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10.1016/0020-1693(94)04222-H V(II)en3 sulfate, Men3: one V, no Mo

M(en)3]OAc2 doi 10.1107/S2053229617006738
	2.2693	2.2085	2.1661	2.1205	2.1693	2.1847 Mn-Zn
Cu 4 x 2.05 2 x 2.39
Λ(δδδ) and Δ(λλλ) 

10.1351/pac198456040491 Formation of metal complexes with ethylenediamine: a critical survey of equilibrium constants, enthalpy and entropy values

10.1039/c6cs00604c JAG
==Perchlorate complexes==

CuOAc
10.1039/C39730000124

{{t|NMR spectroscopy
| nucleus  = 
| nuclear magnetic moment = 
| natural abundance =
| receptivity vs 1H NMR
| chemical shift reference(s)
| chemical shift range (diamagnetic samples)
}}


AgClO4 (H2O): 10.1524/zkri.1995.210.11.879

==To check in the future==
mostly questionable homework:
*[[Infrared spectroscopy]]
*[[Chemical property]]
*[[benzimidazole]]
*[[silicon nitride]]
*[[Tröger's base]]

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| Density = 3.151 g/cm<sup>3</sup>
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Molybdenum oxytrichloride is the  is the [[inorganic compound]] with the formula MoOCl<sub>3</sub>. It is a red paramagnetic solid, one of several [[oxychloride]]s of molybdenum.  The compound is prepared by reduction of [[molybdenum oxotetrachloride]] with [[aluminium]].  One distinction for MoOCl<sub>3</sub> is that it crystallizes with terminal oxo and with bridging oxo ligands (as in NbOCl<sub>3</sub>).<ref>{{cite journal |doi=10.1039/J19690002019}}</ref>

==Structure==
The compound has a polymeric structure consisting of Mo(O)Cl groups linked by chlorides.  Thus, each Mo center is octahedral, but distorted.  Two of the bridging chlorides have Mo-Cl distances near 2.45 Åbut the other two, which are trans to oxo ligands, are long and short, 2.78 and 2.34 Å.  The one terminal chloride is bonded to Mo with a distance of 2.28 Å, the shortest bond.<ref>{{cite journal |doi=10.1039/j19700000022 |title=Crystal and Molecular Structure of Molybdenum(V) Oxide Trichloride |date=1970 |last1=Drew |first1=Michael G. B. |last2=Tomkins |first2=I. B. |journal=Journal of the Chemical Society A: Inorganic, Physical, Theoretical |page=22 }}</ref><ref>{{cite journal |doi=10.1039/j19690002415 |title=Oxide Chlorides of Tungsten and Molybdenum. Part II. Crystal Structure of the Monoclinic Form of Molybdenum Oxide Trichloride |date=1969 |last1=Ferguson |first1=G. |last2=Mercer |first2=M. |last3=Sharp |first3=D. W. A. |journal=Journal of the Chemical Society A: Inorganic, Physical, Theoretical |page=2415 }}</ref>

==Related compounds==
[[Molybdenum dichloride dioxide]], a yellow diamagnetic solid.

==References==
{{reflist}}

{{Molybdenum compounds}}

[[Category:Molybdenum(VI) compounds]]
[[Category:Oxychlorides]]
</nowiki>

==Ref spam project==

===Zwitterion===
*{{Cite journal |last=Novikov |first=Anton P. |last2=Safonov |first2=Alexey V. |last3=German |first3=Konstantin E. |last4=Grigoriev |first4=Mikhail S. |date=2023-12-01 |title=What kind of interactions we may get moving from zwitter to “dritter” ions: C–O⋯Re(O4) and Re–O⋯Re(O4) anion⋯anion interactions make structural difference between L-histidinium perrhenate and pertechnetate |url=https://pubs.rsc.org/en/content/articlelanding/2024/ce/d3ce01164j |journal=CrystEngComm |language=en |doi=10.1039/D3CE01164J |issn=1466-8033}}
===Chlorine===
*{{Cite journal |last=Wheeler |first=Ralph A. |last2=Hoffmann |first2=Roald. |date=1986-10 |title=A new magic cluster electron count and metal-metal multiple bonding |url=https://pubs.acs.org/doi/abs/10.1021/ja00281a025 |journal=Journal of the American Chemical Society |language=en |volume=108 |issue=21 |pages=6605–6610 |doi=10.1021/ja00281a025 |issn=0002-7863}}
*[https://www.researchgate.net/publication/349821179_Synthesis_and_properties_of_new_chloride_technetium_clusters]
*{{Cite journal |last=Zhang |first=Weiwei |last2=Oganov |first2=Artem R. |last3=Goncharov |first3=Alexander F. |last4=Zhu |first4=Qiang |last5=Boulfelfel |first5=Salah Eddine |last6=Lyakhov |first6=Andriy O. |last7=Stavrou |first7=Elissaios |last8=Somayazulu |first8=Maddury |last9=Prakapenka |first9=Vitali B. |last10=Konôpková |first10=Zuzana |date=2013-12-20 |title=Unexpected Stable Stoichiometries of Sodium Chlorides |url=https://www.science.org/doi/10.1126/science.1244989 |journal=Science |language=en |volume=342 |issue=6165 |pages=1502–1505 |doi=10.1126/science.1244989 |issn=0036-8075}}
===Sodium pertechnetate===
*{{Cite journal |last=German |first=K. E. |last2=Grigoriev |first2=M. S. |last3=Garashchenko |first3=B. L. |last4=Kopytin |first4=A. V. |last5=Tyupina |first5=E. A. |date=2017-07-01 |title=Redetermination of the crystal structure of NaTcO4 at 100 and 296 K based on single-crystal X-ray data |url=https://scripts.iucr.org/cgi-bin/paper?wm5391 |journal=Acta Crystallographica Section E: Crystallographic Communications |language=en |volume=73 |issue=7 |pages=1037–1040 |doi=10.1107/S2056989017008362 |issn=2056-9890 |pmc=PMC5499285 |pmid=28775877}}
===Technetium===
*{{Cite journal |last=Zhou |first=Di |last2=Semenok |first2=Dmitrii V. |last3=Volkov |first3=Mikhail A. |last4=Troyan |first4=Ivan A. |last5=Seregin |first5=Alexey Yu. |last6=Chepkasov |first6=Ilya V. |last7=Sannikov |first7=Denis A. |last8=Lagoudakis |first8=Pavlos G. |last9=Oganov |first9=Artem R. |last10=German |first10=Konstantin E. |date=2023-02-06 |title=<nowiki>Synthesis of technetium hydride $\mathrm{Tc}{\mathrm{H}}_{1.3}$ at 27 GPa</nowiki> |url=https://link.aps.org/doi/10.1103/PhysRevB.107.064102 |journal=Physical Review B |volume=107 |issue=6 |pages=064102 |doi=10.1103/PhysRevB.107.064102}}
*{{Cite journal |last=German |first=K. E. |last2=Peretrukhin |first2=V. F. |last3=Gedgovd |first3=K. N. |last4=Grigoriev |first4=M. S. |last5=Tarasov |first5=A. V. |last6=Plekhanov |first6=Yu V. |last7=Maslennikov |first7=A. G. |last8=Bulatov |first8=G. S. |last9=Tarasov |first9=V. P. |last10=Lecomte |first10=M. |date=2005 |title=Tc Carbide and New Orthorhombic Tc Metal Phase |url=https://www.jstage.jst.go.jp/article/jnrs2000/6/3/6_3_211/_article |journal=Journal of Nuclear and Radiochemical Sciences |volume=6 |issue=3 |pages=211–214 |doi=10.14494/jnrs2000.6.3_211}}
*{{cite book| title=The Encyclopedia of the Chemical Elements| editor=Hampel, C. A.| last=Rimshaw |first=S. J.| location=New York| publisher=Reinhold Book Corporation| date=1968| url=https://archive.org/details/encyclopediaofch00hamp| url-access=registration| pages=[https://archive.org/details/encyclopediaofch00hamp/page/689 689–693]}}
*{{cite news| title = Technetium as a Material for AC Superconductivity Applications| last = Autler |first=S. H.| publisher = Proceedings of the 1968 Summer Study on Superconducting Devices and Accelerators|access-date = 2009-05-05|date=1968| url = http://www.bnl.gov/magnets/Staff/Gupta/Summer1968/0049.pdf}}
===Group VII element===
*{{Cite journal |last=German |first=Konstantin E. |last2=Fedoseev |first2=Alexander M. |last3=Grigoriev |first3=Mikhail S. |last4=Kirakosyan |first4=Gayane A. |last5=Dumas |first5=Thomas |last6=Den Auwer |first6=Christophe |last7=Moisy |first7=Philippe |last8=Lawler |first8=Keith V. |last9=Forster |first9=Paul M. |last10=Poineau |first10=Frederic |date=2021-09-24 |title=A 70‐Year‐Old Mystery in Technetium Chemistry Explained by the New Technetium Polyoxometalate [H 7 O 3 ] 4 [Tc 20 O 68 ] ⋅ 4H 2 O |url=https://chemistry-europe.onlinelibrary.wiley.com/doi/10.1002/chem.202102035 |journal=Chemistry – A European Journal |language=en |volume=27 |issue=54 |pages=13624–13631 |doi=10.1002/chem.202102035 |issn=0947-6539}}
===Polyoxometalate===
*{{cite journal |last1=Volkov |first1=Mikhail A. |last2=Novikov |first2=Anton P. |last3=Borisova |first3=Nataliya E. |last4=Grigoriev |first4=Mikhail S. |last5=German |first5=Konstantin E. |title=Intramolecular Re···O Nonvalent Interactions as a Stabilizer of the Polyoxorhenate(VII) |journal=Inorganic Chemistry |date=10 August 2023 |volume=XX |issue=XX |pages=XXXX–XXXX |doi=10.1021/acs.inorgchem.3c01863|pmid=XXX |s2cid=XXXX }}
===Rhenium===
*{{Cite journal |last=Volkov |first=Mikhail A. |last2=Novikov |first2=Anton P. |last3=Borisova |first3=Nataliya E. |last4=Grigoriev |first4=Mikhail S. |last5=German |first5=Konstantin E. |date=2023-08-21 |title=Intramolecular Re···O Nonvalent Interactions as a Stabilizer of the Polyoxorhenate(VII) |url=https://pubs.acs.org/doi/10.1021/acs.inorgchem.3c01863 |journal=Inorganic Chemistry |language=en |volume=62 |issue=33 |pages=13485–13494 |doi=10.1021/acs.inorgchem.3c01863 |issn=0020-1669}}

