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

The electrons of Rutherford's model of the atom are expected to lose energy because they (1) are attracted by the nucleus (2) strike each other (3) are accelerated (4) are in motion

Short Answer

Expert verified
The electrons lose energy because they are accelerated.

Step by step solution

01

- Understand the Problem

The problem asks why electrons in Rutherford's model of the atom are expected to lose energy. Consider the behavior of electrons and the principles of physics that apply to them.
02

- Analyze Each Option

Evaluate each given option: electrons are attracted by the nucleus, strike each other, are accelerated, or are in motion. Determine which of these could cause energy loss.
03

- Examine Electromagnetic Radiation

According to classical physics, when charged particles like electrons are accelerated, they emit electromagnetic radiation, losing energy in the process.
04

- Identify the Correct Cause

As electrons revolve around the nucleus, they are constantly changing direction, which means they are accelerating. The continuous acceleration causes them to emit radiation and lose energy.
05

- Conclude

Because the continuous acceleration of electrons in Rutherford's model leads them to emit radiation, the correct answer is (3) are accelerated.

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.

electron behavior
In Rutherford's model of the atom, electrons move around the nucleus in circular orbits. This behavior is similar to planets orbiting the sun. However, electrons are not just simple particles; they have unique properties:
  • They have a negative charge.
  • Their motion is influenced by the positive charge of the nucleus.
  • In classical physics, accelerated electrons (those changing speed or direction) emit energy.
This means that as electrons continually move in their orbits, they are always accelerating toward the nucleus. The behavior of electrons in Rutherford's model presents a significant issue: they should be losing energy and spiraling into the nucleus, but this does not actually happen. This conflict between expected behavior and actual observations helped pave the way for further developments in atomic theory.
energy loss
Energy loss in Rutherford's model is tied directly to the motion of electrons. When charged particles like electrons are accelerated, they emit energy in the form of electromagnetic radiation. This emission of energy results in energy loss for the electrons. In a stable orbit, you would expect electrons to constantly lose energy, slow down, and eventually spiral into the nucleus.
  • This continuous energy loss is due to the fact that they are being constantly pulled towards the nucleus while moving in an orbit.
  • The expected result would be an atom imploding, which contradicts what we observe in reality.
This concept of energy loss due to acceleration presented a major flaw in Rutherford's model and highlighted the need for more refined atomic theories.
electromagnetic radiation
Electromagnetic radiation is a form of energy emitted by accelerating charged particles. When electrons in Rutherford's model are moving around the nucleus, they are accelerating because their direction changes continuously. According to classical physics, this acceleration makes them emit electromagnetic radiation
  • This radiation is a form of energy loss.
  • It explains why accelerating electrons can't maintain constant energy levels in classical physics.
This phenomenon not only affects atomic models but is also seen in other systems involving accelerating charges. Understanding electromagnetic radiation is crucial for explaining why Rutherford's model couldn't fully describe electron behavior.
classical physics
Classical physics dealt with particles and waves using principles developed before quantum mechanics. According to classical physics, accelerating charges (like electrons in orbit) should emit electromagnetic radiation and lose energy. This was one of the main reasons Rutherford's model had limitations.
  • Classical physics couldn't explain the stability of atoms:
  • If electrons lost energy as predicted, they would spiral into the nucleus.
  • This would make atoms collapse, contradicting everyday experiences and observations.
To solve these contradictions, new theories were needed, such as quantum mechanics, which better described the behavior of electrons on atomic scales. Classical physics’s inability to explain these observations helped push scientific thinking towards more advanced models of the atom.

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

Which best describes the emission spectra of atomic hydrogen? (1) A series of only four lines. (2) A discrete series of lines of equal intensity and equally spaced with respect to wavelength. (3) Several discrete series of lines with both intensity and spacing between decreasing as the wave number increases within each series. (4) A continuous emission of radiation of all frequencies.

Which one of the following statements about atomic number is false? (1) It is equal to the number of protons present in the nucleus. (2) It is a more fundamental property of the atom than the atomic weight. (3) No two elements can have the same atomic number. (4) The atomic number of an element decides its stability.

Which of the following statement is false? (1) The orbit with more number of nodal planes will be of more energy. (2) The orbital with two angular nodes (nodal planes) is f-orbital. (3) The zero probability of finding the electron in \(\mathrm{p}_{x}-\) orbital is in \(y-z\) plane. (4) The orbital which do not has angular nodes is s-orbital.

The wave number of first line in the Balmer series of hydrogen is \(15200 \mathrm{~cm}^{\text {? }}\). The wave number of the first line in the Balmer series of \(\mathrm{Be}^{3+}\) is (1) \(2.43 \times 10^{5} \mathrm{~cm}^{-1}\) (2) \(3.43 \times 10^{5} \mathrm{~cm}^{-1}\) (3) \(4.43 \times 10^{5} \mathrm{~cm}^{-1}\) (4) \(5.43 \times 10^{5} \mathrm{~cm}^{-1}\)

The ratio of the radius of the first Bohr orbit for the electron orbiting around the hydrogen nucleus that of the electron orbiting around the deuterium nucleus is approximately (1) \(1: 1\) (2) \(1: 2\) (3) \(2: 1\) (4) \(1: 4\)

See all solutions

Recommended explanations on Chemistry 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