The successive ionisation enthalpies of an el | vedclass

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(B) $1^{st}$ Ionisation Enthalpy$1012 \ kJ \ mol^{-1}$$2^{nd}$ Ionisation Enthalpy$1907 \ kJ \ mol^{-1}$$3^{rd}$ Ionisation Enthalpy$2955 \ kJ \ mol^{

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$P$

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(B) $1^{st}$ Ionisation Enthalpy$1012 \ kJ \ mol^{-1}$$2^{nd}$ Ionisation Enthalpy$1907 \ kJ \ mol^{-1}$$3^{rd}$ Ionisation Enthalpy$2955 \ kJ \ mol^{-1}$$4^{th}$ Ionisation Enthalpy$4955 \ kJ \ mol^{-1}$$5^{th}$ Ionisation Enthalpy$6275 \ kJ \ mol^{-1}$$6^{th}$ Ionisation Enthalpy$21,260 \ kJ \ mol^{-1}$The jump in ionisation enthalpy occurs between the $5^{th}$ and $6^{th}$ ionisation energy,indicating that the element has $5$ valence electrons. Phosphorus $(P)$ has the electronic configuration $[Ne] 3s^2 3p^3$,which contains $5$ valence electrons. Therefore,the removal of the $6^{th}$ electron requires significantly more energy as it is removed from a stable noble gas core.

The successive ionisation enthalpies of an element $X$ in $(kJ \ mol^{-1})$ are $1012$,$1907$,$2955$,$4955$,$6275$ and $21,260$ respectively. The element $X$ is:

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