CEM 141 MSU Exam 2 Questions with Detailed
Verified Answers
Lights acts as what? Ans: Particle and wave.
Wavelength Ans: The distance (m) of waves from peak to peak. Short: x-ray (red),
long: infrared (blue)
Short - higher energy
Long - lower energy
Frequency (V) Ans: The number of wavefronts per second. Highest: x-ray
Velocity of Light Ans: C = 3.00 X 10^8
= wavelength X frequency
Amplitude Ans: The intensity, height of peaks of waves. Highest: blue light
Energy of Wave (J) Ans: Increases as frequency increases and as wavelength decreases.
Highest: x-ray
Range of Wavelengths Ans: 10^-16 - 10^8 = 24. Only a third are visible
Black Body Radiation Ans: When a mass is heated it emits a type of EM radiation, at
very high temps the mass becomes "white hot" because all wavelengths of visible light
become equally intense
Photoelectric Effect Ans: Metals emit electrons when electromagnetic radiation shines
on the surface, light is transfers energy to the electrons at the metal's surface where
it's transformed into KE that gives the electrons enough energy to leave the atom
, Depends on frequency not intensity
How many electrons are emitted if the light is below it's threshold frequency no
matter the intensity? Ans: None.
What increases the number of electrons to be emitted by the photoelectric effect?
Ans: Intensity.
A particle that transfers light energy with a definable energy, emits one electron
energy of = h (6.626 x 10^-34 J) Ans: Photon.
Energy of light equation? Ans: E = hV.
h Ans: Planck's constant, the energy of a photon.
What happens to the energy when there is a short wavelength? Ans: High energy.
Light from the sun (white light) can be separated by a prism to create this, only a small
part of the full EM spectrum? Ans: Visible Spectrum.
Atomic Emission Spectrum Ans: Spectrum that emits photons, energy diagram:
electron goes down energy levels.
Atomic Absorption Spectrum Ans: Spectrum that absorbs photons, energy diagram:
electrons goes up in energy levels.
Heisenberg Uncertainty Principle Ans: Principle states that we can't accurately
measure both the position and the energy of a small particle (electron)
Bohr's model did - why its wrong.
© Get it right 2025 Getaway - Stuvia US All rights reserved
Verified Answers
Lights acts as what? Ans: Particle and wave.
Wavelength Ans: The distance (m) of waves from peak to peak. Short: x-ray (red),
long: infrared (blue)
Short - higher energy
Long - lower energy
Frequency (V) Ans: The number of wavefronts per second. Highest: x-ray
Velocity of Light Ans: C = 3.00 X 10^8
= wavelength X frequency
Amplitude Ans: The intensity, height of peaks of waves. Highest: blue light
Energy of Wave (J) Ans: Increases as frequency increases and as wavelength decreases.
Highest: x-ray
Range of Wavelengths Ans: 10^-16 - 10^8 = 24. Only a third are visible
Black Body Radiation Ans: When a mass is heated it emits a type of EM radiation, at
very high temps the mass becomes "white hot" because all wavelengths of visible light
become equally intense
Photoelectric Effect Ans: Metals emit electrons when electromagnetic radiation shines
on the surface, light is transfers energy to the electrons at the metal's surface where
it's transformed into KE that gives the electrons enough energy to leave the atom
, Depends on frequency not intensity
How many electrons are emitted if the light is below it's threshold frequency no
matter the intensity? Ans: None.
What increases the number of electrons to be emitted by the photoelectric effect?
Ans: Intensity.
A particle that transfers light energy with a definable energy, emits one electron
energy of = h (6.626 x 10^-34 J) Ans: Photon.
Energy of light equation? Ans: E = hV.
h Ans: Planck's constant, the energy of a photon.
What happens to the energy when there is a short wavelength? Ans: High energy.
Light from the sun (white light) can be separated by a prism to create this, only a small
part of the full EM spectrum? Ans: Visible Spectrum.
Atomic Emission Spectrum Ans: Spectrum that emits photons, energy diagram:
electron goes down energy levels.
Atomic Absorption Spectrum Ans: Spectrum that absorbs photons, energy diagram:
electrons goes up in energy levels.
Heisenberg Uncertainty Principle Ans: Principle states that we can't accurately
measure both the position and the energy of a small particle (electron)
Bohr's model did - why its wrong.
© Get it right 2025 Getaway - Stuvia US All rights reserved
