\documentclass[10pt,a4paper]{article}

% Packages
\usepackage{fancyhdr}           % For header and footer
\usepackage{multicol}           % Allows multicols in tables
\usepackage{tabularx}           % Intelligent column widths
\usepackage{tabulary}           % Used in header and footer
\usepackage{hhline}             % Border under tables
\usepackage{graphicx}           % For images
\usepackage{xcolor}             % For hex colours
%\usepackage[utf8x]{inputenc}    % For unicode character support
\usepackage[T1]{fontenc}        % Without this we get weird character replacements
\usepackage{colortbl}           % For coloured tables
\usepackage{setspace}           % For line height
\usepackage{lastpage}           % Needed for total page number
\usepackage{seqsplit}           % Splits long words.
%\usepackage{opensans}          % Can't make this work so far. Shame. Would be lovely.
\usepackage[normalem]{ulem}     % For underlining links
% Most of the following are not required for the majority
% of cheat sheets but are needed for some symbol support.
\usepackage{amsmath}            % Symbols
\usepackage{MnSymbol}           % Symbols
\usepackage{wasysym}            % Symbols
%\usepackage[english,german,french,spanish,italian]{babel}              % Languages

% Document Info
\author{Arsh.b}
\pdfinfo{
  /Title (9-1-oxidation-and-reduction.pdf)
  /Creator (Cheatography)
  /Author (Arsh.b)
  /Subject (9.1 Oxidation and reduction Cheat Sheet)
}

% Lengths and widths
\addtolength{\textwidth}{6cm}
\addtolength{\textheight}{-1cm}
\addtolength{\hoffset}{-3cm}
\addtolength{\voffset}{-2cm}
\setlength{\tabcolsep}{0.2cm} % Space between columns
\setlength{\headsep}{-12pt} % Reduce space between header and content
\setlength{\headheight}{85pt} % If less, LaTeX automatically increases it
\renewcommand{\footrulewidth}{0pt} % Remove footer line
\renewcommand{\headrulewidth}{0pt} % Remove header line
\renewcommand{\seqinsert}{\ifmmode\allowbreak\else\-\fi} % Hyphens in seqsplit
% This two commands together give roughly
% the right line height in the tables
\renewcommand{\arraystretch}{1.3}
\onehalfspacing

% Commands
\newcommand{\SetRowColor}[1]{\noalign{\gdef\RowColorName{#1}}\rowcolor{\RowColorName}} % Shortcut for row colour
\newcommand{\mymulticolumn}[3]{\multicolumn{#1}{>{\columncolor{\RowColorName}}#2}{#3}} % For coloured multi-cols
\newcolumntype{x}[1]{>{\raggedright}p{#1}} % New column types for ragged-right paragraph columns
\newcommand{\tn}{\tabularnewline} % Required as custom column type in use

% Font and Colours
\definecolor{HeadBackground}{HTML}{333333}
\definecolor{FootBackground}{HTML}{666666}
\definecolor{TextColor}{HTML}{333333}
\definecolor{DarkBackground}{HTML}{800020}
\definecolor{LightBackground}{HTML}{FBF7F8}
\renewcommand{\familydefault}{\sfdefault}
\color{TextColor}

% Header and Footer
\pagestyle{fancy}
\fancyhead{} % Set header to blank
\fancyfoot{} % Set footer to blank
\fancyhead[L]{
\noindent
\begin{multicols}{3}
\begin{tabulary}{5.8cm}{C}
    \SetRowColor{DarkBackground}
    \vspace{-7pt}
    {\parbox{\dimexpr\textwidth-2\fboxsep\relax}{\noindent
        \hspace*{-6pt}\includegraphics[width=5.8cm]{/web/www.cheatography.com/public/images/cheatography_logo.pdf}}
    }
\end{tabulary}
\columnbreak
\begin{tabulary}{11cm}{L}
    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{9.1 Oxidation and reduction Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{Arsh.b} via \textcolor{DarkBackground}{\uline{cheatography.com/179523/cs/37883/}}}
\end{tabulary}
\end{multicols}}

