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Chapter 7: Problem 46

What do we mean by a "lattice of ions"?

Short Answer

Expert verified
A "lattice of ions" refers to the orderly and repeating arrangement of positively charged (cation) and negatively charged (anion) ions in a crystal structure, creating a pattern that repeats in three dimensions. The repeating unit of the lattice is known as the unit cell, which contains the same number of each species of ion as the overall lattice. The properties of a crystalline solid depend on the type of ions and the arrangement of its lattice. Lattices of ions are formed when ionic compounds combine in a solid-state, arranging themselves in specific structural patterns to minimize potential energy and satisfy electrostatic forces, resulting in strong ionic bonds.

Step by step solution

01

Definition of a Lattice of Ions

A "lattice of ions" refers to the orderly and repeating arrangement of positively charged (cation) and negatively charged (anion) ions in a crystal structure. In a lattice, the ions are arranged in such a way that they create a pattern that repeats in three dimensions. These arrangements give the crystalline solid predictable and unique properties.
02

Properties of a Lattice of Ions

1. The lattice is a three-dimensional repeating pattern. 2. The repeating unit of the lattice is known as the unit cell. 3. A unit cell contains the same number of each species of ion as the overall lattice. 4. The positively charged cations and negatively charged anions are electrostatically attracted to each other, creating strong ionic bonds. 5. The properties of a crystalline solid depend on the type of ions and the arrangement of its lattice.
03

Examples of Ionic Lattices

1. Sodium chloride (NaCl): In the NaCl lattice, each sodium ion (Na+) is surrounded by six chloride ions (Cl-), and each chloride ion is surrounded by six sodium ions. This ionic compound forms a cubic lattice structure. 2. Cesium chloride (CsCl): In the CsCl lattice, the cesium ion (Cs+) is surrounded by eight chloride ions (Cl-), forming a cubic structure. The arrangement of CsCl is different from NaCl, indicating that the same ions can form different lattice structures.
04

Unit Cell Representation

To visualize the lattice of ions, we can represent the unit cell as the smallest repeating unit that makes up the lattice structure. This unit cell will contain a specific number of ions, depending on the lattice's arrangement. When the unit cells are repeated in three dimensions, the entire lattice structure is formed.
05

Ionic Lattice Formation

Lattices of ions are formed when ionic compounds are formed through the combination of positively charged cations and negatively charged anions. When ionic compounds are in a solid-state, they arrange themselves in a specific structural pattern, minimizing their potential energy and satisfying the electrostatic forces. This results in the formation of a stable lattice of ions with specific periodic arrangements and strong ionic bonds.

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Key Concepts

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

Ionic Crystal Structure
The arrangement of atoms in a material is what defines its properties, and when it comes to ionic crystal structures, this arrangement is both orderly and meticulous. These structures are composed of positively charged ions, known as cations, and negatively charged ions, or anions. The repetitive organization extends in all three dimensions of space forming a pattern that, at the microscopic level, looks like a never-ending grid. This structure is not random; it maximizes efficiency by ensuring each ion is surrounded by oppositely charged ions, which minimizes repulsion and maximizes attraction.
Unit Cell
Within this vast grid lies the concept of the unit cell, which is essentially the building block of the entire crystal. Think of it as a single brick in a vast wall. This cell is the simplest representation of the crystal's structure and contains all the information needed to build the entire lattice through repetition. To understand a crystal, one must simply understand its unit cell. It's this repetition of the unit cell in three dimensions that constructs the overall crystal. This concept not only simplifies understanding but also greatly aids in calculating properties like density and can indicate how the ions interact within the crystal.
Ionic Bonds
The robust structure of ionic crystals is due to ionic bonds. These bonds result from the electrostatic attractions between the positively and negatively charged ions within the lattice. An ionic bond is the glue that holds the lattice together, creating solid compounds with high melting and boiling points due to the strength of these bonds. The strength of an ionic bond can define many properties of the material, like its hardness and brittleness. An ionic compound will typically break along planes where these strong bonds can be disrupted.
Crystalline Solid Properties
Given their rigid structure, crystalline solids exhibit a set of unique properties. They tend to have sharp melting points, as the heat provided to the system needs to be sufficient to overcome the strong ionic bonds. They also often have high hardness and are poor conductors of electricity in their solid state since ions are fixed in place and cannot move to conduct a current. When dissolved in water or melted, these solids can conduct electricity due to free-moving ions. Moreover, the arrangement of ions in the lattice can result in various geometrical shapes, leading to the diverse and often beautiful crystal forms observed in nature.

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Most popular questions from this chapter

Most covalent molecular substances have much lower melting points than ionic substances. What does this say about the strength of a covalent bond relative to the strength of an ionic bond? Explain your answer.

Water vapor liquefies when cooled below \(100^{\circ} \mathrm{C}\). Gaseous nitrogen liquefies when cooled below \(-196^{\circ} \mathrm{C}\). What does this information tell you about the relative strengths of the intermolecular forces for these molecules?

Why does a gas expand to fill the container it is in, but a liquid and a solid do not?

Which of the following best describes a liquid: (a) The phase of matter in which particles are typically separated by the least distance (b) The phase of matter in which particles are in a fixed, rigid arrangement (c) The phase of matter in which particles completely fill the volume of their container (d) The phase of matter in which particles are in a loose, changeable arrangement but do not completely fill the volume of their container

Explain in molecular terms how heating causes a liquid to change to the gas phase.
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