Competencies for CHEM 1120     summary               76  Items

KEY:

 
text (Chang)
delivery method  evaluation method
x.y  where
l = lecture
T = lecture test
x = chapter
n = notes
Lx = lab number x  (labs are also delivery methods)1
y = section
v = video, slideshows, internet sources available
F = final exam
1,2,3,4,5
TBR General Ed learning outcomes 1-5 - see below
C = critical item question or lecture test

Item
Performance/Task:  The student will: text
sections
delivery
method
eval.
method
TBR learn
objectives
General Equilibria
1
Be able to write the expression for any equilibrium if given a reaction using standard states
14.1-14.3
l, n
T

2
Be able to solve for an unknown quantity in an equailibrium problem when simple substitution is involved (RSCC type 1- when the problem is presented at equilibrium).
14.2-14.3
l, v, L
T, F, L

3
Be able to apply algebra to problems that start out not at equilibrium and approach equilibrium (RSCC type 2)
14.4
l, v, L
T, F, L

4
Be able to apply Le Châtelier's principle to shifts in equilibrium cause by changes in temperature, pressure and concentrations.
14.5
l, v
T

5
Be able to describe the role of a catalyst.
14.5,(13.6)
l
T

Acids and Bases and pH
6
Be able to write any Brønsted-Lowry acid-base reaction (also review from CHEM 1110)
15.1
l, v, L
T, L

7
Be able to describe autoionization and be able to make calculations using the Kw
15.2
l, v, L
T. F, L

8
Be able to calculate the pH given either the [H3O+]} or the [OH-]
15.3
l, v, L
T, C, L

9
Be able to calculate the pH of a strong acid or a strong base
15.4
l, v, L
T, C, L

10
Be able to calculate the pH of a weak acid or a weak base (type 2)
15.5, 15.6
l, v, L
T, C, L

11
Be able to calculate the equilibrium constant for the conjugate of a weak acid or weak base.
15.7
l, v, L
T, C, L

12
Be able to calculate pH of polyprotic acids and know the convention for the 1st, 2nd, etc. ionization constant
15.8
l, v, L
T, L


Review item - know the strong and weak acids and the strong, slightly soluble and weak soluble bases
15.9
l, v, L
T, L

13
Be able to do salt hydrolysis problems to obtain pH
15.10
l, v, L
T, L


Review item - Be able to write the reaction between metal or non-metal oxides and water.
15.11
l, v, L
T, L

14
Know the definition of amphoteric (and amphiprotic) and how it applies to slightly soluble polyprotic hydroxides.
15.11
l, v, L
T, L

15
Know the definition of a Lewis acid and base and be able to identify these in a reaction
15.12
l
T

Buffers, Titrations, Ksp, Kf and Kd
16
Be able to calculate the pH of a buffer.
16.2, 16.3
l, v, L
T, C, L

17
Be able to calculate the titration curve for either a strong acid/weak base titration or a strong base/weak acid titration
16.4
l, v, L
T, L

18
Be able to calculate the pH of an end point a determine the appropriate indicator
16.5
l, v, L
T, L

19
Be able to calculate the common ion effect for solubility using the Ksp (type 1)
16.6, 16.8
l, v, L
T, L

20
Be able to calculate the molar solubility from any starting solution given the Ksp (type 2)
16.6, 16.8
l, v, L
T, L

21
Be able to combine solubility calculations with pH
16.9
l, v, L
T, L

22
Be able to do type 1 or type 2 problems involving complex ions using either the Kf or Kd
16.10
l, v, L
T, L

23
Be able to combine pH, complex ion and solubility problems, especially to the qualitative analysis scheme
16.11
l, v, L
T, L

Thermochemistry*
24
Know the definition of energy and the various forms it might assume.
6.1
l, v
T

25
Know the definitions of the following:  open system, closed system, isolated system, surroundings, a universe, exothermic, endothermic, state function, state of a system
6.2-6.3

l, v
T

26
Be able to give the first law of thermodynamics and make calculations base upon it.
6.4
l, v
T, C

27
Be able to define work, heat, internal energy and enthalpy
6.2-6.4
l, v
T

28
Know the definition of molar heat capacity (at either constant volume or pressure) and be able to do problems involving heat capacity
6.5
l, v
T

29
Be able to calculate the enthalpy of reaction from the standard enthalpies of formation.
6.6
l, v
T, C

30
Be able to calculate the enthalpy of solution from the standard enthalpies of formation of compounds and ions.
6.7+
l, v
T, C

Thermodynamics*
31
Be able to give an explanation of the zeroth law of thermodynanics
6.5
l, v
T

32
Be able to define what a spontaneous process is.
18.2
l, v
T, C

33
Be able to relate entropy to microscopic randomness and how to calculate it give the number of microstates.
18.3
l, v
T

34
Know what is meant by "standard state" and standard (molar) state functions
18.3
l, v
T

35
Be able to give the second law of thermodynamics and make calculations based upon it
18.4
l, v
T, C

36
Be able to tell what the third law of thermodynamic is a reach conclusions based upon it.
18.4
l, v
T

37
Be able to calculate the Gibbs' free energy and know the importance of it in relation to equilibrium.
18.5
l, v, L
T, C, L

38
Be able to derive the equation that relates thermodynamics to the equilibrium constant and relate this to the van't Hoff plot
18.6
l, v, L
T, C, L

