The radius of isoelectronic species:

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(B) An isoelectronic series is a group of ions that all have the same number of electrons. For example,one isoelectronic series could include $O^{2-},

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Decreases with the increase of nuclear charge

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(B) An isoelectronic series is a group of ions that all have the same number of electrons. For example,one isoelectronic series could include $O^{2-}, F^{-}, Na^{+}, Mg^{2+}$. These all have $10$ electrons. The number of protons,however,increases as the atomic number increases,which leads to an increase in nuclear charge. As the nuclear charge increases,the effective nuclear charge experienced by the electrons also increases. Consequently,the nucleus attracts the electrons more strongly,pulling them closer. Therefore,the ionic radii of species in an isoelectronic series decrease as the nuclear charge increases.

Similar Questions

The ionic radii of $N^{3-}$,$O^{2-}$,$F^{-}$,and $Na^{+}$ follow the order:

Arrange the following elements in the increasing order of their atomic radii:
$(i)$ $O, N, F, B, Be, Li, C$
$(ii)$ $P, S, Mg, Na, Al, Si, Cl$
$(iii)$ $K, Na, Li, Cs, Rb$
$(iv)$ $Cl, F, I, At, Br$

Which of the following orders is correct?

In which of the following options,elements are correctly arranged in the increasing order of their atomic radius?

Which of the following represents the incorrect order of ionic size?

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