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Ch.2 - Atoms, Molecules, and Ions
Chapter 2, Problem 38a

Consider the mass spectrometer shown in Figure 2.11. Determine whether each of the following statements is true or false. If false, correct the statement to make it true: (a) The paths of neutral (uncharged) atoms are not affected by the magnet.

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Understand the basic principle of a mass spectrometer, which is used to separate isotopes, molecules, and molecular fragments according to their mass-to-charge ratio. The key components include an ion source, a mass analyzer, and a detector.
Recognize that in a mass spectrometer, particles must be ionized (charged) so that they can be influenced by magnetic and electric fields. Neutral (uncharged) atoms or molecules do not carry a charge.
Recall that the magnetic field in a mass spectrometer is used to deflect the path of the charged particles. The degree of deflection depends on the mass-to-charge ratio of the particles.
Analyze the statement: Since neutral atoms do not have a charge, they will not experience a force from the magnetic field. Therefore, the magnetic field does not affect the paths of neutral atoms.
Conclude that the statement 'The paths of neutral (uncharged) atoms are not affected by the magnet' is true, as neutral atoms will not be deflected by the magnetic field and will continue in a straight path.

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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 involves ionizing chemical species and sorting the ions based on their mass and charge. This technique is crucial for identifying the composition of a sample and determining the structure of molecules.
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Ionization and Charge

In mass spectrometry, ionization is the process of converting atoms or molecules into ions by adding or removing charged particles. Charged ions are influenced by electric and magnetic fields, while neutral atoms remain unaffected. Understanding the role of charge is essential for interpreting the behavior of particles in a mass spectrometer.
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Ionization Energy

Magnetic Fields and Particle Motion

Magnetic fields exert forces on charged particles, causing them to follow curved paths. The direction and radius of the curvature depend on the charge and velocity of the particle, as well as the strength of the magnetic field. Neutral particles, lacking charge, do not experience this force and thus travel in straight lines, which is key to understanding the statement in the question.
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Strong-Field Ligands result in a large Δ and Weak-Field Ligands result in a small Δ.
Related Practice
Textbook Question

(b) Why is the atomic weight of carbon reported as 12.011 in the table of elements and the periodic table in the front inside cover of this text?

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Textbook Question

Only two isotopes of copper occur naturally: 63Cu (atomic mass = 62.9296 amu; abundance 69.17%) 65Cu (atomic mass = 64.9278 amu; abundance 30.83%). Calculate the atomic weight (average atomic mass) of copper.

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Textbook Question

(a) Thomson's cathode-ray tube (Figure 2.4) and the mass spectrometer (Figure 2.11) both involve the use of electric or magnetic fields to deflect charged particles. What are the charged particles involved in each of these experiments?

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Textbook Question

Consider the mass spectrometer shown in Figure 2.11. Determine whether each of the following statements is true or false. If false, correct the statement to make it true: (b) The height of each peak in the mass spectrum is inversely proportional to the mass of that isotope.

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Open Question
Naturally occurring lead has the following isotopic abundances: Isotope Abundance (%) Atomic mass (u) 204Pb 1.4 203.9730, 206Pb 24.1 205.9744, 207Pb 22.1 206.9759, 208Pb 52.4 207.9766. (a) What is the average atomic mass of Pb? (b) Sketch the mass spectrum of Pb.
Textbook Question

Massspectrometry is more often applied to molecules than to atoms. We will see in Chapter 3 that the molecular weight of a molecule is the sum of the atomic weights of the atoms in the molecule. The mass spectrum of H2 is taken under conditions that prevent decomposition into H atoms. The two naturally occurring isotopes of hydrogen are 1H (atomic mass = 1.00783 amu; abundance 99.9885%) and 2H (atomic mass = 2.01410; abundance 0.0115%). (a) How many peaks will the mass spectrum have?

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