39
 Be able to calculate the equilibrium constant from the standard molar Gibbs' free energy
18.6
l, v, L
T, C, L

Electrochemistry
40
Be able to balance redox reactions by the half reaction method.
19.1
l, v, L
T, L

41
Be able to describe how an electrochemical cell works, with it various parts.  Cells include:  Galvanic, Leclanché, mercury, lead storage, Ni-Cd, lithium , fuel cell, concentration cells, Downs cell,  19.2, 19.6
l, v, L
T, L

42
Know the definitions used in electrochemistry including: anode, cathode, electrolyte, anolyte, catholyte, half cell reaction, voltage, electromotive force or emf
19.2
l, v, L
T, L

43
Be able to describe and use standard (reduction) potentials and how they are derived from thermodynamics.
19.3
l, v, L
T, C, L

44
Be able to interconvert from standard molar Gibbs' free energy to standart potentials using the standard hydrogen electrode

l, v
T, C

45
Be able to calculate standard potentials for a cell.
19.3
l, v, L
T, C, L

46
Be able to calculat non-standard potentials for a cell using the Nernst equation.
19..5
l, v, L
T, C, L

47
Be able to recognize whether a radox reaction is spontaneous or not and, related, whether a cells emf is positive or negative.
19.4
l, v, L
T, L

48
Be able to describe the principal mechanism of aqueous corrosion
19.7
l
T

49
Be able to calculate quantities of material evolved (or used) in an electroplating (or galvanic) cell  using Faraday's law
19.8
l, v, L
T, L

Chemical Kinetics
50
Be able to define mathematically the rate of a reaction and how this is related to other expressions of rate.
13.1
l, v, L
T, C, L

51
Be able to determine a rate law and make calculations base upon a rate law. 13.2
l, v, L
T, L

52
Be able to express the simple zero, first, and second order integrated rate laws and use them to make calculations.
13.3
l, v, L
T, L

53
Be able to utilize the concept of "half life" for the first order integrated rate law to make calculations.
13.3
l, v
T, C

54
Be able to explain the collision theory and the transition state theory to calculate the temperature dependance (Arrhenius equation both simple substitution and parametrically) of the rate constant.
13.4
l, v
T

55
Be able to relate reaction mechanisms and elementary steps to obtain the rate law
13.5
l, v
T

56
Know the role of catylsts and be able to site some examples and how it affects a reaction.
13.6
l
T

Organic Chemistry (instructor option)
57
Be able to distinguish the various classes of hydrocarbons and their properties.   (aliphatic, aromatic, alkanes, alkenes, alkynes, cyclic, etc.)
24.1, 24.2
l
T

58
Be able to name the alkanes, alkenes, alkynes and their (functional) substituted derivatives.
24.2
l
T

59
Know the various types of isomers and what the origin is of structural, geometrical and optical isomerism.
24.2
l
T

60
Be able to tell if a molecule has a geometrical isomer or an optical isome
24.2
l
T

61
Be able to describe the substitution reaction and how it is accomplished.
24.2
l
T

62
Be able to describe and predict the addition reaction to alkenes and alkynes
24.2
l
T

63
Know the basic structure of the aromatic hydrocarbons and the role of resonance.
24.3
l
T

64
Be able to name some of the simple substituted aromatics.
24.3
l
T

65
Be able to describe the mechanism of the aromatic substitution reaction.
24.3
l
T

66
Be able to recognize the functional groups:  alcohols, carboxylic acids, esters, ethers, aldhydes, ketones,amines, amides, halogens, nitryls
24.4
l
T

67
Know the important reactions involving the functional groups.
24.4.
l
T

Nuclear Chemistry (instructor option)
68
Know the subatomic particles important in nuclear chemistry and their symbols
23.1
l
T

69
Be able to balance a nuclear reaction and fill in unknown quantities
23.1
l
T

70
Know what is meant by the belt (band, island) of stability be able to predict the type of decay for a radioactive isotope not on the belt
23.2
l
T

71
Be able to calculate the energy released in a nuclear reaction given the isotope masses
23.2
l
T

72
Be able to describe the decay of unstable heavy isotopes and the various decay series
23.3
l
T

73
Be able to do half-life type calculations, include dating techniques
23.3
l
T

74
Be able to describe fusion reactions and know some of the important ones.
23.4, 23.6
l
T

75
Be able to describe fission reactions and know some of the important ones.
23.4, 23.5
l
T

76
Be able to describe some important applications of radioactive isotopes
23.7
l
T

* Thermochemistry and Thermodynamic are supplimented with handouts available on the internet.

TBR General Education Outcomes for Natural Sciences
Learning Outcomes
Item
Students will demonstrate the ability to…..
1
Conduct an experiment, collect and analyze data, and interpret results in a laboratory setting.
2
Analyze, evaluate and test a scientific hypothesis.
3
Use basic scientific language and processes, and be able to distinguish between scientific and non-scientific explanations.
4
Identify unifying principles and repeatable patterns in nature, the values of natural diversity, and apply them to problems or issues of a scientific nature.
5
Analyze and discuss the impact of scientific discovery on human thought and behavior.


1For more details about the CHEM 1110 Laboratories see: http:/www.genchem.net/competencies/lab2comp.html