The Dangers Of Inhalants Among Adolescents

The Dangers Of Inhalants Among Adolescents
Inhalants
This video talked over the classification of drugs known to America as inhalants. According to the
video Inhalants are known to be nitrous oxide solvents, aerosols, and nitrites. Inhalants can be found
and obtained very easily in your local grocery stores, hardware stores and local pharmacies. Because
of their easy accessibility to be found in kitchen and bathroom cabinets, much of its use is among
adolescents. Individuals that consume inhalants normally breathe in the fumes through their nose or
mouth,
Inhalants are known for its rapid rush of euphoria and light headedness only lasts a brief second to a
few minutes. The lungs take in the inhaled chemicals into the bloodstream very quickly and send
them all over the brain and body. Almost all inhalants produce a pleasurable effect by slowing down
brain activity. The danger of these inhalants is the amount of time they can remain in the body after
used. Consistent use of these inhalants can also cause serious harm to vital organs and systems
besides the brain. They can cause nerve damage that can lead to chronic pain, weakness in the
muscles, liver failure and heart damage. ... Show more content on Helpwriting.net ...
While sudden sniffing death syndrome is rare, research show how the toxic poisonings from the
fumes can cause the heart to stop quickly causing a heart attack. There are several signs to indicate a
person using Inhalants. One of the most common signs are the strong chemical odor on the
individuals clothing and breathe. For minors, obvious paint and other stains on their face, hands and
... Get more on HelpWriting.net ...

Methods Of A Solvent System For Extraction
Introduction Extraction is a technique that is commonly used to separate mixtures, despite whether
the components are solids or liquids. One of the most well–known examples of extraction is the
brewing of tea or the making of coffee. Every pot of coffee or cup of tea involves solid–liquid
extraction. The soluble flavor and caffeine are extracted from the solid tea leaves or ground coffee
beans into hot water (the solvent). Insoluble plant material is left behind in the tea bag or coffee
filter. During extraction, the mixture is brought together with a solvent in which the substance of
interest is soluble, but the other substances present in the mixture are insoluble. Typical lab
extractions are of organic compounds out of an aqueous ... Show more content on Helpwriting.net ...
In solid–liquid extractions, a solvent is added to a solid. The insoluble material can then be
separated by either gravity or vacuum filtration. This allows the soluble material to be 'extracted '
into the solvent. The filtered solution can then be used as a solution, or the solvent can be
evaporated to recover the solute in powder or crystalline form In liquid–liquid extractions,
extraction methods differ depending on the density of the solvent that is used. The other method of
extraction that is not used in this experiment is the acid–base extraction. Acid–base extractions are
those in which the water layer is made either acidic or basic in order to convert one component of
the mixture to an ionic compound. This makes it water soluble so that it may be separated from
other hydrophobic organic compounds. Most organics are soluble in polar organic solvents, but only
very small organics or very polar neutral organic compounds are soluble in water. An acid–base
extraction operates on the same principle as solid–liquid and liquid–liquid extractions, but can
provide a further level of fine–tuning. If one or more of the compounds in the mixture to be
separated is acidic or basic, the solubilities of these acidic and basic components can be manipulated
by applying simple acid–base reactions. The solubilities of acidic and basic compounds can then be
changed.
Experimental
A. Solid–Liquid Extraction Firstly, 0.2 g of the mixture

A Pilot Study Of Polybrominated Flame Retardents On...
Abstract
This paper reports the results of a pilot study of polybrominated flame retardents in household dust
collected for a small sample of households in Plymouth. It finds significant levels of pentaBDE
especially in bedrooms. The most likely cause is the continued use of pentaBDE within
polyurethane foam in mattresses and other bedroom furniture, in spite of the ban by the European
Court of Justice in 2004. Further work is called for in order to examine whether this reflects the
widespread continued use of mattresses and furniture bought before 2004. A larger sample size is
envisaged, including more detail on the nature and age of furniture and upholstery in households.
Introduction
The indoor environment is where human beings spend most of their time, whether at home or at
work, resulting in a high level of exposure to dust. Dust is a heterogeneous assortment of particles
derived from differing sources which include trace metals and chemical congeners. In 2004
Polybrominated diphenyl ether (PBDEs) pentaBDE and octaBDE were banned by the European
court of Justice. Although decaBDE is still used in the North American market in residential
upholstered furniture and mattresses. (Chao, et. al. 2014) Polybrominated diphenyl ether (PBDEs)
have been extensively used as flame retardants for highly flammable consumer goods throughout
homes, cars and workplaces. (Webster, et. al. 2015) PBDEs are a class of brominated flame
retardants that have been found in humans and wildlife

Grignard Limiting Reagent Using Bromobenzene
In Experiment 13B we generated a Grignard reagent using bromobenzene (the limiting reagent) and
magnesium in an ether solvent. This Grignard reagent was then reacted with benzophenone,
followed by an acidic workup, to produce triphenylmethanol. The ether solvent was used in this
experiment because is helped to stabilize the Grignard reagent by coordinating its lone pair
electrons, therefore donating electron density to a electron deficient magnesium molecule.
Anhydrous conditions were required because the Grignard reagent is a reactive nucleophile and a
strong base. The anhydrous conditions prevent the Grignard reagent from deprotonating water to
form benzene. We ensured anhydrous conditions by flame drying all of our glassware. The reaction
began with the insertion of magnesium into the carbon–bromine bond to generate the Grignard
reagent. 96 mg of magnesium turnings were ground up with a mortar and pestle in order to remove
any surface oxides and contaminations that may preclude magnesium's ability to react with
unreactive alkyl halides. The magnesium turnings, along with a small crystal of iodine and a drop of
1,2–dibromoethane were added to a round bottom flask. The 1,2–dibromoethane is necessary to
activate the alkyl halide. In a conical vial 2mL of anhydrous ether ... Show more content on
Helpwriting.net ...
The remaining organic layer was washed with sodium bisulfite and brine. The sodium bisulfite was
used to wash away MgOH and neutralize the acid. The solution was dried using anhydrous sodium
sulfate and heated until the solvent evaporated. Anhydrous sodium sulfate is a drying agent used to
remove water from the mixture. The crude mixture was triturated in petroleum ether. Trituration
broke down the crude mixture into a desirable compound that remained insoluble, and impurities,
which were soluble in the liquid. Therefore, the impurities were filtered out using petroleum ether.
This rinsed away the non–polar byproduct,

Grignard Reaction Lab Report
For this experiment, an organometallic reagent was used for the synthesis and isolation of benzoic
acid. The Grignard reaction is the addition reaction of an organometallic reagent, which in this case
was an organomagnesium reagent. An organometallic reagent is a carbon bonded to a metal. This
reagent was combined with an electrophile, a carbonyl compound such as a ketone or aldehyde.
Carbons are electrophilic when bound to a nonmetal thus the atoms are more electronegative than
the carbon and metals are less electronegative than carbon. When the organometallic carbon is used
to attack an electrophilic carbon, a new C–C bond forms and the C=O double bond breaks. By
adding an alkyl or aryl halide, bromide, to magnesium metal in an aprotic solvent ... Show more
content on Helpwriting.net ...
This allows for a weak acid to attach to form the unknown carboxylic acid. Sulfuric acid, a dilute
acid solution, was added to protonate the solution. To minimize the amount of bubbling that
occurred from the exothermic reaction, it was added slowly so that the sulfuric acid reacted with the
excess magnesium. Anhydrous diethyl ether, containing no water, was used as the solvent in
preparing the Grignard reagent because the oxygen contains a lone pair that can interact with the
partial positive on the magnesium which stabilizes the metal complex. Another potential solvent
could be THF, tetrahydrofuran, or hexane, but diethyl ether is a better solvent since it contains
oxygen. The reaction was then reduced with acid to protonate the carboxylate salt which yields a
carboxylic acid product. By adding acid, it also dissolved any excess magnesium metal, so a liquid–
liquid extraction can occur to isolate the product. A liquid–liquid extraction was used since the
experiment involved a liquid solvent that removed a liquid component from the liquid mixture. A
solid–liquid extraction would have been used if components were being removed from a solid by
using a

