Klorin: Perbedaan antara revisi
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Baris 85:
: NaCl + H<sub>2</sub>SO<sub>4</sub> {{overunderset|→|150 °C| }} NaHSO<sub>4</sub> + HCl
: NaCl + NaHSO<sub>4</sub> {{overunderset|→|540–600 °C| }} Na<sub>2</sub>SO<sub>4</sub> + HCl
Pada suhu ruang, asam klorida berwujud gas tak berwarna, sama seperti semua hidrogen halida kecuali [[hidrogen fluorida]], karena hidrogen tak dapat membentuk ikatan hidrogen yang kuat dengan atom klorin yang keelektronegatifannya lebih besar.<ref name="Greenwood809" /> Asam klorida merupakan asam kuat (p''K''<sub>a</sub> = −7) karena ikatan hidrogen dengan klorin terlalu lemah untuk terdisosiasi. Sistem HCl/H<sub>2</sub>O memiliki banyak bentuk hidrat HCl·''n''H<sub>2</sub>O untuk ''n'' = 1, 2, 3, 4, dan 6. Campuran HCl dan H<sub>2</sub>O melebihi 1:1 akan membuat sistem terpisah menjadi 2 fase liquid yang berbeda. Asam klorida membentuk [[azeotrop]] dengan titik didih 108.58 °C pada 20.22 g HCl per 100 g larutan, maka asam klorida tidak dapat dipekatkan lebih jauh lagi melewati ini melalui distilasi.<ref name="Greenwood812">Greenwood and Earnshaw, pp. 812–16</ref>
Baris 94:
: {{chem|Me|4|N|+|HCl|2|-}} + BCl<sub>3</sub> → {{chem|Me|4|N|+|BCl|4|-}} + HCl (penggantian ligan)
: PCl<sub>3</sub> + Cl<sub>2</sub> + HCl → {{chem|PCl|4|+|HCl|2|-}} (oksidasi)
=== Senyawa poliklorin ===
Meskipun klorin adalah oksidator kuat dengan energi ionisasi pertama tinggi, senyawa ini dapat teroksidasi pada kondisi ekstrim membentuk kation {{chem|Cl|2|+}} . Senyawa ini sangat tak stabil dan hanya dikarakterisasi oleh spektrum pita elektronik ketika diproduksi dalam tabung discharge bertekanan rendah. Kation {{chem|Cl|3|+}} yang berwarna kuning lebih stabil dan dapat diproduksi sebagai berikut:<ref name="Greenwood842">Greenwood and Earnshaw, pp. 842–44</ref>
: Cl<sub>2</sub> + ClF + AsF<sub>5</sub> {{overunderset|→|−78 °C| }} {{chem|Cl|3|+|AsF|6|-}}
Reaksi ini dilakukan dalam pelarut [[arsenik pentafluorida]]. Anion triklorida, {{chem|Cl|3|-}}, juga telah dikarakterisasi, analog dengan [[triiodida]].<ref name="Greenwood824">Greenwood and Earnshaw, pp. 824–8</ref>
=== Fluorida klorin ===
The three fluorides of chlorine form a subset of the [[:en:Interhalogen|interhalogen]] compounds yang semuanya [[diamagnetik]].<ref name="Greenwood824" /> Beberapa turunan kation dan anion diketahui, seperti {{chem|ClF|2|-}}, {{chem|ClF|4|-}}, {{chem|ClF|2|+}}, dan Cl<sub>2</sub>F<sup>+</sup>.<ref name="Greenwood835">Greenwood and Earnshaw, pp. 835–42</ref> Beberapa [[:en:Pseudohalogen|pseudohalida]] klorin juga diketahui, seperti [[sianogen klorida]] (ClCN, linear), klorin [[sianat]] (ClNCO), klorin [[tiosianat]] (ClSCN, unlike its oxygen counterpart), and klorin [[azida]] (ClN<sub>3</sub>).<ref name="Greenwood824" />
[[:en:Chlorine_monofluoride|Chlorine monofluoride]] (ClF) is extremely thermally stable, dan dijual komersial dalam botol 500-gram. Merupakan gas tak berwarna yang melebur pada −155.6 °C dan mendidih pada −100.1 °C. It may be produced by the direction of its elements at 225 °C, though it must then be separated and purified from [[:en:Chlorine_trifluoride|chlorine trifluoride]] and its reactants. Its properties are mostly intermediate between those of chlorine and fluorine. It will react with many metals and nonmetals from room temperature and above, fluorinating them and liberating chlorine. It will also act as a chlorofluorinating agent, adding chlorine and fluorine across a multiple bond or by oxidation: for example, it will attack [[:en:Carbon_monoxide|carbon monoxide]] to form [[:en:Carbonyl_chlorofluoride|carbonyl chlorofluoride]], COFCl. It will react analogously with [[:en:Hexafluoroacetone|hexafluoroacetone]], (CF<sub>3</sub>)<sub>2</sub>CO, with a [[:en:Potassium_fluoride|potassium fluoride]] catalyst to produce [[:en:Heptafluoroisopropyl_hypochlorite|heptafluoroisopropyl hypochlorite]], (CF<sub>3</sub>)<sub>2</sub>CFOCl; with [[:en:Nitrile|nitriles]] RCN to produce RCF<sub>2</sub>NCl<sub>2</sub>; and with the sulfur oxides SO<sub>2</sub> and SO<sub>3</sub> to produce ClOSO<sub>2</sub>F and ClSO<sub>2</sub>F respectively. It will also react exothermically and violently with compounds containing –OH and –NH groups, such as water:<ref name="Greenwood824" />
