What is the general chemical reactivity of metals?

Metals generally react by losing electrons to form positive ions, often reacting with non-metals or acids.

In more detail, metals are known for their ability to donate electrons in chemical reactions, a process known as oxidation. This is due to the relatively low ionisation energy of metals, which means they can easily lose electrons to achieve a stable electron configuration. When a metal atom loses electrons, it forms a positive ion, also known as a cation. This is the basis of the general chemical reactivity of metals.

The reactivity of metals can vary greatly. Some metals, like potassium and sodium, are very reactive and can react violently with water or air. These metals are stored under oil to prevent them from coming into contact with moisture in the air. On the other hand, metals like gold and platinum are very unreactive and do not easily form positive ions.

Metals often react with non-metals to form ionic compounds. In these reactions, the metal atom donates electrons to the non-metal atom, resulting in the formation of a positive metal ion and a negative non-metal ion. These oppositely charged ions are then attracted to each other, forming an ionic bond.

Another common reaction of metals is with acids. Metals can react with acids to produce a salt and hydrogen gas. This is a redox reaction, where the metal is oxidised (loses electrons) and the hydrogen in the acid is reduced (gains electrons).

In summary, the general chemical reactivity of metals involves the loss of electrons to form positive ions, with the specific reactions and reactivity levels varying between different metals.