Describe the electron distribution in a polar-covalent bond and its effect on the partial charges...?

Question

Describe the electron distribution in a polar-covalent bond and its effect on the partial charges of the compound.

Answer 1

For this, it is best to use an example.

Herefore, I will use the compound HF.

By looking on an electronegativity chart, you can easily see that the electronegativity difference is 1.7, which makes it a strong polar-covalent bond. However, the electronegativity value for Fluorine is still significantly greater than that for Hydrogen.

This means that the electron pair shared between the two atoms is attracted more to the Fluorine than to the Hydrogen.
This, in tern, means that there is more electron density around the Fluorine than the Hydrogen. Therefore, the fluorine has partial negative charge and the hydrogen has a partial positive charge due to the electron pair being closer to the fluorine atom.