Emission Spectra and the Bohr Model

The video tutorial covers atomic spectroscopy, focusing on how atoms and molecules emit light energy, resulting in unique emission spectra. It explains the difference between continuous and discrete spectra, using examples like flame tests and lamps. The tutorial delves into quantum mechanics, discussing the limitations of classical physics in explaining atomic behavior. It introduces the Bohr model, highlighting quantized energy levels and electron transitions, and explains the concept of quantum leaps. The video concludes with the historical significance of these discoveries in developing atomic models.

What is the primary reason that emission spectra are not continuous like sunlight?

• Atoms reflect light at specific frequencies.

• Atoms absorb all light frequencies.

• Atoms emit light at all frequencies.

• Atoms emit light at specific frequencies.

Which of the following is NOT a method to observe emission spectra?

• Using a helium lamp.

• Performing a flame test.

• Using a mercury lamp.

• Using a prism with sunlight.

Which of the following elements emits a purple light in a flame test?

• Sodium

• Potassium

• Lithium

• Barium

What is the role of a prism in observing emission spectra?

• To absorb light.

• To reflect light.

• To separate light by wavelength.

• To combine light frequencies.

What does the Rydberg formula help to describe?

• The continuous spectrum of sunlight.

• The discrete lines in atomic spectra.

• The absorption of light by metals.

• The reflection of light by surfaces.

Why was the discovery of emission spectra significant in the development of quantum mechanics?

• It showed that all elements emit the same light.

• It disproved the existence of atoms.

• It led to the idea of quantized energy levels.

• It confirmed classical physics.

In the Bohr model, what happens when an electron jumps from a higher energy orbit to a lower one?

• It absorbs a photon.

• It emits a photon.

• It remains in the same orbit.

• It loses its charge.

What does the Bohr model compare the atom to?

• A solar system.

• A plum pudding.

• A continuous spectrum.

• A solid rainbow.

What is the significance of quantized energy levels in the Bohr model?

• Electrons can be between orbits.

• Electrons have fixed energy levels.

• Electrons emit continuous spectra.

• Electrons are stationary.

What is a key limitation of the Bohr model?

• It describes electron clouds.

• It predicts continuous spectra.

• It explains all atomic spectra.

• It only works for hydrogen.