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Chapter 11: Problem 74

Classify each of the following by the type of solid it forms: (a) \(\mathrm{LiCl} ;\) (b) \(\mathrm{BaCl}_{2} ;\) (c) \(\mathrm{BCl}_{3}\); (d) \(\mathrm{CCl}_{4}\); (e) \(\mathrm{NCl}_{3}\).

Short Answer

Expert verified
(a) Ionic, (b) Ionic, (c) Molecular, (d) Molecular, (e) Molecular.

Step by step solution

01

Understanding the Problem

We need to classify compounds into specific types of solids that they form. The common categories are ionic, molecular, covalent network, or metallic solids. To classify, we consider the nature of the bonding in each compound.
02

Classify LiCl as Solid Type

Lithium Chloride (LiCl) consists of a metal (Li) and a non-metal (Cl), suggesting ionic bonding between Li鈦� and Cl鈦� ions. It forms an ionic solid.
03

Classify BaCl2 as Solid Type

Barium Chloride (BaCl鈧�) contains a metal (Ba) bonded to non-metals (Cl). Like LiCl, it forms ionic bonds, creating an ionic solid.
04

Classify BCl3 as Solid Type

Boron Trichloride (BCl鈧�) is a compound where boron (a non-metal) is covalently bonded to chlorine atoms. It forms discrete molecules in the solid state, categorizing it as a molecular solid.
05

Classify CCl4 as Solid Type

Carbon Tetrachloride (CCl鈧�) is made up of one carbon atom covalently bonded to four chlorine atoms, forming molecular units. Therefore, CCl鈧� is a molecular solid.
06

Classify NCl3 as Solid Type

Nitrogen Trichloride (NCl鈧�) consists of a nitrogen atom covalently bonded to three chlorine atoms, forming a molecule. This makes NCl鈧� a molecular solid.

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Key Concepts

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

Ionic Solids
Ionic solids are formed when metals and non-metals come together to share or transfer electrons, creating charged ions. These ions are held together by strong electrostatic forces in a lattice arrangement.
  • Examples of ionic solids include Lithium Chloride (LiCl) and Barium Chloride (BaCl鈧�).
  • They have high melting points due to the strength of the ionic bonds.
  • The rigidity and brittleness of ionic solids come from the lattice structure.
  • They are typically good conductors of electricity in liquid form or when dissolved in water, as the ions are free to move.
In summary, ionic solids are characterized by their formation from ionic bonds, high melting points, and unique electrical properties.
Molecular Solids
Molecular solids are composed of molecules held together by intermolecular forces such as van der Waals forces, hydrogen bonds, or dipole-dipole interactions. These forces are generally weaker than ionic or covalent bonds.
  • Examples include Boron Trichloride (BCl鈧�), Carbon Tetrachloride (CCl鈧�), and Nitrogen Trichloride (NCl鈧�).
  • They usually have lower melting and boiling points compared to ionic or covalent network solids.
  • Molecular solids can be soft and somewhat elastic because the intermolecular forces are weaker.
  • They are often poor electrical conductors because they lack free ions or electrons.
The molecular solid's physical properties are largely dictated by the nature and strength of the intermolecular forces involved.
Covalent Bonding
In covalent bonding, atoms share pairs of electrons to achieve a full outer shell, creating a stable balance of attractive and repulsive forces between atoms. This type of bonding is integral to both molecular and covalent network solids.
  • Molecules like Carbon Tetrachloride (CCl鈧�) rely on covalent bonds to form their structure.
  • Covalent network solids involve extensive networks of covalent bonds, leading to hard materials like diamond.
  • Covalent bonds are strong, needing significant energy to break, which often results in high melting and boiling points for covalent networks.
  • Though typically non-conductive, some covalent networks like graphite conduct electricity due to delocalized electrons.
Essentially, covalent bonding involves the sharing of electrons, contributing to the diverse properties seen in various solid structures.
Solid State Chemistry
Solid state chemistry focuses on understanding the arrangement of atoms in solids and how this arrangement influences their properties. It encompasses various types of solids, including ionic and molecular solids.
  • It helps explain why ionic solids are rigid and have high melting points.
  • Studying molecular solids reveals why they are often more volatile and less dense.
  • Solid state chemistry research has technological applications, such as in materials science for developing new semiconductors, insulators, and other functional materials.
  • It includes the study of crystallography, which is crucial for understanding solid structures at the atomic level.
Overall, solid state chemistry provides critical insights into how solid materials are built and how they perform under various conditions.

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Most popular questions from this chapter

Methane, \(\mathrm{CH}_{4}\), reacts with chlorine, \(\mathrm{Cl}_{2}\), to produce a series of chlorinated hydrocarbons: methyl chloride \(\left(\mathrm{CH}_{3} \mathrm{Cl}\right)\), methylene chloride \(\left(\mathrm{CH}_{2} \mathrm{Cl}_{2}\right)\), chloroform \(\left(\mathrm{CHCl}_{3}\right)\), and carbon tetrachloride \(\left(\mathrm{CCl}_{4}\right) .\) Which compound has the lowest vapor pressure at room temperature? Explain.

Steam at \(100^{\circ} \mathrm{C}\) was passed into a flask containing \(275 \mathrm{~g}\) of water at \(21^{\circ} \mathrm{C}\), where the steam condensed. How many grams of steam must have condensed if the temperature of the water in the flask was raised to \(83^{\circ} \mathrm{C}\) ? The heat of vaporization of water at \(100^{\circ} \mathrm{C}\) is \(40.7 \mathrm{~kJ} / \mathrm{mol}\) and the specific heat is \(4.18 \mathrm{~J} /\left(\mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right)\)

Copper metal has a face-centered cubic structure with all atoms at lattice points and a density of \(8.93 \mathrm{~g} / \mathrm{cm}^{3}\). Its atomic mass is \(63.5\) amu. Calculate the edge length of the unit cell.

Gold has cubic crystals whose unit cell has an edge length of \(407.9 \mathrm{pm}\). The density of the metal is \(19.3 \mathrm{~g} / \mathrm{cm}^{3}\). From these data and the atomic mass, calculate the number of gold atoms in a unit cell, assuming all atoms are at lattice points. What type of cubic lattice does gold have?

Explain why evaporation leads to cooling of the liquid.
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