<html>
<head>
<meta http-equiv="content-type" content="text/html; charset=utf-8">
</head>
<body text="#000000" bgcolor="#FFFFFF">
Quiz 1 will cover the following: Chapter 13 (13.1-13.6) and
Sections 14.1-14.3
<br>
<br>
This is pretty much up through last Monday. The only thing from
today's
<br>
lecture is section 14.3 (the initial rate problems, finished the 2nd
example<br>
today).
For the most part that's how coverage on quizzes will be,<br>
Wed, Fri of one week and Mon of the next week, with maybe a small<br>
amount from the 2nd Wed. This quiz covered last week's material,
this<br>
Monday's and 1 example from section 14.3 from today.<br>
<br>
Section 13.1:
<br>
<br>
Understand the solution process and energy diagrams, how solutions
form,
<br>
ideal, endothermic and exothermic solution formation and the
importance
<br>
of entropy in solution formation. In general, when things mix there
is
<br>
an inc. in entropy (disorder) but this is not always the case. An
inc.
<br>
in entropy is absolutely necessary for an ideal or endothermic
solution
<br>
to form. This is not the case for an exothermic process. An
exothermic
<br>
process already tends to be spont. so an inc. in entropy is not
necessary
<br>
for this type of solution to form. There are cases in which the
delta(H)_soln
<br>
is negative (exothermic) and the entropy decreases (solution is more
ordered)
<br>
and the solution forms. Also, understand the role of attractive
forces
<br>
between particles in solution formation.
<br>
<br>
In the 12th and 13th editions the delta(H)_solvation is referred to
as the
<br>
the delta(H)_mix.
<br>
<br>
I also have a link showing the solution enthalpy diagrams including
a
<br>
discussion about the attractive forces and entropy, "Ch. 13 -
Solution
<br>
Formation and Solubility Effects" in the "Notes" section of the
course web
<br>
page.
<br>
<br>
<a
href="https://cbc-wb01x.chemistry.ohio-state.edu/%7Erzellmer/chem1220/notes/ch13_soln_formation.pdf"><b>Ch.
13 - Solution Formation and Solubility Effects</b></a><br>
<br>
Section 13.2:
<br>
<br>
Solubility, saturated, unsaturated and supersaturated solutions.
<br>
<br>
Section 13.3:
<br>
<br>
Factors affecting solubility - Att. forces ("like dissolves like"),
pressure
<br>
and temp. affects. You're considering temp. effects and "like
dissolves like"
<br>
concepts in exp 1 (SOL).
<br>
<br>
I have summary on line about attractive forces and solubility. See
the link
<br>
"Ch. 11 & 13 - Review of IAF, Solids and Solubility" in the
"notes" section of
<br>
the course web page.
<br>
<br>
<a
href="https://cbc-wb01x.chemistry.ohio-state.edu/%7Erzellmer/chem1220/notes/ch11_12_13_rev.htm"><b>Ch.
11/12 & 13 - Review of IAF, Solids & Solubility</b></a><br>
<br>
Section 13.4:
<br>
<br>
concentration units (know definitions, how to calculate them, how to
use them
<br>
as conversion factors in problems and how to convert from one conc.
unit to
<br>
another - see my examples in the notes and on the class web page on
the easiest
<br>
way to approach these types of problems).
<br>
<br>
Sections 13.5-13.6:
<br>
<br>
Make sure you can do colligative property calculations, including
<br>
for ionic substances or ionizing molecular substances (things that
<br>
dissociate or ionize to give multiple particles, NaCl, HCl, etc.).
<br>
Know what the van't Hoff factor is (effective # particles or
<br>
observed "i" - see "A Closer Look" on page 540, 12th ed.,
<br>
554, 11th ed., page 557, 10th ed. and my notes). Look at the
<br>
link I have about colligative properties under the "Helpful Tidbits"
<br>
link,
<br>
<br>
<a
href="https://cbc-wb01x.chemistry.ohio-state.edu/%7Erzellmer/chem1220/faq/collig_prop.txt"><b>Colligative
Properties</b></a> <br>
<br>
which was e-mailed earlier.
<br>
<br>
Understand how osmosis effects cells.
<br>
<br>
Finally, you should understand what colloids are and how you tell
<br>
whether you have a colloid or a solution (Tyndall effect). Also,
you
<br>
should know the difference between hydrophilic and hydrophobic
colloids.
<br>
<br>
You should review section 2.7-2.8 on ions,
<br>
their charges and polyatomic ions, which stay together as a
<br>
single unit when an ionic compound dissolves. Also, review sections
<br>
4.1-4.3 which deal with electrolytes and nonelectrolytes in solution
<br>
and acid/base reactions. Look at tables 4.2 and 4.3 in relation to
<br>
strong and weak acids and bases.
<br>
<br>
You should be able do to homework problems 13.1-13.114
<br>
<br>
If you are using the 12th edition do homework problems 13.1-13.113
<br>
<br>
If you are using the 11th edition do homework problems 13.1-13.112
<br>
<br>
If you are using the 10th edition do homework problems 13.1-13.107
<br>
<br>
<br>
<br>
Sections 14.1-14.3:
<br>
<br>
Know what rate is and how it is related to concentration (rate law).
<br>
Know what a rate law is and how you can use it, what the order is,
rate
<br>
constant, etc. Know how reaction rates and stoichiometry are
related and
<br>
how the rates of disappearance of reactants and appearance of
products can
<br>
be related to each other and the rate of the reaction (using the
balanced
<br>
equation).
<br>
<br>
Know how to obtain a rate from data and how to use rate data to
determine
<br>
the rate law using the method of initial rates. This is shown in
the book
<br>
in sample ex 14.6 (and the practice exercise) and my notes. You
really need
<br>
to learn how to do this using the second example I used in lecture
(the long
<br>
one). If you don't you will have problems with some of the
end-of-chapter
<br>
exercises (especially the last one for section 14.3).
<br>
<br>
Remember, rate laws can depend on concentration of reactants,
products and
<br>
catalysts. The orders of substances in the rate law can be whole
numbers,
<br>
simple fractions, negative (usually seen for products and
inhibitors). To
<br>
get the overall order you simply add the orders for everything in
the rate
<br>
law. Also, remember in general you can't write the rate law from
the balanced
<br>
chemical equation. It must be determined experimentally. The ONLY
time you
<br>
can write a rate law from a balanced eqn is if you know the reaction
is an
<br>
elementary reaction (a single-step mechanism) and you don't know
this by
<br>
simply looking at the reaction.
<br>
<br>
You should be able do to homework problems 14.1-14.5, 14.17-14.38,
<br>
14.89-14.94, 14.117
<br>
<br>
For those of you using the 12th edition the quiz covers sections
14.1-14.3 and
<br>
homework problems 14.1-14.6, 14.17-14.38, 14.97-14.100, 14.119
<br>
<br>
For those of you using the 11th edition the quiz covers sections
14.1-14.3 and
<br>
homework problems 14.1-14.4, 14.13-14.34, 14.83-14.86, 14.104
<br>
<br>
For those of you using the 10th edition the quiz covers sections
14.1-14.3 and
<br>
homework problems 14.1-14.5, 14.11-14.44, 14.81-14.89, 14.98
<br>
<br>
<br>
Dr. Zellmer
</body>
</html>