more notes and stuff

15 files changed, 1480 insertions, 920 deletions

diff --git a/cer/.DS_Store b/cer/.DS_Store
index 6ce9082..24c39b5 100644
--- a/cer/.DS_Store
+++ b/cer/.DS_Store
diff --git a/cer/sem2/cer.tex b/cer/sem2/cer.tex
index c8331ef..a55a489 100644
--- a/cer/sem2/cer.tex
+++ b/cer/sem2/cer.tex
@@ -1,4 +1,5 @@
-\font\tinyx=cmr8 at 6pt \font\tinym=cmmi8 at 6pt \font\tinyms=cmsy8 at 6pt \def\tiny{\tinym \tinyms \tinyx \baselineskip=6pt}
+\font\tinyx=cmr8 at 6pt \font\tinym=cmmi8 at 6pt \font\tinyxs=cmmi8 at 5pt \font\tinyms=cmmi8 at 5pt
+\def\tiny{\textfont0=\tinyx \textfont1=\tinym \scriptfont0=\tinyxs \scriptfont1=\tinyms \tinyx \baselineskip=6pt}
 \font\headx=cmb8 at 9pt \font\headm=cmmi8 at 9pt \font\headms=cmsy8 at 9pt \def\head{\headm \headms \headx \baselineskip=9pt}
 %\font\bigx=cmb14        \font\bigm=cmmi14        \font\bigms=\def\big{\bigx \bigm \baselineskip=14pt}
 
@@ -60,18 +61,6 @@
   \def\preamb{#1}
 }
 
-%\def\cp#1{#1}
-%\def\preambloop{
-%  & \vrule \text{##}
-%  \advance \@columns by -1
-%  \ifnum \@columns>0 \span\preambloop \fi
-%}
-%\def\makepreamb{
-%  \vrule width 1pt \text{##}
-%  \advance \@columns by -1
-%  \ifnum \@columns>0 \span\preambloop \fi
-%  \vrule width 1pt \cr
-%}
 
 \def\makedata{
   \def\text##1{\tiny \tolerance=10000 \hbadness=10000 \hbox to \@tablewidth{\hskip1em \vbox{\vskip1ex \noindent \advance \@tablewidth by -2.25em \hsize\@tablewidth ##1 \smallskip} \hskip1em} }
@@ -88,8 +77,9 @@
   \column{7.4in}{
     \item{\pad{{\bf Question:} \@question}}
     \item{\pad{{\bf Claim:} \@claim}}
+    \item{\smallskip{\bf Data:}\par\noindent\makedata}
     \item{\row{3.6015in}{2}{
-      \item{ {\bf Evidence:}\par \noindent\makedata\par\smallskip \@evidence \smallskip}
+      \item{ {\bf Evidence:}\par \@evidence \smallskip}
       \item{ {\bf Justification (Reasoning) of the Evidence:} \par\@justification \smallskip }
     }}
   }
diff --git a/cer/sem2/enthalpy/cer.log b/cer/sem2/enthalpy/cer.log
new file mode 100644
index 0000000..5fa8d3a
--- /dev/null
+++ b/cer/sem2/enthalpy/cer.log
@@ -0,0 +1,17 @@
+This is pdfTeX, Version 3.14159265-2.6-1.40.20 (TeX Live 2019) (preloaded format=pdftex 2019.5.8)  3 JUL 2019 23:03
+entering extended mode
+ restricted \write18 enabled.
+ %&-line parsing enabled.
+**../cer.tex
+(../cer.tex)
+*\see
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+<*> \see
+        
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diff --git a/cer/sem2/enthalpy/enthalpy.log b/cer/sem2/enthalpy/enthalpy.log
new file mode 100644
index 0000000..64810f7
--- /dev/null
+++ b/cer/sem2/enthalpy/enthalpy.log
@@ -0,0 +1,24 @@
+This is pdfTeX, Version 3.14159265-2.6-1.40.20 (TeX Live 2019) (preloaded format=pdftex 2019.5.8)  4 JUL 2019 00:01
+entering extended mode
+ restricted \write18 enabled.
+ %&-line parsing enabled.
+**enthalpy.tex
+(./enthalpy.tex (../cer.tex) [1{/usr/local/texlive/2019/texmf-var/fonts/map/pdf
+tex/updmap/pdftex.map}] [2] ) </Users/benrohrer/Library/texlive/2019/texmf-var/
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diff --git a/cer/sem2/enthalpy/enthalpy.pdf b/cer/sem2/enthalpy/enthalpy.pdf
new file mode 100644
index 0000000..205098b
--- /dev/null
+++ b/cer/sem2/enthalpy/enthalpy.pdf
diff --git a/cer/sem2/enthalpy/enthalpy.tex b/cer/sem2/enthalpy/enthalpy.tex
new file mode 100644
index 0000000..a98e9fa
--- /dev/null
+++ b/cer/sem2/enthalpy/enthalpy.tex
@@ -0,0 +1,61 @@
+\input ../cer.tex
+
+\name{Holden Rohrer}
+\course{FVS Chemistry AB 19.3}
+\teacher{Kerr} 
+
+\long\def\makedata{
+  \dimendef\tablewidth=1
+  \def\text##1{\tiny \hbadness=10000 \tolerance=10000 \hbox to \tablewidth{\hskip1em \vbox{\smallskip \noindent \advance \tablewidth by -2.25em \hsize\@tablewidth ##1 \smallskip} \hskip1em}}
+  \def\htext##1{\head \hbadness=10000 \tolerance=10000 \hbox to \tablewidth{\hskip0.5em \vbox{\smallskip \noindent \advance \tablewidth by -1.25em \hsize\@tablewidth ##1 \smallskip} \hskip0.5em}}
+  \def\thickline{\noalign{\hrule height 1pt}} 
+  \def\endliner{\noalign{\hrule height 0.05pt}}
+  \smallskip
+  \tablewidth=1in
+  \def\salign##1{\hbox{\quad \vbox{\smallskip \halign{##1} \smallskip}}}
+  \salign{\tablewidth 5in \vrule width 1pt \text{##} & \vrule width 0.05pt \text{##} & \vrule width 0.05pt \text{##} \vrule width 1pt \cr
+    \thickline
+    \omit \tablewidth 5in \vrule width 1pt \htext{Measurement} & \omit \vrule width 0.05pt \htext{Reaction 1 ($Mg + HCl$)} & \omit \vrule width 0.05pt \htext{Reaction 2 ($MgO + HCl$)} \vrule width 1pt \cr \endliner
+    Mass of HCl (g) & 100.50 & 100.57 \cr \endliner
+    Mass of solid (g) & 0.20 & 1.57 \cr \endliner
+    Total mass of reactants, m (g) & 100.70 & 102.14 \cr \thickline
+    Initial temperature ({\tinym $^{\circ}C$}) & 22.5 & 22.7 \cr \endliner
+    Temperature furthest from initial temperature ({\tinym $^{\circ}C$}) & 31.3 & 30.2 \cr \endliner
+    {\tinym $\Delta T$} ({\tinym $^{\circ}C$}) & 8.8 & 7.5 \cr \thickline
+    Heat released, {\tinym $q=cm\Delta T$} (J) & 3700 & 3200 \cr \endliner
+    Moles of solid reactant (mol) & 0.00823 & 0.0397 \cr \endliner
+    Enthalpy of reaction, {\tinym $\Delta H = {{-q}\over{mol}}*{{kJ}\over{1000J}}$} (kJ/mol) & -450 & -81 \cr \thickline
+  }
+  Combination of $\Delta H_1$, $\Delta H_2$, and $\Delta H_3$ needed (using Hess's Law): $\Delta H_{rxn} = -655{{kJ}\over{mol}}$
+
+  \smallskip
+  \tablewidth 3.5in
+  \salign{\vrule width 1pt \text{##} & \vrule width 0.05pt \text{##} \vrule width 1pt \cr \thickline
+    \omit \vrule width 1pt \htext{Reaction Equation} & \omit \vrule width 0.05pt \htext{$\Delta H$ (kJ/mol)} \vrule width 1pt \cr \endliner
+    Reaction 1: $Mg(s) + 2HCl(aq) \longrightarrow MgCl_2(aq)+H_2(g)$ & -450 \cr \endliner
+    Reaction 2: $MgO(s) + 2HCl(aq) \longrightarrow MgCl_2(aq)+H_2O(l)$ & -81 \cr \endliner
+    Reaction 3: $H_2(g) + {{1}\over{2}}O_2(g) \longrightarrow H_2O(l)$ & -286 (published value) \cr \thickline
+    Magnesium Combustion: $Mg(s)+{{1}\over{2}}O_2(g) \longrightarrow MgO(s)$ & -655 \cr \thickline
+  }
+  The published value for this reaction is -603 kJ/mol. Percent error of experimental value: 8.62\%
+  \smallskip
+}
+
+\question{How can you use Hess's Law to determine a reaction's enthalpy when you can't do so using a calorimeter?}
+\claim{Hess's Law accurately describes the enthalpy of an unknown reaction where other reactions' enthalpies (such that those reactions can be summed to the unknown reaction) are known.}
+
+\evidence{
+\def\enthunit{{{kJ}\over{mol}}}
+This experiment measured two chemical reactions, but three were used based off of commonly known values. The first of these is $Mg(s)+2HCl(aq) \longrightarrow MgCl_2(aq) + H_2(g)$. The enthalpy of this reaction was measured and recorded accurately because HCl was in excess, so the only limiting factor was the metal ($Mg$), of which the weight and molar mass was known. $\Delta T$ was also determined, and because a coffee cup calorimeter was used, that was able to be converted into released energy ($q$). The same process was completed for the dissolution of $MgO$ in $HCl$ by the reaction $MgO + 2HCl(aq) \longrightarrow MgCl_2(aq) + H_2O(l)$. Their respective enthalpies of reaction were $-450\enthunit$ and $-81\enthunit$. The third previously known reaction was the combination of gaseous diatomic hydrogen and oxygen into water. This reaction is impossible to conduct with our tools because it requires a bomb calorimeter to contain the gaseous components. Its enthalpy of reaction was $-286\enthunit$.
+
+From these, the reversal of the second reaction provided $H_2O(l)+MgCl_2(aq) \longrightarrow MgO(s)+2HCl(aq)$ at an enthalpy of $81\enthunit$. This allowed the ``cancelling'' of hydrochloric acid, magnesium chloride, hydrogen, and water when summing the chemical equations. After summation, we are left with $Mg(s) + {{1}\over{2}}O_2(g) \longrightarrow MgO(s)$ at a total enthalpy of $-450-(-81)-286=-450+81-286=-655\enthunit$ by Hess's Law. Because this is so similar to the previously published value of $-603 \enthunit$ (an experimental error of $8.62\%$, well within bounds of statistical significance), it can be considered to be an accurate measure of the enthalpy of the reaction (specifically magnesium combustion; however, this generalises).
+}
+
+\justification{
+Hess's Law's accuracy makes sense because it's logically consistent with enthalpy's property of being a state function. Starting with the assumed 0 enthalpy of elements in their standard form, most bonds release energy, and by conservation of energy, they must have proportionately lower potential energy. This is the energy of formation and is constant between all samples of a substance. In order for energy to be conserved during non-formation or -decomposition chemical reactions, the potential energy difference between products and reactants (enthalpy) must be equal to energy released. This is the foundation of Hess's Law: the known enthalpy amounts allow given compounds' enthalpies of formation to be treated like variables (because enthalpy of formation is an intrinsic property determined only by the identity of the substance and is identical between all samples of the substance) and thus the chemical equations summed like linear equations. This demonstrates the generality of the specific magnesium combustion example shown here.
+}
+
+\makeheader
+\vfil
+\makedoc
+\bye
diff --git a/cer/sem2/enthalpy/rate.tex b/cer/sem2/enthalpy/rate.tex
new file mode 100644
index 0000000..00e010d
--- /dev/null
+++ b/cer/sem2/enthalpy/rate.tex
@@ -0,0 +1,60 @@
+\input ../cer.tex
+
+\name{Holden Rohrer}
+\course{FVS Chemistry AB 19.3}
+\teacher{Kerr (sorry about the stretched out formatting; the writing just wouldn't fit)}
+
+\question{What are the effects of temperature and a reactant's particle size on reaction rate?}
+\claim{If you increase the temperature of a reaction, then the reaction rate will increase because particles experience more collisions at higher temperatures.
