Multiple Choice
Determine the number of bonding electrons and the number of nonbonding electrons in the Lewis dot structure of OF2. Enter the number of bonding electrons followed by the number of nonbonding electrons, separated by a comma.
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following represents the correct Lewis structure for the neutral compound NOF?
A
N with a single bond to O and a double bond to F, with one lone pair on N
B
N with a triple bond to O and a single bond to F, with no lone pairs on N
C
N with a double bond to O and a single bond to F, with one lone pair on N
D
N with a single bond to O and a single bond to F, with one lone pair on N
Verified step by step guidance1
Step 1: Determine the total number of valence electrons for the compound NOF. Nitrogen (N) has 5 valence electrons, oxygen (O) has 6, and fluorine (F) has 7. Add these together to get the total number of valence electrons.
Step 2: Identify the central atom. In this case, nitrogen (N) is the central atom because it is less electronegative than oxygen and fluorine.
Step 3: Arrange the atoms around the central atom and draw single bonds initially. Connect N to O and N to F with single bonds. This uses up 4 valence electrons (2 for each bond).
Step 4: Distribute the remaining valence electrons to satisfy the octet rule, starting with the most electronegative atoms. Place lone pairs on O and F to complete their octets, then place any remaining electrons on N.
Step 5: Adjust the bonding to ensure all atoms have a complete octet. If necessary, convert lone pairs on adjacent atoms into double or triple bonds with the central atom. In this case, form a double bond between N and O to satisfy the octet rule for all atoms, leaving one lone pair on N.
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