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Gallium(III) oxide is an inorganic compound and ultra-wide-bandgap semiconductor with the formula Ga 2 O 3. ... Gallium(III) trioxide is amphoteric. [26]
Many metals (such as zinc, tin, lead, aluminium, and beryllium) form amphoteric oxides or hydroxides. Aluminium oxide (Al 2 O 3) is an example of an amphoteric oxide. Amphoterism depends on the oxidation states of the oxide. Amphoteric oxides include lead(II) oxide and zinc oxide, among many others. [2]
At room temperature, gallium metal is not reactive with air and water because it forms a passive, protective oxide layer. At higher temperatures, however, it reacts with atmospheric oxygen to form gallium(III) oxide, Ga 2 O 3. [4] Reducing Ga 2 O 3 with elemental gallium in vacuum at 500 °C to 700 °C yields the dark brown gallium(I) oxide, Ga ...
Gallium oxide may refer to Gallium(I) oxide, Ga 2 O; Gallium(III) oxide, Ga 2 O 3 This page was last edited on 8 September 2020, at 13:36 (UTC). Text is available ...
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. Each of these compounds are stable, but thallium oxide decomposes at ...
At higher temperatures, however, it reacts with atmospheric oxygen to form gallium(III) oxide, Ga 2 O 3. [34] Reducing Ga 2 O 3 with elemental gallium in vacuum at 500 °C to 700 °C yields the dark brown gallium(I) oxide, Ga 2 O. [33]: 285 Ga 2 O is a very strong reducing agent, capable of reducing H 2 SO 4 to H 2 S.
Gallium is a soft, brittle metal (MH 1.5) that melts at only a few degrees above room temperature. [102] It has an unusual crystalline structure featuring mixed metallic-covalent bonding and low symmetry [102] (BCN 7 i.e. 1+2+2+2). [103] It bonds covalently in most of its compounds, [104] has an amphoteric oxide; [105] and can form anionic ...
Gallium(I) oxide is a brown-black diamagnetic solid which is resistant to further oxidation in dry air. It starts decomposing upon heating at temperatures above 500 °C, and the decomposition rate depends on the atmosphere (vacuum, inert gas, air).