Physics for Geologists, Second edition
Physics for Geologists, Second edition
Physics for Geologists, Second edition
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60 Atomic structure and age-dating<br />
repel. So the electrons are attracted to the nucleus but repel each other.<br />
Moving charges generate a magnetic field.<br />
Particles have energy, and the unit is the electron volt, eV [ML~T-~]. This<br />
is the energy acquired by a particle carrying a single charge when acted on<br />
by a potential difference of one volt. 1 eV = 160.210 x joules (J). Be<br />
careful with units and dimensions here because the symbol is to be seen as<br />
a single symbol: eV, not e x V. An electric charge in coulombs [As] acted<br />
on by a volt [W A-l] gives an energy in watt-seconds which equals joules<br />
[W = J s-'1. The charge on an electron (e) is a fundamental and natural unit<br />
of electricity. Its value is 160.210 x lop2' coulombs (C), and all non-zero<br />
charges are a whole multiple of this.<br />
The number of protons is called the atomic number (Z, which is dimensionless).<br />
Elements are placed in the Periodic Table according to their atomic<br />
number because an element is determined by the charge of the protons in<br />
the nucleus, not by the neutrons. Neutrons and protons are much more<br />
massive than electrons (by factors of 1836.1 and 1838.63, respectively),<br />
and the total number of neutrons (N) and protons (Z) is called the atomic<br />
mass number (A). This is a whole number, dimensionless, that is very nearly<br />
equal to the mass of the atom because of the small mass of the electrons.<br />
The full notation is given by prefixes to the abbreviation of the element; the<br />
atomic number written subscript, and the atomic mass number written superscript,<br />
$. For example, '$ means that there are 6 protons, and 12 protons<br />
and neutrons (so, 6 neutrons) in the nucleus. The symbol is often abbreviated<br />
by leaving out the atomic number, <strong>for</strong> example, 12C. In older works<br />
you may find the superscript prefix after the element abbreviation, as c14.<br />
Isotopes<br />
Some atoms of simple elements have differing numbers of neutrons. Hydrogen<br />
is found in three <strong>for</strong>ms. :H,:H and :H, which we call hydrogen,<br />
deuterium and tritium. These are isotopes of hydrogen. Another example<br />
is carbon, which also has three isotopes: ';c, ' 2 ~<br />
and *:c. Isotopes of an<br />
element have the same general chemical properties (because protons, not<br />
neutrons, determine this) but differ slightly in mass and in some physical<br />
properties. They occupy the same place in the Periodic Table because they<br />
have the same atomic number.<br />
Isotopes are of two sorts: stable and unstable. Certain combinations of<br />
neutrons and protons are stable, others unstable. The unstable isotopes<br />
change spontaneously to a more stable <strong>for</strong>m by emitting or capturing parti-<br />
cles. These unstable isotopes are also called radioisotopes. It turns out that<br />
stable isotopes are those in which Z and N are nearly equal (or Z is about<br />
half A) - a small minority of the isotopes. Tritium, :H, is an unstable isotope<br />
of hydrogen. The decay of an unstable isotope also involves the emission of<br />
quanta of energy. The use of radioisotopes, such as ':c, in age-dating will<br />
be discussed below.<br />
Copyright 2002 by Richard E. Chapman