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JEE Main Physical Chemistry section carries a weightage of 3040 % hence is considered important in the trio Physical, Organic and Inorganic chemistry. Numerical problems on topics like Chemical Kinetics, Equilibrium, Thermodynamics are asked frequently, but states of matter is one such topic in which direct theory questions are asked making it quite an easy chapter to cover from that point of view.

States of matter carries a weightage of 23.2% in Chemistry section, thus 12 questions are necessarily put forward.

Some sub topics repeatedly find place in the questions like Void, Radiusratio, Density and Bravais Lattice.

On a general note, any substance that has mass and occupies space is called matter. The matter is composed of atoms and molecules.

The arrangement of these building blocks gives various states, physical and chemical properties to the matter.
Detailed study notes of States of Matter, based on the latest JEE Main Chemistry Syllabus have been given for reference to the students in the article.
General Properties of Matter
General Properties of Matter
Property  Solid  Liquid  Gas 

Shape  Definite shape  Indefinite shape  Indefinite shape 
Volume  Definite Volume  Definite Volume  Indefinite Volume 
Inter particular Forces  Strong Inter particular Forces  Comparatively weaker Inter particular Forces  Inte rparticular forces are negligible 
Inter particular Space  Negligible inter particular space  Comparatively large inter particular space  Very large Inter particular space 
Particular Motion  Particle motion is restricted to vibratory motion.  Particle motion is very slow  Particle motion is very rapid and also random. 
Packing of Particles  Particles are very Closely packed  Particles are loosely packed  Particles are very loosely packed 
Compressibility  Incompressible  Compressible  Highly Compressible 
Density  Very High Density  Low Density  Very low density 
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Solid
In solid, constituent particles (ions, atoms, or molecules) are closely packed together. The forces between particles are so strong that the particles cannot move freely but can only vibrate. As a result, a solid has a stable, definite shape, and a definite volume. Solids can only change their shape by an outside force, as when broken or cut.
Liquid
A liquid is a nearly incompressible fluid that conforms to the shape of its container but retains a (nearly) constant volume independent of pressure. The volume is definite if the temperature and pressure are constant.

When a solid is heated above its melting point, it becomes liquid, given that the pressure is higher than the triple point of the substance. Intermolecular (or interatomic or interatomic) forces are still important, but the molecules have enough energy to move relative to each other and the structure is mobile.

This means that the shape of a liquid is not definite but is determined by its container. The volume is usually greater than that of the corresponding solid, the bestknown exception being water, H2O. The highest temperature at which a given liquid can exist is its critical temperature.
Gas
Gas is a compressible fluid. In a gas, the molecules have enough kinetic energy so that the effect of intermolecular forces is small (or zero for an ideal gas), and the typical distance between neighbouring molecules is much greater than the molecular size. A gas has no definite shape or volume but occupies the entire container in which it is confined. A liquid may be converted to a gas by heating at constant pressure to the boiling point, or else by reducing the pressure at a constant temperature.
These notes contain all the important GAS LAWS and some important terms and relations.
The gas laws are a set of laws that describe the relationship between THERMODYNAMIC TEMPERATURE ( T ), PRESSURE (P) AND VOLUME (V) of gases.

