Observe the following data ( Delta_i H_1, Del | vedclass

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(A) The reactivity of a metal is determined by its ability to lose electrons,which is inversely proportional to its first ionisation enthalpy $( \Delt

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$ II $

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(A) The reactivity of a metal is determined by its ability to lose electrons,which is inversely proportional to its first ionisation enthalpy $( \Delta_i H_1 )$.Lower $ \Delta_i H_1 $ values indicate that the metal can lose its valence electron more easily,making it more reactive.Comparing the $ \Delta_i H_1 $ values:$ I = 520 \ kJ \ mol^{-1} $$ II = 490 \ kJ \ mol^{-1} $$ III = 1681 \ kJ \ mol^{-1} $$ IV = 2372 \ kJ \ mol^{-1} $Element $ II $ has the lowest first ionisation enthalpy $( 490 \ kJ \ mol^{-1} )$,which indicates it is the most reactive metal among the given options.

Element	$ \Delta_i H_1 $ $( kJ \ mol^{-1} )$	$ \Delta_i H_2 $ $( kJ \ mol^{-1} )$	$ \Delta_{eg} H $ $( kJ \ mol^{-1} )$
$ I $	$ 520 $	$ 7300 $	$ -60 $
$ I.I $	$ 490 $	$ 3051 $	$ -48 $
$ III $	$ 1681 $	$ 3374 $	$ -328 $
$ IV $	$ 2372 $	$ 5251 $	$ +48 $

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