(b) If you react BF 3 to make the ion BF 3 2- , is this ion planar?

Hi everyone for this problem we need to rate the molecular geometry of br cl four minus. So we'll start with the lewis structure. We have B. R. In the middle because chlorine is very electro negative and we'll stick the chlorine around it. Yeah. Now typically chlorine has seven valence electrons. And since it gets one from each of the bonds, we need to add some more. So we have 1234567 and we'll add them to each of the chlorine. So typically bro ming would have seven as well. But because this is a minus ion we need to add one more valence electron. So now roaming has valence electrons. Finally, because this is a -1, we need to put brackets around our Lewis structure and put a minus sign after it. Now this shape, the molecular geometry is known as a square, so it's a square planner. So that's going to be the answer to our problem. I hope this video helped you guys out and I'll see you in the next one

Ch.9 - Molecular Geometry and Bonding Theories

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Brown 14th Edition

Ch.9 - Molecular Geometry and Bonding Theories

Problem 39b

Chapter 9, Problem 39b

(b) If you react BF₃ to make the ion BF₃^2-, is this ion planar?

Verified step by step guidance

Identify the central atom in the molecule BF3, which is boron (B).

Determine the electron configuration of boron. Boron has an atomic number of 5, so its electron configuration is 1s² 2s² 2p¹.

Understand the geometry of BF3. In BF3, boron forms three bonds with fluorine atoms, resulting in a trigonal planar shape due to sp² hybridization.

Consider the addition of two electrons to form BF3²⁻. Adding two electrons to the molecule will affect the electron geometry and hybridization.

Analyze the new geometry. With the addition of two electrons, the central boron atom will have a total of five electron pairs (three bonding pairs and two lone pairs), leading to a trigonal bipyramidal electron geometry. However, the presence of lone pairs will affect the molecular shape, making it non-planar.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the shape of the molecule. Understanding molecular geometry is crucial for predicting the spatial orientation of molecules and their reactivity.

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. In the case of BF3, the boron atom undergoes sp2 hybridization, leading to a trigonal planar geometry. This concept helps explain the bonding and shape of molecules, which is essential for determining if a resulting ion like BF3^2- is planar.

Planarity in Ions

Planarity in ions refers to whether all atoms in the ion lie in the same geometric plane. For an ion to be planar, it typically must have a specific arrangement of bonds and electron pairs that allows for such a configuration. Analyzing the electron distribution and molecular geometry helps determine if the ion BF3^2- maintains a planar structure.