CHARACTERISTICS OF

PARTICLES

• Particles exhibit some characteristics.

They can influence the state and

properties (physical and chemical) of a

substance.

• The three characteristics shown by

particles of matter are as follows.

CHARACTERISTICS OF

PARTICLES

• Particles are tiny.

• Particles have spaces between them

• Particles attract each other

• Particles constantly in motion (or) Particles

are continuously moving

Arrangement of particles

• Arrangement of particles

Plasma

Physical properties

STATES OF MATTER

•The FIVE States of Matter• FIVE States

• Solid

• Liquid

• Gas

• Plasma

• Bose Einstein condensate

STATES OF MATTER

➢Based upon particle arrangement

➢Based upon energy of particles

➢Based upon distance between particles

Kinetic Theory of Matter

Matter is made up of particles

which are in continual random

motion.

Kinetic Theory- the tiny particles

in all forms of matter are in

constant motion

STATES OF MATTER

SOLIDS

•Particles of solids are

tightly packed, vibrating

about a fixed position.

•Solids have a definite

shape and a definite

volume. Heat

STATES OF MATTER

LIQUID

▪ Particles of liquids are

tightly packed, but are

far enough apart to

slide over one

another.

▪ Liquids have an

indefinite shape and a

definite volume. Heat

STATES OF MATTER

GAS

▪ Particles of gases

are very far apart

and move freely.

▪ Gases have an

indefinite shape

and an indefinite

volume. Heat

But what happens if you raise the

temperature to super-high levels…

between

1000°C and 1,000,000,000°C ?

Will everything

just be a gas?

STATES OF MATTER

PLASMA

▪ A plasma is an ionized gas.

▪ A plasma is a very good conductor of electricity and is affected by magnetic fields.

▪ Plasmas, like gases have an indefinite shape and an indefinite volume.

• Plasma is the

common state

of matter

STATES OF MATTER

SOLID LIQUID GAS PLASMA

Tightly packed, in

a regular pattern

Vibrate, but do not

move from place

to place

Close together

with no regular

arrangement.

Vibrate, move

about, and slide

past each other

Well separated

with no regular

arrangement.

Vibrate and move

freely at high

speeds

Has no definite

volume or shape

and is composed

of electrical

charged particles

Some places where plasmas are found…

1. Flames

2. Lightning

3. Aurora (Northern Lights)

The Sun is an example of a star in its

plasma state

COLD PLASMA

COLD PLASMA PEN

BEC

BOSE EINSTEIN CONDENSATE

Bose Einstein condensate

• Fifth form of matter Bose Einstein condensate(BEC).

• In 1920, Indian physicist satyender Nath Bose has done some

calculations for a fifth state of matter.

• Building on his calculations , Einstein predicted a new state of

matter that is Bose Einstein Condensate (BEC).

• In 2001,Eric A. Cornell,Wolfgang Ketterle and Carl E. Wieman of

USA received Nobel prize in physics for achieving “Bose Einstein

Condensation”.

• The Bose Einstein Condensate (BEC) is formed when a low density

gas about 100,000 the density of normal air, under high pressure is

exposed to super low temperatures.

Unit of temperature • The Common Unit of Temperature and SI Unit of Temperature:

• The common unit of measuring temperatures (like melting points, boiling points etc.) is ‘degrees Celsius’ which is written in short form as °C.

• Laboratory thermometers and clinical thermometer are calibrated on Celsius scale of temperature.

• There is another scale of temperature called Kelvin scale of temperature which is used by the scientists mainly for research work. The SI unit of measuring temperature is Kelvin, which is denoted by the symbol K.

• The relation between Kelvin scale and Celsius scale of temperature can be written as:

• Temp. on Kelvin scale=Temp. on Celsius scale + 273

• To convert a temperature on Celsius scale to Kelvin scale, we have to add 273 to the Celsius temperature.

• And to convert a temperature on Kelvin scale to the Celsius scale, we have to subtract 273 from the Kelvin temperature.

Change of State of Matter:

• We can change the physical state of matter in

two ways:

• By changing the temperature (heating or

cooling).

• By changing the pressure (increasing or

decreasing the pressure).

• These two factors decide whether a given

substance would be in a solid, liquid or gaseous

state.

Effect of Change of Temperature:

Solid to Liquid Change: Melting

• The process in which a solid substance changes into a liquid on heating, is called on melting or fusion.

