Explain the observed elemental electronic configurations in terms of the orbital energy, the spin-pairing energy and exchange interactions.
Use graphs of the radial wave functions to explain orbital energy differences arise from shielding/effective nuclear charge and penetration.Define the terms shielding, effective nuclear charge and penetration.Appreciate that, with more than one-electron (in the absence of a magnetic or electric field), the orbital energy depends on two quantum numbers.Appreciate that there is a difference between a one-electron orbital occupation diagram and multi-electron state.Use the Pauli Exclusion Principle to give the correct set of four quantum numbers for any electron in a multi-electron atom.Understand that as a consequence of electron spin, only two electrons can occupy an orbital (Pauli Exclusion Principle), and that this limits the possible quantum numbers an electron in a multi-electron atom can have.Understand that electron spin must be taken into account in the multi-electron atom and that it is the intrinsic angular momentum of the electron.Understand that the model for the multi-electron atom is a modified version of the hydrogen atom with corrections for electron-electron repulsion and exchange.Qualitatively draw the angular wavefunctions for s, p and d orbitals, differentiating between the different p and d orbitals and appreciating the directed nature of the electron density vis-à-vis bonding.
Be able to draw qualitative radial wavefunctions, probability profiles and radial distribution functions for s, p and d orbitals (use these to explain penetration effect and shielding in the multi-electron atom).Define the terms excited state and ground state, and recognize for the hydrogen atom.Tell which quantum number defines the energy of the electron in the one-electron model and use the expression for the energy in terms of this quantum number to calculate wavelength/frequency of light emitted/absorbed by a one-electron atom.Explain what a quantum number is, what it describes and give the possible values for the three quantum numbers that come from the interaction of the electron with the nucleus.Recognize that, in the quantum mechanical model, the electron’s angular momentum as it “orbits” the nucleus is quantized.Explain the term operator, and how it relates to quantum mechanics give an example of an operator.Explain the term wavefunction and how this relates to the electron density and the probability of finding an electron at a certain position in space.Convert between energy and wavelength/frequency using E = h n and ln = c.Describe the following and explain their historical significance: the ultraviolet catastrophe (and Planck’s solution), the photoelectric effect (use equation for), deBroglie’s equation (and be able to use), the Heisenberg uncertainty principle, Bohr’s model of the atom, the Rydberg equation (and be able to use).These outcome statements assume that a student has successfully met the outcomes for CHEM 130.Įlectronic Structure of the Hydrogen Atom An * indicates a topic covered in laboratory.
Note that the number of outcome statements is not necessarily related to the amount of lecture time spent on a topic. Outcome Statements for Chemistry 131: Chemical Principles IIĪt the end of Chemistry 131 a student will have the following skills and knowledge (grouped by topic).
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