Supporting information
Crystallographic Information File (CIF) https://doi.org/10.1107/S0108270106033981/bc3011sup1.cif | |
Structure factor file (CIF format) https://doi.org/10.1107/S0108270106033981/bc3011Isup2.hkl |
Barium azide (98.5%, Schuchardt) was recrystallized twice from aqueous solution by adding ethanol. RbN3 was obtained by mixing aqueous solutions of Ba(N3)2 and Rb2CO3 (99%, Merck) in a 1:1 molar ratio followed by filtration and recrystallization. Transparent colorless single crystals of RbBa2(N3)5 were obtained by slowly evaporating concentrated aqueous solutions of Ba(N3)2 with a sixfold excess of RbN3.
The slight deviation of the β value from 90° was confirmed by powder X-ray diffraction on a single-phase sample, where splitting of relevant reflections, especially for 412 and 412, is evident.
Data collection: EXPOSE in IPDS Software (Stoe & Cie, 1998); cell refinement: CELL in IPDS Software; data reduction: INTEGRATE in IPDS Software; program(s) used to solve structure: SHELXS97 (Sheldrick, 1990); program(s) used to refine structure: SHELXL97 (Sheldrick, 1997); molecular graphics: DIAMOND (Crystal Impact, 2005); software used to prepare material for publication: publCIF (Westrip, 2006).
Ba2N15Rb | F(000) = 508 |
Mr = 570.30 | Dx = 3.310 Mg m−3 |
Monoclinic, P2/n | Ag Kα radiation, λ = 0.56086 Å |
Hall symbol: -P 2yac | Cell parameters from 8000 reflections |
a = 8.6681 (10) Å | θ = 2.7–20.9° |
b = 5.6287 (4) Å | µ = 5.91 mm−1 |
c = 11.7330 (14) Å | T = 293 K |
β = 90.199 (14)° | Potato, colourless |
V = 572.45 (10) Å3 | 0.16 × 0.07 × 0.05 mm |
Z = 2 |
Stoe IPDS-I diffractometer | 2812 independent reflections |
Radiation source: fine-focus sealed tube | 2178 reflections with I > 2σ(I) |
Graphite monochromator | Rint = 0.075 |
ϕ scans | θmax = 28.0°, θmin = 2.7° |
Absorption correction: numerical [X-RED (Stoe & Cie, 2001) and X-SHAPE (Stoe & Cie, 1999)] | h = −14→14 |
Tmin = 0.663, Tmax = 0.815 | k = −9→9 |
16393 measured reflections | l = −19→19 |
Refinement on F2 | 0 restraints |
Least-squares matrix: full | Primary atom site location: structure-invariant direct methods |
R[F2 > 2σ(F2)] = 0.034 | Secondary atom site location: difference Fourier map |
wR(F2) = 0.084 | w = 1/[σ2(Fo2) + (0.054P)2] where P = (Fo2 + 2Fc2)/3 |
S = 1.14 | (Δ/σ)max < 0.001 |
2812 reflections | Δρmax = 1.81 e Å−3 |
87 parameters | Δρmin = −1.25 e Å−3 |
Ba2N15Rb | V = 572.45 (10) Å3 |
Mr = 570.30 | Z = 2 |
Monoclinic, P2/n | Ag Kα radiation, λ = 0.56086 Å |
a = 8.6681 (10) Å | µ = 5.91 mm−1 |
