Yes, lithium is reactive.
Lithium, as a member of the Group 1 Alkali Metals, exhibits high reactivity. This is primarily due to its electronic configuration: it possesses a single valence electron that is readily donated to form chemical bonds and stable compounds. This propensity to lose its valence electron drives its reactivity.
Factors Contributing to Lithium's Reactivity:
- Single Valence Electron: Lithium's outermost shell contains only one electron, which it readily gives up to achieve a more stable electron configuration.
- Low Ionization Energy: The energy required to remove this single electron (ionization energy) is relatively low compared to other elements, making it easier for lithium to participate in chemical reactions.
- Strong Reducing Agent: Due to its ability to easily donate an electron, lithium acts as a strong reducing agent.
Examples of Lithium's Reactivity:
- Reaction with Water: Lithium reacts with water, though less vigorously than sodium or potassium, to produce lithium hydroxide and hydrogen gas:
2Li(s) + 2H₂O(l) → 2LiOH(aq) + H₂(g) - Reaction with Air: Lithium tarnishes in air, forming lithium oxide and lithium nitride. Therefore, it is often stored under oil.
- Formation of Compounds: Lithium readily forms a variety of compounds with other elements, such as lithium chloride (LiCl), lithium fluoride (LiF), and lithium carbonate (Li₂CO₃).
Why Lithium is Never Found in its Pure Form in Nature:
Because of its high reactivity, lithium is never found in its pure, elemental form in nature. It is always found in compounds, having already reacted with other elements in the environment.
In conclusion, lithium's high reactivity, driven by its electronic structure, explains why it is not found in its pure form in nature and readily forms compounds with other elements.
