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Ch.13 - Solids & Modern Materials
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.13 - Solids & Modern MaterialsProblem 48d
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 guidance
1
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.

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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