By Department of Energy
The Chemistry guide used to be constructed to aid nuclear facility working contractors in delivering operators, upkeep team of workers, and the technical employees with the required basics education to make sure a easy figuring out of chemistry. The guide contains info at the atomic constitution of topic; chemical bonding; chemical equations; chemical interactions concerned with corrosion tactics; water chemist!*)' keep an eye on, together with the foundations of water remedy; the dangers of chemical compounds and gases, and uncomplicated gaseous diffusion procedures. this data will offer body of workers with a beginning for realizing the chemical homes of fabrics and how those houses can impose barriers at the operation of kit and structures.
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Extra resources for Chemistry Fundamentals Handbook
Rev. 0 Page 21 CH-01 THE PERIODIC TABLE DOE-HDBK-1015/1-93 Fundamentals of Chemistry Summary The important information from this chapter is summarized below. Periodic Table Summary & The subdivisions of the periodic table are periods, groups, and classes. The horizontal rows are called periods. The vertical columns are called groups. The entire table consists of three classes: metals, non-metals, and semimetals. & The subdivisions of the periodic chart have been explained such that the student should be able to identify them if given a periodic table.
A scientific law is a condensed statement of facts which has been discovered by experiment. There are three basic laws that apply to chemical reactions. They are the Law of Conservation of Mass, the Law of Definite Proportions, and the Law of Multiple Proportions. These laws are described here to help the reader in understanding the reasons elements and compounds behave as they do. 1. The Law of Conservation of Mass This law states that in a chemical reaction the total mass of the products equals the total mass of the reactants.
The three types of electrolytes are acids, bases, and salts. Acids are substances that dissociate in water to produce hydrogen (H+). An example of a common acid is sulfuric acid, H2SO4. In solution, H2 SO4 dissociates to form hydrogen and sulfate ions according to the following equation. , liquid (aq). solid (s), or gas (g). Additional examples of acids are vinegar, aspirin, and lemon juice. These substances share the following common properties. 1. Acid solutions taste sour (acid means "sour" in Latin).