Which among the following elements has the lo | vedclass

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(B) The first ionization energy $(IE_1)$ generally decreases down a group due to the increase in atomic size and shielding effect.For group $14$ eleme

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$Sn$

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(B) The first ionization energy $(IE_1)$ generally decreases down a group due to the increase in atomic size and shielding effect.For group $14$ elements $(C, Si, Ge, Sn, Pb)$,the ionization energy decreases from $C$ to $Sn$.However,$Pb$ shows a higher $IE_1$ than $Sn$ due to the poor shielding effect of $d-$ and $f-$electrons,which leads to a higher effective nuclear charge $(Z_{eff})$ experienced by the valence electrons.Therefore,among the given options,$Sn$ has the lowest $IE_1$ value.

Which among the following elements has the lowest value of $IE_1$?

Similar Questions

The ionisation potentials of $Li$ and $K$ are $5.4 \ eV$ and $4.3 \ eV$ respectively. The ionisation potential of $Na$ will be ................ $eV$.

Which statement is correct regarding ionisation potential?

Assertion $(A)$: $16$th group elements have higher ionisation enthalpy values than $15$th group elements in the corresponding periods.
Reason $(R)$: $15$th group elements have half-filled stable electronic configurations.

Which of the following orders for ionisation energy is correct?

The second ionization potential of $Li$,$Be$,and $B$ is in the order:

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