TEST 1 -  CHEMICAL BONDING

    This test is on the chapter chemical bonding. Chemical bonding 
     is a vast chapter and i hope to upload another test soon.

    I hope that this test will be useful to all my readers.
   
    Answers to this test will be published by 10 p.m on Thursday.

                                    ALL THE BEST

    

                                IONIC EQUILIBRIUM

       Ionic equilibrium is the last physical chemistry chapter in class 
       11. Questions from this chapter are generally straightforward.
       However, there are several different types of questions that
       can be asked. These models will be covered in detail.

   
      

                 

               IMPORTANT EXAMPLES : 

             

 

               

    These were the important points in ionic equilibrium. With this,

     physical chemistry of class 11 comes to an end.

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               PERIODIC PROPERTIES TEST - ANSWERS

  

                            TEST - PERIODIC PROPERTIES

       This test is on the chapter periodic properties. I hope that this
        test will be useful to all my readers.

       Answers to this test will be published by 10 p.m. today .

                                   ALL THE BEST

       
       

THANK YOU

  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

CHEMICAL EQUILIBRIUM 

      Equilibrium is the next topic in physical chemistry and consists

      of both chemical and ionic equilibrium. Questions in this 

      chapter are generally easy in iit jee but most students find

      ionic equilibrium challenging. I hope to cover all models of 

      problems on both these chapters.

      Chemical Equilibrium:

      

       Le Chatelier 's principle :

       1. Increase in concentration of reactants moves the reaction

           forward. ( not for solids)
     

      2. Increase in pressure moves in direction of lesser no of moles

           of gas.

  

      3. Addition of inert gas at constant volume - No change.

      4. Addition of inert gas at constant pressure moves the reaction

          in direction of greater number of  moles.

      5. In the ice water equilibrium, melting point decreases with

          increase in pressure.

    

      6. With increase in temperature , equilibrium constant of an

          endothermic reaction increases. The opposite is true for

          an exothermic reaction.

      NOTE:  Solubility of NaOH increases with temperature

                    although dissolution is an exothermic process.

                                  

                                    THANK YOU

    ATOMIC STRUCTURE TEST -  ANSWERS

        

                    SOLUTIONS TO SELECTED PROBLEMS

  

            

   

                                    

       In question 18 , the 3s, 3p, 3d orbitals are similar in energy.

       Hence degeneracy is 9.

                                     

                                   THANK YOU