{{Cite journal |last=Volkov |first=Mikhail A. |last2=Novikov |first2=Anton P. |last3=Borisova |first3=Nataliya E. |last4=Grigoriev |first4=Mikhail S. |last5=German |first5=Konstantin E. |date=2023-08-21 |title=Intramolecular Re···O Nonvalent Interactions as a Stabilizer of the Polyoxorhenate(VII) |url=https://pubs.acs.org/doi/10.1021/acs.inorgchem.3c01863 |journal=Inorganic Chemistry |language=en |volume=62 |issue=33 |pages=13485–13494 |doi=10.1021/acs.inorgchem.3c01863 |issn=0020-1669}}
<!--

Zwitterion
Some aminoacids bear more than 2 charges and may form mixed salts, <ref>{{Cite journal |last=Novikov |first=Anton P. |last2=Safonov |first2=Alexey V. |last3=German |first3=Konstantin E. |last4=Grigoriev |first4=Mikhail S. |date=2023-12-01 |title=What kind of interactions we may get moving from zwitter to “dritter” ions: C–O⋯Re(O4) and Re–O⋯Re(O4) anion⋯anion interactions make structural difference between L-histidinium perrhenate and pertechnetate |url=https://pubs.rsc.org/en/content/articlelanding/2024/ce/d3ce01164j |journal=CrystEngComm |language=en |doi=10.1039/D3CE01164J |issn=1466-8033}}</ref> where the H-bond systems may vary providing supplementary recognition options.

Chlorine
<ref>{{Cite journal |last=Wheeler |first=Ralph A. |last2=Hoffmann |first2=Roald. |date=1986-10 |title=A new magic cluster electron count and metal-metal multiple bonding |url=https://pubs.acs.org/doi/abs/10.1021/ja00281a025 |journal=Journal of the American Chemical Society |language=en |volume=108 |issue=21 |pages=6605–6610 |doi=10.1021/ja00281a025 |issn=0002-7863}}</ref>

The Table below presents typical oxidation states for chlorine element as given in the secondary schools or colleges. Anyhow in university chemistry courses it should be pointed out that there are more complex chemical compounds, the structure of which can only be explained using modern quantum chemical methods, for example, cluster technetium chloride [(CH<sub>3</sub>)<sub>4</sub>N]<sub>3</sub>[Tc<sub>6</sub>Cl<sub>14</sub>], in which 6 of the 14 chlorine atoms are formally divalent, and oxidation states are fractional [https://www.researchgate.net/publication/349821179_Synthesis_and_properties_of_new_chloride_technetium_clusters] . In addition, all the above chemical regularities are valid for "normal" or close to normal conditions, while at ultra-high pressures (for example, in the cores of large planets), chlorine can exhibit an oxidation state of -3, forming a Na3Cl compound with sodium, which does not fit into traditional concepts of chemistry.<ref>{{Cite journal |last=Zhang |first=Weiwei |last2=Oganov |first2=Artem R. |last3=Goncharov |first3=Alexander F. |last4=Zhu |first4=Qiang |last5=Boulfelfel |first5=Salah Eddine |last6=Lyakhov |first6=Andriy O. |last7=Stavrou |first7=Elissaios |last8=Somayazulu |first8=Maddury |last9=Prakapenka |first9=Vitali B. |last10=Konôpková |first10=Zuzana |date=2013-12-20 |title=Unexpected Stable Stoichiometries of Sodium Chlorides |url=https://www.science.org/doi/10.1126/science.1244989 |journal=Science |language=en |volume=342 |issue=6165 |pages=1502–1505 |doi=10.1126/science.1244989 |issn=0036-8075}}</ref>

Sodium pertechnetate
that has slightly distorted tetrahedron symmetry both at 296 K and at 100 K<ref>{{Cite journal |last=German |first=K. E. |last2=Grigoriev |first2=M. S. |last3=Garashchenko |first3=B. L. |last4=Kopytin |first4=A. V. |last5=Tyupina |first5=E. A. |date=2017-07-01 |title=Redetermination of the crystal structure of NaTcO4 at 100 and 296 K based on single-crystal X-ray data |url=https://scripts.iucr.org/cgi-bin/paper?wm5391 |journal=Acta Crystallographica Section E: Crystallographic Communications |language=en |volume=73 |issue=7 |pages=1037–1040 |doi=10.1107/S2056989017008362 |issn=2056-9890 |pmc=PMC5499285 |pmid=28775877}}</ref> 

