(Polar molecules, Non-polar molecules, etc.)
13 posts • Page 1 of 1
The presence of the two lone pairs on the oxygen makes it so that water has a bent (or angular) shape rather than linear. Lone pairs generally take up more space than bonded pairs do (since the electrons exist in a probability cloud rather than being confined in a bond) and so the repulsion of the lone pairs makes the molecule take on a bent shape. Dr. Lavelle will most likely go over this in more accurate detail on Friday.
JinwooLee_1F wrote:I was looking up the VESPR model of H2O and it wasn't linear, which I expected it to be. Are there new models we are going to learn?
Kind of - right now we have only considered the VSEPR model by looking at atoms. However, we also need to consider lone pairs when determining the molecular geometry of a given molecules, such as H2O. In lecture so far we have only considered shape based on atoms. Once we learn how lone pairs affect molecular shape, we will be able to understand why H2O is not linear, but rather bent.
H2O would be bent, with oxygen in the center and one hydrogen on the lower left of oxygen and the other on the lower right. This is due to the polarity of water, with the hydrogen atoms having partial positive charge and the dipole arrows being directed toward the oxygen (partial negative charge). Otherwise, if it was linear, the dipole arrows would cancel each other (both pointing from hydrogen to oxygen) and water would be nonpolar, which is definitely not the case.
Last edited by Nare Nazaryan 1F on Wed Nov 13, 2019 9:58 pm, edited 1 time in total.
Micah3J wrote:I was wondering about the example of the VSEPR Model of CO3 that we went over in lecture today. Does the double bond cause it to have any polarity?
Yes!! C has partially positive charge and O has partially negative charge.
Who is online
Users browsing this forum: No registered users and 1 guest