Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 8: Problem 16

Use Lewis symbols to represent the reaction that occurs between Ca and F atoms.

Short Answer

Expert verified
The reaction between Calcium (Ca) and Fluorine (F) can be represented using Lewis symbols as follows: \[ \text{Ca} : \: +\: .\: .\: \text{F}\: . \: +\: .\: .\: \text{F}\: . \: \rightarrow \: [\text{Ca}]^{2+}\: +\: [\text{F}]\: -\: .\: .\: .\: . \: +\: [\text{F}]\: -\: .\: .\: .\: . \] The final chemical formula for the compound is \( CaF_2 \), which is Calcium fluoride.

Step by step solution

01

Identify the valence electrons

Each element has a specific number of valence electrons, which are the electrons in the outermost shell of an atom. For Calcium (Ca), which is in Group 2 of the periodic table, it has 2 valence electrons. Fluorine (F), found in Group 17, has 7 valence electrons.
02

Draw the Lewis symbols for each atom

Lewis symbols show the chemical symbol of an element and its valence electrons as dots. For Calcium (Ca), draw two dots around the "Ca" to represent its 2 valence electrons. For Fluorine, place 7 dots around the "F" symbol to represent its 7 valence electrons. The Lewis symbols should look like this: Ca: \[ \text{Ca} : \] F: \[ .\: .\: \text{F}\: . \]
03

Determine the type of bond that will form between the atoms

Calcium is a metal and Fluorine is a non-metal, so they will form an ionic bond. In an ionic bond, electrons are transferred from the metal (Ca) to the non-metal (F) until both reach a stable electron configuration. In the case of Calcium and Fluorine, Calcium will lose its 2 valence electrons to achieve a stable configuration (like a Noble gas with a full outer shell), and each Fluorine atom will gain 1 electron to achieve the same stable configuration.
04

Show the electron transfer using Lewis symbols

We shall show the transfer of electrons from Calcium to two Fluorine atoms. Once Calcium has lost its 2 valence electrons, it will become a positively charged ion with a +2 charge. Each Fluorine atom will gain 1 electron from Calcium and become a negatively charged ion (F⁻). The reaction could be represented like this using Lewis symbols: \[ \text{Ca} : \: +\: .\: .\: \text{F}\: . \: +\: .\: .\: \text{F}\: . \: \rightarrow \: [\text{Ca}]^{2+}\: +\: [\text{F}]\: -\: .\: .\: .\: . \: +\: [\text{F}]\: -\: .\: .\: .\: . \]
05

Write the final chemical formula for the compound

Now that we have represented the reaction using Lewis symbols, we can write the final chemical formula for the ionic compound that forms between Calcium and Fluorine: \( CaF_2 \) This is the formula for Calcium fluoride.

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

In the following pairs of binary compounds determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) \(\mathrm{SiF}_{4}\) and \(\mathrm{LaF}_{3}\), (b) \(\mathrm{FeCl}_{2}\) and \(\mathrm{ReCl}_{6}\) (c) \(\mathrm{PbCl}_{4}\) and \(\mathrm{RbCl}\).

(a) How does a polar molecule differ from a nonpolar one? (b) Atoms \(\mathrm{X}\) and \(\mathrm{Y}\) have different electronegativities. Will the diatomic molecule \(\mathrm{X}-\mathrm{Y}\) necessarily be polar? Explain. (c) What factors affect the size of the dipole moment of a diatomic molecule?

(a) Write one or more appropriate Lewis structures for the nitrite ion, \(\mathrm{NO}_{2}^{-}\). (b) With what allotrope of oxygen is it isoelectronic? (c) What would you predict for the lengths of the bonds in \(\mathrm{NO}_{2}^{-}\) relative to \(\mathrm{N}-\mathrm{O}\) single bonds and double bonds?

Draw Lewis structures for the following: (a) \(\mathrm{SiH}_{4},\) (b) CO, (c) \(\mathrm{SF}_{2}\), (d) \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{H}\) is bonded to \(\mathrm{O})\), (e) \(\mathrm{ClO}_{2}^{-},\) (f) \(\mathrm{NH}_{2} \mathrm{OH}\).

Draw the Lewis structures for each of the following ions or molecules. Identify those that do not obey the octet rule, and explain why they do not: (a) \(\mathrm{SO}_{3}^{2-}\), (b) \(\mathrm{AlH}_{3}\) (c) \(\mathrm{N}_{3}^{-}\) (d) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) (e) \(\mathrm{SbF}_{5}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Analysis

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