+
+{\bf Claim 2:} If you decrease the particle size of a reactant, then the reaction rate will increase because more of the reactants' surface area is exposed allowing more particles to make contact with eachother.}
+
+\long\def\makedata{
+  \dimendef\tablewidth=1
+  \def\text##1{\tiny \hbadness=10000 \tolerance=10000 \hbox to \tablewidth{\hskip1em \vbox{\smallskip \noindent \advance \tablewidth by -2.25em \hsize\@tablewidth ##1 \smallskip} \hskip1em}}
+  \def\htext##1{\head \hbadness=10000 \tolerance=10000 \vrule width 0.05pt \hbox to \tablewidth{\hskip0.5em \vbox{\smallskip \noindent \advance \tablewidth by -1.25em \hsize\@tablewidth ##1 \smallskip} \hskip0.5em}}
+  \def\style{\vrule width 1pt \htext{####} & \vrule width 0.05pt \text{####} & \vrule width 0.05pt \text{####} & \vrule width 0.05pt \text{####} & \vrule width 0.05pt \text{####} & \vrule width 0.05pt \text{####} \vrule width 1pt \crcr
+    \noalign{\hrule height 1pt}
+    \omit \vrule width 1pt \text{Trials} & \omit \htext{\fsub} & \omit \htext{Mass of Tablet ($mg$)} & \omit \htext{Volu\-me of Water ($L$)} & \omit \htext{Reac\-tion Time ($s$)} & \omit \htext{Reac\-tion Rate (${{mg}\over{L}}\over{s}$)} \vrule width 1pt \cr \endliner
+  }
+  \def\endliner{\noalign{\hrule height 0.05pt}}
+  \qquad Table A: Variation of Temperature
+  \smallskip
+  \tablewidth=0.55in
+  \def\fsub{Meas\-ured Reaction Temperature ($^{\circ}C$)}
+  \halign{\span\style
+    $\approx 20^{\circ}C$ & $24^{\circ}C$ & 1,000 & 0.2 & 34.2 & 146 \cr \endliner
+    $\approx 40^{\circ}C$ & $40^{\circ}C$ & 1,000 & 0.2 & 26.3 & 190 \cr \endliner
+    $\approx 65^{\circ}C$ & $65^{\circ}C$ & 1,000 & 0.2 & 14.2 & 352 \cr \endliner
+    $\approx 5^{\circ}C$ & $3^{\circ}C$ & 1,000 & 0.2 & 138.5 & 36 \cr
+    \noalign{\hrule height 1pt}
+  }
+  \bigskip
+  \qquad Table B: Variation of Particle Size (All at Room Temperature)
+  \smallskip
+  \def\fsub{Relat\-ive Particle Size (Small , Med\-ium, Large)}
+  \halign{\span\style
+    Full Tablet & Large & 1000 & 0.2 & 34.5 & 145 \cr \endliner
+    Eight Pieces & Medium & 1000 & 0.2 & 28.9 & 173 \cr \endliner
+    Tiny Pieces & Small & 1000 & 0.2 & 23.1 & 216 \cr
+    \noalign{\hrule height 1pt}
+  }
+  
+}
+
+\evidence{
+  The first claim is proven true by the evidence because the reaction rates do, in fact, increase with increasing temperatures. This is seen in the similar ordering of trials across both features. The temperatures ($T_k$ is the temperature of the $k$th trial) are, in order: $T_4 < T_1 < T_2 < T_3$. The reaction rates are, by a similar convention, $R_4 < R_1 < R_2 < R_3$. This clearly shows correlation of the two variables. In each of the trials, potentially confounding variables were controlled for---the mass of the tablet, volume of water in the beaker, and particle size (none of the tablets were crushed).
+  
+  The second claim follows a similar line of reasoning. Table B follows the changes in tablet size by crushing them into larger numbers of pieces (consequently, each piece has a smaller volume and disproportionately larger surface area and total surface area by the square-cube law). The reaction rate is highest for tiny pieces, slightly lower for eight pieces, and lowest for full, uncrushed tablets (as calculated from the increasing reaction times of the trials in the same order). This part of the experiment also controlled for similar variables: temperature was always room temperature as no heating or cooling occurred, and the masses/volumes of reactants were unchanged between trials. 
+}
+
+\justification{
+  Both of these results make sense within the context of collision theory. The temperature increases both the number of collisions because it is the same as kinetic energy and thus average velocities of the particles (faster particles cause more collisions) and it increases the number of effective collisions. The number of effective collisions increase because as the velocity of the particles go up, it becomes far more likely that the kinetic energy of a given collision is above the activation energy of the reaction.
+  
+  The second result can be justified similarly. The more pieces into which the tablet is crushed, the more of the ``internal'' surface area is exposed to the water. The more surface area is exposed to the water, the more chances there are for the water molecules to collide with the antacid's molecules, and the more reactions occur.
+}
+
+\makeheader
+\vfil
+\makedoc
+\bye
diff --git a/cer/sem2/solubility/solubility.tex b/cer/sem2/solubility/solubility.tex
new file mode 100644
index 0000000..a98e9fa
--- /dev/null
+++ b/cer/sem2/solubility/solubility.tex
@@ -0,0 +1,61 @@
+\input ../cer.tex
+
+\name{Holden Rohrer}
+\course{FVS Chemistry AB 19.3}
+\teacher{Kerr} 
+
+\long\def\makedata{
+  \dimendef\tablewidth=1
+  \def\text##1{\tiny \hbadness=10000 \tolerance=10000 \hbox to \tablewidth{\hskip1em \vbox{\smallskip \noindent \advance \tablewidth by -2.25em \hsize\@tablewidth ##1 \smallskip} \hskip1em}}
+  \def\htext##1{\head \hbadness=10000 \tolerance=10000 \hbox to \tablewidth{\hskip0.5em \vbox{\smallskip \noindent \advance \tablewidth by -1.25em \hsize\@tablewidth ##1 \smallskip} \hskip0.5em}}
+  \def\thickline{\noalign{\hrule height 1pt}} 
+  \def\endliner{\noalign{\hrule height 0.05pt}}
+  \smallskip
+  \tablewidth=1in
+  \def\salign##1{\hbox{\quad \vbox{\smallskip \halign{##1} \smallskip}}}
+  \salign{\tablewidth 5in \vrule width 1pt \text{##} & \vrule width 0.05pt \text{##} & \vrule width 0.05pt \text{##} \vrule width 1pt \cr
+    \thickline
+    \omit \tablewidth 5in \vrule width 1pt \htext{Measurement} & \omit \vrule width 0.05pt \htext{Reaction 1 ($Mg + HCl$)} & \omit \vrule width 0.05pt \htext{Reaction 2 ($MgO + HCl$)} \vrule width 1pt \cr \endliner
+    Mass of HCl (g) & 100.50 & 100.57 \cr \endliner
+    Mass of solid (g) & 0.20 & 1.57 \cr \endliner
+    Total mass of reactants, m (g) & 100.70 & 102.14 \cr \thickline
+    Initial temperature ({\tinym $^{\circ}C$}) & 22.5 & 22.7 \cr \endliner
+    Temperature furthest from initial temperature ({\tinym $^{\circ}C$}) & 31.3 & 30.2 \cr \endliner
+    {\tinym $\Delta T$} ({\tinym $^{\circ}C$}) & 8.8 & 7.5 \cr \thickline
+    Heat released, {\tinym $q=cm\Delta T$} (J) & 3700 & 3200 \cr \endliner
+    Moles of solid reactant (mol) & 0.00823 & 0.0397 \cr \endliner
+    Enthalpy of reaction, {\tinym $\Delta H = {{-q}\over{mol}}*{{kJ}\over{1000J}}$} (kJ/mol) & -450 & -81 \cr \thickline
+  }
+  Combination of $\Delta H_1$, $\Delta H_2$, and $\Delta H_3$ needed (using Hess's Law): $\Delta H_{rxn} = -655{{kJ}\over{mol}}$
+
+  \smallskip
+  \tablewidth 3.5in
+  \salign{\vrule width 1pt \text{##} & \vrule width 0.05pt \text{##} \vrule width 1pt \cr \thickline
+    \omit \vrule width 1pt \htext{Reaction Equation} & \omit \vrule width 0.05pt \htext{$\Delta H$ (kJ/mol)} \vrule width 1pt \cr \endliner
+    Reaction 1: $Mg(s) + 2HCl(aq) \longrightarrow MgCl_2(aq)+H_2(g)$ & -450 \cr \endliner
+    Reaction 2: $MgO(s) + 2HCl(aq) \longrightarrow MgCl_2(aq)+H_2O(l)$ & -81 \cr \endliner
+    Reaction 3: $H_2(g) + {{1}\over{2}}O_2(g) \longrightarrow H_2O(l)$ & -286 (published value) \cr \thickline
+    Magnesium Combustion: $Mg(s)+{{1}\over{2}}O_2(g) \longrightarrow MgO(s)$ & -655 \cr \thickline
+  }
+  The published value for this reaction is -603 kJ/mol. Percent error of experimental value: 8.62\%
+  \smallskip
+}
+
+\question{How can you use Hess's Law to determine a reaction's enthalpy when you can't do so using a calorimeter?}
+\claim{Hess's Law accurately describes the enthalpy of an unknown reaction where other reactions' enthalpies (such that those reactions can be summed to the unknown reaction) are known.}
+
+\evidence{
+\def\enthunit{{{kJ}\over{mol}}}
+This experiment measured two chemical reactions, but three were used based off of commonly known values. The first of these is $Mg(s)+2HCl(aq) \longrightarrow MgCl_2(aq) + H_2(g)$. The enthalpy of this reaction was measured and recorded accurately because HCl was in excess, so the only limiting factor was the metal ($Mg$), of which the weight and molar mass was known. $\Delta T$ was also determined, and because a coffee cup calorimeter was used, that was able to be converted into released energy ($q$). The same process was completed for the dissolution of $MgO$ in $HCl$ by the reaction $MgO + 2HCl(aq) \longrightarrow MgCl_2(aq) + H_2O(l)$. Their respective enthalpies of reaction were $-450\enthunit$ and $-81\enthunit$. The third previously known reaction was the combination of gaseous diatomic hydrogen and oxygen into water. This reaction is impossible to conduct with our tools because it requires a bomb calorimeter to contain the gaseous components. Its enthalpy of reaction was $-286\enthunit$.
+
+From these, the reversal of the second reaction provided $H_2O(l)+MgCl_2(aq) \longrightarrow MgO(s)+2HCl(aq)$ at an enthalpy of $81\enthunit$. This allowed the ``cancelling'' of hydrochloric acid, magnesium chloride, hydrogen, and water when summing the chemical equations. After summation, we are left with $Mg(s) + {{1}\over{2}}O_2(g) \longrightarrow MgO(s)$ at a total enthalpy of $-450-(-81)-286=-450+81-286=-655\enthunit$ by Hess's Law. Because this is so similar to the previously published value of $-603 \enthunit$ (an experimental error of $8.62\%$, well within bounds of statistical significance), it can be considered to be an accurate measure of the enthalpy of the reaction (specifically magnesium combustion; however, this generalises).
+}
+
+\justification{
+Hess's Law's accuracy makes sense because it's logically consistent with enthalpy's property of being a state function. Starting with the assumed 0 enthalpy of elements in their standard form, most bonds release energy, and by conservation of energy, they must have proportionately lower potential energy. This is the energy of formation and is constant between all samples of a substance. In order for energy to be conserved during non-formation or -decomposition chemical reactions, the potential energy difference between products and reactants (enthalpy) must be equal to energy released. This is the foundation of Hess's Law: the known enthalpy amounts allow given compounds' enthalpies of formation to be treated like variables (because enthalpy of formation is an intrinsic property determined only by the identity of the substance and is identical between all samples of the substance) and thus the chemical equations summed like linear equations. This demonstrates the generality of the specific magnesium combustion example shown here.
