P3 Particle Model Of Matter 1

Density (P3.1.1)
1. Density (kg/m3)=mass (kg) DIVIDED BY volume (m3)
2. A measure of how compact a substance is. How much mass a substance contains per it's volume.
  1. In a dense material the particles are tightly packed together. In a less dense material the particles are more spread out.
    1. If you compressed the material, the particles would move closer together making it more dense.
      1. Decreasing volume=increase in density.
  2. REQUIRED PRACTICAL- Finding the density of regular and irregular solids and liquids.
    1. Regular solids- use a balance to measure it's mass, measure the length width and height with a ruler, then calculate the volume using the appropriate calculation for the shape. Use the volume and mass to find density.
    2. Irregular solids- use a balance to measure it's mass, submerge the object in a eureka can with a measuring cylinder beneath the spout, the volume of water displaced into the measuring cylinder is the volume of the object. Use the volume and mass to find density.
    3. Liquids- place a measuring cylinder on a balance and zero the balance, pour 10ml of the liquid into the measuring cylinder and record the liquids mass, pour another 10ml into the measuring cylinder, repeating the process until the cylinder is full and recording the total volume and mass each time. For each measurement ude the formula to find density (remember 1ml=1cm3). Find the mean for your calculated densities.
3. SOLIDS
  1. Solids have a fixed shape, cannot flow and cannot be compressed easily. They have a fixed volume. Their particles are arranged in a regular order. The particles are tightly packed together and have strong bonds. The particles vibrate but don't have much room to move.
4. LIQUIDS
  1. Liquids flow, have a fixed volume and cannot be compressed. Their particles are arranged in a random way and have weaker bonds than a solid. The particles vibrate more than a solid but are still tightly packed.
5. GASSES
  1. Gasses completely fill and take the shape of their container. They can be compressed and they flow. The particles are free to move and have practically no bonds. Gasses have a lower density than liquids and solids and their particles have no pattern and are free to move.
    1. LIQUIDS & GASSES = Fluids
Changes Of State (P3.1.2)
1. A change of state is a physical change NOT a chemical change. You don't end up with a new substance, it's the same substance you started with just in a different form.
  1. The number of particles doesn't change, they're just arranged differently. This means mass is conserved, no mass is lost when the substance changes state.
2. Solid to liquid=melting
3. Liquid to gas=boiling OR evaporating
4. Liquid to solid=freezing
5. Gas to liquid=condensing
6. Solid to gas=sublimating
7. Gas to solid=deposition OR reverse sublimation
Internal Energy (P3.2.1)
1. The internal energy of a system is the total energy that its particles have in their kinetic and potential energy stores.
  1. The particles in a system vibrate or move around, meaning they have energy in their kinetic energy stores.
  2. The particles in a system also have energy in their potential energy stores due to their positions.
  3. Heating the system transfers energy to it's particles because they move faster and gain energy in their kinetic stores. This increases internal energy.
    1. This leads to either a change in temperature or a change in state. If the temperature changes, the size of the change depends on the mass of the substance, the specific heat capacity of the substance and the energy input.
      1. If the substance is heated enough this will lead to a change in state because the particles will have enough energy in their kinetic energy stores to break the bonds and change state.

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