Exam 2 Flashcards

1
Q

Standard state

A

a reference point used to calculate a substance’s properties under different conditions

1 M
1 atm

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2
Q

example of a compound in its standard state

A

CO2 is a gas in the standard state

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3
Q

Why do reactions proceed to a lower energy state when they reach equilibrium? (mathematically)

A

G = -RTln(K)

K=1 at equilibrium, so G will equal 0

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4
Q

Why do reactions proceed to a lower energy state when they reach equilibrium? (conceptually)

A

as a reaction approaches equilibrium Q=K

when Q=K, ln(Q/K)=0 and therefore G=0

*this is still very mathematical

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5
Q

G when Q

A

reaction has more reactants, needs to shift right towards the products, so G is negative

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6
Q

G when Q>K

A

reaction has more products, needs to shift left towards the reactants, so G is positive

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7
Q

G when Q=K

A

system is equilibrium, so G is 0

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8
Q

G when K>1

A

G is negative

equilibrium is a state where there are more products than reactants, so the reaction proceeds right

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9
Q

Graph when K>1

A

equilibrium is closer to products

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10
Q

Graph when K<1

A

equilibrium is closer to reactants

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11
Q

G when K<1

A

G is positive

equilibrium is a state where there are more reactants than products, so the reaction proceeds left

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12
Q

difference between ΔG° and ΔG

A

ΔG° is always the same for a reaction since it is standard conditions and only changes with K. K is a set number at equilibrium.

ΔG differs for a reaction since it is related to ln(Q/K) and Q changes. ΔG is the only one that changes as a reaction proceeds and Q changes.

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13
Q

axial hydrogens are _____ to one another

A

anti

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14
Q

equatorial hydrogens are _____ to one another

A

gauche

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15
Q

gauche

A

60 degrees

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16
Q

after a ring flip, what position does an equatorial constituent have?

A

axial

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17
Q

after a ring flip, what position does a pointing down consitutent have?

A

pointing down

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18
Q

which way do constituents “move” positions when going from right to left in ring flip?

A

clockwise

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19
Q

which way do consitiuents “move” positions when going from left to right in ring flip?

A

counter-clockwise

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20
Q

steric strain

A

the van der Waals repulsion between a substituent and nearby hydrogens

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21
Q

why is the equatorial position favored in cyclohexanes?

A

to minimize the steric strain

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22
Q

why is the equatorial position more favored when the size of the constituents increases?

A

as the steric bulk of the constituents increases, the steric strain also increases, so want to minimize this

23
Q

relationship between ΔG and A-value

A

ΔG can be called an A-value when talking about the equatorial vs. axial position

makes sense that as K increases and there are more axial conformations, ΔG becomes more negative and more stable, which means that A-value points to more axial products

^all adds up

24
Q

A-values

A

indicate how much the equatorial position is favored over the axial position

25
Relationship between ΔG and stability
the more negative ΔG is the more stable it is because it has lower free energy
26
Bronsted-Lowry acid
a substance that can donate a proton (H+)
27
Bronsted-Lowry base
a substance that can accept a proton
28
amphoteric
water's ability to act as an acid or a base
29
autoionization of water
ionize H2O to give off H+ and OH- ions
30
equilibrium constant of the autoionization of water (Kw)
1.0 * 10-14 Kw = [H3O+] [OH-] *when H3O+ > OH- solution is acidic, and vice-versa
31
Lewis acid
a compound that accepts an electron pair
32
Lewis base
a compound that donates an electron pair
33
Arrhenius acid
specifically dissociates into H+ ions in water
34
Arrhenius base
specifically dissociates into OH- ions in water
35
What do curved arrows represent?
collisions of molecules that lead to chemical reactions
36
Where do curved arrows always start?
the Lewis base (electron source)
37
Why are Lewis bases known as nucleophiles?
their negatively charged lone pairs are attracted to the positive nucleus of other atoms
38
Why are Lewis acids known as electrophiles?
their partially positive atoms are attracted to electrons
39
Carbocation
carbon with a formal + charge often a Lewis acid since positive charge is attracted to electrons
40
Acetic acid formula
CH3COOH *weak acid
41
What do we mean by stable?
lower in free energy
42
What does the "p" indicate in like pH?
indicates the -log of whatever follows it for example, pOH = -log (OH)
43
strong electrolyte
a combined name for strong bases and acids there is no equilibrium here. reaction goes to completion
44
inductive affect
ability for electronegative atoms to removed electron density from the other negatively charged constituents through SIGMA bonds can make a conjugate base more stable
45
why do stronger acids have a higher K?
they have more stable conjugate bases (weaker) so the reaction wants to go towards the products in addition, more stable conjugate bases means that enthalpy goes down, so G is most likely negative as well and the reaction will proceed right
46
what does a lower pKa indicate?
a stronger acid there is a greater concentration of H+ ions
47
when is it appropriate to make the size argument when looking at conjugate bases?
if comparing two elements that are actually carrying the negative charge ex: O- vs. S-
48
polarizability
the ability to form instant dipoles
49
relationship between polarizability and size
larger molecules are generally more polarizable than smaller molecules
50
when can you not use the polarizability argument even when looking at elements carrying the negative charge?
if the elements are in the same row of the periodic table there is not a big enough size difference need to be in different rows with different orbitals
51
what should you look at when you are examining the elements carrying the negative charge but they are in the same row?
electronegativity
52
do strong acids have a Ka or pKa?
no there is no equilibrium, so they have no Ka
53
where does the inductive effect occur?
sigma bonds with two electronegative species sharing electron density
54
where does resonance occur?
pi-bonds move electrons through the double bonds