question_answer

In the following, the element with the highest ionisation energy is

A)  \[[Ne]\text{ }3{{s}^{2}}\text{ }3{{p}^{1}}\]         

B)  \[\text{ }\!\![\!\!\text{ }Ne\text{ }\!\!]\!\!\text{  }3{{s}^{2}}3{{p}^{2}}\]

C)  \[\text{ }\!\![\!\!\text{ }Ne\text{ }\!\!]\!\!\text{  }3{{s}^{2}}3{{p}^{2}}\]             

D)  \[\text{ }\!\![\!\!\text{ }Ne\text{ }\!\!]\!\!\text{  }3{{s}^{2}}3{{p}^{4}}\]

Correct Answer: B

Solution :

                  Elements having half-filled or fully filled orbitals are more stable. Hence, much energy is required to remove an electron from the outermost orbit. So, the element with \[\text{ }\!\![\!\!\text{ Ne }\!\!]\!\!\text{  3}{{\text{s}}^{\text{2}}}\text{ 3}{{\text{p}}^{\text{3}}}\]  configuration  has  highest ionisation energy.