NANO MATERIALS

 

Here is the intro and some properties of nano materials..

INTRODUCTION

The word “nano” derives from the latin word “nanus” and Greek word “𝜈 ́𝛼νς,” Both indicating a person of very low height, i.e. a dwarf.  Nanomaterials are conventionally defined as materials having at least a dimension between 1 and 100 nm.

Common types of nanomaterials include nanofilaments, nanotubes, nanowires, nanocables, nanothin film, dendrimers, quantum dots, composite materials, and other materials besides nanopowder. Because of the unique nanoscale (1–100 nm) size, nanomaterials are different from microscopic atoms molecules and macro-objects in terms of their physical, chemical, electrical, and magnetic properties.

On the basis of reduction in size of materials in different dimensions, nanomaterials are classified into three groups.

Surface effects

Nanomaterials possess a large fraction of surface atom per unit volume. This dramatic increase in the ratio of the surface atom to interior atom in nanomaterials is responsible for great change in physical and other properties of the materials. When the size of the object is reduced to a nanometric range the proportion of surface atom increased leading to substantially more reactive surface sites. Thus nanomaterials possess high surface area over volume ratio, which leads them to interact with the environment more effectively compared to bulk materials. The surface atoms have less coordination that lead them to lesser stability and highly reactive than the interior atoms. A further consequence of this lower stability of atoms or molecules at the surface is the lower melting point of surface layers. 

Properties of nanomaterials:

High surface area and quantum effects at the nanoscale are responsible for different properties of nanomaterials compared to bulk materials. The quantum confinement effects describe electrons in terms of energy levels, valence bands, conduction bands, and electron energy band gaps. The confinement means restricting the motion of randomly moving electrons to specific energy levels (discreteness). When the particle size is reduced to nanoscale, the band gap is increased as compared with the bulk materials, and it leads to wider in the separation between the energy levels. Hence, properties such as melting point, fluorescence, electrical conductivity, magnetic permeability, and chemical reactivity change as a function of the size of the particle.

 Electrical properties :

The electrical conductivity of nanomaterials is generally lower than the bulk materials due to the increase of the band gap energy with a decrease in particle size of the nanomaterials. In bulk metals, the valence and conduction bands overlap, while in metal nanoparticles there is a gap between these bands. The gap observed in metal nanoparticles can be similar in size to that seen in semiconductors (< 2 eV) or even insulators (> 2 eV). This results in a metal becoming a semiconductor.  

 Optical properties: 

The optical properties such as reflection, transmission, absorption, and light emission of

the nanomaterials are completely dependent on their electronic structure.  At nanoscale level, nanoparticles are so small that electrons in them are not as much as free to move as in case of bulk material. Due to this quantum confinement of electrons, nanoparticles react differently with light compared to the bulk material.  Optical properties such as emission and adsorption occur when electron transition occurs between the highest occupied molecular orbital, which is a valence band, and the lowest unoccupied molecular orbital, which is essentially the conduction band. This optical bandgap increases with the decrease in particle size. Tuning the nanosize of a semiconductor means tuning of bandgap leading to light of certain wavelength being emitted. Thus the same material emits different colours depending on its size. 

Example: 

It is well known that gold has the characteristic yellow, brilliant color, but when gold is produced in the nanosized dimension range, its color invariably changes to red. In other words, gold shows

a color depending on the size of the gold particles. This phenomenon has an impressive example in the so-called Lycurgus cup now preserved at the British Museum in London. 

This cup was probably created in Rome during the fourth century and shows a different color changing the light from opaque green to bright red. This is the most famous example of the so-called dichroic glass. Actually, it presents some tiny amount of nanosized gold and silver that gives these unusual optical properties. This happens because at the nanoscale range, the electron cloud located on the surface of a gold nanoparticle has the possibility to resonate with different wavelengths of light depending on their frequency. 

