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Organic Chemistry - Blog Posts
Here is a summary for Diels Alder for Ochem:
Crash Course: The Basics of Organic Nomenclature: Crash Course Organic Chemistry #2
Language is complicated, especially in organic chemistry. This episode of Crash Course Organic Chemistry is all about nomenclature. We’ll dive into IUPAC systematic naming of organic molecules, and get to practice with the help of three trusty steps!
D 1/100
•studied physical chemistry today.
•I have a paper tomorrow at university.
•Got in touch with one of my college friend.
Mannich reaction:Compound containing at least one active hydrogen atom, condenses with formaldehyde and primary or secondary amine or ammonia to give the product known as Mannich base.
Studied Chemistry for 100 days.
I am currently enrolled for Msc program.
Group theory-Inorganichemistry
Hi! Let me introduce myself I m Adil and I am doing Msc in chemistry.Its ist sem going on and we are studying Group theory in inorganic chemistry.
How is organic chemistry different from inorganic chemistry?
Difference between Organic and Inorganic chemistry. The key difference between the two is that organic chemistry deals with covalent compounds whereas inorganic chemistry is responsible for the study of mainly ionic compounds. The other differences are given in the table below.
What comes to mind when you think of alcohol? Probably alcoholic drinks like beer or wine. But in organic chemistry alcohols are an important and versatile family of compounds. In this episode of Crash Course Organic Chemistry, we’ll use alcohols as a starting point to get other types of compounds like ethers, epoxides, and more!
Alkanes: Crash Course Organic Chemistry #6:
Alkanes are kind of the wallflowers of organic chemistry, but they still have important functions in the world around us. In this episode of Crash Course Organic Chemistry we’re building our knowledge of organic molecules by learning all about these so called couch potatoes from how they are separated from crude oil to how to use Newman projections to predict torsional strain and steric hinderance. We’ll also learn the names of some common conformers and get an introduction to cycloalkanes.
Polarity, Resonance, and Electron Pushing: Crash Course Organic Chemistry #10:
We’ve all heard the phrase “opposites attract.” It may or may not be true for people, but it’s definitely true in organic chemistry. In this episode of Crash Course Organic Chemistry, we’re learning about electronegativity, polarity, resonance structures, and resonance hybrids. We’ll practice a very important skill for this course that will help us avoid a lot of memorization in the future: electron pushing. It’ll be a lot of trial and error at first, but we all start somewhere!
Breaking Down Alkanes - isn’t it cracking?
Unfortunately, if you’re sitting your A Level chemistry exam, you need to know a little more than the basic properties of alkanes outlined in my last post. Luckily though, this post takes you through fractional distillation and the two types of cracking - isn’t that convenient?
Crude oil contains carbon compounds formed by the effects of pressure and high temperature on plant and animal remnants. It is viscious, black and found in rocks beneath the earth’s surface. It is a mixture of mainly alkane hydrocarbons which are separated by a process called fractional distillation. Crude oil is essential because it is burned as a fuel and each fraction has different properties e.g. diesel, petrol, jet fuel.
Fractional distillation is the continual evaporation and condensation of a mixture which causes fractions to split due to a difference in boiling point. It is important to note that fractional distillation does not separate crude oil into pure compounds but rather less complex mixtures. Fractions are groups of compounds that have similar boiling points and are removed at the same level of a fractionating column.
The first step in this process is to heat crude oil in a furnace until some changes state from a liquid to a vapour. This mixture goes up a fractionating tower or column which is hotter at the bottom than the top and reaches a layer which is cool enough to condense and be collected. Shorter chain molecules are collected at the top where it is cooler since they have lower boiling points.
As you go down the fractionating column, bear in mind that: the column temperature increases, the boiling point increases, the number of carbon atoms increases and the strength of the Van der Waals’ between molecules increases.
Different fractions have different usefulnesses and often, it is the fractions with lower boiling points and shorter chains which are much more purposeful. Therefore there needs to be a process to getting shorter chains because they are the least abundant in crude oil samples. To meet demand, long chain molecules that are less useful are broken down into shorter chain molecules. This is done by cracking.
