl \(^{+}\) ion. d. the F atom. e. none of these. Explain each choice. Justify your choice, and for the choices you did not select, explain what is incorrect about them.

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 Cl\(^{-}\) ion. This is because when an electron is added to the Cl atom, it forms a Cl\(^{-}\) ion and releases energy, which is equivalent to the energy required to remove the same electron from the Cl\(^{-}\) ion to form the neutral Cl atom.

Step by step solution

01

Analyze Option a

Option a suggests that the ionization energy of the chlorine atom is equal to the electron affinity of the Cl atom. However, this is not the case. Ionization energy is the energy required to remove an electron while electron affinity is the energy change when an electron is added. These two processes are not equal in the case of the same atom.
02

Analyze Option b

Option b suggests that the ionization energy of the chlorine atom is equal to the electron affinity of the Cl\(^{-}\) ion. This option is correct. When electron is added to the Cl atom, it forms a Cl\(^{-}\) ion and releases energy, which is equivalent to the energy required to remove the same electron from the Cl\(^{-}\) ion to form the neutral Cl atom. The ionization energy for chlorine is thus equal in magnitude to the electron affinity for the Cl\(^{-}\) ion.
03

Analyze Option c

Option c suggests that the ionization energy of the chlorine atom is equal to the electron affinity of the Cl\(^{+}\) ion. This is incorrect because ionization energy is related to the removal of an electron and electron affinity is related to the addition of an electron. The electron affinity of the Cl\(^{+}\) ion, however, is related to the energy change when an electron is added to the Cl\(^{+}\) ion, not when it is removed.
04

Analyze Option d

Option d suggests that the ionization energy of the chlorine atom is equal to the electron affinity of the F atom. This is incorrect because ionization energy and electron affinity are properties that depend on the specific element and its electronic configuration. The ionization energy of chlorine and the electron affinity of fluorine are not related in terms of magnitude.
05

Analyze Option e

Option e suggests that none of the given choices are correct. Since we have already determined that option b is the correct choice, option e is incorrect.
06

Conclusion

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

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

In the ground state of mercury, Hg, a. how many electrons occupy atomic orbitals with \(n=3 ?\) b. how many electrons occupy \(d\) atomic orbitals? c. how many electrons occupy \(p_{z}\) atomic orbitals? d. how many electrons have spin "up" " \(\left(m_{s}=+\frac{1}{2}\right) ?\)

Write the expected electron configurations for each of the following atoms: Cl, Sb, Sr, W, Pb, Cf.

When the excited electron in a hydrogen atom falls from \(n=5\) to \(n=2,\) a photon of blue light is emitted. If an excited electron in He \(^{+}\) falls from \(n=4,\) to which energy level must it fall so that a similar blue light (as with the hydrogen) is emitted? Prove it. (See Exercise \(174 . )\)

Consider the ground state of arsenic, As. How many electrons have \(\ell=1\) as one of their quantum numbers? How many electrons have \(m_{\ell}=0 ?\) How many electrons have \(m_{\ell}=+1 ?\)

Small daily doses of lithium carbonate taken orally are often given to treat manic-depressive psychoses. This dosage maintains the level of lithium ion in the blood at about \(1 \times 10^{-3} \mathrm{mol} / \mathrm{L}\) . a. What is the formula of lithium carbonate? b. What mass of lithium ion is present per liter of blood in these patients?
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free