Acetaminophen

Acetaminophen

By Eric Zuberi

Period A

Chemistry .1

Introduction

Acetaminophen (C₈H₉NO₂), commonly referred to as Tylenol, is a medicine that is used to treat mild to moderate pains. It is often used for headaches, toothaches, stomach aches, colds, sore throats, reactions to vaccinations, as well as Rheumatoid Arthritis. It is also used to reduce fevers. Because of this, it is classified as an analgesic (pain relieving) and an antipyretic (fever reducing) medicine. Acetaminophen, is the active ingredient in Tylenol. Because it is man-made, it can only be found in a laboratory. It is made in a basic reaction between p-aminophenol and acetic anhydride. The reaction looks like this: C₆H₄(OH)(NH₂) + (CH₃CO)₂O à C₈H₉NO₂. Acetaminophen works by blocking the body’s production of prostaglandins. Prostaglandins are naturally occurring chemicals that cause inflammation and fever. Acetaminophen blocks the development/production of prostaglandins in the central nervous system. Because of this, Acetaminophen reduces our fevers and the inflammation that our body incurs on itself.

Lewis Structure of Acetaminophen

Lewis Structure of Acetaminophen

The picture above is the Lewis structure of Acetaminophen.

Nature of the bonds

Hydrogen to Oxygen is a moderately polar covalent bond. (The difference in electronegativity is 1.24)

Hydrogen to Carbon is a strongly polar covalent bond. (The difference in electronegativity is 0.35)

Hydrogen to Nitrogen is a moderately polar covalent bond. (The difference in electronegativity is 0.84)

Oxygen to Carbon is a moderately polar covalent bond. (The difference in electronegativity is 0.89)

Carbon to Nitrogen is a strongly polar covalent bond. (The difference in electronegativity is 0.49)

Carbon to Carbon is a purely covalent bond. (The difference in electronegativity is 0.00)

VSEPR

Acetaminophen is a linear molecule. This means that all of its bonds have a 180 degree angle.

Polarity

Acetaminophen is a polar molecule. It is polar because certain spots on the molecule are more electronegative that others. You can clearly see this through the arrows that are drawn from the less electronegative element to the more electronegative element.

Intermolecular Forces that Act Upon a Pair of Acetaminophen Molecules

Intermolecular Forces that Act Upon a Pair of Acetaminophen Molecules

Three forces act on pairs of Acetaminophen. These forces are Hydrogen Bonding, Dipole Dipole, and London Dispersion. Hydrogen bonding acts on a pair of Acetaminophen molecules because the Hydrogen in one of the molecules bonds with the Oxygen in the other. This creates a powerful force that is difficult to break. Dipole Dipole forces act upon a pair of Acetaminophen molecules because both Acetaminophen molecules are polar. This force is slightly weaker than Hydrogen Bonding. Finally, London Dispersion Forces also act on a pair of Acetaminophen molecules. London Dispersion Forces act upon all molecules. “The London Dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles.” (Purdue Chemistry Lab) Because electrons are moving at all times, there will always be London Dispersion Forces present between all molecules, including Acetaminophen.  

3-D Acetaminophen Molecule

3-D Acetaminophen Molecule

The molecule above is the 3-D structure of Acetaminophen. As you can clearly see, there are 8 Carbons, 9 Hydrogens, 1 Nitrogen, 2 Oxygens, and 5 Unshared Electron Pairs. Another key feature is the Benzene Ring, which is visible in the center of the molecule. It is made of 6 Carbons, with 4 Hydrogens attached on the outside of the ring.

Conclusion

Conclusion

Acetaminophen is one of the most necessary medicines in the modern day. It is used quite commonly among our society as a pain-killer and as a fever reducer. It has uses with a wide range, including headaches, toothaches, stomach aches, colds, sore throats, reactions to vaccinations, and even Rheumatoid Arthritis. When taking Acetaminophen, you still must pay attention to the amount of it you are taking. If too much Acetaminophen is taken, it can cause liver damage, which can be so severe that it may require a liver transplant or even result in death. Alcohol also speeds up the decomposition of the liver, so taking alcohol along with Acetaminophen is very dangerous. If you are breast feeding or pregnant, then you should consult your doctor before taking Acetaminophen. You should not continue to take Acetaminophen if the symptoms you are taking it for get worse or new symptoms develop. If this happens, consult your doctor immediately.