PERIODIC PROPERTIES

    Periodic Properties is an important chapter in jee mains but is not

    part of jee advanced syllabus. However , it plays an important

    role in understanding inorganic chemistry .In this post , i will 

    be covering the important points in periodic properties. 

    

    NOTES:

    Ionisation Energy :

   1. It is the minimum amount of energy required to remove an 

       electron from the valence shell of an isolated gaseous atom.

   2. The removal of the 2nd electron is naturally more difficult than

       the first. Therefore for any element , IE 3 > IE 2 > IE 1 .

   3. Factors which effect ionisation energy :

       a)  Effective nuclear charge -  

            

            The magnitude of effective nuclear charge increases along

             the period.

            The magnitude of effective nuclear charge decreases 

            slightly down the group.

       b)  Size of the atom :

            Size increases down the group. As a result , the ionisation

            energy decreases. 

       c) Orbital involved :

            Ease of removal :  s < p < d< f

            eg.  Let us compare the IE of K and Cu. The first ionisation

                   energy of copper is more ( this is due to smaller size )

                  However , the second ionisation energy of copper is

                  smaller than potassium because the electron is removed

                  from the d orbital

       d) Nature of Configuration :

           Fully filled and Half filled orbitals have greater IE.

       

       NOTE : IE for transition metals increases along the period and

                     then becomes constant.

   

       ELECTRON AFFINITY:

       1. It is the amount of energy released when an electron is added

           to the outermost shell of a neutral gaseous atom.

       2. For second electron affinity and beyond we need to supply

           energy.

       3. Factors which influence electron affinity:
  
           a) Effective nuclear charge -  Generally , greater the 
                effective nuclear charge , greater the electron affinity.

           b) Size of the atom.

          c) Electronic configuration: Half filled and fully filled 
               orbitals have low electron affinity.


       ELECTRONEGATIVITY :

       

  
         Some important trends and exceptions :

         

  
  

         

     

        Apart from these notes , i advise all of you to go through the
        ncert textbook. Fiitjee students can use the package which
        i found very useful for this chapter.

                                       THANK YOU