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Rubidium oxide is the chemical compound with the formula Rb 2 O. Rubidium oxide is highly reactive towards water, and therefore it would not be expected to occur naturally. Rubidium oxide is highly reactive towards water, and therefore it would not be expected to occur naturally.
Rubidium ozonide is an oxygen rich compound of rubidium. It is an ozonide , meaning it contains the ozonide anion (O 3 − ). It can be created by reacting rubidium superoxide (RbO 2 ) with ozone (O 3 ) in a liquid ammonia solution.
Rubidium forms a number of oxides when exposed to air, including rubidium monoxide (Rb 2 O), Rb 6 O, and Rb 9 O 2; rubidium in excess oxygen gives the superoxide RbO 2. Rubidium forms salts with halogens, producing rubidium fluoride , rubidium chloride , rubidium bromide , and rubidium iodide .
Rubidium sesquioxide is a chemical compound with the formula Rb 2 O 3 or more accurately Rb 4 O 6.In terms of oxidation states, Rubidium in this compound has a nominal charge of +1, and the oxygen is a mixed peroxide (O 2− 2) and superoxide (O − 2) for a structural formula of (Rb +) 4 (O − 2) 2 (O 2− 2). [4]
Inorganic ozonides [1] are dark red salts. The anion has the bent shape of the ozone molecule.. Inorganic ozonides are formed by burning potassium, rubidium, or caesium in ozone, or by treating the alkali metal hydroxide with ozone; this yields potassium ozonide, rubidium ozonide, and caesium ozonide respectively.
It can be created by slowly exposing elemental rubidium to oxygen gas: [3] Rb(s) + O 2 (g) → RbO 2 (s) Like other alkali metal hyperoxides, crystals can also be grown in liquid ammonia. [4] Between 280 and 360 °C, Rubidium superoxide will decompose, leaving not rubidium sesquioxide (Rb 2 O 3), but rather rubidium peroxide (Rb 2 O 2). [3]
Each oxygen atom in its peroxide ion may have a full octet of 4 pairs of electrons. [6] Superoxides are a class of compounds that are very similar to peroxides, but with just one unpaired electron for each pair of oxygen atoms (O − 2). [6] These compounds form by oxidation of alkali metals with larger ionic radii (K, Rb, Cs).
The standard enthalpy of formation of the crystalline rubidium oxalate is 1325.0 ± 8.1 kJ/mol. [9] The decomposition of rubidium oxalate with the release of carbon monoxide and subsequently carbon dioxide and oxygen takes place at 507–527 °C (945–981 °F; 780–800 K). [6] [2] Rb 2 C 2 O 4 → Rb 2 CO 3 + CO↑ Rb 2 CO 3 → Rb 2 O + CO 2 ...