KINETIC PARTICLE
THEORY
By Mehrunnisa Qaisar
SYLLABUS CONTENT
1.1-States of matter
1.2-Kinetic particle theory
1.3-Changes in state of matter and kinetic particle theory
1.4-Diffusion
1.1- STATES OF MATTER
• Matter: Anything that occupies space and
has mass is matter.
• All living and non living things are matter.
• Matter is 5 states:
1. Solid
2. Liquid
3. Gas
4. Plasma
5. Bose- Einstein Condensate
• All these states are interchangeable if specific temperature and pressure conditions
are provided to them.
TABLE OF PROPERTIES
PROPERTIES
SOLID
LIQUID
GAS
SHAPE
FIXED
NOT FIXED
NOT FIXED
VOLUME
FIXED
FIXED
NOT FIXED
COMPRESSIBILITY
NOT COMPRESSABLE
NOT COMPRESSABLE
COMPRESSABLE
1.2- KINETIC PARTICLE THEORY
• Kinetic particle theory: It states that all matter is made up of tiny particles
and that these particles are in constant random motion.
• This theory focuses on three points:
1.
Describes the states of matter.
2.
Explains the difference between the properties of
solids, liquids and gases.
3.
Explains the changes in state of matter.
SOLID STATE
• The particles are closely packed.
• They vibrate at their fixed position.
• They have high attractive forces between its particles.
• All of that causes its shape to be fixed.
• Solids can not be compressed as their particles can not be moved further
close to each other.
• This allows solids to have fixed volume.
LIQUID STATE
• Liquids have lesser attractive forces between its molecules.
• They are usually found in clusters.
• The particles roll over each other as they move.
• This causes liquids to not have a fixed shape.
• The liquid particles even though are not closely packed they still have very
less space between them and hence can not be compressed.
• This phenomena causes liquids to have a fixed volume.
GAS STATE
• The gas particles are always in random motion.
• They move freely and are far apart from each other.
• The gas particles have negligible forces of attraction between them.
• This allows it to not have a fixed shape.
• The vast space between the particles allows it to be compressed as pressure
can cause particles to come together.
• This compressibility factor allows gases to not have a fixed volume
1.3- CHANGES IN STATE OF MATTER
AND THE KINETIC PARTICLE THEORY
• All particles of matter have kinetic energy.
• Moving down the list the kinetic energy decreases:
1.
Gas
2.
Liquid
3.
Solid
• When any matter is heated or is cooled, kinetic energy is either added or
removed from it causing it to affect the motion of the particles.
• This change in movement causes a change of state.
• Melting: It is the process by which a substance changes from solid state to
liquid state at a fixed temperature
• Melting point: It is that temperature at which a solid becomes a liquid.
• The temperature of the substance dose not change until all of the
substance has changed it state completely.
• Boiling: It is a process that occurs when a liquid substance changes its
state to a gas at a fixed temperature.
• Boiling point: It is the temperature at which a substance changes its state
from a liquid to a gas.
• The temperature remains constant
until all of the liquid has been
changed into a gas.
• The boiling point of a substance is
used to find the purity of any
substance.
• When a liquid boils, bubble can be
observed that show the
transition of liquid state
to gas.
• Evaporation: It is the process that occurs when
a liquid state changes to a gaseous state at
a temperature lower than its boiling point.
• Some particles in a liquid have more energy
and thus they easily escape the liquid surface.
• Liquids that evaporate quickly are called volatile liquids.
• Volatile liquids have their boiling points just above room temperature.
BOILING
EVAPRATION
Occurs only at boiling point
Occurs below boiling point
Through out the liquid
Only at the surface
Bubbles are formed
No bubbles formed
HEATING CURVE: IT IS THE GRAPH THAT SHOWS THE
CHANGE OF STATE WHEN A SUBSTANCE IS HEATED, IT IS
PLOTTED AS TEMPERATURE AGAINST TIME.
