[{"@context":"http:\/\/schema.org\/","@type":"BlogPosting","@id":"https:\/\/wiki.edu.vn\/en\/wiki24\/polyhalogen-ions-wikipedia\/#BlogPosting","mainEntityOfPage":"https:\/\/wiki.edu.vn\/en\/wiki24\/polyhalogen-ions-wikipedia\/","headline":"Polyhalogen ions – Wikipedia","name":"Polyhalogen ions – Wikipedia","description":"Polyhalogen ions are a group of polyatomic cations and anions containing halogens only. The ions can be classified into two","datePublished":"2021-02-03","dateModified":"2021-02-03","author":{"@type":"Person","@id":"https:\/\/wiki.edu.vn\/en\/wiki24\/author\/lordneo\/#Person","name":"lordneo","url":"https:\/\/wiki.edu.vn\/en\/wiki24\/author\/lordneo\/","image":{"@type":"ImageObject","@id":"https:\/\/secure.gravatar.com\/avatar\/c9645c498c9701c88b89b8537773dd7c?s=96&d=mm&r=g","url":"https:\/\/secure.gravatar.com\/avatar\/c9645c498c9701c88b89b8537773dd7c?s=96&d=mm&r=g","height":96,"width":96}},"publisher":{"@type":"Organization","name":"Enzyklop\u00e4die","logo":{"@type":"ImageObject","@id":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","url":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","width":600,"height":60}},"image":{"@type":"ImageObject","@id":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/9\/96\/Structures_of_some_isopolyhalogen_cations.png\/650px-Structures_of_some_isopolyhalogen_cations.png","url":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/9\/96\/Structures_of_some_isopolyhalogen_cations.png\/650px-Structures_of_some_isopolyhalogen_cations.png","height":"316","width":"650"},"url":"https:\/\/wiki.edu.vn\/en\/wiki24\/polyhalogen-ions-wikipedia\/","about":["Wiki"],"wordCount":15303,"articleBody":"Polyhalogen ions are a group of polyatomic cations and anions containing halogens only. The ions can be classified into two classes, isopolyhalogen ions which contain one type of halogen only, and heteropolyhalogen ions with more than one type of halogen.Table of ContentsIntroduction[edit]Structure[edit]Higher polyiodides[edit]Bonding[edit]Synthesis[edit]Polyhalogen cations[edit]Polyhalogen anions[edit]Properties[edit]Stability[edit]Color[edit]Chemical properties[edit]See also[edit]References[edit]Introduction[edit]Numerous polyhalogen ions have been found, with their salts isolated in the solid state and structurally characterized. The following tables summarize the known species.[1][2][3][4][5][6]Isopolyhalogen cationsDiatomic species*[Cl2]+, [Br2]+, [I2]+Triatomic species[Cl3]+, [Br3]+, [I3]+Tetraatomic species[Cl4]+, [I4]2+Pentaatomic species[Br5]+, [I5]+Heptaatomic species\u2020[I7]+Higher species[I15]3+* [Cl2]+ can only exist as [Cl2O2]2+ at low temperatures, a charge-transfer complex from O2 to [Cl2]+.[2] Free [Cl2]+ is only known from its electronic band spectrum obtained in a low-pressure discharge tube.[3]\u2020 The existence of [I7]+ is possible but still uncertain.