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Ch.11 - Liquids and Intermolecular Forces
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.11 - Liquids and Intermolecular ForcesProblema 13
Capitolo 11, Problema 13

As a metal such as lead melts, what happens to (a) the average kinetic energy of the atoms? (b) the average distance between the atoms?

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Step 1: Understand that melting is a phase change from solid to liquid, which occurs at a constant temperature for a pure substance.
Step 2: Recognize that during melting, the temperature remains constant, so the average kinetic energy of the atoms, which is directly related to temperature, does not change.
Step 3: Consider the structure of a solid, where atoms are closely packed in a fixed arrangement, and compare it to a liquid, where atoms are more loosely arranged and can move past each other.
Step 4: Realize that as the metal melts, the rigid structure breaks down, allowing atoms to move more freely, which increases the average distance between them.
Step 5: Conclude that during melting, while the average kinetic energy of the atoms remains constant, the average distance between the atoms increases as the solid structure transitions to a liquid state.

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Kinetic Energy and Temperature

Kinetic energy is the energy of motion, and in the context of atoms, it relates to their temperature. As a substance heats up, the average kinetic energy of its atoms increases, leading to more vigorous motion. This is crucial for understanding phase changes, such as melting, where the temperature rises until the solid structure breaks down.
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Kinetic Energy Formulas

Phase Changes

Phase changes refer to the transitions between solid, liquid, and gas states of matter. During melting, a solid absorbs heat, causing its atoms to gain kinetic energy and move apart, transitioning into a liquid state. This process illustrates how energy input affects the arrangement and behavior of atoms in different phases.
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Entropy in Phase Changes

Interatomic Forces

Interatomic forces are the attractive and repulsive forces between atoms that determine the structure and stability of a material. In solids, these forces keep atoms closely packed. As a metal like lead melts, these forces weaken, allowing atoms to move further apart, which increases the average distance between them and facilitates the transition to a liquid state.
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Types of Intermolecular Forces
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At standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (c) The densities of crystalline Cl2 and NH3 at 160 K are 2.02 and 0.84 g/cm3, respectively. Calculate their molar volumes.

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