By Roger Grinter
ISBN-10: 0470013176
ISBN-13: 9780470013175
ISBN-10: 0470013184
ISBN-13: 9780470013182
This publication explores the best way quantum concept has turn into primary to our realizing of the behaviour of atoms and molecules. It appears on the means within which this underlies such a lot of of the experimental measurements we make, how we interpret these experiments and the language which we use to explain our effects. It makes an attempt to supply an account of the quantum idea and a few of its purposes to chemistry.This e-book is for researchers engaged on experimental elements of chemistry and the allied sciences in any respect degrees, from complex undergraduates to skilled learn undertaking leaders, wishing to enhance, by way of self-study or in small research-orientated teams, their realizing of the ways that quantum mechanics should be utilized to their difficulties. The e-book additionally goals to supply priceless history fabric for lecturers of quantum mechanics classes and their scholars.
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Additional info for The Quantum in Chemistry: An Experimentalist's View
Example text
38 38 39 40 40 41 41 44 46 46 46 47 48 . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 0 The Application of Quantum Mechanics INTRODUCTION Consider the hydrogen molecule, H–H. 674 × 10−27 kg and their nuclei are separated by a bond of length ∼74 × 10−12 m. In actual fact, this is the equilibrium bond length of the molecule, for this minute entity is in constant vibration with a frequency of ∼132 × 1012 oscillations per second.
3 Linear momentum, pˆ x . . . . . . . . . . . . 4 Kinetic energy, Wˆ . . . . . . . . . . . . . 5 Angular momentum, Lˆ . . . . . . . . . . . Summary . . . . . . . . . . . . . . . . . . . Bibliography and further reading . . . . . . . . . . . Problems for Chapter 3 . . . . . . . . . . . . . . The Quantum in Chemistry R. Grinter 2005 John Wiley & Sons, Ltd . . . . . . . . . . . .
The lowest spectrum is that of copper and the one immediately above it is iron. The remainder are the spectra of ore samples. 7 Some atomic emission spectra‡ ‡ Christian, Analytical Chemistry, 5th edn, Reprinted with permission of John Wiley & Sons, Inc. 24 From Classical to Quantum Mechanics But in the first decade of the 20th century the sharp lines of the atomic spectrum constituted a theoretical problem of great difficulty. Throughout this decade experimental evidence concerning the structure of the atom was accumulating and in 1911 Ernest Rutherford (1871–1937) proposed a model of the atom in which almost the whole mass of the atom was concentrated in a very small, positively charged nucleus at the centre while the negatively charged electrons occupied a much greater region of space surrounding the nucleus.
The Quantum in Chemistry: An Experimentalist's View by Roger Grinter
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