# Site-Directed Mutagenesis of Myoglobin for Studies of Their Interaction with Iron(III) by Multi-Spectroscopic Techniques

Authors: Qian Tang; Xiao-Jun Peng; Hong-Yu Cao; Yan-Jie Yang; Jing Ma; Jing-Yun Wang; Xue-Fang Zheng
Journal: Journal of Spectroscopy
 (2013)

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## Abstract

In order to investigate how the amino acids on the surface of myoglobin molecule influence myoglobin's structure and function, a variety of spectroscopy techniques were applied in the study of the interaction between Fe(III) and myoglobin (wild type and its mutants, D44K, D60K, and K56D). The results demonstrate that Fe(III) can quench the fluorescence of wild type and mutants of myoglobin, and the quenching mechanisms are static quenching. It is found that the binding distance between Fe(III) and myoglobin mutants gets smaller, the binding capacity increases by the values of binding constant and the bimolecular quenching constant as well as the binding distance. Those data also indicate that the metal ion Fe(III) can interact strongly with myoglobin mutants. The three-dimensional conformation change after surface amino acids are replaced is detected by the UV absorption spectroscopy and fluorescence spectroscopy, which make mutants become more dynamic and change its function and interaction with Fe(III) strongly.


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## Body

## 1. Introduction

Proteins have a variety of important physiological functions. They participate in every reaction of the living body and are essential for the translation of the genetic code of life, transcription of the information, and replication of DNA. Metal elements play an important role in the whole system of life. The most prominent feature for metal elements is to lose electrons and become ions with charges. As a result, metal ions exist in biological fluids in various forms and interact with biomolecules in many ways, which perform kinds of functions in organism, such as electron transfer, oxygen carrier, and enzyme active center‎[1]. Among the different metal elements, iron is one of the most essential trace elements to maintain life, and it executes many functions, such as transport and storage of oxygen, the conversion of energy in the body, drug metabolism, and decomposing and eliminating of active oxygen.Myoglobin (Mb) is an oxygen-binding protein found in the muscle tissues of vertebrates in general and in almost all mammals‎[2]. Due to its simple structure and important biological activity, it has been the model protein for the study of proteins’ interaction with their ligands. The research on interaction between proteins and ligands help to deeply realize the function of proteins in vivo. For a long time, it is believed that the amino acid residues on the surface of proteins exposed to the solvents have very little impact on the proteins’ function ‎[3]. However, Hoffman and his fellows ‎[4] have found that the electron transfer rate between myoglobin mutant D44K and cytochrome b5 increased by an order of magnitude. They also obtained a triple mutant, in which three acidic surface residues surrounding the Mb (horse) heme (Asp44, Asp60, and Glu85) are replaced by Lys [Mb(+6)], and binding and reactivity progressively become correlated by the mutations, the results exhibit both strongly enhanced binding to b5 (bovine) and intracomplex ET from the triplet state of Zn-deuteroporphyrin (ZnD)-substituted Mb to the Fe3+ b5 heme (Fe3+P) ‎[5, 6]. Our group has discussed the issue of interactions between myoglobin and its mutants with ligands, such as gas ‎[7, 8], surfactants ‎[9, 10], and hydrogen peroxide ‎[11], and has obtained many valuable results. The plethora of work performed by Rifkind, Saltman, Gray, Mauk and others in the 1980s with oxyMb and various ferric-complexes revealed that two distinct mechanisms by which sperm whale myoglobin reduces, respectively, complexes of Fe(III) and Cu(II) and, in turn, is oxidized to metmyoglobin have been characterized [11, 12]. Our group also have investigated the interactions between wide-type myoglobin with various metal ions ‎[13–15]. However, detailed study on interactions between metal ions and its mutants has not been reported yet. In order to clarify the impact of specific amino acids residues on the surface of Mb on the structure and function of myoglobin, in the present study, PCR site-directed mutagenesis technique was used to obtain myoglobin mutants D44K, D60K, and K56D and then a variety of spectrographic methods were adopted to study the interactions between metal ion Fe(III) and myoglobins (wild type and mutants).


## 2. Experimental

### 2.1. Instrument and Reagent

Instruments.FP-6500 fluorescence spectrophotometer (Jasco, Japan), J-810 Circular Dichroism (Jasco, Japan), V-560 UV-visible Spectrophotometer (Jasco, Japan), and F-12 cooling and heating circulator (Julabo, Germany).Reagent.Wild-type myoglobin sample (Sigma, USA) was proved to be oxymyoglobin (namely the metMb ‎[16]). 5 × 10−6 mol·L−1 metMb stock solution in NaHPO4-NaH2PO4 buffer (0.05 mol·L, pH = 7.40) was prepared and stored in a refrigerator (4°C). 1 × 10−2 mol·L−1 FeCl3 stock solution was made with FeCl3·6H2O (AR). All of the experimental water is ultrapure water.


### 2.2. Experimental Methods

#### 2.2.1. Preparation of the Mb Mutants‎[3, 17].

In our experiment, we use two-steps (NH4)2SO4 precipitation, Sephadex-G100 gel filtration, DEAE ion-exchange chromatography to purify the proteins. The concentration of myoglobin is measured by UV/VIS spectrophotometer (ε409=157 mM−1·cm−1  ‎[18]).


#### 2.2.2. Spectrometry

Pipette 3 mL of 5 × 10−6 mol·L−1 metMb solution in 1 cm quartz cuvette, and then place it in the V-560 UV-Vis spectrophotometer, add a certain amount of Fe(III) solution (cumulative total volume was less than 40 μL) with a microinjector(each) and mix them, put it aside for 4 min at 298 K, and then measure the UV absorption spectra of the coordinative reaction of metMb with Fe(III). Measure the fluorescence spectroscopy, synchronous fluorescence spectroscopy, and circular dichroism spectroscopy according to the above steps. Measurement for mutants is the same as well.


## 2.1. Instrument and Reagent

Instruments.FP-6500 fluorescence spectrophotometer (Jasco, Japan), J-810 Circular Dichroism (Jasco, Japan), V-560 UV-visible Spectrophotometer (Jasco, Japan), and F-12 cooling and heating circulator (Julabo, Germany).Reagent.Wild-type myoglobin sample (Sigma, USA) was proved to be oxymyoglobin (namely the metMb ‎[16]). 5 × 10−6 mol·L−1 metMb stock solution in NaHPO4-NaH2PO4 buffer (0.05 mol·L, pH = 7.40) was prepared and stored in a refrigerator (4°C). 1 × 10−2 mol·L−1 FeCl3 stock solution was made with FeCl3·6H2O (AR). All of the experimental water is ultrapure water.


## 2.2. Experimental Methods

### 2.2.1. Preparation of the Mb Mutants‎[3, 17].

In our experiment, we use two-steps (NH4)2SO4 precipitation, Sephadex-G100 gel filtration, DEAE ion-exchange chromatography to purify the proteins. The concentration of myoglobin is measured by UV/VIS spectrophotometer (ε409=157 mM−1·cm−1  ‎[18]).