b = 5.6287 (4) Å | T = 293 K |
c = 11.7330 (14) Å | 0.16 × 0.07 × 0.05 mm |
β = 90.199 (14)° |
Stoe IPDS-I diffractometer | 2812 independent reflections |
Absorption correction: numerical [X-RED (Stoe & Cie, 2001) and X-SHAPE (Stoe & Cie, 1999)] | 2178 reflections with I > 2σ(I) |
Tmin = 0.663, Tmax = 0.815 | Rint = 0.075 |
16393 measured reflections |
R[F2 > 2σ(F2)] = 0.034 | 87 parameters |
wR(F2) = 0.084 | 0 restraints |
S = 1.14 | Δρmax = 1.81 e Å−3 |
2812 reflections | Δρmin = −1.25 e Å−3 |
Geometry. All e.s.d.'s (except the e.s.d. in the dihedral angle between two l.s. planes) are estimated using the full covariance matrix. The cell e.s.d.'s are taken into account individually in the estimation of e.s.d.'s in distances, angles and torsion angles; correlations between e.s.d.'s in cell parameters are only used when they are defined by crystal symmetry. An approximate (isotropic) treatment of cell e.s.d.'s is used for estimating e.s.d.'s involving l.s. planes. |
Refinement. Refinement of F2 against ALL reflections. The weighted R-factor wR and goodness of fit S are based on F2, conventional R-factors R are based on F, with F set to zero for negative F2. The threshold expression of F2 > σ(F2) is used only for calculating R-factors(gt) etc. and is not relevant to the choice of reflections for refinement. R-factors based on F2 are statistically about twice as large as those based on F, and R- factors based on ALL data will be even larger. |
x | y | z | Uiso*/Ueq | ||
Ba | 0.26147 (2) | 0.99668 (4) | −0.051000 (17) | 0.01396 (6) | |
Rb | 0.2500 | 0.42675 (13) | 0.2500 | 0.02935 (13) | |
N1 | 0.5000 | 0.5000 | 0.0000 | 0.0188 (8) | |
N2 | 0.4800 (5) | 0.3236 (7) | 0.0511 (4) | 0.0250 (7) | |
N3 | 0.0000 | 0.5000 | 0.0000 | 0.0197 (8) | |
N4 | 0.1358 (4) | 0.5030 (8) | 0.0009 (4) | 0.0262 (7) | |
N5 | 0.2500 | 0.5034 (10) | −0.2500 | 0.0190 (8) | |
N6 | 0.2500 | 0.2957 (10) | −0.2500 | 0.0255 (11) | |
N7 | 0.2500 | 0.7116 (10) | −0.2500 | 0.0321 (14) | |
N8 | 0.0676 (4) | 0.9413 (7) | 0.2303 (3) | 0.0185 (6) | |
N9 | 0.0470 (4) | 1.0041 (8) | 0.1347 (3) | 0.0268 (8) | |
N10 | 0.0871 (5) | 0.8801 (8) | 0.3249 (3) | 0.0298 (8) |
U11 | U22 | U33 | U12 | U13 | U23 | |
Ba | 0.01370 (8) | 0.01516 (9) | 0.01302 (8) | 0.00044 (8) | −0.00018 (5) | −0.00053 (7) |
Rb | 0.0455 (4) | 0.0214 (3) | 0.0212 (2) | 0.000 | 0.0044 (2) | 0.000 |
N1 | 0.0140 (16) | 0.0160 (19) | 0.026 (2) | 0.0018 (17) | −0.0006 (14) | −0.0056 (19) |
N2 | 0.0230 (17) | 0.0205 (18) | 0.0315 (19) | 0.0009 (13) | −0.0008 (14) | 0.0001 (14) |
