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\author{NescafeAbusive32 (nescafeabusive32)}
\pdfinfo{
  /Title (gr-12-electrochemistry.pdf)
  /Creator (Cheatography)
  /Author (NescafeAbusive32 (nescafeabusive32))
  /Subject (Gr. 12 Electrochemistry Cheat Sheet)
}

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        \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{Gr. 12 Electrochemistry Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{NescafeAbusive32 (nescafeabusive32)} via \textcolor{DarkBackground}{\uline{cheatography.com/53385/cs/14465/}}}
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\noindent
\begin{multicols}{3}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}NescafeAbusive32 (nescafeabusive32) \\
  \uline{cheatography.com/nescafeabusive32} \\
  \end{tabulary}
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Published 25th January, 2018.\\
   Updated 25th January, 2018.\\
   Page {\thepage} of \pageref{LastPage}.
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  %\includegraphics[width=48px,height=48px]{dave.jpeg}
  Measure your website readability!\\
  www.readability-score.com
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\begin{document}
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\begin{multicols*}{3}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Redox Reactions}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Redox}} = "{\bf{reduction}} and {\bf{oxidation}}"} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Oxidation:}} {\bf{lose}} electrons (e¯)\{\{nl\}\}(Classical: any reaction involving {\emph{oxygen gas}} (O`2`) - rusting, combustion, etc.)} \tn 
% Row Count 4 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Reduction:}} {\bf{gain}} electrons (e¯)\{\{nl\}\}(Classical: {\emph{reducing}} a metal ore into pure metal)} \tn 
% Row Count 6 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{Both reactions {\bf{always occur together}}} \tn 
% Row Count 7 (+ 1)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\emph{Reducing agent:}} substance that causes {\bf{another substance}} to become {\bf{reduced}}} \tn 
% Row Count 9 (+ 2)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Oxidizing agent:}} substance that causes {\bf{another substance}} to become {\bf{oxidized}}} \tn 
% Row Count 11 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{Reducing agents {\bf{NEVER}} reduce themselves; is always {\bf{oxidized}} to promote reduction} \tn 
% Row Count 13 (+ 2)
% Row 7
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{Oxidizing agents {\bf{NEVER}} oxidize themselves; is always {\bf{reduced}} to promote oxidation} \tn 
% Row Count 15 (+ 2)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{Reducing/oxidizing agents are {\bf{ALWAYS}} reactants} \tn 
% Row Count 16 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{Remember: {\bf{LEO}} the lion says {\bf{GER}} \newline {\bf{L}}ose {\bf{E}}lectrons = {\bf{O}}xidation \newline {\bf{G}}ain {\bf{E}}lectrons = {\bf{R}}eduction \newline  \newline {\bf{Not new reactions:}} many synthesis, decomposition, combustion and single displacement reactions are often redox reactions}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{2.4885 cm} x{2.4885 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Oxidation States/Oxidation Numbers}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Net charge that an atom {\bf{{\emph{would}} have}} if the e¯ pairs in covalent bonds belonged {\bf{entirely}} to the {\bf{more electronegative ion}}} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{All redox reactions require a {\bf{change in O.N.}}} \tn 
% Row Count 4 (+ 1)
% Row 2
\SetRowColor{LightBackground}
\{\{fa-long-arrow-up\}\}{\bf{O.N.}} = oxidation (loss of e¯) & \{\{fa-long-arrow-down\}\}{\bf{O.N.}} = reduction (gain e¯) \tn 
% Row Count 7 (+ 3)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Rules to determine oxidation numbers (O.N.)}}} \tn 
% Row Count 9 (+ 2)
% Row 4
\SetRowColor{LightBackground}
\{\{bt\}\}{\bf{Pure elements}} have O.N. = 0 & \{\{bt\}\}C`(s)` = 0, O`2(s)` = 0, P`4(s)` = 0 \tn 
% Row Count 12 (+ 3)
% Row 5
\SetRowColor{white}
Monoatomic ions have O.N. = their {\bf{charge}} & Al\textasciicircum{}3+\textasciicircum{} = +3, Cl¯ = -1 \tn 
% Row Count 15 (+ 3)
% Row 6
\SetRowColor{LightBackground}
Hydrogen {\bf{always}} has O.N. = +1 (except metal hydrides = -1) & HCl (H = +1); H`2`S (H = +1); CaH`2` (H = -1) \tn 
% Row Count 19 (+ 4)
% Row 7
\SetRowColor{white}
Oxygen {\bf{always}} has O.N. = -2 (except peroxides = -1) & Li`2`O (O = -2); KNO`3` (O = -2); H`2`O`2` (O = -1) \tn 
% Row Count 22 (+ 3)
% Row 8
\SetRowColor{LightBackground}
In a compound, {\bf{groups I}}, {\bf{II}}, and {\bf{IV}} usually have {\bf{O.N. = ionic charge}} & NaCl (Na = +1, Cl = -1); MgO (Mg = +2) \tn 
