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MCAT Miscellaneous > Review 1 > Flashcards

Review 1 Flashcards

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MCAT flashcards
1
Q

3 Indicators and their Range

A
  1. Methyl Red = 4.4 - 6.2
  2. Bromothymol Blue = 6 - 7.6
  3. Phenolphthalein = 8.2 - 10
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2
Q

Two Methods for Alpha amino acid Synthesis

A
  1. Gabriel Synthesis

2. Strecker Synthesis

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3
Q

Gabriel Synthesis

A

N-pthalimidomalonic acid (2 COOEt (One for COOH and the other to activate COOH and N-bound to aromate for Amino Group) -> Alkylated to add R group (use base and R-X) -> Acid-hydrolysis (to add Nitro and carboxy on both siddes) -> Heat to form the alpha-amino acid and addition of H and removal of one of the COOH

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4
Q

Strecker Synthesis

A
  1. Aldehyde or Ketone acts as the backbone for amino acid
  2. :NH3 = Precursor for amino group
  3. KCN = Precursor for Carboxy group
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5
Q

Strecker Synthesis Process

A

Aldehyde or Ketone + :NH3 -> Water and Imine

Imine with Acid and KCN -> Alpha amino nitrile + acid -> amino acid

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6
Q

Transport Proteins

A

The higher the concentration of the ligand, the higher the binding affinity while the lower the concentration of the ligand, the lower the binding affinity

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7
Q

Purines

A

Adenine and Guanine

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8
Q

Pyrimidines

A

Cytosine and Thymine

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9
Q

Difference between Purines and Pyrimidines

A

Purines have a double ring structure and Pyrimidines hae a single ring structure

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10
Q

Why is DNA called an acid even with Nitrogenous bases

A

They have phosphate groups that are usually protonated but remain deprotonated in the solvent.

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11
Q

Saponification

A

Base-Catalyzed Ester hydrolysis of triglycerols that lead to polar and non-polar sides for soaps to function. This is the process by which fats are metabolized.

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12
Q

Types of Lipids

A

Hydrolyzable and Non-hydrolyzable lipids

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13
Q

4 examples of hydrolyzable Lipids

A
  1. Triglycerols - Saponification
  2. Phospholipids - Hydrolyzable because of phosphate
  3. Sphingolipids - Sphingosine + substituting OH for phosphate
  4. Waxes - Hydrolyzable because of the C=O

1 = Energy storage and 2 = Structural function

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14
Q

3 examples of non-hydrolyzable lipids

A
  1. Prostagladins - Inflammation signalling molecule
  2. Steroids - 6-6-6-4 rings with differing substituents for structural purposes
  3. Vitamins - Cofactors
    a. A - Retinol (light sensitivity)
    b. D - Bones (Rickets and Osteoporasis)
    c. E - Antioxidant (protects neurological function)
    d. K - Prothrombin (blood clot)
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15
Q

Effect of Common ion on Solubility

A

Common ione effect decreases solubility and shifts the equilibrium to the left as a result of Le Chatelier’s principles

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16
Q

Effect of pH on solubility

A

If the salt dissociating has a strong conjugate base, it will combine with the proton and form an acid and water. Note it does not work on all salts because the stronger the acid, the weaker the conjugate base. For example:
CaF2, F- will combine with H+ to form a weak acid but AgCl2 will not form an acid because it has a weak conjugate base and strong acid.

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17
Q

Effect on equilibrium of solubility from pH

A

The proton reacts with the specific ion and takes it out of solution, this will shift the equilibrium to the right to relieve the stress

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18
Q

Effect of dissolving NH3 and AgCl2

A

This will lead to the dissolution of AgCl2 into Ag 2+ and Cl-, the Ag 2+ will combine with NH3 to form a complex ion which is highly favorable. The overall effect is that more of AgCl2 will dissolve because the equilibrium shifts to the right

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19
Q

Acid/base NH3 and AgCl2 explanation

A

NH3 acts as a Lewis base (electron pair donor) and Ag2+ acts as a Lewis acid (electron pair acceptor)

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20
Q

CASHNGIA Explanation

A 
C - Chlorates
A - Acetates
S - Sulfates
H - Halides
N - Nitrates
G & I - Group I metals
A - Ammonium
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21
Q

Electromagnetic Spectrum

A 
Radio Waves
Microwave
Infrared
Visible
Ultraviolet (UV) rays
X-rays
Gamma rays
22
Q

RMIVUXG

A

Rose and Malik Invited Vanessa and Umar to Xtra Glasses

23
Q

Separation by Precipitation

A

The compound with the smallest value of molar solubility precipitates from solution first

24
Q

Trick of Ion-exchange Chromatography

A

Exchanges one ion in solution for another which is initially bound to the column

TRICK: The column is filled with an ion exchange resin. The cation to be precipitated must have a lower molar solubility with the anion of the resin than the salt in the resin.

