Multiple Choice
Which of the following represents the correct Lewis dot structure for neutral potassium chloride (KCl)?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
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Which of the following shows the complete Lewis dot structure for NF_3 (nitrogen trifluoride)?
A
N atom in the center with three double bonds to F atoms; N has no lone pairs; each F has two lone pairs.
B
N atom in the center with three single bonds to F atoms; N has three lone pairs; each F has two lone pairs.
C
N atom in the center with three single bonds to F atoms; N has no lone pairs; each F has three lone pairs.
D
N atom in the center with three single bonds to F atoms; N has one lone pair; each F has three lone pairs.
Verified step by step guidance1
Step 1: Determine the total number of valence electrons for NF_3. Nitrogen (N) has 5 valence electrons, and each fluorine (F) has 7 valence electrons. Since there are three fluorine atoms, calculate the total as \$5 + 3 \times 7$.
Step 2: Arrange the atoms with nitrogen as the central atom because it is less electronegative than fluorine, and connect each fluorine atom to nitrogen with a single bond. Each single bond represents 2 shared electrons.
Step 3: Distribute the remaining valence electrons to complete the octets of the fluorine atoms first. Each fluorine needs 8 electrons total (including bonding electrons), so add lone pairs to each fluorine until their octet is complete.
Step 4: Place any leftover electrons on the central nitrogen atom as lone pairs. Check that nitrogen also has a complete octet (8 electrons total) by counting bonding and lone pair electrons.
Step 5: Confirm the Lewis structure by verifying that the total number of electrons used equals the total valence electrons calculated in Step 1, and that all atoms satisfy the octet rule where applicable.
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