Which Parts Of Acetylsalicylic Acid Are Rigid?

Acetylsalicylic acid, also known as aspirin, has a structure that allows for rotation around certain bonds. The single sigma bonds connecting the carbon and oxygen atoms, as well as the single bonds involving hydrogen atoms, are free to rotate.

Let’s break down why this happens:

Sigma Bonds: Sigma bonds are the strongest type of covalent bond. They are formed by the direct overlap of atomic orbitals. This direct overlap allows for free rotation around the bond axis without breaking the bond itself.

Carbon-Oxygen and Carbon-Hydrogen Bonds: In acetylsalicylic acid, the single bonds between carbon and oxygen atoms, as well as carbon and hydrogen atoms, are all sigma bonds. Therefore, these bonds are free to rotate.

Think of it like this: Imagine a ball and socket joint. The ball can rotate freely within the socket, just like the atoms connected by a sigma bond can rotate around the bond axis.

Understanding the Significance of Rotation

Rotation around sigma bonds is crucial for the flexibility and movement of molecules. This flexibility allows molecules to adopt different conformations, which are different spatial arrangements of the atoms. Conformations can influence the molecule’s interactions with other molecules and its overall behavior.

For example, the rotation around the sigma bonds in acetylsalicylic acid allows it to interact with its target enzymes in the body. This interaction ultimately leads to the pain-relieving and anti-inflammatory effects of aspirin.

Note: Rotation around a sigma bond does not occur freely in all cases. Steric hindrance, which is the repulsion between electron clouds of nearby atoms, can restrict rotation. However, in the case of acetylsalicylic acid, the rotation around the sigma bonds is generally free.

Let’s break down the pi bonds in acetylsalicylic acid, also known as aspirin.

Acetylsalicylic acid has a total of five pi bonds. These pi bonds are located in three distinct parts of the molecule:

The benzene ring: The benzene ring contributes three pi bonds. This is because benzene has a special structure with delocalized electrons, meaning the electrons are spread out across the entire ring.
The carboxylic acid group: The carboxylic acid group, -COOH, contributes one pi bond.
The ester group: The ester group, -COO-, contributes one pi bond.

So, we have 3 + 1 + 1 = 5 pi bonds in acetylsalicylic acid.

Understanding Pi Bonds

Pi bonds are a type of covalent bond formed by the sideways overlap of atomic orbitals. They are weaker than sigma bonds, which are formed by the head-on overlap of atomic orbitals. Pi bonds are important for determining the shape and reactivity of molecules. They are also responsible for the unique properties of aromatic compounds like benzene.

Pi Bonds in Acetylsalicylic Acid

The presence of these pi bonds in acetylsalicylic acid influences its chemical behavior. For instance, the benzene ring’s delocalized electrons make it more stable and less reactive compared to a simple alkene. This stability contributes to aspirin’s ability to resist degradation and remain effective for a long time. The pi bond within the carboxylic acid group is responsible for its acidic properties, while the pi bond within the ester group gives aspirin its characteristic properties as a painkiller and anti-inflammatory agent.

Visualizing Pi Bonds

To better visualize these pi bonds, you can draw the Lewis structure of acetylsalicylic acid. The double bonds in the benzene ring, the carboxylic acid group, and the ester group represent the pi bonds. In a molecular model, the pi bonds would be depicted as electron clouds above and below the plane of the molecule.

By understanding the structure and bonding of acetylsalicylic acid, we gain a better understanding of its properties and how it interacts with other molecules. This knowledge is vital for understanding its medicinal applications and how it works to alleviate pain and inflammation.

Okay, let’s break down the structure of acetylsalicylic acid, also known as aspirin.

Aspirin’s chemical formula is C9H8O4. This formula tells us that each molecule of aspirin contains nine carbon atoms, eight hydrogen atoms, and four oxygen atoms.

