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\subsection{Ionic Bonding}  When a metal reacts with a non-metal, ions will be formed if the overall energy change for the reaction is favourable. Electrons are transferred from the metal atoms to the non-metal atoms, giving both a stable electronic structure. The ions formed are held together by opposite charges in an electrostatic bond.\\\\The oppositely charged ions attract strongly in an ionic bond. This builds up into a giant lattice structure.  \subsection{Common Cations and Anions}  \begin{table}[!htb]  \centering  \begin{tabular}{lllll}  \textit{+1} & \textit{+2} & \textit{+3} & \textit{-1} & \textit{-2} \\ \hline  H\textsuperscript{+} & Mg\textsuperscript{2+} & Al\textsuperscript{3+} & F\textsuperscript{-} & O\textsuperscript{2-} \\  Li\textsuperscript{+} & Ca\textsuperscript{2+} & Fe\textsuperscript{3+} & Cl\textsuperscript{-} & CO\textsubscript{3}\textsuperscript{2-} \\  Na\textsuperscript{+} & Ba\textsuperscript{2+} & & Br\textsuperscript{-} & SO\textsubscript{4}\textsuperscript{2-} \\  K\textsuperscript{+} & Fe\textsuperscript{2+} & & I\textsuperscript{-} & \\  NH\textsubscript{4}\textsuperscript{+} & Cu\textsuperscript{2+} & & OH\textsuperscript{-} & \\  & Zn\textsuperscript{2+} & & NO\textsubscript{3}\textsuperscript{-} & \\  & Pb\textsuperscript{2+} & & HCO\textsubscript{3}\textsuperscript{-} & \\  \end{tabular}  \end{table}  \subsection{Common Cations and Anions}  a  \subsection{Making ionic salts}  \begin{itemize}  \item acid + alkali $\Rightarrow$ salt + water