A: solid is heating
Temperature change
No state change
State: solid
Melting point
B: the process of melting occurs
No temperature change
State change
State: solid and liquid
State change completed
C: liquid is heating
Temperature change
No state change
State: Liquid
Boiling Point
D: The process of
boiling
Occurs
No temperature
change
State change
State: liquid and gas
state change
completed
E: gas is heating
Temperature change
No state change
State: Gas
• Freezing: It is the process in which a substance changes from liquid state to
a solid state at fixed temp.
• Freezing point: It is that temperature at which a substance changes from a
liquid to a solid.
• The freezing point and melting point are always the same. For example,
ice melts and freezes at 0 degrees.
• The temperature of the liquid substance stays constant until all liquid has
converted to solid.
• Condensation: It is a process in which a substance changes its state from a
gas to a liquid at a fixed temp.
• When gas touches a cold surface,
condensation takes places and it
changes from gas to a liquid.
• It is the reverse of boiling.
• Sublimation: It is the process in
which a substance turns directly
from a solid to a gas.
• This occurs when the particles at the
surface of the solid have enough
energy to escape, they break free
and thus
convert to gas.
• Desublimation: It is the process in
which gas directly changes from a gas to a
solid.
COOLING CURVE: IT IS THE GRAPH THAT SHOWS THE
CHANGE OF STATE WHEN A SUBSTANCE IS COOLED, IT IS
PLOTTED AS TEMPERATURE AGAINST TIME.
A
B
c
D
E
A: temperature change
state: Gas
No state change
condensation temperature
B: condensation
Temperature constant
State change
State: Gas/liquid
all gas has converted to liquid
C: temperature change
State: liquid
No state change
freezing point
D: freezing
State change
State: solid/liquid
Temperature constant
all liquid has
converted to solid
E: state: solid
No state change
Temperature change
• Exothermic: The process that releases heat is called as an exothermic
process.
• Endothermic: The process that absorbs heat is called as an endothermic
process.
• The heating curve shows an endothermic process as it shows the absorption
of heat.
• The cooling curve shows an exothermic process as it shows the release of
heat.
1.4- DIFFUSION
• The movement of particles from a region of
higher concentration to a region of lower
concentration.
• It is the evidence of the kinetic particle
theory.
• Diffusion in gases:
1.
The rate at which a gas diffuses from higher concentration to
lower concentration is with the help of its molecular mass.
2.
Molecular mass of a gas is the mass of its particles.
3.
It can be calculated by looking at the formulas of the particles
BROWNIAN MOTION
Brownian motion, also called Brownian movement, any of various
physical phenomena in which some quantity is constantly
undergoing small, random fluctuations.
MOLECULAR MASS CALCULATION
GAS
RELATIVE MOLECULAR MASS
Hydrogen (H2 )
1+1=2
Helium (He)
4
Methane (CH₄)
12+1+1+1+1=16
Ammonia (NH3)
14+1+1+1=17
Carbon dioxide (CO₂)
12+16+16=44
Nitrogen (N₂)
14+14=28
Oxygen (O₂)
16+16=32
A
14+1+1+1=17
NH3
RATE OF DIFFUSION
B
C
D
DEMONSTRATION
1+35.5=36.5
HCl
POROUS POT
EXPERIMENT
Fall: When X has a lower Mr than Y the gas X
diffuses into the pot causing the water level
at point Z to fall.
Rise: When X has a higher Mr than Y the gas
y diffuses out of the pot causing the water
level at point Z to rise.
Same: When both gas X and Y have similar
Mr this causes the gases to have same rate
of diffusion inside and out of the pot causing
the level of water at point Z to remain
unchanged.
• Diffusion in liquids:
1.
It is the same as that of gases as liquids move from higher concentration
to a lower concentration.
2.
The diffusion in liquids is much slower than that of gases.
3.
The rate of diffusion increases as the temperature is increased.
4.
This type of diffusion can be seen as a drop of ink is dropped into a glass
of water.
CONCEPT MAP
THANKYOU!!!
ADDITIONAL VIDEO FOR GENERAL
KNOWLEDGE BOSE-EINSTEIN
CONDENSATE
ADDITIONAL VIDEO FOR GENERAL
KNOWLEDGE PLASMA