25
Q

Ionic Rules on Solubility

A
  1. The greater the ionic forces (attraction), the less soluble
  2. The greater the charge, the less soluble
  3. The greater the size, the more soluble
26
Q

Oxides and Solubility

A

Most Oxides and hydroxide salts are only slightly water soluble. KOH and NaOH are notable exceptions that are substantially soluble

27
Q

Phase changes and Solubility

A
  1. Solubility of solids in liquids INCREASE with increasing temperature
  2. Solubility of gases in liquids DECREASE with increasing temperature
  3. Solubility of gases in liquids INCREASE with increasing pressure
28
Q

Colligative Properties

A
  1. Depends on NUMBER of solutes NOT TYPE of solutes
  2. Boiling point elevation and Vapor Pressure depression
  3. Freezing point depression and Osmotic Pressure
29
Q

Vapor Pressure

A

Pressure exerted by gaseous phase of a liquid that evaporated from the exposed surface of a liquid.

  1. Increased intermolecular forces, vapor pressure decreases
  2. Increased temperature, vapor pressure decreases
  3. Atmospheric pressure increases, vapor pressure stays the same
  4. Solute concentration increases, vapor pressure decreases
30
Q

Osmotic Pressure

A

The pressure it would take to stop osmosis from occurring

31
Q

Freezing Point Depression

A
  1. Freezing point DECREASES with soluble impurities added to the solution
  2. Presence of solute particles will interfere with efficient arrangement of the solvent molecules into solid lattice
32
Q

Boiling Point Elevation

A
  1. Boiling point of a solution increases with the addition of impurities
  2. Attributed to both a decreased surface area from which the liquid can evaporate and an increase in the intermolecular forces binding the liquid solution.
33
Q

Boiling Point

A

Pressure at which the vapor pressure of the solution is equal to the atmospheric pressure over the solution

34
Q

Salt Bridge

A
  1. Helps equalize and neutralize salt bridge

2. Helps maintain balance

35
Q

Terminal and Electrodes of Voltaic/Galvanic/Electrochemical Cell

A

Anode - Negative because electrons are generated from here (oxidation occurs here since electrons are generated)

Cathode - Positive because electrons come here and reduction because electrons cause reduction here

36
Q

Factors Affecting the Cathode and Anode

A
  1. Ions
  2. Temperature
  3. Pressure
  4. Concentration
37
Q

Free energy and Cell Potential Relationship

A

G = nFE

38
Q

Define Faraday

A

Magnitude of charge carried by 1 mole of Electron

39
Q

Standard Reduction Potentials

A 
Down - Increasing Reducing agent and Up is increasing oxidizing agent
Ag+
Cu2+
H+
Zn2+
Li+
40
Q

Peculiar Property of Free energy and Standard Potential

A

Standard Potential is an intensive property (does not change)

Free energy is an extensive property (changes)

41
Q

How can Activity series be explained

A

Use the standard reduction potentials

42
Q

Relate Standard Cell Potential and Equilibrium Constant

A

-nFE = -RTlnK
From,

G = -nFE and G = -RTlnK (Remember all are in Standard G)

43
Q

Essence of Nernst Equation

A

To calculate the standard cell potential when in non-standard conditions:

G = G' + RTlnQ
-nFE = -nFE + RTlnQ
44
Q

Standard Conditions

A

Standard Conditions:

  1. Temperature = 25 degrees
  2. Liquids and gases are pure
  3. Solutions = 1 M
  4. Energy of formation = 0
  5. Pressure = 1 atm
45
Q

STP

A

Standard Temperature and Pressure:

  1. Temperature = 0 degrees
  2. Pressure = 1 atm or 1*10^5 Pa
  3. No of moles of gas = 1 mole
  4. Volume = 22.4 L
46
Q

Effect of Q on E

A

As Q increases, E decreases

47
Q

Terminal type and Electrode at a Electrolytic Cell

A

Cathode - Negative (reduction occurs here and electrons are coming from battery source
Anode - Positive (oxidation occurs here because it is the opposite)

48
Q

Concentration Cell

A

Cell is the same electrodes (elements) but voltage generates as a result of tendency to become equally concentrated. Use the Nernst equation to find out what is the voltage since standard cell potential should be zero

49
Q

Difference between Voltaic/Galvanic/Electrochemical cell and Electrolytic cell

A

The former occurs as a result of being spontaneous while the latter is a result of non-spontaneous reaction

50
Q

Redox Reactions Balance

A
  1. Write each of the half reaction
  2. Balance the atoms other than O and H
  3. Balance the oxygen by adding H2O
  4. Balance the hydrogens by adding H+/OH- (Acids/Bases)
  5. Balance the charges by adding electrons
  6. Make the number of electrons equal, and add the half reaction.

MCAT Miscellaneous (17 decks)

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