What is the canonical shape associated with a molecule that has 2 bonded atoms and no lone pairs?

Question

BlackTom AI · Accepted Answer

To analyze the question, we start by identifying the electron-domain geometry for a molecule with two bonded atoms and zero lone pairs.
Option 1: trigonal planar. This would arise if there were three regions of electron density around the central atom, typically leading to a 120-degree arrangement in the plane. Since we only have two bonds and no lone pairs, this geometry does not apply.
Option 2: linear. With two bonded atoms and no lone pairs, the electron domains arrange themselves in a straight line, giving a bond angle of about 180 degrees. This is the canonical shape for such a minimal case.
Option 3: trigonal bipyramidal. This geometry corresponds to five regions of electron density and is characteristic of a central atom bonded to five atoms or groups, not just two.
Option 4: octahedral. This arises when six regions of electron density surround the central atom, forming an octahedral arrangement, which again does not match two bonds and no lone pairs.
Option 5: tetrahedral. This shape results from four regions of electron density around the central atom, leading to bond angles near 109.5 degrees, which is inconsistent with having only two bonds.
In summary, only the scenario with exactly two bonds and zero lone pairs yields a straight-line arrangement of atoms, i.e., a linear shape. The other options describe geometries that require additional bonds or lone pairs to create their characteristic angles and arrangements.

CHEM 110 Section 3 (PM) SP25 Pre-Lecture 17 Quiz C08-1-3

What is the canonical shape associated with a molecule that has 2 bonded atoms and no lone pairs?

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