You can also express the formula as CH3COOC6H4COOH. This extended formula gives a clearer picture of how the atoms are arranged in the molecule. It shows that aspirin has a salicylic acid core (C6H4COOH) attached to an acetyl group (CH3COO).

The molecular mass of aspirin is approximately 180.159 g/mol. This means that one mole of aspirin weighs 180.159 grams.

Now, let’s dive a bit deeper into aspirin’s structure to understand how it works:

The structure of aspirin is a benzene ring with a carboxylic acid group (-COOH) attached to it. This carboxylic acid group is responsible for aspirin’s anti-inflammatory and pain-relieving properties. The acetyl group attached to the salicylic acid is crucial for its stability and allows it to be absorbed more easily by the body.

Here’s a breakdown of the key components of aspirin’s structure:

Benzene Ring: This is a stable six-carbon ring with alternating single and double bonds.
Carboxylic Acid Group (-COOH): This group is acidic and is responsible for aspirin’s pain-relieving and anti-inflammatory effects.
Acetyl Group (CH3COO): This group is attached to the salicylic acid core and makes aspirin more stable and easier to absorb.

Understanding the structure of aspirin allows us to appreciate how it interacts with our bodies and helps to relieve pain and inflammation.

Aspirin is a common over-the-counter medication used to relieve pain, fever, and inflammation. It’s a white crystalline powder with a molecular weight of 180.16 g/mol. It has a melting point of 135°C and is insoluble in water, but soluble in alcohol and ether.

Aspirin’s physical properties are important for its effectiveness. Its crystalline structure allows it to be easily absorbed into the bloodstream. Its insolubility in water prevents it from being broken down in the stomach, allowing it to reach the small intestine, where it is absorbed. Its solubility in alcohol and ether makes it possible to produce different formulations of aspirin, such as tablets, capsules, and liquids. These properties help ensure aspirin’s effectiveness and make it a valuable drug for treating a variety of ailments.

Let’s delve deeper into these properties and how they impact aspirin’s functionality.

Melting Point: The melting point of aspirin is a crucial characteristic. It tells us the temperature at which aspirin transitions from a solid to a liquid state. This information is important for manufacturing and storage as it helps ensure the stability and integrity of the drug. A high melting point suggests that aspirin can withstand a considerable amount of heat before breaking down, making it stable for storage and use.

Solubility: Aspirin’s solubility in different solvents dictates how it interacts with the body and how it’s administered. Its insolubility in water is beneficial because it prevents the drug from being broken down in the acidic environment of the stomach. This allows aspirin to reach the small intestine, where it’s absorbed into the bloodstream. Its solubility in alcohol and ether allows for different formulations, such as tablets, capsules, and liquids, catering to diverse needs and preferences. This versatility in formulation expands aspirin’s accessibility and ease of use.

Crystalline Structure: Aspirin’s crystalline structure contributes to its effectiveness. It allows the drug to be easily absorbed into the bloodstream, maximizing its bioavailability. This structure also influences its physical properties, such as its melting point and solubility. A well-defined crystal structure ensures consistent quality and efficacy, making it a reliable medication.

Understanding these properties is vital in appreciating aspirin’s role as a widely used and effective medication.

Aspirin has four rotatable bonds. These bonds are responsible for the different possible conformations, or shapes, of the aspirin molecule. Let’s break down these bonds:

The C=O bond of the carboxyl group: This bond is located within the carboxylic acid functional group of aspirin. The carbon atom in this group is attached to a hydroxyl group (-OH) and a double-bonded oxygen atom. This C=O bond can rotate freely.
The C=O bond of the acetoxy group: Aspirin also has an acetoxy group, which is an ester group. The C=O bond in this group is also capable of rotation.
The C-O linkage of the acetoxy group: This bond connects the carbon atom of the acetoxy group to the oxygen atom. This single bond also allows for rotational freedom.
The O-H positioning on the carboxyl group: This bond connects the oxygen atom of the hydroxyl group to the hydrogen atom. Rotation around this bond allows the hydroxyl group to take on different positions in space.

