ࡱ>   bjbj .---8ey-(VXXXXXX$q^||"""|V"V"""` -*|"B0"|"" "||" :  1. Draw a Lewis structure for each species including lone pairs and formal charges. a. sodium hydroxide b. sodium methoxide c. lithium ethoxide d. potassium t-butoxide e. hydronium ion f. nitrite ion g. cyanide ion h. hydrogen carbonate ion i. nitrate ion j. amide ion (NH2)- k. ammonium ion l. protonated methanol (CH3OH2)+ m. F3B-NH3 n. protonated acetone (CH3-COH-CH3)+ 2. For all resonance structures: include lone pairs and show formal charges, if any. a. Ozone, O3, has two equivalent resonance structures. Draw both resonance contributors. b. Draw three equivalent resonance structures for the nitrate ion, (NO3)-. c. Draw a Lewis structure for acetaldehyde, C2H4O, then draw a non-equivalent resonance structure. Label each structure as major or minor contributor. 3. Draw all resonance structures for the carbocation below. Used curved arrows to show the movement of electrons from one resonance form to the next. Include all non-zero formal charges for each structure that you draw.  EMBED ChemDraw.Document.6.0  4. Which ion is more stable? Use resonance theory to illustrate how the ionic charge may be delocalized.  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