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Hydride

January 01, 1970

This article is about binary compounds of hydrogen with another element. For the anion of hydrogen, see Hydrogen anion.

In chemistry, a hydride is formally the anion of hydrogen (H−), a hydrogen atom with two electrons.[1] The term is applied loosely. At one extreme, all compounds containing covalently bound H atoms are also called hydrides: water (H2O) is a hydride of oxygen, ammonia is a hydride of nitrogen, etc. For inorganic chemists, hydrides refer to compounds and ions in which hydrogen is covalently attached to a less electronegative element. In such cases, the H centre has nucleophilic character, which contrasts with the protic character of acids. The hydride anion is very rarely observed.

Sodium hydride as an example of hydride salt

Almost all of the elements form binary compounds with hydrogen, the exceptions being He,[2] Ne,[3] Ar,[4] Kr,[5] Pm, Os, Ir, Rn, Fr, and Ra.[6][7][8][9] Exotic molecules such as positronium hydride have also been made.

Bonds edit

Bonds between hydrogen and the other elements range from being highly ionic 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,[citation needed] bulk metals (interstitial), or 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 edit

 
Tris(trimethylsilyl)silane is an example of a hydride with a weak bond to H. It is used as a source of hydrogen atoms.[10]
 
Metal hydrides (e.g. H2RhCl(PPh3)2 derived from Wilkinson's catalyst) are intermediates in hydrogenation catalysis.

Hydride ion edit

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.

  ΔH = −1676 kJ/mol

The low electron affinity of hydrogen and the strength of the H–H bond (ΔHBE = 436 kJ/mol) means that the hydride ion would also be a strong reducing agent

  E⊖ = −2.25 V

Types of hydrides edit

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:[6]

  • 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 edit

These are stoichiometric compounds of hydrogen. 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 alkaline earth metals. 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.[12]

 

Typical solvents for such reactions are ethers. Water and other protic solvents cannot 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.

 
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.

 

Covalent hydrides edit

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; for example, 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 (NaBH4) and lithium aluminium hydride and hindered reagents such as DIBAL.

Interstitial hydrides or metallic hydrides edit

 
Metal hydride for hydrogen storage applications

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. Neutron diffraction studies have shown that hydrogen atoms randomly occupy the octahedral interstices in the metal lattice (in an fcc lattice there is one octahedral hole per metal atom). The limit of absorption at normal pressures is PdH0.7, indicating that approximately 70% of the octahedral holes are occupied.[13]

Many interstitial hydrides have been 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.[14]

 
Structure of [HRu6(CO)18]−, a metal cluster with an interstitial hydride ligand (small turquoise sphere at center).[15]

Transition metal hydride complexes edit

Main article: Transition metal hydride

Transition metal hydrides include compounds that can be classified as covalent hydrides. Some are even classified as interstitial hydrides[citation needed] 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)4 and H2Fe(CO)4. The anions potassium nonahydridorhenate [ReH9]2− and [FeH6]4− are examples from the growing collection of known molecular homoleptic metal hydrides.[16] As pseudohalides, hydride ligands are capable of bonding with positively polarized hydrogen centres. This interaction, called dihydrogen bonding, is similar to hydrogen bonding, which exists between positively polarized protons and electronegative atoms with open lone pairs.

Protides edit

Hydrides containing protium are known as protides.

Deuterides edit

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.

Tritides edit

Hydrides containing tritium are known as tritides.

Mixed anion compounds edit

Mixed anion compounds exist that contain hydride with other anions. These include boride hydrides, carbohydrides, hydridonitrides, oxyhydrides and others.

Appendix on nomenclature edit

Protide, deuteride and tritide are used to describe ions or compounds that contain enriched hydrogen-1, deuterium or tritium, respectively.

In the classic meaning, hydride refers to any compound 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:[9]

According to the convention above, the following are "hydrogen compounds" and not "hydrides":[citation needed]

Examples:

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 edit

According to IUPAC convention, by precedence (stylized electronegativity), hydrogen falls between group 15 and group 16 elements. Therefore, we have NH3, "nitrogen hydride" (ammonia), versus H2O, "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 edit

