Describe the structure of atoms and use nuclear notation () to deduce the number of protons, neutrons, and electrons in atoms and ions.
Define isotopes and perform calculations involving non-integer relative atomic masses and abundance of isotopes from given data. Specific examples of isotopes need not be learned.
Electron configurations
Understand emission spectra and qualitatively describe the relationship between color, frequency, wavelength, and energy across the electromagnetic spectrum. Distinguish between a continuous and line spectrum.
Describe the emission spectrum of the hydrogen atom, including the relationship between the lines and energy transitions to the first, second, and third energy series. Ignore the names of the different series.
Deduce the maximum number of electrons that can occupy each energy level, using the formula 2n2.
Recognize the shape and orientation of an s atomic orbital and the three p atomic orbitals.
Apply the Aufbau Principle, Hunds Rule, and the Pauli Exclusion Principle to deduce electron configurations for atoms and ions up toZ= 36. Recall full electron configurations, condensed electron configurations, and orbital diagrams of these elements. Recall the exceptions of Cr and Cu.