Review 1

Question 1

3 Indicators and their Range

Answer 1

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

Question 2

Two Methods for Alpha amino acid Synthesis

Answer 2

1. Gabriel Synthesis

2. Strecker Synthesis

Question 3

Gabriel Synthesis

Answer 3

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

Question 4

Strecker Synthesis

Answer 4

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

Question 5

Strecker Synthesis Process

Answer 5

Aldehyde or Ketone + :NH3 -> Water and Imine

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

Question 6

Transport Proteins

Answer 6

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

Question 7

Purines

Answer 7

Adenine and Guanine

Question 8

Pyrimidines

Answer 8

Cytosine and Thymine

Question 9

Difference between Purines and Pyrimidines

Answer 9

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

Question 10

Why is DNA called an acid even with Nitrogenous bases

Answer 10

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

Question 11

Saponification

Answer 11

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.

Question 12

Types of Lipids

Answer 12

Hydrolyzable and Non-hydrolyzable lipids

Question 13

4 examples of hydrolyzable Lipids

Answer 13

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

Question 14

3 examples of non-hydrolyzable lipids

Answer 14

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)

Question 15

Effect of Common ion on Solubility

Answer 15

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

Question 16

Effect of pH on solubility

Answer 16

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.

Question 17

Effect on equilibrium of solubility from pH

Answer 17

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

Question 18

Effect of dissolving NH3 and AgCl2

Answer 18

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

Question 19

Acid/base NH3 and AgCl2 explanation

Answer 19

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

Question 20

CASHNGIA Explanation

Answer 20

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

Question 21

Electromagnetic Spectrum

Answer 21

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

Question 22

RMIVUXG

Answer 22

Rose and Malik Invited Vanessa and Umar to Xtra Glasses

Question 23

Separation by Precipitation

Answer 23

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

Question 24

Trick of Ion-exchange Chromatography

Answer 24

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.

Question 25

Ionic Rules on Solubility

Answer 25

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

Question 26

Oxides and Solubility

Answer 26

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

Question 27

Phase changes and Solubility

Answer 27

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

Question 28

Colligative Properties

Answer 28

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

Question 29

Vapor Pressure

Answer 29

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

Question 30

Osmotic Pressure

Answer 30

The pressure it would take to stop osmosis from occurring

Question 31

Freezing Point Depression

Answer 31

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

Question 32

Boiling Point Elevation

Answer 32

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.

Question 33

Boiling Point

Answer 33

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

Question 34

Salt Bridge

Answer 34

1. Helps equalize and neutralize salt bridge | 2. Helps maintain balance

Question 35

Terminal and Electrodes of Voltaic/Galvanic/Electrochemical Cell

Answer 35

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

Question 36

Factors Affecting the Cathode and Anode

Answer 36

1. Ions 2. Temperature 3. Pressure 4. Concentration

Question 37

Free energy and Cell Potential Relationship

Answer 37

G = nFE

Question 38

Define Faraday

Answer 38

Magnitude of charge carried by 1 mole of Electron

Question 39

Standard Reduction Potentials

Answer 39

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

Question 40

Peculiar Property of Free energy and Standard Potential

Answer 40

Standard Potential is an intensive property (does not change) Free energy is an extensive property (changes)

Question 41

How can Activity series be explained

Answer 41

Use the standard reduction potentials

Question 42

Relate Standard Cell Potential and Equilibrium Constant

Answer 42

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

Question 43

Essence of Nernst Equation

Answer 43

To calculate the standard cell potential when in non-standard conditions: ``` G = G' + RTlnQ -nFE = -nFE + RTlnQ ```

Question 44

Standard Conditions

Answer 44

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

Question 45

STP

Answer 45

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

Question 46

Effect of Q on E

Answer 46

As Q increases, E decreases

Question 47

Terminal type and Electrode at a Electrolytic Cell

Answer 47

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

Question 48

Concentration Cell

Answer 48

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

Question 49

Difference between Voltaic/Galvanic/Electrochemical cell and Electrolytic cell

Answer 49

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

Question 50

Redox Reactions Balance

Answer 50

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.