kaliums

Kaliums refers to the chemical element potassium in some Latin-based naming conventions. In contemporary chemistry, the element is commonly known as potassium (symbol K, atomic number 19). The name Kalium is the Latin origin of potassium, and the symbol K derives from kalium. In English-language usage, potassium and its compounds are the standard terms, while Kalium appears in historical or specialized scientific contexts.

Kalium is an alkali metal in group 1 of the periodic table. It is a soft, silvery-white metal that oxidizes rapidly in air and reacts vigorously with water to form potassium hydroxide and hydrogen gas. It is highly reactive and must be stored under oil or in an inert atmosphere to prevent tarnishing and reaction with moisture. The element has several isotopes, of which potassium-40 is naturally occurring and radioactive.

Occurrence and production: Potassium is the seventh most abundant element in the Earth's crust. It occurs mainly in minerals such as sylvite (KCl) and carnallite, and in seawater. Industrial production centers on mining potash deposits and processing the salts to produce compounds like potassium chloride (KCl) and potassium sulfate (K2SO4) for fertilizer. Potassium metal, less common in commerce, is produced by electrolysis of fused salts, typically potassium chloride.

Uses and biological role: The largest use of potassium compounds is in agriculture as potash fertilizers, which help regulate plant water balance and nutrient uptake. Potassium salts also serve in glassmaking, ceramics, and various industrial processes. Biologically, potassium is an essential electrolyte, critical for nerve impulses, muscle function, and fluid balance. Diets typically obtain potassium from fruits, vegetables, and dairy products.

Safety: Potassium metal is highly reactive with water and air, requiring careful handling. Compounds are generally safe when used as directed, but excessive intake can lead to hyperkalemia, particularly in individuals with kidney impairment.