The first ionization enthalpies of Li,Be,and | vedclass

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Question

(A) The correct value is $800 \ kJ \ mol^{-1}$.In the second period,the ionization enthalpy increases from $Li$ to $Ne$ with some exceptions.Specifica

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$800 \ kJ \ mol^{-1}$

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(A) The correct value is $800 \ kJ \ mol^{-1}$.In the second period,the ionization enthalpy increases from $Li$ to $Ne$ with some exceptions.Specifically,$Be$ $(1s^2 2s^2)$ has a higher ionization enthalpy than $B$ $(1s^2 2s^2 2p^1)$ because $Be$ has a stable fully-filled $2s$ orbital.Therefore,the order of first ionization enthalpy for these elements is $Li Since $B$ must be lower than $Be$ $(899 \ kJ \ mol^{-1})$,$800 \ kJ \ mol^{-1}$ is the appropriate value.

The first ionization enthalpies of $Li$,$Be$,and $C$ are $520$,$899$,and $1086 \ kJ \ mol^{-1}$ respectively. Which of the values $800$ or $900 \ kJ \ mol^{-1}$ is more likely for the first ionization enthalpy of $B$? Why?

Similar Questions

Discuss the trend of the first ionisation enthalpy in the same period and explain why it occurs.

Which of the following represents the correct order of first ionization enthalpy?
$(i) \ Li < B < Be < C$ $(ii) \ O < N < F$ $(iii) \ Be < N < Ne$

Which of the following elements are at the peaks of the ionization energy trend?

Which has maximum first ionization potential?

The correct decreasing order of the first ionisation enthalpies of the five elements $Be, B, C, N, F$ is:

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