Learning Outcomes for UNIT 2

Each student should have a good grasp of the following learning outcomes for unit 2. Unit 2 is assessed on Exam 2 which is on Tuesday 10/4/11 from 7-9 PM. Read the bulleted points and self assess yourself on how well you know the topic.

Students will be able to...

• Students will understand and perform quantitative calculations based on the relationship between wavelength, energy, and the speed of light.
• Students will define wavelength, frequency, and energy of a photon.
• Students will understand, identify, and rank the different types of light radiation.
• Describe the photoelectric effect and relate the energy of a photon, the work function, and the kinetic energy of the electrons. Students should also be able to describe the effect of the intensity and the energy of the light.
• Students should understand atomic absorption and emission spectra contain discrete, very sharp lines from transition of electrons between discrete energy levels.
• The student will understand QM is a model and that solutions to the Schödinger equation yield wavefunctions and energies.
• Understand that the wavefunction can be used to find a radial distribution function that describes the probability of an electron as a function of distance away from the nucleus.
• The student will list, define, and describe the three quantum numbers for the H-atom wavefunctions and know what possible combinations of quantum numbers are allowed.
• Define the atomic orbital names based on quantum numbers.
• Apply the Rydberg formula to predict the energy of transitions between two n levels in the hydrogen atom.
• Describe the difference between one electron systems and multi-electron systems
• Apply the Aufbau principle to determine the configuration for any atom or ion
• Predict the electronic configuration based on position of the element on the periodic table.
• Recognize that there are exceptions to the Aufbau principles and where they are likely to occur on the periodic table and why.
• Use Hund’s rule to determine electron configuration using an orbital diagram (electrons in individual orbitals with spins)
• Student will use the shell model of multielectron atoms to describe the concept of core vs. valence electrons
• Define ionization energy.
• Describe the concept of electronic shielding and effective nuclear charge (Zeff) and their relationship to trends in ionization energy, atomic and ionic radii
• Student will be able to draw the Lewis structures for molecular compounds and ions.
• Draw the resonance structures for a molecule or polyatomic ion.
• Apply formal charges to structures and use them to predict the most likely structure
• Use Lewis structures to predict and explain relative bond strength and lengths in a compound
• Recognize and apply exceptions to the octet rule.
• Identify metals and non-metals and predict types of compounds (ionic/covalent) between different elements.
• Student will be able to relate coulombs law and lattice energy.
• Use Lewis structures to predict and explain relative bond strength and lengths in a compound
• Name basic binary ionic compounds including polyatomic ions.
• Name basic covalent compounds containing two elements.