Which of the following elements will have the | vedclass

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(B) The first ionisation energy decreases down a group as the atomic size increases and the valence electron is further from the nucleus.$Mg$ and $Ca$

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$Rb$

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(B) The first ionisation energy decreases down a group as the atomic size increases and the valence electron is further from the nucleus.$Mg$ and $Ca$ belong to Group $2$,while $Li$ and $Rb$ belong to Group $1$.Among the given elements,$Rb$ $(Rubidium)$ is in the $5^{th}$ period of Group $1$,making it the largest atom with the weakest attraction for its valence electron.Therefore,$Rb$ has the lowest first ionisation energy.

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

Which of the following elements will have the lowest first ionisation energy?

Similar Questions

Which of the following is not the correct increasing order of ionisation energy?

The first ionization potentials in electron volts $(eV)$ of nitrogen and oxygen atoms are respectively given by:

Which among the following elements has the highest first ionization enthalpy?

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:

Which of the following electronic configurations has the highest ionization enthalpy?

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