Big Chemical Encyclopedia

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

Articles Figures Tables About

Equivalent hybrid orbitals

Two hybrid AOs, sp and sp, will have the same shape if the/i to mixing ratios are equal. Is it possible to combine the 2s and 2p orbitals on Li in such a way that we obtain two hybrid orbitals that are both orthogonal and have the same shape  [Pg.128]

This means that if we want to form two equivalent hybrids, the mixing ratios of both must be equal to unity, and the hybrids are [Pg.128]

Our results for the hybridization of one 5-orbital with one p-orbital may be generalized [Pg.128]

We now go on to calculate the electron density created by one electron in each of the two sp hybrid orbitals formed by combination of a 2s and a 2pz orbital  [Pg.128]


Ethylene is planar with bond angles close to 120° (Figure 2 15) therefore some hybridization state other than sp is required The hybridization scheme is determined by the number of atoms to which carbon is directly attached In sp hybridization four atoms are attached to carbon by ct bonds and so four equivalent sp hybrid orbitals are required In ethylene three atoms are attached to each carbon so three equivalent hybrid orbitals... [Pg.89]

We saw in Chapter 1 that the carbon-carbon double bond can be described in two ways. In valence bond language (Section 1.8), the carbons are sp2-hybridized and have three equivalent hybrid orbitals that lie in a plane at angles of 120° to one another. The carbons form a cr bond by head-on overlap of sp2 orbitals and a tt bond by sideways overlap of unhybridized p orbitals oriented... [Pg.178]

In this case, there are three equivalent hybrid orbitals, each called sp (trigonal hybridization). This method of designating hybrid orbitals is perhaps unfortunate since nonhybrid orbitals are designated by single letters, but it must be kept in mind that each of the three orbitals is called sp. These orbitals are shown in Figure 1.4. The three axes are all in one plane and point to the comers of an equilateral triangle. This accords with the known structure of boron trifluoride (BF3), a planar molecule with angles of 120°. [Pg.7]

We now have two normalized, equivalent hybrid orbitals, one directed along the z axis and the other making an angle of a with the first. However, these orbitals are not necessarily orthogonal to each other for arbitrary a. The allowed hybrid angles a are those for which the overlap integral (hi h2) vanishes... [Pg.375]

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. [Pg.76]

In order for VSEPR theory to make sense, it must be combined with another idea hybridization. Hybridization refers to the mixing of atomic orbitals into new, hybrid orbitals of equal energy. Electron pairs occupy equivalent hybrid orbitals. It s important to realize that the hybrid orbitals cire all equivalent, because that helps you understand the shapes that emerge from the electron pairs trying to distance themselves from one another. If electrons in a pure p orbital are trying to distance themselves from electrons in another p orbital and from electrons in an s orbital, the resulting shape may not be symmetrical, because s orbitals cire different from p orbitals. But if all these electrons occupy identical hybrid orbitals (each orbital is a little bit s and a little bit p), then the resulting shape is more likely to be symmetrical. [Pg.75]

Figure 8.9 (a) Orientation of ABj molecule in Cartesian coordinate system. (b) Set of equivalent hybrid orbitals, 4> 2, (c) Set of equivalent a orbitals on pendent... [Pg.224]

Most hybridizations result in equivalent hybrid orbitals, i.e., all the hybrid orbitals are identical in composition (% s and % p character) and in spatial orientation with respect to each other. They have very high symmetries, culminating in tetrahedral and octahedral symmetry. In the case of dsp hybrid orbitals, the resulting... [Pg.122]

Mathematically, the formation of sp3 or tetrahedral orbitals for methane is more complicated but not basically different. The results are four equivalent hybrid orbitals, each containing one part s to three parts p in each wave function, directed to the corners of a tetrahedron. As in the case of sp hybrids, the hybridization of s and p has... [Pg.623]

SOLUTION According to Example 3.3, SF4 has a trigonal bipyramidal arrangement of electron pairs. We can construct five equivalent hybrid orbitals by mixing an s-orbital with three p-orbitals and one d-orbital. The result is five sp3d orbitals. [Pg.265]

Pauling showed that the quantum mechanical wave functions for s and p atomic orbitals derived from the Schrodinger wave equation (Section 5.7) can be mathematically combined to form a new set of equivalent wave functions called hybrid atomic orbitals. When one s orbital combines with three p orbitals, as occurs in an excited-state carbon atom, four equivalent hybrid orbitals, called sp3 hybrids, result. (The superscript 3 in the name sp3 tells how many p atomic orbitals are combined to construct the hybrid orbitals, not how many electrons occupy each orbital.)... [Pg.272]

Recalling from Section 3.4.1, we use the s orbital and the pz orbital to form two equivalent hybrid orbitals, one pointing in the +z direction and the other in the —z direction. These two orbitals are called sp hybrids, since they are formed by one s and one p orbital. The wavefunctions of the sp hybrid orbitals are given by eqs. (3.4.6) and (3.4.7). In matrix form the wavefunction are... [Pg.104]

