/*! 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 36 Explain why, for isoelectronic i... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 36

Explain why, for isoelectronic ions, the anions are larger than the cations.

Short Answer

Expert verified
Isoelectronic anions are larger than cations because they have gained additional electrons, creating more repulsion within the electron cloud and expanding its size.

Step by step solution

01

Understanding Isoelectronic Ions

Isoelectronic ions are atoms or molecules that have the same number of electrons or the same electronic structure. Common examples include Na+ and F-, which both have 10 electrons. Though these ions originate from different atoms, they become isoelectronic due to gaining or losing electrons.
02

Interpreting the Size of Ions

When considering ions, it's important to note that gaining or losing electrons affects their size. For anions, which gain electrons, the additional negative charges result in increased repulsion, expanding the electron cloud and hence, the size of the ion. For cations, which lose electrons, losing negative charges results in less repulsion, leading to a more compact electron cloud.
03

Comparing Anions and Cations

When comparing isoelectronic anions and cations, the anions will always be larger. This is because they have gained additional electrons, leading to increased repulsion and expansion of the electron cloud. In contrast, the cations, having lost electrons, will have less repulsion and a more compact electron cloud, making them smaller in 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.

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

With reference to the periodic table, name (a) a halogen element in the fourth period, (b) an element \(\operatorname{sim}\) ilar to phosphorus in chemical properties, (c) the most reactive metal in the fifth period, \((\) d) an element that has an atomic number smaller than 20 and is similar to strontium.

Why are the Group \(1 \mathrm{~B}\) elements more stable than the Group IA elements even though they seem to have the same outer electron configuration \(n s^{1}\) in which \(n\) is the principal quantum number of the outermost shell?

Define ionic radius. How does the size change when an atom is converted to (a) an anion and (b) a cation?

What is the characteristic of the electron configuration of stable ions derived from representative elements?

What do we mean when we say that two ions or an atom and an ion are isoelectronic?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Kinetics

Read Explanation

Inorganic 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.