References edit

  1. ^ "hydron (H02904)". IUPAC. 24 February 2014. doi:10.1351/goldbook.H02904. Retrieved 11 May 2021.
  2. ^ Helium hydride exists as an ion.
  3. ^ Neonium is an ion, and the HNe excimer exists also.
  4. ^ Argonium exists as an ion.
  5. ^ Kryptonium ion exist as a cation.
  6. ^ a b Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the elements (2nd ed.). Boston, Mass: Butterworth-Heinemann. ISBN 0-7506-3365-4. OCLC 48138330.
  7. ^ Lee, J.D. (2008). Concise Inorganic Chemistry (5th ed.). Wiley. ISBN 978-81-265-1554-7.
  8. ^ Massey, A.G. (2000). Main Group Chemistry. Inorganic Chemistry. Wiley. ISBN 978-0-471-49039-5.
  9. ^ a b Nomenclature of Inorganic Chemistry ("The Red Book") (PDF). IUPAC Recommendations. 2005. Par. IR-6.
  10. ^ Chatgilialoglu, Chryssostomos; Ferreri, Carla; Landais, Yannick; Timokhin, Vitaliy I. (2018). "Thirty Years of (TMS)3SiH: A Milestone in Radical-Based Synthetic Chemistry". Chemical Reviews. 118 (14): 6516–6572. doi:10.1021/acs.chemrev.8b00109. PMID 29938502. S2CID 49413857.
  11. ^ Grochala, Wojciech; Edwards, Peter P. (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.
  12. ^ Brown, H. C. (1975). Organic Syntheses via Boranes. New York: John Wiley & Sons. ISBN 0-471-11280-1.
  13. ^ Palladium hydride
  14. ^ Züttel, Andreas (2003). "Materials for hydrogen storage". Materials Today. 6 (9): 24–33. doi:10.1016/s1369-7021(03)00922-2.
  15. ^ Jackson, Peter F.; Johnson, Brian F. G.; Lewis, Jack; Raithby, Paul R.; McPartlin, Mary; Nelson, William J. H.; Rouse, Keith D.; Allibon, John; Mason, Sax A. (1980). "Direct location of the interstitial hydride ligand in [HRu6(CO)18]– by both X-ray and neutron analyses of [Ph4As][HRu6(CO)18] by Both X-ray and Neutron Analyses of [Ph4As][HRu6(CO)18]". Journal of the Chemical Society, Chemical Communications (7): 295. doi:10.1039/c39800000295.
  16. ^ A. Dedieu (Editor) Transition Metal Hydrides 1991, Wiley-VCH, Weinheim. ISBN 0-471-18768-2

Bibliography edit

W. M. Mueller, J. P. Blackledge, G. G. Libowitz, Metal Hydrides, Academic Press, N.Y. and London, (1968)

External links edit

 
Look up hydride in Wiktionary, the free dictionary.
  •   Media related to Hydrides at Wikimedia Commons

