For each structure below:
1) Draw a Lewis Structure
2) Determine the geometry around the central atom (or atoms).
3) Make the model of the structure with a model kit. Does the model show
the geometry of the compound?
4) Determine the hybridization of each central atom.
5) Determine which bonds are polar.
6) Determine if the molecule is polar using part 2 and 5 together.
7) If there are resonance structures possible, draw each of them.
8) If there are more than one possible structure (isomers) draw each
isomer.
CH4
H3 O+
C2H2Br2
NO3SCl4
C2H5OH
SF6
ClF3
NH3
O2
C 2 H2
C2H4Cl2
SCl6
C3H7OH
ClF5
XeF2
H2O
N2
SO2
PCl3
O3
C6H12
XeF4
BF3
N 2 H2
SO42PCl5
NH4+
C6H14
PCl5
CH2Cl2
P4
CO2
SCl2
CH2O
C4H9OH
SF4
Start with ClO1-, then make ClO21-, ClO31-, and ClO41-. Identify the shape of
each. Write the name of each ion. Sketch each one.
Results & Discussion:
Describe the effect of the number of lone pairs and bonds on the shape and
bond angle of the molecule and relate the shapes of the molecules you built to
their expected polarity.