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Trisulfur
The S3 molecule, known as trisulfur, sulfur trimer, thiozone, or triatomic sulfur, is a cherry-red allotrope of sulfur. It comprises about 10% of vaporised sulfur at 713 K (440 °C; 824 °F) and 1,333 Pa (10.00 mmHg; 0.1933 psi). It has been observed at cryogenic temperatures as a solid. Under ordinary conditions it converts to cyclooctasulfur.
In terms of structure and bonding S3 and ozone (O3) are similar. Both adopt bent structures and are diamagnetic. Although represented with S=S double bonds, the bonding situation is more complex.
The S–S distances are equivalent and are 191.70±0.01 pm, and with an angle at the central atom of 117.36°±0.006°. However, cyclic S3, where the sulfur atoms are arranged in an equilateral triangle with three single bonds (similar to cyclic ozone and cyclopropane), is calculated to be higher in energy than the bent structure experimentally observed. A similar structure has been predicted for ozone, but has not been observed.
The name thiozone was invented by Hugo Erdmann in 1908 who hypothesized that S3 comprises a large proportion of liquid sulfur. However its existence was unproven until the experiments of J. Berkowitz in 1964. Using mass spectrometry, he showed that sulfur vapour contains the S3 molecule. Above 1,200 °C (2,190 °F) S3 is the second most common molecule after S2 in gaseous sulfur. In liquid sulfur the molecule is not common until the temperature is high, such as 500 °C (932 °F). However, small molecules like this contribute to most of the reactivity of liquid sulfur. S3 has an absorption peak of 425 nm (violet) with a tail extending into blue light.
S3 can also be generated by photolysis of S3Cl2 embedded in a glass or matrix of solid noble gas.
S3 occurs naturally on Io in volcanic emissions. S3 is also likely to appear in the atmosphere of Venus at heights of 20 to 30 km, where it is in thermal equilibrium with S2 and S4. The reddish colour of Venus' atmosphere at lower levels is likely to be due to S3.
S3 reacts with carbon monoxide to make carbonyl sulfide and S2.
Formation of compounds with a defined number of sulfur atoms is possible:
Trisulfur
The S3 molecule, known as trisulfur, sulfur trimer, thiozone, or triatomic sulfur, is a cherry-red allotrope of sulfur. It comprises about 10% of vaporised sulfur at 713 K (440 °C; 824 °F) and 1,333 Pa (10.00 mmHg; 0.1933 psi). It has been observed at cryogenic temperatures as a solid. Under ordinary conditions it converts to cyclooctasulfur.
In terms of structure and bonding S3 and ozone (O3) are similar. Both adopt bent structures and are diamagnetic. Although represented with S=S double bonds, the bonding situation is more complex.
The S–S distances are equivalent and are 191.70±0.01 pm, and with an angle at the central atom of 117.36°±0.006°. However, cyclic S3, where the sulfur atoms are arranged in an equilateral triangle with three single bonds (similar to cyclic ozone and cyclopropane), is calculated to be higher in energy than the bent structure experimentally observed. A similar structure has been predicted for ozone, but has not been observed.
The name thiozone was invented by Hugo Erdmann in 1908 who hypothesized that S3 comprises a large proportion of liquid sulfur. However its existence was unproven until the experiments of J. Berkowitz in 1964. Using mass spectrometry, he showed that sulfur vapour contains the S3 molecule. Above 1,200 °C (2,190 °F) S3 is the second most common molecule after S2 in gaseous sulfur. In liquid sulfur the molecule is not common until the temperature is high, such as 500 °C (932 °F). However, small molecules like this contribute to most of the reactivity of liquid sulfur. S3 has an absorption peak of 425 nm (violet) with a tail extending into blue light.
S3 can also be generated by photolysis of S3Cl2 embedded in a glass or matrix of solid noble gas.
S3 occurs naturally on Io in volcanic emissions. S3 is also likely to appear in the atmosphere of Venus at heights of 20 to 30 km, where it is in thermal equilibrium with S2 and S4. The reddish colour of Venus' atmosphere at lower levels is likely to be due to S3.
S3 reacts with carbon monoxide to make carbonyl sulfide and S2.
Formation of compounds with a defined number of sulfur atoms is possible:
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