From 4d160b54aea0203f94b49e3534d768367dcc8ce4 Mon Sep 17 00:00:00 2001
From: Holden Rohrer <hdawg7797@yahoo.com>
Date: Thu, 27 Jun 2019 09:47:44 -0400
Subject: new stuff

---
 cer/sem1/flame/flame.tex | 35 +++++++++++++++++++++++++++++++++++
 1 file changed, 35 insertions(+)
 create mode 100644 cer/sem1/flame/flame.tex

(limited to 'cer/sem1/flame/flame.tex')

diff --git a/cer/sem1/flame/flame.tex b/cer/sem1/flame/flame.tex
new file mode 100644
index 0000000..80a8f45
--- /dev/null
+++ b/cer/sem1/flame/flame.tex
@@ -0,0 +1,35 @@
+\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.}
+
+\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
-- 
cgit