• The temperature at which a solid substance melts and changes into a liquid at atmospheric pressure, is called melting point of substance. For example, the ice melts at a temperature of 0°C to form liquid water, so the melting point of ice is 0°C (zero degree Celsius). At melting point, ice changes its state from solid to liquid.

• Different solids have different melting points. Higher the melting point of a solid substance, greater will be the force of attraction between its particles.

• The melting point of a solid is an indication of the strength of the force of attraction between its particles.

• When a solid substance is heated, the heat energy makes its particles vibrate more vigorously. At the melting point, the particles of a solid have sufficient kinetic energy to overcome the strong forces of attraction holding them in fixed positions and break to form small groups of particles and the solid melts to form a liquid.

Liquid to Gas Change: Boiling (or Vaporization):

• The process in which a liquid substance changes into a gas rapidly on heating, is called boiling.

• The temperature, at which a liquid boils and changes rapidly into a gas at atmospheric pressure, is called boiling point of the liquid.

• For example, when water is heated to a temperature of 100 °C (hundred degree Celsius).

• Different liquids have different boiling points.

• The boiling point of a liquid is a measure of the force of attraction between its particles.

• When a liquid is heated, the heat energy makes its particles move even faster. At the boiling point the particles of liquid have sufficient kinetic energy to overcome the forces of attraction holding them together and separate into individual particles. And the liquid boils to form a gas.

Gas to Liquid Change:

Condensation

• The process of changing a gas (or vapour) to a liquid by cooling is called condensation.

• When steam (or water vapour) changes into water on cooling, it is called condensation of steam.

• When a gas is cooled enough, then its particles lose so much kinetic energy that they slow down, move closer together until they start being attracted to each other, and form a liquid.

Liquid to solid change: Freezing

• The process of changing a liquid into a

solid by cooling is called freezing.

• For example, when water is cooled, it gets

converted into a solid called ‘ice’. This is

called freezing of water. Freezing means

solidification.

Change of State of Matter:

Latent Heat

• Latent heat:

• The heat energy which has to be supplied to change the state of a substance is called its latent heat.

• Latent heat does not raise (or increase) the temperature. But latent heat has always to be supplied to change the state of a substance .The word ‘latent’ means ‘hidden’.

• The latent heat which we supply is used up in overcoming the forces of attraction between the particles of substance during the change of state. Latent heat does not increase the kinetic energy of the particles of the substance, so the temperature of a substance does not rise during the change of state.

• Latent heat is of two types:

• Latent heat of fusion

• Latent heat of vaporization.

Latent Heat of Fusion (solid to

liquid change):

• The heat which is going into ice but not increasing its temperature, is the energy required to change the state of ice from solid to liquid (water). This is known as the latent heat of fusion of ice (or latent heat of melting of ice).

• The latent heat of fusion (or melting) of a solid is the quantity of heat in joules required to convert 1 kilogram of the solid (at its melting point) to liquid, without any change in temperature.

• The latent heat of fusion of ice is 3.34×105 joules per kilogram (or 3.34 ×105 j/kg).

Latent Heat of Vaporization

(liquid to gas change):

• The latent heat of vaporization of a liquid is the

quantity of heat in joules required to convert 1

kilogram of the liquid (at its boiling point) to vapour or

gas, without any change in temperature.

The latent heat of vaporization of water is

22.5×105 joules per kilogram (or 22.5×105 j/kg).

Note: It has been found that the burns caused by

steam are much more severe than those caused by

boiling water though both of them are at the same

temperature of 100 °C. This is due to the fact that

steam contains more heat, in the form of latent heat,

than boiling water.

Sublimation• The transition of a substance on heating/with out heating

directly from its solid phase to gaseous phase, without

changing into the liquid phase (or vice versa) is

called sublimation.

Effect of change in pressure on

state of matter

.• 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.

Change of state by applying pressure

Evaporation• The phenomenon by which molecules in liquid state undergo a spontaneous

transition to the gaseous phase at any temperature below its boiling point is called evaporation.

• For example, the gradual drying of damp clothes is caused by the evaporation of water to water vapour.

• Factors affecting evaporation

• 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 rate of evaporation decreases with an increase in humidity.

• Wind speed: The rate of evaporation increases with an increase in wind speed.

• Cooling due to evaporation

• During evaporation, the particles of a liquid absorb energy from the surroundings to overcome the interparticle forces of attraction and undergo the phase change. The absorption of heat from the surrounding makes the surrounding cool.For example, sweating cools down our body.

• Physical Nature of Matter