CEM 141 MSU EXAM 2 QUESTIONS & ANSWERS
Lights acts as what? - Answer -Particle and wave.
Wavelength - Answer -The distance (m) of waves from peak to peak. Short: x-ray (red),
long: infrared (blue)
Short - higher energy
Long - lower energy
Frequency (V) - Answer -The number of wavefronts per second. Highest: x-ray
Velocity of Light - Answer -C = 3.00 X 10^8
= wavelength X frequency
Amplitude - Answer -The intensity, height of peaks of waves. Highest: blue light
Energy of Wave (J) - Answer -Increases as frequency increases and as wavelength
decreases. Highest: x-ray
Range of Wavelengths - Answer -10^-16 - 10^8 = 24. Only a third are visible
Black Body Radiation - Answer -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 - Answer -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? - Answer -None.
What increases the number of electrons to be emitted by the photoelectric effect? -
Answer -Intensity.
A particle that transfers light energy with a definable energy, emits one electron
energy of = h (6.626 x 10^-34 J) - Answer -Photon.
Energy of light equation? - Answer -E = hV.
h - Answer -Planck's constant, the energy of a photon.
What happens to the energy when there is a short wavelength? - Answer -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? - Answer -Visible Spectrum.
Atomic Emission Spectrum - Answer
-Spectrum that emits photons, energy diagram: electron goes down energy levels.
Atomic Absorption Spectrum - Answer
-Spectrum that absorbs photons, energy diagram: electrons goes up in energy levels.
Heisenberg Uncertainty Principle - Answer -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.
Schrodinger's Wave Equation - Answer -Treated electron as waves derived by
mathematical descriptions of energies.
Psi = wave function of an electron
Psi^2 = probability of finding an electron.
Atomic Orbitals - Answer -Regions of space where electrons with a particular quantized
energy have a high probability of being found, described by quantum numbers.
What are the quantum numbers? - Answer -n, l, ml, and ms.
Lights acts as what? - Answer -Particle and wave.
Wavelength - Answer -The distance (m) of waves from peak to peak. Short: x-ray (red),
long: infrared (blue)
Short - higher energy
Long - lower energy
Frequency (V) - Answer -The number of wavefronts per second. Highest: x-ray
Velocity of Light - Answer -C = 3.00 X 10^8
= wavelength X frequency
Amplitude - Answer -The intensity, height of peaks of waves. Highest: blue light
Energy of Wave (J) - Answer -Increases as frequency increases and as wavelength
decreases. Highest: x-ray
Range of Wavelengths - Answer -10^-16 - 10^8 = 24. Only a third are visible
Black Body Radiation - Answer -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 - Answer -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? - Answer -None.
What increases the number of electrons to be emitted by the photoelectric effect? -
Answer -Intensity.
A particle that transfers light energy with a definable energy, emits one electron
energy of = h (6.626 x 10^-34 J) - Answer -Photon.
Energy of light equation? - Answer -E = hV.
h - Answer -Planck's constant, the energy of a photon.
What happens to the energy when there is a short wavelength? - Answer -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? - Answer -Visible Spectrum.
Atomic Emission Spectrum - Answer
-Spectrum that emits photons, energy diagram: electron goes down energy levels.
Atomic Absorption Spectrum - Answer
-Spectrum that absorbs photons, energy diagram: electrons goes up in energy levels.
Heisenberg Uncertainty Principle - Answer -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.
Schrodinger's Wave Equation - Answer -Treated electron as waves derived by
mathematical descriptions of energies.
Psi = wave function of an electron
Psi^2 = probability of finding an electron.
Atomic Orbitals - Answer -Regions of space where electrons with a particular quantized
energy have a high probability of being found, described by quantum numbers.
What are the quantum numbers? - Answer -n, l, ml, and ms.
