Predict a likely mode of decay for each unstable nuclide. b. Ru-90 c. P-27 d. Sn-100

Verified step by step guidance

1. Identify the atomic number of the element. Ruthenium (Ru) has an atomic number of 44.
2. Determine the neutron number by subtracting the atomic number from the mass number: Neutron number = 90 - 44.
3. Compare the neutron-to-proton (N/Z) ratio to the stable range for elements around ruthenium. For elements with atomic numbers around 44, a stable N/Z ratio is approximately 1.25.
4. Evaluate if the nuclide is neutron-rich or neutron-poor. If the N/Z ratio is higher than the stable range, the nuclide is neutron-rich.
5. Predict the mode of decay: Neutron-rich nuclides typically undergo beta decay (β-) to convert a neutron into a proton, thereby reducing the N/Z ratio.

Key Concepts

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 involving the transformation of the nucleus into a more stable state. Understanding the type of decay is crucial for predicting the behavior of unstable nuclides.

Beta Decay

Beta decay is a specific type of nuclear decay where a neutron in the nucleus is transformed into a proton, emitting a beta particle (an electron or positron) and an antineutrino or neutrino. This process increases the atomic number of the element by one, resulting in the formation of a new element. It is a common decay mode for nuclides that are neutron-rich.

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, Ru-90, with its specific neutron-to-proton ratio, may undergo beta decay if it is found to be unstable.