Chapter 24 Notes PDF

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General Chemistry Textbook Notes and Practice Problems
Nuclear Chemistry...

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24 Introduction and Quick Prep

24.1a Nuclear vs. Chemical Reactions

24.1b Natural Radioactive Decay

24.1c Radioactive Decay and Balancing Nuclear Reactions

24.2a Band of Stability

24.2b Binding Energy

24.2c Relative Binding Energy

24.3a Rate of Decay

24.3b Radioactive Dating

24.4a Types of Fission Reactions

24.4b Nuclear Fuel

24.4c Nuclear Power

24.5a Stellar Synthesis of Elements

24.5b Induced Synthesis of Elements

24.5c Nuclear Medicine

24.5d Radioactivity in the Home

24.5 Mastery

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Unit Study Guide 24: Nuclear Chemistry

Key Terms nuclear reaction A reaction involving one or more atomic nuclei, resulting in a change in the identities of the isotopes alpha ( ) particle A helium nucleus ejected from certain radioactive substances beta ( ) particle An electron ejected at high speed from certain radioactive substances positron A particle having the same mass as an electron but a positive charge gamma ray High-energy electromagnetic radiation nuclide A nucleus with a specific makeup of neutrons and protons parent nucleus The nucleus undergoing a transformation in a radioactive decay reaction daughter nucleus The nucleus (or nuclei) produced in a radioactive decay reaction alpha decay The process where a nucleus emits an alpha particle beta decay A nuclear decay process that occurs when a neutron in an unstable nucleus is converted to a proton and an electron and the nuclear electron is ejected from the nucleus positron emission A type of radioactive decay that occurs when a proton in an unstable nucleus is converted to a neutron and a positron and the positron is ejected from the nucleus electron capture A nuclear process in which an inner-shell electron is captured band of stability A graphical representation of nuclei that are stable with respect to radioactive decay radioactive decay series A series of nuclear reactions by which a radioactive isotope decays to form a stable isotope binding energy ( ) The energy required to separate a nucleus into individual protons and neutrons mass defect The difference between the mass of the nuclear particles that make up a nucleus and the mass of an atom of the isotope of interest nucleon A nuclear particle, either a neutron or a proton fusion The highly exothermic process by which comparatively light nuclei combine to form heavier nuclei fission https://ng.cengage.com/static/nb/ui/evo/index.html?eISBN=9781305657571&snapshotId=2236523&id=1083220706&

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The highly exothermic process by which very heavy nuclei split to form lighter nuclei Geiger counter A device that detects ionizing radiation activity A measure of the rate of nuclear decay, the number of disintegrations observed in a sample per unit time curie A unit of radioactivity becquerel The SI unit of radioactivity; chain reaction A self-sustaining fission reaction critical mass The minimum mass of fissile material needed to sustain a critical chain reaction breeder reactor A nuclear reactor that produces fissile material at a greater rate than fissile material is consumed nuclear reactor A container in which a controlled nuclear reaction occurs moderator A substance used in a nuclear reactor to slow the neutrons and increase reaction efficiency control rod Rods that are inserted between the fuel rods in a nuclear reactor to slow or stop the chain reaction by absorbing neutrons plasma A gaslike phase of matter that consists of charged particles neutrino A massless, chargeless particle emitted by some nuclear reactions trans-uranium element The elements in the periodic table with atomic numbers greater than

Key Concepts Nuclear Reactions Nuclear reactions differ from chemical reactions in that nuclear reactions involve changes to the particles in the nucleus (24.1a). Natural radioactive decay is the process where an unstable nucleus emits energy and a small particle and is thereby transformed into a more stable nucleus (24.1b). The most common decay products are alpha particles, beta particles, positrons, and gamma rays (24.1b). Nuclear reactions are always balanced for charge and mass (24.1c). The most common decay processes are alpha decay, beta emission, positron emission, and electron capture (24.1c).

Nuclear Stability A plot of stable and unstable isotopes shows that for elements with neutrons than protons (24.2a). No nuclei with are stable (24.2a). https://ng.cengage.com/static/nb/ui/evo/index.html?eISBN=9781305657571&snapshotId=2236523&id=1083220706&

, a stable nucleus has more

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Nuclides with are most likely to decay by emitting an alpha particle (24.2a). Nuclides with too many neutrons are most likely to decay by emitting a beta particle (24.2a). Nuclides with too few neutrons are most likely to decay by emitting a positron or by electron capture (24.2a). The mass of an isotope is always less than the sum of the mass of its component particles (24.2b). The mass defect for an isotope is directly related to its binding energy (24.2b). A plot of relative binding energies shows that

has the most stable relative binding energy (24.2c).

Kinetics of Radioactive Decay Radioactive decay processes follow first-order kinetics (24.3a). The integrated first-order rate law relates the initial amount or activity of the radioactive material, the amount or activity at a specific time, the rate constant, and time (24.3a). Carbon dating is based on the natural abundance of material (24.3b).

and can be used to date objects containing organic

Fission and Fusion Fission can occur naturally or be induced by neutron bombardment (24.4a). Chain reactions, fission reactions that produce neutrons that can cause additional fission reactions, can be subcritical, critical, or supercritical (24.4a). The nuclear fuel used in most nuclear reactors and weapons, a mixture of and , must be enriched in before it is used in any application (24.4b). A nuclear power plant uses the energy produced by a fission reaction to generate electricity (24.4c). Nuclear fusion is a potential energy source, but it has proved difficult to initiate and sustain controlled fusion in a laboratory setting (24.4c).

Applications and Uses of Nuclear Chemistry Nuclear reactions that take place in stars and in interstellar gases help us understand the relative abundance of elements in the universe (24.5a). Elements and isotopes that do not occur naturally can be synthesized in bombardment reactions using particles generated in a cyclotron or a linear particle accelerator (24.5b). Radioisotopes are used in the medical imaging and treatment of diseases (24.5c). Household applications of nuclear chemistry include the use of radioisotopes in smoke detectors, the gamma irradiation of food, and the naturally occurring radon gas that can enter a home through a basement or foundation (24.5d).

Key Equations

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