Cracking is a process where long chain hydrocarbon molecules are broken down into shorter chain molecules which are in high demand. This can be done one of two ways - thermal or catalytic.
Thermal cracking involves heating long chain alkanes to high temperatures - usually between 1000 - 1200K. It also uses high pressures up to 70atm and takes just one second. It only needs a second because the conditions could decompose the molecule completely to produce carbon and hydrogen instead. The conditions produce shorter chain alkanes and mostly alkenes.
A typical equation for this:
Decane -> octane + ethene
C10H22 -> C8H18 + C2H4
Catalytic cracking also breaks down long alkanes by heat under pressure using the presence of a zeolite catalyst. Temperature used is approx. 800-1000K and the pressure is often between 1-2 atm. Zeolite is an acidic mineral with a honeycomb structure, made from aluminium oxide and silicion dioxide. The honeycomb structure gives the catalyst a larger surface area which increases ROR. Factories which catalytically crack are often operated continuously for around 3 years at a time and produce branched alkanes, cycloalkanes and aromatic compounds.
You need to be able to compare the conditions of catalytic and thermal cracking for the A Level exam. Know that thermal cracking has a high temperature and pressure, a short duration, no catalyst and produces a high percentage of alkenes and some short chain alkanes. Catalytic uses a catalyst, a high temperature, a low pressure and produces aromatic hydrocarbons and motor fuels.
SUMMARY
Crude oil contains carbon compounds formed by the effects of pressure and high temperature on plant and animal remnants. I It is a mixture of mainly alkane hydrocarbons which are separated by a process called fractional distillation.
Fractional distillation is the continual evaporation and condensation of a mixture which causes fractions to split due to a difference in boiling point.
It is important to note that fractional distillation does not separate crude oil into pure compounds but rather less complex mixtures.
Fractions are groups of compounds that have similar boiling points and are removed at the same level of a fractionating column.
The first step in this process is to heat crude oil in a furnace until some changes state from a liquid to a vapour. This mixture goes up a fractionating tower or column which is hotter at the bottom than the top and reaches a layer which is cool enough to condense and be collected. Shorter chain molecules are collected at the top where it is cooler since they have lower boiling points.
As you go down the fractionating column, bear in mind that: the column temperature increases, the boiling point increases, the number of carbon atoms increases and the strength of the Van der Waals’ between molecules increases.
Fractions with lower boiling points and shorter chains are much more purposeful but are the least abundant in crude oil samples. To meet demand, long chain molecules that are less useful are broken down into shorter chain molecules.
Cracking is a process where long chain hydrocarbon molecules are broken down into shorter chain molecules which are in high demand.
Thermal cracking involves heating long chain alkanes to high temperatures - usually between 1000 - 1200K. It also uses high pressures up to 70atm and takes just one second. It only needs a second because the conditions could decompose the molecule completely to produce carbon and hydrogen instead. The conditions produce shorter chain alkanes and mostly alkenes.
Catalytic cracking also breaks down long alkanes by heat under pressure using the presence of a zeolite catalyst. Temperature used is approx. 800-1000K and the pressure is often between 1-2 atm. Zeolite is an acidic mineral with a honeycomb structure, made from aluminium oxide and silicion dioxide. The honeycomb structure gives the catalyst a larger surface area which increases ROR.
You need to be able to compare the conditions of catalytic and thermal cracking for the A Level exam. Know that thermal cracking has a high temperature and pressure, a short duration, no catalyst and produces a high percentage of alkenes and some short chain alkanes. Catalytic uses a catalyst, a high temperature, a low pressure and produces aromatic hydrocarbons and motor fuels.
Happy studying!
