Organic Chemistry about Ester

ESTER

Odor is a product innovated for both men and women to make them cool, sexy, and fresh. Over the past decades people are going to be crazy to search and get methods to get perfume .Perfumes are known as ester. And here we are going to introduce one of the great inventions in the organic chemistry field.  What are esters?

Esters are chemical compounds consisting of a carbonyl adjacent to an ether linkage. They are derived from carboxylic acids. A carboxylic acid contains the -COOH group, and in an ester the hydrogen in this group is replaced by a hydrocarbon group of some kind.with a hydroxyl compound such as an alcohol or phenol. Esters are usually derived from an inorganic acid or organic acid in which at least one -OH (hydroxyl) group is replaced by an -O-alkyl (alkoxy) group, and most commonly from carboxylic acids and alcohols. That is, esters are formed by condensing an acid with an alcohol.

A common ester - ethyl ethanoate

Ethyl acetate is one of the carboxylic acid esters. Carboxylic acid esters are among the most pleasant-smelling organic compounds. They contribute to the flavours and fragrances of fruits and flowers.  Many are excellent solvent and reaction intermediates.  And the common esters are volatile liquids.The name of an ester contains two parts, the first part is the 'alcohol part' and the second part is the 'acid part'.For ethyl acetate, the IUPAC name is ethyl ethanoate.  'Ethyl' is the 'alcohol part' while 'ethanoate' is the 'acid part'.  The name ethyl acetate is only the name based on the common name for the acid, and the common name of ethanoic acid is the acetic acid.The most commonly discussed ester is ethyl ethanoate. In this case, the hydrogen in the -COOH group has been replaced by an ethyl group.

Esterification of carboxylic acids

The common way is the Fischer esterification, which involves treating a carboxylic acid with an alcohol in the presence of a dehydrating agent:

The equilibrium constant for such reactions is about 5 for typical esters, e.g., ethyl acetate. The reaction is slow in the absence of a catalyst. Sulfuric acid is a typical catalyst for this reaction. Many other acids are also used such as polymeric sulfonic acids. Since esterification is highly reversible, the yield of the ester can be improved using Le Chatelier's principle:

·        using the alcohol in large excess (i.e., as a solvent)

·        using a dehydrating agent: sulfuric acid not only catalyzes the reaction but sequesters water (a reaction product). Other drying agents such as molecular sieves are also effective.

·        removal of water by physical means such as distillation

Ethanoic acid reacts with ethanol in the presence of concentrated sulphuric acid as a catalyst to produce the ester, ethyl ethanoate. The reaction is slow and reversible. To reduce the chances of the reverse reaction happening, the ester is distilled off as soon as it is formed  .

List of other Ester

Organic Chemistry about Soap and Detergent

Soap and Detergent

Soaps and detergents contain "surfactants"---compounds with molecules that line up around water to break the "surface tension" that holds it together in drops. They contain a combination of fats (or triglycerides) and alkali that create molecules with two unique chemical ends. One end, the "hydrophilic" end, is attracted to water, and the other, the "hydrophobic" end, is repelled by water but attracted to grease and oil. The hydrophobic ends bond with dirt, and the hydrophilic ends line up around them, encapsulating dirt and grease with a layer of molecules that will allow the dirt to float through the water and ride it down the drain. Surfactants can be anionic (negatively charged) or non-ionic (no charge). Soap, the original surfactant compound, was made with fats such as lard and alkali from wood ashes or lye. Today a wide variety of organic and petroleum-based fatty acids are used, and sodium or potassium hydroxides have replaced wood ash or lye in commercially prepared soaps and detergents.

SOAPS

Soaps are water-soluble sodium or potassium salts of fatty acids. Soaps are made from fats and oils, or their fatty acids, by treating them chemically with a strong alkali.First let's examine the composition of fats, oils and alkalis; then we'll review the soap-making process.

SURFACTANTS IN DETERGENTS

A detergent is an effective cleaning product because it contains one or more surfactants. Because of their chemical makeup, the surfactants used in detergents can be engineered to perform well under a variety of conditions. Such surfactants are less sensitive than soap to the hardness minerals in water and most will not form a film.

Detergent surfactants were developed in response to a shortage of animal and vegetable fats and oils during World War I and World War II. In addition, a substance that was resistant to hard water was needed to make cleaning more effective. At that time, petroleum was found to be a plentiful source for the manufacture of these surfactants. Today, detergent surfactants are made from a variety of petrochemicals (derived from petroleum) and/or oleochemicals (derived from fats and oils).

Anionic Surfactants

The chemical reacts with hydrocarbons derived from petroleum or fats and oils to produce new acids similar to fatty acids.

A second reaction adds an alkali to the new acids to produce one type of anionic surfactant molecule.

Non-ionic Surfactants

non-ionic surfactant molecules are produced by first converting the hydrocarbon to an alcohol and then reacting the fatty alcohol with ethylene oxide.

These non-ionic surfactants can be reacted further with sulphur-containing acids to form another type of anionic surfactant.

