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Our range of Sulphur is a chemical element with symbol S and atomic number 16. It is an abundant, multivalent non-metal. Under normal conditions, sulfur atoms form cyclic octatomic molecules with chemical formula S8. Symbol: S Electron configuration: Ne 3s2 3p4 Atomic number: 16 Melting point: 115.2 A C Discovered: 2000 BC Atomic mass: 32.065 A 0.005 u Sulfur or sulphur is a chemical element with symbol S and atomic number 16. It is an abundant, multivalent non-metal. Under normal conditions, sulfur atoms form cyclic octatomic molecules with chemical formula S8. Sulfur burns with a blue flame concomitant with formation of sulfur dioxide, notable for its peculiar suffocating odor. Sulfur is insoluble in water but soluble in carbon disulfide and, to a lesser extent, in other nonpolar organic solvents, such as benzene. The fourth and sixth ionization energies are 4556 and 8495.8 kJA.mola 1, the magnitude of the figures caused by electron transfer between orbitals; these states are only stable with strong oxidants as fluorine,oxygen, and chlorine. Sulfur forms over 30 solid allotropes, more than any other element Besides S8, several other rings are known.[7] Removing one atom from the crown gives S7, which is more deeply yellow than S8. HPLC analysis of "elemental sulfur" reveals an equilibrium mixture of mainly S8, but with S7 and small amounts of S6.Larger rings have been prepared, including S12 and S18.
Our range of Sulphur is a chemical element with symbol S and atomic number 16. It is an abundant, multivalent non-metal. Under normal conditions, sulfur atoms form cyclic octatomic molecules with chemical formula S8. Symbol: S Electron configuration: Ne 3s2 3p4 Atomic number: 16 Melting point: 115.2 A C Discovered: 2000 BC Atomic mass: 32.065 A 0.005 u Sulfur or sulphur is a chemical element with symbol S and atomic number 16. It is an abundant, multivalent non-metal. Under normal conditions, sulfur atoms form cyclic octatomic molecules with chemical formula S8. Sulfur burns with a blue flame concomitant with formation of sulfur dioxide, notable for its peculiar suffocating odor. Sulfur is insoluble in water but soluble in carbon disulfide and, to a lesser extent, in other nonpolar organic solvents, such as benzene. The fourth and sixth ionization energies are 4556 and 8495.8 kJA.mola 1, the magnitude of the figures caused by electron transfer between orbitals; these states are only stable with strong oxidants as fluorine,oxygen, and chlorine. Sulfur forms over 30 solid allotropes, more than any other element Besides S8, several other rings are known.[7] Removing one atom from the crown gives S7, which is more deeply yellow than S8. HPLC analysis of "elemental sulfur" reveals an equilibrium mixture of mainly S8, but with S7 and small amounts of S6.Larger rings have been prepared, including S12 and S18.
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