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Choose the correct option:

List I

List II
 

IE1

IE2

IE3

    

       I       

    2080   

    3963   

   6130   

     (a)      

H

II

520

7297

11810

(b)

Li

III

900

1758

14810

(c)

      Be      

IV

800

2428

3600

(d)

B
       

(e)

Ne
Option: 1

I       II     III     IV

a      b      c      d


Option: 2

I       II     III     IV

c      b      e       d


Option: 3

I       II     III     IV

b      c      d       e


Option: 4

I       II     III     IV

e      b      c      d


Answers (1)

best_answer

Comparison between different I.E. -

  • Comparison of IE1 and IE2 of oxygen and nitrogen

Oxygen has electronic configuration as 1s22s22p4. After IE1, its electronic configuration becomes 1s22s22p3. Now nitrogen has electronic configuration as 1s22s22p3. After IE1, its electronic configuration becomes 1s22s22p2.

Thus in case of oxygen, after IE1, O+ has achieved the stable half filled electronic configuration and hence more energy is required in IE2 to remove an electron further. Similarly, nitrogen already has a stable half filled electronic configuration, thus more energy is required for IE1 to remove the first electron.

Therefore, the order of different ionisation enthalpies is followed as mentioned below: 

(i) N(IE1) > O(IE1)            (ii) O(IE2) > N(IE2)

-

The first ionisation energy of noble gases is always very high, thus Neon has the highest first ionisation energy. Now, after removing the first electron, Li becomes Li+ with completely filled 1s orbital. Thus removing the second electron now requires a lot of energy, thus second ionisation energy of Li is much higher than the first ionisation energy. Similarly with beryllium, after removal of two electrons, it achieves the completely filled 1s orbital and then removing the third electron from the 1s orbital is very hard. Thus, third ionisation energy is much higher than the second ionisation energy.

Therefore, Option(4) is correct

Posted by

vinayak

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