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\author{VanessaG}
\pdfinfo{
  /Title (genchem-i-chem-121-mega-review.pdf)
  /Creator (Cheatography)
  /Author (VanessaG)
  /Subject (GenChem I (CHEM 121) Mega Review Cheat Sheet)
}

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    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{GenChem I (CHEM 121) Mega Review Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{VanessaG} via \textcolor{DarkBackground}{\uline{cheatography.com/32617/cs/13440/}}}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}VanessaG \\
  \uline{cheatography.com/vanessag} \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Not Yet Published.\\
   Updated 7th December, 2017.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
  www.readability-score.com
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\mymulticolumn{4}{x{8.4cm}}{\bf\textcolor{white}{UNIT 1 -{}- Concepts!}}  \tn
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Proving atoms exist & integer ratios (= represent units of mass= atoms) &  &  \tn 
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Law of \seqsplit{conservation} of mass & atoms/are not created nor destroyed only \seqsplit{rearranged} &  &  \tn 
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Atomic Molecular Theory & All matter is made up of atoms & Elements can't be \seqsplit{decomposed} into simpler \seqsplit{substances} , composed of identical atoms, all elements are defined = elements are composed of atoms & Compounds are chemical \seqsplit{substances} of elements \tn 
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 & \#s and masses of atoms are conserved in a chemical RXN & Compounds are composed of molecules & Atoms of the same element are identical \seqsplit{(=identical} mass) \tn 
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All atoms of a single element have the same \seqsplit{characteristic} mass. & Each compound consists of identical molecules, which are small, identical particles formed of atoms combined in simple whole number ratios. & The number and masses of these atoms do not change during a chemical \seqsplit{transformation}.     Each element is composed of very small, identical particles called atoms. & Each small atom is \seqsplit{surrounded} by molecules, which allow bonds to form between \seqsplit{neighboring} atoms. \tn 
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Law of {\bf{definite}} \seqsplit{Proportions} (aka LAw of Constant \seqsplit{Compositions)} & elements combine in definite \seqsplit{proportions} {\emph{by mass}} to make a certain compound & compound composed of {\emph{fixed ratio}} of elements by {\bf{mass}} & {\emph{NO INTEGERS}} \tn 
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 & Same compund {\bf{{\emph{do not}}}} compare {\emph{different}} compounds &  &  \tn 
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Law of {\bf{Multiple}} \seqsplit{Proportions} & compare multiple compounds made of the {\bf{{\emph{same}}}} elements if we fix the mass of one element, the other elements' masses across those compounds will be related in a simple integer ratio & must include examples where a specific \seqsplit{element/atom} bonds to the same element with different simple integer ratios & {\emph{INTEGERS}} \tn 
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Law of Combining {\bf{Volumes}} & At fixed temp and pressure gases combine in simple integer ratios by volume & \seqsplit{Avogadro's} Law= At a fixed Temp and Presure {\emph{equal volumes}} of gases contain {\emph{equal \#s of particles}} &  \tn 
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\mymulticolumn{4}{x{8.4cm}}{Diatomic particle : H2 O2 N2 F2 Cl2 Br2 I2} \tn 
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\seqsplit{Rutherfords's} gold foil \seqsplit{experiment} & alpha particles shot through a thin gold foil sheet  \{\{nl\}\} &  &  \tn 
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 & most went straight through = atoms are mostly made of empty space & some slightly \seqsplit{deflected=} \seqsplit{positively} charged nucleus & very few bounced back= \tn 
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Mosely's Xray frequency data & sqrt of frequency is \seqsplit{prportional} to atmoic number & = atomic number measures \# protons since &  \tn 
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Emperical Formula & simplify ratios?? & P4O10=P2O5 &  \tn 
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Molecular Formula & as is no \seqsplit{simplification} &  &  \tn 
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\seqsplit{Determining} {\bf{moles}} & M=n/V & where M = Molarity \{\{nl\}\} n = moles (of solute) \{\{nl\}\} V = volume in liters (in solution) &  \tn 
