Sulfur Cycle Britt Gumerman & Olivia Kolditz Pathway of movement Sulfur reactions Storage areas Inoranic and organic Human impact

Impact of Human Intervention Burning sulfur- containing coal and oil to produce electric power. Refining sulfur-containing petroleum to make gasoline, heating oil, and other useful products. Since the Industrial Revolution, human activities have contributed to the amount of sulfur that enters the atmosphere. Using smelting to convert sulfur compounds of metallic minerals into free metals such as copper, lead, and zinc The sulfur released by humans such as sulfur dioxides and sulfur aerosols also results in acid rain Result of acid rain

Reaction to sulfur with air Sulfur burns in air to form the gaseous dioxide sulfur(IV) oxide, SO 2. S 8 (s) + 8O 2 (g) → 8SO 2 (g) Reaction of sulfur with water Sulfur does not react with water under normal conditions. Reaction of sulfur with the halogens Sulfur reacts with all the halogens upon heating. Sulfur reacts with fluorine, F 2, and burns to form the hexafluoride sulfur(VI) fluoride. S 8 (s) + 24F 2 (g) → 8SF 6 (l) [orange] Reaction of sulfur with acids Sulfur does not react with dilute non-oxidizing acids. Reaction of sulfur with bases Sulfur reacts with hot aqueous potassium hydroxide, KOH, to form sulfide and thiosulphate species. S 8 (s) + 6KOH(as) → 2K 2 S 3 + K 2 S 2 O 3 + 3H 2 O(l)

1)Terrestrial rocks 2) Ocean sediments Terrestrial rockOcean sediments

Sodium dithionite, Na 2 S 2 O 4 Thiosulfates (S 2 O 3 2− ) Sulfides (S 2− ) Sulfites (SO 3 2− ) Sulfates (SO 4 2− ) Thioethers Sulfonium Thiols Thiolates Sulfoxides Sulfones Located in Earth’s crust Located in acid deposits