The graph shows the variation of Ionization P | vedclass

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(A) In a group,the Ionization Potential $(I.P.)$ generally decreases from top to bottom due to an increase in atomic size and shielding effect.However

Vedclass · Accepted Answer

$13$ group

Vedclass · Answer

(A) In a group,the Ionization Potential $(I.P.)$ generally decreases from top to bottom due to an increase in atomic size and shielding effect.However,the graph shows an irregular trend $(A > B  D This specific zig-zag pattern of $I.P.$ values is characteristic of elements in group $13$ (e.g.,$B, Al, Ga, In, Tl$).In group $13$,the $I.P.$ decreases from $B$ to $Al$,then increases from $Al$ to $Ga$ due to poor shielding of $d$-electrons,decreases from $Ga$ to $In$,and increases from $In$ to $Tl$ due to poor shielding of $f$-electrons.Therefore,the group is $13$.

Element	$IE_1$	$IE_2$	$IE_3$
$P$	$495.8$	$4562$	$6910$
$Q$	$737.7$	$1451$	$7733$
$R$	$577.5$	$1817$	$2745$

The graph shows the variation of Ionization Potential $(I.P.)$ with Atomic Number $(At. No.)$ for elements $A$ to $E$. If these elements belong to the same group in the periodic table,identify the group.

Similar Questions

The first three ionisation energies (in $kJ/mol$) of three representative elements are given below:

Element $IE_1$ $IE_2$ $IE_3$

$P$ $495.8$ $4562$ $6910$

$Q$ $737.7$ $1451$ $7733$

$R$ $577.5$ $1817$ $2745$

Which of the following options is incorrect?

Which of the following species has the lowest ionization potential?

The correct order of ionisation energy of $C$,$N$,$O$,and $F$ is

Of the following isoelectronic ions,the one which has the lowest ionisation potential is

The first ionisation energy of oxygen is less than that of nitrogen. Which of the following is the correct reason for this observation?

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