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(C) The ionization enthalpy $(IE)$ is the energy required to remove an electron from a gaseous atom or ion.$(i)$ Removing an electron from a positivel

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$i, iii$

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(C) The ionization enthalpy $(IE)$ is the energy required to remove an electron from a gaseous atom or ion.$(i)$ Removing an electron from a positively charged ion $(Be^{+})$ requires more energy than removing it from a neutral atom $(Be)$ because the effective nuclear charge is higher in the ion. Thus,$IE(Be^{+}) > IE(Be)$ is correct.$(ii)$ $Be > Be^{+}$ is incorrect based on the logic above.$(iii)$ Across a period from left to right,$IE$ generally increases. Since $C$ is to the right of $Be$,$IE(C) > IE(Be)$ is correct.$(iv)$ $B$ has a lower $IE$ than $Be$ because $Be$ has a stable fully-filled $2s^{2}$ configuration. Thus,$IE(B)  Be$ incorrect.Therefore,the correct statements are $(i)$ and $(iii)$.

Which of the following represents the correct order of ionization enthalpy?
$(i) Be^{+} > Be$ $(ii) Be > Be^{+}$ $(iii) C > Be$ $(iv) B > Be$

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Which of the following represents the correct order of ionization enthalpy?$(i) Be^{+} > Be$ $(ii) Be > Be^{+}$ $(iii) C > Be$ $(iv) B > Be$