Match the type of elements (in List I) with the corresponding electronic configuration (in List II).

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Solution

(A) Inert gas elements beongs to zero group. Their valence shell electronic configuration is $1 s^{2}$ to $n s^{2} n p^{6}$ .
(B) Main group elements belongs to s and p block. Their valence shell electronic configuration is $n s^{1}$ to $n s^{2} n p^{5}$ .
(C) Transition elements belongs to d block. Their valence shell electronic configuration is $(n - 1) d^{1 - 9} n s^{2}$ .
(D) Inner transition elements belongs to f block. Their valence shell electronic configuration is $(n - 2) f^{1 - 14} (n - 1) s^{2} p^{6} d^{10} n s^{2}$ .

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List-I (Electronic configuration of elements )	List-II (I.E. in kJ/mol)
(a) $1 s^{2} 2 s^{2}$	(i) 801
(b) $1 s^{2} 2 s^{2} 2 p^{4}$	(ii) 899
(c) $1 s^{2} 2 s^{2} 2 p^{3}$	(iii) 1314
(d) $1 s^{2} 2 s^{2} 2 p^{1}$	(iv) 1402

	List-I		List-II
	Electonic configuration of elements		$Δ_{1} H (i n k J m o l^{- 1})$
(a)	$1 s^{2} 2 s^{2}$	(i)	$801$
(b)	$1 s^{2} 2 s^{2} 2 p^{4}$	(ii)	$899$
(c)	$1 s^{2} 2 s^{2} 2 p^{3}$	(iii)	$1314$
(d)	$1 s^{2} 2 s^{2} 2 p^{1}$	(iv)	$1402$

\begin{matrix} L i s t - I & L i s t - I I (I) 1 s^{2} & (P) Element shows highest negative oxidation state. (I I) 1 s^{2} 2 s^{2} 2 p^{5} & (Q) Element shows highest first ionisation enthalpy. (I I I) 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5} & (R) Element shows highest electronegativity on Pauling scale. (I V) 1 s^{2} 2 s^{2} 2 p^{2} & (S) Element shows maximum electron gain enthalpy (most exothermic). (T) Configuration belongs to C l (U) configuration belongs to C \end{matrix}

\begin{matrix} List-I & List - II P. & 1 s^{2} & 1. & Element shows highest negative oxidation state Q. & 1 s^{2} 2 s^{2} 2 p^{5} & 2. & Element shows highest first ionisation enthalpy R. & 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5} & 3. & Element shows highest electronegativity on Pauling scale S. & 1 s^{2} 2 s^{2} 2 p^{2} & 4. & Element shows maximum electron gain enthalpy (most exothermic) \end{matrix}

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