1 Rate Analysis of Oxygen Dissociation from Native and Oxy-Cobalt Myoglobin Advanced Inorganic Chemistry, Johns Hopkins University 3003 North Charles Street, Baltimore, MD 21218 [email protected] Jamal N. Shillingford
Dec 14, 2015
1
Rate Analysis of Oxygen Dissociation from Native and Oxy-Cobalt Myoglobin
Advanced Inorganic Chemistry, Johns Hopkins University3003 North Charles Street, Baltimore, MD 21218
[email protected] N. Shillingford
2
Myoglobin is a globular protein responsible for reversible binding and transport of oxygen through the muscles of the body by use of an iron containing heme cofactor.
The cobalt(II) analog of myoglobin can also reversibly bind molecular oxygen, forming 1:1 adducts with this ligand. Studies have shown that oxygen binding occurs at a comparable rate to that of the iron species, but there is a significant difference between their rates of oxygen dissociation.
In this study, I explore the disparity in the rates of oxygen dissociation of the two complexes in their conversion from the oxygenated to the deoxygenated forms. There is expected to be a faster rate of dissociation for the cobalt analog due to weaker binding of the oxygen to the metal center.
Abstract
H
Co(III)Mb-O2Co(II)Mb + O2
kon
koff
Fe(III)Mb-O2Fe(II)Mb + O2koff
kon
Vs.
3
CoIIMb
heme
Cobalt (II)
Histidine 93
Histidine 64
Protoporphyrin IX
Cobalt (II) Myoglobin Protein Structure
4
Active Sites of oxy-FeMb and oxy-CoMb
O2
2.17 Å
2.06 Å
2.77 Å
3.01 Å
2.95 Å
2.72 Å
Brucker, Eric A.; Olson, John S.; Phillips, George N. Jr. J. Bio. Chem. 1996, 271, 25419-25422
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Dissociation of Oxygen from Cobalt Myoglobin
chemed.chem.purdue.edu/.../1biochem/blood3.html
6
Method
Na2S2O4
Oxymyoglobin was prepared by dissolving a measured amount in minimal buffer, and adding excess sodium dithionite. It was then passed through a G-25 Sephadex column for purification.
Known concentrations of both the hydrosulfite solution and the diluted myoglobin species were mixed in a vial and immediately added to a cuvette, where the reaction was monitored kinetically at predetermined wavelengths.
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Absorption Spectrum for oxyCoMb and deoxyCoMb
Wavelength (nm)375 400 425 450 475 500 525 550
Abs
orba
nce
(AU
)
0.025
0.05
0.075
0.1
0.125
0.15
0.175
0.2
0.225
0.25
42
6
35
2
53
2
57
0
38
0
Wavelength (nm)200 300 400 500 600 700 800 900
Abs
orba
nce
(AU
)
0
0.5
1
1.5
2
2.5
3
3.5
4
40
6
55
5
48
54
92
48
432
3
Wavelength (nm)350 400 450 500 550 600
Abs
orba
nce
(AU
)
0
0.5
1
1.5
2
2.5
3
3.5
35
6
53
8
57
1
48
54
92
48
2 55
6
Wavelength (nm)520 540 560 580 600
Abso
rban
ce (A
U)
0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
538
571
556
OxyCoMb DeoxyCoMb
Porphyrin лл*
N-band Soret-band
Q-band
d d
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Crystal Field Splitting and Distortion
A. Eaton and J. Hofrichter, in Methods in Enzymology, Vol. 76, Academic Press, 1981.
eg
t2g
b1g (d x2-y
2)
a1g (d z2)
eg (dxz,dyz)
eg (dxy)
3d
Free metal Octahedral field
Tetragonal field
Rhombic field
d yz
d xz
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Crystal Field Analysis
Deoxy-Fe(II)Mb
(3d6, s=2)
high spin
weak field
d x2-y
2
d z2
d yzd xz
d xy
d x2-y
2
d z2
d yz
d xz
d xy
Oxy-Fe(II)Mb
(3d6, s=0)
low spin
strong field
d x2-y
2
d z2
d yz
d xz
d xy
Deoxy-Co(II)Mb
(3d7, s=1/2)
low spin
strong field
d x2-y
2
d z2
d yz
d xz
d xy
Oxy-Co(II)Mb
(3d7, s=1/2)
