The electronic configuration of four elements is given below. Which has the tendency to form covalent as well as ionic bonds?

1 s^{2}

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1 s^{2}, 2 s^{2}, 2 p^{2}

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1 s^{2}, 2 s^{2}, 2 p^{5}

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1 s^{2}, 2 s^{2}, 2 p^{6}

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Solution

The correct option is B $1 s^{2}, 2 s^{2}, 2 p^{5}$
Halogen element, any of the six non metallic elements that constitute Group 17 (Group VIIa) of the periodic table. The halogen elements are (F), (Cl), (Br), (I), (At).

Element $(1 s^{2}, 2 s^{2} 2 p^{5})$ can form ionic as well as covalent bond (halogens) .

Thus Option $C$ is correct.

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{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{1}

\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}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{1}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{5}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6} {4 s}^{1}

{(I E)}_{1}

{(I E)}_{4}

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{1}

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