The borosulfates are heteropoly anion compounds which have sulfate groups attached to boron atoms. Other possible terms are sulfatoborates or boron-sulfur oxides. The ratio of sulfate to borate reflects the degree of condensation. With [B(SO4)4]5- there is no condensation, each ion stands alone. In [B(SO4)3]3- the anions are linked into a chain, a chain of loops, or as [B2(SO4)6]6− in a cycle. Finally in [B(SO4)2]− the sulfate and borate tetrahedra are all linked into a two or three-dimensional network. These arrangements of oxygen around boron and sulfur can have forms resembling silicates. The first borosulfate to be discovered was K5[B(SO4)4] in 2012. [1] Over 75 unique compounds are known.
They are distinct from the borate sulfates which have separate, uncondensed sulfate and borate ions.
Related compounds include boroselenates, borotellurates, [2] and also boroantimonates, borogallates, borogermanates, borophosphates, boroselenites and borosilicates. [3]
Borosulfates are formed by heating boric oxide, oleum, or sulfuric acid, with metal carbonates. The degree of condensation is varied with the ratio of oleum to sulfuric acid. Pure oleum is more likely to yield compounds with disulfate groups.
When heated to around 500 °C the borosulfates decompose by emitting SO3 vapour and form a metal sulfate and boric oxide. [4]
chem | mw | crystal system | space group | unit cell Å | volume | density | comment | references | |
---|---|---|---|---|---|---|---|---|---|
boron sulfate | B2S2O9 | 229.74 | monoclinic | C2 | a=7.7600 b=4.1664 c=8.6134 β=94.785 Z=2 | 277.51 | 2.749 | no cations; 3D mesh | [5] |
H[B(HSO4)4] | monoclinic | P21/c | a=15.6974, b=11.436, c=8.5557; β=90.334°; Z=8 | superacid | [6] [7] | ||||
H3O[B(SO4)2] | P4/ncc | a=9.1377, c=7.3423; Z=4 | [7] | ||||||
H[B(SO4)(S2O7)] | monoclinic | P21/c | a=15.697 b=11.4362 c=8.5557 β=90.334 | [2] | |||||
Li[B(SO4)2] | Pc | a = 7.635, b = 9.342, c = 8.432, and β = 92.55° | 3D network, like tectosilicate | [6] [8] | |||||
Li[B(S2O7)2] | orthorhombic | P212121 | a = 10.862, b = 10.877, c = 17.769 | [6] [8] | |||||
Li5[B(SO4)4] | orthorhombic | P21/c | a=8.0191 b=10.2111 c=15.0401 | [2] | |||||
Be[B2(SO4)4] | monoclinic | C2/c | a= 23.856, b= 7.3507, c= 12.3235, β= 98.724(2)°, Z=8 | 2136.1 | 2.58 | colourless | [9] | ||
NH4[B(SO4)2] | P4/ncc | a=9.1980 c=7.2458 | decompose 320 °C, proton conductor | [2] [10] | |||||
NH4[B(S2O7)2] | monoclinic | Cc | a=11.4403 b=14.9439 c=13.8693 β=93.662 | [6] [2] | |||||
(NH4)2B4SO10 | 271.38 | monoclinic | C2 | a=11.3685 b=6.5541 c=12.8328 β=106.247 4 | 918.0 | 1.964 | SHG 1.1 × KDP; min PM wavelength 252 nm; decompose 300 °C | [11] | |
