This document provides an overview of the key topics in the chapter on matter from a 9th grade science textbook. It defines matter as anything that occupies space and has mass. It describes the three common states of matter - solid, liquid, and gas - and their characteristic properties. It also discusses less common states like plasma and Bose-Einstein condensate. The document outlines various processes by which matter can change states, like melting, boiling, sublimation, and evaporation. It explains how temperature and pressure can affect a substance's state and cause changes between solid, liquid, and gas. In closing, it reviews the factors that influence the rate of evaporation.

1. MATTER IN OUR SURROUNDINGS
CHAPTER:1
CLASS:IX

2. MATTER
Matter is anything that occupies space
and has mass that is they have mass and
volume.

3. LEARNING OBJECTIVES
STUDENTS WILL BE ABLE TO:
 Define matter
 Illustrate the properties of particles of matter
 Describe the states of matter with their properties
 Tell the effect of pressure and temperature on the states of matter
 Determine the various processes of conversation of states
 Define evaporation
 Illustrate the factors responsible for the rate of evaporation

4. PHYSICAL NATURE OF
MATTER
Matter is made up of particles, these
particles unite together and form matter.
Particles are very small in size and are
unable to see with naked eyes.

5. CHARACTERISTICS OF PARTICLES
 PARTICLES OF MATTER HAVE SPACE BETWEEN THEM
Particles of one type of matter fits into or occupies the spaces present between particles of other.
For example- dissolve salt/ sugar/ dettol in water.
 PARTICLES OF MATTER ARE CONTINUOUSLY MOVING
Particles of matter possess kinetic energy. As the temperature increases particles move faster.
For example: the fragrance of incense stick placed in the corner of a room spread in the whole room, smell of the
cooking food, perfumes used by us.
 PARTICLES OF MATTER ATTRACT EACH OTHER
Particles of matter have force acting between them. This force keeps the particles together and this force of
attraction varies from one matter to another.
For example: it is difficult to break a iron ball than chalk while we easily cut the water flow coming from the tap
and we easily move here and there in the air.

6. STATES OF
MATTER

7. 20.

8. 1. SOLID
2. LIQUID
3. GAS
4. PLASMA
5. BOSE-EINSTEIN
CONDENSATE

9. SOLID STATE
CHARACTERISTICS:
 HAVE DISTINCT SHAPE
 HAVE DISTINCT BOUNDARIES
 HAVE FIXED VOLUME
 HAVE NEGLIGIBLE COMPRESSIBILITY
 PARTICLES VIBRATE BACK AND FORTH IN THE SAME POSITION
 PARTICLES ARE HELD TOGETHER BY STRONG FORCE OF ATTRACTION

10. LIQUID STATE
CHARACTERISTICS:
 DO NOT HAVE A FIXED SHAPE
 HAVE FIXED VOLUME
 ARE NOT RIGID
 PARTICLES MOVE FREELY
 PARTICLES HAVE GREATER SPACE BETWEEN THEM AS COMPARED TO SOLID
 SOLID, LIQUID AND GASES CAN DIFFUSE INTO LIQUIDS.

11. GASEOUS STATE
CHARACTERISTICS:
 DO NOT HAVE FIXED SHAPE AND VOLUME
 ARE HIGHLY COMPRESSIBLE
 HAVE HIGH RATE OF DIFFUSION
 LARGE SPACE PRESENT BETWEEN THE PARTICLES
 PARTICLES HAVE HIGHEST KINTIC ENERGY & MOVE VERY RANDOMLY

12. PLASMA
CHARACTERISTICS:
 CONSIST OF SUPER ENERGETIC AND SUPER EXCITED PARTICLES
 PARTICLES ARE PRESESNT IN IONISED STATE. EXAMPLE: FLUORESCENT
TUBE(HELIUM AND SOME OTHER GASES) & NEON SIGN BULBS(NEON GAS IS
PRESENT)
 THE GAS GETS CHARGED/IONISED WHENEVER ELECTRIC ENERGY FLOWS
THROUGH IT. THIS CHARGING UP CREATES A PLASMA GLOWING INSIDE THE
TUBE OR BULB.
 THE PLASMA GLOWS WITH A SPECIAL COLOUR DEPENDING ON THE NATURE OF
GAS.
 THE SUN & STARS GLOW DUE TO THE PRESENCE OF PLASMA IN THEM (PLASMA
IS CREATED IN STARS DUE TO VERY HIGH TEMPERATURE)

13. BOSE-EINSTEIN
CONDENSATE
 In 1920, Indian Physicist Satyendra Nath Bose performed certain
calculations for 5th state of matter.
 On the basis of his calculations Einstein predicted a new state of matter
“THE BOSE – EINSTEIN CONENSATE”
 In 2001, Eric A. Cornell, Wolfgang Ketterle & Carl E. Weiman of USA
received Nobel prize in Physics for achieving BEC of rubidium(Rb).
 BEC is formed by cooling a gas of extremely low density at 0Kelvin -
which on condensation forms liquid because of loss of energy. They are
super unexcited and super cold atoms.

