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Chapter 19: Problem 7

What are transuranium elements and how are they synthesized?

Short Answer

Expert verified
Transuranium elements are synthetic chemical elements with atomic numbers greater than 92, which are not found naturally. They are synthesized through a series of neutron capture and beta decay processes. Neutron capture increases the mass of an atom without changing its atomic number, followed by beta decay which converts a neutron into a proton, creating a new element. This process can be repeated to create higher atomic number elements. To create heavier transuranium elements, particle accelerators are used to smash atomic nuclei together. However, synthesizing these elements is challenging due to their short half-lives and instability.

Step by step solution

01

Transuranium Elements Definition

Transuranium elements are chemical elements with atomic numbers greater than 92, uranium being the last naturally occurring element. These elements do not exist in nature and are synthetically produced.
02

Neutron Capture

The synthesis of transuranium elements starts with a process called neutron capture, in which an atom captures one or more neutrons. This addition of neutrons increases the mass of the atom but does not change the atomic number.
03

Beta Decay

The atom, after gaining neutrons through neutron capture, undergoes a process called beta decay. In beta decay, a neutron is converted into a proton by emitting an electron (also known as a beta particle). This process increases the atomic number of the atom by 1, effectively creating a new element.
04

Repetition of Process

To synthesize transuranium elements with higher atomic numbers, the neutron capture and beta decay processes are repeated multiple times. Each repetition increases the atomic number of the synthesized element and gets us closer to the desired transuranium element.
05

Particle Accelerator

To speed up the synthesis process and create heavier transuranium elements, scientists use particle accelerators. These machines accelerate atomic nuclei to extremely high speeds and smash them into target nuclei. The collision can result in the creation of new elements, including transuranium elements.
06

Challenges in Synthesis

The synthesis of transuranium elements can be challenging due to short half-lives and instability. Many of these elements decay very quickly, which makes their detection and characterization difficult. Researchers continue to investigate new ways to create and study these elements in hope of gaining a better understanding of their properties and potential applications.

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Most popular questions from this chapter

What is the rate of decay from 1.00 mol of radioactive nuclides having the following half-lives: \(12,000\) years? 12 hours? 12 seconds?

The only stable isotope of fluorine is fluorine-19. Predict possible modes of decay for fluorine-21, fluorine-18, and fluorine-17.

To determine the \(K_{\mathrm{sp}}\) value of \(\mathrm{Hg}_{2} \mathrm{I}_{2},\) a chemist obtained a solid sample of \(\mathrm{Hg}_{2} \mathrm{I}_{2}\) in which some of the iodine is present as radioactive 131 \(\mathrm{I}\) . The count rate of the \(\mathrm{Hg}_{2} \mathrm{I}_{2}\) sample is \(5.0 \times 10^{11}\) counts per minute per mole of I. An excess amount of $\mathrm{Hg}_{2} \mathrm{I}_{2}(s)$ is placed into some water, and the solid is allowed to come to equilibrium with its respective ions. A \(150.0-\mathrm{mL}\) sample of the saturated solution is withdrawn and the radioactivity measured at 33 counts per minute. From this information, calculate the \(K_{\mathrm{sp}}\) value for \(\mathrm{Hg}_{2} \mathrm{I}_{2}\) $$ \mathrm{Hg}_{2} \mathrm{I}_{2}(s) \rightleftharpoons \mathrm{Hg}_{2}^{2+}(a q)+2 \mathrm{I}^{-}(a q) \qquad K_{\mathrm{sp}}=\left[\mathrm{Hg}_{2}^{2+}\right]\left[\mathrm{I}^{-}\right]^{2} $$

The most significant source of natural radiation is radon-222. $^{222} \mathrm{Rn},\( a decay product of \)^{238} \mathrm{U},$ is continuously generated in the earth's crust, allowing gaseous Rn to seep into the basements of buildings. Because \(^{222} \mathrm{Rn}\) is an \(\alpha\) -particle producer with a relatively short half-life of 3.82 days, it can cause biological damage when inhaled. a. How many \(\alpha\) particles and \(\beta\) particles are produced when $^{238} \mathrm{U}\( decays to \)^{222} \mathrm{Rn}$ ? What nuclei are produced when \(^{222} \mathrm{Rn}\) decays? b. Radon is a noble gas so one would expect it to pass through the body quickly. Why is there a concern over inhaling \(^{222} \mathrm{Rn}\) ? c. Another problem associated with \(^{222} \mathrm{Rn}\) is that the decay of \(^{222} \mathrm{Rn}\) produces a more potent \(\alpha\) -particle producer $\left(t_{1 / 2}=3.11 \mathrm{min} \text { ) that is a solid. What is the identity of the }\right.$ solid? Give the balanced equation of this species decaying by \(\alpha\) -particle production. Why is the solid a more potent \(\alpha\) -particle producer? d. The U.S. Environmental Protection Agency (EPA) recommends that 222 Rn levels not exceed 4 \(\mathrm{pCi}\) per liter of air $\left(1 \mathrm{Ci}=1 \text { curie }=3.7 \times 10^{10} \text { decay events per second; }\right.$ \(1 \mathrm{pCi}=1 \times 10^{-12} \mathrm{Ci}\) . Convert 4.0 \(\mathrm{pCi}\) per liter of air into concentrations units of \(^{222} \mathrm{Rn}\) atoms per liter of air and moles of \(^{2222} \mathrm{Rn}\) per liter of air.

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