\fancyfoot[L]{ \footnotesize
\noindent
\begin{multicols}{3}
\begin{tabulary}{5.8cm}{LL}
  \SetRowColor{FootBackground}
  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}Arsh.b \\
  \uline{cheatography.com/arsh-b} \\
  \end{tabulary}
\vfill
\columnbreak
\begin{tabulary}{5.8cm}{L}
  \SetRowColor{FootBackground}
  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Published 25th March, 2023.\\
   Updated 25th March, 2023.\\
   Page {\thepage} of \pageref{LastPage}.
\end{tabulary}
\vfill
\columnbreak
\begin{tabulary}{5.8cm}{L}
  \SetRowColor{FootBackground}
  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Sponsor}}  \\
  \SetRowColor{white}
  \vspace{-5pt}
  %\includegraphics[width=48px,height=48px]{dave.jpeg}
  Measure your website readability!\\
  www.readability-score.com
\end{tabulary}
\end{multicols}}




\begin{document}
\raggedright
\raggedcolumns

% Set font size to small. Switch to any value
% from this page to resize cheat sheet text:
% www.emerson.emory.edu/services/latex/latex_169.html
\footnotesize % Small font.

\begin{multicols*}{2}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Definitions}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{{\emph{Oxidation and reduction can be considered in terms of oxygen gain/hydrogen loss, electron transfer or change in oxidation number.}}} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{The definition that covers all types of redox (reduction-oxidation) reactions is based on the transfer of electrons.} \tn 
% Row Count 6 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{{\bf{Oxidation}} is the loss of electrons by a chemical species, and can be identified when:\{\{nl\}\}a species loses electrons\{\{nl\}\}a species loses hydrogen atoms\{\{nl\}\}a species gains oxygen atoms\{\{nl\}\}the oxidation state of an atom increases.} \tn 
% Row Count 11 (+ 5)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{{\bf{Reduction}} is the gain of electrons by a chemical species, and occurs when:\{\{nl\}\}a species Gaines electrons\{\{nl\}\}a species loses hydrogen atoms\{\{nl\}\}a species loses oxygen atoms\{\{nl\}\}the oxidation state of an atom decreases.} \tn 
% Row Count 16 (+ 5)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{{\emph{An oxidizing agent is reduced and a reducing agent is oxidised.}}} \tn 
% Row Count 18 (+ 2)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{An {\bf{oxidising agent}} is a substance that oxidises another substance and is reduced itself by gaining electrons.} \tn 
% Row Count 21 (+ 3)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{A {\bf{reducing agent}} is a substance that reduces another substance and is oxidised itself by losing electrons.} \tn 
% Row Count 24 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Half-equations}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{{\emph{ Identification of the species oxidized and reduced and the oxidizing and reducing agents, in redox reactions.}}} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{A {\bf{half-equation}} is an equation that shows the changes that happen in a redox reaction dude to either oxidation or reduction only.} \tn 
% Row Count 6 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{The {\bf{oxidation half-equation}} is a half-equation that shows only the chemical changes that happen in a redox reaction due to oxidation.} \tn 
% Row Count 9 (+ 3)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{The {\bf{reduction half-equation}} is a half-equation that shows only the chemical changes that happen in a redox reaction due to reduction.} \tn 
% Row Count 12 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Rules to write half-equations}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{Assign oxidation states to determine which atoms are being oxidized and which are being reduced.} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{Write half-equations for oxidation and reduction as follows:\{\{nl\}\}balance the atoms other than H and O\{\{nl\}\}balance each half-equation for O by adding H2O as needed\{\{nl\}\}balance each half-equation for H by adding H+ as needed\{\{nl\}\}balance each half-equation for charge by adding electrons to the sides with the more positive charge\{\{nl\}\}check that each half-equation is balanced for atoms and for charge} \tn 
% Row Count 11 (+ 9)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{Equalise the number of electrons in the two half-equations by multiplying each appropriately.} \tn 
% Row Count 13 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{Add the two half-equations together, cancelling out anything that is the same on both sides.} \tn 
% Row Count 15 (+ 2)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{{\bf{Balanced oxidation half-equations will have electrons on the product side. Balanced reduction half-equations will have electrons on the reactant side.}}} \tn 
% Row Count 19 (+ 4)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Rules for oxidation state}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{{\emph{Deduction of the oxidation states of an atom in an ion or compound.}}} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{{\bf{Oxidation state}} is a measure of how many electrons an atom has gained or lost when forming a compound.} \tn 
% Row Count 5 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{Atoms in the free (uncombined) element have an oxidation state of zero.} \tn 