+}
+
+\makeheader
+\vfil
+\makedoc
+\bye
diff --git a/notes/.notes.tex.swp b/notes/.notes.tex.swp
deleted file mode 100644
index dccbbe3..0000000
--- a/notes/.notes.tex.swp
+++ /dev/null
diff --git a/notes/notes.aux b/notes/notes.aux
index e828f40..e245c72 100644
--- a/notes/notes.aux
+++ b/notes/notes.aux
@@ -18,229 +18,261 @@
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diff --git a/notes/notes.out b/notes/notes.out
index b125ffc..b085e71 100644
--- a/notes/notes.out
+++ b/notes/notes.out
@@ -214,3 +214,35 @@
 \BOOKMARK [3][-]{subsubsection.7.3.2}{Calorimetry Definition}{subsection.7.3}% 214
 \BOOKMARK [3][-]{subsubsection.7.3.3}{Bomb Calorimetry}{subsection.7.3}% 215
 \BOOKMARK [3][-]{subsubsection.7.3.4}{The Calorie Content of Foods}{subsection.7.3}% 216
+\BOOKMARK [2][-]{subsection.7.4}{Thermochemical Equations}{section.7}% 217
+\BOOKMARK [3][-]{subsubsection.7.4.1}{Enthalpy}{subsection.7.4}% 218
+\BOOKMARK [3][-]{subsubsection.7.4.2}{Enthalpy of Reaction}{subsection.7.4}% 219
+\BOOKMARK [3][-]{subsubsection.7.4.3}{Manipulating Equations}{subsection.7.4}% 220
+\BOOKMARK [3][-]{subsubsection.7.4.4}{Enthalpy of Combustion}{subsection.7.4}% 221
+\BOOKMARK [2][-]{subsection.7.5}{Enthalpy and Phase Changes}{section.7}% 222
+\BOOKMARK [3][-]{subsubsection.7.5.1}{Heat and Phase Changes}{subsection.7.5}% 223
+\BOOKMARK [3][-]{subsubsection.7.5.2}{Effects of Heat on Phase Changes}{subsection.7.5}% 224
+\BOOKMARK [3][-]{subsubsection.7.5.3}{Relationship between Enthalpy}{subsection.7.5}% 225
+\BOOKMARK [3][-]{subsubsection.7.5.4}{Sweat and Temperature Regulation}{subsection.7.5}% 226
+\BOOKMARK [2][-]{subsection.7.6}{Enthalpy of Reaction}{section.7}% 227
+\BOOKMARK [3][-]{subsubsection.7.6.1}{Equation Combination}{subsection.7.6}% 228
+\BOOKMARK [3][-]{subsubsection.7.6.2}{Diagramming Hess's Law}{subsection.7.6}% 229
+\BOOKMARK [3][-]{subsubsection.7.6.3}{Reaction Energy Diagrams and Enthalpy Diagrams}{subsection.7.6}% 230
+\BOOKMARK [1][-]{section.8}{Mixtures, Solutions, and Solubility}{}% 231
+\BOOKMARK [2][-]{subsection.8.1}{Mixtures and Solutions}{section.8}% 232
+\BOOKMARK [3][-]{subsubsection.8.1.1}{Heterogenous and Homogenous Mixtures}{subsection.8.1}% 233
+\BOOKMARK [3][-]{subsubsection.8.1.2}{Solution}{subsection.8.1}% 234
+\BOOKMARK [3][-]{subsubsection.8.1.3}{Suspensions and Colloids}{subsection.8.1}% 235
+\BOOKMARK [3][-]{subsubsection.8.1.4}{The Tyndall Effect}{subsection.8.1}% 236
+\BOOKMARK [3][-]{subsubsection.8.1.5}{Techniques to Separate Solutions}{subsection.8.1}% 237
+\BOOKMARK [2][-]{subsection.8.2}{Reactions in Aqueous Solutions}{section.8}% 238
+\BOOKMARK [3][-]{subsubsection.8.2.1}{Polarity of Water}{subsection.8.2}% 239
+\BOOKMARK [3][-]{subsubsection.8.2.2}{Ionization}{subsection.8.2}% 240
+\BOOKMARK [3][-]{subsubsection.8.2.3}{State of Matter in Chemical Reactions}{subsection.8.2}% 241
+\BOOKMARK [3][-]{subsubsection.8.2.4}{Double-Displacement Reactions}{subsection.8.2}% 242
+\BOOKMARK [3][-]{subsubsection.8.2.5}{Types of Electrolytes}{subsection.8.2}% 243
+\BOOKMARK [2][-]{subsection.8.3}{Solutions and Solubility}{section.8}% 244
+\BOOKMARK [3][-]{subsubsection.8.3.1}{The Dissolving Process}{subsection.8.3}% 245
+\BOOKMARK [3][-]{subsubsection.8.3.2}{The Rate of Dissolution}{subsection.8.3}% 246
+\BOOKMARK [3][-]{subsubsection.8.3.3}{Solubility}{subsection.8.3}% 247
+\BOOKMARK [3][-]{subsubsection.8.3.4}{Environmental Conditions' Effects on Solubility}{subsection.8.3}% 248
diff --git a/notes/notes.pdf b/notes/notes.pdf
index 6b2c8c9..6b4fdd9 100644
--- a/notes/notes.pdf
+++ b/notes/notes.pdf
diff --git a/notes/notes.tex b/notes/notes.tex
index 61bc1a8..ea8ad9d 100644
--- a/notes/notes.tex
+++ b/notes/notes.tex
@@ -662,7 +662,7 @@ colorlinks=true
 	\subsubsection{Activation Energy}
 	Activation energy ($E_A$) is the minimum amount of energy to initiate a chemical reaction (this is brought on by an increase in free energy of compounds during the reaction---meaning that energy is absorbed by the reaction before the ``hump'' of the activation energy is reached). This is a barrier to the reaction and must be overcome before the reaction will proceed. For all stable compounds, the reaction energy is positive because otherwise they are unstable and decompose readily (the higher the activation energy, the less likely the reaction is to occur and thus more slowly it occurs).
 	\subsubsection{Chemical Bonds}
-	Chemical reactions rearrange atoms in molecules by making and/or breaking bonds. Bonds, as mentioned in previous units, are stable electron configurations---implying that energy must be input to start decomposing or making bonds. Note that energy still must be input to start most spontaneous reactions, but they will continue on their own because energy from previous reactions supplies activation energy for other reactant molecules.
+	Chemical reactions rearrange atoms in molecules by making and/or breaking bonds. Bonds, as mentioned in previous units, are stable electron configur\-ations---implying that energy must be input to start decomposing or making bonds. Note that energy still must be input to start most spontaneous reactions, but they will continue on their own because energy from previous reactions supplies activation energy for other reactant molecules.
 	\subsubsection{Reaction Rate}
 	Reaction rate is how quickly reactants convert to products. This depends inversely on activation energy. High activation energies (like in graphite to diamond reaction) mean low reaction rates, and low activation energies (like baking soda and vinegar) mean very high reaction rates. This is completely unrelated to $\Delta G_{rxn}$.
 	\subsubsection{Collision Theory}
@@ -670,7 +670,7 @@ colorlinks=true
 	\subsubsection{Effective Collisions}
 	Effective Collisions, as mentioned in the previous topic, are necessary (as compared to simply collisions where all possible touching of molecules results in a reaction) for chemical reactions to occur. What contrasts these effective collisions is a high enough kinetic energy and the reactants' facing the correct directions to exchange atoms.
 	\subsubsection{Effect of Concentration on Reaction Rate}
-	Similar to temperature increasing collision rate by increasing pressure/temperature, concentration causes more frequent collisions---increasing the rate of reaction (concentration meaning number of molecules per volume in an aqueous solution, for example).
+	Similarly to temperature increasing collision rate by increasing molecule movement and pressure, increased concentration causes more frequent collis\-ions---increasing the rate of reaction (concentration meaning number of molecules per volume in an aqueous solution, for example).
 	\subsubsection{Effect of Pressure on Reaction Rate}
 	There are 2 other ways to increase pressure other than temperature: increasing the amount of reactants and decreasing volume (which makes sense with the ideal gas law). However, note that increasing the pressure is only useful with reactions exclusively between gases because liquids and solids don't become more dense with higher pressures.
 	\subsubsection{Effects of Surface Area on Reaction Rate}
@@ -750,6 +750,74 @@ colorlinks=true
 	A bomb calorimeter is a specific type of calorimeter which doesn't use a bath of water (solution) for the reaction. Instead, it has a separated vessel inside of a bath of water to measure more reactions. This are often used to measure combustion heat release.
 	\subsubsection{The Calorie Content of Foods}
 	Nutrition information labels give calorie counts (note that a food Calorie is a kilocalorie or $4.184kJ$). These are determined with bomb calorimeters by burning the food and determining heat released during the combustion reaction.
+    \subsection{Thermochemical Equations}
+        \subsubsection{Enthalpy}
+	Bonds contain potential energy, and breaking or forming bonds can release or absorb energy. All reactants and products contain chemical energy. Enthalpy ($H$) measures the heat and internal energy in a system. Enthalpy in a chemical reaction is a state function, a type of function which depends only on the beginning and end of the process (not the middle). This makes sense because enthalpy of reaction is the same if a catalyst is used or not. Enthalpy is also a linear function, so the only important part is the potential energy of the involved reactants and products. This potential energy is called enthalpy of formation ($\Delta H_f$). It is defined relative to the zero-point of an element in a ``standard state'' at STP. Chlorine gas, for example has a $\Delta H_f$ of $0 \frac{kJ}{mol}$.
+	\subsubsection{Enthalpy of Reaction}
+	Enthalpy of a reaction ($\Delta H_{rxn}$) is the energy absorbed (positive) or released (negative) during a chemical reaction. Hess's Law of heat formation states that this property is linear with enthalpy of formation, i.e. the enthalpy of a reaction is the enthalpy of the reactants subtracted from the enthalpy of the products. A thermochemical equation is a chemical equation which includes this information and states of involved substances.
+	\subsubsection{Manipulating Equations}
+	If the direction of a chemical equation is reversed, $\Delta H_{rxn}$ becomes $-\Delta H_{rxn}$. If a chemical equation is multiplied by a coefficient $k$, $\Delta H_{rxn}$ becomes $k\Delta H_{rxn}$. Note that $\Delta H_{rxn}$ typically refers to integer molar amounts of compounds in a balanced chemical equation.
+	\subsubsection{Enthalpy of Combustion}
+	Combustion, another chemical reaction, also has a certain amount of enthalpy. Combustion reactions are typically very formulaic, so the energy of a given combustion reaction (such as burning propane) is known by the scientific community. Note, however, combustion enthalpy can still be determined with standard techniques.
+    \subsection{Enthalpy and Phase Changes}
+        \subsubsection{Heat and Phase Changes}
+	Previously, heating and cooling curves have been described. These are graphs of a substance across temperature and added heat, showing its phase changes. While in different states of matter, substances have different specific heats. While changing between substances, temperature is constant, but energy is not. For melting, the energy to transform a mole of a substance at the melting point, but completely solid, is called the molar heat of fusion ($\Delta H_{fus}$). The heat of fusion can also be given in terms of $\frac{J}{g}$ but is typically provided as $\frac{J}{mol}$. The energy released during the opposite process, freezing, is equal to $-\Delta H_{fus}$. Boiling/vaporizing follows a similar pattern: the molar heat of vaporization is $\Delta H_{vap}$, and the molar heat of condensation (not a real measurement) is $-\Delta H_{vap}$. These can also be given in terms of mass.
+	\subsubsection{Effects of Heat on Phase Changes}
+	During phase changes, temperature doesn't change, so kinetic energy doesn't change. However, heat input has to increase some form of energy, so it increases potential energy---enough so that the movement of the particles overcomes the intermolecular forces. Similar to chemical reactions, potential energy increases during endothermic reactions and decreases during exothermic reactions.
+	\subsubsection{Relationship between Enthalpy}
+	$\Delta H_{vap} > \Delta H_{fus} > 0$
+	\subsubsection{Sweat and Temperature Regulation}
+	Because evaporation is endothermic, the human body uses sweat to cool itself by making sweat evaporate (temperature doesn't increase because no temperature changes occur during phase changes).
+    \subsection{Enthalpy of Reaction}
+        \subsubsection{Equation Combination}
+	By Hess's Law of Heat Formation, chemical equations can be added like linear equations. This is most useful for combined processes (like writing photosynthesis from its component reactions). The goal of combining equations is to write a balanced equation of the products respective to reactants as chosen.
+	\subsubsection{Diagramming Hess's Law}
+	Because enthalpy is a state function, and the potential energy of a given compound or group of compounds is constant, a set of chemical equations can be diagrammed as a set of transformations from one set of compounds (i.e. $2C(s)+H_2(g)$ to $C_2H_2(g)$ is one transformation), and from that, the difference in the final product's potential energy and the reactants is the change in enthalpy. Note also that upwards arrows on the diagram are positive, and downward arrows are negative.
+	\subsubsection{Reaction Energy Diagrams and Enthalpy Diagrams}
+	Reaction energy diagrams and enthalpy diagrams are both ways to describe the change in potential energy of a chemical reaction. Enthalpy diagrams are more detailed in the process, but reaction energy diagrams describe reaction progress with more detail. Also, reaction energy diagrams only display one reaction at a time unlike enthalpy diagrams displaying the total and individual reactions. Both put energy on the vertical axis.
+\section{Mixtures, Solutions, and Solubility}
+    \subsection{Mixtures and Solutions}
+        \subsubsection{Heterogenous and Homogenous Mixtures}
+	As described extensively in previous lessons, homogenous mixtures are approximately congruent between any two arbitrarily chosen volumes, but heterogenous mixtures are not.
+	\subsubsection{Solution}
+	A solution is a type of homogenous mixture which appear as one phase. It has two components: a solvent (the ``dissolver''), and a solute (the ``dissolved'').
+	\subsubsection{Suspensions and Colloids}
+	Suspensions are similar to solutions, but instead of being homogenous they are heterogenous mixtures which have large enough particles to settle out or be filtered out. This includes muddy rivers, milk, and blood. Colloids are a subset of suspensions with significantly smaller particles dispersed in a way that makes it difficult to easily filter or quickly settle.
 
+	A few features of suspensions, colloids, and suspensions can be used to differentiate them. The first of these is Brownian motion: the constant random motion of particles is observed in colloids and solutions but not in suspensions. Quick settling is observed in suspensions by definition but not in most colloids or any solutions.
+	\subsubsection{The Tyndall Effect}
+	The Tyndall Effect differentiates colloids from solutions because they can be easily confused. In colloids, light passing through is scattered by the particles like dust in air or flour in water. This scattering, the Tyndall Effect, notably does not occur in solutions. The scattering of light looks like a coherent beam of light.
+	\subsubsection{Techniques to Separate Solutions}
+	There are a few common techniques to separate solutions. These have been listed before, and include distillation (boiling liquids and collecting the vapor of liquids as they boil at different temperatures), crystallization (vaporizing the solvent to leave the solute(s)), and chromatography (separating solutes by density or particle size).
