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Step 1:I'll solve this step-by-step, following the LaTeX formatting guidelines precisely:
Step 2:: Understand Formal Charge Calculation
- $$B$$ = Number of bonding electrons
Formal charge is calculated using the formula: Where:
Step 3:: Determine Valence Electrons for Nitrogen
- Nitrogen has $$5$$ valence electrons
- Nitrogen is in Group 5A
Step 4:: Determine Valence Electrons for Hydrogen
- Hydrogen has $$1$$ valence electron
- Hydrogen is in Group 1A
Step 5:: Draw Lewis Structure of NH^3
- Nitrogen forms $$3$$ single bonds with hydrogen atoms
- One lone pair remains on nitrogen
Step 6:: Calculate Formal Charge for Nitrogen
\text{Formal Charge}_{\text{N}} = 5 - 2 - \frac{6}{2} = 0
- N_{N} = 2 (lone pair electrons)
Step 7:: Calculate Formal Charge for Hydrogen
\text{Formal Charge}_{\text{H}} = 1 - 0 - \frac{2}{2} = 0
- N_{H} = 0
Final Answer
The formal charge for both nitrogen and hydrogen atoms in NH^3 is 0.
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