* Electronegativity: Chlorine has a high electronegativity, meaning it has a strong tendency to attract electrons towards itself when it forms chemical bonds.

* Electron Configuration: Chlorine has seven electrons in its outermost shell. It needs one more electron to achieve a stable, full outer shell (like the noble gases). This makes it highly reactive and eager to gain an electron.

Examples:

* In a covalent bond with a less electronegative element (like hydrogen in HCl), chlorine will pull the shared electrons closer to itself, creating a partial negative charge on the chlorine atom.

* When chlorine reacts with a metal (like sodium in NaCl), it gains an electron from the metal, forming a negatively charged chloride ion (Cl⁻).

In summary: Chlorine's strong electronegativity and electron configuration make it an electron acceptor, leading it to attract electrons in chemical reactions.