/*! 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 11 Explain why ions with charges gr... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 9: Problem 11

Explain why ions with charges greater than 3 are seldom found in ionic compounds.

Short Answer

Expert verified
Ions with charges greater than 3 are less frequently found in ionic compounds due to the higher ionization energy required to remove or add more than three electrons, which leads to less stable atomic configurations and is energetically unfavorable.

Step by step solution

01

Understanding Ionization Energy

Ionization energy is the amount of energy required to remove an electron from an atom or ion. The ionization energy of an atom increases with each successive electron removed. This is due to the increase in positive charge of the nucleus, which pulls electrons closer and hence, requires more energy to remove them.
02

Understanding Valence Electrons

Valence electrons are the outermost electrons in an atom and the ones involved in chemical reactions. Atoms strive to fill or empty their outermost electron shell to achieve stability, depending on which process requires less energy. This 'octet rule' is why atoms generally form ions with charges of 1, 2 or 3, either by gaining or losing that number of electrons to achieve a stable, full outer shell.
03

Applying these Concepts to Ionic Compounds

Ions in ionic compounds generally have charges of +1, +2, -1, -2, +3, or -3. Charges greater than 3 are less common because removing or adding more than three electrons requires significantly more ionization energy and typically represents a less stable configuration. Such an atom would have to gain or lose more than three electrons to achieve a full or empty outer shell, which is energetically unfavorable. Hence, ions with charges greater than 3 are seldom found in ionic compounds.

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!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Ionization Energy
Ionization energy is the energy needed to remove an electron from an atom. This concept is crucial in understanding why ions with charges greater than 3 are rare in ionic compounds. Each electron removed from an atom requires more energy than the previous one. This is because there's increased positive charge in the nucleus, which holds the electrons tightly. As more electrons are removed, the atom becomes positively charged. Removing additional electrons means overcoming even greater nuclear attraction, leading to a steep rise in ionization energy. This explains why forming ions with charges greater than 3 is energetically unfavorable.
Valence Electrons
Valence electrons are the outermost electrons of an atom. They are the ones that participate in chemical reactions. Atoms are always looking for ways to be stable. Stability is achieved when the outer electron shell is either completely filled or emptied. To get to this stability, atoms will either lose or gain electrons, focusing on the valence electrons. The goal is energetically efficient: for example, losing one or two valence electrons if it brings an atom closer to a stable configuration is preferred. There is a practical energy limit to how many electrons can feasibly be lost or gained, usually resulting in ions with charges of +1, +2, or +3.
The Octet Rule
The octet rule is a guideline that helps understand why atoms gain, lose, or share electrons. According to this rule, atoms tend to adjust their electron configuration to have eight electrons in their outermost shell. This is known as an 'octet.' A full outer shell makes the atom more stable, mimicking the electron configuration of noble gases. However, many atoms are not inherently stable and must interact with others to achieve this ideal configuration. Therefore, they form ions that typically have charges of +1, +2, or -3, solving their stability problems with minimal energy expenditure.
Ion Stability
Ion stability refers to how likely it is for an ion to remain in its charged state without further reactions. Generally, ions exist to reach a more stable form. This is why ion charges rarely exceed 3. When an ion has a charge greater than 卤3, the energy required to achieve such a state is significant and often not compensated by a corresponding energy gain in forming a compound. Ions with lesser charges have the right balance of energy expenditure and stability, allowing them to effectively participate in forming stable ionic compounds. Thus, ions with charges higher than 3 are rare due to high ionization energies and low resultant stability.

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

What is lattice energy and what role does it play in the stability of ionic compounds?

In the vapor phase, beryllium chloride consists of discrete \(\mathrm{BeCl}_{2}\) molecules. Is the octet rule satisfied for Be in this compound? If not, can you form an octet around Be by drawing another resonance structure? How plausible is this structure?

Do formal charges represent actual separation of charges?

Although nitrogen dioxide \(\left(\mathrm{NO}_{2}\right)\) is a stable compound, there is a tendency for two such molecules to combine to form dinitrogen tetroxide \(\left(\mathrm{N}_{2} \mathrm{O}_{4}\right) .\) Why? Draw four resonance structures of \(\mathrm{N}_{2} \mathrm{O}_{4},\) showing formal charges.

Classify the following bonds as ionic, polar covalent, or covalent, and give your reasons: (a) the \(\mathrm{SiSi}\) bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3},\) (b) the \(\mathrm{SiCl}\) bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3}\), (c) the CaF bond in \(\mathrm{CaF}_{2}\), (d) the \(\mathrm{NH}\) bond in \(\mathrm{NH}_{3}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Ionic and Molecular Compounds

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.