Transition metal chloride complex

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Octahedral molecular geometry is a common structural motif for homoleptic metal chloride complexes. Examples include MCl6 (M = Mo, W), [MCl6] (M = Nb, Ta, Mo, W, Re), [MCl6] (M = Ti Zr, Hf, Mo, Mn, Re, Ir, Pd, Pt), and [MCl6] (M = Ru Os, Rh, Ir). Tungsten-hexachloride-from-xtal-3D-balls.png
Octahedral molecular geometry is a common structural motif for homoleptic metal chloride complexes. Examples include MCl6 (M = Mo, W), [MCl6] (M = Nb, Ta, Mo, W, Re), [MCl6] (M = Ti Zr, Hf, Mo, Mn, Re, Ir, Pd, Pt), and [MCl6] (M = Ru Os, Rh, Ir).

In chemistry, a transition metal chloride complex is a coordination complex that consists of a transition metal coordinated to one or more chloride ligand. The class of complexes is extensive. [1]

Contents

Bonding

Halides are X-type ligands in coordination chemistry. They are both σ- and π-donors. Chloride is commonly found as both a terminal ligand and a bridging ligand. The halide ligands are weak field ligands. Due to a smaller crystal field splitting energy, the homoleptic halide complexes of the first transition series are all high spin. Only [CrCl6]3− is exchange inert.

Homoleptic metal halide complexes are known with several stoichiometries, but the main ones are the hexahalometallates and the tetrahalometallates. The hexahalides adopt octahedral coordination geometry, whereas the tetrahalides are usually tetrahedral. Square planar tetrahalides are known for Pd(II), Pt(II), and Au(III). Examples with 2- and 3-coordination are common for Au(I), Cu(I), and Ag(I).

Due to the presence of filled pπ orbitals, halide ligands on transition metals are able to reinforce π-backbonding onto a π-acid. They are also known to labilize cis-ligands. [2] [3]

Homoleptic complexes

Homoleptic complexes (complexes with only chloride ligands) are often common reagents. Almost all examples are anions.

