List the Instructor's student learning outcomes that are relevant to the GEP Natural Sciences Objective 1:
Obj.O 1) Use the methods and processes of science in testing hypotheses, solving problems and making decisions

A) Compare and contrast various historical models of the atom, explaining how the models evolved with new experimental results
B) Describe the interaction between light and matter, and how energies of atoms and molecules are quantized
C) Predict three dimensional shapes and orbital hydridization of molecules based on their Lewis structures
D) Determine if precipitation, redox and acid/base reactions are extensive

Measure(s) for the above outcome(s): Describe the assessments that will be used to determine if students have achieved the outcome. Including a relevant example assignment/question/prompt is encouraged for clarity.

All measures are through assignment and exam questions. Sample questions are given below:

OBJECTIVE A) Compare and contrast various historical models of the atom, explaining how the models evolved with new experimental results
1) Of the following experiments, which one gives evidence for quantized energy levels?
A) Thomson’s cathode ray experiment
B) Millikan’s oil drop experiment
C) Rutherford’s gold foil experiment
D) atomic spectrum of hydrogen
E) mass spectrometry

OBJECTIVE B) Describe the interaction between light and matter, and how energies of atoms and molecules are quantized
1) Consider the following transitions in the Bohr model of the atom:
A) n = 2 to n = 4 B) n = 6 to n = 3; C) n = 3 to n = 5; D) n = 2 to n = 1
Which of these is the emission process that gives the photon of greatest wavelength?
2) Which of the following statements about levels and sublevels is NOT correct?
A) The 2p sublevel can contain up to six electrons
B) The 4d sublevel can contain up to ten electrons
C) The 5s sublevel contains two orbitals
D) The n=4 level contains four sublevels
E) The n=3 level contains nine orbitals

OBJECTIVE C) Predict three dimensional shapes and orbital hydridization of molecules based on their Lewis structures
1) Answer the following questions for SeO2 and SbO33-, where all atoms obey the octet rule.
a) (10 each) Draw the Lewis structure for each species (if resonance structures exist, only draw one).

SeO2 : SbO33- :

b) (3 each) If you haven’t done so already, add formal charges to your structure.

The remaining parts of this question will be graded on the structures you have drawn above.
c) (3 each) Yes or no, do other resonance structures exist for:

SeO2 ________ SbO33- ________

d) (3 each) Based on your structure, what is the:

SeO bond order in SeO2 ________ SbO bond order in SbO33- ________

e) (3 each) How many sigma bonds are in SeO2 ________ SbO33- ________

f) (3 each) How many pi bonds are in SeO2 ________ SbO33- ________

g) (5 each) What is/are the bond angle(s) in SeO2 _______ SbO33- ________

h) (5 each) Based on your structure, what is the shape of

SeO2 ________ SbO33- ________
i) (5 each) Based on your structure, what is the hybridization at

Se in SeO2 ________ Sb in SbO33- ________

OBJECTIVE D) Determine if precipitation, redox and acid/base reactions are extensive
1) For each combination of 0.1 M aqueous solutions listed, state (yes or no) whether a precipitate will form. IF YES, then provide the chemical formula of the solid. IF NO, write “None” for chemical formula.
a) V(NO3)2 and Cu(C2H3O2)2 b) Cr(ClO4)3 and K2S c) Ba(NO3)2 and Li2SO4

ppt form? ____________________ __________________ ___________________

Formula? ____________________ __________________ ___________________

2) A galvanic electrochemical cell is constructed using the Sn2+/Sn and Fe2+/Fe half reactions. What reaction takes place at the cathode?
A) Sn → Sn2+ + 2 e1- C) Fe → Fe2+ + 2 e1-
B) Sn2+ + 2 e1- → Sn D) Fe2+ + 2 e1- → Fe

3) Consider the following two acid base reactions:
I) HNO2 + H2O II) H2CO3 + Na2SO4

Which of these reactions are extensive?
A) I only B) II only C) both I and II D) neither I nor II

Write a balanced net equation for each reaction
Reaction I : _________________________
Reaction II : _________________________

List the Instructor's student learning outcomes that are relevant to the GEP Natural Sciences Objective 2:
Obj. 2) Make inferences from and articulate, scientific concepts, principles, laws, and theories, and apply this knowledge to problem solving.

A) Describe forms of energy in a chemical system and apply Coulomb’s law to determine the energy of interaction of charges
B) Predict relative atomic radii, ionization energies and electronegativities of elements based on periodic table location and on orbital energy diagrams
C) Correlate K, Go, activation energies and reaction rates for reversible processes
D) Describe the dissolving process and calculate the molarity of a solution

Measure(s) for the above outcome(s): Describe the assessments that will be used to determine if students have achieved the outcome. Including a relevant example assignment/question/prompt is encouraged for clarity.

All measures are through assignment and exam questions. Sample questions are given below:

OBJECTIVE A) Describe forms of energy in a chemical system and apply Coulomb’s law to determine the energy of interaction of charges
1) Consider the following scenarios:
A) a 3- charge and a 2+ charge at 4 units of distance apart
B) a 3- charge and a 1- charge at 2 units of distance apart
C) a 2+ charge and a 0 charge at 3 units of distance apart
D) a 4+ charge and a 1- charge at 2 units of distance apart
E) a 2+ charge and a 1+ charge at 2 units of distance apart
Which one is the highest energy scenario?
Which one is the lowest energy scenario?

OBJECTIVE B) Predict relative atomic radii, ionization energies and electronegativities of elements based on periodic table location and on orbital energy diagrams
1) From the following list of elements, select the one with the smallest ionization energy.
A) As B) Cl C) Ga D) K E) Mg

2) Atoms with small electronegativities will generally have:
A) small radii and low energy valence electrons
B) small radii and high energy valence electrons
C) large radii and low energy valence electrons
D) large radii and high energy valence electrons

Given the energy diagram at the right, select the statement that is TRUE.
A) Z has the largest electron affinity
B) X has the smallest electron affinity
C) Y has the smallest ionization energy
D) X has largest ionization energy
E) none of these statements are true

OBJECTIVE C) Correlate K, Go, activation energies and reaction rates for reversible processes
1) Consider the following reaction:
PCl5(g) → PCl3(g) + Cl2(g)
If this reaction is endothermic, what can you say about the spontaneity?
A) The reaction is spontaneous at both low and high temperature
B) The reaction is spontaneous at low temperature, but non-spontaneous at high temperature
C) The reaction is non-spontaneous at low temperature, but spontaneous at high temperature
D) The reaction is non-spontaneous at both low and high temperature
2) Starting with equal amounts of reactants and products in a system where kf is greater than kr,
A) there are mostly reactants at equilibrium and Ea(f) is greater than Ea(r)
B) there are mostly products at equilibrium and Ea(f) is greater than Ea(r)
C) there are mostly reactants at equilibrium and Ea(f) is less than Ea(r)
D) there are mostly products at equilibrium and Ea(f) is less than Ea(r)
3) In a reversible reaction where the value of Go is negative,
A) the value of K is less than 1 and the reaction is extensive
B) the value of K is greater than 1 and the reaction is extensive
C) the value of K is less than 1 and the reaction is not extensive
D) the value of K is greater than 1 and the reaction is not extensive

D) Describe the dissolving process and calculate the molarity of a solution
1) You need to prepare 500 mL of a 0.225 M solution of CuCl2. Calculate how many grams of CuCl2 are needed.