Question

which option describes the molecule geometry of a molecule with one bond and three lone pairs? (1 point) angled octahedral linear tetrahedral

Explanation:

To determine the molecular geometry for a molecule with 1 bond and 3 lone pairs, we use VSEPR theory. The total number of electron domains (bond + lone pairs) is \(1 + 3 = 4\). The electron - domain geometry for 4 domains is tetrahedral, but the molecular geometry (considering only the bonds) with 1 bond and 3 lone pairs is linear. Let's analyze the other options:

• "Angled" (or bent) geometries typically occur with 2 bonds and 1 or 2 lone pairs (e.g., \(H_2O\) has 2 bonds and 2 lone pairs, bent geometry).
• "Octahedral" electron - domain geometry occurs with 6 electron domains (e.g., 6 bonds or a combination of bonds and lone pairs that sum to 6).
• "Tetrahedral" molecular geometry occurs when there are 4 bonds (e.g., \(CH_4\)) or 3 bonds and 1 lone pair (e.g., \(NH_3\) has a trigonal pyramidal molecular geometry, which is a deviation from tetrahedral due to the lone pair, but still related to the tetrahedral electron - domain geometry).

Answer:

linear