draw the lewis structure for the phosphorus tribromide (pbr₃) molecule.
draw the lewis structure for the phosphorus tribromide (pbr₃) molecule.
Answer
Explanation:
Step1: Determine valence - electrons
Phosphorus (P) has 5 valence electrons and bromine (Br) has 7 valence electrons. For $PBr_3$, the total number of valence electrons is $5 + 3\times7=26$.
Step2: Identify the central atom
Phosphorus is the central atom as it is less electronegative than bromine.
Step3: Connect atoms with single bonds
Connect the P atom to each of the 3 Br atoms with single bonds. Each single bond uses 2 electrons, so 6 electrons are used in bonding.
Step4: Distribute remaining electrons
We have $26 - 6=20$ electrons remaining. Place these electrons as lone - pairs on the atoms to satisfy the octet rule. Each Br atom gets 3 lone - pairs (6 electrons per Br), and the P atom gets 1 lone - pair.
Answer:
The Lewis structure of $PBr_3$ has a central P atom with 1 lone - pair, single - bonded to 3 Br atoms, and each Br atom has 3 lone - pairs.