Class 9 Science(chemistry) chap 1 notes

 Chapter 1 

Matter in our surroundings

This article brings you the CBSE Class 9 Science notes on chapter 1 'Matter in Our Surroundings'. These chapter notes are prepared by the subject expert and cover every important topic from the chapter. In between these notes, exercise questions are provided. Students must solve these questions to test their understanding about the learned topics. These questions will help you to track your preparation level and get a hold on the subject. 

• In this chapter 1 MATTER IN OUR SURROUNDINGS we cover following topics 

• Matter,states of matter and its properties,  characteristics of matter

• Diffusion and its application, Brownian movement,change of state of matter, evaporation

Keynotes of chapter 1  Matter in our surroundings are

Matter :-Anything which occupy space and have mass  is called Matter.

For example: chair, car, water ,air, mountain, etc.

It exists in the form of  five basic elements The PANCH TATVA - air, water, sky, soil, fire.

States of matter:-

Matter can be classified as Solid, liquid amd gas on the basis of their interparticle forces and the arrangement of particles.

These three forms of matter are imterconvertible by  increasing or decreasing temperature and pressure

For example: ice can be converted from solid to liquid by increasing the temperature.

Solids:

• have a fixed shape and cannot flow, because their particles cannot move from place to place
• cannot be compressed (squashed), because their particles are close together and have no space to move into

Liquids:

• flow and take the shape of their container, because their particles can move around each other
• cannot be compressed, because their particles are close together and have no space to move into

Gases:

• flow and completely fill their container, because their particles can move quickly in all directions
• can be compressed, because their particles are far apart and have space to move in all directions.

• Solid	Liquid	Gas
  Constituent particles are very closely packed.	Constituent particles are less closely packed.	Constituent particles are far apart from each other.
  Force of attraction between particles is very strong.	Force of attraction between particles is less strong.	Force of attraction between particles is negligible.
  Force of attraction between particles is very strong.	Kinetic energy between particles is more than that in solids.	Particles have maximum kinetic energy.
  Have definite shape and volume.	Do not have definite shape but definite volume.	Neither have definite shape nor definite volume.
  Have high density and and can not be diffused.	Density is lower than solids and can diffuse.	Density is least and can easily diffuse.
  Incompressible.	Almost incompressible.	Highly compressible.

Characteristics of matter :- 

• everything that we touch,see, hear, smell and feel is matter.

• matter is made up of really tiny particles which are known as atom and atoms can not be seen by naked eyes.Atoms have space between them and these particles attract each other due to  the force of attraction.

•The particles of which matter is comprised  of influence its state and its properties ( physical and chemical properties).

Diffusion :-

 Particles of matter intermix on their own with each other. They do so by getting into the spaces between the particles. This intermixing of particles of two different types of matter on their own is called diffusion. 

Applications of Diffusion:

Dissolving a solid in a liquid:

• When a crystal of potassium permanganate is placed in a beaker of water, the water slowly turns purple on its own, even without stirring.
• Both potassium permanganate crystal and water are made up of tiny particles.
• When the potassium permanganate crystal is put in water, the purple colored particles of potassium permanganate spread throughout water making the whole water look purple.
• Actually, on dissolving, the particles of potassium permanganate get into the spaces between the particles of water.
• This shows that the particles have spaces between them and are continuously moving on their own.

 

Mixingof two gases:

• Fragrance of an incense stick (agarbatti) lightened in one corner of a room, spreads in the whole room quickly.
• The particles of gases (or vapours) produced by burning the incense stick move rapidly in all directions and mix with the moving particles of air in the room
• This also shows that the partices of matter are constantly moving.

 Brownian movement:- It is the random motion of particles suspended in a fluid [a liquid or a gas] resulting from their collision with the fast-moving molecules in the  fluid.this movement was  given by Robert Brown[Scottish Botanist].

Try the following questions:

Q1. What are the conditions for something to be called matter?

Q2. Why do gases neither have fixed volume nor fixed shape?

Q3. How does the smell of food being cooked in the kitchen reaches us even from a considerable distance?

Q4. Explain why does diffusion occurs more quickly in gases than in liquids?

