91Ó°ÊÓ

Draw line structures corresponding to the following compounds. Show all lone pair electrons (and don't forget that non-zero formal charges are part of a correctly drawn structure!) a) 2,2,4 -trimethylpentane b) 3 -phenyl-2-propenal c) 6-methyl-2,5-cyclohexadienone d) 3 -methylbutanenitrile e) 2,6 -dimethyldecane f) 2,2,5,5 -tetramethyl- 3 -hexanol g) methyl butanoate h) \(N\) -ethylhexanamide

Draw correct Lewis structures for ozone \(\left(\mathrm{O}_{3}\right)\), azide ion, \(\left(\mathrm{N}_{3}^{-}\right),\) and bicarbonate ion, \(\mathrm{HCO}_{3}^{-}\). Include lone pair electrons and formal charges, and use your General Chemistry textbook to review VSEPR theory, which will enable you to draw correct bond geometries.

Draw one example each of compounds fitting the descriptions below, using line structures. Be sure to include all non-zero formal charges. All atoms should fit one of the common bonding patters discussed in this chapter. There are many possible correct answers - be sure to check your drawings with your instructor or tutor. a) an 8 -carbon molecule with secondary alcohol, primary amine, amide, and cis-alkene groups b) a 12 -carbon molecule with carboxylate, diphosphate, and lactone (cyclic ester) groups. c) a 9-carbon molecule with cyclopentane, alkene, ether, and aldehyde groups

a) Draw four constitutional isomers with the molecular formula \(\mathrm{C}_{4} \mathrm{H}_{8}\). b) Draw two open-chain (non-cyclic) constitutional isomers of cyclohexanol (there are more than two possible answers).

Draw structures of four different amides with molecular formula \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{NO}\).