[1]Heteropolyhalogen cationsTriatomic species[ClF2]+, [Cl2F]+, [BrF2]+, [IF2]+, [ICl2]+, [IBrCl]+, [IBr2]+, [I2Cl]+, [I2Br]+Pentaatomic species[ClF4]+, [BrF4]+, [IF4]+, [I3Cl2]+Heptaatomic species[ClF6]+, [BrF6]+, [IF6]+Isopolyhalogen anionsTriatomic species[Cl3]\u2212, [Br3]\u2212, [I3]\u2212Tetraatomic species[Br4]2\u2212, [I4]2\u2212Pentaatomic species[I5]\u2212Heptaatomic species[I7]\u2212Octaatomic species[Br8]2\u2212, [I8]2\u2212Higher species[I9]\u2212, [I10]2\u2212, [I10]4\u2212, [I11]\u2212, [I12]2\u2212, [I13]3\u2212, [I16]2\u2212, [I22]4\u2212, [I26]3\u2212, [I26]4\u2212, [I28]4\u2212, [I29]3\u2212Heteropolyhalogen anionsTriatomic species[ClF2]\u2212, [BrF2]\u2212, [BrCl2]\u2212, [IF2]\u2212, [ICl2]\u2212, [IBrF]\u2212, [IBrCl]\u2212, [IBr2]\u2212, [I2Cl]\u2212, [I2Br]\u2212, [AtBrCl]\u2212, [AtBr2]\u2212, [AtICl]\u2212, [AtIBr]\u2212, [AtI2]\u2212Pentaatomic species[ClF4]\u2212, [BrF4]\u2212, [IF4]\u2212, [ICl3F]\u2212, [ICl4]\u2212, [IBrCl3]\u2212, [I2Cl3]\u2212, [I2BrCl2]\u2212, [I2Br2Cl]\u2212, [I2Br3]\u2212, [I4Cl]\u2212, [I4Br]\u2212Hexaatomic species[IF5]2\u2212Heptaatomic species[ClF6]\u2212, [BrF6]\u2212, [IF6]\u2212, [I3Br4]\u2212Nonaatomic species[IF8]\u2212Structure[edit]  Structures of some isopolyhalogen cations  Solid state structures of the polyhalogen ions [BrF2]+, [ClF2]+, [ICl2]+ in their [SbF6]\u2212 salts.  Solid state structure of [I3Cl2]+ in [I3Cl2]+[AsCl6]\u2212.  Structure of the [I2F12]2\u2212 dimer present in [Me4N]+[IF6]\u2212.Most of the structures of the ions have been determined by IR spectroscopy, Raman spectroscopy and X-ray crystallography. The polyhalogen ions always have the heaviest and least electronegative halogen present in the ion as the central atom, making the ion asymmetric in some cases. For example, [Cl2F]+ has a structure of [Cl\u2212Cl\u2212F]\u2212 but not [Cl\u2212F\u2212Cl]\u2212.In general, the structures of most heteropolyhalogen ions and lower isopolyhalogen ions were in agreement with the VSEPR model. However, there were exceptional cases. For example, when the central atom is heavy and has seven lone pairs, such as [BrF6]\u2212 and [IF6]\u2212, they have a regular octahedral arrangement of fluoride ligands instead of a distorted one due to the presence of a stereochemically inert lone pair. More deviations from the ideal VSEPR model were found in the solid state structures due to strong cation-anion interactions, which also complicates interpretation of vibrational spectroscopic data. In all known structures of the polyhalogen anion salts, the anions make very close contact, via halogen bridges, with the counter-cations.[4] For example, in the solid state, [IF6]\u2212 is not regularly octahedral, as solid state structure of [(CH3)4N]+[IF6]\u2212 reveals loosely bound [I2F11]2\u2212 dimers. Significant cation-anion interactions were also found in [BrF2]+[SbF6]\u2212, [ClF2]+[SbF6]\u2212, [BrF4]+[Sb6F11]\u2212.