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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:
Boron oxide (B 2 O 3) is slightly acidic, aluminium and gallium oxide (Al 2 O 3 and Ga 2 O 3 respectively) are amphoteric, indium(III) oxide (In 2 O 3) is nearly amphoteric, and thallium(III) oxide (Tl 2 O 3) is a Lewis base because it dissolves in acids to form salts.
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 ...
Indium tin oxide (ITO) is a ternary composition of indium, tin and oxygen in varying proportions. Depending on the oxygen content, it can be described as either a ceramic or an alloy . Indium tin oxide is typically encountered as an oxygen-saturated composition with a formulation of 74% In, 8% Sn, and 18% O by weight.
Antimony also forms a mixed-valence oxide, antimony tetroxide (Sb 2 O 4), which features both Sb(III) and Sb(V). [26] Unlike oxides of phosphorus and arsenic, these oxides are amphoteric, do not form well-defined oxoacids, and react with acids to form antimony salts. Antimonous acid Sb(OH) 3 is unknown, but the conjugate base sodium antimonite ...
Ion–dipole and ion–induced dipole forces are stronger than dipole–dipole interactions because the charge of any ion is much greater than the charge of a dipole moment. Ion–dipole bonding is stronger than hydrogen bonding. [8] An ion–dipole force consists of an ion and a polar molecule interacting.
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.