In This Experiment The Following Materials Were Used:...
In this experiment the following materials were used: spatula, glass stir rod, small test tube and rack,
six large test tubes, 10mL graduated cylinder, grease marker, 100 mL beaker(s), glass jar with lid,
Sharpie marker, pipettes with bulb, two 2 dram vials with black lids, funnel, 50–100 mL graduated
cylinder, filter paper, hotplate, 400–600mL beaker and ice, watch glass and ½ of a glass petri dish.
In addition, the organic compound, benzoic acid, the inorganic compound, iron sulfate, and all
chemicals in table 2 were used. Hazards associated with this experiment include glassware breaking
and cutting through skin. There was the danger of burning oneself through the use of the burner.
Hazards associated with chemicals are that they are ... Show more content on Helpwriting.net ...
(In this case, six mL of ethanol was added to the six test tubes). The latter two steps were repeated
for compound 2. The six test tubes were then placed in a labeled jar filled with a third of diethyl
ether and was put away to be checked on in a week. When checked, there was no indication of
crystal formation. The only change that was present was that the jar had small black particles
floating around in the diethyl ether due to sharpie remnants.
The next part of the experiment was the liquid to liquid diffusion. Two vials were obtained and
labeled (1 and 2). Then in a beaker, 50 mg of the first compound was dissolved with 2–5 mL of a
solvent from Part A that the two compounds readily dissolved in (which in this case was ethanol).
This solution was then transferred into the first vial. By referring to table three from the experiment,
a new miscible solvent with a lower density (than the solvent used) was chosen to be added onto the
solution in the vial. This meticulous procedure consisted of adding 2–3 pipette full amounts of the
lower density solvent onto the solution in the vial with the precaution of not allowing the solvents to
mix. After obtaining the layered solutions, the cap was screwed and the vial was placed in a certain
area to be referred back to in week for potential crystal formation. These series of steps were
repeated for the second compound. For both the benzoic acid solution and the iron sulfate solution,
two pipette full

Grignard Reagent Lab Report
The purpose of this experiment is to prepare a Grignard reagent by reacting with alkyl or aryl halide
and to ultimately react the Grignard reagent with carbon dioxide in order to produce carboxylate.
The formed carboxylate is then protonated with an acid to produce carboxylic acid that could be
used with liquid–liquid extraction to isolate the unknown acid from the other products from side
reactions. The final unknown product is identified by measuring the melting point and calculating
the molecular weight obtained from titration.
Organometallic compounds are compounds that contain carbon–metal bonds (C–M bonds), in which
carbon bears a partial negative charge because metal is less electronegative than the carbon. This
partial negative charge of the carbon atom allows it to be a good nucleophile that attacks the
electrophile to make a new carbon–carbon bond. There are several examples of organometallic
compounds, such as organolithium, Gilman reagents, and Grignard reagents (organomagnesium
reagent). In this experiment, Grignard reagents are prepared and reacted with other electrophilic
carbon to form a new carbon–carbon bond. Victor Grignard discovered Grignard reagent around
1890s and received a Noble Prize in 1912 with his discoveries. In this experiment, an alkyl halide or
aryl halide is reacted with magnesium metal to prepare a Grignard reagent (R–MgX). In this
Grignard reagent preparation reaction, halide is typically used with bromine (sometimes with
chlorine, not

Synthesis and Ir Analysis of...
Synthesis and IR Analysis of trans–[Bis(inosinato)palladium(II)]
Abstract
In this lab we synthesized trans–[Bis(inosinato) palladium(II)] for IR analysis. After completion of
the reaction 84.4% of the product was collected. IR spectrum of the product and inosine was
analyzed to determine how the inosine is bonded to the metal, palladium. From the IR analysis, it
was determined that when inosine reacts with palladium, a shift of about 65 cm–1 in the carbonyl
stretch was observed.
Introduction:
In this experiment, trans–[Bis(inosinato)palladium(II)], was synthesized. The general reaction
equation for the reaction is shown below: KOH
(1) K2[PdCl4] + 2 inosine trans–[Pd(inosine–H+)2] + ... Show more content on Helpwriting.net ...
A total of 1.5 mL was added to produce a pH of around 6. The mixture was stirred for an additional
30 minutes. The light yellow precipitate was collected by suction filtration using a Hirsch funnel.
The product was washed with two 1–mL portions of cold methanol followed by two 1–mL portions
of diethyl ether. The product was dried in the oven at 110°C. The IR spectrum as a KBr pellet was
obtained for the product and inosine for analysis.
Results and Discussion:
After completion of the reaction, the percent yield was collected for the product and is shown in
Table 1. Synthesis of the yellow solid Trans–[Bis(inosinato)palladium(II)] was 84.4%.
Table 1. Synthesis Results | Compound | Yield | Appearance | 1 | Trans–[Bis(inosinato)palladium(II)]
| 84.4 % | Yellow solid |
The result from the IR spectra for Trans–[Bis(inosinato)palladium(II)], and inosine are summarized
in Table 2 and 3. It is important to note that Trans–[Bis(inosinato)palladium(II)] compound had an
extra carbonyl peak at 1712.21 cm–1 which is from inosine impurity.
Table 1. IR ANALYSIS: trans–[Bis(inosinato)palladium(II)] Frequency (cm−1) | Bond Responsible |
3388.55 | O–H stretch | 2928.24 | SP³ C–H stretches | 1712.21 | C=O inosine impurity | 1636.64 |

Discussion The Grignard reaction involves the use of a Grignard agent, or an organomagnesium
halide, to an aldehyde or a ketone to form either a secondary or tertiary alcohol, respectively. Using
this reaction with formaldehyde leads to a primary alcohol. Grignard reagents can also be used in
important reactions such as in the addition of an excess of a Grignard reagent to an ester to give a
tertiary alcohol so that the two alkyl groups are symmetrical. Grignard reagents are formed though
the interaction of magnesium metal with alkyl or alkenyl halides. They are extremely good
nucleophiles, reacting with electrophiles such as carbonyl compounds, like aldehydes, esters, carbon
dioxide, ketones, etc., and epoxides. Grignard reagents are also ... Show more content on
Helpwriting.net ...
The Grignard reagent can be made through adding the halogenolkane to small pieces of magnesium
in a flask that contains diethyl ether. The lone pair electrons from two ether molecules form a
complex with the magnesium in the Grignard reagent to stabilize the organometallic compound in
order to increase the reagents' ability to react. The mixture in the flask was warmed over a water
bath for 30 minutes after the flask has been fitted to a reflux condenser. Everything should have
remained dry with minimal exposure to air because Grignard reagents react with water. If this
happens, the final results can be contaminated. The Grignard reactions cannot be classified as
nucleophilic substitutions, even though the reactions are clearly substitution reactions. The
functional carbon atom was reduced, resulting in the polarity of functional group being inverted; an
electrophilic carbon became a nucleophilic carbon. This resulted in the alkyl halide and the Grignard
reagents being excellent nucleophiles. The basic reaction of the Grignard reaction involves the
nucleophilic attack of the carbanionic carbon in the organometallic reagent to the electrophilic
carbon in the carbonyl to form