Technetium
When reacting with [[hydrogen]] at high pressure, it forms the hydride TcH1.3.<ref>{{Cite journal |last=Zhou |first=Di |last2=Semenok |first2=Dmitrii V. |last3=Volkov |first3=Mikhail A. |last4=Troyan |first4=Ivan A. |last5=Seregin |first5=Alexey Yu. |last6=Chepkasov |first6=Ilya V. |last7=Sannikov |first7=Denis A. |last8=Lagoudakis |first8=Pavlos G. |last9=Oganov |first9=Artem R. |last10=German |first10=Konstantin E. |date=2023-02-06 |title=<nowiki>Synthesis of technetium hydride $\mathrm{Tc}{\mathrm{H}}_{1.3}$ at 27 GPa</nowiki> |url=https://link.aps.org/doi/10.1103/PhysRevB.107.064102 |journal=Physical Review B |volume=107 |issue=6 |pages=064102 |doi=10.1103/PhysRevB.107.064102}}</ref>


The unit cell parameters of the orthorhombic Tc metal were reported when Tc is contaminated with carbon (a = 0.2805(4), b = 0.4958(8), c = 0.4474(5)·nm for Tc-C with 1.38 wt% C and a = 0.2815(4), b = 0.4963(8), c = 0.4482(5) •nm for Tc-C with 1.96 wt% C ). <ref>{{Cite journal |last=German |first=K. E. |last2=Peretrukhin |first2=V. F. |last3=Gedgovd |first3=K. N. |last4=Grigoriev |first4=M. S. |last5=Tarasov |first5=A. V. |last6=Plekhanov |first6=Yu V. |last7=Maslennikov |first7=A. G. |last8=Bulatov |first8=G. S. |last9=Tarasov |first9=V. P. |last10=Lecomte |first10=M. |date=2005 |title=Tc Carbide and New Orthorhombic Tc Metal Phase |url=https://www.jstage.jst.go.jp/article/jnrs2000/6/3/6_3_211/_article |journal=Journal of Nuclear and Radiochemical Sciences |volume=6 |issue=3 |pages=211–214 |doi=10.14494/jnrs2000.6.3_211}}</ref> The metal form is slightly [[paramagnetism|paramagnetic]], meaning its [[dipole|magnetic dipoles]] align with external [[magnetic field]]s, but will assume random orientations once the field is removed.<ref name="enc">{{cite book| title=The Encyclopedia of the Chemical Elements| editor=Hampel, C. A.| last=Rimshaw |first=S. J.| location=New York| publisher=Reinhold Book Corporation| date=1968| url=https://archive.org/details/encyclopediaofch00hamp| url-access=registration| pages=[https://archive.org/details/encyclopediaofch00hamp/page/689 689–693]}}</ref> Pure, metallic, single-crystal technetium becomes a [[type-II superconductor]] at temperatures below 7.46&nbsp;[[Kelvin|K]].{{sfn|Schwochau|2000|p=96}}{{efn|Irregular crystals and trace impurities raise this transition temperature to 11.2&nbsp;K for 99.9% pure technetium powder.{{sfn|Schwochau|2000|p=96}} }} Below this temperature, technetium has a very high [[London penetration depth|magnetic penetration depth]], greater than any other element except [[niobium]].<ref>{{cite news| title = Technetium as a Material for AC Superconductivity Applications| last = Autler |first=S. H.| publisher = Proceedings of the 1968 Summer Study on Superconducting Devices and Accelerators|access-date = 2009-05-05|date=1968| url = http://www.bnl.gov/magnets/Staff/Gupta/Summer1968/0049.pdf}}</ref>


Group VII element
Polyoxotechnetate (polyoxometalate of technetium) contains both Tc(V) and Tc(VII) in ratio 4: 16 and is obtained as the [[hydronium]] salt [H<sub>7</sub>O<sub>3</sub>]<sub>4</sub>[Tc<sub>20</sub>O<sub>68</sub>]·4H<sub>2</sub>O by concentrating an HTcO4 solution. <ref>{{Cite journal |last=German |first=Konstantin E. |last2=Fedoseev |first2=Alexander M. |last3=Grigoriev |first3=Mikhail S. |last4=Kirakosyan |first4=Gayane A. |last5=Dumas |first5=Thomas |last6=Den Auwer |first6=Christophe |last7=Moisy |first7=Philippe |last8=Lawler |first8=Keith V. |last9=Forster |first9=Paul M. |last10=Poineau |first10=Frederic |date=2021-09-24 |title=A 70‐Year‐Old Mystery in Technetium Chemistry Explained by the New Technetium Polyoxometalate [H 7 O 3 ] 4 [Tc 20 O 68 ] ⋅ 4H 2 O |url=https://chemistry-europe.onlinelibrary.wiley.com/doi/10.1002/chem.202102035 |journal=Chemistry – A European Journal |language=en |volume=27 |issue=54 |pages=13624–13631 |doi=10.1002/chem.202102035 |issn=0947-6539}}</ref>
		
Polyoxometalate
The only polyoxorhenate formed in acidic conditions in presence of pyrazolium cation. The first empirically isolated polyoxorhenate was the white {{chem2|[Re4015](2-)}}. It contains Re(VII) in both octahedral and tetrahedral coordination {{cite journal |last1=Volkov |first1=Mikhail A. |last2=Novikov |first2=Anton P. |last3=Borisova |first3=Nataliya E. |last4=Grigoriev |first4=Mikhail S. |last5=German |first5=Konstantin E. |title=Intramolecular Re···O Nonvalent Interactions as a Stabilizer of the Polyoxorhenate(VII) |journal=Inorganic Chemistry |date=10 August 2023 |volume=XX |issue=XX |pages=XXXX–XXXX |doi=10.1021/acs.inorgchem.3c01863|pmid=XXX |s2cid=XXXX }}</ref>
	'''Rhenium'''
	
	The first empirically isolated polyoxorhenate was the white [Re<sub>4</sub>O<sub>15</sub>]<sup>2−</sup> and contained Re(VII) in both octahedral and tetrahedral coordination. <ref>{{Cite journal |last=Volkov |first=Mikhail A. |last2=Novikov |first2=Anton P. |last3=Borisova |first3=Nataliya E. |last4=Grigoriev |first4=Mikhail S. |last5=German |first5=Konstantin E. |date=2023-08-21 |title=Intramolecular Re···O Nonvalent Interactions as a Stabilizer of the Polyoxorhenate(VII) |url=https://pubs.acs.org/doi/10.1021/acs.inorgchem.3c01863 |journal=Inorganic Chemistry |language=en |volume=62 |issue=33 |pages=13485–13494 |doi=10.1021/acs.inorgchem.3c01863 |issn=0020-1669}}</ref>


Perrhenate may undergo condensation with formation of small rhenium [[polyoxometalate]] Re<sub>4</sub>{{chem|O|15|2-}} <ref>{{Cite journal |last=Volkov |first=Mikhail A. |last2=Novikov |first2=Anton P. |last3=Borisova |first3=Nataliya E. |last4=Grigoriev |first4=Mikhail S. |last5=German |first5=Konstantin E. |date=2023-08-21 |title=Intramolecular Re···O Nonvalent Interactions as a Stabilizer of the Polyoxorhenate(VII) |url=https://pubs.acs.org/doi/10.1021/acs.inorgchem.3c01863 |journal=Inorganic Chemistry |language=en |volume=62 |issue=33 |pages=13485–13494 |doi=10.1021/acs.inorgchem.3c01863 |issn=0020-1669}}</ref> where one central Re has octahedral oxygen coordination while 3 other are tetrahedral.-->


==Photo-nano-H2-==
* [[Artificial photosynthesis]]
* [[Electrochemiluminescence]]

*


*
*[[Photoelectrochemistry]]
*[[Photoelectrochemical cell]]
*[[Photoelectrolysis]]

*[[Electrolysis of water]]
*[[Photocatalytic water splitting]]
*[[Water splitting]]

*[[Hydrogen production]]
*[[Photohydrogen]]
*[[Green hydrogen]]
*[[Solar hydrogen panel]]
*[[Solar–hydrogen energy cycle]]

*[[Photoelectrochemical reduction of CO2]]





==MisterChemistry==
<ref>{{cite journal|doi=10.1016/S0165-9936(03)01008-2 |title=Synthetic chelating agents and compounds exhibiting complexing properties in the aquatic environment |date=2003 |last1=Knepper |first1=T. |journal=Trac Trends in Analytical Chemistry |volume=22 |issue=10 |pages=708–724 }}</ref>.

