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Chapter 23: Problem 76

Which transition metal atom is present in each of the following biologically important molecules: (a) hemoglobin, (b) chlorophylls, (c) siderophores, (d) hemocyanine.

Short Answer

Expert verified
The transition metal atoms present in each of the biologically important molecules are: (a) Hemoglobin - Iron (Fe), (b) Chlorophylls - Magnesium (Mg), (c) Siderophores - Iron (Fe), and (d) Hemocyanin - Copper (Cu).

Step by step solution

01

(a) Hemoglobin

Hemoglobin is a protein responsible for carrying oxygen in the blood of vertebrates. The transition metal atom present in hemoglobin is Iron (Fe). Iron is a part of the heme group, which is responsible for binding to oxygen and allowing the hemoglobin molecule to transport oxygen throughout the body.
02

(b) Chlorophylls

Chlorophylls are photosynthetic pigments found in plants, algae, and photosynthetic bacteria. They play an essential role in converting light energy into chemical energy through the process of photosynthesis. The transition metal atom present in chlorophyll molecules is Magnesium (Mg). Magnesium is located at the center of the chlorophyll molecule, helping to capture and transfer light energy for photosynthesis.
03

(c) Siderophores

Siderophores are small molecules produced by certain bacteria and fungi to sequester iron from their environment. They have a high affinity for iron and are involved in iron acquisition, storage, and transport. The transition metal atom present in siderophores is Iron (Fe). The siderophores bind to iron, allowing the organisms to take up the essential nutrient from their surroundings.
04

(d) Hemocyanin

Hemocyanin is an oxygen-carrying protein found in some invertebrates, such as crustaceans and mollusks. It is an alternative to hemoglobin, which is commonly found in vertebrates. The transition metal atom present in hemocyanin is Copper (Cu). Hemocyanin contains copper ions in its active site, which binds to oxygen and allows the protein to transport oxygen throughout the organism's body.

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Most popular questions from this chapter

Metallic elements are essential components of many important enzymes operating within our bodies. Carbonic anhydrase, which contains \(\mathrm{Zn}^{2+}\) in its active site, is responsible for rapidly interconverting dissolved \(\mathrm{CO}_{2}\) and bicarbonate ion, \(\mathrm{HCO}_{3}^{-}\). The zinc in carbonic anhydrase is tetrahedrally coordinated by three neutral nitrogencontaining groups and a water molecule. The coordinated water molecule has a \(\mathrm{p} K_{a}\) of \(7.5,\) which is crucial for the enzyme's activity. (a) Draw the active site geometry for the \(\mathrm{Zn}(\mathrm{II})\) center in carbonic anhydrase, just writing "N" for the three neutral nitrogen ligands from the protein. (b) Compare the \(\mathrm{p} K_{a}\) of carbonic anhydrase's active site with that of pure water; which species is more acidic? (c) When the coordinated water to the \(\mathrm{Zn}(\mathrm{II})\) center in carbonic anhydrase is deprotonated, what ligands are bound to the \(\mathrm{Zn}(\mathrm{II})\) center? Assume the three nitrogen ligands are unaffected. \((\mathbf{d})\) The \(\mathrm{p} K_{a}\) of \(\left[\mathrm{Zn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) is \(10 .\) Suggest an explanation for the difference between this $\mathrm{p} K_{a}$ and that of carbonic anhydrase. (e) Would you expect carbonic anhydrase to have a deep color, like hemoglobin and other metal-ion-containing proteins do? Explain.

Give the number of (valence) \(d\) electrons associated with the central metal ion in each of the following complexes: (a) $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right] \mathrm{Cl}_{2}$, (b) $\mathrm{K}_{2}\left[\mathrm{Cu}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\right]$, (c) \(\left[\mathrm{Os}(\mathrm{en})_{3}\right] \mathrm{Cl}_{3}\), (d) \([\mathrm{Cr}(\mathrm{EDTA})] \mathrm{SO}_{4}\), , (e) $\left[\mathrm{Cd}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{2}$

In 2001 , chemists at SUNY-Stony Brook succeeded in synthesizing the complex trans-[Fe(CN) \(\left._{4 (\mathrm{CO})_{2}\right]^{2-},\) which could be a model of complexes that may have played a role in the origin of life. (a) Sketch the structure of the complex. (b) The complex is isolated as a sodium salt. Write the com- (c) What is the oxidation state of Fe plete name of this salt. in this complex? How many \(d\) electrons are associated with the Fe in this complex? (d) Would you expect this complex to be high spin or low spin? Explain.

Indicate the coordination number and the oxidation number of the metal for each of the following complexes: (a) \(\mathrm{K}_{2} \mathrm{PtCl}_{4}\) (b) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right] \mathrm{Br}_{2}\) (c) \(\mathrm{OsO}_{4}\) (d) \(\left[\mathrm{Mn}(\mathrm{en})_{3}\right]\left(\mathrm{NO}_{3}\right)_{2}\) (e) $\left[\mathrm{Cr}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{3}$ (f) \(\left[\mathrm{Zn}(\mathrm{bipy})_{2}\right]\left(\mathrm{ClO}_{4}\right)_{2}\)

Consider an octahedral complex, \(\mathrm{MA}_{2} \mathrm{~B}_{4}\). How many geometric isomers are expected for this compound? Will any of the isomers be optically active? If so, which ones?
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