STATES OF MATTER

States of Matter

  1. Solid

    • Definite shape and volume.

    • Particles are tightly packed in a fixed arrangement.

    • Strong intermolecular forces restrict particle movement.

  2. Liquid

    • Definite volume but takes the shape of the container.

    • Particles are close together but can move past each other.

    • Weaker intermolecular forces than in solids.

  3. Gas

    • No definite shape or volume; fills the entire container.

    • Particles are far apart and move freely.

    • Very weak intermolecular forces.

  4. Phase Changes

    • Melting: Solid to liquid (endothermic).

    • Freezing: Liquid to solid (exothermic).

    • Evaporation: Liquid to gas (endothermic).

    • Condensation: Gas to liquid (exothermic).

    • Sublimation: Solid to gas (endothermic) without passing through liquid state.

    • Deposition: Gas to solid (exothermic) without passing through liquid state.

Diffusion

  • Definition: The movement of particles from an area of higher concentration to an area of lower concentration until evenly spread.

  • Factors Influencing Diffusion:

    • Concentration Gradient: A greater difference in concentration accelerates diffusion.

    • Temperature: Increased temperature enhances particle kinetic energy, thus increasing diffusion rate.

    • Particle Size: Smaller particles diffuse more rapidly than larger ones.

    • Medium of Diffusion: Gases diffuse more quickly than liquids because of increased space between particles in gases.

  • Real-World Examples:

    • The dispersion of perfume scent throughout a room.

    • Food coloring dispersing in water.

  • Applications in Real Life:

    • Essential biological functions, such as oxygen transfer in the lungs.

    • Various industrial processes, including techniques for separation such as chromatography.