1st row

1st Transition Series
Complexcolourelectron config.structuregeometrycomments
TiCl4 colourless(t2g)0 Tetrahedral-tetrachlorometallate-3D-bs-20.png tetrahedral
[Ti2Cl9]−white/colourlessd0d0 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png face-sharing bioctahedronTi-Cl(terminal) = 2.23 Å, 2.45 (terminal)
(N(PCl3)2)+ salt) [4]
[Ti2Cl9]3-orange(t2g)1(t2g)1 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png face-sharing bioctahedronTi-Ti =3.22 Å
Ti-C1(terminal) = 2.32-2.35 Å,
Ti-Cl(bridge) = 2.42-2.55 Å
((NEt4+)3)3 salt) [5]
[Ti2Cl10]2−colourlessd0d0 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png bioctahedral
[Ti3Cl12]3-green(t2g)1(t2g)1(t2g)1 Face-shared-trioctahedral-dodecachlorotrimetallate-3D-bs-20.png face-sharing trioctahedronTi-Ti = 3.19, 3.10 Å (terminal)
Ti-C1(terminal) = 2.36 Å (terminal),
Ti-Cl(bridge) = 2.50 Å
((PPh4+)3)3 salt) [6]
[TiCl6]2−yellowd0 Octahedral-hexachlorometallate-3D-bs-20.png octahedralPPh4+ salt
Ti-Cl = 2.33 Å [7]
VCl4 red(t2g)1 Tetrahedral-tetrachlorometallate-3D-bs-20.png tetrahedralV1−Cl = 2.29 Å
V2Cl10 violet(t2g)0 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png edge-shared bioctahedronV1−Cl(bridging) = 2.48 Å
V1−Cl(terminal) = 2.16-2.21 Å [8]
[VCl6]2-red(t2g)1 Octahedral-hexachlorometallate-3D-bs-20.png octahedralV1−Cl = 2.29 Å [9]
[CrCl6]3−pink [3] (t2g)3 Octahedral-hexachlorometallate-3D-bs-20.png octahedral [10] [3]
[Cr2Cl9]3−red(d3)2 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png face-sharing bioctahedronCr-Cl(terminal) = 2.31 Å, 2.42 (terminal)
(Et2NH2+ salt) [11]
[MnCl4]2− [12] pale pink to while(eg)2(t2g)3 Tetrahedral-tetrachlorometallate-3D-bs-20.png tetrahedralMn-Cl bond length = 2.3731-2.3830 Å [13]
[MnCl6]2−dark red(t2g)3(eg)1 Octahedral-hexachlorometallate-3D-bs-20.png octahedralMn-Cl distance = 2.28 Å
K+ salt [14] )
salt is isostructural with K2PtCl6
[MnCl6]3−brown [3] (t2g)3(eg)1 Octahedral-hexachlorometallate-3D-bs-20.png octahedral [10] [3]
[Mn2Cl6]2−yellow-green(eg)2(t2g)3 Bitetrahedral-hexachlorometallate-3D-bs-20.png bitetrahedralMn-Cl(terminal) bond length = 2.24 Å
Mn-Cl(terminal) bond length = 2.39 Å [15]
(PPN+)2 salt
[Mn3Cl12]6−pink(t2g)3(eg)2 Face-shared-trioctahedral-dodecachlorotrimetallate-3D-bs-20.png cofacial trioctahedronMn-Cl distance = --- Å
[(C(NH2)3]+ 6 salt [16]
[FeCl4]2− [12] cream(eg)3(t2g)3 Tetrahedral-tetrachlorometallate-3D-bs-20.png tetrahedral((Et4N+)2 salt) [12]
[FeCl4]− (eg)2(t2g)3 Tetrahedral-tetrachlorometallate-3D-bs-20.png tetrahedralFe-Cl bond length = 2.19 Å [17]
[FeCl6]3−orange(t2g)3(eg)2 Octahedral-hexachlorometallate-3D-bs-20.png octahedral [3]
[Fe2Cl6]2−pale yellow(eg)2(t2g)3 Bitetrahedral-hexachlorometallate-3D-bs-20.png bitetrahedralFe-Cl(terminal) bond length = 2.24 Å
Fe-Cl(terminal) bond length = 2.39 Å [15]
(PPN+)2 salt
[CoCl4]2− [12] blue [12] (eg)4(t2g)3 Tetrahedral-tetrachlorometallate-3D-bs-20.png tetrahedral
[Co2Cl6]2−blue [15] (eg)4(t2g)3 Bitetrahedral-hexachlorometallate-3D-bs-20.png bitetrahedralMn-Cl(terminal) bond length = 2.24 Å
Co-Cl(terminal) bond length = 2.35 Å [15]
(PPN+)2 salt
[NiCl4]2− [12] blue [12] (eg)4(t2g)4 Tetrahedral-tetrachlorometallate-3D-bs-20.png tetrahedralNi-Cl bond length = 2.28 Å
(Et4N+)2 salt [18]
[Ni3Cl12]6−orange [19] (t2g)6(eg)2 Face-shared-trioctahedral-dodecachlorotrimetallate-3D-bs-20.png confacial trioctahedral((Me2NH2+)2)8 salt
double salt with two Cl−
Ni-Cl bond length = 2.36-2.38 Å [19]
[CuCl4]2− [12] orange [20]
yellow (flattened tetrahedral) [21]
green (square planar) [22] 		(t2g)6(eg)3 Flattened-tetrahedral-tetrachlorometallate-3D-bs-20.png flattened tetrahedral
or square planar [23] [24] 		Cu-Cl bond length = 2.24 Å
[Cu2Cl6]2−red[(t2g)6(eg)3]2 Edge-shared-bis-square-planar-hexachlorodimetallate-3D-bs-20.png edge-shared bis(square planar) [25] Cu-Cl(terminal) = 2.24 Å
Cu-Cl(bridging) = 2.31 Å
[ZnCl4]2−white/colorlessd10 Tetrahedral-tetrachlorometallate-3D-bs-20.png tetrahedral

2nd row

Some homoleptic complexes of the second row transition metals feature metal-metal bonds.

