States of Matter - WordPress.com€¦ · 1/2/2018 · States of Matter SOLID LIQUID GAS. Kinetic...
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States of MatterSOLID LIQUID GAS
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Kinetic molecular theory
Explains the behaviour of the particles in all 3 states of matter
TB. pg 56
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Model (textbook page 56)
1. PARTICLES
2. CONSTANT MOTION
3. SPACES
4. FORCES
5. COLLISIONS
6. AVERAGE KINETIC ENERGY CONSTANT
TB. pg 56
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Robert Brown
“Brownian Movement”
The random movement of microscopic particles suspended in a liquid or gas, caused by collisions with molecules of the surrounding medium.
TB. pg 45
Write this
down
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Important Definitions
Diffusion
Movement of the particles of a substance in between particles of a second substance – from an area of highconcentration to an area of lowconcentration
TB. pg 46
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SOLIDS• Particles only vibrate
• Extremely small spaces between the spaces
• Very strong forces between the particles
• Diffusion does not occur
• Cannot be compressed
• Retains its shape
• Particles arranged in a crystal lattice
• Has a specific melting point under standard conditions
TB. pg 47
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LIQUIDS• Particles move randomly but in a restricted fashion
• Smaller spaces between the particles than in gases
• Forces between the particles are weaker than in solids
• Diffusion occurs
• Collisions between the particles
• Fills the base of the container
• Takes on the shape of the bottom of the container
• Liquids exert pressure in all directions
• Has a specific boiling point and freezing point under standard conditions
TB. pg 47
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GAS• Particles move randomly and quickly
• Huge open spaces between the particles
• Weak or negligible forces between particles
• Diffusion occurs and it is faster than in liquids
• More intense collisions occur between particles than in liquids
• Is compressible
• Gas exerts pressure in all directions
• Has a specific condensation point under standard circumstances
TB. pg 47
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STATE CHANGE
WHAT IS THIS?
TB. pg 47
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The possible state changes are:
1.Melting
2.Evaporating
3.Condensing
4.Freezing
5.Crystallizing
6.SublimationTB. pg 47
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• Melting point: The temperature at which a solid completely changes into a liquid.
• Freezing point: The temperature at which a liquid completely changes into a solid.
• Boiling point: The temperature of a liquid at which the pressure of the vapour inside the bubbles (vapour pressure) is equal to the surrounding atmospheric pressure.
TB. pg 47
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• The chemical composition stays the same
• Particle size
• Particle Shape
• Number of particles
During a phase changeThe physical properties change
Forces between particles are
weakened or broken.
In molecular substances – weak
intermolecular forces broken first –
requires small amounts of energy
• More organised structure = greater
forces between particles
• Less organised structure = less force
between particles
TB. pg 47+49
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INTERMOLECULAR
FORCES
INTRAMOLECULAR
FORCES
H
H
HH
O
O• Requires a lot more
energy
• Strong forces• Requires little energy
• Van de Waals forces
• No chemical bonds made
• Can be reversed
Phase change
TB. pg 48
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Looking inside molecules during a
STATE CHANGE
TB. pg 49
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During condensation…
• Speed of particles: Slow down
• Spaces: Decrease
• Collisions: Less intense
• Forces: Stronger
• Arrangement: Still random
TB. pg 49
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During Freezing…
• Speed of particles: Slow down
even more
• Spaces: Decrease (almost touch)
• Collisions: Vibrate
• Forces:Very strong
• Arrangement: Orderly
TB. pg 49
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During Melting…
• Speed of particles: Speed up
• Spaces: Increase
• Collisions: Increase
• Forces: Weaker
• Arrangement: Less orderly
TB. pg 49
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During Evaporation…
• Speed of particles: Extremely fast
• Spaces: Large (far apart)
• Collisions: Severe (high velocity)
• Forces: Very weak
• Arrangement: Random
TB. pg 49
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Energy changes during a
STATE CHANGE
TB. pg 49
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• It’s a Solid• fixed positions: vibrate (forces of attraction and
repulsion)
• heated: vibrate more energetically = increases
average kinetic energy = temperature rises
• doesn’t change phase yet:
• Has “kinetic and potential energy”
TB. pg 49
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• It’s still a solid • Heated to a temperature at which melting begins –
further heat transfer does not increase kinetic
energy but potential energy.
• Lattice is now breaking apart into liquid phase –
particle more free to move
• Only when ALL have broken free – heat makes
kinetic energy increase and temperature now
increases
TB. pg 49
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• Now it’s a liquid• When liquids temperature reaches boiling point –
temperature remains constant until all liquid bonds
broken and all has been changed into vapour.
• Heat added during boiling – increases potential
energy
• Usually takes more energy to vaporise than to
melt….WHY?
TB. pg 49
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the heating / cooling curve
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Represents phase change on a graph
If read from left to right: HEATING CURVE
If read from right
to left: COOLING
CURVE
DRAW THISEXPLANATION PG. 50
TIME (s)
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To remember:During a phase change:
- Average kinetic energy remains the same
- Speed does not change
- Temperature remains constant
- Energy is used to break bonds between
particles from existing structure rather than to
make them move faster.
Potential energy
increases.
0
5
10
15
20
25
30
35
40
TB. pg 50
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CLASS
ACTIVITY
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1.1 What will the phase be of substance X at room temperature? (1)
1.2 What is the boiling point of substance X? (1)
1.3 Substance X was heated for 27 minutes. Why does the temperature
between time 4 – 8 minutes stay constant although heat was added? (2)
1.4 What happens to the particles of substance X between 0 – 4 minutes? (1)
1.5 At what stage (I, II, III, IV and V) will the particles have the most energy?
Give a reason for your answer. (3)
1.6 Is the substance Water? Why or why not? (2)
[10]
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• 1.1 Liquid √ (1)
• 1.2 55°C √ (1)
• 1.3 Energy that is added is used to break particles out of their existing structure / state √ and not to make the particles vibrate / move faster √ (2)
• 1.4 The particles are in a solid state and as energy is added the particles start vibrating more until they are able to “break” out of the solid structure and form a liquid. √ (1)
• 1.5 V √ Highest temperature √ indicates highest kinetic energy √ (3)
• ONLY 1 mark if say: particles are in the gaseous phase.
• 1.6 NO √ - Water boils at 100°C and not 55°C √ (2)
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: Heating and
Cooling curves
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Determining the state of a substances by looking at melting
and boiling points
M BSOLID LIQUID GAS
Eg. Water 0 ºC 100 ºC
ice Water vapour
Which state is water at:
78℃?-8℃?
10℃?
10𝟏℃?
TB. pg 51
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Practice: Use the table on page 51
According to the melting and boiling points in the table,
determine the state of the following compounds:
1.HF at 0℃?
2. Chlorine at -100℃?
3. Ammonia at -24℃?
4. HBr at -66℃?
TB. pg 51
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HomeworkExercise 3 pg. 52-53Exercise 4 pg. 57-60
TB. pg 53-60
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