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# Why does caesium $(Cs)$ have a larger atomic radius than lithium $(Li)$?(A) Atomic radius increases as you move from right to left and top to bottom(B) Atomic radius increases as you go from left to right and bottom to top on a periodic table(C) Both $(Cs)$ and $(Li)$ have the same atomic radius.(D) It cannot be determined which element has the higher atomic radius

Last updated date: 09th Aug 2024
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Hint: Atomic radius of a chemical element in the measure of the size of its atom. Usually, it is the distance of the nucleus to the outermost shell containing electrons. Both $(Cs)$ and $(Li)$ belong to group 1 and the atomic radii comparisons can be done by the regular trends we observe when we come from top to bottom in a group. The same is discussed below,

In the question it is mentioned that Caesium $(Cs)$ have a larger atomic radius than Lithium $(Li)$. Let us see the reason behind the statement. Firstly, let us understand what periodicity means?
Since, in group $1$ Lithium $(Li)$is at the top, so it has least shell and as a result least size as compared to caesium $(Cs)$ which is placed last in group and so it has largest number of shell and hence biggest size.