Interchalcogen (original) (raw)
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The chalcogens react with each other to form interchalcogen compounds.[1]
Although no chalcogen is extremely electropositive,[note 1] nor quite as electronegative as the halogen fluorine (the most electronegative element), there is a large difference in electronegativity between the top (oxygen = 3.44 — the second most electronegative element after fluorine) and bottom (polonium = 2.0) of the group. Combined with the fact that there is a significant trend towards increasing metallic behaviour while descending the group (oxygen is a gaseous nonmetal, while polonium is a silvery post-transition metal[note 2]), this causes the interchalcogens to display many different kinds of bonding: covalent, ionic, metallic, and semimetallic.[note 3][1]
Known binary interchalcogens
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| O | |||||
|---|---|---|---|---|---|
| O | O2, O3, O4, O8 | S | |||
| S | S2O, SO, S2O2, SO2, SO3 | S2, S3, S6, S7, S8, S∞ | Se | ||
| Se | SeO2, SeO3 | Se_x_S_y_ | Se6, Se7, Se8, Se∞ | Te | |
| Te | TeO, TeO2, TeO3, Te2O5 | Te_x_S_y_ (many unknown) | Te_x_Se_y_ (many unknown) | Te∞ | Po |
| Po | PoO, PoO2, PoO3 | PoS (many unknown) | Po_x_Se_y_ (many unknown) | Po_x_Te_y_ (unknown) | Po∞ |
Bonding in the binary interchalcogens
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Going down the above table, there is a transition from covalent bonding (with discrete molecules) to ionic bonding; going across the table, there is a transition from ionic bonding to metallic bonding. (Covalent bonding occurs when both elements have similar high electronegativities; ionic bonding occurs when the two elements have very different electronegativities, one low and the other high; metallic bonding occurs when both elements have similar low electronegativities.) For example, in the leftmost column of the table (with bonds to oxygen), O2 and O3 are purely covalent, SO2 and SO3 are polar molecules, SeO2 forms chained polymers (stretching in one dimension), TeO2 forms layered polymers (stretching in two dimensions), and PoO2 is ionic with the fluorite structure (spatial polymers, stretching in three dimensions); in the bottom row of the table (with bonds to polonium), PoO2 and PoS are ionic, Po_x_Se_y_ and Po_x_Te_y_ are semimetallic, and Po∞ is metallic.[1]
Summary of known binary interchalcogens
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Sulfur chalcogenides
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Molecular structure of sulfur monoxide.
- Lower sulfur oxides, S_x_O_y_ where the ratio x:y is greater than 1:2
- Disulfur monoxide, S2O
- Disulfur dioxide, S2O2
- Sulfur monoxide, SO
- Sulfur dioxide, SO2
- Sulfur trioxide, SO3
- Higher sulfur oxides, SO_x_ where x > 3
Selenium chalcogenides
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Molecular structure of selenium trioxide.
- Selenium dioxide, SeO2
- Selenium trioxide, SeO3
- Many "alloys" of selenium and sulfur in different concentrations with semimetallic bonding, Se_x_S_y_
- "Selenium monosulfide", SeS
- "Selenium disulfide", SeS2, actually a 2:1 mixture of _cyclo_-Se3S5 and _cyclo_-Se2S6
- "Selenium trisulfide", SeS3, actually occurring as an 8-membered cyclic compound Se2S6 (diselenacyclooctasulfane), where two sulfur atoms in the molecule of cyclooctasulfur are replaced by selenium atoms
Tellurium chalcogenides
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Crystal structure of tellurium dioxide.
- Tellurium monoxide, TeO (unstable transient species)
- Tellurium dioxide, TeO2
- Tellurium trioxide, TeO3
- Ditellurium pentoxide, Te2O5[2]
- Many "alloys" of tellurium and sulfur in different concentrations with semimetallic bonding, Te_x_S_y_
- Many "alloys" of tellurium and selenium in different concentrations with semimetallic bonding, Te_x_Se_y_
Polonium chalcogenides
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Unit cell of polonium dioxide (cubic modification). Po: white; O: yellow.
- Polonium monoxide, PoO
- Polonium dioxide, PoO2
- Polonium trioxide, PoO3
- Polonium monosulfide, PoS
- Many "alloys" of polonium and selenium in different concentrations with semimetallic bonding, Po_x_Se_y_
- Many "alloys" of polonium and tellurium in different concentrations with semimetallic bonding, Po_x_Te_y_
- Interhalogen
- Hydrogen chalcogenide
^ This article uses Pauling electronegativity throughout.
^ The classification of polonium as a post-transition metal or a metalloid is disputed.
^ The heavier halogens are sufficiently electronegative to prevent ionic or metallic bonding in the interhalogens, and the lighter pnictogens are not sufficiently electronegative to allow ionic or metallic bonding in the interpnictogens.
^ a b c Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.), Inorganic Chemistry, translated by Eagleson, Mary; Brewer, William, San Diego/Berlin: Academic Press/De Gruyter, pp. 585–586, ISBN 0-12-352651-5
^ Lindqvist, O.; Moret, J. (1973). "The crystal structure of ditellurium pentoxide, Te2O5". Acta Crystallographica Section B: Structural Crystallography and Crystal Chemistry. 29 (4): 643–650. doi:10.1107/S0567740873003092.