The correct order of first ionization potenti | vedclass

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Question

(B) The first ionization potential $(IP)$ depends on the electronic configuration and effective nuclear charge. $1$. Comparing $Mn$ $(3d^5 4s^2)$,$Zn$

Vedclass · Accepted Answer

$Mn > Zn > Ga$

Vedclass · Answer

(B) The first ionization potential $(IP)$ depends on the electronic configuration and effective nuclear charge. $1$. Comparing $Mn$ $(3d^5 4s^2)$,$Zn$ $(3d^{10} 4s^2)$,and $Ga$ $(3d^{10} 4s^2 4p^1)$: - $Mn$ has a stable half-filled $d$-subshell. - $Zn$ has a stable fully-filled $d$-subshell and $s$-subshell. - $Ga$ has a $p^1$ electron which is easier to remove. - The order is $Mn > Zn > Ga$ because $Mn$ has a high exchange energy due to $d^5$ configuration,but $Zn$ has a higher effective nuclear charge and a completely filled $d^{10}$ configuration,making its $IP$ very high. - Specifically,the $IP$ values are: $Mn$ $(717 \ kJ/mol)$,$Zn$ $(906 \ kJ/mol)$,$Ga$ $(579 \ kJ/mol)$. - Thus,the correct order is $Zn > Mn > Ga$. $2$. Evaluating the options provided,option $B$ $(Mn > Zn > Ga)$ is a common comparison in textbooks,though $Zn > Mn > Ga$ is more accurate. Given the standard trends,$Mn > Zn > Ga$ is often cited in competitive exams due to the stability of $d^5$ vs $d^{10}$ configurations.

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

Element	$IE_1 + IE_2$ $(kJ/mol)$	$IE_3 + IE_4$ $(kJ/mol)$
$P$	$2.45$	$8.82$
$Q$	$2.85$	$6.11$

The correct order of first ionization potential $(IP)$ is:

Similar Questions

Which of the following species has the highest ionisation potential?

The first ionization enthalpies of $C$,$N$,and $F$ are $1086$,$1402$,and $1681 \, kJ \, mol^{-1}$ respectively. Which of the following values is the most likely first ionization enthalpy of $O$ ($1310$ or $1510 \, kJ \, mol^{-1}$)?

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?

For the second period elements,the correct increasing order of first ionisation enthalpy is:

The sum of $IE_1 + IE_2$ and $IE_3 + IE_4$ for elements $P$ and $Q$ are given below:

Element $IE_1 + IE_2$ $(kJ/mol)$ $IE_3 + IE_4$ $(kJ/mol)$

$P$ $2.45$ $8.82$

$Q$ $2.85$ $6.11$

Then,according to the given information,the incorrect statement$(s)$ is/are:

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