Big Chemical Encyclopedia

Chemical substances, components, reactions, process design ...

Articles Figures Tables About

Iodide ion radius

The small fluoride ion (radius = 1.19 A) is not easily polarized (distorted) by cations, whereas the large iodide ion (radius = 2.06 A) is. As a result, compounds containing ions show greater covalent character than those containing ions. The properties of Cl and Br ions are intermediate between those of and T. [Pg.945]

Determining the iodide ion radius in the lithium iodide (Lii) crystal... [Pg.339]

A) A three-dimensional view of the crystal.Cross section through a layer of ions. Iodide ions are assumed to be spheres in contact with one another.The distance between iodine nuclei (426 pm) is determined experimentally. One-half of this distance (213 pm) equals the iodide ion radius. [Pg.339]

Estimate a value for the radius of the iodide ion. The distance between the lithium and iodine nuclei in lithium iodide is 300 pm. [Pg.86]

Lithium iodide crystallizes in the NaCl lattice in spite of the fact that r+/r is less than 0.414. Its density is 3.49 g/cm3. Calculate from these data the ionic radius of the iodide ion. [Pg.179]

The values of AGfc calculated above are listed in Table IX and plotted against (l/rA+) in Fig. 3. The straight line is drawn with slope calculated from Eq. (75), using Ds = 78.5, D0 = 1.78, for water at 25°C. The points for iodide ion is clearly unacceptable, as already discussed, but it seems unlikely that any revision will bring AGFC(I) up from zero to the predicted value of ca. 70 kcal mole - h Clearly more data are needed before the continuum theory can be subjected to even an approximate quantitative test, but already we may forecast that the dependence of AGFC on ionic radius will be less sensitive than Eq. (75) implies. [Pg.219]

Explain the fact that the ionic radius of cesium ion is less than that of iodide ion. [Pg.257]

In the case of the iodide ion with a radius of 206 pm, the value of pad for gas phase adsorption is 3.3x10 C m, or 10.0 debyes. For adsorption from solution, the dipole moment can be estimated when the charge density due to adsorbed ions Oad is equal and opposite to the charge density on the metal Om. On the basis of equation (10.8.8), the potential drop across the inner layer under these circumstances is... [Pg.564]

The volume does not change with the nitrate ion but with an iodide ion it swells. On the other hand, volume shrinks -with chlorine, sulfate, and phosphate ions [21]. The effect of anions on the swelling behavior of gels relates to the ratio (n/vi), the valence n of the anion, and radius of the ion... [Pg.1443]

In the lithium iodide crystal, the Li-1 distance is 3.02 A. Calculate the iodide radius, assuming that the iodide ions are in contact... [Pg.578]

Several additional, more complicated structure types are known for ionic compounds. For example, according to the radius ratio, one could expect the rutile type for strontium iodide (rSr2+ /i = 0.54). In fact, the structure consists of Sr2+ ions with a coordination number of 7 and anions having two different coordination numbers, 3 and 4. [Pg.55]

The above speculation [21] may be extended to include the related quaternary ammonium compounds such as xylocholine (XXXIX). It is probable that the volumes of the guanidinium ion and the trimethylammonium group are similar. The ionic radius of the guanidinium ion (IX) is about 3A the ionic radius of the tetramethylammonium ion has been estimated [300] to be 3-4A, although rather smaller values have also been proposed [301-303]. Crystallographic analyses of muscarine iodide [304], choline chloride [305] and acetylcholine bromide [306] have revealed that the carbon to nitrogen distance is about l-SA, and that a hydrogen bond (C-H-0 distance 2-87-3 07A) exists in the crystals of these compounds. [Pg.173]

Thirdly, there is the purely structural argument from Relative Size if ions of one type are much the largest, they will effectively fix the structure since the others can pack between them. This argument, which makes no assumption whatever about electron-clouds, is often referred only to lithium iodide, but much more evidence is available. Such questions of crystal-form and isomorphism are in fact the most important applications of ionic-radius systems in chemistry and mineralogy (cp. the classical work of V. M. Goldschmidt (2)). [Pg.62]


See other pages where Iodide ion radius is mentioned: [Pg.150]    [Pg.150]    [Pg.265]    [Pg.168]    [Pg.110]    [Pg.96]    [Pg.224]    [Pg.314]    [Pg.55]    [Pg.84]    [Pg.19]    [Pg.228]    [Pg.314]    [Pg.57]    [Pg.1170]    [Pg.215]    [Pg.20]    [Pg.1858]    [Pg.84]    [Pg.30]    [Pg.51]    [Pg.26]    [Pg.100]    [Pg.255]    [Pg.265]    [Pg.25]    [Pg.280]    [Pg.795]    [Pg.45]    [Pg.330]    [Pg.558]    [Pg.109]   
See also in sourсe #XX -- [ Pg.339 ]




SEARCH



Iodid-Ion

Iodide ions

Ion radius

© 2024 chempedia.info