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Final Flashcards

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
What are the complexometric titration indicators?
Eriochrome Black T Murexide
26
What methods can be used to quantitatively determine the concentration of an oxalic acid?
acidi-alkalimetry permanganometry
27
Can a carbonyl group act as a nucleophile?
YES
28
Lactic, malic and beta-hydroxy-butyric acids are all...
chiral
29
What is a geometric isomer?
cis/trans
30
What happens in an addition rxn generally?
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)
31
What is a heteroatom?
Some atom other than H or C in an organic compound
32
What reacts with an aldehyde to form an oxime?
hydroxylamine
33
What is markovnikovs rule?
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)
34
What is Zaitsev's rule?
When asymmetrical alcohols or alkyl halides undergo elimination rxns, the H leaves from the beta carbon with LESS H atoms attached ex: 2-pentanol
35
Ketones can't oxidize to...
carboyxlic acids
36
What forms oxaloacetic acid via dehydrogenation?
malic acid
37
How does an anhydride look?
central O bonded to 2 carbonyl (C=O) with 2 R groups
38
What forms from phenol and alcohol? from 2 alcohols?
- phenol**ether** (some kind of ether) - ether
39
What is lugols solution?
I2 and KI in water
40
What is the freezing point depression equation?
**ΔTfp = Osm x 1.86**
41
What happens to specific conductance of weak electrolytes with dilution?
it DECREASES
42
What kind of rxns do aromatic hydrocarbons tend to undergo?
**electrophilic substitution**
43
What is the max number of bonds sulphur can form?
6
44
What kind of compounds can saturate an alkene's double bond?
halogens (ex: Cl2) Hydrogen-halogenides (ex: HCl) Water Molecular Hydrogen w/ catalyst
45
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)
Emf = 0.06(pHanode - pHcathode)
46
What are the functional groups in a quinone?
**carbonyls**
47
How does a catalyst affect a reaction?
* changes mechanism * decreases activation energy * changes rate constant
48
What is the product of an alcohol and a ketone?
**hemiketale**
49
What is the formula for osmotic pressure?
**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
Is the overall rate of a multistep rxn the sum of the exponents of the concentration in the rate eqns of each reaction?
....no
51
What is a redox electrode and what is the eqn for calculating its potential?
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
What 2 oxides of nitrogen are free radicals?
NO and NO2
53
Does carboxyl group form an H bridge with H2O, making carboxylic acids miscible with water?
NO
54
How does voltage of a cell relate to the oxidizing capabilities of its components?
Higher voltage means its a STRONGER cathode and thus is more readily reduced and is a STRONGER OXIDIZER
55
What special group do acetone and oxaloacetic acid contain?
oxo groups =O
56
What is special about tartarate, isocitrate and 1,2-dimethylcyclohexane?
they have more than one chiral center
57
What do malic, citric and lactic acids have in common?
they are hydroxycarboxylic means they have an -OH and a -COOH
58
What is a meso compound?
something with n \> 1 chiral centers but less than 2n stereoisomers
59
what is the eqn for boiling point elevation?
**ΔTbp = Osm \* 0.512**
60
what is the osmolarity of blood?
0.3
61
What is the Nernst equation for the electrode potential of a half cell?
E = E° + (0.06/Z) log C
62
How is pH determined if concentration and pKa are known?
**pH = (pKa - log C)/2**
63
How can pH be determine with Ka and concentration?
**[H+] = √(Ka \* C)**
64
What is the first law of thermodynamics?
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
What is the 2nd law of thermodynamics?
The entropy of the universe does not change for reversible processes and increases for spontaneous processes. (entropy can decrease for individual systems, though)
66
What is the third law of thermodynamics?
The entropy of a pure crystalline substance at 0 Kelvin is zero.
67
What is the Daniell cell and its voltage?
Cu/CuSO4 cathode, Zn/ZnSO4 anode 1.1 V
68
What is Hess' law?
the change in enthalpy for any chemical reaction is the same whether the reaction occurs in one or several steps
69
What is the equation that relates Gibbs free energy to the equilibrium constant (K) of a chemical reaction ?
ΔG = -5.7 log K this produces an answer in kJ/mole (based on ΔG = RT ln K)
70
What are reversible and irreversible processes?
**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
What indicator is used for pH of about 3.5?
Methyl Orange
72
What indicator is used for pH of about 7?
Bromophenol blue
73
What indicator is used for basic pHs of about 10?
phenolphthalein
74
What indicator is used for pH of around 5?
methyl red
75
What must always be accounted for when calculating the pH of very dilute acid or base solutions? Why?
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
What are the -1 "ates"?
Br Cl N Bro Clown
77
What are the -2 "ates"?
Si C Cr S Sick Chris
78
What are the -3 "ates"?
B P As (if you get a ) B (you will) Pass
79
What are the 3 oxygen "-ates"?
Cl Br Si C N B Clobber Sick Newb
80
What are the 4 oxygen "-ates"?
Cr P As S Crap Ass
81
What are the -1 "ides"?
F I Cl H Br Fickle Hebrew
82
What are the -2 "ides"?
S O So...
83
What are the minus 3 "ides"?
N P No problem
84
What are the +1 cations?
Cs Rb Li K Fr Au Na H Ag Cuss Rub Lick Frown A Hag
85
What are the +2 cations?
Ca Zn Ba Mg Casbah Mug (oops no n...)
86
What are the +3 cations?
B Al Ball
87
Explain the rules of the **-ous/-ic system**
* 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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