Absorption and Emission Spectra Quiz

What happens when an electron in an atom drops to a lower energy level?

• It splits into two electrons.

• It emits a photon.

• It absorbs a photon.

• It remains at the same energy level.

What is the result when white light passes through an element and certain wavelengths are absorbed?

• Dark lines appear in the spectrum.

• The light becomes invisible.

• All wavelengths are absorbed.

• The light changes color.

How can we identify elements using their emission spectra?

• By observing the color of the element.

• By counting the number of electrons.

• By measuring the temperature of the element.

• By matching the spectra to known fingerprints.

Why do all hydrogen atoms have the same absorption and emission spectra?

• They have the same energy levels.

• They emit different photons.

• They have different energy levels.

• They absorb different wavelengths.

What evidence do absorption and emission spectra provide about electron energy levels?

• They show that energy levels are continuous.

• They prove that energy levels are random.

• They indicate that energy levels are quantized.

• They suggest that electrons have no energy levels.

What would happen if electron energy levels were not quantized?

• Spectra would be identical for all elements.

• Spectra would show random lines.

• Spectra would not exist.

• Spectra would be completely black.

What is a common misconception about absorption and emission spectra?

• They can measure any wavelength.

• They are only used for hydrogen.

• They only measure visible light.

• They are not related to electron energy levels.

What is the relationship between wavelength and frequency in the context of spectra?

• They are directly proportional.

• They are inversely proportional.

• They are unrelated.

• They are the same.

What does each line on an absorption or emission spectrum represent?

• A change in energy between two specific levels.

• A random energy change.

• A change in energy between multiple levels.

• A constant energy level.

How can absorption and emission spectra be represented besides using wavelength?

• Using temperature.

• Using mass.

• Using frequency.

• Using color.