With reference to the concept of ionisation p | vedclass

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(D) The ionisation potential generally decreases down a group and increases across a period from left to right. $B$ (Boron) is a non-metal in period $

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$Cs < U < K < B$

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(D) The ionisation potential generally decreases down a group and increases across a period from left to right. $B$ (Boron) is a non-metal in period $2$,which has a high ionisation potential. $K$ (Potassium) and $Cs$ (Caesium) are alkali metals in group $1$,where $Cs$ is below $K$,so $Cs$ has a lower ionisation potential than $K$. $U$ (Uranium) is an actinoid with a relatively low ionisation potential compared to non-metals like $B$. Comparing these,the correct order of increasing ionisation potential is $Cs < U < K < B$.

With reference to the concept of ionisation potential,which one of the following sets is correct?

Similar Questions

If the first ionisation enthalpy of $Li$,$Be$,and $C$ respectively are $520$,$899$,and $1086 \ kJ \ mol^{-1}$,the first ionisation enthalpy (in $kJ \ mol^{-1}$) of $B$ will be:

In the given graph,which point represents an alkali metal with the least atomic number?

The $3^{rd}$ ionisation energy amongst $Li$,$Be$,$B$ and $C$ is lowest for

The first ionisation energies of alkaline earth metals are higher than those of the alkali metals. This is because

Which of the following represents the correct order of ionization enthalpy?
$(i) Be^{+} > Be$ $(ii) Be > Be^{+}$ $(iii) C > Be$ $(iv) B > Be$

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