+
+	Colloids are slightly easier to separate. Centrifuges (spinning the colloid to separate solutes by density with centrifugal force), long standing (leaving the solute to settle out of the solvent), and boiling/heating (heating or running electricity through the colloid to coagulate---thicken to a solid or semisolid---it).
+    \subsection{Reactions in Aqueous Solutions}
+        \subsubsection{Polarity of Water}
+	Water is a highly polar covalent compound. The Oxygen has a partial negative charge, and the Hydrogens/hydrogen end have a partial positive. This makes it better as a dissociative solvent for ionic compounds. Dissociation is when ionic compounds separate into their respective ions with the same charges they have while in the compound. These individual atoms (like $Na^+$ or $Br^-$ from $NaBr$) and their parent compounds (such as $NaBr$) are called electrolytes.
+
+	Dissociation occurs in significant amounts in aqueous solutions because of a process called hydration. Water molecules' partially negative oxygen atoms surround positive ions (cations) like $Na^+$ to help them stay in solution and prevent reassociation. In order to cancel the electric charge, more than one water molecules surround the ions. Similarly, the partially negative hydrogen side surrounds negative ions (anions) like $Cl^-$.
+	\subsubsection{Ionization}
+	Water can also dissolve some covalent compounds by ionizing them---a chemical reaction. For example, sulfur dioxide ($SO_2$, a covalent compound) takes $OH^-$ from the water molecule to make itself a negative ion. This also occurs with ammonia and hydrochloric acid. Note that this, like dissociation, only occurs to water-soluble molecules.
+	\subsubsection{State of Matter in Chemical Reactions}
+	As described in the lesson on chemical equation symbols, symbols like $(g)$ and $(l)$ describe the state of matter of reactants and products (gas and liquid, respectively), and $(aq)$ describes reactants or products dissolved in an aqueous solution. Where insoluble products form (remaining as $(s)$ instead of becoming $(aq)$ like with $AgCl$), gases either bubble out of the solution and solids form precipitates separate from but within the solution.
+	\subsubsection{Double-Displacement Reactions}
+	Double-displacement reactions occur when ions switch places in ionic compounds. These often occur in aqueous solutions, and when they do, ionic compounds in aqueous solution can be represented as their individual ions in aqueous solution (e.g. $NaCl(aq)=Na^+(aq) + Cl^-(aq)$ but $AgCl(s) \neq Ag^+(s) + Cl^-(s)$).
+
+	After these dissociated ions are rewritten, any ion which is on both sides in the same phase can be eliminated (e.g. $H^+(aq) + Cl^-(aq) + Na^+(aq) + OH^-(aq) \longrightarrow Na^+(aq) + Cl^- + H_2O(l)$ becomes $H^+(aq) + OH^- \longrightarrow H_2O(l)$). This is called a net ionic equation. Notably, if all reactants and products are aqueous in a double-displacement reaction, the net ionic equation is empty and thus no real reaction has occurred. This leads us to show that double-displacement reactions in solution occur only when a gas, precipitate, or pure liquid are formed.
+	\subsubsection{Types of Electrolytes}
+	Strong electrolytes and weak electrolytes are the two types of electrolytes. Strong electrolytes dissociate or ionize completely like $HCl(g)$ or $KOH(s)$. This means that they conduct electricity very well when in solution. Weak electrolytes, on the other hand partially dissociate or ionize because their reactions are easily reversible---meaning that a significant amount of reactant is left in the solution. Nonelectrolytes aren't really electrolytes beccause they don't dissociate or ionize in solution. These solutions do not conduct electricity.
+    \subsection{Solutions and Solubility}
+        \subsubsection{The Dissolving Process}
+	Dissolution does not occur instantaneously. It's a process which requires that solute molecules or ions are attracted to solvent molecules, causing the solvent to try and surround the solute. This pulls apart the solute from the other solute molecules, and completes the mixing process. The necessary attraction between solute and solvent is why the ``like dissolves like'' rule tends to accurately describe dissolution of solutions (e.g. water, a highly polar covalent molecule easily dissolves highly polar ionic compounds).
+	\subsubsection{The Rate of Dissolution}
+	The rate of dissolution is how quickly a solid solute dissolves in a liquid solvent. This increases proportionally with stirring, surface area, and temperature.
+	\subsubsection{Solubility}
+	Solubility is the ``amount of solute which will dissolve in a volume of solvent at a given temperature and pressure.'' This changes only with the solute's and solvent's identity. This is different from the dissolution rate and follows the like dissolves like rule significantly.
+
+	The concentration of a solute compared to the maximum concentration based on solubility defines three types of solutions: unsaturated solutions have less solute than the ``maximum,'' saturated solutions have exactly an equal amount, and supersaturated solutions have higher than the maximum. Supersaturated solutions are highly unstable and are typically created by slowly cooling a saturated solution at a higher temperature.
+	\subsubsection{Environmental Conditions' Effects on Solubility}
+	Increasing temperature increases the solubility of solids and liquids but decreases the solubility of gases. Increasing pressure, however, increases the solubility of gases and does not affect the solubility of solids and liquids.
+	
+	Solubility graphs show the change in solubility with temperature. These are determined experimentally because they are different for different solutes. These can be used to determine if a given solution is saturated, unsaturated, or supersaturated at a specific temperature.
 \end{document}
 
diff --git a/notes/notes.toc b/notes/notes.toc
index 04ce7f3..6afb3d7 100644
--- a/notes/notes.toc
+++ b/notes/notes.toc
@@ -1,216 +1,248 @@
-\contentsline {section}{\numberline {Unit I:}Atomic Structure and the Periodic Table}{7}{section.1}% 
-\contentsline {subsection}{\numberline {Lesson 1:}The Historical Development of Atomic Theory}{7}{subsection.1.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.1:}Dalton's Atomic Theory}{7}{subsubsection.1.1.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.2:}Discovery of the Electron}{7}{subsubsection.1.1.2}% 
-\contentsline {subsubsection}{\numberline {Topic 1.3:}Plum Pudding Model}{8}{subsubsection.1.1.3}% 
-\contentsline {subsubsection}{\numberline {Topic 1.4:}Discovery of the Nucleus}{8}{subsubsection.1.1.4}% 
-\contentsline {subsection}{\numberline {Lesson 2:}The Modern Atomic Theory}{8}{subsection.1.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.1:}Theories of Light}{8}{subsubsection.1.2.1}% 
-\contentsline {subsubsection}{\numberline {Topic 2.2:}Einstein and the Photoelectric Effect}{9}{subsubsection.1.2.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.3:}Discrete Emission Lines}{9}{subsubsection.1.2.3}% 
-\contentsline {subsubsection}{\numberline {Topic 2.4:}Problems with the Bohr Model and the Electron Cloud Model}{9}{subsubsection.1.2.4}% 
-\contentsline {subsection}{\numberline {Lesson 3:}Atomic Spectra}{10}{subsection.1.3}% 
-\contentsline {subsubsection}{\numberline {Topic 3.1:}Bohr's Explanation of Atomic Emission and Absorption}{10}{subsubsection.1.3.1}% 
-\contentsline {subsubsection}{\numberline {Topic 3.2:}Absorption and Emission Spectra}{10}{subsubsection.1.3.2}% 
-\contentsline {subsubsection}{\numberline {Topic 3.3:}Spectroscopy}{10}{subsubsection.1.3.3}% 
-\contentsline {subsection}{\numberline {Lesson 4:}The Structure of the Atom}{10}{subsection.1.4}% 
-\contentsline {subsubsection}{\numberline {Topic 4.1:}The Atom's Components}{10}{subsubsection.1.4.1}% 
-\contentsline {subsubsection}{\numberline {Topic 4.2:}Atomic Mass Unit}{11}{subsubsection.1.4.2}% 
-\contentsline {subsubsection}{\numberline {Topic 4.3:}Atomic Number}{11}{subsubsection.1.4.3}% 
-\contentsline {subsubsection}{\numberline {Topic 4.4:}Ions}{11}{subsubsection.1.4.4}% 
-\contentsline {subsubsection}{\numberline {Topic 4.5:}Isotopes}{11}{subsubsection.1.4.5}% 
-\contentsline {subsection}{\numberline {Lesson 5:}Nuclear Fission and Nuclear Fusion}{12}{subsection.1.5}% 
-\contentsline {subsubsection}{\numberline {Topic 5.1:}Nuclear Decay}{12}{subsubsection.1.5.1}% 
-\contentsline {subsubsection}{\numberline {Topic 5.2:}Fission}{12}{subsubsection.1.5.2}% 
-\contentsline {subsubsection}{\numberline {Topic 5.3:}Fusion}{13}{subsubsection.1.5.3}% 
-\contentsline {subsubsection}{\numberline {Topic 5.4:}Cold Fusion}{13}{subsubsection.1.5.4}% 
-\contentsline {subsection}{\numberline {Lesson 6:}Elements, Compounds, and Mixtures}{13}{subsection.1.6}% 
-\contentsline {subsubsection}{\numberline {Topic 6.1:}Physical vs Chemical Properties/Changes}{13}{subsubsection.1.6.1}% 
-\contentsline {subsubsection}{\numberline {Topic 6.2:}Classification of Matter}{13}{subsubsection.1.6.2}% 
-\contentsline {subsubsection}{\numberline {Topic 6.3:}Separation of Mixtures}{14}{subsubsection.1.6.3}% 
-\contentsline {subsection}{\numberline {Lesson 7:}Atomic Numbers and Electron Configurations}{14}{subsection.1.7}% 
-\contentsline {subsubsection}{\numberline {Topic 7.1:}Quantum Numbers}{14}{subsubsection.1.7.1}% 
-\contentsline {subsubsection}{\numberline {Topic 7.2:}Shells, Subshells, and Orbitals}{15}{subsubsection.1.7.2}% 
-\contentsline {subsubsection}{\numberline {Topic 7.3:}The Pauli Exclusion Principle}{15}{subsubsection.1.7.3}% 
-\contentsline {subsubsection}{\numberline {Topic 7.4:}Electron Configuration and Orbital Notation}{15}{subsubsection.1.7.4}% 
-\contentsline {subsubsection}{\numberline {Topic 7.5:}Aufbau Principle}{16}{subsubsection.1.7.5}% 
-\contentsline {subsubsection}{\numberline {Topic 7.6:}Dot Structures/Bohr Diagrams}{16}{subsubsection.1.7.6}% 
-\contentsline {subsection}{\numberline {Lesson 8:}The History and Arrangement of the Periodic Table}{16}{subsection.1.8}% 
-\contentsline {subsubsection}{\numberline {Topic 8.1:}The Periodic Table}{16}{subsubsection.1.8.1}% 
-\contentsline {subsubsection}{\numberline {Topic 8.2:}Early Attempts at a Periodic Table}{16}{subsubsection.1.8.2}% 
-\contentsline {subsubsection}{\numberline {Topic 8.3:}The Modern Periodic Table}{17}{subsubsection.1.8.3}% 
-\contentsline {subsubsection}{\numberline {Topic 8.4:}Metals, Nonmetals, and Semimetals}{17}{subsubsection.1.8.4}% 
-\contentsline {subsubsection}{\numberline {Topic 8.5:}Periods and Groups}{17}{subsubsection.1.8.5}% 
-\contentsline {subsubsection}{\numberline {Topic 8.6:}Minor Groups}{17}{subsubsection.1.8.6}% 
-\contentsline {subsection}{\numberline {Lesson 9:}Electrons and the Periodic Table}{18}{subsection.1.9}% 
-\contentsline {subsubsection}{\numberline {Topic 9.1:}Noble-Gas Notation}{18}{subsubsection.1.9.1}% 
-\contentsline {subsubsection}{\numberline {Topic 9.2:}Core and Valence Electrons}{19}{subsubsection.1.9.2}% 
-\contentsline {subsubsection}{\numberline {Topic 9.3:}Valence Electron Blocks}{19}{subsubsection.1.9.3}% 
-\contentsline {subsection}{\numberline {Lesson 10:}Periodic Trends}{19}{subsection.1.10}% 
-\contentsline {subsubsection}{\numberline {Topic 10.1:}Trends of Atomic Radii}{19}{subsubsection.1.10.1}% 
-\contentsline {subsubsection}{\numberline {Topic 10.2:}Trends of Ionic Radii}{19}{subsubsection.1.10.2}% 
-\contentsline {subsubsection}{\numberline {Topic 10.3:}Transition Metal Exceptions}{19}{subsubsection.1.10.3}% 
-\contentsline {subsubsection}{\numberline {Topic 10.4:}Ionization Energy}{20}{subsubsection.1.10.4}% 
-\contentsline {subsubsection}{\numberline {Topic 10.5:}Trends in Electron Affinity}{20}{subsubsection.1.10.5}% 
-\contentsline {subsubsection}{\numberline {Topic 10.6:}Trends in Electronegativity}{20}{subsubsection.1.10.6}% 
-\contentsline {section}{\numberline {Unit II:}States and Properties of Matter}{21}{section.2}% 
-\contentsline {subsection}{\numberline {Lesson 1:}Gases}{21}{subsection.2.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.1:}Kinetic-Molecular Theory}{21}{subsubsection.2.1.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.2:}Properties of Gases}{21}{subsubsection.2.1.2}% 
-\contentsline {subsection}{\numberline {Lesson 2:}Liquids}{22}{subsection.2.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.1:}Particles in Liquids}{22}{subsubsection.2.2.1}% 
-\contentsline {subsubsection}{\numberline {Topic 2.2:}Intermolecular Forces and State Changes}{22}{subsubsection.2.2.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.3:}Viscosity}{22}{subsubsection.2.2.3}% 
-\contentsline {subsubsection}{\numberline {Topic 2.4:}Surface Tension}{22}{subsubsection.2.2.4}% 
-\contentsline {subsubsection}{\numberline {Topic 2.5:}Other Properties}{22}{subsubsection.2.2.5}% 
-\contentsline {subsection}{\numberline {Lesson 3:}Solids and Plasmas}{23}{subsection.2.3}% 
-\contentsline {subsubsection}{\numberline {Topic 3.1:}Crystals and Amorphous Solids}{23}{subsubsection.2.3.1}% 
-\contentsline {subsubsection}{\numberline {Topic 3.2:}Plasma Properties}{23}{subsubsection.2.3.2}% 
-\contentsline {subsubsection}{\numberline {Topic 3.3:}Plasma in Nature and in Technology}{23}{subsubsection.2.3.3}% 
-\contentsline {subsection}{\numberline {Lesson 4:}Phase Changes}{23}{subsection.2.4}% 
-\contentsline {subsubsection}{\numberline {Topic 4.1:}Molecular Motion and Phase Changes}{23}{subsubsection.2.4.1}% 
-\contentsline {subsubsection}{\numberline {Topic 4.2:}Diagramming Phase Changes}{24}{subsubsection.2.4.2}% 
-\contentsline {subsection}{\numberline {Lesson 5:}Changes in Matter}{24}{subsection.2.5}% 
-\contentsline {subsubsection}{\numberline {Topic 5.1:}Matter}{24}{subsubsection.2.5.1}% 
-\contentsline {subsubsection}{\numberline {Topic 5.2:}Physical and Chemical Properties}{24}{subsubsection.2.5.2}% 
-\contentsline {subsubsection}{\numberline {Topic 5.3:}Extensive and Intensive Physical Properties}{24}{subsubsection.2.5.3}% 
-\contentsline {subsubsection}{\numberline {Topic 5.4:}Characteristic Properties}{25}{subsubsection.2.5.4}% 
-\contentsline {subsubsection}{\numberline {Topic 5.5:}Chemical and Physical Changes}{25}{subsubsection.2.5.5}% 
-\contentsline {section}{\numberline {Unit III:}Chemical Bonds and Compounds}{25}{section.3}% 
-\contentsline {subsection}{\numberline {Lesson 1:}Ionic Bonding}{25}{subsection.3.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.1:}Ionic Bonding}{25}{subsubsection.3.1.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.2:}Crystals}{25}{subsubsection.3.1.2}% 
-\contentsline {subsubsection}{\numberline {Topic 1.3:}Polyatomic Ions}{26}{subsubsection.3.1.3}% 
-\contentsline {subsubsection}{\numberline {Topic 1.4:}The Formation of Crystal Lattices}{26}{subsubsection.3.1.4}% 
-\contentsline {subsubsection}{\numberline {Topic 1.5:}Properties Resultant from Lattice Energy}{26}{subsubsection.3.1.5}% 
-\contentsline {subsection}{\numberline {Lesson 2:}Covalent Bonding}{26}{subsection.3.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.1:}Orbital Overlap}{26}{subsubsection.3.2.1}% 
-\contentsline {subsubsection}{\numberline {Topic 2.2:}Equal and Unequal Sharing of Electrons}{27}{subsubsection.3.2.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.3:}Lewis Structures}{27}{subsubsection.3.2.3}% 
-\contentsline {subsubsection}{\numberline {Topic 2.4:}Exceptions to the Octet Rule}{27}{subsubsection.3.2.4}% 
-\contentsline {subsubsection}{\numberline {Topic 2.5:}Double and Triple Bonds}{27}{subsubsection.3.2.5}% 
-\contentsline {subsubsection}{\numberline {Topic 2.6:}Resonance Structures}{28}{subsubsection.3.2.6}% 
-\contentsline {subsubsection}{\numberline {Topic 2.7:}Properties of Covalent Compounds}{28}{subsubsection.3.2.7}% 
-\contentsline {subsection}{\numberline {Lesson 3:}Metallic Bonding}{28}{subsection.3.3}% 
-\contentsline {subsubsection}{\numberline {Topic 3.1:}The Electron Sea}{28}{subsubsection.3.3.1}% 
-\contentsline {subsubsection}{\numberline {Topic 3.2:}Molecular Orbitals}{28}{subsubsection.3.3.2}% 
-\contentsline {subsubsection}{\numberline {Topic 3.3:}Resultant Properties}{28}{subsubsection.3.3.3}% 
-\contentsline {subsubsection}{\numberline {Topic 3.4:}Alloys}{29}{subsubsection.3.3.4}% 
-\contentsline {subsection}{\numberline {Lesson 4:}Intermolecular Forces}{29}{subsection.3.4}% 
-\contentsline {subsubsection}{\numberline {Topic 4.1:}Intramolecular vs Intermolecular Forces}{29}{subsubsection.3.4.1}% 
-\contentsline {subsubsection}{\numberline {Topic 4.2:}Hydrogen Bonds}{29}{subsubsection.3.4.2}% 
-\contentsline {subsubsection}{\numberline {Topic 4.3:}Van der Waals Forces}{30}{subsubsection.3.4.3}% 
-\contentsline {subsubsection}{\numberline {Topic 4.4:}Applications of Intermolecular Forces}{30}{subsubsection.3.4.4}% 
-\contentsline {subsection}{\numberline {Lesson 5:}Nomenclature of Ionic Compounds}{30}{subsection.3.5}% 
-\contentsline {subsubsection}{\numberline {Topic 5.1:}Charge of Ions}{30}{subsubsection.3.5.1}% 
-\contentsline {subsubsection}{\numberline {Topic 5.2:}Nomenclature of Ionic Compounds}{30}{subsubsection.3.5.2}% 
-\contentsline {subsubsection}{\numberline {Topic 5.3:}Polyatomic Ions}{31}{subsubsection.3.5.3}% 
-\contentsline {subsubsection}{\numberline {Topic 5.4:}Transition Metals}{31}{subsubsection.3.5.4}% 
-\contentsline {subsection}{\numberline {Lesson 6:}Nomenclature of Covalent Compounds}{31}{subsection.3.6}% 
-\contentsline {subsubsection}{\numberline {Topic 6.1:}Nomenclature for Covalent Compounds}{31}{subsubsection.3.6.1}% 
-\contentsline {subsubsection}{\numberline {Topic 6.2:}Exceptions}{31}{subsubsection.3.6.2}% 
-\contentsline {subsubsection}{\numberline {Topic 6.3:}Acids and Bases}{31}{subsubsection.3.6.3}% 
-\contentsline {subsection}{\numberline {Lesson 7:}Polymers}{32}{subsection.3.7}% 
-\contentsline {subsubsection}{\numberline {Topic 7.1:}Formation of Polymers}{32}{subsubsection.3.7.1}% 
-\contentsline {subsubsection}{\numberline {Topic 7.2:}Polymer Classification}{32}{subsubsection.3.7.2}% 
-\contentsline {subsection}{\numberline {Lesson 8:}Properties and Uses of Saturated Hydrocarbons}{33}{subsection.3.8}% 
-\contentsline {subsubsection}{\numberline {Topic 8.1:}Isomers and Hydrocarbons}{33}{subsubsection.3.8.1}% 
-\contentsline {subsubsection}{\numberline {Topic 8.2:}Hydrocarbon Notation}{33}{subsubsection.3.8.2}% 
-\contentsline {subsubsection}{\numberline {Topic 8.3:}Straight Chains, Branched Chains, and Cycloalkanes}{33}{subsubsection.3.8.3}% 
-\contentsline {subsubsection}{\numberline {Topic 8.4:}Properties}{33}{subsubsection.3.8.4}% 
-\contentsline {subsubsection}{\numberline {Topic 8.5:}Alkane Uses}{34}{subsubsection.3.8.5}% 
-\contentsline {subsubsection}{\numberline {Topic 8.6:}Nomenclature}{34}{subsubsection.3.8.6}% 
-\contentsline {subsection}{\numberline {Lesson 9:}Properties and Uses of Unsaturated Hydrocarbons}{34}{subsection.3.9}% 
-\contentsline {subsubsection}{\numberline {Topic 9.1:}Alkenes, Alkynes}{34}{subsubsection.3.9.1}% 
-\contentsline {subsubsection}{\numberline {Topic 9.2:}Cis Isomers and Trans Isomers}{35}{subsubsection.3.9.2}% 
-\contentsline {subsubsection}{\numberline {Topic 9.3:}Aromatic Hydrocarbons}{35}{subsubsection.3.9.3}% 
-\contentsline {subsubsection}{\numberline {Topic 9.4:}Boiling Points and Vapor Pressure}{35}{subsubsection.3.9.4}% 
-\contentsline {subsubsection}{\numberline {Topic 9.5:}Properties of Unsaturated Hydrocarbons}{35}{subsubsection.3.9.5}% 
-\contentsline {subsubsection}{\numberline {Topic 9.6:}Applications of Unsaturated Hydrocarbons}{35}{subsubsection.3.9.6}% 
-\contentsline {section}{\numberline {Unit IV:}Chemical Reactions and Limiting Reactants}{36}{section.4}% 
-\contentsline {subsection}{\numberline {Lesson 1:}Evidence of Chemical Reactions}{36}{subsection.4.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.1:}Chemical Changes and Chemical Reactions}{36}{subsubsection.4.1.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.2:}Rate of a Chemical Reaction}{36}{subsubsection.4.1.2}% 
-\contentsline {subsubsection}{\numberline {Topic 1.3:}Indicators/Evidence of a Chemical Reaction}{36}{subsubsection.4.1.3}% 
-\contentsline {subsection}{\numberline {Lesson 2:}Writing and Balancing Chemical Equations}{36}{subsection.4.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.1:}Equations}{36}{subsubsection.4.2.1}% 
-\contentsline {subsection}{\numberline {Lesson 3:}Percent Composition and Molecular Formula}{37}{subsection.4.3}% 
-\contentsline {subsubsection}{\numberline {Topic 3.1:}Mole Ratios}{37}{subsubsection.4.3.1}% 
-\contentsline {subsubsection}{\numberline {Topic 3.2:}Empirical and Molecular Formulae}{37}{subsubsection.4.3.2}% 
-\contentsline {subsubsection}{\numberline {Topic 3.3:}Percent Composition}{37}{subsubsection.4.3.3}% 
-\contentsline {subsection}{\numberline {Lesson 4:}Types of Reactions}{38}{subsection.4.4}% 
-\contentsline {subsubsection}{\numberline {Topic 4.1:}Types of Chemical Reactions}{38}{subsubsection.4.4.1}% 
-\contentsline {subsubsection}{\numberline {Topic 4.2:}Differentiating Single and Double Replacement Reactions}{38}{subsubsection.4.4.2}% 
-\contentsline {subsubsection}{\numberline {Topic 4.3:}Activity Series}{38}{subsubsection.4.4.3}% 
-\contentsline {subsection}{\numberline {Lesson 5:}Limiting Reactant and Percent Yield}{38}{subsection.4.5}% 
-\contentsline {subsubsection}{\numberline {Topic 5.1:}Limiting Reactants and Stoichiometry}{38}{subsubsection.4.5.1}% 
-\contentsline {subsubsection}{\numberline {Topic 5.2:}Theoretical Yield and Percent Yield}{39}{subsubsection.4.5.2}% 
-\contentsline {section}{\numberline {Unit V:}Stoichiometry and the Gas Laws}{39}{section.5}% 
-\contentsline {subsection}{\numberline {Lesson 1:}Molar Masses}{39}{subsection.5.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.1:}Moles and Avogadro's Number}{39}{subsubsection.5.1.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.2:}Molar Mass and Average Atomic Mass}{39}{subsubsection.5.1.2}% 
-\contentsline {subsection}{\numberline {Lesson 2:}Introduction to Stoichiometry}{39}{subsection.5.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.1:}Stoichiometry and Ratios}{39}{subsubsection.5.2.1}% 
-\contentsline {subsection}{\numberline {Lesson 3:}Stoichiometric Calculations}{40}{subsection.5.3}% 
-\contentsline {subsubsection}{\numberline {Topic 3.1:}Molar Mass and Mass-to-Mole Ratio}{40}{subsubsection.5.3.1}% 
-\contentsline {subsubsection}{\numberline {Topic 3.2:}Interchemical Calculations}{40}{subsubsection.5.3.2}% 
-\contentsline {subsection}{\numberline {Lesson 4:}Gas Laws}{40}{subsection.5.4}% 
-\contentsline {subsubsection}{\numberline {Topic 4.1:}Boyle's Law}{40}{subsubsection.5.4.1}% 
-\contentsline {subsubsection}{\numberline {Topic 4.2:}Other Laws}{40}{subsubsection.5.4.2}% 
-\contentsline {subsubsection}{\numberline {Topic 4.3:}Partial Pressure}{40}{subsubsection.5.4.3}% 
-\contentsline {subsection}{\numberline {Lesson 5:}The Ideal Gas Law}{41}{subsection.5.5}% 
-\contentsline {subsubsection}{\numberline {Topic 5.1:}Avogadro's Law}{41}{subsubsection.5.5.1}% 
-\contentsline {subsubsection}{\numberline {Topic 5.2:}Derivation of the Ideal Gas Law}{41}{subsubsection.5.5.2}% 
-\contentsline {subsection}{\numberline {Lesson 6:}Gas Stoichiometry}{41}{subsection.5.6}% 
-\contentsline {subsubsection}{\numberline {Topic 6.1:}Implications of Molar Volume: Avogadro's Principle}{41}{subsubsection.5.6.1}% 
-\contentsline {section}{\numberline {Unit VI:}Reaction Rates and Equilibrium}{41}{section.6}% 
-\contentsline {subsection}{\numberline {Lesson 1:}Reaction Rate}{41}{subsection.6.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.1:}Energy Diagrams and $\Delta G$}{41}{subsubsection.6.1.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.2:}Activation Energy}{42}{subsubsection.6.1.2}% 
-\contentsline {subsubsection}{\numberline {Topic 1.3:}Chemical Bonds}{42}{subsubsection.6.1.3}% 
-\contentsline {subsubsection}{\numberline {Topic 1.4:}Reaction Rate}{42}{subsubsection.6.1.4}% 
-\contentsline {subsubsection}{\numberline {Topic 1.5:}Collision Theory}{42}{subsubsection.6.1.5}% 
-\contentsline {subsubsection}{\numberline {Topic 1.6:}Effective Collisions}{42}{subsubsection.6.1.6}% 
-\contentsline {subsubsection}{\numberline {Topic 1.7:}Effect of Concentration on Reaction Rate}{43}{subsubsection.6.1.7}% 
-\contentsline {subsubsection}{\numberline {Topic 1.8:}Effect of Pressure on Reaction Rate}{43}{subsubsection.6.1.8}% 
-\contentsline {subsubsection}{\numberline {Topic 1.9:}Effects of Surface Area on Reaction Rate}{43}{subsubsection.6.1.9}% 
-\contentsline {subsection}{\numberline {Lesson 2:}Reaction Pathways}{43}{subsection.6.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.1:}Reaction Pathway Graphs}{43}{subsubsection.6.2.1}% 
-\contentsline {subsubsection}{\numberline {Topic 2.2:}Exothermic Reactions}{43}{subsubsection.6.2.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.3:}Endothermic Reaction Pathway}{44}{subsubsection.6.2.3}% 
-\contentsline {subsubsection}{\numberline {Topic 2.4:}Activation Energy and the Activated Complex}{44}{subsubsection.6.2.4}% 
-\contentsline {subsection}{\numberline {Lesson 3:}Catalysts}{44}{subsection.6.3}% 
-\contentsline {subsubsection}{\numberline {Topic 3.1:}Catalysts}{44}{subsubsection.6.3.1}% 
-\contentsline {subsubsection}{\numberline {Topic 3.2:}How Catalysts Work}{44}{subsubsection.6.3.2}% 
-\contentsline {subsubsection}{\numberline {Topic 3.3:}Heterogenous Catalysts}{44}{subsubsection.6.3.3}% 
-\contentsline {subsubsection}{\numberline {Topic 3.4:}Enzymes}{45}{subsubsection.6.3.4}% 
-\contentsline {subsection}{\numberline {Lesson 4:}Reversible Reactions and Equilibrium}{45}{subsection.6.4}% 
-\contentsline {subsubsection}{\numberline {Topic 4.1:}Equilibrium in Reversible Reactions}{45}{subsubsection.6.4.1}% 
-\contentsline {subsubsection}{\numberline {Topic 4.2:}Forward and Reverse Reaction Rates}{45}{subsubsection.6.4.2}% 
-\contentsline {subsubsection}{\numberline {Topic 4.3:}Chemical Equilibrium}{45}{subsubsection.6.4.3}% 
-\contentsline {subsubsection}{\numberline {Topic 4.4:}The Equilibrium Constant ($K_{eq}$)}{46}{subsubsection.6.4.4}% 
-\contentsline {subsection}{\numberline {Lesson 5:}Shifts in Equilibrium}{46}{subsection.6.5}% 
-\contentsline {subsubsection}{\numberline {Topic 5.1:}Changes in Reactant or Product Concentration}{46}{subsubsection.6.5.1}% 
-\contentsline {subsubsection}{\numberline {Topic 5.2:}Common Ion}{46}{subsubsection.6.5.2}% 
-\contentsline {subsubsection}{\numberline {Topic 5.3:}Changes in Pressure}{46}{subsubsection.6.5.3}% 
-\contentsline {subsubsection}{\numberline {Topic 5.4:}Changes in Temperature}{46}{subsubsection.6.5.4}% 
-\contentsline {subsubsection}{\numberline {Topic 5.5:}Reaction Quotient}{47}{subsubsection.6.5.5}% 
-\contentsline {section}{\numberline {Unit VII:}Energy in Chemical Reactions}{47}{section.7}% 
-\contentsline {subsection}{\numberline {Lesson 1:}Energy}{47}{subsection.7.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.1:}Basic Definitions}{47}{subsubsection.7.1.1}% 
-\contentsline {subsubsection}{\numberline {Topic 1.2:}Potential Energy}{47}{subsubsection.7.1.2}% 
-\contentsline {subsubsection}{\numberline {Topic 1.3:}Mechanical Energy}{47}{subsubsection.7.1.3}% 
-\contentsline {subsubsection}{\numberline {Topic 1.4:}Thermal Energy}{47}{subsubsection.7.1.4}% 
-\contentsline {subsubsection}{\numberline {Topic 1.5:}Electromagnetic and Chemical Energy}{47}{subsubsection.7.1.5}% 
-\contentsline {subsubsection}{\numberline {Topic 1.6:}Law of Conservation of Energy}{48}{subsubsection.7.1.6}% 
-\contentsline {subsubsection}{\numberline {Topic 1.7:}Energy Transfer and Transformation}{48}{subsubsection.7.1.7}% 
-\contentsline {subsubsection}{\numberline {Topic 1.8:}Sources of Energy}{48}{subsubsection.7.1.8}% 
-\contentsline {subsection}{\numberline {Lesson 2:}Heat}{48}{subsection.7.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.1:}Thermal Energy}{48}{subsubsection.7.2.1}% 
-\contentsline {subsubsection}{\numberline {Topic 2.2:}Heat and Conduction}{48}{subsubsection.7.2.2}% 
-\contentsline {subsubsection}{\numberline {Topic 2.3:}Heat Flow during Chemical Processes}{49}{subsubsection.7.2.3}% 
-\contentsline {subsection}{\numberline {Lesson 3:}Calorimetry}{49}{subsection.7.3}% 
-\contentsline {subsubsection}{\numberline {Topic 3.1:}Specific Heat Capacity}{49}{subsubsection.7.3.1}% 
-\contentsline {subsubsection}{\numberline {Topic 3.2:}Calorimetry Definition}{49}{subsubsection.7.3.2}% 
-\contentsline {subsubsection}{\numberline {Topic 3.3:}Bomb Calorimetry}{49}{subsubsection.7.3.3}% 
-\contentsline {subsubsection}{\numberline {Topic 3.4:}The Calorie Content of Foods}{49}{subsubsection.7.3.4}% 
+\contentsline {section}{\numberline {Unit I:}Atomic Structure and the Periodic Table}{8}{section.1}% 
+\contentsline {subsection}{\numberline {Lesson 1:}The Historical Development of Atomic Theory}{8}{subsection.1.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.1:}Dalton's Atomic Theory}{8}{subsubsection.1.1.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.2:}Discovery of the Electron}{8}{subsubsection.1.1.2}% 
+\contentsline {subsubsection}{\numberline {Topic 1.3:}Plum Pudding Model}{9}{subsubsection.1.1.3}% 
+\contentsline {subsubsection}{\numberline {Topic 1.4:}Discovery of the Nucleus}{9}{subsubsection.1.1.4}% 
+\contentsline {subsection}{\numberline {Lesson 2:}The Modern Atomic Theory}{9}{subsection.1.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.1:}Theories of Light}{9}{subsubsection.1.2.1}% 
+\contentsline {subsubsection}{\numberline {Topic 2.2:}Einstein and the Photoelectric Effect}{10}{subsubsection.1.2.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.3:}Discrete Emission Lines}{10}{subsubsection.1.2.3}% 
+\contentsline {subsubsection}{\numberline {Topic 2.4:}Problems with the Bohr Model and the Electron Cloud Model}{10}{subsubsection.1.2.4}% 
+\contentsline {subsection}{\numberline {Lesson 3:}Atomic Spectra}{11}{subsection.1.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.1:}Bohr's Explanation of Atomic Emission and Absorption}{11}{subsubsection.1.3.1}% 
+\contentsline {subsubsection}{\numberline {Topic 3.2:}Absorption and Emission Spectra}{11}{subsubsection.1.3.2}% 
+\contentsline {subsubsection}{\numberline {Topic 3.3:}Spectroscopy}{11}{subsubsection.1.3.3}% 
+\contentsline {subsection}{\numberline {Lesson 4:}The Structure of the Atom}{11}{subsection.1.4}% 
+\contentsline {subsubsection}{\numberline {Topic 4.1:}The Atom's Components}{11}{subsubsection.1.4.1}% 
+\contentsline {subsubsection}{\numberline {Topic 4.2:}Atomic Mass Unit}{12}{subsubsection.1.4.2}% 
+\contentsline {subsubsection}{\numberline {Topic 4.3:}Atomic Number}{12}{subsubsection.1.4.3}% 
+\contentsline {subsubsection}{\numberline {Topic 4.4:}Ions}{12}{subsubsection.1.4.4}% 
+\contentsline {subsubsection}{\numberline {Topic 4.5:}Isotopes}{12}{subsubsection.1.4.5}% 
+\contentsline {subsection}{\numberline {Lesson 5:}Nuclear Fission and Nuclear Fusion}{13}{subsection.1.5}% 
+\contentsline {subsubsection}{\numberline {Topic 5.1:}Nuclear Decay}{13}{subsubsection.1.5.1}% 
+\contentsline {subsubsection}{\numberline {Topic 5.2:}Fission}{13}{subsubsection.1.5.2}% 
+\contentsline {subsubsection}{\numberline {Topic 5.3:}Fusion}{14}{subsubsection.1.5.3}% 
+\contentsline {subsubsection}{\numberline {Topic 5.4:}Cold Fusion}{14}{subsubsection.1.5.4}% 
+\contentsline {subsection}{\numberline {Lesson 6:}Elements, Compounds, and Mixtures}{14}{subsection.1.6}% 
+\contentsline {subsubsection}{\numberline {Topic 6.1:}Physical vs Chemical Properties/Changes}{14}{subsubsection.1.6.1}% 
+\contentsline {subsubsection}{\numberline {Topic 6.2:}Classification of Matter}{14}{subsubsection.1.6.2}% 
+\contentsline {subsubsection}{\numberline {Topic 6.3:}Separation of Mixtures}{15}{subsubsection.1.6.3}% 
+\contentsline {subsection}{\numberline {Lesson 7:}Atomic Numbers and Electron Configurations}{15}{subsection.1.7}% 
+\contentsline {subsubsection}{\numberline {Topic 7.1:}Quantum Numbers}{15}{subsubsection.1.7.1}% 
+\contentsline {subsubsection}{\numberline {Topic 7.2:}Shells, Subshells, and Orbitals}{16}{subsubsection.1.7.2}% 
+\contentsline {subsubsection}{\numberline {Topic 7.3:}The Pauli Exclusion Principle}{16}{subsubsection.1.7.3}% 
+\contentsline {subsubsection}{\numberline {Topic 7.4:}Electron Configuration and Orbital Notation}{16}{subsubsection.1.7.4}% 
+\contentsline {subsubsection}{\numberline {Topic 7.5:}Aufbau Principle}{17}{subsubsection.1.7.5}% 
+\contentsline {subsubsection}{\numberline {Topic 7.6:}Dot Structures/Bohr Diagrams}{17}{subsubsection.1.7.6}% 
+\contentsline {subsection}{\numberline {Lesson 8:}The History and Arrangement of the Periodic Table}{17}{subsection.1.8}% 
+\contentsline {subsubsection}{\numberline {Topic 8.1:}The Periodic Table}{17}{subsubsection.1.8.1}% 
