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MCAT Biochem (Mine) > Chapter 3: Biochem Basics > Flashcards

Chapter 3: Biochem Basics Flashcards

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MCAT flashcards
1
Q

What are the two forms of energy in chemistry?

A
  1. Kinetic energy
  2. Potential energy
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2
Q

What is the equation for Gibbs free energy?

A

Delta G = delta H - T delta S (T represents temp & H represents enthalpy)

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3
Q

What is the equation for enthalpy?

A

Delta H = delta E + PdeltaV (E represents the bond energy of products in the system & P is pressure, & V is volume)

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4
Q

Delta G increases when delta H _________ & decreasing with increasing entropy

A

Increases

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5
Q

Delta G is spontaneous when its ________ & nonspontaneous when its __________

A

Negative, positive

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6
Q

The value of delta G depends on the _____________ of the reactants & products

A

concentration

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7
Q

What is the equation for delta G related to equilibrium constant

A

delta G = -RT lnKeq

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8
Q

If we wanted to calculate the delta G for a reaction in the body what is the equation?

A

delta G = delta G prime + RT ln Q (Q uses the actual concentration of the products & reactants not the equilibriums)

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9
Q

All reactions proceed through a ___________________ that is unstable & takes a lot of energy to produce

A

transition state (TS

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10
Q

The __________________ is the energy required to produce the transition state

A

Activation energy (Ea)

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11
Q

A catalyst lowers the Ea of a reaction ___________ changing the delta G

A

Without

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12
Q

Oxidation is a ________ of electrons & Reductions are a _______ of electrons

A

Loss, Gain

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13
Q

How do you recognize oxidation reactions?

A
  1. Gain of oxygen atoms
  2. Loss of hydrogen atoms
  3. Loss of electrons
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14
Q

How do you recognize reduction reactions?

A
  1. Loss of oxygen atoms
  2. Gain of hydrogen atoms
  3. Gain of electrons
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15
Q

What is the Bronsted -Lowry definition of acids & bases?

A

Acids are proton (H+) donor & bases are proton (H+) acceptors

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16
Q

What is the lewis acid & base definition?

A

Acids are electron-pair acceptors & bases are electron pair donors

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17
Q

The larger the Ka value the _____________ the acid & the smaller the Ka value the ____________ the acid

A

Stronger, weaker

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18
Q

The lager the Kb value the __________ the base and the smaller the Kb the _________ the base

A

Stronger, weaker

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19
Q

Amphoteric substances

A

Substances that can act as a base & acid

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20
Q

The acid with the lower pKa is the __________ acid & the base with the lower pKb is the ___________ base

A

Stronger

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21
Q

Buffer

A

Is a solution that resist changing pH when small amount of acid or base is added

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22
Q

The buffer system for our blood plasma is the ____________

A

Bicarbonate system

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23
Q

Gibbs free energy is the amount of energy in a reaction available to do ___________ work

A

Chemical

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24
Q

If delta G equal 0 means what

A

Its at equilibrium

25
Q

_________ is the study of how quickly a reaction occurs but its does not determine whether or not a reaction will occur

A

Kinetics

26
Q

A __________ lowers the energy of the transition state, which decreases the Ea and increases the amount of product formed per unit of time

A

catalyst

27
Q

When a reaction is favorable (or spontaneous) means it will occur in the ___________ direction

A

Forward

28
Q

When a reaction is unfavorable (or nonspontaneous) means it will occur in the ___________ direction

A

Reverse

29
Q

In a reaction if there is a compound that has been oxidized or reduce then it means its a __________ pair

A

redox

30
Q

When an molecule is in its standard state (ex. O2) its oxidation state is __________ but when its in a compound its oxidation will be positive or negative

A

zero

31
Q

When dealing with the Bicarbonate buffer system when you hold your breath what happens?

A

When you hold your breath the CO2 concentration in your blood increase which will increase H2CO3 (carbonic acid) which will decrease the pH

32
Q

Kinetic energy comes from __________ of molecules

A

Movement

33
Q

Potential energy comes from energy stored in _________ bonds

A

Chemmical

34
Q

1st law of thermodynamics

A

States that the energy of the universe is constant (when energy of the system decrease the energy of the surroundings increase)

35
Q

2nd law of thermodynamics

A

States that the disorder (entropy) of the universe tends to increase (spontaneous reactants tend to increase the disorder of the universe)

36
Q

Favorable reactions have a _________ delta G

A

Negative

37
Q

Reactions with a negative delta G are _____________ & reactions with a positive delta G are ________

A

Exergonic (energy leaves the system), endergonic (energy is added)

38
Q

The sign of thermodynamic quantities depends on the point of view of the _________

A

System (not the surroundings)

39
Q

A negative delta G means that the system will go to a _________ free energy state ( & a system always moves in the direction of the lowest free energy )

A

Lower

40
Q

A ____________ Keq means that more products are present at equilibrium & equilibrium tends to move toward the lowest energy state so when Keq is ______ products have lower free energy than reactants

A

Large

41
Q

_____ is irrelevant to free energy of products & reactants only Keq is

A

Q

42
Q

At equilibrium how is Q related
to Keq?

A

Its equal (Q=Keq) so forward reaction rate = reverse reaction rate & the net concentrations of reactants & products don’t change

43
Q

When delta G = 0 what does it mean for the reaction

A

Its at equilibrium so it occurs at the same rate for the forward & reverse reactions

44
Q

Enzymes only have a kinetic role not a thermodynamic so it will only affect the ______ not concentration of products & reactants

A

rate

45
Q

When oxidation occurs so does a ___________ reaction an

A

Reduction (redox pair)

46
Q

What is the bicarbonate buffer system

A
  1. H2CO3 ———-> H+ CO3
  2. CO2 +H2O —–> H2CO3
47
Q

A positive delta S means what?

A

Increase in disorder

48
Q

A negative delta S means what?

A

An increase in order (but entropy is favorable when its an increase in disorder)

49
Q

When delta G is negative but delta H is positive what can that tell you?

A

That its working against the reaction since a positive delta H means an input of energy but a negative delta G means its spontaneous & happens on its own

50
Q

A more negative delta G means what?

A

An increase in spontaniety

51
Q

A negative delta H means what & a positive delta H means what>?

A

Positive means its endothermic (input of energy due to bonds forming) & negative means it’s exothermic (energy released due to bonds breaking which would increase the disorder (positive delta S)

52
Q

1st law of thermodynamics

A

The energy of the universe is constant (where energy of the system decrease the energy of the surroundings increase)

53
Q

2nd law of thermodynamics

A

The entropy tends to increase

54
Q

The value of delta G depends on _______________ of reactants & products

A

Concentrations

55
Q

_____ is the concentration at any point & k is the concentration at equilibrium

A

Q

56
Q

Even though a reaction may be spontaneous it will be slow due to what?

A

A large activation energy

57
Q

When one atom is reduced another must be __________

A

Oxidized (redox pair)

58
Q

Any anion or any neutral species with a lone pair of electrons can function as a _______

A

Base

59
Q

Hassel Balch equation

A

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

MCAT Biochem (Mine) (4 decks)

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