The different combinations of rotations around these four bonds allow aspirin to exist in a variety of conformations. This is important because the shape of a molecule can affect its biological activity. For instance, the specific shape of an aspirin molecule might influence how it binds to a target protein in the body, ultimately affecting its effectiveness as a pain reliever.

To visualize these rotatable bonds:

Imagine the aspirin molecule like a puzzle. Each bond acts as a hinge where different pieces can rotate. Each possible combination of rotations results in a unique arrangement of these pieces, leading to various conformations of the aspirin molecule. While these rotations might appear subtle, they have a significant impact on the molecule’s interactions with other molecules.

It’s important to remember:

While aspirin has four rotatable bonds, its biological activity is largely influenced by the interactions between these bonds and surrounding molecules. The shape of the molecule and its ability to interact with its environment play a critical role in how aspirin functions as a medicine.

Acetylsalicylic acid, commonly known as aspirin, is a white crystalline solid at room temperature. This means it’s a solid substance with a distinct crystal structure, making it look like tiny, sparkly grains. You’ll find it in most medicine cabinets, and it’s often used to relieve pain and reduce fever.

But here’s something interesting: aspirin is also slightly acidic. This means it can dissolve in water and release hydrogen ions, which makes the solution slightly acidic. In fact, at 25 degrees Celsius, aspirin has an acid dissociation constant of 3.5.

This tells us that aspirin is not very strong acid. It’s actually a relatively weak acid, and that’s why it’s safe to take as a medicine. The acid dissociation constant is a measure of how readily a substance will give up its hydrogen ions in water. The lower the value, the weaker the acid.

Here’s a simple way to think about it: imagine aspirin like a shy person who doesn’t like to share their things. It’s not going to readily give up its hydrogen ions to make the solution very acidic.

Knowing that aspirin is a white crystalline solid and a weak acid helps us understand how it works as a medication. It’s the combination of its physical form and chemical properties that make it an effective pain reliever.

Let’s talk about acetylsalicylic acid, commonly known as aspirin, and its bond angles.

You might be wondering, “Why are bond angles important?” Well, they tell us a lot about the shape of a molecule. And knowing the shape helps us understand how a molecule interacts with other molecules. This is really important in chemistry!

So, the bond angles in acetylsalicylic acid are:

120 degrees for angles 1 and 3. These angles involve the oxygen-carbon-oxygen (O-C-O) and carbon-carbon-oxygen (C-C-O) bonds.
109.5 degrees for angle 2. This angle involves the carbon-carbon-carbon (C-C-C) bond.

Now, why are these specific angles? It all boils down to something called hybridization. Basically, hybridization is a way of mixing atomic orbitals to create new hybrid orbitals with different shapes and energies.

In acetylsalicylic acid, the carbon atoms in angles 1 and 3 use sp2 hybridization, which gives them a trigonal planar geometry, resulting in a 120 degree bond angle. The carbon atom in angle 2 uses sp3 hybridization, which gives it a tetrahedral geometry, resulting in a 109.5 degree bond angle.

Let’s break it down:

sp2 hybridization: This involves mixing one s orbital and two p orbitals, resulting in three sp2 hybrid orbitals. These orbitals lie in the same plane and are arranged at 120 degrees to each other. This leads to the trigonal planar geometry we see in angles 1 and 3.

sp3 hybridization: This involves mixing one s orbital and three p orbitals, resulting in four sp3 hybrid orbitals. These orbitals point towards the corners of a tetrahedron with 109.5 degree angles between them. This leads to the tetrahedral geometry we see in angle 2.

So, the hybridization of the carbon atoms directly determines the bond angles in acetylsalicylic acid. This knowledge helps us understand its structure and how it interacts with other molecules. Pretty cool, huh?

