Bonds of Common Compounds

Lead (II) Chloride

• polar covalent

Cl (3.0) - Pb (1.8) = 1.2

• The intermolecular force upon PbCl2 is dipole-dipole.  This compound has a partial positive and a partial negative end, therefore resulting in a dipole-dipole force.
• The stronger the intermolecular force is, the more energy required to boil the liquid or melt the solid.  Out of my five compounds, PbCl2 has the highest melting point of 501° Celsius.  This concludes that it has the strongest intermolecular force.

Lead Dioxide 

• Non polar covalent.  The electronegativity is polar, but the molecule is symmetrical, therefore it is not polar. 
• Lead forms a double bond with each oxygen, forming a linear geometric molecule.
• It's dipole-dipole bonds attract the negatives to the positives  

O (3.5) - Pb (1.8) = 1.7

Lead (II) Acetate

• Forms a triangle (120°)
• Boils at 117.1° C, dipole-dipole force is weak upon the molecule

Lead (II) Bromide 

Br (2.8) - Pb (1.8) = 1.0

• This compound is polar, therefore it has a dipole-dipole intermolecular force.  There is a weak attraction that occurs between the negatively and positively charged atoms.
• The melting point for the solid form of this compound is 373° Celsius

Lead (II) Nitrate

• Pb(NO3)2 has the lowest melting point.  This concludes that Lead Nitrate requires the least amount of energy to melt this compound in solid form.  Also, it has the weakest intermolecular force out of my five compounds.