What is orbital hybridization

The word hybridization means mixing and when used in the context of atomic orbitals, it describes a way of deriving spatially directed orbitals which may be used within VB theory. Like aU bonding theories, orbital hybridization is a model, and should not be taken to be a real phenomenon. 

Hybrid orbitals may be formed by mixing the characters of atomic orbitals that are close in energy. The character of a hybrid orbital depends on the atomic orbitals involved and their percentage contributions. The labels given to hybrid orbitals reflect the contributing atomic orbitals, e.g. an sp hybrid possesses equal amounts of s and p orbital character. 

Hybrid orbitals are generated by mixing the characters of atomic orbitals. 

A polyatomic species contains three or more atoms. 

A set of hybrid orbitals provides a bonding picture for a molecule in terms of localized cr-bonds. 

The notation sp means that one s atomic orbital and one p atomic orbital mix to form a set of two hybrid orbitals with different directional properties. 

One possible combination of a 2s atomic orbital and 2px atomic orbital is shown in Fig. 5.2a. In the figure, the colour of the orbital lobe corresponds to a particular phase (see Section 1.6) and the addition of the 2s component reinforces one lobe of the Ip atomic orbital but diminishes the other. Equation 5.1 represents the combination mathematically. The wavefunction ipspbyhnA describes a normalized (see Section 2.2) sp hybrid orbital which possesses 50% s and 50% p character. Although eq. 5.1 and Fig. 5.2a refer to the combination of 2s and 2px atomic orbitals, this could just as well be 2s with 2py or 2p, or 3 with Px, and so on. 

Equations 5.1 and 5.2 represent two wavefunctions which are equivalent in every respect except for their directionalities with respect to the x axis. Although the orbital energies of the initial 2s and 2px atomic orbitals were different, mixing leads to two hybrid orbitals of equal energy. 

---

The orientation of bonds on a central atom of a molecule that has no lone pairs can be any of those listed below. What is the hybridization of the orbitals used by each central atom for its bonding pairs (a) tetrahedral (b) trigonal bipyramidal ... 

The composition of hybrids can be discussed quantitatively. The outcome is that, if two equivalent hybrids composed of an s-orbital and two p-orbitals make an angle B to each other, then the hybrids can be regarded as sp with X = —cos fl/cos2 (20). What is the hybridization of the two O—H bonds in H20 ... 

Exercise 1.8. What is the hybridization of the carbon orbitals which form the C—H and C—C bonds of cyclopropane (HCH = 114°) Verify that if the carbon hybrids which are used for the C—H bonds are exactly sp2, then the two equivalent hybrids for the C—C bonds must be sp5 and the interorbital angle is 101.5° ... 

What is the hybridization at the N and each C in this molecule Indicate the type of bond and the orbitals that are overlapping to form it for each of the designated bonds (for example, aCsp3 + Hli),... 

Consider H2C=C=CH2. What is the hybridization and geometry at each C Indicate the bond types for each of the carbon—carbon bonds. Draw the molecule, showing the overall geometry and the p orbitals that overlap to form the pi bonds. (The molecule is not planar.) Is it conjugated ... 

What is the hybridization at each nitrogen of the amino acid histidine What kind of orbital is occupied by the unshared pair of electrons on each nitrogen Explain. 

Problem 1.4. What is the hybridization of the O atom in furan In what kind of orbitals do the lone pairs reside How many lone pairs are used in resonance ... 

Write the Lewis formulas and predict the hybrid orbitals and the shapes of these polyatomic ions and covalent molecules (a) HgCl2 (b) BF3 (c) Bp4 (d) SbCl5 (e) SbFg". (a) What is the hybridization of each C in these molecules (i) H2C=0 (ii) HC=N (iii) CH3CH2CH3 (iv) ketene, H2C=C=0. (b) Describe the shape of each molecule. The following fluorides of xenon have been well charac-... 

What is the hybridization of atomic orbitals Why is it impossible for an isolated atom to exist in the hybridized state ... 

When two atoms are bonded by a triple bond, what is the hybridization of the orbitals that make up the tr-bond component of the bond ... 

The lactic acid molecule, CH3CH(OH)COOH, gives sour milk its unpleasant, sour taste, (a) Draw the Lewis structure for the molecule, assuming that carbon always forms four bonds in its stable compounds, (b) How many tt and how many cr bonds are in the molecule (c) Which CO bond is shortest in the molecule (d) What is the hybridization of atomic orbitals around the carbon atom associated with that short hond (e) What are the approximate bond angles around each carbon atom in the molecule ... 

Recall the shorthand notation used for benzene.) (a) What is the hybridization at the N atom in each of the substances (b) How many unhybridized atomic orbitals are there on the N and the C atoms in each of the substances (c) Predict the N — N — C angles in each of the substances, (d) Azobenzene is said to have greater delocalization of its Tr electrons than hy-drazobenzene. Discuss this statement in light of your answers to (a) and (b). (e) All the atoms of azobenzene lie in one plane, whereas those of hydrazobenzene do not. Is this observation consistent with the statement in part (d) (f) Azobenzene is an intense red-orange color, whereas hydrazobenzene is nearly colorless. Which molecule would be a better one to use in a solar energy conversion device (See the Chemistry Put to Work box for more information about solar cells.)... 

A. What is the hybridization state of the circled nitrogens What kind of orbital contains the lone pairs identified in these circles ... 

What is the hybridization of the highlighted atoms in the following structures What are your estimates for the bond angles around these highlighted atoms In each case, in what kind of orbital does the lone pair of electrons on the nitrogen reside ... 

Specify which hybrid orbitals are used by carbon atoms in these species (a) CO, (b) CO2, (c) CN. What is the hybridization state of the central N atom in the azide ion, N3 (Arrangement of atoms NNN.)... 

PROBLEM 11.61 The Alkane halogenation reaction is also a radical process. Select this reaction and watch it several times. What is the hybridization of the central carbon of the intermediate Select the SOMO (singly occupied molecular orbital) track. Why has the calculation come up with this hybridization Is the hybridization fixed or does it change ... 

---