[NH4]3[B(SO4)3] | 343.12 | orthorhombic | Ibca | a=7.2858 b=14.7048 c=22.7052 Z=8 | 2433.2 | 1.928 | decompose 320 °C chains | [12] [1] | |
Na[B(SO4)2] | monoclinic | P2/c | a=5.434 b=7.570 c=7.766 β=99.74 | [2] | |||||
Na[B(S2O7)2] | monoclinic | P21/c | a=10.949, b=8.49, c=12.701; β=110.227°; Z=4 | [6] [7] | |||||
Na5[B(SO4)4]-I | orthorhombic | Pca21 | a = 10.730, b = 13.891, c = 18.197 | [8] | |||||
Na5[B(SO4)4]-II | orthorhombic | P212121 | a = 8.624, b = 9.275, c = 16.671 | [8] | |||||
α-Mg4[B2O(SO4)6] | 711.22 | trigonal | P3 | a=8.0165 c=7.4858 Z=1 | 416.62 | 2.835 | colourless | [4] | |
β-Mg4[B2O(SO4)6] | 711.22 | hexagonal | P3 | a = 13.9196, c = 7.4854, Z = 3 | 1253 | 2.821 | colourless | [4] | |
Mg[B2(SO4)4] | 430.17 | monoclinic | C2/c | a = 17.443, b = 5.3145, c = 14.2906 β = 126.323° Z = 4 | 1067.3 | 2.677 | phyllosilicate structure colourless decompose 550 °C | [4] | |
β-Mg[B2(SO4)4] | monoclinic | P21/n | a=7.9100 b=8.0815 c=9.0376 β=111.37° Z=2 | 269.01 | 2.667 | colourless decompose 550 °C | [13] | ||
K[B(SO4)2] | P4/ncc | a=8.9739 c=7.4114 | [2] | ||||||
K[B(S2O7)2] | monoclinic | Cc | a=11.3368, b=14.66, c=13.6650; β=94.235°; Z=8 | [6] [7] | |||||
pentapotassium borosulfate | K5[B(SO4)4] | P41 | a=9.9023 c=16.1871 | 1687.2 | 2.471 | first discovered | [6] [14] | ||
K3[B(SO4)3] | orthorhombic | Ibca | a = 7.074, b = 14.266, c = 22.58 | [6] [8] | |||||
K4[BS4O15(OH)] | monoclinic | I2/a | a=14.524 b=7.3916 c=15.7857 β=115.50 | [2] | |||||
CaB2S4O16 | monoclinic | P21/c | a=5.5188 b=15.1288 c=13.2660 β=92.88 | sheet | [2] | ||||
Mn[B2(SO4)4] | monoclinic | P21/n | a = 8.0435, b = 7.9174, c = 9.3082, β = 110.94° Z=2 | 553.63 | colourless | [15] | |||
α-Mn4[B2O(SO4)6] | 833.74 | trigonal | P3 | a=8.1086 c=7.7509 Z=1 | 441.3 | 3.137 | colourless | [4] | |
β-Mn4[B2O(SO4)6] | 833.74 | trigonal | P3 | a=13.9196 c=7.4854 | |||||
α-Co[B2(SO4)4] | monoclinic | C2/c | a=17.4254 b=5.3397 c=14.3214 β=126.03° Z=4 | 269.40 | 2.860 | pink | [13] | ||
β-Co[B2(SO4)4] | monoclinic | P21/n | a=7.8892 b=8.1042 c= 9.0409 β=111.29° Z=2 | 269.29 | 2.803 | pink | [13] | ||
α-Co4[B2O(SO4)6] | 849.70 | trigonal | P3 | a=7.991 c=7.669 Z=1 | 418.0 | 3.376 | pink | [4] | |
α-Ni4[B2O(SO4)6] | 848.82 | trigonal | P3 | a=7.9359 c=7.4398 Z=1 | 405.77 | 3.474 | yellow | [4] | |
Cu[B(SO4)2(HSO4)] | triclinic | P1 | a=5.3096 b=7.0752 c=11.1977 α=81.154 β=80.302 γ=80.897 | cyclic | [2] | ||||
Cu[B2(SO4)4] | triclinic | P1 | a=5.2470 b=7.1371 c=7.9222 α=73.814 β=70.692 γ=86.642 | chain | [2] | ||||
Zn[B2(SO4)4] | monoclinic | P21/n | a = 8.0435, b = 7.9174, c = 9.3082, β = 111.26° Z=2 | 534.36 | colourless | [15] | |||