Alkanes: Saturated Hydrocarbons
So you want to be an organic chemist? Well, learning about hydrocarbons such as alkanes is a good place to start…
Alkanes are a homologous series of hydrocarbons, meaning that each of the series differs by -CH2 and that the compounds contain carbon and hydrogen atoms only. Carbon atoms in alkanes have four bonds which is the maximum a carbon atom can have - this is why the molecule is described to be saturated. Saturated hydrocarbons have only single bonds between the carbon atoms.
The general formula of an alkane is CnH2n+2 where n is the number of carbons. For example, if n = 3, the hydrocarbon formula would be C3H8 or propane. Naming alkanes comes from the number of carbons in the chain structure.
Here are the first three alkanes. Each one differs by -CH2.
Shorter chain alkanes are gases at room temperature, medium ones are liquids and the longer chain alkanes are waxy solids.
Alkanes have these physical properties:
1. They are non-polar due to the tiny difference in electronegativity between the carbon and hydrogen atoms.
2. Only Van der Waals intermolecular forces exist between alkane molecules. The strength of these increase as relative molecular mass increases therefore so does the melting/boiling point.
3. Branched chain alkanes have lower melting and boiling points than straight chain isomers with the same number of carbons. Since atoms are further apart due to a smaller surface area in contact with each other, the strength of the VDWs is decreased.
4. Alkanes are insoluble in water but can dissolve in non-polar liquids like hexane and cyclopentane. Mixtures are separated by fractional distillation or a separating funnel.
The fractional distillation of crude oil, cracking and the combustion equations of the alkanes will be in the next post.
SUMMARY
Alkanes are a homologous series of hydrocarbons. Carbon atoms in alkanes have four bonds which is the maximum a carbon atom can have - this is why the molecule is described to be saturated. Saturated hydrocarbons have only single bonds between the carbon atoms.
The general formula of an alkane is CnH2n+2 where n is the number of carbons.
Shorter chain alkanes are gases at room temperature, medium ones are liquids and the longer chain alkanes are waxy solids.
They are non-polar.
Only Van der Waals intermolecular forces exist between alkane molecules. The strength of these increase as relative molecular mass increases therefore so does the melting/boiling point.
Branched chain alkanes have lower melting and boiling points than straight chain isomers with the same number of carbons.
Alkanes are insoluble in water but can dissolve in non-polar liquids like hexane. Mixtures are separated by fractional distillation or a separating funnel.
Nomenclature - what in the organic chemistry is it?
Organic chemistry is so widely studied it requires a standard system for naming compounds, developed by IUPAC. Nomenclature is simply naming these organic compounds.
So, you want to be an organic chemist? Well, it starts here. Are you ready?
(psst… once you’ve learnt this theory, try a quiz here!)
1. Count your longest continuous chain of carbons.
Bear in mind that some chains may be bent. You’re looking for the longest chain of subsequent carbon atoms. This number correlates to root names that indicate the carbon chain length, listed below:
The second part of naming your base comes from the bonding in the chain. Is it purely single bonds or are there double bonds in there? If you are familiar with carbon chemistry, you’ll know that saturated hydrocarbons are called alkanes and unsaturated hydrocarbons are called alkenes. Therefore, the syllable -ane is used when it has only single bonds and the syllable -ene is used when it has some double bonds. For example:
Sometimes carbon chains exist in rings rather than chains. These have the prefix of -cyclo.
2. Identify your side chains attached to this main carbon and name them.
Side chains are added as prefixes to the root names. Sometimes called substituents, these are basically anything that comes off the carbon chain. Examples of the prefixes are listed below:
There are other prefixes such as fluoro (-F) and chloro (-Cl) which can describe what is coming off the chain.
3. Identify where each side chain is attached and indicate the position by adding a number to the name.
We aim to have numbers as small as possible. For example, if bromine is on the second carbon of a 5-carbon saturated chain, we number it as 2-bromopentane instead of 4-bromopentane, since it would essentially be 2-bromopentane if it was flipped. Locant is the term used for the number which describes the position of the substitute group, e.g. the ‘2′ in 2-chlorobutane is the locant.
