kalium

Kalium, the Latin name for the chemical element potassium, is a soft, silvery‑white alkali metal with the symbol K and atomic number 19. It belongs to group 1 of the periodic table and is the seventh most abundant element in the Earth’s crust, occurring primarily in minerals such as feldspar, sylvite, and carnallite. In its elemental form, kalium reacts vigorously with water, producing hydrogen gas and a strongly alkaline solution of potassium hydroxide.

Physically, kalium has a low melting point of 63.5 °C and a boiling point of 759 °C, making it liquid near room temperature under certain conditions. Its high electrochemical potential renders it an excellent reducing agent and a key component in many industrial processes. The metal is harvested mainly by electrolytic reduction of potassium chloride derived from evaporite deposits.

Biologically, kalium ions are essential electrolytes in all living cells. They maintain osmotic balance, regulate nerve impulse transmission, and are crucial for muscle contraction, including cardiac function. The human body typically contains about 2.5 g of potassium, predominantly in the intracellular fluid. Dietary sources such as bananas, potatoes, and legumes supply the element, and deficiencies can lead to hypokalemia, while excess intake may cause hyperkalemia, both of which have serious health implications.

Industrially, kalium compounds are employed in the manufacture of fertilizers (potash), glass, soaps, and in the production of high‑energy batteries, especially alkaline and lithium‑ion types. Its isotopes, notably ^40K, are used for radiometric dating in geology and archaeology. The element’s reactivity, biological importance, and versatile applications make kalium a cornerstone of both natural processes and modern technology.