Match the electronic configuration (List 1) with the values of (IE) the elements in the nth period (List 2).

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Solution

The electronic configurations and the ionization energies are matched as shown below.
A) ${n s}^{2}$ - 1200
B) ${n s}^{2} {n p}^{1}$ - 1400
C) ${n s}^{2} {n p}^{3}$ - 1500
D) ${n s}^{2} {n p}^{6}$ - 4000
In a give period, the alkali metals and the alkaline earth metals have very low values of ionization energy whereas noble gases have very high values of ionization energies as the ionization will result in breaking of the noble gas configuration.

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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}

n \in I^{+}

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