Question 22

Amongst the following elements whose electronic configuration are given below, the one having the highest ionisation enthaply is

(a) $[N e] 3 s^{2} 3 p^{1}$

(b) $[N e] 3 s^{2} 3 p^{3}$

(c) $[N e] 3 s^{2} 3 p^{2}$

(d) $[A r] 3 d^{10} 4 s^{2} 4 p^{3}$

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Solution

The elestronic configuration of options (b) and (d) have exactly half-filled 3p orbitals (b) represents phosphorus and (c) represents arsenic but (b) is smaller in size than (d).

Hence, (b) has highest ionisation enthalpy. Ionisation enthalpy increases left to right in the periodic table as the size decreases.

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Similar questions

Amongst the following elements (whose electronic configurations are given below), the one having the highest ionisation energy is

4

= [N e] 3 s^{2} 3 p^{3}

= [A r] 3 d^{10} 4 s^{2} 4 p^{3}

= [H e] 2 s^{2} 2 p^{5}

= [N e] 3 s^{1}

Write the electronic configurations of the following ions:
(a) $H^{-}$
(b) $N a^{+}$
(c) $O^{2 -}$
(d) $F^{-}$

(ii) What are the atomic numbers of elements whose outermost electrons are represented by
(a) 3 $s^{1}$
(b) 2 $p^{3}$ and
(c) 3 $p^{5}$ ?

Which atoms are indicated by the following configurations?
(a) [He] 2 $s^{1}$
(b) [Ne] 3 $s^{2} 3 p^{3}$
(c) [Ar] 4 $s^{2} 3 d^{1}$

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