Concept:The geometry of ammonia is defined by \( \text{sp}^3 \) hybridization with one lone pair.
Formula:$$ \text{Type} = \text{AB}_3\text{E} \implies \text{Trigonal Pyramidal} $$
Solution:- Nitrogen has 5 valence electrons. It uses 3 to bond with Hydrogen atoms, leaving 1 lone pair.
- The 4 electron domains arrange tetrahedrally to minimize repulsion, but the presence of the lone pair makes the observable molecular shape trigonal pyramidal.
Why other options are incorrect:- Option B: Occurs in \( \text{sp} \) hybridized molecules without distorting lone pairs.
- Option C: Describes the electron domain geometry, but the molecular shape (excluding the invisible lone pair) is pyramidal.
- Option D: Occurs in \( \text{sp}^2 \) molecules (like \( \text{BF}_3 \)) with no lone pairs.
Quality & Fidelity Assurance:
Every question on BeambePrep is rigorously curated against the official PMDC syllabus with zero filler, zero out-of-syllabus content, and zero typos. When an authentic past paper originally contained a historical mistake or ambiguity from the examining board (such as UHS or NUMS), BeambePrep faithfully reflects the original paper while detailing the nuance and scientific consensus in the autopsy above.