The first ionization enthalpy of Na,Mg and Si | vedclass

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Question

(C) The general trend for the first ionization enthalpy across the third period is: $Na < Al < Mg < Si$.Given values are:$IE(Na) = 496 \ kJ \ mol^{-1}

Vedclass · Accepted Answer

$577$

Vedclass · Answer

(C) The general trend for the first ionization enthalpy across the third period is: $Na Given values are:$IE(Na) = 496 \ kJ \ mol^{-1}$$IE(Mg) = 737 \ kJ \ mol^{-1}$$IE(Si) = 786 \ kJ \ mol^{-1}$Based on the periodic trend,the ionization enthalpy of $Al$ should be greater than $Na$ but less than $Mg$.Therefore,$496 Among the given options,only $577 \ kJ \ mol^{-1}$ falls within this range.Thus,the correct option is $(C)$.

The first ionization enthalpy of $Na$,$Mg$ and $Si$,respectively,are: $496, 737$ and $786 \ kJ \ mol^{-1}$. The first ionization enthalpy $(kJ \ mol^{-1})$ of $Al$ is

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