Which of the following statements correctly describes the Lewis dot structure of the ClF_2^+ ion?

• A. Fluorine is the central atom, bonded to two chlorine atoms, with two lone pairs on fluorine.
• B. Chlorine is the central atom, bonded to two fluorine atoms, with no lone pairs on chlorine.
• C. Chlorine is the central atom, bonded to two fluorine atoms, with three lone pairs on chlorine.
• D. Chlorine is the central atom, bonded to two fluorine atoms, with one lone pair on chlorine.

Answer: (D)

Verified step by step guidance

1. Step 1: Identify the central atom by considering electronegativity and bonding preferences. Chlorine (Cl) is less electronegative than fluorine (F), so chlorine is typically the central atom in ClF_2^+.
2. Step 2: Determine the total number of valence electrons. Chlorine has 7 valence electrons, each fluorine has 7, and since the ion has a +1 charge, subtract one electron from the total count: Total electrons = 7 (Cl) + 2 × 7 (F) - 1 (charge).
3. Step 3: Draw single bonds between the central chlorine atom and each fluorine atom, using 2 electrons per bond. Subtract these bonding electrons from the total valence electrons to find the remaining electrons for lone pairs.
4. Step 4: Distribute the remaining electrons as lone pairs, first completing the octets of the fluorine atoms (each fluorine needs 6 more electrons to complete its octet after bonding).
5. Step 5: Assign any leftover electrons to the central chlorine atom as lone pairs. Then, check the formal charges to ensure the structure is consistent with the +1 charge on the ion, confirming that chlorine has one lone pair.