(D) For isoelectronic species,the number of electrons is the same,so the size is determined by the effective nuclear charge $(Z)$.As the nuclear charg

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(D) For isoelectronic species,the number of electrons is the same,so the size is determined by the effective nuclear charge $(Z)$.As the nuclear charge $(Z)$ increases,the force of attraction between the nucleus and the electrons increases,which pulls the electron cloud closer to the nucleus.Therefore,the size is inversely proportional to the nuclear charge: $\text{Size} \propto \frac{1}{Z}$.

Class 11 Chemistry Classification of Elements and Periodicity in Properties Atomic and Ionic radii

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The size of the isoelectronic species $Cl^{-}$,$Ar$,and $Ca^{2+}$ is affected by

JEE MAIN 2019 All JEE MAIN

A
Principal quantum number of valence shell
B
Azimuthal quantum number of valence shell
C
Electron-electron interaction in the outer orbitals
D
Nuclear charge

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Class 11 Questions

Class 11

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Chapter

Classification of Elements and Periodicity in Properties

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Atomic and Ionic radii

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The increasing order of the atomic radii of the following elements is
$a. C, b. O, c. F, d. Cl, e. Br$

DifficultJEE MAIN 2020

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Which of the following is the incorrect order of ionic radius?

Difficult

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Explain why cations are smaller and anions larger in radii than their parent atoms.

Medium

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The largest element among $O$,$Se$,$S$,and $Te$ is:

EasyAP EAMCET 2020

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Match $Column\, A$ with $Column\, B$:
$Column\, A$ (ion) $Column\, B$ (radius)
$(i)$ $Li^{+}$ $(p)$ $216\, pm$
$(ii)$ $Na^{+}$ $(q)$ $195\, pm$
$(iii)$ $Br^{-}$ $(r)$ $60\, pm$
$(iv)$ $I^{-}$ $(s)$ $95\, pm$

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$Column\, A$ (ion)	$Column\, B$ (radius)
$(i)$ $Li^{+}$	$(p)$ $216\, pm$
$(ii)$ $Na^{+}$	$(q)$ $195\, pm$
$(iii)$ $Br^{-}$	$(r)$ $60\, pm$
$(iv)$ $I^{-}$	$(s)$ $95\, pm$

The size of the isoelectronic species $Cl^{-}$,$Ar$,and $Ca^{2+}$ is affected by

Similar Questions

The increasing order of the atomic radii of the following elements is$a. C, b. O, c. F, d. Cl, e. Br$

Which of the following is the incorrect order of ionic radius?

Explain why cations are smaller and anions larger in radii than their parent atoms.

The largest element among $O$,$Se$,$S$,and $Te$ is:

Match $Column\, A$ with $Column\, B$:$Column\, A$ (ion)$Column\, B$ (radius)$(i)$ $Li^{+}$$(p)$ $216\, pm$$(ii)$ $Na^{+}$$(q)$ $195\, pm$$(iii)$ $Br^{-}$$(r)$ $60\, pm$$(iv)$ $I^{-}$$(s)$ $95\, pm$

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The increasing order of the atomic radii of the following elements is
$a. C, b. O, c. F, d. Cl, e. Br$

Match $Column\, A$ with $Column\, B$:
$Column\, A$ (ion) $Column\, B$ (radius)
$(i)$ $Li^{+}$ $(p)$ $216\, pm$
$(ii)$ $Na^{+}$ $(q)$ $195\, pm$
$(iii)$ $Br^{-}$ $(r)$ $60\, pm$
$(iv)$ $I^{-}$ $(s)$ $95\, pm$