Textbook Question
Which solid in each pair has the higher melting point and why? d. NaCl(s) or CaO(s)
Ch.13 - Solids & Modern Materials
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Chapter 13, Problem 48d
Which solid in each pair has the higher melting point and why?
a. Fe(s) or CCl4(s)
b. KCl(s) or HCl(s)
c. Ti(s) or Ne(s)
d. H2O(s) or H2S(s)
Verified step by step guidance1
Identify the type of intermolecular forces present in each compound.
Recognize that H_2O(s) has hydrogen bonding, while H_2S(s) has dipole-dipole interactions.
Understand that hydrogen bonds are generally stronger than dipole-dipole interactions.
Conclude that stronger intermolecular forces result in a higher melting point.
Determine that H_2O(s) has a higher melting point than H_2S(s) due to the presence of hydrogen bonding.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Intermolecular Forces
Intermolecular forces are the attractions between molecules that influence physical properties like melting and boiling points. Stronger intermolecular forces typically result in higher melting points. In the case of H2O and H2S, hydrogen bonding in H2O is a significant intermolecular force that contributes to its higher melting point compared to the weaker dipole-dipole interactions in H2S.
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Hydrogen Bonding
Hydrogen bonding is a specific type of strong dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine. In solid H2O, each water molecule can form up to four hydrogen bonds, creating a stable and structured lattice that requires more energy to break, thus resulting in a higher melting point than H2S, which lacks such extensive hydrogen bonding.
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Melting Point
The melting point is the temperature at which a solid becomes a liquid, reflecting the energy required to overcome the forces holding the solid's particles together. The melting point can vary significantly between substances based on their molecular structure and the strength of their intermolecular forces. In this comparison, H2O has a higher melting point than H2S due to its stronger hydrogen bonds.
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Related Practice
Textbook Question
Classify each of the following as a component of a silicate ceramic, an oxide ceramic, or a nonoxide ceramic. a. B4C
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)
Textbook Question
Which solid has the highest melting point? Why? C(s, diamond), Kr(s), NaCl(s), H2O(s)
Textbook Question
Identify the structure of each of the two unit cells shown in Problem 52 as the rock salt structure, zinc blende structure, fluorite structure, antifluorite structure, or none of these.
Textbook Question
An oxide of rhenium crystallizes with the unit cell shown here (rhenium=gray; oxygen=red). What is the formula of the oxide?