low spin
strong field
A. Eaton and J. Hofrichter, in Methods in Enzymology, Vol. 76, Academic Press, 1981.
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Absorption Spectrum for oxyMb metMb
543
Wavelength (nm)350 375 400 425 450 475 500 525 550
Abs
orba
nce
(AU
)
0
0.02
0.04
0.06
0.08
0.1
0.12
0.14
0.16 411
485
463
596
572
462
λmax OxyMb
λmax metMb
At low concentrations of dithionite (< 3.6 mM in solution), oxymyoglobin is observed to convert to the metmyoglobin species, with release of superoxide, rather than oxygen.
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Absorption Spectrum of oxyMbdeoxyMb
Wavelength (nm)400 425 450 475 500 525 550 575
Abs
orba
nce
(AU
)
0
0.02
0.04
0.06
0.08
0.1
0.12
0.14
0.16
433
485
584
578
488
596
591
At a high concentration of dithionite (≈ 12 mM in solution), oxymyoglobin is observed to convert to the deoxygenated form, which indicates release of oxygen rather than superoxide.
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Wavelength (nm)400 500
Ab
sorb
an
ce (
AU
)
0
0.05
0.1
0.15
0.2
0.25
0.3
Absorbance ChangesoxyCoMbdeoxyCoMb
Isosbestic point
426 nm
407 nm
532 nm 571 nm
555 nm
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Kinetic Results (Cobalt Myoglobin)
Time(s)100 200 300 400 500
Abs
orba
nce
(AU
)
0.06
0.08
0.1
0.12
0.14
0.16
0.18
Measurements performed using a UV-Visible Spectrophotometer (pH 7.0, 22°C).
426 nm
(oxyCoMb)
407 nm
(deoxyCoMb)
1.7516 μM oxyCoMb + 12 mM sodium Dithionite
Time(s)100 200 300 400 500
Abs
orba
nce
(AU
)
0.04
0.06
0.08
0.1
0.12
0.14
0.16
0.18
0.2
1.7516 μM oxyCoMb + 3.6 mM sodium Dithionite
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Time(s)100 200 300 400 500
Abs
orba
nce
(AU
)
0.02
0.04
0.06
0.08
0.1
0.12
0.14
0.16
0.18
Kinetic Results (Native Myoglobin)
Measurements performed using a UV-Visible Spectrophotometer (pH 7.0, 22°C).
417 nm
(oxyMb)
409 nm
(deoxyMb)
1.2577 μM oxyMb + 3.6 mM sodium Dithionite
1.1913 μM oxyMb + 1.2 mM sodium Dithionite
Time(s)100 200 300 400 500 600 700 800
Abs
orba
nce
(AU
)
0.02
0.04
0.06
0.08
0.1
0.12
0.14
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Calculation of x
x(ε426nm OxyCoMb) + y(ε426nm deoxyCoMb) = A1/Ci
x(ε407nm OxyCoMb) + y(ε407nm deoxyCoMb) = A2/Ci
x is a fractional concentration and y= 1-x
x(ε426nm OxyCoMb) + (1-x)(ε426nm deoxyCoMb) = A1/Ci
x(ε426nm OxyCoMb) + (-x)(ε426nm deoxyCoMb) + (ε426nm deoxyCoMb)= A1/Ci
x(ε426nm OxyCoMb- ε426nm deoxyCoMb) + (ε426nm deoxyCoMb)= A1/Ci
x(ε426nm OxyCoMb- ε426nm deoxyCoMb) = A1/Ci - (ε426nm deoxyCoMb)
x = A1/Ci - (ε426nm deoxyCoMb)
(ε426nm OxyCoMb- ε426nm deoxyCoMb)
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-16
-15.5
-15
-14.5
-14
-13.5
0 50 100 150 200
y = -13.721 - 0.0115x R2= 0.9943
ln(x
)
Time (s)
Approximation of Dissociation Rate Constant
At atmospheric levels of O2 (≈ 234 μM), the dissociation rate of the axial ligand at the sixth coordinate position is approximately one order of magnitude faster in the Cobalt containing analog compared to the native species.
