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Perbromic acid – HBrO 4 [161] Aluminium Bromide – AlBr 3 [11] Ammonium bromide – NH 4 Br [37] Boron tribromide – BBr 3 [146] Bromic acid – HBrO 3 [162] Bromine monoxide – Br 2 O [163] Bromine pentafluoride – BrF 5 [164] Bromine trifluoride – BrF 3 [165] Bromine monofluoride – BrF [166] Calcium bromide – CaBr 2 [167] Carbon ...
Mineral acids are used in many sectors of the chemical industry as feedstocks for the synthesis of other chemicals, both organic and inorganic. Large quantities of these acids – especially sulfuric acid, nitric acid, and hydrochloric acid – are manufactured for commercial use in large plants.
Phosphoric acids and phosphates; Phosphorus oxoacid; Platinum–samarium; Plutonium selenide; Plutonium silicide; Potassium bifluoride; Potassium pentasulfide; Potassium sulfide; Praseodymium(III) fluoride; Praseodymium(III) nitride; Praseodymium(III) oxalate; Praseodymium(IV) fluoride
An inorganic compound is typically a chemical compound that lacks carbon–hydrogen bonds — that is, a compound that is not an organic compound. [1] [2] The study of inorganic compounds is a subfield of chemistry known as inorganic chemistry.
Acetic acid: an organic acid; is one of the simplest carboxylic acids: Acetone: an organic compound; simplest example of the ketones: Acetylene: a hydrocarbon and the simplest alkyne; widely used as a fuel and chemical building block Ammonia: inorganic; the precursor to most nitrogen-containing compounds; used to make fertilizer Ammonium hydroxide
A monosaccharide with nine carbons. An example is sialic acid. Periodic acid: Periodic acid Or per-iodic acid, is pronounced / ˌ p ɜːr aɪ ˈ ɒ d ɪ k / PURR-eye-OD-ik and not * / ˌ p ɪər i ˈ ɒ d ɪ k / PEER-ee-OD-ik. It refers to one of two interconvertible species: HIO 4 (metaperiodic acid), or H 5 IO 6 (orthoperiodic acid
Inorganic compounds exhibit a range of bonding properties. Some are ionic compounds, consisting of very simple cations and anions joined by ionic bonding.Examples of salts (which are ionic compounds) are magnesium chloride MgCl 2, which consists of magnesium cations Mg 2+ and chloride anions Cl −; or sodium hydroxide NaOH, which consists of sodium cations Na + and hydroxide anions OH −.
The strength of an inorganic acid is dependent on the oxidation state for the atom to which the proton may be attached. Acid strength is solvent-dependent. For example, hydrogen chloride is a strong acid in aqueous solution, but is a weak acid when dissolved in glacial acetic acid.