SA 560B; 826-5719
Hour Exam 3 Study Guide
Spring 2015 version
Review
Homework since Exam II (see suggested problems on Schedule). Review Quizzes (see Keys on my Moodle site), particularly those on materials since exam II. Review nomenclature
so that you can read questions and understand them. Review concepts
from exams I & II that we have used in looking at additional systems
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).
Thermochemistry (Chapter 6)
Understand/define exothermic and endothermic. What are exothermic and endothermic reactions. What is heat? work? energy? enthalpy? 
E = q + w. H= E - w. When are enthalpy
and energy equal? Be able to solve heat capacity problems, calorimeter
problems. Understand thermochemical equations (what happens to H if the reaction is rewritten
in reverse? What is a formation reaction? What are: standard state,
standard heat of formation, standard enthalpy of formation? H°f . Know Hess's Law.
Be able to solve heat/enthalpy of formation problems. Module 11(Thermochemistry)
Electrons, Atoms and Periodicity (Chapter 7)
What are De Broglie waves? 
= h/mv. When is this equation used? What is the relationship between
m & f? m & ?
Be able to rearrange and to solve problems with this equation.
Module 12 (Energy & Light) 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 
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 ( 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
vs r plot? Remember there is always one node at infinity. Atomic Orbitals supplement
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? Be familiar with energy and filling diagrams.
What is spin? How does it effect orbital filling? What is paramagnetism?
when does it occur?
Be able to give electronic configurations
using all three of the conventions we have discussed. 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,...) Module 13(Quantum Numbers, Electronic Structure of Atoms & Periodicity)
Discuss/Understand 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 groups of elements. Where
are the transition metals? the lanthanide's? the actinides?
Chemical Bonding (Chapter 8)
What is electronegativity? 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.
What is an ionic bond? How is it formed?
What forces maintain it? Anion. Cation. Ion pair. 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? 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"? How are electrons arranged in each?
What is a Lewis Structure? What is it intended to show? For which
elements are Lewis structures most useful? (A groups) Be able to
draw Lewis structures for all the A-group elements in their atomic
and predicted ionic forms. Kernel vs. inert gas core. See also Lewis Structures Module
Be able to draw a correct Lewis structure for any
covalent molecule made up of atoms from the "A": groups.
(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 A-grp elements does the octet rule not hold?
(H to 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? Be
able to predict chemical stoichiometry using Lewis structures,
and balancing.
Bond dissociation energy.
Bond length. 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.) Understand/be able to calculate reaction enthalpies (H) given bond energies. How does bond length vary with multiple bonding?
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 in Discussion manual, p LN-4). What relations are there between electronic configuration
and molecular shape? Does a given electron configuration always
give the same molecular shape? Explain. Polarity: Be able to determine whether
a given bond is polar or not. Be able to determine whether
a given molecule is polar or not. Defend your decision (think
charge separation [differences in electronegativity] and geometry). See also VSEPR Theory and Molecular Geometry Module
You will be provided with a Periodic Table and Useful Constants/Equations etc. (on Moodle)
© R A Paselk
Last modified 12 April 2015
C109 Lecture Notes