The figure that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule. (c) Which of the following elements will lead to an AF4 molecule with the shape in (iii): Be, C, S, Se, Si, Xe? i.

ii.

iii.

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Identify the shape of the AF4 molecule in the given image. The shape shown is a seesaw geometry.

Determine the electron domain geometry that leads to a seesaw shape. A seesaw shape arises from a trigonal bipyramidal electron domain geometry with one lone pair.

Count the total number of valence electrons for each element in the list: Be, C, S, Se, Si, Xe.

Determine which of these elements can form a molecule with 5 electron domains (4 bonding pairs and 1 lone pair).

Select the element that fits the criteria. The element must have 6 valence electrons to form a seesaw shape with 4 fluorine atoms and 1 lone pair.

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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. Common geometries include linear, trigonal planar, tetrahedral, and octahedral, each corresponding to specific bond angles and arrangements.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

VSEPR theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs in the valence shell of the central atom. According to this theory, electron pairs will arrange themselves as far apart as possible to minimize repulsion, leading to specific molecular shapes that can be identified based on the number of bonding and non-bonding electron pairs.

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding in a molecule. This process helps explain the geometry of molecules by allowing for the formation of equivalent bonds. For example, in a tetrahedral geometry, the central atom undergoes sp3 hybridization, resulting in four equivalent hybrid orbitals that form bonds with surrounding atoms.