Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

A particle is trapped in a spherical infinite well. The potential energy is 0 for \(ra\) Which. if any, quantization conditions would you expect it to share with hydrogen, and why?

Short Answer

Expert verified
The main similarities are, both spherical infinite well and hydrogen atom have quantized energies due to boundary conditions and wave-like properties of particles. However, the reason for quantization differs. For hydrogen, it's a result of 1/r potential and spherical harmonics in the Schrödinger's equation solution, while for an infinite spherical well, it's due to the particle's confinement within \(r<a\).

Step by step solution

01

Understand the Spherical Infinite Well

In a spherical infinite well, the potential energy is defined as zero for \(ra\). This is a boundary condition where the particle is confined to the space with \(r<a\). Essentially, the particle is free to move within the sphere, but cannot exist outside the sphere.
02

Review the Properties of Hydrogen Atom

Think about the features that characterize a hydrogen atom. A hydrogen atom consists of a single proton and a single electron. The potential energy is negative due to the electrostatic attraction between the proton and the electron and it goes to zero as the electron moves far from the nucleus. As a result, the energy levels of a hydrogen atom are quantized; there are certain distinct energy levels an electron can occupy.
03

Compare with the Infinite Well

Relate this to the spherical infinite well. The main similarity is that both scenarios have quantized energy levels. In both the infinite well and in the hydrogen atom, the particle (or electron, in the case of hydrogen) can only exist at certain energy levels, a consequence of the wave-like properties of particles and the required boundary conditions.
04

Deduce the Differences

Although there are similarities, there are differences as well. For the hydrogen atom, the quantization arises from the 1/r potential and resulting spherical harmonics in the solution of Schrödinger's equation. While for the infinite spherical well, the quantization comes from the boundary conditions (being confined within \(r<a\)).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Spherical Infinite Well
Imagine a particle that is absolutely confined within a spherical region of space. This is the concept of a spherical infinite well, an idealized model often used in quantum mechanics to understand how particles behave when they're trapped. In practice, this well is a region where the potential energy is zero if the particle is within a radius, denoted as \(r < a\), and infinite if the particle attempts to pass beyond that boundary, \(r > a\).

Due to quantum effects, a particle in such a well cannot possess just any energy; its energy must be quantized. This means it can only occupy certain allowed energy levels. This phenomenon is similar to what you might observe in the electron configurations in an atom. A productive way to imagine this well is to think of it as a 'quantum prison' where the allowed energy levels correspond to the different ways the particle can resonate within the 'prison walls' without escaping.
Hydrogen Atom Properties
The hydrogen atom, the simplest atom in the universe, exhibits fascinating quantum properties. It consists of a solitary proton and a single electron, attracted to each other by electrostatic forces. These forces result in a potential energy that becomes less negative as the separation between the particles increases, eventually reaching zero as the distance becomes very large.

Quantization of energy levels is a signature trait of the hydrogen atom, showing that the electron can only inhabit discrete energy levels or 'orbits'. This concept was historically introduced by Niels Bohr and later more accurately described by quantum mechanics. Astonishingly, if you were to measure the energy of an electron in a hydrogen atom, you would find that it can only have specific, discrete values, much like rungs on a ladder. Understanding these discrete energy levels is essential in grasping the fundamental behavior of atoms and the principles of chemistry.
Schrödinger's Equation
At the heart of quantum mechanics lies Schrödinger's equation, a mathematical formula that describes how the quantum state of a physical system changes over time. It is the key equation of quantum mechanics, akin to Newton's laws in classical mechanics. For systems like the hydrogen atom or a particle trapped in a spherical well, it is Schrödinger's wave equation that determines the allowed energy levels and the behavior of the particles.

The solutions to Schrödinger's equation are wave functions that can give us the probability of finding a particle in a particular location. These wave functions must satisfy certain boundary conditions, such as vanishing at the walls of an infinite well, or matching the behaviour around a proton in the case of a hydrogen atom. The equation intricately balances the particle's kinetic and potential energies to reveal the quantum nature of the system. As an essential tool, mastering Schrödinger's equation is like possessing a magical key that unlocks the secrets of microscopic realms.
Wave-Like Properties of Particles
One of the most startling revelations of quantum mechanics is that particles exhibit wave-like properties. This tenet is fundamentally at odds with our everyday experiences but is pivotal in understanding the behavior of particles on microscopic scales. According to de Broglie, every particle has a wavelength associated with its momentum, leading to phenomena like diffraction and interference, which were previously thought to be exclusive to waves.

This wave-particle duality allows for the concept of quantization in systems like the spherical infinite well and hydrogen atom. Because particles have wave-like properties, they must 'fit' into the spaces they occupy in such a way that the wave function remains continuous and finite. The classic analogy is that of standing waves on a stringed musical instrument - only certain wavelengths 'fit' on the string, much like only certain energy levels are permitted for a particle in a quantized system. These concepts are not only fundamental to understanding the microscopic world but also have practical implications in the development of technologies such as lasers, semiconductors, and quantum computers.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

An electron is in an \(n=4\) state of the hydrogen atom. (a) What is its energy? (h) What properties besides energy are quantized, and what values might be found if these properties were to he measured?

How many different \(3 d\) states are there? What physical property (as supposed to quantum number) distinguishes them, and what different values may this property assume?

Classically, an orbiting charged particle radiates elecIromagnetic energy, and for an electron in atomic dimensions, if would lead to collupse in considerably less than the wink of an eye. (a) By equating the centripetal and Coulomb forces, show that for a classical charge \(-e\) of mass \(m\) held in circular orbit by its attraction to a fixed charge \(+e\), the following relationship holds: \(\omega=e r^{-1 / 2} / \sqrt{4 \pi \varepsilon_{0} m}\). (b) Electromagnetism tells us that a charge whose acceleration is a radiates power \(P=e^{2} a^{2} / 6 e_{f} f^{\prime}\). Shuw that thiv can also be expressed in terms of the orbit radius, as \(P=e^{6} /\left(96 m^{2} \varepsilon_{0}^{3} m c^{3} r^{\lambda}\right)\). Then calculate the energy lowt per orbit in terms of \(r\) by multiplying this power by the period \(T=2 \pi / \omega\) and using the formula from part (a) to eliminate \(\omega(\mathrm{c})\) in such a classical orbit. the total mechanical energy is half the potential energy (see Section 4.4), or \(E_{\text {orbu }}=-e^{2 / 8} \pi \varepsilon_{0} r .\) Calculate the change in energy per change in \(r, d E_{\text {obi }} l d r\). From this and the energy lost per orbit from part (b). determine the change in \(r\) per orbit and evaluate it for a typical orbit radius of \(10^{-10} \mathrm{~m}\). Would the electron's radius change much in a single orbit? (d) Argue that dividing \(d E_{\text {arbiu }} / d r\) by \(P\) and multiplying by dr gives the time required for \(r\) to change by \(d r\). Then. sum these times for all radii from \(r_{\text {initial }}\) to a final radius of \(0 .\) Evaluate your result for \(r_{\text {hiniul }}=10^{-10} \mathrm{~m}\). (One limitation of this extimate is that the electron would eventually be moving relativistically.)

For an elecTron in the \(\left(n, C, m_{e}\right)=(2,0,0)\) state in a hydrogen atom. (a) write the solution of the time-independent Schrödinger equation, and (b) verify explicitly that it is a solution with the expected angular momentum and eneRgy.

Is the potential energy of an electron in a hydrogen atom well defined? Is the kinetic energy well defined? Justify your answers. (You need not actually calculate uncertainties.)

See all solutions

Recommended explanations on Physics Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free