which is the correct lewis structure for pbr₃?

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Accepted Answer

# Brief Explanations:
Lewis structures show valence - electron distribution. Phosphorus ($P$) has 5 valence electrons and each bromine ($Br$) has 7. In $PBr_3$, $P$ forms three single bonds with $Br$ atoms (using 3 of its 5 valence electrons). The remaining 2 valence electrons on $P$ form a lone pair. Each $Br$ atom has 6 non - bonding electrons (lone pairs) after forming a single bond.

- In the first structure, there are no lone pairs shown on $Br$ atoms, so it is incorrect.
- In the fourth structure, the central atom is wrongly assigned (should be $P$ not $Br$ as $P$ is less electronegative and forms the central atom in $PBr_3$), so it is incorrect.
- Comparing the second and third structures: The third structure has all the lone pairs accounted for (6 on each $Br$ and 2 on $P$). The second structure may be missing some lone - pair representation (if we assume full compliance with Lewis structure rules where all valence electrons are shown as bonds or lone pairs).

# Answer:
The third structure (the one with $\colon Br\colon - P - \colon Br\colon$ and $\colon Br\colon$ below $P$, with all $Br$ having 6 additional dots around them and $P$ having 2 additional dots) is the correct Lewis structure for $PBr_3$.

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