Which halogen can displace all the other halogens from their compounds?

Halogens are elements in Group 17 of the periodic table, including fluorine (F₂), chlorine (Cl₂), bromine (Br₂), and iodine (I₂). They show similar chemical behavior but differ in reactivity. Reactivity of halogens decreases down the group: fluorine > chlorine > bromine > iodine.

Displacement reactions involve a more reactive halogen displacing a less reactive halogen from its compound. Fluorine, being the most reactive halogen due to its high electronegativity and strong oxidizing ability, can displace chlorine, bromine, and iodine from their halide salts. For example, fluorine reacts with sodium chloride (NaCl) to produce sodium fluoride (NaF) and chlorine gas.

Chlorine can displace bromine and iodine but cannot displace fluorine. Bromine can displace iodine only. Iodine is the least reactive halogen and cannot displace any other halogen from its compounds.

This trend in halogen reactivity is caused by the atomic size and electron affinity. Fluorine has a small atomic radius and a high tendency to gain an electron, making it a powerful oxidizing agent. Its strong ability to attract electrons allows it to break bonds of less reactive halogen compounds and replace them.

Understanding halogen displacement reactions is important in inorganic chemistry, especially in predicting chemical behavior, redox reactions, and industrial applications. Fluorine’s exceptional reactivity makes it useful in producing fluorine-containing compounds, including polymers, refrigerants, and pharmaceuticals.

This question emphasizes the reactivity trend of halogens and the role of fluorine as the most powerful halogen in chemical reactions.