Exact Mass: 63.9374
Exact Mass Matches: 63.9374
Found 15 metabolites which its exact mass value is equals to given mass value 63.9374,
within given mass tolerance error 0.01 dalton. Try search metabolite list with more accurate mass tolerance error
0.001 dalton.
zinc ion
A - Alimentary tract and metabolism > A16 - Other alimentary tract and metabolism products > A16A - Other alimentary tract and metabolism products > A16AB - Enzymes D000970 - Antineoplastic Agents > D059003 - Topoisomerase Inhibitors > D059004 - Topoisomerase I Inhibitors C307 - Biological Agent > C29726 - Enzyme Replacement or Supplement Agent D004791 - Enzyme Inhibitors
Zinc
Zinc, also known as zinc ion or zn2+, is a member of the class of compounds known as homogeneous transition metal compounds. Homogeneous transition metal compounds are inorganic compounds containing only metal atoms,with the largest atom being a transition metal atom. Zinc can be found in a number of food items such as sunburst squash (pattypan squash), star fruit, kelp, and common salsify, which makes zinc a potential biomarker for the consumption of these food products. Zinc can be found primarily in blood, cerebrospinal fluid (CSF), saliva, and urine, as well as in human brain, erythrocyte and liver tissues. Zinc exists in all living species, ranging from bacteria to humans. In humans, zinc is involved in several metabolic pathways, some of which include pantoprazole action pathway, pyruvate metabolism, cimetidine action pathway, and phenylbutazone action pathway. Zinc is also involved in several metabolic disorders, some of which include gamma-glutamyltransferase deficiency, 3-phosphoglycerate dehydrogenase deficiency, MNGIE (mitochondrial neurogastrointestinal encephalopathy), and cystathionine beta-synthase deficiency. Moreover, zinc is found to be associated with continuous ambulatory peritoneal dialysis, kidney disease, chronic renal failure, and hemodialysis. Zinc is a non-carcinogenic (not listed by IARC) potentially toxic compound. The element was probably named by the alchemist Paracelsus after the German word Zinke (prong, tooth). German chemist Andreas Sigismund Marggraf is credited with discovering pure metallic zinc in 1746. Work by Luigi Galvani and Alessandro Volta uncovered the electrochemical properties of zinc by 1800. Corrosion-resistant zinc plating of iron (hot-dip galvanizing) is the major application for zinc. Other applications are in electrical batteries, small non-structural castings, and alloys such as brass. A variety of zinc compounds are commonly used, such as zinc carbonate and zinc gluconate (as dietary supplements), zinc chloride (in deodorants), zinc pyrithione (anti-dandruff shampoos), zinc sulfide (in luminescent paints), and zinc methyl or zinc diethyl in the organic laboratory . Ingestion of large doses of zinc causes stomach cramps, nausea, and vomiting. Acute inhalation of large amounts of zinc causes metal fume fever, which is characterized by chills, fever, headache, weakness, dryness of the nose and throat, chest pain, and coughing. Dermal contact with zinc results in skin irritation (L49) (T3DB). Zinc is an essential element, necessary for sustaining all life. It is a trace element in the diet, forming an essential part of many enzymes, and playing an important role in protein synthesis and in cell division. Physiologically, it exists as an ion in the body. It is estimated that 3000 of the hundreds of thousands of proteins in the human body contain zinc prosthetic groups. In addition, there are over a dozen cell types in the human body that secrete zinc ions, and the roles of these secreted zinc signals in medicine and health are now being actively studied. Intriguingly, brain cells in the mammalian forebrain are one type of cell that secretes zinc, along with its other neuronal messenger substances. Cells in the salivary gland, prostate, immune system, and intestine are other types that secrete zinc. Obtaining a sufficient zinc intake during pregnancy and in young children is a problem, especially among those who cannot afford a good and varied diet. Zinc deficiency is associated with anemia, short stature, hypogonadism, impaired wound healing, and geophagia. Brain development is stunted by zinc deficiency in utero and in youth. Zinc is an activator of certain enzymes, such as carbonic anhydrase. Carbonic anhydrase is important in the transport of carbon dioxide in vertebrate blood. Even though zinc is an essential requirement for a healthy body, too much zinc can be harmful. Excessive absorption of zinc can also suppress copper and iron absorption. The free zinc ion in solution is highly toxic to plants, invertebrates, and even vertebrate fish. The Free Ion Activity Model (FIAM) is well-established in the literature and shows that just micromolar amounts of the free ion kill some organisms.