*[[User contributions for Dhansora210]] spammer
*[[User:MisterChemistry]]
*[[User contributions for CuriousKemist]] ?

==Phth==
The question of how these plastics are affecting the population has arisen as plasticizer use in everyday items has increased. Additionally, if there are any disparities in how these plasticizers may affect minority populations and if they are more susceptible to complications. It has been found that exposure to phthalates is more likely in women and people of color.[14] In one study, researchers looked into potential differences between gender and race as well as potential consequences of this higher phthalate exposure. The study paid particular attention to the relationship between urinary phthalate metabolites and risk factors for diabetes in individuals with no previous diabetes diagnosis. It was found that while there were no statistically significant differences between men and women overall, there were differences between Mexican-Americans, blacks, and whites in terms of the overall risk of disturbance of glucose homeostasis. With Mexican-Americans having a fasting blood glucose (FBG) increase of 5.82 mg/dL, blacks having a fasting blood glucose increase of 3.63 mg/dL, and whites having a fasting blood glucose increase of 1.79 mg/dL, there was evidence of an increased risk for minorities.[14] Overall, the study concludes that phthalates may alter glucose homeostasis and insulin sensitivity, and that different populations may be more severely impacted. Higher levels of some phthalate metabolites were associated with elevated FBG, fasting insulin, and insulin resistance.
In a different study looking at the presence of phthalate metabolites in pregnant women, it was found that non-Hispanic black women and Hispanic women had higher levels of some phthalate metabolites, indicating potential racial disparities in pregnancy outcomes.[15]

==Population info W hemis==
{{sticky header}}
{| class="wikitable sortable sticky-header"
|+2021 list by the [[World Bank]]<ref name="auto"/>
|-
! Country || Total Fertility rate <br /> in 2021<br /><small>(births/woman)</small>||population (M)||area mi<sup>2</sup>||Pop density||per cap income (k, PPP)
|-
|-
| [[Haiti]] || 2.81 || 8.8 || 10 || 989 || 3.2
|-
| [[Bolivia]]|| 2.62 || 12.1 || 424 || 27 || 10.3
|-
| [[Paraguay]] || 2.47 || 6.1 || 157 || 39 || 15.5
|-
| [[Guyana]] || 2.40 || 0.79 || 83 || 9.1 || 61
|-
| [[Guatemala]] || 2.40 || 18 || 42 || 334 || 10.6
|-
| [[Honduras]] || 2.36 || 9.6 || 43 || 220 || 7.2
|-
| [[Suriname]] || 2.35 || 0.632 || 63 || || 18.3
|-
| [[Panama]] || 2.33 || 4.3 || 29 || 145 || 42.7
|-
| [[Nicaragua]] || 2.32 || 6.4 || 50 || 132 || 7.6
|-
| [[Dominican Republic]] || 2.27 || 11.4 || 18.7 || 570 || 25.5
|-
|-bgcolor=eeeeff
| '''{{noflag}} World''' ||| '''2.27'''
|-
| [[Venezuela]] || 2.21 || 30.5 || 354 || 87 || 8
|-
| [[Peru]] || 2.19 || 33.5 || 1285 || 60 || 15.9
|-
|-
|-bgcolor=eeeeff
| '''[[Total fertility rate#Replacement rates|Population replacement]]''' || '''2.10'''
|-
| [[Ecuador]] || 2.03 || 17.4 || 109 || 179 || 13.3
|-
| [[Belize]] || 2.01 || 0.44 || 8.9 || 46 || 11.1
|-
| [[Argentina]] || 1.89 || 47.3 ||1073 || 37 || 26.5
|-
| [[Mexico]] || 1.82 || 130 || 761  || 158 || 25
|-
| [[El Salvador]] || 1.80 || 6.6 || 8.1  || 840 || 11.7
|-
| [[Colombia]] || 1.72 || 52.156 || 440 || 118 || 19.5
|-
| [[United States]] || 1.66  || 379.6 || 335 || 34 || 80
|-
| [[Brazil]] || 1.64 || 203 || 3.287 || 65 || 20
|-
| [[Chile]] || 1.54|| 18,549 || 292 || 62 || 29.9
|-
|Costa Rica]] || 1.53 || 5 || 19.7 || 85 || 27
|-
| [[Uruguay]] || 1.49 || 3.44 || 68 ||50.5 || 28.9
|-
| [[Russia]] || 1.49 || 147 ||6.6 || 22 || 35.3
|-
| [[Cuba]] || 1.44|| 11 || 48.2 || 264 || ??
|-
| [[Jamaica]] || 1.35||2734||4.2||689||13
|-

|-
|}
|}==Other==
4+3] CYCLOADDITION IN WATER. SYNTHESIS OF 2,4-endo,endo-DIMETHYL-8-OXABICYCLO[3.2.1]OCT-6-EN-3-ONE
Mark Lautens and Giliane Bouchain
Org. Synth. 2002, 79, 251
DOI: 
<ref>{{cite journal |doi=10.15227/orgsyn.078.0212 |title=&#91;4 + 3&#93; Cycloaddition of Aminoallyl Cations with 1,3-Dienes: 11-Oxatricyclo&#91;4.3.1.12,5&#93;Undec-3-En-10-One |journal=Organic Syntheses |date=2002 |volume=78 |page=212 }}</ref>
[4 + 3] CYCLOADDITION OF AMINOALLYL CATIONS WITH 1,3-DIENES: 11-OXATRICYCLO[4.3.1.12,5]UNDEC-3-EN-10-ONE
Jonghoon Oh, Chewki Ziani-Cherif, Jong-Ryoo Choi, and Jin Kun Cha,
Org. Synth. 2002, 78, 212
DOI:

==Marginal cruft==
*[[Lithium beryllide]], fiction supported by theory.
*[[Urea-formaldehyde}} belabored description of emissions.

==MG chem thing==
*Cotton and Wilkinson's Advanced Inorganic Chemistry" (6th Edition): "Part 1 Survey of Principles", "Part 2 The Chemistry of the Main Group Elements", etc
*Shriver and Atkins Inorganic Chemistry (5th Edition): MG chem not in index.  "Nonmetal" refers to p 262 showing the periodic table highlighting elements above the B-Po diagonal.
*Elschenbroich's "Organometallic Chemistry"  main sections: "Introduction" (chapters 1-3), "Main-Group Organometallics" (chapters 4-11), "Organometallic Chemistry of the Transition Metals" (chapters 12-18)

==Notes and projects==
[[Hexamethylenetetramine]]
[[Alpha hydroxy acid]], ck sources, list main examples

*[[Bicyclobutane]]
Quinolizine is a [[heterocyclic organic compound]] with the formula (C4H4)2CHNH.  A colorless solid, it is one of the isomers of dihydroquinoline, but with a [[secondary amine]] at the bridge site.  The saturated derivative of quinolizine is [[quinolizidine]].

A '''transition metal diamine complex''' is a [[coordination compound]] containing one or more [[diamine]] ligands. Such complexes played a role in the development of coordination chemistry, particularly with regards to the stereochemistry of [[chelate ring]]s.

