Why does the successive ionization enthalpy o | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) The first ionization enthalpy is the energy required to remove the first electron from a neutral atom. After the removal of the first electron,the

Vedclass · Accepted Answer

Due to the increased electrostatic attraction between the remaining electrons and the nucleus as the positive charge on the ion increases.

Vedclass · Answer

(C) The first ionization enthalpy is the energy required to remove the first electron from a neutral atom. After the removal of the first electron,the remaining electrons are more strongly attracted by the nucleus because the effective nuclear charge per electron increases. Consequently,removing the second and third electrons requires significantly more energy,leading to the order $1^{st} < 2^{nd} < 3^{rd}$.

Why does the successive ionization enthalpy of an element increase in the order: $1^{st} < 2^{nd} < 3^{rd}$?

Similar Questions

How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?

The ionization energy of boron is less than that of beryllium because

The correct order of first ionisation enthalpy of the given elements is:

Which is the correct order of the first ionization potential of $N$,$O$,and $C$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module