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(B) The successive ionization potentials are $5.98, 18.8, 28.4, 120.1, 154 \ eV$. There is a large jump in energy between the $3^{rd}$ ionization pote

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$Al$

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(B) The successive ionization potentials are $5.98, 18.8, 28.4, 120.1, 154 \ eV$. There is a large jump in energy between the $3^{rd}$ ionization potential $(28.4 \ eV)$ and the $4^{th}$ ionization potential $(120.1 \ eV)$. This indicates that the element has $3$ valence electrons in its outermost shell. Among the given options,both Boron $(B)$ and Aluminium $(Al)$ belong to Group $13$ and have $3$ valence electrons. However,the ionization energy values provided are characteristic of Aluminium,as Boron has significantly higher ionization potentials due to its smaller atomic size.

$I.E.$	$1^{st}$	$2^{nd}$	$3^{rd}$	$4^{th}$	$5^{th}$
Value	$577.5$	$1810$	$2750$	$11580$	$14820$

Element	Ionization enthalpy $(kJ \ mol^{-1})$ $(1^{st}, 2^{nd}, 3^{rd})$
$A$	$899, 1757, 14847$
$B$	$737, 1450, 7731$

Starting from the $1^{st}$,the successive ionization potentials of an element are respectively $5.98, 18.8, 28.4, 120.1, 154 \ eV$. The element is

Similar Questions

For one of the elements,various successive ionization enthalpies (in $kJ \cdot mol^{-1}$) are given below:

$I.E.$ $1^{st}$ $2^{nd}$ $3^{rd}$ $4^{th}$ $5^{th}$

Value $577.5$ $1810$ $2750$ $11580$ $14820$

The element is:

In which of the following arrangements,the order is $NOT$ according to the property indicated against it?

For the second period elements,the correct increasing order of first ionisation enthalpy is:

Which factors influence the value of ionization enthalpy?

Consider the following ionization enthalpies of two elements $A$ and $B$.

Element Ionization enthalpy $(kJ \ mol^{-1})$ $(1^{st}, 2^{nd}, 3^{rd})$

$A$ $899, 1757, 14847$

$B$ $737, 1450, 7731$

Which of the following statements is correct?

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