[2]General structures of selected heteropolyhalogen ionsLinear (or almost linear)[ClF2]\u2212, [BrF2]\u2212, [BrCl2]\u2212, [IF2]\u2212, [ICl2]\u2212, [IBr2]\u2212, [I2Cl]\u2212, [I2Br]\u2212Bent[ClF2]+, [Cl2F]+, [BrF2]+, [IF2]+, [ICl2]+, [I2Cl]+, [IBr2]+, [I2Br]+, [IBrCl]+Square planar[ClF4]\u2212, [BrF4]\u2212, [IF4]\u2212, [ICl4]\u2212Disphenoidal (or seesaw)[ClF4]+, [BrF4]+, [IF4]+Pentagonal planar\u2021[IF5]2\u2212Octahedral[ClF6]+, [BrF6]+, [IF6]+, \u00b6[ClF6]\u2212, [BrF6]\u2212, [IF6]\u2212Square antiprismatic[IF8]\u2212\u2021 [IF5]2\u2212 is one of the two XYn-type species known to have the rare pentagonal planar geometry, the other being [XeF5]\u2212.\u00b6 [ClF6]\u2212 is distorted octahedral as the stereochemical inert-pair effect is not significant in the chlorine atom.The [I3Cl2]+ and [I3Br2]+ ions have a trans–Z-type structure, analogous to that of [I5]+.  Solid state structure of [BrF4]+ in [BrF4]+[Sb2F11]\u2212.Higher polyiodides[edit]The polyiodide ions have much more complicated structures. Discrete polyiodides usually have a linear sequence of iodine atoms and iodide ions, and are described in terms of association between I2, I\u2212 and [I3]\u2212 units, which reflects the origin of the polyiodide. In the solid states, the polyiodides can interact with each other to form chains, rings, or even complicated two-dimensional and three-dimensional networks.Bonding[edit]The bonding in polyhalogen ions mostly invoke the predominant use of p-orbitals. Significant d-orbital participation in the bonding is improbable as much promotional energy will be required, while scant s-orbital participation is expected in iodine-containing species due to the inert-pair effect, suggested by data from M\u00f6ssbauer spectroscopy. However, no bonding model has been capable of reproducing such wide range of bond lengths and angles observed so far.[3]As expected from the fact that an electron is removed from the antibonding orbital when X2 is ionized to [X2]+, the bond order as well as the bond strength in [X2]+ gets higher, consequently the interatomic distances in the molecular ion is less than those in X2.Linear or nearly-linear triatomic polyhalides have weaker and longer bonds compared with that in the corresponding diatomic interhalogen or halogen, consistent with the additional repulsion between atoms as the halide ion is added to the neutral molecule. Another model involving the use of resonance theory exists, for example, [ICl2]\u2212 can be viewed as the resonance hybrid of the following canonical forms:Evidence supporting this theory comes from the bond lengths (255\u00a0pm in [ICl2]\u2212 and 232\u00a0pm in ICl(g)) and bond stretching wavenumbers (267\u00a0and 222\u00a0cm\u22121 for symmetric and asymmetric stretching in [ICl2]\u2212 compared with 384\u00a0cm\u22121 in ICl), which suggests a bond order of about 0.5 for each I\u2013Cl bonds in [ICl2]\u2212, consistent with the interpretation using the resonance theory. Other triatomic species [XY2]\u2212 can be similarly interpreted.[2]Even though they have a reduced bond order, all three halogen atoms are tightly bound. The fluorine\u2013fluorine bond of trifluoride, with bond order 0.5, has a bond-strength is 30\u00a0kcal\/mol, only 8\u00a0kcal\/mol less than the fluorine\u2013fluorine bond in difluorine whose bond order is 1.