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Chapter 21: Problem 39

Explain how an atomic bomb works.

Short Answer

Expert verified
An atomic bomb operates on the principle of nuclear fission. Two subcritical masses of a fissile material are brought to a supercritical state by conventional explosives. A neutron source then triggers a nuclear reaction where the key element (uranium-235 or plutonium-239) breaks into two smaller nuclei and releases energy. The fission process causes a chain reaction and the energy created results in an explosion.

Step by step solution

01

Understanding the Structure

An atomic bomb generally comprises two parts of a sub-critical mass of fissile material (usually uranium-235 or plutonium-239) that, combined, will start a nuclear chain reaction. These pieces are placed in a casing and monitored by a neutron source.
02

Distribution and Initiation

To initiate the explosive chain reaction, conventional explosives placed around the bomb first detonate to bring the sub-critical masses to a supercritical state. The neutron source then emits neutrons to trigger the nuclear reaction.
03

Nuclear Fission and Chain Reaction

The key element in an atomic bomb, Uranium-235 or Plutonium-239, undergoes fission when it absorbs a neutron, breaking into two smaller nuclei and releasing several millions of electron volts of energy. This fission process also releases more neutrons which can then cause further fission in a chain reaction leading to an explosion.
04

The Explosion and Resulting Aftermath

When the chain reaction is allowed to proceed at an uncontrolled rate, it releases a massive amount of energy all at once, leading to an explosion. The aftermath of such an explosion includes not just the blast, but radioactive fallout that can cause contamination.

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Most popular questions from this chapter

Given that \(\mathrm{H}(g)+\mathrm{H}(g) \longrightarrow \mathrm{H}_{2}(g) \quad \Delta H^{\circ}=-436.4 \mathrm{~kJ}\) calculate the change in mass (in kg) per mole of \(\mathrm{H}_{2}\) formed.

For each pair of isotopes listed, predict which one is less stable: (a) \({ }_{3}^{6} \mathrm{Li}\) or \({ }_{3}^{9} \mathrm{Li},\) (b) \({ }_{11}^{23} \mathrm{Na}\) or \({ }_{11}^{25} \mathrm{Na},\) (c) \({ }_{20}^{48} \mathrm{Ca}\) or \({ }_{21}^{48} \mathrm{Sc}\).

Consider this redox reaction: $$ \begin{array}{r} \mathrm{IO}_{4}^{-}(a q)+2 \mathrm{I}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \\ \mathrm{I}_{2}(s)+\mathrm{IO}_{3}^{-}(a q)+2 \mathrm{OH}^{-}(a q) \end{array} $$ When \(\mathrm{KIO}_{4}\) is added to a solution containing iodide ions labeled with radioactive iodine- \(128,\) all the radioactivity appears in \(\mathrm{I}_{2}\) and none in the \(\mathrm{IO}_{3}^{-}\) ion. What can you deduce about the mechanism for the redox process?

Which of the following poses a greater health hazard: a radioactive isotope with a short half-life or a radioactive isotope with a long half-life? Explain. [Assume same type of radiation \((\alpha\) or \(\beta)\) and comparable energetics per particle emitted.

Complete these nuclear equations and identify \(\mathrm{X}\) in each case: (a) \({ }_{12}^{26} \mathrm{Mg}+{ }_{1}^{1} \mathrm{p} \longrightarrow{ }_{2}^{4} \alpha+\mathrm{X}\) (b) \({ }_{27}^{59} \mathrm{Co}+{ }_{1}^{2} \mathrm{H} \longrightarrow{ }_{27}^{60} \mathrm{Co}+\mathrm{X}\) (c) \({ }_{92}^{235} \mathrm{U}+{ }_{0}^{1} \mathrm{n} \longrightarrow{ }_{36}^{94} \mathrm{Kr}+{ }_{56}^{139} \mathrm{Ba}+3 \mathrm{X}\) (d) \({ }_{24}^{53} \mathrm{Cr}+{ }_{2}^{4} \alpha \longrightarrow{ }_{0}^{1} \mathrm{n}+\mathrm{X}\) (e) \({ }_{8}^{20} \mathrm{O} \longrightarrow{ }_{9}^{20} \mathrm{~F}+\mathrm{X}\)
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