In Bohr's model, what prevents the electron from spiraling into the nucleus?
Understand the Problem
The question is asking about the Bohr model of the atom, specifically why electrons do not spiral into the nucleus, and provides multiple-choice answers to evaluate.
Answer
Quantization of energy levels prevents the electron from spiraling into the nucleus.
In Bohr's model, the electron is prevented from spiraling into the nucleus by being confined to discrete energy levels or stationary orbits. These levels are quantized, meaning electrons do not emit radiation while in these specific orbits, preventing energy loss and collapse into the nucleus.
Answer for screen readers
In Bohr's model, the electron is prevented from spiraling into the nucleus by being confined to discrete energy levels or stationary orbits. These levels are quantized, meaning electrons do not emit radiation while in these specific orbits, preventing energy loss and collapse into the nucleus.
More Information
Bohr introduced the concept of quantized orbits, which means electrons can only exist in a set of allowed energy levels around the nucleus. This idea was revolutionary because it contradicted classical physics, where accelerated charges like electrons should emit radiation continuously.
Tips
A common mistake is assuming electrons lose energy and emit radiation while orbiting. Bohr's model specifically states electrons in stationary orbits do not emit radiation, explaining their stability.
Sources
- The Bohr Model - Chemistry LibreTexts - chem.libretexts.org
- How did Bohr's model explain why the electron didn't spiral into the nucleus? - Quora - quora.com
AI-generated content may contain errors. Please verify critical information
