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2013 | OriginalPaper | Chapter

1. Aspects of Physical Chemistry

Author : Ian W. M. Smith

Published in: Astrochemistry and Astrobiology

Publisher: Springer Berlin Heidelberg

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Abstract

Some of those topics in physical chemistry that are especially relevant to astrochemistry and astrobiology are introduced in this chapter. I start with some discussion of the chemical elements: their relative abundances, their electronic structure, and how chemical bonds are formed in simple molecules. This leads to a discussion of how changes between energy levels lead to molecular spectra that can be used to identify molecules at a distance – even the vast distances from Earth to astronomical objects. Having considered forces within molecules, I then discuss the weaker forces between molecules, including hydrogen bonding. The next section focuses on chemical reactions from both the standpoint of thermodynamics and that of chemical kinetics. Finally, some consideration is given to surface processes, which can occur on the dust particles found in the interstellar medium, and enzyme kinetics, which is of great importance in biology.

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next chapter The Molecular Universe
Footnotes
1
The notation 2 1H specifies the number of protons, 1, and the number of nucleons (protons + neutrons), 2. Any electrically neutral atom contains the same number of electrons and protons. To refer to an ion, a superscript after the chemical symbol is added. Thus a deuteron is signified by 2 1H1+. The number of protons in an elemental atom corresponds to its atomic number, Z.
 
2
These elements, heavier than lithium, are all referred to by astronomers as ‘metals’ – somewhat to the amusement, or bemusement, of those trained as chemists.
 
3
This total does not include the isotopomers of several species that have also been observed.
 
4
By convention, the ‘forward’ reaction is that proceeding from left to right in the chemical equation, and the ‘reverse’ reaction is that proceeding from right to left.
 
5
Associated with each vibration in a molecule, there is ‘zero-point energy’ corresponding approximately to ½hv where v is the frequency of the vibration. Consequently, as shown in Fig. 1.2, the lowest vibrational energy level with the quantum number v = 0, has an energy ½hv above the minimum of the potential energy curve.
 
6
A catalyst accelerates the rate of reaction without changing the position of equilibrium and without itself being changed during the course of reaction. As the equilibrium constant is not changed, it means that any catalyst must accelerate the rates of forward and reverse reactions in equal proportions. The changes in rate occur because the catalyst lowers the Gibbs energies of activation for the forward and reverse reactions.
 
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Metadata
Title
Aspects of Physical Chemistry
Author
Ian W. M. Smith
Copyright Year
2013
Publisher
Springer Berlin Heidelberg
Book
Astrochemistry and Astrobiology

Print ISBN: 978-3-642-31729-3

Electronic ISBN: 978-3-642-31730-9

Copyright Year: 2013

DOI
https://doi.org/10.1007/978-3-642-31730-9_1

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