α-Zn4[B2O(SO4)6] | 875.46 | trigonal | P3 | a=7.9971 c=7.4895 Z=1 | 414.81 | 3.505 | colourless | [4] | |
Rb3[B(SO4)3] | orthorhombic | Ibca | a = 7.2759, b = 14.794, c = 22.637 | [8] | |||||
Rb4[B2O(SO4)4] | orthorhombic | Pnma | a=8.0415 b=10.647 c=20.425 | [2] | |||||
Rb5[B(SO4)4] | tetragonal | P43212 | a=10.148 c=16.689 Z=4 | band gap 3.99 eV | [2] [16] | ||||
Rb3HB4S2O14 | P63/m | a = 6.502, c = 19.02 Z=2 | [17] | ||||||
LiRb4[B(SO4)4] | 743.8 | monoclinic | a=7.5551, c=14.560, c=7.5517 β=90.2372 Z=2 | transparent | [18] | ||||
LiRb4[B(SO4)4] | 743.8 | tetragonal | I4 | a=7.6128, c=14.631, Z=2 | at 500K | [18] | |||
Sr[B2(SO4)4] | 493.48 | orthorhombic | Pnma | a=12.574 b=12.421 c=7.319 Z=4 | 1143.1 | 2.867 | decompose 400 °C | [6] [1] | |
Sr[B2(SO4)3(S2O7)] | 573.54 | monoclinic | P21/n | a = 7.470, b = 15.334, c = 12.220, β = 93.29° Z=4 | 1397.5 | 2.726 | [6] | ||
Sr[B2O(SO4)3] | orthorhombic | Pnma | a=1657.3 b=12.037 c=4.39484 | [6] [2] | |||||
Sr[B3O(SO4)4(SO4H)] | 617.36 | monoclinic | P21/c | a = 11.3309, b= 7.1482, c = 19.355, β = 106.878°, Z = 4 | 1500.1 | 2.73 | colourless; Sr in 9 coordination by sulfate oxygens | [19] | |
Y2[B2(SO4)6] | monoclinic | C2/c | a=13.5172 b=11.3941 c=10.8994 β=93.447 | cyclic | [12] [2] | ||||
Ag[B(SO4)2] | P4/ncc | a=8.6679 c=7.2897 | [2] | ||||||
Ag[B(S2O7)2] | monoclinic | P21/c | a = 9.507, b = 9.601, c = 11.730, β = 98.35° Z=4 | 1059.3 | 2.953 | colourless | [20] | ||
Cd[B2(SO4)4] | [21] | ||||||||
Cd[B2O(SO4)3] | 438.20 | orthorhombic | Pnma | a=8.9692 b=11.520 c=8.7275 Z=4 | 901.8 | 3.23 | colourless | [21] | |
Cd4[B2O(SO4)6] | trigonal | P3 | a=8.2222 c=7.9788 Z=1 | 467.14 | 3.78 | colourless | [21] | ||
(I4)[B(S2O7)2]2 | triclinic | P1 | a = 11.3714 b = 11.5509 c = 12.7811 α = 68.638° β = 68.275° γ = 64.626° Z=2 | 1366.16 | 2.999 | orange-brown | [22] | ||
Cs2[B2O(SO4)3] | monoclinic | P2/c | a=14.765 b=6.710 c=12.528 β=104.50 | [17] | |||||
Cs3HB4S2O14 | P63/m | a = 6.5648, c = 19.5669 Z=2 | [17] | ||||||
Cs[B(SO4)(S2O7)] | monoclinic | P21/c | a=10.4525, b=11.319, c=8.2760; β=103.206; Z=4 | [6] [7] | |||||
Cs3Li2[B(SO4)4] | monoclinic | P21/n | a=13.7698 c=8.2376 c=13.9066 β=91.778 | [12] [2] | |||||
Cs3Na2[B(SO4)4] | monoclinic | P21/c | a=13.6406 b=7.9475 c=13.9573 β=990.781 | [12] [2] | |||||
CsK4[B(SO4)4] | P43212 | a=9.9433 c=16.881 | [12] [2] | ||||||
Ba[B2(SO4)4] | orthorhombic | Pnna | a = 12.791, b = 12.800, c = 7.317 Z = 4 | [6] [23] | |||||
Ba[B2O(SO4)3] | orthorhombic | Pnma | a=17.1848 b=12.3805 c=4.4226 | [6] | |||||
Ba[B(S2O7)2]2 | monoclinic | I2/a | a = 11.6077, b = 8.9144, c = 21.303, β = 104.034° Z = 4 | chains | [6] [23] | ||||
