Which of the following best represents the correct Lewis dot structure for neutral FeBr compound?

• A. Fe with six dots and Br with one dot, connected by a single bond
• B. Fe with eight dots and Br with no dots, connected by a double bond
• C. Fe with two dots and Br with seven dots, connected by a triple bond
• D. Fe with no dots and two Br atoms, each with six dots, both connected to Fe by single bonds

Answer: (D)

Verified step by step guidance

1. Step 1: Identify the elements involved and their valence electrons. Iron (Fe) is a transition metal and typically does not follow the octet rule strictly, while bromine (Br) is a halogen with 7 valence electrons.
2. Step 2: Determine the total number of valence electrons available for bonding. For FeBr, consider Fe's valence electrons (commonly 2 or more depending on oxidation state) and Br's 7 valence electrons each.
3. Step 3: Consider the typical bonding patterns. Bromine usually forms one single bond to complete its octet, and Fe can form multiple bonds with halogens, often coordinating with two Br atoms in a neutral compound.
4. Step 4: Draw the Lewis structure with Fe in the center bonded to two Br atoms, each Br having six dots (three lone pairs) to complete their octets, and Fe having no lone pairs but forming two single bonds with the Br atoms.
5. Step 5: Verify that the overall structure is neutral and that each atom satisfies its typical valence requirements: Br atoms have full octets, and Fe is bonded appropriately without extra lone pairs.