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Classical physics predicted that electrons orbit the nucleus like:
Particles in a cloud
Satellites randomly
Planets around the sun
Fixed points
According to classical physics, atoms should:
Be stable
Collapse due to spiraling electrons
Classical physics could explain discrete spectral lines.
True
False
In Bohr’s model, electrons:
Are stationary
Exist only in a cloud
Can have any energy
Move in fixed circular orbits
Electron transitions in Bohr’s model produce:
Discrete spectral lines
Only infrared light
No energy
Continuous radiation
Bohr’s model works perfectly for multi-electron atoms.
True
False
What happens when an electron jumps from a higher to a lower energy level?
A photon is absorbed
Nothing happens
A photon is emitted
Electron disappears
Which of the following is a limitation of Bohr’s model?
Ignores the nucleus
Does not have energy levels
Cannot explain multi-electron atoms
Cannot predict hydrogen spectrum
The electron cloud model shows electrons as:
Fixed orbits
Circling nuclei like planets
Probability regions
Stationary particles
The electron cloud model keeps quantized energy levels.
True
False
In the photoelectric effect, electrons are ejected when:
Metal is hot
Light frequency is above threshold
Any light shines on the metal
Light intensity is high enough
Increasing light intensity can eject electrons if the frequency is too low.
True
False
Einstein explained the photoelectric effect using:
Classical electricity
Bohr’s orbitals
Continuous wave theory
Photon theory (light as particles)
Which formula represents photon energy?
E = hf
V = IR
E = mc²
F = ma
Which parts of the atom interact to produce spectral lines?
Only the nucleus
Nucleus and electrons
Only photons
Neutrons and photons
Photon emission occurs when an electron absorbs energy and jumps to a higher level.
True
False
