CHMA11H3 Study Guide - Final Guide: Molecular Orbital Theory, Valence Bond Theory, Trigonal Planar Molecular Geometry

Give the approximate bond angle for a molecule with an octahedral shape.

A) 109.5°
B) 180°
C) 120°
D) 105°
E) 90°

1. The molecular geometry (shape) of the PF4+ ion is __________. 

1. Tetrahedral

2. Trigonal planar

3. Trigonal bipyramidal 

4. Octahedral 

5. Trigonal pyramidal

2. Using VSEPR Theory, the predicted Cl-B-Cl bond angle for BCl3 is __________.

1. 180° 

2. 107° 

3. 120° 

4. 109.5° 

5. 90°

3. Using VSEPR Theory the molecular geometry (shape) for SF4 is __________.

1. Square planar

2. Trigonal bipyramidal 

3. T-shaped 

4. Octahedral 

5. See-saw

Draw the Lewis structure for , then answer the following questions:

a. How many valence electrons does this compound have?

b. How many bonded electrons does this compound have?

c. How many lone pairs of electrons does this compound have?

d. How many single bonds does this compound have?

e. How many double bonds does this compound have?

f. What is the electron group arrangement (aka electron pair geometry) (enter one of the following: linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral)?

g. What is the molecular arrangement (aka shape) (enter one of the following: linear, trigonal planar, tetrahedral, trigonal pyramidal, bent, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal, square planar)?

h. Predict the approximate bond angle (enter e.g. 90, 109.5, 120, 180, <109.5, >109.5).