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(A) Metallic character is defined by the ease with which an element can lose electrons. Across a period (from left to right),the metallic character de

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$K > Na > Al > Be$

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(A) Metallic character is defined by the ease with which an element can lose electrons. Across a period (from left to right),the metallic character decreases due to an increase in effective nuclear charge. Down a group,the metallic character increases due to an increase in atomic size and decrease in ionization enthalpy. Comparing the given elements: $K$ (Potassium) is in Group $1$,Period $4$. $Na$ (Sodium) is in Group $1$,Period $3$. $Al$ (Aluminium) is in Group $13$,Period $3$. $Be$ (Beryllium) is in Group $2$,Period $2$. Since $K$ is below $Na$,$K > Na$. Since $Na$ is to the left of $Al$ in the same period,$Na > Al$. Since $Al$ is in the $3^{rd}$ period and $Be$ is in the $2^{nd}$ period,$Al > Be$. Thus,the correct order of metallic character is $K > Na > Al > Be$.

Column $A$	Column $B$
$(i) \; Na_{2}O$	$(a) \; Neutral$
$(ii) \; Al_{2}O_{3}$	$(b) \; Basic$
$(iii) \; N_{2}O$	$(c) \; Acidic$
$(iv) \; Cl_{2}O_{7}$	$(d) \; Amphoteric$

The correct order of the metallic character of the elements $Be, Al, Na, K$ is

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