N3 | 0.025 (2) | 0.0161 (19) | 0.0182 (18) | 0.0060 (19) | 0.0037 (15) | 0.0040 (17) |
N4 | 0.0193 (14) | 0.032 (2) | 0.0270 (17) | 0.0012 (15) | 0.0021 (12) | 0.0031 (15) |
N5 | 0.025 (2) | 0.022 (2) | 0.0110 (15) | 0.000 | 0.0008 (14) | 0.000 |
N6 | 0.041 (3) | 0.017 (3) | 0.019 (2) | 0.000 | 0.003 (2) | 0.000 |
N7 | 0.064 (4) | 0.015 (3) | 0.018 (2) | 0.000 | −0.004 (2) | 0.000 |
N8 | 0.0163 (13) | 0.0203 (15) | 0.0188 (13) | 0.0004 (11) | 0.0003 (11) | −0.0017 (11) |
N9 | 0.0165 (13) | 0.040 (2) | 0.0240 (15) | 0.0005 (15) | −0.0017 (11) | 0.0061 (16) |
N10 | 0.034 (2) | 0.034 (2) | 0.0206 (16) | 0.0005 (17) | −0.0023 (14) | 0.0020 (15) |
Ba—N7 | 2.834 (3) | Rb—N8 | 3.308 (4) |
Ba—N9i | 2.845 (4) | N1—N2 | 1.173 (4) |
Ba—N9 | 2.869 (4) | N1—N2ii | 1.173 (4) |
Ba—N2ii | 2.876 (4) | N1—Rbii | 3.6762 (5) |
Ba—N6iii | 2.880 (3) | N2—Baii | 2.876 (4) |
Ba—N2iii | 2.897 (4) | N2—Bavii | 2.897 (4) |
Ba—N10iv | 3.027 (4) | N3—N4 | 1.177 (4) |
Ba—N4 | 3.047 (4) | N3—N4ix | 1.177 (4) |
Ba—N4iii | 3.112 (4) | N3—Rbix | 3.6641 (5) |
Ba—N10v | 3.255 (5) | N4—Bavii | 3.112 (4) |
Ba—Rbiii | 4.2831 (6) | N5—N6 | 1.169 (8) |
Ba—Bavi | 4.3011 (7) | N5—N7 | 1.172 (8) |
Rb—N10iv | 3.047 (5) | N6—Bax | 2.880 (3) |
Rb—N10 | 3.047 (5) | N6—Bavii | 2.880 (3) |
Rb—N4iv | 3.112 (4) | N7—Baxi | 2.834 (3) |
Rb—N4 | 3.112 (4) | N8—N10 | 1.174 (5) |
Rb—N2 | 3.129 (4) | N8—N9 | 1.190 (5) |
Rb—N2iv | 3.129 (4) | N8—Rbiii | 3.165 (4) |
Rb—N8vii | 3.165 (4) | N9—Bai | 2.845 (4) |
Rb—N8viii | 3.165 (4) | N9—Rbiii | 3.251 (4) |
Rb—N9vii | 3.251 (4) | N10—Baiv | 3.027 (4) |
Rb—N9viii | 3.251 (4) | N10—Baxii | 3.255 (5) |
Rb—N8iv | 3.308 (4) | N10—Rbiii | 3.499 (5) |
N7—Ba—N9i | 71.61 (9) | N8vii—Rb—N8viii | 60.62 (13) |
N7—Ba—N9 | 127.79 (10) | N10iv—Rb—N9vii | 138.01 (10) |
N9i—Ba—N9 | 69.60 (13) | N10—Rb—N9vii | 118.82 (11) |
N7—Ba—N2ii | 70.74 (10) | N4iv—Rb—N9vii | 131.43 (11) |
N9i—Ba—N2ii | 136.91 (12) | N4—Rb—N9vii | 62.62 (11) |
N9—Ba—N2ii | 121.09 (12) | N2—Rb—N9vii | 84.21 (11) |
N7—Ba—N6iii | 70.24 (13) | N2iv—Rb—N9vii | 80.17 (10) |
N9i—Ba—N6iii | 72.02 (9) | N8vii—Rb—N9vii | 21.32 (9) |
N9—Ba—N6iii | 125.91 (9) | N8viii—Rb—N9vii | 70.62 (10) |
N2ii—Ba—N6iii | 113.00 (10) | N10iv—Rb—N9viii | 118.82 (11) |
N7—Ba—N2iii | 136.15 (9) | N10—Rb—N9viii | 138.01 (10) |
N9i—Ba—N2iii | 139.11 (12) | N4iv—Rb—N9viii | 62.62 (11) |
N9—Ba—N2iii | 95.81 (12) | N4—Rb—N9viii | 131.43 (11) |
N2ii—Ba—N2iii | 83.67 (12) | N2—Rb—N9viii | 80.17 (10) |
N6iii—Ba—N2iii | 89.12 (11) | N2iv—Rb—N9viii | 84.21 (11) |
N7—Ba—N10iv | 127.80 (12) | N8vii—Rb—N9viii | 70.62 (10) |
