Atomic orbitals mixing

The formation of the BeF2 molecule can be explained by assuming that, as two fluorine atoms approach Be, the atomic orbitals of the beryllium atom undergo a significant change. Specifically, the 2s orbital is mixed or hybridized with a 2p orbital to form two new sp hybrid orbitals. (Figure 7.12). 

Table 3.2 summarizes the relation between electron arrangement and hybridization type. No matter how many atomic orbitals we mix together, the number of hybrid orbitals is always the same as the number of atomic orbitals with which we started ... 

Atoms in the second row (such as C, N, O, and F) have one s orbital and three p orbitals in the valence shell. These orbitals are usually mixed together to give us hybridized orbitals (sp, sp, and sp). We get these orbitals by mixing the properties of i and p orbitals. What do we mean by mixing ... 

In some atoms, the p and s orbitals are mixed together to form several equivalent, hybridized orbitals. The most common example is carbon, where there are four orbitals that are formed by mixing one s orbital with three p orbitals to give four equivalent orbitals designated as sp3 orbitals. 

The carbon atom (6C) has the electron configuration of ls22s22p2. There are 4 valence electrons, of which only two are unpaired in the ground state. During the formation of carbon compounds, one 2s and three 2p orbitals combine to give four identical sp3 orbitals by the promotion of an electron from the 2s orbital to a 2p orbital. These 4 unpaired orbitals then mix to form four identical sp3 hybrid orbitals. 

Hybridisation is the process of mixing atomic orbitals within an atom to generate a set of new atomic orbitals called hybrid orbitals. In the case of a carbon atom, the one 2s orbital can mix with the three 2p orbitals to form four hybrid orbitals known as sp hybrid orbitals. 

State the number and type of atomic orbitals that mix to form the set of sp d hybrid orbitals. 

Although Taube s pyrazine Ru"—Ru dimer was produced by the Ag oxidation of [(NHjljRu—NC4H4N—Ru(NH3)5] , attempts to prepare similar Ru"-Ru " complexes from [(NH3)5Ru(C5H4N)2Ru(NH3)5]" and [(NHjljRu—NC5H4C2H4C5H4N—Ru(NH3)5]" were unsuccessful. Cyclic voltammetric data indicated a two-electron oxidation to Ru" -Ru " dimers. In view of the identical ligands around each Ru atom, Mayoh and Day have questioned the localization of the Ru valencies in Taube s dimer into discrete Ru" and Ru " centres. However, a theoretical calculation of the conditions necessary for valence trapping in any mixed valence system, showed that the condition is indeed satisfied by the above Ru compound. Other workers have suggested that the available data on this complex could also be explained by a molecular orbital scheme in which the Ru ion and pyrazine-filled n (or k ) molecular orbitals are mixed, and the unpaired electron is mainly but un-symmetrically shared by the two cations. ... 

When two N atoms form a molecule we have the possibility that there could be three bonds, one from the two Pa orbitals, and two from the four pj orbitals. Some mixing of the 2s with the p orbitals might lead to hybridization. No other possibilities seem likely. We show the principal configurations in the HLSP function and standard tableaux function cases in Tables 11.15 and 11.16, respectively. We see that the same orbitals are present in both main structures. The situation with... 

The trick is to make two equivalent orbitals in Be out of the atomic orbitals so that each hydrogen will see essentially the same electronic environment. We can accomplish this by mixing the 2s orbital and one of the empty 2p orbitals (say, the 2p ) to form two equivalent orbitals we call sp" hybrids, since they have both s and p characteristics. As with molecular orbital theory, we have to end up with the same number of orbitals we started with. The bonding lobes on the new spa and spb orbitals on Be are 180° apart, just as we need to form BeH2. In this manner, we can mix any type of orbitals we wish to come up with specific bond angles and numbers of equivalent orbitals. The most common combinations are sp, sp, and sp hybrids. In sp hybrids, one and one p orbital are mixed to get two sp orbitals, both of which... 

In pyridine the energetically high-lying 2s and 2px AO s of the N atom mix to form the n MO. In X -phosphorin a similar situation arises if one mixes the high-lying 3s and 3px orbitals of phosphorus. Since the s orbital component is greater... 

Fig. 11 0 Competition by ligands for Ihe ir bonding d orbilul of a central metal atom. Relative overtop is symbolized by the shaded areas, (a) Equal aod strong tr bonds resulting from equal and good overlap of Ihe two carbon monoxide sr orbitals with the meial J orbital (b) Superior overlap of carbon monoxide t orbital wilh polarized metal d orbiial compared lo poorer overlap between ligand <1 and metal d orbitals. Polarization (mixing of higher energy wave functions) occurs so as to maximize total overlap Recall that the overlap integral includes both spatial and intensive properties Ihe represemation above is a graphic simplification.

We use different hybridization schemes to describe different arrangements of electron pairs. For example, to explain a trigonal planar electron arrangement, we mix one s-orbital with two p-orbitals and so produce three sp2 hybrid orbitals. They point toward the corners of an equilateral triangle (Fig. 3.19a). A linear arrangement of pairs requires two hybrid orbitals, so we mix an s-orbital with a p-orbital to obtain two sp hybrid orbitals (Fig. 3.19b). Table 3.2 summarizes the relationship between electron arrangement and hybridization type. No matter how many atomic orbitals we mix together, the number of hybrid orbitals is always the same as the number of atomic orbitals we started with, so N atomic orbitals produce N hybrid orbitals. 

Another type of orbital is one that originates from the mixing of the different atomic orbitals and is called a hybrid orbital. Hybridization (mixing) of atomic orbitals results in a new set of orbitals with different... 

The valence bond model constructs hybrid orbitals which contain various fractions of the character of the pure component orbitals. These hybrid orbitals are constructed such that they possess the correct spatial characteristics for the formation of bonds. The bonding is treated in terms of localised two-electron two-centre interactions between atoms. As applied to first-row transition metals, the valence bond approach considers that the 45, 4p and 3d orbitals are all available for bonding. To obtain an octahedral complex, two 3d, the 45 and the three 4p metal orbitals are mixed to give six spatially-equivalent directed cfisp3 hybrid orbitals, which are oriented with electron density along the principal Cartesian axes (Fig. 1-9). 

Fig. 4.5 Hybridization is forming new atomic orbitals, on an atom, by mathematically mixing (combining) original atomic orbitals on that atom. Mixing two orbitals gives two hybrid orbitals, and in general n AOs give n hybrid AOs. Orbitals are mathematical functions and so can be added and subtracted as shown in the figure...

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