Active Metal
Definition and meaning of Active Metal in chemistry.
An active metal is a metal that readily loses electrons to form positive ions and readily reacts with other substances. Active metals are typically found on the left side of the periodic table and display high chemical reactivity.
In more detail
Active metals have low ionization energies and low electronegativities, making them highly reactive with water, oxygen, and acids. When they react, they often release hydrogen gas or heat. Reactivity increases as you move down a group in the periodic table. The alkali metals (Group 1) and alkaline earth metals (Group 2) are the most active metals.
Key facts
| Location | Left side of the periodic table |
|---|---|
| Key Property | Low ionization energy; readily loses electrons |
| Common Examples | Sodium (Na), potassium (K), calcium (Ca), magnesium (Mg) |
| Field | Inorganic Chemistry |
Sodium (Na) is a highly active metal that reacts vigorously with water to produce sodium hydroxide (NaOH) and hydrogen gas (H2), releasing significant heat in the process.
Frequently asked questions
Why are active metals so reactive?
Active metals have low ionization energies, requiring minimal energy to remove electrons from their outer shells, making them eager to lose electrons and form cations.
How do active metals differ from transition metals?
Active metals (mainly Groups 1-2) readily lose electrons and form stable cations, while transition metals have variable oxidation states and are less reactive overall.