By Francis A. Carey, Robert M. Giuliano
A industry prime, conventional method of natural Chemistry all through all 8 variations, natural Chemistry has been designed to satisfy the desires of the "mainstream," two-semester, undergraduate natural chemistry direction. This best-selling textual content offers scholars a great figuring out of natural chemistry through stressing how primary response mechanisms functionality and reactions take place.
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Sample text
It is often convenient to speak of the valence electrons of an atom. These are the outermost electrons, the ones most likely to be involved in chemical bonding and reactions. For second-row elements these are the 2s and 2p electrons. Because four orbitals (2s, 2px, 2py , 2pz) are involved, the maximum number of electrons in the valence shell of any second-row element is 8. Neon, with all its 2s and 2p orbitals doubly occupied, has eight valence electrons and completes the second row of the periodic table.
A neutral nitrogen has five electrons in its valence shell. The electron count for nitrogen in nitric acid is one less than that of a neutral nitrogen atom, so its formal charge is ϩ1. Electrons in covalent bonds are counted as if they are shared equally by the atoms they connect, but unshared electrons belong to a single atom. Thus, the oxygen that is doubly bonded to nitrogen has an electron count of six (four electrons as two unshared pairs ϩ two electrons from the double bond). Because this is the same as a neutral oxygen atom, its formal charge is 0.
Helium, neon, and argon belong to the class of elements known as noble gases or rare gases. The noble gases are characterized by an extremely stable “closed-shell” electron configuration and are very unreactive. Structure determines properties and the properties of atoms depend on atomic structure. All of an element’s protons are in its nucleus, but the element’s electrons are distributed among orbitals of various energy and distance from the nucleus. More than anything else, we look at its electron configuration when we wish to understand how an element behaves.