Introduction: Organometallic compounds are compounds that contain carbon–metal bond. Grignard
reagents, formed by reacting organic halide with suspensions of Mg turnings in an anhydrous
condition, are one of the most versatile organic reagents as it undergoes a variety of reactions
including synthesis of Malachite green and Benzoic acid. Malachite green is an organic compound
which can be used as dyes, stains and as an antimicrobial in aquaculture while benzoic acid can be
used as preservatives, antiseptic and analgesic. Grignard reagent can form a new carbon–carbon
bond through nucleophilic addition mechanism. A Nucleophilic addition reaction is an addition
reaction where a chemical compound with an electron deficiency or electrophilic π bond reacts with
electron rich nucleophile, creating a new σ bond. Grignard reagent is a strong base and a strong
nucleophile so they can easily react with the protons that are more acidic than those found on ...
Show more content on Helpwriting.net ...
Benzoic acid (0.05g) was taken in a round bottom flask and the reaction vessel was placed in an ice
bath. The Grignard reagent (), HCl (0.5mL, 3M) and MTBE (0.5mL) was added to the reaction
vessel dropwise and mixed well. After removing all the aqueous layer and drying the MTBE, the
product was analyzed using GC–MS. Results: The major component of the Grignard reaction was
prepared by reacting 4–Bromo–N, N–dimethylaniline with magnesium turnings using THF as a
solvent in an anhydrous condition as shown in equation 1. Methyl benzoate was reacted with the
Grignard reagent in an anhydrous condition in the presence of THF, followed by hydrolysis in order
to obtain green colored dye known as Malachite green, as shown in equation 2. The phenyl
magnesium bromide reacts with carbon dioxide in presence of THF and later treated with acid,
benzoic acid is formed, as shown in equation

Grignard Reactions Lab
Grignard Reactions
Introduction
Grignard reactions are of extreme importance in synthesis of many organic compounds. Because of
the extreme nucleophilic tendencies of the Grignard reagent (typically denoted RMgX, where R is
an organic nucleophile, and X is a halide), we find that Grignard reagents are extremely useful for
the addition of organic fragments. The Grignard reagent's extreme nucleophilicity can be explained
by its unique bonding abilities. Because the carbon–magnesium bond is neither fully covalent nor
fully ionic, this creates a very stable yet reactive region at the pseudohalide. Furthermore, the
relatively similar electronegativities of the two adjacent atoms create a strong pole between the two,
while still stable enough to ... Show more content on Helpwriting.net ...
The product appeared to be as desired, a visibly green dye.
The second reaction was prepared by synthesis of the reagent, benzoic acid. This reagent was
prepared from phenylmagnesium bromide and carbon dioxide in anhydrous THF. this is shown in
Scheme 2 below. (2)
Scheme 2: Synthesis of and Isolation of Benzoic Acid The above reaction was carried out and was
unsuccessful, yielding almost no amount of product. The desired appearance of the product was a
white crystalline compound. Since barely any product was isolated benzoic acid in the lab was
substituted for the next reaction.
The third reaction was prepared by synthesis of the reagent, benzoate. This reagent was prepared
from phenylmagnesium bromide with benzoic acid in anhydrous THF. this reaction produced
benzoic acid, benzene and water. This is shown in Scheme 3 below. (3)
Scheme 3: Reaction of Benzoic Acid with PhMgBr The above reaction was carried out and was
successful for most students, yielding a significant amount of product. One of two possible products
was made, the other being triphenyl methanol. The melting point of this product is, showing that we
did in fact make the expected product.

Extraction Lab Report
Extraction
Aleigha Spaulding
Joseph Osazee
10–6–15
Abstract:
This report presents the percentage recoveries found when using the solid–liquid and liquid–liquid
extraction techniques to extract a strong acid, weak acid, base, and neutral compound from a
mixture. During the solid–liquid section of the experiment, 0.5 M NaHCO , 0.5 M NaOH, 0.5 M
HCl, and distilled water are used to dissolve and separate the acid, phenol, and amine solutions from
the mixture, leaving the neutral compound remaining. After adding 3 M HCl to the acid and phenol
solutions and3 M NaOH to the amine solution, the solutions and solids formed were filtered and the
percent recovery of each was calculated. The percent recovery was around a range of 20 % to 22 %
for the acid, phenol, and amine, but the neutral had a much higher percentage about 60 %. After
using similar techniques for the liquid–liquid extraction section of the experiment, removing the
clear lower layer of the two immiscible liquids each time, the percent recovery was around 50 % –
55% for the acid and neutral. The percentages for the phenol and amine were lower. In both sections
of the experiment, some percentage of the acid, phenol, amine, and neutral compounds was
recovered, so that part of the experiment was successful.
Introduction:
Extraction is defined as a process for separation of compounds in a mixture based on difference in
their solubility. Extractions have been in use for centuries, and there are many

An Unknown Grignard Reagent Experiment Essay
Grignard
5. Introduction In this experiment, an unknown Grignard reagent was prepared from an aryl halide.
The unknown reagent was then reacted with carbon dioxide to form a carboxylic acid. The solid acid
was then isolated and recrystallized before the melting point was taken. The precipitate was then
dissolved in water and titrated to determine the molecular weight. The melting point and molecular
weight were then used to determine the unknown acid obtained from the experiment.
6. Data and Results The product obtained had a melting point of approximately 107 °C and a weight
of .324 grams. Some of the product would not dissolve in water and so was removed through
vacuum filtration, which left .141 g not dissolved in solution. It took 13.2 mL of sodium hydroxide
to turn the solution of the product dissolved in water pink. A molecular weight of 138.63 g/mol was
calculated from the data. These results indicate that the product was 2–methylbenzoic acid, the
Grignard reagent was 2–methylphenylmagnesium bromide, and the unknown bromide solution was
2–methylbromobenzene. Calculations showed that the limiting reagent of the Grignard preparation
was magnesium and that the experiment had a 23.13 % yield. 7. Discussion and Conclusion
Organometallic compounds, such as Grignard reagents, are molecules containing carbon–metal
bonds and are often used to create new carbon–carbon bonds. Grignard reagents–or
organomagnesims– are specifically those that have a carbon–magnesium bond.

Organometallic Reactions : Identification Of An Unknown...
LAB 7: ORGANOMETALLIC REACTIONS: IDENTIFICATION OF AN UNKNOWN
BROMIDE (Preparative) Introduction The first purpose of the lab was to prepare an unknown
organomagnesium bromide, an organometallic reagent, reacting an unknown aryl bromide with
magnesium in anhydrous ether. The unknown was chosen from a predetermined list of benzoic acid
derivatives with varying molecular weights and melting points (see Supplement C). The second
purpose of this lab was to prepare an unknown carboxylic acid by reacting the unknown aryl–
magnesium bromide with carbon dioxide and diethyl ether then protonating.The third purpose of
this lab was to determine the neutralization equivalence point of the unknown carboxylic acid by
titrating with sodium hydroxide. The fourth purpose of this lab was to ascertain the identity of the
unknown carboxylic acid, and thus the original unknown aryl bromide, using its molecular weight
determined from neutralization and melting point. Data and Results Compound Molecular Weight
(g/mol) Melting Point (°C) Unknown Carboxylic Acid (R––COOH) 121.18 116–119 Discussion
Organometallic reagents are compounds with carbon–metal (R––M) bond. In the carbon–metal
bond, carbon is more electronegative than the metal atom which creates a dipole moment where
carbon possesses a partial negative charge and the metal atom possessing a partial positive charge
(Rδ–––Mδ+). The partial negative charge on the carbon allows it to act as a strong nucleophile or
base similar to

For this lab, certain actions were performed to facilitate the optimal conditions for the Grignard
reaction to proceed. As mentioned above, forming the Grignard reagent and the Grignard reaction
must take place in dry, anhydrous conditions. This was why the glassware was initially placed in the
oven to evaporate any moisture that was present on the glassware. Additionally, the magnesium used
in the experiment needed to be dry too, so it was also placed in the oven to be heated. Creating a dry
environment was also why the reaction vessel was covered in the septum because it helped prevent
the moisture in the air from entering the reaction. Having water in the reaction vessel would destroy
the Grignard reagent and hinder the Grignard reaction. Because the reaction needed to be done in
dry and anhydrous conditions, diethyl ether was used as the solvent because it was aprotic meaning
that the formation of phenylmagnesium bromide and the Grignard reaction would not be hindered
by the protonation of water and alcohols3.
Additionally, creating a dry environment for the reaction tried to reduce the formation of side
products. One possible side product was benzene, which was formed during the protonation of the
carbanion on the benzene ring during the formation of the Grignard reagent4. The carbanion was
very basic meaning that if there was any water in the glassware or moist air in the environment,
some of the carbanion will be protonated by the water creating benzene instead of

