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Each Ba 2+ center is bound by two water ligands and six hydroxide ligands, which are respectively doubly and triply bridging to neighboring Ba 2+ centre sites. [4] In the octahydrate, the individual Ba 2+ centers are again eight coordinate but do not share ligands. [5] Coordination sphere about an individual barium ion in Ba(OH) 2.H 2 O.
The molecular formula C 2 H 4 Br 2 (molar mass: 187.86 g/mol, exact mass: 185.8680 u) may refer to: 1,1-Dibromoethane (ethylidene dibromide)
[9]: 2–3 Reactions with water and alcohols are also exothermic and release hydrogen gas: [9]: 3 Ba + 2 ROH → Ba(OR) 2 + H 2 ↑ (R is an alkyl group or a hydrogen atom) Barium reacts with ammonia to form the electride [Ba(NH 3) 6](e −) 2, which near room temperature gives the amide Ba(NH 2) 2. [11] The metal is readily attacked by acids.
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1,2-Dibromoethane, also known as ethylene dibromide (EDB), is an organobromine compound with the chemical formula C 2 H 4 Br 2. Although trace amounts occur naturally in the ocean, where it is probably formed by algae and kelp, substantial amounts are produced industrially. It is a dense colorless liquid with a faint, sweet odor, detectable at ...
[1] [2] An addition reaction is limited to chemical compounds that have multiple bonds. Examples include a molecule with a carbon–carbon double bond (an alkene) or a triple bond (an alkyne). Another example is a compound that has rings (which are also considered points of unsaturation).
Bond energies to bromine tend to be lower than those to chlorine but higher than those to iodine, and bromine is a weaker oxidising agent than chlorine but a stronger one than iodine. This can be seen from the standard electrode potentials of the X 2 /X − couples (F, +2.866 V; Cl, +1.395 V; Br, +1.087 V; I, +0.615 V; At, approximately +0.3 V ...
Barium bromide is a precursor to chemicals used in photography and to other bromides. Historically, barium bromide was used to purify radium in a process of fractional crystallization devised by Marie Curie.