==Diamine ligands==
The principal diamine ligand is [[ethylenediamine]] (1,2-diaminoethane, abbreviated en).  It is the premier and simplest diamine ligand, which enjoys utility outside of coordination chemistry.  Related diamines include:
* [[propylenediamine]] (1,2-diaminopropane, pn), which is notable as being chiral.
* [[trimethylenediamine]] (1,3-diaminopropane, tn), which forms 6-membered MN<sub>2</sub>C<sub>3</sub> chelate rings.
* trans-[[1,2-diaminocyclohexane]] (chxn), which is notable as being chiral but also C<sub>2</sub>-symmetric.
* [[tetramethylethylenediamine]] (tmeda), a di-tertiaryamiine that is widely used to form complexes alkali and alkaline earth metal.

==Homoleptic complexes==
===Derivatives of en, pn, tn, chxn===
Numerous homoleptic complexes are known of the type [M(diamine)<sub>3</sub>]<sup>n+</sup> M = Cr(III), Co(III), Rh(III), Rh(III), Ir(III), Ni(II), amd Pt(IV). One specific example is found in the hydrated salt [Co(chxn)<sub>3</sub>]Cl<sub>3</sub>.<ref>{{cite journal |doi=10.1107/S0567740870004387|title=The crystal structure of (−)589-tris&#91;(+)-trans-1,2-diaminocyclohexane&#93;cobalt(III) chloride pentahydrate, (−)589-&#123;Co&#91;(+)-CHXN&#93;3&#125;Cl3.5H2O |year=1970 |last1=Marumo |first1=F. |last2=Utsumi |first2=Y. |last3=Saito |first3=Y. |journal=Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry |volume=26 |issue=10 |pages=1492–1498 }}</ref> Pd(II), Pt(II), and Au(III) form homoleptic complexes of the type [M(diamin)<sub>2</sub>]<sup>n+</sup>.

==References==
<references />Über die Einwirkung von Quecksilbersalzen auf Eisenpentacarbonyl
H. Hock, H. Stuhlmann
First published: 10. Oktober 1928 https://doi.org/10.1002/cber.19280610907
Volume61, Issue9
10. Oktober 1928
Pages 2097-2101

In [[chemistry]], persulfide refers to the [[functional group]] R-S-S-H.<ref>{{cite journal |doi=10.1039/c5mb00216h|title=Persulfides: Current knowledge and challenges in chemistry and chemical biology |year=2015 |last1=Park |first1=Chung-Min |last2=Weerasinghe |first2=Laksiri |last3=Day |first3=Jacob J. |last4=Fukuto |first4=Jon M. |last5=Xian |first5=Ming |journal=Molecular Biosystems |volume=11 |issue=7 |pages=1775–1785 }}</ref>  Persulfides are intermediates in the biosynthesis of [[iron-sulfur protein]]s and are invoked a precursors to [[hydrogen sulfide]], a signalling molecule.

Compared to [[thiol]]s (R-S-H), persulfides are uncommon.  They are thermodynamically unstable with respect to loss of elemental sulfur:
:RSSH  RSH + 1/8S<sub>8</sub>
Nonetheless they are kinetically stable.

The S-H bond is both more acidic and more fragile than in thiols.  The [[bond dissociation energy]] is 22 kcal/mol weaker than a thiol.  This effect is attributed to the stability of the RSS. radical.  The pK<sub>a</sub> is 6.2 is much lower than the pK<sub>a</sub> of 7.5 for thiols.  Thus persulfides exist predominantly in the ionized form at neutral pH.

==References==

Mann, B. E.; Taylor, B. E. I3C NMR Data for Organometallic Compounds·, Academic Press: London, 1981
isbn 0124691501


==ZrBrx==
ZrBr3 density 4.45
10.1021/ic50154a056 doi

ZrBr Corbett
0.1021/ic50174a041

==References==

==Chemical compoundss==
[[File:Chlorid manganatý.JPG|thumb|left|upright=0.55|[[Manganese(II) chloride]] crystals – the pale pink color of Mn(II) salts is due to a [[Spin-forbidden reactions|spin-forbidden]] 3d transition.<ref>{{cite book|title=Shriver and Atkins' Inorganic Chemistry|date=2010|publisher=Oxford University Press|isbn=978-0-19-923617-6|chapter=Ch. 20}}</ref>]]

Manganese is renown for adopting many [[oxidation state]]s, ranging from −3 to +7. 
===Halides===
The dihalides of Mn are common reagents. 

===Oxides===
Manganese dioxide is the most important compound as it comprises the main mineral and a component of some batteries.  Alkali metal salts of manganate (MnO<sub>4</sub><sup>2-</sup>) and permanganate (MnO<sub>4</sub><sup>-</sup>) are deep green and violet. Other more esoteric oxidees are the oxyhalides (MnO<sub>3</sub>F and MnO<sub>3</sub>Cl) and the explosive molecule Mn<sub>2</sub>O<sub>7</sub>.

CAS Registry Number 7450-69-3 ~293~46 C6 H9 N2 O2 P Phosphorodiamidic acid, phenyl ester Molecular Weight 172.12 Melting Point (Experimental) Value: 185 °C 

CdTe
MoCl3 and bromide and iodide
Molybdenum(II) bromide

{{Chembox
| ImageFile = 
| ImageSize = 
| ImageAlt = 
| IUPACName = 
| OtherNames = Benzo[g]quinoline
|Section1={{Chembox Identifiers
| CASNo = 260-36-6
| PubChem = 
| SMILES = }}
|Section2={{Chembox Properties
| Formula = 
| MolarMass =
| Appearance = 
| Density = 1.329 g/cm<sup>3</sup><ref>{{cite journal |doi=10.1021/ol3003089|title=&#91;4 + 4&#93; Photodimerization of Azaanthracenes in Both Solution and Solid Phase Controlled by Cation−π Interactions |year=2012 |last1=Yamada |first1=Shinji |last2=Kawamura |first2=Chiaki |journal=Organic Letters |volume=14 |issue=6 |pages=1572–1575 }}</ref>
| MeltingPtC = 247
| BoilingPt = 
| Solubility = }}
|Section3={{Chembox Hazards
| MainHazards = 
| FlashPt = 
| AutoignitionPt = }}
}}

'''1-Azaanthracene''' is one of several isomers of benzo[[quinoline]]. A colorless solid, it is prepared by cyclization of 2-benzyl derivative of nicotinaldehyde.<ref>{{cite journal |doi=10.1002/jhet.5570360218|title=General preparative route to benzo&#91;g&#93;quinolines (1-azaanthracenes) |year=1999 |last1=Krapcho |first1=A. Paul |last2=Gilmor |first2=Timothy P. |journal=Journal of Heterocyclic Chemistry |volume=36 |issue=2 |pages=445–452 }}</ref>

'''Violanthronequinone''' is prepared by coupling of benzanthrone to 4,4-bibenzanthronyl.  The latter is oxidative ring closure to [[violanthrone]], which sustains oxidation to give the [[violanthronequinone]]. Reduction  with sodium hydrogen sulfite
give 16,17-dihydroxyviolanthrone, O-methylation of which gives the dimethoxy diol called Caledon Jade Green.<ref name=UllmannDye>{{ Ullmann | last1= Bien|first1=H.-S.| last2=Stawitz |first2=J.| last3= Wunderlich|first3=K. | title = Anthraquinone Dyes and Intermediates | doi = 10.1002/14356007.a02_355|year=2005 }}</ref>==Ln2O3==
M2O3 is a basic oxide.  Insoluble in water, this ...-colored solid absorbs atmospheric water to form the trihydroxide. It dissolve in acidic water to form aquo complex [M(H2O)n]3+.  The oxide is produced both by burning the metal or roasting the hydroxides or calcining the carbonate.  