La2[B2(SO4)6] | monoclinic | C2/c | a=1379.2 b=1158.9 c=1139.5 β=93.611 | cyclic | [12] [2] | ||||
Ce2[B2(SO4)6] | monoclinic | C2/c | 13.740 b=11.5371 c=11.3057 β=93.661 | cyclic | [12] [2] | ||||
Pr2[B2(SO4)6] | monoclinic | C2/c | a=13.711 b=11.5305 c=11.2643 β=93.668 | cyclic | [12] [2] | ||||
Nd2[B2(SO4)6] | monoclinic | C2/c | a=13.6775 b=11.51.34 11.2046 β=93.5909 | cyclic | [12] [2] | ||||
Sm2[B2(SO4)6] | monoclinic | C2/c | a=13.633 b=11.492 c=11.112 β=93.567 | cyclic | [12] [2] | ||||
Eu2[B2(SO4)6] | monoclinic | C2/c | a=13.602 b=11.470 c=11.050 β=93.465 | cyclic | [12] [2] | ||||
Gd2[B2(SO4)6] | monoclinic | C2/c | a=13.5697 b=11.4426 c=11.0271 β= | cyclic | [12] [2] | ||||
Tb2[B2(SO4)6] | monoclinic | C2/c | a=13.5601 b=11.42.48 c=10.9881 β=93.534 | cyclic | [12] [2] | ||||
Dy2[B2(SO4)6] | monoclinic | C2/c | a=13.568 b=11.425 c=10.9703 β=93.540 | cyclic | [12] [2] | ||||
Ho2[B2(SO4)6] | monoclinic | C2/c | a=13.505 b=11.409 c=10.921 β=93.453 | cyclic | [12] [2] | ||||
Er2[B2(SO4)6] | monoclinic | C2/c | a=13.551 b=11.411 c=10.882 β=93.41 | cyclic | [12] [2] | ||||
Tm2[B2(SO4)6] | monoclinic | C2/c | a=13.4981 b=11.3617 10.8327 β=93.4500 | cyclic | [12] [2] | ||||
Yb2[B2(SO4)6] | monoclinic | C2/c | a=13.495 b=11.3452 c=10.7961 β=93.390 | cyclic | [12] [2] | ||||
Lu2[B2(SO4)6] | monoclinic | C2/c | a=13.469 b=11.364 c=10.799 β=93.369 | cyclic | [12] [2] | ||||
Pb[B2(SO4)4] | 613.05 | orthorhombic | Pnna | a=12.516 b=12.521 c=7.302 Z=4 | 114.43 | 3.558 | loop chain | [2] [24] | |
Pb[B2O(SO4)3] | orthorhombic | P21/m | a=4.4000 b=12.1019 c=8.6043 | [2] | |||||
Bi2[B2(SO4)6] | 659.08 | orthorhombic | C2/c | a = 13.568, b = 11.490, c = 11.106 Z=4 | 1728.8 | 3.894 | [12] | ||
(H3O)Bi[B(SO4)2]4 | 1039.72 | I4 | a=11.857, c=8.149 Z=2 | 1156.84 | 2.99 | colourless; non-linear optical | [12] | ||
(UO2)[B(SO4)2(SO3OH)] | 569.52 | triclinic | P1 | a=5.448 b=7.021 c=13.522 α =92.248° β =95.347° γ =101.987° Z=2 | 3.762 | green | [25] | ||
(UO2)2[B2O(SO4)3(SO3OH)2] | 1058.23 | monoclinic | P21/n | a=10.872 b=11.383 c=14.812 β=92.481 Z=4 | 3.838 | yellow | [25] |
In chemistry tellurate is a compound containing an oxyanion of tellurium where tellurium has an oxidation number of +6. In the naming of inorganic compounds it is a suffix that indicates a polyatomic anion with a central tellurium atom.
Silver sulfate is the inorganic compound with the formula Ag2SO4. It is a white solid with low solubility in water.
Alexander C. Filippou has been a Professor of Inorganic Chemistry at the Rheinische-Friedrich-Wilhelms-University Bonn since 2005.
Ulrich "Uli" Kortz is a German chemist and professor, working in the area of synthetic polyoxometalate chemistry.