14. CHANGES IN THE STATE OF MATTER
1. EFFECT OF TEMPERATURE
On increasing temperature the kinetic energy the particles
increases and solid becomes liquid and liquid becomes gas.
SOLID LIQUID GAS

15. MELTING POINT
 MELTING POINT: The temperature at which a solid melts to become a liquid
at a atmospheric pressure is known as melting point.
 Melting point of ice is: 273.13Kelvin or 0 degree celcius
 During melting there is no change in the temperature till the whole solid
Melts into liquid even after reaching its melting point.

16. So where does this heat go
This heat is used up in changing the state by overcoming the forces
of attraction between the particles. As this heat energy is absorbed
by ice without showing any rise in temperature.
 LATENT HEAT OF FUSION: the amount of heat energy
that is required to change 1kg of a solid into liquid at room
atmospheric pressure at its melting point (particles in
water at 273K have more energy as compared to particles
in ice at same temperature).

17. BOILING POINT
BOILING POINT: The temperature at which a liquid starts boiling at the atmospheric
pressure is known as its boiling point.
BOILING POINT OF WATER: 373K/ 100 DEGREE CELCIUS

18. WHEN A LIQUID BOILS, ITS
TEMPERATURE REMAINS SAME
SO, WHERE DOES THE HEAT ENERGY GO
This heat is used up in overcoming the force of attraction between
the particles. As this heat energy is absorbed by liquid without
showing any rise in temperature.
LATENT HEAT OF FUSION: The amount of heat energy that is
required to change 1kg of liquid into vapour/gas at atmospheric
pressure at its boiling point.

19. SUBLIMATION
A change of state directly from solid to gas without changing into liquid
state or vice-versa is called sublimation.
For example: ammonium chloride, naphthalene balls, camphor etc.

20. 2. EFFECT OF PRESSURE
When we apply pressure and compress a gas, the particles of
matter come closer and there is change of state.
For example: LPG, CNG, solid carbon dioxide( known as dry ice
as solid carbon dioxide directly changes into gaseous state on
decrease of pressure to 1 atmosphere without converting into
liquid.

21. THUS, PRESSURE AND TEMPERATURE DETERMINE
THE STATE OF A SUBSTANCE- SOLID, LIQUID AND
GAS.

22. PROCESSES OF INTERCONVERSION
Condensation: is the process by which water vapor in the air is changed into liquid water. In other
words, the water in the air, a gas known as water vapor, from your hot shower cooled when it met the
surface of the cold mirror. This caused the water vapor to condense, or turn into its liquid.
Vaporisation :is the process when a liquid changes into a gas, the process is called vaporization.
Fusion: occurs when a substance changes from a solid to a liquid.
Solidification: also known as freezing, is a phase change of matter that results in the production
of a solid. Generally, this occurs when the temperature of a liquid is lowered below its freezing
point.
Sublimation: A change of state directly from solid to gas without changing into liquid state or
vice-versa is called sublimation.

23. EVAPORATION
Evaporation: The process of a liquid changing into vapour (or gas) even below its
boiling point is called evaporation. The wet clothes dry due to evaporation of
water present in them.
Thus the fast moving particles (or molecules) of a liquid are constantly escaping
from the liquid to form vapor (or gas).

24. FACTORS AFFECTING EVAPORATION
 The rate of evaporation is affected by the following factors:
 Temperature: The rate of evaporation increases with an
increase in temperature.
 Surface area: The rate of evaporation increases with an
increase in surface area.
 Humidity: The amount of water vapour present in the air
is called humidity. The rate of evaporation decreases with
an increase in humidity.
 Wind speed: Evaporation increases with an increase in
wind speed.

25. HOW DOES EVAPORATION CAUSE COOLING?
 During evaporation, the liquid keeps on evaporating. The particles of liquid absorb
energy from the surrounding to regain the energy lost during evaporation. This
absorption of energy from the surroundings make the surroundings cold.
APPLICATIONS:

26. WHY DO WE SEE DROPLETS ON THE OUTER SURFACE OF
A GLASS CONTAINING ICE-COLD WATER?
This is due to water vapour present in air on coming in
contact with the cold glass of water, loses energy and gets
converted to liquid state, which we see as water droplets.

27. THANK YOU
Made by: Monika Pal
TGT science
KV NERIST