Suppose a molecule with six electron groups is confined to two dimensions and has a hexagonal planar electron geometry. A molecule with six electron groups arranged in a hexagonal planar geometry. The top and bottom groups are labeled 1 and 4, respectively. The two groups next to 1 are labeled 2 and the two groups next to 4 are labeled 3. If two of the six groups are lone pairs, where would they located?

The two lone pairs will be located at the top and at the bottom of the plane.

The VSEPR theory is a model that helps to predict the shape of a molecule based on the repulsions associated with the electron groups on the central atom.

Given that a hexagonal planar electron geometry possibly has 6 electron groups. The description of how the electron groups are arranged can be seen in the first image below.

If two of the six groups are lone pairs, we know that lone pairs repel each other. As such, in this arrangement, the lone pairs will occpy the opposite direction which is the top and the bottom of the plane in order to have minimum repulsion as possible.

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Above and below the plane of a square

Explanation:

The number of electron groups often determine the shape of a molecule. When we have a coordination number of six, one of the possible arrangement of groups is the hexagonal planar geometry. In this arrangement, six electron groups are arranged in the same plane.

If two among the groups are replaced by lone pairs, the substituents will arrange themselves at the corners of a square while the lone pairs will be found above and below the plane of the square. This is the square planar geometry.

it's c. elements are placed in rows based on how may valencies electrons have.

it takes on an electronical energy