+\contentsline {subsubsection}{\numberline {Topic 8.2:}Early Attempts at a Periodic Table}{17}{subsubsection.1.8.2}% 
+\contentsline {subsubsection}{\numberline {Topic 8.3:}The Modern Periodic Table}{18}{subsubsection.1.8.3}% 
+\contentsline {subsubsection}{\numberline {Topic 8.4:}Metals, Nonmetals, and Semimetals}{18}{subsubsection.1.8.4}% 
+\contentsline {subsubsection}{\numberline {Topic 8.5:}Periods and Groups}{18}{subsubsection.1.8.5}% 
+\contentsline {subsubsection}{\numberline {Topic 8.6:}Minor Groups}{18}{subsubsection.1.8.6}% 
+\contentsline {subsection}{\numberline {Lesson 9:}Electrons and the Periodic Table}{19}{subsection.1.9}% 
+\contentsline {subsubsection}{\numberline {Topic 9.1:}Noble-Gas Notation}{19}{subsubsection.1.9.1}% 
+\contentsline {subsubsection}{\numberline {Topic 9.2:}Core and Valence Electrons}{20}{subsubsection.1.9.2}% 
+\contentsline {subsubsection}{\numberline {Topic 9.3:}Valence Electron Blocks}{20}{subsubsection.1.9.3}% 
+\contentsline {subsection}{\numberline {Lesson 10:}Periodic Trends}{20}{subsection.1.10}% 
+\contentsline {subsubsection}{\numberline {Topic 10.1:}Trends of Atomic Radii}{20}{subsubsection.1.10.1}% 
+\contentsline {subsubsection}{\numberline {Topic 10.2:}Trends of Ionic Radii}{20}{subsubsection.1.10.2}% 
+\contentsline {subsubsection}{\numberline {Topic 10.3:}Transition Metal Exceptions}{20}{subsubsection.1.10.3}% 
+\contentsline {subsubsection}{\numberline {Topic 10.4:}Ionization Energy}{21}{subsubsection.1.10.4}% 
+\contentsline {subsubsection}{\numberline {Topic 10.5:}Trends in Electron Affinity}{21}{subsubsection.1.10.5}% 
+\contentsline {subsubsection}{\numberline {Topic 10.6:}Trends in Electronegativity}{21}{subsubsection.1.10.6}% 
+\contentsline {section}{\numberline {Unit II:}States and Properties of Matter}{22}{section.2}% 
+\contentsline {subsection}{\numberline {Lesson 1:}Gases}{22}{subsection.2.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.1:}Kinetic-Molecular Theory}{22}{subsubsection.2.1.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.2:}Properties of Gases}{22}{subsubsection.2.1.2}% 
+\contentsline {subsection}{\numberline {Lesson 2:}Liquids}{23}{subsection.2.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.1:}Particles in Liquids}{23}{subsubsection.2.2.1}% 
+\contentsline {subsubsection}{\numberline {Topic 2.2:}Intermolecular Forces and State Changes}{23}{subsubsection.2.2.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.3:}Viscosity}{23}{subsubsection.2.2.3}% 
+\contentsline {subsubsection}{\numberline {Topic 2.4:}Surface Tension}{23}{subsubsection.2.2.4}% 
+\contentsline {subsubsection}{\numberline {Topic 2.5:}Other Properties}{23}{subsubsection.2.2.5}% 
+\contentsline {subsection}{\numberline {Lesson 3:}Solids and Plasmas}{24}{subsection.2.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.1:}Crystals and Amorphous Solids}{24}{subsubsection.2.3.1}% 
+\contentsline {subsubsection}{\numberline {Topic 3.2:}Plasma Properties}{24}{subsubsection.2.3.2}% 
+\contentsline {subsubsection}{\numberline {Topic 3.3:}Plasma in Nature and in Technology}{24}{subsubsection.2.3.3}% 
+\contentsline {subsection}{\numberline {Lesson 4:}Phase Changes}{24}{subsection.2.4}% 
+\contentsline {subsubsection}{\numberline {Topic 4.1:}Molecular Motion and Phase Changes}{24}{subsubsection.2.4.1}% 
+\contentsline {subsubsection}{\numberline {Topic 4.2:}Diagramming Phase Changes}{25}{subsubsection.2.4.2}% 
+\contentsline {subsection}{\numberline {Lesson 5:}Changes in Matter}{25}{subsection.2.5}% 
+\contentsline {subsubsection}{\numberline {Topic 5.1:}Matter}{25}{subsubsection.2.5.1}% 
+\contentsline {subsubsection}{\numberline {Topic 5.2:}Physical and Chemical Properties}{25}{subsubsection.2.5.2}% 
+\contentsline {subsubsection}{\numberline {Topic 5.3:}Extensive and Intensive Physical Properties}{25}{subsubsection.2.5.3}% 
+\contentsline {subsubsection}{\numberline {Topic 5.4:}Characteristic Properties}{26}{subsubsection.2.5.4}% 
+\contentsline {subsubsection}{\numberline {Topic 5.5:}Chemical and Physical Changes}{26}{subsubsection.2.5.5}% 
+\contentsline {section}{\numberline {Unit III:}Chemical Bonds and Compounds}{26}{section.3}% 
+\contentsline {subsection}{\numberline {Lesson 1:}Ionic Bonding}{26}{subsection.3.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.1:}Ionic Bonding}{26}{subsubsection.3.1.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.2:}Crystals}{26}{subsubsection.3.1.2}% 
+\contentsline {subsubsection}{\numberline {Topic 1.3:}Polyatomic Ions}{27}{subsubsection.3.1.3}% 
+\contentsline {subsubsection}{\numberline {Topic 1.4:}The Formation of Crystal Lattices}{27}{subsubsection.3.1.4}% 
+\contentsline {subsubsection}{\numberline {Topic 1.5:}Properties Resultant from Lattice Energy}{27}{subsubsection.3.1.5}% 
+\contentsline {subsection}{\numberline {Lesson 2:}Covalent Bonding}{27}{subsection.3.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.1:}Orbital Overlap}{27}{subsubsection.3.2.1}% 
+\contentsline {subsubsection}{\numberline {Topic 2.2:}Equal and Unequal Sharing of Electrons}{28}{subsubsection.3.2.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.3:}Lewis Structures}{28}{subsubsection.3.2.3}% 
+\contentsline {subsubsection}{\numberline {Topic 2.4:}Exceptions to the Octet Rule}{28}{subsubsection.3.2.4}% 
+\contentsline {subsubsection}{\numberline {Topic 2.5:}Double and Triple Bonds}{28}{subsubsection.3.2.5}% 
+\contentsline {subsubsection}{\numberline {Topic 2.6:}Resonance Structures}{29}{subsubsection.3.2.6}% 
+\contentsline {subsubsection}{\numberline {Topic 2.7:}Properties of Covalent Compounds}{29}{subsubsection.3.2.7}% 
+\contentsline {subsection}{\numberline {Lesson 3:}Metallic Bonding}{29}{subsection.3.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.1:}The Electron Sea}{29}{subsubsection.3.3.1}% 
+\contentsline {subsubsection}{\numberline {Topic 3.2:}Molecular Orbitals}{29}{subsubsection.3.3.2}% 
+\contentsline {subsubsection}{\numberline {Topic 3.3:}Resultant Properties}{29}{subsubsection.3.3.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.4:}Alloys}{30}{subsubsection.3.3.4}% 
+\contentsline {subsection}{\numberline {Lesson 4:}Intermolecular Forces}{30}{subsection.3.4}% 
+\contentsline {subsubsection}{\numberline {Topic 4.1:}Intramolecular vs Intermolecular Forces}{30}{subsubsection.3.4.1}% 
+\contentsline {subsubsection}{\numberline {Topic 4.2:}Hydrogen Bonds}{30}{subsubsection.3.4.2}% 
+\contentsline {subsubsection}{\numberline {Topic 4.3:}Van der Waals Forces}{31}{subsubsection.3.4.3}% 
+\contentsline {subsubsection}{\numberline {Topic 4.4:}Applications of Intermolecular Forces}{31}{subsubsection.3.4.4}% 
+\contentsline {subsection}{\numberline {Lesson 5:}Nomenclature of Ionic Compounds}{31}{subsection.3.5}% 
+\contentsline {subsubsection}{\numberline {Topic 5.1:}Charge of Ions}{31}{subsubsection.3.5.1}% 
+\contentsline {subsubsection}{\numberline {Topic 5.2:}Nomenclature of Ionic Compounds}{31}{subsubsection.3.5.2}% 
+\contentsline {subsubsection}{\numberline {Topic 5.3:}Polyatomic Ions}{32}{subsubsection.3.5.3}% 
+\contentsline {subsubsection}{\numberline {Topic 5.4:}Transition Metals}{32}{subsubsection.3.5.4}% 
+\contentsline {subsection}{\numberline {Lesson 6:}Nomenclature of Covalent Compounds}{32}{subsection.3.6}% 
+\contentsline {subsubsection}{\numberline {Topic 6.1:}Nomenclature for Covalent Compounds}{32}{subsubsection.3.6.1}% 
+\contentsline {subsubsection}{\numberline {Topic 6.2:}Exceptions}{32}{subsubsection.3.6.2}% 
+\contentsline {subsubsection}{\numberline {Topic 6.3:}Acids and Bases}{32}{subsubsection.3.6.3}% 
+\contentsline {subsection}{\numberline {Lesson 7:}Polymers}{33}{subsection.3.7}% 
+\contentsline {subsubsection}{\numberline {Topic 7.1:}Formation of Polymers}{33}{subsubsection.3.7.1}% 
+\contentsline {subsubsection}{\numberline {Topic 7.2:}Polymer Classification}{33}{subsubsection.3.7.2}% 
+\contentsline {subsection}{\numberline {Lesson 8:}Properties and Uses of Saturated Hydrocarbons}{34}{subsection.3.8}% 
+\contentsline {subsubsection}{\numberline {Topic 8.1:}Isomers and Hydrocarbons}{34}{subsubsection.3.8.1}% 
+\contentsline {subsubsection}{\numberline {Topic 8.2:}Hydrocarbon Notation}{34}{subsubsection.3.8.2}% 
+\contentsline {subsubsection}{\numberline {Topic 8.3:}Straight Chains, Branched Chains, and Cycloalkanes}{34}{subsubsection.3.8.3}% 
+\contentsline {subsubsection}{\numberline {Topic 8.4:}Properties}{34}{subsubsection.3.8.4}% 
+\contentsline {subsubsection}{\numberline {Topic 8.5:}Alkane Uses}{35}{subsubsection.3.8.5}% 
+\contentsline {subsubsection}{\numberline {Topic 8.6:}Nomenclature}{35}{subsubsection.3.8.6}% 
+\contentsline {subsection}{\numberline {Lesson 9:}Properties and Uses of Unsaturated Hydrocarbons}{35}{subsection.3.9}% 
+\contentsline {subsubsection}{\numberline {Topic 9.1:}Alkenes, Alkynes}{35}{subsubsection.3.9.1}% 
+\contentsline {subsubsection}{\numberline {Topic 9.2:}Cis Isomers and Trans Isomers}{36}{subsubsection.3.9.2}% 
+\contentsline {subsubsection}{\numberline {Topic 9.3:}Aromatic Hydrocarbons}{36}{subsubsection.3.9.3}% 
+\contentsline {subsubsection}{\numberline {Topic 9.4:}Boiling Points and Vapor Pressure}{36}{subsubsection.3.9.4}% 
+\contentsline {subsubsection}{\numberline {Topic 9.5:}Properties of Unsaturated Hydrocarbons}{36}{subsubsection.3.9.5}% 
+\contentsline {subsubsection}{\numberline {Topic 9.6:}Applications of Unsaturated Hydrocarbons}{36}{subsubsection.3.9.6}% 
+\contentsline {section}{\numberline {Unit IV:}Chemical Reactions and Limiting Reactants}{37}{section.4}% 
+\contentsline {subsection}{\numberline {Lesson 1:}Evidence of Chemical Reactions}{37}{subsection.4.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.1:}Chemical Changes and Chemical Reactions}{37}{subsubsection.4.1.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.2:}Rate of a Chemical Reaction}{37}{subsubsection.4.1.2}% 
+\contentsline {subsubsection}{\numberline {Topic 1.3:}Indicators/Evidence of a Chemical Reaction}{37}{subsubsection.4.1.3}% 
+\contentsline {subsection}{\numberline {Lesson 2:}Writing and Balancing Chemical Equations}{37}{subsection.4.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.1:}Equations}{37}{subsubsection.4.2.1}% 
+\contentsline {subsection}{\numberline {Lesson 3:}Percent Composition and Molecular Formula}{38}{subsection.4.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.1:}Mole Ratios}{38}{subsubsection.4.3.1}% 
+\contentsline {subsubsection}{\numberline {Topic 3.2:}Empirical and Molecular Formulae}{38}{subsubsection.4.3.2}% 
+\contentsline {subsubsection}{\numberline {Topic 3.3:}Percent Composition}{38}{subsubsection.4.3.3}% 
+\contentsline {subsection}{\numberline {Lesson 4:}Types of Reactions}{39}{subsection.4.4}% 
+\contentsline {subsubsection}{\numberline {Topic 4.1:}Types of Chemical Reactions}{39}{subsubsection.4.4.1}% 
+\contentsline {subsubsection}{\numberline {Topic 4.2:}Differentiating Single and Double Replacement Reactions}{39}{subsubsection.4.4.2}% 
