Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 15

Explain the importance of lattice energy in the formation of a salt.

Short Answer

Expert verified
Lattice energy is central to the formation of salt because it is the energy released as the positive and negative ions come together, hence stabilizing the ionic bond formed. In other words, the ionic compound is more stable the greater the lattice energy.

Step by step solution

01

Understanding Lattice Energy

Lattice energy, often denoted as U, is the energy required to separate one mole of a solid ionic compound into a gas of its constituent ions. Alternatively, it can be defined as the energy released during the formation of one mole of an ionic compound from its gaseous ions.
02

Understanding Ionic Bonds

In the case of a salt like NaCl, there is an ionic bond between the sodium (Na) and the chlorine (Cl) ions. This bond is formed due to the transfer of an electron from sodium to chlorine. As a result, sodium becomes a Na+ ion, and chlorine becomes a Cl- ion.
03

Role of Lattice Energy in Salt Formation

Lattice energy plays a crucial role in the formation of a salt (NaCl in this case). It is the energy that is being released when the Na+ and Cl- ions come together to form an ionic bond. This released energy helps to stabilize the ionic bond, making the formation of a salt possible.
04

Stability of Ionic Compounds

The greater the lattice energy, the stronger the forces between the ions, and the more stable the ionic compound. This makes the resulting salt crystallize into a structure which lowers the overall energy of the system and thus renders it more stable.

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

What does a metal atom need to do in order to form a cation?

Write formulas for the following ionic compounds. \begin{equation} \begin{array}{l}{\text { a. lithium sulfate }} \\ {\text { b. strontium nitrate }} \\ {\text { c. ammonium acetate }} \\ {\text { d. titanium(III) sulfate }}\end{array} \end{equation}

Use the following terms to create a concept map: atoms, valence electrons, ions, cations, anions, and ionic compounds.

Why are there no rules for naming Group 18 ions?

Graphing Calculator Calculating the Number of Valence Electrons The graphing calculator can run a program that can determine the number of valence electrons in an atom, given its atomic number. Go to Appendix C. If you are using a TI-83 Plus, you can download the program VALENCE and run the application as directed. If you are using another calculator, your teacher will provide you with keystrokes to use. After you have run the program, answer these questions. How many valence electrons are there in the following atoms? \begin{equation} \begin{array}{l}{\text { a. Rutherfordium, Rf, atomic number } 104} \\ {\text { b. Gold, Au, atomic number } 79} \\ {\text { c. Molybdenum, Mo, atomic number } 42} \\ {\text { d. Indium, In, atomic number } 49}\end{array} \end{equation}
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

The Earths Atmosphere

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