metal hydride!

metal hydride

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1) "Metal" -- As to metal hydride 1met·al Pronunciation: 'me-t&l Function: noun Usage: often attributive Etymology: Middle English, from Anglo-French, from Latin metallum mine, metal, from Greek metallon 1 : any of various opaque, fusible, ductile, and typically lustrous substances that are good conductors of electricity and heat, form cations by loss of electrons, and yield basic oxides and hydroxides; especially : one that is a chemical element as distinguished from an alloy 2 a : METTLE 1a b : the substance out of which a person or thing is made 3 : glass in its molten state 4 a : printing type metal b : matter set in metal type 5 : ROAD METAL 6 : HEAVY METAL Pronunciation Symbols Hot metal work from a blacksmith In chemistry, a metal (Greek: Metallon) is an element that readily forms positive ions (cations) and has metallic bonds. Metals are sometimes described as a lattice of positive ions surrounded by a cloud of delocalized electrons. The metals are one of the three groups of elements as distinguished by their ionization and bonding properties, along with the metalloids and nonmetals. On the periodic table, a diagonal line drawn from boron (B) to polonium (Po) separates the metals from the nonmetals. Most elements on this line are metalloids, sometimes called semi-metals; elements to the lower left are metals; elements to the upper right are nonmetals. A modern definition of metals is that they have overlapping conduction bands and valence bands in their electronic structure. This definition opens up the category for metallic polymers and other organic metals, which have been made by researchers and employed in high-tech devices. These synthetic materials often have the characteristic silvery-grey reflectiveness (luster) of elemental metals. The traditional definition focuses on the bulk properties of metals. They tend to be lustrous, ductile, malleable, and good conductors of electricity, while nonmetals are generally brittle (if solid), lack luster, and are insulators. 1 Chemical properties 2 Physical properties 3 Alloys 4 Categories 4.1 Base metal 4.2 Ferrous metal 4.3 Noble metal 4.4 Precious metal 5 Extraction 6 Metallurgy 7 Applications 8 Astronomy 9 See also 10 External link Most metals are chemically reactive, reacting with oxygen in the air to form oxides over varying timescales (for..." 2) "Hydride" -- As to metal hydride hy·dride Pronunciation: 'hI-"drId Function: noun : a compound of hydrogen with a more electropositive element or group Pronunciation Symbols Hydride is the name given to the negative ion of hydrogen, H−. It is also used as a more general term to describe compounds of hydrogen with other elements, particularly those of groups 1–16, whether or not they actually contain hydride ions. Protide, deuteride and tritide are used in the same way to describe ions or compounds which contain enriched hydrogen-1, deuterium or tritium respectively. The variety of compounds formed by hydrogen is vast, arguably greater than that of any other element. Virtually every element of the periodic table (except the noble gases) forms one or more hydrides. These may be classified into three main types by the predominant nature of their bonding: Ionic hydrides, also known as saline hydrides; Covalent hydrides; Interstitial hydrides, which may be described as having metallic bonding. 1 Hydride ion 2 Precedence convention 3 Ionic hydrides 4 Covalent hydrides 5 Interstitial hydrides of the transitional metals 6 Usage 7 External links 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 most of the chemistry of the hydride ion is dominated by the highly exothermic production of dihydrogen: H− + H+ → H2; ΔH = −1675 kJ/mol As a result, the hydride ion is one of the strongest bases known. It will extract protons from almost all other hydrogen-containing compounds, including liquid ammonia but with the exception of saturated hydrocarbons. The hydride ion is unknown in solution, as it would react with virtually any solvent, e.g. NaH + H2O → H2 + NaOH; ΔH = −83.6&#..." 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