January 01, 1970
hydride, this, article, about, binary, compounds, hydrogen, with, another, element, anion, hydrogen, hydrogen, anion, chemistry, hydride, formally, anion, hydrogen, hydrogen, atom, with, electrons, term, applied, loosely, extreme, compounds, containing, covale. This article is about binary compounds of hydrogen with another element For the anion of hydrogen see Hydrogen anion In chemistry a hydride is formally the anion of hydrogen H a hydrogen atom with two electrons 1 The term is applied loosely At one extreme all compounds containing covalently bound H atoms are also called hydrides water H2O is a hydride of oxygen ammonia is a hydride of nitrogen etc For inorganic chemists hydrides refer to compounds and ions in which hydrogen is covalently attached to a less electronegative element In such cases the H centre has nucleophilic character which contrasts with the protic character of acids The hydride anion is very rarely observed Sodium hydride as an example of hydride salt Almost all of the elements form binary compounds with hydrogen the exceptions being He 2 Ne 3 Ar 4 Kr 5 Pm Os Ir Rn Fr and Ra 6 7 8 9 Exotic molecules such as positronium hydride have also been made 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 Protides 4 6 Deuterides 4 7 Tritides 4 8 Mixed anion compounds 5 Appendix on nomenclature 5 1 Precedence convention 6 See also 7 References 8 Bibliography 9 External linksBonds editBonds between hydrogen and the other elements range from being highly ionic 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 citation needed bulk metals interstitial or 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 edit nbsp Tris trimethylsilyl silane is an example of a hydride with a weak bond to H It is used as a source of hydrogen atoms 10 nbsp Metal hydrides e g H2RhCl PPh3 2 derived from Wilkinson s catalyst are intermediates in hydrogenation catalysis 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 H2 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 vacuum 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 11 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 editSee 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 2 displaystyle ce H H gt H2 nbsp DH 1676 kJ mol The low electron affinity of hydrogen and the strength of the H H bond DHBE 436 kJ mol means that the hydride ion would also be a strong reducing agent H 2 2 e 2 H displaystyle ce H2 2e lt gt 2H nbsp E 2 25 VTypes of hydrides editAccording 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 6 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 edit These are stoichiometric compounds of hydrogen 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 alkaline earth metals 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 12 C 6 H 5 C O CH 3 acetophenone KH potassium hydride C 6 H 5 C O CH 2 K H 2 displaystyle ce overset acetophenone C6H5C O CH3 overset potassium hydride KH gt C6H5C O CH2K H2 nbsp Typical solvents for such reactions are ethers Water and other protic solvents cannot 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 2 O H 2 g NaOH displaystyle ce NaH H2O gt H2 g NaOH nbsp DH 83 6 kJ mol DG 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 lithium hydride AlCl 3 LiAlH 4 3 LiCl displaystyle ce overset lithium hydride 4 LiH AlCl3 gt LiAlH4 3 LiCl nbsp Covalent hydrides edit 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 for example 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 NaBH4 and lithium aluminium hydride and hindered reagents such as DIBAL Interstitial hydrides or metallic hydrides edit nbsp Metal hydride for hydrogen storage applications 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 Neutron diffraction studies have shown that hydrogen atoms randomly occupy the octahedral interstices in the metal lattice in an fcc lattice there is one octahedral hole per metal atom The limit of absorption at normal pressures is PdH0 7 indicating that approximately 70 of the octahedral holes are occupied 13 Many interstitial hydrides have been 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 14 nbsp Structure of HRu6 CO 18 a metal cluster with an interstitial hydride ligand small turquoise sphere at center 15 Transition metal hydride complexes edit Main article Transition metal hydride Transition metal hydrides include compounds that can be classified as covalent hydrides Some are even classified as interstitial hydrides citation needed 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 4 and H2Fe CO 4 The anions potassium nonahydridorhenate ReH9 2 and FeH6 4 are examples from the growing collection of known molecular homoleptic metal hydrides 16 As pseudohalides hydride ligands are capable of bonding with positively polarized hydrogen centres This interaction called dihydrogen bonding is similar to hydrogen bonding which exists between positively polarized protons and electronegative atoms with open lone pairs Protides edit Hydrides containing protium are known as protides Deuterides edit 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 Tritides edit Hydrides containing tritium are known as tritides Mixed anion compounds edit Mixed anion compounds exist that contain hydride with other anions These include boride hydrides carbohydrides hydridonitrides oxyhydrides and others Appendix on nomenclature editProtide deuteride and tritide are used to describe ions or compounds that contain enriched hydrogen 1 deuterium or tritium respectively In the classic meaning hydride refers to any compound 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 9 alkali and alkaline earth metals metal hydride boron borane BH3 aluminium alumane AlH3 gallium gallane GaH3 indium indigane InH3 thallium thallane TlH3 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 citation needed oxygen water oxidane when substituted synonym hydrogen oxide hydrogen peroxide sulfur hydrogen sulfide sulfane when substituted 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 edit According to IUPAC convention by precedence stylized electronegativity hydrogen falls between group 15 and group 16 elements Therefore we have NH3 nitrogen hydride ammonia versus H2O 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 editParent hydride Hydron hydrogen cation Hydronium Proton Hydrogen ion Hydride compressor SuperhydridesReferences edit hydron H02904 IUPAC 24 February 2014 doi 10 1351 goldbook H02904 Retrieved 11 May 2021 Helium hydride exists as an ion Neonium is an ion and the HNe excimer exists also Argonium exists as an ion Kryptonium ion exist as a cation a b Greenwood N N Earnshaw A 1997 Chemistry of the elements 2nd ed Boston Mass Butterworth Heinemann ISBN 0 7506 3365 4 OCLC 48138330 Lee J D 2008 Concise Inorganic Chemistry 5th ed Wiley ISBN 978 81 265 1554 7 Massey A G 2000 Main Group Chemistry Inorganic Chemistry Wiley ISBN 978 0 471 49039 5 a b Nomenclature of Inorganic Chemistry The Red Book PDF IUPAC Recommendations 2005 Par IR 6 Chatgilialoglu Chryssostomos Ferreri Carla Landais Yannick Timokhin Vitaliy I 2018 Thirty Years of TMS 3SiH A Milestone in Radical Based Synthetic Chemistry Chemical Reviews 118 14 6516 6572 doi 10 1021 acs chemrev 8b00109 PMID 29938502 S2CID 49413857 Grochala Wojciech Edwards Peter P 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 Brown H C 1975 Organic Syntheses via Boranes New York John Wiley amp Sons ISBN 0 471 11280 1 Palladium hydride Zuttel Andreas 2003 Materials for hydrogen storage Materials Today 6 9 24 33 doi 10 1016 s1369 7021 03 00922 2 Jackson Peter F Johnson Brian F G Lewis Jack Raithby Paul R McPartlin Mary Nelson William J H Rouse Keith D Allibon John Mason Sax A 1980 Direct location of the interstitial hydride ligand in HRu6 CO 18 by both X ray and neutron analyses of Ph4As HRu6 CO 18 by Both X ray and Neutron Analyses of Ph4As HRu6 CO 18 Journal of the Chemical Society Chemical Communications 7 295 doi 10 1039 c39800000295 A Dedieu Editor Transition Metal Hydrides 1991 Wiley VCH Weinheim ISBN 0 471 18768 2Bibliography editW M Mueller J P Blackledge G G Libowitz Metal Hydrides Academic Press N Y and London 1968 External links edit nbsp Look up hydride in Wiktionary the free dictionary nbsp Media related to Hydrides at Wikimedia Commons Retrieved from https en wikipedia org w index php title Hydride amp oldid 1221581163, wikipedia, wiki, book, books, library,

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