Hybridization sp orbitals

Fig. 4-3.—Square of bond strength (dashed curves) and calculated bond-energy values (full curves) for hybrid sp orbitals varying from pure p orbitals (a 0, left) to pure s orbitals (a = 10, right). The upper pair of curves are for L orbitals (2 and 2p), and the lower, with shifted vertical scale, for M orbitals (3s and 3p).

The initial interaction of the excited mercury atom with the alkane molecule presumably takes the form of a slight overlap of the p-orbital of the 3Pi atom with the C-H sigma bond of the alkane molecule. In the formation of the cyclic intermediate (TS-2), the two hybrid sp-orbitals of mercury are very likely simultaneously involved through... 

Hybrid com seed comes from corn plants that have particular properties worth preserving. One plant may produce sweet kernels another may produce long ears. Cross-breeding of the two plants will produce seeds that grow sweet-kernel, long-eared corn. A better ear of corn is produced. When group IIA, IIIA, and IVA families bond, the s and p orbitals combine to form hybrid sp orbitals, where bonding occurs. The sp orbitals replace the individual s and p orbitals to provide more stable locations for the bonds and a more stable molecule. A better molecule is formed. 

Bundle (548) has pointed out that resonating, hybrid sp orbitals arc probably active in bonding in interstitial carbides and nitrides. 

If one carbon 2s orbital combines with one carbon 2p orbital, two hybrid sp orbitals are formed, and two p orbitals are unchanged. 

The direction of a chemical bond directly determines the structure of covalent compounds. For example, in diamond (its electron configuration being ls 2s 2p ), four hybrid sp orbitals are formed due to the destruction of a spin bond at s levels and the excitation of three electrons at p levels, they are directed from the centre to the vertices of regular tetrahedron. The angle between the axes of orbitals is equal to 109°28. ... 

Figure 1.5. Atomic orbitals hybrid sp orbitals, (a) Cross-section and approximate shape of a single orbital. Strongly directed along one axis. (d) Representation as a sphere, with small back lobe omitted, (c) Two orbitals, with axes lying along a straight line.

Figure 8-7 Diagram of the two linear hybridized sp orbitals (green) of an atom. These lie in a straight line, and the two unhybridized p orbitals p (tan, cross-hatched) and p, (tan, hatched) lie in the perpendicular plane and are perpendicular to each other.

Figure 8-8 The acetylene molecule, C2H2. (a) The overlap diagram of two rp-hybridized carbon atoms and two r orbitals from two hydrogen atoms. The hybridized sp orbitals on each C are shown in green and the unhybridized p orbitals are shown in tan. The dashed lines, each connecting two lobes, indicate the side-by-side overlap of the four unhybridized p orbitals to form two tr bonds. There are two C—H cr bonds, one C—C cr bond (green, hatched), and two C—C it bonds (hatched and cross-hatched). This makes the net carbon-carbon bond a triple bond, (b) The tr bonding orbitals tan) are positioned with one above and below the Une of the cr bonds (green) and the other behind and in front of the line of the cr bonds.

Sigma bonds between p orbitals and hybridized sp orbitals... 

The correct answer is (D). According to electron configuration of carbon, the carbon atom shouldhave two electrons in the 2s orbital and one in each of the two 2p orbitals. The four carbon-hydrogen bonds in methane should be different because of the different orbitals, yet experimental evidence shows them to be the same. The solution is that one of the 2s electrons is raised to ap orbital, and the result is the fonnation of four identical hybridized sp orbitals. 

Figure 2.11 Cartoons of contours of i/r for the equivalent representations of oxygen lone pairs in an ether as in two sp orbitals or one p and one sp orbital and an electron density contour. Note that hybrid sp orbitals do not have a node at the nucleus, as a pure p orbital does, but rather one behind the nucleus, between it and the small lobe.

Hybridization to four 2sp3 orbitals occurs before bonding to four atoms. Three hybrid sp2 orbitals form if there is a double bond so the C atom is bonded to three atoms and one electron remains in the p orbital. Two hybrid sp orbitals occur if there is a triple bond or two double bonds. In this case, C is bonded to two atoms with two electrons remaining in p orbitals. 

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