2nd Transition Series
Complexcolourelectron config.structuregeometrycomments
[ZrCl6]2−yellowd0 Octahedral-hexachlorometallate-3D-bs-20.png octahedralZr-Cl distance = 2.460 Å
(Me4N+)2 salt [27]
[Zr2Cl10]2−colorless(d0)2 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png edge-shared bioctahedralZr-Cl = 2.36 Å (terminal), 2.43 Å (bridging)
N(PCl3)2)+ salt [4]
Nb2Cl10 yellow(d0)2 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png edge-shared bioctahedral [Nb2Cl10]3.99 Å [28]
[NbCl6]−yellowd0 Octahedral-hexachlorometallate-3D-bs-20.png octahedralNb-Cl = 2.34 Å
N(PCl3)2)+ salt [4]
[Nb6Cl18]2−black(d2)4(d3)2 (14 cluster electrons) Octahedral-octadecachlorohexametallate-3D-bs-20.png cluster Nb---Nb bondingNb-Cl = 2.92 Å
(K+)2 salt [29]
MoCl6 blackd0 Octahedral-hexachlorometallate-3D-bs-20.png octahedronMo−Cl = 2.28 -2.31 Å [8]
[MoCl6]2−yellow(t2g)2 Octahedral-hexachlorometallate-3D-bs-20.png octahedronMo−Cl = 2.37, 2.38, 2.27 Å [30]
[MoCl6]3−pink(t2g)3 Octahedral-hexachlorometallate-3D-bs-20.png octahedral
[Mo2Cl8]4− purple [31] 2(d4) Octachlorodimetallate-view-2-3D-bs-20.png Mo-Mo quadruple bond
[Mo2Cl9]3−2(d3) Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png face-shared bioctahedralMo-Mo (triple) bond length = 2.65 Å
Mo-Cl (terminal) bond length = 2.38 Å
Mo-Cl (bridging) bond length = 2.49 Å [32] [33]
Mo2Cl10 green(d1)2 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png edge-sharing bioctahedra [34]
[Mo2Cl10]2−(d2)2 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png edge-sharing bioctahedra [35]
[Mo5Cl13]2−brown [31] d2d2d2d2d3 Tridecachloropentametallate-3D-bs-20.png incomplete octahedron [36]
[Mo6Cl14]2− yellowd4 Tetradecachlorohexametallate-3D-bs-20.png octahedral cluster(4-HOPyH+)2 salt [37]
[TcCl6]2−yellow(t2g)3 Octahedral-hexachlorometallate-3D-bs-20.png octahedronTc-Cl = 2.35 Å for As(C6H5)4+ salt [38]
[Tc2Cl8]2−green(t2g)4 Octachlorodimetallate-view-2-3D-bs-20.png Tc-Tc quadruple bondTc-Tc = 2.16, Tc-Cl = 2.34 Å for NBu4+ salt [39]
[RuCl6]2−brown(t2g)4 Octahedral-hexachlorometallate-3D-bs-20.png octahedral(EtPPh3+)2 salt [40]
[Ru2Cl9]3−red[(t2g)5]2 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png cofacial bioctahedralRu-Ru bond length = 2.71 Å; Ru-Cl(terminal) = 2.35 Å, Ru-Cl(bridging) = 2.36 Å ((Et4N)+)3 salt [41]
[Ru3Cl12]4−green(d5)2(d6) Face-shared-trioctahedral-dodecachlorotrimetallate-3D-bs-20.png cofacial trioctahedralRu-Ru bond lengths = 2.86 Å
Ru-Cl bond lengths = 2.37-2.39 Å
(Et4N+)2(H7O3+)2 salt [42]
[RhCl6]3−red(t2g)6 Octahedral-hexachlorometallate-3D-bs-20.png octahedralH2N+(CH2CH2NH3+)2 salt) [43]
[Rh2Cl9]3−red-brown(t2g)6 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png octahedralRh-Cl(terminal) = 2.30 Å, Rh-Cl(terminal) = 2.40 Å
((Me3CH2Ph)+)3 salt) [32]
[PdCl4]2−brownd8 Square-planar-tetrachlorometallate-view-3-3D-bs-20.png square planar
[Pd2Cl6]2− [44] red ((Et4N+)2 salt)d8 Edge-shared-bis-square-planar-hexachlorodimetallate-3D-bs-20.png square planar
[Pd3Cl8]2− [45] orange brown ((Bu4N+)2 salt)d8 Octachlorotrimetallate-3D-bs-20.png square planar
[PdCl6]2−brownd6 Octahedral-hexachlorometallate-3D-bs-20.png octahedralPd(IV)
[Pd6Cl12]yellow-brownd8 Dodecachlorohexametallate-3D-bs-20.png square planar [46]
[AgCl2]−white/colorlessd10 Linear-dichlorometallate-3D-bs-20.png linearsalt of [K(2.2.2-crypt)]+ [47]
[CdCl4]2−white/colorlessd10 Tetrahedral-tetrachlorometallate-3D-bs-20.png tetrahedralEt4N+ salt, Cd-Cl distance is 2.43 Å [26]
[Cd2Cl6]2−white/colorlessd10 Bitetrahedral-hexachlorometallate-3D-bs-20.png edge-shared bitetrahedron(C6N3(4-C5H4N)33+ salt [48]
[Cd3Cl12]6−white/colorlessd10 Face-shared-trioctahedral-dodecachlorotrimetallate-3D-bs-20.png octahedral (central Cd)
pentacoordinate (terminal Cd's)
cofactial trioctahedral		(C6N3(4-C5H4N)33+ salt [48]
(3,8-Diammonium-6-phenylphenanthridine3+)2 [49]
[Cd6Cl19]7−white/colorlessd10 Octahedral-nonadecachlorohexametallate-3D-bs-20.png octahedron of octahedra4,4'-(C6H3(2-Et)NH3+)2 salt [50]

