1. Understand the meaning of the following terms: electromagnetic radiation, wavelength, and frequency. Know the equation that relates frequency and wavelength and be able to use it to perform calculations.
2. Understand the relationships between energy of radiation, the wavelength, and frequency of the radiation. Ex. Does a relatively long wavelength correspond to high or low energy? Be able to rank colors within the visible portion of the spectrum based on their energy.
3. Be able to use Planck’s equation to perform calculations involving energy. Understand what it means to say that energy is quantized.
4. Understand what a photon is. Be familiar with the two “important conclusions from the work of Planck and Einstein” described in your textbook.
5. Review
chapter 2 to be able to describe
6. Using the Bohr model of the atom, explain why elements glow a unique color when heated in a flame. What electronic transitions are taking place in the process? How do quantized electronic transitions relate to emission line spectra? Explain why atoms of different elements exhibit unique colors in a flame.
7. Be familiar with the main features of the Bohr model and how this model can be used to describe quantized electron transitions. Also be aware that the Bohr model does not work for atoms other than hydrogen and that our current model of the atom is not derived from the Bohr model.
8. Understand that the current model of the atom describes electron orbitals as regions where there is a high probability of finding an electron within a specified volume of space surrounding the nucleus.
9. Know possible values for quantum numbers n, l, ml, and ms for a given atom. Know what information is conveyed by each of these quantum numbers. Be able to assign quantum numbers to describe the distribution of electrons within atoms.
10. Understand what is meant by the following terms as they relate to electrons in an atom: atomic orbital, energy level, sublevel, spatial orientation of an orbital, spin, nodes, degenerate. (Note: these terms will be described in more detail in class.)
11. Be able to write orbital notations (using arrows) and electron configurations for any atom using the Aufbau order of atomic orbitals and Hund’s rule. Be able to differentiate between valence electrons and core electrons. Understand that valence electrons affect the chemical properties of an element.
12. Be familiar with the various “blocks” in the periodic table which correspond to particular sublevels being filled. Also understand how the period numbers relate to energy levels and how the group numbers of the main group elements relate to numbers of valence electrons. (See also Figures 7.27 & 7.28)
13. Understand what is meant by the terms first and second ionization energy, and be familiar with the trend for first ionization energy found in the periodic table. Understand the relationship between strength of ionization energy and formation of cations or anions.
14. Understand what is meant by the term electron affinity, and be familiar with the trend for electron affinity found in the periodic table. Understand the relationship between electron affinity and formation of cations or anions.
15. Be familiar with the trend for atomic radius found in the periodic table. Be able to explain this trend using concepts such as effective nuclear charge, screening/shielding, and energy levels.