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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

Radioactive cobalt-60 is used to study defects in vitamin \(\mathrm{B}_{12}\) absorption because cobalt is the metallic atom at the center of the vitamin \(\mathrm{B}_{12}\) molecule. The nuclear synthesis of this cobalt isotope involves a three-step process. The overall reaction is iron-58 reacting with two neutrons to produce cobalt-60 along with the emission of another particle. What particle is emitted in this nuclear synthesis? What is the binding energy in J per nucleon for the cobalt-60 nucleus (atomic masses: \(^{60} \mathrm{Co}=\) \(59.9338 \mathrm{u} ;^{-1} \mathrm{H}=1.00782\) u)? What is the de Broglie wavelength of the emitted particle if it has a velocity equal to \(0.90 c,\) where \(c\) is the speed of light?

A rock contains 0.688 \(\mathrm{mg}^{206} \mathrm{Pb}\) for every 1.000 \(\mathrm{mg}^{238} \mathrm{U}\) present. Assuming that no lead was originally present, that all the \(^{206}\mathrm{P}\) formed over the years has remained in the rock, and that the number of nuclides in intermediate stages of decay between \(^{238} \mathrm{U}\) and \(^{206 \mathrm{P}} \mathrm{b}\) is negligible, calculate the age of the rock. (For \(38 \mathrm{U}, t_{1 / 2}=4.5 \times 10^{9}\) years.)

The stable isotopes of boron are boron-10 and boron-11. Four radioactive isotopes with mass numbers 8, 9, 12, and 13 are also known. Predict possible modes of radioactive decay for the four radioactive isotopes of boron.

Phosphorus-32 2 is a commonly used radioactive nuclide in biochemical research, particularly in studies of nucleic acids. The half-life of phosphorus-32 is 14.3 days. What mass of phosphorus- 32 is left from an original sample of 175 \(\mathrm{mg}\) \(\mathrm{Na}_{3}^{32} \mathrm{PO}_{4}\) after 35.0 days? Assume the atomic mass of \(^{32} \mathrm{P}\) is 32.0 \(\mathrm{u} .\)

The earth receives \(1.8 \times 10^{14} \mathrm{kJ} / \mathrm{s}\) of solar energy. What mass of solar material is converted to energy over a \(24-\mathrm{h}\) period to provide the daily amount of solar energy to the earth? What mass of coal would have to be burned to provide the same amount of energy? (Coal releases 32 \(\mathrm{kJ}\) of energy per gram when burned.)
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