: H<sub>2</sub>O + 2 ClF → 2 HF + Cl<sub>2</sub>O
[[Klorin trifluorida]] (ClF<sub>3</sub>) berbentuk cairan tak berwarna volatil yang melebur pada −76.3 °C dan mendidih pada 11.8 °C. It may be formed by directly fluorinating gaseous chlorine or chlorine monofluoride at 200–300 °C. It is one of the most reactive known chemical compounds, reacting with many substances which in ordinary circumstances would be considered chemically inert, such as [[asbestos]], concrete, and sand. Senyawa ini meledak apabila berkontak dengan air dan sebagian besar senyawa organik lain. The list of elements it sets on fire is diverse, containing [[hidrogen]], [[kalium]], [[fosfor]], [[Arsen|arsenik]], [[antimon]], [[Belerang|sulfur]], [[selenium]], [[telurium]], [[bromin]], [[Iodin|iodine]], and powdered [[molibdenum]], [[Wolfram|tungsten]], [[rodium]], [[iridium]], and [[:en:Iron|iron]]. An impermeable fluoride layer is formed by [[natrium]], [[magnesium]], [[aluminium]], [[seng]], [[timah]], and [[perak]], which may be removed by heating. When heated, even such [[:en:Noble_metal|noble metals]] as [[:en:Palladium|palladium]], [[platina]], and [[:en:Gold|gold]] are attacked and even the [[:en:Noble_gas|noble gases]] [[xenon]] and [[radon]] do not escape fluorination. [[Nikel]] containers are usually used due to that metal's great resistance to attack by chlorine trifluoride, stemming from the formation of an unreactive nickel fluoride layer. Its reaction with [[hidrazin]] to form hydrogen fluoride, nitrogen, and chlorine gases was used in experimental rocket motors, but has problems largely stemming from its extreme [[:en:Hypergolic_propellant|hypergolicity]] resulting in ignition without any measurable delay. For these reasons, it was used in bomb attacks during the [[:en:Second_World_War|Second World War]] by the Nazis. Today, it is mostly used in nuclear fuel processing, to oxidise [[uranium]] to [[uranium heksafluorida]] for its enriching and to separate it from [[plutonium]]. It can act as a fluoride ion donor or acceptor (Lewis base or acid), although it does not dissociate appreciably into {{chem|ClF|2|+}} and {{chem|ClF|4|-}} ions.<ref name="Greenwood828">Greenwood and Earnshaw, pp. 828–31</ref>
[[:en:Chlorine_pentafluoride|Chlorine pentafluoride]] (ClF<sub>5</sub>) is made on a large scale by direct fluorination of chlorine with excess [[:en:Fluorine|fluorine]] gas at 350 °C and 250 atm, and on a small scale by reacting metal chlorides with fluorine gas at 100–300 °C. It melts at −103 °C and boils at −13.1 °C. It is a very strong fluorinating agent, although it is still not as effective as chlorine trifluoride. Only a few specific stoichiometric reactions have been characterised. [[:en:Arsenic_pentafluoride|Arsenic pentafluoride]] and [[:en:Antimony_pentafluoride|antimony pentafluoride]] form ionic adducts of the form [ClF<sub>4</sub>]<sup>+</sup>[MF<sub>6</sub>]<sup>−</sup> (M = As, Sb) and water reacts vigorously as follows:<ref name="Greenwood832">Greenwood and Earnshaw, pp. 832–35</ref>
: 2 H<sub>2</sub>O + ClF<sub>5</sub> → 4 HF + FClO<sub>2</sub>
The product, [[:en:Chloryl_fluoride|chloryl fluoride]], is one of the five known chlorine oxide fluorides. These range from the thermally unstable FClO to the chemically unreactive [[:en:Perchloryl_fluoride|perchloryl fluoride]] (FClO<sub>3</sub>), the other three being FClO<sub>2</sub>, F<sub>3</sub>ClO, and F<sub>3</sub>ClO<sub>2</sub>. All five behave similarly to the chlorine fluorides, both structurally and chemically, and may act as Lewis acids or bases by gaining or losing fluoride ions respectively or as very strong oxidising and fluorinating agents.<ref name="Greenwood875">Greenwood and Earnshaw, pp. 875–80</ref>
== Produksi dan keberadaan ==
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