Oxygen covalent bonds

Oxyanions consist of an atom of an element plus some number of atoms of oxygen covalently bonded to it. The name of the anion is given by the name of the element with its ending changed to either -ate or -ite. In some cases, it is also necessary to add the prefix per- or hypo- to distinguish all the possible oxyanions from one another. For example, there are four oxyanions of chlorine, which are named as follows ... 

A recent study (1) has demonstrated that the electrochemical oxidation of hydroxide ion yields hydroxyl radical ( OH) and its anion (O"-). These species in turn are stabilized at glassy carbon electrodes by transition-metal ions via the formation of metal-oxygen covalent bonds (unpaired d electron with unpaired p electron of -OH and O- ). The coinage metals (Cu, Ag, and Au), which are used as oxygen activation catalysts for several industrial processes (e.g., Ag/02 for production of ethylene oxide) (2-10), have an unpaired electron (d10s1 or d9s2 valence-... 

Sodium sulfate, Na2S04 32 (1 + 1 -f 6 + 24) valence electrons. This contains sodium ions and sulfate ion. The bonds between sodium and the outside of the sulfate (that is, the oxygen) are ionic. The positive sodium atoms are represented without valence electrons, that is, with the neon structure. The sulfur-to-oxygen bonds within the sulfate ion are largely covalent. The sulfate ion must be arranged so that there are no oxygen-to-oxygen covalent bonds, otherwise the compound would have the... 

Just as for cations, there are three types of anions for naming purposes. Monatomic anions are easy to name. A second type, oxoanions, are anions that contain oxygen covalently bonded to another element. Table 6.3 presents some important... 

Nature of Chemical Bonds for Oxygen in its Compounds Table 3-4 Examples of Oxygen Covalent Bonding with Nonmetals... 

The formation of the same iron-oxygen covalent bonds from either (1) oxidized iron plus oxy anions via electron-transfer (redox) reactions or (2) radical-radical coupling reactions is summarized in Table 3-11. The valence-electron hybridization for the iron center is included as well as the spin state and estimated covalent bond-formation free energy (AGbf)- A similar set of reactions and data for iron-porphyrin compounds is presented in Table 3-12. Section a emphasizes that, just as the combination of a proton with a hydroxide ion yields a covalent H-OH bond (Table 3-11), (1) the combination of protons and porphyrin dianion (Por -) yields covalent porphine (H2Por), and (2) the addition of Lewis acids (Zn2+ or Fe2+) to porphine (H Por) oxidatively displaces protons to give covalent-bonded ZnilPor and Fe iPor. 

The picture of the ground state of the rare-earth atom in RO2 emerging from our discussion is that in each case, owing to R-oxygen covalent bonding, only a fraction c of the delocalized 4f electron remains on the R site. Its presence is detected in XAS by transitions to the 4f-admixture within the conduction continuum. The remaining fraction (1 - c) is used up in a partial ionic type of bonding and, as a result, appears as a... 

Be4(CH3C00)5 has a central oxygen covalently bonded to four beryllium atoms in the shape of a tetrahedron. The six acetate ions span the edges of the tetrahedron. 

Given the already mentioned importance that 0 H, CO, and CO2 derivatives have had as potential intermediates in the water gas shift reaction and the relevance that late transition metal complexes containing metal-oxygen covalent bonds have in... 

A recent discussion concludes that high-valent transition metal ions such as iron(IV) are thermodynamically incompatible with the strongly electronegative 0x0 dianion, particularly when electron transfer results in unpaired valence electrons that can stabilize each other via covalent bond formation. Such stabilization of the two unpaired electrons of ground-state atomic oxygen attenuate its redox potential and it reactivity to an extent proportional to the energy of the metal-oxygen covalent bond. 

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