Rev. 0CH-01Page 23Fundamentals of ChemistryDOE-HDBK-1015/1-93CHEMICAL BONDINGCHEMICAL BONDINGThe development of matter, no matter what the form, is the result of thepractical application of the assumptions, hypotheses, theories, and laws thatchemists have formulated from their research into the nature of matter,energy, and change. This chapter will address some of these theories andlaws. Chemical bonds and how atoms bond to form molecules will bediscussed. In addition, an introduction to organic chemistry is provided.EO 2.1 DEFINE the following terms:a.Ionic bondsc.Covalent bondsb.Van der Waals forcesd.Metallic bondsEO 2.2 DESCRIBE the physical arrangement and bonding of a polarmolecule.EO 2.3 DESCRIBE the three basic laws of chemical reactions.EO 2.4 STATE how elements combine to form chemical compounds.EO 2.5 EXPLAIN the probability of any two elements combining toform a compound.EO 2.6 DEFINE the following terms:a.Mixtured.Soluteb.Solvente.Solutionc.Solubilityf.EquilibriumChemicalBondingAs stated in the previous chapter, the number of electrons in the outer, or valence, shelldetermines the relative activity of the element. The arrangement of electrons in the outer shellexplains why some elements are chemically very active, some are not very active, and othersare inert. In general, the fewer electrons an element must lose, gain, or share to reach a stableshell structure, the more chemically active the element is. The likelihood of elements formingcompounds is strongly influenced by the completion of the valence shell and by the stabilityof the resulting molecule. The more stable the resulting molecules are, the more likely thesemolecules are to form. For example, an atom that "needs" two electrons to completely fill thevalence shell would rather react with another atom which must give up two electrons tosatisfy its valence.
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