Hybridization and bonding schemes

Citric acid has the molecular structure (shown on right) Using Figure 12-16 as a guide, the flowing hybridization and bonding scheme is obtained for citric acid ... 

PROCEDURE FOR... Hybridization and Bonding Scheme EXAMPLE 10.6 Hybridization and Bonding Scheme Write a hybridization and bonding scheme for bromine trifluoride, BrFs. EXAMPLE 10.7 Hybridization and Bonding Scheme Write a hybridization and bonding scheme for acetaldehyde, 0 H3C—C—H... 

FOR PRACTICE 10.6 Write a hybridization and bonding schane for XeF4. FOR PRACTICE 10.7 Write a hybridization and bonding scheme for HCN. 

Use valence bond theory to write a hybridization and bonding scheme for CO2. FOR MORE PRACTICE 10.8... 

Writing Hybridization and Bonding Schemes Using Valence Bond Theory (10.7) Examples 10.6-10.8 For Practice 10.6-10.8 For More Practice 10.8 Exercises 61-66... 

Write a hybridization and bonding scheme for each molecule. 

Write a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. 

Using Experimental Data to Assist in Selecting a Hybridization and Bonding Scheme... 

Formic acid, HCOOH, is an irritating substance released by ants when they bite (formica is Latin, meaning "ant"). A structural formula with bond angles is given here. Propose a hybridization and bonding scheme consistent with this structure. 

PRACTICE EXAMPLE A Acetonitrile is an industrial solvent. Propose a hybridization and bonding scheme consistent with its structure. 

PRACTICE EXAMPLE B A reference source on molecular structures lists the following data for dinitrogen monoxide (nitrous oxide), N2O Bond lengths N—N = 113 pm N—O = 119pm bond angle = 180°. Show that the Lewis structure of N2O is a resonance hybrid of two contributing structures, and describe a plausible hybridization and bonding scheme for each. 

Write two contributing structures to the resonance hybrid for HN3, and describe a plausible hybridization and bonding scheme for each structure. 

Draw a Lewis structure for the urea molecule, CO(NH2)2, and predict its geometric shape with the VSEPR theory. Then revise your assessment of this molecule, given the fact that all the atoms lie in the same plane, and all the bond angles are 120". Propose a hybridization and bonding scheme consistent with these experimental observations. 

Draw a scheme for the hybridization and bonding in methyl cation, CH3, and methyl anion, CH3. ... 

One more hybridization scheme is important m organic chemistry It is called sp hybridization and applies when carbon is directly bonded to two atoms as m acetylene The structure of acetylene is shown m Figure 2 18 along with its bond distances and bond angles Its most prominent feature is its linear geometry... 

For most purposes, hydroearbon groups ean be eonsidered to be nonpolar. There are, however, small dipoles associated with C—H bonds and bonds between earbons of different hybridization or substitution pattern. For normal sp earbon, the earbon is found to be slightly negatively charged relative to hydrogen. The electronegativity order for hybridized carbon orbitals is sp > sp > sp. Scheme 1.1 lists the dipole moments of some hydrocarbons and some other organic molecules. 

On the basis of these values one can conclude that, with increasing bond orders, the force constants rise, suggesting that the S—O bond of sulphoxides should have more semipolar character than that of sulphones. Furthermore, molecular diffraction measurements20 and Parachors21 for sulphoxides also suggest that the S—O bond in sulphoxides should have a semipolar single-bond representation while the S—O bond in sulphones is described by double bonds or better as the resonance hybride shown in Scheme 1. 

Triatomic species can be linear, like CO2, or bent, like O3. The principles of orbital overlap do not depend on the identity of the atoms involved, so all second-row triatomic species with 16 valence electrons have the same bonding scheme as CO2 and are linear. For example, dinitrogen oxide (N2 O) has 16 valence electrons, so it has an orbital configuration identical to that of CO2. Each molecule is linear with an inner atom whose steric number is 2. As in CO2, the bonding framework of N2 O can be represented with sp hybrid orbitals. Both molecules have two perpendicular sets of three tt molecular orbitals. The resonance structures of N2 O, described... 

---