Sometimes there are two or more side chains e.g. a methyl group and a chlorine attached to a pentane. In these cases, these rules apply:
1. Names are written alphabetically.
2. A separate number is needed for each side chain or group.
3. Hyphens are used to separate numbers and letters.
This would be named 2-chloro-3-methyl-pentane. This is because the longest chain of carbons is 5 (pentane), the chlorine is on the second carbon (2-chloro) and the methyl group is on the third carbon (3-methyl). It is 2-chloro rather than 4-chloro as we aim to have as small as numbers as possible.
Another variation of this step to be aware of is how many of the same side chains or groups there are, for example, having two methyl groups would be dimethyl rather than solely methyl. Each group must also be given numbers separated by commas to show where each one is located.
The list of these prefixes is found here:
Convention does not usually require mono- to go before a single group or side chain.
4. Number the positions of double bonds if applicable.
Alkenes and other compounds have double bonds. These must be indicated with numbers. For example, pent-2-ene shows that the double bond is between carbon 2 and carbon 3. The number goes in the middle of the original root name e.g. butene, pentene.
(!) Below is a list of functional groups that you may need to study for the AS and A Level chemistry exams. “R” represents misc. carbons. It is important to know that some groups are more prioritised than naming. From the most to least priority: carboxylic acid, ester, acyl chloride, nitrile, aldehyde, ketone, alcohol, amine, alkene, halogenalkane. It is worthwhile learning these.
bigger version here (I suggest downloading and printing it)
But wait, there’s more:
Here are some things to bear in mind when naming organic compounds:
1. The letter ‘e’ is removed when there are two vowels together e.g. propanone rather than propaneone. The ‘e’ isn’t removed when it is next to consonant, e.g. propanenitrile isn’t propannitrile.
2. When compounds contain two different, one is named as part of the unbranched chain and the other is named as a substituent. Which way round this goes depends on the priority.
SUMMARY
Count your longest continuous chain of carbons.
Chains may be bent. You’re looking for the longest chain of subsequent carbon atoms. This number correlates to root names that indicate the carbon chain length, e.g. pentane.
The second part of naming your base comes from the bonding in the chain. Is it purely single bonds or are there double bonds in there? The syllable -ane is used when it has only single bonds and the syllable -ene is used when it has some double bonds.
Rings have the prefix of -cyclo.
Identify your side chains attached to this main carbon and name them.
Side chains are added as prefixes to the root names. Sometimes called substituents, these are basically anything that comes off the carbon chain.
There are other prefixes such as fluoro (-F) and chloro (-Cl) which can describe what is coming off the chain.
Identify where each side chain is attached and indicate the position by adding a number to the name.
We aim to have numbers as small as possible. Locant is the term used for the number which describes the position of the substitute group, e.g. the ‘2′ in 2-chlorobutane is the locant.
Sometimes there are two or more side chains e.g. a methyl group and a chlorine attached to a pentane. In these cases, names are written alphabetically, a separate number is needed for each side chain or group and hyphens are used to separate numbers and letters.
When there are two or more of the same side chains or substituent groups, these must also be given numbers separated by commas to show where each one is located.
Number the positions of double bonds if applicable.
Alkenes and other compounds have double bonds. These must be indicated with numbers. The number goes in the middle of the original root name e.g. butene, pentene.
It is worthwhile learning the other functional groups that can be added on.They have varying priorities.
The letter ‘e’ is removed when there are two vowels together e.g. propanone rather than propaneone. The ‘e’ isn’t removed when it is next to consonant, e.g. propanenitrile isn’t propannitrile.
When compounds contain two different, one is named as part of the unbranched chain and the other is named as a substituent. Which way round this goes depends on the priority.
Happy studying guys!
Haloalkanes and Their Angelic Reactions: Part One
Haloalkanes are more commonly referred to as halogenoalkanes. Obviously you’ve already read my post on halogenoalkanes and their properties so there’s no surprise that you’re itching to read what I’ve got to say about these beauties and their reactions! Should we delve in?
