NEET Study Notes for State of Matter:Everything that surrounds us is made up of matter. Anything that occupies space and has mass is called matter. The different characteristics of matter enable us to classify them into- solids, liquids and gases, liquids. The other state in which matter can be found is called Plasma, Bose-Einstein Condensate and neutron degenerate matter.
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Attractive and repulsive forces that exist between the particles of a substance are called Intermolecular forces. Physical and chemical properties id substances are determined by the intermolecular forces between them. , For eg- if the intermolecular force between molecules is higher, the boiling point will also be high.
Intermolecular forces are also known as electrostatic forces. The intermolecular interactions are:
Example- On combining NaCl with water, Ion dipole interaction occurs between polar water molecules and sodium chloride ions.
The attractive forces between polar molecules is called the Dipole-Dipole interaction. The difference in electronegativity due to the covalent bond gives rise to Polar molecules with permanent dipoles. The positive part of a molecule is attracted to the negative part of the other molecule.
Example- In HCL molecules, dipole-dipole interactions occur, The electronegative element of Chlorine is more than Hydrogen. Hydrogen attracts a positive charge whereas Chlorine attracts a negative charge.
An ion is placed near a non-polar molecule for polarization. Due to this the non-polar molecules become charged and acts as induced dipoles. This bond between ions and induced dipoles is called the Ion induced dipolar interaction.
When polar molecules are placed near non-polar molecules, the transformation of non-polar molecules into induced dipoles. This interaction is known as dipole-induced dipole interaction. On damage of the electron cloud, the molecule acts as a dipole polar molecule permanent dipole transforms the neutral molecule's dipole.
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Laws that describe the relationship among thermodynamic temperature (T), pressure and volume of a gas are known as Gas Laws.
In a given mass of gas, the volume is inversely proportional to the pressure at constant temperature
V ∝ 1 / p or PV = K
where K is constant and its value depends on mass, temperature, and nature of gas
On mass and temperature being equal
As Density is inversely proportional to 1/V
Hence P ∝ D
At constant pressure, volume of given mass of gas is directly proportional to the temperature
V ∝ T
where V is the volume of gas
T is the temperature
At constant volume, the pressure of the specified mass of gas is directly proportional to the temperature.
V ∝ T or
At constant temperature and pressure, the volume of gas is directly proportional to to the number of molecules. Thus if the volume of gas is the equal number of moles or molecules will also be equal to the ideal gas only when the volume is equal.
Mathematically, Avogadro’s Law can be expressed as
V/n is constant
or
where v is the volume of gas
n is the number of molecules
This law is also known as general gas equation. When Charle’s law, Boyle’s Law and Gay-Lussacs’s law is combined, combined gas law is obtained. The relationship between volume, pressure and temperature for a specific volume of gas is determined.
Mathematically, combined gas law is expressed as
PV/T = k
Ideal gas is also known as perfect gas as the relationship among pressure, volume, temperature and gas quantity is established.
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Ideal Gas Law is established by a combination of the four laws- Gay Lussac Law, Avogadro’s Law, Charles, and Combined Law. In this law, combined gas law is transformed into ideal gas law and the addition of Avogadro’s law takes place.
Ideal Gas Law can be represented as
PV = nRT
Where for the gas,
P is the pressure
R is the universal gas constant
V is the volume
n is the number of molecules
T is temperature
Mathematically Kinetic Gas Equation can be represented as
PV = 1/3mNU2
where m is the mass of molecule gas
N is the number of molecules
U = Root mean square velocity
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For one mole of gas, Van Der Waal’s Equation is
where b is the co-volume
a is the attractive force magnitude between molecules of gas
The increase and decrease of temperature causes the liquefication of gases,
Critical Temperature is the temperature above which gas cannot be liquified, even if the pressure is high. For example- The critical temperature of CO2 is 31.1°C.
Gas can be liquified by two main factors
The state of Liquid is composed of molecules that are small and due to the weak intermolecular force, molecules of the liquid are in constant motions that are random. The kinetic energy of liquid molecules is directly proportional to the temperature.
Induced dipole<dipolle attraction<Hydrogen bonding
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The pressure exerted by the vapor phase or condensed phase in a state of equilibrium at a specific temperature is called vapor pressure or vapor equilibrium pressure. Vapor pressure depends upon the following factors:
Surface tension is defined as the force that acts on the liquid surface and has a tendency to shrink the surface area. S.I unit of Surface tension is Nm–1. Drop Number method can be used for measuring surface tension.
Surface tension depends upon
The friction force that acts between layers of liquid that are in movement across each other with different velocities is called viscosity. In order to compare the viscosity of liquids, coefficient of viscosity is used. S.I unit of Viscosity is Nsm2
Read NEET Study Notes on Chemical Kinetics
The temperature at which the vapor pressure is equal to the atmospheric pressure of the liquid is called the Boiling Point.
Question: According to which law, at constant pressure, the volume of an ideal gas is directly proportional to its temperature?
Answer: Charle’s Law
Question: In which property of gases, is a constant R or universal gas constant observed?
Answer: Ideal gases
Question: Which condition is necessary for Charle’s Law?
Answer: constant pressure
Question: What is the necessary condition for carbon monoxide to operate on the ideal gas law?
Answer: high temperature, low-pressure
Question: How much will gas molecule’s average velocity increase when the temperature is doubled?
Answer: 1.4
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