Magnetic properties:

Compared to bulk materials nanomaterials show a variety of unusual magnetic behavior due to the surface or interface effects. The magnetic properties of a magnet are described by its magnetisation curve (called hysteresis curve which is the variation of intensity of magnetisation with applied magnetic field). These curves show the property like whether a magnet can be used as permanent magnet or a electromagnet etc…. The size of the material can change the property of a magnet by changing the magnetisation curves. Thus nanostructuring of bulk magnetic materials leads to changes in the curves which can produce soft or hard magnets with improved properties. Thus the nanomaterials may become superparamagnetic, even though their corresponding bulk materials are not magnetic. For example, Fe3O4 nanoparticles showed superparamagnetic-like behavior, even though bulk iron oxide (Fe3O4) is ferromagnetic. Exceptional surface energy and the flipped orientation of the spin electrons of the Fe3O4 nanoparticles are responsible for this phenomenon.  Superparamagnetic nanoparticles are not magnetic when located in a zero magnetic field, but they quickly become magnetized after an external magnetic field is applied. When they are below the superparamagnetic diameter, the nanoparticles can revert quickly to a nonmagnetized state after an external magnet is removed

 Mechanical properties 

 Mechanical properties of nanomaterials may reach the theoretical strength, which are one or two orders of magnitude higher than that of single crystals in the bulk form. The enhancement in mechanical strength is simply due to the reduced probability of defects. Carbon nanotubes are 100 times stronger than steel but six times lighter. 

HALOALKANES AND HALOARENES

 Dear Students,

In this post, I have shared the theoretic basis of haloalkanes and haloarenes in Q and A format. Thisi is useful for your examination purpose.

Haloalkanes and haloarenes are compounds in which one or more hydrogen atoms in a hydrocarbon have been replaced with halogen atoms. The difference between haloalkanes and haloarenes is that haloalkanes are derived from alkanes while haloarenes are derived from aromatic hydrocarbons. Haloalkanes are commonly referred to as alkyl halides whereas haloarenes are commonly referred to as aryl halides.

In haloalkanes, the halogen atoms are attached to sp3 hybridized carbon atoms. In haloarenes, the halogen atoms are attached to sp2 hybridized carbon atom. The difference in the hybridization state of the carbon atom in C-X (carbon-halogen) bond is responsible for the different reactivates and properties of these compounds.

You can download the study material from the below link.

Haloalkanes-Haloarenes

LAWS OF THERMODYNAMICS

 

First law of thermodynamics:

The first law of thermodynamics states that heat is a form of energy, and  that heat energy cannot be created or destroyed.  It can, however, be transferred from one location to another location or converted to one from to other forms of energy. 

Whenever a system goes through any change due to the interaction of heat, work and internal energy, it is followed by numerous energy transfers and conversions. However, during these transfers, there is no net change in the total energy. Thus, according to first law of thermodynamics the energy of the universe remains the same.  This is known as the principle of conservation of energy. Any gain in energy by the system will correspond to a loss in energy by the surroundings, or any loss in energy by the system will correspond to a gain in energy by the surroundings.

ΔE = q + w

 ΔE -  Change in internal energy 

ΔE =  Efinal - Einitial

A positive value of ΔE results when Efinal > Einitial, indicating that the system has gained energy from its surroundings. A negative value of ΔE results when Efinal < Einitial, indicating that the system has lost energy to its surroundings. 

Endothermic and Exothermic Processes:

When a process occurs in which the system absorbs heat, the process is called endothermic (endo- means “into”). During an endothermic process, such as the melting of ice, heat flows into the system from its surroundings. If we, as part of the surroundings, touch a container in which ice is melting, the container feels cold to us because heat has passed from our hand to the container. A process in which the system loses heat is called exothermic (exo- means “out of”). During an exothermic process, such as the combustion of gasoline, heat exits or flows out of the system into the surroundings.

To understand the meaning of the first law, we can take the common example of a heat engine. In a heat engine, the thermal energy is converted into mechanical energy. Heat engines are mostly categorized as open systems. The basic working principle of a heat engine is that it makes use of the different relationships between heat, pressure and volume of a gas. A heat engine is a system which converts heat into work by taking heat from the reservoir (hot body) to carry out some work. There is a discharge of some heat to the sink (cold body). In this system, there will also be some waste in the form of heat. 

