Synthesis, Crystal Structure, and Thermal Properties of Na₅[SnS₄]Cl·13H₂O

Abstract

Reaction of Na 2 S with SnCl 4 ·5H 2 O in aqueous alkaline sodium hydroxide solution leads to the formation of Na 5 [SnS 4 ]Cl·13H 2 O (1). The compound crystallizes monoclinic in space group P2 1 /m with two formula units in the unit cell. In the crystal structure the Na + cations are octahedrally coordinated and are linked into layers by bridging water molecules, μ 3 bridging Clanions and μ 1,1 bridging S atoms of [SnS 4 ] 4anions. Extended hydrogen bonding interactions generate a three-dimensional network. Investigations using differential thermoanalysis, thermogravimetry, and differential scanning calorimetry shows that upon heating in open crucibles the water can be removed leading to the formation of the anhydrate that is stable at room

Room‐Temperature Solid‐State Transformation of Na4SnS4 ⋅ 14H2O into Na4Sn2S6 ⋅ 5H2O: An Unusual Epitaxial Reaction Including Bond Formation, Mass Transport, and Ionic Conductivity

“…All S 2− anions of [Sn 2 S 6 ] 4− have bonds to Na + : S brid (S1, S3) have bonds to two Na + and S term (S2, S4) are involved in one respectively three Na−S bonds (Figure 2, bottom). While the Na−O bonds are similar to those of I , the average Na−S bond is significantly longer but is in agreement with literature data [2,5,15,20] . The Na1O 3 S 3 octahedron and the Na2O 2 S 3 trigonal bipyramid (Figure 2, bottom and Figure S8) share common edges to form a (Na1Na2)O 3 S 6 secondary building unit, which are joined to generate a 3D network structure (Figure 2, bottom).…”

“…In the structure of I , Na1 is octahedrally coordinated by five H 2 O molecules and one S 2− anion, while Na2/Na3 are in an octahedral environment of six H 2 O molecules (Figure 2, top and Figure S6). All bond lengths are in the range of the sum of ionic radii [ r Na (CN=6): 1.02 Å, O 2− : 1.35 Å, S 2− : 1.84 Å; Sn 4+ : 0.55 Å; Table S2] [18] and match literature data [2,5, 19, 20] . The plausibility of the structure model is also underlined by the global instability index GII, i. e. the root mean squared average bond valence sum mismatch, which is 0.17 and hence in the acceptable range <0.2 both for C 2/ c as for Cc .…”

“…All bond lengths are in the range of the sum of ionic radii [ r Na (CN=6): 1.02 Å, O 2− : 1.35 Å, S 2− : 1.84 Å; Sn 4+ : 0.55 Å; Table S2] [18] and match literature data. [ 2 , 5 , 19 , 20 ] The plausibility of the structure model is also underlined by the global instability index GII, i. e. the root mean squared average bond valence sum mismatch, which is 0.17 and hence in the acceptable range <0.2 both for C 2/ c as for Cc . The Na + centered polyhedra are connected through common corners and edges to form a 3D structure (Figure 2 , top).…”

Re‐investigation of Barium‐Gold(I)‐Tetra‐Thiostannate(IV), Ba[Au2SnS4], with Short AuI···AuI Separation Showing Luminescence Properties

“…[ 4-. Charge compensation is achieved by different cations including main group metal cations, [1][2][3][4][5][6][7][8][9] combinations of main group and transition metal cations, [10][11][12][13][14][15][16][17][18][19][20][21][22] transition metal cations and/or complexes, [23][24][25][26][27][28][29][30][31][32][33][34] and organic ammonium and/or metal cations. [35][36][37][38][39][40] Several of these compounds exhibit interesting physico-chemical properties like second harmonic generation, [17,18] efficient ion exchange behavior for rare earth cations, [41] promising properties as anode materials in lithium ion batteries, [39] selective heavy metal cation sequestration from aqueous solutions, [8] photoconductivity,…”

“…[SnS 4 ] 4– , [Sn 2 S 6 ] 4– , [Sn 2 S 5 ] 2– , [Sn 2 S 7 ] 6– , [Sn 2 S 8 ] 2– , [Sn 3 S 7 ] 2– , [Sn 4 S 9 ] 2– , [Sn 4 S 10 ] 4– , or [Sn 5 S 12 ] 4– . Charge compensation is achieved by different cations including main group metal cations, [ 1–9 ] combinations of main group and transition metal cations, [ 10–22 ] transition metal cations and/or complexes, [ 23–34 ] and organic ammonium and/or metal cations. [ 35–40 ] Several of these compounds exhibit interesting physico‐chemical properties like second harmonic generation, [ 17,18 ] efficient ion exchange behavior for rare earth cations, [ 41 ] promising properties as anode materials in lithium ion batteries, [ 39 ] selective heavy metal cation sequestration from aqueous solutions, [ 8 ] photoconductivity, [ 28 ] or photocatalytic activity for dye degradation, [ 30 ] to name just a few.…”