STUDY GUIDE - TEST 2:
CHAPTERS 4-6

CH123: General Chemistry - Fall 2003

Dr. Jakubowski

For the second examination, you should be able to:

1. Understand the relationships among mole, molecular or atomic weight, and mass, be able to write, interpret chemical equations, and solve quantitative problems about chemical reactions given descriptions of the reactions.
2. Identify the molecular/ionic species in water when a substance is added to water.
3. Write the molecular, ionic, and net ionic equations for the reactions of strong electrolytes in water.
4. Identify precipitation reactions, and predict the products of precipitation reactions based on solubility rules.
5. Define acid and a base, identify acid/base reactions, and predict the products of the reactions.
6. Know the common strong acids (nitric, hydrochloric, sulfuric), the weak acid (acetic acid), the strong bases (oxide, hydroxide) and the weak base ammonia.
7. Rank the relative strength of acids and bases based on writing chemical equations
8. Define oxidation, reduction, oxidizing agent, reducing agent
9. Determine/assign oxidations numbers of all atoms in a substance and understand how to use oxidation numbers in identifying and analyzing redox reactions.
10. Balance redox equations using either the half-reaction method in acidic solution .
11. Do stoichiometry problems based on redox titrations.
12. Describe interference (constructive, destructive), and diffraction, and their use in understanding the properties of waves and particles.
13. Explain the photoelectric effect and how Einstein's interpretation of it altered our view of light. 
14. Explain, with diagram and words, the Rutherford, Bohr, and Schrodinger's models of the atom, and describe the successes and limitations of each of these theories.  (For example, explain how each of the above theories explains (or cannot explain) atomic absorption and emission spectra.
15. Discuss the Copenhagen interpretation (views of Born, Heisenberg, and Bohr) of quantum mechanics.
16. Describe the significance of the quantum numbers n, l, m_l, and m_s.
17. Draw  for 1s, 2s  and 2p orbitals:  graphs of electron probability  vs distance from the nucleus, and cartoon pictures representing the electron density and the shapes of the orbitals.
18. Write the quantum number for the electrons in specific orbitals
19. Describe orbitals and the relative energy of the orbitals in hydrogen and polyelectronic atoms.
20. Explain the meaning of core electrons, valence electrons, shielding, penetration, core charge, and Z_eff.
21. Explain and use the Aufbau principles, Pauli Exclusion Principle and Hund's rule to write the electron configuration of atoms and ions (1s²2s²sp⁶... etc) in the periodic table, and to draw orbital diagrams (placing arrows in boxes representing the orbitals) for these configurations.
22. Explain the term degeneracy and why for the hydrogen atom the s, p, d, and f orbitals in the same shell (same n value) are degenerate, but for other elements, the orbitals in a given shell are not.
23. Explain how the shape of the present Periodic Table can be accounted for by quantum theory.
24. Explain periodic trends in ionization energy, electron affinity, atom and ion size, core charge and chemical reactivity for the elements in the Periodic Table with respect to electron configuration and Zeff.
25. Draw energy diagrams showing the relationships between the energy of electrons in an atom, and the ionization energy. 
26. Define lattice energies and predict which ionic compounds have lower and higher lattice energies.
27. Given energy values like ionization energy, and electron affinities, use a Born-Haber thermodynamic cycle to calculate lattice energy.
28. Understand and write products of rx's of Gp I and IIA element
29. Explain, and manipulate the following formulas:
    • c =ul
    • p = mv ; p_ang  =  mvr
    • λ= h/p
    • E = hυ
    • E = mc²
    • F=ma
    • ΔpΔx > h/4π = h_bar/2
    • E_kin = mv²/2
    • E_pot = -ke²/r (electrostatic)  E_pot = mgh (gravitational potential)
    • F_coul. = kQ₁Q₂/r²
    • E_tot = mv²/2  - ke²/r  = -ke²/2r   => The Bohr equation for H assuming a stable atom with a classical inward Coulombic force balanced by kinetic energy
    • Bohr quantum postulate:  p_ang  =  mvr = nh_bar
    • Bohr equations for hydrogen:  r=n²A; v=C/n, E=-B/n² = -1312/n²  (kJ/mol).