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The following exergonic equilibrium gives rise to the triiodide ion: . I 2 + I − ⇌ I − 3. In this reaction, iodide is viewed as a Lewis base, and the iodine is a Lewis acid.The process is analogous to the reaction of S 8 with sodium sulfide (which forms polysulfides) except that the higher polyiodides have branched structures.
Hydrolysis occurs only slowly in water forming arsenic trioxide and hydroiodic acid.The reaction proceeds via formation of arsenous acid which exists in equilibrium with hydroiodic acid.
The polyiodides are a class of polyhalogen anions composed entirely of iodine atoms. [1] [2] The most common member is the triiodide ion, I −3.Other known larger polyiodides include [I 4] 2−, [I 5] −, [I 6] 2−, [I 7] −, [I 8] 2−, [I 9] −, [I 10] 2−, [I 10] 4−, [I 11] 3−, [I 12] 2−, [I 13] 3−, [I 14] 4-, [I 16] 2−, [I 22] 4−, [I 26] 3−, [I 26] 4−, [I 28] 4− and ...
[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
In its pure state, boron triiodide forms colorless, otherwise reddish, shiny, air and hydrolysis-sensitive [3] crystals, which have a hexagonal crystal structure (a = 699.09 ± 0.02 pm, c = 736.42 ± 0.03 pm, space group P6 3 /m (space group no. 176)). [4] Boron triiodide is a strong Lewis acid and soluble in carbon disulfide. [2]
Antimony triiodide is the chemical compound with the formula Sb I 3. This ruby-red solid is the only characterized "binary" iodide of antimony, i.e. the sole compound isolated with the formula Sb x I y. It contains antimony in its +3 oxidation state. Like many iodides of the heavier main group elements, its structure depends
Thallium triiodide is a chemical compound of thallium and iodine with formula TlI 3. Unlike the other thallium trihalides, which contain thallium(III), TlI 3 is a thallium(I) salt and contains the triiodide ion, I − 3. An appreciation as to why Tl + is not oxidised to Tl 3+ in the reaction: Tl 3+ + 2 I − → Tl + + I 2
2 ions – the latter, in any case, are much less stable than the bifluoride ions (HF − 2) due to the very weak hydrogen bonding between hydrogen and iodine, though its salts with very large and weakly polarising cations such as Cs + and NR + 4 (R = Me, Et, Bu n) may still be isolated.