Question

1. A molecule has 2 double bonds on the central atom and no lone pairs. Predict the electron geometry. Predict the molecule geometry. What do you think the bond angles would be?
Ans-The molecular and electron geometry is linear and the bond angles is 180 degrees.

2. For each of the molecules below, determine the electron geometry, molecule geometry, and bond angles. Draw pictures to show your geometries.

a. CCl4 (4 Cl atoms, no lone pairs on C)




b. PF3 (3 F atoms, 1 lone pair on P)




c. OF2 (2 F atoms, 2 lone pairs on O)




d. I3- (2 I atoms and 3 lone pairs on central I)

3. Use any resources required to add names to all the geometries in the table on page 3.

Answer 1

Answer:

The Lewis electron-pair approach can be used to predict the number and types of bonds between the atoms in a substance, and it indicates which atoms have lone pairs of electrons. This approach gives no information about the actual arrangement of atoms in space, however. We continue our discussion of structure and bonding by introducing the valence-shell electron-pair repulsion (VSEPR) model

Answer 2

Question:-1. A molecule has 2 double bonds on the central atom and no lone pairs. Predict the electron geometry. Predict the molecule geometry. What do you think the bond angles would be?

Answer:-The molecular and electron geometry is linear and the bond angles is 180 degrees.

Question:- For each of the molecules below, determine the electron geometry, molecule geometry, and bond angles. Draw pictures to show your geometries.