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  /Title (chemistry-1030-unit-5-bonding-and-nomenclature.pdf)
  /Creator (Cheatography)
  /Author (chantalcramm)
  /Subject (Chemistry 1030: Unit 5 - Bonding and Nomenclature Cheat Sheet)
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    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Chemistry 1030: Unit 5 - Bonding and Nomenclature Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{chantalcramm} via \textcolor{DarkBackground}{\uline{cheatography.com/169234/cs/35427/}}}
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Not Yet Published.\\
   Updated 13th November, 2022.\\
   Page {\thepage} of \pageref{LastPage}.
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Review}}  \tn
% Row 0
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\mymulticolumn{1}{x{5.377cm}}{Valance Electron: Group Number.} \tn 
% Row Count 1 (+ 1)
% Row 1
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\mymulticolumn{1}{x{5.377cm}}{Compound: A substance composed of two or more elements in fixed, definite proportions.} \tn 
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\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Forming Ions}}  \tn
% Row 0
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\mymulticolumn{1}{x{5.377cm}}{Atoms of metals have few valance electrons (1-2) thus they tend to lose electrons to form a positive ion (cations).} \tn 
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% Row 1
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\mymulticolumn{1}{x{5.377cm}}{Atoms of non-metals have many valance electrons (4-7) thus they tend to gain electrons to form negative ions (anions).} \tn 
% Row Count 6 (+ 3)
% Row 2
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\mymulticolumn{1}{x{5.377cm}}{They do this to become stable in their outer shell.} \tn 
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\mymulticolumn{3}{x{5.377cm}}{\bf\textcolor{white}{Ionic Bonding: Type I}}  \tn
% Row 0
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% Row Count 2 (+ 2)
% Row 1
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 & MgBr\textasciicircum{}2\textasciicircum{} & Magnesium Brom{\emph{ide}} \tn 
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1 = I & 3 = III & 5 = V & 7 = VII \tn 
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% Row 1
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2 = II & 4 = IV & 6 = VI & 8 = VIII \tn 
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\mymulticolumn{4}{x{5.377cm}}{\bf\textcolor{white}{Ionic Bonding: Type II}}  \tn
% Row 0
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\seqsplit{Format:} & Name of Cation \seqsplit{(metal)} & (Charge of cation (metal) in roman numerals) & Base name of Anion (non-metal) + {\emph{ide}} \tn 
% Row Count 4 (+ 4)
% Row 1
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% Row 2
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CuCl\textasciicircum{}2\textasciicircum{} & Copper & (II) & Chlor{\emph{ide}} \tn 
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% Row 0
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% Row 1
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Step Three: & Label the bonding and non-bonding electrons. \tn 
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% Row 1
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\mymulticolumn{1}{x{5.377cm}}{Bonding involved valance electrons only.} \tn 
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% Row 1
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% Row 4
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% Row 1
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\mymulticolumn{1}{x{5.377cm}}{Each of the following is consider {\emph{one electron group}}:} \tn 
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% Row 2
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% Row 3
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% Row 4
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\mymulticolumn{1}{x{5.377cm}}{Example: CH\textasciicircum{}4\textasciicircum{} has 4 electron groups (4 single bonds, 0 lone pairs)} \tn 
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% Row 0
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Straight Line: & Bond in plane of paper. \tn 
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% Row 1
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Hashed Line: & Bonding going into paper. \tn 
% Row Count 3 (+ 1)
% Row 2
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Wedge: & Bond coming out of the paper. \tn 
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% Row 0
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Single Bond: & One pair of electrons shared between two atoms (Cl\textasciicircum{}2\textasciicircum{}) \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
Double Bond: & Two pairs of electrons shared between two atoms. (O\textasciicircum{}2\textasciicircum{}) \tn 
% Row Count 6 (+ 3)
% Row 2
\SetRowColor{LightBackground}
Triple Bond: & Three pairs of electrons shared between two atoms. (N\textasciicircum{}2\textasciicircum{}) \tn 
% Row Count 9 (+ 3)
% Row 3
\SetRowColor{white}
Bonding Electrons: & Electrons shared between atoms. \tn 
% Row Count 11 (+ 2)
% Row 4
\SetRowColor{LightBackground}
Non-Bonding Electrons: & Electrons only found on one atom. (Lone pairs) \tn 
% Row Count 13 (+ 2)
% Row 5
\SetRowColor{white}
Overall: & Draw the lewis structure and determine how they will bond with one another to have full outer shells (8). \tn 
% Row Count 18 (+ 5)
% Row 6
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 & Identify the bonding and non-bonding electrons. \tn 
% Row Count 20 (+ 2)
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Ionic Bonding: & Covalent Bonding: \tn 
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% Row 1
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Metal + One or more non-metals. & All non-metals. \tn 
% Row Count 4 (+ 2)
% Row 2
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Electrons are transferred. & Electrons are shared. \tn 
% Row Count 6 (+ 2)
% Row 3
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Ions are formed. & Ions are not formed. \tn 
% Row Count 8 (+ 2)
% Row 4
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Ex. NaHCO\textasciicircum{}3\textasciicircum{} or NaCl & Ex. F\textasciicircum{}2\textasciicircum{} or CO\textasciicircum{}2\textasciicircum{} \tn 
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% Row 2
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% Row 3
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% Row Count 4 (+ 1)
% Row 4
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\mymulticolumn{1}{x{5.377cm}}{CS\textasciicircum{}2\textasciicircum{}} \tn 
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Step One: & Draw the lewis structure for each atom separetly. \tn 
% Row Count 2 (+ 2)
% Row 1
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Step Two: & The atom that has the most unpaired electrons is the central atom. \tn 
% Row Count 5 (+ 3)
% Row 2
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Step Three: & The other atoms will share electrons with the central atom. \tn 
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% That's all folks
\end{multicols*}

\end{document}