Ch 06
Explain the basic behavior of waves, including travelling waves and standing waves[C]
Describe the wave nature of light [C]
Use appropriate equations to calculate related light-wave properties such as frequency, wavelength, and energy [R]
Distinguish between line and continuous emission spectra [A]
Describe the particle nature of light [C]
RESOURCES: Course video, "Electromagnetic Radiation and Quantization"
Describe the Bohr model of the hydrogen atom [C]
Use the Rydberg equation to calculate energies of light emitted or absorbed by hydrogen atoms [R]
RESOURCES: Course video, "Atomic Line Spectra and Bohr Atom"
Extend the concept of wave–particle duality that was observed in electromagnetic radiation to matter as well [C]
Understand the general idea of the quantum mechanical description of electrons in an atom, and that it uses the notion of three-dimensional wave functions, or orbitals, that define the distribution of probability to find an electron in a particular part of space [C]
List and describe traits of the four quantum numbers that form the basis for completely specifying the state of an electron in an atom [A]
Derive the predicted ground-state electron configurations of atoms [A]
Identify and explain exceptions to predicted electron configurations for atoms and ions [A]
Relate electron configurations to element classifications in the periodic table [A]
RESOURCES: Course video,"Electron Configurations"
Describe and explain the observed trends in atomic size, ionization energy, and electron affinity of the elements [A]
RESOURCES: Course video,"Periodic Trends"