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% Document Info
\author{liviabrookes}
\pdfinfo{
  /Title (chemistry.pdf)
  /Creator (Cheatography)
  /Author (liviabrookes)
  /Subject (Chemistry Cheat Sheet)
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\noindent
\begin{multicols}{3}
\begin{tabulary}{5.8cm}{C}
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    \vspace{-7pt}
    {\parbox{\dimexpr\textwidth-2\fboxsep\relax}{\noindent
        \hspace*{-6pt}\includegraphics[width=5.8cm]{/web/www.cheatography.com/public/images/cheatography_logo.pdf}}
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\begin{tabulary}{11cm}{L}
    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Chemistry Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{liviabrookes} via \textcolor{DarkBackground}{\uline{cheatography.com/164261/cs/35180/}}}
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\noindent
\begin{multicols}{3}
\begin{tabulary}{5.8cm}{LL}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}liviabrookes \\
  \uline{cheatography.com/liviabrookes} \\
  \end{tabulary}
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\columnbreak
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Published 3rd November, 2022.\\
   Updated 3rd November, 2022.\\
   Page {\thepage} of \pageref{LastPage}.
\end{tabulary}
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Sponsor}}  \\
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  \vspace{-5pt}
  %\includegraphics[width=48px,height=48px]{dave.jpeg}
  Measure your website readability!\\
  www.readability-score.com
\end{tabulary}
\end{multicols}}




\begin{document}
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\begin{multicols*}{3}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Decomposition Reactions}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Metal Carbonates}}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{when metal carbonates decompose they form a metal oxide and carbon dioxide gas.} \tn 
% Row Count 3 (+ 2)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{eg. when solid green copper carbonate is heated, a black solid and a colourless gas is formed. The gas turns limewater cloudy when bubbled through it.} \tn 
% Row Count 6 (+ 3)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{copper carbonate -{}-\textgreater{} copper oxide + carbon dioxide} \tn 
% Row Count 7 (+ 1)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\emph{an exception of this rule is silver carbonate, which decomposes to form silver metal, carbon dioxide, and oxygen.}}} \tn 
% Row Count 10 (+ 3)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Metal Hydroxides}}} \tn 
% Row Count 11 (+ 1)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{when metal hydroxides decompose they form a metal oxide and water.} \tn 
% Row Count 13 (+ 2)
% Row 7
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{eg. when solid white calcium hydroxide is heated, a white solid and a colourless liquid is formed. The liquid turns blue cobolt chloride paper pink.} \tn 
% Row Count 16 (+ 3)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{calcium hydroxide -{}-\textgreater{} calcium oxide + water} \tn 
% Row Count 17 (+ 1)
% Row 9
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Metal Hydrogen Carbonates}} (bicarbonates)} \tn 
% Row Count 18 (+ 1)
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{when metal hydrogen carbonates decompose they form a metal carbonate, carbon dioxide, and water.} \tn 
% Row Count 20 (+ 2)
% Row 11
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{eg. sodium bicarbonate -{}-\textgreater{} sodium carbonate + carbon dioxide + water} \tn 
% Row Count 22 (+ 2)
% Row 12
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Catalytic Decomposition}}} \tn 
% Row Count 23 (+ 1)
% Row 13
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{a catalyst reduces the amount of energy needed for a reaction to proceed. They allow reactions to take place at room temperature that would otherwise require higher temperatures.} \tn 
% Row Count 27 (+ 4)
% Row 14
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{Hydrogen peroxide: the decomposition can be sped up by the catalyst manganese dioxide (MnO₂).} \tn 
% Row Count 29 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Combination/Synthesis Reactions}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{Chemical reactions where the atoms of one element react with the atoms of another element to form a single compound.} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{element {\bf{A}} + element {\bf{B}} -{}-\textgreater{} element {\bf{AB}}} \tn 
% Row Count 4 (+ 1)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Combination Reactions with Oxygen}}} \tn 
% Row Count 5 (+ 1)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{-sometimes called oxidation reactions} \tn 
% Row Count 6 (+ 1)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{-when heat/light is produced it is also known as combustion/burning} \tn 
