Which of the following statements correctly describes the Lewis dot structure of the neutral compound C2H3N (acetonitrile)?

• A. The structure contains a carbon-nitrogen double bond and all hydrogens are bonded to nitrogen.
• B. The structure contains a nitrogen-nitrogen single bond and all hydrogens are bonded to carbon.
• C. The structure contains a carbon-carbon triple bond and a nitrogen atom bonded to one of the carbons.
• D. The structure contains a carbon-carbon double bond and a nitrogen atom bonded to both carbons.

Answer: (C)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for the molecule C2H3N. Carbon has 4 valence electrons, hydrogen has 1, and nitrogen has 5. Calculate the sum: \$2 \times 4 + 3 \times 1 + 5$.
2. Step 2: Use the valence electrons to draw a skeletal structure. Typically, carbon atoms bond to each other, hydrogens bond to carbons, and nitrogen bonds to carbon. Consider common bonding patterns and the octet rule.
3. Step 3: Assign bonds between atoms. Since the molecule is acetonitrile, expect a triple bond between the two carbon atoms or between carbon and nitrogen. Check which arrangement satisfies the octet rule for all atoms.
4. Step 4: Place the hydrogens on the carbon atoms, as hydrogens usually bond to carbon rather than nitrogen in this molecule. Verify that each hydrogen has one bond and carbon has four bonds total.
5. Step 5: Confirm the final Lewis structure by counting electrons around each atom to ensure the octet rule is satisfied (except for hydrogen, which follows the duet rule). This will help identify the correct bonding pattern among the options.