### 2.2.2. Spectrometry

Pipette 3 mL of 5 × 10−6 mol·L−1 metMb solution in 1 cm quartz cuvette, and then place it in the V-560 UV-Vis spectrophotometer, add a certain amount of Fe(III) solution (cumulative total volume was less than 40 μL) with a microinjector(each) and mix them, put it aside for 4 min at 298 K, and then measure the UV absorption spectra of the coordinative reaction of metMb with Fe(III). Measure the fluorescence spectroscopy, synchronous fluorescence spectroscopy, and circular dichroism spectroscopy according to the above steps. Measurement for mutants is the same as well.


## 2.2.1. Preparation of the Mb Mutants‎[3, 17].

In our experiment, we use two-steps (NH4)2SO4 precipitation, Sephadex-G100 gel filtration, DEAE ion-exchange chromatography to purify the proteins. The concentration of myoglobin is measured by UV/VIS spectrophotometer (ε409=157 mM−1·cm−1  ‎[18]).


## 2.2.2. Spectrometry

Pipette 3 mL of 5 × 10−6 mol·L−1 metMb solution in 1 cm quartz cuvette, and then place it in the V-560 UV-Vis spectrophotometer, add a certain amount of Fe(III) solution (cumulative total volume was less than 40 μL) with a microinjector(each) and mix them, put it aside for 4 min at 298 K, and then measure the UV absorption spectra of the coordinative reaction of metMb with Fe(III). Measure the fluorescence spectroscopy, synchronous fluorescence spectroscopy, and circular dichroism spectroscopy according to the above steps. Measurement for mutants is the same as well.


## 3. Result and Discussion

### 3.1. Interaction between Protein and Fe(III)

#### 3.1.1. Ultraviolet Absorption Spectroscopy

Figure1 shows the UV absorption spectra of Fe(III) with myoglobin and its mutants. Near 280 nm, Mbs’ absorption intensity increases gradually with the increase of the concentration of Fe(III), and there is a slight blue shift. Mbs’ absorption peak at the 280 nm is caused by the transition of the aromatic heterocyclic of the tryptophan and tyrosine in the peptide chain ‎[19]. The above data show that Fe(III) can interact strongly with Mbs, which indicate that they form a new complex and the conformation of Mb molecules change. The aromatic heterocyclic hydrophobic groups of the tryptophan and tyrosine residues inside the molecules of exposed Fe(III) expose when they interact with Fe(III), as the hydrophobic interactions between hydrophobic groups inside the molecules weaken and polarity enhance, the π-π* and n-π* transition energy increases, which make the absorption peak of proteins move towards the short wavelength direction and the peak intensity gradually increase.The effect of Fe(III) on UV absorption spectra of Mb (WT), Mb (D44K), Mb (D60K), and Mb (K56D) (298 K)CMb = 5 × 10−6 mol·L−1, 1–9. C (Fe(III))/10−6 mol·L−1 = 0, 1, 2, 3, 4, 5, 6, 7, 8, C(Mb(D44K)), C(Mb(D60K)), C(Mb(K56D))  = 5 × 10−6 mol·L−1, C (Fe(III))/10−6 mol·L−1 = 0, 0.5, 1, 1.5.
(a)
(b)
(c)
(d)