Essay On Inhalants
Hundreds of household products are being misused as inhalants. Some of these products include nail
polish remover, hair spray, cleaning fluids, spray paint, and the propellant in aerosol whipped cream
("Inhalants", 2010). Inhalants are breathable chemical vapors that users intentionally inhale because
of the chemical's mind–altering effects (National Institute on Drug Abuse [NIDA], 2010). The trend
in inhalant abuse is growing among the young community throughout the country. Surveys have
shown in 2008 2 million Americans of 12 or over reported using inhalants (NIDA, 2010). Young
children from the age of 12 to 17 are the primary age group of abusers (National Drug Intelligence
Center [NDIC], 2001). The numbers reflect that it is becoming ... Show more content on
Helpwriting.net ...
Nitrites are a group of chemicals including cyclohexyl nitrite, amyl nitrite, and butyl nitrite. Instead
of acting on the central nervous system for the euphoric effect, nitrites dilate blood vessels, relax the
muscles, and are used for sexual enhancement (NDIC, 2001). Amyl nitrite consists of a clear,
yellowish liquid that is sold in a cloth, covered sealed bulb. This type of nitrite is also known as a
snapper or popper because the bulb makes a snapping sound when it is broken (Missouri
Department of Mental Health, n.d.). On the other hand, butyl nitrite comes in small bottles sold as
video head cleaner, room odorizer, leather cleaner and liquid aroma (NIDA, 2010). One category
may sound worse than the other, but in reality they are all equally harmful and all cause short term
and long term effects to a person's health.
All effects of inhalants are harmful to the body. However, the short term effects on a person can be
brutal. Immediately after inhaling, users feel intoxication and other side effects. These effects
include slurred speech, dizziness, confusion, and uncoordinated movements. Furthermore, users
may also experience nausea, vomiting, lightheadedness, hallucinations, and delusions ("Inhalants",
2010). Loss of inhibition has been reported by users as well as drowsiness and headaches. When a
person inhales nitrites, the blood vessels are dilated, the heart rate is increased, and there is a
sensation of heat and excitement that lasts several

Naphthalene And Salicylic Acid Lab Report
The purpose of this experiment is to separate a mixture of salicylic acid and naphthalene using
extraction, recrystallization and sublimation techniques. Extraction is the separation of compounds
from a mixture based on their relative solubilities in different solvents. Sublimation is the process of
separation by which a substance transitions from the solid phase into the gas phase, skipping the
liquid phase. Recrystallization involves dissolving a substance in an appropriate solvent then
crystallizing it as it cools (impurities remain in solution). The melting points of the substances were
determined in order to assess their purity and the percent recovery of pure naphthalene and salicylic
acid were calculated. According to the results, the melting point of pure naphthalene was between
86°C –89°C range, whereas for pure salicylic acid was 167°C –170°C. Both determined melting
points were higher compared to the literature value of 80.26°C and 158.6°C for pure naphthalene
and salicylic acid respectively. Lastly, the percent recovery for pure naphthalene and salicylic acid
were 17.7% and 71.2% accordingly. In this experiment were used three separation techniques:
extraction, sublimation and recrystallization. During the first method, 0.70 g sample of salicylic
acid–naphthalene mixture was dissolved in 10 ml of diethyl ether. The solution was placed in a
separatory funnel and 10 ml of saturated aqueous sodium bicarbonate solution was added to it. After
the initial gas was

Grignard Reagent From An Unknown Aryl Halide
7) Discussion:
In this experiment, the goal is to prepare a Grignard reagent from an unknown aryl halide and
identify the identity of the aryl halide by converting it to a carboxylic acid to determine its melting
point and molar mass (determined by titration). The experiment began by dissolving 0.25g of
magnesium powder in a 25mL round–bottom with 5mL of anhydrous ether and stirring with a stir
bar. Then the round–bottom flask was set up for reflux using a Claisen adapter where the vertical
part is covered with a septum to prevent air from mixed with the solution. The septum is very
important because the Grignard product can react with oxygen to produces a carboxylic acid, which
is not wanted. Also, the choice of anhydrous solvent is important because the Grignard product can
react with water to produce an alkane. With the reflux set up, the next step was to add the halide.
1.2mL of the unknown bromoarene mixed with 2.5mL ether was slowly added dropwise through the
septum using the needle and syringe. The bromoarene had to be added slowly because there
Grignard product would undergo another unwanted side reaction by reacting with the unknown
bromoarene. The product with be a new carbon–carbon bond between the unknown bromoarene and
the Grignard product. If the bromoarene is added slowly, the chances of the Grignard product
reacting with the bromoarene over the magnesium is low because magnesium exists in larger
concentration in the solution. Once all the unknown bromoarene

Advantages And Disadvantages Of Extraction
Chapter Five
Discussion
Extraction is a process by which substances and active constituents are separated from the original
matrix, extraction process depends on many physical and chemical characteristics. Extraction is
divided into two types liquid phase extraction and solid phase extraction depending on the physical
phase of extraction agent(Rezaee et al., 2006). In our study, we have adopted liquid phase extraction
for several reasons. Firstly, simple, inexpensive, relatively precise and wide range methods for
separation, identification, and quantification of drugs, poisons, and herbal medicine. Secondly, An
equilibrium distribution is established by the ratio between two phases will be influenced by the
choice of the extracting solvent, the pH value of the aqueous phase and the ratio of the volumes of
the organic to aqueous phases (Ahadi et al., 2011). ... Show more content on Helpwriting.net ...
regia unripe fruit using two extraction methods (microwave and soxhlet methods). The selection of
solvents was based on the gradual increase in the polarity, ethyl acetate, acetone, ethanol, methanol,
and water. The highest efficient solvent for extraction was water as the total yield weight of the
extracts was 3.4 g in the fatted and defatted J. regia using microwave and soxhlet methods. Whereas,
the lowest efficient solvent for extraction was ethyl acetate as the total yield weight of the extracts
was only 0.74 g. The increase in the polarity of the extraction solvent has conferred a significant
increase in yield amount as there were 4.6 fold increases in the amount of yield between the lowest
polarity solvent (ethyl acetate) and the highest polarity solvent (water) regardless to the extraction

In the Grignard Synthesis of Malachite Green, 4–bromo–N,N–dimethylaniline (aniline) and
Magnesium (Mg) in the solvent THF were reacted to form the Grignard reagent. From there, ester
methylbenzoate was used, along with HCL to yield Malachite Green. It is important to note that the
Grignard reagent is very moisture sensitive. Due to this, it is possible for side reactions to occur.
Due to the basicity of the Grignard reagent, any exposure to moisture or water will cause the reagent
to deprotonate water and deter from the actual reaction that is desired. Thus, several precautions
were taken to prevent side reactions from occurring, such as oven–drying the glassware for 30
minutes and using a dry disposable syringe fitted with a metal needle. ... Show more content on
Helpwriting.net ...
Because magnesium is a very electropositive metal, it is reactive and inserts itself in between the
carbon on the aniline ring and the bromine atom. A cloudy brown–grayish solution formed and
bubbles emerged and these processes were indicators that the Grignard reagent was proceeding. The
bubbles formed was from the hydrogen gas that arised from the unreacted magnesium specks. It was
formed from the quenching step, where HCL was added to the reaction flask and two chlorine ions
reacted with the unreacted Magnesium ions to form MgCl2 and h2. This formation of H2 was the
hydrogen gas that was produced and appeared in the form of

