Drawbacks of Rutherford's Theory

The video discusses the application of Newton's laws in classical mechanics, which works well for large systems like the solar system but fails for small systems like atoms. It highlights the limitations of Rutherford's atomic model, which couldn't explain atomic stability or spectra. The video explains that electrons lose energy in a discontinuous manner, leading to line spectra, contrary to continuous spectra predicted by classical theories.

Why can't Newton's laws of motion be used to calculate the orbit of an electron in an atom?

• Because electrons are too large

• Because electrons do not move

• Because electrons are not charged

• Because electrons are too small

What happens to an electron in Rutherford's model when it loses energy?

• It gains energy and moves faster

• It moves away from the nucleus

• It remains in the same orbit

• It takes a spiral path towards the nucleus

According to Maxwell's electromagnetic theory, what happens to a charged particle when it is accelerated?

• It gains mass

• It becomes neutral

• It loses energy as electromagnetic radiation

• It stops moving

What type of spectra do atoms actually emit?

• Continuous spectra

• Line spectra

• Random spectra

• No spectra

What does the emission of line spectra by atoms suggest about energy loss?

• Energy loss is not continuous

• Energy loss is non-existent

• Energy loss is random

• Energy loss is continuous