Boiling point of hydrides

FIGURE 6.8 Boiling points of hydrides of groups IVA,VA, VIA, and VIIA. 

Besides the elemental state, also volatile compounds of superheavy elements have been considered. K. Bachmann et al. [107] extrapolated the boiling points of hydrides, methyl- and ethyl compounds of elements 113 through 117. N. Trautmann et al. [108] showed, that short-lived 216Po (T1/2 = 0.15 s) was volatilized using ethyl radicals, probably as diethylpolonium. 

FIG. 15-8. Melting points and boiling points of hydrides of non-metallic elements, showing abnormally high values for hydrogen fluoride, water, and ammonia, caused by hydrogen-bond formation. 

FIGURE 10.12 Trends in the boiling points of hydrides of some main-group elements and the noble gases. 

Trends in the boiling points of hydrides reveal the special nature of intermolecular forces when H is bonded to N, O, or F. The attractive forces are much stronger than normal dipole-dipole forces, and the orientation of the bond is linear, with the hydrogen located between the two heavy atoms. Hydrogen bonds are 2 to 5 times stronger than dipole-dipole interactions. 

Figure 2.5 shows the boiling points of the hydrides in elements of Groups IV. V, VI and VII. Clearly there is an attractive force between the molecules of the hydrides of fluorine, oxygen and nitrogen... 

Heat of vaporization, 66 see also Vaporization Helium, 91 boiling point, 63 heat of vaporization, 105 interaction between atoms, 277 ionization energy, 268 molar volume, 60 on Sun, 447 source, 91 Hematite, 404 Hemin, structure of, 397 Hess s Law, 111 Heterogeneous, 70 systems and reaction rate, 126 n-Hexane properties, 341 Hibernation, 2 Hildebrand, Joel H.. 163 Holmium, properties, 412 Homogeneous, 70 systems and reaction rate, 126 Hydration, 313 Hydrazine, 46, 47, 231 Hydrides of third-row elements, 102 boiling point of. 315 Hydrocarbons, 340 unsaturated, 342... 

FIGURE 5.8 The boiling points of most of the molecular hydrides of the p-block elements show a smooth increase with molar mass in each group. However, three compounds—ammonia, water, and hydrogen fluoride are strikingly out of line. 

The anomalously high boiling points of the hydrides NH3, H20 and HF, compared with the other hydrides in groups 5, 6 and 7, are explained... 

The boiling points of four groups of hydrides. The break in the trends for NH3, H2O, and HF is due to hydrogen bonding. The dashed line shows the likely boiling point of water, if no hydrogen bonding were present. 

Chlorides of sulfonic acids can be reduced either partially to sulfinic acids, or completely to thiols. Both reductions are accomplished in high yields with lithium aluminum hydride. An inverse addition technique at a temperature of —20° is used for the preparation of sulfinic acids, while the preparation of thiols is carried out at the boiling point of ether [69S]. 

Diborane(6) and tetraborane(lO) are colorless gases at ambient temperature and pressure. Diborane has a repulsive odor. Higher boranes up to nine boron atoms are colorless hquids. Decaborane(14) is a colorless crystalline solid. Pentaborane(ll) andhexaborane(12) are unstable compounds. The densities and melting and boiling points of selected boron hydrides are shown in the following table ... 

Fio. 12-2.—The melting points and boiling points of isoelectronic sequences of hydride molecules. 

Molecules in polar liquids such as water, liquid ammonia, sulfuric acid, and chloroform are held together by dipole-dipole and hydrogen bonding interactions. For molecules of comparable size, these are stronger than London forces resulting in the familiar trends in boiling points of nonmetal hydrides. For the heavier molecules, such as H2S, H,Se, PH3, and HI, dipole effects are not particularly important (the elec-... 

Boiling Points of the Covalent Binary Hydrides of Groups 4A, 5A, 6A, and 7A... 

Table 9-1. Boiling Points of Some Simple Hydrides...

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