Editing Lithium (section)

=== Of lithium metal ===
Lithium reacts with water easily, but with noticeably less vigor than other alkali metals. The reaction forms [[hydrogen]] gas and [[lithium hydroxide]].<ref name="krebs" /> When placed over a flame, lithium compounds give off a striking crimson color, but when the metal burns strongly, the flame becomes a brilliant silver. Lithium will ignite and burn in oxygen when exposed to water or water vapor. In moist air, lithium rapidly tarnishes to form a black coating of [[lithium hydroxide]] (LiOH and LiOH·H<sub>2</sub>O), [[lithium nitride]] (Li<sub>3</sub>N) and [[lithium carbonate]] (Li<sub>2</sub>CO<sub>3</sub>, the result of a secondary reaction between LiOH and [[carbon dioxide|CO<sub>2</sub>]]).<ref name="kamienski" /> Lithium is one of the few metals that react with [[nitrogen]] gas.<ref>{{cite book |page=47 |url={{google books |plainurl=y |id=yb9xTj72vNAC |page=47}} |title=The history and use of our earth's chemical elements: a reference guide |author=Krebs, Robert E. |publisher=Greenwood Publishing Group |date=2006 |isbn=978-0-313-33438-2 |url-status=live |archive-url=https://web.archive.org/web/20160804025424/https://books.google.com/books?id=yb9xTj72vNAC&pg=PA47 |archive-date=4 August 2016}}</ref><ref>{{Cite journal |author1=Institute, American Geological |author2=Union, American Geophysical |author3=Society, Geochemical |title=Geochemistry international |volume=31 |issue=1–4 |page=115 |date=1 January 1994 |url={{google books |plainurl=y |id=77McAQAAIAAJ}} |url-status=live |archive-url=https://web.archive.org/web/20160604195805/https://books.google.com/books?id=77McAQAAIAAJ |archive-date=4 June 2016 |website=Google Books}}</ref>

Because of its reactivity with water, and especially nitrogen, lithium metal is usually stored in a hydrocarbon sealant, often [[petroleum jelly]]. Although the heavier alkali metals can be stored under [[mineral oil]], lithium is not dense enough to fully submerge itself in these liquids.<ref name="emsley" />

Lithium has a [[diagonal relationship]] with [[magnesium]], an element of similar atomic and [[ionic radius]]. Chemical resemblances between the two metals include the formation of a [[nitride]] by reaction with N<sub>2</sub>, the formation of an [[lithium oxide|oxide]] ({{chem|Li|2|O}}) and peroxide ({{chem|Li|2|O|2}}) when burnt in O<sub>2</sub>, [[salt (chemistry)|salts]] with similar [[solubility|solubilities]], and thermal instability of the [[carbonate]]s and nitrides.<ref name="kamienski">{{Cite book |first=Conrad W. |last=Kamienski |author2=McDonald, Daniel P. |author3=Stark, Marshall W. |author4=Papcun, John R. |chapter=Lithium and lithium compounds |title=Kirk-Othmer Encyclopedia of Chemical Technology |publisher=John Wiley & Sons, Inc. |date=2004 |doi=10.1002/0471238961.1209200811011309.a01.pub2 |isbn=978-0-471-23896-6}}</ref><ref name="Greenwood">{{Greenwood&Earnshaw1st|pages=97–99}}</ref> The metal reacts with hydrogen gas at high temperatures to produce [[lithium hydride]] (LiH).<ref>{{cite web |url=http://www.lyon.edu/webdata/users/fbeckford/CHM%20120/Lecture%20Notes/Chapter-14.ppt |archive-url=https://web.archive.org/web/20051104025202/http://www.lyon.edu/webdata/users/fbeckford/CHM%20120/Lecture%20Notes/Chapter-14.ppt |archive-date=4 November 2005 |title=University of Lyon course online (powerpoint) slideshow |access-date=27 July 2008 |author=Beckford, Floyd |quote=definitions:Slides 8–10 (Chapter 14)}}</ref>

Lithium forms a variety of binary and ternary materials by direct reaction with the main group elements. These [[Zintl phase]]s, although highly covalent, can be viewed as salts of polyatomic anions such as Si<sub>4</sub><sup>4-</sup>, P<sub>7</sub><sup>3-</sup>, and Te<sub>5</sub><sup>2-</sup>.  With graphite, lithium forms a variety of [[intercalation compound]]s.<ref name="Greenwood" />

It dissolves in ammonia (and amines) to give [Li(NH<sub>3</sub>)<sub>4</sub>]<sup>+</sup> and the [[solvated electron]].<ref name="Greenwood" />