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.

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

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

Which of the following has the least ionization potential?

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

The first ionization potential values (in $eV$) for nitrogen and oxygen atoms are respectively:

The first ionisation potential will be maximum for

The $CORRECT$ order of first ionisation enthalpy is:

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