% Row Count 7 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{In simple ions, the oxidation state is the same as the charge on the ion.} \tn 
% Row Count 9 (+ 2)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{The oxidation states of all the atoms in a neutral (uncharged) compound must add up to zero.} \tn 
% Row Count 11 (+ 2)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{The oxidation states of all the atoms in a polyatomic ion must add up to the charge on the ion.} \tn 
% Row Count 13 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{The usual oxidation state for an element is the same as the charge on its most common ion.} \tn 
% Row Count 15 (+ 2)
% Row 7
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{Most main group non-metals, the elements at the bottom of group 14, and transition elements have oxidation states that vary in different compounds – depending on the conditions and other elements present.} \tn 
% Row Count 20 (+ 5)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{1.596 cm} x{2.356 cm} x{3.648 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{3}{x{8.4cm}}{\bf\textcolor{white}{Common oxidation states}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{3}{x{8.4cm}}{{\emph{Deduction of the oxidation states of an atom in an ion or compound.}}} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\seqsplit{Substance} & Usual oxidation state & Exceptions \tn 
% Row Count 4 (+ 2)
% Row 2
\SetRowColor{LightBackground}
Group 1 metals & +1 &  \tn 
% Row Count 6 (+ 2)
% Row 3
\SetRowColor{white}
Group 2 metals & +2 &  \tn 
% Row Count 8 (+ 2)
% Row 4
\SetRowColor{LightBackground}
\seqsplit{Halogens} & -1 & (when Cl is combines with O or F) \tn 
% Row Count 10 (+ 2)
% Row 5
\SetRowColor{white}
Oxygen & -2 & Peroxides \tn 
% Row Count 11 (+ 1)
% Row 6
\SetRowColor{LightBackground}
\seqsplit{Hydrogen} & +1 & Metal hydrides \tn 
% Row Count 12 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}---}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Redox titration}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{A redox titration determines the concentration of an unknown solution by titrating it against a standard solution. A colour change associated with the redox reaction shows when the equivalence point has been reached.} \tn 
% Row Count 5 (+ 5)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Activity series}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{{\emph{The activity series ranks metals according to the ease with which they undergo oxidation.}}} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{8.4cm}}{Metals are ranked in the activity series according to how easily they lose electrons and are oxidized.} \tn 
% Row Count 5 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{8.4cm}}{The activity series can be used to predict whether or not a redox reaction that involves a metal can happen.} \tn 
% Row Count 8 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{4 cm} x{4 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Winkler Method}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{8.4cm}}{{\emph{The Winkler Method can be used to measure biochemical oxygen demand (BOD), used as a measure of the degree of pollution in a water sample.}}} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{8.4cm}}{{\bf{Biochemical oxygen demand}} (BOD) is the quantity of oxygen needed to break down organic matter in a sample of water over a 5-day period at a set temperature.} \tn 
% Row Count 7 (+ 4)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{8.4cm}}{A high BOD means that high levels of bacteria or algae are present in the water, resulting in a low level of dissolved oxygen.} \tn 
% Row Count 10 (+ 3)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{8.4cm}}{The {\bf{Winkler method}} uses a series of three redox reactions to determine the concentration of dissolved oxygen in a water sample.} \tn 
% Row Count 13 (+ 3)
% Row 4
\SetRowColor{LightBackground}
Dissolved oxygen reacts with Mn\textasciicircum{}2+\textasciicircum{} ions in basic conditions to form MnO2. & MnO2(s) + O2(aq) +4OH\textasciicircum{}-\textasciicircum{}(aq) -\textgreater{} 2MnO2(s) + 2H2O(l) \tn 
% Row Count 17 (+ 4)
% Row 5
\SetRowColor{white}
MnO2 reacts with I\textasciicircum{}-\textasciicircum{} in acidic conditions to form Mn\textasciicircum{}2+\textasciicircum{} & MnO2(s) + 2I\textasciicircum{}-\textasciicircum{}(aq) +4H\textasciicircum{}+\textasciicircum{}(aq) -\textgreater{} Mn\textasciicircum{}2+\textasciicircum{}(aq) + I2(aq) +2H2O(l) \tn 
% Row Count 21 (+ 4)
% Row 6
\SetRowColor{LightBackground}
I2 is titrated with S2O3\textasciicircum{}2-\textasciicircum{} to give I\textasciicircum{}-\textasciicircum{} and S4O6\textasciicircum{}2-\textasciicircum{} & 2S2O3\textasciicircum{}2–\textasciicircum{}(aq) + I\textasciicircum{}2\textasciicircum{}(aq) ➝ S4O6\textasciicircum{}2–\textasciicircum{}(aq) + 2I\textasciicircum{}–\textasciicircum{}(aq) \tn 
% Row Count 24 (+ 3)
% Row 7
\SetRowColor{white}
The moles of dissolved oxygen in the original solution can be calculated from the moles of S2O3\textasciicircum{}2-\textasciicircum{} used in the final reaction. & {\emph{n}}(S2O3\textasciicircum{}2–\textasciicircum{}) = 4{\emph{n}}(O2) \tn 
% Row Count 31 (+ 7)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}


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

\end{document}