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

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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: $Na  Al < Si$.

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

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

Similar Questions

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

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

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

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

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

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

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

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.

The correct order of first ionisation enthalpy of group-$13$ elements is

For elements $B$,$C$,$N$,$Li$,$Be$,$O$ and $F$,the correct order of first ionization enthalpy is:

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