Which statement is false regarding the Lewis structure for XeF_4?

• A. Xenon has two lone pairs in the Lewis structure of XeF_4.
• B. The formal charge on xenon in XeF_4 is +2.
• C. Each fluorine atom in XeF_4 has three lone pairs.
• D. XeF_4 has a square planar molecular geometry.

Answer: (B)

Verified step by step guidance

1. Step 1: Recall the Lewis structure of XeF_4. Xenon (Xe) is the central atom bonded to four fluorine (F) atoms. Xenon has 8 valence electrons, and each fluorine has 7 valence electrons.
2. Step 2: Determine the total number of valence electrons: Xe contributes 8 electrons, and each of the 4 fluorines contributes 7 electrons, for a total of \$8 + 4 \times 7 = 36$ valence electrons.
3. Step 3: Draw single bonds between xenon and each fluorine atom, using 8 electrons (4 bonds × 2 electrons each). Distribute the remaining electrons to complete the octets of fluorine atoms first (each fluorine needs 6 more electrons as lone pairs).
4. Step 4: After completing fluorine octets, place the remaining electrons on xenon as lone pairs. Xenon will have two lone pairs, which accounts for the remaining 4 electrons.
5. Step 5: Calculate the formal charge on xenon using the formula: \(\text{Formal charge} = \text{Valence electrons} - \text{Nonbonding electrons} - \frac{1}{2} \times \text{Bonding electrons}\). Verify if the formal charge on xenon is +2 or zero to identify the false statement.