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\seqsplit{Rutherfords's} gold foil \seqsplit{experiment} \{\{nl\}\} alpha particles shot through a thin gold foil sheet & most alpha particels went straight through = atoms are mostly made of empty space & some slightly \seqsplit{deflected=} \seqsplit{positively} charged nucleus & very few bounced \seqsplit{back=nucleus} is much more massice than alpha particle and really small in position \tn 
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\mymulticolumn{4}{x{8.4cm}}{nuclei are {\bf{tiny}} {\bf{positively}} charged {\bf{small}} and {\bf{massive}}} \tn 
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Mosely's Xray frequency data & sqrt of frequency is \seqsplit{prportional} to atmoic number = atomic number measures \# protons since & integer units - counting something = protons \{\{nl\}\} \seqsplit{courelated} mass &  \tn 
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\seqsplit{Ionization} Energy & minimum amount of energy required to remove an electron \{\{IE felt relative to specific electron\}\} & {\bf{COULOMBS LAW}} \{\{nl\}\} V(r)=(q1 * q2)/r &  \tn 
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 &  & V(r) is potential energy \{\{nl\}\} negative because opposite charges attract 	\{\{nl\}\} Positive when salike chgs repel &  \tn 
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 & Periodic trend: & left to right -\textgreater{} \{\{nl\}\} charges increase PE & \{\{nl\}\} top to bottom: radius increases lowering PE \{\{nl\}\} \seqsplit{decreasing} IE \tn 
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\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Ionization Energy Graph}}  \tn
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\seqsplit{Ionization} Energy (con't) & electron electron repulsion decreases ionization energy of electron &  &  \tn 
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\seqsplit{Successive} IE & large drop indicates new shell e\textasciicircum{}-\textasciicircum{} must be removed from &  &  \tn 
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\seqsplit{Photoelectric} effect & E=hv \{\{nl\}\} where v is frequency and h is Planck's constant & c=lambda* frequency \{\{nl\}\} lambda is frequency & E = \seqsplit{(hc)/λ} \tn 
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 & Planck's constant (h)= \{\{nl\}\} speed of light (c)= \{\{nl\}\} &  &  \tn 
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 & Rydberg's equation : \{\{nl\}\} Rydberg's constant: 1.097x10\textasciicircum{}-7\textasciicircum{} \{\{nl\}\} &  &  \tn 
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More intense light above \seqsplit{threshold	frequency} produces more electrons, greater current & More \seqsplit{intense	light	above} threshold frequency does not \seqsplit{produce	electrons	with	greater} kinetic energy & When intensity is \seqsplit{fixed:presence} of threshold frequency implies \seqsplit{relationship} between frequency and energy – if light is above frequency threshold, the current remains fixed & Kinetic energy of electrons increases when frequency is increased – simple linear \seqsplit{relationship} \tn 
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§ Summary of \seqsplit{experimental} results: light which has \seqsplit{sufficiently} high \seqsplit{frequency	will} eject electrons whether the \seqsplit{intensity	is} low or high– & {\bf{increasing intensity gives more electrons	}}but not more energetic \seqsplit{electrons–} & {\bf{increasing frequency gives more energetic electrons}} but not more of them &  \tn 
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\begin{tabularx}{8.4cm}{x{1.8 cm} x{1.656 cm} x{1.872 cm} x{1.872 cm} }
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frequency of light = color of light and amount of energy carried & \seqsplit{intensity} of light = number of e\textasciicircum{}-\textasciicircum{} & KE of electron = increases as frequency increases and {\emph{not}} affected by intensity & current = affected by intensity (increase current there is an increase \seqsplit{intensity)} \{\{nl\}\} \seqsplit{unaffected} by chnage in frequency \tn 
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\mymulticolumn{4}{x{8.4cm}}{must reach {\bf{threshold frequency}} of no electrons will be emitted}  \tn 
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Photo \seqsplit{emmision} & electrons jump down energy levels emmit light \{\{nl\}\} light absorbed when electrons jump up (get excited) & specific \seqsplit{frequencies} of light emitted because between specific energy levels and energy is quantized {\bf{{\emph{}}}}{\emph{*}} &  \tn 
