Acetone
Acetone (systemic name: propanone)
is an organic compound with the chemical formula CH3COCH3 belonging to the
family of ketones and is the simplest representative of this family. Acetone is
a colorless, flammable liquid with a melting point of −95.4 °C and a boiling
point of 56.53 °C. One of the most popular household uses is its use as a nail
polish remover. Acetone is also used in the manufacture of plastics, fibres,
medicines and other chemicals.
Acetone dissolves in water, alcohol and ether.
Acetone is an important organic solvent. It is usually the preferred solvent
for cleaning purposes in the laboratory. About 5.1 million tons per year were
produced worldwide in 2009, mainly for use as a solvent and in the production
of MMA and BPA. Known household uses for acetone are as the active ingredient
in nail polish removal and as a polish thinner.
It is also a common building block
in organic chemistry. Acetone is produced naturally within the human body and
is also eliminated as a result of normal metabolic processes. Reproductive
toxicity tests have shown that acetone has little ability to cause reproductive
problems. In fact, the body naturally increases the level of acetone in
pregnant women, nursing mothers, and children because their need is high or high.
Energy leads to higher acetone production and the medical community is now
using the ketogenic diet, which increases acetone within the body, to reduce
epileptic attacks or seizures in infants and children with refractory epilepsy.
Properties of Acetone
Name of Molecule: Acetone
Molecular Geometry: Trigonal planar
Hybridization: sp2
Molecular Formula: CH3COCH3
Molecular Weight: 58.08 g/mol
Bond Pairs: 10
Lone Pairs: 2
Other names for acetone
·
propan-2-one
· Dimethyl ketone
· Dimethyl carbonyl
· β-Ketopropane
· Propanone
· 2-Propanone
· Dimethyl formaldehyde
· Pyroacetic spirit
· Ketone propane
Medical and cosmetic uses
Acetone is used in a variety of
general medical and cosmetic applications and is also listed as an ingredient
in food additives and food packaging. Acetone is commonly used in the skin
rejuvenation process in offices and medical spas. Since the days of ancient
Egypt, people have been using chemical peeling methods to rejuvenate the skin.
Some of the common agents used
today for chemical peeling are salicylic acid, glycolic acid and also (30%) of
salicylic acid in ethyl alcohol and trichloroacetic acid (methyl chloroform).
Chemical peels, the skin must be cleaned properly and the excess fat must be
removed. This process is known as the removal or removal of fat and in this
process acetone or subtisol or a combination of these agents is commonly used.
Laboratory uses
In the laboratory, acetone is used
as a polar, non-protonated solvent in a variety of organic reactions such as
(SN2) reactions. The use of the solvent acetone is critical to Jones'
oxidation. It is also a common solvent for rinsing laboratory glassware due to
its low cost and volatility however it does not form an azotrope with water.
Despite its common use as a putative drying agent, it is only effective by
displacing and loosening the buildup.
Acetone can be cooled using dry
ice (-78°C) without freezing. Dry ice acetone baths are commonly used to
conduct reactions at low temperatures. The acetone gives off light or
radiation. Fluorescent under UV light and its vapor can be used as radioactive
reagents in fluid flow experiments.
Household uses
Acetone is often the main
ingredient in cleaning agents, for example, as a nail polish remover. Ethyl
acetate is another organic solvent that can also be used occasionally. Acetone
is a strong glue remover that easily removes scale from glass, porcelain, or
porcelain.
Acetone can also be used as an
artistic or cosmetic agent when it is rubbed against the back of a laser print
or when a photographic image is placed face down on another surface and it is
highly polished or shimmered so that the image ink is transferred to the
surface of the destination.
Cuticles resulting from applying
wigs and mustaches by immersing the item in an acetone bath and then removing
the remnants of glue or glue with a strong brush. Some car enthusiasts also add
acetone at a ratio of about one to 500 parts to the fuel, after claims to
improve fuel consumption and engine life.
Toxicity
Acetone is believed to have slight
toxicity in normal use and there is no strong evidence of chronic health
effects if basic precautions are followed.
In very high concentrations of
vapor, acetone causes irritation and, like many other solvents, can affect and
inhibit the functioning of the central nervous system. OR is also a severe
irritant in contact with the eyes and potentially hazardous to aspiration or
pulmonary respiration. In one documented case, ingestion of a large amount of
acetone resulted in systemic poisoning although the patient eventually
recovered completely.
Some sources estimate (LD50) for
human ingestion at (1,159) g/kg, inhalation (LD50) by rats given as (44) g/m3
for more than four hours. It has been shown that acetone has antiepileptic
effects in animal models of epilepsy in the absence of toxicity, when it is
ingested in concentrations measured in mmol. It has been hypothesized that the
high-fat, low-carb ketogenic diet may be used in practice to combat drug
resistance to epilepsy in children as it increases acetone levels in the brain.
Environmental influences
Acetone evaporates rapidly even
from water and soil and once in the atmosphere it is broken down by ultraviolet
radiation with a half-life of 22 days. Acetone dissolves slowly in soil,
animals or waterways where it is sometimes consumed by microorganisms, but it
is considered a major pollutant of groundwater due to the high water solubility
(LD50) of acetone in fish (8.3 g/L of water) or about 0.8%) over 96 hours and
the environmental half-life of about (1-10 days).
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