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Chapter 9: Problem 21

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

Short Answer

Expert verified
Lattice energy is the energy required to convert one mole of an ionic solid into its individual ions in gaseous states, and it plays a critical role in the stability of ionic compounds. The higher the lattice energy, the more stable the ionic compound. It depends on the charge and radii of the ions, with higher charges and smaller radii resulting in stronger interactions and thus, higher lattice energy.

Step by step solution

01

Define Lattice Energy

Lattice energy can be defined as the energy required to convert one mole of an ionic solid into its constituent ions in gaseous states. It is an exothermic process, meaning it releases energy, and is usually reported in kilojoules per mole (kJ/mol). In mathematical form, this can be represented as: M\(^{+}\)X\(^{-}\)(s) --> M\(^{+}\)(g) + X\(^{-}\)(g) where M\(^{+}\) and X\(^{-}\) represent the cations and anions in the ionic compound.
02

Role of Lattice Energy in Stability of Ionic Compounds

The lattice energy plays a key role in the stability of ionic compounds. The higher the lattice energy, the stronger are the forces of attraction between the ions, and thus, requiring more energy to separate them. Therefore, ionic compounds with higher lattice energy are more stable. Conversely, those with lower lattice energy are less stable. The stability and hence the lattice energy, depends on the charges of the ions and the radii of the ions in the compound. The lattice energy increases with increasing charge and decreasing ionic radii.
03

Example of Lattice Energy

For instance, consider Sodium Chloride (NaCl), when Na and Cl combine to form the NaCl compound and lattice, there is a release of energy due to the formation of ionic bonds. This energy (lattice energy) contributes towards the stability of NaCl. The factors that influenced this stability are the charges of the Na and Cl ions, and their radii. The released lattice energy makes the NaCl compound more stable.

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Most popular questions from this chapter

Write three resonance structures for the isocyanate ion (CNO \(^{-}\) ). Rank them in importance.

Write Lewis structures for these molecules: (a) ICl, (b) \(\mathrm{PH}_{3}\) (c) \(\mathrm{P}_{4}\) (each \(\mathrm{P}\) is bonded to three other P atoms), (d) \(\mathrm{H}_{2} \mathrm{~S},\) (e) \(\mathrm{N}_{2} \mathrm{H}_{4}\) (f) \(\mathrm{HClO}_{3},(\mathrm{~g}) \mathrm{COBr}_{2}\) (C is bonded to \(\mathrm{O}\) and \(\mathrm{Br}\) atoms ).

List these bonds in order of increasing ionic character: the lithium-to- fluorine bond in \(\mathrm{LiF},\) the potassium-to-oxygen bond in \(\mathrm{K}_{2} \mathrm{O},\) the nitrogen-tonitrogen bond in \(\mathrm{N}_{2}\), the sulfur-to-oxygen bond in \(\mathrm{SO}_{2}\), the chlorine-to-fluorine bond in \(\mathrm{ClF}_{3}\).

A rule for drawing plausible Lewis structures is that the central atom is invariably less electronegative than the surrounding atoms. Explain why this is so.

Name one ionic compound that contains only nonmetallic elements.
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