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Ch.21 - Nuclear Chemistry
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.21 - Nuclear ChemistryProblema 2
Capitolo 21, Problema 2

Write the balanced nuclear equation for the reaction represented by the diagram shown here. [Section 21.2]
Diagram illustrating beta decay with two points connected by a red arrow.

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Identify the initial and final nuclei in the diagram. The initial nucleus is at (Z, N) = (6, 8), which corresponds to Carbon-14 (14^C). The final nucleus is at (Z, N) = (7, 7), which corresponds to Nitrogen-14 (14^N).
Recognize that the red arrow indicates a beta decay process, where a neutron is converted into a proton, emitting a beta particle (electron) and an antineutrino.
Write the general form of the beta decay equation: ^A_ZX -> ^A_{Z+1}Y + ^0_{-1}e + antineutrino.
Substitute the identified nuclei into the equation: ^14_6C -> ^14_7N + ^0_{-1}e + antineutrino.
Ensure the equation is balanced in terms of both mass number (A) and atomic number (Z). The mass number remains 14 on both sides, and the atomic number increases from 6 to 7, with the emission of a beta particle (electron) balancing the charge.

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Beta Decay

Beta decay is a type of radioactive decay in which a beta particle (an electron or a positron) is emitted from an atomic nucleus. This process occurs when a neutron in the nucleus transforms into a proton, emitting an electron (beta-minus decay) or when a proton transforms into a neutron, emitting a positron (beta-plus decay). Understanding beta decay is crucial for writing balanced nuclear equations.
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Beta Decay

Nuclear Equation

A nuclear equation represents the transformation of atomic nuclei during radioactive decay or nuclear reactions. It includes the symbols for the reactants and products, along with their atomic numbers and mass numbers. Balancing nuclear equations is essential to ensure that the number of nucleons (protons and neutrons) and charge are conserved during the reaction.
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Nuclear Binding Energy

Conservation of Mass and Charge

In nuclear reactions, the conservation of mass and charge states that the total mass number and total charge must remain constant before and after the reaction. This principle is fundamental when balancing nuclear equations, as it ensures that the number of protons and neutrons, as well as the overall charge, are equal on both sides of the equation.
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Law of Conservation of Mass
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Domanda del libro di testo

Indicate whether each of the following nuclides lies within the belt of stability in Figure 21.2: (a) neon-24. For any that do not, describe a nuclear decay process that would alter the neutron-to-proton ratio in the direction of increased stability. [Section 21.2]

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Domanda del libro di testo

In the sketch below, the red spheres represent protons and the gray spheres represent neutrons. (c) Based on its atomic number and mass number, do you think the product nucleus is stable or radioactive? [Section 21.3]

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Domanda del libro di testo

The steps below show three of the steps in the radioactive decay chain for 23290Th. The half-life of each isotope is shown below the symbol of the isotope. (a) Identify the type of radioactive decay for each of the steps (i), (ii), and (iii). [Sections 21.2 and 21.4]


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