Question

Liquids and solids are (more/less) compressible than are gases.

Short answer

Liquids and solids are LESS compressible than gases due to the more closely packed particles and stronger intermolecular forces.

Step-by-step solution

Understand the States of Matter

There are three main states of matter: solids, liquids, and gases. In solids, the particles are tightly packed together and have a defined shape and volume. In liquids, particles are still packed fairly close together but can move a bit more freely, allowing them to take the shape of their container while retaining a fixed volume. In gases, particles are in constant motion and are very spread out, and they have no defined shape or volume, instead adopting the shape and volume of their container.

Compare Compressibility

Compressibility refers to the capacity of a substance to reduce its volume when subjected to pressure. This property mainly depends on the spacing between particles and the forces acting between them. Solids and liquids have very limited space between their particles, and there are strong forces holding them together. Hence, they are difficult to compress. On the other hand, gases have a large amount of space between their particles with weak forces between them, making them much easier to compress.

Determine the Answer

Based on this comparison of the three states of matter, we can conclude that liquids and solids are LESS compressible than gases due to the more closely packed particles and stronger intermolecular forces.

Key concepts

States of Matter

The exploration of the states of matter is a fundamental concept in science that describes the distinct forms that different phases of matter take on. Solids are characterized by their rigid structure and fixed shape and volume. This rigidity is due to the closely packed arrangement of particles, which are mainly in vibrational motion about fixed points.

Liquids, on the other hand, have a definite volume but no fixed shape. They adapt to the shape of their container because their particles are less tightly packed than in solids, allowing them to move around and slide past one another. This fluidity is what distinguishes liquids from solids.

Gases are the most energetic state of matter under standard conditions and are composed of particles that are much farther apart compared to solids and liquids. These particles move freely at high speeds, colliding with each other and the walls of their container, leading to the gas occupying the entire available volume. Understanding these states is crucial to grasping other material properties, such as compressibility.

Compressibility of Substances

Looking at a substance's compressibility reveals how it responds to external pressure. Essentially, compressibility is an indication of how much a substance can decrease in volume when pressure is applied. Each state of matter has a characteristic response: solids and liquids are typically much less compressible than gases.

In solids, atoms and molecules are packed so tightly that there is very little room to compress further, except under extreme pressures. Liquids have a slight amount more room between particles and thus a minimal amount of compressibility, but it is substantively less than gases.

Gases, which are composed of widely spaced particles, have a lot of room to 'squeeze' closer together, making them significantly more compressible. This difference in compressibility ties into many practical applications, ranging from pneumatic systems using compressed air to the behavior of different materials under mechanical stress.

Intermolecular Forces

The concept of intermolecular forces is central to understanding the behavior of different states of matter, especially when compressing a substance. These are the forces that mediate interaction between molecules, dictating how closely they can pack together and how they move in relation to one another.

In solids, the intermolecular forces are so strong that they keep the molecules tightly bound in a fixed arrangement. Liquids exhibit a balance of attractive forces strong enough to maintain close contact between molecules but not strong enough to hold them rigidly in place, hence their ability to flow.

In gases, these intermolecular forces are minimal, as evidenced by the large distances between particles and the ease with which gases expand to fill a container. Understanding these subtle yet powerful forces helps to grasp a range of phenomena, from why water forms droplets to how refrigerants transition between liquid and gaseous states in cooling systems.