Let’s talk about pi bonds. First, we need to understand what a pi bond is. You know how sigma bonds are created when orbitals overlap end-to-end? Well, pi bonds are formed by the side-by-side overlap of atomic orbitals. This side-by-side overlap creates an electron cloud above and below the plane of the molecule.

Now, how do we know how many pi bonds are in a molecule? Here’s the trick: pi bonds are always found in double and triple bonds. If we look at a double bond, there’s one sigma bond and one pi bond. And if we have a triple bond, there’s one sigma bond and two pi bonds.

Let’s break it down:

Single bond: one sigma bond
Double bond: one sigma bond and one pi bond
Triple bond: one sigma bond and two pi bonds

To figure out the number of pi bonds, we simply count the number of double and triple bonds in the molecule. If we have two double bonds, then we have two pi bonds. If there are no double or triple bonds, then there are no pi bonds.

It’s important to remember that the pi bond is weaker than the sigma bond. This is because the overlap between the atomic orbitals in a pi bond is not as strong as the overlap in a sigma bond. The pi bond also restricts the rotation of the molecule around the bond axis.

Let’s look at an example. Take ethene (C2H4). Ethene has a double bond between the two carbon atoms. This double bond consists of one sigma bond and one pi bond. This pi bond is formed by the overlap of the p orbitals of the two carbon atoms.

That’s how to find the number of pi bonds in a molecule. Just count the double and triple bonds, and you’ll know how many pi bonds are present. Keep in mind the strength of the pi bond and its effect on the rotation of the molecule.

Acetylsalicylic acid, commonly known as aspirin, is a rigid molecule due to its structural features. The key factor contributing to its rigidity is the presence of a six-membered ring with alternating alkane and alkene bonds. This arrangement creates a planar and relatively inflexible structure.

Furthermore, acetylsalicylic acid has 21 sigma bonds, which are strong single bonds. These bonds restrict the rotation of the molecule’s various parts, further increasing its rigidity. The presence of a heterocyclic ring, containing an oxygen atom within the ring structure, also adds to the molecule’s overall rigidity.

Let’s delve deeper into the concept of rigidity in the context of acetylsalicylic acid. Rigidity refers to the molecule’s resistance to bending or deformation. The structure of acetylsalicylic acid, with its aromatic ring and numerous sigma bonds, makes it more difficult for the molecule to change its shape. This rigidity has a significant impact on its properties.

Think of a bicycle wheel. A wheel with spokes is much more rigid than a wheel without them. The spokes provide the structure that prevents the wheel from collapsing or deforming. Similarly, the aromatic ring, the sigma bonds, and the heterocyclic ring in acetylsalicylic acid act like spokes, giving the molecule its rigidity.

The rigidity of acetylsalicylic acid is directly related to its reactivity. The molecule’s structural stability makes it less likely to undergo chemical reactions with other molecules. This property is essential for aspirin’s effectiveness as a drug.

Because of this inherent stability, acetylsalicylic acid can remain stable for long periods and can be stored at room temperature without significant degradation. It also allows for a consistent and predictable therapeutic effect when it is ingested as medication. In essence, acetylsalicylic acid’s rigidity is a key factor in its medicinal properties.

Let’s figure out how many bonds are in acetylsalicylic acid, which you might know as aspirin. This is a pretty important compound, used for pain relief and to reduce fever.

First, we need to understand what kinds of bonds we’re dealing with. There are two main types of chemical bonds: sigma bonds (σ) and pi bonds (π). Sigma bonds are the strongest type of covalent bond, formed by the direct overlap of atomic orbitals. Pi bonds are weaker and are formed by the lateral overlap of atomic orbitals.

Now, let’s look at acetylsalicylic acid. The molecule has a total of 13 sigma bonds and 5 pi bonds. This is because there are 5 single bonds which are sigma bonds. There are also 2 double bonds, each having one sigma bond and one pi bond. And, finally, there are 6 sigma bonds in the benzene ring. All these bonds add up to 13 sigma bonds.

