(C) The electronic configuration of $Be$ $(Z=4)$ is $1s^2 2s^2$,which is a fully filled $s$-orbital.The electronic configuration of $B$ $(Z=5)$ is $1s

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Boron has only one electron in $p$-sub-shell

(C) The electronic configuration of $Be$ $(Z=4)$ is $1s^2 2s^2$,which is a fully filled $s$-orbital.The electronic configuration of $B$ $(Z=5)$ is $1s^2 2s^2 2p^1$.Removing an electron from $Be$ requires breaking a stable,fully filled $2s$ subshell,which requires more energy.In contrast,the electron in $B$ is removed from the $2p$ subshell,which is easier to remove as it is shielded by the $2s$ electrons and is at a slightly higher energy level.

Class 11 Chemistry Classification of Elements and Periodicity in Properties Ionisation energy

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The first ionization energy of boron is less than that of beryllium because

A
Boron has higher nuclear charge
B
Atomic size of boron is more than that of beryllium
C
Boron has only one electron in $p$-sub-shell
D
Atomic size of boron is less than that of beryllium

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Classification of Elements and Periodicity in Properties

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Ionisation energy

Which of the following electronic configurations is associated with the biggest jump between the second and third ionization energies?

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The energy required to remove an electron of a gaseous atom from its ground state is called

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Observe the following statements.
Statement $(A)$: In general,the ionisation potential value decreases on moving down in the group.
Statement $(B)$: The $1$st ionisation potential of sodium is greater than that of potassium.
Correct answer is:

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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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Starting from the $1^{st}$,the successive ionization potentials of an element are respectively $5.98, 18.8, 28.4, 120.1, 154 \ eV$. The element is

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The first ionization energy of boron is less than that of beryllium because

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Which of the following electronic configurations is associated with the biggest jump between the second and third ionization energies?

The energy required to remove an electron of a gaseous atom from its ground state is called

Observe the following statements.Statement $(A)$: In general,the ionisation potential value decreases on moving down in the group.Statement $(B)$: The $1$st ionisation potential of sodium is greater than that of potassium.Correct answer is:

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:

Starting from the $1^{st}$,the successive ionization potentials of an element are respectively $5.98, 18.8, 28.4, 120.1, 154 \ eV$. The element is

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Observe the following statements.
Statement $(A)$: In general,the ionisation potential value decreases on moving down in the group.
Statement $(B)$: The $1$st ionisation potential of sodium is greater than that of potassium.
Correct answer is: