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<p class="MsoNormal"><span style="font-family:"Arial",sans-serif">Someone asked me about what they needed to know about<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-family:"Arial",sans-serif">solids and where to find the information.<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-family:"Arial",sans-serif"><o:p> </o:p></span></p>
<p class="MsoNormal"><span style="font-family:"Arial",sans-serif">This is sections 11.7 and 11.8 in the 10th and 11th editions and
<br>
this same material from the 11th edition is on Carmen for those using<br>
the 12th - 14th editions. Remember, no matter which edition<br>
you're using we are not using chapter 12.<br>
<br>
I covered the primitive(simple), body-centered and face-centered <br>
cubic structures. I gave a lot of info about these (# particles/<span class="SpellE">uc</span>,
<br>
how the particles touch, relationship between edge-length and radius, <br>
coordination number, % empty space, type of holes the particles <br>
are in, etc.). I also covered close-packing of spheres and we saw <br>
a non-cubic type of packing (Hexagonal close-packing, hcp) and learned <br>
the cubic-close packed (<span class="SpellE">ccp</span>) structure is the same as a
<span class="SpellE">fcc</span> structure. <br>
All of this discussion was for identical particles in the <span class="SpellE">u.c.</span> (i.e. same
<br>
size, like all Fe atoms, all CO2 molecules, etc.) <br>
<br>
This was all covered in section 11.7 in the 10th and 11th editions <br>
Some of this is summarized in the following link (found at the "Notes"<br>
link on my web page):<br>
<br>
<a href="https://www.asc.ohio-state.edu/zellmer.1/chem1250/notes/unit_cell_table.pdf"><b>Chapter 11/12 - Unit Cell Table for Identical Sized Particles</b></a><br>
<br>
I covered the NaCl structure in detail and a few things about three<br>
other ionic crystal structures.<br>
<br>
In the 10th and 11th editions the structure of NaCl is discussed in <br>
section 11.7 and <span class="SpellE">CsCl</span>, ZnS and CaF2 are discussed in section 11.8.
<br>
For the 12th - 14th editions use what's on Carmen (from the 11th ed.).<br>
<br>
NaCl is described as a face-centered cubic unit cell. The problem is<br>
it doesn't look like the <span class="SpellE">fcc</span> unit cell described for a substance in which<br>
all particles are identical. I explained why it is called a <span class="SpellE">
fcc</span> structure and<br>
how it differs from the <span class="SpellE">fcc</span> unit cell for identical sized particles in lecture.<br>
For NaCl understand the unit cells and related information given in class,<br>
notes and the textbook for NaCl. This includes its structure, placement<br>
of the ions, how anions and cations touch (along an edge), relationship<br>
between edge length and radii of the ions, number of nearest neighbors<br>
and what they are, for both the cation and anion, type of "hole" each ion<br>
"sits" in, unit cell calculations, etc. I don't generally refer to NaCl as<br>
face-centered but call it the "NaCl structure". So in a problem I might state<br>
something like "the substance has an NaCl like structure". You should<br>
know what that means.<br>
<br>
For <span class="SpellE">CsCl</span>, ZnS and CaF2 you should know where the atoms are in the
<span class="SpellE">u.c.</span><br>
and the number of formula units in a unit cell.<br>
<br>
In doing unit cell calc. for ionic structures you must know how many<br>
formula units there are in a unit cell (e.g. NaCl, ZnS and CaF2 all have<br>
4 <span class="SpellE">f.u</span>. per unit cell, <span class="SpellE">CsCl</span> has 1 fu/<span class="SpellE">uc</span>). For
<span class="SpellE">CsCl</span>, ZnS and CaF2 you only<br>
need to know the # fu/<span class="SpellE">uc</span>. I've included a link to a table with all the<br>
information for these 4 ionic structures. You should know what's listed<br>
for NaCl. For the other 3 ionic crystal structures just know the placement<br>
of the ions and the #fu/uc. You can find what you need for these ionic<br>
