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Aluminium oxide (or aluminium(III) oxide) is a chemical compound of aluminium and oxygen with the chemical formula Al 2 O 3. It is the most commonly occurring of several aluminium oxides, and specifically identified as aluminium oxide. It is commonly called alumina and may also be called aloxide, aloxite, or alundum in various forms and ...
A thermite reaction using iron(III) oxide. The sparks flying outwards are globules of molten iron trailing smoke in their wake. In the following example, elemental aluminum reduces the oxide of another metal, in this common example iron oxide, because aluminum forms stronger and more stable bonds with oxygen than iron: Fe 2 O 3 + 2 Al → 2 Fe ...
Aluminothermic reactions are exothermic chemical reactions using aluminium as the reducing agent at high temperature. The process is industrially useful for production of alloys of iron. [1] The most prominent example is the thermite reaction between iron oxides and aluminium to produce iron itself: Fe 2 O 3 + 2 Al → 2 Fe + Al 2 O 3
Schematic illustration of one reaction cycle of the ALD process, using the trimethylaluminium (TMA) -water process to make thin aluminium oxide films as (simplified) example. There, the starting surface contains hydroxyls (OH groups) as reactive sites; Step 1 is the reaction of TMA; Step 2 is a purge or evacuation step, Step 3 is the reaction ...
Aluminium oxides or aluminum oxides are a group of inorganic compounds with formulas including aluminium (Al) and oxygen (O). Aluminium(I) oxide ( Al 2 O ) Aluminium(II) oxide ( AlO ) (aluminium monoxide)
A fine powder of aluminium reacts explosively on contact with liquid oxygen; under normal conditions, however, aluminium forms a thin oxide layer (~5 nm at room temperature) [43] that protects the metal from further corrosion by oxygen, water, or dilute acid, a process termed passivation.
The water in the air actually sticks to the alumina itself in between the tiny passages as the air passes through them. The water molecules become trapped so that the air is dried out as it passes through the filter. This process is reversible. If the alumina desiccant is heated to ~200 °C, it will release the trapped water.
Well known examples are the vanadyl(IV) and uranyl(VI) ions. They can be viewed as particularly stable hydrolysis products in a hypothetical reaction such as [V(H 2 O) 6] 4+ → [VO(H 2 O) 5] 2+ + 2H + The vanadium has a distorted octahedral environment (point group C 4v) of one oxide ion and 5 water molecules. [61] Titanyl, TiO 2+, has a ...