NS6: CPF

Question 1

phenol nomenclature

Answer 1

contain two –OH groups are termed diols. For diols (as well as substituted benzene rings in general), the terms ortho (o), meta (m), and para (p) describe the orientation of the groups relative to each other.

An ortho configuration involves two groups immediately adjacent to each other

meta structures have two substituents separated by a single carbon

para diols include two –OH groups immediately across from each other on the ring.

Question 2

quinone nomenclature

Answer 2

Quinone contains two carbonyl groups formed via C=O bonds on carbons within its ring structure.

Semiquinone: addition of a single hydrogen atom to a quinone produces an unstable free radical species; more likely to be reduced than a quinone

Further reduction can yield a hydroquinone

Question 3

what is ubiquinone and why is it important

Answer 3

Ubiquinone is an electron carrier involved in complexes I, II, and III of the electron transport chain.

Its amphipathic structure (polar head and long alkyl tail) allows it to be both lipid-soluble and a functional electron carrier.

When carrying one electron, one of its carbonyl (C=O) groups is reduced to an alcohol, resulting in a molecule known as ubisemiquinone, and when carrying two electrons—as is commonly the case—both carbonyl (C=O) groups are reduced, and the molecule is termed ubiquinol.

Question 4

carboxylic acid derivatives (3)

Answer 4

In carboxylic acid (–COOH) derivatives, the –OH is replaced by something else.

Amides are carboxylic acid derivatives with an amine (–NH2, –NHR, or NR1R2) attached to the carbonyl carbon instead of the –OH group.

In esters, the –OH group is replaced by an –OR group.

Acid anhydrides are formed by the condensation of two carboxylic acids; that is, the substituent that replaces the –OH of one carboxylic acid is another carboxylic acid.

Amides are the most stable (least reactive) of the carboxylic acid derivatives because the amino substituent is a very poor leaving group
– esters have intermediate reactivity and acid anhydrides are highly reactive.

Question 5

IR peaks to know

Answer 5

Broad peak at 3300 cm-1 > O-H (hydroxyl)
Carboxylic acids > 3000 cm-1
Sharp peak at 3300 cm-1 > N-H
Sharp peak at 1750 cm-1 > C=O (carbonyl)

Question 6

H NMR ppms to know

Answer 6

Hydrogens on sp3 carbons > 0 to 3 ppm
Hydrogens on sp2 carbons > 4.6 to 6.0 ppm
Hydrogens on sp carbons > 2.0 to 3.0 ppm
Aldehyde Hydrogens > 9 to 10 ppm
Carboxylic acids Hydrogens > 10.5 to 12 ppm
Aromatics Hydrogens > 6.0 to 8.5 ppm

Question 7

strong nucleophiles have ___

Answer 7

greater electron density (either through possessing more lone pairs or more charge) and less steric hindrance

Question 8

give wavelength in terms of frequency, velocity, and energy

Answer 8

Recall that E = hf relates the energy of the photon to its frequency, and v = fλ relates frequency, wavelength, and speed.

Rearranging the second equation for frequency gives f = v/λ. Now we can substitute for f in the first equation, giving E = hv/λ. Rearranging this equation for wavelength gives λ = hv/E.

Question 9

redox agents?

Answer 9

Being oxidized = reducing agent
Being reduced = oxidizing agent
LEO goes GER

Question 10

Arrhenius acid / base

Answer 10

Acids = substances that dissociate in a manner that increases the concentration of protons (H+ ions) in solution
Bases = dissociation of a base increases the concentration of hydroxide (OH−) ions

Question 11

Lewis acid / base

Answer 11

Acids = electron lone pair acceptors
Bases = electron lone pair donors

** do not accept radicals!! only pairs

Question 12

Bronsted / lowry acid / base

Answer 12

Acids = proton donor
Bases = proton acceptor

Question 13

oxidation states of the periodic table

• diatomic
• Alkali metals
• Alkaline metals

Answer 13

Diatomic elements have oxidation states of zero. Otherwise, oxidation states are summed to equal the charge of the molecule.

The oxidation state of alkali metals (the first column in the periodic table) is always +1 (at least for the MCAT)

alkaline earth metals (the second column in the periodic table) is always +2.

Question 14

oxidation states of the periodic table

• halogens
• H
• O

Answer 14

The oxidation state of F is −1, because it is the most electronegative element.
Other halogens will usually have an oxidation state of −1, unless they are bonded to a more electronegative halogen, N, or O.
– In that case, their oxidation state may be +1, +3, +4 (for Br), +5, or even +7

The oxidation state of H is +1, except when it is bonded to a more electropositive element, in which case it will be −1.
– most common reducing agents NaH, NaBH4, and LiAlH4

The oxidation state of O is usually −2, with some important exceptions, such as peroxides, in which it is −1.

Question 15

enol v enolate

Answer 15

enols are good nucleophiles, but their conjugate bases – enolates – are even better

know the structure; (1) until perfect

Question 16

KMnO4

Answer 16

reagent that is commonly used to oxidize alcohols to carboxylic acids

recall that permanganate MnO4 has a charge of -1

Question 17

In surfactant-substrate interactions, depending on the surfactant and the substrate, we may observe what IMF(s)?

Answer 17

London dispersion forces
Hydrogen bonding
Ion-dipole interactions

Question 18

GLUT4

Answer 18

insulin-regulated glucose transporter found primarily in adipose tissues and striated muscle (skeletal and cardiac)

Question 19

when does beta decay happen?

Answer 19

Positive beta decay, also known as positron emission, occurs when the proton-to-neutron ratio is too high.

Whereas negative beta decay, aka electron emission, occurs when that ratio is too low.

Question 20

young’s modulus

Answer 20

measure of the stiffness of an elastic solid material where t the slope of the graph is stress over strain

The higher the Young’s modulus, the stiffer the solid material is, thus it has the greatest resistance to deformation.

Question 21

photon speed

Answer 21

The speed of photons is equivalent to the speed of light and doesn’t depend on the energy of the photons.

on the other hand, Higher frequency refers to higher energy.

Question 22

laminar flow through a pipe

Answer 22

Laminar flow is due to shear forces (friction) between the fluid and the solid surface of the tube.

This results in layers having a gradient of velocities, in which the flow is the fastest in the middle of the tube (where friction is low) and slowest near the surface (where friction is high).

Question 23

what kind of radiation breaks bonds / causes denaturation?

Answer 23

Non-ionizing radiation does not break bonds and thus will not be able to denature proteins.

Vs. Irradiating the proteins with X-rays or gamma rays certainly can denature them, but these are forms of ionizing radiation.

Vs. Heat will cause the protein to unfold and will eventually denature

Question 24

what does a high SASA (solvent-accessible surface areas) imply?

Answer 24

means that the residue in question has a large surface area that is exposed to the solvent, which implies it is likely at the surface of the protein

Surface residues are less likely to be “keystones” for the protein structure, as those sorts of residues tend to be found in the protein’s core.

Question 25

what should u know about the volume flow rate equation

Answer 25

Volume flow rate is proportional to the radius raised to the fourth power.

Question 26

what happens to your body (specifically blood) when you live at higher elevation?

Answer 26

A person living at a higher elevation will produce more blood cells because there is less oxygen in the air. The kidney has receptors that read the oxygen levels in the blood and produce erythropoietin in order to produce more blood cells.

Question 27

kinetic friction equation + work equation

Answer 27

Fnet = ma = Fapplied – Fk, where Fk is the force of kinetic friction.

To calculate work, we use W = Fd cos θ.