By Glen E. Rodgers
This confirmed ebook introduces the fundamentals of coordination, solid-state, and descriptive main-group chemistry in a uniquely available demeanour, that includes a "less is extra" method. in line with the "less is extra" philosophy, the publication doesn't assessment themes lined typically chemistry, yet quite strikes at once into themes crucial to inorganic chemistry. Written in a conversational prose type that's relaxing and straightforward to appreciate, this ebook provides not just the fundamental theories and techniques of inorganic chemistry (in 3 self-standing sections), but in addition loads of the background and purposes of the self-discipline. This variation positive factors new paintings, extra assorted functions, and a brand new icon process. And to raised support readers know the way the likely disparate subject matters of the periodical desk attach, the ebook bargains revised insurance of the author's "Network of Interconnected principles" on new complete colour endpapers, in addition to on a handy tear-out card.
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Additional info for Descriptive Inorganic, Coordination, and Solid-State Chemistry, Third Edition
Such coordinated metal ions are sometimes referred to as complex cations or anions. Typically, coordination compounds are characterized by a wide range of bright colors. Varying the number and types of the ligands often significantly changes the color and also the magnetic characteristics of the compound. Some examples of coordinated (or complex) ions you may have encountered in earlier courses include the colorless [Ag(NH3)2]1 cation (often discussed in connection with the Group I qualitative analysis scheme), the dark blue [Cu(NH3)4]21 ion (a good test for the presence of 9 Copyright 2011 Cengage Learning.
1 Now how might you explain such data? More important, from a historical point of view, how did the chemists of the late 1860s, who had been schooled in the relatively new but extraordinarily successful ideas of organic chemistry, explain such data? 1, it seemed to have been fairly well established by then that each element has a valence, sometimes called a combining capacity, which is a single fixed value. Furthermore, many workers had found that organic compounds could be pictured as vast chains of carbon atoms composed of radicals and groups of various types that also appeared to have fixed valences.
Linus Pauling and others proposed that the overlap of atomic orbitals or special hybrid orbitals would result in a bond connecting one atom to another. Also developed during this time was the theory that molecules might be a group of nuclei held together by electronic confined waves appropriately called molecular (as opposed to atomic) orbitals. All of these ideas—from electron-dot diagrams to the valence-shell electron-pair repulsion (VSEPR) theory to valence-bond (VB) and molecular orbital (MO) theories—still aid modern chemists in picturing the structure and bonding of compounds.