Accepted answer
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The n2h4 lewis structure for hydrazine consists of two nitrogen atoms bonded to each other, with each nitrogen also bonded to two hydrogen atoms. This molecule contains only single covalent bonds.
Step-by-Step Construction
1) Total Valence Electrons
| Species | Count | Valence e⁻ | Subtotal |
|---|---|---|---|
| N | 2 | 5 | 10 |
| H | 4 | 1 | 4 |
| Total Sum | 14 | ||
2) Connecting the Backbone
Place the two Nitrogen atoms as the central pair and attach two Hydrogens to each. This uses 5 single bonds (10 electrons).
3) Final Electron Placement
Remaining 4 electrons are placed as lone pairs—one on each nitrogen. This completes the octet for both nitrogen atoms.
Formal Charge Calculations
| Atom | Valence | Non-bonding | Bonding | Formal Charge |
|---|---|---|---|---|
| N (each) | 5 | 2 | 6 | 5 - 2 - (6/2) = 0 |
| H (each) | 1 | 0 | 2 | 1 - 0 - (2/2) = 0 |
Key Features
- Connectivity: H₂N–NH₂
- Bond Types: 5 Single Covalent Bonds
- Lone Pairs: 2 Total (1 on each Nitrogen)
- Geometry: Each Nitrogen is trigonal pyramidal (sp³ hybridized)
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