Textbook Question
Which solid in each pair has the higher melting point and why? d. NaCl(s) or CaO(s)
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Ch.13 - Solids & Modern Materials
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving93
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities44
- Ch.5 - Introduction to Solutions and Aqueous Solutions69
- Ch.6 - Gases97
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom48
- Ch.9 - Periodic Properties of the Elements73
- Ch.10 - Chemical Bonding I: The Lewis Model76
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory70
- Ch.12 - Liquids, Solids & Intermolecular Forces41
- Ch.13 - Solids & Modern Materials40
- Ch.14 - Solutions76
- Ch.15 - Chemical Kinetics90
- Ch.16 - Chemical Equilibrium56
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium127
- Ch.19 - Free Energy & Thermodynamics78
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry60
- Ch.22 - Organic Chemistry115
Chapter 13, Problem 40b
Identify each solid as molecular, ionic, or atomic. b. CO2(s)
Verified step by step guidance1
Identify the type of bonding present in the solid CO2.
Recognize that CO2 is composed of nonmetal atoms (carbon and oxygen).
Understand that CO2 forms covalent bonds between carbon and oxygen atoms.
Recall that molecular solids are composed of molecules held together by intermolecular forces.
Conclude that CO2(s) is a molecular solid because it consists of CO2 molecules held together by weak intermolecular forces.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Solids
Molecular solids are composed of molecules held together by intermolecular forces such as van der Waals forces, dipole-dipole interactions, or hydrogen bonds. These solids typically have low melting and boiling points compared to ionic or atomic solids. An example is solid carbon dioxide (CO2), which forms when gas is cooled and solidifies into a molecular structure.
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04:13
Crystalline vs Amorphous Solids
Ionic Solids
Ionic solids consist of positively and negatively charged ions held together by strong electrostatic forces known as ionic bonds. These solids generally have high melting and boiling points due to the strength of the ionic interactions. Common examples include sodium chloride (NaCl) and magnesium oxide (MgO).
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00:34Ionic Solid Identification Example
Atomic Solids
Atomic solids are composed of atoms held together by covalent bonds, metallic bonds, or van der Waals forces. They can be further categorized into covalent network solids, like diamond, which have very high melting points, and metallic solids, which conduct electricity and have variable melting points. Atomic solids are characterized by their strong bonding and structural integrity.
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Related Practice
Textbook Question
Rhodium has a density of 12.41 g/cm3 and crystallizes with the face-centered cubic unit cell. Calculate the radius of a rhodium atom.
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Textbook Question
Which solid in each pair has the higher melting point and why?
a. TiO2(s) or HOOH(s)
b. CCl4(s) or SiCl4(s)
c. Kr(s) or Xe(s)
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Textbook Question
Which solid has the highest melting point? Why? C(s, diamond), Kr(s), NaCl(s), H2O(s)
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Textbook Question
Plonium crystallizes with a simple cubic structure. It has a density of 9.3 g/cm3, a radius of 167 pm, and a molar mass of 209 g/mol. Use these data to calculate Avogadro's number (the number of atoms in one mole).
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