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Chapter 16: Problem 50

How do we interpret the subscripts for the full symbols of an electron and a positron?

Short Answer

Expert verified
The subscripts for the full symbols of an electron (\(e^-\)) and a positron (\(e^+\)) represent their respective electric charges. The electron has a negative charge, while the positron has a positive charge. Both charges have a magnitude equal to the elementary charge, approximately \(\pm 1.6 \times 10^{-19}\) Coulombs.

Step by step solution

01

Identify the full symbols of an electron and a positron

In particle physics, an electron is represented by the symbol \(e^-\) and a positron is represented by the symbol \(e^+\). Here, we are asked to interpret the subscripts for these full symbols.
02

Understand what subscripts represent in the context of particle physics

In particle physics, subscripts usually denote the charge of the particle, its spin, or other quantum numbers. In this case, the subscripts for the electron and positron symbols: \(e^-\) and \(e^+\), represent their respective electric charges.
03

Interpret the subscript for the electron

For the electron symbol, \(e^-\), the subscript is the negative sign. This indicates that the electron has a negative charge. The magnitude of this charge is equal to the elementary charge, approximately \(-1.6 \times 10^{-19}\) Coulombs.
04

Interpret the subscript for the positron

For the positron symbol, \(e^+\), the subscript is the positive sign. This indicates that the positron has a positive charge. The magnitude of this charge is also equal to the elementary charge, approximately \(1.6 \times 10^{-19}\) Coulombs. In conclusion, the subscripts for the full symbols of an electron and a positron represent their respective electrical charges. The electron has a negative charge, and the positron has a positive charge, both having a magnitude equal to the elementary charge.

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Most popular questions from this chapter

What happens to an atom's nucleus when it undergoes beta emission?

The isotopes \({ }^{17} \mathrm{~F}^{20} \mathrm{~F}\), and \({ }^{21} \mathrm{~F}\) are all radioactive, decaying either by beta emission or by positron emission. Name the decay process for each isotope.

If you were looking to find or create superheavy atoms, approximately what range of atomic number would you expect for their nuclei?

What is the band of stability, and why do radioactive isotopes appear on it?

Which has the larger binding energy per mole of nucleons, \({ }_{2}^{4}\) He (molar mass \(4.00150 \mathrm{~g} / \mathrm{mol}\) ) or \({ }_{3}^{6} \mathrm{Li}\) (molar mass \(6.01348 \mathrm{~g} / \mathrm{mol}\) )? [Useful masses: proton, \(1.00730 \mathrm{~g} / \mathrm{mol}\); neutron, \(1.00870 \mathrm{~g} / \mathrm{mol} ;\) electron, \(0.00055 \mathrm{~g} / \mathrm{mol}]\)
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