structures marked in <b><span style="color:red">RED</span></b> at the following link (found at the "Notes" link on<br>
my web page):<br>
<br>
<a href="https://www.asc.ohio-state.edu/zellmer.1/chem1250/notes/ionic_unit_cell_table_filled.pdf"><b>Chapter 11/12 - Unit Cell Table for Ionic Structures (know stuff in red)</b></a><br>
<br>
Furthermore, I would highly suggest using dimensional analysis to <br>
do unit-cell calculations rather than the way shown in the book. I<br>
did them this way in class and I think in the long run it makes them <br>
easier. You will find you can do the <span class="SpellE">uc</span> calc. for ionic structures in the
<br>
same way as you do for atoms or molecules if you think in terms of <br>
"formula-units" (<span class="SpellE">f.u</span>.) for the ionic compounds. NaCl is the "formula unit"
<br>
for sodium chloride. You treat it just as if it were a molecule. For <br>
CO2, which is a <span class="SpellE">fcc</span> structure, you have 4 CO2 molecules per
<span class="SpellE">u.c.</span> and <br>
for NaCl you have 4 NaCl <span class="SpellE">f.u</span>. per <span class="SpellE">
u.c.</span> Thus, you can do a density<br>
calculation the same way for CO2 and NaCl as you would for something<br>
like the Ag example I did in class (using the MW for CO2 or the formula wt. <br>
for NaCl and the number of particles/<span class="SpellE">uc</span> in the same way you would use
<br>
the atomic wt. and # atoms/<span class="SpellE">uc</span> for an atom like Ag). <br>
<br>
For unit cell calculations you should be able determine the following:<br>
<br>
1) density (g/cm^3)<br>
2) volume (cm^3/<span class="SpellE">uc</span>) - includes edge length and particle radius<br>
3) AW, MW, FW (g/mol)<br>
4) unit cell type (<span class="SpellE">sc</span>, bcc, <span class="SpellE">
fcc</span>) - (#particles/uc)<br>
5) Avogadro's Number (#particles/mol)<br>
<br>
I've included the units you're after when doing these problems using<br>
dimensional analysis. This includes calculations for ionic structures<br>
(particle radius for just NaCl). <br>
<br>
There is a web site where you can look at these structures in 3-D and<o:p></o:p></span></p>
<p class="MsoNormal"><span style="font-family:"Arial",sans-serif">rotate them around.<br>
<br>
<a href="http://undergrad-ed.chemistry.ohio-state.edu/xtal/index.html">http://undergrad-ed.chemistry.ohio-state.edu/xtal/index.html</a><br>
<br>
Once there, click on "Crystal Structures" at the bottom. At the top of<br>
the page which comes up you can load the structures for a single type<br>
of particle (<span class="SpellE">sc</span>, bcc, <span class="SpellE">fcc</span>) using the "Bravais Lattices" drop down box or<br>
the ionic structures using the "Other Compounds" drop down box.<br>
<br>
It's easiest to understand things if you click the "All atoms" button. <br>
Ask for more than 1 unit cell when trying to see the nearest neighbors <br>
(<span class="SpellE">coord</span>. #). Also, for the ionic compounds it's much easier to see the
<br>
nearest neighbors if you click on "Connect Atoms" toward the bottom <br>
of the window (you sometimes have to click it twice). <br>
<br>
Also, look at the links I have for <span class="SpellE">ch</span> 11/12 ("Notes" link). I have the three<br>
unit cell calculation examples done in lecture. The table given in the notes<br>
with the info about the unit cells for identical particles (including packing) and<br>
a table for the 4 ionic structures in the notes (with the info you should know<br>
in <span style="color:red">red</span>). The links for these last two things were given above.<br>
<br>
Also, look at the last page of the chapter 11 (12) notes. You will find a table<br>
summarizing the 4 types of solids and their properties. This can be found<br>
on my class web page ("Notes" link),<br>
<br>
<a href="https://www.asc.ohio-state.edu/zellmer.1/chem1250/notes/Table_13-10_solids_no_lines.pdf"><b>Types of Solids and Their Properties</b></a><br>
<br>
<br>
I hope this makes sense. <br>
<br>
Dr. Zellmer <o:p></o:p></span></p>
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