N9i—Ba—N10iv | 134.91 (12) | N8viii—Rb—N9viii | 21.32 (9) |
N9—Ba—N10iv | 67.54 (11) | N9vii—Rb—N9viii | 85.94 (14) |
N2ii—Ba—N10iv | 61.89 (12) | N10iv—Rb—N8iv | 20.77 (9) |
N6iii—Ba—N10iv | 148.30 (11) | N10—Rb—N8iv | 57.89 (11) |
N2iii—Ba—N10iv | 59.65 (12) | N4iv—Rb—N8iv | 70.33 (10) |
N7—Ba—N4 | 68.71 (12) | N4—Rb—N8iv | 95.46 (10) |
N9i—Ba—N4 | 74.41 (11) | N2—Rb—N8iv | 84.78 (10) |
N9—Ba—N4 | 68.19 (12) | N2iv—Rb—N8iv | 114.59 (10) |
N2ii—Ba—N4 | 73.01 (11) | N8vii—Rb—N8iv | 178.56 (7) |
N6iii—Ba—N4 | 133.13 (11) | N8viii—Rb—N8iv | 120.82 (10) |
N2iii—Ba—N4 | 136.92 (11) | N9vii—Rb—N8iv | 158.08 (9) |
N10iv—Ba—N4 | 77.37 (12) | N9viii—Rb—N8iv | 110.72 (9) |
N7—Ba—N4iii | 131.93 (11) | N10iv—Rb—N8 | 57.89 (11) |
N9i—Ba—N4iii | 74.92 (12) | N10—Rb—N8 | 20.77 (9) |
N9—Ba—N4iii | 67.03 (12) | N4iv—Rb—N8 | 95.46 (10) |
N2ii—Ba—N4iii | 147.92 (11) | N4—Rb—N8 | 70.33 (10) |
N6iii—Ba—N4iii | 67.19 (11) | N2—Rb—N8 | 114.59 (10) |
N2iii—Ba—N4iii | 64.30 (11) | N2iv—Rb—N8 | 84.78 (10) |
N10iv—Ba—N4iii | 100.25 (12) | N8vii—Rb—N8 | 120.82 (10) |
N4—Ba—N4iii | 132.09 (13) | N8viii—Rb—N8 | 178.56 (7) |
N7—Ba—N10v | 77.30 (9) | N9vii—Rb—N8 | 110.72 (9) |
N9i—Ba—N10v | 131.40 (11) | N9viii—Rb—N8 | 158.08 (9) |
N9—Ba—N10v | 154.36 (11) | N8iv—Rb—N8 | 57.75 (12) |
N2ii—Ba—N10v | 57.08 (12) | N2—N1—N2ii | 180.0 (4) |
N6iii—Ba—N10v | 62.64 (8) | N2—N1—Rb | 53.8 (2) |
N2iii—Ba—N10v | 58.85 (11) | N2ii—N1—Rb | 126.2 (2) |
N10iv—Ba—N10v | 93.67 (11) | N2—N1—Rbii | 126.2 (2) |
N4—Ba—N10v | 126.51 (11) | N2ii—N1—Rbii | 53.8 (2) |
N4iii—Ba—N10v | 101.37 (11) | Rb—N1—Rbii | 180.0 |
N7—Ba—Rbiii | 176.659 (7) | N1—N2—Baii | 114.4 (2) |
N9i—Ba—Rbiii | 105.13 (9) | N1—N2—Bavii | 115.1 (2) |
N9—Ba—Rbiii | 49.36 (9) | Baii—N2—Bavii | 96.33 (12) |
N2ii—Ba—Rbiii | 112.01 (8) | N1—N2—Rb | 108.6 (2) |
N6iii—Ba—Rbiii | 109.72 (9) | Baii—N2—Rb | 127.94 (15) |
N2iii—Ba—Rbiii | 46.93 (8) | Bavii—N2—Rb | 90.52 (11) |
N10iv—Ba—Rbiii | 53.93 (9) | N4—N3—N4ix | 180.0 (4) |
N4—Ba—Rbiii | 109.95 (8) | N4—N3—Rb | 53.5 (2) |
N4iii—Ba—Rbiii | 46.52 (8) | N4ix—N3—Rb | 126.5 (2) |
N10v—Ba—Rbiii | 105.72 (8) | N4—N3—Rbix | 126.5 (2) |
N7—Ba—Bavi | 105.37 (2) | N4ix—N3—Rbix | 53.5 (2) |
N9i—Ba—Bavi | 175.95 (8) | Rb—N3—Rbix | 180.0 |
N9—Ba—Bavi | 114.42 (7) | N3—N4—Ba | 111.7 (2) |
N2ii—Ba—Bavi | 42.02 (8) | N3—N4—Bavii | 109.6 (3) |
N6iii—Ba—Bavi | 104.54 (2) | Ba—N4—Bavii | 132.09 (13) |
N2iii—Ba—Bavi | 41.66 (8) | N3—N4—Rb | 108.8 (2) |
N10iv—Ba—Bavi | 49.05 (9) | Ba—N4—Rb | 101.57 (12) |
N4—Ba—Bavi | 107.24 (7) | Bavii—N4—Rb | 86.97 (10) |
