Difference between revisions of "Ammonium"
| (7 intermediate revisions by the same user not shown) | |||
| Line 1: | Line 1: | ||
| − | '''Ammonium''' is | + | '''Ammonium''' is a [[cation]] with a formula of '''NH<sub>4</sub><sup>+</sup>'''. It is pseudo-metallic in its properties and greatly resembles alkali metals. |
== Free ammonium == | == Free ammonium == | ||
| − | Free "metallic" ammonium does not exist as a pure substance, but it can be prepared as an amalgam with mercury. The amalgam of ammonium is a grey substance, often spongy (in high concentrations, ammonium spontaneously decomposes into [[ammonia]] and [[hydrogen]], producing gas bubbles which give it its characteristic sponginess). Low-concentration amalgams of ammonium react with water, evolving hydrogen and forming a water solution of ammonia (the "ammonium hydroxide"), like alkali metals. High concentrations evolve a mixture of ammonia and hydrogen. | + | Free "metallic" ammonium does not exist as a pure substance, but it can be prepared as an [[amalgam]] with [[mercury]]. The amalgam of ammonium is a grey substance, often spongy (in high concentrations, ammonium spontaneously decomposes into [[ammonia]] and [[hydrogen]], producing gas bubbles which give it its characteristic sponginess). Low-concentration amalgams of ammonium react with water, evolving hydrogen and forming a water solution of [[ammonia]] (the "ammonium hydroxide"), like alkali metals. High concentrations evolve a mixture of ammonia and hydrogen.<ref>https://www.youtube.com/watch?v=Hp9PIXOYaEA</ref> |
== Ammonium salts == | == Ammonium salts == | ||
| − | Both "ammonium hydroxide" (a solution of ammonia in water, in which the ionic species NH<sub>4</sub>OH is a minor tautomer) and gaseous freebase ammonia are capable of forming salts with acids. These salts look and behave like typical alkali metal salts, in that they are colorless or colored by the anion, and soluble in water. Heat causes them to decompose into ammonia and the acid, sometimes reversibly, sometimes - when the acid itself decomposes - irreversibly. | + | Both "ammonium hydroxide" (a solution of ammonia in water, in which the ionic species NH<sub>4</sub>OH is a minor tautomer) and gaseous freebase ammonia are capable of forming salts with acids. These salts look and behave like typical alkali metal salts, in that they are colorless or colored by the anion, and soluble in water. Heat causes them to decompose into ammonia and the acid, sometimes reversibly (like in the case of haloacids), sometimes - when the acid itself decomposes - irreversibly. |
| − | Ammonium salts of strongly oxidizing acids are known to be energetic materials. | + | Ammonium salts of strongly oxidizing acids are known to be energetic materials. However, some ammonium salts of potent oxidizing species are not possible to synthesize, since they immediately decompose. One example is ammonium ferrate. |
== Substituted ammoniums == | == Substituted ammoniums == | ||
| − | Ammonium forms a large amount of organic derivatives, which can be divided into two groups: quaternary | + | Ammonium forms a large amount of organic derivatives, which can be divided into two groups: quaternary ammonium ions and everything else. The "usual" (non-quaternary) organic ammonium derivatives should be more properly thought of as derivatives of ''[[ammonia]]'' that form ammonium-like cations: they are organic bases that can exist in freebase form, just like ammonia itself, they typically do not form stable, isolable hydroxides and are weak or mid-strength bases. Quaternary ammoniums do not exist as freebases, but form stable, isolable ionic hydroxides that behave like alkali metal hydroxides; these are typically strong bases. |
| + | |||
| + | ==References== | ||
| + | <references/> | ||
| + | ===Relevant Sciencemadness threads=== | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=4619 Ammonium salts preparation....] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=73370 Sensitive ammonium compounds and synthesis] | ||
| − | |||
| − | |||
| − | |||
| − | |||
[[Category:Ions]] | [[Category:Ions]] | ||
[[Category:Cations]] | [[Category:Cations]] | ||
Latest revision as of 18:22, 2 January 2023
Ammonium is a cation with a formula of NH4+. It is pseudo-metallic in its properties and greatly resembles alkali metals.
Contents
Free ammonium
Free "metallic" ammonium does not exist as a pure substance, but it can be prepared as an amalgam with mercury. The amalgam of ammonium is a grey substance, often spongy (in high concentrations, ammonium spontaneously decomposes into ammonia and hydrogen, producing gas bubbles which give it its characteristic sponginess). Low-concentration amalgams of ammonium react with water, evolving hydrogen and forming a water solution of ammonia (the "ammonium hydroxide"), like alkali metals. High concentrations evolve a mixture of ammonia and hydrogen.[1]
Ammonium salts
Both "ammonium hydroxide" (a solution of ammonia in water, in which the ionic species NH4OH is a minor tautomer) and gaseous freebase ammonia are capable of forming salts with acids. These salts look and behave like typical alkali metal salts, in that they are colorless or colored by the anion, and soluble in water. Heat causes them to decompose into ammonia and the acid, sometimes reversibly (like in the case of haloacids), sometimes - when the acid itself decomposes - irreversibly.
Ammonium salts of strongly oxidizing acids are known to be energetic materials. However, some ammonium salts of potent oxidizing species are not possible to synthesize, since they immediately decompose. One example is ammonium ferrate.
Substituted ammoniums
Ammonium forms a large amount of organic derivatives, which can be divided into two groups: quaternary ammonium ions and everything else. The "usual" (non-quaternary) organic ammonium derivatives should be more properly thought of as derivatives of ammonia that form ammonium-like cations: they are organic bases that can exist in freebase form, just like ammonia itself, they typically do not form stable, isolable hydroxides and are weak or mid-strength bases. Quaternary ammoniums do not exist as freebases, but form stable, isolable ionic hydroxides that behave like alkali metal hydroxides; these are typically strong bases.
