For an element,the values of IP_1, IP_2, IP_3 | vedclass

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(B) The ionization energy values are given as: $IP_1 = 7.1 \ eV$,$IP_2 = 14.3 \ eV$,$IP_3 = 34.5 \ eV$,$IP_4 = 46.8 \ eV$,and $IP_5 = 162.2 \ eV$. To

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$Si$

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(B) The ionization energy values are given as: $IP_1 = 7.1 \ eV$,$IP_2 = 14.3 \ eV$,$IP_3 = 34.5 \ eV$,$IP_4 = 46.8 \ eV$,and $IP_5 = 162.2 \ eV$. To identify the element,we look for the largest jump in successive ionization energy values. The jump from $IP_4$ $(46.8 \ eV)$ to $IP_5$ $(162.2 \ eV)$ is very large,which indicates that the $5^{th}$ electron is being removed from a stable,noble gas-like inner shell configuration. This implies the element has $4$ valence electrons. Among the given options,$Si$ (Silicon) has an electronic configuration of $[Ne] 3s^2 3p^2$,which has $4$ valence electrons. Therefore,the element is $Si$.

For an element,the values of $IP_1, IP_2, IP_3, IP_4$ and $IP_5$ are $7.1, 14.3, 34.5, 46.8$ and $162.2 \ eV$ respectively. Which of the following is the most likely element?

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