Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the neutral compound CF2S?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the ion IBr2^-?
A
The central iodine atom is surrounded by two bromine atoms and one lone pair, with a single positive charge.
B
The central bromine atom is bonded to two iodine atoms and three lone pairs, with a single positive charge.
C
The central bromine atom is bonded to two iodine atoms and has two lone pairs, with a single negative charge.
D
The central iodine atom is surrounded by two bromine atoms and three lone pairs, with a single negative charge.
Verified step by step guidance1
Identify the central atom in the ion IBr2⁻. Generally, the least electronegative atom (excluding hydrogen) is the central atom. Between iodine (I) and bromine (Br), iodine is less electronegative, so iodine is the central atom.
Determine the total number of valence electrons available. Iodine has 7 valence electrons, each bromine has 7 valence electrons, and there is an extra electron due to the negative charge. So, total valence electrons = 7 (I) + 2 × 7 (Br) + 1 (charge) = 22 electrons.
Draw single bonds between the central iodine atom and each bromine atom. Each bond uses 2 electrons, so subtract 4 electrons from the total to account for bonding.
Distribute the remaining electrons as lone pairs to satisfy the octet rule for the bromine atoms first, then place any leftover electrons on the central iodine atom as lone pairs.
Count the lone pairs on the central iodine atom and confirm the overall charge. The iodine should have three lone pairs, and the ion carries a single negative charge, matching the correct Lewis structure description.
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