Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the neutral compound C3H8O (propanol)?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the neutral compound SF3N?
A
Sulfur is the central atom, bonded to three fluorine atoms and one nitrogen atom, with one lone pair on sulfur.
B
Nitrogen is the central atom, bonded to three sulfur atoms and one fluorine atom, with no lone pairs on nitrogen.
C
Fluorine is the central atom, bonded to three sulfur atoms and one nitrogen atom, with one lone pair on fluorine.
D
Sulfur is the central atom, bonded to three nitrogen atoms and one fluorine atom, with two lone pairs on sulfur.
Verified step by step guidance1
Step 1: Determine the central atom by considering electronegativity and bonding capacity. Typically, the least electronegative atom (excluding hydrogen) is the central atom. Here, sulfur (S), nitrogen (N), and fluorine (F) are present. Fluorine is the most electronegative and usually terminal, so it is unlikely to be central. Between sulfur and nitrogen, sulfur is less electronegative and can expand its octet, making it a good candidate for the central atom.
Step 2: Count the total number of valence electrons for the molecule SF3N. Sulfur has 6 valence electrons, each fluorine has 7, and nitrogen has 5. Calculate the sum: \(6 + (3 \times 7) + 5\).
Step 3: Arrange the atoms with sulfur in the center bonded to three fluorine atoms and one nitrogen atom. Draw single bonds connecting sulfur to each fluorine and to nitrogen. Each bond represents 2 electrons.
Step 4: Distribute the remaining valence electrons to satisfy the octet rule for the terminal atoms first (fluorine and nitrogen). Fluorine atoms typically have three lone pairs, and nitrogen usually has one lone pair if bonded to sulfur.
Step 5: Assign any leftover electrons to the central sulfur atom as lone pairs. Since sulfur can have an expanded octet, it may have one lone pair after bonding to the four atoms. Confirm that the total number of electrons used matches the total valence electrons calculated in Step 2.
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