Lectures 22/23: Redoxreactions and Oxidative Phosphorylation Flashcards
Glutamate dehydrogenase
Catalyzes the reversible conversion of ketoglutarate and glutamate
Can be cataplerotic or anaplerotic
Pyruvate carboxylase
Catalyses irreversible reaction of pyruvate to oxaloacetate
Anaplerotic and gluconeogenic enzyme
Anaplerotic carboxylation
Conversion of pyruvate to oxaloacetate by pyruvate carboxylase
Acetyl-CoA
Oxidation of pyruvate to acetyl-CoA is irreversible
High levels inhibit pyruvate dehydrogenase
High levels activate pyruvate carboxylase: converted to citric acid cycle intermediates that are glucogenic
Glucogenic
Metabolites that can be converted to glucose through gluconeogenesis
Ketogenic
Metabolites that cannot be converted to glucose through gluconeogenesis
Oxidation
Loss of electrons
Oxidation NADH and QH2 generate ATP
Reduction
Gain of electrons
Redox through transfer of a hydride ion
Niacin
Vitamin B3
Nicotinamide
Nicotinamide adenine dinucleotide
NAD+
NADH carries two electrons that it can give up easily
In oxidative phosphorylation, reduces O2 to H2O to drive formation of ATP
FAD
Accepts two protons and two electrons to become FADH2
No change in charge of the molecule
Riboflavin (vitamin B12)
FADH2 reduced Q to QH2: carries two electrons that it can give up easily
In oxidative phosphorylation, reduces O2 to H2O to drive formation of ATP
Reduction potential
Tendency of a substance to accept electrons to become reduced
Measured in volts
Higher means that substance is more easily reduces and is a stronger oxidant
Rejects energy change that would occur if electrons were transferred
Written as a half reaction
Standard reduction potential
Reduction of potential of substances under standard conditions
Standard reduction potential E*’ is a characteristic of each redox active substance and reflects its affinity for electrons
Oxidation potential
Opposite in sign to standard reduction potential
Positive reduction potential
Higher: greater tendency to accept electrons and therefore become reduced
Negative reduction potential
Most negative: least tendency to accept electrons and become reduced
Electrons flow spontaneously from a species with a more negative E’ to a species with a more positive E’
Nernst Equation
Defines actual reduction potential
deltaE*’
deltaE’= E’ (e acceptor) - E*’ (e donor)
Spontaneous when positive
Standard free energy change
deltaG’= -nFdeltaE’
Spontaneous when deltaE’ is positive and deltaG’ is negative
Oxidative phosphorylation
Takes place in mitochondria
Occurs over the inner membrane
Proteins accumulate in inter membrane space
Series of redox reactions generates protein gradient to fuel ATP synthesis: electrons passed down electron transport chain of complexes I-IV
Protons flow back into mitochondrial matrix through complex V (ATP synthase) and fuel the synthesis of ATP
Inner membrane
Proton-Rich
Impermeable to several metabolites (ATP, ADP) and ions (H, OH, K, Cl, Phosphate) and fully permeable to O2, H20, CO2
Compartmentation of mitochondria
Allows pathway control through controlling the localization of metabolites
Special transport systems to transport metabolites
NADH made during glycolysis must get to the mitochondrial matrix to by reoxidizes and ATP made in mitochondrial matrix must be transported into the cytosol (ADP and P must get to matrix from cytosol)
Malate-aspartate shuttle
Interaction of cytosolic malate dehydrogenase and matrix malate dehydrogenase to transport NADH to mitochondrial matrix via oxidation of malate to oxaloacetate
Complex I
Transfers electrons from NADH to H and transports 4H into inter membrane space
Energy release by oxidation of NADH used to transport H using proton pump
H transport is against concentration and charge gradient: requires energy
NADH - FMN - Fe-S - Q