Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the formate ion, HCO2-?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Ions
Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the ion ICl_2^-?
A
The central iodine atom is surrounded by two chlorine atoms and one lone pair, resulting in a trigonal planar geometry.
B
The central iodine atom is surrounded by two chlorine atoms and three lone pairs, resulting in a linear geometry.
C
The central iodine atom is surrounded by two chlorine atoms and no lone pairs, resulting in a linear geometry.
D
The central iodine atom is surrounded by two chlorine atoms and two lone pairs, resulting in a bent geometry.
Verified step by step guidance1
Identify the central atom in the ion ICl_2^-. Since iodine (I) is less electronegative than chlorine (Cl), iodine will be the central atom.
Determine the total number of valence electrons. Iodine has 7 valence electrons, each chlorine has 7 valence electrons, and there is an extra electron due to the negative charge. So, total valence electrons = 7 (I) + 2 × 7 (Cl) + 1 (charge) = 22 electrons.
Draw single bonds between the central iodine atom and each chlorine atom. Each bond uses 2 electrons, so subtract 4 electrons from the total, leaving 18 electrons to be placed as lone pairs.
Distribute the remaining 18 electrons as lone pairs, first completing the octets on the chlorine atoms (each needs 6 more electrons to complete octet), then place the remaining electrons as lone pairs on the iodine atom.
Count the number of lone pairs on iodine after distribution. Use the VSEPR theory to determine the molecular geometry based on the number of bonding pairs (2) and lone pairs on iodine. This will help confirm the correct geometry and the correct description of the Lewis structure.
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