principles of bioenergetics -...
TRANSCRIPT
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Principles of Bioenergetics
Lehninger 3rd ed. Chapter 14
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Metabolism
• A highly coordinated cellular activity aimed at achieving the following goals: – Obtain chemical energy. – Convert nutrient molecules into the cell’s
own characteristic molecules. – Degrade biomolecules.
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Carbon Flow
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Nitrogen Flow
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Catabolism & Anabolism
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Divergence & Convergence
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Synthesis versus Degradation
• Most cells posses the enzymes to both synthesize and degrade a particular molecule. Is this not wasteful?
• No, since the cell: – Regulates each process. – Segregates their location.
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Antoine Lavoisier
“…respiration is nothing but a slow combustion of carbon and hydrogen…” (A.L. Lavoisier 1743-1794)
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Bioenergetics
• The quantitative study of cellular energy transductions and the chemical reactions underlying these transductions.
• Obviously, biological energy transductions obey the laws of Thermodynamics.
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ΔG = ΔH −TΔS
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• G: Gibbs free energy at constant temperature and pressure; Units are Joule per mole.
• H: Enthalpy; Units are Joule per mole. • Τ: Temperature; Units in Kelvins. • S: Entropy; Units are Joule per mole
times temperature in Kelvins. €
ΔG = ΔH −TΔS
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ΔG: Free Energy at constant temperature and pressure (Joules per mole)
• If ΔG < 0 then the reaction will be spontaneous. • The value of ΔG is directly related to the equilibrium
constant
• Actual free energy depends on the reactant and product concentrations: aA + bB cC + dD
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ΔG0 = −RT lnKeq
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ΔG = ΔG0 + RT ln [C]c[D]d
[A]a[B]b
12 Free energies are additive, thus a favorable reaction (ΔG1 < 0) can drive an unfavorable reaction (ΔG2 > 0), when ΔG1 + ΔG2 <0
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• According to Boltzmann: S = k ln W where W is the number of states in the system.
• Thus any reaction such as ��� aA + bB ⇌ cC + dD ���
in which a+b < c+d, can be said to be driven by entropy.
S: entropy
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C6H12O6 + 6O2 → 6CO2 + 6H2O
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Phosphoryl groups and ATP
• ATP: Adenosine triphosphate, a ribo-nucleotide, is the energy currency of the cell.
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• Relieves electrostatic repulsion between the negatively charges phosphates.
• Inorganic phosphate can be stabilized by resonance hybrid.
• ADP2- can ionize. • The products are better solvated than the
reactants.
Why is the hydrolysis of ATP highly exergonic?
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ΔG' 0 = −30.5kJ /mol
Under standard conditions:
But in the cell the phosphorylation potential ΔGp is:
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ΔGp = ΔG' 0 + RT ln [ADP][Pi][ATP]
= −51.8kJ /mol
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ATP4− +H2O→ ADP3− + Pi2− +H+
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High Energy Phosphorylated Compounds
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Thioesters hydrolysis is also highly exergonic
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Making use of ATP
• Since the ATP hydrolysis is very favorable (i.e. ΔG << 0) it can drive unfavorable reactions, but how?
• It does so not by “harnessing” the energy of hydrolysis, but rather through the coupling of group transfer.
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Biological Oxidation-Reduction
• The flow of electrons can do work. • Electrons flow from a reducing agent to an
oxidizing agent due to their different electron affinities.
• This difference in affinities is called the electromotive force (emf).
• The reducing agent undergoes oxidation and the oxidized undergoes reduction.
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Redox reactions can be described as Half-reactions:
Fe2+ + Cu2+ ⇌ Fe3+ + Cu+
(1) Fe2+ ⇌ Fe3+ + e- (2) Cu2+ + e- ⇌ Cu+
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Redox reactions in bio-chemicals
2OH-+2Cu2+ Cu2O H2O+2e-+
R
C
O
H
R
C
O
O
H
R
C
O
H
R
C
O
O
H
+ 4OH- + 2Cu2+ + Cu2O 2H2O+
+ 2OH- + 2e- H2O+
29 Electronegativity series: O > N > S > C > H
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Dehydrogenation = oxidation
• Carbon is less electronegative than all atoms it is bound to, except hydrogen.
• Thus all atoms that bind to carbon oxidize it except hydrogen.
• Thus removing a hydrogen and replacing that bond with any other atom (including carbon) is synonymous with oxidation.
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Electron transfer modes • Directly as electrons:���
Fe2+ + Cu2+ ⇌ Fe3+ + Cu+ • As hydrogen atoms:���
AH2 ⇌ A + 2e- + H+ • As a hydride ion (H-):���
AH2 + B+ ⇌ A + BH + H+ • Direct combination with oxygen:���
R-CH3 + 1/2O2 ⇌ R-CH2-OH
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Reduction potentials = e- affinity
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E = E 0 +RTnℑ
ln [electron acceptor][electron donor]
= E 0 +0.026V
nln [electron acceptor]
[electron donor]ΔG = −nℑΔE, or ΔG' 0 = −nℑΔE ' 0
ℑ = 96,480 J/V ⋅molR = 8.315 J/mol ⋅K
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Glucose oxidation is highly exergonic
• The complete oxidation of glucose is our major source of energy.���
C6H12O6 + 6O2 → 6CO2 + 6H2O • The process involves many steps each catalyzed
by a specific enzyme.���
ΔG’0 = -2,840 kJ/mol
35 NAD+, NADP+, FAD & FMN:���universal electron carriers
• NAD+ (nicotinamide adenine dinucleotide) and NADP + (phosphorylated form of NAD+) are reversal redox cofactors in which.
• In their capacity as reducing agents, the substrate undergoes a double dehydrogenation (oxidation) and NAD+ (or NADP+) accepts a hydride ion (H-), with a release of a H+ to the environment.
NAD+ + 2e- + 2H+ ⇌ NADH + H+���
CH3CH2OH + NAD+ ⇌ CH3CHO + NADH + H+
Ethanol
Acetaldehyde
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C
O
O
H
N
N
C
H
3
N
Nicotinic acid Nicotine
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FMN, FAD and flavoproteins • Flavoproteins are enzymes that use FMN or FAD
cofactors in redox reactions. • The cofactor is derived from riboflavin (vitamin
B2). • FAD and FMN can accept either 1 or 2 hydrogens,
thereby accepting 1 or 2 electrons, and are therefore more versatile than NAD+ or NADP+.
• The fully reduced forms are written as FADH2 and FMNH2
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N
N
N
H
C
H
3
C
H
3
N
O
O
C
H
2
C
H
O
H
C
H
O
H
C
H
O
H
C
H
2
O
H
Riboflavin (B2)
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