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Iron(II) sulfide or ferrous sulfide (Br.E. sulphide) is one of a family of chemical compounds and minerals with the approximate formula Fe S. Iron sulfides are often iron-deficient non-stoichiometric .
Iron sulfide or Iron sulphide can refer to range of chemical compounds composed of iron and sulfur. Minerals. By increasing order of stability: Iron(II) sulfide, FeS;
Iron(II,III) sulfide is a blue-black (sometimes pinkish [citation needed]) chemical compound of iron and sulfur with formula Fe 3 S 4 or FeS·Fe 2 S 3, which is much similar to iron(II,III) oxide. It occurs naturally as the sulfide mineral greigite and is magnetic. It is a bio-mineral produced by and found in magnetotactic bacteria.
The mineral marcasite, sometimes called "white iron pyrite", is iron sulfide (FeS 2) with orthorhombic crystal structure. It is physically and crystallographically distinct from pyrite, which is iron sulfide with cubic crystal structure. Both structures contain the disulfide S 2 2− ion, having a short bonding distance between the sulfur atoms.
The best known sulfide is pyrite (FeS 2), also known as fool's gold owing to its golden luster. [7] It is not an iron(IV) compound, but is actually an iron(II) polysulfide containing Fe 2+ and S 2− 2 ions in a distorted sodium chloride structure. [12]
The best known sulfide is iron pyrite (FeS 2), also known as fool's gold owing to its golden luster. [63] It is not an iron(IV) compound, but is actually an iron(II) polysulfide containing Fe 2+ and S 2− 2 ions in a distorted sodium chloride structure. [67] Pourbaix diagram of iron
Crystallographically the structure of chalcopyrite is closely related to that of zinc blende ZnS . [18] The unit cell is twice as large, reflecting an alternation of Cu + and Fe 3+ ions replacing Zn 2+ ions in adjacent cells. In contrast to the pyrite structure chalcopyrite has single S 2− sulfide anions
Three sulfide ions bridge two iron ions each, while the fourth sulfide bridges three iron ions. Their formal oxidation states may vary from [Fe 3 S 4] + (all-Fe 3+ form) to [Fe 3 S 4] 2− (all-Fe 2+ form). In a number of iron–sulfur proteins, the [Fe 4 S 4] cluster can be reversibly converted by oxidation and loss of one iron ion to a [Fe 3 ...