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Rubidium oxide is highly reactive towards water, and therefore it would not be expected to occur naturally. The rubidium content in minerals is often calculated and quoted in terms of Rb 2 O. In reality, the rubidium is typically present as a component of (actually, an impurity in) silicate or aluminosilicate.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
The tables below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure. Units of solubility are given in grams of substance per 100 millilitres of water (g/100 ml), unless shown otherwise. The substances are listed in alphabetical order.
Rubidium reacts violently with water and can cause fires. To ensure safety and purity, this metal is usually kept under dry mineral oil or sealed in glass ampoules in an inert atmosphere. Rubidium forms peroxides on exposure even to a small amount of air diffused into the oil, and storage is subject to similar precautions as the storage of ...
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]
Solubility in water. reacts [3] Related compounds Other anions. Rubidium oxide Rubidium superoxide: Other cations. Lithium peroxide Sodium peroxide Potassium peroxide
Rubidium carbonate, Rb 2 C O 3, is a convenient compound of rubidium; it is stable, not particularly reactive, and readily soluble in water, and is the form in which rubidium is usually sold. Preparation
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.