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

Given two statements below :
Statement $I:$ In $Cl_2$ molecule the covalent radius is double of the atomic radius of chlorine.
Statement $II:$ Radius of anionic species is always greater than their parent atomic radius.
Choose the most appropriate answer from options given below :

The incorrect decreasing order of atomic radii is:

Which one of the following is the smallest in size?

Increasing order of atomic radii is

What do atomic radius and ionic radius mean? Describe them.

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