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...othane starts from [[trichloroethylene]], which is reacted with [[hydrogen fluoride]] in the presence of [[antimony trichloride]] at 130°C to form 2-chloro-1,

...h is then ring-closed to an epoxide. A ring opening reaction with hydrogen fluoride in tetrahydrofuran gives dexamethasone.<ref>{{Cite journal|doi=10.1021/ja01

* [[Sodium hydrogen carbonate]] * [[Sodium fluoride]]

...]], and [[chloride]] salts. Like silver, mercury reacts with atmospheric [[hydrogen sulfide]]. Mercury even reacts with solid sulfur flakes, which are used in ...cury were confirmed in September 2007, with the synthesis of [[mercury(IV) fluoride]] ({{chem|HgF|4}}) using matrix isolation techniques.<ref name="WangX">{{ci

| OtherAnions = [[Sodium fluoride]]<br/>[[Sodium bromide]]<br/>[[Sodium iodide]] ...olved in water. Along with chlorine, this [[chloralkali process]] yields [[hydrogen]] gas and [[sodium hydroxide]], according to the [[chemical equation]]

...ueous [[solution]], leaving the surface silicon atoms covalently bonded to hydrogen. Since all surface Si atoms are fully co-ordinated, hydrogen termination leads to enhanced stability in ambient environments unlike a 'c

...imiting further escape of depleted UF₆. Release of the hydrogen fluoride gas to the atmosphere is also slowed by the plug formation.<ref>[http://web ...in [[fission bomb]]s and as a nuclear explosive in [[Teller–Ulam design|hydrogen bomb]]s. It is a potential containment material for a [[Shaped charge#Nucle

Ethylene fluorohydrin is obtained differently, by boiling [[hydrogen fluoride]] with a 5–6% solution of ethylene oxide in [[diethyl ether]]. The ether ====Addition of hydrogen cyanide====

| +3 || [[Manganese(III) fluoride|{{chem|MnF|3}}]] ...se oxide-hydroxide MnO(OH) during discharging, preventing the formation of hydrogen at the anode of the battery.<ref name="BattHist"/>

...e]], [[hydrogen fluoride]], [[hydrogen bromide]], [[hydrogen chloride]], [[hydrogen sulfide]], [[phosgene]], polyamide-amine dyes, mustard gas and [[ozone]]. I

Chromium, unlike metals such as iron and nickel, does not suffer from [[hydrogen embrittlement]]. However, it does suffer from nitrogen embrittlement, react Chromium(VI) compounds in solution can be detected by adding an acidic [[hydrogen peroxide]] solution. The unstable dark blue [[chromium(VI) peroxide]] (CrO<

...ct electrolysis of a molten mixture of [[beryllium fluoride]] and [[sodium fluoride]] by [[Paul Lebeau]] in 1898 yielded the first significant pure samples of ...alkali to form the beryllate anion, Be(OH)₄²⁻, and hydrogen gas. The solutions of salts, e.g. [[beryllium sulfate]] and [[beryllium nit

...he states, hydrochloric acid can be oxidized using manganese dioxide, or [[hydrogen chloride]] gas oxidized catalytically by air to form elemental chlorine gas ...d iodide salts to bromine and iodine, respectively. But it cannot oxidize fluoride to fluorine. It makes are variety of "interhalogen compounds" such as the

...nodes of impure lead and cathodes of pure lead in an electrolyte of silica fluoride.<ref name="samans"/><ref name="leadorg"/> ...stem is plotted on the y axis in terms of volts relative to the [[standard hydrogen electrode]]. The diagram shows the form of the element which is most chemic

...ulfide|H₂S]], [[hydrogen telluride|H₂Te]], and the [[hydrogen halide|hydrohalic acids]]. However, Davy failed to develop a new theory, co === Liebig's hydrogen theory of acids ===

...ust be dissolved in it, which binds away many of these rare hydrogen ions. Hydrogen ions in water can be written simply as H⁺ or as [[hydronium]] (H ...nic strength]] of a solution - for example, the pH of a 0.05 M [[potassium hydrogen phthalate]] solution can vary by as much as 0.5 pH units as a function of a

...[strong acid|strong]] [[mineral acid]] with the molecular formula {{chem|[[hydrogen|H]]|2}}{{chem|link=sulfate|SO|4}}. It is soluble in [[water]] at all concen or, alternatively, [[hydrogen sulfide]] ({{chem|H|2|S}}) gas is incinerated to {{chem|SO|2}} gas:

...increased understanding of [[agostic complex]]es wherein hydrocarbons and hydrogen serve as ligands. Noncoordinating anions are important components of many [ ...etal ions, such as cations containing Zr(IV) centers, which can abstract [[fluoride]] from these anions. Other anions, such as [[triflate]]s were considered to

...stereospecific]]ity. The silyl protecting group is removed with [[hydrogen fluoride]] to alcohol '''14''' and then activated as an [[mesyl]] [[leaving group]]

|doi=10.1126/science.141.3586.1171|pmid=17751791}}</ref> and [[radon fluoride]].<ref>{{cite journal |title=Radon Fluoride