The first ionisation potential of Na,Mg,Al an | vedclass

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

Question

(A) As we move across the period,nuclear charge increases and atomic size decreases,hence ionization enthalpy generally increases.For $Al$ $(3s^{2} 3p

Vedclass · Accepted Answer

$Na  Al < Si$

Vedclass · Answer

(A) As we move across the period,nuclear charge increases and atomic size decreases,hence ionization enthalpy generally increases.For $Al$ $(3s^{2} 3p^{1})$,the electron is removed from a partially filled $3p$ orbital.For $Mg$ $(3s^{2})$,the electron is removed from a stable,fully filled $3s$ orbital.Removal of an electron from a stable,fully filled orbital requires more energy than removal from a partially filled orbital.Thus,the ionization enthalpy of $Mg$ is greater than that of $Al$.The correct order of first ionization enthalpies is: $Na  Al < Si$.

The first ionisation potential of $Na$,$Mg$,$Al$ and $Si$ are in the order :-

Similar Questions

If first ionization enthalpy $(\Delta_i H)$ values of $Na$,$Mg$ and $Si$ are respectively $496$,$737$ and $786 \ kJ \ mol^{-1}$,the first ionization enthalpy value of $Al$ (in $kJ \ mol^{-1}$) will be

Which of the following elements has the maximum first ionization potential?

The electronic configuration of elements $A, B$ and $C$ are $[He] 2s^1, [Ne] 3s^1$ and $[Ar] 4s^1$ respectively. Which one of the following orders is correct for the first ionization potentials (in $kJ \ mol^{-1}$) of $A, B$ and $C$?

The first ionization potentials $\left( eV \right)$ of $Be$ and $B$ respectively are:

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

Vedclass Test Series

Exam Paper Generator

Online Exam Module