[Chemistry Class Notes] on Phenol Acidity Pdf for Exam

Phenol is a common name for a compound. It is attached to a hydroxyl group to an atom number of an atomic ring.The IUPAC name of phenol is benzonal. The substitution of phenol with either the Ortho meta para or the numbering system can be employed. In either of the cases, the parent molecule is to be referred to as phenol. Common names and given to certain phenols for example phenols are known as cresols. Due to their high acidity, phenols are also known as carbolic acids.

Phenols are the organic compounds having benzene ring bonding to a hydroxyl group, which are also known as carbolic acids (phenol carbolic acid). Phenols usually react with active metals such as potassium, sodium and forms phenoxide. Happening such reactions of phenols with metals indicates it is acidic in nature.

 

Phenols also react with aqueous sodium hydroxide to produce phenoxide ions. It shows the acidity of phenols is higher compared to alcohol and water molecules as well.

 

Explaining the acidity of phenol

The acidity of phenol is because of its ability to lose the hydrogen ion forming phenoxide ions.

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Similarly, phenols can also lose H+ from the -OH group by showing acidic behavior.

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This phenoxide ion structure has a few special properties that are:

• Phenoxide ion is well established due to the resonance

• The oxygen is connected to sp² carbon, which has a high electronegativity.

So, the carbon will pull e^– from the oxygen. And, this makes the phenoxide ion stable due to the distribution of the electronegative charge. 

• Since the phenoxide ion is completely stable, phenol readily loses a hydrogen ion and shows the acidic character

• However, if any substituent is attached to the benzene ring, the stability of the phenoxide ion will be affected

Let’s look at the effect of substituents on the acidity of Phenols.

• If electron-donating groups are substituted on phenol, they push those electrons on the negative charged O. And, this reduces the phenoxide ion’s stability.

• So, if the electron-donating groups are substituted on phenol, resultantly, its acidity reduces. Due to this reason, cresol is less acidic than phenol.

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• But, if the electron-withdrawing groups are substituted with phenol, they pull the electrons from the negatively charged O, which increases the stability of the phenoxide ion.

• So, if the electron-withdrawing groups are substituted for phenol, it increases its acidity. Because of this, nitrophenol is more acidic than phenol.

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• Thereby, the position of the substituent group also affects the acidity of phenol. The substituent at ortho and para position has a more significant influence on acidity compared to the meta position. 

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• If a substituent is an EWG (Electron Withdrawing Group), delocalization of negative charge will be more when it lies in ortho and para position. So, EWG will cause an increased acidity rate when the group is at ortho and para positions compared to meta positions.

Resonance of Phenol

When more than one Lewis structure can be drawn, either the ion or the molecule is said to have resonance.

 

Resonance is a concept where electrons are delocalized over three or more atoms of a compound or molecule and the Lewis structure of that molecule cannot be depicted as a single and straightforward structure. 

 

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Observe that three of the four contributing structures possess a positive charge on the molecule’s oxygen atom. Therefore, the true hybrid structure must have a partial positive charge. Since oxygen is an electronegative element, the electrons in the oxygen-hydrogen bond orbital attract to the oxygen atom, resulting in partially positive hydrogen.

 

The loss of a hydrogen ion to a base creates a phenoxide ion, which is completely resonance stabilized.

 

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Also, observe that the phenoxide anion results upon the removal of hydroxy hydrogen by a base. This anion is resonance stabilized by delocalization of an electron pair all over the molecule, such as depicted by the contributing structures.

 

Properties of Phenol as an Acid

A few of the phenol’s properties by combining with different solutions are listed below.

The pH value of a typical dilute solution of phenol in water is approximately to be of 5 – 6 depending on its concentration. It means a very dilute solution is not really acidic enough to turn a litmus paper ultimately to red. Whereas litmus paper will be blue at pH = 8, and at the same time, red at pH = 5. If anything in between exists, it will be shown with some shade of “neutral.” Phenol reacts with the sodium hydroxide solution resulting in a colorless solution with sodium phenoxide.

 

During this reaction, the hydrogen ion was removed by the strongly basic hydroxide ion in the sodium hydroxide solution.

Phenol is not acidic enough to react with any of these. Going towards another approach, carbonate and hydrogen carbonate ions are not solid enough to remove a hydrogen ion from phenol. Unlike most acids, phenol does not give carbon dioxide when you mix it with one of them. In addition, this lack of reaction is quite useful. You can also recognize phenol because of the reasons listed below.

Physical Properties of Phenol Acidity

• Physical state: Phenols are colourless solids or liquids. However, due to oxidation they mostly turn reddish-brown in the atmosphere.

• Boiling point: An increase in the number of carbon atoms due to Van Der Waals forces, increases the boiling point of phenol.

• Solubility in water: Phenols are readily soluble in water due to their ability to form hydrogen bonding but the solubility decreases due to the addition of other hydrophobic groups and the ring.

• Reactions involv
  ing O–H bond cleavage: Phenols react with metals such as Na, K, and AI, etc with the release of hydrogen gas to form phenoxide.

Conclusion

This is all about the structural, physical, and chemical properties of phenol. Its unique properties due to the resonance of the constituent atoms of the molecule make it different. Focus on the conceptual description here and understand how it behaves in different chemicalreactions.