Lithium (fraeGreek:λίθος,romanised:lithos,lit.'stane') is achemical element wi the seembolLi anatomic nummer3. It is a saft, siller-whitemetal belangin tae thealkali metal group o chemical elements. Unner staundart condeetions, it is the lichtest metal annthe lichtest solit element. Lik aw alkali metals, lithium is heichly reactive an flammable, an is stored in mineral ile. Whan cut, it exhibits a metallic luster, but wet air corrodes it swift-like tae a dull sillery gray, then black tarnish. It niver occurs freely in naitur, but juist in (uisually ionic) compoonds, sic as pegmatitic minerals, that war ance the main soorce o lithium. Due tae its solubility as an ion, it is present in ocean watter an is commonly taen frae brines. Lithium metal is isolatit electrolytically frae a mixtur o lithium chloride an potassium chloride.[citation needit]
Thenucleus o the lithium atom verges on instability, as the twa stable lithiumisotope fund in nature hae amang the lawest bindin energies per nucleon o aw stable nuclides. Fae its relative nuclear instability, lithium is less common in the solar seestem nor 25 o the first 32 chemical elements even tho its nuclei are verra li ht: it is an exception tae the trend that hivier nuclei are less common.[1] For relatit raisons, lithium haes important uises innuclear physics. The transmutation o lithium atoms taehelium in 1932 wis the first fully man-made nuclear reaction, an lithium deuteride serves as afusion fuel in staged thermonuclear wappens.[2]
Lithium an its compoonds hae twa three industrial applications, includin heat-resistant gless anceramics, lithium grease lubricants, flux additives for airn, steel an aluminium production, lithium batteries, anlithium-ion batteries. The uises consume mair nor three quarter o lithium production.[citation needit]
Lithium battery
Lithium is seen in biological seestems in trace amoonts; its functions arenae confirmed. Lithium salts hae pruiven tae be uisefu as a drug in the treatment furbipolar disorder in humans.[citation needit]
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