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Amorphous indium oxide is insoluble in water but soluble in acids, whereas crystalline indium oxide is insoluble in both water and acids. The crystalline form exists in two phases, the cubic (bixbyite type) [1] and rhombohedral (corundum type). Both phases have a band gap of about 3 eV. [3] [4] The parameters of the cubic phase are listed in ...
Although an amphiprotic species must be amphoteric, the converse is not true. For example, a metal oxide such as zinc oxide, ZnO, contains no hydrogen and so cannot donate a proton. Nevertheless, it can act as an acid by reacting with the hydroxide ion, a base: ZnO + 2 OH − + H 2 O → [Zn(OH) 4] 2−. Zinc oxide can also act as a base:
In a similar way to aluminium salts, indium(III) ions can be toxic to the kidney when given by injection. [21] Indium tin oxide and indium phosphide harm the pulmonary and immune systems, predominantly through ionic indium, [91] though hydrated indium oxide is more than forty times as toxic when injected, measured by the quantity of indium ...
The bond length, or the minimum separating distance between two atoms participating in bond formation, is determined by their repulsive and attractive forces along the internuclear direction. [3] As the two atoms get closer and closer, the positively charged nuclei repel, creating a force that attempts to push the atoms apart.
Intermolecular hydrogen bonding is responsible for the high boiling point of water (100 °C) compared to the other group 16 hydrides, which have little capability to hydrogen bond. Intramolecular hydrogen bonding is partly responsible for the secondary , tertiary , and quaternary structures of proteins and nucleic acids .
Numerous investigations have found an explanation for this effect. The oxygens of the carbonyl and the hydroxyl group chelate the indium of the organoindium intermediate as illustrated below on the left by the two green bonds. The incipient C-C bond, illustrated in red, creates a six-member ring in a chair conformation.
The oxide (PtO 2) is amphoteric, with acidic properties predominating; it can be fused with alkali hydroxides (MOH; M = Na, K) or calcium oxide (CaO) to give anionic platinates, such as red Na 2 PtO 3 and green K 2 PtO 3. The hydrated oxide can be dissolved in hydrochloric acid to give the hexachlormetallate(IV), H 2 PtCl 6. [20]
An oxide is a chemical compound in which one or more oxygen atoms combined with another element, such as H 2 O or CO 2. Based on their acid-base characteristics, oxides can be classified into four categories: acidic oxides, basic oxides, and amphoteric oxides and neutral oxides.