[7]Synthesis[edit]The formation of polyhalogen ions can be viewed as the self-dissociation of their parent interhalogens or halogens:2 XYn \u21cc [XYn\u22121]+ + [XYn+1]\u22123 X2 \u21cc [X3]+ + [X3]\u22124 X2 \u21cc [X5]+ + [X3]\u22125 X2 \u21cc 2 [X2]+ + 2 [X3]\u2212Polyhalogen cations[edit]There are two general strategies for preparing polyhalogen cations:By reacting the appropriate interhalogen with a Lewis acid (such as the halides of B, Al, P, As, Sb) either in an inert or oxidizing solvent (such as anhydrous HF) or without one, to give a heteropolyhalogen cation.XYn + MYm \u2192 [XYn\u22121]+ + [MYm+1]\u2212By an oxidative process, in which the halogen or interhalogen is reacted with an oxidizer and a Lewis acid to give the cation:Cl2 + ClF + AsF5 \u2192 [Cl3]+[AsF6]\u2212In some cases the Lewis acid (the fluoride acceptor) itself acts as an oxidant:3 I2 + 3 SbF5 \u2192 2 [I3]+[SbF6]\u2212 + SbF3Usually the first method is employed for preparing heteropolyhalogen cations, and the second one is applicable to both. The oxidative process is useful in the preparation of the cations [IBr2]+, [ClF6]+, [BrF6]+, as their parent interhalogens, IBr3, ClF7, BrF7 respectively, has never been isolated:Br2 + IOSO2F \u2192 [IBr2]+[SO3F]\u22122 ClF5 + 2 PtF6 \u2192 [ClF6]+[PtF6]\u2212 + [ClF4]+[PtF6]\u2212BrF5 + [KrF]+[AsF6]\u2212 \u2192 [BrF6]+[AsF6]\u2212 + KrThe preparation of some individual species are briefly summarized in the table below with equations:[1][2][3][4]Synthesis of some polyhalogen cationsSpeciesRelevant chemical equationAdditional conditions required[Cl2]+ (as [Cl2O2]+)Cl2 + [O2]+[SbF6]\u2212 \u2192 [Cl2O2]+[SbF6]\u2212in anhydrous HF at low temperatures[Br2]+Br2 (in BrSO3F) + 3 SbF5 \u2192 [Br2]+[Sb3F16]\u2212 (not balanced)at room temperature[I2]+2 I2 + S2O6F2 \u2192 2 [I2]+[SO3F]\u2212in HSO3F[Cl3]+Cl2 + ClF + AsF5 \u2192 [Cl3]+[AsF6]\u2212at a temperature of 195 K (-78 \u00b0C)[Br3]+3 Br2 + 2 [O2]+[AsF6]\u2212 \u2192 2 [Br3]+[AsF6]\u2212 + 2 O2[I3]+3 I2 + S2O6F2 \u2192 2 [I3]+[SO3F]\u2212[Cl4]+2 Cl2 + IrF6 \u2192 [Cl4]+[IrF6]\u2212in anhydrous HF, at a temperature below 193 K (-80 \u00b0C)[I4]2+2 I2 + 3 AsF5 \u2192 [I4]2+[AsF6]\u22122 + AsF3in liquid SO2[Br5]+8 Br2 + 3 [XeF]+[AsF6]\u2212 \u2192 3 [Br5]+[AsF6]\u2212 + 3 Xe + BrF3[I5]+2 I2 + ICl + AlCl3 \u2192 [I5]+[AlCl4]\u2212[I7]+7 I2 + S2O6F2 \u2192 2 I7SO3F[ClF2]+ClF3 + AsF5 \u2192 [ClF2]+[AsF6]\u2212[Cl2F]+2 ClF + AsF5 \u2192 [Cl2F]+[AsF6]\u2212at a temperature below 197 K[BrF2]+5 BrF3 + 2 Au \u2192 3 BrF + 2 [BrF2]+[AuF4]\u2212with excess BrF3 required[IF2]+IF3 + AsF5 \u2192 [IF2]+[AsF6]\u2212[ICl2]+ICl3 + SbCl5 \u2192 [ICl2]+[SbCl6]\u2212[IBr2]+Br2 + IOSO2F \u2192 [IBr2]+[SO3F]\u2212[ClF4]+ClF5 + SbF5 \u2192 [ClF4]+[SbF6]\u2212[BrF4]+BrF5 + AsF5 \u2192 [BrF4]+[AsF6]\u2212[IF4]+IF5 + 2 SbF5 \u2192 [IF4]+[Sb2F11]\u2212[ClF6]+\u2021Cs2[NiF6] + 5 AsF5 + ClF5 \u2192 [ClF6]+[AsF6]\u2212 + Ni[AsF6]2 + 2 Cs[AsF6][BrF6]+[KrF]+[AsF6]\u2212 + BrF5 \u2192 [BrF6]+[AsF6]\u2212 + Kr[IF6]+IF7 + BrF3 \u2192 [IF6]+[BrF4]\u2212\u2021 