gen-briefly-explain-electronegativity-and-one-common-misconcepti-02d9

Briefly explain electronegativity and one common misconception about it.

## Electronegativity **Electronegativity** is the measure of an atom's ability to attract shared electrons toward itself when bonded to another atom. It's essentially a "tug-of-war" strength for electrons in a chemical bond. Elements like fluorine have high electronegativity (strong pull), while elements like sodium have low electronegativity (weak pull). ## Common Misconception Many students confuse **electronegativity** with **electron affinity**. - **Electronegativity** refers to electron attraction *in a bond* (between two atoms) - **Electron affinity** is the energy change when an isolated atom *gains* an electron In other words, electronegativity is about sharing electrons in molecules, while electron affinity is about a single atom accepting an electron completely. Though they're related concepts, they describe different situations and even have different units (electronegativity is often unitless, like the Pauling scale).