deletions | additions       diff --git a/newpage_section_EL7_subsection_Formation__.tex b/newpage_section_EL7_subsection_Formation__.tex  index c33f915..39de1c9 100644  --- a/newpage_section_EL7_subsection_Formation__.tex  +++ b/newpage_section_EL7_subsection_Formation__.tex 
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& Zn\textsuperscript{2+} & & NO\textsubscript{3}\textsuperscript{-} & \\  & Pb\textsuperscript{2+} & & HCO\textsubscript{3}\textsuperscript{-} & \\  \end{tabular}  \end{table}  \subsection{Making ionic salts}  \begin{itemize}  \item acid + alkali $\Rightarrow$ salt + water  \item acid + base $\Rightarrow$ salt + water  \item acid + carbonate $\Rightarrow$ salt + water + carbon dioxide  \item acid + metal $\Rightarrow$ salt + hydrogen  \end{itemize}  \subsection{Ionic substances in solution}  Ionic substances tend to dissolve readily in water. The following do not:  \begin{itemize}  \item Barium/Calcium/Lead/Silver Sulfates  \item Silver/Lead Halides  \item All Metal Carbonates  \item Metal Hydroxides (Except Group 1 and Ammonium Hydroxide}  \end{itemize}  When they dissolve, ions are surrounded by the water molecules, and spread out. They then behave independently of each other.  \subsection{Ion Testing}  \begin{table}[!htb]  \centering  \begin{tabular}{llll}  \textit{Ion} & \textit{Solution added} & \textit{PPT Formed} & \textit{Colour} \\ \hline  Cu\textsuperscript{2+} & Sodium Hydroxide & Copper Hydroxide & Blue \\ \hline  Fe\textsuperscript{2+} & Sodium Hydroxide & Iron(II) Hydroxide & Green \\ \hline  Fe\textsuperscript{3+} & Sodium Hydroxide & Iron(III) Hydroxide & Brown \\ \hline  Pb\textsuperscript{2+} & Potassium Iodide & Lead Iodide & Yellow \\ \hline  Cl\textsuperscript{-} & Silver Nitrate & Silver Chloride & White \\ \hline  Br\textsuperscript{-} & Silver Nitrate & Silver Bromide & Cream \\ \hline  I\textsuperscript{-} & Silver Nitrate & Silver Iodide & Yellow \\ \hline  SO\textsubscript{4}\textsuperscript{2-} & Barium Chloride & Barium Sulfate & White \\ \hline  \end{tabular}  \end{table}