#### 3.1.2. Fluorescence Spectrum

(1) Fluorescence Quenching Mechanism.Figure 2 is the fluorescence spectra of the interaction between Fe(III) and different Mbs, respectively. As it is showed from the fluorescence spectra, Fe(III) causes regularly the fluorescence quenching of the proteins, which proves that the interaction and energy transfer between the proteins and Fe(III). The experimental result is consistent with that of the UV spectra. The fluorescence spectra are not distorted, which indicates that the energy transfer between them is nonradiative transfer ‎[20].Effect of Fe(III) on the fluorescence spectra of Mbs (25°C).C (Mb (WT, D44K, D60K): 5 × 10−6 mol·L−1, 1–9, C (Fe(III))/10−5 mol·L−1: 0, 0.5, 1, 1.5, 2, 2.5, 3, 3.5, and 4, resp. C (Mb (K56D)): 5 × 10−6 mol·L−1; 1–9, C (Fe(III))/10−6 mol·L−1: 0, 1, 2, 3, 4, 5, 6, 7, 8, and 9, respectively.
(a)
(b)
(c)
(d)Fluorescence quenching can be caused by dynamic quenching and static quenching. The dynamic quenching follows the following equation of Stern-Volmer‎[21–23]:
(1)F0F=1+Kqτ0[Q]=1+Ksv[Q].In (1), F0 and F are the fluorescence intensity of the protein solution with quenching body Q not added or added, respectively, Kq is the bimolecular quenching constant, τ0 is the average life expectancy of the fluorescent molecules when quenching body does not exist, Ksv is the dynamic quenching constant, and [Q] is the concentration of quenching body Q.The fluorescence quenching was measured at three different temperatures (289, 298, and 313 K), and (1) was applied for data processing. The results are shown in Figure 3. Within the concentration dimension of our experiment, when the concentration of Fe(III) increases, the Stern-Volmer curve shows good linear relationship, and the slope of the straight line decreases with temperature increasing. It is demonstrated that the fluorescence quenching mechanisms of Fe(III) on Mb (WT), Mb (D44K), Mb (D60K) and Mb (K56D) are attributed to static quenching, respectively. Table 1 shows the fluorescence quenching constants of Fe(III) for various kinds of Mbs. All of the, Kqs, are greater than maximum diffusion or collision quenching constant 2 × 1010 L·mol‒1 s‒1  ‎[24] between the various types of quenching body and the biological macromolecules. These data further show that the fluorescence quenching mechanisms of Fe(III) with various Mbs are not dynamic quenching but static quenching. The order of magnitude of Fe(III) on dynamic quenching constant and bimolecular quenching constant of the Mbs is the same, but the value of the mutant is greater than the wild type.Table 1
The bimolecular quenching constant  (Kq), the dynamic quenching constants (Ksv), the correlation coefficients (R) in Stern-Volmer curve.
Mb and Mutants
T/K
K
q/L·mol−1·s−1
K
s
v/L·mol−1
Mb (WT)
289
1.12
×
10
12
1.12
×
10
4
298
1.04
×
10
12
1.04
×
10
4
310
0.903
×
10
12
0.903
×
10
4
Mb (D44K)
289
1.51
×
10
12
1.51
×
10
4
298
1.40
×
10
12
1.40
×
10
4
310
1.29
×
10
12
1.29
×
10
4
Mb (D60K)
289
1.14
×
10
12
1.14
×
10
4
298
1.09
×
10
12
1.09
×
10
4
310
1.04
×
10
12
1.04
×
10
4
Mb (K56D)
289
1.7
×
10
12
1.7
×
10
4
298
1.62
×
10
12
1.62
×
10
4
310
1.46
×
10
12
1.46
×
10
4Stern-Volmer plot of several Mbs quenched by Fe(III) at different temperatures.
(a)
(b)
(c)
(d)For static quenching, a new compound forms between the quenching molecule and the fluorescent substance molecules, which is according to the following double reciprocal equation of Lineweaver-Burk‎[15]:
(2)(F0-F)-1=F0-1+Ka-1·F0-1[Q]-1.
See results in Figure 4 and Table 2.Table 2
The binding constants (Ka) and relative coefficient (R) in lineweaver-Burk curve.
Mb and mutants
T/K
K
a/ L·mol−1
Mb (WT)
289
1.06
×
10
4
298
1.00
×
10
4
310
0.926
×
10
4
Mb (D44K)
289
1.39
×
10
4
298
1.23
×
10
4
310
1.10
×
10
4
Mb (D60K)
289
1.18
×
10
4
298
1.11
×
10
4
310
1.03
×
10
4
Mb (K56D)
289
1.67
×
10
4
298
1.61
×
10
4
310
1.56
×
10
4Lineweaver-Burk plot of Mbs quenched by Fe(III) at different temperatures.
(a)
(b)
(c)
(d)The double reciprocal curve linear of the Lineweaver-Burk is shown in Figure4 and Table 2. All of the binding constant value is high, and the different temperatures affect on the binding constants at a certain extent, which indicates that Fe(III) and Mbs has formed stable complex. The binding constants of Fe(III) to fluorescence quenching of myoglobin have the same order of magnitude, but the mutant value is greater than wild type.(2) Binding Constants and Number of Binding Sites.For static quenching, it is assumed that biological macromolecules has n identical and independent binding sites, the relationship between fluorescence intensity and quenching body can be derived from the formula of the binding constant between fluorescent molecules and quenching molecules ‎[25, 26] as
(3)lg[F0-FF]=lgK+nlg[Q].lg[(F0-F)/F] to lg[Q] plot (Figure 5), the binding constant K and binding site number n of the quenching body and fluorescent molecules can be calculated according to the slope and intercept of the straight line. As it can be seen from Table 3, the binding constants obtained by this method basically conform to Ka value obtained from the Lineweaver-Burk figure, binding ability decreases with the increasing temperature, the average numbers of binding sites of Fe(III) and Mb (WT) Mb (D44K), Mb(D60K), and Mb(K56D) are 1.0121, 1.0334, 1.0103, and 0.9894, respectively, which are approximately equal to 1.Table 3
The binding constants (K), the binding numbers (n), and their correlations (R) at different temperatures.
Mb mutants
T/K
K/( L·mol−1)
n
R
Mb (WT)
289
1.48
×
10
4
1.0226
0.9997
298
1.18
×
10
4
1.0128
0.9995
310
9.81
×
10
4
1.0009
0.9994
Mb (D44K)
289
2.23
×
10
4
1.0424
0.9989
298
1.78
×
10
4
1.0296
0.9986
310
1.58
×
10
4
1.0282
0.9990
Mb (D60K)
289
1.47
×
10
4
1.0180
0.9989
298
1.28
×
10
4
1.0135
0.9986
310
1.12
×
10
4
0.9994
0.9990
Mb (K56D)
289
1.99
×
10
4
1.0133
0.999
298
1.6
×
10
4
0.9989
0.999
310
0.9
×
10
4
0.956
1Double-lg plot at different temperatures.
(a)
(b)
(c)
(d)


#### 3.1.3. Types of Interaction Force

The interaction force between quenching body and biological macromolecules mainly comes from van der Waals’ force, electrostatic forces, hydrogen bonding, and hydrophobic‎[25]. Enthalpy can be taken as a constant in our experiment. Therefore, the reaction of enthalpy change, free energy change, and entropy change can be calculated based on the following thermodynamic formula‎ [27, 28]:
(4)lnka=-ΔHRT+ΔSR,ΔG=ΔH-TΔS,
where K is the static quenching constant, T is the experimental temperature, and ΔH, ΔG, and ΔS are, respectively the enthalpy, free energy change, and entropy change. The calculated results are shown in Table 4.Table 4
The thermodynamic parameters between Fe(III) and Mb mutants.
Mb mutants
ΔH/KJ·mol−1
ΔG/KJ·mol−1
ΔS/J·mol−1·K−1
Mb (WT)
−14.53
−23.03
29.44
−23.30
−23.65
Mb (D44K)
−8.20
−22.91
50.95
−23.38
−23.98
Mb (D60K)
−4.78
−22.53
61.42
−23.08
−23.82
Mb (K56D)
−4.314
−23.49
66.34
−24.08
−25.08Table4 shows that four kinds of the Mbs perform similar natures ΔH < 0, ΔG < 0, ΔS > 0. ΔH < 0, ΔG < 0, which indicate that the combination of Fe(III) and Mbs is exothermic process and spontaneous process, ΔH < 0, ΔS > 0 indicate that the main force is the electrostatic force ‎[15]. The enthalpy changes ΔH between Fe(III) and Mb (WT) or Mb (D44K) or Mb (D60K) or Mb (K56D) are 62.36%, 35.07%, 20.71%, and 17.92%, respectively, at 298 K. The contribution from the entropy change ΔS are 37.64%, 64.93%, 79.29% and 82.08%, respectively at 298 K. The enthalpy change contribution of mutants becomes weak, while entropy change contribution becomes strong. Thus entropy driving force cannot be ignored.


#### 3.1.4. Action Distance

Figure6 shows the overlays of fluorescence spectra of different myoglobin and absorption spectra of Fe(III) whose molar ratios are 1 : 1, respectively. According to the Förster dipole-dipole nonradiative energy transfer theory ‎[17, 29], the binding distances of the tryptophan residues (in wild type, Mb (D44K), Mb (D60K) and Mb (K56D)) and Fe(III) are 3.18 nm, 3.05 nm, 3.15 nm, and 2.38 nm, respectively, which indicate that the interacted distance of mutated myoglobin and metal ions Fe(III) becomes smaller. All binding distances are less than 7 nm, which indicates that nonradiative energy transfer can occur between Mbs and Fe(III). The above data have proved that the Fe(III) and proteins formed the complexes without fluorescence, so the energy transfer of them should be attributed to the intramolecular nonradiative energy transfer ‎[27].Overlap of the fluorescence spectra of Mbs (a) and the absorption spectra of Fe(III) (b).
(a)
(b)
(c)
(d)