3rd row

3rd Transition Series
Complexcolourelectron config.structuregeometrycomments
[HfCl6]2−whited0 Octahedral-hexachlorometallate-3D-bs-20.png octahedralHf-Cl distance = 2.448 A
((Me4N+)2 salt) [27]
[Hf2Cl10]2−colorless/whited0 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png edge-shared bioctahedral [51]
[Hf2Cl9]−colorless/white(d0)2 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png face-shared bioctahedral [52]
[TaCl5]whited0 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png edge-shared bioctahedral
[TaCl6]−white/colourlessd0 Octahedral-hexachlorometallate-3D-bs-20.png octahedralTa-Cl = 2.34 Å
(N(PCl3)2)+ salt) [4]
[Ta6Cl18]2-greend0 Octahedral-hexachlorometallate-3D-bs-20.png octahedralTa-Ta = 2.34 Å
(H+2 salt hexahydrate [53]
WCl6 blued0 Octahedral-hexachlorometallate-3D-bs-20.png octahedral2.24–2.26 Å [54]
[WCl6]2−(t2g)2 Octahedral-hexachlorometallate-3D-bs-20.png octahedralW-Cl distances range from 2.34 to 2.37 Å
(PPh4+ salt) [55]
[WCl6]−(t2g)1 Octahedral-hexachlorometallate-3D-bs-20.png octahedralW-Cl distance = 2.32 Å
(Et4N+ salt) [56]
W2Cl10 black [57] (t2g1)2 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png bioctahedralW-W distance = 3.814 Å [58]
[W2Cl8]4−blue2(d4) Octachlorodimetallate-view-2-3D-bs-20.png W-W quadruple bonddW-W = 2.259 Å [Na(tmeda)+]4 salt [59]
[W2Cl9]2−d3d2 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png face-sharing bioctahedralW-W distance = 2.54 Å
W-Cl(terminal) = 2.36 Å, W-Cl(bridge) = 2.45 Å
((PPN+)2 salt) [60]
[W2Cl9]3−d3d3 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png octahedralW-Cl distance = 2.32 Å
(Et4N+ salt) [60]
[W3Cl13]3−d3,d3,d4 Tridecachlorotrimetallate-3D-bs-20.png [W3(μ3-Cl)(μ-Cl)3Cl9]3-W-W distances = 2.84 Å [61]
[W3Cl13]2−d3,d4,d4 Tridecachlorotrimetallate-3D-bs-20.png [W3(μ3-Cl)(μ-Cl)3Cl9]2- [61] W-W distances = 2.78 Å [61]
[W6Cl14]2-yellow [62] (d4)6 Tetradecachlorohexametallate-3D-bs-20.png see Mo6Cl12
[ReCl6]−red-brown(t2g)2 Octahedral-hexachlorometallate-3D-bs-20.png octahedralRe-Cl distance = 2.24-2.31 Å
(PPh4+ salt) [63]
[ReCl6](t2g)1 Octahedral-hexachlorometallate-3D-bs-20.png octahedralRe-Cl distance = 226.3(6) Å [8]
[ReCl6]2−green(t2g)3 Octahedral-hexachlorometallate-3D-bs-20.png octahedralRe-Cl distance = 2.35-2.38 Å
((PPN+)2 salt) [64]
[Re2Cl9]2−(t2g)3(t2g)4 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png face-sharing bioctahedralRe-Re distance = 2.48 Å