In this reaction, the active oxidizing species is [NiF3]+, which is formed in situ in the Cs2[NiF6]\/AsF5\/HF system. It is an even more powerful oxidizing and fluorinating agent than PtF6.Polyhalogen anions[edit]For polyhalogen anions, there are two general preparation strategies as well:By reacting an interhalogen or halogen with a Lewis base, most likely a fluoride:[(CH3CH2)4N]+Y\u2212 + XYn \u2192 [(CH3CH2)4N]+[XYn+1]\u2212X2 + X\u2212 \u2192 [X3]\u2212By oxidation of simple halides:KI + Cl2 \u2192 K+[ICl2]\u2212The preparation of some individual species are briefly summarized in the table below with equations:[1][2][3][4]Synthesis of some polyhalogen anionsSpeciesRelevant chemical equationAdditional conditions required[Cl3]\u2212, [Br3]\u2212, [I3]\u2212X2 + X\u2212 \u2192 [X3]\u2212 (X = Cl, Br, I)[Br3]\u2212Br2 + [(CH3CH2CH2CH2)4N]+Br\u2212 \u2192 [(CH3CH2CH2CH2)4N]+[Br3]\u2212in 1,2-dichloroethane or liquid sulfur dioxide. [Br3]\u2212 does not exist in solution and is only formed when the salt crystallizes out.[Br5]\u22122 Br2 + [(CH3CH2CH2CH2)4N]+Br\u2212 \u2192 [(CH3CH2CH2CH2)4N]+[Br5]\u2212in 1,2-dichloroethane or liquid sulfur dioxide, with excess Br2[ClF2]\u2212ClF + CsF \u2192 Cs+[ClF2]\u2212[BrCl2]\u2212[8]:\u200av1p294\u200aBr2 + Cl2 + 2 CsCl \u2192 2 Cs+[BrCl2]\u2212[ICl2]\u2212[8]:\u200av1p295\u200aKI + Cl2 \u2192 K+[ICl2]\u2212[IBr2]\u2212[8]:\u200av1p297\u200aCsI + Br2 \u2192 Cs+[IBr2]\u2212[AtBr2]\u2212, [AtICl]\u2212, [AtIBr]\u2212, [AtI2]\u2212AtY + X\u2212 \u2192 [AtXY]\u2212 (X = I, Br, Cl; Y = I, Br)[ClF4]\u2212NOF + ClF3 \u2192 [NO]+[ClF4]\u2212[BrF4]\u22126 KCl + 8 BrF3 \u2192 6 K+[BrF4]\u2212 + 3 Cl2 + Br2excess BrF5 needed[IF4]\u22122 XeF2 + [(CH3)4N]+I\u2212 \u2192 [(CH3)4N]+[IF4]\u2212 + 2 Xethe reactants were mixed at 242 K, then warmed to 298 K for the reaction to proceed[ICl4]\u2212[8]:\u200av1p298\u200aKI + ICl3 \u2192 K+[ICl4]\u2212[IF5]2\u2212IF3 + 2 [(CH3)4N]+F\u2212 \u2192 [(CH3)4N+]2[IF5]2\u2212[IF6]\u2212IF5 + CsF \u2192 Cs+[IF6]\u2212[I3Br4]\u2212Ph4P]+Br\u2212 + 3 IBr \u2192 [Ph4P]+[I3Br4]\u2212[IF8]\u2212IF7 + [(CH3)4N]+F\u2212 \u2192 [(CH3)4N]+[IF8]\u2212in acetonitrileThe higher polyiodides were formed upon crystallization of solutions containing various concentrations of I\u2212 and I2. For instance, the monohydrate of K+[I3]\u2212 crystallizes when a saturated solution containing appropriate amounts of I2 and KI is cooled.[8]:\u200av1p294\u200aProperties[edit]Stability[edit]In general, a large counter cation or anion (such as Cs+ and [SbF6]\u2212) can help stabilize the polyhalogen ions formed in the solid state from lattice energy considerations, as the packing efficiency increases.The polyhalogen cations are strong oxidizing agents, as indicated by the fact that they can only be prepared in oxidative liquids as a solvent, such as oleum. The most oxidizing and therefore most unstable ones are the species [X2]+ and [XF6]+ (X = Cl, Br), followed by [X3]+ and [IF6]+.The stability of the [X2]+ salts (X = Br, I) are thermodynamically quite stable. However, their stability in solution depends on the superacid solvent. For example, [I2]+ is stable in fluoroantimonic acid (HF with 0.2 N SbF5, H0 = \u221220.65), but disproportionates to [I3]+, [I5]+ and I2 when weaker fluoride acceptors, like NbF5, TaF5 or NaF, are added instead of SbF5.