Medium
The atomic radii of the elements across the second period of the periodic table:
- Adecrease due to increase in atomic number
- Bdecrease due to increase in effective nuclear charge
- Cdecrease due to increase in atomic weights
- Dincrease due to increase in the effective nuclear charge
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Similar Questions
The size of isoelectronic species $F^{-},$ $Ne$ and $Na^{+}$ is affected by
$(a)$ Nuclear charge $(Z)$
$(b)$ Valence principal quantum number $(n)$
$(c)$ Electron-electron interaction in the outer orbitals
$(d)$ None of the factors because their size is the same.
$(a)$ Nuclear charge $(Z)$
$(b)$ Valence principal quantum number $(n)$
$(c)$ Electron-electron interaction in the outer orbitals
$(d)$ None of the factors because their size is the same.
Easy
View SolutionIn period $4$ of the periodic table, the elements with the highest and lowest atomic radii are respectively:
DifficultJEE MAIN 2026
View SolutionHow does the atomic radius change across a period in the periodic table?
Medium
View SolutionWhich of the following options represents the correct ionic radii in $\mathring{A}$ of $N^{3-}, O^{2-}$ and $F^{-}$, respectively?
For $Na^{+}$,$Mg^{2+}$,$F^{-}$,and $O^{2-}$; the correct order of increasing ionic radii is
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