Unit+2-+VSEPR

__**The VSEPR Model**__

- This term stands for valence shell electron pair repulsion model - This model is used to determine the shape of the bond - Click [|HERE] to view a helpful video about the VSEPR model

__**Understanding VSEPR**__

- Lone pairs are able to exert more repulsive force than electrons in a bond - When there are lone pairs, they will push away the electrons associated with the other atoms in the compound, and this creates smaller bond angles - You can determine what shape the bond is by first drawing the compound's Lewis structure. Then you can use the chart to find out what shape the bond is. (compare number of lone pairs and shared pairs) Examples: 1) A bent molecule (ex. water) will have hydrogen 104.5 degrees apart from one another 2) A tetrahedral molecule such as methane (CH 4 ) will have hydrogen 109.5 degrees apart from one another (this is due to the additional repulsion that comes from lone pairs of electrons) 3) H 2 is an example of a linear bond this is because it has no lone pairs, 2 shared pairs (2 total pairs), and the shape resembles a straight line. 4) PH 3 is an example of a trigonal pyramidal bond because it has one lone pair, 4 total pairs, and 3 shared pairs. 5) To get more practice or want more of a challenge, visit the [|VSEPR] page on ChemPractice.

__**Note:**__ The following flow chart can be helpful to determine what a compound's bonding shape is.