Unit 4; Chemical Bonding and Structure

Electrostatic attraction between oppositely charged ions.

• High boiling and melting point bc strong electrostatic attraction

• Low electrical conductivity when solid bc ions are held in a fixed position

• Brittle & shatter when layers of ions are incorrectly aligned

• High solubility bc water molecules are attracted to the oppositely charged ions

The electrostatic attraction between positively charged nuclei and shared pairs of bonding electrons.

• EN 0.5-1.7 = Polar Covalent

• EN 0.1-0.4 = Non-Polar Covalent

• EN 0 = Pure Covalent

If a molecule is symmetrical, it is non-polar no matter the types of bonds.

• Weakest

• Between all atoms and molecules

• Only between polar molecules

• Caused by the difference in electronegativity

• Molecules that have a nitrogen, oxygen or fluorine atom directly bonded to a hydrogen atom.

• Strongest

• Occurs in all directions between the positive ions and delocalized electrons within the lattice structure.

• Malleable bc the layers of metal ion slide over each other without breaking the bonds

• Delocalized electrons conduct heat and make for a high electrical conductivity.

Homogeneous mixtures composed of two or more metals or a metal and a non-metal. Often stronger and more resistant to corrosion than their component elements.