There are a few different kinds of reactions you must learn for the A Level exam that involve halogenoalkanes.
The first is the synthesis of chloroalkanes via the photochemical chlorination of the alkanes. I know it looks scary, but don’t worry, it is simpler than it sounds. It essentially means “forming chloroalkanes through chlorinating an alkane in the presence of sunlight”.
Chlorine will react with methane when UV light is present and will form several kinds of chloroalkanes and fumes of hydrogen chloride gas. Chloromethane was once commonly used as a refridgerant. Depending on how many chlorine molecules there are, there will be different compounds formed:
methane + chlorine -> chloromethane + hydrogen chloride
CH4 + Cl2 -> CH3Cl + HCl
or
methane + chlorine -> trichloromethane + hydrogen chloride
CH4 + 3Cl2 -> CHCl3 + 3HCl
When undergone in real life, mixtures of halogenoalkanes are produced with some long chain alkanes which can be separated out with fractional distillation.
To understand what happens in an overall chemical reaction, chemists use mechanisms. These basically show the step-by-step process that is usually shown by a simple symbol equation that summarises everything.
The chlorination of methane is something you must learn the mechanism for. It’s pretty easy but involves a lot of steps and must be revised periodically to remember them.
The actual reaction is a substitution reaction because one atom or group is replaced by another. Since the chlorine involved is a free radical, it can also be called a free-radical substitution reaction.
1. Initiation
UV light is essential for the first step in the mechanism. This breaks the Cl-Cl covalent bond so that each chlorine leaves with one electron from the shared pair. Chlorine free radicals, with one unpaired electron in the outer shell, are formed. Free radicals are only formed if a bond splits evenly - each atom getting one of the two electrons. The name given to this is homolytic fission.
2. Propagation
This has two sub-steps
(a) Chlorine free radicals (highly reactive) react with methane to form hydrogen chloride and leave a methyl free radical.
Cl• + CH4 -> HCl + •CH3
(b) This free radical then reacts with another chlorine to form chloromethane and another chlorine free radical. Producing free radicals is a chain reaction which is why it is such a problem in ozone depletion - a little amount can cause a lot of destruction.
•CH3 + Cl2 -> CH3Cl + •Cl
3. Termination
This step stops the chain reaction. It only happens when two free radicals collide to form a molecule in several ways:
Cl• + Cl• -> Cl2
UV light would just break down the chlorine molecule again, so although this is technically a termination reaction it is not the most efficient.
Cl• + •CH3 -> CH3Cl
Forming one molecule of methane uses one chlorine and one methyl free radical.
•CH3 + •CH3 -> C2H6
Ethane can be formed from two methyl free radicals - this is why there are longer chain alkanes in the mixture.
This whole process is how organic halogenoalkanes are the product of photochemical reactions of halogens with alkanes in UV light - made via free radical substitution mechanisms in chain reaction.
Another reaction you need to know is a nucleophilic substitution reactions. A nucleophile is an electron pair donor or proton acceptor - the name comes from Greek origins (”loves nucleus”) - such as hydroxide ions, cyanide ions or ammonia molecules. Hydroxide and cyanide ions are negative but ammonia is neutral.
Halogenoalkanes have a polar bond because of the difference between the highly electronegative halogen and the carbon atom. The 𝛿+ carbon can go under nucleophilic attack. The mechanism for negatively charged nucleophiles these in general is:
Nu represents the nucleophile. This example is with a bromoalkane. Make sure to include curly arrows that begin at a lone pair or the centre of a bond and end at an atom or centre of bond, and delta (slight) charges.
Lets look at a more specific example:
One nucleophile that can be used is a hydroxide ion, found in either water or sodium hydroxide. In this case, you need to know about aqueous sodium hydroxide or potassium hydroxide and a halogenoalkane. This takes place at room temperature but is slow so is often refluxed (continuously boiled and condensed back into the reaction flask). Reflux apparatus is shown below:
The halogenoalkane is dissolved into ethanol since it is insoluable in water and this solution along with the aqueous hydroxide can mix. The product produced is an alcohol, which is organic.