A very basic diagram of the heat engine is given below:

THERMODYNAMICS

 

The word ‘thermodynamics’ is derived from two words: thermo and dynamics. ‘Thermo’ stands for heat while ‘dynamics’ is used in connection with a mechanical motion which involves ‘work’. 

Broadly speaking, thermodynamics is a branch of science that deals with heat, work and temperature, and their relation to energy, radiation and physical properties of matter. It explains how thermal energy (heat energy) is converted to other forms of energy and how matter is affected by this process.

Different Branches of Thermodynamics:

• Classical Thermodynamics
• Statistical Thermodynamics
• Chemical Thermodynamics
• Equilibrium Thermodynamics

In classical thermodynamics, temperature and pressure are taken into consideration, which helps us to calculate other properties and predict the characteristics of the matter undergoing the process.

Chemical thermodynamics is the study of how work and heat relate to each other in chemical reactions

and in changes of states.

THERMODYNAMIC TERMS AND BASIC CONCEPTS: 

To study the basic concepts of thermodynamics it is important to study a few terms and definitions which must be understood clearly.

Thermodynamic Systems:

A system is that part of the universe which is under thermodynamic study and the rest of the

universe is surroundings. The real or imaginary surface separating the system from the

surroundings is called the boundary

There are three types of systems:

Open System –

 In an open system, the mass and energy both may be transferred between the system and surroundings. A steam turbine is an example of an open system.

Closed System – 

In the closed system, the transfer of energy takes place but the transfer of mass doesn’t take place. Refrigerator, compression of gas in the piston assembly, etc., are examples of closed systems.

Isolated System – 

An isolated system cannot exchange energy and mass with its surroundings. The universe is considered an isolated system.

THERMODYNAMIC PROCESS:

The change of thermodynamic state from one condition to another condition ( change in temperature or pressure) is called thermodynamic process. One example of a thermodynamic process is increasing the temperature of a fluid while maintaining a constant pressure.

REVERSIBLE PROCESS:

A reversible process for a system is defined as a process that, once having taken place, can be reversed, and in so doing leaves no change in either the system or surroundings. In reality, there are no truly reversible processes. One way to make real processes approximate reversible process is to carry out the process in a series of small or infinitesimal steps.

For example, transferring heat across a temperature difference of 0.00001 °F "appears" to be more reversible than for transferring heat across a temperature difference of 100 °F. Therefore, by cooling or heating the system in a number of infinitesimally small steps, we can approximate a reversible process.

IRREVERSIBLE PROCESS

An irreversible process is a process that cannot return both the system and the surroundings to their original conditions. That is, the system and the surroundings would not return to their original conditions if the process was reversed. 

For example, an automobile engine does not give back the fuel it took to drive up a hill as it coasts back down the hill.

Isothermal Process

An isothermal process is a thermodynamic process that takes place at a constant temperature. It means that an isothermal process occurs in a system where the temperature remains constant. However, to keep the temperature of the system constant, heat must be transferred into the system or shifted out of the system.

In simple terms, in the isothermal process: T = constant. This implies, the change in temperature will be zero i.e., ΔT=0

Examples:

Melting and Evaporation, etc. 

Working in the refrigerator is an isothermal process. The temperature of the surroundings changes irrespective of changes in the internal temperature of the refrigerator. Excess heat is removed and transmitted to the surrounding.

Adiabatic Process:

An adiabatic process is a thermodynamic process that can take place without any heat transfer between a system and its surrounding. Here, neither heat nor energy is not transferred into or out of the system. Therefore, in an adiabatic process, the only way the energy transfer takes place between a system and its surroundings is the work. 

Examples:

1. Release of air from a pneumatic tyre.

 A pneumatic tire consists of an outer rubber layer, an inner chamber that contains compressed air and a tread pattern. This type of tire works by utilizing the air-filled chamber to provide cushioning and absorb shocks. Under a load, the tire compresses the air inside, distributing the weight evenly and reducing the impact on surfaces. The design allows for a smooth, stable ride, while the tread pattern on the tire provides grip and traction. The tire's flexibility and the pressurized air inside enable it to adapt to different terrains and surfaces. When a tyre bursts, the sudden release of the high-pressure air inside the tyre causes the air to rapidly expand. This rapid expansion of the gas occurs without any heat transfer to or from the surroundings, as the process happens too quickly for significant heat exchange to take place.

