Monoxide density

Yurganov, L. N., E. I. Grechko, and A. V. Dzhola, Variations of Carbon Monoxide Density in the Total Atmospheric Column over Russia between 1970 and 1995 Upward Trend and Disturbances, Attributed to the Influence of Volcanic Aerosols and Forest Fires, Geophys. Res. Lett., 24, 1231-1234 (1997). 

The pronounced and R branch contours in the first and second overtone spectra of CO (Figures 6.2-1 and 6.2-2) clearly indicate appreciable rotational freedom in dense carbon monoxide. The wavenumbers of maximum absorption in the P and in the / branch, i>/>(max) and i jffmax), of the first overtone (Fig. 6.2-4) and of the second overtone (Fig. 6.2-5) at various temperatures are plotted as a function of the pure carbon monoxide density. As is to be expected, the separation between these two maxima increases with the temperature. In all experimental spectra, the solid line in both figures indicates the arithmetic mean, i> , of the maximum positions of the P and the R branch. slightly decreases with the density but is independent of the temperature. The straight line formed by Urn in Fig. 6.2-4 can be extrapolated to = 4261.9 cm, which is very close to the literature value = 4260.1 cm for the pure vibrational transition in the gas phase (Bouanich et al., 1981). Similarly, extrapolation of the second overtone data in Fig. 6.2-5... 

In the manufacture of steel, pure oxygen is blown through molten iron to remove some of the carbon impurity. If the combustion of carbon is efficient, carbon dioxide (density = 1.80 g/L) is produced. Incomplete combustion produces the poisonous gas carbon monoxide (density = 1.15 g/L) and should be avoided. If you measure a gas density of 1.77 g/L, what do you conclude ... 

Chlorine heptoxide is more stable than either chlorine monoxide or chlorine dioxide however, the CX C) detonates when heated or subjected to shock. It melts at —91.5°C, bods at 80°C, has a molecular weight of 182.914, a heat of vapori2ation of 34.7 kj/mol (8.29 kcal/mol), and, at 0°C, a vapor pressure of 3.2 kPa (23.7 mm Hg) and a density of 1.86 g/mL (14,15). The infrared spectmm is consistent with the stmcture O CIOCIO (16). Cl O decomposes to chlorine and oxygen at low (0.2—10.7 kPa (1.5—80 mm Hg)) pressures and in a temperature range of 100—120°C (17). It is soluble in ben2ene, slowly attacking the solvent with water to form perchloric acid it also reacts with iodine to form iodine pentoxide and explodes on contact with a flame or by percussion. Reaction with olefins yields the impact-sensitive alkyl perchlorates (18). 

The density of Hquid carbon monoxide at various temperatures is Hsted in Table 4 (5,7). The density of gaseous carbon monoxide (7) can be calculated direcdy from the equation of state using the compressibihty factor at the temperature and pressure of interest. 

Values of the viscosity of gaseous carbon monoxide have been reported (5,8,15,16). Vapor viscosity values and their relationship to density have been tabulated over a wide range of conditions (15). Values for Hquid carbon monoxide may be obtained (7). 

FIG. 2-8 Temperatnre-entropy diagram for carbon monoxide. Pressure P, in atmospheres density p, in grams per cubic enthalpy H, in joules per gram. (From Must and Stewart, NBS Tech. Note 202, 1963.)... 

Random ethylene-carbon monoxide copolymers have been known for many years and have properties somewhat similar to low density polyethylene. Alternating ECO copolymers were first produced long ago by Reppe of BASF in... 

The first and rate-determining step involves carbon monoxide dissociation from the initial pentacarbonyl carbene complex A to yield the coordinatively unsaturated tetracarbonyl carbene complex B (Scheme 3). The decarbonyla-tion and consequently the benzannulation reaction may be induced thermally, photochemically [2], sonochemically [3], or even under microwave-assisted conditions [4]. A detailed kinetic study by Dotz et al. proved that the initial reaction step proceeds via a reversible dissociative mechanism [5]. More recently, density functional studies on the preactivation scenario by Sola et al. tried to propose alkyne addition as the first step [6],but it was shown that this... 

Figure 2.14. The molecular orbitals of gas phase carbon monoxide, (a) Energy diagram indicating how the molecular orbitals arise from the combination of atomic orbitals of carbon (C) and oxygen (O). Conventional arrows are used to indicate the spin orientations of electrons in the occupied orbitals. Asterisks denote antibonding molecular orbitals, (b) Spatial distributions of key orbitals involved in the chemisorption of carbon monoxide. Barring indicates empty orbitals.5 (c) Electronic configurations of CO and NO in vacuum as compared to the density of states of a Pt(lll) cluster.11 Reprinted from ref. 11 with permission from Elsevier Science.

Carbon monoxide is a colorless, odorless, flammable, almost insoluble, very toxic gas that condenses to a colorless liquid at — 90°C. It is not very reactive, largely because its bond enthalpy (1074 kj-mol-1) is higher than that of any other molecule. However, it is a Lewis base, and the lone pair on the carbon atom forms covalent bonds with J-block atoms and ions. Carbon monoxide is also a Lewis acid, because its empty antibonding Tr-orbitals can accept electron density from a... 

The lobes of electron density outside the C-O vector thus offer cr-donor lone-pair character. Surprisingly, carbon monoxide does not form particularly stable complexes with BF3 or with main group metals such as potassium or magnesium. Yet transition-metal complexes with carbon monoxide are known by the thousand. In all cases, the CO ligands are bound to the metal through the carbon atom and the complexes are called carbonyls. Furthermore, the metals occur most usually in low formal oxidation states. Dewar, Chatt and Duncanson have described a bonding scheme for the metal - CO interaction that successfully accounts for the formation and properties of these transition-metal carbonyls. 

In low oxidation states, transition metals possess filled or partly filled d shells. The Dewar-Chatt-Duncanson model envisages some of that electron density in (local) d (e.g. d., d y) orbitals being donated into the empty n orbitals of the carbon monoxide ... 

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