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The changes of state of matters
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Melting
- Solid is heated, the particles obtain energy and vibrate at a faster rate.
- The vibration keeps increasing as the temperature increase until it reaches the melting point.
- At the melting point, the particles obtain enough energy to overcome the attractive forces between the particles.
- Therefore, the matter in solid state changes to a liquid.
- During melting, the temperature remains constant. This is because the heat energy is used to break the bond
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Vaporisation
- Occurs in two conditions: either evaporation or boiling.
- Evaporation occurs only on the surface of the liquid and at a slower rate.
- Boiling occurs to the whole liquid and happens very fast.
- Both will cause the attractive forces between particles to break and change the state from liquid to gas.
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Freezing
- Temperature drops and the heat energy is released.
- As the heat is released, the kinetic energy decreases, the movement of particles are slower and the particles are pulled closer by the strong forces between particles.
- Therefore, the physical state of the matter will change from liquid to solid.
- The temperature stays at the freezing point because the heat is released constantly.
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Condensation
- A process by which a gas or vapour changes to liquid state at a certain temperature.
- When the temperature drops, the gas loses its kinetic energy, and therefore it will change the physical state of matter to the liquid.
- Condensation occurs at or below the boiling point of the substance
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Sublimation
- A process of conversion of a substance from the solid to the vapour state without its becoming liquid.
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The melting point of naphthalene
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Heating curve of naphthalene |
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A
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- The particle are very closely packed together in an orderly manner
- The force between the particles is very strong.
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A-B
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- The naphthalene is heated the energy is converted to kinetic energy
- The temperature increase, the kinetic energy increase and the molecules vibrate faster about their fixed position.
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B
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- The naphthalene molecules have received enough energy to overcome the force of attraction between them.
- Some of the molecules begin to move freely.
- The naphthalene starts to melt and changes into a liquid.
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B-C
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- Naphthalene exists in both state, solid and liquid.
- The temperature remains constant because the heat is used to overcome the force of attraction.
- The constant temperature is called the melting point.
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C
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- The napthalene has turned into liquid completely
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C-D
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- The naphthalene is in the liquid state
- The temperature keeps increasing and gain more energy.
- The particle is then moving faster because the kinetic energy is increasing.
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The freezing point of naphthalene
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Cooling curve of naphthalene |
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P
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- The substance exists in the gaseous state
- Have very high energy and moving randomly
- The intermolecular force is weak.
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P-Q
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- The particles lose kinetic energy during cooling,
- The particle getting closer to each other and the temperature drops.
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S
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- The substance is still in the gas state
- The gas begins to condense and become liquid.
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Q-R
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- Stronger bonds form as gas change into a liquid.
- The substances exist both in gas and liquid.
- The energy produced during the formation of bonds is equal to the heat released to the surroundings during cooling.
- This is known as the freezing point.
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R
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- The substances exist fully in the liquid state
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R-S
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- The temperature keeps decreasing, causing the naphthalene molecules to lose heat energy.
- The movement of the particles slow down and move close to each other.
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