Untitled Quiz

Reactivity of halogens decreases down the group. Stronger oxidising agents displace weaker ones.

Halogens' ability to gain electrons. Chlorine is a stronger oxidising agent than bromine, which is stronger than iodine.

A stronger halogen displaces a weaker halogen from a compound.

The ability of an atom to attract electrons in a covalent bond.

Melting and boiling points increase down the group due to increasing van der Waals forces.

Weak intermolecular forces between molecules caused by temporary dipoles.

Ions formed from halogens by gaining an electron; e.g., Cl⁻.

Different colours reveal the presence of particular free halogens (colour of solution indicates specific halogen).

Reactions between chlorine, bromine, and iodine in solution with potassium halide ions (bromide and iodide). These reactions show how reactivity increases down the group.

Halogens (Cl2, Br2, I2) can act as oxidizing agents; they accept electrons and are reduced. This is demonstrated by chlorine displacing bromine and iodine from potassium bromide and potassium iodide solutions.

Chlorine displaces bromine and iodine, bromine displaces iodine. This shows reactivity trends down the halogen group. A more reactive halogen will displace a less reactive one!

Adding silver nitrate to an acidic solution of halide ions produces different coloured precipitates based on the halide ion present. Nitric acid is used to remove carbonate interference.

Nitric acid is added to remove carbonate ions, preventing the formation of a silver carbonate precipitate that would interfere with the silver halide precipitations.

H2SO4 acts as a proton donor (acid) in reactions with metal halides, producing hydrogen halide gases.

Bromide (Br⁻) ions are stronger reducing agents than chloride (Cl⁻) or fluoride (F⁻) ions, meaning they readily lose electrons.

H2SO4, in the presence of bromide or iodide ions, can act as an oxidizing agent in reducing the sulfur from +6 to +4 oxidation state.

Iodide ions (I⁻) are the strongest reducing agents among the halides, capable of reducing H2SO4 to various oxidation products, like sulfur.

2NaBr + 3H2SO4 → 2NaHSO4 + SO2 + Br2 + 2H2O

The color of the precipitate formed when silver ions react with halide ions (Cl-, Br-, I-).

Concentrated ammonia dissolves silver bromide, dilute ammonia dissolves silver chloride, and silver iodide does not dissolve in ammonia.

The ability of halide ions (F-, Cl-, Br-, I-) to donate electrons, increasing down the group.

Fluoride and Chloride ions react with sulfuric acid via acid-base reactions, not redox reactions.

A substance that donates electrons in a chemical reaction.

A chemical reaction where an acid and a base neutralize each other.

A chemical reaction involving the transfer of electrons between reactants.

Formation of white steamy fumes of hydrogen fluoride (HF) gas during the reaction of fluoride with sulfuric acid.

A chemical reaction involving both oxidation and reduction. H2SO4, acts as both acid and oxidizing agent, oxidizing iodine and reducing itself to SO2, S, or H2S.

A reaction where a single substance is both oxidized and reduced.

Chlorine gas reacts with water to produce hypochlorous acid (HClO) and hydrochloric acid (HCl).

Chlorine is used to kill bacteria in water treatment systems.

The process where a substance loses electrons.

The process where a substance gains electrons.

A gas (H₂S) with a characteristic foul smell like rotten eggs

A colorless gas (SO2) containing sulfur.