Temperature: Common and SI units

• Common unit: Degree Celsius (^oC)
• SI unit: Kelvin (K)
• Relation between common unit and SI unit of temperature:

                                    0 ^oC = 273K

Change of State of Matter: 
Physical states of matter can be interconverted into each other by following two ways:

1. By changing the temperature

2. By changing the pressure 

1. Effect of Change of Temperature:

Solid to liquid:

• On increasing the temperature of solids, the kinetic energy of the particles increases which overcomes the forces of attraction between the particles thereby solid gets converted to a liquid.

• Melting: Change of solid state of a substance into liquid is called melting.
• Melting point: The temperature at which a solid melts to become a liquid at the atmospheric pressure is called its melting point.
• Melting point of ice is 0^oc.

(a) Liquid to gas:

• On heating a liquid like water, the kinetic energy of its particles increases as high as in a gas, thus causing the liquid to change to a gas.

• Boiling: The change of a liquid substance into gas on heating is called boiling.
• Boiling point: The temperature at which a liquid boils and changes rapidly into a gas at the atmospheric pressure is called its boiling point.
• Boiling point if water is 100^oC.

(b) Gas to liquid:

• On cooling a gas like steam (or water vapour), the kinetic energy of its particles is lowered down, causing them to move slowly and bringing them closer, forming a liquid.

• Condensation: The process, in which a gas, on cooling, turns into a liquid at a specific temperature is called condensation or liquefaction.

(c) Liquid to solid:

• When a liquid is cooled down by lowering its temperature, its particles lose the kinetic energy and come to a stationary position, causing the liquid to turn to soilid.

• Freezing: The change of a liquid substance into soilid by lowering its temperature is called freezing.
• Freezing point: The temperature at which the state of a substance changes from a liquid to a solid is called the freezing point of that substance.

Fusion:The process of melting, that is, change of solid state into liquid state is also known as fusion. 

Latent heat: The heat energy that is required to change the state of a substance without causing any ruse in the temperature of the substance is called latent heat. Since, the heat energy is hidden in the bulk of the matter, it is called latent heat.

• Latent heat of fusion: The heat energy required to convert 1 kilogram of a solid into liquid at atmospheric pressure, at its melting point, is known as the latent heat of fusion
• Latent heat of vaporisation: The heat energy required to convert 1 kilogram of liquid into gas, at atmospheric pressure, at its boiling point, is known as the latent heat of vaporisation
  Note: Water vapour at 373 K have more energy than water at the same temperature because
  particles in steam have absorbed extra energy in the form of latent heat of vaporisation.

Sublimation: The change of state of a substance directly from a solid to gas or gas to solid, without changing into the liquid state, is called sublimation. 

2. Effect of change of pressure

• Gas to liquid: Gases can be liquefied by applying pressure and reducing the temperature. When a high pressure is applied to a gas, it gets compressed and if the temperature is lowered, the gas is liquefied.
• Solid CO₂ gets converted directly to gaseous state on decrease of pressure to 1 atmosphere without coming into liquid state. This is the reason that solid carbon dioxide is also known as dry ice. 

Evaporation:
The process of conversion of a substance from the liquid state to the gaseous state at any temperature below its boiling point is called evaporation or vaporisation.

Factors affecting the rate of evaporation:

• Surface area: The rate of evaporation increases on increasing the surface area of the liquid.
• Temperature: The rate of evaporation increases with an increase in temperature.
• Humidity: Decrease in the humidity increases the rate of evaporation.
• Wind speed: An increase in the wind speed increases the rate of evaporation.

Evaporation causes cooling:
During the process of evaporation, the particles of liquid absorb energy or latent heat of vaporisation from the surrounding to get converted to gaseous state. This absorption of energy from the surroundings make the surroundings cold.

For example: sweating cools down our bodyibody

physical quantities and their SI units:

Try the following questions:

Q1. What is the common name of solid carbon dioxide?

Q2. Why does temperature remain constant during the boiling of water even though heat is being supplied continuously?

Q3. Why does the naphthalene balls kept in stored clothes in our home disappear over a period of time?

This is the complete explanation of CHAPTER 1 MATTER IN OUR SURROUNDINGS OF CLASS 9 SCIENCE NCERT.The exaplanation of CHAPTER 1 is according to the latest syallbus of CBSE.This will help student to better understand the CHAPTER and help in solving the question.

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