The second ionization enthalpy of an element | vedclass

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

Question

(A) The first ionization enthalpy $(IE_1)$ is the energy required to remove the first electron from a neutral atom. After the removal of the first ele

Vedclass · Accepted Answer

The cation is always smaller than the neutral atom

Vedclass · Answer

(A) The first ionization enthalpy $(IE_1)$ 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 increases while the number of electrons decreases. Additionally,the cation formed is smaller than the neutral atom,which increases the electrostatic force of attraction between the nucleus and the remaining electrons. Therefore,more energy is required to remove the second electron,making the second ionization enthalpy $(IE_2)$ always greater than the first $(IE_1)$.

The second ionization enthalpy of an element is always higher than its first ionization enthalpy because

Similar Questions

The element having the greatest difference between its first and second ionization energies is:

Amongst the following elements,the highest ionization energy is

Triad-$I$ $[N^{3-}, O^{2-}, Na^{+}]$
Triad-$II$ $[N^{+}, C^{+}, O^{+}]$
Choose the species of lowest $IP$ from triad-$I$ and highest $IP$ from triad-$II$ respectively.

If first ionization enthalpies of element $X$ and $Y$ are $419 \ kJ \ mol^{-1}$ and $590 \ kJ \ mol^{-1}$,respectively and second ionization enthalpies of $X$ and $Y$ are $3069 \ kJ \ mol^{-1}$ and $1145 \ kJ \ mol^{-1}$,respectively. Then the correct statement is :-

Which of the following statements is correct regarding the first $(I)$ and second $(II)$ ionization enthalpies of sodium $(Na)$ and magnesium $(Mg)$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module