Multiple Choice
Draw the Lewis Dot Structure for POCl3.
10. Chemical Bonding
Lewis Dot Structures: Exceptions (Simplified)
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Draw the Lewis Dot Structure for the radical hydroxide, OH.
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Verified step by step guidance1
Identify the total number of valence electrons available. Oxygen has 6 valence electrons and hydrogen has 1 valence electron, totaling 7 valence electrons.
Recognize that the hydroxide radical (OH) has an unpaired electron, making it a radical species. This means one electron will not be paired in the Lewis structure.
Place the oxygen atom in the center as it is more electronegative, and connect it to the hydrogen atom with a single bond. This bond uses 2 of the 7 available valence electrons.
Distribute the remaining 5 valence electrons around the oxygen atom to satisfy its octet as much as possible. Place 3 lone pairs (6 electrons) around the oxygen, but remember that one electron will remain unpaired due to the radical nature.
Ensure that the unpaired electron is clearly shown in the structure, typically placed on the oxygen atom, as it is the more electronegative element and can better accommodate the unpaired electron.
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