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Chapter 9: Problem 12

The masses of individual atoms can be determined with great precision, yet there is considerable uncertainty about the exact size of an atom. Explain why this is the case.

Short Answer

Expert verified
The mass of an atom can be measured precisely using a mass spectrometer which operates on deterministic principles, while the size of an atom bears uncertainty due to the probabilistic behavior of electrons as explained by the uncertainty principle. Hence while atomic mass can be accurately determined, atomic size measurement bears uncertainty.

Step by step solution

01

Explain Atomic Mass Measurement

Atomic mass is measured using an instrument called a mass spectrometer, which works based on the principle of the movement of ions in magnetic and electric fields. The mass of an atom can be calculated precisely since it is discerned from the trajectory of the atom's ions in the known fields.
02

Describe Atomic Size Measurement

The size of an atom is typically defined by the space in which its electrons move around the nucleus. However, since electrons in an atom do not have definite orbits but exist in a cloud-like area called an electron cloud, it is difficult to determine the precise boundary of an atom. This is why there is uncertainty in measuring the atomic size.
03

Compare Measurement Techniques

From the above explanations, it is clear that the determination of atomic mass and atomic size involves different techniques. While the measurement of atomic mass is deterministic because it is a property intrinsic to the atom, the measurement of atomic size is probabilistic due to the uncertainty principle governing the behavior of electrons in an atom. This difference explains why atomic mass can be accurately measured while the size of an atom bears considerable uncertainty.

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Most popular questions from this chapter

Arrange the following elements in order of decreasing metallic character: $\mathrm{Sc}, \mathrm{Fe}, \mathrm{Rb}, \mathrm{Br}, \mathrm{O}, \mathrm{Ca}, \mathrm{F}, \mathrm{Te}.$

Compare the elements \(\mathrm{Na}, \mathrm{Mg}, \mathrm{O},\) and \(\mathrm{P}.\) (a) Place the elements in order of increasing ionization energy. (b) Place the elements in order of increasing electron affinity.

The following species are isoelectronic with the noble gas krypton. Arrange them in order of increasing radius and comment on the principles involved in doing so: $\mathrm{Rb}^{+}, \mathrm{Y}^{3+}, \mathrm{Br}^{-}, \mathrm{Sr}^{2+}, \mathrm{Se}^{2-}.$

Assuming that the seventh period is 32 members long, what should be the atomic number of the noble gas following radon (Rn)? Of the alkali metal following francium (Fr)? What would you expect their approximate atomic masses to be?

Must all atoms with an odd atomic number be paramagnetic? Must all atoms with an even atomic number be diamagnetic? Explain.
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