Nuclear Chemistry 267 in C#.NET

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Nuclear Chemistry 267
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U Rapid Review
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Know how nuclear equations are balanced: The same sums of both mass and atomic numbers appear on both sides of the equation Know the five naturally occurring decay modes:
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4 1 Alpha emission, in which a helium nucleus, 2 He , is emitted from the nucleus 0 2 Beta emission in which an electron, 1e, is emitted from the nucleus This is due to the conversion of a neutron into a proton plus the beta particle 3 Gamma emission, in which high-energy electromagnetic radiation is emitted from the nucleus This commonly accompanies the other types of radioactive decay It is due to the conversion of a small amount of matter into energy 0 4 Positron emission, in which a positron, +1 e , a particle having the same mass as an electron but a positive charge, is emitted from the nucleus This is due to a proton converting into a neutron and the positron 5 Electron capture, in which an inner-shell electron is captured by a proton in the nucleus with the formation of a neutron X-rays are emitted as the electrons cascade down to fill the vacancy in the lower energy level
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Know that nuclear stability is best related to the neutron-to-proton ratio (n/p), which starts at about 1/1 for light isotopes and ends at about 15/1 for heavier isotopes with atomic numbers up to 83 All isotopes of atomic number greater than 84 are unstable and will commonly undergo alpha decay Below atomic number 84, neutron-poor isotopes will probably undergo positron emission or electron capture, while neutron-rich isotopes will probably undergo beta emission Know that the half-life, t 1/2, of a radioactive isotope is the amount of time it takes for one-half of the sample to decay Know how to use the appropriate equations to calculate amounts of an isotope remaining at any given time, or use similar data to calculate the half-life of an isotope Know how to use Einstein s equation E = mc 2 to calculate the amount of energy produced from a mass defect (the amount of matter that was converted into energy)
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CHAPTER
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Organic Chemistry
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IN THIS CHAPTER Summary: Organic chemistry is the study of the chemistry of carbon Almost all the compounds containing carbon are classified as organic compounds Only a few for example, carbonates and cyanides are classified as inorganic It used to be thought that all organic compounds had to be produced by living organisms, but this idea was proven wrong in 1828 when German chemist Friedrich W hler produced the first organic compound from inorganic starting materials Since that time, chemists have synthesized many organic compounds found in nature and have also made many never found naturally It is carbon s characteristic of bonding strongly to itself and to other elements in long, complex chains and rings that gives carbon the ability to form the many diverse and complex compounds needed to support life
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KEY IDEA
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Keywords and Equations
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No keywords or equations specific to this chapter are listed on the AP exam
Alkanes
Alkanes are members of a family of organic compounds called hydrocarbons, compounds of carbon and hydrogen These hydrocarbons are the simplest of organic compounds, but are extremely important to our society as fuels and raw materials for chemical industries We heat our homes and run our automobiles through the combustion (burning) of these hydrocarbons Paints, plastics, and pharmaceuticals are often made from hydrocarbons Alkanes are hydrocarbons that contain only single covalent bonds within their molecules They are called saturated hydrocarbons because they are bonded to the maximum number of other atoms These alkanes may be straight-chained hydrocarbons, in which the carbons are sequentially bonded; branched hydrocarbons, in which another hydrocarbon group is bonded to the hydrocarbon backbone ; or they may be cyclic, in which the hydrocarbon is composed entirely or partially of a ring system The straight-chained and branched
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