Zinc
D018977 - Micronutrients > D014131 - Trace Elements Although zinc is an essential requirement for good health, excess zinc can be harmful. Excessive absorption of zinc suppresses copper and iron absorption. The free zinc ion in solution is highly toxic to plants, invertebrates, and even vertebrate fish. The Free Ion Activity Model is well-established in the literature, and shows that just micromolar amounts of the free ion kills some organisms. A recent example showed 6 micromolar killing 93\\% of all Daphnia in water.; Binary compounds of zinc are known for most of the metalloids and all the nonmetals except the noble gases. The oxide ZnO is a white powder that is nearly insoluble in neutral aqueous solutions, but is amphoteric, dissolving in both strong basic and acidic solutions. The other chalcogenides (ZnS, ZnSe, and ZnTe) have varied applications in electronics and optics. Pnictogenides (Zn3N2, Zn3P2, Zn3As2 and Zn3Sb2), the peroxide (ZnO2), the hydride (ZnH2), and the carbide (ZnC2) are also known. Of the four halides, ZnF2 has the most ionic character, whereas the others (ZnCl2, ZnBr2, and ZnI2) have relatively low melting points and are considered to have more covalent character.; Brass, which is an alloy of copper and zinc, has been used since at least the 10th century BC. Impure zinc metal was not produced in large scale until the 13th century in India, while the metal was unknown to Europe until the end of the 16th century. Alchemists burned zinc in air to form what they called "philosophers wool" or "white snow". The element was probably named by the alchemist Paracelsus after the German word Zinke. German chemist Andreas Sigismund Marggraf is normally given credit for discovering pure metallic zinc in 1746. Work by Luigi Galvani and Alessandro Volta uncovered the electrochemical properties of zinc by 1800. Corrosion-resistant zinc plating of steel (hot-dip galvanizing) is the major application for zinc. Other applications are in batteries and alloys, such as brass. A variety of zinc compounds are commonly used, such as zinc carbonate and zinc gluconate (as dietary supplements), zinc chloride (in deodorants), zinc pyrithione (anti-dandruff shampoos), zinc sulfide (in luminescent paints), and zinc methyl or zinc diethyl in the organic laboratory.; Cadmium zinc telluride (CZT) is a semiconductive alloy that can be divided into an array of small sensing devices. These devices are similar to an integrated circuit and can detect the energy of incoming gamma ray photons. When placed behind an absorbing mask, the CZT sensor array can also be used to determine the direction of the rays. Zinc is used as the anode or fuel of the zinc-air battery/fuel cell providing the basis of the theorized zinc economy.; Groups at risk for zinc deficiency include the elderly, vegetarians, and those with renal insufficiency. The zinc chelator phytate, found in seeds and cereal bran, can contribute to zinc malabsorption in those with heavily vegetarian diets. There is a paucity of adequate zinc biomarkers, and the most widely used indicator, plasma zinc, has poor sensitivity and specificity. Diagnosing zinc deficiency is a persistent challenge.; In weak basic solutions containing Zn2+ ions, the hydroxide Zn(OH)2 forms as a white precipitate. In stronger alkaline solutions, this hydroxide is dissolved to form zincates ([Zn(OH)4]2?). The nitrate Zn(NO3)2, chlorate Zn(ClO3)2, sulfate ZnSO4, phosphate Zn3(PO4)2, molybdate ZnMoO4, cyanide Zn(CN)2, arsenite Zn(AsO2)2, arsenate Zn(AsO4)2?8H2O and the chromate ZnCrO4 (one of the few colored zinc compounds) are a few examples of other common inorganic compounds of zinc. One of the simplest examples of an organic compound of zinc is the acetate (Zn(O2CCH3)2).; Organozinc compounds are those that contain zinc?carbon covalent bonds. Diethylzinc ((C2H5)2Zn) is a reagent in synthetic chemistry. It was first reported in 1848 from the reaction of zinc and ethyl iodide, and was the first compound known to contain a metal?carbon sigma bond. Decamethyldizincocen...
Zinc cation
A - Alimentary tract and metabolism > A16 - Other alimentary tract and metabolism products > A16A - Other alimentary tract and metabolism products > A16AB - Enzymes D000970 - Antineoplastic Agents > D059003 - Topoisomerase Inhibitors > D059004 - Topoisomerase I Inhibitors C307 - Biological Agent > C29726 - Enzyme Replacement or Supplement Agent D004791 - Enzyme Inhibitors