[4]14 [I2]+ + 5 F\u2212 \u2192 9 [I3]+ + IF5For polyhalogen anions with the same cation, the more stable ones are those with a heavier halogen at the center, symmetric ions are also more stable than asymmetric ones. therefore the stability of the anions decrease in the order:[I3]\u2212 > [IBr2]\u2212 > [ICl2]\u2212 > [I2Br]\u2212 > [Br3]\u2212 > [BrCl2]\u2212 > [Br2Cl]\u2212Heteropolyhalogen ions with a coordination number larger than or equal to four can only exist with fluoride ligands.Color[edit]Most polyhalogen ions are intensely colored, with deepened color as the atomic weight of the constituent element increases. The well-known starch-iodine complex has a deep blue color due to the linear [I5]\u2212 ions present in the amylose helix.[4] Some colors of the common species were listed below:[3]fluorocations tend to be colorless or pale yellow, other heteropolyhalogen ions are orange, red or deep purple[4]compounds of [ICl2]+ are wine red to bright orange; while that of [I2Cl]+ are dark brown to purplish black[Cl3]+ is yellow[Cl4]+ is blue[2][Br2]+ is cherry red[Br3]+ is brown[Br5]+ is dark brown[I2]+ is bright blue[I3]+ is dark brown to black[I4]2+ is red to brown[I5]+ is green or black, the salt [I5]+[AlCl4]\u2212 exists as greenish-black needles, but appears brown-red in thin sections[I7]+ is black, if its existence in the compound [I7]+[SO3F]\u2212 has been firmly established[I15]3+ is black[5][ICl2]\u2212 is scarlet red[ICl4]\u2212 is golden-yellowpolyiodides have very dark colors, either dark brown or dark blueChemical properties[edit]The heteropolyhalogen cations are explosively reactive oxidants, and the cations often have higher reactivity than their parent interhalogens and decompose by reductive pathways. As expected from the highest oxidation state of +7 in [ClF6]+, [BrF6]+ and [IF6]+, these species are extremely strong oxidizing agents, demonstrated by the reactions shown below:2 O2 + 2 [BrF6]+[AsF6]\u2212 \u2192 2 [O2]+[AsF6]\u2212 + 2 BrF5 + F2Rn + [IF6]+[SbF6]\u2212 \u2192 [RnF]+[SbF6]\u2212 + IF5Polyhalogen cations with lower oxidation states tend to disproportionate. For example, [Cl2F]+ is unstable in solution and disproportionate completely in HF\/SbF5 mixture even at 197 K:2 [Cl2F]+ \u2192 [ClF2]+ + [Cl3]+[I2]+ reversibly dimerizes at 193 K, and is observed as the blue color of paramagnetic [I2]+ dramatically shifts to the red-brown color of diamagnetic [I2]+, together with a drop in paramagnetic susceptibility and electrical conductivity when the solution is cooled to below 193 K:[2]2 [I2]+ \u21cc [I4]2+The dimerization can be attributed to the overlapping of the half-filled \u03c0* orbitals in two [I2]+.