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\author{Emergybuttonse}
\pdfinfo{
  /Title (chemistry-9701-3-chemical-bonding-as-level.pdf)
  /Creator (Cheatography)
  /Author (Emergybuttonse)
  /Subject (Chemistry (9701): 3. Chemical Bonding, AS level Cheat Sheet)
}

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    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Chemistry (9701): 3. Chemical Bonding, AS level Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{Emergybuttonse} via \textcolor{DarkBackground}{\uline{cheatography.com/207489/cs/44367/}}}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}Emergybuttonse \\
  \uline{cheatography.com/emergybuttonse} \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Published 15th September, 2024.\\
   Updated 15th September, 2024.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
  www.readability-score.com
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\begin{multicols*}{3}

\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Definitions}}  \tn
% Row 0
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\mymulticolumn{1}{x{5.377cm}}{{\bf{Electronegativity}} is the ability of an atom to attract a pair of electrons towards itself in a covalent bond} \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Ionic bonding}} is the electrostatic attraction between oppositely charged ions (positively charged   cations and negatively charged anions} \tn 
% Row Count 6 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Metallic bonding}} is the electrostatic attraction between positive metal ions and delocalised   electrons} \tn 
% Row Count 9 (+ 3)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Covalent bonding}} is electrostatic attraction between the nuclei of two atoms and a shared pair of electrons} \tn 
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% Row 4
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\mymulticolumn{1}{x{5.377cm}}{{\bf{Bond energy}} is the energy required to break one mole of a particular covalent bond in the gaseous state} \tn 
% Row Count 15 (+ 3)
% Row 5
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Bond length}} is the internuclear distance of two covalently bonded atoms} \tn 
% Row Count 17 (+ 2)
% Row 6
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Sigma bond}} is the covalent bond formed by 'head on' overlap of atomic orbitals} \tn 
% Row Count 19 (+ 2)
% Row 7
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Pi Bond}} is the covalent bond formed by sideways overlap of atomic orbitals} \tn 
% Row Count 21 (+ 2)
% Row 8
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Dipole-Dipole}} Forces are intermolecular attractions between molecules which are permanently polarised} \tn 
% Row Count 24 (+ 3)
% Row 9
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Hydrogen Bond}} is the electrostatic attraction between a hydrogen atom which is bonded to a very electronegative atom and \seqsplit{an electronegative atom of a neighbouring molecule}} \tn 
% Row Count 28 (+ 4)
% Row 10
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{{\bf{Van Der Waals Forces}} are intermolecular forces of attraction which arise from temporary dipoles in molecules} \tn 
% Row Count 31 (+ 3)
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\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Dative bonding}}  \tn
\SetRowColor{LightBackground}
\mymulticolumn{1}{p{5.377cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/emergybuttonse_1726375382_SmartSelect_20240915_101150_Flexcil.jpg}}} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
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\begin{tabularx}{5.377cm}{x{2.09034 cm} x{2.88666 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Properties of water}}  \tn
% Row 0
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High melting \& boiling points & Water has high melting and boiling points which is caused by the strong intermolecular forces of hydrogen bonding between the molecules \tn 
% Row Count 6 (+ 6)
% Row 1
\SetRowColor{white}
High surface tension & Surface tension is the ability of a liquid surface to resist any external forces. The water molecules at the surface of liquid are bonded to other water molecules through hydrogen bonds These molecules pull downwards on the surface molecules causing the surface them to become compressed and more tightly together at the surface \tn 
% Row Count 21 (+ 15)
% Row 2
\SetRowColor{LightBackground}
Density & In ice the water molecules are packed in a 3D hydrogen-bonded network in a rigid lattice. Each oxygen atom is surrounded by hydrogen atoms. This way of packing the molecules in a solid and the relatively long bond lengths of the hydrogen bonds means that the water molecules are slightly further apart than in the liquid form \tn 
