Predict a likely mode of decay for each unstable nuclide. c. In-132

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Identify the atomic number and mass number of the nuclide In-132. Indium (In) has an atomic number of 49.

Determine the neutron number by subtracting the atomic number from the mass number: Neutron number = 132 - 49.

Compare the neutron-to-proton ratio of In-132 to the stable isotopes of indium. A high neutron-to-proton ratio suggests beta decay.

Consider the position of In-132 on the chart of nuclides. Nuclides with a high neutron-to-proton ratio typically undergo beta decay to convert a neutron into a proton.

Conclude that the likely mode of decay for In-132 is beta decay, where a neutron is converted into a proton, emitting a beta particle (electron) and an antineutrino.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Nuclear Decay

Nuclear decay refers to the process by which an unstable atomic nucleus loses energy by emitting radiation. This can occur through various modes, including alpha decay, beta decay, and gamma decay, each characterized by the type of particle or energy released. Understanding the specific decay mode is crucial for predicting the behavior of unstable nuclides.

Isotopes and Stability

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons. The stability of an isotope depends on the ratio of neutrons to protons; an imbalance can lead to instability and subsequent decay. For example, Indium-132 (In-132) is an isotope that may undergo decay due to its neutron-to-proton ratio.

Decay Chains

Decay chains are sequences of decays that occur when a radioactive nuclide transforms into a series of other nuclides until a stable one is reached. Each step in the chain can involve different decay modes, and understanding these chains is essential for predicting the final products of a given unstable nuclide, such as In-132.

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