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\seqsplit{quantum} \seqsplit{numbers} & n= size \{\{nl\}\} {\bf{1}}s, {\bf{2}}p {\bf{3}}d & l= shape \{\{nl\}\} 1{\bf{s}}, 2{\bf{p}}, 3{\bf{d}} \{\{nl\}\} 0 to n-1 & m(l) = \{\{noshy\}\}orientation \{\{nl\}\} (ex: 2p-x, 2p-y, 3d-xy) \{\{nl\}\} m(s) = spin + 1/2 -1/2 \{\{nl\}\} Range: -l to +l \tn 
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\seqsplit{Rydberg} \seqsplit{equation} & n=shell  n1= 1st energy shell n2= second enrgy shell  mn & use to calculate Energy emitted when e\textasciicircum{}-\textasciicircum{} moves between shells &  \tn 
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 & (if E(light) fixed) \{\{nl\}\} \seqsplit{E(light)=hv} = IE(e\textasciicircum{}-\textasciicircum{})+IE(e\textasciicircum{}-\textasciicircum{}) &  &  \tn 
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{\bf{Visisble}} light range & \textasciitilde{}400-750 ish & \seqsplit{Ultraviolet} - lower energy less than \textasciitilde{} 375nm & Infrared - higher \seqsplit{frequencies} past \textasciitilde{}800 \tn 
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\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Rydberg Equation}}  \tn
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\mymulticolumn{1}{x{8.4cm}}{(1.097x10\textasciicircum{}7\textasciicircum{})m\textasciicircum{}-1\textasciicircum{} = Rydberg's constant}  \tn 
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LEWIS DOT STRUCTURES & A: Available (valence electrons (number of atoms)) \{\{nl\}\} N: Needed (8(nuber of element)+ 2(number of element) )\{\{nl\}\} B: S/2 \{\{nl\}\} S: N-A \{\{nl\}\} U: \{\{nl\}\} &  &  \tn 
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 & 8 - octet if follow octet rule \{\{nl\}\} 2 for duet if follow duet rule &  &  \tn 
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Core Charge & \# protons (atomic number) - \# inner shell electrons &  &  \tn 
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 & CAN calculate for e\textasciicircum{}-\textasciicircum{} added and use to figure which has a greater electron affinity &  &  \tn 
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Formal Charge & valence electrons - bonds- lone electrons ({\emph{not lone pairs}}) &  &  \tn 
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Finding Limiting reagent & take moles of substance A and find how many moles of B gotten & take moles of substance B and find moles of substance A needed & compare moles of each substance \tn 
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 & moles A/1 * moles B/moles A (in \seqsplit{equation)=} moles B needed & moles B/1 * moles A/moles B (in \seqsplit{equation)=} moles A needed & moles A : moles B \seqsplit{(calcuated)} \{\{nl\}\} mol A: mole B in equation \tn 
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Finding \seqsplit{Emperical} formula & find moles of each substance & find \seqsplit{corresponding} element's moles based off of &  \tn 
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\seqsplit{emperical} formulas in \seqsplit{combustion} & * calculate g of C and H and subtract from original \seqsplit{compound's} mass which gives O's mass & then calculate moles of O & compare ratio of C:H:O \{\{nl\}\} and this gives empirical sub numbers \tn 
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Finding \seqsplit{molecular} formula & after \seqsplit{calculating} Emperical, given molecular weight divide by that of Emperical & multiply ratios by this for sub numbers &  \tn 
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Bond Order & $\frac{1}{2}$ (\# electrons \seqsplit{bonding-\#electrons} \seqsplit{antibonding)} &  &  \tn 
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Proving Law of Multiple \seqsplit{proportions} & fix one element and &  &  \tn 
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\vfill
\columnbreak
\begin{tabularx}{8.4cm}{x{1.656 cm} x{1.8 cm} x{1.872 cm} x{1.872 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{4}{x{8.4cm}}{\bf\textcolor{white}{Calculations (cont)}}  \tn
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{4}{x{8.4cm}}{OXIDATION RULES} \tn 
% Row Count 1 (+ 1)
% Row 11
\SetRowColor{white}
Molarity & =mol/L &  &  \tn 
% Row Count 2 (+ 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}{Oxidation Rules}}  \tn
\SetRowColor{LightBackground}
\mymulticolumn{1}{p{8.4cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/vanessag_1512584836_Oxidation rules -- Open stax.PNG}}} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{Crystalline Structures}}  \tn
\SetRowColor{LightBackground}
\mymulticolumn{1}{p{8.4cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/vanessag_1512585250_Crystalline solids -- open stax.PNG}}} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{1.512 cm} x{2.088 cm} x{2.88 cm} p{0.72 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{4}{x{8.4cm}}{\bf\textcolor{white}{Bonds \textasciitilde{} metallic ionic covalent}}  \tn
