CBSE Class 11 Chemistry States Of Matter Notes Set 04

5.States  of Matter

Some Important Points and Terms of the Chapter

1.  Intermolecular forces : are the forces of attraction and repulsion between interacting particles (atoms and molecules). This term does not include the electrostatic forces that exist between the two oppositely charged ions and the forces that hold atoms of a molecule together i.e., covalent bonds. Attractive intermolecular forces are known as van der Waals forces, in honour of Dutch scientist Johannes van der Waals (1837-1923).

2.  Dipole - Dipole Forces:Dipole-dipole forces act between the molecules possessing permanent dipole. Ends of the dipoles possess ―partial charges‖ and these charges are shown by Greek letter delta (δ

3.  Dipole -Induced Dipole Forces: This type of attractive forces operate between the polar molecules having permanent dipole and the molecules lacking permanent dipole. Permanent dipole of the polar molecule induces dipole on the electrically neutral molecule by deforming its electronic cloud.Thus an 

4.  Dispersion Forces or London Forces:Atoms and nonpolar molecules are electrically symmetrical and have no dipole moment because their electronic charge cloud is symmetrically distributed. But a dipole may develop momentarily even in such atoms and molecules. This can be understood as follows. Suppose we have two atoms ‗A‘ and ‗B‘ in the close vicinity of each other (Fig. 5.1a NCERT page 133). It may so happen that momentarily electronic charge distribution in one of the atoms, say ‗A‘, becomes unsymmetrical i.e., the charge cloud is more on one side than the other (Fig. 5.1 b and c NCERT page 133). This results in the development of instantaneous dipole on the atom ‗A‘ for a very short time. This instantaneous or transient dipole distorts the electron density of the other atom ‗B‘, which is close to it and as a consequence a dipole is induced in the atom ‗B‘. The temporary dipoles of atom ‗A‘ and ‗B‘ attract each other. Similarly temporary dipoles are induced in molecules also. This force of attraction was first proposed by the German physicist Fritz London, and for this reason force of attraction between two temporary dipoles is known as London force. Another name for this force is dispersion force.

5.  Hydrogen bond: Hydrogen bond is represented by a dotted line (– – –) while a solid line represents the covalent bond. Thus, hydrogen bond can be defined as the attractive force which binds hydrogen atom of one molecule with theelectronegative atom (F, O or N) of another molecule this is special case of dipole-dipole interaction.. 

6. Boyleís Law (Pressure – Volume Relationship): At constant temperature, the pressure of a fixed amount (i.e., number of moles n) of gas varies inversely with its volume. This is known as Boyleís law.

 

14. Density and Molar Mass of a Gaseous Substance:M= P dRT

15. Daltonís Law of Partial Pressures: It states that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases i.e., the pressures which these gases would exert if they were enclosed separately in the same volume and under the same conditions of temperature. In a mixture of gases, the pressure exerted by the individual gas is called partial pressure. Mathematically, pTotal = p1+p2+p3+......(at constant T, V) where pTotal is the total pressure exerted by the mixture of gases and p1, p2 , p3 etc. are partial pressures of gases.

16. KINETIC MOLECULAR THEORY OFGASES:

• Gases consist of large number of identical particles (atoms or molecules) that are so small and so far apart on the average that the actual volume of the molecules is negligible in comparison to the empty space between them. They are considered as point masses. This assumption explains the great compressibility of gases.explains the great compressibility of gases.

• There is no force of attraction between the particles of a gas at ordinary temperature and pressure. The support for this assumption comes from the fact that gases expand and occupy all the space available to them.

• Particles of a gas are always in constant and random motion. If the particles were at rest and occupied fixed positions, then a gas would have had a fixed shape which is not observed.

• Particles of a gas move in all possible directions in straight lines. During their random motion, they collide with each other and with the walls of the container. Pressure is exerted by the gas as a result of collision of the particles
with the walls of the container.

• Collisions of gas molecules are perfectly elastic. This means that total energy of molecules before and after the collision remains same.

17. Behaviour Of Real Gases: Deviation From Ideal Gas:Real gases show deviations from ideal gas law (a)Pressure correction: pressure exerted by the gas is lower than the pressure exerted by the ideal gas.

Constants a and b are called van der Waals constants
19. Significance of Vander wall parameter: Vander wall parameter a is the measure of intermolecular forces while b is the measure of effective size of gaseous molecules Unit of a = bar L3 mol-2 Unit of b = L mol-1

20. The deviation from ideal behaviour can be measured in terms of compressibility factor Z, which is the ratio of product pV and nRT. Mathematically Z= pV /nRT

21. The temperature at which a real gas obeys ideal gas law over an appreciable range of pressure is called Boyle temperature or Boyle point.

22. Critical temperature (TC)of a gas is highest temperature at which liquifaction of the gas first occurs. Liquifaction of so called permanent gase Volume of one mole of the gas at critical temperature is called critical volume (VC) and
pressure at this temperature is called critical pressure (pC). The critical temperature, pressure and volume are called critical constants

Please refer to attached file for CBSE Class 11 Chemistry States Of Matter Notes Set D