PURIFICATION TECHNIQUE - I

 

Dear students,

It is known that organic compounds can be derived from natural sources and these are mixed with other substances and are impure. Similarly compounds prepared in the laboratory  are also mixed with other by products formed during the course of the reaction. To purify such compounds, various methods are adopted. Some of the common methods are as follows

Crystallization

Sublimation

Distillation

Extraction

Chromatography

In this post we are about to discuss two methods of purification. They are as follows.

Solvent Extraction: 

Extraction means drawing (pulling out) a compound out of a mixture using a solvent. It means organic compounds have a "choice" of two solvents that they can dissolve in. It requires two solvents that are not miscible in each other. Usually one of the solvents is water. The other solvent is a liquid that does not dissolve very well in water, such as diethyl ether.

The process of removing organic substance from its aqueous solution by mixing with suitable organic solvent is termed solvent extraction. It is also called as liquid-liquid extraction and partitioning. It is an equilibrium process and is a convenient technique can be carried out using separating funnel.

Principle of Solvent Extraction

It is based on the fact that different substances have different solubility in different solvents.

Procedure:

The aqueous solution of the given solute (organic substance) is taken in a separating funnel. It is mixed with the organic solvent. The funnel is closed, and its contents are shaken well. It is then allowed to remain undisturbed for some time. Water and organic solvent will form separate layers, and the  solute will be transferred from aqueous layer to the organic layer. In the funnel, the solvent forms the upper layer while the water forms the lower layer. The two layers can be recovered by opening the stop cock and collecting them in separate bakers. On evaporating the organic solvent, the solute can be recovered.

It is important to note that extraction is more efficient (i.e., higher purification) when the process is repeated. For example, benzoic acid can be extracted from its water solution using benzene. 

It is based on the distribution law, also called the Nernst’s distribution law. It states that if a solute X distributes itself between two immiscible solvents A and B, at constant temperature and X is in the same molecular condition in both solvents, then

The constant 𝐾D (or simply K) is called the distribution coefficient or Partition coefficient or Distribution ratio. 

Applications:

It is used in perfumes, vegetable oil, biodiesel processing, etc.

It is used to segregate hazardous contaminants from sludge and sediments.

In the petrochemical industry, it is used to separate and purify different components of crude oil.

It is used for the separation and purification of organic compounds.

It removes oil and grease that  spilled into water. This helps clean up environmental pollution.

Crystallization:

It is a purification technique used to separate solids from a solution. In this method, the impurities are dissolved in a suitable solvent and then filtered to remove impurities.

Principle: 

An impure organic solid is completely dissolved in a small amount of solvent by boiling. The hot solution is allowed to cool slowly. The impurities remain in the solution (called the "mother liquor") while the organic substance comes out as pure crystals . It is then filtered and dried.

Procedure:

Step 1: Take some water in a beaker

Step 2: Add organic substance (impure) and stir it

Step 3: Now heat the solution

Step 4: Add more impure substance.

Step 5: After some time there will be a point at which no more substance can be dissolved in water. This stage is the saturation point, and the solution is referred to as a saturated solution

Step 6: Now filter the substance with the help of a filter paper

Step 7: Collect the filtrate in a glass bowl and cool it slowly

Step 8: You will observe that some fine crystals are formed in the bowl

Step 9: The process of filtration can separate these crystals.

Selection of solvent:

(a) It dissolves more of the substance at higher temperature than at room temperature 

(b) The impurities are either insoluble or dissolve in solution (in the mother liquor) upon crystallization, 

(c) which is not highly inflammable and 

(d) which does not react chemically with the compound to be crystallized. 

The most commonly used solvents for crystallization are: water, alcohol, ether, chloroform, carbon- tetrachloride, acetone, benzene, petroleum ether etc. 

Fractional crystallization: 

The process of separation of different components of a mixture by repeated crystallizations is called fractional crystallization.

Examples:

(a) Sugar having an impurity of common salt can be crystallized from hot ethanol since sugar

dissolves in hot ethanol but common salt does not.