% Row Count 8 (+ 2)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{-the product is more stable than the reactants} \tn 
% Row Count 9 (+ 1)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{-can have a unique flame colour (see important observations)} \tn 
% Row Count 11 (+ 2)
% Row 7
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Ionic Compounds}}} \tn 
% Row Count 12 (+ 1)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\emph{when metal elements combine with non-metal elements.}}} \tn 
% Row Count 14 (+ 2)
% Row 9
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{-valence electrons are transferred from the metal to the non-metal} \tn 
% Row Count 16 (+ 2)
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{-the metal forms a positive ion and the non-metal forms a negative ion} \tn 
% Row Count 18 (+ 2)
% Row 11
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{-the ions are held together by electrostatic forces of attraction (positive-negative)} \tn 
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% Row 12
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Covalent Compounds}}} \tn 
% Row Count 21 (+ 1)
% Row 13
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\emph{when non-metals combine with other non-metals.}}} \tn 
% Row Count 22 (+ 1)
% Row 14
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{-bonding electrons are shared so that each atom has a stable full valence electron shell} \tn 
% Row Count 24 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{1.24425 cm} x{3.73275 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Definitions}}  \tn
% Row 0
\SetRowColor{LightBackground}
{\bf{Protons}} & positive charge, large mass, in the atom nucleus, top left number \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
{\bf{Neutrons}} & neutral charge, large mass, in the atom nucleus, subtract the number of protons from the bottom right number \tn 
% Row Count 7 (+ 4)
% Row 2
\SetRowColor{LightBackground}
{\bf{Electrons}} & negative charge, very tiny mass, in the outer shells, top left number \tn 
% Row Count 10 (+ 3)
% Row 3
\SetRowColor{white}
{\bf{Anion}} & negatively charged ion \tn 
% Row Count 11 (+ 1)
% Row 4
\SetRowColor{LightBackground}
{\bf{Cation}} & positively charged ion \tn 
% Row Count 12 (+ 1)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{The number of protons deciphers the atom. The number of neutrons can change to create {\bf{isotropes}}.} \tn 
% Row Count 14 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{When forming equations, always put the cation first eg. Na + Cl -{}-\textgreater{} NaCl not ClNa} \tn 
% Row Count 16 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{p{0.4977 cm} p{0.4977 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Chemical Reactions}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{'During a chemical reaction matter cannot be created nor destroyed.'} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{This is the {\bf{law of conservation of mass}}.} \tn 
% Row Count 3 (+ 1)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{This means that the reactants and products shown in a chemical equation must balance.} \tn 
% Row Count 5 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Eg. 4Fe +3O₂-{}-\textgreater{}2Fe₂O₃} \tn 
% Row Count 6 (+ 1)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{In this equation, the 4 is a {\bf{coefficient}}. These are whole numbers that multiply the following atom/molecule.} \tn 
% Row Count 9 (+ 3)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{In this equation, the 2 is a {\bf{subscript}}. These are whole numbers that represent the number of atoms/molecules immediately proceeding it.} \tn 
% Row Count 12 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Precipitation Reactions}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\emph{soluble means dissolvable}}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{-some ionic salts will readily dissolve in water- these are soluble} \tn 
% Row Count 3 (+ 2)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{-when they dissolve the ions dissociate (break apart into their + and - ions)} \tn 
% Row Count 5 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{-other ionic salts will only sparingly dissolve in water- these are considered insoluble} \tn 
% Row Count 7 (+ 2)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{AB}} + {\bf{CD}} -{}-\textgreater{} {\bf{AD}} + {\bf{BC}}} \tn 
% Row Count 8 (+ 1)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{-a precipitate will only form if one of the products formed is insoluble} \tn 
% Row Count 10 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{-you will observe the solution becoming cloudy and typically white solids will form} \tn 
% Row Count 12 (+ 2)
% Row 7
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{eg. lead nitrate + sodium carbonate -{}-\textgreater{} lead carbonate + sodium nitrate} \tn 