Re-Cl distances = 2.42 Å (bridge), 2.33 Å (terminal)
((Et4N+)2 salt) [65]
[Re2Cl9]−((t2g)3)2 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png face-sharing bioctahedralRe-Re distance = 2.70 Å
Re-Cl distances = 2.41 (bridge), 2.28 Å (terminal)
(Bu4N+ salt) [65]
[OsCl6]−dark green(t2g)3 Octahedral-hexachlorometallate-3D-bs-20.png octahedraldOs-Cl = 2.30 Å for Et4N+ [66] and Ph4P+ [67] salts
[OsCl6]2−yellow-orange(t2g)4 Octahedral-hexachlorometallate-3D-bs-20.png octahedral [67] Os-Cl distance 2.33 Å
[Os2Cl8]2−green(d5)2 Square-antiprismatic-octachlorodimetallate-view-2-3D-bs-20.png square antiprismdOs-Os = 2.182 Å, dOs-Cl = 2.32 Å (Bu4N+)2 salt [68]
[Os2Cl10]2−green(d4)2 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png octahedraldOs-Cl(terminal) = 2.30 Å dOs-Cl(bridging) = 2.42 Å (Et4N+)2 salt [66]
[IrCl6]3−red(t2g)6 Octahedral-hexachlorometallate-3D-bs-20.png octahedralIr-Cl = 2.36 Å [69]
[IrCl6]2−brown(t2g)5 Octahedral-hexachlorometallate-3D-bs-20.png octahedralIr-Cl = 2.33 Å [70]
[Ir2Cl9]3−-((t2g)6)2 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png bi-octahedral [71]
[PtCl4]2−pinkd8 Square-planar-tetrachlorometallate-view-3-3D-bs-20.png square planar
[PtCl6]2−yellowd6 Octahedral-hexachlorometallate-3D-bs-20.png octahedralPt-Cl distance = 2.32 Å
Et4N+ salt, ((Me4N+)2 salt) [27]
[Pt2Cl9]−red (Bu4N+ salt)((t2g)6)2 Face-shared-bioctahedral-nonachlorodimetallate-3D-bs-20.png octahedralPt-Clt and Pt-Clbridge = 2.25, 2.38 Å [72]
[Pt2Cl10]2−yellow-brown (PPN+ salt)((t2g)6)2 Edge-shared-bioctahedral-decachlorodimetallate-3D-bs-20.png edge-shared bioctahedralPt-Clt and Pt-Clbridge = 2.27, 2.37 Å [72]
[Pt6Cl12]yellow-brown(d8)6 Dodecachlorohexametallate-3D-bs-20.png square planarPt-Cl = 2.31 [73]
[AuCl2]−white/colorlessd10 Linear-dichlorometallate-3D-bs-20.png linearAu-Cl distances of 2.28 Å
NEt4+ salt [74]
Au4Cl8 black(d10)2(d8)2 Au4Cl8-structure-based-on-xtal-3D-bs-20.png linear and square planarrare example of mixed valence, molecular chloride [75]
[AuCl4]−yellowd8 Square-planar-tetrachlorometallate-view-3-3D-bs-20.png square planarAu-Cl distances of 2.26 Å
NBu4+ salt [76]
[HgCl4]2−white/colorlessd10 Tetrahedral-tetrachlorometallate-3D-bs-20.png tetrahedralHg-Cl distance is 2.46 Å [26]
Et4N+ salt
[Hg2Cl6]2−white/colorlessd10 Bitetrahedral-hexachlorometallate-3D-bs-20.png edge-shared bitetrahedralHg-Cl distance is 2.46 Å [77]
Bu4N+ salt