(b) A mixture of benzoic acid and naphthalene can be separated from hot water in which

benzoic acid dissolves but naphthalene does not. 

SEPARATION AND PURIFICATION TECHNIQUES

 

Methods of Separation:

Most of the time the substances that we see around us are not in their pure form. They are basically a mixture of two or more substances. Interestingly, mixtures tend to also come in different forms. Therefore, there are several types of separation techniques that are used in segregating a mixture of substances. As for the need for separation, it is usually done to remove all the unwanted materials and obtain useful components.

Methods Of Separating Mixtures:

• Evaporation
• Filtration or Sedimentation
• Separating Funnel
• Magnetic Separation

Evaporation

Evaporation is a technique that is used in separating a mixture, usually a solution of a solvent and a soluble solid. In this method, the solution is heated until the organic solvent evaporates where it turns into a gas and mostly leaves behind the solid residue.

Filtration or Sedimentation:

The most common method of separating a liquid from an insoluble solid is the filtration. Take, for example, the mixture of sand and water. Filtration is used here to remove solid particles from the liquid. Various filtering agents are normally used like filtering paper or other materials.

Separating Funnel

Separating funnel is used mainly to segregate two immiscible liquids. The mechanism involves taking advantage of the unequal density of the particles in the mixture. Oil and water can be easily separated using this technique.

Magnetic Separation:

When one substance in the mixture has some magnetic properties then this method is quite useful. Strong magnets are commonly used to separate magnetic elements.

ANESTHETICS

 

What Is Anesthesiology?

Anesthesiology is an important branch of medicine as it makes surgery safe, feasible and possible. During and after surgery the patient feel the pain and discomfort hence they may be given anesthesia.

Anesthetic is basically a medicine that acts as a sedative. The term anesthesia means loss of sensation. It produces loss of sensation to all types of cells and especially those of nervous sysem.. The important aspect of anesthetics are the loss of consciousness is reversible. 

Types:

1. General - complete loss of consciousness all over the body.

2. Local - lack of sensation in the area being operated on.

Ether:

The discovery of ether for the use as an anesthetic was in 1846 which marked the birth of a modern age in anesthesiology. The first true demonstration of ether as an inhalation anesthetic was on October 16, 1846 by William T.G. Morton, a Boston dentist. He discovered the anesthetic properties of ether in his search to provide patients with relief from painful dental procedures.

Preparation:

Advantages:

1. safe

2. does not modify blood pressure

3. economical

4. can be stored properly 

Disadvantages: 

1. induction of ether is slow

2. inflammable

3. recovery is slow.

Chloroform:

Chloroform or trichloromethane is an alkylchloride with the formula CHCl3. It is a very volatile, colorless, strong-smelling, dense liquid that serves as a powerful general anesthetic,  and sedative. 

Preparation:

Industrially, chloroform is produced by heating a mixture of chlorine and either methyl chloride (CH3Cl) or methane (CH4). At 400–500 °C, free radical halogenation occurs, converting these precursors to progressively more chlorinated compounds:

CH4 + Cl2 → CH3Cl + HCl

CH3Cl + Cl2 → CH2Cl2 + HCl

CH2Cl2 + Cl2 → CHCl3 + HCl

Disadvantages:

The anesthetic use of chloroform has been discontinued, because it caused deaths from respiratory failure and cardiac arrhythmias. Following chloroform-induced anesthesia, some patients suffered nausea, vomiting, , jaundice, and coma owing to hepatic dysfunction. 

Chloroform converts slowly in the presence of UV light and air to the extremely poisonous gas, phosgene (COCl2), releasing HCl in the process.

2 CHCl3 + O2 → 2 COCl2 + 2 HCl

ARTIFICIAL SWEETENERS

 Dear all,

We know about sugars and it gives sweet taste in our food stuffs. Sugars are used in our everyday life. There are wide variety of sugar brands we know. In this post we are going to discuss about sweeteners. 

What are sugars?

 Sugars are carbohydrates, found naturally in most plants. It is composed of carbon,  hydrogen,  and oxygen. All green plants make sugar through photosynthesis, the process plants use to transform the sun’s energy into food.

