Why manganese have high metallic radius as compared to other metals?

Question

Answer

Once you start pairing the electrons in the d block, you are adding more negative particles that repel the valence 4s, making the atomic radius increase. The repelling of the 4s electron pair isn't nearly as significant for Scandium-Manganese due to those elements having unpaired electrons in their d orbitals.

Answer

Explanation of why manganese has a high metallic radius compared to other metals

Definition of metallic radius

Metallic radius is the distance between the nuclei of two adjacent atoms in a metallic crystal. In other words, it is the distance between the centers of the positive ions in a metal.

Manganese's atomic structure

Manganese has an atomic number of 25 and its electronic configuration is 1s2 2s2 2p6 3s2 3p6 4s2 3d5. It has five valence electrons in its 3d orbital and two in its 4s orbital.

The reason behind manganese's high metallic radius

Manganese has a high metallic radius compared to other metals due to its electronic configuration. Manganese's 3d electrons are not tightly bound to the nucleus, and so they are easily shared with neighboring atoms in a metallic crystal. This results in a greater distance between the nuclei of adjacent atoms, leading to a larger metallic radius.

Comparison with other metals

Other metals, such as iron and nickel, have smaller metallic radii because their 3d electrons are tightly bound to the nucleus, making it harder for them to be shared with neighboring atoms. This results in a smaller distance between the nuclei of adjacent atoms, leading to a smaller metallic radius.

Conclusion

In conclusion, manganese has a high metallic radius compared to other metals due to its electronic configuration. Its 3d electrons are not tightly bound to the nucleus, allowing them to be easily shared with neighboring atoms in a metallic crystal, resulting in a larger distance between the nuclei of adjacent atoms.

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