### 3.2. The Comparison of Experimental Data Between a Variety of Myoglobin and Fe(III) Interactions

Table5 shows that the strength of the combination between Fe(III) and protein is as follows:  Mb (K56D) > Mb (D44K) > Mb (D60K) > Mb (WT), the distances of combination are as follows: Mb(WT) > Mb (D60K) > Mb (D44K) > Mb (K56D). Thus, the surface amino acid residues of Asp56, Asp44, and Lys60 can affect myoglobin’s function. The mutants change the volume of residue side chain, which make close residue side chains direction change, even make conformation of the side chains of these mutant residues and several other residues’ main chains change. Mb (K56D) has more negative charge after it was mutated, which significantly enhances its binding ability with positive-electric Fe(III). Thus, the amino acids on the surface of protein have a definite impact on protein’s function ‎[30, 31].Table 5
The comparison of experimental data of Mb (WT) and Mb mutants, respectively, (25C°).
Mbs
K
q
K
a
n
r
Mb (WT)
1.04
×
10
12
1.00
×
10
4
1.0128
3.18
Mb (D60K)
1
.
09
×
10
12
1
.
11
×
10
4
1.0135
3.15
Mb (D44K)
1.40
×
10
12
1.23
×
10
4
1.0296
3.05
Mb (K56D)
2.36
×
10
12
2.13
×
10
4
1.0525
2.38


### 3.3. Structure Comparison

In order to further study the effect of surface amino acids on function and structure of myoglobin, here we discuss the relationship between structure and function.


#### 3.3.1. UV Absorption Spectroscopy

280 nm absorption peak is formed due to theπ-π* and n-π* transition of Myglobin’s aromatic amino acids. Figure 7 shows the UV absorption spectra of myoglobin (wild type and mutants). The maximum absorption spectrum of wild-type myoglobin is at 276 nm position, while the maximum absorption of three mutants is at 280 nm position (Figure 7). The surface charges of myoglobin change after the surface amino acids were replaced, which affects the internal aromatic amino acid microenvironments, increases it’s hydrophobicity, and decreases π-π* and n-π* transition energy, furthermore induces peaks shifted.Figure 7
Absorbance spectra of 5μM myoglobin and mutants.


#### 3.3.2. Fluorescence Spectroscopy

Fluorescence spectrometric methods have many advantages‎[32], such as high sensitivity, less volume of sample, high selectivity, and simplicity. It is often used as an important mean to the study of protein conformation changes. Figure 8 shows fluorescence emission spectra of myoglobin (wild type and its mutants). The maximum emission peaks of Mb (WT), Mb (D44K), Mb (D60K), and Mb (K56D) are 323 nm, 330 nm, 336 nm, and 329.6 nm, respectively, in 280 nm excitation wavelength. The mutant (D44K, D60K, and K56D) maximum mission peaks red shift compared to wild-type myoglobin. The shift of D60K location is maximal, and shift is 11.2 nm compared to wild-type Mb. The displaced amino acids on the surface of myoglobin induce the polarity of aromatic amino acid hydrophobic box to be changed, weaken its polarity, reduce its fluorescence energy, and shift emission peak position. The above results are consistent with ultraviolet spectroscopy.Figure 8
Fluorescence spectra of 5μM myoglobin and mutants.


#### 3.3.3. Circular Dichroism Spectroscopy

Figure9 displays the CD spectra of wild-type and mutant Mbs, and all of them show three peaks in 192 nm (+), 202 (−), and 222 (−), which are α-helix typical characteristic peaks [33–35]. The peak position and the strength for wild type, D44K, and D60K are at the same level, only the strength of the K56D changes slightly. This proves that the surface amino acid changes have little effect on myoglobin second structures.Figure 9
CD spectra of 5μM myoglobin and mutants.Therefore, the changes of amino acids on the surface of myoglobin have great impact on its tertiary structure microenvironment, but little effect on the secondary structure. The stability and integrality of proteins’ tertiary structure is important for protein to put in practice its function accurately. The little changes in the three-dimensional structure of the microenvironment have large effect to its function.


## 3.1. Interaction between Protein and Fe(III)

### 3.1.1. Ultraviolet Absorption Spectroscopy

Figure1 shows the UV absorption spectra of Fe(III) with myoglobin and its mutants. Near 280 nm, Mbs’ absorption intensity increases gradually with the increase of the concentration of Fe(III), and there is a slight blue shift. Mbs’ absorption peak at the 280 nm is caused by the transition of the aromatic heterocyclic of the tryptophan and tyrosine in the peptide chain ‎[19]. The above data show that Fe(III) can interact strongly with Mbs, which indicate that they form a new complex and the conformation of Mb molecules change. The aromatic heterocyclic hydrophobic groups of the tryptophan and tyrosine residues inside the molecules of exposed Fe(III) expose when they interact with Fe(III), as the hydrophobic interactions between hydrophobic groups inside the molecules weaken and polarity enhance, the π-π* and n-π* transition energy increases, which make the absorption peak of proteins move towards the short wavelength direction and the peak intensity gradually increase.The effect of Fe(III) on UV absorption spectra of Mb (WT), Mb (D44K), Mb (D60K), and Mb (K56D) (298 K)CMb = 5 × 10−6 mol·L−1, 1–9. C (Fe(III))/10−6 mol·L−1 = 0, 1, 2, 3, 4, 5, 6, 7, 8, C(Mb(D44K)), C(Mb(D60K)), C(Mb(K56D))  = 5 × 10−6 mol·L−1, C (Fe(III))/10−6 mol·L−1 = 0, 0.5, 1, 1.5.
(a)
(b)
(c)
(d)


