The order of ionisation potential between He^ | vedclass

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(C) Both $He^{+}$ and $H$ are hydrogen-like species containing only one electron.The ionization potential $(I.P.)$ is directly proportional to the squ

Vedclass · Accepted Answer

$I.P. (He^{+}) > I.P. (H)$

Vedclass · Answer

(C) Both $He^{+}$ and $H$ are hydrogen-like species containing only one electron.The ionization potential $(I.P.)$ is directly proportional to the square of the atomic number $(Z^2)$ for hydrogen-like species.For $H$ atom,$Z = 1$.For $He^{+}$ ion,$Z = 2$.Since $Z_{He^{+}} > Z_{H}$,the effective nuclear charge experienced by the electron in $He^{+}$ is greater than in $H$.Therefore,$I.P. (He^{+}) > I.P. (H)$.

$B$	$801$
$Al$	$577$
$Ga$	$579$
$In$	$558$
$Tl$	$589$

The order of ionisation potential between $He^{+}$ ion and $H$ atom (both species are in gaseous state) is

Similar Questions

The first ionization enthalpy values (in $kJ\,mol^{-1}$) of group $13$ elements are :

$B$ $801$

$Al$ $577$

$Ga$ $579$

$In$ $558$

$Tl$ $589$

How would you explain this deviation from the general trend?

The electronic configuration of an element with the largest difference between the $1^{st}$ and $2^{nd}$ ionisation energies is

Which of the following processes will have the maximum ionization energy?

Which of the following elements has the lowest ionization potential?

Explain the deviation in the ionization enthalpy of some elements from the general trend using the provided graph.

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