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Chapter 2: Problem 5

A sample of a radioactive element is found to be losing mass gradually. Explain what is happening to the sample.

Short Answer

Expert verified
The radioactive sample is losing mass because it is undergoing radioactive decay, a process whereby unstable atomic nuclei break down and release energy in the form of radiation. These expelled particles reduce the overall mass of the sample over time.

Step by step solution

01

Understanding Radioactivity and Decay

Radioactivity is a process where unstable atomic nuclei break down and release energy in the form of radiation. It typically happens when an atom has too many protons, too many neutrons, or an excess energy in the nucleus. The energy is then released, transforming the atom into a different type of atom or isotope, which could be a less/more massive form.
02

Connection with Loss of Mass

During radioactive decay, the atomic particles that make up the radioactive element are released in the form of radiation. This release means that the radioactive element gradually loses particles, which decreases its overall mass. So, the particle that is expelled by the radioactive decay contributes to a reduction in the mass of the original sample. Over time, this gradual expulsion of particles will decrease the mass of the radioactive sample.
03

Deeper Understanding through Example

For instance, in alpha decay, an alpha particle (which consists of 2 neutrons and 2 protons) is released. This particle is actually a helium nucleus. So, if a sample undergoes alpha decay, it loses some mass because the mass of the helium nucleus is subtracted from the mass of the original atom.

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Most popular questions from this chapter

Which of the following compounds are likely to be ionic? Which are likely to be molecular? \(\mathrm{SiCl}_{4}\), LiF, \(\mathrm{BaCl}_{2}, \mathrm{~B}_{2} \mathrm{H}_{6}, \mathrm{KCl}, \mathrm{C}_{2} \mathrm{H}_{4}\)

What are allotropes? Give an example. How are allotropes different from isotopes?

Draw two different structural formulas based on the molecular formula \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\). Is the fact that you can have more than one compound with the same molecular formula consistent with Dalton's atomic theory?

What is the difference between an atom and a molecule?

For each of these species, determine the number of protons and the number of neutrons in the nucleus: \({ }_{2}^{3} \mathrm{He},{ }_{2}^{4} \mathrm{He},{ }_{12}^{24} \mathrm{Mg},{ }_{12}^{25} \mathrm{Mg},{ }_{22}^{48} \mathrm{Ti},{ }_{35}^{79} \mathrm{Br},{ }_{78}^{195} \mathrm{Pt}\)
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