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Chapter 2: Problem 37

Iodine has many radioactive isotopes. Iodine-123 is a radioactive isotope used for obtaining images of the thyroid gland. Iodine-123 is administered to patients in the form of sodium iodide capsules that contain \(123 \mathrm{I}^{-}\) ions. Determine the number of neutrons, protons, and electrons in a single \(^{123} \mathrm{I}^{-}\) ion.

Short Answer

Expert verified
In a single \(^{123} \mathrm{I}^{-}\) ion, there are 53 protons, 70 neutrons, and 54 electrons.

Step by step solution

01

Determine the number of protons

The number of protons in an isotope is equivalent to the atomic number of that element. The atomic number of iodine (\( \mathrm{I} \)) is 53. So, there are 53 protons in \(^{123} \mathrm{I}^{-}\).
02

Determine the number of neutrons

The mass number of an isotope is the sum of the number of protons and neutrons in the nucleus. So, to find the number of neutrons in \(^{123} \mathrm{I}^{-}\), subtract the number of protons from the mass number. Hence, the number of neutrons is 123 - 53 = 70.
03

Determine the number of electrons

In a neutral atom, the number of electrons is the same as the number of protons. However, in an ion like \(^{123} \mathrm{I}^{-}\), the negative charge indicates that there is one extra electron. So, the number of electrons is 53 (protons) + 1 (extra from the negative charge) = 54.

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Key Concepts

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

Iodine-123
Iodine-123 is a noteworthy radioactive isotope. It plays a significant role in nuclear medicine, primarily due to its optimal half-life of approximately 13.2 hours and its gamma radiation emissions. These properties make it especially useful for creating images in diagnostic procedures without unnecessarily prolonging radiation exposure for the patient. This isotope behaves similarly to non-radioactive iodine and is predominantly utilized in the form of sodium iodide (NaI) capsules. When administered, it participates in the thyroid gland's natural iodine uptake processes, allowing for effective imaging of thyroid function and structure. Furthermore, Iodine-123 decays into a stable form of Xenon, ensuring that it does not leave any long-lasting radioactive residue in the body.
  • Optimal half-life: 13.2 hours
  • Gamma radiation emission
  • Used in sodium iodide form
Thyroid Imaging
Thyroid imaging is crucial in diagnosing and managing thyroid-related disorders. The thyroid gland is responsible for producing hormones that regulate metabolism, and its dysfunction can lead to a variety of health issues. Utilizing Iodine-123 in thyroid scans provides clear images of the gland. Once administered, Iodine-123 is selectively absorbed by the thyroid, where it mimics the behavior of natural iodine. Gamma cameras are then employed to detect the gamma rays emitted by the isotope, capturing detailed images that reveal the size, shape, and activity of the thyroid. These scans are essential for identifying conditions like hyperthyroidism, Graves' disease, or thyroid nodules.
  • Diagnostic tool for thyroid disorders
  • Targeted absorption by thyroid gland
  • Gamma camera imaging process
Atomic Structure
Understanding atomic structure is vital in grasping how isotopes like Iodine-123 function. An atom consists of three main components: protons, neutrons, and electrons. The number of protons defines the element and is known as the atomic number. For iodine, this number is 53, indicating 53 protons. The mass number of an isotope is the sum of protons and neutrons; for Iodine-123, the mass number is 123, leading to 70 neutrons (123 - 53 = 70). Electrons are equal to protons in neutral atoms, but in ions, this can change. The ion Iodine-123 in its negative form ("")] has an additional electron, totaling 54 electrons (53 protons + 1 extra electron).
  • Atomic number: 53 for iodine
  • Mass number: sum of protons and neutrons
  • Extra electron in negatively charged ions

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Most popular questions from this chapter

Hydrogen and chlorine atoms react to form simple diatomic molecules in a 1: 1 ratio, that is, \(\mathrm{HCl}\). The natural abundances of the chlorine isotopes are \(75.77 \%^{35} \mathrm{Cl}\) and \(24.23 \%^{37} \mathrm{Cl} .\) The natural abundances of \(^{2} \mathrm{H}\) and \(^{3} \mathrm{H}\) are \(0.015 \%\) and less than \(0.001 \%,\) respectively. (a) How many different HCl molecules are possible, and what are their mass numbers (that is, the sum of the mass numbers of the H and Cl atoms)? (b) Which is the most abundant of the possible HCl molecules? Which is the second most abundant?

In Example \(2-1,\) we established that the mass ratio of magnesium to magnesium oxide is 0.455 g magnesium/ \(0.755 \mathrm{g}\) magnesium oxide. (a) What is the ratio of oxygen to magnesium oxide, by mass? (b) What is the mass ratio of oxygen to magnesium in magnesium oxide? (c) What is the percent by mass of magnesium in magnesium oxide?

Bromine has two naturally occurring isotopes. One of them, bromine-79, has a mass of 78.918336 u and a natural abundance of \(50.69 \% .\) What must be the mass and percent natural abundance of the other isotope, bromine-81?

Refer to the periodic table inside the front cover and identify (a) the element that is in group 14 and the fourth period (b) one element similar to and one unlike sulfur (c) the alkali metal in the fifth period (d) the halogen element in the sixth period

Determine the only possible isotope (E) for which the following conditions are met: \(\bullet\)The mass number of \(\mathrm{E}\) is 2.50 times its atomic number. \(\bullet\)The atomic number of \(\mathrm{E}\) is equal to the mass number of another isotope (Y). In turn, isotope Y has a neutron number that is 1.33 times the atomic number of \(Y\) and equal to the neutron number of selenium- 82 .
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