Oklahoma State General Chemistry F26
Dr Latifi · 9 lectures with notes
Every lecture with its full transcript and chapters, and one search across all 9 lectures.
Gen Chem_Ch 6_9th_Photoelectric Effect (2)
At fixed 400 nm wavelength, doubling light intensity increases emitted-electron count, not each electron’s maximum kinetic energy.
Gen Chem_Ch 6_15th_Radial Distribution (3)
Orbital penetration explains why 3s is lowest among the n=3 orbitals and why 4s fills before 3d.
Gen Chem_Ch 6_19th_Exceptions in Electron Configuration
Chromium and copper shift an s electron into the d subshell because half-filled or filled d subshells are more stable.
Gen Chem_Ch 6_17th_Electron Configuration (2)
Use orbital filling order, highest n, and noble-gas shorthand to write and interpret electron configurations.
Gen Chem_Ch 6_16th_Electron Configuration
Electron configurations follow energy, Pauli exclusion, and Hund's rule, with shell capacities of 2, 8, and 18 electrons.
Gen Chem_Ch 6_18th_Electron Configuration (3)
Use electron configurations to identify valence electrons, predict magnetic behavior, and write ion configurations, including transition-metal cations.
Gen Chem_Ch 6_14th_Radial Distribution (2)
A 4p orbital has one angular node, two radial nodes, and a farther-out most probable radius than 2p or 3p.
Gen Chem_Ch 6_13th_Radial Distribution Graph
A 3s orbital has two radial nodes, dividing its radial distribution into three probability regions.
Gen Chem_Ch 6_12th_d Orbitals
An l value of 2 defines five d orbitals that hold 10 electrons and have two angular nodes.