LMS

Volume is inversely proportional to pressure

Graph between pressure and constant K is straight line parallel to pressure axis 

gases are soluble in water at high temperature which increase the forces of attraction in gases so solubility increases. 

Volume of gas is directly proportional to temperature,127°C =400K which is highest with lowest pressure 

The original volume of a gas at 0°C is 273cm3 at constant pressure. Its volume at 273°C becomes 546 cm3 because volume of given mass of gas double on doubling the temperature at kelvin scale Calculation:The original volume (V1) of gas at 0°C or 273K = 273 cm3The new volume (V2) of gas at 273°C or 546K =?According to Charles’s law

If temperature is taken in Celsius scale we can use this equation.

Derivation of the Van der waal’s equation is not conclusion of the kinetic theory of gases.Van der Waal’s equation for non-ideal gases cannot be derived from kinetic molecular theory but gas laws and temperature interpretation can be derived from KMT.

Molecules of gas do not have forces of attraction 

‘a’ constant of NH3 is greater than that of N2  because NH3 is polar while N2 is non-polar and ‘b’ constant of NH3 is less than that of N2 because N2  molecule  is larger in size as compared to NH3 is correct according to the Van der Waal’s equation.‘a’ = attractive forces constant‘b’ = effective volume constantNH3 has greater intermolecular forces than N2 and N2 has little greater volume at closest approach in the gaseous state

Pressure taken on X-axis and Z= PV / nRT at Y-axis

London dispersion forces are strongest in I2.London dispersion forces polarizabilityI2 is more polarizable due to large size of molecule so it is solid at room temperature.Intermolecular forces or polarizability orderI2 > Br2 > Cl2 > F2

London dispersion forces are present in I2, H2 and He.because theses are non polar in nature (London dispersion forces are present in all kinds of molecules).

Types of molecules polar and non-polar molecules solid and all type of forces present between molecules solid. 

It is present between non-polar.

boiling point polarizibility molecular size

Acetone has weaker forces of attraction among all of given compounds

Greater the size of molecule, greater the polarizability, greater the forces of attractions hence greater the heat of vapourization

CH3-NH2 have hydrogen bonding

Greater the size of molecule, greater the polarizability, greater the forces of attractions

Vapor pressure of a liquid depends upon intermolecular forces but does not depends upon amount of substance, surface area and size of liquid container.

HCl have weakest forces which makes HCl most volatile and have lowest heat of vaporization 

Vapour pressure increases by increasing temperature 

Stronger intermolecular force lowest will be vapour pressure there is strong intermolecular force than   CH3OH, C2H5OH , HF

have two hydrogen bond and have one hydrogen bond 

Greater the external pressure greater the boiling point 

SO2 is polar and SO3 is non-polar it dipole moment is zero due to perfectly triangular.

Greater the forces of attraction lower the vapour pressure 

Acetone and chloroform are soluble in each other due to inter molecular hydrogen bonding.Intermolecular hydrogen bonding is present between H of chloroform and O of acetone 

Density of water decreases from 4°C to 0°C due to increase sin distance between their molecule 

Those compound which form strong hydrogen bond with water. NH3 form H-Bond with water.

HCl have dipole dipole force of attraction

Hydrogen bonding present in water 

Greater electronegativity difference grater the forces of attraction 

CH4 is non-polar molecule 

Below 4ºC empty spaces are created.Above and below 4°C molecules of H2O are at larger distances as compared to distance at 4°C

Liquid molecule have fix volume 

Glue is amorphous solid Pseudo solid is also called amorphous solid

Ionic solids show isomorphism and polymorphism.  Allotropy shown by element.

Graphite has layer structure 

Melting point and boiling point is not anisotropic behaviour 

Two types of intermolecular forces are responsible for holding the particles together.(i) Dipole – dipole interactions or hydrogen bonding.(ii) Van der Waal’s forces or London forces.

Molecular solids have very weak intermolecular forces due to which molecular solids are soft 

Each Na+ surrounded by 6 Cl.

α-angle lies between side b & cb-angle lies between side a & cg-angle lies between side b & a

Unit cell is the smallest part, has all features of the entire crystal