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% Document Info
\author{anniemeow}
\pdfinfo{
  /Title (cs36510.pdf)
  /Creator (Cheatography)
  /Author (anniemeow)
  /Subject (0000000 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{0000000 Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{anniemeow} via \textcolor{DarkBackground}{\uline{cheatography.com/173776/cs/36510/}}}
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\noindent
\begin{multicols}{3}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}anniemeow \\
  \uline{cheatography.com/anniemeow} \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Not Yet Published.\\
   Updated 14th January, 2023.\\
   Page {\thepage} of \pageref{LastPage}.
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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
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\begin{document}
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% www.emerson.emory.edu/services/latex/latex_169.html
\footnotesize % Small font.

\begin{multicols*}{3}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Understandings}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{- Atoms of different elements combine in fixed ratios to form compounds which have different propertied from their component elements. \newline % Row Count 3 (+ 3)
 - Mixtures contain more than one element and/or compound that are not chemically bonded together and so retain their individual properties. \newline % Row Count 6 (+ 3)
 - Mixtures are either homogeneous or heterogeneous.% Row Count 8 (+ 2)
} \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}{1.1 Intro to the Particulate Nature of Matter}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{States of Matter:}} \newline % Row Count 1 (+ 1)
 - There are 3 (excluding plasma) states of matter: \newline % Row Count 3 (+ 2)
     1. Solid \newline % Row Count 4 (+ 1)
     2. Liquid \newline % Row Count 5 (+ 1)
     3. Gas \newline % Row Count 6 (+ 1)
{\bf{Temperature:}} \newline % Row Count 7 (+ 1)
 - The SI unit for temperature is {\bf{kelvin (K)}} \newline % Row Count 8 (+ 1)
temperature (K) = temperature (Celcius) + 273.15 \newline % Row Count 9 (+ 1)
{\bf{Ions:}}  \newline % Row Count 10 (+ 1)
An {\bf{ion}} is a charged species. {\bf{Anions}} are negatively charged and {\bf{cations}} are positively charged. \newline % Row Count 13 (+ 3)
 - you can remember this by remembering "CATions are PAWSitive" \newline % Row Count 15 (+ 2)
{\bf{The Atom Economy:}} \newline % Row Count 16 (+ 1)
The Atom Economy looks at the level of efficiency of chemical reactions by comparing the molecular mass of atoms in the reactants with the molecular mass of useful compounds. \newline % Row Count 20 (+ 4)
percentage of atom economy = molecular mass of atoms of useful products/molecular mass of atoms in reactants x 100\%% Row Count 23 (+ 3)
} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
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\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{1.1 Intro to the Particulate Nature of Matter}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{States of Matter:}} \newline % Row Count 1 (+ 1)
 - There are 3 (excluding plasma) states of matter: \newline % Row Count 3 (+ 2)
     1. Solid \newline % Row Count 4 (+ 1)
     2. Liquid \newline % Row Count 5 (+ 1)
     3. Gas \newline % Row Count 6 (+ 1)
{\bf{Temperature:}} \newline % Row Count 7 (+ 1)
 - The SI unit for temperature is {\bf{kelvin (K)}} \newline % Row Count 8 (+ 1)
temperature (K) = temperature (Celcius) + 273.15 \newline % Row Count 9 (+ 1)
{\bf{Ions:}}  \newline % Row Count 10 (+ 1)
An {\bf{ion}} is a charged species. {\bf{Anions}} are negatively charged and {\bf{cations}} are positively charged. \newline % Row Count 13 (+ 3)
 - you can remember this by remembering "CATions are PAWSitive" \newline % Row Count 15 (+ 2)
{\bf{The Atom Economy:}} \newline % Row Count 16 (+ 1)
The Atom Economy looks at the level of efficiency of chemical reactions by comparing the molecular mass of atoms in the reactants with the molecular mass of useful compounds. \newline % Row Count 20 (+ 4)
percentage of atom economy = molecular mass of atoms of useful products/molecular mass of atoms in reactants x 100\%% Row Count 23 (+ 3)
} \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}{1.1 Intro to the Particulate Nature of Matter}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{States of Matter:}} \newline % Row Count 1 (+ 1)
 - There are 3 (excluding plasma) states of matter: \newline % Row Count 3 (+ 2)
     1. Solid \newline % Row Count 4 (+ 1)
     2. Liquid \newline % Row Count 5 (+ 1)
     3. Gas \newline % Row Count 6 (+ 1)
{\bf{Temperature:}} \newline % Row Count 7 (+ 1)
 - The SI unit for temperature is {\bf{kelvin (K)}} \newline % Row Count 8 (+ 1)
temperature (K) = temperature (Celcius) + 273.15 \newline % Row Count 9 (+ 1)
{\bf{Ions:}}  \newline % Row Count 10 (+ 1)
An {\bf{ion}} is a charged species. {\bf{Anions}} are negatively charged and {\bf{cations}} are positively charged. \newline % Row Count 13 (+ 3)
 - you can remember this by remembering "CATions are PAWSitive" \newline % Row Count 15 (+ 2)
{\bf{The Atom Economy:}} \newline % Row Count 16 (+ 1)
