A to A^{+} + e, E_{1} and A^{+} to A^{2+} + e | vedclass

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

Question

(A) $E_{1}$ represents the first ionization energy $(I.E._{1})$,which is the energy required to remove the first electron from a neutral atom.$E_{2}$

Vedclass · Accepted Answer

$E_{1} < E_{2}$

Vedclass · Answer

(A) $E_{1}$ represents the first ionization energy $(I.E._{1})$,which is the energy required to remove the first electron from a neutral atom.$E_{2}$ represents the second ionization energy $(I.E._{2})$,which is the energy required to remove the second electron from a unipositive ion $(A^{+})$.Since the $A^{+}$ ion has a higher effective nuclear charge and a smaller size compared to the neutral atom $A$,it holds the remaining electrons more tightly.Therefore,more energy is required to remove the second electron than the first,leading to the relationship $E_{1} < E_{2}$.

$A \to A^{+} + e, E_{1}$ and $A^{+} \to A^{2+} + e, E_{2}$. The energy required to pull out the two electrons are $E_{1}$ and $E_{2}$ respectively. The correct relationship between the two energies is:

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 first four ionization energy values of an element are $191$,$578$,$872$ and $5962 \ kcal$. The number of valence electrons in the element is

Which among the following orders of second $IP$ (Ionization Potential) is correct?

How many ionisation energies can carbon have?

Which of the following elements will have the lowest first ionisation energy?

Vedclass Test Series

Exam Paper Generator

Online Exam Module