1.Build or draw the Lewis structure for each of the molecules listed below.
H2O, NH3, CH4, CO2
2.Build or draw a model of each of the Lewis structures using any of the materials listed above. Here are the steps:

a. For each molecule, represent each element with a spherical (ball shaped) object.
b. Each single bond should be represented with a straight object, two straight objects should be used between two atoms to represent a double bond, and three straight objects should be used between two atoms represent a triple bond.
c. Remember that the lone pairs on the central atom take up space and play a role in determining the shape of the molecule. Represent each lone pair (nonbonded pairs of valence electrons) on the central atom with a nonbonded object. The bonds and lone pairs on the central atom should be spread apart as much as possible. See example in lesson as a reference.



For each of your molecular models, include a Lewis structure drawing or picture of your model. On your drawing or picture, include the following information:
1.What is the central atom?
2.How many atoms are bonded to the central atom?
3.How many lone pairs of electrons are on the central atom?
4.How many single bonds are there in this molecule?
5.How many multiple bonds (double and/or triple) are there in this molecule?


For each of your molecules, answer the following questions:
1.Determine the electronegativity between the atoms of each molecule.
2.Identify the bond as either ionic or covalent.
3.State whether the molecule is polar or non polar.
4.Identify the structure as having hydrogen bonding, dipole-dipole moments or London dispersion forces (LDF).