The order of first ionization potentials of e | vedclass

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Question

(B) The first ionization potential $(IE_1)$ increases across a period from left to right and decreases down a group.For the given elements:$1$. $Li$ $

Vedclass · Accepted Answer

$Be > B > Li > Na$

Vedclass · Answer

(B) The first ionization potential $(IE_1)$ increases across a period from left to right and decreases down a group.For the given elements:$1$. $Li$ $(2s^1)$ and $Be$ $(2s^2)$ are in the $2^{nd}$ period.$2$. $B$ $(2s^2 2p^1)$ is also in the $2^{nd}$ period.$3$. $Na$ $(3s^1)$ is in the $3^{rd}$ period.Comparing $Li, Be, B$: $Be$ has a fully filled $2s$ orbital,making it more stable than $B$. Thus,$IE_1$ of $Be > B > Li$.Comparing with $Na$: $Na$ has the lowest $IE_1$ because it is in the $3^{rd}$ period.The correct order is $Be > B > Li > Na$.

$I.P.$ \text{ Trend}	Reason
$A$. $N > O$	Half-filled configuration
$B$. $Zr < Hf$	Lanthanide contraction
$C$. $Na > K$	$Z_{eff}$
$D$. $Al < Ga$	Transition contraction

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

The order of first ionization potentials of elements $Li, Be, B, Na$ is:

Similar Questions

Identify the incorrect match regarding Ionization Potential $(I.P.)$ trends:

$I.P.$ \text{ Trend} Reason

$A$. $N > O$ Half-filled configuration

$B$. $Zr < Hf$ Lanthanide contraction

$C$. $Na > K$ $Z_{eff}$

$D$. $Al < Ga$ Transition contraction

Highest energy will be absorbed to eject out the electron in the configuration:

In which of the following electronic configurations will there be a large difference between the second and third ionization energy?

In which of the following arrangements is the order not correct according to the property indicated against it?

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?

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