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Chapter 4: Problem 88

Explain what must occur before a radioactive atom stops to undergo further radioactive decay

Short Answer

Expert verified
A radioactive atom stops decaying once it becomes a stable isotope.

Step by step solution

01

Understand Radioactive Decay

Radioactive decay is the process by which an unstable atomic nucleus loses energy by emitting radiation, such as alpha particles, beta particles, or gamma rays. This process continues until a stable isotope is reached.
02

Identify Stable Isotopes

A stable isotope is an isotope of an element that does not undergo radioactive decay. An atom stops undergoing further radioactive decay once it transforms into a stable isotope through successive decay events. This stable form does not emit radiation and thus does not decay further.
03

Comprehend Half-lives

The time it takes for half of the radioactive atoms in a sample to decay is called a half-life. Over multiple half-lives, a radioactive substance may decay to a level where it effectively stops changing due to reaching a stable form, ending further decay.
04

Analyze the End of Decay

The decay process in a radioactive atom stops once it reaches a non-radioactive or stable form, meaning the atom has transformed into an isotope that will not further decay.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Stable isotopes
Every chemical element has isotopes. These are different forms of the same element, distinguished by a varying number of neutrons in their nuclei. While some isotopes are radioactive and decay over time, stable isotopes do not. Once an unstable, radioactive atom has transformed into a stable isotope, it ceases to emit radiation.
This is because stable isotopes are energetically favorable and are not subject to further decay.
Essentially, stable isotopes are the endpoint in the lifecycle of decay for radioactive atoms. They help scientists understand how elements evolve over time and provide insights into natural processes that depend on element stability.
Half-life
The concept of half-life is pivotal in understanding radioactive decay. A half-life is the time required for half of the radioactive atoms in a sample to transform into something different, often turning into more stable isotopes.
Knowing the half-life of a radioactive material allows scientists to predict how quickly a sample will decay.
For example:
  • If a substance has a half-life of 1,000 years, then half of it will remain unchanged after that period.
  • Another 1,000 years will see half of the remaining radioactive material decay, and so on.
This process continues, moving the substance closer to becoming completely stable, at which point its decay ceases.
Radioactive atoms
Radioactive atoms are characterized by an unstable nucleus that loses energy in the form of radiation. These atoms continue to undergo decay until they reach a stable form. The process involves emission of alpha particles, beta particles, or gamma rays.
Unstable isotopes can be naturally occurring, such as Uranium-238, or artificially created in laboratories.
Reasons why atoms are radioactive include:
  • Imbalance of protons and neutrons in the nucleus.
  • Excess of energy within the atom.
Understanding radioactive atoms is critical in fields ranging from archaeology, where they help date ancient artifacts, to medicine, where they're used in imaging and treatments.

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Most popular questions from this chapter

Infer Sulfur's average atomic mass is close to the whole number \(32 .\) Chlorine's average atomic mass is 35.453 , which is not a whole number. Suggest a possible reason for this difference.

Challenge Nitrogen has two naturally occurring isotopes, \(\mathrm{N}-14\) and \(\mathrm{N}-15 .\) Its atomic mass is 14.007 . Which isotope is more abundant? Explain your answer.

Explain what keeps the electrons confined in the space surrounding the nucleus.

Relative Abundances Magnesium constitutes about 2\(\%\) of Earth's crust and has three naturally occurring isotopes. Suppose you analyze a mineral and determine that it contains the three isotopes in the following proportions: Mg- 24 (abundance = \(79 \% ), \mathrm{Mg}-25\) (abundance \(=10 \% ),\) and \(\mathrm{Mg}-26\) (abundance = 11 \(\%\) ). If your friend analyzes a different mineral containing magnesium, do you expect her to obtain the same relative abundances for each magnesium isotope? Explain your reasoning.

What type of reaction involves changes in the nucleus of an atom?
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