Three atoms have the following electron configurations respectively:
(i) ${1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{1}$
(ii) ${1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{5}$
(iii) ${1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6} {4 s}^{1}$
(a) Which of the three has the largest ${(I E)}_{1}$ ?
(b) Which has the largest ${(I E)}_{4}$ ?
Write your answer as a two digit number.
Ex - If answer for a & b is 3 & 2 respectively, answer as 32.

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Solution

The element with electronic configuration $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}$ (iii) has half filled s orbital making it stable than other two elements. Hence, $I E_{1}$ for (iii) is the most.
The element with electronic configuration $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}$ (i) has the least number of electrons and if 4 electrons are removed, the proton to electron ratio will be highest in it making $I E_{4}$ in it as the highest.

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\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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