Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 122

Order the atoms in each of the following sets from the least exothermic electron affinity to the most. a. \(\mathrm{N}, \mathrm{O}, \mathrm{F}\) b. Al, Si, \(\mathrm{P}\)

Short Answer

Expert verified
For set A, the order from the least exothermic electron affinity to the most is: \(N < O < F\). For set B, the order is: \(Al < Si < P\).

Step by step solution

01

Locating the atoms on the periodic table

Locate the elements nitrogen (N), oxygen (O), and fluorine (F) on the periodic table. They are all in the second period (row) and are in the following order: N, O, F.
02

Applying the electron affinity trend

Since all three elements are in the same period of the periodic table, we can apply the general trend of electron affinity increasing from left to right in the same period. This means that nitrogen (N) has the least exothermic electron affinity, followed by oxygen (O), and finally fluorine (F) with the most exothermic electron affinity.
03

Ordering the atoms based on electron affinity

Using the information from Steps 1 and 2, we can order the atoms in Set A from the least exothermic electron affinity to the most: N < O < F. #Set B: Al, Si, P#
04

Locating the atoms on the periodic table

Locate the elements aluminum (Al), silicon (Si), and phosphorous (P) on the periodic table. They are all in the third period (row) and are in the following order: Al, Si, P.
05

Applying the electron affinity trend

Since all three elements are in the same period of the periodic table, we can apply the general trend of electron affinity increasing from left to right in the same period. This means that aluminum (Al) has the least exothermic electron affinity, followed by silicon (Si), and finally phosphorous (P) with the most exothermic electron affinity.
06

Ordering the atoms based on electron affinity

Using the information from Steps 1 and 2, we can order the atoms in Set B from the least exothermic electron affinity to the most: Al < Si < P.

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

"Lithium" is often prescribed as a mood-stabilizing drug. Do you think the "lithium" prescribed is in the elemental form? What is the more likely form of lithium to be prescribed as a drug?

Calculate the wavelength of light emitted when each of the following transitions occur in the hydrogen atom. What type of electromagnetic radiation is emitted in each transition? a. \(n=3 \rightarrow n=2\) b. \(n=4 \rightarrow n=2\) c. \(n=2 \rightarrow n=1\)

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 \(\mathrm{kJ} / \mathrm{mol}\) ?

Give a possible set of values of the four quantum numbers for all the electrons in a boron atom and a nitrogen atom if each is in the ground state.

Write the expected electron configurations for each of the following atoms: Sc, Fe, P, Cs, Eu, Pt, Xe, Br.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

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