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Chapter 8: Problem 59

Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify your answers. a. \(\mathrm{NaCl}, \mathrm{KCl} \quad\) d. Fe \((\mathrm{OH})_{2}, \mathrm{Fe}(\mathrm{OH})_{3}\) b. \(\mathrm{LiF}, \mathrm{LiCl} \quad\) e. \(\mathrm{NaCl}, \mathrm{Na}_{2} \mathrm{O}\) c. \(\mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{MgO} \quad\) f. \(\mathrm{MgO}, \mathrm{BaS}\)

Short Answer

Expert verified
The compounds with the most exothermic lattice energy in each pair are: a. NaCl, due to Na鈦� having a smaller radius than K鈦�. b. LiF, due to F鈦� having a smaller radius than Cl鈦�. c. MgO, due to higher combined charge of ions. d. Fe(OH)鈧�, due to Fe鲁鈦� having a higher charge than Fe虏鈦�. e. Na鈧侽, due to higher combined charge of ions. f. MgO, due to Mg虏鈦� and O虏鈦� having smaller radii than Ba虏鈦� and S虏鈦�.

Step by step solution

01

Observe the charge of the ions in both compounds

Both NaCl and KCl have ions with a charge of +1 and -1, so the charge of the ions will not affect our comparison.
02

Compare the size of the ions in both compounds

Sodium ion (Na+) has a smaller radius than potassium ion (K+), while chloride ion (Cl-) has the same size in both compounds. Since the ionic radius of Na+ is smaller than K+, NaCl will have a stronger electrostatic force and therefore a more exothermic lattice energy. #b. Compare LiF and LiCl
03

Observe the charge of the ions in both compounds

Both LiF and LiCl have ions with a charge of +1 and -1, so the charge of the ions will not affect our comparison.
04

Compare the size of the ions in both compounds

Lithium ion (Li+) has the same size in both compounds, but fluoride ion (F-) has a smaller radius than chloride ion (Cl-). As a result, LiF will have a stronger electrostatic force, and thus a more exothermic lattice energy. #c. Compare Mg(OH)鈧� and MgO
05

Observe the charge of the ions in both compounds

Mg虏鈦� has the same charge in both compounds, while O虏鈦� has a charge of -2 and OH鈦� has a charge of -1. MgO has a higher combined charge of both ions and thus stronger electrostatic attraction.
06

Compare the size of the ions in both compounds

The size of the ions does not need to be considered in this case since the charges of the ions are different with MgO having stronger electrostatic attraction. Therefore, MgO has a more exothermic lattice energy. #d. Compare Fe(OH)鈧� and Fe(OH)鈧�
07

Observe the charge of the ions in both compounds

Fe虏鈦� has a charge of +2 in Fe(OH)鈧�, and Fe鲁鈦� has a charge of +3 in Fe(OH)鈧�, while OH鈦� has a charge of -1 in both compounds. Since the charge of the ions in Fe(OH)鈧� is greater, it has stronger electrostatic attraction and more exothermic lattice energy. #e. Compare NaCl and Na鈧侽
08

Observe the charge of the ions in both compounds

Na鈦� has a charge of +1 in both compounds, while Cl鈦� has a charge of -1 in NaCl, and O虏鈦� has a charge of -2 in Na鈧侽. Na鈧侽 has a higher combined charge and thus stronger electrostatic attraction.
09

Compare the size of the ions in both compounds

The size of the ions does not need to be considered in this case since the charges of the ions are different with Na鈧侽 having stronger electrostatic attraction. Therefore, Na鈧侽 has a more exothermic lattice energy. #f. Compare MgO and BaS
10

Observe the charge of the ions in both compounds

Mg虏鈦� and O虏鈦� in MgO have charges of +2 and -2 respectively, while Ba虏鈦� and S虏鈦� in BaS also have charges of +2 and -2 respectively. Since the charges are the same, we'll need to compare the size of the ions.
11

Compare the size of the ions in both compounds

Magnesium ion (Mg虏鈦�) is smaller than barium ion (Ba虏鈦�), while oxide ion (O虏鈦�) is smaller than sulfide ion (S虏鈦�). The stronger electrostatic force will be present in the compound with the smallest ions, which is MgO. Thus, MgO will exhibit a more exothermic lattice energy.