The Preparation Of Grignard Reagents
The preparation of Grignard reagents typically involves the reaction of an alkyl halide or aryl halide
with magnesium metal in an anhydrous ethereal solvent. This reaction results in the formation of a
carbon–magnesium complex within an alkyl magnesium halide or aryl magnesium halide. Grignard
reagents are considered to be strong nucleophiles and strong bases that have the ability to react with
acidic proton sources and carbonyl functional groups. The preparation of Grignard reagents must be
conducted in aprotic solvents to minimize interactions with strong proton sources that may result in
undesired products. Furthermore, the solvent chosen for the reaction must dissolve everything in
solution. Commonly used solvents in Grignard reactions are diethyl ether and tetrahydrofuran
(THF). They are preferred over hexane solvents due to the presence of an oxygen atom which
contains a lone electron pair that attracts the partially positive magnesium metal, resulting in
increased stability. As mentioned previously, Grignard reagents are strong nucleophiles. Thus, there
is a possibility that they may react with other molecules in side–reactions. One such side–reaction
involves the Grignard reagent reacting with molecular oxygen (O2) to form a peroxide molecule. In
another side–reaction, the Grignard reagent may react with carbon dioxide (CO2) to form a
carboxylate molecule. These side–reactions can pose a problem since molecular oxygen and carbon
dioxide are in excess under normal

Separating Acids and Neutral Compounds by Solvent Extraction
Separating Acids and Neutral Compounds by Solvent Extraction Introduction The purpose of this
experiment was to use solvent extraction techniques in order to separate a mixture consisting of a
carboxylic acid (p–toulic acid), a phenol (p–tert–butylphenol), and a neutral compound (acetanilide).
Extraction is the process of selectively dissolving one or more of the compounds of a mixture into
an appropriate solvent, the solution that contains these dissolved compounds is called an extract
(Manion, 2004). Impurities that are present in the solution can be removed by extracting them from
the original solvent into another solvent. This is done by mixing two immiscible (insoluble to one
another) solvents (Manion, 2004). By mixing the ... Show more content on Helpwriting.net ...
This process was then repeated two more times with subsequent additions of 10 mL of the 0.5M
aqueous NaHCO3 and the aqueous layers drained off into the above mention labeled 100–mL
beaker. Finally 5 mL of deionized water was placed into the funnel and mixed. The water was then
drained off into the beaker containing the aqueous solution extracts. The solution was then saved
until need later in the experiment. The extraction of the p–tert–butylphenol was then carried out in
the exact same fashion as the p–toulic acid, with the exception that the aqueous solution added to the
remaining ether solution was 10 mL of 0.5M NaOH. The solution was mixed and the gas was in the
funnel, along with the extraction of the aqueous layer three times into a clean and labeled 100–mL
beaker. As in the previous step an addition of 5 mL of deionized water was used in the final
extraction step. The extracted solution was also saved for later in the experiment as was the ether
layer remaining in the separatory funnel. 3 The retained solution from the NaHCO3 extraction was
used to precipitate the P–toulic acid. Drop wise 3M HCl was added to the extracted solution
carefully until no more precipitate was formed and the solution tested acidic, with a pH reading less
than 3 as indicated by pH paper testing. A piece of clean filter paper was then weighed and the mass
recorded in a lab notebook. A vacuum filtration system was constructed with a Buchner funnel

Tonic Water Cornstarch Procedure
RESEARCH
"Magic Mud" is mainly a mixture of a dusty substance known as "Cornstarch", and a liquid known
as "Tonic Water". When you apply pressure to the substance of Magic Mud, it will act as if it were a
solid. Once you stop applying pressure to it, the substance will act as if it were a liquid. To make this
happen you should apparently mix tonic water and cornstarch for a long period of time to allow this
chemical reaction to occur. What I wanted to know is if this would still be possible if I replaced
tonic water for a very reliable source that everyone that owns a house has; which is regular water
When the cornstarch is mixed with tonic water for a long period of time, instead of dissolving as if
you were making Kool–Aid. The substance will not dissolve, and as a result will form a suspension.
A suspension is when a substance does not dissolve, due to this the solid particles (from the
cornstarch) are freely moving around IN THE INSIDE, while the liquid particles (from the tonic
water) are staying IN THE OUTSIDE of the substance.
RESEARCH CONT.
This makes sense, since at first glance the mixture of Magic Mud seems like a liquid, but once you
dig your hand into the mixture you can actually feel the substance as a solid when you apply
pressure, but once you stop ... Show more content on Helpwriting.net ...
Magic Mud behaves as a non–Newtonian fluid, because when it is shocked or in other words
pressure is applied. Most of the water runs through the grains of cornstarch, due to this cornstarch
particles that were left behind were there to act as a solid when enough pressure was applied. As
soon as the pressure is released, the water particles flow back through the grains, and as a result the
mixture started acting as a liquid again. According to scientists, there are apparently two theories
proposing the reason why thickening in Magic Mud

Naphthalene Inhalation Study
Risk Assessment 1. Naphthalene is a white organic solid compound with a distinctive odor (ATSDR,
2005). Numerous results from the animal studies showed that naphthalene is potentially considered
to be a human carcinogen. The studied indicated the fast absorption of naphthalene by inhalation,
oral and dermal administration (22–73%; up to 84%; 50% respectively) (Preuss et al., 2003).
Distribution of naphthalene occurs at fairly rapid rate without significant accumulation in body
tissues (Preuss et al., 2003). Once absorbed, naphthalene undergoes metabolic activation and
conjugation (Preuss et al., 2003). Naphthalene metabolites such as naphthoquinones prompt reactive
oxygen species production that ultimately leads to DNA damage and carcinogenic transition of cells
(Preuss et al., 2003). The US National Toxicology Program (NTP) reports indicate the results from
long–term inhalation study conducted on rats that showed notably increased incidence of lung and
nasal tumours (Preuss et al., 2003). Despite of the lack of human studies, the findings of the NTP
allowed to admit naphthalene as a potential human carcinogen (Preuss et ... Show more content on
Helpwriting.net ...
Average weight of an adult female of 66 kg is derived from the table "Average body weights, 1995
National Nutrition Survey". Thus, daily consumption of naphthalene from tap water for 66 kg
female is 700 µg / 66kg = 10.6 µg /kg /day. 3. The IRIS RfD totals 2E–2 mg/kg–day which converts
to 0.02 mg/kg/day or 20 µg/kg/day. The value of 10.6 µg/kg/day is far less than acceptable dose of
naphthalene established by the US EPA's IRIS program. Therefore, there should be no health
concern about naphthalene adverse effects and the tape water is safe for drinking. 4. According to
the US EPA naphthalene was designated to Group C as "possible human carcinogen" (Preuss et al.,
2003). This group includes chemicals with insufficient evidence of carcinogenicity in animals and
the absence or little human data (EPA,

Grignard Reagent Of Triphenylmethanol
Introduction:
Grignard reagents are form when an alkyl halide is treated with magnesium to have the form of R–
Mg–X. Grignard reagents are typically very strong nucleophiles because of the difference between
the carbon and magnesium's electronegativity. Alcohol typically is a result of a Grignard reaction.
The reaction involves reacting a Grignard reagent with a carbonyl. The purpose of this experiment is
to prepare a triphenylmethanol. The success of the experiment can be proved by comparing the
boiling point that is provided and by using the reading of an IR spectrum.
Procedure:
A. Preparation of Triphenylmethanol:
Reaction of Bromobenzene with Magnesium: 4 mmol of magnesium were weighed and left in the
round bottom flask. An apparatus was set up for the addition under reflux and a drying tube was
attached to the apparatus. 6 mL portion of anhydrous diethyl ether was transferred to a dry–4–dram
vial. Then, 4 mmol of dry bromobenzene was moved to a 3 mL conical vial and dissolved in a 1 mL
of anhydrous diethyl ether. The flask was detached momentarily to rub the magnesium pieces while
the flask was warmed by hand. 2 mL of diethyl ether was transferred to the bromobenzene conical
vial. The reaction was supposed to boil at that time, but nothing happened except for very few
bubbles. Then, ether was added to the reaction. The reaction was moved to a 40˚C water bath for
about 15 minutes.
Reaction of Phenylmagnesium Bromide with Benzophenone: A 3–mL conical vial was used to

