E.1 - 3 - Electron Energy Levels and Photons

What does a negative gravitational potential energy value for a bowling ball signify?

• The bowling ball is moving upwards.

• The bowling ball is below the defined zero-height reference point.

• The bowling ball has no kinetic energy.

• The bowling ball is losing mass.

What does a negative energy value for an electron in an atom indicate?

• The electron is moving freely in space.

• The electron is about to be ejected from the atom.

• The electron is bound to the atom and requires energy to escape.

• The electron has gained energy and is in an excited state.

Which of the following best describes the ground state of an electron in an atom?

• The state where the electron has zero potential energy.

• The state where the electron is moving freely in space.

• The state with the largest magnitude of negative energy an electron can have.

• The state where the electron is excited and moving up energy levels.

What does it mean for the energy of an electron in an atom to be "quantized"?

• The electron's energy can continuously change to any value.

• The electron can only exist at specific, discrete energy levels.

• The electron's energy is always negative.

• The electron's energy is directly proportional to its speed.

What does it mean for an electron's energy to be "quantized" in an atom?

• It can have any energy value within a continuous range.

• It can only exist at specific, discrete energy levels.

• Its energy continuously changes as it orbits the nucleus.

• Its energy is always zero.

What happens when an electron in an atom loses energy and moves to a lower energy level?

• It absorbs a photon.

• It creates a new energy level.

• It emits a photon.

• It gains mass.

Why might a photon pass through an atom without being absorbed by an electron?

• The photon's energy is too high.

• The photon's energy is too low.

• The photon's energy does not exactly match the difference between two energy levels.

• The electron is already at the highest energy level.

How do the possible energies of photons that can be emitted by an atom relate to the possible energies of photons that can be absorbed by the same atom?

• Emitted photon energies are always higher than absorbed photon energies.

• Absorbed photon energies are always higher than emitted photon energies.

• The possible energies of emitted photons are exactly the same as the possible energies of absorbed photons.

• There is no direct relationship between emitted and absorbed photon energies.

What is the energy of a photon emitted when an electron transitions from energy level n=3 to n=1 in an atom with the given energy levels (n=4: -0.85 eV, n=3: -1.51 eV, n=2: -3.40 eV, n=1: -13.60 eV)?

• 1.55 eV

• 12.09 eV

• 12.75 eV

• 10.20 eV

Which transition will result in the emission of a photon with the smallest possible wavelength?

• From E4 to E3

• From E3 to E2

• From E2 to E1

• From E4 to E1