By James E. House;Kathleen A. House
This e-book covers the synthesis, reactions, and houses of parts and inorganic compounds for classes in descriptive inorganic chemistry. It is appropriate for the one-semester (ACS-recommended) path or as a complement ordinarily chemistry classes. excellent for significant and non-majors, the booklet comprises wealthy graphs and diagrams to augment the content material and maximize studying. comprises multiplied insurance of chemical bonding and stronger therapy of Buckminster FullerenesIncorporates new business purposes matched to key issues within the textual content
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Additional info for Descriptive Inorganic Chemistry, Second Edition
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1996). Inorganic Chemistry. San Diego, CA: Academic Press. This book is subtitled “An Industrial and Environmental Perspective,” and it deals at length with some of the important commercial processes. Problems 1. What are the names of the solid, liquid, and gaseous regions of the earth’s crust? 2. What metal is the primary component of the earth’s core? 3. Elements such as copper and silver are present in the earth’s crust in very small percentages. What is it about these elements that makes their recovery economically feasible?
7) gives h mv ð2:8Þ nh 2π ð2:9Þ 2πr ¼ n which can be rearranged to give mvr ¼ It should be noted that this relationship is identical to Bohr’s assumption about stable orbits (shown in Eq. 1)! In 1926, Erwin Schrödinger made use of the wave character of the electron and adapted a previously known equation for three-dimensional waves to the hydrogen atom problem. The result is known as the Schrödinger wave equation for the hydrogen atom, which can be written as ∇2 Ψ þ 2m ðE À VÞΨ ¼ 0 ħ2 ð2:10Þ where Ψ is the wave function, ħ is h/2π, m is the mass of the electron, E is the total energy, V is the potential energy (in this case the electrostatic energy) of the system, and ∇2 is the Laplacian operator: ∇2 ¼ ∂2 ∂2 ∂2 þ þ ∂x2 ∂y2 ∂z2 ð2:11Þ The wave function is, therefore, a function of the coordinates of the parts of the system that completely describes the system.
These situations are referred to as antibonding cases. Because the degree to which electron density increases between two nuclei depends on the overlap integral, covalent bond strength essentially depends on that quantity. 10 Some types of overlap of orbitals that can lead to bond formation (S > 0). 11 Nonbonding arrangements of orbitals (S ¼ 0). 12 Some antibonding arrangements of orbitals. conditions that lead to larger overlap integral values will generally increase the bond strength. A large value of the overlap integral occurs under the following conditions: 1.