### 3.1.2. Fluorescence Spectrum

(1) Fluorescence Quenching Mechanism.Figure 2 is the fluorescence spectra of the interaction between Fe(III) and different Mbs, respectively. As it is showed from the fluorescence spectra, Fe(III) causes regularly the fluorescence quenching of the proteins, which proves that the interaction and energy transfer between the proteins and Fe(III). The experimental result is consistent with that of the UV spectra. The fluorescence spectra are not distorted, which indicates that the energy transfer between them is nonradiative transfer ‎[20].Effect of Fe(III) on the fluorescence spectra of Mbs (25°C).C (Mb (WT, D44K, D60K): 5 × 10−6 mol·L−1, 1–9, C (Fe(III))/10−5 mol·L−1: 0, 0.5, 1, 1.5, 2, 2.5, 3, 3.5, and 4, resp. C (Mb (K56D)): 5 × 10−6 mol·L−1; 1–9, C (Fe(III))/10−6 mol·L−1: 0, 1, 2, 3, 4, 5, 6, 7, 8, and 9, respectively.
(a)
(b)
(c)
(d)Fluorescence quenching can be caused by dynamic quenching and static quenching. The dynamic quenching follows the following equation of Stern-Volmer‎[21–23]:
(1)F0F=1+Kqτ0[Q]=1+Ksv[Q].In (1), F0 and F are the fluorescence intensity of the protein solution with quenching body Q not added or added, respectively, Kq is the bimolecular quenching constant, τ0 is the average life expectancy of the fluorescent molecules when quenching body does not exist, Ksv is the dynamic quenching constant, and [Q] is the concentration of quenching body Q.The fluorescence quenching was measured at three different temperatures (289, 298, and 313 K), and (1) was applied for data processing. The results are shown in Figure 3. Within the concentration dimension of our experiment, when the concentration of Fe(III) increases, the Stern-Volmer curve shows good linear relationship, and the slope of the straight line decreases with temperature increasing. It is demonstrated that the fluorescence quenching mechanisms of Fe(III) on Mb (WT), Mb (D44K), Mb (D60K) and Mb (K56D) are attributed to static quenching, respectively. Table 1 shows the fluorescence quenching constants of Fe(III) for various kinds of Mbs. All of the, Kqs, are greater than maximum diffusion or collision quenching constant 2 × 1010 L·mol‒1 s‒1  ‎[24] between the various types of quenching body and the biological macromolecules. These data further show that the fluorescence quenching mechanisms of Fe(III) with various Mbs are not dynamic quenching but static quenching. The order of magnitude of Fe(III) on dynamic quenching constant and bimolecular quenching constant of the Mbs is the same, but the value of the mutant is greater than the wild type.Table 1
The bimolecular quenching constant  (Kq), the dynamic quenching constants (Ksv), the correlation coefficients (R) in Stern-Volmer curve.
Mb and Mutants
T/K
K
q/L·mol−1·s−1
K
s
v/L·mol−1
Mb (WT)
289
1.12
×
10
12
1.12
×
10
4
298
1.04
×
10
12
1.04
×
10
4
310
0.903
×
10
12
0.903
×
10
4
Mb (D44K)
289
1.51
×
10
12
1.51
×
10
4
298
1.40
×
10
12
1.40
×
10
4
310
1.29
×
10
12
1.29
×
10
4
Mb (D60K)
289
1.14
×
10
12
1.14
×
10
4
298
1.09
×
10
12
1.09
×
10
4
310
1.04
×
10
12
1.04
×
10
4
Mb (K56D)
289
1.7
×
10
12
1.7
×
10
4
298
1.62
×
10
12
1.62
×
10
4
310
1.46
×
10
12
1.46
×
10
4Stern-Volmer plot of several Mbs quenched by Fe(III) at different temperatures.
(a)
(b)
(c)
(d)For static quenching, a new compound forms between the quenching molecule and the fluorescent substance molecules, which is according to the following double reciprocal equation of Lineweaver-Burk‎[15]:
(2)(F0-F)-1=F0-1+Ka-1·F0-1[Q]-1.
See results in Figure 4 and Table 2.Table 2
The binding constants (Ka) and relative coefficient (R) in lineweaver-Burk curve.
Mb and mutants
T/K
K
a/ L·mol−1
Mb (WT)
289
1.06
×
10
4
298
1.00
×
10
4
310
0.926
×
10
4
Mb (D44K)
289
1.39
×
10
4
298
1.23
×
10
4
310
1.10
×
10
4
Mb (D60K)
289
1.18
×
10
4
298
1.11
×
10
4
310
1.03
×
10
4
Mb (K56D)
289
1.67
×
10
4
298
1.61
×
10
4
310
1.56
×
10
4Lineweaver-Burk plot of Mbs quenched by Fe(III) at different temperatures.
(a)
(b)
(c)
(d)The double reciprocal curve linear of the Lineweaver-Burk is shown in Figure4 and Table 2. All of the binding constant value is high, and the different temperatures affect on the binding constants at a certain extent, which indicates that Fe(III) and Mbs has formed stable complex. The binding constants of Fe(III) to fluorescence quenching of myoglobin have the same order of magnitude, but the mutant value is greater than wild type.(2) Binding Constants and Number of Binding Sites.For static quenching, it is assumed that biological macromolecules has n identical and independent binding sites, the relationship between fluorescence intensity and quenching body can be derived from the formula of the binding constant between fluorescent molecules and quenching molecules ‎[25, 26] as
(3)lg[F0-FF]=lgK+nlg[Q].lg[(F0-F)/F] to lg[Q] plot (Figure 5), the binding constant K and binding site number n of the quenching body and fluorescent molecules can be calculated according to the slope and intercept of the straight line. As it can be seen from Table 3, the binding constants obtained by this method basically conform to Ka value obtained from the Lineweaver-Burk figure, binding ability decreases with the increasing temperature, the average numbers of binding sites of Fe(III) and Mb (WT) Mb (D44K), Mb(D60K), and Mb(K56D) are 1.0121, 1.0334, 1.0103, and 0.9894, respectively, which are approximately equal to 1.Table 3
The binding constants (K), the binding numbers (n), and their correlations (R) at different temperatures.
Mb mutants
T/K
K/( L·mol−1)
n
R
Mb (WT)
289
1.48
×
10
4
1.0226
0.9997
298
1.18
×
10
4
1.0128
0.9995
310
9.81
×
10
4
1.0009
0.9994
Mb (D44K)
289
2.23
×
10
4
1.0424
0.9989
298
1.78
×
10
4
1.0296
0.9986
310
1.58
×
10
4
1.0282
0.9990
Mb (D60K)
289
1.47
×
10
4
1.0180
0.9989
298
1.28
×
10
4
1.0135
0.9986
310
1.12
×
10
4
0.9994
0.9990
Mb (K56D)
289
1.99
×
10
4
1.0133
0.999
298
1.6
×
10
4
0.9989
0.999
310
0.9
×
10
4
0.956
1Double-lg plot at different temperatures.
(a)
(b)
(c)
(d)


### 3.1.3. Types of Interaction Force

The interaction force between quenching body and biological macromolecules mainly comes from van der Waals’ force, electrostatic forces, hydrogen bonding, and hydrophobic‎[25]. Enthalpy can be taken as a constant in our experiment. Therefore, the reaction of enthalpy change, free energy change, and entropy change can be calculated based on the following thermodynamic formula‎ [27, 28]:
(4)lnka=-ΔHRT+ΔSR,ΔG=ΔH-TΔS,
where K is the static quenching constant, T is the experimental temperature, and ΔH, ΔG, and ΔS are, respectively the enthalpy, free energy change, and entropy change. The calculated results are shown in Table 4.Table 4
The thermodynamic parameters between Fe(III) and Mb mutants.
Mb mutants
ΔH/KJ·mol−1
ΔG/KJ·mol−1
ΔS/J·mol−1·K−1
Mb (WT)
−14.53
−23.03
29.44
−23.30
−23.65
Mb (D44K)
−8.20
−22.91
50.95
−23.38
−23.98
Mb (D60K)
−4.78
−22.53
61.42
−23.08
−23.82
Mb (K56D)
−4.314
−23.49
66.34
−24.08
−25.08Table4 shows that four kinds of the Mbs perform similar natures ΔH < 0, ΔG < 0, ΔS > 0. ΔH < 0, ΔG < 0, which indicate that the combination of Fe(III) and Mbs is exothermic process and spontaneous process, ΔH < 0, ΔS > 0 indicate that the main force is the electrostatic force ‎[15]. The enthalpy changes ΔH between Fe(III) and Mb (WT) or Mb (D44K) or Mb (D60K) or Mb (K56D) are 62.36%, 35.07%, 20.71%, and 17.92%, respectively, at 298 K. The contribution from the entropy change ΔS are 37.64%, 64.93%, 79.29% and 82.08%, respectively at 298 K. The enthalpy change contribution of mutants becomes weak, while entropy change contribution becomes strong. Thus entropy driving force cannot be ignored.