N4iii—Ba—Bavi | 105.93 (7) | N6—N5—N7 | 180.0 |
N10v—Ba—Bavi | 44.62 (7) | N5—N6—Bax | 125.76 (9) |
Rbiii—Ba—Bavi | 77.919 (12) | N5—N6—Bavii | 125.76 (9) |
N10iv—Rb—N10 | 66.27 (17) | Bax—N6—Bavii | 108.47 (18) |
N10iv—Rb—N4iv | 90.53 (11) | N5—N7—Ba | 124.47 (10) |
N10—Rb—N4iv | 76.10 (11) | N5—N7—Baxi | 124.47 (10) |
N10iv—Rb—N4 | 76.10 (11) | Ba—N7—Baxi | 111.05 (19) |
N10—Rb—N4 | 90.53 (11) | N10—N8—N9 | 179.6 (5) |
N4iv—Rb—N4 | 164.15 (16) | N10—N8—Rbiii | 96.6 (3) |
N10iv—Rb—N2 | 69.10 (11) | N9—N8—Rbiii | 83.4 (3) |
N10—Rb—N2 | 131.88 (11) | N10—N8—Rb | 67.0 (3) |
N4iv—Rb—N2 | 121.65 (10) | N9—N8—Rb | 113.3 (3) |
N4—Rb—N2 | 61.74 (10) | Rbiii—N8—Rb | 120.82 (10) |
N10iv—Rb—N2iv | 131.88 (11) | N8—N9—Bai | 117.6 (3) |
N10—Rb—N2iv | 69.10 (11) | N8—N9—Ba | 128.1 (3) |
N4iv—Rb—N2iv | 61.74 (10) | Bai—N9—Ba | 110.40 (13) |
N4—Rb—N2iv | 121.65 (10) | N8—N9—Rbiii | 75.3 (3) |
N2—Rb—N2iv | 158.61 (16) | Bai—N9—Rbiii | 130.66 (15) |
N10iv—Rb—N8vii | 159.03 (10) | Ba—N9—Rbiii | 88.60 (10) |
N10—Rb—N8vii | 120.80 (11) | N8—N10—Baiv | 145.6 (4) |
N4iv—Rb—N8vii | 110.16 (10) | N8—N10—Rb | 92.2 (3) |
N4—Rb—N8vii | 83.88 (10) | Baiv—N10—Rb | 103.56 (13) |
N2—Rb—N8vii | 96.01 (10) | N8—N10—Baxii | 103.7 (3) |
N2iv—Rb—N8vii | 64.83 (10) | Baiv—N10—Baxii | 86.33 (11) |
N10iv—Rb—N8viii | 120.80 (11) | Rb—N10—Baxii | 135.29 (16) |
N10—Rb—N8viii | 159.03 (10) | N8—N10—Rbiii | 64.0 (3) |
N4iv—Rb—N8viii | 83.88 (10) | Baiv—N10—Rbiii | 81.69 (11) |
N4—Rb—N8viii | 110.16 (10) | Rb—N10—Rbiii | 118.44 (14) |
N2—Rb—N8viii | 64.83 (10) | Baxii—N10—Rbiii | 106.04 (13) |
N2iv—Rb—N8viii | 96.01 (10) |
Symmetry codes: (i) −x, −y+2, −z; (ii) −x+1, −y+1, −z; (iii) x, y+1, z; (iv) −x+1/2, y, −z+1/2; (v) x+1/2, −y+2, z−1/2; (vi) −x+1, −y+2, −z; (vii) x, y−1, z; (viii) −x+1/2, y−1, −z+1/2; (ix) −x, −y+1, −z; (x) −x+1/2, y−1, −z−1/2; (xi) −x+1/2, y, −z−1/2; (xii) x−1/2, −y+2, z+1/2. |
Experimental details
Crystal data | |
Chemical formula | Ba2N15Rb |
Mr | 570.30 |
Crystal system, space group | Monoclinic, P2/n |
Temperature (K) | 293 |
a, b, c (Å) | 8.6681 (10), 5.6287 (4), 11.7330 (14) |
β (°) | 90.199 (14) |
V (Å3) | 572.45 (10) |
Z | 2 |
Radiation type | Ag Kα, λ = 0.56086 Å |
µ (mm−1) | 5.91 |
Crystal size (mm) | 0.16 × 0.07 × 0.05 |
Data collection | |
Diffractometer | Stoe IPDS-I diffractometer |
Absorption correction | Numerical [X-RED (Stoe & Cie, 2001) and X-SHAPE (Stoe & Cie, 1999)] |
Tmin, Tmax | 0.663, 0.815 |
No. of measured, independent and observed [I > 2σ(I)] reflections | 16393, 2812, 2178 |
