PRODUCT IDENTIFICATION

67-64-1

58.08

TOXICITY

Dimethyl ketone; Pyroacetic acid;

SMILES

The most common process is as a co-product with phenol.

CLASSIFICATION

GENERAL DESCRIPTION

PHYSICAL AND CHEMICAL PROPERTIES

AUTOIGNITION

465 C

NFPA RATINGS

REFRACTIVE INDEX

APPLICATIONS

APPEARANCE

PURITY

99.5% min [G.C.]

COLOR, APHA

5 max

WATER

0.3% max

CLARITY IN WATER

Clear

ACIDITY

0.002% max

90 min (minutes)

0.001% max (g/100ml)

56 C

Carbonyl groups are: 

• Aldehydes (X and Y = H; X = H, Y = alkyl or aryl)
• Ketones (X and Y = alkyl or aryl)
• Carboxylic acids (X = OH, Y = H, alkyl, or aryl)
• Esters (X = O-alkyl or aryl; Y = H, alkyl, or aryl)
• Amides (X = NH, N-alkyl, or N-aryl; Y = H, alkyl, or aryl)
• Acid halides
• Acid anhydrides
• Lactones
• Lactams

Ketone has the general formula RCOR' where the groups R and R' may be the same or different, or incorporated into a ring (R and R' are alkyl, aryl, or heterocyclic radicals). The simplest example, R and R´ are methyl group, is acetone (also called 2-propanone, CH₃COCH₃) which is one of the most important ketones used in industry (low molecular weight ketones are general purpose solvents.) In the IUPAC system, the suffix -one is used to describe ketone with the numbering of the carbon atom at the end that gives the lower number. For example, CH₃CH₂COCH₂CH₂CH₃ is named 3-hexanone because the whole chain contains six carbon atoms and the oxygen is connected to the third carbon from the lower number. There are aromatic ketones of which acetophenone and bezophenone are examples. Ketones can be made by the oxidation of secondary alcohols and the destructive distillation of certain salts of organic acids. In addition to as polar solvents, ketones are important intermediates in the syntheses of organic compounds such as alkoxides, hydroxyalkynes, imines, alcohols (primary, secondary as well as tertiary), acetals, thioacetals, phosphine oxides, geminal diols, hydrazones, organic sulfite and cyanohydrins.

Polarity

The most common solvent is water. Other common solvents which dissolve substances that are insoluble (or nearly insoluble) in water are acetone, alcohol, formic acid, acetic acid, formamide. BTX, carbon disulfide, diemthyl sulfoxide, carbon tetrachloride, chloroform, ether, tetrahydrofuran, furfural, hexane and turpentine. They may be classified as polar and non-polar. Polar solvents, like water, have molecules whose electric charges are unequally distributed, leaving one end of each molecule more positive than the other. Usually polar solvent has O-H bond of which water (HOH), (CH₃OH) and acetic acid (CH₃COOH) are examples. Propanol, butanol, formic acid, formamide are polar solvents. Dipolar solvents which contain a C-O solid bond without O-H bond are acetone [(CH₃)₂C=O], ethyl acetate (CH₃COOCH₂CH₃), methyl ethyl ketone, acetonitrile, N,N-dimethylformamide and diemthyl sulfoxide. Nonpolar solvents, like carbon tetrachloride (CCl₄), benzene (C₆H₆), and diethyl ether ( CH₃CH₂OCH₂CH₃), have molecules whose electric charges are equally distributed and are not miscible with water. Hexane, tetrahydrofuran and methylene chloride are non-polar solvents. Polar solvents are hydrophilic but non-polar solvents are lipophilic. Polar reactants will dissolve in polar solvents. Non-polar solvents dissolve non-polar compounds best. Oil and water don't mix but separate into two layers. There are three measures of the polarity as "dipole moment", "dielectric constant" and "miscibility with water". Though low dipole moments and small dielectric constants indicates non-polar solvents, sharp boundaries between polar and non-polar solvents are not available. The polarity reflects the balance between a polar component (OH) and a non-polar hydrocarbon component, existing in the same molecule. If hydrocarbon character increases relatively, the polarity decreases. On an operational basis, solvents that are miscible with water are polar.

Polar Protic and Dipolar Aprotic

Protic refers to a hydrogen atom attached to an electronegative atom. Protic solvents can donate an H+ (proton) since they contain dissociable H+, such as hydrogen attached to oxygen as in a hydroxyl group, nitrogen as in a amine group. Examples are water, methanol, ethanol, formic acid, hydrogen fluoride and ammonia. Aprotic solvents don't has O-H bond but a C=O bond typically. Examples are acetone [(CH₃)₂C=O] and ethyl acetate (CH₃COOCH₂CH₃). Polar protic solvents are useful in S_N1 reaction, while polar aprotic solvents are S_N2 reaction.