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How Does Reaction vs Diffusion Regulate ROS/RNS Biology?
Sunrise Free Radical SchoolSociety for Free Radical Biology and Medicine
14th Annual MeetingNov. 16, 2007
J. R. Lancaster, Jr.Center for Free Radical BiologyDepartments of Anesthesiology,
Environmental Health Sciences, and Physiology & Biophysics
The University of Alabama at Birmingham
•Diffusibility
•Kinetics of Reaction
Two Properties Characteristic of Small, Uncharged, Highly Reactive Molecules
Kinetics of Reaction•Rate vs Rate Constant
•How Reactions Really Occur: Importance of Solvent Diffusion
•Sources and Sinks
•Crowding in the Cytoplasm
•Spatial Confinement of NO
•Net Movement of Collections of Molecules
•Significance of zero order kinetics
Diffusibility
How Reactions Really Occur
In order for two molecules to react, they must collide. However, of the billions of chemical reactions, only a handful are rapid enough that the reaction will occur after only a few collisions. Thus, virtually all reactions occur only after the two molecules collide in “just the right way.” In the gaseous phase, the distance between molecules is great enough to insure that molecules will separate rapidly after the collision. In the condensed phase, however (in aqueous solution or in tissue), individual molecules are surrounded by a “cage” of solvent (H2O) molecules. Thus, parts of the “walls” of these cages must move away from two solutes (reactants) in order for collisions to occur:
Once this happens, however, the molecular pair is surrounded by the solvent cage which means that during the lifetime of the cage (which is 10-10 – 10-8 sec) the reactant molecules are colliding repeatedly. This is termed an “encounter.”
If the probability of the reaction is high enough that the reaction will occur every time there is an encounter, then the rate of the reaction (the overall rate) will depend only on how fast the two molecules will form an encounter. This is called the “diffusion limit.” No reaction can occur more rapidly than this limit.
This limit is in the range 109-1010 M-1s-1 (this is the value for k). Many reactions of radicals occur at this diffusion limit.
Dk T
r4
S tokes ’ L aw :
For N O (r = 1.4 x 10 m) in H O at 37 C , D = 2740 m /s
-10
o
22
D (m 2 /s ) N O (H 2O ) 3 3 0 0
N O (B ra in ) 3 8 1 0E th a n o l 11 0 0G lu co se 5 7 0S u crose 4 6 0
M yo g lo b in 11 3H em og lo b in 6 9
Temperature (kinetic energy)
Viscosity (solvent mobility)
Solute size
The Diffusion Constant: How Fast a Molecule Moves
Compartment A
Probability for NO moving from A to B:k x [NO]aProbability for NO moving from B to A:k x [NO]bIf [NO] = [NO], No Net Movement(NO's will just "change places")If [NO] > [NO], Net Movement from A to BIf [NO] > [NO], Net Movement from B to A
a b
a bb a
NOa
NOb
Compartment B
CONCLUSION: The only thing that "makes"molecules move from one place to anotheris the presence of concentration gradients.Molecules will move "downhill".always
kk
Net Movement of Collections of Molecules
Theoretical Predictions of Diffusion in Aqueous Solution
Method 1: Analytical SolutionsMethod 2: Numerical Solutions
Analytical Solutions: based on Fick’s Laws
An Example: Diffusion away from a sphere:
The Bible: Crank “The
Mathematics of Diffusion”:
][][][ 2
NOkr
NOD
t
NO
2/1
2ln
e][
][ tDr
o
r
NO
NO
[NO]o
[NO]r
r
For a given half-life of NO, what is r if [NO]r is 50% of [NO]o?
(the shorter the half-life the faster NO disappears as it travels, and so r will decrease)
Steady-State:
.
Point Source (2 µm diameter cell)
.
0 2 4 6 8 100
1x105
2x105
3x105
4x105
5x105
Num
ber
of C
ells
Aff
ecte
d
Half-Life (sec)
For cells 2 m diameter (3.35 x 10-14 L/cell); [NO]r/[NO]o
= 0.5:
For a half-life of 5 seconds, one NO-producing cell will affect 150,000 others
0.00 0.05 0.10 0.15 0.200
200
400
600
800
1000
1200
1400
Num
ber
of C
ells
Aff
ecte
d
Half-Life (sec)
For a half-life of 0.05 seconds, one NO-producing cell will affect 150 others
Leone et al. BBRC 221:37 (96)
Porterfield et al. AJP 281:L904 (01)
Malinski et al. BBRC 193:1076 (93)
175 m
Experimental:
Cell
100 µm
Beckman in “Nitric Oxide: Principles and Actions” Lancaster, ed. (1996)
Comparison with Other Reactive Species:
NO(N+1)NO(N-1)
N-1 N N+1
k3 k3
A Numerical Solution: Illustration of the Effect of Diffusion on Reaction:
Lancaster Meth. Enz. 268:31(96)
Entry or exit will affect ONLY the concentration of the species
k4NO(N)
NO3-
NOxk2
kf
How do we incorporate diffusion?:
)(42
)()1(3)1(3)(
)(
2
Nf
NNNN
NOkkk
NONOkNOkdt
NOd
k4NO(N)
NO3-
NOxk2
kfNO(N+1)NO(N-1)
N-1 N N+1
k3 k3
Lancaster in “Nitric Oxide Biology and Pathobiology” LJ Ignarro, ed. (00)
Lancaster Meth. Enz. 268:31(96)
Sources and Sinks:
Khan et al. PNAS 101:15944(04)
Stamler et al. Cell 106:675(01)
Spatial Confinement of NO
Lancaster Meth. Enz. 268:31(96)
Only way to spatially confine NO: Change its r (reaction)
Polarographic Measurement of D:
The Ilkovic Equation:
DA only in the Nernst layer!
