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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 needed to separate a solid ionic compound into gaseous ions. It indicates the compound's stability; higher lattice energy means greater stability.

Step by step solution

01

Define Lattice Energy

Lattice energy is the amount of energy required to completely separate one mole of a solid ionic compound into its gaseous ions. It is a measure of the strength of the forces holding the ions together in the crystal lattice.
02

Understand the Role in Stability

Lattice energy contributes significantly to the stability of ionic compounds. Higher lattice energy indicates stronger attraction between ions, resulting in a more stable ionic compound. It affects melting point, solubility, and hardness.
03

Relationship with Ionic Properties

Lattice energy depends on two main factors: the charge of the ions and the radius of the ions. Greater charge and smaller ionic radii result in higher lattice energies, leading to greater stability of the ionic compound.

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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 structures formed by the attraction between positively charged ions (cations) and negatively charged ions (anions). This electrostatic attraction creates a strong bond that holds the ions together. Typically, these compounds are made up of metals and non-metals. Metal atoms lose electrons to become cations, while non-metal atoms gain these electrons to become anions.
  • An example of an ionic compound is sodium chloride (NaCl), where sodium (Na) donates an electron to chlorine (Cl).
  • This transfer of electrons follows the Octet Rule, where atoms strive to achieve a full outer shell of electrons.
  • The resulting product typically has high melting and boiling points due to the strength of the ionic bonds.
In solid form, these compounds do not conduct electricity because the ions are fixed in place within a crystal lattice. However, when dissolved in water or melted, the ions become free to move around, enabling electricity conduction.
Crystal Lattice
The crystal lattice is a three-dimensional structure that is both key to understanding ionic compounds and provides insight into their substantial strength and stability. This ordered arrangement allows ions to maximize their attractive interactions while minimizing repulsive forces.
  • The lattice structure is usually shown as a repeating pattern of unit cells, reflecting the periodic arrangement of ions.
  • It aids in explaining why ionic compounds, like salt, have high melting and boiling points.
  • The continuous network of alternating positive and negative ions results in a "giant" lattice system.
Understanding the crystal lattice helps explain the behavior of ionic compounds under various conditions, such as temperature and pressure, and contributes to their characteristic brittleness. This brittleness occurs because when stress is applied, like charges can shift to nearby ions, causing repulsive forces to dominate and the solid to shatter.
Ionic Properties
The properties of ionic compounds are distinct due to the nature of their ionic bonds. Firstly, the crystal lattice itself contributes significantly to these properties. Secondly, the lattice energy also has a huge role to play in determining these characteristics.
  • High Melting and Boiling Points: These arise because a substantial amount of energy is required to break the strong ionic bonds.
  • Solubility in Water: Ionic compounds tend to dissolve in polar solvents like water. The polar water molecules interact with the charged ions, effectively pulling them apart.
  • Electrical Conductivity: Although solid ionic compounds are non-conductors of electricity, they become good conductors when dissolved or molten as the ions are free to move.
Moreover, ionic compounds are generally hard but brittle, illustrating a balance between strong attraction and potential repulsion within the crystal lattice. Comprehending ionic properties not only highlights their industrial applicability but also enhances our grasp of their chemical behaviors.

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Most popular questions from this chapter

Write Lewis structures for these ions: (a) \(\mathrm{O}_{2}^{2-}\), (b) \(\mathrm{C}_{2}^{2-},(\mathrm{c}) \mathrm{NO}^{+}\), (d) \(\mathrm{NH}_{4}^{+}\). Show formal charges.

Give an example of an ion or molecule containing Al that (a) obeys the octet rule, (b) has an expanded octet, and (c) has an incomplete octet.

What is a coordinate covalent bond? Is it different from a normal covalent bond?

In the vapor phase, beryllium chloride consists of discrete molecular units \(\mathrm{BeCl}_{2}\). Is the octet rule satisfied for Be in this compound? If not, can you form an octet around Be by drawing another resonance structure? How plausible is this structure?

The bond enthalpy of \(\mathrm{F}_{2}(g)\) is \(156.9 \mathrm{~kJ} / \mathrm{mol}\). Calculate \(\Delta H_{\mathrm{f}}^{\circ}\) for \(\mathrm{F}(g)\).
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