As is well known, if we construct four equivalent hybrid orbitals using one s and three p atomic orbitals, the hybrids would point toward the four comers of a tetrahedron. However, is this the only way to construct four such hybrids If not, what other atomic orbitals can be used to form such hybrid orbitals To answer these questions, we need to determine the representations spanned by the four hybrid orbitals that point toward the corners of a tetrahedron ... [Pg.232]

We can now go on to apply the same ideas to some other simple molecules. In boron trifluoride, for example, we start with the boron atom, which has three outer-shell electrons in its normal or ground state, and three fluorine atoms, each with seven outer electrons. As shown in the upper diagram, one of the three boron electrons is unpaired in the ground state. In order to explain the trivalent bonding of boron, we postulate that the atomic s- and p orbitals in the outer shell of boron mix to form three equivalent hybrid orbitals. These particular orbitals are called sp2 hybrids, meaning that this set of orbitals is derived from one s-orbital and two p-orbitals of the free atom. [Pg.41]

Carlin uses hybrid orbitals to form bonds in. organic molocuios. When forming only single bonds with tetrahedral geometry, carbon has four e< uiv-alent p hybrid orbitals. Vtlien forming a double bond with planar geometry. carbon has three equivalent hybrid orbitals and one unhybndized... [Pg.47]

But the outer s and p orbitals in carbon form four equivalent hybridized orbitals sp ), as shown in Figure 3.24. In this arrangement, there are now four unpaired electrons that can bond with other atoms. This leads to carbon being a special atom that can form all kinds of long chain molecules. You might also notice that with this hybridization, the valence electrons in carbon are as far from one another as possible. With the electrons as far away as possible from one another, this is clearly a lower energy situation than the one shown in Figure 3.23. [Pg.59]

Quantum mechanics gives a more detailed picture of ethylene and the carbon-carbon double bond. To form bonds with three other atoms, carbon makes use of three equivalent hybrid orbitals orbitals, formed by the mixing of one s and... [Pg.144]

Hybridization explains the observed shapes of molecules by the presence of equivalent hybrid orbitals. [Pg.271]

Even though the valence would be correct after promotion, the structure still would be wrong. Beryllium hydride would have two different kinds of bonds, and methane would have three identical bonds formed by overlap of H(ls) with the C(2p) orbitals and a different bond formed by H(ls) and C(2s). Pauling proposed that new orbitals with the proper symmetry for bond formation could be formed by hybridization of 2s and 2p orbitals after promotion. The Be(2s) and Be(2pz) orbitals would combine to form two equivalent hybrid orbitals oriented 180° apart. The C(2s) would hybridize with the three C 2p) orbitals to give four equivalent new orbitals in a tetrahedral arrangement around the carbon atom. [Pg.256]

There is a close relationship between the VSEPR theory discussed in Section 3.9 and the hybrid orbital approach, with steric numbers of 2, 3, and 4 corresponding to sp, sp, and sp hybridization, respectively. The method can be extended to more complex structures (fsp hybridization (see Sec. 8.7), which gives six equivalent hybrid orbitals pointing toward the vertices of a regular octahedron, is applicable to molecules with steric number 6. Both theories are based on minimizing the energy by reducing electron-electron repulsion. [Pg.260]

For these two orbitals on Be to become equivalent, they must hybridize to give two orbitals intermediate between the r and p orbitals. These are called sp hybrid orbitals. Consistent with Hund s Rule, each of these equivalent hybrid orbitals on Be would contain one electron. [Pg.315]

To explain bonding in methane, VB theory uses hypothetical hybrid orbitals, which are atomic orbitals obtained when two or more nonequivalent orbitals of the same atom combine in preparation for covalent bond formation. Hybridization is the term applied to the mixing of atomic orbitals in an atom (usually a central atom) to generate a set of hybrid orbitals. We can generate four equivalent hybrid orbitals for carbon by mixing the 2s orbital and the three 2p orbitals ... [Pg.385]

Carbon has the electronic configuration 1 s22s22p2 with two unpaired electrons, and yet we know that carbon in its compounds almost invariably forms four bonds. The proposed solution to this was to reorganize the 2s and the three 2p orbitals to form four equivalent hybrid orbitals. If this is done, four identical orbitals directed towards the corners of a tetrahedron are produced. The formation of just one of these orbitals from a 2s and three 2p orbitals is shown in Figure 3.22. With one... [Pg.34]


See other pages where Equivalent hybrid orbitals is mentioned: [Pg.207]    [Pg.4]    [Pg.4]    [Pg.198]    [Pg.27]    [Pg.15]    [Pg.15]    [Pg.164]    [Pg.27]    [Pg.158]    [Pg.99]    [Pg.198]    [Pg.878]    [Pg.15]    [Pg.7]    [Pg.220]   


SEARCH



Equivalent orbitals

Hybrid orbital

Hybrid orbitals Hybridization

Orbital equivalent

Orbital hybridization

Orbitals hybrid

Orbitals hybridization

Orbitals, hybridized

© 2024 chempedia.info