Metals with high reactivity, such as potassium, sodium and calcium, react with cold water producing a metal hydroxide and hydrogen gas.

Less reactive metals, like magnesium, react only with steam to form metal oxide and hydrogen gas.

Metals such as copper, gold, and silver do not react with water at all since they are very unreactive.

Reactivity series of metals is a list of metals that starts with the most reactive metal at the top and the least reactive at the bottom. The order is potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, lead, copper, silver, gold and platinum.

Displacement reactions occur when a more reactive metal displaces a less reactive metal from its compound.

During a displacement reaction, the more reactive metal tends to lose electrons (oxidation) and the less reactive metal gains those electrons (reduction). This phenomenon is also known as redox reaction

The reactivity of a metal can be determined by its willingness to lose electrons and form positive ions.

Metal oxides are basic in nature; they react with acids to form salt and water, a neutralisation reaction. For instance, copper oxide reacts with hydrochloric acid to form copper chloride and water.

The metallic oxides of the highly reactive metals like sodium and potassium are alkaline and dissolve in water to give alkalis.

When metal carbonates react with acid, they produce a salt, water, and carbon dioxide.

Some metals, like zinc and iron, can react with both acids and bases and are called amphoteric metals.

The extraction of metals from their ores depends on the reactivity of the metal. Highly reactive metals are extracted by electrolysis, moderately reactive metals are extracted by reduction using carbon, while unreactive metals are found as uncombined elements in the earth.

Corrosion is a natural process that converts a refined metal into a more chemically stable form such as oxide, hydroxide, or sulphide. Iron rusts when it comes in contact with moist air, forming iron (III) oxide.

Metallic bonding is the strong attraction between positively charged metal ions and the sea of delocalized electrons surrounding them.

The tendency of a metal to displace hydrogen from acids is known as the reactivity of metals.

Alloys are mixtures of two or more metals. They are formed to improve the properties of metals. For example, steel is an alloy of iron and a small amount of carbon, which makes it stronger and more flexible than pure iron.

Learn to predict the products of the reactions between metals and acids, water, and oxygen.

Understanding the reactivity series of metals, displacement reactions, and simple electrolysis can help in understanding the extraction of metals and their reactivity.

Regular practise of questions and problems based on reactions of metals will enhance knowledge and application skills.