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Key Concepts

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

Ionic Compounds
Ionic compounds are fascinating types of substances formed through the transfer of electrons. This electron transfer results in the creation of positive and negative ions. These ions are what makes ionic compounds so unique and significant. They bond together due to opposite charges, forming a well-organized, stable structure. Ionic compounds include common substances like table salt (NaCl).
  • Typically involve a metal and a non-metal.
  • The bond formed is known as an ionic bond, which is strong and stable.
  • They tend to have high melting and boiling points due to strong ionic bonds.
  • Most ionic compounds dissolve in water, creating solutions that conduct electricity.
Understanding the properties and behaviors of ionic compounds is crucial because these characteristics explain their high lattice energy and why they are essential in many chemical reactions.
Electrostatic Attraction
Electrostatic attraction is a fundamental concept in chemistry that explains how ionic bonds form the backbone of ionic compounds. When ions of opposite charges come together, they experience a force known as electrostatic attraction. This is similar to how magnets work, simply pulling each other closer due to their opposite ends.
  • Stronger electrostatic attraction means a more stable ionic bond.
  • Compounds with higher charges will experience greater attraction.
  • Smaller ionic radii also contribute to stronger attractions.
  • This attraction is crucial for lattice energy, as seen in various compound comparisons.
By understanding electrostatic attraction, we can better predict the behaviors of ionic substances, such as their stability, solubility, and boiling points.
Ionic Radius
The ionic radius is the measure of an ion's size within a crystal lattice. It plays a critical role in determining the strength of electrostatic attraction in ionic compounds. Smaller ions can pack closer together, which usually results in a stronger bond.
  • Ions with smaller radii lead to greater lattice energies.
  • This is because the closer the ions are, the stronger the attraction.
  • Considerations of ionic radius are crucial, especially when ions have the same charge.
  • Ions like Na+ compared to K+ show how size affects lattice energy.
Understanding ionic radii allows us to predict not just the physical properties of a compound but also its chemical reactivity and vibrancy in different environments.
Ionic Charge
Ionic charge is pivotal when it comes to understanding lattice energy in ionic compounds. It essentially represents the strength of the attraction between ions. Higher charges result in stronger bonds due to increased electrostatic forces.
  • Compounds with higher ionic charges tend to have more exothermic lattice energies.
  • For example, MgO with Mg2+ and O2- shows stronger force than Mg(OH)2 with Mg2+ and OH-.
  • The more significant the difference in charges, the stronger the lattice energy.
  • This explains why compounds like Fe(OH)3 have more exothermic lattice energies compared to Fe(OH)2 due to higher ionic charge differences.
Grasping the concept of ionic charge helps illustrate why certain compounds are more stable and energetically favored, thus impacting their chemical applications.

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Most popular questions from this chapter

List all the possible bonds that can occur between the elements P, Cs, O, and H. Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form for each bond.

Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form between the following pairs of elements. a. \(\mathrm{Rb}\) and \(\mathrm{Cl} \quad\) d. \(\mathrm{Ba}\) and \(\mathrm{S}\) b. \(\mathrm{S}\) and \(\mathrm{S} \quad\) e. \(\mathrm{N}\) and \(\mathrm{P}\) c. \(\mathrm{C}\) and \(\mathrm{F} \quad\) f. \(\mathrm{B}\) and \(\mathrm{H}\)

What do each of the following sets of compounds/ions have in common with each other? a. \(\mathrm{SO}_{3}, \mathrm{NO}_{3}^{-}, \mathrm{CO}_{3}^{2-}\) b. \(\mathrm{O}_{3}, \mathrm{SO}_{2}, \mathrm{NO}_{2}-\)

In general, the higher the charge on the ions in an ionic compound, the more favorable the lattice energy. Why do some stable ionic compounds have \(+1\) charged ions even though \(+4,+5,\) and \(+6\) charged ions would have a more favorable lattice energy?

Predict the molecular structure (including bond angles) for each of the following. a. \(\mathrm{PCl}_{3}\) b. \(\mathrm{SCl}_{2}\) c. \(\mathrm{SiF}_{4}\)
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