Which of the following halogens has the highest electronegativity?

Electronegativity is the ability of an atom to attract electrons in a chemical bond. Among halogens, the electronegativity values vary according to their position in the periodic table. Fluorine has the highest electronegativity of all elements, with a value of 3.98 on the Pauling scale. This is due to its small atomic size, high nuclear charge, and strong attraction for bonding electrons.

Chlorine, bromine, and iodine are below fluorine in Group 17 of the periodic table. Electronegativity decreases down the group because the atomic size increases, and the bonding electrons are farther from the nucleus. Therefore, the electronegativity order for the halogens is:

F > Cl > Br > I

Fluorine’s extremely high electronegativity makes it highly reactive and a strong oxidizing agent. It forms strong bonds with most elements and can even oxidize other halogens under suitable conditions. Its small atomic radius and strong effective nuclear charge allow it to attract shared electrons more effectively than chlorine, bromine, or iodine.

Chlorine is the second most electronegative halogen, followed by bromine and iodine. This trend explains many chemical properties of halogens, including bond strengths, acid strengths of hydrogen halides, and reactivity in halogen displacement reactions.

Understanding electronegativity trends among halogens is crucial in inorganic chemistry to predict chemical behavior, bond polarity, and molecular properties. In summary, fluorine has the highest electronegativity among halogens due to its small size and strong nuclear attraction, making it the most reactive and strongly electron-attracting halogen in the periodic table