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+This is pdfTeX, Version 3.14159265-2.6-1.40.20 (TeX Live 2019) (preloaded format=pdftex 2019.5.8)  12 JUN 2019 19:56
+entering extended mode
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+ %&-line parsing enabled.
+**flame.tex
+(./flame.tex (../cer.tex)
+! Missing } inserted.
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+                }
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+                   &
+<argument> { \head Ionic Compound in Solution &
+                                                Observed Flame Color \cr \no...
+
+\text ...skip 1ex \noindent \hsize \@tablewidth #1
+                                                   \smallskip }} 
+\makedata ...\@data \noalign {\hrule height 1pt} }
+                                                   
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diff --git a/cer/flame/flame.pdf b/cer/flame/flame.pdf
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diff --git a/cer/flame/flame.tex b/cer/flame/flame.tex
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+\input ../cer.tex
+
+\name{Holden Rohrer}
+\course{FVS Chemistry AB 19.3}
+\teacher{Kerr}
+
+\question{Based on a substance's properties, how can you determine whether its bonds are ionic or covalent?}
+\claim{If a substance is solid at room temperature, has a crystalline structure, dissolves easily in water, and conducts electricity well, then it likely contains ionic bonds. Otherwise, it likely contains covalent bonds.}
+
+%\def\data{
+%  \datastyle{1.65in}
+\data{2}{1.65in}{
+  \head Ionic Compound in Solution & Observed Flame Color \cr
+  \noalign{\hrule}
+  $HCl$ Solution (baseline) \ampsub blue \endlinex
+  0.5M calcium chloride ($CaCl_2$) \ampsub orange-red \endlinex
+  0.5M sodium chloride ($NaCl$) \ampsub orange-yellow \endlinex
+  0.5M barium chloride ($BaCl_2$) \ampsub pale green \endlinex
+  0.5M lithium chloride ($LiCl$) \ampsub red \endlinex
+  0.5M copper(II) chloride ($CuCl_2$) \ampsub blue-green \endlinex
+  0.5M cesium chloride ($CsCl$) \ampsub blue-violet \endlinex
+  Unknown Solution \#1 \ampsub red \endlinex
+  Unknown Solution \#2 \ampsub blue-violet \endlinex
+}
+\evidence{%\parsub \noindent\data\parsub\smallskip
+\qquad\qquad\qquad\qquad Lab Results\parsub
+Metal ion in Unknown Solution \#1: Lithium \parsub 
+Metal ion in Unknown Solution \#2: Cesium \parsub
+}
+
+\justification{
+This makes sense
+}
+
+\makeheader
+\makedoc
+\bye
diff --git a/cer/flame/flame0.log b/cer/flame/flame0.log
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+entering extended mode
+ restricted \write18 enabled.
+ %&-line parsing enabled.
+**flame0.tex
+(./flame0.tex
+LaTeX2e <2018-12-01>
+(../cer.tex)
+
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+
+See the LaTeX manual or LaTeX Companion for explanation.
+Type  H <return>  for immediate help.
+ ...                                              
+                                                  
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+                
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diff --git a/cer/flame/flame0.pdf b/cer/flame/flame0.pdf
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--- /dev/null
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diff --git a/cer/flame/flame0.tex b/cer/flame/flame0.tex
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+\input ../cer.tex
+
+\name{Holden Rohrer}
+\course{FVS Chemistry AB 19.3}
+\teacher{Kerr}
+
+\question{How can you use flame color to identify the metal ion in an unknown compound?}
+\claim{If an unknown metal ion's flame color matches that of a known metal ion, then the metal ion likely is the same because metal ions produce characteristic colors when burned.}
+
+\def\data{
+  \let\rr=\cr
+  \def\width{1.65in}
+  \def\text##1{\ \tiny \tolerance=10000 \hbadness=10000 \hbox to \width{\vbox{\vskip1ex \noindent \hsize\width ##1 \smallskip}} }
+  \halign{\vrule width 1pt \text{##} & \vrule \text{##} \vrule width 1pt \cr
+  \noalign{\hrule height 1pt}
+  \head Ionic Compound in Solution & Observed Flame Color \cr
+  \noalign{\hrule}
+  $HCl$ Solution (baseline) & blue \cr \noalign{\hrule height 0.05pt}
+  0.5M calcium chloride ($CaCl_2$) & orange-red \cr \noalign{\hrule height 0.05pt}
+  0.5M sodium chloride ($NaCl$) & orange-yellow \cr \noalign{\hrule height 0.05pt}
+  0.5M barium chloride ($BaCl_2$) & pale green \cr \noalign{\hrule height 0.05pt}
+  0.5M lithium chloride ($LiCl$) & red \cr \noalign{\hrule height 0.05pt}
+  0.5M copper(II) chloride ($CuCl_2$) & blue-green \cr \noalign{\hrule height 0.05pt}
+  0.5M cesium chloride ($CsCl$) & blue-violet \cr \noalign{\hrule height 0.05pt}
+  Unknown Solution \#1 & red \cr \noalign{\hrule height 0.05pt}
+  Unknown Solution \#2 & blue-violet \cr \noalign{\hrule height 0.05pt}
+  \noalign{\hrule height 1pt}
+  }
+}
+\def\makedata{\data}
+
+\evidence{%\parsub \noindent\data\parsub\smallskip
+\qquad\qquad\qquad\qquad Lab Results\parsub
+\qquad Metal ion in Unknown Solution \#1: Lithium \parsub 
+\qquad Metal ion in Unknown Solution \#2: Cesium \parsub
+I know that the claim is true because all studied metal-chloride salts have different colors. The $LiCl$ salt, for example, burns a characteristic red which is backed up by an identical chemical solution burning the same color. All other examples on the above list have unique colors, and all samples of the same ions produce the same colors (as can be logically expected). The other example of the last property allowing identification of a given metal ion is $CsCl$, the second unknown solution which is blue-violet in both cases. This also gives a good clue as to the investigative question: one can determine the given metal ion of an unknown substance by cross-checking its flame test with the flame test of known substances.
+}
+
+\justification{
+The ability to identify which metal ion is in a given unknown substance makes sense because when heating occurs from the Bunsen Burner, electrons within the metal ion become excited when they absorb the light. Then, they release photons in line with their atomic (emission) spectrum. The mixture of these photons produces a specific color---the characteristic color of the flame. Because atomic spectra are unique, any given set of compounds with different metal ions will always have different characteristic colors. These are also consistent between two atoms of the same element, further corroborating previously noted properties. As described in the evidence section, these properties of consistency and uniqueness mean that a cross-checking procedure would work to identify an unknown ionic compound's metal ion.
+}
+
+\makeheader
+\makedoc
+\bye