The general reaction is:
R-CH2X + NaOH -> CH3CH2OH + NaX
Where X represents a halogen.
You must learn the mechanism for this reaction. The lone pair on the hydroxide attacks the carbon atom attached to the halogen and this causes both carbon electrons to move to the halogen which becomes a halide ion.
The reaction of a hydroxide ion can also be classed as a hydrolysis reaction as it breaks down chemical bonds with water or hydroxide ions. The speed of reaction depends on the strength of the bond - a stronger carbon-halogen bond, a slower reaction.
C-I is the most reactive (reactivity increases down group 7) and C-F is therefore the least reactive and strongest.
Part two of this post will cover nucleophilic substitution of cyanide ions and ammonia molecules, as well as elimination reactions.
SUMMARY
You need to know about the synthesis of chloroalkanes via the photochemical chlorination of the alkanes. - “forming chloroalkanes through chlorinating an alkane in the presence of sunlight”.
Chlorine will react with methane when UV light is present and will form several kinds of chloroalkanes and fumes of hydrogen chloride gas. Depending on how many chlorine molecules there are, there will be different compounds formed.
When undergone in real life, mixtures of halogenoalkanes are produced with some long chain alkanes which can be separated out with fractional distillation.
To understand what happens in an overall chemical reaction, chemists use mechanisms. These basically show the step-by-step process.
The chlorination of methane is something you must learn the mechanism for. The actual reaction is a substitution reaction because one atom or group is replaced by another.
The first step is initiation - UV light is essential for the first step in the mechanism. This breaks the Cl-Cl covalent bond so that each chlorine leaves with one electron from the shared pair. Chlorine free radicals, with one unpaired electron in the outer shell, are formed. Free radicals are only formed if a bond splits evenly - each atom getting one of the two electrons.
Step two is propagation: (a) Chlorine free radicals (highly reactive) react with methane to form hydrogen chloride and leave a methyl free radical (b) this free radical then reacts with another chlorine to form chloromethane and another chlorine free radical. Producing free radicals is a chain reaction which is why it is such a problem in ozone depletion - a little amount can cause a lot of destruction.
To stop the chain reaction, the final step is termination. It only happens when two free radicals collide to form a molecule in several ways: two chlorine free radicals forming a chlorine molecule, two methyl FRs forming ethane or a chlorine FR and a methyl FR forming chloromethane.
Ethane contributes to the longer chain alkanes in the mixture.
Another reaction you need to know is a nucleophilic substitution reactions. A nucleophile is an electron pair donor or proton acceptor, such as hydroxide ions, cyanide ions or ammonia molecules. Hydroxide and cyanide ions are negative but ammonia is neutral.
Halogenoalkanes have a polar bond because of the difference between the highly electronegative halogen and the carbon atom. The 𝛿+ carbon can go under nucleophilic attack.
Nu represents the nucleophile. Make sure to include curly arrows that begin at a lone pair or the centre of a bond and end at an atom or centre of bond, and delta (slight) charges.
One nucleophile that can be used is a hydroxide ion, found in either water or sodium hydroxide. In this case, you need to know about aqueous sodium hydroxide or potassium hydroxide and a halogenoalkane. This takes place at room temperature but is slow so is often refluxed (continuously boiled and condensed back into the reaction flask). The halogenoalkane is dissolved into ethanol since it is insoluable in water and this solution along with the aqueous hydroxide can mix. The product produced is an alcohol, which is organic.
The general reaction is :R-CH2X + NaOH -> CH3CH2OH + NaX where X represents a halogen
The lone pair on the hydroxide attacks the carbon atom attached to the halogen and this causes both carbon electrons to move to the halogen which becomes a halide ion.
The reaction of a hydroxide ion can also be classed as a hydrolysis reaction as it breaks down chemical bonds with water or hydroxide ions.