It adopts a ... structure according to X-ray crystallography.  As such each M is seven-coordinate.

=== Inorganic esters ===
[[Image:Phosphate Group.svg|130px|thumb|A phosphoric acid ester]]
Esters can also be derived from  inorganic acids.  
*[[Phosphoric acid]] forms [[phosphate ester]]s, e.g. [[triphenylphosphate]]
*[[sulfuric acid]] forms [[organosulfate|sulfate ester]]s, e.g., [[dimethylsulfate]]
*[[nitric acid]] forms [[organic nitrate|nitrate esters]], e.g. [[methyl nitrate]]
*[[boric acid]] forms [[borate#Borate esters|borate]]s, e.g. [[trimethylborate]]. 
*[[carbonic acid]] forms [[carbonate ester]]s, e.g. [[ethylene carbonate]]
Inorganic acids that exist as tautomers form diverse esters
*orthophosphorous acid forms two kinds of [[phosphite esters]]s, e.g. [[triethylphosphite]] (P(OEt)<sub>3</sub>) and [[diethylphosphite]] (HP(O)(OEt)<sub>2</sub>).

Inorganic acids that are unstable or elusive form stable esters.
*[[chromic acid]], which has never been detected, forms [[di-tert-butyl chromate]]
*[[sulfurous acid]], which is rare, forms [[dimethylsulfite]].

== TheFreeDictionary ==
to replace ref
Propenyl 
Synthetic element 
Glycolic acid 
Hydrate 
Supermolecule 
Mercapturic acid 
Glucose-6-phosphate dehydrogenase deficiency 
Calcium hydride
Isotopes of oxygen
Germanide
Prostacyclin 
A68 protein 
CS gas 
Hugo Schiff 
Amphotericin B
Butyl nitrate
Flow cytometry
Chalcogen

==Various==
[[File:HgCo(SCN)4.jpg|thumb|sample of HgCo(SCN)4]]
{{cite journal|doi=10.15227/orgsyn.084.0209|title=Mono Carbamate Protection of Aliphatic Diamines Using Alkyl Phenyl Carbonates |journal=Organic Syntheses |year=2007 |volume=84 |page=209 }}
MONO CARBAMATE PROTECTION OF ALIPHATIC DIAMINES USING ALKYL PHENYL CARBONATES
Michael Pittelkow, Rasmus Lewinsky, and Jørn B. Christensen
Org. Synth. 2007, 84, 209
DOI: 
==?==
rac
-59 °C
Boiling Point (Experimental)
Value: 188.2 °C
Density (Experimental)
Value: 1.036 g/cm3 | Condition: Temp: 25 °C

4254-15-3 (2S)-1,2-Propanediol, 
Molecular Weight
Boiling Point (Experimental)
Value: 88.7 °C | Condition: Press: 13 Torr
Density (Experimental)
Value: 1.0364 g/cm3 | Condition: Temp: 20 °C

4254-14-2 = R enantiomer
==SES==
Joshua R. Sacher and Steven M. Weinreb "DISCUSSION ADDENDUM for: 2-Trimethylsilylethanesulfonyl Chloride (SES-Cl) Org. Synth. 2012, 89, 34-43. {{doi|10.15227/orgsyn.089.0034}}

=OM chem=

The roots of the term "organometallic", "organo-" and "metallic" are convenient starting points for defining the scope of this family of compounds.  As mentioned above, the metal can include any metallic element.  The organic ligands more diverse, but can be classified as follows:
*alkyl and aryl ligands.  
Formally viewed as anions, alkyl and aryl ligands are the quintessential organic ligands and such compounds find pervasive applications.  
The parent alkyl and aryl ligands are methyl (CH<sub>3</sub>) and phenyl (C<sub>6</sub>H<sub>5</sub>). 
Homoleptic complexes,  consisting only of such ligands, include [[hexamethyltungsten]] and [[triphenylaluminium]].  More commonly, alkyl and aryl ligands are found in mixed ligand complexes e.g., [[Petasis reagent|dicyclopentadienyltitanium dimethyl]] and [[phenylmagnesium bromide|PhMgBr(OEt<sub>2</sub>)<sub>2</sub>]].
Beyond methyl and phenyl, myriad other alkyl and aryl ligands are known<nowiki><ref name= Elschenbroich/></nowiki>

*alkene ligands.  
{{main|transition metal alkene complexes}}
Formally viewed as 2e donor ligands, alkenes form diverse complexes and are important substrates for many practical processes.  
The parent ligand is ethylene, C<sub>2</sub>H<sub>4</sub>.  Incidentally ethylene is the feedstock for the production of [[polyethylene]], which in turn is catalyzed by organometallic compounds.  Homoleptic complexes of ethylene are known, such as tris(ethylene)nickel(0).  More commonly, ethylene as a ligand is encountered in mixed ligand complexes, such as [[chlorobis(ethylene)rhodium dimer]]. 
Beyond ethylene, many alkenes exhibit affinity for metal centers.  Also common are [[diene]], [[triene]], and even tetraene ligands. Examples include [[bis(cyclooctatetraene)nickel(0)]] and [[bis(η8-cyclooctatetraenyl)uranium(IV)]].  Special subset of triene-like ligands are [[arene]]s, which most commonly bind metals via all six carbon centers.
*combinations of alkyl and alkene groups give rise to diverse families of anionic ligands including [[allyl]] (C3H5) and [[cyclopentadienyl]] (C5H5) ligands, as well as substituted derivatives.  Examples include [[allylpalladium chloride dimer]] and [[ferrocene]].
*alkyne ligands
Formally viewed as 2e or, more rarely, 4e, Lewis bases, alkynes readily form adducts with transition metals.  
The parent ligand is acetylene (C<sub>2</sub>H<sub>2</sub>). 
Homoleptic complexes,  consisting only of such ligands, includes W(C<sub>2</sub>Ph<sub>2</sub>)<sub>3</sub>.  
More commonly, alkynes are found in mixed ligand complexes e.g., Pt(PPh<sub>3</sub>)<sub>2</sub>(C<sub>2</sub>Ph<sub>2</sub>)(CO)<sub>6</sub> and the [[tetrahedrane]] Co<sub>2</sub>(C<sub>2</sub>H<sub>2</sub>)(CO)<sub>6</sub>
Beyond acetylene itself, myriad other derivatives are known, even including unstable alkynes such as dichloroacetylene<nowiki><ref name= Elschenbroich/></nowiki>

*alkylidene ligands
{{main|transition metal carbene complex}}
Formally viewed as 2e Lewis bases, a variety of alkylidenes form adducts with transition metals.  
The parent ligand is [[methylene]] (CH<sub>2</sub>), a highly reactive entity in the absence of its complexes 
Homoleptic complexes,  consisting only of alkylidene, includes derivatives of [[N-heterocyclic carbene]]s, such as Pd([[IMes]])2.  
More commonly, carbenes are found in mixed ligand complexes e.g., W(CO)<sub>5</sub>)CPh<sub>2</sub>.

*alkylidyne ligands
{{main|Transition metal carbyne complex}}
*carbido ligands
Carbon atoms are not stable in the condensed phase, but many carbides are known usually as refractory solids.  Many molecular complexes of "C" are known but in almost all cases, the carbon is a [[bridging ligand]].  Examples include Fe6C(CO)16]2-, Fe5C(CO)15, and Fe4C(CO)14.  In rare cases, complexes are known featuring a terminal carbido ligand, e.g. 
*saturated hydrocarbons
{{main|Agostic interactions}}
Saturated hydrocarbons are important ligands.  They weakly basic and most such complexes have been fully characterized only when the interaction is part of a chelating ligand.  Unlike other ligands in this list, agostic interactions are a form of [[3-center, 2-electron bonding]].