Boyle's law,

Charles's law,

Gay Lussac's law,

Avogadro law,

Ideal gas equation,

Dalton's law of partial pressure,

Graham’s law of diffusion

Kinetic Theory of Gases

Vander Waal's equation
Boyle’s Law
Practice with JEE Main Question Paper
Boyle’s Law
The volume of a given mass of a gas is inversely proportional to its pressure at a constant temperature.
; V ∝ 1 / p or PV = K
K is a constant and its value depends on the mass, temperature and nature of the gas.
∴ p1V1 = p2V2 ......=K
ALSO, density d ∝ 1/V
Hence, P ∝ D
Example
We all have seen a syringe while visiting a doctor. It is a medical device used to inject or withdraw fluid. It consists of a hollow cylinder called a barrel and a sliding plunger attached to it. The working principle of a syringe is like a reciprocating pump. When the plunger is pushed, the fluid will inject, and when the plunger is pulled, the fluid will withdraw the pushing of the plunger reduces the volume of the fluid in the barrel. This reduction in the volume causes a momentary increase in the pressure of the fluid, and the fluid is injected into the patient's body. In a similar way, the pulling of the plunger increases the volume of the fluid. It results in a momentary decrease in the pressure of the fluid, and external fluid is withdrawn.
Charles’ Law
Charles’ Law
The volume of the given mass of a gas increases or decrease by 1 / 273 of its volume for each degree rise or fall of temperature respectively at constant pressure.
Vt = Vo (1 + t / 273) t constant p
or
The volume of a given mass of a gas is directly proportional to the absolute temperature at constant pressure.
V ∝ T (at constant p), V / T = constant or V1 / T1 = V2 / T2
Absolute zero is the theoretically possible temperature at which the volume of the gas becomes zero. It is equal to O°C or 273.15K.
Isobars A graph of V vs T at constant pressure is known as isobar
Charles’law explains that gases expand on heating, so hot air is less dense than cold air.
Example
The human lungs are spongy airfilled organs play an important role in respiration. Air flows in when the lungs expand and flow out when they contract. In winters, the temperature of air decreases. As a consequent, the temperature of the air inside the body also decreases. According to Charles's law states volume is directly proportional to temperature. Hence, the volume of the air decreases with temperature. It shrinks the lungs and physical activities like jogging become difficult in freezing winter days.
Gay Lussac’s Law
Gay Lussac’s Law
The pressure of a given mass of gas increases or decreases by 1 /273 of its pressure for each degree rise or fall of temperature respectively at constant volume.
pt = po (1 + t / 273) at constant V and n
or
The pressure of a given mass of a gas at constant volume is directly proportional to absolute temperature.
p ∝ T or p = KT or p / T = K at constant V and n or P1 / T1 = P2 / T2
Isochores A graph of p vs T at constant volume is known as isochore
Avogadro’s Law
Example
In hot summer days, the inflated tyres of vehicles may burst. The bursting of tyres is caused by GayLussac's law. The inflated tyres are under high pressure. When the temperature of the air rises, the pressure of the gas in the tubes increases. After an unbearable point, the tyres fracture.
Avogadro’s Law
It states that equal volumes of all gases under the same conditions of temperature and pressure contain an equal number of molecules.
Mathematically
V infi; n (at constant T and p) or V / n = K
Molar gas volume The volume of one mole of a gas, i.e., 224 Lat STP(0°C, 1 atm) i_!S known as molar gas volume
Ideal Gas Equation
Ideal Gas Equation
V ∝1 / p, T and n constant (Boyle’s law)
V ∝ T, p and n constant (Charles’ law)
V ∝ n, p and T constant (Avogadro’s law)
⇒ V ∝ nT / p or pV ∝ nT or pV = nRT.
This is known as an ideal gas equation. R is known as the universal gas constant.
From the ideal gas equation, density.
d = pM / RT (where, M = molecular mass)
Example
Balloon filled with helium weighs much less than an identical balloon filled with air. Both balloons contain the same number of molecules. Helium atoms have a lower mass than either oxygen mPal Gas Equation
Graham’s Law of Diffusion
Similar conditions of temperature and pressure, the rates of diffusion of gases are inversely proportional to the square root of their densities.
Mathematically, r1 / r2 = √d2 / √d1 = √M2 / √M1
[Diffusion is the tendency of gases to distribute itself uniformly throughout the available space while effusion is the movement of gas through a small hole when it is subjected to pressure].
Example
The gases with different densities can be separated using Graham's law. It is also helpful in determining the molar mass of unknown gases by comparing the rate of diffusion of unknown gas to known gas. We can separate the isotopes of an element using Graham's law. A common example is enriching uranium from its isotope
Dalton’s Law of Partial Pressure
Dalton’s Law of Partial Pressure
At constant temperature. the total pressure. exerted by a mixture of nonreacting gases. is the sum of partial pressures of different gases present in the mixture.
p = p1 + p2 + p3 + ….
The Partial pressure of a gas = mole fraction of the gas * total pressure.
If n1, n2 and n3 are moles of nonreacting gases filled in a vessel of volume V at temperature T, the total pressure, p is given by
pV = (n1 + n2 + n3)RT
This is the equation of state of a gaseous mixture,
[Aqueous tension It is the pressure exerted by water vapours at a particular temperature. It depends upon temperature.]
The Pressure of a dry gas can be determined by Dalton’s law. When a gas is collected over water, its observed pressure is equal to the sum of the pressure of dry gas and the pressure of water vapour (aqueous tension) then
The Pressure of dry gas = pressure of moist gas – aqueous tension.
Example
It refers to the effects of which partial pressure might have on scuba divers. While the total gas pressure increases as a diver increase their descent, the partial pressure of each gas involved increases as well which might cause harm to the diver's body if proper actions are not carried out.
Kinetic Theory of Gases
Based on the basic postulates regarding the structure of gases, it is possible to derive a theoretical expression for the pressure of an ideal gas. The expression is
pV = 1/3mNun2
m is the mass of each molecule of a gaseous system occupying volume V and exerting pressure p, N is the number of molecules contained in it and un2 is the mean square speed, defined as
u2= (u12+u22+u32+......+un2)/N
From the above equation, it is possible to derive the various experimentally observed gaseous laws
Van der Waals’ Equation
Van der Waals’ Equation
Van der Waals’ obtained the following equation for n. moles of a gas.
(p + n2a/Vm2) (Vmnb) = RT
can also be written as
(p + n2a/V2) (Vnb) = nRT
where,
b = excluded volume or covolume = 4 * actual volume of gas molecules
a = magnitude of attractive forces between gas molecules.
The greater the value of ‘a’, the greater the strength of van der Waals’ forces and greater is the ease with which a gas can be liquefied.
Vapour pressure
The pressure exerted by the vapours above the liquid surface when these are in equilibrium with the liquid at a given temperature is known as the vapour pressure of the liquid.
The vapour pressure of a liquid depends on:

Nature of liquid

Temperature: Vapour pressure increases with increasing temperature.
Example
The amount of water vapour will increase and the pressure will increase if a bottle of water is heated up
Boiling point
The temperature, at which vapour pressure of liquids becomes equal to the atmospheric pressure, is called the boiling point.
Example
Milk is a mix of butterfat and water so it is slightly heavier than water. The boiling points of liquids are due to the gravity of the liquid. Water boils at 100 degrees Celsius (212 degrees Fahrenheit). While milk boils at 212.3 degrees Fahrenheit.
Surface Tension
It is the force acting per unit length perpendicular to the imaginary line drawn on the surface of the liquid. It is denoted γ (gamma);
SI unit: Nm1
Dimensions: kgs2
The magnitude of surface tension of a liquid depends on the attractive forces between the molecules. It is measured with the help of an apparatus, called stalagmometer.
Surface tension decreases as the temperature increases. Rise or fall of liquid in a capillary tube is due to surface tension.
Example
Water insects are able to walk water because of the wax secreted on their legs combined with surface tension's elasticlike cover.
Viscosity
Viscosity is a measure of resistance to flow which arises due to friction between layers of fluid.
When there is a regular gradation of velocity, in passing from one layer to the next, it is called laminar flow.
F = η Adv / dz
where F = forces required to maintain the flow of layers.
A = area of contact
dv/ dz = velocity gradient; (the change in velocity with distance.)
‘η’ is proportionality constant and is called the coefficient of viscosity. The Viscosity of the coefficient is the force when the velocity gradient is unity and the area of contact is unit area. CGS unit of coefficient of viscosity is poise S.I. unit of coefficient of viscosity is Nsm2.
Example
Water has a low or "thin" viscosity, for example, while honey has a "thick" or high viscosity.