Acetone: Difference between revisions
imported>David E. Volk (start) |
imported>David E. Volk (acid base behavior) |
||
| Line 1: | Line 1: | ||
{{subpages | {{subpages}} | ||
Acetone, is an aprotic solvent widely in organic chemistry reactions. Because it has a high dipole moment it can be used for organic reactions in which ionic reagants are use or in which ionic reaction intermediates are produced. Nucleophilic reactions procede faster in acetone, compared to alcohols, because anions are less well solvated. | Acetone, is an aprotic solvent widely in organic chemistry reactions. Because it has a high dipole moment it can be used for organic reactions in which ionic reagants are use or in which ionic reaction intermediates are produced. Nucleophilic reactions procede faster in acetone, compared to alcohols, because anions are less well solvated. | ||
== physical properties == | == physical properties == | ||
Acetone, chemical formula CH<sub>3</sub>C(=O)CH<sub>3</sub>, is a planar, highly polar molecule with a dipole | Acetone, chemical formula CH<sub>3</sub>C(=O)CH<sub>3</sub>, is a planar, highly polar molecule with a large dipole (<math>\mu</math> = 2.88) and large dielectric constant (<math>\epsilon</math> = 20.7). The presence of a central carbonyl group, with only one carbon on each side, makes it the smallest [[ketone]]. Its high dielectric constant means that it can separate ionic charges fairly well. Acetone has a very high vapor pressure, is flammable and boils at 56.5 Celcius. Although acetone has two possible forms, the keto- and the enol-forms (see figure), the keto- form is greatly favored for acetone. | ||
== acid-base features == | |||
The oxygen atom of acetone has two lone electron pairs that can be shared with [[Lewis acid-base theory|Lewis acids]], and thus is a [[Lewis acid-base theory|Lewis base]]. Lewis acids such as AlCl<sub>3</sub> or BF<sub>3</sub> can form complexes with acetone in which the metal atom shares some of the oygen atoms electron pairs. The resulting partial positive charge on the carbonyl oxygen atom is stabilized by a resonance structure in which the carbonyl double bond becomes a single bond and donates electrons to the oxygen. As a result, the carbonyl carbon atom becomes partially charged and becomes more electrophilic. Protonation of the carbonyl oxygen also enhances the electrophility in a similar manner. | |||
Acetone can also function as a very weak acid, with a pK<sub>a</sub> of 19. When a base removes one proton from either of the non-carbonyl carbons of acetone, a [[carbanion]] is produced in which one of the carbon has a negative charge. This structure has an resonance from, an [[enolate]] ion, in which a double bond is formed between this negative carbon and the carbonyl carbon, the C-O bond becomes a single bond, and the negative charge is placed on the oxygen atom. This is the deprotonated enol form. | |||
[[Category:CZ Live]] | [[Category:CZ Live]] | ||
[[Category:Chemistry Workgroup]] | [[Category:Chemistry Workgroup]] | ||
Revision as of 11:19, 6 December 2007
Acetone, is an aprotic solvent widely in organic chemistry reactions. Because it has a high dipole moment it can be used for organic reactions in which ionic reagants are use or in which ionic reaction intermediates are produced. Nucleophilic reactions procede faster in acetone, compared to alcohols, because anions are less well solvated.
physical properties
Acetone, chemical formula CH3C(=O)CH3, is a planar, highly polar molecule with a large dipole ( = 2.88) and large dielectric constant ( = 20.7). The presence of a central carbonyl group, with only one carbon on each side, makes it the smallest ketone. Its high dielectric constant means that it can separate ionic charges fairly well. Acetone has a very high vapor pressure, is flammable and boils at 56.5 Celcius. Although acetone has two possible forms, the keto- and the enol-forms (see figure), the keto- form is greatly favored for acetone.
acid-base features
The oxygen atom of acetone has two lone electron pairs that can be shared with Lewis acids, and thus is a Lewis base. Lewis acids such as AlCl3 or BF3 can form complexes with acetone in which the metal atom shares some of the oygen atoms electron pairs. The resulting partial positive charge on the carbonyl oxygen atom is stabilized by a resonance structure in which the carbonyl double bond becomes a single bond and donates electrons to the oxygen. As a result, the carbonyl carbon atom becomes partially charged and becomes more electrophilic. Protonation of the carbonyl oxygen also enhances the electrophility in a similar manner.
Acetone can also function as a very weak acid, with a pKa of 19. When a base removes one proton from either of the non-carbonyl carbons of acetone, a carbanion is produced in which one of the carbon has a negative charge. This structure has an resonance from, an enolate ion, in which a double bond is formed between this negative carbon and the carbonyl carbon, the C-O bond becomes a single bond, and the negative charge is placed on the oxygen atom. This is the deprotonated enol form.