According to kinetic molecular model in gases,

Analysis of the Question

This question tests your understanding of the Kinetic Molecular Theory (KMT), specifically how it describes the behavior and arrangement of gas particles compared to solids and liquids.

Explanation of the Concept

The Kinetic Molecular Theory provides a model to explain the behavior of matter in its three states:

• Solids: Particles are packed closely together in a fixed, regular pattern. They only vibrate about fixed positions. (This describes Option A and B).
• Liquids: Particles are close together but can move past one another. They have no fixed shape but have a fixed volume.
• Gases: According to the KMT, gas molecules are in constant, random motion. Because the intermolecular forces between them are negligible, they are very far apart compared to their size. Consequently, they expand to fill the entire volume of any container they are placed in.

Step-by-Step Solution

1. Evaluate Option A: This describes the structure of a solid. Particles in a gas are not closely packed.
2. Evaluate Option B: This also describes a solid. Gas particles do not have strong intermolecular bonds holding them in fixed positions.
3. Evaluate Option C: This aligns perfectly with the KMT for gases. Because gas molecules have high kinetic energy and weak intermolecular forces, they spread out to occupy all available space.
4. Evaluate Option D: This describes a state closer to a liquid or a dense fluid, not the ideal behavior of gas molecules as defined by the kinetic model.

Conclusion

The kinetic molecular model emphasizes that gas molecules are far apart and move randomly, allowing them to fill any container available to them.

Exam Tip: When dealing with KMT questions, remember the "Space" rule: Solids = No space (packed), Liquids = Little space (sliding), Gases = Maximum space (far apart).