The first four I.E. values of an element are | vedclass

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(C) The ionization energy $(I.E.)$ values provided are $I.E._1 = 284 \ kJ \ mol^{-1}$,$I.E._2 = 412 \ kJ \ mol^{-1}$,$I.E._3 = 656 \ kJ \ mol^{-1}$,an

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$3$

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(C) The ionization energy $(I.E.)$ values provided are $I.E._1 = 284 \ kJ \ mol^{-1}$,$I.E._2 = 412 \ kJ \ mol^{-1}$,$I.E._3 = 656 \ kJ \ mol^{-1}$,and $I.E._4 = 3210 \ kJ \ mol^{-1}$.Calculating the successive differences:$I.E._2 - I.E._1 = 412 - 284 = 128 \ kJ \ mol^{-1}$$I.E._3 - I.E._2 = 656 - 412 = 244 \ kJ \ mol^{-1}$$I.E._4 - I.E._3 = 3210 - 656 = 2554 \ kJ \ mol^{-1}$There is a very large jump in energy between the third and fourth ionization energies $(2554 \ kJ \ mol^{-1})$,which indicates that the fourth electron is being removed from a stable,noble gas-like core configuration.Therefore,the element has $3$ valence electrons.

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

The first four $I.E.$ values of an element are $284, 412, 656$ and $3210 \ kJ \ mol^{-1}$. The number of valence electrons in the element are

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Which one of the following is the correct order of the second ionisation potential of $Na$,$Ne$,$Mg$,and $Al$?

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?

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

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