Where do we get sugars?

The most common sugar is sucrose  in sugarcane and sugar beets.

malt syrup is derived by breaking down the starches in cooked rice.

Lactose is the naturally occurring form of sugar in milk products.

Fructose, a sugar found in fruits and honey.

   

What makes sugar sweet?

The sweetness of sugar comes from a chemical interaction between sugar molecules and sweet taste receptor cells, which are found in our taste buds of our tongue. Different types of sugars can have varying levels of sweetness. Fructose is the sweetest of all naturally occurring sugars.

Artificial Sweeteners:

 Artificial sweeteners are chemically synthesized substances that are used instead of sucrose (natural sugar) to sweeten foods and beverages. They are many times sweeter than sugar and much smaller amounts (200 to 20,000 times less) are needed to create the same level of sweetness. The caloric content of sweeteners  is very small, so it is described as nonnutritive. 

It can be used directly in processed food such as puddings, dairy products, candy, soft drinks, baked goods, jams and many other foods and beverages.

Below is the list of some common artificial sweeteners commonly used.

1. Saccharin:

 It was discovered in 1879 and is considered the oldest non-nutritive sweetener. It is about 300 times more sweet than sucrose, but it has a bitter aftertaste. It cannot be used in products where baking of food is necessary as it becomes unstable when it is heated. But it can be used to sweeten candies, drinks, and toothpaste.

Structure:

sodium ortho benzenesulphonamide

2. Aspartame:

In 1879 Aspartame was discovered and it was found that it is approximately 200 times sweeter than sugar.  It is commonly used as a tabletop sweetener and is also used in a variety of foods. When it is heated it breaks down into amino acids and loses its sweetness, so it cannot be used for baked foods. It is only used in soft drinks and cold foods.

3-amino-N-(α-carboxyphenethyl)succinamic acid N-methyl ester

3. Cyclamate:

Cyclamate is an artificial sweetener and is about 30–50 times sweeter than sucrose (table sugar). It is the least potent of the commercially used artificial sweeteners. Hence, it is often used with other artificial sweeteners, especially saccharin. It is stable under heating. 

cyclohexylsulfamate

Advantages of Artificial Sweeteners

Weight Control:

 If we want to lose weight, then we should use an artificial sweetening agent as virtually it carries zero calories. One gram of sugar carries 4 calories, and one teaspoon of sugar contains about 4 grams of sugar. So by eating 1 teaspoon also we gain 16 calories. So in the case of weight control, an artificial sweetening agent is the best option. 

Diabetes:

 It also helps in controlling diabetes as it does not raise the blood sugar levels because it does not contain the carbohydrates in it.

Here is the link for study material

STUDY MATERIAL

COORDINATION POLYMERIZTION

Dear students,

This post is about polymerization using  coordination complexes. Transition metal compounds along with group 13 halides are generally used as catalysts. The first catalyst of this type was Ziegler - Natta catalyst. Here the mechanism of this polymerization is discussed.

Coordination Polymerization by Jim Livingston on Scribd

Coordination polymeriztion

ANTIPYRETICS

 Dear students...

This post discuss about antipyretics and anesthetics.

Antipyretics:

A drug that prevents or reduces fever by lowering the body temperature from a raised state. They work by influencing the body's hypothalamus(which keeps the body balanced in a stable state called homeostasis) the region responsible for regulating temperature. During an infection or illness, the body releases certain chemicals called pyrogens, which trigger the hypothalamus to increase the body's temperature as a defense mechanism. Antipyretic drugs intervene in this process, helping to bring down the elevated temperature and provide relief from associated symptoms like discomfort, chills, and body aches.

Some of the common antipyretics used in daily life are discussed here.

Aspirin:

Aspirin is a nonsteroidal anti-inflammatory drug (NSAID). It was the first of this class of drug to be discovered. Also known as acetylsalicylic acid (ASA) is a commonly used drug for the treatment of pain and fever due to various causes. Acetylsalicylic acid has both anti-inflammatory and antipyretic effects. This drug also inhibits platelet aggregation and is used in the prevention of blood clots stroke, and myocardial infarction

Therapeutic uses:

Fever

Head ache

Inflamation

  

Paracetamol:

It is a class of para-aminophenol derivatives. It has both antipyretic and analgesic effects. It occurs as white crystalline powder, odourless and soluble in alcohol and sodium hydroxide solution.  It is also soluble in boiling water and the solution is acidic in nature. It is used in the form of tablets, suspensions, syrups. The usual dose is 0.5 to 1.0 g for every four hours.