The borate fluorides or fluoroborates are compounds containing borate or complex borate ions along with fluoride ions that form salts with cations such as metals. They are in the broader category of mixed anion compounds. They are not to be confused with tetrafluoroborates (BF4) or the fluorooxoborates which have fluorine bonded to boron.
An oxyhydride is a mixed anion compound containing both oxide O2− and hydride ions H−. These compounds may be unexpected as the hydrogen and oxygen could be expected to react to form water. But if the metals making up the cations are electropositive enough, and the conditions are reducing enough, solid materials can be made that combine hydrogen and oxygen in the negative ion role.
The selenide iodides are chemical compounds that contain both selenide ions (Se2−) and iodide ions (I−) and one or metal atoms. They are in the class of mixed anion compounds or chalcogenide halides.
The sulfate fluorides are double salts that contain both sulfate and fluoride anions. They are in the class of mixed anion compounds. Some of these minerals are deposited in fumaroles.
The nitridosilicates are chemical compounds that have anions with nitrogen bound to silicon. Counter cations that balance the electric charge are mostly electropositive metals from the alkali metals, alkaline earths or rare earth elements. Silicon and nitrogen have similar electronegativities, so the bond between them is covalent. Nitrogen atoms are arranged around a silicon atom in a tetrahedral arrangement.
The borophosphates are mixed anion compounds containing borate and phosphate anions, which may be joined together by a common oxygen atom. Compounds that contain water or hydroxy groups can also be included in the class of compounds.
The borotellurates are heteropoly anion compounds which have tellurate groups attached to boron atoms. The ratio of tellurate to borate reflects the degree of condensation. In [TeO4(BO3)2]8- the anions are linked into a chain. In [TeO2(BO3)4]10− the structure is zero dimensional with isolated anions. These arrangements of oxygen around boron and tellurium can have forms resembling silicates. The first borotellurates to be discovered were the mixed sodium rare earth compounds in 2015.
The boroselenates are chemical compounds containing interlinked borate and selenate groups sharing oxygen atoms. Both selenate and borate groups are tetrahedral in shape. They have similar structures to borosulfates and borophosphates. The borotellurates' tellurium atom is much bigger, so TeO6 octahedra appear instead.
Borate sulfates are mixed anion compounds containing separate borate and sulfate anions. They are distinct from the borosulfates where the borate is linked to a sulfate via a common oxygen atom.
Borate nitrates are mixed anion compounds containing separate borate and nitrate anions. They are distinct from the boronitrates where the borate is linked to a nitrate via a common oxygen atom.
The borate iodides are mixed anion compounds that contain both borate and iodide anions. They are in the borate halide family of compounds which also includes borate fluorides, borate chlorides, and borate bromides.
Arsenide iodides or iodide arsenides are compounds containing anions composed of iodide (I−) 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 bromides, phosphide iodides, and antimonide iodides.
Oxalate sulfates are mixed anion compounds containing oxalate and sulfate. They are mostly transparent, and any colour comes from the cations.
Homoleptic azido compounds are chemical compounds in which the only anion or ligand is the azide group, -N3. The breadth of homoleptic azide compounds spans nearly the entire periodic table. With rare exceptions azido compounds are highly shock sensitive and need to be handled with the upmost caution. Binary azide compounds can take on several different structures including discrete compounds, or one- two, and three-dimensional nets, leading some to dub them as "polyazides". Reactivity studies of azide compounds are relatively limited due to how sensitive they can be. The sensitivity of these compounds tends to be correlated with the amount of ionic or covalent character the azide-element bond has, with ionic character being far more stable than covalent character. Therefore, compounds such as silver or sodium azide – which have strong ionic character – tend to possess more synthetic utility than their covalent counterparts. A few other notable exceptions include polymeric networks which possess unique magnetic properties, group 13 azides which unlike most other azides decompose to nitride compounds (important materials for semiconductors), other limited uses as synthetic reagents for the transfer for azide groups, or interest in high energy density materials.
Selenite sulfates are mixed anion compounds containing both selenite (SeO3), and sulfate (SO4) anions.
When values of birefingence are very high, the property is termed giant birefringence which more generically is called giant optical anisotropy. Values for giant birefringence exceed 0.3. Much bigger numbers are termed "colossal birefringence". These are achieved using nanostructures.