Basicity of Carboxylate ion || Organic Chemistry || Conjugate base || Withdrawing Groups | Shorts ||

When a carboxylic acid donates its proton, it becomes a negatively charged ion, RCOO−, called a carboxylate ion. Carboxylate is the conjugate base of a carboxylic acid, RCOO − .
A carboxylate ion is the conjugate base of a carboxylic acid. The carboxylate ion undergoes delocalization of the negative charge. Hence, the carboxylate ion becomes more resonance stabilized.
A carboxylate ion is much more stable than the corresponding alkoxide ion because of the existence of resonance structures for the carboxylate ion which disperse its negative charge.
The carboxylate ion is an anion, or ion with a negative charge, and is the conjugate base of a carboxylic acid. It is formed when a carboxylic acid is deprotonated by a base, such as sodium hydroxide or sodium bicarbonate.
Carboxylate ions are stabilized by resonance, which delocalizes the negative charge between two more electronegative oxygen atoms. This makes carboxylate ions more stable than phenoxide ions, which have a less efficient delocalization of the negative charge.
Carboxylic acids are the strongest among organic acids, as they readily lose the hydroxyl proton to form a resonance-stabilized carboxylate ion.
The carboxylate ions act as good nucleophiles.
Basicity of Carboxylate ion || Basic Concept of Basicity ||Organic Chemistry || Conjugate base || Withdrawing Groups | Shorts ||

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#conjugate_base #Ka_values #carboxylic_acids #Acetic_acid #Brønsted–Lowry_acids #strong_mineral_acids #more_acidic_than_alcohols #negative_charge #delocalise #delocalize #resonance #electron_withdrawing_group #carboxylate_to_carboxylic_acid #conjugate_base_of_a_carboxylic_acid #polar #less_polar #organic_acids #removal_of_a_proton #delocalization_of_the_negative_charge #resonating #deprotonated_state #acidic_&_basic_character #carboxylate_ion #alkoxide_ion #resonance_stabilized

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