Therapeutic Uses:

Joint and muscle pain

Ibuprofen (Brufen):

Ibuprofen is a non-steroidal anti-inflammatory drug (NSAID) derived from propionic acid. It was first launched against rheumatoid arthritis.  Ibuprofen is insoluble in water, but very soluble in most organic solvents like ethanol.

Synthesis:

It is synthesized by the acylation of iso-butylbenzol by acetyl chloride. The resulting iso-butylbenzophenone (3.2.21) is reacted with sodium cyanide, giving oxynitrile (3.2.22), which upon reaction with hydroiodic acid in the presence of phosphorus is converted into 2-(4-iso-butylphenyl)propionic acid (3.2.23), which subsequently undergoes phases of dehydration, reduction, and hydrolysis.

Below is the link to download the study material.

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ANTIBIOTICS -II

 Dear students,

Here we are going to see about the next two antibiotics.

Chloramphenicol

Chloramphenicol is an antibiotic and is in the class of antimicrobials that inhibits protein synthesis. Chloramphenicol is a synthetically manufactured broad-spectrum antibiotic. It was initially isolated from the bacteria Streptomyces venezuelae in 1948 and was the first bulk produced synthetic antibiotic. It can be used against Gram-positive, Gram-negative, and anaerobic bacteria. It works by inhibiting protein synthesis thereby preventing the formation of bacterial protein.  Chloramphenicol can be administered topically ear drops, or as an eye ointment. It can also be given intravenous injection or taken as oral capsules. 

Structure:

It is a dichloro-substituted acetamide containing a nitrobenzene ring, an amide bond and two alcohol functions.  In 1949 a team of scientists at Parke-Davis including Mildred Rebstock published their identification of the chemical structure and their synthesis.

         

Therapeutic Uses:

1. Typhoid

A life-threatening infection caused by the bacterium Salmonella Typhi. Without treatment, there is a small chance of death from typhoid fever complications.

2. Whoophing cough:

Whooping cough (pertussis) is a highly contagious respiratory tract infection. In many people, it's marked by a severe hacking cough followed by a high-pitched intake of breath that sounds like "whoop." Once you become infected with whooping cough, it takes about seven to 10 days for signs and symptoms to appear, though it can sometimes take longer.

 

3. Urinary Tract Infection:

 

A urinary tract infection (UTI) is an infection in any part of the urinary system. The urinary system includes the kidneys, ureters, bladder and urethra. Most infections involve the lower urinary tract — the bladder and the urethra. Women are at greater risk of developing a UTI than are men. Urinary tract infections are often treat with antibiotics.

II Streptomycin:

Streptomycin is the first discovered aminoglycoside antibiotic, originally isolated from the bacteria streptomyces griseus. It is now primarily used as part of the multi-drug treatment of pulmonary tuberculosis. It has additional activity against several aerobic gram-negative bacteria.  It interferes with ribosomal peptide/protein synthesis. It binds to bacterial ribosome, inhibiting its functionality and halting further protein synthesis through inhibition of peptide bond formation. 

Selman Waksman and eventually Albert Schatz were recognized with the Nobel Prize in Medicine for their discovery of streptomycin and its antibacterial activity. 

Structure: 

Streptomycin is a amino cyclitol glycoside that consists
 of streptidine having a disaccharyl moiety
 attached at the 4-position. 

Therapeutic Uses:

1. Tuberculosis

Tuberculosis (TB) is an infectious disease that most often affects the lungs and is caused by a type of bacteria. It spreads through the air when infected people cough, sneeze or spit. Certain conditions can increase a person’s risk for tuberculosis disease:

diabetes (high blood sugar), weakened immune system (for example, HIV or AIDS), tobacco use.

Below is the link for the study material

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