Multiple Choice
Which of the following best describes the correct Lewis dot structure for the neutral compound S2O?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following is the correct Lewis dot structure for the neutral compound PBr_3?
A
A phosphorus atom with three single bonds to three bromine atoms, and two lone pairs on phosphorus; each bromine atom has two lone pairs.
B
A phosphorus atom with three double bonds to three bromine atoms, and no lone pairs on phosphorus; each bromine atom has two lone pairs.
C
A phosphorus atom with three single bonds to three bromine atoms, and no lone pairs on phosphorus; each bromine atom has three lone pairs.
D
A phosphorus atom with three single bonds to three bromine atoms, and one lone pair on phosphorus; each bromine atom has three lone pairs.
Verified step by step guidance1
Step 1: Determine the total number of valence electrons in PBr_3. Phosphorus (P) has 5 valence electrons, and each bromine (Br) atom has 7 valence electrons. Since there are three bromine atoms, calculate the total as: \(5 + 3 \times 7\).
Step 2: Draw the skeletal structure with phosphorus as the central atom bonded to three bromine atoms. Connect each Br to P with a single bond, which uses 2 electrons per bond.
Step 3: Subtract the electrons used in bonding from the total valence electrons to find the number of remaining electrons to be placed as lone pairs.
Step 4: Assign lone pairs to the bromine atoms first to complete their octets. Each bromine needs 8 electrons total (including bonding electrons), so add lone pairs accordingly.
Step 5: Place any remaining electrons as lone pairs on the phosphorus atom. Check that phosphorus has a complete octet (or expanded octet if applicable) and that the total number of electrons matches the total valence electrons calculated.
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