Rint | 0.075 |
(sin θ/λ)max (Å−1) | 0.837 |
Refinement | |
R[F2 > 2σ(F2)], wR(F2), S | 0.034, 0.084, 1.14 |
No. of reflections | 2812 |
No. of parameters | 87 |
Δρmax, Δρmin (e Å−3) | 1.81, −1.25 |
Computer programs: EXPOSE in IPDS Software (Stoe & Cie, 1998), CELL in IPDS Software, INTEGRATE in IPDS Software, SHELXS97 (Sheldrick, 1990), SHELXL97 (Sheldrick, 1997), DIAMOND (Crystal Impact, 2005), publCIF (Westrip, 2006).
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The chemistry of metal azides has been developing fast recently, exemplified by syntheses and characterization of new binaries M(N3)6 (M = Mo or W) for the d metals (Haiges et al., 2005) and U(N3)73− for the f elements (Crawford et al., 2005) just in the past year.
On the other side, more stable azides of the s metals have been known for a long time. Alkali metal azides, especially NaN3, are classical sources of pure metals and/or nitrogen. Alkaline earth metal azides have not been used for this purpose as extensively owing to their somewhat more violent thermal decomposition and the greater effort needed to obtain solvent-free azides. Anhydrous barium azide can be relatively easily obtained because of the large cation size; its crystallization (Manno, 1965; Marinkas, 1966) and crystal structure (Choi, 1969; Walitzi & Krischner, 1970) attracted some attention previously because of its potential as a high-energy material. Recently, it was shown that Ba(N3)2 can be employed as a valuable precursor, e.g. for the preparation of barium pernitride BaN2 by controlled thermal decomposition (Vajenine et al., 2001). Moreover, anhydrous barium azide can also be used as a barium and nitrogen source in the syntheses of new intermetallic (Smetana et al., 2006a) and subnitride (Smetana et al., 2006b) phases.
Therefore, the search for new complex azides is important for the development of nitride chemistry. Especially numerous are the mixed azides of alkali and alkaline earth metals. Anhydrous coumpounds with compositions Cs7Ca4(N3)15 (Krischner et al., 1984), CSSR(N3)3 (Krischner et al., 1981a), Cs2Sr(N3)4 (Krischner et al., 1981b), and CsBa2(N3)5 (Krischner et al., 1982) have been reported so far. Additionally, a number of hydrated azides have been described: K2Ca(N3)4·4H2O (Krischner et al., 1980), Rb2Ca(N3)4·4H2O (Mautner & Krischner, 1988), CsCa(N3)3·H2O (Krischner, Mautner & Kratky, 1983), Cs5Ca2(N3)9·2H2O (Saracoglu et al., 1983), Cs6Ca(N3)8·2H2O (Krischner, Saracoglu et al., 1983), and K2.24Sr1.34(N3)4.92·6.16H2O (Walitzi & Krischner, 1978).
