(Polar molecules, Non-polar molecules, etc.)
4 posts • Page 1 of 1
The easiest way to classify shape is to look at the lewis structure of the molecule and determine how many lone pairs and bonding regions there are. Since regions of electron density need to be spaced out symmetrically, this leads to the molecules shape. One you know the electron lone pairs and bonding regions, you will then be able to classify the molecules shape.
SCl4 has a Lewis structure of a central atom S with four Chlorines around it with a lone pair on the central atom. A central atom with four bonded atoms and one lone pair has a seesaw shape. ICl3 has a Lewis structure with I as the central atom and 3 Chlorines surrounding with with two lone pairs. A central atom with 3 bonded atoms and 2 lone pairs is T-shaped. So in order to determine shape, you must draw out the Lewis structure first.
SCl4 has the seesaw shape that Dr. Lavelle talked about in class today (I also believe this is known as a trigonal bipyramidal but I might be wrong with that). ICl4 is square planar. All four bonded atoms are 90 degrees from the central atoms.
Who is online
Users browsing this forum: No registered users and 2 guests