Acetylide

In chemistry, an acetylide is a compound that can be viewed as the result of replacing one or both hydrogen atoms of acetylene (ethyne) Template:Chem2 by metallic or other cations. Calcium carbide is an important industrial compound, which has long been used to produce acetylene for welding and illumination. It is also a major precursor to vinyl chloride.<ref name=Ullmann/> Other acetylides are reagents in organic synthesis.

Nomenclature

The term acetylide is used loosely. It apply to an acetylene Template:Chem2, where R = H or a side chain that is usually organic.<ref name="IUPAC">Template:GoldBookRef</ref> The nomenclature can be ambiguous with regards to the distinction between compounds of the type Template:Chem2 and Template:Chem2. When both hydrogens of acetylene are replaced by metals, the compound can also be called carbide, e.g. calcium carbide Template:Chem2, which is calcium acetylide. When only one hydrogen atom is replaced, the anion may be called hydrogen acetylide or the prefix mono- may be attached to the metal, as in monosodium acetylide or sodium hydrogen acetylide, Template:Chem2. An acetylide may be a salt (ionic compound) containing the anion Template:Chem2, Template:Chem2, or Template:Chem2, as in disodium acetylide Template:Chem2 or cobalt(II) acetylide Template:Chem2.<ref name=nish2005>Junichi Nishijo, Kentaroh Kosugi, Hiroshi Sawa, Chie Okabe, Ken Judai, Nobuyuki Nishi (2005): "Water-induced ferromagnetism in cobalt acetylide CoC2 nanoparticles". Polyhedron, volume 24, issues 16–17, pages 2148-2152. {{#invoke:doi|main}}</ref> Other acetylides have the metal bound to the carbon atom(s) by covalent bonds, being therefore coordination or organometallic compounds.

Alkali and alkaline earth acetylides

Alkali metal and alkaline earth metal acetylides have the general formula Template:Chem2 (M = Li, Na, K, etc) and Template:Chem2 (M' = Mg, Ca, etc).They are sometimes represented as Template:Chem2 and Template:Chem2, but they are covalent compounds. Rather than salt-like, they can be considered Zintl phase compounds, containing Template:Chem2 ions, with a triple bond between the two carbon atoms. They undergo ready hydrolysisto form acetylene and metal oxides. Their solutions in ammonia are proposed to contain solvated Template:Chem2 ions.<ref>Template:Cite journal</ref>

The Template:Chem2 ion has a closed shell ground state of ¹ΣTemplate:Su, making it isoelectronic to a neutral molecule Template:Chem2, which may afford it some gas-phase stability.<ref>Template:Cite journal</ref>

Organometallic acetylides

Some acetylides, particularly of transition metals, show evidences of covalent character, e. g. for being neither dissolved nor decomposed by water and by radically different chemical reactions. That seems to be the case of silver acetylide and copper acetylide, for example.

In the absence of additional ligands, metal acetylides adopt polymeric structures wherein the acetylide groups are bridging ligands.

• Na2C2structure.jpg

  Structure of sodium acetylide Template:Chem2.<ref>Template:Cite journal</ref> Color code: gray = C, blue = Na.

• K2C2 unit cell.png

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• XAPGIF2.png

  Portion of the structure of the polymer copper(I) phenylacetylide Template:Chem2.<ref>Template:Cite journal</ref>

• CAMNEJ.svg

  Structure of the cluster formed from Template:Chem2 complexed to N,N,N′,N′-tetramethyl-1,6-diaminohexane (methylene groups omitted for clarity). Color key: turquoise = Li, blue = N.<ref>Template:Cite journal</ref>

Preparation

Of the type Template:Chem2

Acetylene and terminal alkynes are weak acids:<ref name=Viehe>Template:Cite journal</ref>

Template:Chem2

Monopotassium and monosodium acetylide can be prepared by reacting acetylene with bases like sodium amide<ref name=Coffman /> or with the elemental metals, often at room temperature and atmospheric pressure.<ref name=Viehe /> Copper(I) acetylide can be prepared by passing acetylene through an aqueous solution of copper(I) chloride because of a low solubility equilibrium.<ref name=Viehe /> Similarly, silver acetylides can be obtained from silver nitrate.

In organic synthesis, acetylides are usually prepared by treating acetylene and alkynes with organometallic<ref name=Midland1990>Template:Cite journal</ref> or inorganic<ref name=Coffman>Template:Cite journal</ref> Classically, liquid ammonia was used for deprotonations, but ethers are now more commonly used.

Lithium amide,<ref name=Viehe /> LiHMDS,<ref name="Reich2001">Template:Cite journal</ref> or organolithium reagents, such as butyllithium (Template:Chem2),<ref name=Midland1990 /> are frequently used to form lithium acetylides:

Template:Chem2

Of the type Template:Chem2 and Template:Chem2

Calcium carbide is prepared industrially by heating carbon with lime (calcium oxide) at approximately 2,000 °C.<ref name=Ullmann>Template:Cite book</ref> A similar process can be used to produce lithium carbide.

Dilithium acetylide, Template:Chem2, competes with the preparation of the monolithium derivative Template:Chem2.<ref name=Coffman/>

Reactions

Ionic acetylides are typically decomposed by water with evolution of acetylene:

Template:Chem2

Template:Chem2

Acetylides of the type Template:Chem2 are widely used in alkynylations in organic chemistry. They are nucleophiles that add to a variety of electrophilic and unsaturated substrates.

A classic application is the Favorskii reaction, such as in the sequence shown below. Here ethyl propiolate is deprotonated by n-butyllithium to give the corresponding lithium acetylide. This acetylide adds to the carbonyl center of cyclopentanone. Hydrolysis liberates the alkynyl alcohol.<ref>Template:Cite journal</ref>

Reaction of ethyl propiolate with n-butyllithium to form the lithium acetylide.

The dimerization of acetylene to vinylacetylene proceeds by insertion of acetylene into a copper(I) acetylide complex.<ref>Template:Cite journal</ref>

Coupling reactions

Acetylides are sometimes used as intermediates in coupling reactions. Examples include Sonogashira coupling, Cadiot-Chodkiewicz coupling, Glaser coupling and Eglinton coupling.

Hazards

Some acetylides are notoriously explosive.<ref name="CataldoCasari2007">Template:Cite journal</ref> Formation of acetylides poses a risk in handling of gaseous acetylene in presence of metals such as mercury, silver or copper, or alloys with their high content (brass, bronze, silver solder).

See also

• Sodium hydrogen acetylide
• Calcium acetylide
• Strontium acetylide
• Barium acetylide
• Copper(I) acetylide
• Silver(I) acetylide
• Ethynyl
• Ethynyl radical
• Diatomic carbon (neutral C₂)
• Acetylenediol