Molecular Shapes Simulation Chloe conatser January 2016 p6
Initial Question~How does the number of substituents around a central atom affect the shape of a molecule?
Hypothesis~
I believe the number of substiuents you have. I.e. Two substienuents will create a linear shape and Three substiunets will create a tripyrmidal.
To test this theory, you will use a simulation online.(http://phet.colorado.edu/en/ simulation/molecule-shapes). To collect data and prove/disprove your hypothesis take screenshots of the molecules you are testing, and the justify them.
Molecule One, H20
The H2O molecule has two lone pairs, and two pairs with Hydrogen. The main element is Oxygen.
Molecule Two, NH3
The NH3 molecule has one lone pair and 3 bonds with Hyrdogen. The main element is Nitrogen.
Molecule Three, CH4
The CH4 molecule has four bonds with Hydrogen and 0 lone pairs. The main element is Carbon.
Molecule Four BrF5
Molecule BrF5 has one lone pair and 5 bonds with Flourine. The main element is Bromine.
Molecule Five SF6
Molecule SF6 has 0 lone pairs and 6 bonds with Flourine. The main element is Sulfur.
Conclusion
The final substiuent for a molecule, I believe determines the shape. For instance molecule four, and five both end with fluorine. They are both octahedrals. A similar situation arose with molecule two and three, where both ended in hydrogen. Each had different number if substiunets, however the ending pairs were the same. If all the electron valances are filled the electron geometry will be the same as the molecular geometry. This is decided by the lone pairs. We know this by comparing molecule 4 and 5.