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Final Flashcards

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1
Q

What are the characteristics of SN1 reactions?

A
  • 2 steps: bond breaks… bond is made
  • 1st order rate
  • happens more with tertiary, less with secondary, not at all with primary leaving grps
  • results in racemization at stereocenter
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2
Q

What are some characteristics of SN2 rxns?

A
  • 1 step: bond broken and made simultaneously
  • inverts stereoconfiguration (via backside attack)
  • most likely with primary, less with secondary, impossible with tertiary leaving grps
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3
Q

How does an aldehyde look?

A
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4
Q

How does a ketone look and what is its suffix?

A

“-one”

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5
Q

What does carboxylic acid look like?

A

(hydroxyl and aldehyde)

also known as carboxyl group -COOH

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6
Q

What is a carbonyl group?

A

C=O

can be aldehydes, ketones, carboxylic acids etc.

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7
Q

What do an alcohol and aldehyde form via nuc. addition?

A

hemiacetal

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8
Q

What do hemiacetals plus alcohol minus water form via nuc. sub.?

A

acetal

(2 ethers in a row)

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9
Q

What do alcohols plus ketones form?

A

hemiketal

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10
Q

What do hemiketals plus alcohol minus water form?

A

ketals

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11
Q

What do primary, secondary and tertiary alcohols oxidize to?

A
  1. primary - aldehydes (or carbox. acids)
  2. secondary - ketones
  3. tertiary - don’t oxidize
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12
Q

How do enols and phenols compare pH wise to alcohols?

A

they are stronger acids

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13
Q

How are ethers named?

A

name the substituent on either side of the O atom and then add “ether”

ex: ‘phenol methyl ether’ has a phenol and a methyl grp attached to the central O

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14
Q

What happens in an organic oxidation rxn?

A

usually an O is added or two Hs are lost

(seems counterintuitive, but look at oxi state of C)

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15
Q

What is a disulfide bridge?

A

2 single-bonded sulphurs which connect 2 R groups

(middle structure below)

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16
Q

What is the formula for Ksp?

A

If rxn is XaYb (s) = aX (aq) + bY (aq) then…

Ksp = [X]a[Y]b

(in other words, ignore the solid and raise the concentrations of the aqueous products to their stoichiometric coeffs)

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17
Q

What is the formula for enthalpy change of a solution?

A

ΔHsoln = ΔHhydration + ΔHlattice

  • Hydration enthalpy is usually exothermic (negative)
  • Lattice energy is usually endothermic (positive) because energy must be put in to break lattice structure
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18
Q

What is the Henderson-Hasselbalch for pOH?

As in, if given pKb …

A

pOH = pKb + log [HB+]/[B]

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19
Q

What is the Henderson Hasselbalch equation for buffers?

A

pH = pKa + log [A-]/[HA]

(remember salt over acid)

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20
Q

What is the bunsen coefficient?

A

the number of ml of a gas (under standard conditions) soluble in 1 ml solvent at given temperature and 1 atm pressure

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21
Q

What is are the two formulas for Gibbs free energy?

(one concerning enthalpy/entropy and one concerning equilibrium constant)

A

ΔG = ΔH - TΔS

ΔG = -RT ln K

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22
Q

What is the equation for Emf of a concentration cell?

A

Emf = 0.06/z * log (Ccat/Can)

or

Emf = 0.06/z * log (C1/C2)

where C1 is > C2

and z = charge differene between oxidized and reduced form

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23
Q

Where is hydrogen gas formed in a system of hydrogen electrodes?

A

at the positive pole

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24
Q

If given standard potentials of half cells and asked to determine which reactions concerning those half cells are spontaneous, how can this be determined?

A

If standard potential is negative, then an oxidation reaction is spontaneous (remember ANode OXidation)

If standard potential is positive, then a reduction is spontaneous (remember REDuction CAThode)

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25
Q

What are the complexometric titration indicators?

A

Eriochrome Black T

Murexide

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26
Q

What methods can be used to quantitatively determine the concentration of an oxalic acid?

