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The nf3 lewis structure represents nitrogen trifluoride, NF3. A correct Lewis structure must satisfy the octet rule for all atoms and verify the distribution of 26 total valence electrons.
Step 1: Count Total Valence Electrons
| Atom | Group Contribution | Subtotal |
|---|---|---|
| N (1) | Group 15: 5 e⁻ | 5 |
| F (3) | Group 17: 7 e⁻ each | 21 |
| Total Valence Electrons | 26 | |
Step 2 & 3: Skeleton and Octet Completion
Connect Nitrogen to three Fluorine atoms with single bonds. Distribute lone pairs to complete Fluorine's octets first, then place the remaining pair on Nitrogen.
Step 4: Formal Charges
| Atom | Valence | Lone e⁻ | Bonds | Formal Charge |
|---|---|---|---|---|
| N | 5 | 2 | 3 | 5 - 2 - 3 = 0 |
| F | 7 | 6 | 1 | 7 - 6 - 1 = 0 |
Step 5: Molecular Geometry (VSEPR)
The central Nitrogen has 4 electron domains (3 bonding pairs + 1 lone pair). This results in a Trigonal Pyramidal molecular geometry.
Summary
- Valence Electrons: 26
- Geometry: Trigonal Pyramidal (AX₃E)
- Bond Angle: ~102° (less than the ideal 109.5° due to lone pair repulsion)
- Polarity: Polar (dipoles do not cancel)
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