We know there are 2 double bonds (with one pi bond each), and there are also three additional pi bonds in the benzene ring. This makes a total of 5 pi bonds.

So, acetylsalicylic acid contains 13 sigma bonds and 5 pi bonds. This is a lot of bonds, but they are all essential for the molecule’s structure and function.

Aspirin is the brand name for acetylsalicylic acid, which is the common name for 2-(acetyloxy)benzoic acid. You might be wondering what acetylsalicylic acid looks like. It’s a white, crystalline powder that’s odorless and tasteless.

Let’s break down the structure of acetylsalicylic acid to understand its appearance better. It’s a relatively simple molecule with a benzene ring at its core. Attached to this ring is a carboxyl group (-COOH), which is responsible for its acidic properties. The other side of the benzene ring is connected to an acetyl group (-COCH3), which is what gives acetylsalicylic acid its pain-relieving properties.

This structure is important because it’s what gives acetylsalicylic acid its unique properties. The benzene ring gives it stability, while the carboxyl and acetyl groups give it its acidic and pain-relieving properties, respectively.

You won’t typically see acetylsalicylic acid in its pure form, though. It’s usually combined with other ingredients to make it easier to take, such as binders, fillers, and coatings. This is why aspirin tablets look the way they do.

Acetylsalicylic acid is a remarkable compound with a simple structure but powerful effects. Its unique chemical makeup allows it to work wonders for pain relief and other conditions. Next time you reach for an aspirin, remember the white, crystalline powder that’s making you feel better.

Which parts of acetylsalicylic acid are rigid? | Quizlet

Acetylsalicylic acid is the active ingredient in aspirin. It took 35.17 mL of 0.5065 M sodium hydroxide to react completely with 3.210 g of acetylsalicylic acid. Acetylsalicylic acid has one acidic hydrogen. Quizlet

Acetylsalicylic Acid Structure: Detailed Explanations – Lambda

In this section, we will explore the rigid parts of acetylsalicylic acid, namely the benzene ring and the acetyl group. The Benzene Ring: A Rigid Structure The techiescience.com

Solved The Structure of acetylsalicylic acid (aspinn) is

The Structure of acetylsalicylic acid (aspinn) is shown below (Figure 1) You may want to reference (pages 236-248) Section 7.3 while completing this problem. HOw many pi bonds are present in acetylsalicylic acid? Chegg

Solved The structure of acetylsalicylic acid (aspirin) is

Which parts of acetylsalicylic acid are rigid? the C-C bonds the ring structure the C = O bonds the C-H bonds the C-O. Show transcribed image text. There are 4 steps to solve this one. Expert-verified. Step 1. Chegg

The structure of acetylsalicylic acid (aspirin) is shown

The partial Lewis structure that follows is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and there are no unshared electron pairs in the molecule. The carbon—carbon Pearson

SOLVED: Which parts of acetylsalicylic acid are rigid? the C

The C−C bonds: These bonds are not particularly rigid. They allow for rotation and movement. So, the rigid parts of acetylsalicylic acid are the ring structure Numerade

How many sigma/pi bonds are in the aspirin structure? | Socratic

Aspirin is the brand name for acetylsalicylic acid, which is the common name for 2- (acetyloxy)benzoic acid. This compound looks like this: In a single bond, Socratic

Acetylsalicylic acid (Aspirin ) – C9H8O4 – Formula,

Aspirin’s chemical name is 2-Acetoxybenzoic acid. Aspirin, a chemical called acetylsalicylic acid (ASA), is widely used worldwide as an anti-inflammatory and antipyretic drug. Formula and structure: the molecular BYJU’S

10.3: Analgesics – Chemistry LibreTexts

The acetylsalicylic acid molecule does contain an organic acid functional group (COOH). As a result of this molecular structure, Aspirin products can be harsh on the stomach libretexts.org