|
|
| Goal
I. Understand the terms used to describe a solution and the characteristics
of its components. |
Objectives: To meet the requirements of Goal
I, you must be able to:
-
distinguish between
the
solution, solvent, solute; and then determine
which
component of a solution is the solvent and which is the solute;
-
explain the
term solubility (p. 77) and the terms saturated, unsaturated,
supersaturated (pp. 493-494), concentrated and dilute (p. 118)
used to describe solutions;
-
explain the term
electrolyte (p. 142 Fig. 4.7) and distinguish between strong, weak and
nonelectrolytes in terms of:
-
the proportion of solute that forms ions, and
-
the ability of a solution to conduct
an electric current;
-
classify an electrolyte
as an acid, base or a salt from its formula;
-
use Table 4.2 (p.143)
to classify acids and bases as strong or weak; (Memorize
this table)
-
use Table 4.1 (p.141)
to classify an ionic compound as soluble, slightly insoluble or insoluble;
-
write equations
representing the ionization of strong and weak acids and bases in water,
and for the dissociation of soluble salts in water.[Top]
| Goal II. Use tabulated
data to predict products and write equations for some commonly encountered
reactions. |
Objectives: To meet the requirements of Goal
II, you must be able to:
-
predict whether
a precipitate will form when solutions of salts are mixed; then write
molecular, complete ionic and net ionic equations for any reaction which
occurs;
-
recognize the general
trends in reactivity of elements within a group or a period of the periodic
table;
-
predict whether
a single displacement reaction will occur when hydrogen or an elemental
metal is added to a solution of salt (given an activity series for metals,
Fig. 4.20);
write molecular and net
ionic equations for any reaction which occurs (pp. 160-162);
-
predict whether
a replacement reaction will occur when an elemental halogen is added to
a solution containing a halide ion; write molecular and net ionic equations
for any reactions which occur (p. 162);
-
determine whether
a compound insoluble in water will dissolve by adding a given reactant.
[Top]
| Goal III. Use Standard
quantitative concentration units; solve stoichiometric problems involving
reagents in solution. |
Objectives: To meet the requirements of Goal
III, you must be able to:
-
distinguish between
concentration expressed as mass percent and volume percent (pp. 499-500);
-
calculate moles
or grams of solute, volume of solution, molarity, given two of the three
quantities;
-
solve problems concerning
the dilution of a solution with water;
-
explain the terms
titration, standard solution, indicator;
-
explain the significance
of the end point in a titration and how it is determined;
-
calculate the quantity
of any other reactant or product given the quantity of any reactant or
product in a titration (in grams, moles or concentration and volume of
solution);
-
solve titration
problems. [Top]
|
Unit 4 Assignments
|
| Read: |
Text
Chapter 3.5, pp. 116-123
Text Chapter 4.1,
4.2, pp. 134-148; 4.4, pp. 156-164 |
| Video
Programs: |
- Solubility
and Precipitation
- Acids
and Bases
- Molarity
and pH
- Solution
Stoichiometry, pH, Titration
|
| Textbook
Assignments: |
Read
and Understand all "Sample Problems," "Follow
Up Problems" and the blue-colored problems at the
end of the chapters.
The
answers for the Follow Up Problems are at the end
of the chapter; the answers for the blue-colored
problems are in Appendix C.
|
| ChemSkill
Builder Assignments: |
Mandatory
assignments to be submitted for grade
Chapter 5, Sections
5.1, 5.2, 5.3, 5.5, 5.6 (Solubility Rules, Metathesis
Reactions, Ionic Equations, Predicting Products,
single replacement/ activity)
Chapter 3, Section
3.5 (acids, bases, salts, electrolytes)
Chapter 10, Sections
10.1, 10.2 (Redox identifying species, determining
oxidation numbers)
Chapter 6, Sections
6.2, 6.3 (Titrations, Volumetric Analysis)
Note:
do NOT do Section 6.5
|
| Do Cyber Lab 4 |
See CHM 111 Laboratory Guide. Submit via mail to ELI. |
| Take
Exam 2 |
Exam
2 covers Units 3 and 4. You will be given a copy of the Periodic Table.
You may use a 3" x 5" hand-written study card for Exams 1, 2, 3, 4, and 5. (NOT TO BE USED FOR THE NOMENCLATURE TEST.) You must hand-write the information you would like to have on your card yourself -- no technology miracles allowed. Formulas, constants, definitions, concepts, solubility tables, etc., may be on the study card. NO SAMPLE PROBLEMS are allowed to be on the card. You may write on both sides of the study card. The card must be submitted with your exam. Any abuse of this privilege will result in a failing grade for the course. |
| Note:
Complete Solutions, including all units of measurement,
must be shown for all problems. |
[Top]
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