Arsenic compounds structure

Dechnicke K, Shihada A-F (1976) Structural and Bonding Aspects in Phosphorus Chemistry-Inorganic Derivates of Oxohalogeno Phosphoric Acids. 28 51-82 Denning RG (1992) Electronic Structure and Bonding in Actinyl Ions. 79 215-276 Dhubhghaill OMN, Sadler PJ (1991) The Structure and Reactivity of Arsenic Compounds. 

The use of biocides is spread across the whole polymer range, e.g., paints, ropes, textiles, fibres, etc. Many are copper, silver or arsenic compounds and also various heterocyclic compounds, e.g., isothiazolines (which have some structural resemblance to penicillin). 

Fendorf S, Eich MJ, Grossl P, Sparks DL (1997) Arsenate and chromate retention mechanisms on goethite. 1. Surface structure. Environ Sci Technol 31 315—320 Francesconi KA, Kuehnelt D (2002) Arsenic compounds in the environment. In Environmental chemistry of arsenic. In Frankenberger WT Jr (ed) Marcel Dekker, New York, Chapter 3, pp 51-94... 

There are no structure-activity relationships applicable to estimating acute exposure limits for arsine. The nature and rapidity of its toxicity are notably different from other inorganic arsenic compounds. 

DubhghaUI. O. M. Ni, Sadler, P. J. The Structure and Reactivity of Arsenic Compounds. Biological Activity and Drug Design. Vol. 78, pp. 129-190. 

In chemical combination, arsenic can exist in oxidation state III or V and can have a coordination number of 3, 4, 5, or 6. In marine samples, arsenic is mainly found in the V oxidation state, although, usually as a consequence of biological factors, arsenic (III) compounds can also occur and may at times be predominant. The properties and analysis of the various arsenic-containing compounds of significance in marine arsenic research are briefly discussed, and information is provided on their synthesis. For ease of reference, the arsenic compounds frequently mentioned by name (or abbreviation/acronym) are listed in Table IV together with their structure numbers. 

The most common structures of arsenic compounds are tetrahedral and pyramidal, which are similar when the sterically active lone pair is counted. Tetrahedral symmetry holds the potential for chirality and indeed many chiral organoarsenic compounds have been prepared. Arsenic may also use d orbitals for (d-d)n bonding and for hybridization with s2 and p3 orbitals, resulting in trigonal bipyramidal or octahedral structures. In the former the more electronegative substituents occupy the apical position. 

Arsenate Poisoning Arsenate is structurally and chemically similar to inorganic phosphate (P4), and many enzymes that require phosphate will also use arsenate. Organic compounds of arsenate are less stable than analogous phosphate compounds, however. For example, acyl arsenates decompose rapidly by hydrolysis ... 

Figure 2.2 Structures of common arsenic compounds. Many of the structures partially or fully deprotonate under natural conditions (see Chapters 2, 3, and 4).

Pankratov, A.N. and Uchaeva, I.M. (2000) A semiempirical quantum chemical testing of thermodynamic and molecular properties of arsenic compounds. Journal of Molecular Structure (Theochem), 498, 247-54. 

It might be thought that the vibrational analysis for PC1 F5 was redundant, since the electron diffraction data provided complete structural information. This is not quite true the two studies were in fact complementary. In the radial distribution functions obtained from electron diffraction, some of the peaks were ill-resolved their better resolution in order to obtain accurate structural parameters was assisted by the amplitudes of vibration which can be calculated by normal coordinate analysis. The vibrational study was also valuable when, in 1987, the same team tackled the structural characterisation of the analogous arsenic compounds. These presented some experimental difficulties, because they are thermally less stable than their phosphorus analogues they tend to decompose to give As(III) species, e.g. 

All attempts to prepare a spirocyclic hexacoordinate antimonate complex 168 and a tetracoordinate spirostibonium ion 167 or onium-ate combinations of these, according to structural and synthetic principles elaborated with corresponding phosphorus and arsenic compounds, met with failure138). When, for example,-... 

Reaction of Cp LnCl with LiPRR yielded [57] Cp2Ln PR3. When lithium cyclohexyl phosphide is used [Cp7YbPhC6Hn] is formed and [Cp2YbPHPh] is obtained with lithium phenylphosphide. These products are not stable in solution and decompose to yield polymeric compounds [CpYbPCgHi 1 ] and [CpYbPPh],. The compound [Cp2Lu(PPh)2Li(tmed) l/2toluene] has been characterized by X-ray analysis [100] with Lu-P distances of 2.782(1) A and 2.813(2) A. The arsenic compound analogous to the phosphorus compound has the same structure [101]. 

Uncatalyzed reactions of isocyanato- and isothiocyanatophosphanes [Eq. (41)] have been mentioned in Section III,A,2. The structure assignment of 81a has been made on the basis of analogy with the homologous arsenic compound (81b), the X-ray structure of which has been determined. 

Ni Dhubhghaill, O.M., Sadler, P.J. (1991). The structure and reactivity of arsenic compounds biological activity and drug design. In Bioinorganic Chemistry, Vol. 78, pp. 129-90. Springer, Berlin. 

DOT CLASSIFICATION 6.1 Label Poison OSHA PEL TWA 0.5 mg(As)/m3 SAFETY PROFILE Human poison by inhalation. Poison experimentally by intravenous route. Human systemic effects by inhalation changes in function or structure of salivary glands, nausea or vomiting, cough. May be irritating to skin, eyes, and mucous membranes. A vomiting type of poison gas (non-persistent). When heated to decomposition it emits very toxic fumes of As and CT. See also ARSENIC COMPOUNDS. 

The anion derived from 1,2-phenylenephosphorochloridite is one of the rare examples of a radiogenic radical anion produced by electron capture by a phosphine. In the case of arsenic compounds, AsCls" and AsFj" were produced by y-irradiation of polycrystalline trihalogenoarsines at 77 This last species exhibits hyperfine coupling with As (T// = 666MHz), two of one kind (r y = 240MHz) and one F of another kind (T// = 78MHz). These arsenic radical anions adopt an approximate planar T-shape structure with the unpaired electron located in an orbital perpendicular to the molecular plane. 

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