How do you find the geometry of #TeCl_4# using the VSEPR method?

1 Answer
Dec 31, 2016

Answer:

Draw the lewis structure to find the electronic geometry and use it to determine the molecular geometry.

Explanation:

For #TeCl_4#, we have 4 bonded species about the central and 1 lone pair of electron about the central atom.

With 5 electron cloud about the central species, #"Te"#, the electronic geometry will be trigonal bipyramidal .

To determine the molecular geometry, we consider the ratio of bonded species to lone pair about the central atom.

There are five electron clouds around the central atom, and the ratio of bonded species to lone pair is 4:1, so the #TeCl_4# species experiences:
"see-saw" molecular geometry, with ideal bond angles of #90^∘, 120^∘ and 180^∘#.

However, the lone pair of electron about the #"Te"# species will cause repulsion and distort the actual bond angles, pushing them further away from itself.

This means the actual bond angles for #TeCl_4# will be slightly less than #90^∘, 120^∘ and 180^∘#.

Consider the graphic below:
enter image source here