A Brief Note On The Independent Research Project
Independent Research Project
Student's Number: _______________________________
VARIABLES:
Independent variable: substances– Sugar, Salt, kerosene, Margarine, Salicylic Acid, Vaseline
Dependent variable: whether it is soluble and creates an emulsion
Controlled variables: 1mL of substances Sugar, Salt, kerosene, Margarine, Salicylic Acid, Vaseline,
and 5mL of solvents Water, Vegetable oil, Ethanol, amount of swirls to mix around
 Independent variable identified
 Dependent variable identified
 Some control variables identified
 All control variables identified Total
/4
METHOD:
1. Gather all materials that are available from the above list.
2. Measure 5mL of a solvent (water) and pour into different test tubes 6 times using a measuring
cylinder.
3. Collect 1mL of each substance from the list (Sugar, Salt, kerosene, Margarine, Salicylic Acid, and
Vaseline) using a spatula.
4. Set one of the substances (i.e. Sugar) into one of the test tubes containing water.
5. Record observation of whether it dissolved or did not dissolve, in the results table below; and
repeat for the other 5 substances.
6. Pour the water in the test tubes containing the substances down the sink, EXCEPT the test tubes
containing kerosene and oil.
7. Clean test tubes with test tube cleaner and warm soapy water in the sink.
8. Dry the test tubes once cleaned and repeat experiment using vegetable oil then with ethanol.
9. Record results for each experiment and compare results with other

Environmental Impact And Sustainability Issues Related For...
Environmental Impact and Sustainability Issues related to PBDEs
In chapter fourteen of our textbook, Environment: The Science Behind The Stories, it is made clear
that the United States does not use the precautionary principle approach when it comes to evaluating
how toxic a substance is (Withgott & Laposata, 2014, p. 382). This lack of precaution has proven to
be dangerous when it comes to chemicals, especially when using polybrominated diphenyl ethers
(PBDEs). PBDEs are chemically engineered flame retardants used during the manufacturing process
of clothing, bedding, and many other household goods. These flame retardants work by eliminating
the fire's oxygen supply, resulting in less damage to the item and a decrease in the chance of a larger
fire (Hester & Harrison, 2013, p. 45). While PBDEs may have been necessary during a time when
there were fewer fire regulations, it is clear that the negative effects of these flame retardants
outweigh the benefits in today's times.
According to the journal of Environmental Science & Technology (2016), the toxicity of PBDEs
was first discovered in Sweden, when a study exposed an unsafe and increasing level of flame
retardants in the breast milk of women. This study showed that PBDEs were potentially toxic and
highly bioaccumulative, meaning that they accumulate in the body instead of being broken down.
PBDEs were identified as mutagens, as well as possible carcinogens. Because of these findings,
PBDEs were banned in some countries and

Grignard Reagent Lab Report
the purpose of this experiment is to prepare a Grignard reagent by reacting with alkyl or aryl halide
and to ultimately react the Grignard reagent with carbon dioxide in order to produce carboxylate.
The formed carboxylate is then protonated with an acid to produce carboxylic acid that could be
used with liquid–liquid extraction to isolate the unknown acid from the other products from side
reactions. The final unknown product is identified by measuring the melting point and calculating
the molecular weight obtained from titration.
Organometallic compounds are compounds that contain carbon–metal bonds (C–M bonds), in which
carbon bears a partial negative charge because metal is less electronegative than the carbon. This
partial negative charge of the carbon atom allows it to be a good nucleophile that attacks the
electrophile to make a new carbon–carbon bond. There are several examples of organometallic
compounds, such as organolithium, Gilman reagents, and Grignard reagents (organomagnesium
reagent). In this experiment, Grignard reagents are prepared and reacted with other electrophilic
carbon to form a new carbon–carbon bond. Victor Grignard discovered Grignard reagent around
1890s and received a Noble Prize in 1912 with his discoveries. In this experiment, an alkyl halide or
aryl halide is reacted with magnesium metal to prepare a Grignard reagent (R–MgX). In this
Grignard reagent preparation reaction, halide is typically used with bromine (sometimes with
chlorine, not

Grignard Reaction Process Of Phhenylmagenisum Bomide
DISCUSSION The aim of this experiment was to effectively carry out a Grignard reaction process
that uses Grignard reagent to synthesize alcohol and creates a new carbon–carbon bond within the
reaction. In this experiment, phenylmagenisum bromide is the Grignard reagent reacted with
benzaldehyde to synthesize the final product, diphenylmethanol (alcohol) close to its 100 %
theoretical yield. Diethyl ether solvent was used to keep away any water/moisture that could destroy
the Grignard reagent and react to form a hydrocarbon instead of an alcohol. Therefore, experiment
execution need a lot of precision and precautious to make sure that the apparatus used/reused as well
as the reaction itself is dry and away from water or moisture. There ... Show more content on
Helpwriting.net ...
This part of the experiment was carried out by mixture of 1.5 mL benzaldehyde in 4 mL dry diethyl
ether solution into the formed Grignard reagent dropwise through the Claisen adaptor of the
glassware–setup apparatus. These small droplets created a vigorous fizzing within the reaction
mixture and color change to light pinkish/reddish and very bad/strong smell was observed. These
vigorous fizzing in the reaction meant that the magnesium alkoxide salt has been formed when the
nucleophilic phenylmagenisum bromide reagent attacks the carbonyl benzaldehyde (electrophile).
This mixture was allowed to cool down for few minutes and 5 mL of cool water was added to
mixture along with dropwise of 6 mL of 20% HCl through Claisen adaptor. This created change the
color of the mixture as well as created two homogenous layers a white layer on top and yellowish
green layer on the bottom of round–bottom flask. This layered mixture was transferred and further
separated into the separator funnel to separate the aqueous layer and the ether layer by shaking the
mixture which helped to protonate the alkoxide salt and started to form the alcohol product. The
aqueous clear layer (bottom layer) was removed since it is the denser layer while less dense ether
layer was washed with water and saturated sodium bisulphite solution. This part is crucial as use of
sodium bisulphite was done to wash out all the acid from ether layer so that there is

Benzophenone Lab Report
Abstract
Bromobenzene was reacted with Magnesium and anhydrous ether to create a Grignard reagent.
Benzophenone was added to the reagent in order to produce triphenylmethanol. The final product's
melting point was measured at 40.5–44°C; too low to be triphenylmethanol. The final product was
determined to be benzophenone, indicating that no reaction occurred. Grignard reagents were likely
deactivated by water, causing the reaction to not occur.
Introduction1,2,3
This experiment was designed to work with the preparation and use of Grignard reagents1. Grignard
reagents are used in reactions to create new carbon–carbon bonds between structures2. For this
experiment, the Grignard reagent used was magnesium bromide1. The magnesium bromide
substituent was added to bromobenzene to make it ... Show more content on Helpwriting.net ...
Observations and Results
A heating mantle and variac were set up for a 50 ml round bottom flask. 1.5g of p–bromo–n,n–
dimethylaniline was measured under the hood and placed into the flask. 2.5ml of anhydrous ether
was used to dissolve the bromobenzene, which was mixed with 0.27 g of magnesium. This solution
was mixed by using a magnetic stir rod until bromobenzene and magnesium were completely
dissolved.
Separately, 20.0 mmol of benzophenone was combined with 10 ml of anhydrous ether. The mixture
had a slightly layered appearance. Using a pipette dropper, drops of the benzophenone ether solution
were added to the original Grignard reagent solution. Drops were added slowly, contact caused a
slightly bubbling. This was heated using a reflux apparatus while the reaction took

3-Hexylthiophene Lab Report
Poly (3–hexylthiophene) Molecular Bottlebrushes via Romp Macromolecular Architecture
Enhanced Aggregation is a process, which uses the Grignard metathesis polymerization. Grignard
metathesis polymerization is a technique that uses a living chain growth mechanism in order to
produce the regioregular polymer poly (3–hexylthiophene). The synthesis demonstrates the addition
of poly (norbornene) backbone and rr–P3HT side chains. Grignard metathesis is conducted in order
to allow the polymerization of poly (3–hexylthiophene) to take place in a room temperature and to
decrease the cost and increase the efficiency of the technique. Poly (3–hexylthiphene) the product of
head to tail coupling is a class of polymers that maintain a great level of solubility, ... Show more
The reason for not reaching the goal was due to the loss of solvent during the reaction. A step in the
procedure was to reflux the reactant with the Tetrahydrofuran solvent and during the reflux process
the condenser wasn't attached properly, which thus caused the solvent to escape. Due to the reduced
level of moisture the reaction didn't perform properly. Also, when the product was measured under
the mass spectrometry the molecular weight of the product didn't match up to the expected results
and this thus indicates the presence of impurities in the product. The reaction was repeated second
time in order to avoid the mistakes and to produce a greater amount of the product. This time the
reaction was performed during the day and insight in order to avoid any error that may cause if the
reaction is continued into the night. We also made sure the reaction was given the exact amount of
time nothing more or nothing less than the required amount to avoid any side reactions and any
mishap from occurring. At the end of the reaction we produced three grams of product with no sign
of impurity indicated through the