% Row Count 27 (+ 5)
% Row 9
\SetRowColor{white}
In a {\bf{neutral}} compound\textasciicircum{}1\textasciicircum{}, {\bf{ΣO.N. = 0}} & CF`4` (C = +4, F = -1) \tn 
% Row Count 30 (+ 3)
\end{tabularx}
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\vfill
\columnbreak
\begin{tabularx}{5.377cm}{x{2.4885 cm} x{2.4885 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Oxidation States/Oxidation Numbers (cont)}}  \tn
% Row 10
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In a polyatomic ion, {\bf{ΣO.N. = ion's charge}} & NO`3`¯ (N = 5, O = -2; Σ O.N. = -1) \tn 
% Row Count 3 (+ 3)
% Row 11
\SetRowColor{white}
In molecular compunds with {\bf{no O}} or {\bf{H}}, the {\bf{more electronegative atom}} has O.N. = its usual charge & CS`2` (S = -2), Li`3`N (N = -3)~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ \tn 
% Row Count 19 (+ 16)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\bf{Note:}} The atoms {\bf{do not actually have these charges}}! \newline  \newline \textasciicircum{}{[}1{]}\textasciicircum{} If a compound contains a polyatomic ion, the {\bf{charge on the other ion}} is the {\bf{opposite}} to the {\bf{polyatomic ion's charge}} (ex. KIO`3` - K = +1 because IO`3` is 1-) \newline  \newline {\bf{Format for O.N.:}} "±\#" ({\bf{not}} "\#±" - ionic charges)}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
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\begin{tabularx}{5.377cm}{x{2.4885 cm} x{2.4885 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Half-Reactions and Disproportionate Reactions}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Most often, one atom is reduced and another is oxidized, but sometimes the same atom can be {\bf{oxidized and reduced in the same redox reaction}}} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}\{\{ac\}\}{\bf{Cu`2`O`(aq)` + H`2`SO`4(aq)` \{\{fa-long-arrow-right\}\} Cu`(s)` + CuSO`4 (aq)` + H`2`O`(l)`}}} \tn 
% Row Count 6 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{Cu \{\{fa-long-arrow-right\}\} +1 to 0 \{\{fa-long-arrow-right\}\} gain 1 e¯ \{\{fa-long-arrow-right\}\} {\bf{reduced}}} \tn 
% Row Count 9 (+ 3)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{Cu \{\{fa-long-arrow-right\}\} +1 to +2 \{\{fa-long-arrow-right\}\} lose 1 e¯ \{\{fa-long-arrow-right\}\} {\bf{oxidized}}} \tn 
% Row Count 12 (+ 3)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\} Since both of these happen in the {\bf{same reaction}}, it is {\bf{disproportionate}}} \tn 
% Row Count 14 (+ 2)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\emph{Half-reaction:}} reactions made from overall net ionic equations that focus on 1 specific atom} \tn 
% Row Count 16 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{ac\}\}{\bf{Zn`(s)` + CuSO`4(aq)` \{\{fa-long-arrow-right\}\} ZnSO`4(aq)` + Cu`(s)`}}} \tn 
% Row Count 18 (+ 2)
% Row 7
\SetRowColor{white}
{\bf{Zn`(s)` \{\{fa-long-arrow-right\}\}  ZnSO`4(aq)`}} & {\bf{CuSO`4(aq)` \{\{fa-long-arrow-right\}\} Cu`(s)`}} \tn 
% Row Count 21 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
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\begin{tabularx}{5.377cm}{x{1.64241 cm} x{3.33459 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Electrochemical Cells}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\bf{Two types}} of electrochemical cells:} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
{\emph{Galvanic cells}} & arrangement of 2 connected {\emph{half-cells}} that {\bf{spontaneously}} produce an electric current; e¯ always flow from high potential \{\{fa-long-arrow-right\}\} low potential \tn 
% Row Count 8 (+ 7)
% Row 2
\SetRowColor{LightBackground}
{\emph{Electrolytic cells}} & arrangement of 2 connected {\emph{half-cells}} that  uses electrical energy to produce a {\bf{non-spontaneous}} electric current; e¯ always flow from low potential \{\{fa-long-arrow-right\}\} high potential \tn 
% Row Count 16 (+ 8)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Parts of an electrochemical cell}}} \tn 
% Row Count 17 (+ 1)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\emph{Electrolyte:}} solution that contains aqueous ions ({\bf{cations}} (+) and {\bf{anions}} (-))} \tn 
% Row Count 19 (+ 2)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Electrode:}} solid metal conductor where redox reactions occur ({\bf{cathode}} (oxidation) and {\bf{anode}} (reduction))} \tn 
% Row Count 22 (+ 3)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\emph{Salt bridge:}} tube that {\bf{contains an electrolyte solution}} and {\bf{connects the 2 half-cells}}; used to {\bf{maintain electrical neutrality}}} \tn 
