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Chapter 24: Problem 27

Why is helium found in deposits of uranium and thorium ores? What kind of radioactive emission produces it?

Short Answer

Expert verified
Helium is found in uranium and thorium ores due to alpha decay, which emits alpha particles that form helium atoms.

Step by step solution

01

- Understand the relationship between uranium, thorium, and helium

Helium is found in deposits of uranium and thorium ores because these elements undergo radioactive decay. Over time, uranium and thorium atoms break down, leading to the formation of helium atoms.
02

- Identify the type of radioactive emission

During the radioactive decay of uranium and thorium, they emit alpha particles. An alpha particle consists of 2 protons and 2 neutrons, which is essentially the nucleus of a helium atom.
03

- Explain the formation of helium

When uranium or thorium emits an alpha particle, this particle can capture two electrons from the surrounding environment to form a neutral helium atom. Therefore, the presence of helium in such deposits is a direct result of alpha decay.

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Key Concepts

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

Radioactive Decay
Radioactive decay is a natural process by which unstable atomic nuclei lose energy by emitting radiation. This occurs in elements like uranium and thorium, which are not stable.
There are different types of radioactive decay, but the one we are focusing on here is alpha decay.
Alpha decay is when an unstable nucleus emits an alpha particle, losing some of its energy and mass and transforming into a different element.
For example, uranium-238 decays into thorium-234 by emitting an alpha particle, and thorium-234 decays into radium-226 in a similar manner.
Alpha decay changes the original element into a new one while emitting radiation in the form of alpha particles.
Alpha Particles
Alpha particles are a type of radiation emitted during radioactive decay. They are made up of 2 protons and 2 neutrons, which is the same as a helium-4 nucleus.
Because of their composition, alpha particles are relatively heavy and carry a positive charge.
They do not travel very far and can be stopped by a sheet of paper or even the outer layer of human skin.
However, if alpha particles are ingested or inhaled, they can cause significant damage to living tissues.
The emission of alpha particles from uranium and thorium is what eventually leads to the formation of helium.
Helium Formation
Helium formation in uranium and thorium deposits is a direct result of alpha decay.
When an alpha particle is emitted during the decay process, it can capture two electrons from its surroundings.
This turns the alpha particle, which is initially just a helium nucleus, into a fully formed neutral helium atom.
Over millions of years, this process leads to a significant accumulation of helium in uranium and thorium ores.
This is why helium is often found in deposits of uranium and thorium.

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Most popular questions from this chapter

A sample of cobalt- \(60\left(t_{1 / 2}=5.27 \mathrm{yr}\right),\) a powerful \(\gamma\) emitter used to treat cancer, was purchased by a hospital on March 1 ,2012. The sample must be replaced when its activity reaches \(70 . \%\) of the original value. On what date must it be replaced?

Seaborgium- 263 (Sg), the first isotope of element 106 synthesized, was produced, along with four neutrons, by bombarding californium- 249 with oxygen-18. The \({ }^{263} \mathrm{Sg}\) then underwent a series of decays starting with three \(\alpha\) emissions. Write balanced equations for the synthesis and the three \(\alpha\) emissions of \({ }^{263} \mathrm{Sg}\).

Write balanced nuclear equations for the following: (a) Alpha decay of \({ }^{234} \mathrm{U}\) (b) Electron capture by neptunium- 232 (c) Positron emission by \({ }_{7}^{12} \mathrm{~N}\)

Write balanced nuclear equations for the following: (a) Formation of \({ }^{186}\) Ir through electron capture (b) Formation of francium- 221 through \(\alpha\) decay (c) Formation of iodine- 129 through \(\beta^{-}\) decay

In the 1950 s, radioactive material was spread over the land from aboveground nuclear tests. A woman drinks some contaminated milk and ingests \(0.0500 \mathrm{~g}\) of \({ }^{90} \mathrm{Sr}\), which is taken up by bones and teeth and not eliminated. (a) How much \({ }^{90} \mathrm{Sr}\left(t_{1 / 2}=\right.\) \(29 \mathrm{yr}\) ) is present in her body after \(10 \mathrm{yr} ?\) (b) How long will it take for \(99.9 \%\) of the \({ }^{90} \mathrm{Sr}\) that she ingested to decay?
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