% Row 0
\SetRowColor{LightBackground}
\seqsplit{metallic} bonding & between two metals & low EA/ IE/ EN &  \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
ionic bonding & forms salts (nonmetal and metal) &  &  \tn 
% Row Count 5 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\seqsplit{metallic} solids & shiny \{\{nl\}\} conductors \{\{nl\}\} insoluble in water \{\{nl\}\} "ductile" \{\{nl\}\} malleable \seqsplit{moderate-high} melting points &  &  \tn 
% Row Count 16 (+ 11)
% Row 3
\SetRowColor{white}
ionic solid  -{}- salts & hard and brittle \{\{nl\}\} white \{\{nl\}\} soluble in water \{\{nl\}\} {\emph{not}} good conductor (unless in solution \seqsplit{(dissolved)} or melted) \{\{nl\}\} {\emph{very}} high melting point &  &  \tn 
% Row Count 31 (+ 15)
\end{tabularx}
\par\addvspace{1.3em}

\vfill
\columnbreak
\begin{tabularx}{8.4cm}{x{1.512 cm} x{2.088 cm} x{2.88 cm} p{0.72 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{4}{x{8.4cm}}{\bf\textcolor{white}{Bonds \textasciitilde{} metallic ionic covalent (cont)}}  \tn
% Row 4
\SetRowColor{LightBackground}
\seqsplit{covalent} solids & hard \{\{nl\}\} high melting points & high IE/EN/EA? &  \tn 
% Row Count 3 (+ 3)
% Row 5
\SetRowColor{white}
\seqsplit{molecular} solids & soft \{\{nl\}\} low melting pt &  &  \tn 
% Row Count 6 (+ 3)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{4}{x{8.4cm}}{} \tn 
% Row Count 6 (+ 0)
% Row 7
\SetRowColor{white}
\seqsplit{metallic} solids & shiny because... \{\{nl\}\} band theory where the d and s electron energy levels are so close together  adn in a lattice there are so many and they are so close they seem to form almost a band that has many energy levels for electrons to jump to. & malleable because in the lattice the electrons are delocalized while the nuclei are not. This means that when  manipulated the electons can freely move making the structure malleable &  \tn 
% Row Count 28 (+ 22)
\hhline{>{\arrayrulecolor{DarkBackground}}----}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{8.4cm}}{\bf\textcolor{white}{unit cells}}  \tn
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\mymulticolumn{1}{p{8.4cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/vanessag_1510075762_unit cell faces.JPG}}} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{3.84 cm} x{4.16 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Webassign questions to look at}}  \tn
% Row 0
\SetRowColor{LightBackground}
{\bf{Webassign}} & {\bf{Question}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
HW 02: WebAssign Questions (Homework) & HELP: 8, 9, 13 \{\{nl\}\} Solidify: 10, 11, 14, \tn 
% Row Count 4 (+ 3)
% Row 2
\SetRowColor{LightBackground}
HW 02: CDS Questions (Homework) & 1 \{\{nl\}\} REVIEW: 2 \tn 
% Row Count 6 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{p{0.72 cm} x{4.248 cm} x{1.512 cm} p{0.72 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{4}{x{8.4cm}}{\bf\textcolor{white}{Assessing the Student Response tips}}  \tn
% Row 0
\SetRowColor{LightBackground}
LoMP & make sure one element ({\emph{mass}}) is {\bf{{\emph{fixed}}}} & make sure ra &  \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{4}{x{8.4cm}}{LoDP} \tn 
% Row Count 3 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}----}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{p{0.72 cm} p{0.72 cm} p{0.72 cm} p{0.72 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{4}{x{8.4cm}}{\bf\textcolor{white}{Unit 3 -{}- Concepts!}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{4}{x{8.4cm}}{} \tn 
% Row Count 0 (+ 0)
\hhline{>{\arrayrulecolor{DarkBackground}}----}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{p{0.8 cm} p{0.8 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Unit 4 -{}- Concepts!}}  \tn
% Row 0
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{8.4cm}}{} \tn 
% Row Count 0 (+ 0)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}

\begin{tabularx}{8.4cm}{x{3.84 cm} x{4.16 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{8.4cm}}{\bf\textcolor{white}{Review! dummy}}  \tn
% Row 0
\SetRowColor{LightBackground}
{\bf{Test}} & {\bf{Question}} \tn 
% Row Count 1 (+ 1)
% Row 1
\SetRowColor{white}
Unit 1 Test & Question 3 \tn 
% Row Count 2 (+ 1)
% Row 2
\SetRowColor{LightBackground}
 & Question 5 \tn 
% Row Count 3 (+ 1)
% Row 3
\SetRowColor{white}
 & Question 7 \tn 
% Row Count 4 (+ 1)
% Row 4
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{8.4cm}}{Unit 2 Test} \tn 
% Row Count 5 (+ 1)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
\end{tabularx}
\par\addvspace{1.3em}


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

\end{document}