Question

group 15memebers have more ionasiation enthalpy than group 14member due to​

Answer 1

Answer:

Because of the extra stable half-filled p orbitals electronic configuration and smaller size, the ionisation enthalpy of the group 15 elements is much greater than that of group 14 elements in the corresponding periods.

Answer 2

Question:

Why do group 15 members have more ionisationation enthalpy than group 16 members?

Answer:

This is due to the fact that group 15 elements have half filled extra stable p orbitals.  Hence it is diificult to remove an electron from the valence shell. The ionisation enthalpy of group 16 is lower because the removal of an electron results in the extra stable half filled configuration.

More information:

→ Due to increase in atomic size, ionisation enthalpy decreases down the group.

→ Ionisation enthalpy increases across a period due to decrease in atomic size.

→ The electronic configuration of group 15 elements is ns² np³

→ The group 15 elements are nitrogen, phosphorus, arsenic, antimony, bismuth and moscovium.

→ The electronic configuration of group 16 elements is ns² np⁴

→ The group 16 elements are oxygen, sulphur, selenium, tellurium, polonium and livermorium. They are also called as chalcogens.