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Hydride
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<p>In <a href="/facts/Chemistry/SrNqkGVm">chemistry</a>, a hydride is formally the <a href="/facts/Anion/wrbwhF3z">anion</a> of <a href="/facts/Hydrogen/BoYHjl0J">hydrogen</a> (H−), a hydrogen ion with two electrons. In modern usage, this is typically only used for ionic bonds, but it is sometimes (and has been more frequently in the past) applied to all <a href="/facts/Chemical_compound/37FXqqtv">compounds</a> containing <a href="/facts/Covalent_bond/EzMLf3Pz">covalently bound</a> H <a href="/facts/Atom/FoQ4kGN5">atoms</a>. In this broad and potentially archaic sense, <a href="/facts/Water/0lkXnJPK">water</a> (H2O) is a hydride of <a href="/facts/Oxygen/acyn6o8r">oxygen</a>, <a href="/facts/Ammonia/MtLtJFtz">ammonia</a> is a hydride of <a href="/facts/Nitrogen/Nf1QpGDz">nitrogen</a>, etc. In covalent compounds, it implies hydrogen is attached to a less <a href="/facts/Electronegative/H7Vq7Uah">electronegative</a> <a href="/facts/Chemical_element/0jducgWD">element</a>. In such cases, the H centre has nucleophilic character, which contrasts with the protic character of acids. The hydride anion is very rarely observed. </p> <p>Almost all of the elements form <a href="/facts/Binary_compounds_of_hydrogen/kBDn9hjI">binary compounds with hydrogen</a>, the exceptions being <a href="/facts/Helium/yRul93TG">He</a>, <a href="/facts/Neon/5bF1FwGL">Ne</a>, <a href="/facts/Argon/QX6NRH6d">Ar</a>, <a href="/facts/Krypton/llkNlCke">Kr</a>, <a href="/facts/Promethium/8xvCz9Rg">Pm</a>, <a href="/facts/Osmium/1TjXD69n">Os</a>, <a href="/facts/Iridium/TFQutoj1">Ir</a>, <a href="/facts/Radon/0V9arWKl">Rn</a>, <a href="/facts/Francium/P3Rz4gDP">Fr</a>, and <a href="/facts/Radium/VWo5gkzn">Ra</a>. <a href="/facts/Exotic_atom/FrPmnXvk">Exotic molecules</a> such as <a href="/facts/Positronium_hydride/D8v289Np">positronium hydride</a> have also been made. </p>