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Chapter 18: Problem 60

Each of the following isotopes has been used medically for the purpose indicated. Suggest reasons why the particular element might have been chosen for this purpose. a. cobalt-57, for study of the body's use of vitamin \(\mathbf{B}_{12}\) b. calcium- \(47,\) for study of bone metabolism c. iron-59, for study of red blood cell function

Short Answer

Expert verified
Cobalt-57 is used for studying the body's use of vitamin B12 because it is chemically similar to both iron and vitamin B12. It binds with B12, creating a radioactive complex that emits gamma radiation, and allows tracking of B12 absorption and utilization. Calcium-47 is used for studying bone metabolism due to its biochemical similarity to stable calcium isotopes, permitting it to act as a radiotracer for bone mineralization/demineralization processes. Lastly, Iron-59 is used to study red blood cell function as it is a crucial component of hemoglobin. Its radioactivity allows researchers to non-destructively monitor the uptake and distribution of iron, providing insights into the life cycle, production, and degradation of red blood cells.

Step by step solution

01

I - Cobalt-57 for studying body's use of vitamin B12

We will examine the properties of cobalt-57 and try to determine why it is chosen for studying the body's use of vitamin B12. Cobalt-57 is a radioactive isotope with a half-life of 271.79 days. The decay of cobalt-57 emits gamma radiation, which can be detected easily without causing significant harm to the body tissues. Gamma radiation has high penetrating power, so it can be picked up by gamma cameras for diagnostic purposes. Since cobalt is chemically very similar to both iron and vitamin B12, it can be used as a tracer to track the absorption and utilization of vitamin B12 in the body. Cobalt-57 binds with B12, creating a radioactive complex that can be detected using gamma cameras, thus mapping the use of vitamin B12.
02

II - Calcium-47 for studying bone metabolism

Let's look at Calcium-47 and determine why it is used for studying bone metabolism. Calcium-47 is a radioactive isotope with a half-life of 4.54 days. It decays, emitting beta particles which can be detected with minimal disturbance to the biological tissues. Since the primary component of bones is calcium, using a calcium isotope is ideal for studying bone metabolism. Calcium-47 is biochemically indistinguishable from the stable calcium isotopes, making it a perfect radiotracer for studying how bones mineralize or demineralize over time. Being radioactive, Calcium-47 can be detected externally, allowing researchers to monitor its movement in the body and gain insights into the bone-building processes.
03

III - Iron-59 for studying red blood cell function

Now, let's analyze why iron-59 is used to study red blood cell function. Iron-59 is a radioactive isotope with a half-life of 45 days. It emits beta rays during decay, which can be detected without causing significant harm to the body tissues. Iron is a crucial component of hemoglobin, a protein that carries oxygen in red blood cells. For this reason, using iron tracers is logical for studying RBC functions. Iron-59 is biologically similar to stable iron isotopes and, when injected, is distributed throughout the body and taken up by red blood cells. The radioactivity of iron-59 enables researchers to monitor its uptake and distribution in a non-destructive manner, providing insights into the life cycle, production, and degradation of red blood cells.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Cobalt-57 and Vitamin B12 Absorption
Cobalt-57 is a radioactive isotope which plays a unique and crucial role in the medical field, specifically in studying how the body uses vitamin B12. One of its key features is its half-life of 271.79 days. This long half-life is ideal for prolonged research studies as it allows optimal time for tracking without the need for frequent re-dosing.
Additionally, cobalt-57 emits gamma radiation. This type of radiation, although penetrating, is safe enough in small doses for the body and is detectable using gamma cameras. This detection allows for external monitoring of cobalt-57 inside the body, helping doctors to visualize the utilization process of vitamin B12.
Cobalt-57 chemically resembles iron and has important similarities with vitamin B12. This makes it an effective tracer. By binding to vitamin B12, cobalt-57 creates a traceable complex. Researchers can study this complex to understand better how vitamin B12 is absorbed and utilized, especially in patients who might have deficiencies or malabsorption issues.
Calcium-47 in Bone Metabolism Studies
Calcium-47 is another important radioactive isotope, vital for understanding bone metabolism. With a half-life of 4.54 days, it鈥檚 practical for short-term studies aimed at observing rapid changes in bone structure or metabolism.
Bones predominantly consist of calcium; hence, using an isotope of calcium makes logical sense for such studies. Calcium-47 emits beta particles, which can be detected externally. This emission offers a non-invasive way to track and study how bones mineralize (build up) and demineralize (break down) over time.
  • Calcium-47 fits seamlessly into the biochemical processes of the body, indistinguishable from its stable counterparts, making it a perfect tracer.
  • Its behavior helps provide insights into how diseases affect bone density, such as osteoporosis, by seeing how the metabolism changes at the cellular level.
This close mimicry means calcium-47 integrates naturally into ongoing processes, lending a clear picture of bone health dynamics.
Iron-59 and Red Blood Cell Function
Iron-59 is a crucial isotope used to study red blood cell (RBC) function. Its 45-day half-life strikes a balance between being long enough to capture detailed information and short enough to minimize radiation exposure over time.
The isotope decays by emitting beta particles, providing a safe way to monitor its path through the body. In the realm of hematology, iron is essential for hemoglobin, the protein responsible for oxygen transport in RBCs. Consequently, iron-59 is used to trace how iron moves within the body, giving valuable insights into RBC production and health.
  • Iron-59 behaves similarly to stable iron, a feature that makes it compatible with normal physiological processes.
  • It helps researchers understand anomalies in RBC function, iron absorption, and distribution.
Studying iron-59 provides a window into diagnosing and managing blood-related conditions, such as anemia, by enabling efficient tracking of iron dynamics within the circulatory system.

