1.1 understand the arrangement, movement and energy of the particles in each
of the three states of matter: solid, liquid and gas
Solids have a fixed shape and volume. Their particles are arranged regularly and are tightly packed. They do not flow, and the particles vibrate about a fixed point. They have the strongest forces of attraction and are usually the most dense.
Liquids have a fixed volume, but their shape changes to fit the container. The particles have weaker forces of attraction than solids, but stronger than gases. The particles can flow over each other, and they are irregularly arranged.
Gases have no fixed shape or volume, they can be compressed, and they change shape to fit the container. They move randomly in different directions and collide with other particles. There are wide gaps between the particles and almost no forces of attraction between them.
1.2 understand how the interconversions of solids, liquids and gases are
achieved and recall the names used for these interconversions
Melting- Solid --> Liquid
Achieved by heating, increased thermal energy means the particles gain kinetic energy.
Boiling- Liquid --> Gas
Achieved by heating, increased thermal energy means the particles gain kinetic energy.
Freezing- Liquid --> Solid
Achieved by cooling, decreased thermal energy means the particles lose kinetic energy.
Achieved by cooling, decreased thermal energy means the particles lose kinetic energy.
Condensing- Gas --> Liquid
Achieved by cooling, decreased thermal energy means the particles lose kinetic energy.
Evaporation- Liquid--> Gas
Some particles on the surface move faster than average and have enough energy to break the bonds and become a gas.
Achieved by cooling, decreased thermal energy means the particles lose kinetic energy.
Evaporation- Liquid--> Gas
Some particles on the surface move faster than average and have enough energy to break the bonds and become a gas.
Sublimation- Solid--> Gas
Achieved by a sudden increase n temperature or high pressure conditions. e.g dry ice.
Achieved by a sudden increase n temperature or high pressure conditions. e.g dry ice.
1.3 explain the changes in arrangement, movement and energy of particles
during these interconversions.
Melting- The solid particles vibrate at an increasing speed with increased temperature until the forces of attraction can no longer hold them together, and it changes state.
Boiling- The liquid is heated to the point that all the forces of the attraction within it are broken and bubbles of gas are formed throughout the liquid.
Evaporation- Faster particles on the surface of the liquid have enough energy to break free from their bonds and evaporate to form a gas.
Condensing- The gas is cooled and the particles move slowly enough that they can form attractions between each other and form a liquid.
Freezing- If a liquid is cooled, the particles will begin to lose kinetic energy and their movement will slow until the forces of attraction will hold them in place as a solid.
Subliming- The particles gain kinetic energy very quickly, allowing all forces of attraction to break quickly and form a gas.
Melting- The solid particles vibrate at an increasing speed with increased temperature until the forces of attraction can no longer hold them together, and it changes state.
Boiling- The liquid is heated to the point that all the forces of the attraction within it are broken and bubbles of gas are formed throughout the liquid.
Evaporation- Faster particles on the surface of the liquid have enough energy to break free from their bonds and evaporate to form a gas.
Condensing- The gas is cooled and the particles move slowly enough that they can form attractions between each other and form a liquid.
Freezing- If a liquid is cooled, the particles will begin to lose kinetic energy and their movement will slow until the forces of attraction will hold them in place as a solid.
Subliming- The particles gain kinetic energy very quickly, allowing all forces of attraction to break quickly and form a gas.
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