Draw the Lewis Dot Structure for the following ion:PCl₄⁺.

• A.
• B.
• C.
• D.

Answer: (B)

Verified step by step guidance

1. Identify the total number of valence electrons available. Phosphorus (P) has 5 valence electrons, and each Chlorine (Cl) has 7 valence electrons. Since the ion has a +1 charge, subtract one electron from the total.
2. Calculate the total number of valence electrons: 5 (from P) + 4*7 (from 4 Cl atoms) - 1 (due to the +1 charge) = 32 electrons.
3. Place the phosphorus atom in the center as it is less electronegative than chlorine, and arrange the four chlorine atoms around it.
4. Form single bonds between the phosphorus atom and each chlorine atom. Each bond uses 2 electrons, so 4 bonds will use 8 electrons.
5. Distribute the remaining electrons to satisfy the octet rule for each chlorine atom. Each chlorine should have 6 more electrons to complete its octet, using up the remaining 24 electrons. Ensure the structure reflects the +1 charge by enclosing it in brackets and indicating the charge.