### 3.1.4. Action Distance

Figure6 shows the overlays of fluorescence spectra of different myoglobin and absorption spectra of Fe(III) whose molar ratios are 1 : 1, respectively. According to the Förster dipole-dipole nonradiative energy transfer theory ‎[17, 29], the binding distances of the tryptophan residues (in wild type, Mb (D44K), Mb (D60K) and Mb (K56D)) and Fe(III) are 3.18 nm, 3.05 nm, 3.15 nm, and 2.38 nm, respectively, which indicate that the interacted distance of mutated myoglobin and metal ions Fe(III) becomes smaller. All binding distances are less than 7 nm, which indicates that nonradiative energy transfer can occur between Mbs and Fe(III). The above data have proved that the Fe(III) and proteins formed the complexes without fluorescence, so the energy transfer of them should be attributed to the intramolecular nonradiative energy transfer ‎[27].Overlap of the fluorescence spectra of Mbs (a) and the absorption spectra of Fe(III) (b).
(a)
(b)
(c)
(d)


## 3.1.1. Ultraviolet Absorption Spectroscopy

Figure1 shows the UV absorption spectra of Fe(III) with myoglobin and its mutants. Near 280 nm, Mbs’ absorption intensity increases gradually with the increase of the concentration of Fe(III), and there is a slight blue shift. Mbs’ absorption peak at the 280 nm is caused by the transition of the aromatic heterocyclic of the tryptophan and tyrosine in the peptide chain ‎[19]. The above data show that Fe(III) can interact strongly with Mbs, which indicate that they form a new complex and the conformation of Mb molecules change. The aromatic heterocyclic hydrophobic groups of the tryptophan and tyrosine residues inside the molecules of exposed Fe(III) expose when they interact with Fe(III), as the hydrophobic interactions between hydrophobic groups inside the molecules weaken and polarity enhance, the π-π* and n-π* transition energy increases, which make the absorption peak of proteins move towards the short wavelength direction and the peak intensity gradually increase.The effect of Fe(III) on UV absorption spectra of Mb (WT), Mb (D44K), Mb (D60K), and Mb (K56D) (298 K)CMb = 5 × 10−6 mol·L−1, 1–9. C (Fe(III))/10−6 mol·L−1 = 0, 1, 2, 3, 4, 5, 6, 7, 8, C(Mb(D44K)), C(Mb(D60K)), C(Mb(K56D))  = 5 × 10−6 mol·L−1, C (Fe(III))/10−6 mol·L−1 = 0, 0.5, 1, 1.5.
(a)
(b)
(c)
(d)


## 3.1.2. Fluorescence Spectrum

(1) Fluorescence Quenching Mechanism.Figure 2 is the fluorescence spectra of the interaction between Fe(III) and different Mbs, respectively. As it is showed from the fluorescence spectra, Fe(III) causes regularly the fluorescence quenching of the proteins, which proves that the interaction and energy transfer between the proteins and Fe(III). The experimental result is consistent with that of the UV spectra. The fluorescence spectra are not distorted, which indicates that the energy transfer between them is nonradiative transfer ‎[20].Effect of Fe(III) on the fluorescence spectra of Mbs (25°C).C (Mb (WT, D44K, D60K): 5 × 10−6 mol·L−1, 1–9, C (Fe(III))/10−5 mol·L−1: 0, 0.5, 1, 1.5, 2, 2.5, 3, 3.5, and 4, resp. C (Mb (K56D)): 5 × 10−6 mol·L−1; 1–9, C (Fe(III))/10−6 mol·L−1: 0, 1, 2, 3, 4, 5, 6, 7, 8, and 9, respectively.
(a)
(b)
(c)
(d)Fluorescence quenching can be caused by dynamic quenching and static quenching. The dynamic quenching follows the following equation of Stern-Volmer‎[21–23]:
(1)F0F=1+Kqτ0[Q]=1+Ksv[Q].In (1), F0 and F are the fluorescence intensity of the protein solution with quenching body Q not added or added, respectively, Kq is the bimolecular quenching constant, τ0 is the average life expectancy of the fluorescent molecules when quenching body does not exist, Ksv is the dynamic quenching constant, and [Q] is the concentration of quenching body Q.The fluorescence quenching was measured at three different temperatures (289, 298, and 313 K), and (1) was applied for data processing. The results are shown in Figure 3. Within the concentration dimension of our experiment, when the concentration of Fe(III) increases, the Stern-Volmer curve shows good linear relationship, and the slope of the straight line decreases with temperature increasing. It is demonstrated that the fluorescence quenching mechanisms of Fe(III) on Mb (WT), Mb (D44K), Mb (D60K) and Mb (K56D) are attributed to static quenching, respectively. Table 1 shows the fluorescence quenching constants of Fe(III) for various kinds of Mbs. All of the, Kqs, are greater than maximum diffusion or collision quenching constant 2 × 1010 L·mol‒1 s‒1  ‎[24] between the various types of quenching body and the biological macromolecules. These data further show that the fluorescence quenching mechanisms of Fe(III) with various Mbs are not dynamic quenching but static quenching. The order of magnitude of Fe(III) on dynamic quenching constant and bimolecular quenching constant of the Mbs is the same, but the value of the mutant is greater than the wild type.Table 1
The bimolecular quenching constant  (Kq), the dynamic quenching constants (Ksv), the correlation coefficients (R) in Stern-Volmer curve.
Mb and Mutants
T/K
K
q/L·mol−1·s−1
K
s
v/L·mol−1
Mb (WT)
289
1.12
×
10
12
1.12
×
10
4
298
1.04
×
10
12
1.04
×
10
4
310
0.903
×
10
12
0.903
×
10
4
Mb (D44K)
289
1.51
×
10
12
1.51
×
10
4
298
1.40
×
10
12
1.40
×
10
4
310
1.29
×
10
12
1.29
×
10
4
Mb (D60K)
289
1.14
×
10
12
1.14
×
10
4
298
1.09
×
10
12
1.09
×
10
4
310
1.04
×
10
12
1.04
×
10
4
Mb (K56D)
289
1.7
×
10
12
1.7
×
10
4
298
1.62
×
10
12
1.62
×
10
4
310
1.46
×
10
12
1.46
×
10
4Stern-Volmer plot of several Mbs quenched by Fe(III) at different temperatures.
(a)
(b)
(c)
(d)For static quenching, a new compound forms between the quenching molecule and the fluorescent substance molecules, which is according to the following double reciprocal equation of Lineweaver-Burk‎[15]:
(2)(F0-F)-1=F0-1+Ka-1·F0-1[Q]-1.
See results in Figure 4 and Table 2.Table 2
The binding constants (Ka) and relative coefficient (R) in lineweaver-Burk curve.
Mb and mutants
T/K
K
a/ L·mol−1
Mb (WT)
289
1.06
×
10
4
298
1.00
×
10
4
310
0.926
×
10
4
Mb (D44K)
289
1.39
×
10
4
298
1.23
×
10
4
310
1.10
×
10
4
Mb (D60K)
289
1.18
×
10
4
298
1.11
×
10
4
310
1.03
×
10
4
Mb (K56D)
289
1.67
×
10
4
298
1.61
×
10
4
310
1.56
×
10
4Lineweaver-Burk plot of Mbs quenched by Fe(III) at different temperatures.
(a)
(b)
(c)
(d)The double reciprocal curve linear of the Lineweaver-Burk is shown in Figure4 and Table 2. All of the binding constant value is high, and the different temperatures affect on the binding constants at a certain extent, which indicates that Fe(III) and Mbs has formed stable complex. The binding constants of Fe(III) to fluorescence quenching of myoglobin have the same order of magnitude, but the mutant value is greater than wild type.(2) Binding Constants and Number of Binding Sites.For static quenching, it is assumed that biological macromolecules has n identical and independent binding sites, the relationship between fluorescence intensity and quenching body can be derived from the formula of the binding constant between fluorescent molecules and quenching molecules ‎[25, 26] as
(3)lg[F0-FF]=lgK+nlg[Q].lg[(F0-F)/F] to lg[Q] plot (Figure 5), the binding constant K and binding site number n of the quenching body and fluorescent molecules can be calculated according to the slope and intercept of the straight line. As it can be seen from Table 3, the binding constants obtained by this method basically conform to Ka value obtained from the Lineweaver-Burk figure, binding ability decreases with the increasing temperature, the average numbers of binding sites of Fe(III) and Mb (WT) Mb (D44K), Mb(D60K), and Mb(K56D) are 1.0121, 1.0334, 1.0103, and 0.9894, respectively, which are approximately equal to 1.Table 3
The binding constants (K), the binding numbers (n), and their correlations (R) at different temperatures.
Mb mutants
T/K
K/( L·mol−1)
n
R
Mb (WT)
289
1.48
×
10
4
1.0226
0.9997
298
1.18
×
10
4
1.0128
0.9995
310
9.81
×
10
4
1.0009
0.9994
Mb (D44K)
289
2.23
×
10
4
1.0424
0.9989
298
1.78
×
10
4
1.0296
0.9986
310
1.58
×
10
4
1.0282
0.9990
Mb (D60K)
289
1.47
×
10
4
1.0180
0.9989
298
1.28
×
10
4
1.0135
0.9986
310
1.12
×
10
4
0.9994
0.9990
Mb (K56D)
289
1.99
×
10
4
1.0133
0.999
298
1.6
×
10
4
0.9989
0.999
310
0.9
×
10
4
0.956
1Double-lg plot at different temperatures.
(a)
(b)
(c)
(d)