Grignard Lab
A Grignard–Like Organic Reaction
The Synthesis of 1–phenyl–3–buten–1–ol
Introduction
The Grignard reaction is an important synthetic process by which a new carbon to carbon bond is
formed. Magnesium metal is first reacted with an organic halide forming the Grignard reagent. The
Grignard reaction is the addition of an organomagnesium halide (Grignard reagent) to a ketone or
aldehyde, to form a tertiary or secondary alcohol, respectively. For example, the reaction with
formaldehyde leads to a primary alcohol. Grignard Reagents are also used in the following
important reactions: The addition of an excess of a Grignard reagent to an ester or lactone gives a
tertiary alcohol in which two alkyl groups are the same, and the addition of a ... Show more content
on Helpwriting.net ...
The reaction is carried out in saturated aqueous ammonium chloride solution. Thus no special drying
of solvents, reagents, or glassware is required. The reaction mechanism for this experiment can be
seen below (Fig. 2)
DATA | | | | | | Obtained Values | | | | | | Weight of Zinc powder | 0.165 g | | | | | Volume of NH4Cl (aq) |
1.0 mL | | | | | Volume of Benzaldehyde | 0.105 mL | | | | | Volume of THF | 0.5 mL | | | | | Volume of
Allyl Bromide | 0.205 mL | | | | | Weight of Final Product | 0.0514 g | | | | | | | | | | | Percent Yield * | | | | |
| Compound | Expected | Actual | % | | | 1–phenyl–3–buten–1–ol | 0.153 g | 0.0514 g | 33.60% | | | | | | |
| | TLC | | | | | | solvent system: 30% ether–hexane | | | | | Compound | Rf Value | | | | | Benzaldehyde |
0.75 | | | | | 1–phenyl–3–buten–1–ol | 0.25 | | | | | | | | | | | * Please see calculation section Fig. 3 for
further details. | | | | | | | | | | | | | | | Density (g/cm3) ++ | | | Formula Weight (g/mol) ++ | Compound | | |
Zinc | 65.38 | | Benzaldehyde | 1.04 | | Benzaldehyde | 106.12 | | 1–phenyl–3–buten–1–ol | 0.992 | |
Allyl Bromide | 120.99 | | NH4Cl (aq) | 1.53 | | 1–phenyl–3–buten–1–ol | 148.2 | | THF | 0.8892 | |
Allyl Zinc Bromide | 186.37 | | Allyl Bromide | 1.40 | | | | | Diethyl Ether | 0.7134 | |

Grignard Reaction Lab
The Grignard Reaction
Huzaifa Amjad, Maitlyn Mullen, Sebastian Eady
Introduction:
A Grignard reagent is an extremely reactive chemical compound used in the synthesis of
hydrocarbons, alcohols, carboxylic acids, and other compounds (1). Grignard reagents have a
formula of RMgX, where R is an alkyl or aryl group and X is a halogen. The balanced equation is
shown below in Equation 1. 2RMgX  R2Mg + MgX2 Eq. 1
Grignard reagents form on the surface of metals. Most undergo reactions with ether (2). The reason
that the Grignard synthesis is so valuable is due to the fact that it can form carbon–carbon bonds
from carbon nucleophiles. Some of ... Show more content on Helpwriting.net ...
In the Grignard reagent the polarity changes as the partial negative charge is placed on the carbon
atom. This is due to the carbon atom being attached to a very electropositive metal atom,
magnesium. This makes the carbon atom act as a carbanion leading to the availability of a
nucleophile (3). In order to use a Grignard reagent to make the carbon–carbon bonds, there must be
absolutely minimal moisture in the surrounding environment as well as in the glassware in which
the experiment is conducted (1). The reason for this is because the partially negative R group on the
Grignard reagent is a strong base and will react with weak acids like water. Once the Grignard
reagent reacts with water it will form a carbon–hydrogen bond and will not form a carbon–carbon
bond. This is why all glassware is being placed in an oven to dry. The Grignard reaction mechanism
is shown in figure 2. Figure 2. Grignard reaction mechanism, the bond between the carbon and
magnesium attached tot eh carbon with the oxygen double bond. In the end the carbon is attached to
three benzene

Solid Phase Of Polymer Bound 2
A 1,3,4–thiadiazole library was constructed by solid–phase organic synthesis. The key step of this
solid–phase synthesis involves the preparation of polymer–bound 2–amido–5–amino–1,3,4–
thiadiazole resin by the cyclization of thiosemicarbazide resin using p–TsCl as the desulfurative
agent, followed by the functionalization of resin by alkylation, acylation, alkylation/acylation, and
Suzuki coupling reaction. Both the alkylation and acylation reactions chemoselectively occurred at
the 2–amide position of 2–amido–5–amino–1,3,4–thiadiazole resin and the 5–amine position of 2–
amido–5–amino–1,3,4–thiadiazole resin, respectively. Finally, these functionalized 1,3,4–thiadiazole
resins were treated with trifluoroacetic acid in dichloromethane, ... Show more content on
Helpwriting.net ...
Lee et al. compared the binding affinity of compounds containing 1,3,4–oxadiazole or 1,3,4–
thaidiazole in the same chemical structure toward CB1 receptor in the process of development of
obesity drug.9 Both 1,3,4–oxadiazoles and 1,3,4–thiadiazoles were also used for the development
potent antibacterial agent by Kumar et al.10 Asai et al. reported dramatic difference in the binding
affinity between 1,3,4–oxadiazole and 1,3,4–thiadiazole toward signal transducers and activators of
transcription.11 Because of these biologically interesting properties of 1,3,4–thiadiazole and 1,3,4–
oxadiazole, these core skeletons have been targeted for synthesis by organic and medicinal chemists,
and as a result, many synthetic methodologies have been developed in the literature.12 Among these
synthetic methodologies, solid–phase synthesis effectively facilitates the generation of various
1,3,4–thiadiazoles and 1,3,4–oxadiazoles in a short time.13 In our own research area, we have
developed solid–phase synthetic methodology to produce 1,3,4–oxadiazoles and 1,3,4–
thiadiazoles.14 However, unfortunately our methodology was limited to synthesize diverse 1,3,4–
thiadiazole derivatives. It was only suitable to generate p–nitro substituted 1,3,4–thiadiazoles
(Scheme 1a). To improve over

Synthesis Of 1-Bromobutane Lab Report
The Williamson Ether Synthesis reaction carried out in this experiment involved the substitution
reaction of the compounds sodium ethoxide and 1–bromobutane under reflux conditions to yield the
products 1–ethoxybutane and sodium bromide. Several wet–bench chemistry techniques were
utilized throughout the process, and these included reflux, extraction and washing, as well as short
path distillation. These techniques allowed for the reaction to proceed faster and allowed for the
separation and extraction of the product of interest, 1–ethoxybutane. Here, reflux allowed for the
solvent to be recycled in heating the reaction mixture, extraction and washing allowed for the
product of interests to be extracted into the diethyl ether layer and for the undesired products to be
washed out, and short–path distillation allowed for the separation of ether and 1–ethoxybutane due
to large differences ... Show more content on Helpwriting.net ...
Many organic reactions are long and utilize a solvent that is generally volatile. Under these
conditions, the solvent can easily evaporate and be lost to the air and it is inefficient to continuously
replenish the solvent concentration. Reflux allowed for the solvent to be conserved and recycled
because the gas vapors produced from when the solvent boiled with the addition of heat condensed
and fell back into the flask. This recycled the solvent and ensured it was not lost. Additionally, the
temperature at which reflux occurs is generally near the boiling point of the solvent, and indicates
that the reaction can proceed for 55 more minutes, a much shorter duration than the actual reaction
time. For example, the refluxing temperature in this experiment was nearly 89 degree Celsius, which
is close to the boiling point of ethanol of 90 degrees Celsius. Thus, reflux allowed for the
conservation of the solvent and for the reaction to be run at shorter

