The IE_1 and IE_2 of three elements A,B,and C | vedclass

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(D) The metallic or non-metallic character of an element can be predicted by the difference between its successive ionization energies. For element $A

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$C$

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(D) The metallic or non-metallic character of an element can be predicted by the difference between its successive ionization energies. For element $A$: The difference between $IE_2$ and $IE_1$ is $2650 - 400 = 2250 \ kJ/mol$. This large jump indicates that $A$ is an alkali metal (Group $1$). For element $B$: The difference between $IE_2$ and $IE_1$ is $1070 - 550 = 520 \ kJ/mol$. This relatively small difference suggests that $B$ is an alkaline earth metal (Group $2$). For element $C$: The $IE_1$ value is $1150 \ kJ/mol$,which is significantly higher than those of $A$ and $B$. High ionization energy is a characteristic property of non-metals. Therefore,element $C$ represents a non-metal.

Element	$A, B, C$
$IE_1$	$400, 550, 1150$
$IE_2$	$2650, 1070, 2090$

The $IE_1$ and $IE_2$ of three elements $A$,$B$,and $C$ are given as : ( $IE$ in $kJ/mol$ )

Element $A, B, C$

$IE_1$ $400, 550, 1150$

$IE_2$ $2650, 1070, 2090$

Identify the element which represents a nonmetal.

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The $IE_1$ and $IE_2$ of three elements $A$,$B$,and $C$ are given as : ( $IE$ in $kJ/mol$ ) Element $A, B, C$ $IE_1$ $400, 550, 1150$ $IE_2$ $2650, 1070, 2090$ Identify the element which represents a nonmetal.