## 3.1.3. Types of Interaction Force

The interaction force between quenching body and biological macromolecules mainly comes from van der Waals’ force, electrostatic forces, hydrogen bonding, and hydrophobic‎[25]. Enthalpy can be taken as a constant in our experiment. Therefore, the reaction of enthalpy change, free energy change, and entropy change can be calculated based on the following thermodynamic formula‎ [27, 28]:
(4)lnka=-ΔHRT+ΔSR,ΔG=ΔH-TΔS,
where K is the static quenching constant, T is the experimental temperature, and ΔH, ΔG, and ΔS are, respectively the enthalpy, free energy change, and entropy change. The calculated results are shown in Table 4.Table 4
The thermodynamic parameters between Fe(III) and Mb mutants.
Mb mutants
ΔH/KJ·mol−1
ΔG/KJ·mol−1
ΔS/J·mol−1·K−1
Mb (WT)
−14.53
−23.03
29.44
−23.30
−23.65
Mb (D44K)
−8.20
−22.91
50.95
−23.38
−23.98
Mb (D60K)
−4.78
−22.53
61.42
−23.08
−23.82
Mb (K56D)
−4.314
−23.49
66.34
−24.08
−25.08Table4 shows that four kinds of the Mbs perform similar natures ΔH < 0, ΔG < 0, ΔS > 0. ΔH < 0, ΔG < 0, which indicate that the combination of Fe(III) and Mbs is exothermic process and spontaneous process, ΔH < 0, ΔS > 0 indicate that the main force is the electrostatic force ‎[15]. The enthalpy changes ΔH between Fe(III) and Mb (WT) or Mb (D44K) or Mb (D60K) or Mb (K56D) are 62.36%, 35.07%, 20.71%, and 17.92%, respectively, at 298 K. The contribution from the entropy change ΔS are 37.64%, 64.93%, 79.29% and 82.08%, respectively at 298 K. The enthalpy change contribution of mutants becomes weak, while entropy change contribution becomes strong. Thus entropy driving force cannot be ignored.


## 3.1.4. Action Distance

Figure6 shows the overlays of fluorescence spectra of different myoglobin and absorption spectra of Fe(III) whose molar ratios are 1 : 1, respectively. According to the Förster dipole-dipole nonradiative energy transfer theory ‎[17, 29], the binding distances of the tryptophan residues (in wild type, Mb (D44K), Mb (D60K) and Mb (K56D)) and Fe(III) are 3.18 nm, 3.05 nm, 3.15 nm, and 2.38 nm, respectively, which indicate that the interacted distance of mutated myoglobin and metal ions Fe(III) becomes smaller. All binding distances are less than 7 nm, which indicates that nonradiative energy transfer can occur between Mbs and Fe(III). The above data have proved that the Fe(III) and proteins formed the complexes without fluorescence, so the energy transfer of them should be attributed to the intramolecular nonradiative energy transfer ‎[27].Overlap of the fluorescence spectra of Mbs (a) and the absorption spectra of Fe(III) (b).
(a)
(b)
(c)
(d)


## 3.2. The Comparison of Experimental Data Between a Variety of Myoglobin and Fe(III) Interactions

Table5 shows that the strength of the combination between Fe(III) and protein is as follows:  Mb (K56D) > Mb (D44K) > Mb (D60K) > Mb (WT), the distances of combination are as follows: Mb(WT) > Mb (D60K) > Mb (D44K) > Mb (K56D). Thus, the surface amino acid residues of Asp56, Asp44, and Lys60 can affect myoglobin’s function. The mutants change the volume of residue side chain, which make close residue side chains direction change, even make conformation of the side chains of these mutant residues and several other residues’ main chains change. Mb (K56D) has more negative charge after it was mutated, which significantly enhances its binding ability with positive-electric Fe(III). Thus, the amino acids on the surface of protein have a definite impact on protein’s function ‎[30, 31].Table 5
The comparison of experimental data of Mb (WT) and Mb mutants, respectively, (25C°).
Mbs
K
q
K
a
n
r
Mb (WT)
1.04
×
10
12
1.00
×
10
4
1.0128
3.18
Mb (D60K)
1
.
09
×
10
12
1
.
11
×
10
4
1.0135
3.15
Mb (D44K)
1.40
×
10
12
1.23
×
10
4
1.0296
3.05
Mb (K56D)
2.36
×
10
12
2.13
×
10
4
1.0525
2.38


## 3.3. Structure Comparison

In order to further study the effect of surface amino acids on function and structure of myoglobin, here we discuss the relationship between structure and function.


