We’re asked to determine which of the following elements: Li, B, N, Al, P, and Cl will lead to an AF3 molecule with the shape in (ii) as shown below:
To do so, we first need to draw a Lewis structure for a molecule AF3 where A = central atom, F = terminal atoms for each given element.
For this, we need to do the following steps:
Step 1: Assign elements to form a bond and Determine the central atom in the resulting molecule.
Step 2: Calculate the total number of valence electrons present.
Step 3: Draw the Lewis structure for the molecule.
Step 4: Determine the shape of the molecule and whether it matches the shape in (ii):
The possible molecular shapes are:
Note that the shapes that follow an AF3 (or AX3) molecule are: trigonal planar, trigonal pyramidal and T-shaped.
From the given ball and stick figures, we can see that:
This figure shows ball-and-stick drawings of three possible shapes of an AF3 molecule.
Which of the following elements will lead to an AF3 molecule with the shape in (ii): Li, B, N, Al, P, Cl?
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Molecular vs Electron Geometry concept. You can view video lessons to learn Molecular vs Electron Geometry. Or if you need more Molecular vs Electron Geometry practice, you can also practice Molecular vs Electron Geometry practice problems.
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Based on our data, we think this problem is relevant for Professor Robins' class at UNLV.