Making of Soap

Soap is made two ways. The first, called "saponification," involves cooking fats and adding alkali to the mix at the end to form soap and two byproducts, water and glycerin. The second, called hydrolization, splits the fats and oils into fatty acids and glycerin using steam under pressure. It distills the acids and neutralizes them with alkali. Homemade soap hobbyists make five or six bars of soap using a pound of animal or vegetable oils, two ounces of lye (or other alkali) and about a cup of water. The oils are melted while the akali is added to the water and heated to approximately 110 degrees Fahrenheit. The lye water is added gradually to the cooled oils. The mixture gradually is simmered and re-simmered until a gelatinous substance called "trace" is formed. The trace is poured into molds and must age for several weeks to cure completely.

Making of Detergent

During the past century, the shortage of animal and vegetable fats during World War I and World War II led to the development of detergents, multiple-surfactant, hydrocarbon-based cleaners. Detergents, unlike soap, depend on chemical reactions for their formation. Petroleum-based oils (including "oleo," a compound used to make a replacement for butter) are combined with chemicals such as sulfuric acid, sulfur trioxide or ethylene oxide to form a fatty acid, which is combined with an alkali to form yet another molecule, an anionic surfactant. A second type of process converts a hydrocarbon into a fatty alcohol that then combines with another chemical such as ethylene dioxide to form a nonionic surfactant. Homemade detergents are made by combining a bar of laundry soap such as Fels Naptha or Zote (both of which contain petroleum distillates) with a pound each of washing soda (sodium carbonate) and borax (Sodium borate decahydrate). The combination can be powdered in a blender or the soap can be liquefied with water over heat; then the soda and borax are added to make a liquid.

Process of Soap and Detergent in cleaning

Detergents and soaps are used for cleaning because pure water can't remove oily, organic soiling. Soap cleans by acting as an emulsifier. Basically, soap allows oil and water to mix so that oily grime can be removed during rinsing. Detergents were developed in response to the shortage of the animal and vegetable fats used to make soap during World War I and World War II. Detergents are primarily surfactants, which could be produced easily from petrochemicals. Surfactants lower the surface tension of water, essentially making it 'wetter' so that it is less likely to stick to itself and more likely to interact with oil and grease.
Modern detergents contain more than surfactants. Cleaning products may also contain enzymes to degrade protein-based stains, bleaches to de-color stains and add power to cleaning agents, and blue dyes to counter yellowing. Like soaps, detergents have hydrophobic or water-hating molecular chains and hydrophilic or water-loving components. The hydrophobic hydrocarbons are repelled by water, but are attracted to oil and grease. The hydrophilic end of the same molecule means that one end of the molecule will be attracted to water, while the other side is binding to oil. Neither detergents nor soap accomplish anything except binding to the soil until some mechanical energy or agitation is added into the equation. Swishing the soapy water around allows the soap or detergent to pull the grime away from clothes or dishes and into the larger pool of rinse water. Rinsing washes the detergent and soil away. Warm or hot water melts fats and oils so that it is easier for the soap or detergent to dissolve the soil and pull it away into the rinse water. Detergents are similar to soap, but they are less likely to form films (soap scum) and are not as affected by the presence of minerals in water (hard water).

Difference between Soap and Detergent

Soap is a triacylglyceride derviative (fat) while detergents are often produced synthetically. The head-group of soap a molecule is usually a carboxylate anion while common detergents often use phosphate or sulfate head-groups (ie Sodium Dodecyl Sulfate). Soap's effectiveness is greatly affected by the presence of certain minerals in solution such as those typically associated with hard water. Detergents are usually not affected by minerals in solution. The downside to detergents is the fact that most of them are not biodegradable; although some can be chemically modified to allow for degradation by microorganisms usually by the addition of a branched methyl group).

Example of some Soap and Detergent molecule

Example of some Detergent molecule

Detergents and soaps are used for cleaning because pure water can't remove oily, organic soiling. Soap cleans by acting as an emulsifier. Basically, soap allows oil and water to mix so that oily grime can be removed during rinsing. Detergents were developed in response to the shortage of the animal and vegetable fats used to make soap during World War I and World War II. Detergents are primarily surfactants, which could be produced easily from petrochemicals. Surfactants lower the surface tension of water, essentially making it 'wetter' so that it is less likely to stick to itself and more likely to interact with oil and grease.

Modern detergents contain more than surfactants. Cleaning products may also contain enzymes to degrade protein-based stains, bleaches to de-color stains and add power to cleaning agents, and blue dyes to counter yellowing. Like soaps, detergents have hydrophobic or water-hating molecular chains and hydrophilic or water-loving components. The hydrophobic hydrocarbons are repelled by water, but are attracted to oil and grease. The hydrophilic end of the same molecule means that one end of the molecule will be attracted to water, while the other side is binding to oil. Neither detergents nor soap accomplish anything except binding to the soil until some mechanical energy or agitation is added into the equation. Swishing the soapy water around allows the soap or detergent to pull the grime away from clothes or dishes and into the larger pool of rinse water. Rinsing washes the detergent and soil away. Warm or hot water melts fats and oils so that it is easier for the soap or detergent to dissolve the soil and pull it away into the rinse water. Detergents are similar to soap, but they are less likely to form films (soap scum) and are not as affected by the presence of minerals in water (hard water).

