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Draw the Lewis structure for PCl6−, then answer the following questions:
11. Bonding & Molecular Structure
Lewis Dot Structures: Ions
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In the Lewis dot structure of the chlorate anion (ClO3-), how is the central chlorine atom surrounded?
A
Two bonding pairs and two unshared pairs of electrons
B
One bonding pair and three unshared pairs of electrons
C
Three bonding pairs and one unshared pair of electrons
D
Two double bonds and no unshared pairs of electrons
Verified step by step guidance1
Identify the total number of valence electrons in the chlorate anion (ClO3-). Chlorine has 7 valence electrons, each oxygen has 6, and the extra negative charge adds 1 more electron, giving a total of 7 + (3 * 6) + 1 = 26 valence electrons.
Place the chlorine atom in the center as it is less electronegative than oxygen, and connect each oxygen atom to the chlorine atom with a single bond. This uses up 6 electrons (2 electrons per bond).
Distribute the remaining 20 electrons to satisfy the octet rule for the oxygen atoms first. Each oxygen needs 8 electrons total, including the bonding pair. Distribute 6 electrons to each oxygen atom as lone pairs, using up 18 electrons.
With 2 electrons remaining, place them as a lone pair on the central chlorine atom. Now, check the formal charges to see if the structure can be optimized.
To minimize formal charges, form a double bond between the chlorine and one of the oxygen atoms by converting one lone pair from an oxygen atom into a bonding pair. This results in the chlorine atom having three bonding pairs and one lone pair of electrons.
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