When chlorine gas is bubbled through a solution of sodium chloride, a chemical reaction occurs, forming sodium hypochlorite and sodium chloride: One example is the reaction between chlorine and sodium. The word halogen comes from the Greek words "hal" or "halo," meaning salt, and "gen," meaning to produce. As we move down the group, the reactivity decreases, and the reactions become less vigorous. Sure! The reactions between halogens and metals also form salts and are redox reactions. It's important to note that the reversibility of this reaction is due to the weaker oxidizing power of iodine compared to fluorine. This means that the reaction can go in both directions, and the products can react to form the reactants again. However, when iodine reacts with hydrogen, the reaction is only partial, and an equilibrium is formed. In this reaction, hydrogen is oxidized and loses electrons, while fluorine is reduced and gains electrons. In this reaction, the halogens act as oxidizing agents, and their reactivity decreases as you move down the group.įor example, when fluorine reacts with hydrogen, it does so explosively, forming hydrogen fluoride gas. Remember that halogens become less reactive as you move down the periodic table, so chlorine is more reactive than bromine in this case.Īnother example of a redox reaction involving halogens is when they react with hydrogen to form hydrogen halides, such as HX. For example, if you add chlorine to a sodium bromide solution, chlorine would displace bromine since it's more reactive. The halogen atoms then gain electrons to form halide ions, which are reduced. In a displacement reaction, the more reactive halogen atoms oxidise the less reactive halide ions, causing the halide ions to lose electrons and form halogen atoms. This occurs when a more reactive halogen replaces a less reactive halide in a compound. Let's take a closer look at one type of reaction that involves halogens - a displacement reaction. In fact, fluorine is one of the most potent oxidising agents out there! To recap redox reactions, check out Redox. In general, the oxidising power of the halogens decreases as you go down the group. Compare Standard and Premium Digital here.Īny changes made can be done at any time and will become effective at the end of the trial period, allowing you to retain full access for 4 weeks, even if you downgrade or cancel.This means that an oxidising agent takes electrons from another species and gains them itself. You may also opt to downgrade to Standard Digital, a robust journalistic offering that fulfils many user’s needs. If you’d like to retain your premium access and save 20%, you can opt to pay annually at the end of the trial. If you do nothing, you will be auto-enrolled in our premium digital monthly subscription plan and retain complete access for $69 per month.įor cost savings, you can change your plan at any time online in the “Settings & Account” section. For a full comparison of Standard and Premium Digital, click here.Ĭhange the plan you will roll onto at any time during your trial by visiting the “Settings & Account” section. Premium Digital includes access to our premier business column, Lex, as well as 15 curated newsletters covering key business themes with original, in-depth reporting. Standard Digital includes access to a wealth of global news, analysis and expert opinion. During your trial you will have complete digital access to FT.com with everything in both of our Standard Digital and Premium Digital packages.
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