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Chapter 7: Problem 71

What is the physical significance of the value of \(\psi^{2}\) at a particular point in an atomic orbital?

Short Answer

Expert verified
The physical significance of the value of \(\psi^2\) at a particular point in an atomic orbital is that it represents the probability density of finding an electron at that location. A higher value of \(\psi^2\) indicates a greater likelihood of the electron being present in that specific region, while a lower value denotes a lower probability. This helps in visualizing electron distribution in atomic orbitals and understanding their shapes and properties.

Step by step solution

01

Understanding the wave function

The wave function, denoted by \(\psi\), is a mathematical representation of the electron's quantum state within an atom. It provides information about the probability of the electron's position, momentum, and other properties.
02

Squaring the wave function

By squaring the wave function (\(\psi^2\)), we obtain the probability density. Probability density is used to determine the likelihood of finding a particle in a given region of space. In other words, the higher the value of \(\psi^2\) at a point, the more probable it is to find an electron in that region.
03

Probability density in atomic orbitals

In atomic orbitals, \(\psi^2\) represents the probability density of finding an electron in a specific location around the nucleus. It is essential to emphasize that \(\psi^2\) is not an exact position but rather an indication of the electron's probability distribution across space.
04

Physical significance of \(\psi^2\) in an atomic orbital

The physical significance of the value of \(\psi^2\) in an atomic orbital relates to the likelihood of finding an electron at that particular point. A higher value of \(\psi^2\) signifies a higher probability that the electron will be found in that location, while a lower value indicates a lower probability. This information allows us to visualize the electron distribution in atomic orbitals and understand their shapes and properties.

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Most popular questions from this chapter

Using the Heisenberg uncertainty principle, calculate \(\Delta x\) for each of the following. a. an electron with \(\Delta v=0.100 \mathrm{~m} / \mathrm{s}\) b. a baseball (mass \(=145 \mathrm{~g}\) ) with \(\Delta v=0.100 \mathrm{~m} / \mathrm{s}\) c. How does the answer in part a compare with the size of a hydrogen atom? d. How does the answer in part b correspond to the size of a baseball?

Order the atoms in each of the following sets from the least exothermic electron affinity to the most. a. \(\mathrm{N}, \mathrm{O}, \mathrm{F}\) b. \(\mathrm{Al}, \mathrm{Si}, \mathrm{P}\)

Complete and balance the equations for the following reactions. a. \(\mathrm{Cs}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow\) b. \(\mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \rightarrow\)

Calculate the velocities of electrons with de Broglie wavelengths of \(1.0 \times 10^{2} \mathrm{~nm}\) and \(1.0 \mathrm{~nm}\), respectively.

Draw atomic orbital diagrams representing the ground-state electron configuration for each of the following elements. a. \(\mathrm{Na}\) b. \(\mathrm{Co}\) c. \(\mathrm{Kr}\) How many unpaired electrons are present in each element?
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