+\contentsline {subsubsection}{\numberline {Topic 4.3:}Activity Series}{39}{subsubsection.4.4.3}% 
+\contentsline {subsection}{\numberline {Lesson 5:}Limiting Reactant and Percent Yield}{39}{subsection.4.5}% 
+\contentsline {subsubsection}{\numberline {Topic 5.1:}Limiting Reactants and Stoichiometry}{39}{subsubsection.4.5.1}% 
+\contentsline {subsubsection}{\numberline {Topic 5.2:}Theoretical Yield and Percent Yield}{40}{subsubsection.4.5.2}% 
+\contentsline {section}{\numberline {Unit V:}Stoichiometry and the Gas Laws}{40}{section.5}% 
+\contentsline {subsection}{\numberline {Lesson 1:}Molar Masses}{40}{subsection.5.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.1:}Moles and Avogadro's Number}{40}{subsubsection.5.1.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.2:}Molar Mass and Average Atomic Mass}{40}{subsubsection.5.1.2}% 
+\contentsline {subsection}{\numberline {Lesson 2:}Introduction to Stoichiometry}{40}{subsection.5.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.1:}Stoichiometry and Ratios}{40}{subsubsection.5.2.1}% 
+\contentsline {subsection}{\numberline {Lesson 3:}Stoichiometric Calculations}{41}{subsection.5.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.1:}Molar Mass and Mass-to-Mole Ratio}{41}{subsubsection.5.3.1}% 
+\contentsline {subsubsection}{\numberline {Topic 3.2:}Interchemical Calculations}{41}{subsubsection.5.3.2}% 
+\contentsline {subsection}{\numberline {Lesson 4:}Gas Laws}{41}{subsection.5.4}% 
+\contentsline {subsubsection}{\numberline {Topic 4.1:}Boyle's Law}{41}{subsubsection.5.4.1}% 
+\contentsline {subsubsection}{\numberline {Topic 4.2:}Other Laws}{41}{subsubsection.5.4.2}% 
+\contentsline {subsubsection}{\numberline {Topic 4.3:}Partial Pressure}{41}{subsubsection.5.4.3}% 
+\contentsline {subsection}{\numberline {Lesson 5:}The Ideal Gas Law}{42}{subsection.5.5}% 
+\contentsline {subsubsection}{\numberline {Topic 5.1:}Avogadro's Law}{42}{subsubsection.5.5.1}% 
+\contentsline {subsubsection}{\numberline {Topic 5.2:}Derivation of the Ideal Gas Law}{42}{subsubsection.5.5.2}% 
+\contentsline {subsection}{\numberline {Lesson 6:}Gas Stoichiometry}{42}{subsection.5.6}% 
+\contentsline {subsubsection}{\numberline {Topic 6.1:}Implications of Molar Volume: Avogadro's Principle}{42}{subsubsection.5.6.1}% 
+\contentsline {section}{\numberline {Unit VI:}Reaction Rates and Equilibrium}{42}{section.6}% 
+\contentsline {subsection}{\numberline {Lesson 1:}Reaction Rate}{42}{subsection.6.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.1:}Energy Diagrams and $\Delta G$}{42}{subsubsection.6.1.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.2:}Activation Energy}{43}{subsubsection.6.1.2}% 
+\contentsline {subsubsection}{\numberline {Topic 1.3:}Chemical Bonds}{43}{subsubsection.6.1.3}% 
+\contentsline {subsubsection}{\numberline {Topic 1.4:}Reaction Rate}{43}{subsubsection.6.1.4}% 
+\contentsline {subsubsection}{\numberline {Topic 1.5:}Collision Theory}{43}{subsubsection.6.1.5}% 
+\contentsline {subsubsection}{\numberline {Topic 1.6:}Effective Collisions}{43}{subsubsection.6.1.6}% 
+\contentsline {subsubsection}{\numberline {Topic 1.7:}Effect of Concentration on Reaction Rate}{44}{subsubsection.6.1.7}% 
+\contentsline {subsubsection}{\numberline {Topic 1.8:}Effect of Pressure on Reaction Rate}{44}{subsubsection.6.1.8}% 
+\contentsline {subsubsection}{\numberline {Topic 1.9:}Effects of Surface Area on Reaction Rate}{44}{subsubsection.6.1.9}% 
+\contentsline {subsection}{\numberline {Lesson 2:}Reaction Pathways}{44}{subsection.6.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.1:}Reaction Pathway Graphs}{44}{subsubsection.6.2.1}% 
+\contentsline {subsubsection}{\numberline {Topic 2.2:}Exothermic Reactions}{44}{subsubsection.6.2.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.3:}Endothermic Reaction Pathway}{45}{subsubsection.6.2.3}% 
+\contentsline {subsubsection}{\numberline {Topic 2.4:}Activation Energy and the Activated Complex}{45}{subsubsection.6.2.4}% 
+\contentsline {subsection}{\numberline {Lesson 3:}Catalysts}{45}{subsection.6.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.1:}Catalysts}{45}{subsubsection.6.3.1}% 
+\contentsline {subsubsection}{\numberline {Topic 3.2:}How Catalysts Work}{45}{subsubsection.6.3.2}% 
+\contentsline {subsubsection}{\numberline {Topic 3.3:}Heterogenous Catalysts}{45}{subsubsection.6.3.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.4:}Enzymes}{46}{subsubsection.6.3.4}% 
+\contentsline {subsection}{\numberline {Lesson 4:}Reversible Reactions and Equilibrium}{46}{subsection.6.4}% 
+\contentsline {subsubsection}{\numberline {Topic 4.1:}Equilibrium in Reversible Reactions}{46}{subsubsection.6.4.1}% 
+\contentsline {subsubsection}{\numberline {Topic 4.2:}Forward and Reverse Reaction Rates}{46}{subsubsection.6.4.2}% 
+\contentsline {subsubsection}{\numberline {Topic 4.3:}Chemical Equilibrium}{46}{subsubsection.6.4.3}% 
+\contentsline {subsubsection}{\numberline {Topic 4.4:}The Equilibrium Constant ($K_{eq}$)}{47}{subsubsection.6.4.4}% 
+\contentsline {subsection}{\numberline {Lesson 5:}Shifts in Equilibrium}{47}{subsection.6.5}% 
+\contentsline {subsubsection}{\numberline {Topic 5.1:}Changes in Reactant or Product Concentration}{47}{subsubsection.6.5.1}% 
+\contentsline {subsubsection}{\numberline {Topic 5.2:}Common Ion}{47}{subsubsection.6.5.2}% 
+\contentsline {subsubsection}{\numberline {Topic 5.3:}Changes in Pressure}{47}{subsubsection.6.5.3}% 
+\contentsline {subsubsection}{\numberline {Topic 5.4:}Changes in Temperature}{47}{subsubsection.6.5.4}% 
+\contentsline {subsubsection}{\numberline {Topic 5.5:}Reaction Quotient}{48}{subsubsection.6.5.5}% 
+\contentsline {section}{\numberline {Unit VII:}Energy in Chemical Reactions}{48}{section.7}% 
+\contentsline {subsection}{\numberline {Lesson 1:}Energy}{48}{subsection.7.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.1:}Basic Definitions}{48}{subsubsection.7.1.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.2:}Potential Energy}{48}{subsubsection.7.1.2}% 
+\contentsline {subsubsection}{\numberline {Topic 1.3:}Mechanical Energy}{48}{subsubsection.7.1.3}% 
+\contentsline {subsubsection}{\numberline {Topic 1.4:}Thermal Energy}{48}{subsubsection.7.1.4}% 
+\contentsline {subsubsection}{\numberline {Topic 1.5:}Electromagnetic and Chemical Energy}{48}{subsubsection.7.1.5}% 
+\contentsline {subsubsection}{\numberline {Topic 1.6:}Law of Conservation of Energy}{49}{subsubsection.7.1.6}% 
+\contentsline {subsubsection}{\numberline {Topic 1.7:}Energy Transfer and Transformation}{49}{subsubsection.7.1.7}% 
+\contentsline {subsubsection}{\numberline {Topic 1.8:}Sources of Energy}{49}{subsubsection.7.1.8}% 
+\contentsline {subsection}{\numberline {Lesson 2:}Heat}{49}{subsection.7.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.1:}Thermal Energy}{49}{subsubsection.7.2.1}% 
+\contentsline {subsubsection}{\numberline {Topic 2.2:}Heat and Conduction}{49}{subsubsection.7.2.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.3:}Heat Flow during Chemical Processes}{50}{subsubsection.7.2.3}% 
+\contentsline {subsection}{\numberline {Lesson 3:}Calorimetry}{50}{subsection.7.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.1:}Specific Heat Capacity}{50}{subsubsection.7.3.1}% 
+\contentsline {subsubsection}{\numberline {Topic 3.2:}Calorimetry Definition}{50}{subsubsection.7.3.2}% 
+\contentsline {subsubsection}{\numberline {Topic 3.3:}Bomb Calorimetry}{50}{subsubsection.7.3.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.4:}The Calorie Content of Foods}{50}{subsubsection.7.3.4}% 
+\contentsline {subsection}{\numberline {Lesson 4:}Thermochemical Equations}{50}{subsection.7.4}% 
+\contentsline {subsubsection}{\numberline {Topic 4.1:}Enthalpy}{50}{subsubsection.7.4.1}% 
+\contentsline {subsubsection}{\numberline {Topic 4.2:}Enthalpy of Reaction}{51}{subsubsection.7.4.2}% 
+\contentsline {subsubsection}{\numberline {Topic 4.3:}Manipulating Equations}{51}{subsubsection.7.4.3}% 
+\contentsline {subsubsection}{\numberline {Topic 4.4:}Enthalpy of Combustion}{51}{subsubsection.7.4.4}% 
+\contentsline {subsection}{\numberline {Lesson 5:}Enthalpy and Phase Changes}{51}{subsection.7.5}% 
+\contentsline {subsubsection}{\numberline {Topic 5.1:}Heat and Phase Changes}{51}{subsubsection.7.5.1}% 
+\contentsline {subsubsection}{\numberline {Topic 5.2:}Effects of Heat on Phase Changes}{52}{subsubsection.7.5.2}% 
+\contentsline {subsubsection}{\numberline {Topic 5.3:}Relationship between Enthalpy}{52}{subsubsection.7.5.3}% 
+\contentsline {subsubsection}{\numberline {Topic 5.4:}Sweat and Temperature Regulation}{52}{subsubsection.7.5.4}% 
+\contentsline {subsection}{\numberline {Lesson 6:}Enthalpy of Reaction}{52}{subsection.7.6}% 
+\contentsline {subsubsection}{\numberline {Topic 6.1:}Equation Combination}{52}{subsubsection.7.6.1}% 
+\contentsline {subsubsection}{\numberline {Topic 6.2:}Diagramming Hess's Law}{52}{subsubsection.7.6.2}% 
+\contentsline {subsubsection}{\numberline {Topic 6.3:}Reaction Energy Diagrams and Enthalpy Diagrams}{52}{subsubsection.7.6.3}% 
+\contentsline {section}{\numberline {Unit VIII:}Mixtures, Solutions, and Solubility}{53}{section.8}% 
+\contentsline {subsection}{\numberline {Lesson 1:}Mixtures and Solutions}{53}{subsection.8.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.1:}Heterogenous and Homogenous Mixtures}{53}{subsubsection.8.1.1}% 
+\contentsline {subsubsection}{\numberline {Topic 1.2:}Solution}{53}{subsubsection.8.1.2}% 
+\contentsline {subsubsection}{\numberline {Topic 1.3:}Suspensions and Colloids}{53}{subsubsection.8.1.3}% 
+\contentsline {subsubsection}{\numberline {Topic 1.4:}The Tyndall Effect}{53}{subsubsection.8.1.4}% 
+\contentsline {subsubsection}{\numberline {Topic 1.5:}Techniques to Separate Solutions}{53}{subsubsection.8.1.5}% 
+\contentsline {subsection}{\numberline {Lesson 2:}Reactions in Aqueous Solutions}{54}{subsection.8.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.1:}Polarity of Water}{54}{subsubsection.8.2.1}% 
+\contentsline {subsubsection}{\numberline {Topic 2.2:}Ionization}{54}{subsubsection.8.2.2}% 
+\contentsline {subsubsection}{\numberline {Topic 2.3:}State of Matter in Chemical Reactions}{54}{subsubsection.8.2.3}% 
+\contentsline {subsubsection}{\numberline {Topic 2.4:}Double-Displacement Reactions}{54}{subsubsection.8.2.4}% 
+\contentsline {subsubsection}{\numberline {Topic 2.5:}Types of Electrolytes}{55}{subsubsection.8.2.5}% 
+\contentsline {subsection}{\numberline {Lesson 3:}Solutions and Solubility}{55}{subsection.8.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.1:}The Dissolving Process}{55}{subsubsection.8.3.1}% 
+\contentsline {subsubsection}{\numberline {Topic 3.2:}The Rate of Dissolution}{55}{subsubsection.8.3.2}% 
+\contentsline {subsubsection}{\numberline {Topic 3.3:}Solubility}{55}{subsubsection.8.3.3}% 
+\contentsline {subsubsection}{\numberline {Topic 3.4:}Environmental Conditions' Effects on Solubility}{55}{subsubsection.8.3.4}%