Is Measurement of D with Electrodes Truly Reflective of Diffusion in Cells?:
“Macromolecular Crowding: an Important but neglected Aspect of the Intracellular Environment” Curr. Opin. Struct. Biol. 11:114(01)
Crowding in the Cytoplasm
Four factors that account for slowed diffusion:-- Slowed diffusion in fluid-phase cytoplasm-- Probe binding to intracellular components-- Probe collisions with intracellular components (crowding)
What are the data?
Verkman “Solute and Macromolecule Diffusion in Cellular Aqueous Compartments” Trends Biochem Sci 27:27 (02)
Kao et al. “Determinants of the Translational Mobility of a Small Solute in Cell Cytoplasm” J Cell Biol. 120:175 (93)
Two determinants of how fast a reaction occurs: Concentrations of reactants and rate constant: kA B
Akdt
Bd
For many reactions involving radicals, rate constants (k) are very large:
Rate ConstantRate
RATE VS. RATE CONSTANT:
Kirsch et al. Chem. Eur. J. 7:3313 (01)
109
k23
k24
k22
k30
k31
k32
k33
k34
k35k-32
k27
k28
k29
k25
k26 GS
GSOOGSSG -
[GSO ]xO + Products42 -
O + Products52 -
GSH
GSOH + NO2-
GSNO +H + NO+ -
2ONOO-
GSNO
GSSG[GSOONO]
GSOONO2GSONO2
GSSG
GSNO2
NO +H
2-
+
NO2
NO2
NO2
NO2
O2
GSOO
GS
HCO3-
GSH
GS-
N O2 3
GSOH 86%14%
CO 3-
O 2-O2
NO
NO
“All” Reactions:
Most Important Biologically:
k23
k24
k22
k30
k31
k32
k33
k34
k35k-32
k27
k28
k29
k25
k26 GS
GSOOGSSG -
[GSO ]xO + Products42 -
O + Products52 -
GSH
GSOH + NO2-
GSNO +H + NO+ -
2ONOO-
GSNO
GSSG[GSOONO]
GSOONO2
GSONO2
GSSG
GSNO2
NO +H
2
-
+
NO2
NO2
NO2
NO2O2
GSOO
GS
HCO3-
GSH
GS -
N O2 3
GSOH 86%14%
CO 3-
O 2-O2
NO
NO
B
A
C
WHY?
RATE VS. RATE CONSTANTLancaster Chem Res Toxicol 19:1160 (06)
An example: Reactions of GSH with RNS
NO2
NO + O2
GS
GSNO GSNO
N O2 3
NO
NO
GSH
GSHNO2-
RATE VS. RATE CONSTANT:
109 M-1s-12 x 107 M-1s-
1
Rate Constants
1 M5000 M
Rate = 2 x 107 x 5 x 10-3 = 105 M/s
Rate = 109 x 10-
6 = 103 M/s
3 x 109 M-1s-
16.6 x 107 M-1s-
1
Rate of C formation is independent of concentration of B (“zero order” in [B]). Only determined by the rate of formation of A.
k1k2
AB
C
1
12
21
2
0
kv
kBAk
BAkkdt
Ad
BAkdt
Cdv
Significance of Zero Order Kinetics:
0 10 20 30 40 50 600
20
40
60
80
RS
NO
(pm
ol/m
g)(
)
Time (min)
0
300
600
900
[NO
] (nM
)(
)
0 10 20 30 40 50 60 700
50
100
150
200
O2 (
M)
Time (min)
0 15 30 45 600.0
2.5
5.0
7.5
10.0
O2 (M
)
Time (min)
An Experimental Example: Measurement protein RSNO in cells treated with NO donor (Sper/NO); Simultaneous measurement of O2 and NO:
Rate of RSNO Formation is Zero Order in [NO]
0 10 20 30 40 50 600
20
40
60
80
RS
NO
(pm
ol/m
g)(
)
Time (min)
0
300
600
900
[NO
] (nM
)(
)
0 10 20 30 40 50 60 700
50
100
150
200
O2 (
M)
Time (min)
0 15 30 45 600.0
2.5
5.0
7.5
10.0
O2 (M
)
Time (min)
An Experimental Example: Measurement protein RSNO in cells treated with NO donor (Sper/NO); Simultaneous measurement of O2 and NO:
Also not dependent on [O2]
Inconsistent with2NO + O2
NO +NO2
2NO2
N O2 3
N O + RSH2 3 RSNO + NO + H2- +
Consistent with
RS + NO RSNO
Charles BosworthHarry MahtaniJose ToledoBill Gates
American Cancer SocietyNIH
Sunrise Free Radical School, 2007
Society for Free Radical Biology and Medicine
14th Annual Meeting
Washington, D.C.