It describes the stoichiometry of some chemical reactions in which one element or ligand is replaced by an atom or group.

are usually aqueous compounds (or very rarely in a molten state) and

Here is a condensed version of the same:[1] Similarly, the halogens with the highest propensity to acquire electrons are the most reactive.

The activity series for halogens is: [1][2][3] Due to the free state nature of

Here one cation replaces another: (Element A has replaced B in compound BC to become a new compound AC and the free element B.)

Some examples are: These reactions are exothermic and the rise in temperature is usually in the order of the reactivity of the different metals.

[5] If the reactant in elemental form is not the more reactive metal, then no reaction will occur.

Here one anion replaces another: (Element A has replaced B in the compound CB to form a new compound CA and the free element B.)

Again, the less reactive halogen cannot replace the more reactive halogen: Metals react with acids to form salts and hydrogen gas.

However, less reactive metals cannot displace the hydrogen from acids.

The metal oxides further dissolve in water to form alkalies.

The reaction can be extremely violent with alkali metals as the hydrogen gas catches fire.

[2] Metals like gold and silver, which are below hydrogen in the reactivity series, do not react with water.

Coke or more reactive metals are used to reduce metals by carbon from their metal oxides,[6] such as in the carbothermic reaction of zinc oxide (zincite) to produce zinc metal: and the use of aluminium to produce manganese from manganese dioxide: Such reactions are also used in extraction of boron, silicon, titanium and tungsten.

Using highly reactive metals as reducing agents leads to exothermic reactions that melt the metal produced.

[6] a(Haematite) Silver tarnishes due to the presence of hydrogen sulfide, leading to formation of silver sulfide.

[7][2] Chlorine is manufactured industrially by the Deacon's process.

The reaction takes place at about 400 to 450 °C in the presence of a variety of catalysts such as

Bromine and iodine are extracted from brine by displacing with chlorine.

Reactivity series by RSC Halogen displacement reaction by RSC Chlorine water reacting with Iodide and Bromide, YouTube