A

acidi-alkalimetry

permanganometry

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27
Q

Can a carbonyl group act as a nucleophile?

A

YES

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28
Q

Lactic, malic and beta-hydroxy-butyric acids are all…

A

chiral

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29
Q

What is a geometric isomer?

A

cis/trans

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30
Q

What happens in an addition rxn generally?

A

A double bond breaks via something like HCl … the H goes on the C with more Hs …. the Cl goes on the C with less

(Markovnikov’s rule)

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31
Q

What is a heteroatom?

A

Some atom other than H or C in an organic compound

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32
Q

What reacts with an aldehyde to form an oxime?

A

hydroxylamine

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33
Q

What is markovnikovs rule?

A

In addition reactions using H-containing molecules, the H bonds to the C atom of the double bond with MORE Hs attached

Ex: Propene plus HCl becomes 2-chloropropane (bc H from HCl bonds to end C w/ more Hs)

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34
Q

What is Zaitsev’s rule?

A

When asymmetrical alcohols or alkyl halides undergo elimination rxns, the H leaves from the beta carbon with LESS H atoms attached

ex: 2-pentanol

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35
Q

Ketones can’t oxidize to…

A

carboyxlic acids

36
Q

What forms oxaloacetic acid via dehydrogenation?

A

malic acid

37
Q

How does an anhydride look?

A

central O bonded to 2 carbonyl (C=O) with 2 R groups

38
Q

What forms from phenol and alcohol?

from 2 alcohols?

A
  • phenolether (some kind of ether)
  • ether
39
Q

What is lugols solution?

A

I2 and KI in water

40
Q

What is the freezing point depression equation?

A

ΔTfp = Osm x 1.86

41
Q

What happens to specific conductance of weak electrolytes with dilution?

A

it DECREASES

42
Q

What kind of rxns do aromatic hydrocarbons tend to undergo?

A

electrophilic substitution

43
Q

What is the max number of bonds sulphur can form?

A

6

44
Q

What kind of compounds can saturate an alkene’s double bond?

A

halogens (ex: Cl2)

Hydrogen-halogenides (ex: HCl)

Water

Molecular Hydrogen w/ catalyst

45
Q

What is the equation for Emf of a concentration cell of two hydrogen electrodes?

(or any cell where both solutions are acidic and pH can be calculated)

A

Emf = 0.06(pHanode - pHcathode)

46
Q

What are the functional groups in a quinone?

A

carbonyls

47
Q

How does a catalyst affect a reaction?

A
  • changes mechanism
  • decreases activation energy
  • changes rate constant
48
Q

What is the product of an alcohol and a ketone?

A

hemiketale

49
Q

What is the formula for osmotic pressure?

A

π = Osm * R * T

In these relationships, R = 8.3145 J/k mol is the normal gas constant and R’= 0.0821 L atm/K mol is the gas constant expressed in terms of liters and atmospheres.

50
Q

Is the overall rate of a multistep rxn the sum of the exponents of the concentration in the rate eqns of each reaction?

A

….no

51
Q

What is a redox electrode and what is the eqn for calculating its potential?

A

A redox electrode contains both the oxidized and reduced form of an ion in its solution. (ex: Fe2+ and Fe3+)

E = E° + (0.06/Z) log (Cox/Cred)

52
Q

What 2 oxides of nitrogen are free radicals?

A

NO and NO2

53
Q

Does carboxyl group form an H bridge with H2O, making carboxylic acids miscible with water?

A

NO

54
Q

How does voltage of a cell relate to the oxidizing capabilities of its components?

A

Higher voltage means its a STRONGER cathode and thus is more readily reduced and is a STRONGER OXIDIZER

55
Q

What special group do acetone and oxaloacetic acid contain?

A

oxo groups

=O

56
Q

What is special about tartarate, isocitrate and 1,2-dimethylcyclohexane?

A

they have more than one chiral center

57
Q

What do malic, citric and lactic acids have in common?

