CEM 141 MSU Exam 2 Questions and Answers Already Passed

CEM 141 MSU Exam 2 Questions and Answers Already Passed Lights acts as what? Particle and wave. Wavelength The distance (m) of waves from peak to peak. Short: x-ray (red), long: infrared (blue) Short - higher energy Long - lower energy Frequency (V) The number of wavefronts per second. Highest: x-ray Velocity of Light C = 3.00 X 10^8 = wavelength X frequency Amplitude The intensity, height of peaks of waves. Highest: blue light Energy of Wave (J) Increases as frequency increases and as wavelength decreases. Highest: x-ray Range of Wavelengths 10^-16 - 10^8 = 24. Only a third are visible Black Body Radiation 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 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? None. What increases the number of electrons to be emitted by the photoelectric effect? Intensity. A particle that transfers light energy with a definable energy, emits one electron energy of = h (6.626 x 10^-34 J) Photon. Energy of light equation? E = hV. h Planck's constant, the energy of a photon. What happens to the energy when there is a short wavelength? 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? Visible Spectrum. Atomic Emission Spectrum Spectrum that emits photons, energy diagram: electron goes down energy levels. Atomic Absorption Spectrum Spectrum that absorbs photons, energy diagram: electrons goes up in energy levels. Heisenberg Uncertainty Principle 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 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 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? n, l, ml, and