### 3.3.1. UV Absorption Spectroscopy

280 nm absorption peak is formed due to theπ-π* and n-π* transition of Myglobin’s aromatic amino acids. Figure 7 shows the UV absorption spectra of myoglobin (wild type and mutants). The maximum absorption spectrum of wild-type myoglobin is at 276 nm position, while the maximum absorption of three mutants is at 280 nm position (Figure 7). The surface charges of myoglobin change after the surface amino acids were replaced, which affects the internal aromatic amino acid microenvironments, increases it’s hydrophobicity, and decreases π-π* and n-π* transition energy, furthermore induces peaks shifted.Figure 7
Absorbance spectra of 5μM myoglobin and mutants.


### 3.3.2. Fluorescence Spectroscopy

Fluorescence spectrometric methods have many advantages‎[32], such as high sensitivity, less volume of sample, high selectivity, and simplicity. It is often used as an important mean to the study of protein conformation changes. Figure 8 shows fluorescence emission spectra of myoglobin (wild type and its mutants). The maximum emission peaks of Mb (WT), Mb (D44K), Mb (D60K), and Mb (K56D) are 323 nm, 330 nm, 336 nm, and 329.6 nm, respectively, in 280 nm excitation wavelength. The mutant (D44K, D60K, and K56D) maximum mission peaks red shift compared to wild-type myoglobin. The shift of D60K location is maximal, and shift is 11.2 nm compared to wild-type Mb. The displaced amino acids on the surface of myoglobin induce the polarity of aromatic amino acid hydrophobic box to be changed, weaken its polarity, reduce its fluorescence energy, and shift emission peak position. The above results are consistent with ultraviolet spectroscopy.Figure 8
Fluorescence spectra of 5μM myoglobin and mutants.


### 3.3.3. Circular Dichroism Spectroscopy

Figure9 displays the CD spectra of wild-type and mutant Mbs, and all of them show three peaks in 192 nm (+), 202 (−), and 222 (−), which are α-helix typical characteristic peaks [33–35]. The peak position and the strength for wild type, D44K, and D60K are at the same level, only the strength of the K56D changes slightly. This proves that the surface amino acid changes have little effect on myoglobin second structures.Figure 9
CD spectra of 5μM myoglobin and mutants.Therefore, the changes of amino acids on the surface of myoglobin have great impact on its tertiary structure microenvironment, but little effect on the secondary structure. The stability and integrality of proteins’ tertiary structure is important for protein to put in practice its function accurately. The little changes in the three-dimensional structure of the microenvironment have large effect to its function.


## 3.3.1. UV Absorption Spectroscopy

280 nm absorption peak is formed due to theπ-π* and n-π* transition of Myglobin’s aromatic amino acids. Figure 7 shows the UV absorption spectra of myoglobin (wild type and mutants). The maximum absorption spectrum of wild-type myoglobin is at 276 nm position, while the maximum absorption of three mutants is at 280 nm position (Figure 7). The surface charges of myoglobin change after the surface amino acids were replaced, which affects the internal aromatic amino acid microenvironments, increases it’s hydrophobicity, and decreases π-π* and n-π* transition energy, furthermore induces peaks shifted.Figure 7
Absorbance spectra of 5μM myoglobin and mutants.


## 3.3.2. Fluorescence Spectroscopy

Fluorescence spectrometric methods have many advantages‎[32], such as high sensitivity, less volume of sample, high selectivity, and simplicity. It is often used as an important mean to the study of protein conformation changes. Figure 8 shows fluorescence emission spectra of myoglobin (wild type and its mutants). The maximum emission peaks of Mb (WT), Mb (D44K), Mb (D60K), and Mb (K56D) are 323 nm, 330 nm, 336 nm, and 329.6 nm, respectively, in 280 nm excitation wavelength. The mutant (D44K, D60K, and K56D) maximum mission peaks red shift compared to wild-type myoglobin. The shift of D60K location is maximal, and shift is 11.2 nm compared to wild-type Mb. The displaced amino acids on the surface of myoglobin induce the polarity of aromatic amino acid hydrophobic box to be changed, weaken its polarity, reduce its fluorescence energy, and shift emission peak position. The above results are consistent with ultraviolet spectroscopy.Figure 8
Fluorescence spectra of 5μM myoglobin and mutants.


## 3.3.3. Circular Dichroism Spectroscopy

Figure9 displays the CD spectra of wild-type and mutant Mbs, and all of them show three peaks in 192 nm (+), 202 (−), and 222 (−), which are α-helix typical characteristic peaks [33–35]. The peak position and the strength for wild type, D44K, and D60K are at the same level, only the strength of the K56D changes slightly. This proves that the surface amino acid changes have little effect on myoglobin second structures.Figure 9
CD spectra of 5μM myoglobin and mutants.Therefore, the changes of amino acids on the surface of myoglobin have great impact on its tertiary structure microenvironment, but little effect on the secondary structure. The stability and integrality of proteins’ tertiary structure is important for protein to put in practice its function accurately. The little changes in the three-dimensional structure of the microenvironment have large effect to its function.


## 4. Consclusion

The above studies show that Fe(III) and Mbs (wild type and mutants) formed new complexes without fluorescence, which cause protein’s fluorescence quenched. All of quenching types are static fluorescence quenching, the acting forces are electrostatic interactions, and the binding constants are 1. The three-dimensional structure of mutant proteins changes after mutation, which also leads to changing interactions between Fe(III) and Mbs changed. At the same temperature, the binding distances of Fe(III) and Mbs are as follows: Mb (WT) > Mb (D60K) > Mb (D44K) > Mb (K56D), and protein binding strength: Mb (K56D) > Mb (D44K) > Mb (D60K) > Mb (WT). In short, it is concluded that Fe(III) has stronger interactions with mutant proteins compared with the experimental data of the wild-type myoglobin. Displacement of Asp44, Asp60, and Lys56 amino acids on the surface of myoglobin have a certain impact on the three-dimensional structure and function of myoglobin.



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*Source: 314345-2012-09-02.xml*