Question

In gaseous substances, the individual molecules are relatively (close/far apart) and are moving freely, rapidly, and randomly.

Short answer

In gaseous substances, the individual molecules are relatively \(far\) apart and are moving freely, rapidly, and randomly.

Step-by-step solution

Gaseous substances are one of the states of matter. They have no fixed shape or volume and contain particles that move around freely. These particles have more energy and move more rapidly compared to those in solid or liquid states. #Step 2: Identifying the distance between particles in a gas#

In a gaseous substance, the individual molecules have a lot of kinetic energy, which means they are constantly moving and colliding with each other and the walls of their container. Due to this constant movement and the low intermolecular forces, the molecules are far apart from each other compared to particles in solids and liquids. #Step 3: Describing the movement of particles in a gas#

The movements of the particles in a gaseous substance are free, rapid, and random. They constantly collide with each other and the walls of the container. This is due to the high kinetic energy they possess compared to particles in solid or liquid states. #Step 4: Putting it all together#

To answer the question, in gaseous substances, the individual molecules are relatively far apart and are moving freely, rapidly, and randomly.

Key concepts

Gaseous State

In the gaseous state, substances exist with no fixed shape or volume, which is quite different from solids and liquids. The gas molecules spread out to fill any available space in their container due to the lack of strong intermolecular forces keeping them together. This characteristic of gases makes them highly compressible since there is a considerable amount of space between the particles. Such a state allows gases to diffuse rapidly and mix with other gases easily.
- The molecules are so far apart that it is difficult for them to settle in any set pattern or structure. - Gases can be easily compressed since the particles have much distance to cover and can be pushed closer together. - Gases occupy more volume than solids or liquids at the same temperature and pressure because their molecules move around freely in all directions.
Understanding the gaseous state is crucial to explain why balloons inflate with helium, why we can smell fragrances, or why gases create pressure inside containers.

Kinetic Energy

Kinetic energy plays a crucial role in defining the behavior of gas molecules. Kinetic energy refers to the energy possessed by an object due to its motion. In gases, kinetic energy is intricately tied to temperature; higher temperatures mean higher kinetic energy. Why is this important?
- More kinetic energy leads to faster-moving particles, increasing the frequency and force of their collisions with each other and the walls of a container. - Kinetic energy is why gases can expand to fill a container and why heating a gas typically raises the pressure it exerts. - In a state of thermal equilibrium, the average kinetic energy of gas particles is directly proportional to the temperature of the gas in Kelvin.
This is why heating a gas can lead to changes such as expansion or increased pressure. It is also why gas molecules in a hot environment are more likely to react, contributing to higher rates of chemical reactions.

Molecular Motion

Molecular motion in gases is characterized by free, rapid, and random movements. Due to their high kinetic energy, gas molecules move more vigorously compared to those in the solid and liquid states.
- This uninhibited movement results in gas molecules frequently colliding with one another and the walls of their containers, leading to what we observe as gas pressure. - The randomness of molecular motion means that over time, gas molecules fill their container evenly, no matter where they start. - Molecular motion is also essential for processes like diffusion, where gases spread out to evenly fill a space or intermix with other gases.
The randomness and speed of molecular motion explain many physical properties of gases, such as their ability to exert pressure uniformly in a container, their tendency to diffuse quickly, and the way they respond energetically to changes in temperature.