Hydride - wikipedia Hydride In chemistry, a hydride is the anion of hydrogen, H, or, more commonly, it is a compound in which one or more hydrogen centres have nucleophilic, reducing, or basic properties. In compounds that are regarded as hydrides, the hydrogen atom is bonded to a more electropositive element or group. Compounds containing hydrogen bonded to metals or metalloid may also be referred to as hydrides. Almost all of the elements form binary compounds with hydrogen, the exceptions being He, Ne, Ar, Kr, Pm, Os, Ir, Rn, Fr, and Ra. Contents 1 Bonds 2 Applications 3 Hydride ion 4 Types of hydrides 4.1 Ionic hydrides 4.2 Covalent hydrides 4.3 Interstitial hydrides or metallic hydrides 4.4 Transition metal hydride complexes 4.5 Deuterides 5 Appendix on nomenclature 5.1 Precedence convention 6 See also 7 References 8 Bibliography 9 External links Bonds Bonds between hydrogen and other elements range from highly to somewhat covalent. Some hydrides, e.g. boron hydrides, do not conform to classical electron - counting rules, and the bonding is described in terms of multi-centered bonds, whereas the interstitial hydrides often involve metallic bonding. Hydrides can be discrete molecules, oligomers or polymers, ionic solids, chemisorbed monolayers, bulk metals ( interstitial ), and other materials. While hydrides traditionally react as Lewis bases or reducing agents, some metal hydrides behave as hydrogen - atom donors and act as acids. Applications Hydrides such as sodium borohydride, lithium aluminium hydride, diisobutylaluminium hydride ( DIBAL ) and super hydride, are commonly used as reducing agents in chemical synthesis. The hydride adds to an electrophilic center, typically unsaturated carbon. Hydrides such as sodium hydride and potassium hydride are used as strong bases in organic synthesis. The hydride reacts with the weak Bronsted acid releasing H. Hydrides such as calcium hydride are used as desiccants, i.e. drying agents, to remove trace water from organic solvents. The hydride reacts with water forming hydrogen and hydroxide salt. The dry solvent can then be distilled or vac transferred from the `` solvent pot ''. Hydrides are important in storage battery technologies such as nickel - metal hydride battery. Various metal hydrides have been examined for use as a means of hydrogen storage for fuel cell - powered electric cars and other purposed aspects of a hydrogen economy. Hydride complexes are catalysts and catalytic intermediates in a variety of homogeneous and heterogeneous catalytic cycles. Important examples include hydrogenation, hydroformylation, hydrosilylation, hydrodesulfurization catalysts. Even certain enzymes, the hydrogenase, operate via hydride intermediates. The energy carrier Nicotinamide adenine dinucleotide reacts as a hydride donor or hydride equivalent. Hydride ion See also : Hydrogen anion Free hydride anions exist only under extreme conditions and are not invoked for homogeneous solution. Instead, many compounds have hydrogen centres with hydridic character. Aside from electride, the hydride ion is the simplest possible anion, consisting of two electrons and a proton. Hydrogen has a relatively low electron affinity, 72.77 kJ / mol and reacts exothermically with protons as a powerful Lewis base. H + H → H ; ΔH = − 1676 kJ / mol The low electron affinity of hydrogen and the strength of the H -- H bond ( ∆ H = 436 kJ / mol ) means that the hydride ion would also be a strong reducing agent H + 2e ⇌ 2H ; E = − 2.25 V Types of hydrides According to the general definition every element of the periodic table ( except some noble gases ) forms one or more hydrides. These substances have been classified into three main types according to the nature of their bonding : Ionic hydrides, which have significant ionic bonding character. Covalent hydrides, which include the hydrocarbons and many other compounds which covalently bond to hydrogen atoms. Interstitial hydrides, which may be described as having metallic bonding. While these divisions have not been used universally, they are still useful to understand differences in hydrides. Ionic hydrides Ionic or saline hydrides are composed of hydride bound to an electropositive metal, generally an alkali metal or alkaline earth metal. The divalent lanthanides such as europium and ytterbium form compounds similar to those of heavier alkali metal. In these materials the hydride is viewed as a pseudohalide. Saline hydrides are insoluble in conventional solvents, reflecting their non-molecular structures. Ionic hydrides are used as bases and, occasionally, as reducing reagents in organic synthesis. C H C ( O ) CH + KH → C H C ( O ) CH K + H Typical solvents for such reactions are ethers. Water and other protic solvents can not serve as a medium for ionic hydrides because the hydride ion is a stronger base than hydroxide and most hydroxyl anions. Hydrogen gas is liberated in a typical acid - base reaction. NaH + H O → H ( g ) + NaOH ΔH = − 83.6 kJ / mol, ΔG = − 109.0 kJ / mol Often alkali metal hydrides react with metal halides. Lithium aluminium hydride ( often abbreviated as LAH ) arises from reactions of lithium hydride with aluminium chloride. 