draw the lewis structure for the (pcl₄⁺) ion.
draw the lewis structure for the (pcl₄⁺) ion.
Answer
Explanation:
Step1: Determine valence - electrons
Phosphorus (P) has 5 valence electrons, and each chlorine (Cl) has 7 valence electrons. The ion has a + 1 charge. So the total number of valence electrons is $5+(4\times7)-1=32$.
Step2: Identify the central atom
Phosphorus is the central atom as it is less electronegative than chlorine.
Step3: Connect atoms with single bonds
Connect the P atom to each of the 4 Cl atoms with single bonds. Each single bond uses 2 electrons, so 8 electrons are used so far.
Step4: Distribute remaining electrons
We have $32 - 8=24$ electrons remaining. Place these electrons as lone - pairs on the Cl atoms. Each Cl atom gets 3 lone - pairs to complete its octet.
Answer:
The Lewis structure has a P atom in the center bonded to 4 Cl atoms with single bonds, and each Cl atom has 3 lone - pairs of electrons around it.