Using the formal charge as a reference, find out the number of unpaired or non-bonding electrons on the marked atom.

Add the missing lone-pair electrons and formal charges to complete the structures of the compounds shown below:

i.

ii.

Consider the line-angle structure shown below:

(1) Identify the total number of carbon atoms.

(2) Label each carbon (use a through l).

(3) Determine the number of hydrogens at each carbon atom.

(4) Provide the condensed structural formula.

How many hydrogen atoms are bonded to each indicated carbon in the structure of the morphine derivative shown below?

Consider the following line-angle drawing:

(i) Determine the number of carbons in the molecule. 

(ii) Determine the number of hydrogens of the encircled carbon.

(iii) Determine if the boxed carbon is 1°, 2°, 3°, or 4°.

Write the appropriate Lewis structures for these free radicals ･CH₃ and ･CH(CH₃)₂.

Draw Lewis structures with the appropriate formal charges for these compounds and ions (CH₃)₂O—BCl₃, H₃CNH₃⁺, NaOC(CH₃)₃, and (CH₃)₂C=OH⁺.

Draw Lewis structures for the following molecular formulas: C₂H₄ (one double bond), C₄H₆ (two double bonds), and C₄H₆ (one triple bond). Mark all non-bonding electrons in each structure.

Draw a skeletal structure corresponding to each of the following condensed structures.

a. CH₃CH₂CH(CH₃)CH₂CH₂CH(CH₃)₂

b. (CH₃)₃COC(CH₃)₃

c.  (CH₃)₂CHOH

Provide the skeletal structure for CH₃CH₂CH₂COOH.

What are the condensed structures of the following compounds drawn as models?

(black = C, white = H, red = O, green = Cl)

Consider the formula, C₁₂H₁₈O₂BrF. Provide the index of hydrogen deficiency of the compound.

Determine the IHD for the following molecule.