Zinc bis(dimethyldithiocarbamate)

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Ziram
Chemical structure of Ziram
Zinc-dimethyldithiocarbamate-from-xtal-3D-balls.png
Names
IUPAC name
(μ-Dimethylcarbamodithioato-1κS,2κS′)(μ-dimethylcarbamodithioato-1κS′,2κS)bis[(dimethylcarbamodithioato-κ2S,S′)zinc]
Other names
zinc dimethyldithiocarbamate, Ziram
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.004.808 Edit this at Wikidata
UNII
Properties
C6H12N2S4Zn
Molar mass 305.80 g·mol−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Zinc dimethyldithiocarbamate is a coordination complex of zinc with dimethyldithiocarbamate. It is a pale yellow solid that is used as a fungicide, the sulfur vulcanization of rubber, and other industrial applications.[1]

Applications[]

Known as ziram in agriculture, it was introduced in the United States in 1960 as a broad-spectrum fungicide. It was used to address scab on apples and pears, leaf curl in peaches, and anthracnose and blight in tomatoes. In 1981, additional uses for ziram were approved, including the prevention of leaf blight and scab on almonds, shot-hole in apricots, brown rot and leaf spot in cherries, and scab and anthracnose in pecans. Ziram also began to be used on residential ornaments as a bird and mammal repellent.[2] As a protectant fungicide, it active on the plant’s surface where it forms a chemical barrier between the plant and a fungus. A protectant fungicide is not absorbed into the plant and must be applied prior to infection. Ziram can either be directly sprayed on to a plant’s leaf or it can be used as a soil and seed treatment. The top five crops ziram is used on are: almonds, peaches, nectarines, pears, and table and raisin grapes.[3]

Alternatively, ziram is used as an additive ingredient in industrial adhesives, caulking, and paint. It also serves as a bird and mammal repellent on outdoor ornamental items.

Chemistry[]

The compound is a prototypical zinc dithiocarbamate, a broad class of coordination complexes with the formulae Zn(R2NCS2)2, where R can be varied. Such compounds are produced by treating zinc and dithiocarbamate (R2NCS2−), as illustrated with dimethyldithiocarbamate:[4]

2 (CH3)2NCS2− + Zn2+ → Zn((CH3)2NCS2)2

Annually, approximately 1.9 million pounds of the active ziram ingredient are used. Ziram is often sold in powder or granule form.[2]

Zinc bis(diethyldithiocarbamate) complexes degrade thermally to give zinc sulfide.[5]

Structure[]

Compounds of the type Zn(S2CNR2)2 are dimeric, i.e. their proper formula is [Zn(S2CNR2)2]2. Each Zn center is in a distorted pentacoordinate site, with four Zn-S bonds of 2.3 Å length and one Zn---S interaction >2.8 Å in length. Mono-zinc derivatives are obtained by adding strong ligands (L) such as amines, which give adducts Zn(S2CNR2)2L.[6]

Structure of [Zn(S2CNEtMe)2]2.[7]

Ecological effects[]

Ziram only moderately persists in soils, as it has a field half-life of 30 days[3] In water, ziram is the most stable of all metallic dithiocarbamate fungicides, which means degradation is rather slow. If ziram reaches the bottom of a body of water, it may stay there for months.[3]

The U.S. Environmental Protection Agency has concluded that ziram poses a low toxicity risk to mammals, a moderate risk to birds, and a high risk to aquatic species. After reviewing studies that investigated the effect of ziram on aquatic organisms, the Pesticide Action Network Pesticide Database concluded that its LC50 dose (amount of pesticide that is lethal to 50% of the test organisms within the stated study time) for amphibians places it in the "highly toxic" category.

See also[]

References[]

  1. ^ Van Gysel, August B.; Musin, Willy (2000). "Methylamines". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_535.
  2. ^ Jump up to: a b "Ziram" (PDF). EPA R.E.D Facts. United States Environmental Protection Agency. Retrieved April 26, 2015.
  3. ^ Jump up to: a b c "Ziram". Extension Toxicology Network Pesticide Information Profiles. Cornell University, Oregon State University, the University of Idaho, and the University of California at Davis and the Institute for Environmental Toxicology, Michigan State University. Retrieved April 26, 2015.
  4. ^ Rüdiger Schubart (2000). "Dithiocarbamic Acid and Derivatives". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a09_001.
  5. ^ Shen, Shuling; Zhang, Yejun; Peng, Long; Xu, Bing; Du, Yaping; Deng, Manjiao; Xu, Huarui; Wang, Qiangbin (2011). "Generalized Synthesis of Metal Sulfide Nanocrystals from Single-Source Precursors: Size, Shape and Chemical Composition Control and Their Properties". CrystEngComm. 13: 4572. doi:10.1039/c0ce00982b. ISSN 1466-8033.
  6. ^ N. Sreehari, Babu Varghese, P. T. Manoharan (1990). "Crystal and molecular structure of dimeric bis[N,N-di-n-propyldithiocarbamato]zinc(II) and the study of exchange-coupled copper(II)-copper(II) pairs in its lattice". Inorg. Chem. 29: 4011–4015. doi:10.1021/ic00345a020.CS1 maint: uses authors parameter (link)
  7. ^ Mahid Motevalli, PaulO'Brien, John R.Walsh, Ian M.Watson. "Synthesis, characterization and x-ray crystal structures of asymmetric bis(dialkyldithiocarbamates) of zinc: Potential precursors for ZnS deposition". Polyhedron. doi:10.1016/0277-5387(95)00559-5.CS1 maint: multiple names: authors list (link)

External links[]

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