Resonance structures minor contributors

These structures are not equal in estimated energy. The first structure has the positive charge on nitrogen. The second has the positive charge on carbon, and the carbon atom does not have an octet. The first structure is more stable because it has an additional bond and all the atoms have octets. Many stable ions have a positive charge on a nitrogen atom with four bonds (see the Summary Table, page 13). We call the more stable resonance form the major contributor, and the less stable form is the minor contributor. The structure of the actual compound resembles the major contributor more than it does the minor contributor. 

As noted in Figure 3.16, acetic acid has only a small amount of resonance stabilization because the lower structure is only a minor contributor to the resonance hybrid. Acetate ion has a large amount of resonance stabilization because it has two equivalent contributors to the hybrid. 

A molecule or ion for which two or more valid Lewis structures can be drawn, differing only in the placement of the valence electrons. These Lewis structures are called resonance forms or resonance structures. Individual resonance forms do not exist, but we can estimate their relative energies. The more important (lower-energy) structures are called major contributors, and the less important (higher-energy) structures are called minor contributors. When a charge is spread over two or more atoms by resonance, it is said to be delocalized and the molecule is said to be resonance stabilized, (pp. 14-18)... 

In the following sets of resonance forms, label the major and minor contributors and state which structures would be of equal energy. Add any missing resonance forms. 

For each of the following compounds, draw the important resonance forms. Indicate which structures are major and minor contributors or whether they would have the same energy. 

The last resonance structure is a minor contributor because its carbon lacks a complete electron octet. 

When two resonance structures are different, the hybrid looks more like the better resonance structure. The better resonance structure is called the major contributor to the hybrid, and all others are minor contributors. The hybrid is the weighted average of the contributing resonance structures. What makes one resonance structure better than another There are many factors, but for now, we will learn just two. 

Problem 1.15 Label the resonance structures in each pair as major, minor, or equal contributors to the hybrid. Then draw the hybrid. 

Although the resonance hybrid is some combination of all of its valid resonance structures, the hybrid more closely resembles the most stable resonance structure. Recall from Section 1.5C that the most stable resonance structure is called the major contributor to the hybrid, and the less stable resonance structures are called the minor contributors. Two identical resonance structures are equal contributors to the hybrid. 

Structures B and C have charge separation and fewer bonds than A, making them less stable resonance structures and only minor contributors to the resonance hybrid. B and C both contain a double bond between the centrsil carbon atoms, however, so the hybrid must have a partial double bond there. This makes the c entral C—C bond shorter than a C-C single bond in an alkane. 

Some data for BF3 show a shorter than expected B—F bond. Shorter bonds indicate double-bond character, so the structure with the B=F bond may be a minor contributor to a resonance hybrid.) The main way electron-deficient atoms attain an octet is by forming additional bonds in reactions. When BF3 reacts with ammonia, for instance, a compound forms in which boron attains its octet ... 

A better resonance structure is one that has more bonds and fewer charges. The better structure is the major contributor and all others are minor contributors. To draw the resonance hybrid, use dashed lines for bonds that are in only one resonance structure, and use partial charges when the charge is on different atoms in the resonance structures. 

A better resonance structure is one that has more bonds and fewer charges. The better structure is the major contributor and all others are minor contributors. 

We can show this resonance stabilization for conjugated double bonds of butadiene in terms of Lewis structures, as shown below. The dipolar form is the minor contributor to the resonance hybrid because it takes energy to separate charges. 

The hydroxyl oxygen atom can donate an electron pair to carbon to give resonance structure 3 in which every atom has a Lewis octet. This stabilizes the C=0 group, and the carbonyl carbon atom is less electrophilic than that of aldehydes or ketones. However, since this contributing structure has a positively charged oxygen atom, it is only a minor contributor to the resonance hybrid. 

In addition to the Kekule-type contributors to the pyridine resonance hybrid shown on page 391, there are three minor dipolar contributors. Draw their structures. Do they suggest a reason why pyridine is deactivated (relative to benzene) toward reaction with electrophiles and a reason why substitution, when it does occur, takes place at the 3-position ... 

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