[Cl4]+ in [Cl4]+[IrF6]\u2212 is structurally analogous to [I4]2+, but decomposes at 195 K to give Cl2, and salts of [Cl3]+ instead of [Cl2]+.[2]Attempts to prepare ClF7 and BrF7 by fluorinating [ClF6]+ and [BrF6]+ using NOF have met with failure, because the following reactions occurred:[3][ClF6]+[PtF6]\u2212 + NOF \u2192 [NO]+[PtF6]\u2212 + ClF5 + F2[BrF6]+[AsF6]\u2212 + 2 NOF \u2192 [NO]+[AsF6]\u2212 + [NO]+[BrF6]\u2212 + F2The anions are less reactive compared to the cations, and are generally weaker oxidants than their parent interhalogens. They are less reactive towards organic compounds, and some salts are of quite high thermal stability. Salts containing polyhalogen anions of the type M+[XmYnZp]\u2212, where m + n + p = {3, 5, 7, 9…}, tend to dissociate into simple monohalide salts between M+ and the most electronegative halogen, so that the monohalide has the highest lattice energy. An interhalogen is usually formed as the other product. The salt [(CH3)4N]+[ClF4]\u2212 decomposes at about 100 \u00b0C, and salts of [ClF6]\u2212 are thermally unstable and can explode even at \u221231 \u00b0C.[4]See also[edit]References[edit]^ a b c d King, R. Bruce (2005). “Chlorine, Bromine, Iodine, & Astatine: Inorganic Chemistry”. Encyclopedia of Inorganic Chemistry (2nd\u00a0ed.). Wiley. p.\u00a0747. ISBN\u00a09780470862100.^ a b c d e f g h i Housecroft, Catherine E.; Sharpe, Alan G. (2008). “Chapter 17: The group 17 elements”. Inorganic Chemistry (3rd\u00a0ed.). Pearson. p.\u00a0547. ISBN\u00a0978-0-13-175553-6.^ a b c d e f g Greenwood, Norman  N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd\u00a0ed.). Butterworth-Heinemann. p.\u00a0835. ISBN\u00a0978-0-08-037941-8.^ a b c d e f g h Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999). Advanced Inorganic Chemistry (6th\u00a0ed.). Wiley. ISBN\u00a0978-0471199571.^ a b Wiberg, Egon; Wiberg, Nils; Holleman, Arnold Frederick (2001). Inorganic Chemistry. Academic Press. pp.\u00a0419\u2013420. ISBN\u00a00-12-352651-5.^ Sonnenberg, Karsten; Mann, Lisa; Redeker, Frenio A.; Schmidt, Benjamin; Riedel, Sebastian (2020-02-04). “Polyhalogen and Polyinterhalogen Anions from Fluorine to Iodine”. Angewandte Chemie International Edition. 59 (14): 5464\u20135493. doi:10.1002\/anie.201903197. ISSN\u00a01433-7851. PMID\u00a031090163. S2CID\u00a0155093006.^ Bra\u00efda, Beno\u00eet; Hiberty, Philippe C. (2004). “What Makes the Trifluoride Anion F3\u2013 So Special? A Breathing-Orbital Valence Bond ab Initio Study” (PDF). J. Am. Chem. Soc. 126 (45): 14890\u201314898. doi:10.1021\/ja046443a. PMID\u00a015535716. S2CID\u00a023159174.^ a b c d e Brauer, G., ed. (1963). Handbook of Preparative Inorganic Chemistry (2nd\u00a0ed.). New York: Academic Press."},{"@context":"http:\/\/schema.org\/","@type":"BreadcrumbList","itemListElement":[{"@type":"ListItem","position":1,"item":{"@id":"https:\/\/wiki.edu.vn\/en\/wiki24\/#breadcrumbitem","name":"Enzyklop\u00e4die"}},{"@type":"ListItem","position":2,"item":{"@id":"https:\/\/wiki.edu.vn\/en\/wiki24\/polyhalogen-ions-wikipedia\/#breadcrumbitem","name":"Polyhalogen ions – Wikipedia"}}]}]