User:Mongslaw/draft amino acid chelate

this will be the draft page for amino acid chelate article. using borate article as an initial template.

An amino acid chelate in chemistry is an organometallic molecule consisting of a metal atom chelated by at least one ligand that is an amino acid.

Structure
The metal atom of an amino acid chelate is typically a divalent cation: amino acids form coordination complexes, rather than chelates, with monovalent cations such as potassium and sodium. Amino acids are polydentate ligands able to form ionic bonds with the metal atom at the carboxyl group and covalent bonds via electron pair sharing with nitrogen at the amine group.

Uses
Amino acid chelates are used commercially in plant, animal and human nutrition.

boron oxoanions, with boron in oxidation state +3. The simplest borate ion is the trigonal planar, BO33−, although many others are known. BO33− forms salts with metallic elements. Boron found in nature is commonly as a borate mineral. Boron is also found combined with silicate to form complex borosilicate minerals such as the tourmalines. Many borates are readily hydrated and contain structural hydroxide groups and should formally be considered as hydroxoborates.

Aqueous chemistry
In aqueous solution borate exists in many forms. In acid and near-neutral conditions, it is boric acid, commonly written as H3BO3 but more correctly B(OH)3. The pKa of boric acid is 9.14 at 25°C. Boric acid does not dissociate in aqueous solution, but is acidic due to its interaction with water molecules, forming tetrahydroxyborate:


 * B(OH)3 + H2O B(OH)$− 4$ + H+
 * Ka = 5.8x10−10 mol/l; pKa = 9.24.

Polymeric anions containing structural OH units (polyhydroxoborates) are formed at pH 7–10 if the boron concentration is higher than about 0.025 mol/L. The best known of these is the ion found in the mineral borax:


 * 4 B(OH)$− 4$ + 2 H+ B4O5(OH)$2− 4$ + 7 H2O

Even though boric acid adds hydroxide to form B(OH)$− 4$, the fictitious ions are easier to use for pKa values and other calculations. Thus for a typical polyprotic acid, the deprotonation series dihydrogen borate [H2BO$− 3$], hydrogen borate [HBO$2− 3$], and borate [BO$3− 3$] may be written as pH increases.

Polymeric ions
A number of polymeric borate ions are known in anhydrous compounds, which are made by reacting B(OH)3 or B2O3 with metal oxides, for example:
 * diborate B2O54− e.g. in Mg2B2O5 (suanite)
 * triborate B3O75- in CaAlB3O7 (johachidolite)
 * tetraborate B4O96− in e.g. Li6B4O9
 * metaborates containing the linear [BO2−]n with three coordinate boron e.g. in LiBO2, CaB2O4
 * metaborates containing 3 and four coordinate boron, often these are high pressure modifications.

Common borate salts
Common borate salts include sodium metaborate, NaBO2, and sodium tetraborate, Na2B4O7, which is usually encountered as borax the so-called decahydrate, and actually contains the hydroxoborate ion, B4O5(OH)4 2− and is formulated Na2[B4O5(OH)4]·8H2O.

Boron, California contains large borax deposits and is used extensively for borate mining. The Atacama Desert in Chile also contains mineable borate concentrations. Gerry, New York has been described by Agapito Associates Inc. as a "very nice place to mine for [borate]" although it is uncertain how much damage that might do to the surrounding area.

Various forms of borate are used as wood preservatives or fungicides such as disodium octaborate tetrahydrate.

Borate esters
Borate esters are organic compounds of the type B(OR)3 where R is an organic residue (for example alkyl or aryl). Borate esters include trimethyl borate, B(OCH3)3, which is used as a precursor to boronic esters for Suzuki couplings.