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The most common types of nuclear radiation are alpha and beta radiation, and the processes for each are respectively alpha decay and beta decay.<ref>http://hyperphysics.phy-astr.gsu.edu/hbase/nuclear/radact.html</ref> There can also be gamma radiation associated with a nuclear decay. Alpha particles are [[helium]] nuclei (two protons and two neutrons); beta particles are high-energy [[electron]]s; gamma rays are high-energy [[photon]]s.  Alpha particles can normally be stopped by a sheet of paper or healthy human skin. Beta particles and gamma rays can penetrate one's body to cause great harm. Gamma radiation is also a form of electro-magnetic radiation, like X-rays or visible light.  (Contemporary jargon refers to alpha and beta ''particles'' and gamma ''rays'', though quantum mechanics makes the two actually the same.)

The most common types of nuclear radiation are alpha and beta radiation, and the processes for each are respectively alpha decay and beta decay.<ref>http://hyperphysics.phy-astr.gsu.edu/hbase/nuclear/radact.html</ref> There can also be gamma radiation associated with a nuclear decay. Alpha particles are [[helium]] nuclei (two protons and two neutrons); beta particles are high-energy [[electron]]s; gamma rays are high-energy [[photon]]s.  Alpha particles can normally be stopped by a sheet of paper or healthy human skin. Beta particles and gamma rays can penetrate one's body to cause great harm. Gamma radiation is also a form of electro-magnetic radiation, like X-rays or visible light.  (Contemporary jargon refers to alpha and beta ''particles'' and gamma ''rays'', though quantum mechanics makes the two actually the same.)

All forms of radioactivity follow the fundamental rules of mass and energy balance.

All forms of radioactivity follow the fundamental rules of mass and energy conservation, taking into account their interrelationship due to the formula [[E=mc²]].  In fact, radioactive decay illustrates this formula clearly, while chemical transformations involve a mass change so small as to be imperceptible.

==Alpha Decay==

==Alpha Decay==

As stated above, an alpha particle is the nucleus of a Helium atom, i.e., two protons and two neutrons. This arrangement means the alpha particle has a charge of +2, and an atomic mass of 4, the symbol for which is <math>{{}_2^4}He^{+2}</math>.

As stated above, an alpha particle is the nucleus of a Helium atom, i.e., two protons and two neutrons. This arrangement means the alpha particle has a charge of +2, and an atomic mass of 4, the symbol for which is <math>{{}_2^4}He^{+2}</math>.

For example, the most common [[isotope]] of Uranium is Uranium-238. The [[mass number]],<ref>The mass number is the (integer) number of nucleons. It is very close to the [[atomic mass]] of the isotope measured in amu, because the masses of protons and neutrons are very close, and the deviations (due to [[E=mc²]]) are small. So the terms are often used nearly interchangeably.</ref> 238, is the sum of the number of protons and the number of neutrons. Since all Uranium atoms have 92 protons, there are 146 neutrons. The initial step in Uranium-238 decaying (eventually) into Lead-206 is an alpha decay:

For example, the most common [[isotope]] of Uranium is Uranium-238. The [[mass number]],<ref>The mass number is the (integer) number of nucleons. It is very close to the [[atomic mass]] of the isotope measured in amu, because the masses of protons and neutrons are very close, and the deviations (due to E=mc²) are small. So the terms are often used nearly interchangeably.</ref> 238, is the sum of the number of protons and the number of neutrons. Since all Uranium atoms have 92 protons, there are 146 neutrons. The initial step in Uranium-238 decaying (eventually) into Lead-206 is an alpha decay:

<center><math>{{}_{92}^{238}}U </math> &rarr; <math>{{}_2^4}He + {{}_{90}^{234}}Th</math></center>

<center><math>{{}_{92}^{238}}U </math> &rarr; <math>{{}_2^4}He + {{}_{90}^{234}}Th</math></center>

Note that the proton count (92) is conserved, as is are the mass numbers (238). So the neutron count (146) is also balanced. No particles are created or destroyed.

Note that the proton count (92) is conserved, as is are the mass numbers (238). So the neutron count (146) is also balanced. No particles are created or destroyed; they are simply pulled apart.

This decay releases about 4.3 MeV of kinetic energy, in the form of the motion of the alpha particle. In chemical terms we would say that this decay is an exothermic reaction. The energy comes from the potential nuclear energy of the Uranium atom&mdash;the Uranium atom has a higher potential energy (by 4.3 Mev) than the sum of the potential energies of the Thorium and Helium atoms.  A careful accounting of the atomic masses (remember, atomic mass is only approximately equal to mass number) will show that mass was lost, in accordance with [[E=mc²]].

This decay releases about 4.3 MeV of kinetic energy, in the form of the motion of the alpha particle. In chemical terms we would say that this decay is an exothermic reaction. The energy comes from the potential nuclear energy of the Uranium atom&mdash;the Uranium atom has a higher potential energy (by 4.3 Mev) than the sum of the potential energies of the Thorium and Helium atoms.  A careful accounting of the atomic masses (remember, atomic mass is only approximately equal to mass number) will show that mass was lost, in accordance with [[E=mc²]].

