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\author{Liliaeve}
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  /Title (chemistry-exam-2-unit-6.pdf)
  /Creator (Cheatography)
  /Author (Liliaeve)
  /Subject (Chemistry Exam 2: Unit 6 Cheat Sheet)
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    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Chemistry Exam 2: Unit 6 Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{Liliaeve} via \textcolor{DarkBackground}{\uline{cheatography.com/216606/cs/47372/}}}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}Liliaeve \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Not Yet Published.\\
   Updated 19th November, 2025.\\
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\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{3.833cm}}{\bf\textcolor{white}{Atomic Mass (atomic weight)}}  \tn
% Row 0
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\mymulticolumn{1}{x{3.833cm}}{weighted average mass of atoms of a given element} \tn 
% Row Count 1 (+ 1)
% Row 1
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% Row Count 2 (+ 1)
% Row 2
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\mymulticolumn{1}{x{3.833cm}}{amu = 1.66 x 10\textasciicircum{}-27\textasciicircum{}} \tn 
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\begin{tabularx}{3.833cm}{X}
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\mymulticolumn{1}{x{3.833cm}}{\bf\textcolor{white}{Formula Mass (formula weight)}}  \tn
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\mymulticolumn{1}{x{3.833cm}}{relative mass of an individual compound} \tn 
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% Row 1
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\mymulticolumn{1}{x{3.833cm}}{sum of the atomic weights of all the atoms in a compound} \tn 
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% Row 2
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\mymulticolumn{1}{x{3.833cm}}{\bf\textcolor{white}{Mole (mol)}}  \tn
% Row 0
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\mymulticolumn{1}{x{3.833cm}}{1 mole = 6.022 x 10\textasciicircum{}23\textasciicircum{} (atoms, molecules, or ions)} \tn 
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% Row 1
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\mymulticolumn{1}{x{3.833cm}}{Moles used most often to convert to {\bf{atoms}} or {\bf{compounds}}} \tn 
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% Row 2
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% Row 3
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% Row 4
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\begin{tabularx}{3.833cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{3.833cm}}{\bf\textcolor{white}{Limiting Reactant}}  \tn
% Row 0
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\mymulticolumn{1}{x{3.833cm}}{Chemistry questions that ask about theoretical yield (amount of product) or percent yield} \tn 
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% Row 1
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\mymulticolumn{1}{x{3.833cm}}{} \tn 
% Row Count 2 (+ 0)
% Row 2
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\mymulticolumn{1}{x{3.833cm}}{{\bf{Limiting reactant - the reactant that is completely used up in a reaction}}} \tn 
% Row Count 4 (+ 2)
% Row 3
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\mymulticolumn{1}{x{3.833cm}}{- the amount of product produced is dependent on the amount of starting materials or reactants} \tn 
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% Row 4
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\mymulticolumn{1}{x{3.833cm}}{- often one reactant will limit the reaction by getting completely used up and thus ending the reaction} \tn 
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% Row 5
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\mymulticolumn{1}{x{3.833cm}}{- thus, the number of moles of limiting reactant determines the number of moles of product that can form} \tn 
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% Row 6
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% Row 7
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\mymulticolumn{1}{x{3.833cm}}{All chemistry questions that use molar ratios from a chemical reaction equation to convert from one side of the reaction to the other, must include the following steps:} \tn 
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% Row 8
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\mymulticolumn{1}{x{3.833cm}}{{\bf{1. Write the complete balanced chemical reaction equation}}} \tn 
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% Row 9
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% Row 10
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% Row 11
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% Row 12
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% Row 13
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\mymulticolumn{1}{x{3.833cm}}{{\bf{3. Determine the theoretical yield = amount of product}}} \tn 
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% Row 14
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\mymulticolumn{1}{x{3.833cm}}{a. based on the limiting reactant} \tn 
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% Row 15
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\mymulticolumn{1}{x{3.833cm}}{{\bf{4. Determine the percent yield of the product}}} \tn 
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% Row 16
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\mymulticolumn{1}{x{3.833cm}}{a. based on the theoretical yield} \tn 
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\mymulticolumn{1}{x{3.833cm}}{\bf\textcolor{white}{Limiting Reactant (cont)}}  \tn
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\mymulticolumn{1}{x{3.833cm}}{\bf\textcolor{white}{Avogadro's \#}}  \tn
% Row 0
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% Row 1
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\mymulticolumn{1}{x{3.833cm}}{Used to convert *particles to moles (and vice versa)} \tn 
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% Row 3
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% Row 4
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% Row 5
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% Row 0
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% Row 1
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% Row 0
