Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 117

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

Short Answer

Expert verified
For the pair (C and N): a. N has a more favorable electron affinity. b. N has a higher ionization energy. c. C has a larger atomic size. For the pair (Ar and Br): a. Br has a more favorable electron affinity. b. Ar has a higher ionization energy. c. Br has a larger atomic size.

Step by step solution

01

Pair 1: C and N

First, let's analyze the pair of atoms, Carbon (C) and Nitrogen (N). They are both in the same period (period 2). a. Since N is to the right of C in period 2, it has a more favorable (exothermic) electron affinity. b. N is closer to the top right corner, so it has a higher ionization energy. c. C is larger in size compared to N, as the size decreases across a period.
02

Pair 2: Ar and Br

Next, let's analyze the pair of atoms, Argon (Ar) and Bromine (Br). They are both in the same group (group 18, noble gases, and group 17, halogens, respectively). a. Since Ar is a noble gas, it has no electron affinity, while Br has a favorable (exothermic) electron affinity. b. Ar is in a higher period (period 3) compared to Br (period 4), so Ar should have a higher ionization energy. c. Br is lower on the periodic table (period 4) compared to Ar (period 3), so Br has a larger atomic size.
03

Summary of the answers

For the pair (Carbon and Nitrogen): a. Nitrogen has a more favorable electron affinity. b. Nitrogen has a higher ionization energy. c. Carbon has a larger atomic size. For the pair (Argon and Bromine): a. Bromine has a more favorable electron affinity. b. Argon has a higher ionization energy. c. Bromine has a larger atomic size.

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

The bright yellow light emitted by a sodium vapor lamp consists of two emission lines at \(589.0\) and \(589.6 \mathrm{~nm}\). What are the frequency and the energy of a photon of light at each of these wavelengths? What are the energies in \(\mathrm{kJ} / \mathrm{mol}\) ?

Answer the following questions based on the given electron configurations, and identify the elements. a. Arrange these atoms in order of increasing size: \([\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{6} ;[\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{1} ;[\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{3}\) b. Arrange these atoms in order of decreasing first ionization energy: \([\mathrm{Ne}] 3 s^{2} 3 p^{5} ;[\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{3} ;[\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{5}\).

The four most abundant elements by mass in the human body are oxygen, carbon, hydrogen, and nitrogen. These four elements make up about \(96 \%\) of the human body. The next four most abundant elements are calcium, phosphorus, magnesium, and potassium. Write the expected ground-state electron configurations for these eight most abundant elements in the human body.

For each of the following pairs of elements \(\begin{array}{ll}(\mathrm{Mg} \text { and } \mathrm{K}) & (\mathrm{F} \text { and } \mathrm{Cl})\end{array}\) pick the atom with a. more favorable (exothermic) electron affinity. b. higher ionization energy. c. larger size.

One of the emission spectral lines for \(\mathrm{Be}^{3+}\) has a wavelength of \(253.4 \mathrm{~nm}\) for an electronic transition that begins in the state with \(n=5 .\) What is the principal quantum number of the lower-energy state corresponding to this emission? (Hint: The Bohr model can be applied to one- electron ions. Don't forget the \(Z\) factor: \(Z=\) nuclear charge \(=\) atomic number. \()\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Inorganic Chemistry

Read Explanation

Kinetics

Read Explanation

Nuclear Chemistry

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