Which property describes an atom's ability to attract electrons in a molecule?

• A. Covalent
• B. Electronegativity
• C. Ionization energy
• D. Valence electrons

Answer: (B)

Electronegativity is the tendency of an atom to attract electrons toward itself when it forms a bond. This concept explains why in a covalent bond the shared electrons are not always shared equally, leading to polar bonds and partial charges on the atoms. Covalent describes the type of bond (sharing electrons) rather than how strongly electrons are drawn to one atom. Ionization energy is the energy required to remove an electron from a neutral atom, not about attracting electrons in a bond. Valence electrons are the outer-shell electrons involved in bonding, not the ability to pull electrons from another atom. Therefore, the property that describes an atom’s ability to attract electrons in a molecule is electronegativity.