Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 8: Problem 18

Which ionic compound is expected to form from combining the following pairs of elements? (a) calcium and nitrogen, (b) cesium and bromine, (c) strontium and sulfur, (d) aluminum and selenium.

Short Answer

Expert verified
The ionic compounds formed by the given pairs of elements are: a) Calcium nitride: Ca₃N₂ b) Cesium bromide: CsBr c) Strontium sulfide: SrS d) Aluminum selenide: Al₂Se₃

Step by step solution

01

Identify the charges of the ions formed by each element

First, write down the symbols and charges of the ions for each element in the given pairs. You can find the charges using the periodic table; elements in the same group tend to form ions with the same charge. a) Calcium (Ca) and nitrogen (N): Ca^(2+), N^(3-) b) Cesium (Cs) and bromine (Br): Cs^(1+), Br^(-) c) Strontium (Sr) and sulfur (S): Sr^(2+), S^(2-) d) Aluminum (Al) and selenium (Se): Al^(3+), Se^(2-)
02

Determine the ratio of ions needed to form a neutral compound

To form a neutral ionic compound, the total positive charge must be equal to the total negative charge. Find the least common multiple of the charges of the positive and negative ions of each pair to achieve charge balance. a) Ca^(2+) and N^(3-): least common multiple is 6. b) Cs^(1+) and Br^(-): least common multiple is 1. c) Sr^(2+) and S^(2-): least common multiple is 2. d) Al^(3+) and Se^(2-): least common multiple is 6.
03

Write the chemical formula for each compound

Now that we have the ratio of ions for each compound, write the chemical formula by using subscripts to indicate the number of ions needed to achieve charge balance. a) Calcium nitride: Ca₃N₂ (3 Ca^(2+) ions with 2 N^(3-) ions) b) Cesium bromide: CsBr (1 Cs^(1+) ion with 1 Br^(-) ion) c) Strontium sulfide: SrS (1 Sr^(2+) ion with 1 S^(2-) ion) d) Aluminum selenide: Al₂Se₃ (2 Al^(3+) ions with 3 Se^(2-) ions) Now we have the chemical formulas for the ionic compounds formed by the given pairs of elements: a) Ca₃N₂ - Calcium nitride b) CsBr - Cesium bromide c) SrS - Strontium sulfide d) Al₂Se₃ - Aluminum selenide

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

Although \(\mathrm{I}_{3}^{-}\) is a known ion, \(\mathrm{F}_{3}^{-}\) is not. \((\mathbf{a})\) Draw the Lewis structure for \(I_{3}^{-}\) (it is linear, not a triangle). (b) One of your classmates says that \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{F}\) is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because it would violate the octet rule. Is this classmate possibly correct? (d) Yet another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{F}\) is too small to make bonds to more than one atom. Is this classmate possibly correct?

(a) Does the lattice energy of an ionic solid increase or decrease (i) as the charges of the ions increase, (ii) as the sizes of the ions increase? (b) Arrange the following substances not listed in Table 8.1 according to their expected lattice energies, listing them from lowest lattice energy to the highest: MgS, KI, GaN, LiBr.

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 RbCl.

(a) The nitrate ion, \(\mathrm{NO}_{3}^{-}\), has a trigonal planar structure with the \(\mathrm{N}\) atom as the central atom. Draw the Lewis structure(s) for the nitrate ion. (b) Given \(S=\mathrm{O}\) and \(\mathrm{S}-\mathrm{O}\) bond lengths are \(158 \mathrm{pm}\) and \(143 \mathrm{pm}\) respectively, estimate the sulphuroxygen bond distances in the ion.

(a) Use Lewis symbols to represent the reaction that occurs between Li and O atoms. (b) What is the chemical formula of the most likely product? (c) How many electrons are transferred? (d) Which atom loses electrons in the reaction?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

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