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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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Most popular questions from this chapter

Cathode rays (a) may be positively or negatively charged (b) are a form of electromagnetic radiation similar to visible light (c) have properties identical to \(\beta\) particles (d) have masses that depend on the cathode that emits them

For the ion \(^{228} \mathrm{Ra}^{2+}\) with a mass of 228.030 u, determine (a) the numbers of protons, neutrons, and electrons in the ion; (b) the ratio of the mass of this ion to that of an atom of \(^{16} \mathrm{O}\) (refer to page 47 ).

The four naturally occurring isotopes of strontium have the atomic masses 83.9134 u; 85.9093 u; 86.9089 u; and 87.9056 u. The percent natural abundance of the lightest isotope is \(0.56 \%\) and of the heaviest, \(82.58 \%\) Estimate the percent natural abundances of the other two. Why is this result only a rough approximation?

A particular silver solder (used in the electronics industry to join electrical components) is to have the atom ratio of \(5.00 \mathrm{Ag} / 4.00 \mathrm{Cu} / 1.00 \mathrm{Zn}\). What masses of the three metals must be melted together to prepare \(1.00 \mathrm{kg}\) of the solder?

William Prout (1815) proposed that all other atoms are built up of hydrogen atoms, suggesting that all elements should have integral atomic masses based on an atomic mass of one for hydrogen. This hypothesis appeared discredited by the discovery of atomic masses, such as 24.3 u for magnesium and 35.5 u for chlorine. In terms of modern knowledge, explain why Prout's hypothesis is actually quite reasonable.
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