How is electronegativity best defined?

Electronegativity is best defined as the ability of an atom to attract electrons in a covalent bond. This concept is crucial in understanding how different atoms interact with one another during chemical bonding. Electronegativity values can indicate how strongly an atom will pull shared electrons towards itself when bonded to another atom. Higher electronegativity means a greater tendency to attract electrons, which influences the nature of the bonding (whether it is ionic or covalent) and the resulting molecular structure and properties.

In contrast, other options present concepts that do not accurately capture the essence of electronegativity. The total number of electrons an atom possesses is a reflection of its atomic number and does not directly determine its ability to attract electrons in covalent interactions. The ability of an atom to lose electrons easily pertains more to electropositivity, which is the opposite concept of electronegativity, indicating that it readily gives up electrons rather than attracting them. Lastly, the amount of energy required to remove an electron refers to ionization energy, a separate property that relates to the strength of an atom's hold on its electrons rather than how it interacts with other atoms in terms of attracting shared electrons in bonds. Understanding electronegativity helps predict bonding behavior and the polarity