The skeleton structure of dinitrogen difluoride is F N N F. The Lewis structure of N
F
contains ? 2 single bonds, 1 triple bond and 6 lone pairs. ? 3 single bonds and 8 lone pairs. ? 2 single bonds, 1 double bond and 8 lone pairs. ? 3 single bonds and 9 lone pairs. ? 2 single bonds, 1 double bond and 6 lone pairs.
The Correct Answer and Explanation is:
The correct answer is: ✅ 2 single bonds, 1 double bond and 8 lone pairs.
Explanation:
Dinitrogen difluoride (N₂F₂) has the skeletal structure F–N=N–F. It contains two nitrogen atoms and two fluorine atoms. To determine the Lewis structure, start by calculating the total number of valence electrons:
- Each nitrogen atom has 5 valence electrons: 5 × 2 = 10
- Each fluorine atom has 7 valence electrons: 7 × 2 = 14
- Total: 10 + 14 = 24 valence electrons
Next, place a single bond between each atom to establish the skeletal framework:
F–N–N–F uses 3 single bonds, which account for 6 electrons.
Subtracting these gives: 24 – 6 = 18 electrons remaining.
Now distribute lone pairs:
- Each fluorine atom typically has 3 lone pairs (6 electrons) to satisfy the octet rule.
2 F atoms × 6 electrons = 12 electrons - 18 – 12 = 6 electrons remaining
At this point, each nitrogen atom has only 6 electrons around it (from one bond with fluorine and one bond with the other nitrogen). To satisfy the octet rule, form a double bond between the two nitrogen atoms:
- Change the N–N single bond to a double bond, adding 2 more shared electrons
- This uses 2 of the 6 remaining electrons, leaving 4
Finally, place one lone pair on each nitrogen atom (2 electrons each)
- Now all atoms have full octets
Final bonding summary:
- 2 single bonds (each N–F bond)
- 1 double bond (N=N)
- 8 lone pairs total:
- 3 on each fluorine = 6
- 1 on each nitrogen = 2
The Lewis structure of N₂F₂ therefore contains 2 single bonds, 1 double bond and 8 lone pairs.