4 LiH + AlCl → LiAlH + 3 LiCl Covalent hydrides According to some definitions, covalent hydrides cover all other compounds containing hydrogen. Some definitions limit hydrides to hydrogen centres that formally react as hydrides, i.e. are nucleophilic, and hydrogen atoms bound to metal centers. These hydrides are formed by all the true non-metals ( except zero group elements ) and the elements like Al, Ga, Sn, Pb, Bi, Po, etc., which are normally metallic in nature, i.e., this class includes the hydrides of p - block elements. In these substances the hydride bond is formally a covalent bond much like the bond made by a proton in a weak acid. This category includes hydrides that exist as discrete molecules, polymers or oligomers, and hydrogen that has been chem - adsorbed to a surface. A particularly important segment of covalent hydrides are complex metal hydrides, powerful soluble hydrides commonly used in synthetic procedures. Molecular hydrides often involve additional ligands such as, diisobutylaluminium hydride ( DIBAL ) consists of two aluminum centers bridged by hydride ligands. Hydrides that are soluble in common solvents are widely used in organic synthesis. Particularly common are sodium borohydride ( NaBH ) and lithium aluminium hydride and hindered reagents such as DIBAL. Interstitial hydrides or metallic hydrides Interstitial hydrides most commonly exist within metals or alloys. They are traditionally termed ' compounds ', even though they do not strictly conform to the definition of a compound ; more closely resembling common alloys such as steel. In such hydrides, hydrogen can exist as either atomic, or diatomic entities. Mechanical or thermal processing, such as bending, striking, or annealing may cause the hydrogen to precipitate out of solution, by degassing. Their bonding is generally considered metallic. Such bulk transition metals form interstitial binary hydrides when exposed to hydrogen. These systems are usually non-stoichiometric, with variable amounts of hydrogen atoms in the lattice. In materials engineering, the phenomenon of hydrogen embrittlement results from the formation of interstitial hydrides. Hydrides of this type form according to either one of two main mechanisms. The first mechanism involves the adsorption of dihydrogen, succeeded by the cleaving of the H-H bond, the delocalisation of the hydrogen 's electrons, and finally, the diffusion of the protons into the metal lattice. The other main mechanism involves the electrolytic reduction of ionised hydrogen on the surface of the metal lattice, also followed by the diffusion of the protons into the lattice. The second mechanism is responsible for the observed temporary volume expansion of certain electrodes used in electrolytic experiments. Palladium absorbs up to 900 times its own volume of hydrogen at room temperatures, forming palladium hydride. This material has been discussed as a means to carry hydrogen for vehicular fuel cells. Interstitial hydrides show certain promise as a way for safe hydrogen storage. During last 25 years many interstitial hydrides were developed that readily absorb and discharge hydrogen at room temperature and atmospheric pressure. They are usually based on intermetallic compounds and solid - solution alloys. However, their application is still limited, as they are capable of storing only about 2 weight percent of hydrogen, insufficient for automotive applications. Transition metal hydride complexes Main article : Transition metal hydride Transition metal hydrides include compounds that can be classified as covalent hydrides. Some are even classified as interstitial hydrides and other bridging hydrides. Classical transition metal hydride feature a single bond between the hydrogen centre and the transition metal. Some transition metal hydrides are acidic, e.g., HCo ( CO ) and H Fe ( CO ). The anions ( ReH ) and ( FeH ) are examples from the growing collection of known molecular homoleptic metal hydrides. As pseudohalides, hydride ligands are capable of bonding with positively polarized hydrogen centres. This interaction, called dihydrogen bond is similar to hydrogen bonding which exists between positively polarized protons and electronegative atoms with open lone pairs. Deuterides Hydrides containing deuterium are known as deuterides. Some deuterides, such as LiD, are important fusion fuels in thermonuclear weapons, and useful moderators in nuclear reactors. Appendix on nomenclature Protide, deuteride, and tritide are used to describe ions or compounds, which contain enriched hydrogen - 1, deuterium or tritium, respectively. In the classic meaning, hydride refers to any compounds hydrogen forms with other elements, ranging over groups 1 -- 16 ( the binary compounds of hydrogen ). The following is a list of the nomenclature for the hydride derivatives of main group compounds according to this definition : alkali and alkaline earth metals : metal hydride boron : borane, BH aluminium : alumane, AlH gallium : gallane, GaH indium : indigane, InH thallium : thallane, TlH carbon : alkanes, alkenes, alkynes, and all hydrocarbons silicon : silane germanium : germane tin : stannane lead : plumbane nitrogen : ammonia ( ' azane ' when substituted ), hydrazine phosphorus : phosphine ( note ' phosphane ' is the IUPAC recommended name ) arsenic : arsine ( note ' arsane ' is the IUPAC recommended name ) antimony : stibine ( note ' stibane ' is the IUPAC recommended name ) bismuth : bismuthine ( note ' bismuthane ' is the IUPAC recommended name ) helium : helium hydride ( only exists as an ion ) According to the convention above, the following are `` hydrogen compounds '' and not `` hydrides '' : oxygen : water ( ' oxidane ' when substituted ; synonym : oxygen hydride ), hydrogen peroxide sulfur : hydrogen sulfide ( ' sulfane ' when substituted ) synonym : sulfur hydride selenium : hydrogen selenide ( ' selane ' when substituted ) tellurium : hydrogen telluride ( ' tellane ' when substituted ) polonium : hydrogen polonide ( ' polane ' when substituted ) halogens : hydrogen halides Examples : nickel hydride : used in NiMH batteries palladium hydride : electrodes in cold fusion experiments lithium aluminium hydride : a powerful reducing agent used in organic chemistry sodium borohydride : selective specialty reducing agent, hydrogen storage in fuel cells sodium hydride : a powerful base used in organic chemistry diborane : reducing agent, rocket fuel, semiconductor dopant, catalyst, used in organic synthesis ; also borane, pentaborane and decaborane arsine : used for doping semiconductors stibine : used in semiconductor industry phosphine : used for fumigation silane : many industrial uses, e.g. manufacture of composite materials and water repellents ammonia : coolant, fuel, fertilizer, many other industrial uses hydrogen sulfide : component of natural gas, important source of sulfur Chemically, even water and hydrocarbons could be considered hydrides. All metalloid hydrides are highly flammable. All solid non-metallic hydrides except ice are highly flammable. But, when hydrogen combines with halogens, it produces acids rather than hydrides, and they are not flammable. Precedence convention According to IUPAC convention, by precedence ( stylized electronegativity ), hydrogen falls between group 15 and group 16 elements. Therefore, we have NH, ' nitrogen hydride ' ( ammonia ), versus H O, ' hydrogen oxide ' ( water ). This convention is sometimes broken for polonium, which on the grounds of polonium 's metallicity is often referred to as ' polonium hydride ' instead of the expected ' hydrogen polonide '. See also Parent hydride Hydron ( hydrogen cation ) Hydronium Proton Hydrogen ion Hydride compressor References ^ Jump up to : Greenwood, N.N. ; & Earnshaw, A. ( 1997 ). Chemistry of the Elements ( 2nd Edn. ), Oxford : Butterworth - Heinemann. ISBN 0 - 7506 - 3365 - 4. Jump up ^ Concise Inorganic Chemistry J.D. Lee Jump up ^ Main Group Chemistry, 2nd Edition A.G. Massey ^ Jump up to : Nomenclature of Inorganic Chemistry IUPAC Recommendations 2005 ( Red Book ) Par. IR - 6 - Full text ( PDF ) Jump up ^ Grochala, Wojciech ; Peter P. Edwards ( 2004 - 03 - 01 ). `` Thermal Decomposition of the Non-Interstitial Hydrides for the Storage and Production of Hydrogen ''. Chemical Reviews. 104 ( 3 ) : 1283 -- 1316. doi : 10.1021 / cr030691s. PMID 15008624. Jump up ^ Brown, H.C. ( 1975 ). Organic Syntheses via Boranes. New York : John Wiley & Sons. ISBN 0 - 471 - 11280 - 1. Jump up ^ A. Dedieu ( Editor ) Transition Metal Hydrides 1991, Wiley - VCH, Weinheim. ISBN 0 - 471 - 18768 - 2 Bibliography W.M. Mueller, J.P. Blackledge, G.G. Libowitz, Metal Hydrides, Academic Press, N.Y. and London, ( 1968 ) External links Look up hydride in Wiktionary, the free dictionary. Retrieved from `` https://en.wikipedia.org/w/index.php?title=Hydride&oldid=785942712 '' Categories : Hydrides Anions Hydrogen storage Functional groups Hidden categories : All articles with unsourced statements Articles with unsourced statements from April 2014 Articles with unsourced statements from August 2008 Articles with unsourced statements from October 2013 Articles with unsourced statements from July 2010 Talk Contents About Wikipedia Беларуская Български Bosanski Català Čeština Dansk Deutsch Eesti Ελληνικά Español Esperanto فارسی Français Gaeilge Հայերեն हिन्दी Hrvatski Bahasa Indonesia Italiano עברית Latviešu Magyar Nederlands 日本 語 Plattdüütsch Polski Português Română Русский Scots Simple English Slovenščina Српски / srpski Srpskohrvatski / српскохрватски Suomi Svenska ไทย Українська 中文 Edit links This page was last edited on 16 June 2017, at 09 : 47. Text is available under the Creative Commons Attribution - ShareAlike License ; additional terms may apply. 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Question: how do non metals react with hydrogen explain with an example
Answer: oxygen: water ('oxidane' when substituted; synonym: oxygen hydride), hydrogen peroxide