Quiz 1 material (ch 13, 14.1-14.3)

[robert zellmer]

Quiz 1 will cover the following:  Chapter 13 (13.1-13.6) and Sections 
14.1-14.3

This is pretty much up through this past Monday. The only thing from today's
(Wed.) lecture is section 14.3 (the initial rate problems, we'll finish the
2nd example tomorrow).   For the most part that's how coverage on quizzes
will be, Wed, Fri of one week and Mon of the next week, with maybe a small
amount from the 2nd Wed.  This quiz covers last week's material, this past
Monday's and 1 example from section 14.3 from today.

Section 13.1:

Understand the solution process and energy diagrams, how solutions form,
ideal, endothermic and exothermic solution formation and the importance
of entropy in solution formation.  In general, when things mix there is
an inc. in entropy (disorder) but this is not always the case. An inc.
in entropy is absolutely necessary for an ideal or endothermic solution
to form.  This is not the case for an exothermic process.  An exothermic
process already tends to be spont. so an inc. in entropy is not necessary
for this type of solution to form.  There are cases in which the 
delta(H)_soln
is negative (exothermic) and the entropy decreases (solution is more 
ordered)
and the solution forms.  Also, understand the role of attractive forces
between particles in solution formation.

In the 12th-14th editions the delta(H)_solvation is referred to as the
the delta(H)_mix.  This is step 3 (solute-solvent att. forces step),
the exothermic step in the solution process as seen in my figures in the
notes and Figure 13.4.  The book doesn't show an ideal solution figure but
I have it in the notes.

I also have a link showing the solution enthalpy diagrams including a
discussion about the attractive forces and entropy, "Ch. 13 - Solution
Formation and Solubility Effects" in the "Notes" section of the course web
page.

*Ch. 13 - Solution Formation and Solubility Effects* 
<https://cbc-wb01x.chemistry.ohio-state.edu/%7Erzellmer/chem1220/notes/ch13_soln_formation.pdf> 


Section 13.2:

Solubility, saturated, unsaturated and supersaturated solutions.

Section 13.3:

Factors affecting solubility - Att. forces ("like dissolves like"), 
pressure
and temp. affects. You're considering temp. effects and "like dissolves 
like"
concepts in exp 1 (SOL).

I have summary on line about attractive forces and solubility. See the link
below in the "Notes" section of my course web page.

*Ch. 11/12 & 13 - Review of IAF, Solids & Solubility* 
<https://cbc-wb01x.chemistry.ohio-state.edu/%7Erzellmer/chem1220/notes/ch11_12_13_rev.htm>


Section 13.4:

concentration units (know definitions, how to calculate them, how to use 
them
as conversion factors in problems and how to convert from one conc. unit to
another - see my examples in the notes and on the class web page on the 
easiest
way to approach these types of problems).

Sections 13.5-13.6:

Make sure you can do colligative property calculations, including
for ionic substances or ionizing molecular substances (things that
dissociate or ionize to give multiple particles, NaCl, HCl, etc.).
Know what the van't Hoff factor is (effective # particles or
observed "i" - see "A Closer Look" on page 551, 14th ed., page 558,
13th ed., page 540, 12th ed., 554, 11th ed., page 557, 10th ed.
and my notes).  Look at the link I have about colligative properties
under the "Helpful Tidbits" link,

*Colligative Properties* 
<https://cbc-wb01x.chemistry.ohio-state.edu/%7Erzellmer/chem1220/faq/collig_prop.txt> 


which was e-mailed earlier.  It discusses colligative properties and
"i" (the van't Hoff factor).

Understand how osmosis effects cells.

Finally, you should understand what colloids are and how you tell
whether you have a colloid or a solution (Tyndall effect). Also, you
should know the difference between hydrophilic and hydrophobic colloids.

You should review Ch 11 material.  Review section 2.7-2.8 on ions,
their charges and polyatomic ions, which stay together as a single unit
when an ionic compound dissolves.  Also, review sections 4.1-4.3 which
deal with electrolytes and nonelectrolytes in solution and acid/base 
reactions.
Look at tables 4.2 and 4.3 in relation to strong and weak acids and bases.

*Homework coverage (you should be able to all problems in the given 
ranges)**:*

For those of you using the 14th edition the quiz covers sections 13.1-13.6
You should be able do to homework problems 13.1-13.114

For those of you using the 13th edition the quiz covers sections 13.1-13.6
You should be able do to homework problems 13.1-13.114

For those of you using the 12th edition the quiz covers sections 13.1-13.6
You should be able do to homework problems 13.1-13.113

For those of you using the 11th edition the quiz covers sections 13.1-13.6
You should be able do homework problems 13.1-13.112

*For the on-line homework:**
*
Do ch 11 tutorial as a review.  Do ch 13 homework.  Remember there
are the DSM questions and review problems for Ch 13 (plus a tutorial
which isn't for credit).


Sections 14.1-14.3:

Know what rate is and how it is related to concentration (rate law).
Know what a rate law is and how you can use it, what the order is, rate
constant, etc.  Know how reaction rates and stoichiometry are related and
how the rates of disappearance of reactants and appearance of products can
be related to each other and the rate of the reaction (using the balanced
equation).

Know how to obtain a rate from data and how to use rate data to determine
the rate law using the method of initial rates.  This is shown in the book
in sample ex 14.6 (and the practice exercise) and my notes.  You really 
need
to learn how to do this using the second example I used in lecture (the 
long
one).  If you don't you will have problems with some of the end-of-chapter
exercises (especially the last one for section 14.3).

Remember, rate laws can depend on concentration of reactants, products and
catalysts.  The orders of substances in the rate law can be whole numbers,
simple fractions, negative (usually seen for products and inhibitors).  To
get the overall order you simply add the orders for everything in the rate
law.  Also, remember in general you can't write the rate law from the 
balanced
chemical equation.  It must be determined experimentally.  The ONLY time 
you
can write a rate law from a balanced eqn is if you know the reaction is an
elementary reaction (a single-step mechanism) and you don't know this by
simply looking at the reaction.

*Homework coverage (you should be able to all problems in the given 
ranges)**:**
**
*For those of you using the 14th edition the quiz covers sections 14.1-14.3
You should be able do to homework problems 14.1-14.5, 14.17-14.38,
14.89-14.94, 14.117

For those of you using the 13th edition the quiz covers sections 14.1-14.3
You should be able do to homework problems 14.1-14.5, 14.17-14.38,
14.89-14.94, 14.117

For those of you using the 12th edition the quiz covers sections 14.1-14.3
You should be able do to homework problems 14.1-14.6, 14.17-14.38,
14.97-14.100, 14.119

For those of you using the 11th edition the quiz covers sections 14.1-14.3
You should be able do to homework problems 14.1-14.4, 14.13-14.34,
14.83-14.86, 14.104

*For the on-line homework:**
*
Do ch 14 homework. Remember there are the DSM questions and review
problems for Ch 14 (plus a tutorial which isn't for credit).


Dr. Zellmer
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