Why does an ionic bond transfer electrons instead of sharing?

The modern definition of electronegativity is due to Linus Pauling. It is the power of an atom in a molecule to attract electrons to itself.

When the electronegativity difference between the two atoms is greater than 2.0, the bond is considered ionic; i.e. there is complete transfer (between the two atoms) of the electrons in the bond. The electronegativity (according to Pauling scale) of chlorine is 3.0, while the electronegativity of sodium is 0.9.

So, electrons are transferred because of a larger electronegativity difference.

aliasger2709 aliasger2709 · Answer 2 · 2021-12-15T13:33:08+01:00

When there is a whole transfer of valence electron between the atoms is called an ionic bond. In this type of bond construction, the atoms get contrarily charged.

The ionic bonds are formed due to electronegativity. According to Pauling, the capability of an atom to draw electrons towards itself is called electronegativity.

When there is a huge contrast in electronegativity between the atoms, the electrons are completely transferred between the atoms.

The atom that relinquishes an electron are called a cation and is positive whereas the atom that acquires an electron are called anions and are negatively charged.

Therefore, due to electronegativity, ionic bonds are formed.

To learn more about ionic bonds follow the link:

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