Grignard Synthesis of Triphenylmethanol Lab Report Essay
The Grignard Synthesis of Triphenylmethanol Organic Chemistry Lab II March 19, 2012 Abstract
The purpose of this experiment was to synthesize the Grignard reagent, phenyl magnesium bromide,
and then use the manufactured Grignard reagent to synthesize the alcohol, triphenylmethanol, by
reacting with benzophenone and protonation by H3O+. The triphenylmethanol was purified by
recrystallization. The melting point, Infrared Spectroscopy, 13C NMR, and 1H NMR were used to
characterize and confirm the recrystallized substance was triphenylmethanol. Introduction A
Grignard reagent is a type of organometallic, which consists of a bond between a metal and a
carbon. There are three types of carbon–metal bonds: ionic, polar covalent, and ... Show more
Grignard reagents also react with the least hindered carbon on an epoxide to break the ring in order
to relieve ring strain. A reaction of the Grignard reagent and carbon dioxide results in an acid, and
reaction of a nitrile and a Grignard reagent produce a carbonyl via an imine intermediate. These are
show below, respectively. Grignard reagents are reactive enough to also attach esters; however, two
equivalents of the Grignard reagent are usually added because less then two equivalents leave a
large quantity of unreactive ester. This reaction forms a tertiary alcohol. Grignard reagents cannot be
synthesized from alcohols because instead of reacting with the halide to form the Grignard reagent,
the alcohol is deprotenated. Grignard reagents also cannot be synthesized from molecules with a
carbonyl group. Solvent choice is important in Grignard reagent formation. The solvent must be
non–reactive with a negatively charged carbon (ex. acetone or anything even slightly acidic), and
the solvent cannot have a carbonyl group. The solvent must be a volatile solvent that provides a
blanket of solvent over the reaction solution so that oxygen and moisture in the air are excluded
from the reaction. Oxygen and moisture in the air are very slightly acidic and would disrupt the
synthesis of a Grignard reagent. Anhydrous ether (R2O) is often used as a solvent in creating
Grignard reagents because it keeps out water and oxygen, makes the

Our Experiment to Separate a Mixture of Organic Compounds...
Purpose/Introduction
What were we trying to accomplish with this experiment? What method did we implement to
accomplish the task? What techniques were used to purify and identify the product(s) of the
reaction? In this experiment, an acid–base extraction was done to separate a mixture of an unknown
acid and fluorene, a neutral compound. The possible unknown acids were 2–chlorobenzoic acid, 3–
chlorobenzoic acid, and 3–methylbenzoic acid. The purification of the isolated unknown acid was
performed by recrystallization and its identity was established by analyzing the melting point range
of the pure product and comparing it to the provided standards. In addition, a mixed melting point
experimentation enhanced the fidelity of the unknown's ... Show more content on Helpwriting.net ...
Initially, the organic carboxylic acid becomes a charged species after it is deprotonated by a base
like sodium hydroxide, producing a carboxylic salt. After completing the extraction, an acid, such as
hydrochloric acid, is added to the basic aqueous solution causing the sodium carboxylate salt to
change back to the default carboxylic acid, which will precipitate out of solution since it is water
insoluble. Recrystallization is a technique when a solute is dissolved in a hot solvent (destruction of
the impure crystal lattice) and is then precipitated out of solution as the solvent is immediately
cooled (selectively producing a purer lattice). The unknown acid was recrystallized using hot water
followed by hot ethanol in order to dissolve the solid, followed by cooling which resulted in the
precipitation of the desired product. Afterward, melting point experimentation was used to match the
melting point data of the unknown acid with the provided standards of the known acids. If there is a
melting point depression, one has acted as an impurity to the other compound. In contrast, if there is
no noticeable decrease in melting point relative to the two separate compounds; it is safe to say that
they are the same substance.
Reaction:
Results
What was the unknown identity of the acid after conducting melting point

Synthesis Of Grignard Reagent And Benzaldehyde
Introduction: This experiment involved the synthesis of diphenylmethanal from phenylmagnesium
bromide which is a Grignard reagent, and benzaldehyde which is a carbonyl group. The goal of this
experiment was to investigate the ability of the Grignard reaction to yield the theoretical predicted
product and evaluate its efficiency. The Grignard reaction is an important reaction because of its
ability to allow the formation of carbon–carbon bonds. These formations of C–C sigma bonds, then
allow for the formation or making of large or complex synthetic molecules from very simple
reagents. These complex molecules are then used in many different areas such as the pharmaceutical
industry. Also, one must note that Grignard reagents are strong nucleophiles that can attack carbonyl
groups that can form substituted alcohols after the protonation step. The reaction occurred as
follows. The first step consisted in the formation of the Grignard reagent. That was done through the
use of an organic halide provided in the lab and Magnesium. The organic halide used was
bromobenzene. The second step consisted of reacting the Grignard reagent formed in the first step
with benzaldehyde. The third and final step consisted of using the product of the second step and
diluting it with HCl (Hydrochloric Acid). Finally, the product obtained of this whole reaction was
diphenylmethonal ( please refer to the drawing below for a more visual approach). The creation of
this product can also be

The Grignard Synthesis of Triphenylmethanol
Abstract: The purpose of this lab was to synthesize triphenylmethanol from benzophenone and
bromobenzene by the formation of a Grignard compound with the reagents bromobenzene and
magnesium metal. The bromobenzene was first transformed into the Grignard compound and was
then reacted with the benzophenone to make the final product. The mixture was then mixed with
sulfuric acid and the organic layer was extracted via a separatory funnel. The mixture was then
recrystallized from methanol and was allowed to dry and the percent yield, melting point, and the IR
was obtained. The mass of the product obtained was 5.45 grams and the percentage yield was
determined to be 41.95%. The melting point range obtained from the final product was 89–91°C ...
Show more content on Helpwriting.net ...
5.3 mL of bromobenzne and 15 mL of anhydrous ether was then placed into the separatory funnel
and was shaken and vented in order to mix the solution. Half of the bromobenzene solution was
added first into the round bottom flask and as soon as a color change was observed, the remaining
half of the bromobenzene was added drop wise into the round bottom flask. The mixture was then
refluxed on a heating mantle for 10 minutes until most of the magnesium has been consumed. After
the initial mixture has refluxed, 9.11 grams of benzophenone was dissolved in 100 mL of anhydrous
ether in a beaker and was then transferred into the separatory on the reflux apparatus. This solution
was then added to the Grignard reagent at a drop wise rate while stirring. After the benzophenone
was added, the mixture was then refluxed for 15 minutes on a heating mantle. After the mixture
finished refluxing, the flask was then cooled on ice. A sulfuric acid solution was then prepared by
pouring 4.5 mL of concentrated H2SO4 over 50 grams of ice and then diluted to 75 mL by adding
enough tap water to reach 75 mL. The sulfuric acid solution was then cooled on ice. The Claisen
adapter was then removed from the 250 mL round bottom flask and the condenser was then attached
to the top of the round bottom flask which was then put on ice. The sulfuric acid solution was then
poured through the condenser in order to protonate the product. A stirring rod was then used to
dislodge any solid that was stuck to

The Dangers Of Inhalants Among Adolescents

Recommandé

Recommandé

Contenu connexe

Plus de Tara Smith

Plus de Tara Smith (20)

Dernier

Dernier (20)

The Dangers Of Inhalants Among Adolescents