The speed of reaction depends on the strength of the bond - a stronger carbon-halogen bond, a slower reaction. C-I is the most reactive (reactivity increases down group 7) and C-F is therefore the least reactive and strongest.
Gradually falling back in love with studying 🫶
Doing organic chemistry always helps me enjoy what I study
really trying my best to get into organic chemistry 2 studying but i’m so over it i need to start pchem and continue with my other math courses like im tired
taking my ‘intro’ class to my major (quantitative analysis for chemistry) any advice is appreciated!!!
I love how my chem notes have these game-loading-screen-tip type of lines;
“alcoholates are like salts” thanks I guess but how does it relate to phenols ???
This reminded me of the isonitrile freezer at my previous internship.
For those who don't know, isonitriles (aka isocyanides) are a class of compounds that contain this motif:
They are known to smell very bad and many synthesis pathways to those compounds were discovered because of their stench. (I personally think they smell like a mixture of rotten cabbage and burned rubber but more ''artificial'')
So in that lab, we had a freezer dedicated to them, and even with sealed bottles in à -20°C freezers in a separated and ventilated cabinet, you would still be able to detect their odour if you stood next to it (not strongly, but still detectable).
We had to move that freezer to a new lab, it stayed unplugged for 15 to 20 minutes, and in the 5 minutes we need to power it back in the new lab, the entire room had filled with that isonitrile stench (mind you that freezer had not been open during the entire operation). Thankfully we did that on a Friday afternoon and by Monday the smell had disappeared.
Just for reference this is from the MSDS of benzyl isonitrile :
found on a fridge in my lab, haha
22/2/2020
We love tutorials! Photo is a bit bad but it’s late and I feel bad for neglecting this account haha
07/02/2020
Organic chemistry is addictive torture
01/02/2020 - 1/100 days of productivity
Happy February! New month, new me? I’m going to do the productivity challenge again.
My mum visited me at uni today so I spent the afternoon with her in Birmingham. I decided to condense 3 handouts from my lecture course on carbonyl chemistry onto one summary page this morning before I met her, and I finished it off after she left to get the train home.
I decided to write up the mechanism for Swern oxidation even though it’s beyond the scope of the first year course; it helps me remember the conditions if I actually know what each reagent does!
30/7/19
I’m a few days into creating this journal of chemistry fundamentals that I should know as a refresher before I start uni at the end of September. It’s a long way away yet, but I’d rather ease my brain into the work and kill my boredom in a fun way than panic, work too hard and burn myself out before I even start!
I hope you’re doing well!
10/3/19
Gotta love that NMR!
Also can we appreciate those perfect hexagons because it took ages to draw those ahaha
Have a great Sunday!
25/11/18 - 77 days of productivity
This is why I love chemistry. It’s messy yet highly predictable, and all molecules are intrinsically related to one another - even if it’s hard to get from one to the other in a single step.
I mentioned nucleophilic acyl substitution on my personal statement, and I’m just reminding myself of it - just in case Cambridge decide to grill me on it. In fact, as much as I HATE my personal statement, I’m going through it all. But my grey mildliner is healing my heart :)
PhLE Review Day 2 & 3💊👨💻👨🔬📚
house, online, self-review
28,29 May 2024
2nd day of review for the Board Exam. I read McMurry Organic Chemistry e-book yesterday afternoon. But I wasn't able to review Medicinal Organic Chemistry last night, I went outside with my cousins, aunt, mommy, and grandma. I already felt sleep last night and I fell asleep. For this day, 3rd day, I did a scan on my Quality Control 1 Lecture notes also. I'm currently reading Medicinal Organic Chemistry this night. I'm gonna read later DDS and Physical Pharmacy. Tomorrow will be group study online (for Pharmaceutical Calculations) also after the scheduled subjects tomorrow. TUESDAY: Organic Chemistry, Medicinal Organic Chemistry WEDNESDAY: Physical Pharmacy, Drug Delivery Systems, Quality Control 1