What is the molecular geometry around the N atom in the molecule depicted?

Question

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The question asks for the molecular geometry around the nitrogen (N) atom in the depicted molecule. Since the image is not described here, we rely on the common scenario for N in many organic or inorganic compounds where N has three sigma bonds and one lone pair.

Option 1: trigonal planar. This geometry arises when the nitrogen has three sigma bonds and no lone pairs, giving three electron domains arranged in a plane with 120° angles. If a lone pair were present (as is typical for N in many neutral amines), trigonal planar would be incorrect because lone pairs count as electron domains and alter the geometry.

Option 2: trigonal pyramid. This is the geometry that results when nitrogen has four electron domains: three bonds and one lone pair. The three bonding pairs form a base (a triangle), while the lone pair occupies the fourth position, producing a pyramidal shape with bond angles slightly less than 109.5° (often near 107° in typical amines). This matches the common case of N with three bonds and a lone pair, which is a very typical scenario for N-containing molecules.

Option 3: tetrahedral. This geometry occurs when there are four bonds and no lone pairs, giving a symmetrical tetrahedral arrangement of four ligands around N. If N had four bonds, this would be tetrahedral, but that would imply four substituents attached to N and no lone pair, which is less common for neutral N in many simple compounds and contradicts the typical three-bond-one-lone-pair case.

Option 4: bent. The bent (or V-shaped) geometry describes molecules like water, where there are two bonding pairs and two lone pairs around the central atom, leading to a bent shape. For nitrogen with three bonds and one lone pair, the arrangement is not bent in the same sense; the expected geometry is trigonal pyramidal, not bent, unless the bonding pattern differs (e.g., only two bonds).

In summary, given the standard scenario for nitrogen with three σ bonds and one lone pair, the electron-domain geometry is tetrahedral, but the molecular geometry is trigonal pyramidal. The other options are inconsistent with having three bonds plus a lone pair: trigonal planar would require no lone pair, tetrahedral would require four bonds, and bent would require two bonds with two lone pairs. Therefore, the most plausible molecular geometry around N in this context is trigonal pyramid.

What is the molecular geometry around the N atom in the molecule depicted?

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