=Molecular sieve=
[[File:Molecular Sieve5.jpg|thumb|A sealed canister, commonly filled with [[silica gel]] and other molecular sieves used as [[desiccant]] in drug containers to keep contents dry. |350x350px]]
[[File:MSN vials.JPG|thumb|150px|Vials of [[mesoporous silica]]]]
A '''molecular sieve''' is a material with pores (very small holes) of uniform size. These pore diameters are of the dimensions of small molecules, thus large molecules cannot be absorbed, while smaller molecules can. Many molecular sieves are used as [[desiccant]]s. Some examples include [[activated charcoal]] and [[silica gel]].<nowiki><ref>{{cite web|url=http://chemistry.about.com/od/chemistryglossary/g/Molecular-Sieve-Definition.htm |title=Molecular Sieve Definition - Definition of Molecular Sieve - What Is a Molecular Sieve? |publisher=Chemistry.about.com |date=2013-12-18 |accessdate=2014-02-26}}</ref></nowiki>

==Porosity==
The diameter of a molecular sieve is measured in [[Angstroms|ångströms]] (Å) or [[nanometres]] (nm). According to [[International Union of Pure and Applied Chemistry|IUPAC]] notation, [[microporous material]]s have pore diameters of less than 2&nbsp;nm (20 Å) and [[Macropore|macroporous materials]] have pore diameters of greater than 50&nbsp;nm (500 Å); the [[mesoporous material|mesoporous]] category thus lies in the middle with pore diameters between 2 and 50&nbsp;nm (20–500 Å).<nowiki><ref>{{cite journal|author=J. Rouquerol |display-authors=etal |title=Recommendations for the characterization of porous solids (Technical Report)|journal=Pure & Appl. Chem|volume=66|date=1994|pages=1739–1758|url=http://www.iupac.org/publications/pac/66/8/1739/pdf/|format=free download pdf|doi=10.1351/pac199466081739|issue=8}}</ref></nowiki>  Molecular sieves are microporous.

==Materials==
===Zeolites===
[[Zeolites]] are the most common molecular sieves.  They consist of anionic aluminosilicate frameworks, where the charges are neutralized by protons and alkali metal and alkaline earth cations.  Because of the uniformity and rigidity of their frameworks, zeolitic molecular sieves "discriminate, and organize molecules with precisions that
can be less than 1 Å."<nowiki><ref>Mark E. Davis, Raul F. Lobo "Zeolite and molecular sieve synthesis" Chem. Mater., 1992, 4 (4), pp 756–768.{{DOI|10.1021/cm00022a005}}</ref></nowiki>

{|class="wikitable"
|+ Illustrative zeolitic molecular sieves and applications
! zeolite type
! pore size in angstroms
! approximate formula
! typical application
|-
| zeolite A||3.8 || Na12[(AlO2)12(SiO2)12|| desiccant for natural gas
|-
| zeolite A||4.4 || Ca5Na2[(AlO2)12(SiO2)12|| separation of alkanes
|-
| zeolite A||2.9 || K12[(AlO2)12(SiO2)12|| desiccant for ethylene
|-
| zeolite X||8.0 || Sr21Ba22[(AlO2)86(SiO2)106|| separation of xylene isomers
|}
=Hydrolysis=
{{distinguish|hydrogenolysis|hydroxylation|water splitting}}
[[Image:Hydrolysis.png|thumb|alt=Hydrolysis Reaction|300px|right|Generic mechanism for a hydrolysis reaction. (The 2-way harpoons as the yield symbol indicates an equilibrium in which hydrolysis and [[condensation reaction|condensation]] can go both ways.)]]
'''Hydrolysis''' ({{IPAc-en|h|aɪ|ˈ|d|r|ɒ|l|ᵻ|s|ɪ|s}}; {{ety|gre|hydro-|water||lysis|to unbind}}) usually means the cleavage of chemical bonds by the addition of [[Properties of water|water]]. 

Hydrolysis can be the reverse of a [[condensation reaction]] in which two molecules join together into a larger one and eject a water molecule. Thus hydrolysis adds water to break down, whereas condensation builds up by removing water.  Often, hydrolysis or saccharification is a step in the degradation of a substance

{{Chembox
| ImageFile = 
| ImageSize = 
| ImageAlt = 
| IUPACName = 
| OtherNames = 
|Section1={{Chembox Identifiers
| CASNo = 598-99-2
| PubChem = 
| SMILES = }}
|Section2={{Chembox Properties
| C=3|H=3|O=2|Cl=3 
| MolarMass =
| Appearance = colorless liquid
| Density = 1.515 g/cm<sup>3</sup>
| MeltingPtC = -17.5
| BoilingPtC = 153.8
| Solubility = }}
|Section3={{Chembox Hazards
| MainHazards = 
| FlashPt = 
| AutoignitionPt = }}
}}

Methyl trichloroacetate is the [[organic compound]] with the formula Cl<sub>3</sub>CCO<sub>2</sub>CH<sub>3</sub>.==Examples==
===Esters and amides===
Esters undergo hydrolysis  to give alcohols and carboxylic acids:

These reactions can be accelerated by acids and bases.  Enzymes called esterases catalyze this reaction.

Acid–base-catalysed hydrolyses are very common; one example is the hydrolysis of [[amide]]s or [[ester]]s. Their hydrolysis occurs when the [[nucleophile]] (a nucleus-seeking agent, e.g., water or hydroxyl ion) attacks the carbon of the [[Carbonyl|carbonyl group]] of the [[ester]] or [[amide]]. In an aqueous base, hydroxyl ions are better nucleophiles than polar molecules such as water. In acids, the carbonyl group becomes protonated, and this leads to a much easier nucleophilic attack. The products for both hydrolyses are compounds with [[carboxylic acid]] groups.

===Salts===
A common kind of hydrolysis occurs when a [[salt (chemistry)|salt]] of a [[weak acid]] or [[weak base]] (or both) is dissolved in water. [[Self-ionization of water|Water spontaneously ionizes]] into [[Hydroxide|hydroxide anions]] and [[Hydronium|hydronium cations]]. The salt also dissociates into its constituent anions and cations. For example, [[sodium acetate]] dissociates in water into [[sodium]] and [[acetate]] ions. Sodium ions react very little with the hydroxide ions whereas the acetate ions combine with hydronium ions to produce [[acetic acid]]. In this case the net result is a relative excess of hydroxide ions, yielding a [[solution|basic solution]].

[[Strong acids]] also undergo hydrolysis.  For example, dissolving [[sulfuric acid]] (H<sub>2</sub>SO<sub>4</sub>) in water is accompanied by hydrolysis to give [[hydronium]] and [[bisulfate]], the sulfuric acid's [[conjugate acid|conjugate base]]. For a more technical discussion of what occurs during such a hydrolysis, see [[Brønsted–Lowry acid–base theory]].

Perhaps the oldest commercially practiced example of ester hydrolysis is [[saponification]] (formation of soap). It is the hydrolysis of a [[triglyceride]] (fat) with an aqueous base such as [[sodium hydroxide]] (NaOH). During the process, [[glycerol]] is formed, and the [[fatty acid]]s react with the base, converting them to salts. These salts are called soaps, commonly used in households.

However, proteases do not catalyse the hydrolysis of all kinds of proteins. Their action is stereo-selective: Only proteins with a certain tertiary structure are targeted as some kind of orienting force is needed to place the amide group in the proper position for catalysis. The necessary contacts between an enzyme and its substrates (proteins) are created because the enzyme folds in such a way as to form a crevice into which the substrate fits; the crevice also contains the catalytic groups. Therefore, proteins that do not fit into the crevice will not undergo hydrolysis. This specificity preserves the integrity of other proteins such as [[hormone]]s, and therefore the biological system continues to function normally.