In this study we focused on ternary azides of alkali metals with barium. The synthesis of the hitherto only known azide of this kind, CsBa2(N3)5, was reproduced and a new rubidium compound with the same stoichiometry was obtained. Our attempts to prepare ternary azides of barium with potassium or sodium were unsuccessful.
The crystal structures of orthorhombic CsBa2(N3)5 and monoclinic RbBa2(N3)5 are similar. The arrangements of the metal ions in both azides can be regarded as distorted variants of the AlB2-type structure (Fig. 1); graphite-like sheets of barium ions are separated by alkali metal cations. Azide anions occupy the voids between the cations, whereby a slight difference in their coordination environment leads to a lower crystal symmetry in the case of RbBa2(N3)5.
The coordination polyhedra of rubidium and barium in RbBa2(N3)5 are shown in Fig. 2. The barium cations are surrounded by ten terminal N atoms of azide groups in the form of a trigonal prism with four additional caps. The Ba—N distances range from 2.834 (3) to 3.255 (5) Å, which is comparable to the ranges for ninefold coordinated barium in CsBa2(N3)5 [2.816 (6)–3.087 (6) Å] and Ba(N3)2 [2.883 (3)–2.985 (3) Å]. The rubidium coordination can be described as a polyhedron intermediate between a cube and a square antiprism. Here the distances to the terminal N atoms [3.047 (5)–3.251 (4) Å] are only slightly shorter than the closest contacts to the central atoms of the azide groups [3.165 (4)–3.308 (4) Å]. Two additional capping azide groups lie much farther away at 4.352 (5) Å, favoring the thermal motion of the rubidium cations along the a axis. Eightfold coordination of rubidium is also found in RbN3, with Rb—N distances of 3.099 Å (Choi & Prince, 1976), and in Rb2Ca(N3)4·4H2O [six Rb—N contacts of 2.967 (7)–3.133 (7) Å with two additional water molecules].
The coordination environments of the four crystallographically inequivalent azide groups in RbBa2(N3)5 are shown in Fig. 3. The arrangement of the metal cations can be described as distorted octahedra of four barium and two trans-rubidium cations. These two rubidium positions lie farther away (cf. the rubidium environment above) in the case of the N6/N5/N7 azide group, resulting in a 4 + 2 coordination. The nearly side-on coordination of the azide group to rubidium is particularly evident for the N9/N8/N10 group. The latter is also the only azide group not restricted to be linear by symmetry, though this anion is almost linear with a bonding angle of 179.6 (5)°. The N—N distances range from 1.169 (8) to 1.190 (5) Å and are thus in a good agreement with the structures of other known azide compounds.
In comparison to CsBa2(N3)5, in which three of four crystallographically inequivalent azide groups are in a fivefold coordination and only one is in a sixfold coordination by metal cations, the average coordination number of the azide groups in RbBa2(N3)5 is slightly higher (six for three azide groups and four for one) owing to the smaller size of Rb+ compared with Cs+. This minute difference is apparently sufficient to favorize the monoclinic structure for the rubidium compound.
An alternative description of the crystal structure of RbBa2(N3)5 is instructive. If the positions of the central atoms of the azide groups alone are considered (i.e. the centers of mass of the anions), then the ternary azide may be described as a slightly distorted variant of the Ga3Pt5 structure (Bhan & Schubert, 1960) with the metal cations in the gallium positions and the azide groups in the platinum sites. The latter intermetallic phase is in turn an ordered 2 × 2 × 1 superstructure of the fcc packing with 16 atoms in the unit cell [Z = 2 as in RbBa2(N3)5]. The observed axis ratio of a:b:c = 1.54:1:2.08 for the azide group illustrates the degree of distortion compared with the expected value of 2:1:2 for the ideal fcc lattice. Interestingly, the crystal structure of CsBa2(N3)5 can also be reduced to the Ga3Pt5 structure type.
According to our preliminary results, thermal decomposition of the ternary azides RbBa2(N3)5 and CsBa2(N3)5 leads to BaN2 accompanied by evaporation of the alkali metal.