Of the two isotopes of tungsten, 160W and 185W, one decays by b emission and one decays by a emission. Which does which? Explain.

Key Concepts

Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This difference in neutron count results in varying atomic masses and can influence the stability of the nucleus. For tungsten, the isotopes 160W and 185W represent two different atomic masses, which can affect their decay processes.

Alpha and Beta Decay

Alpha decay involves the emission of an alpha particle, which consists of two protons and two neutrons, leading to a decrease in atomic number by two and mass number by four. In contrast, beta decay occurs when a neutron is transformed into a proton, emitting a beta particle (an electron) and increasing the atomic number by one. The type of decay is influenced by the stability of the isotopes.

Nuclear Stability

Nuclear stability is determined by the ratio of neutrons to protons in an atomic nucleus. Isotopes with an optimal ratio tend to be stable, while those with too many or too few neutrons may undergo radioactive decay to achieve stability. The specific decay mode (alpha or beta) is influenced by this stability, with heavier isotopes often favoring alpha decay and lighter or neutron-rich isotopes favoring beta decay.