STUDY GUIDE - TEST 2:
CH123: General Chemistry - Fall 2006
For the second examination, you should be able to:
- 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.
- Identify the molecular/ionic species in water when a substance is
added to water.
- Write the molecular, ionic, and net ionic equations for the reactions
of strong electrolytes in water.
- Identify precipitation reactions, and predict the products of
precipitation reactions based on solubility rules.
- Define acid and a base, identify acid/base reactions, and predict the
products of the reactions.
- Know the formula and Lewis structures of the common strong acids (nitric, hydrochloric,
sulfuric), the weak acid (acetic acid), the strong bases (oxide, hydroxide)
and the weak base ammonia.
- Rank the relative strength of acids and bases based on
writing chemical equations, and based on comparisons of the relative
stability of the conjugate base produced.
- Define oxidation, reduction, oxidizing agent, reducing agent
- Determine/assign oxidations numbers of all atoms in a substance and
understand how to use oxidation numbers in identifying and analyzing redox reactions
and in comparing the relative strength of a series of molecules with the
- Balance redox equations usingthe half-reaction method
in acidic or basic solution .
- Do stoichiometry problems based on redox titrations.
- Given tables showing the relative strength of
oxidizing/reducing agents and acids/bases, predict likely pairs of stronger
oxidizing and reducing agents, and of stronger acids and bases, that would
likely react to form weaker pairs.
- Describe interference (constructive, destructive), and
diffraction, and their use in understanding the properties of waves and
- Explain the photoelectric effect and how Einstein's
interpretation of it altered our view of light.
- Mathematically interpret the graphs of Ekin
vs frequency (υ) in the
- 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.
- Discuss the meaning and differences in the
the probability amplitude,
the probability amplitude as depicted in electron cloud maps, and the radial
- Describe the significance of the quantum numbers n, l,
ml, and ms.
- 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
- Write the quantum number for the electrons in specific
- Describe orbitals and the relative energy of the
orbitals in hydrogen and polyelectronic atoms.
- Explain the meaning of core electrons, valence
electrons, shielding, penetration, core charge, and Zeff.
- 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.
- 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.
- Explain how the shape of the present Periodic Table can
be accounted for by quantum theory.
- 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
- Draw energy diagrams showing the relationships between
the energy of electrons in an atom, and the ionization energy.
- Define lattice energies and predict which ionic
compounds have lower and higher lattice energies.
- Given energy values like ionization energy, and
electron affinities, use a Born-Haber thermodynamic cycle to calculate
- Explain, and manipulate the following formulas:
- c =ul
- p = mv ; pang = mvr
- λ= h/p
- E = hυ
- E = mc2
- ΔpΔx > h/4π
- Ekin = mv2/2
- Epot = -ke2/r (electrostatic)
Epot = mgh (gravitational potential)
- Fcoul. = kQ1Q2/r2
- Etot = mv2/2 - ke2/r
= -ke2/2r => The Bohr equation for H assuming
a stable atom with a classical inward Coulombic force balanced by
- Bohr quantum postulate: pang
= mvr = nh/2π
- Bohr equations for hydrogen: E=-B/n2 = -1312/n2 (kJ/mol
e) = -2.18 x 10-18/n2 J/e