As with the alpha decay, notice that the particle count is again conserved. The energy released by this decay is 0.55 MeV.

As with the alpha decay, notice that the particle count is again conserved. The energy released by this decay is 0.55 MeV.

An interesting note about Strontium-90 is that is a synthetic isotope (meaning, it is not found naturally occurring, but must be manufactured) that is a by-product of nuclear weapons explosions. In the 1950s and 1960s, it was common to test nuclear weapons by exploding them in the very high upper atmosphere. Unfortunately, this resulted in a large amount of Strontium-90 particles that eventually settled back to earth, contaminating grass lands. The grasses were eaten by cattle, and the cattle were eaten by humans.

An interesting note about Strontium-90 is that is a synthetic isotope (meaning, it is not found naturally occurring, but must be manufactured) that is a by-product of nuclear weapons explosions. In the 1950s and 1960s, it was common to test nuclear weapons by exploding them in the very high upper atmosphere. Unfortunately, this resulted in a large amount of Strontium-90 particles that eventually settled back to earth, contaminating grass lands. The grasses were eaten by cattle, and the cattle were eaten (and their milk consumed) by humans.

Since Strontium is chemically very similar to Calcium (it is in the same column in the Periodic Table), any entrance of Strontium in the body will tend to replace the Calcium in our bones. In the case of Strontium-90, this meant that radioactive Strontium was now chemically bonded to our bones, and the 1970s saw a rise in bone cancer as a result. Fortunately, this type of testing was halted, and the [[half-life]] of Strontium-90 is a relatively short 28 years, meaning, at this point most of the synthetic, radioactive Strontium-90 produced by weapons testing has decayed out of the environment.

Since Strontium is chemically very similar to Calcium (it is in the same column in the Periodic Table), any entrance of Strontium in the body will tend to replace the Calcium in our bones. In the case of Strontium-90, this meant that radioactive Strontium was now chemically bonded to people's bones, and the 1970s saw a rise in bone cancer as a result. Fortunately, this type of testing was halted, and the [[half-life]] of Strontium-90 is a relatively short 28 years, meaning, at this point most of the synthetic, radioactive Strontium-90 produced by weapons testing has decayed out of the environment.

==Energy of Radioactive Decay==

==Energy of Radioactive Decay==

Just for a point of comparison, it takes about a minute to boil a cup of water in a 1000 Watt microwave. One Watt is equivalent to one Joule per second, so it takes 60,000 Joules of energy to boil a cup of water. But a single Joule of energy is the same as 6.24x10¹⁸ eV!

Just for a point of comparison, it takes about a minute to boil a cup of water in a 1000 Watt microwave. One Watt is equivalent to one Joule per second, so it takes 60,000 Joules of energy to boil a cup of water. But a single Joule of energy is the same as 6.24x10¹⁸ eV!

So even when a nuclear decay has an associated energy in the thousands (keV) or millions (MeV) of electron volts, we're still billions of factors away from having enough energy to boil a cup of water. The danger is not from a single atomic decay, but from many trillions of atomic decays occurring within rapid succession, in which case we do reach energies capable of producing serious burns on the skin.

So even when a nuclear decay has an associated energy in the thousands (keV) or millions (MeV) of electron volts, the decay of one atom is still billions of factors away from having enough energy to boil a cup of water. But, when measured in the more usual way, of Joules per kilogram of reactant, the energy release is enormous.  The energy released by the decay of 1 gram of Polonium-210 is 2.5x10¹³ Joules.  (It isn't released all at once; the half-life is 138 days.)

 

<!-- This section is specifically referenced, under this name, by other articles, such as the "Radiometric dating" page.  Do not change this name without repairing those other pages. -->

Although the exact mechanisms of alpha, beta, and gamma decay are quite different, all three are dictated by the rules of [[quantum mechanics]].  These rules dictate a fixed probability, per second, that a nucleus will decay.  So a nucleus has some probability, say P, surviving one second without decaying.  For Polonium-210, P=.99999994, for example.  For U-238, P=.999999999999999995.

 

After 2 seconds, the fraction of material left is P².  After 10 seconds, it is P¹⁰, and so on.  So the fraction remaining is an exponential function of time.  This is the reason for the characteristic exponential decay of radioactive substances.  The type of decay doesn't matter; the decay is always exponential.  The usual way this is described is the ''half-life'', which is the time for one half of the sample to disintegrate.  The half-life can be seen to be log(1/2) / log(P).  Half-lives can vary from quantities like 10^-21 seconds for Beryllium-13, to 10¹⁸ years (far more than the age of the universe) for Tungsten-182.

 

While the mechanisms for decay, and hence the half-lives of various isotopes, are well understood on theoretical grounds, the calculations are so complex that half-lives are measured experimentally.  The measured half-lives of the various isotopes of elements are known to be fixed quite accurately.  Careful astronomical observations show that half-lives have not changed significantly in billions of years&mdash;spectral lines from distant galaxies would have shifted perceptibly if the constants involved had changed.  In some cases radioactive decay itself can be observed and measured in distant galaxies when a supernova explodes and ejects radioactive nuclei.

==Antiquated notions==

==Antiquated notions==