To draw the electron dot structure for acetonitrile (C2H3N), we start by identifying the number of valence electrons available. Carbon (C) has 4 valence electrons, hydrogen (H) has 1, and nitrogen (N) has 5. In total, we have:
- 2 Carbons: 2 x 4 = 8
- 3 Hydrogens: 3 x 1 = 3
- 1 Nitrogen: 1 x 5 = 5
Total valence electrons = 8 + 3 + 5 = 16.
In acetonitrile, the structure consists of a carbon (C) triple bonded to a nitrogen (N), and the other carbon (C) is single bonded to three hydrogen (H) atoms. The basic structure looks like this:
H H \ / C ≡ N / \ H H
In this structure, one carbon atom is bonded to three hydrogen atoms, while the other carbon is triple bonded to nitrogen. This configuration allows nitrogen to achieve a stable octet while still forming strong bonds with carbon.
Answer to Part B: The nitrogen atom in acetonitrile has 5 electrons in its outer shell. This is due to the 5 valence electrons that nitrogen possesses, which allows it to bond effectively with carbon, resulting in a stable molecule.
Answer to Part C: In terms of bonding and nonbonding electrons, nitrogen in this molecule is involved in a triple bond with one carbon atom, contributing 3 electrons to this bond. As a result, there are:
- Bonding Electrons: 3 (from the triple bond)
- Nonbonding Electrons: 2 (one lone pair)
This configuration allows nitrogen to satisfy the octet rule while facilitating strong bonding with carbon.