Propose potential resonance structures for each compound and determine which resonance structure is most stable and which is least stable. H. H H. H- H-C=C_N- H. I- CH エー○ エーO

Are the arrows shown to create the resonance structures valid? [9+0] O yes O no

Based on the arrows already drawn, draw the resonance structures (making sure to include any charges), and highlight which structure is most important/present for each molecule صدار H N [2 I ]

Which bond should have the highest bond dissociation energy? Ο NΝ O N=N O N-N Ο N-Η

Draw a second resonance structure for each ion.

3. Keeping in mind that all row two elements need to have 8 electrons and each bond contains two electrons, draw the missing lone pair electrons on each O or N below. Then, assign the missing formal charges to each O or N. H H H H H H C H- H- C H- 中长子长 H H H

Label the resonance structures in each pair as major, minor, or equal contributors to the hybrid. Then draw the hybrid. a. CH3-C-N-CH3 I HH CH3-C=N-CH3 HH b. CHg=c&l, H CH₂-C=CH₂ H

How do you find the resonances?

Draw two resonance structures for the molecule shown. Indicate based on formal charges whether any of the structures is more stable (major contributor). + JEN -C - NH3

4. Convert the following structures into bond line structures. C-H ннн нон нн Н-с-с-с-о-н Н-с-с-с—Н Н-с-с-о-с-н H H H H H H нн H C. H- H-N H Ó H il н-с-с-с-с-н H H H H нн