Heteroleptic complexes

Heteroleptic complexes containing chloride are numerous. Most hydrated metal halides are members of this class. Hexamminecobalt(III) chloride and Cisplatin (cis-Pt(NH3)2Cl2) are prominent examples of metal-ammine-chlorides.

Hydrates

"Nickel dichloride hexahydrate" consists of the chloride complex trans-[NiCl2(H2O)4 plus water of crystallization. MCl2(aq)6forFeCoNi.png
"Nickel dichloride hexahydrate" consists of the chloride complex trans-[NiCl2(H2O)4 plus water of crystallization.

As indicated in the table below, many hydrates of metal chlorides are molecular complexes. [78] [79] These compounds are often important commercial sources of transition metal chlorides. Several hydrated metal chlorides are not molecular and thus are not included in this tabulation. For example the dihydrates of manganese(II) chloride, nickel(II) chloride, copper(II) chloride, iron(II) chloride, and cobalt(II) chloride are coordination polymers.

Formula of
hydrated metal halides		Coordination
sphere of the metal
TiCl3(H2O)6 trans-[TiCl2(H2O)4]+ [80]
VCl3(H2O)6 trans-[VCl2(H2O)4]+ [80]
CrCl3(H2O)6 trans-[CrCl2(H2O)4]+
CrCl3(H2O)6 [CrCl(H2O)5]2+
CrCl2(H2O)4 trans-[CrCl2(H2O)4]
CrCl3(H2O)6 [Cr(H2O)6]3+ [81]
MnCl2(H2O)6 trans-[MnCl2(H2O)4]
MnCl2(H2O)4 cis-[MnCl2(H2O)4] [82]
FeCl2(H2O)6 trans-[FeCl2(H2O)4]
FeCl2(H2O)4 trans-[FeCl2(H2O)4]
FeCl3(H2O)6 one of four hydrates of ferric chloride, [83]
FeCl3(H2O)2.5 cis-[FeCl2(H2O)4]+ [84]
CoCl2(H2O)6 trans-[CoCl2(H2O)4]
CoCl2(H2O)4 cis-[CoCl2(H2O)4]
NiCl2(H2O)6 trans-[NiCl2(H2O)4]
NiCl2(H2O)4 cis-[NiCl2(H2O)4]

Adducts

Metal chlorides form adducts with ethers to give transition metal ether complexes.

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<span class="mw-page-title-main">Monofluorophosphate</span> Chemical compound

Monofluorophosphate is an anion with the formula PO3F2−, which is a phosphate group with one oxygen atom substituted with a fluoride atom. The charge of the ion is −2. The ion resembles sulfate in size, shape and charge, and can thus form compounds with the same structure as sulfates. These include Tutton's salts and langbeinites. The most well-known compound of monofluorophosphate is sodium monofluorophosphate, commonly used in toothpaste.