Organic Chemistry about Drugs

Drugs

Where Do Drugs Come From? 61% of the 877 small molecules introduced as drugs worldwide from 1981-
2002 were inspired by “Natural Products” (J. Nat. Prod. 2003, 1022). Hence, the discovery, biological profiling (SAR),
and preparation of natural products is of paramount importance in terms of public health.

Organic chemistry in medical field

Organic chemistry is necessary in the medical fields. All living organisms consist of plenty of organic matter. The organic compounds in the various materials which are vital and important to sustain life. Proteins, carbohydrates and fat are all organic compounds contributed to the structure of the human body. Organic compounds are enzymes and incentive materials that are essential for the occurrence of biological processes.  Drugs are also composed mainly of organic compounds. Doctor or pharmacist won’t be effective if he  is not sufficiently aware of the structure and function of the organic compounds of organic chemistry and pharmaceuticals and must understand properly the medication description that he offers the patient.  It is clear that the organic molecules is necessary to sustain life. Understanding of these compounds is critical in the medical field, not only to understand the basic biological functions, but also to predict the scenarios in the body and which may be due to disruption of organic materials. Completion of a medical organic chemistry can only be achieved understanding of organic chemistry.

Analgesics

Analgesics, also known as "painkillers", are medicines which relieve pain. Most analgesics are safe to use when taken as prescribed or instructed by your doctor or pharmacist, in conjunction with the manufacturer’s instructions on the packaging. Some extra precautions may apply to patients with pre-existing medical conditions such as kidney failure or gastric ulcers.


This page outlines some commonly used over-the-counter analgesics, including what they are used for, possible side effects and risks associated with using them outside the directions on the packet. The painkillers covered are:

• aspirin
• codeine (in combination products)
• ibuprofen
• paracetamol.

Analgesics are available in many forms. These include tablets, capsules, suppositories, soluble powders and liquids. Analgesics are generally swallowed, and their intended purpose is to relieve pain. Some can also be used to reduce fever, help relieve the symptoms of cold and ’flu, reduce inflammation and swelling, control diarrhea, and suppress coughs.

Morphine:

               
Used as early as 4000 BC, the main ingredient of opium, it was not until 1803 that Morphine was first identified and isolated by the German pharmacist Serturner. He called this alkaloid "Morphia" after Morpheus, the Greek God of Dreams. Morphine is used medicinally to alleviate severe pain. Morphine was
used during the American Civil War as a surgical anesthetic and was sent home with many soldiers for relief of pain. At the end of the war, over 400,000 people had the army disease, morphine addiction. It is obtained from opium poppy pod, used as early as 4000 BC. It has potent analgesic and euphoric properties. Morphine composes 10-15% of dry weight of the poppy. 95% of morphine extracted is converted to codeine.

Structure of Codeine

Structure of Morphine

Aspirin

Willow Tree

Aspirin and the Willow Tree: The father of modern medicine, Hippocrates, who lived sometime between 460 B.C and 377 B.C. left historical records of pain relief treatments, including the use of powder made from the bark and leaves of the willow tree to heal headaches, pains and fevers. The active ingredient in willow bark, termed salicin, was isolated in 1828, by Buchner, a pharmacy professor of at the University of Munich. By 1829, the French chemist Leroux improved the extraction procedure, obtaining ~30g of salicin from 1.5kg of willow bark. Later, in 1838, the Italian chemist Piria split salicin into a sugar and an aromatic component (salicylaldehyde) and converted the latter, by hydrolysis and oxidation, to a crystalline, colorless acid, that he named “salicylic acid.” However, salicylic acid was tough on stomachs. In 1853, Gerhardt neutralized salicylic acid by buffering it with sodium (sodium salicylate) and acetyl chloride, creating acetylsalicylic acid. Gerhardt had no desire to market his product and abandoned his discovery. In 1899, the German chemist Hoffmann, who worked for Bayer, rediscovered Gerhardt's formula, and gave it to his father who was suffering from arthritis. With good results, Felix Hoffmann convinced Bayer to market the new wonder drug. Aspirin was patented on March 6, 1889.


          

Aspirin Structure and for medical use

Therefore, from all this we can conclude that Organic compounds, lead a very important role in our lives, it is the basic material in our food. Synthetic carbohydrates and protein, fatty acids, vitamins, enzymes and others are only organic compounds, as well as clothing types and components of petroleum and natural gas, organic compounds are important to humans. Scientists were able to manufacture many of the organic compounds that have a key role in our daily lives; such as medicines, pesticides, fertilizers, cosmetics, plastics, and detergents, etc... which has had the greatest impact on human progress.