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% Row 1
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% Row 2
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\mymulticolumn{1}{x{3.833cm}}{OR} \tn 
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% Row 3
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\mymulticolumn{1}{x{3.833cm}}{mol / g} \tn 
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% Row 4
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\mymulticolumn{1}{x{3.833cm}}{{\bf{Element:}} molar mass = atomic mass} \tn 
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% Row 5
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\begin{tabularx}{3.833cm}{p{0.3433 cm} p{0.3433 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{3.833cm}}{\bf\textcolor{white}{Types of Chemistry Problems}}  \tn
% Row 0
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\mymulticolumn{2}{x{3.833cm}}{{\bf{Problem type \#1}}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{the provided information includes the amount (such as mass or moles) of one reactant and no information about the second reactant} \tn 
% Row Count 4 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{the limiting reactant is assumed to be the reactant whose amount was provided. Any assumption made should be stated in the answer to the problem} \tn 
% Row Count 7 (+ 3)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{{\bf{no calculations are necessary}}} \tn 
% Row Count 8 (+ 1)
% Row 4
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\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 8 (+ 0)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{{\bf{Problem type \#2}}} \tn 
% Row Count 9 (+ 1)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{the provided information includes the amount (such as mass or moles) of one reactant and the second reactant is in excess} \tn 
% Row Count 12 (+ 3)
% Row 7
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{the limiting reactant is automatically the reactant whose amount was provided, as "in excess" means there is an unlimited amount present of that reactant} \tn 
% Row Count 16 (+ 4)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{{\bf{no calculations are necessary}}} \tn 
% Row Count 17 (+ 1)
% Row 9
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 17 (+ 0)
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{{\bf{Problem type \#3}}} \tn 
% Row Count 18 (+ 1)
% Row 11
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{the provided information includes the amount (such as mass or moles) of both reactants} \tn 
% Row Count 20 (+ 2)
% Row 12
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{the limiting reactant could be either reactant} \tn 
% Row Count 21 (+ 1)
% Row 13
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{{\bf{calculations must be performed to determine which one}}} \tn 
% Row Count 23 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
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\begin{tabularx}{3.833cm}{x{1.09856 cm} x{2.33444 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{3.833cm}}{\bf\textcolor{white}{Ionic Compounds}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{since inoic compounds are held together through electrostatic interactions, only {\bf{physical}} means are needed to separate them} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 3 (+ 0)
% Row 2
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\mymulticolumn{2}{x{3.833cm}}{Atoms are balance in ionic compounds and molecules} \tn 
% Row Count 4 (+ 1)
% Row 3
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\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 4 (+ 0)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{{\bf{Potassium oxide}}} \tn 
% Row Count 5 (+ 1)
% Row 5
\SetRowColor{white}
Cation: & K+ \tn 
% Row Count 6 (+ 1)
% Row 6
\SetRowColor{LightBackground}
Anion: & O\textasciicircum{}-2\textasciicircum{} \tn 
% Row Count 7 (+ 1)
% Row 7
\SetRowColor{white}
Goal: & no overall charge \tn 
% Row Count 8 (+ 1)
% Row 8
\SetRowColor{LightBackground}
Formula: & K\textasciitilde{}2\textasciitilde{}O \tn 
% Row Count 9 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
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\mymulticolumn{2}{x{3.833cm}}{\bf\textcolor{white}{Covalent Compounds}}  \tn
% Row 0
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\mymulticolumn{2}{x{3.833cm}}{Breaking a covalent bond requires a chemical reaction. For atoms of a molecule to be separated, bonds must be broken and new bonds must be formed} \tn 
% Row Count 3 (+ 3)
% Row 1
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\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 3 (+ 0)
% Row 2
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\mymulticolumn{2}{x{3.833cm}}{{\bf{Methane}}} \tn 
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% Row 3
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Elements: & C \& H \tn 
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% Row 4
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Atoms: & 1C \& 4H \tn 
% Row Count 6 (+ 1)
% Row 5
\SetRowColor{white}
Goal: & octet rule as possible \tn 
% Row Count 7 (+ 1)
% Row 6
\SetRowColor{LightBackground}
Formula & CH\textasciitilde{}4\textasciitilde{} \tn 
% Row Count 8 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
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\begin{tabularx}{3.833cm}{p{0.51495 cm} x{2.91805 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{3.833cm}}{\bf\textcolor{white}{Percent Yield}}  \tn
% Row 0
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\mymulticolumn{2}{x{3.833cm}}{{\bf{Percent yield (\%) =}}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{actual yield (g) / theoretical yield (g) x 100\%} \tn 
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% Row 2
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\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 2 (+ 0)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{{\bf{Theoretical yield or expected yield}}} \tn 
% Row Count 3 (+ 1)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{amount of product expected from a given amount of reactant based on the coefficients in the {\bf{balanced}} chemical equation} \tn 
% Row Count 6 (+ 3)
% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 6 (+ 0)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{{\bf{Actual yield or experimental yield}}} \tn 
