The first three ionisation energies (in kJ/mo | vedclass

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(C) For element $P$,the large jump between $IE_1$ $(495.8)$ and $IE_2$ $(4562)$ indicates it has $1$ valence electron,identifying it as an alkali meta

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$R$: $s-block$ element

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(C) For element $P$,the large jump between $IE_1$ $(495.8)$ and $IE_2$ $(4562)$ indicates it has $1$ valence electron,identifying it as an alkali metal.For element $Q$,the large jump between $IE_2$ $(1451)$ and $IE_3$ $(7733)$ indicates it has $2$ valence electrons,identifying it as an alkaline earth metal.For element $R$,the jumps between $IE_1, IE_2,$ and $IE_3$ are relatively small,suggesting it has $3$ valence electrons (e.g.,Aluminum),making it a $p-block$ element.Since $P, Q,$ and $R$ represent elements with $1, 2,$ and $3$ valence electrons respectively,they are likely in the same period (e.g.,$Na, Mg, Al$).Thus,the statement '$R$: $s-block$ element' is incorrect.

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

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?

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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?