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\author{geminifourth04 (shreyasree)}
\pdfinfo{
  /Title (chemical-bonding-a-level-h2-2.pdf)
  /Creator (Cheatography)
  /Author (geminifourth04 (shreyasree))
  /Subject (Chemical Bonding (A level) - H2 \#2 Cheat Sheet)
}

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    \vspace{-2pt}\large{\bf{\textcolor{DarkBackground}{\textrm{Chemical Bonding (A level) - H2 \#2 Cheat Sheet}}}} \\
    \normalsize{by \textcolor{DarkBackground}{geminifourth04 (shreyasree)} via \textcolor{DarkBackground}{\uline{cheatography.com/184627/cs/42796/}}}
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  \mymulticolumn{2}{p{5.377cm}}{\bf\textcolor{white}{Cheatographer}}  \\
  \vspace{-2pt}geminifourth04 (shreyasree) \\
  \uline{cheatography.com/shreyasree} \\
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  \mymulticolumn{1}{p{5.377cm}}{\bf\textcolor{white}{Cheat Sheet}}  \\
   \vspace{-2pt}Not Yet Published.\\
   Updated 21st March, 2024.\\
   Page {\thepage} of \pageref{LastPage}.
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  Measure your website readability!\\
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\begin{tabularx}{5.377cm}{p{0.4977 cm} p{0.4977 cm} }
\SetRowColor{DarkBackground}
\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Ionic Bonding}}  \tn
% Row 0
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\mymulticolumn{2}{x{5.377cm}}{Electrostatic attraction between cations and anions} \tn 
% Row Count 2 (+ 2)
% Row 1
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\mymulticolumn{2}{x{5.377cm}}{Formed due to large difference (\textgreater{}2) in electronegativity} \tn 
% Row Count 4 (+ 2)
% Row 2
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\mymulticolumn{2}{x{5.377cm}}{Ionic bonding is not always present between nonmetal and metal (eg. AlCl3 is covalent molecule)} \tn 
% Row Count 6 (+ 2)
% Row 3
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\mymulticolumn{2}{x{5.377cm}}{Transfer of electrons from a metal atom to a non metal atom} \tn 
% Row Count 8 (+ 2)
% Row 4
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\mymulticolumn{2}{x{5.377cm}}{Metal atom gives away electrons and becomes a cation} \tn 
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% Row 5
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\mymulticolumn{2}{x{5.377cm}}{Non- metal atom accepts electrons and becomes anion} \tn 
% Row Count 12 (+ 2)
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Giant Ionic Structure}}  \tn
% Row 0
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\mymulticolumn{2}{x{5.377cm}}{In solid state, anions and cation are held in fixed alternate positions in a giant ionic crystal lattice} \tn 
% Row Count 3 (+ 3)
% Row 1
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\mymulticolumn{2}{x{5.377cm}}{Cations attract anions in every direction around them} \tn 
% Row Count 5 (+ 2)
% Row 2
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\mymulticolumn{2}{x{5.377cm}}{Ionic bonds exist extensively throughout the structure} \tn 
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Strength of ionic bond}}  \tn
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\mymulticolumn{2}{x{5.377cm}}{Indicated by lattice energy (LE)} \tn 
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% Row 1
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\mymulticolumn{2}{x{5.377cm}}{LE is the amount of heat energy evolved when 1 mole of solid ionic compound was formed from its gaseous ions} \tn 
% Row Count 4 (+ 3)
% Row 2
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\mymulticolumn{2}{x{5.377cm}}{Directly translates to the amount of heat energy required to break the ionic bond} \tn 
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% Row 3
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\mymulticolumn{2}{x{5.377cm}}{Magnitude of LE : Product of respective charges of the ions/ sum of the respective  radius of both ions} \tn 
% Row Count 9 (+ 3)
% Row 4
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\mymulticolumn{2}{x{5.377cm}}{More LE -\textgreater{} stronger electrostatic attraction between cation and anion -{}-\textgreater{} more stronger ionic bond} \tn 
% Row Count 11 (+ 2)
% Row 5
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\mymulticolumn{2}{x{5.377cm}}{Greater numerator -\textgreater{} higher charge -\textgreater{} greater LE required -\textgreater{} stronger ionic bond} \tn 
% Row Count 13 (+ 2)
% Row 6
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\mymulticolumn{2}{x{5.377cm}}{Smaller denominator -\textgreater{} lower radius -\textgreater{} greater LE required -\textgreater{} stronger ionic bond} \tn 
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% Row 7
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\mymulticolumn{2}{x{5.377cm}}{Explain answers in terms of value of (q+ x q-) and (r+ + r-) and then link to the LE formula} \tn 
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Physical properties of Giant ionic structureHi}}  \tn
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\mymulticolumn{2}{x{5.377cm}}{High MP/BP : large amount of energy required to overcome strong electrostatic forces of attraction between cations and anions} \tn 
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% Row 1
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\mymulticolumn{2}{x{5.377cm}}{Discussing difference in MP/BP: structure -\textgreater{} compare (q+ x q-) and (r+ + r-) -\textgreater{} compare LE -\textgreater{} strength of esf -\textgreater{} energy required to overcome esf -\textgreater{} link} \tn 
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% Row 2
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\mymulticolumn{2}{x{5.377cm}}{Electrical Conductivity: ionic compounds are good electrical conductors in molten/aqueous state as the ions are free from their fixed , alternate positions in the giant crystal ionic lattice -\textgreater{} presence of mobile ions able to carry charges throughout the compound} \tn 
% Row Count 13 (+ 6)
% Row 3
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Hardness: {\bf{Very}} hard ( large amount of energy to overcome strong esf) but they are brittle & When a force is applied along a particular plane -\textgreater{} layers of ions slide -\textgreater{} ions of same charge meet and repel one another -\textgreater{} shatters crystal along fault line \tn 
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Solubility}}  \tn
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\mymulticolumn{2}{x{5.377cm}}{Ionic compounds are soluble in water (not non-polar solutions)} \tn 
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% Row 1
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\mymulticolumn{2}{x{5.377cm}}{when ionic compound is added to water -\textgreater{} ion-dipole attraction established between oppositely charged ions and the polar water molecules (ions are completely solvated) -\textgreater{} when ion-dipole attraction releases sufficient energy -\textgreater{} enough to overcome the strong esf between the cations and anions -\textgreater{} breakdown of the solid ionic crystal lattice -\textgreater{} solid dissolved} \tn 
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\mymulticolumn{2}{x{5.377cm}}{\bf\textcolor{white}{Covalent character in ionic bond}}  \tn
% Row 0
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\mymulticolumn{2}{x{5.377cm}}{not all ionic bonds are pure -\textgreater{} some possess a certain degree covalent character} \tn 
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% Row 1
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\mymulticolumn{2}{x{5.377cm}}{in these cases, cations will polarise the anion (attract the electron cloud towards itself -\textgreater{} part of the electron cloud of O2- gets drawn to the region in between both ions -\textgreater{} electron cloud ends up being shared between ions} \tn 
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% Row 2
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\mymulticolumn{2}{x{5.377cm}}{factors affecting extent of covalent character -\textgreater{} increased polarising power of cation (increased charge density -\textgreater{} small size and higher charge) and larger anions (easier to polarise) -\textgreater{} size of anions decreases down the group} \tn 
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% That's all folks
\end{multicols*}

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