/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 117 Write equations corresponding to... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 7: Problem 117

Write equations corresponding to the following. a. the fourth ionization energy of Se b. the electron affinity of \(\mathrm{S}^{-}\) c. the electron affinity of \(\mathrm{Fe}^{3+}\) d. the ionization energy of \(\mathrm{Mg}\)

Short Answer

Expert verified
a. \(Se^{3+} + IE_{4} \rightarrow Se^{4+} + e^{-}\) b. \(S^{-} + e^{-} \rightarrow S^{2-} + EA\) c. \(Fe^{3+} + e^{-} \rightarrow Fe^{2+} + EA\) d. \(Mg + IE \rightarrow Mg^{+} + e^{-}\)

Step by step solution

01

a. The fourth ionization energy of Se

To find the fourth ionization energy of Se, we need to determine the initial and final states of the selenium atom in this process. After three ionizations, we have the Se鲁鈦� ion (three electrons removed). The fourth ionization implies the removal of another electron from this ion. The general formula for ionization energy is: Atom/ion + Ionization Energy 鈫� Atom/ion鈦� + e鈦� Applying this to Se: Se鲁鈦� + IE鈧� 鈫� Se鈦粹伜 + e鈦�
02

b. The electron affinity of \(\mathrm{S}^{-}\)

Electron affinity refers to the energy change that occurs when an electron is added to a gaseous atom or ion. For this case, we are considering the addition of an electron to a sulfur ion, S鈦�. The general formula for electron affinity is: Atom/ion + e鈦� 鈫� Atom/ion鈦� + Electron Affinity Applying this to S鈦�: S鈦� + e鈦� 鈫� S虏鈦� + EA
03

c. The electron affinity of \(\mathrm{Fe}^{3+}\)

In this case, we are considering the electron affinity of an iron ion, Fe鲁鈦�. We need to add an electron to this ion. Using the general formula for electron affinity: Fe鲁鈦� + e鈦� 鈫� Fe虏鈦� + EA
04

d. The ionization energy of \(\mathrm{Mg}\)

For the ionization energy of magnesium, Mg, we need to remove one electron from the gaseous atom. Using the general formula for ionization energy: Mg + IE 鈫� Mg鈦� + e鈦�

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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

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. \(\mathrm{Al}, \mathrm{Si}, \mathrm{P}\)

It takes \(7.21 \times 10^{-19} \mathrm{~J}\) of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this?

How many orbitals in an atom can have the designation \(5 p, 3 d_{z^{2}}\), \(4 d, n=5, n=4 ?\)

Give the name and formula of each of the binary compounds formed from the following elements. a. \(\mathrm{Li}\) and \(\mathrm{N}\) b. \(\mathrm{Na}\) and \(\mathrm{Br}\) c. \(\mathrm{K}\) and \(\mathrm{S}\)

Without looking at data in the text, sketch a qualitative graph of the third ionization energy versus atomic number for the elements Na through Ar, and explain your graph.
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Chemistry Branches

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.