% Row Count 36 (+ 15)
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\mymulticolumn{2}{x{5.377cm}}{Hydrogen bonding in water, causes it to have anomalous properties such as high melting and boiling points, high surface tension and anomalous density of ice compared to water}  \tn 
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\begin{tabularx}{5.377cm}{x{1.89126 cm} x{3.08574 cm} }
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Factors influencing electronegativity}}  \tn
% Row 0
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Nuclear charge & Increase in nuclear charge increases electronegativity \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
Atomic radius & Increase in atomic radius decreases electronegativity \tn 
% Row Count 6 (+ 3)
% Row 2
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Shielding by inner shells & Shielding causes decrease in electronegativity \tn 
% Row Count 8 (+ 2)
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\begin{tabularx}{5.377cm}{x{3.38436 cm} x{1.59264 cm} }
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Paulings electronegativity to predict bonds}}  \tn
% Row 0
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{\bf{Paulings electronegativity}} & {\bf{Bond}} \tn 
% Row Count 2 (+ 2)
% Row 1
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\textless{} 1.0 & Covalent \tn 
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1.0 - 2.0 & Polar covalent \tn 
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\textgreater{} 2.0 & Ionic \tn 
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Metallic bonding}}  \tn
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\mymulticolumn{1}{x{5.377cm}}{In a metal, atoms are packed together in a lattice \newline Electrostatic attraction increases with: \newline ~ Increase in positive charge \newline ~ Decrease in size of metal ions  \newline ~ Increase in number of mobile electrons}  \tn 
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\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{σ and π bonds}}  \tn
% Row 0
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\mymulticolumn{1}{x{5.377cm}}{A pi bond is weaker than a sigma bond because the overlapping of charge   clouds is less than in a sigma bond} \tn 
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\mymulticolumn{1}{x{5.377cm}}{H₂ has 1 σ bond} \tn 
% Row Count 4 (+ 1)
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\mymulticolumn{1}{x{5.377cm}}{C₂H₆ has only σ bonds} \tn 
% Row Count 5 (+ 1)
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\mymulticolumn{1}{x{5.377cm}}{C₂H₄ has 1 σ and 1 π bond} \tn 
% Row Count 6 (+ 1)
% Row 4
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\mymulticolumn{1}{x{5.377cm}}{HCN has 1 σ and 2 π bonds} \tn 
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% Row 5
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\mymulticolumn{1}{x{5.377cm}}{N₂ has 1 σ and 2 π bonds} \tn 
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\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{VSEPR Theory and Molecular Shapes}}  \tn
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\mymulticolumn{1}{p{5.377cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/emergybuttonse_1726377565_Screenshot 2024-09-15 104847.png}}} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
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\begin{tabularx}{5.377cm}{x{2.04057 cm} x{2.93643 cm} }
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Van der Waals' Forces \& Dipoles}}  \tn
% Row 0
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Id - id forces increase with & Increasing number of electrons (and atomic number) in the molecule \tn 
% Row Count 3 (+ 3)
% Row 1
\SetRowColor{white}
 & Increasing the places where the molecules come close together \tn 
% Row Count 6 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{2}{x{5.377cm}}{For small molecules with the same number of electrons, pd - pd forces are stronger than id - id} \tn 
% Row Count 8 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
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\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Order of bond strength}}  \tn
\SetRowColor{LightBackground}
\mymulticolumn{1}{p{5.377cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/emergybuttonse_1726383198_SmartSelect_20240915_122244_Flexcil.jpg}}} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
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\begin{tabularx}{5.377cm}{X}
