Correct increasing order of first ionisation | vedclass

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(A) As we move across the period,nuclear charge increases and atomic size decreases,hence ionisation enthalpy generally increases.For $Al$ $([Ne] 3s^2

Vedclass · Accepted Answer

$Na  Al < Si$

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(A) As we move across the period,nuclear charge increases and atomic size decreases,hence ionisation enthalpy generally increases.For $Al$ $([Ne] 3s^2 3p^1)$,the electron is removed from a partially filled $3p$ orbital,whereas for $Mg$ $([Ne] 3s^2)$,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.Therefore,the ionisation enthalpy of $Mg$ is greater than that of $Al$.The correct order of first ionisation enthalpies is: $Na  Al < Si$.

List-$I$ ($IE_1, IE_2, IE_3$ in $kJ \ mol^{-1}$)	List-$II$ (Element)
$A$. $1510$	$1$. $H$
$B$. $495, 6500, 10200$	$2$. $Li$
$C$. $840, 1630, 13100$	$3$. $Be$
$D$. $600, 2050, 3100$	$4$. $B$

List-$I$ (Electronic configuration)	List-$II$ ($\Delta_{i}H$ in $kJ\ mol^{-1}$)
$(a)$ $1s^{2} 2s^{2}$	$(i)$ $801$
$(b)$ $1s^{2} 2s^{2} 2p^{4}$	$(ii)$ $899$
$(c)$ $1s^{2} 2s^{2} 2p^{3}$	$(iii)$ $1314$
$(d)$ $1s^{2} 2s^{2} 2p^{1}$	$(iv)$ $1402$

Correct increasing order of first ionisation potential is

Similar Questions

The first ionization energy is the lowest for which of the following elements?

The first ionization enthalpy of $O$ is less than that of $N$,because .........

Match List-$I$ with List-$II$ with correct code:

List-$I$ ($IE_1, IE_2, IE_3$ in $kJ \ mol^{-1}$) List-$II$ (Element)

$A$. $1510$ $1$. $H$

$B$. $495, 6500, 10200$ $2$. $Li$

$C$. $840, 1630, 13100$ $3$. $Be$

$D$. $600, 2050, 3100$ $4$. $B$

Ionization energy increases in the order

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