Measurements were conducted using a UV-visible spectrophotometer (22 °C, pH 7.0, 12 mM Sodium Dithionite)
(1.7516 μM) OxyCoMb DeoxyCoMb
Koff =
(1.115 + 0.001) x 10-2 s-
-14.9
-14.8
-14.7
-14.6
-14.5
-14.4
-14.3
-14.2
-14.1
0 100 200 300 400 500 600
y = -14.222 - 0.0010685x R2= 0.99353
ln (
x)Time (s)
Koff =
(1.069 + 0.007) x 10-3 s-
(1.2356 μM) OxyMb DeoxyMb
t1/2 = 62 s t1/2 = 648 s
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Interaction between the Metal Center and Oxygen
Superoxide ion
CoII
O
O
His64
His93
Na2S2O4, 2H+
CoIII
O
O
His64
His93
CoII
His64
His93
+ O2+ H2O2
+ NaHSO32-
pH 7.0, 22oC
•Both the Cobalt and Iron metal centers have resonance forms which involve a superoxide ion.
•Upon addition of the dithionite, numerous reactions may occur which include release of oxygen, reduction of the metal, release of superoxide and its reaction with two hydrogen ions to form hydrogen peroxide.
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Possible Reaction of Fe in solution
Compound 1 Compound 2
FeIII
OO
FeII
OO
O2- + FeIII 2H+
FeIII+ H2O2
FeIV
O
FeIV
O
SO2-
FeII + HSO3-
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Conclusions
The studies of the dissociation of oxygen from the myoglobin analogs utilizing sodium dithionite were unsuccessful for several reasons. The concentration of dithionite was not great enough for the reaction to be pseudo first order. The reaction occurs too fast at such concentrations. The lengthy reduction of the metal species by dithionite and the use of an open system lead to the production of numerous radicals and species in various oxidation states, resulting in complex kinetic behavior.
The rate of dissociation of oxygen from the cobalt analog should have been on the order of 103 s- while that of the native species should have been about two orders of magnitude less, based on previous temperature jump relaxation analysis.
The dissociation of superoxide prior to reduction of the metal species by hydrosulfite was observed, but only an approximate rate of dissociation could be determined due to the complex nature of the reaction.
This experiment could be improved by using the stopped-flow apparatus at low temperatures. Also, in place of hydrosulfite, a ligand which binds more strongly to the myoglobin may be more appropriate in determination of the rate of oxygen dissociation.
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References
[1] Hoffman, B. M.; Petering, D. H. Proc. Nat. Acad. Sci. 1970, 67, 637.
[2] Spilburg, Curtis A.; Hoffman, Brian M.; Petering, Davind H. J. Bio. Chem. 1972, 247, 4219-4223.
[3] Brucker, Eric A.; Olson, John S.; Phillips, George N. Jr. J. Bio. Chem. 1996, 271, 25419-25422.
[4] Matsuo, Takashi; Tsuruta, Takashi; Maehara, Keiko; Sato, Hideaki; Hisaeda, Yoshio; Hayashi, Takashi. Inorg. Chem. 2005, 44, 9391-9396.
[5] Ikedai-Saito, Masao; Yamamoto, Haruhiko; Imai, Kiyohiro, Kayne, Frederick J.; Yonetani, Takashi. J. Bio. Chem. 1977, 252, 620-624.
[6] Yonetani, Takashi. J. Bio. Chem. 1967, 242, 5008-5013.
[7] Charles Dickinson
[8] Alan Bruha
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[10] Hambright, Peter, Lemelle, Stephanie. Inorganica Chimica Act, 92 (1984), 167-172.