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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 14a
Capitolo 11, Problema 14a

At room temperature, Si is a solid, CCl4 is a liquid, and Ar is a gas. List these substances in order of (a) increasing intermolecular energy of attraction

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1. The intermolecular energy of attraction is determined by the type of bonding and the strength of the forces between the particles in a substance. The stronger the forces, the higher the intermolecular energy of attraction.
2. Silicon (Si) is a solid at room temperature because it forms a covalent network structure, where each atom is bonded to its neighbors by strong covalent bonds. This results in a very high intermolecular energy of attraction.
3. Carbon tetrachloride (CCl4) is a liquid at room temperature. It is a molecular compound with polar covalent bonds, but the molecule as a whole is nonpolar due to its symmetrical tetrahedral shape. Therefore, the intermolecular forces are weaker dispersion forces, resulting in a lower intermolecular energy of attraction than Si.
4. Argon (Ar) is a gas at room temperature. It is a noble gas and exists as individual atoms. The only intermolecular forces present are weak dispersion forces, which result in a very low intermolecular energy of attraction.
5. Therefore, the order of increasing intermolecular energy of attraction is Ar < CCl4 < Si.

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Intermolecular Forces

Intermolecular forces are the forces of attraction or repulsion between neighboring particles (atoms, molecules, or ions). These forces determine the physical properties of substances, such as boiling and melting points. Stronger intermolecular forces result in higher energy requirements to change states, while weaker forces allow for easier transitions between solid, liquid, and gas phases.
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Intermolecular vs Intramolecular Forces

States of Matter

The states of matter—solid, liquid, and gas—are defined by the arrangement and energy of particles. In solids, particles are closely packed and vibrate in fixed positions, leading to strong intermolecular forces. In liquids, particles are still close but can move past one another, resulting in moderate intermolecular forces. Gases have particles that are far apart and move freely, indicating weak intermolecular forces.
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Element States of Matter

Temperature and Energy

Temperature is a measure of the average kinetic energy of particles in a substance. At room temperature, the kinetic energy of particles in gases is higher than in liquids and solids, which affects their intermolecular interactions. As temperature increases, the energy can overcome intermolecular forces, leading to phase changes, such as melting or boiling.
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Temperature vs Heat
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Domanda del libro di testo

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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Domanda del libro di testo

(c) What happens to a gas if you put it under extremely high pressure?

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Domanda del libro di testo

At standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (d) Are the molar volumes in the solid state as similar as they are in the gaseous state?

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Domanda del libro di testo

(a) How does the average kinetic energy of molecules com- pare with the average energy of attraction between mole- cules in solids, liquids, and gases?

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Domanda del libro di testo

At standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively (b) On cooling to 160 K, both substances form crystalline solids. Do you expect the molar volumes to decrease or increase on cooling the gases to 160 K?

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