% Row Count 7 (+ 1)
% Row 7
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{amount of product isolated from a reaction} \tn 
% Row Count 8 (+ 1)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 8 (+ 0)
% Row 9
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{{\bf{Percent Yield (\%)}}} \tn 
% Row Count 9 (+ 1)
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{indicates the quantity of product produced} \tn 
% Row Count 10 (+ 1)
% Row 11
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 10 (+ 0)
% Row 12
\SetRowColor{LightBackground}
Step 1. & determine the limiting reactant (LR) (method 1 or 2) \tn 
% Row Count 12 (+ 2)
% Row 13
\SetRowColor{white}
Step 2. & determine the theoretical yield of each product separately using the mass of the LR \tn 
% Row Count 15 (+ 3)
% Row 14
\SetRowColor{LightBackground}
Step 3. & Determine the percent yield of each product separately using the theoretical yields calculated in step 2 and the actual yields provided \tn 
% Row Count 19 (+ 4)
% Row 15
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 19 (+ 0)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
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\begin{tabularx}{3.833cm}{x{1.09856 cm} x{2.33444 cm} }
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\mymulticolumn{2}{x{3.833cm}}{\bf\textcolor{white}{Polyatomic Ions}}  \tn
% Row 0
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\mymulticolumn{2}{x{3.833cm}}{{\bf{Calcium Acetate}}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
Cation: & Ca\textasciicircum{}2+\textasciicircum{} \tn 
% Row Count 2 (+ 1)
% Row 2
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Anion: & CH\textasciitilde{}3\textasciitilde{}CO\textasciitilde{}2-\textasciitilde{} \tn 
% Row Count 3 (+ 1)
% Row 3
\SetRowColor{white}
Goal: & no overall charge \tn 
% Row Count 4 (+ 1)
% Row 4
\SetRowColor{LightBackground}
Formula: & Ca(CH\textasciitilde{}3\textasciitilde{}CO\textasciitilde{}2\textasciitilde{})\textasciitilde{}2\textasciitilde{} \tn 
% Row Count 5 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{3.833cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{3.833cm}}{\bf\textcolor{white}{Balancing Chemical Reaction Equations}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{3.833cm}}{{\bf{Stoichiometry}} - used to balance chemical equations} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{3.833cm}}{- matter can neither be created nor destroyed} \tn 
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% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{3.833cm}}{- the same number of atoms of every element must be on both sides of the equation} \tn 
% Row Count 5 (+ 2)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{3.833cm}}{} \tn 
% Row Count 5 (+ 0)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{3.833cm}}{{\bf{Steps to balance a chemical reaction:}}} \tn 
% Row Count 6 (+ 1)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{3.833cm}}{1. write the equation with the correct chemical formulas for the reactants and products} \tn 
% Row Count 8 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{3.833cm}}{1. determine if the equation is balanced by counting the number of atoms of each element on both sides of the equation} \tn 
% Row Count 11 (+ 3)
% Row 7
\SetRowColor{white}
\mymulticolumn{1}{x{3.833cm}}{3. balance the equation using coefficients one element at a time} \tn 
% Row Count 13 (+ 2)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{3.833cm}}{4. check to ensure that the smallest whole numbers have been used as coefficients} \tn 
% Row Count 15 (+ 2)
% Row 9
\SetRowColor{white}
\mymulticolumn{1}{x{3.833cm}}{5. double check that the equation is now balanced by counting the number of atoms of each element on both sides of the equation} \tn 
% Row Count 18 (+ 3)
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{3.833cm}}{} \tn 
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% Row 11
\SetRowColor{white}
\mymulticolumn{1}{x{3.833cm}}{Balancing chemical reactions with {\bf{Polyatomic ions}}:} \tn 
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% Row 12
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{3.833cm}}{1. if the bonds in polyatomic ions are {\bf{NOT}} broken during the reaction (same on both sides of the equation), then treat the polyatomic ion as a unit} \tn 
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% Row 13
\SetRowColor{white}
\mymulticolumn{1}{x{3.833cm}}{2. if the bonds in polyatomic ions {\bf{ARE}} broken during the reaction (not the same on both sides of the equation), then separate out all of the elements for balancing} \tn 
% Row Count 28 (+ 4)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{3.833cm}{p{0.3433 cm} p{0.3433 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{3.833cm}}{\bf\textcolor{white}{Percent Error}}  \tn
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\mymulticolumn{2}{x{3.833cm}}{indicates the quality of the data produced} \tn 
% Row Count 1 (+ 1)
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\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{{\bf{Percent error (\%)}}} \tn 
% Row Count 2 (+ 1)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{{[}theoretical value (g/mol) - experimental value (g/mol){]} / {[}theoretical value (g/mol){]} x 100\%} \tn 
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% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{} \tn 
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% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{{\bf{Accepted value or theoretical value}}} \tn 
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% Row 5
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{value determined from other scientists doing the same experiement with multiple replicates or the actual value of an unknown made for you} \tn 
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% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{} \tn 
% Row Count 8 (+ 0)
% Row 7
\SetRowColor{white}
\mymulticolumn{2}{x{3.833cm}}{{\bf{Actual value or experimental value}}} \tn 
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% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{3.833cm}}{value determined from your own experimentation} \tn 
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\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}


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

\end{document}