Upon hydrolysis, an [[amide]] converts into a [[carboxylic acid]] and an [[amine]] or [[ammonia]] (which in the presence of acid are immediately converted to ammonium salts). One of the two oxygen groups on the carboxylic acid are derived from a water molecule and the amine (or ammonia) gains the hydrogen ion. The hydrolysis of [[peptide bond|peptides]] gives [[amino acid]]s.

:[[File:Acid-CatAmideHydrolMarch.png|320 px|thumb|Mechanism for acid-catalyzed hydrolysis of an amide.]]

Many [[polyamide]] polymers such as [[nylon 6,6]] hydrolyse in the presence of strong acids. The process leads to [[depolymerization]].  For this reason nylon products fail by fracturing when exposed to small amounts of acidic water. Polyesters are also susceptible to similar [[polymer degradation]] reactions. The problem is known as [[environmental stress cracking]].

===ATP===
ATP hydrolysis is highly exothermic.  The energy released in this process supplies energy for many biological processes. 

Hydrolysis is related to [[energy metabolism]] and storage. All living cells require a continual supply of energy for two main purposes: the [[biosynthesis]] of micro and macromolecules, and the active transport of ions and molecules across cell membranes. The energy derived from the [[oxidation]] of nutrients is not used directly but, by means of a complex and long sequence of reactions, it is channelled into a special energy-storage molecule, [[adenosine triphosphate]] (ATP).  The ATP molecule contains [[pyrophosphate]] linkages (bonds formed when two phosphate units are combined together) that release energy when needed. ATP can undergo hydrolysis in two ways: the removal of terminal phosphate to form [[adenosine diphosphate]] (ADP) and inorganic phosphate, or the removal of a terminal diphosphate to yield [[adenosine monophosphate]] (AMP) and [[pyrophosphate]]. The latter usually undergoes further cleavage into its two constituent phosphates. This results in biosynthesis reactions, which usually occur in chains, that can be driven in the direction of synthesis when the phosphate bonds have undergone hydrolysis.

===Polysaccharides {{anchor|saccharification}}===
[[File:Sucrose-inkscape.svg|thumb|Sucrose. The glycoside bond is  represented by the central oxygen atom, which holds the two monosaccharide units together.]]
[[Carbohydrate]]s undergo hydrolysis. In the presence of water, they break down into its component sugars.  For example,  [[sucrose]] hydrolyzes into [[glucose]] and [[fructose]]).  This process is termed '''saccharification'''.  Enzymes that hydrolyse glycosidic bonds are called "[[glycoside hydrolase]]s" or "glycosidases".   [[Lactase]] is essential for digestive hydrolysis of [[lactose]] in milk; many adult humans do not produce lactase and [[lactose intolerance|cannot digest the lactose]] in milk (not a disorder).

Malt made from [[barley]] is used as a source of β-amylase to break down [[starch]] into the disaccharide [[maltose]], which can be used by yeast to [[brewing|produce beer]].  Other [[amylase]] enzymes may convert starch to glucose or to oligosaccharides.  [[Cellulose]] is first hydrolyzed to [[cellobiose]] by [[cellulase]] and then cellobiose is further hydrolyzed to [[glucose]] by [[beta-glucosidase]]. Animals such as cows ([[ruminants]]) are able to hydrolyze cellulose into cellobiose and then glucose because of [[Symbiosis|symbiotic]] bacteria that produce cellulases.

===Metal aqua ions===
{{Main|Metal ions in aqueous solution}}

Metal ions are [[Lewis acid]]s, and in aqueous solution they form [[metal aqua ion]]s of the general formula M(H<sub>2</sub>O)<sub>n</sub><sup>m+</sup>.<nowiki><ref>{{Cite book |author=Burgess, J. |year=1978 |title=Metal ions in solution |location=New York |publisher=Ellis Horwood}}</ref><ref>{{cite book | last = Richens | first =D. T. | title = The chemistry of aqua ions: synthesis, structure, and reactivity: a tour through the periodic table of the elements | publisher = Wiley | year = 1997 | isbn = 0-471-97058-1}}</ref></nowiki> The aqua ions undergo hydrolysis, to a greater or lesser extent. The first hydrolysis step is given generically as

: M(H<sub>2</sub>O)<sub>n</sub><sup>m+</sup> + H<sub>2</sub>O {{eqm}} M(H<sub>2</sub>O)<sub>n−1</sub>(OH)<sup>(m−1)+</sup> + H<sub>3</sub>O<sup>+</sup>

Thus the aqua [[cations]] behave as acids in terms of [[Brønsted-Lowry acid-base theory]]. This effect is easily explained by considering the [[inductive effect]] of the positively charged metal ion, which weakens the O-H bond of an attached water molecule, making the liberation of a proton relatively easy.

The [[Acid dissociation constant|dissociation constant]], pK<sub>a</sub>, for this reaction is more or less linearly related to the charge-to-size ratio of the metal ion.<nowiki><ref name="bm">Baes, C.F.; Mesmer, R.E. ''The Hydrolysis of Cations'', (1976), Wiley, New York</ref></nowiki> Ions with low charges, such as Na<sup>+</sup> are very weak acids with almost imperceptible hydrolysis. Large divalent ions such as Ca<sup>2+</sup>, Zn<sup>2+</sup>, Sn<sup>2+</sup> and Pb<sup>2+</sup> have a pK<sub>a</sub> of 6 or more and would not normally be classed as acids, but small divalent ions such as Be<sup>2+</sup> undergo extensive hydrolysis. Trivalent ions like Al<sup>3+</sup> and Fe<sup>3+</sup> are weak acids whose pK<sub>a</sub> is comparable to that of [[acetic acid]]. Solutions of salts such as BeCl<sub>2</sub> or Al(NO<sub>3</sub>)<sub>3</sub> in water are noticeably [[acidic]]; the hydrolysis can be [[le chatelier's principle|suppressed]] by adding an acid such as [[nitric acid]], making the solution more acidic.

Hydrolysis may proceed beyond the first step, often with the formation of polynuclear species via the process of [[olation]].<ref name="bm"/> Some "exotic" species such as Sn<sub>3</sub>(OH)<sub>4</sub><sup>2+</sup><nowiki><ref>{{greenwood&Earnshaw|page=384}}</ref></nowiki> are well characterized. Hydrolysis tends to proceed as [[pH]] rises leading, in many cases, to the precipitation of a hydroxide such as Al(OH)<sub>3</sub> or AlO(OH). These substances, major constituents of [[bauxite]], are known as [[laterite]]s and are formed by leaching from rocks of most of the ions other than aluminium and iron and subsequent hydrolysis of the remaining aluminium and iron.

=reminders=
https://en.wikipedia.org/wiki/Special:Contributions/Teun71
https://en.wikipedia.org/wiki/Special:Contributions/Isabelabicalho
Polyhydroxybutyrate
Methane
CAS 109-01-3 NMe piperazine
15400 refs
Piperazine, 1-methyl-
mp -6 °C
bp 138 °C
Density 0.89928 g/cm3 
505-66-8  1248 refs

5687-07-0  DACO
78-80 °C only 76 refs

6572-95-8  
DTO
bp 43-46 °C 10 Torr
4% of S(CH3CH2CH2)2S, b. 245-6°, m. -15°
Meadow, J. R.; Reid, E. E., "Ring compounds and polymers from polymethylene dihalides and dimercaptans", J. Am. Chem. Soc. 1934, 56, 2177-2180. 10.1021/ja01325a058