A

they are hydroxycarboxylic

means they have an -OH and a -COOH

58
Q

What is a meso compound?

A

something with n > 1 chiral centers but less than 2n stereoisomers

59
Q

what is the eqn for boiling point elevation?

A

ΔTbp = Osm * 0.512

60
Q

what is the osmolarity of blood?

A

0.3

61
Q

What is the Nernst equation for the electrode potential of a half cell?

A

E = E° + (0.06/Z) log C

62
Q

How is pH determined if concentration and pKa are known?

A

pH = (pKa - log C)/2

63
Q

How can pH be determine with Ka and concentration?

A

[H+] = √(Ka * C)

64
Q

What is the first law of thermodynamics?

A

the change in the internal energy of a closed system is equal to the amount of heat supplied to the system, minus the amount of work done by the system on its surroundings

65
Q

What is the 2nd law of thermodynamics?

A

The entropy of the universe does not change for reversible processes and increases for spontaneous processes.

(entropy can decrease for individual systems, though)

66
Q

What is the third law of thermodynamics?

A

The entropy of a pure crystalline substance at 0 Kelvin is zero.

67
Q

What is the Daniell cell and its voltage?

A

Cu/CuSO4 cathode, Zn/ZnSO4 anode

1.1 V

68
Q

What is Hess’ law?

A

the change in enthalpy for any chemical reaction is the same whether the reaction occurs in one or several steps

69
Q

What is the equation that relates Gibbs free energy to the equilibrium constant (K) of a chemical reaction ?

A

ΔG = -5.7 log K

this produces an answer in kJ/mole

(based on ΔG = RT ln K)

70
Q

What are reversible and irreversible processes?

A

Reversible - the system changes in such a way that the system and surroundings can be put back in their original states by exactly reversing the process

Irreversible - cannot be undone by exactly reversing the change to the system (all spontaneous processes are irreversible)

  • In irreversible process below, replacing the partition would not create the same two compartments. Work must be done to void the left compartment of gas.
71
Q

What indicator is used for pH of about 3.5?

A

Methyl Orange

72
Q

What indicator is used for pH of about 7?

A

Bromophenol blue

73
Q

What indicator is used for basic pHs of about 10?

A

phenolphthalein

74
Q

What indicator is used for pH of around 5?

A

methyl red

75
Q

What must always be accounted for when calculating the pH of very dilute acid or base solutions?

Why?

A

the H+ and OH- content of water

because without it, a very dilute acid may appear to be pH > 7 and a very dilute base may appear to be pH < 7

76
Q

What are the -1 “ates”?

A

Br Cl N

Bro Clown

77
Q

What are the -2 “ates”?

A

Si C Cr S

Sick Chris

78
Q

What are the -3 “ates”?

A

B P As

(if you get a ) B (you will) Pass

79
Q

What are the 3 oxygen “-ates”?

A

Cl Br Si C N B

Clobber Sick Newb

80
Q

What are the 4 oxygen “-ates”?

A

Cr P As S

Crap Ass

81
Q

What are the -1 “ides”?

A

F I Cl H Br

Fickle Hebrew

82
Q

What are the -2 “ides”?

A

S O

So…

83
Q

What are the minus 3 “ides”?

A

N P

No problem

84
Q

What are the +1 cations?

A

Cs Rb Li K Fr Au Na H Ag

Cuss Rub Lick Frown A Hag

85
Q

What are the +2 cations?

A

Ca Zn Ba Mg

Casbah Mug (oops no n…)

86
Q

What are the +3 cations?

A

B Al

Ball

87
Q

Explain the rules of the -ous/-ic system

A
  • lower oxidation number uses the suffix “-ous”
  • higher oxidation numbers uses the suffix “-ic”

​

Oxidation numbers:

  • ferrous/ferric = Fe2+/Fe3+
  • cuprous/cupric = Cu+/Cu2+
  • mercurous/mercuric = Hg+/Hg2+

Z Old Medical Chemistry (9 decks)

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