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Home / Chemistry / Understanding Ionic Radius

Understanding Ionic Radius

Last Updated on Feb 20, 2025
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Ever wondered about the term ionic radii? In this article, we will explore what ionic radii are and how they vary across the groups and periods of the modern periodic table .

What Does Ionic Radius Mean?

Simply put, ionic radius is the distance from the nucleus of an ion to the edge of its electron cloud.

An ion comes into existence when an atom either loses or gains electrons. An atom that loses an electron becomes a cation, while one that gains an electron becomes an anion. The ionic radius is essentially the distance between the nucleus of an ion and its outermost shell.

The atomic size of a cation is smaller than its parent atom, while an anion is larger than its parent atom. This is due to the increase in the total number of electrons when an atom becomes an anion, which results in more electron-electron repulsion and reduces the net effective nuclear charge.

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Ionic Radius and the Periodic Table

Let's consider a different example,

  • Radius of sodium = 186pm.
  • Radius of sodium ion = 95pm.

Species with the same number of electrons, such as N 3- and Al 3+ , are termed as isoelectronic species. Despite having the same number of electrons, they do not have the same ionic radius due to the difference in their effective nuclear charges.

The radius of a cation is smaller than that of an anion because cations have a greater positive charge (i.e., more protons), which results in a stronger attraction for the outermost electrons and hence a smaller size.

Trends in Ionic Radius in Groups

In the periodic table, as we move down a group, atoms add an extra shell (or electrons), leading to an increase in the ionic radius of the elements.

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Trends in Ionic Radius Across a Period

To understand the trends in the ionic radius of elements across a period, let's consider period 2. Here, we observe that the atomic radius first decreases, then suddenly increases, and then gradually decreases again. This is because the elements at the start of a period tend to form cations, while those towards the end of a period form anions.

The formation of ions, which results from the gain or loss of electrons, plays a crucial role in chemical reactions , leading to the creation of new substances. Understanding the ionic radii helps us study the various chemical bonds formed during a reaction.

To learn more about the elements of the periodic table and their properties, continue exploring our resources.

 

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Frequently Asked Questions

Atomic radius is the mean or typical distance from the centre of the nucleus to the boundary of the surrounding shells of electrons.

Ionic radius is the distance from the nucleus of an ion up to which it has an influence on its electron cloud.

When an atom loses an electron it forms a cation and when it gains an electron it becomes an anion.

Atoms and ions which consist of an equal number of electrons are considered electronic species.

An anion is relatively larger in size than its parent atom. This is because when an atom gains electrons the total number of electrons increases which tends to create more repulsion between electrons and thus overshadows the net effective nuclear charge.
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