We saw in Chapter 2 “Elements, Atoms, and the Periodic Table” that atoms are composed of subatomic particles—protons, neutrons, and electrons. Protons and neutrons are located in the nucleus and provide most of the mass of the atom, while electrons circle the nucleus in shells and subshells and account for an atom’s radius.

We also introduced in Chapter 2 “Elements, Atoms, and the Periodic Table” the notation for succinctly representing an isotope of a particular atom:

[latex]_{6}^{12}\textrm{C}[/latex]

The element in this example, represented by the symbol C, is carbon. Its atomic number, 6, is the lower left subscript on the symbol and is the number of protons in the atom. The mass number, the superscript to the upper left of the symbol, is the sum of the number of protons and neutrons in the nucleus of this particular isotope. In this case, the mass number is 12, which means that the number of neutrons in the atom is 12 − 6 = 6 (that is, the mass number of the atom minus the number of protons in the nucleus equals the number of neutrons). Occasionally, the atomic number is omitted in this notation because the symbol of the element itself conveys its characteristic atomic number. The two isotopes of hydrogen, ²H and ³H, are given their own names: deuterium (D) and tritium (T), respectively. Another way of expressing a particular isotope is to list the mass number after the element name, like carbon-12 or hydrogen-3.

Atomic theory in the 19th century presumed that nuclei had fixed compositions. But in 1896, the French scientist Henri Becquerel found that a uranium compound placed near a photographic plate made an image on the plate, even if the compound was wrapped in black cloth. He reasoned that the uranium compound was emitting some kind of radiation that passed through the cloth to expose the photographic plate. Further investigations showed that the radiation was a combination of particles and electromagnetic rays, with its source being the atomic nucleus. These emanations were ultimately called radioactivity.

There are three main forms of radioactive emissions. The first is called an alpha particle, which is symbolized by the Greek letter α. An alpha particle is composed of two protons and two neutrons, and so is the same as a helium nucleus. Therefore [latex]_{2}^{4}\textrm{He}[/latex]  is used to represent an alpha particle.  It has a 2+ charge. When a radioactive atom emits an alpha particle, the original atom’s atomic number decreases by two (because of the loss of two protons), and its mass number decreases by four (because of the loss of four nuclear particles). We can represent the emission of an alpha particle with a chemical equation—for example, the alpha-particle emission of uranium-235 is as follows:

[latex]_{92}^{235}\textrm{U}\rightarrow[/latex]  [latex]_{2}^{4}\textrm{He} +_{90}^{231}\textrm{Th} [/latex] 

How do we know that a product of the reaction is   [latex]_{90}^{231}\textrm{Th}[/latex]  ? Use the law of conservation of matter, which says that matter cannot be created or destroyed. This means there must be the same number of protons and neutrons on both sides of the chemical equation. If the uranium nucleus loses 2 protons, there are 90 protons remaining, identifying the element as thorium. Moreover, if 4 nuclear particles are lost from the original 235, there are 231 remaining. Thus, we use subtraction to identify the isotope of the thorium atom—in this case,  [latex]_{90}^{231}\textrm{Th}[/latex] .

Chemists use the names parent isotope and daughter isotope to represent the original atom and the product other than the alpha particle. In the previous example, [latex]_{92}^{235}\textrm{U}[/latex] is the parent isotope, and  [latex]_{90}^{231}\textrm{Th}[/latex] is the daughter isotope. When one element changes into another in this manner, it undergoes radioactive decay.

The second major type of radioactive emission is called a beta particle, symbolized by the Greek letter β. A beta particle is an electron ejected from the nucleus (not from the shells of electrons about the nucleus) and has a 1− charge. We can also represent a beta particle as [latex]_{-1}^{0}\textrm{e}[/latex]  or β. The net effect of beta particle emission on a nucleus is that a neutron is converted to a proton. The overall mass number stays the same, but because the number of protons increases by one, the atomic number goes up by one. Carbon-14 decays by emitting a beta particle:

[latex]_{6}^{14}\textrm{C}\rightarrow[/latex] [latex]_{7}^{14}\textrm{N}+[/latex] [latex]_{-1}^{0}\textrm{e}[/latex]

Again, the sum of the atomic numbers is the same on both sides of the equation, as is the sum of the mass numbers. Note that the electron must be  assigned an “atomic number” of 1−, equal to its charge, for this to work.

The third major type of radioactive emission is not a particle but rather a very energetic form of electromagnetic radiation called gamma rays, symbolized by the Greek letter γ. Gamma rays themselves do not carry an overall electrical charge, but they may knock electrons out of atoms in a sample of matter and make it electrically charged.  Therefore,  gamma rays are considered to be ionizing radiation. In the radioactive decay of radon-222, both alpha and gamma radiation are emitted, with the latter having an energy of 8.2 × 10⁻¹⁴ J per nucleus decayed:

[latex]_{86}^{222}\textrm{Rn}\rightarrow[/latex] [latex]_{2}^{4}\textrm{He}+_{84}^{218}\textrm{Po}+\gamma[/latex]

This may not seem like much energy, but if 1 mol of radon atoms were to decay, the gamma ray energy would be 49 million kJ!

Occasionally, an atomic nucleus breaks apart into smaller pieces in a radioactive process called spontaneous fission (or fission). Typically, the daughter isotopes produced by fission are a varied mix of products, rather than a specific isotope as with alpha and beta particle emission. Often, fission produces excess neutrons that will sometimes be captured by other nuclei, possibly inducing additional radioactive events. Uranium-235 undergoes spontaneous fission to a small extent. One typical reaction is

[latex]_{92}^{235}\textrm{U}\rightarrow[/latex] [latex]_{56}^{139}\textrm{Ba}+_{36}^{94}\textrm{Kr}+2_{0}^{1}\textrm{n}[/latex]

where [latex]_{0}^{1}\textrm{n}[/latex]  is a neutron. As with any nuclear process, the sums of the atomic numbers and the mass numbers must be the same on both sides of the equation. Spontaneous fission is found only in large nuclei. The smallest nucleus that exhibits spontaneous fission is lead-208.