Question

Each molecule of hemoglobin, the oxygen carrier in blood, contains four Fe atoms. Explain how you would use the radioactive \({ }_{26}^{59} \mathrm{Fe}\left(t_{\frac{1}{2}}=46\right.\) days) to show that the iron in a certain food is converted into hemoglobin.

Short answer

You can use \({ }_{26}^{59}\mathrm{Fe}\) by introducing it into the food. Once ingested, trace the isotope in the body using a radiation detector. Detecting this isotope in the hemoglobin shows that the iron in the food was converted into hemoglobin.

Step-by-step solution

Understanding radioactive isotopes

Radioactive isotopes, often referred as radioisotopes, are atoms with unstable nuclei that decay over time, emitting radiation. The rate at which this decay occurs is measured by a property called half-life, that is, the time it takes for half of a sample of a radioactive isotope to decay. Here, the isotope \({ }_{26}^{59}\mathrm{Fe}\) has a half-life of 46 days.

Introducing radioactive isotopes into food

Include the isotope \({ }_{26}^{59}\mathrm{Fe}\) into the food. This can be done by growing plants in a soil containing this isotope, or by using it in a form that can be mixed with food directly.

Tracing the radioactive isotopes

Once the food containing the isotope \({ }_{26}^{59}\mathrm{Fe}\) is ingested, we can then trace this isotope in the body to make sure whether this isotope ends up in the hemoglobin of the consumer. Use a radioactivity detector for this purpose.

Identifying the radioactive isotopes in Hemoglobin

By detecting \({ }_{26}^{59}\mathrm{Fe}\) in the blood, particularly in the hemoglobin, provides evidence that the iron from the food has been incorporated into the hemoglobin.

Interpretation of Results

The presence of the radioisotope in hemoglobin is solid evidence that the iron in food is converted into hemoglobin. However, the absence of the isotope doesn't necessarily imply that the conversion team doesn't take place, as it may simply be that the iron isn't being properly absorbed from the stomach, or it might be being used in other parts of the body.

Key concepts

Hemoglobin

Hemoglobin is a protein found in red blood cells that is crucial for transporting oxygen from the lungs to tissues throughout the body. It has a unique structure composed of four subunits, each containing an iron ion, which is vital for its function. The iron ions in hemoglobin play a crucial role in binding oxygen molecules, allowing red blood cells to carry and release oxygen as needed.

Understanding hemoglobin's structure is essential because it explains why iron deficiencies can lead to serious health issues like anemia. When there is insufficient iron, hemoglobin production decreases, resulting in less oxygen being transported throughout the body. This can cause symptoms like fatigue, weakness, and shortness of breath.

By studying hemoglobin, researchers can also develop ways to track the incorporation of iron from dietary sources into the body. Using radioactive isotopes, scientists can pinpoint how iron from consumed food becomes a part of hemoglobin, assisting in better understanding nutritional impacts and iron absorption.

Iron Isotope

An iron isotope is a variant of iron atoms that differ in the number of neutrons in their nucleus. Some isotopes of iron are stable, while others are radioactive, meaning they decay over time and emit radiation. One such radioactive isotope is \({ }_{26}^{59} ext{Fe}\), which has a relatively short half-life of 46 days.

Iron isotopes can be instrumental in scientific research and medical applications. In studies evaluating nutritional absorption, radioactive iron isotopes like \({ }_{26}^{59} ext{Fe}\) are used as tracers. By adding this isotope to food, scientists can trace its journey through the body and determine whether it ultimately becomes part of hemoglobin in red blood cells.

The usage of iron isotopes can help unveil information about how dietary iron is absorbed and utilized within the body. Through such research, improvements in dietary recommendations and treatments for iron deficiencies can be derived. However, handling and utilizing radioactive isotopes require strict safety protocols to minimize exposure and potential health risks.

Half-Life

When we talk about radioactive isotopes, the term half-life frequently comes up. The half-life is the amount of time it takes for half of a given sample of the radioactive isotope to decay into another element. This concept is fundamental for understanding how long a radioactive substance remains active within a system.

For the iron isotope \({ }_{26}^{59} ext{Fe}\), its half-life is 46 days. This means that every 46 days, half of the \({ }_{26}^{59} ext{Fe}\) in a given sample will have decayed. Understanding the half-life of a radioactive isotope is crucial because it helps scientists and researchers design studies and experiments around the isotopic behavior.

Knowing the half-life allows researchers to predict how long the radioactive isotopes will be traceable in a subject's body after ingestion and helps in planning safe and effective usage of these isotopes. By carefully measuring the decay and presence over time, valuable insights into metabolic processes, such as the incorporation of iron into hemoglobin, can be obtained.