The Atom Economy looks at the level of efficiency of chemical reactions by comparing the molecular mass of atoms in the reactants with the molecular mass of useful compounds. \newline % Row Count 20 (+ 4)
percentage of atom economy = molecular mass of atoms of useful products/molecular mass of atoms in reactants x 100\%% Row Count 23 (+ 3)
} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
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\par\addvspace{1.3em}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{1.2 The Mole Concept}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Relative Atomic Mass, Relative Formula Mass, and Molar Mass}} \newline % Row Count 2 (+ 2)
 - {\bf{Isotopes}} are atoms of the same element that have the same number of protons in the nucleus but different numbers of neutrons. \newline % Row Count 5 (+ 3)
 - {\bf{relative abundance}} of each isotope is a measure of the percentage that occurs in a sample of the element. \newline % Row Count 8 (+ 3)
 - {\bf{Relative Atomic Mass}} a weighted average of the atomic masses of its isotopes. \newline % Row Count 10 (+ 2)
 - {\bf{Relative Molecular Mass}} (Relative Formula Mass) combining the {\bf{Relative Atomic Mass}} values of the individual atoms or ions \newline % Row Count 13 (+ 3)
 - {\bf{Molar Mass}} is the mass of one mole of substance \newline % Row Count 15 (+ 2)
 - A mole (Avogadro's constant, L) is 6.02x10\textasciicircum{}23 \newline % Row Count 16 (+ 1)
{\bf{Mole Calculations}} \newline % Row Count 17 (+ 1)
no. of particles x L = moles \newline % Row Count 18 (+ 1)
moles x molar mass = mass (g) \newline % Row Count 19 (+ 1)
{\bf{Experimental Empirical and Molecular Formula Determination}} \newline % Row Count 21 (+ 2)
 - {\bf{Qualitative analysis}}: what elements are present within the substance, and what is the purity of the substance \newline % Row Count 24 (+ 3)
 - {\bf{Quantitative Analysis}}: what is the relative mass, and what is the exact composition \newline % Row Count 26 (+ 2)
 - {\bf{Empirical Formula}} is the simplest whole number ratio of atoms or amount of each element present in a compound. \newline % Row Count 29 (+ 3)
 - {\bf{Molecular Formula}} the actual number of atoms or amount of each element present in a compound.% Row Count 31 (+ 2)
} \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}{1.3 Reacting Masses and Volumes}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{The Limiting Reagent}} \newline % Row Count 1 (+ 1)
 - the {\bf{Liniting Reagent}} is the reactant that will be completely consumed during the reaction (it is usually the more expensive one) \newline % Row Count 4 (+ 3)
{\bf{Theoretical and Experimental Yields}} \newline % Row Count 5 (+ 1)
 - the {\bf{theoretical yield}} is the expected amount of products which is theoretically possible if the reaction is done under ideal conditions. \newline % Row Count 8 (+ 3)
 - the {\bf{experimental yield}} is the actual amount of product produced during experimentation. \newline % Row Count 10 (+ 2)
 - {\bf{percentage yield}}=experimental yield/theoretical yield \newline % Row Count 12 (+ 2)
{\bf{The Limiting Reagent}} \newline % Row Count 13 (+ 1)
 - the {\bf{Liniting Reagent}} is the reactant that will be completely consumed during the reaction (it is usually the more expensive one) \newline % Row Count 16 (+ 3)
{\bf{Avogadro's Law and the Molar Volume of Gases}} \newline % Row Count 17 (+ 1)
The Kinetic Theory of Gases: \newline % Row Count 18 (+ 1)
1. Gases are made up of very small particles, separated by large distances. Most of the volume occupied by a gas is empty space. \newline % Row Count 21 (+ 3)
2. Gaseous particles are constantly moving in straight lines, but random directions \newline % Row Count 23 (+ 2)
3. Gaseous particles undergo elastic collisions with eachother and the walls of the container. No loss of kinetic energy occurs \newline % Row Count 26 (+ 3)
4. Gaseous particles exert no force of attraction on other gases.  \newline % Row Count 28 (+ 2)
Under conditions of {\bf{ Standard Temperature and Pressure (STP)}} an ideal gas obeys the four postulates stated above.  \newline % Row Count 31 (+ 3)
} \tn 
\end{tabularx}
\par\addvspace{1.3em}

\vfill
\columnbreak
\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{1.3 Reacting Masses and Volumes (cont)}}  \tn
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{ - The molar volume of any gas is identical at a given temperature and pressure. \newline % Row Count 2 (+ 2)
{\bf{The Gas Laws}} \newline % Row Count 3 (+ 1)
 - Pressure is inversely proportional to 1/volume \newline % Row Count 4 (+ 1)
 - pressure 1 x volume 1 = pressure 2 x volume 2 \newline % Row Count 5 (+ 1)
 - volume 1/temperature 1 = volume 2/temperature 2 \newline % Row Count 7 (+ 2)
pV = nRT \newline % Row Count 8 (+ 1)
pressure x volume = number of moles x ideal gas constant x temperature \newline % Row Count 10 (+ 2)
{\bf{Concentration}} \newline % Row Count 11 (+ 1)
 - {\bf{Solution}} is a homogeneous mixture of a {\bf{solute}} that has been dissolved in a {\bf{solvent}}. \newline % Row Count 13 (+ 2)
 - concentration = no. of moles/volume% Row Count 14 (+ 1)
} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}


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

\end{document}