% Row Count 25 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{During the lifespan of the cell, the anode {\bf{decreases in mass}}, while the cathode {\bf{increases in mass}}}  \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Cell Potential}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{The measure of the {\bf{electric potential difference}} (voltage) between 2 half-cells} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Standard cell:}} galvanic cell in which all entities are at {\bf{SATP}} and all solution concentrations are {\bf{1.0 mol/L}}} \tn 
% Row Count 5 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Standard cell potential}} (ΔE°): the ability of each half cell to {\bf{gain e¯}} ({\bf{reduction}})} \tn 
% Row Count 7 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\bf{Cell potential formula:}}} \tn 
% Row Count 8 (+ 1)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{\{\{ac\}\}{\bf{ΔE°`(cell)` = E°`cathode` - E°`anode`}}} \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}{Batteries}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Cell:}} {\bf{2 connected electrodes}} in contact with an {\bf{electrolyte}}} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Battery:}} {\bf{2 or more}} cells connected {\bf{in series}}; voltage of battery is the {\bf{sum of the voltage of all the cells}}} \tn 
% Row Count 5 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{Different kinds of batteries are made for {\bf{different sized devices}}; the {\bf{bigger}} the battery, the {\bf{more electrolytic solution}}, and the {\bf{longer it lasts}}} \tn 
% Row Count 9 (+ 4)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Alkaline battery:}} a battery that uses an {\bf{alkaline}} ({\bf{basic}}) electrode rather than an acid} \tn 
% Row Count 11 (+ 2)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\bf{Primary vs secondary cells}}} \tn 
% Row Count 12 (+ 1)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{\{\{bt\}\}{\emph{Primary cells:}} {\bf{non-rechargeable}} cells that run until reactants are {\bf{used up}} (galvanic cells)} \tn 
% Row Count 15 (+ 3)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\emph{Secondary cells:}} cells that can be {\bf{recharged}} by adding an {\bf{electric current}} (galvanic when being used, electrolytic when being recharged)} \tn 
% Row Count 18 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{x{2.38896 cm} x{2.58804 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Corrosion}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bb\}\}The {\bf{breakdown/deterioration of metal}}  by a {\bf{redox reaction}}} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
{\bf{Conditions required for corrosion}} & {\bf{Conditions that accelerate corrosion}} \tn 
% Row Count 4 (+ 2)
% Row 2
\SetRowColor{LightBackground}
Oxygen (O`2`) & High temperature \tn 
% Row Count 5 (+ 1)
% Row 3
\SetRowColor{white}
Water (H`2`O`(l)`) & Salt and/or other electrolytes \tn 
% Row Count 7 (+ 2)
% Row 4
\SetRowColor{LightBackground}
 & Decrease in pH (more acidity) \tn 
% Row Count 9 (+ 2)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\emph{Rusting:}} the corrosion of iron (Fe) {\bf{specifically}}} \tn 
% Row Count 11 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
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\begin{tabularx}{5.377cm}{x{2.4885 cm} x{2.4885 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Corrosion Prevention}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\bf{Method 1: Galvanize the metal}}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\emph{Galvanizing:}} process where a metal (usually steel) is {\bf{coated with a thick layer of zinc (Zn)}} to prevent corrosion} \tn 
% Row Count 4 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\bf{Method 2: Cathodic protection}}} \tn 
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% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{\{\{bt\}\}{\emph{Cathodic protection:}} form of corrosion prevention in which {\bf{e¯ are continuously supplied}} to the metal being protected, making it a {\bf{cathode}}} \tn 
% Row Count 9 (+ 4)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{{\bf{Two forms:}}} \tn 
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% Row 5
\SetRowColor{white}
{\bf{Sacrificial anode}} ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ ~ & the oxidation of a more active metal attached to the metal being protected prevents the protected metal from corrosion \tn 
% Row Count 19 (+ 9)
% Row 6
\SetRowColor{LightBackground}
{\bf{Impressed current}} & e¯ from a direct current (DC) power source are continuously supplied to the protected metal \tn 
% Row Count 24 (+ 5)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}


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

\end{document}