Reference no: EM132438743

1. What is a major difference between the quantum model of the atom and the Bohr model?

• Electrons orbit in elliptical orbits of varying distance from the nucleus.
• Electrons cannot transition between energy levels.
• Electrons eventually collapse into the nucleus.
• Electron orbitals are redefined as probable regions where the electron could be located.

2. What accounts for absorption spectra of elements?

• electrons moving in opposite directions around the nucleus
• electrons spinning around the nucleus within orbits
• electrons moving from low energy levels to high energy levels
• electrons moving from high energy levels to low energy levels

3. A cool gas cloud is situated between a bright star and the earth. What type of spectrum would you expect to observe through that gas cloud?

• absorption spectra
• noncontinuous spectra
• continuous spectra
• emission spectra

4. In a chemistry technique known as flame photometry, a sample gets burned in a high-temperature flame, and the amount of light at a specific wavelength is measured to identify the elements within the sample. Which of the following is this technique based upon?

• continuous spectra
• noncontinuous spectra
• emission spectra
• absorption spectra

5. Which of the following properties of light can only be explained by wave theory?

• refraction
• interference
• reflection
• velocity

6. Why do photoelectrons all have the same energy when illuminated with a given frequency of light?

• Each photon has the same energy, which gets transferred to a single photoelectron.
• The photons must be absorbed to cause the electron to jump energy levels and leave the atom.
• Multiple photons must strike an electron to eject it.
• The intensity, not the wavelength, determines the energy of the photoelectron.