The electronic configurations of four element | vedclass

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(C) The electronic configurations are:$(I) \, 1s^2$: Helium $(He)$,a noble gas,inert.$(II) \, 1s^2 2s^2 2p^2$: Carbon $(C)$,which has $4$ valence elec

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$III$

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(C) The electronic configurations are:$(I) \, 1s^2$: Helium $(He)$,a noble gas,inert.$(II) \, 1s^2 2s^2 2p^2$: Carbon $(C)$,which has $4$ valence electrons. It primarily forms covalent bonds but can form carbides (ionic) with electropositive metals.$(III) \, 1s^2 2s^2 2p^5$: Fluorine $(F)$,which has $7$ valence electrons. It forms ionic bonds with metals and covalent bonds with non-metals.$(IV) \, 1s^2 2s^2 2p^6$: Neon $(Ne)$,a noble gas,inert.Between $II$ and $III$,$III$ (Fluorine) is the most electronegative element and is well-known for forming strong ionic bonds with metals and covalent bonds with non-metals. However,in the context of typical chemistry curriculum questions regarding the ability to form both,$III$ is the standard answer.

The electronic configurations of four elements are given below:
$(I) \, 1s^2 \, (II) \, 1s^2 2s^2 2p^2 \, (III) \, 1s^2 2s^2 2p^5 \, (IV) \, 1s^2 2s^2 2p^6$
Which element has the ability to form both ionic and covalent bonds?

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The electronic configurations of four elements are given below:$(I) \, 1s^2 \, (II) \, 1s^2 2s^2 2p^2 \, (III) \, 1s^2 2s^2 2p^5 \, (IV) \, 1s^2 2s^2 2p^6$Which element has the ability to form both ionic and covalent bonds?