Which species has the largest F-A-F bond angle, where A is the central atom?

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To determine which species has the largest F–A–F bond angle, we need to consider the geometry around the central atom A and how lone pairs influence bond angles.
Option BF3: boron trifluoride has a trigonal planar geometry with no lone pairs on the central boron. All F–B–F angles are about 120 degrees, which is larger than the angles in the other options.
Option CF4: carbon tetrafluoride adopts a perfect tetrahedral geometry with bond angles of about 109.5 degrees. While substantial, these angles are smaller than the 120-degree angles in BF3.
Option NF3: nitrogen trifluoride features a trigonal pyramidal shape due to one lone pair on nitrogen. Lone pairs repel bonding pairs and push the bond angles down from the ideal tetrahedral value, giving angles around 107 degrees, smaller than 109.5 and certainly smaller than 120 degrees.
Option OF2: oxygen difluoride has two lone pairs on oxygen, producing a bent (V-shaped) structure with an angle typically around 103 degrees. This is noticeably smaller than the angles in the other molecules listed.
Option "I am unsure and need to study this concept to prepare for the exam": while honesty about studying is fine, this choice does not reflect the chemical reasoning and the actual geometries discussed above.
Across these analyses, BF3 consistently presents the largest F–A–F angle because its central atom uses three bonding pairs in a planar arrangement without lone-pair repulsion, yielding the widest separation between fluorine atoms compared to the other geometries.

CHEM 1210 AU2025 (15738) CHEM 1210 Practice Exam #4 v2 (Ch 7.1–7.4, 8, 9.1–9.6)- Requires Respondus LockDown Browser

Which species has the largest F-A-F bond angle, where A is the central atom?

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