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Chapter 2: Problem 104

Which one of the following pairs are isotopes? A. \(\mathrm{O}_2\) and \(\mathrm{O}_3\) B. \({ }^{35} \mathrm{Cl}\) and \({ }^{37} \mathrm{Cl}\) C. \(\mathrm{I}_2(\mathrm{~g})\) and \(\mathrm{I}_2(\mathrm{~s})\) D. \(\mathrm{F}^{+}\)and \(\mathrm{F}^{-}\)

Short Answer

Expert verified
Option B: \({ }^{35} \text{Cl} \) and \({ }^{37} \text{Cl} \) are isotopes.

Step by step solution

01

Define Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This means they have the same atomic number but different mass numbers.
02

Analyze Option A

Option A: \(\text{O}_2 \) and \(\text{O}_3 \). These are different molecular forms of oxygen (dioxygen and ozone). They are not isotopes because they are different molecules, not different forms of the same atom.
03

Analyze Option B

Option B: \({ }^{35} \text{Cl} \) and \({ }^{37} \text{Cl} \). These are both forms of chlorine with different mass numbers (35 and 37), but the same atomic number (17). Therefore, these are isotopes.
04

Analyze Option C

Option C: \(\text{I}_2(\text{~g}) \) and \(\text{I}_2(\text{~s}) \). This refers to iodine in gaseous and solid states, respectively. Changing the state of matter does not change the atomic composition, so these are not isotopes.
05

Analyze Option D

Option D: \(\text{F}^{+} \) and \(\text{F}^{-} \). These are fluorine ions with different charges, not different numbers of neutrons. Therefore, these are not isotopes.
06

Conclusion

The pair that are isotopes is \({ }^{35} \text{Cl} \) and \({ }^{37} \text{Cl} \) (Option B).

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Key Concepts

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

Atomic Number
The atomic number of an element is a fundamental property that defines the identity of the element. It is represented by the symbol 'Z'. The atomic number is the number of protons in the nucleus of an atom. For example, the atomic number of hydrogen is 1 because it has one proton in its nucleus. The atomic number determines the element's position on the periodic table and its chemical properties. Elements with the same atomic number have the same chemical behavior because they have the same number of protons and electrons.
Mass Number
The mass number, represented by the symbol 'A', is the total number of protons and neutrons in an atom's nucleus. For instance, if an atom has 6 protons and 6 neutrons, its mass number is 12. Unlike the atomic number, the mass number can vary for atoms of the same element. This variation is due to the different possible numbers of neutrons, leading to the formation of isotopes. Isotopes have the same number of protons but different numbers of neutrons, hence different mass numbers.
Chemical Elements
Chemical elements are substances made of only one kind of atom. They are the simplest forms of matter that cannot be broken down using chemical reactions. Each element is defined by its atomic number. For example, oxygen (O) is an element with an atomic number of 8, meaning every oxygen atom has 8 protons. Elements are organized in the periodic table, which classifies them by similar chemical properties. Scientists can identify and study elements based on their atomic structure, and each element has unique characteristics that determine its chemical behavior.

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