| Syllabus / Schedule | 
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| Chem 109, Dr. Paselk |
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Summer 2002 |
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Review: Problem sets since Exam I. Review nomenclature so that you can read questions and understand them. Review concepts, nomenclature, etc. from exam I that we have used in looking at additional system etc.
Be able to: convert numbers to scientific notation and
use numbers expressed in scientific notation; do all calculations
with proper significant figures; make all conversions within the
metric system (SI), name compounds given formulae, write formulae
given names.
Thermochemistry: Understand/define exothermic and endothermic. What are exothermic and endothermic reactions. What is heat? work? energy? enthalpy? DE = q + w. DH = DE - w. When are enthalpy and energy equal? Be able to solve heat capacity problems and calorimeter problems. Understand thermochemical equations (what happens to DH if the reaction is rewritten in reverse? What is a formation reaction? What are: standard state, standard heat of formation, standard enthalpy of formation? DH°f Know Hess's Law. Be able to solve heat/enthalpy of formation problems.
Electrons: What are De Broglie waves? l = h/mv. When is this equation used? What is the relationship between m & n (= f)? m & l? Be able to rearrange and to solve problems with this equation.
What does the Schrödinger equation describe? What are nodes? Be able to apply the concept of nodes to standing waves (as on a string) and to electron distributions. What does Y2 refer to for electrons and atoms? Be able to draw and to interpret cross-sectional diagrams of electron distributions in atoms for s & p orbitals. Be able to draw and interpret probability density (Y2 vs. r) plots for s & p orbitals for any value of n. How is the number of nodes related to n? How is a node represented on a Y2 vs r plot? Remember there is always one node at infinity.
What is an orbital? How many electrons can one orbital accommodate? What is a shell? Know number and letter designations (n= 1,2,3.. or K,L,M,...).What is a subshell? How are shells and subshells related to energy? What is spin? How does it effect orbital filling? What is paramagnetism? when does it occur?
Be familiar with energy and filling diagrams. Be able to give electronic configurations using all three of the conventions we have discussed (spectroscopic, orbital filling, noble-gas core). Know which orbitals are being filled for different regions of the periodic table.
Know what the four quantum numbers are and be able to assign quantum numbers to any electron in an atom, or to give an orbital designation for a set of quantum numbers. What information does each of the quantum numbers convey? (energy, orbital shape etc.) What is the Pauli Exclusion Principle and why is it important? How are nodes related to quantum numbers? (n = # nodes, l = angular nodes,...)
Chemical Periodicity: Discuss the various periodic properties we have discussed (atomic radii, ionization energies, electron affinities, electronegativities, stoichiometric ratios, metallic vs. non-metallic properties) and know the trends. How do these periodicity's relate to electronic configuration? Be able to explain trends, etc. in the plots of these properties. Be able to describe the properties of elements in grps I-A, II-A, VII-A, & VIII-A. Be able to name each of these grps of elements. Where are the transition metals? the lanthanide's? the actinides?
Chemical Bonding: What is an ionic bond? How is it formed? What forces maintain it? Anion. Cation. Ion pair. What is the octet rule? Be able to apply the octet rule to guess the ionic forms of the various "A" group elements. Why are outer electron shell octets so stable? Understand/be able to explain the energetics of ionic reactions. Be able to do a Born-Haber calculation given appropriate data. (In other words, you need to be able to recognize the required steps.)
What is a Lewis Structure? What is it intended to show? For which elements are Lewis structures most useful? (representative elements = "A" grps) Be able to draw Lewis structures for all the representative elements in their atomic and predicted ionic forms. Kernel vs. inert gas core. Be able to predict chemical stoichiometry using Lewis structures, and balancing.
What is a covalent bond? How do ionic and covalent bonds differ? How is it possible for an ionic bond to be "strong" and unstable while a covalent bond may be stable while not being as "strong"? Which electrons are involved in covalent bonding? What is electronegativity? Know electronegativity values for H and Li-F. How is it used? Be able to use electronegativity (both quantitatively and qualitatively [hi,lo rules]) to predict the ionic/covalent nature of a bond. Bond dissociation energy. Be able to calculate the energy in a reaction from bond energies. Bond length. Be able to draw a correct Lewis structure for any covalent molecule made up of atoms from the representative elements. (Remember-you use Electronegativity to determine covalent or ionic first!) When do you need to use multiple bonds? Resonance? Are multiple bonds real? What does resonance represent in the real molecule? Be able to make proper resonance based sets of Lewis structures. For which representative elements does the octet rule not hold? (H - B) When is valence expansion required? Be able to draw correct expanded valence shell Lewis structures. Which orbitals are involved in expanded valence shells? What is the outermost shell of an atom? Does the outer-most shell of an atom need to have any electrons in it?
Polar vs. non-polar bonding. Be able to assign Formal charges to each atom in a molecule. What are Formal charges useful for?
VSEPR Theory: What is VSEPR theory? Be able to use the VSEPR method to determine the geometry of a molecule, including demonstrating the process involved-what assumptions are made with this model. Know the various orientations of electron pairs around a central atom and the various molecular geometry's they predict (handout). What relations are there between electronic configuration and molecular shape? Does a given electron configuration always give the same molecular shape? Explain. Be able to determine whether a given molecule is polar or not. Be able to defend your decision (think charge separation and geometry).
Solids: What is a solid? crystal? glass? How do we know about the detailed structures of solids? Be able to solve simple problems using the Bragg eqn. What is a lattice? a unit cell? Know the three cubic unit cells. How many "atoms" are there in each? Be able to solve density and volume problems involving unit cells. What is close packing? What kinds of bonds and forces hold solids together? What are van der Waal's forces? London dispersion forces? hydrogen bonds? dipole-dipole bonds? Be familiar with the various types of solids (molecular, ionic, covalent metallic), their characteristic properties, and how these correlate with the bonds/forces holding them together. What is lattice energy? How is it calculated? Heat of crystallization. Sublimation.
Liquids: Define/describe: weak forces, Hydrogen bonds, vapor pressure, phase change, boiling, solid,. Why is water's boiling point so high (vapor pressure so low)? How does it compare to other molecules? Are there any molecules with similarly high boiling points? Why do liquids boil? When? Why are boiling points lower in the mountains? Explain cooling by evaporation. Be able to solve problems using the Clausius-Clapeyron equation. Molar heats of vaporization and condensation. Be able to describe/draw (with labels-DKE and PE; melting, vaporization etc.; heating etc.) a heating/cooling curve. Be able to interpret this curve, including why it looks this way. Be able to draw phase diagrams for water and a typical liquid such as carbon dioxide. Be able to interpret these diagrams. Where are solid, liquid and gas phases on these diagrams? Be able to predict what will happen along a typical constant temperature or pressure line on such a diagram. What is supercooling? superheating? Why do they occur? What is bumping? a seed crystal? Explain sublimation, triple point critical point. Equilibrium vapor pressure.
Solutions: Define/describe: solution, salt, solvent, solute, saturated solution, unsaturated solution, super saturated solution, mass %, ppm, ppb, molarity (M), molality (m), mole fraction (X), neutralization, equivalent (in chemical reactions). Why do some substances dissolve in each other? Why do others not? ("Like Dissolves Like"). Be able to solve problems involving concentrations as we have seen in class and in the lab: find mass %, molarity, molality, mole fraction of solutions given their components. Be able to find concentrations of solutions after dilution or mixing with other components. Be able to do problems in problem set.
| Syllabus / Schedule |
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© R A Paselk
Last modified 11 July 2002
