Label the partial charge $($bond polarity$),+,-,$ of all polar bonds.

Add the correct number of bonded H$\text{'}$s and electron pairs to make the bonding and formal charge correct. All of the bonds between $C,Cl,O,$ and $N$ are shown. Show the bonds to $H$ around the molecule. You are given nonH atoms and correct formal charge.

$C-C=C-C-=C$

$Cl-C^{+}-C-C-C$

$N-=C-C$

$C-O^{+}=C-C^{-}$

${?}^{+}N-C$

Draw the Lewis Bond$-$line Structure for the following molecules. $($These are not correct unless you include formal charge and all lone pair electrons.$)$

$C{H}_{2}BrCHB{r}_2$

$H_{2}CCO{H}^{-}$give $2$ structures

This is a correct structure. Add the lone pair electrons to the molecule, and label the geometry and hybridization of the five atoms in the ring.