Multiple Choice
Which of the following best describes the correct Lewis dot structure for neutral HNO?
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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 phosphorus tribromide, PBr_3?
A
Phosphorus atom in the center with three single bonds to bromine atoms, and one lone pair on phosphorus; each bromine has three lone pairs.
B
Phosphorus atom in the center with three double bonds to bromine atoms, and no lone pairs on phosphorus; each bromine has two lone pairs.
C
Phosphorus atom in the center with three single bonds to bromine atoms, and no lone pairs on phosphorus; each bromine has three lone pairs.
D
Phosphorus atom in the center with three single bonds to bromine atoms, and two lone pairs on phosphorus; each bromine has two lone pairs.
Verified step by step guidance1
Step 1: Determine the total number of valence electrons available. 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: \(5 + 3 \times 7 = 26\) valence electrons.
Step 2: Place the phosphorus atom in the center because it is less electronegative than bromine, and arrange the three bromine atoms around it.
Step 3: Form single bonds between the phosphorus atom and each bromine atom. Each single bond consists of 2 electrons, so 3 bonds use \(3 \times 2 = 6\) electrons.
Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule. Start by placing lone pairs on the bromine atoms to complete their octets. Each bromine needs 8 electrons total (including bonding electrons), so add three lone pairs (6 electrons) to each bromine.
Step 5: Assign any leftover electrons to the phosphorus atom as lone pairs. Since phosphorus can have an expanded octet but typically in PBr\(_3\) it has one lone pair, place one lone pair (2 electrons) on phosphorus to complete its octet.
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