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Most popular questions from this chapter

Many elements have been synthesized by bombarding relatively heavy atoms with high-energy particles in particle accelerators. Complete the following nuclear equations, which have been used to synthesize elements. a. \(\quad+\frac{4}{2} H e \rightarrow 243 B k+\frac{1}{0} n\) b. \(^{238} \mathrm{U}+^{12}_{6} \mathrm{C} \rightarrow$$\quad$$+6_{0}^{1} n\) c. \(^{249} \mathrm{Cf}+$$\quad$$\rightarrow \frac{260}{105} D b+4 \frac{1}{6} n\) d. \(^{249} \mathrm{Cf}+^{10}_{5} \mathrm{B} \rightarrow \frac{257}{153} \mathrm{Lr}+\)__________

A rock contains \(0.688 \mathrm{mg}^{206} \mathrm{Pb}\) for every \(1.000 \mathrm{mg}\) \(^{238} \mathrm{U}\) present Assuming that no lead was originally present, that all the \(^{206} \mathrm{Pb}\) formed over the years has remained in the rock, and that the number of nuclides in intermediate stages of decay between \(^{238} \mathrm{U}\) and \(^{206} \mathrm{Pb}\) is negligible, calculate the age of the \(\text { rock. For }^{238} \mathbf{U}, t_{1 / 2}=4.5 \times 10^{9} \text { years. }\)

A recent study concluded that any amount of radiation exposure can cause biological damage. Explain the differences between the two models of radiation damage, the linear model and the threshold model.

The most significant source of natural radiation is radon-222. \(^{222} \mathrm{Rn},\) a decay product of \(^{238} \mathrm{U},\) is continuously generated in the earth's crust, allowing gaseous Rn to seep into the basements of buildings. Because \(^{222} \mathrm{Rn}\) is an \(\alpha\) -particle producer with a relatively short half-life of 3.82 days, it can cause biological damage when inhaled. a. How many \(\alpha\) particles and \(\beta\) particles are produced when \(^{238} \mathrm{U}\) decays to \(^{222} \mathrm{Rn} ?\) What nuclei are produced when \(^{222} \mathrm{Rn}\) decays? b. Radon is a noble gas so one would expect it to pass through the body quickly. Why is there a concern over inhaling \(^{222} \mathrm{Rn} ?\) c. Another problem associated with \(^{222} \mathrm{Rn}\) is that the decay of \(^{222} \mathrm{Rn}\) produces a more potent \(\alpha\) -particle producer \(\left(t_{1 / 2}=\right.\) 3.11 min) that is a solid. What is the identity of the solid? Give the balanced equation of this species decaying by \(\alpha\) particle production. Why is the solid a more potent \(\alpha\) -particle producer? d. The U.S. Environmental Protection Agency (EPA) recommends that \(^{222}\) Rn levels not exceed 4 pCi per liter of air (1 \(\mathrm{Ci}=1\) curie \(=3.7 \times 10^{10}\) decay events per second; \(1 \mathrm{pCi}=1 \times 10^{-12} \mathrm{Ci}\). Convert \(4.0 \mathrm{pCi}\) per liter of air into concentrations units of \(^{222} \mathrm{Rn}\) atoms per liter of air and moles of \(^{222}\) Rn per liter of air.

Calculate the binding energy per nucleon for \(\frac{2}{1} \mathrm{H}\) and \(^{3}_{1}\) \(\mathrm{H}\). The atomic masses are \(\frac{2}{1} \mathrm{H}, 2.01410 \mathrm{u} ;\) and \(\frac{3}{1} \mathrm{H}, 3.01605 \mathrm{u}\)
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