% Row Count 14 (+ 2)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{colourless solution of lead nitrate mixed with colourless solution of sodium carbonate forms white precipitate of lead carbonate in a colourless solution of sodium nitrate.} \tn 
% Row Count 18 (+ 4)
% Row 9
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{two soluble solutions were mixed together which allowed ions to exchange, forming the insoluble lead carbonation as a precipitate.} \tn 
% Row Count 21 (+ 3)
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{lead carbonate is insoluble because lead ions and carbonate ions are more attracted to each other than they are to water.} \tn 
% Row Count 24 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{1.29402 cm} x{3.68298 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Important Observations}}  \tn
% Row 0
\SetRowColor{LightBackground}
{\bf{Metals}} & silvery grey except copper which is pinky orange. Copper metal formed in a displacement reaction is reddy-brown. \tn 
% Row Count 4 (+ 4)
% Row 1
\SetRowColor{white}
{\bf{Gas}} & oxygen, hydrogen, and carbon dioxide are all colourless. \tn 
% Row Count 6 (+ 2)
% Row 2
\SetRowColor{LightBackground}
{\bf{Carbonates}} & white solids except copper carbonate which is a green solid and silver carbonate which is a yellow solid. \tn 
% Row Count 10 (+ 4)
% Row 3
\SetRowColor{white}
{\bf{Hydroxides}} & white solids except iron (II) hydroxide which is a green solid, iron (III) hydroxide which is an orange/red solid, and copper hydroxide which is a blue solid. \tn 
% Row Count 16 (+ 6)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Hydrogen peroxide is a colourless liquid.} \tn 
% Row Count 17 (+ 1)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Manganese dioxide is a black solid which catalyses the decomposition of hydrogen peroxide into water and oxygen gas.} \tn 
% Row Count 20 (+ 3)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\bf{Combination Reaction Observations}}} \tn 
% Row Count 21 (+ 1)
% Row 7
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Magnesium burns with a bright light to form a grey-white ash of MgO.} \tn 
% Row Count 23 (+ 2)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Sulfur; yellow non-metal- burns with a blue flame to form a colourless gas with a suffocating, choking odour, SO₂.} \tn 
% Row Count 26 (+ 3)
% Row 9
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Carbon; black non-metal- burns with a yellowy flame to make a colourless gas CO₂.} \tn 
% Row Count 28 (+ 2)
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Iron + Sulfur react when heated- glows and forms a black non-magnetic solid of FeS.} \tn 
% Row Count 30 (+ 2)
\end{tabularx}
\par\addvspace{1.3em}

\vfill
\columnbreak
\begin{tabularx}{5.377cm}{x{1.29402 cm} x{3.68298 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Important Observations (cont)}}  \tn
% Row 11
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Hydrogen; colourless gas + O₂ will explode with a small flame. After heating the solid glows a red-hot and a black solid is formed.} \tn 
% Row Count 3 (+ 3)
% Row 12
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{{\bf{Tests for Products Observations}}} \tn 
% Row Count 4 (+ 1)
% Row 13
\SetRowColor{LightBackground}
Hydrogen & gas burns with a squeaky pop \tn 
% Row Count 5 (+ 1)
% Row 14
\SetRowColor{white}
Carbon Dioxide & gas turns colourless limewater cloudy/milky \tn 
% Row Count 7 (+ 2)
% Row 15
\SetRowColor{LightBackground}
Oxygen & gas relights a glowing splint \tn 
% Row Count 8 (+ 1)
% Row 16
\SetRowColor{white}
Water & turns blue cobolt chloride paper pink \tn 
% Row Count 10 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Displacement Reactions}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{when a single atom 'displaces' another metal ion from within a compound.} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{More reactive metals on the activity series replace a less reactive metal ion from the compound. Ag is the least reactive metal.} \tn 
% Row Count 5 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{metal {\bf{A}} +compound {\bf{BC}} -{}-\textgreater{} compound {\bf{AC}} +element {\bf{B}}} \tn 
% Row Count 7 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{eg. Mg+FeSO₄-{}-\textgreater{}Fe+MgSO₄ because magnesium is more reactive than iron} \tn 
% Row Count 9 (+ 2)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{To form an {\bf{ionic equation}}, we get rid of the negative ion (spectator ion) because it is not involved in the reaction.} \tn 
% Row Count 12 (+ 3)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{eg. to form Mg + Fe2+ -{}-\textgreater{} Fe + Mg2+*} \tn 
% Row Count 13 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{*the 2+ is written as a little number top right of the element.}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}


% That's all folks
\end{multicols*}

\end{document}