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Ch.2 - Atoms, Molecules, and Ions
All textbooksBrown 15th EditionCh.2 - Atoms, Molecules, and IonsProblem 94c
Chapter 2, Problem 94c

The natural abundance of 3He is 0.000137%. (c) Based on your answer to part (b), what would need to be the precision of a mass spectrometer that is able to differentiate between peaks that are due to 3He+ and 3H+?

Verified step by step guidance
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Step 1: Understand the problem. The question is asking for the precision of a mass spectrometer that can differentiate between ^3He+ and ^3H+. The precision of a mass spectrometer is determined by its ability to distinguish between two ions with very close mass-to-charge ratios.
Step 2: Recall that the mass-to-charge ratio (m/z) is the key parameter that a mass spectrometer uses to differentiate between ions. For a singly charged ion, the m/z ratio is equal to the mass of the ion.
Step 3: Calculate the difference in mass between ^3He+ and ^3H+. The mass of ^3He is approximately 3 atomic mass units (amu) and the mass of ^3H (also known as tritium) is also approximately 3 amu. However, there is a slight difference between the two due to the difference in the number of neutrons.
Step 4: The precision of the mass spectrometer must be greater than this difference in mass in order to differentiate between the two ions. This means that the mass spectrometer must be able to detect differences in mass that are less than the difference between the mass of ^3He and ^3H.
Step 5: Express the required precision as a percentage of the mass of the ions. This is typically how precision is reported for mass spectrometers.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Mass Spectrometry

Mass spectrometry is an analytical technique used to measure the mass-to-charge ratio of ions. It allows for the identification and quantification of different isotopes and molecules in a sample. The precision of a mass spectrometer is crucial for distinguishing between ions with very similar mass, such as isotopes of hydrogen, which is essential in this context.
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Isotopes and Natural Abundance

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons, resulting in different masses. The natural abundance of an isotope refers to its relative occurrence in nature, expressed as a percentage. Understanding the natural abundance of isotopes like 3He and 3H is important for determining the required precision in mass spectrometry to differentiate between them.
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Resolution in Mass Spectrometry

Resolution in mass spectrometry refers to the ability of the instrument to distinguish between two closely spaced mass peaks. Higher resolution allows for better differentiation between ions with similar masses, which is critical when analyzing isotopes with small differences in mass. The required resolution can be calculated based on the natural abundance and the expected peak separation of the isotopes in question.
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Related Practice
Textbook Question

Suppose a scientist repeats the Millikan oil-drop experiment but reports the charges on the drops using an unusual (and imaginary) unit called the warmomb (wa). The scientist obtains the following data for four of the drops: Droplet Calculated Charge (wa) A 3.84⨉10−8 B 4.80⨉10−8 C 2.88⨉10−8 D 8.64⨉10−8 (d) What is the conversion factor between warmombs and coulombs?

Textbook Question

The natural abundance of 3He is 0.000137%. (a) How many protons, neutrons, and electrons are in an atom of 3He?

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Textbook Question

The natural abundance of 3He is 0.000137%. (b) Based on the sum of the masses of their subatomic particles, which is expected to be more massive, an atom of 3He or an atom of 3H (which is also called tritium)?

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Textbook Question

Identify the element represented by each of the following symbols and give the number of protons and neutrons in each: (a) 7433X

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Textbook Question

Identify the element represented by each of the following symbols and give the number of protons and neutrons in each: (b) 12753X (c) 8636X (d) 6730X

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Textbook Question

The nucleus of 6Li is a powerful absorber of neutrons. It exists in the naturally occurring metal to the extent of 7.5%. In the era of nuclear deterrence, large quantities of lithium were processed to remove 6Li for use in hydrogen bomb production. The lithium metal remaining after removal of 6Li was sold on the market. (b) The atomic masses of 6Li and 7Li are 6.015122 and 7.016004 u, respectively. A sample of lithium depleted in the lighter isotope was found on analysis to contain 1.442% 6Li. What is the average atomic weight of this sample of the metal?

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