Physical properties of some organic solvents

Table 1.1. Physical properties of some organic solvents...

Some Physical Properties of Some Organic Solvents (Tested at 25°C Unless Otherwise Indicated) ... 

Physica.1 Properties. Physical properties of some typical diorganotin compounds are shown in Table 6. The diorganotin chlorides, bromides, and iodides are soluble in many organic solvents and, except for dimethyltin dichloride, are insoluble in water. 

Due to the physieal and ehemical differences between the numerous organic and inorganic solvents it is diffieult to organise them in a useful seheme. Here, five attempts at a elassifieation of solvents are presented, which should prove useful to the chemist. Due to broad definitions, some overlapping of these is unavoidable. As has been customary in previous reviews non-aqueous organic solvents will reeeive partieular attention [1-15, 103-108, 172, 174-177]. Extensive compilations of chemical and physical properties of non-aqueous solvents can be found in references [11-14, 104, 106, 175, 177]. 

Some physical properties of some solvents including their melting points, boiling points, dielectric constants, viscosities, dipole moments, D.N., and A.N. are summarized in Table 9.1, and the molecular structures of some organic solvenfs for organic electrolytes of lithium-ion batteries are shown in Figure 9.1. 

In general, the peilluoioepoxides have boiling points that are quite similar to those of the corresponding fluoroalkenes. They can be distinguished easily from the olefins by it spectroscopy, specifically by the lack of olefinic absorption and the presence of a characteristic band between 1440 and 1550 cm . The nmr spectra of most of the epoxides have been recorded. Litde physical property data concerning these compounds have been pubhshed (Table 1). The stmcture of HFPO by electron diffraction (13) as well as its solubility and heats of solution in some organic solvents have been measured (14,15). 

Citric acid, anhydrous, crystallizes from hot aqueous solutions as colorless translucent crystals or white crystalline powder. Its crystal form is monoclinic holohedra. Citric acid is dehquescent in moist air. Some physical properties are given in Table 1 (1 3). The solubiUty of citric acid in water and some organic solvents is given in Table 2. The pH and specific gravity of aqueous solutions of citric acid are shown in Table 3. 

Once such effects had been noted, it became necessary to interpret the observed results and to classify the solvents. The earliest attempts at this were by Stobbe, who reviewed the effects of solvents on keto-enol tautomers [4]. Since then many attempts have been used to explain solvent effects, some based on observations of chemical reactions, others on physical properties of the solvents, and yet others on spectroscopic probes. All of these have their advantages and disadvantages and no one approach can be thought of as exclusively right . This review is organized by type of measurement, and the available information is then summarized at the end. 

Physical properties of alkynes [49, p. 251] are essentially similar to those of alkanes and alkenes. These compounds are weakly polar and are insoluble in water, but they are quite soluble in organic solvents of low polarity (e.g., ether, benzene, CCl ). Chemically, alkynes are more reactive than alkanes but behave like alkenes. The triple bond appears to be less reactive than the double bond in some reagents while more reactive in others. In a chemical reaction, the triple bond is usually broken into a double bond, which may eventually split into single bonds. 

Water has physical hemical properties that are very different from those of other solvents [1] and its role in enhancing the reactivity and selectivity of some organic reactions is still a debated question. Recent experimental studies [3e, 9] and computer simulations [10] seem to indicate, at least with respect to the rate enhancement of aqueous Diels Alder reactions, that the main effects are due to the enforced hydrophobic interactions and hydrogen bond interactions. 

Some physical properties of 3-propyl-4-ethylsydnone have been determined at various temperatures <1997BCJ315>. The dielectric constant (e = 64.6 at 25°C) is high compared to many organic solvents and close to that of propylene carbonate (e = 64.9), a typical nonaqueous polar solvent. 

Table 2 summarizes some chemical and physical properties of the most frequently used organic solvents in inorganic electrochemistry. As aqueous solutions have only a limited use in inorganic electrochemistry they will not be considered herein. 

As noted in Section 4.2.1, the gas phase has proven to be a useful medium for probing the physical properties of carbanions, specifically, their basicity. In addition, the gas phase allows chemists to study organic reaction mechanisms in the absence of solvation and ion-pairing effects. This environment provides valuable data on the intrinsic, or baseline, reactivity of these systems and gives useful clues as to the roles that solvent and counterions play in the mechanisms. Although a variety of carbanion reactions have been explored in the gas phase, two will be considered here (1) Sn2 substitutions and (2) nucleophilic acyl substitutions. Both of these reactions highlight some of the characteristic features of gas-phase carbanion chemistry. 

Tab. 1.1 Physical properties of organic solvents and some inorganic solvents of electrochemical importance... 

Some selected chemical and physical properties of naphthalene are given in Table I. Naphthalene is very slightly soluble in water but is appreciably soluble in many organic solvents, e.g.. 1.2,3,4-tctrahydronaphthalene, phenols, ethers, carbon disulfide, chloroform, benzene, coal-tar naphtha, carbon tetrachloride, acetone, and decahydronaphthalene. 

Scheme 1 provides names and structure formulas of the most important organic and inorganic polar aprotic solvents used in modern electrochemistry. Table 1 summarizes some of the physical properties of several solvents appearing in... 

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