\SetRowColor{DarkBackground}
\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Electronegativity relations}}  \tn
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\mymulticolumn{1}{p{5.377cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/emergybuttonse_1726333044_SmartSelect_20240914_221841_Flexcil.jpg}}} \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}{Ionic bonding}}  \tn
\SetRowColor{LightBackground}
\mymulticolumn{1}{p{5.377cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/emergybuttonse_1726373948_SmartSelect_20240915_094831_Flexcil.jpg}}} \tn 
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{Ionic bonds are non-directional, each cation will attract any neighbouring anion   and vice versa to form a huge ionic lattice}  \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}{Covalent bonding dot and cross}}  \tn
\SetRowColor{LightBackground}
\mymulticolumn{1}{p{5.377cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/emergybuttonse_1726374812_SmartSelect_20240915_100149_Flexcil.jpg}}} \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}{Special octets}}  \tn
\SetRowColor{LightBackground}
\mymulticolumn{1}{p{5.377cm}}{\vspace{1px}\centerline{\includegraphics[width=5.1cm]{/web/www.cheatography.com/public/uploads/emergybuttonse_1726374954_SmartSelect_20240915_100500_Flexcil.jpg}}} \tn 
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\mymulticolumn{1}{x{5.377cm}}{If the central atom is from Period 2 of the Periodic Table, the total number of  electrons surrounding it cannot exceed eight(but can less than eight). \newline If the central atom is from Period 3 and beyond, the total number of electrons surrounding it can exceed eight}  \tn 
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\begin{tabularx}{5.377cm}{p{0.54747 cm} x{4.42953 cm} }
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Hybridisation: sp, sp$^{\textrm{2}}$, sp$^{\textrm{3}}$}}  \tn
% Row 0
\SetRowColor{LightBackground}
sp & two different bonds(one may be triple bond) \tn 
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% Row 1
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sp\textasciicircum{}2\textasciicircum{} & three different bonds(one may be double bond) \tn 
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% Row 2
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sp\textasciicircum{}3\textasciicircum{} & four different bonds \tn 
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\hhline{>{\arrayrulecolor{DarkBackground}}--}
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\begin{tabularx}{5.377cm}{x{2.68758 cm} x{2.28942 cm} }
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Hydrogen bonding}}  \tn
% Row 0
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\mymulticolumn{2}{x{5.377cm}}{Hydrogen bonding is the strongest form of intermolecular bonding} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{For hydrogen bonding to take place the following is needed:} \tn 
% Row Count 4 (+ 2)
% Row 2
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A species which has an O or N (very electronegative) atom with an available lone pair of electrons & A species with an -OH or -NH group \tn 
% Row Count 9 (+ 5)
% Row 3
\SetRowColor{white}
\mymulticolumn{2}{x{5.377cm}}{For hydrogen bonding to take place, the angle between the -OH/-NH and the hydrogen bond is 180\textasciicircum{}o\textasciicircum{}} \tn 
% Row Count 11 (+ 2)
\hhline{>{\arrayrulecolor{DarkBackground}}--}
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\begin{tabularx}{5.377cm}{X}
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\mymulticolumn{1}{x{5.377cm}}{\bf\textcolor{white}{Bond Energy and Bond Length: Reactivity}}  \tn
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\mymulticolumn{1}{x{5.377cm}}{Shorter bond length generally means higher bond energy, making molecules less reactive} \tn 
% Row Count 2 (+ 2)
% Row 1
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{Triple bonds are the shortest and strongest covalent bonds due to the large electron density between the nuclei of the two atoms} \tn 
% Row Count 5 (+ 3)
% Row 2
\SetRowColor{LightBackground}
\mymulticolumn{1}{x{5.377cm}}{Triple bonds are the shortest and strongest covalent bonds due to the large electron density between the nuclei of the two atoms} \tn 
% Row Count 8 (+ 3)
% Row 3
\SetRowColor{white}
\mymulticolumn{1}{x{5.377cm}}{The reactivity of a covalent bond is greatly influenced by: The bond polarity, the bond strength, the bond type (σ/π)} \tn 
% Row Count 11 (+ 3)
\hhline{>{\arrayrulecolor{DarkBackground}}-}
\end{tabularx}
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% That's all folks
\end{multicols*}

\end{document}