Chemistry:Disulfur dinitride
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| Names | |
|---|---|
| Preferred IUPAC name
Disulfur dinitride | |
| Systematic IUPAC name
1λ4,3,2,4-Dithiadiazete | |
| Other names
Cyclic sulfur(II,IV) nitride
1,3-dithia-2,4-diazacyclobutan-2,4-diyl | |
| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
PubChem CID
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| Properties | |
| S 2N 2 | |
| Molar mass | 92.1444 g/mol |
| Appearance | colourless crystals |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Disulfur dinitride is the chemical compound with the formula S
2N
2.
Preparation and reactions
Passing gaseous S
4N
4 over silver metal wool at 250–300 °C at low pressure (1mm Hg) yields cyclic S
2N
2. The silver reacts with the sulfur produced by the thermal decomposition of the S
4N
4 to form Ag
2S, and the resulting Ag
2S catalyzes the conversion of the remaining S
4N
4 into the four-membered ring S
2N
2,[1]
- S
4N
4 + 8 Ag → 4 Ag
2S + 2 N
2 - S
4N
4 → 2 S
2N
2
An alternative uses the less explosive S
4N
3Cl.[2][clarification needed]
S
2N
2 decomposes explosively above 30°C, and is shock sensitive.[1] It readily sublimes, and is soluble in diethyl ether. Traces of water cause it to polymerize into S
4N
4.[2] In the solid state it spontaneously polymerizes forming (SN) {n}.[1] It forms adducts with Lewis acids via a nitrogen atom, e.g. S
2N
2 · BCl
3, S
2N
2 · 2AlCl
3, S
2N
2 · SbCl
5, S
2N
2 · 2SbCl
5.[2][3]
Structure and bonding
The S
2N
2 molecule is a four-membered ring, with alternating S and N atoms. One S atom has valence 4 and the other S atom has valence 2. Both nitrogen atoms has valence 3. The molecule is almost square and planar. The S–N bond lengths are 165.1pm and 165.7pm and the bond angles are very close to 90°.[1] The S
2N
2 molecule is isoelectronic with the cyclic S2+
4 dication and has 6π electrons.[2] The bonding has been investigated using a spin-coupled valence bond method [4] and is described as having four framework sigma bonds, with the N atoms bearing a high negative charge and the S atoms a corresponding positive charge. Two π electrons from the sulfur atoms are coupled across the ring making the molecule overall a singlet diradical.
See also
References
- ↑ 1.0 1.1 1.2 1.3 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ↑ 2.0 2.1 2.2 2.3 Wiberg, E.; Holleman, A. F. (2001). Inorganic Chemistry. Elsevier. ISBN 0-12-352651-5.
- ↑ Patton R. L.; Raymond, K. N. (1969). "The Crystal and Molecular Structure of S2N2(SbCl5)2". Inorganic Chemistry 8 (11): 2426–2431. doi:10.1021/ic50081a035.
- ↑ Gerratt, J.; McNicholas, S. J.; Karadakov, P. B.; Sironi, M.; Raimondi, M.; Cooper, D. L. (1996). "The Extraordinary Electronic Structure of N2S2". Journal of the American Chemical Society 118 (27): 6472–6476. doi:10.1021/ja953994f.
| NH3 | He(N2)11 | ||||||||||||||||
| Li3N | Be3N2 | BN | β-C3N4 g-C3N4 |
N2 | NxOy | NF3 | Ne | ||||||||||
| Na3N | Mg3N2 | AlN | Si3N4 | PN P3N5 |
SxNy SN S4N4 |
NCl3 | Ar | ||||||||||
| K3N | Ca3N2 | ScN | TiN | VN | CrN Cr2N |
MnxNy | FexNy | CoN | Ni3N | CuN | Zn3N2 | GaN | Ge3N4 | As | Se | NBr3 | Kr |
| Rb3N | Sr3N2 | YN | ZrN | NbN | β-Mo2N | Tc | Ru | Rh | PdN | Ag3N | CdN | InN | Sn | Sb | Te | NI3 | Xe |
| Cs3N | Ba3N2 | Hf3N4 | TaN | WN | Re | Os | Ir | Pt | Au | Hg3N2 | TlN | Pb | BiN | Po | At | Rn | |
| Fr3N | Ra3N | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
| ↓ | |||||||||||||||||
| La | CeN | Pr | Nd | Pm | Sm | Eu | GdN | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac | Th | Pa | UN | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||
 |  |
