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