Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 41

Identify each statement as true or false. If it is false, rewrite it so that it is true: (a) Ionization energies are always negative quantitites. (b) Oxygen has a larger first ionization energy than fluorine. (c) The second ionization energy of an atom is always greater than its first ionization energy.

Short Answer

Expert verified
(a) False. Corrected statement: "Ionization energies are always positive quantities." (b) False. Corrected statement: "Fluorine has a larger first ionization energy than oxygen." (c) True. The second ionization energy of an atom is always greater than its first ionization energy.

Step by step solution

01

(a) Verify the statement related to the sign of ionization energies.

Ionization energy is the amount of energy required to remove an electron from an atom in its gaseous state. Since energy is being used to remove an electron, it is a positive quantity. So the statement "Ionization energies are always negative quantities" is false. To rewrite the statement to make it true, we can say: "Ionization energies are always positive quantities."
02

(b) Compare the first ionization energies of oxygen and fluorine.

First ionization energy is the energy required to remove the first electron from an atom. In general, ionization energies increase going across a period (left to right) in the periodic table. Oxygen and Fluorine are both in the same period, with oxygen to the left of fluorine. Therefore, fluorine should have a higher first ionization energy than oxygen. So, the statement "Oxygen has a larger first ionization energy than fluorine" is false. To rewrite the statement to make it true, we can say: "Fluorine has a larger first ionization energy than oxygen."
03

(c) Compare the first and second ionization energies of an atom.

The first ionization energy refers to the energy needed to remove the first valence electron from an atom, while the second ionization energy is the energy needed to remove another electron after the first one has been removed. Since removing an electron makes the atom more positively charged, thus increasing the force of attraction between the remaining electrons and the nucleus, the second ionization energy would be greater than the first ionization energy. Thus, the statement "The second ionization energy of an atom is always greater than its first ionization energy" is true. No changes are needed for this statement.

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

Identify at least two ions that have the following ground-state electron configurations: (a) \([\mathrm{Ar}] ;\) (b) \([\mathrm{Ar}] 3 d^{5}\); (c) \([\mathrm{Kr}] 5 s^{2} 4 d^{10}\)

Consider \(\mathrm{S}, \mathrm{Cl}\), and \(\mathrm{K}\) and their most common ions. (a) List the atoms in order of increasing size. (b) List the ions in order of increasing size. (c) Explain any differences in the orders of the atomic and ionic sizes.

Based on their positions in the periodic table, predict which atom of the following pairs will have the smaller first ionization energy: (a) \(\mathrm{Cl}, \mathrm{Ar} ;\) (b) \(\mathrm{Be}, \mathrm{Ca}\) (c) \(\mathrm{K}\), Co; (d) \(\mathrm{S}, \mathrm{Ge} ;\) (e) Sn. Te.

(a) What is the trend in first ionization energies as one proceeds down the group 7 A elements? Explain how this trend relates to the variation in atomic radii. (b) What is the trend in first ionization energies as one moves across the fourth period from \(\mathrm{K}\) to \(\mathrm{Kr}\) ? How does this trend compare with the trend in atomic radii?

Use electron configurations to explain the following observations: (a) The first ionization energy of phosphorus is greater than that of sulfur. (b) The electron affinity of nitrogen is lower (less negative) than those of both carbon and oxygen. (c) The second ionization energy of oxygen is greater than the first ionization energy of fluorine. (d) The third ionization energy of manganese is greater than those of both chromium and iron.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

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