<span class="mw-page-title-main">Difluorophosphate</span> Chemical compound

Difluorophosphate or difluorodioxophosphate or phosphorodifluoridate is an anion with formula PO2F−2. It has a single negative charge and resembles perchlorate and monofluorosulfonate in shape and compounds. These ions are isoelectronic, along with tetrafluoroaluminate, phosphate, orthosilicate, and sulfate. It forms a series of compounds. The ion is toxic to mammals as it causes blockage to iodine uptake in the thyroid. However it is degraded in the body over several hours.

The telluride iodides are chemical compounds that contain both telluride ions (Te2−) and iodide ions (I−). They are in the class of mixed anion compounds or chalcogenide halides.

Sulfidostannates, or thiostannates are chemical compounds containing anions composed of tin linked with sulfur. They can be considered as stannates with sulfur substituting for oxygen. Related compounds include the thiosilicates, and thiogermanates, and by varying the chalcogen: selenostannates, and tellurostannates. Oxothiostannates have oxygen in addition to sulfur. Thiostannates can be classed as chalcogenidometalates, thiometallates, chalcogenidotetrelates, thiotetrelates, and chalcogenidostannates. Tin is almost always in the +4 oxidation state in thiostannates, although a couple of mixed sulfides in the +2 state are known,

A chloride nitride is a mixed anion compound containing both chloride (Cl−) and nitride ions (N3−). Another name is metallochloronitrides. They are a subclass of halide nitrides or pnictide halides.

A Phosphide chloride is a mixed anion compound containing both phosphide (P3−) and chloride (Cl−) ions.

Arsenide bromides or bromide arsenides are compounds containing anions composed of bromide (Br−) and arsenide (As3−). They can be considered as mixed anion compounds. They are in the category of pnictidehalides. Related compounds include the arsenide chlorides, arsenide iodides, phosphide bromides, and antimonide bromides.

Arsenide chlorides or chloride arsenides are compounds containing anions composed of chloride (Cl−) and arsenide (As3−). They can be considered as mixed anion compounds. They are in the category of pnictidehalides. Related compounds include the arsenide bromides, arsenide iodides, phosphide chlorides, and antimonide chlorides.

An iodide nitride is a mixed anion compound containing both iodide (I−) and nitride ions (N3−). Another name is metalloiodonitrides. They are a subclass of halide nitrides or pnictide halides. Some different kinds include ionic alkali or alkaline earth salts, small clusters where metal atoms surround a nitrogen atom, layered group 4 element 2-dimensional structures, and transition metal nitrido complexes counter-balanced with iodide ions. There is also a family with rare earth elements and nitrogen and sulfur in a cluster.

Carbide chlorides are mixed anion compounds containing chloride anions and anions consisting entirely of carbon. In these compounds there is no bond between chlorine and carbon. But there is a bond between a metal and carbon. Many of these compounds are cluster compounds, in which metal atoms encase a carbon core, with chlorine atoms surrounding the cluster. The chlorine may be shared between clusters to form polymers or layers. Most carbide chloride compounds contain rare earth elements. Some are known from group 4 elements. The hexatungsten carbon cluster can be oxidised and reduced, and so have different numbers of chlorine atoms included.

<span class="mw-page-title-main">Transition metal ether complex</span>

In chemistry, a transition metal ether complex is a coordination complex consisting of a transition metal bonded to one or more ether ligand. The inventory of complexes is extensive. Common ether ligands are diethyl ether and tetrahydrofuran. Common chelating ether ligands include the glymes, dimethoxyethane (dme) and diglyme, and the crown ethers. Being lipophilic, metal-ether complexes often exhibit solubility in organic solvents, a property of interest in synthetic chemistry. In contrast, the di-ether 1,4-dioxane is generally a bridging ligand.

Indium(I) chloride is the chemical compound with the formula InCl. Indium monochloride occurs as a yellow cubic form below 120 °C and above this temperature as a red orthorhombic form. InCl is one of three known indium chlorides.

References

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