1.  Water molecule dipole moment

2.  The polarity of water affects its properties –Causes water to remain liquid at higher temperature –Permits ionic compounds to dissolve in it

3.  In water, Oxygen pulls on the electrons more than the hydrogens do.  This makes the Oxygen end slightly negative and the Hydrogen end slightly positive.  Water molecules attract to each other with hydrogen bonds. Describe the polar covalent bond and it’s effects between water molecules.

5.  Most molecules you learned about in Biology are covalently bonded molecules.

6.  Knowing how many valence electrons an atom has allows you to predict how many covalent bonds it can form.  Now you can draw Lewis dot structures of molecules! Be able to draw the Lewis diagrams of covalent molecules.

8. Metallic Bond – 2a.1  Metal atoms don’t hold on to electrons well in bonds.  This means that electrons are delocalized - free to roam from metal atom to metal atom  These are called metallic bonds and give metals the ability to conduct electricity (electrons) Describe the metallic bond.

11.  Polyatomic ions work in the same way as simple ions  The covalent bonds hold the polyatomic ion together so it behaves as a unit Ionic Compounds Containing Polyatomic Ions

13. 2-

14. -

15. +

16. +

17.  In any substance at any temperature, the forces holding the material together are constantly working against the internal energy of particle motion.  In a solid, there is not enough energy to overcome the Intermolecular forces  In a liquid, there is more energy, but only enough to allow the liquid to take the shape of its container  In a gas, the energy has completely overcome the Intermolecular forces

18.  As temperature (molecular motion) increases, molecules can break free of their IM forces  Melting  boiling Explain how Intermolecular forces and molecular motion interact to create solids, liquids, and gases.

19. 1.) Draw the Lewis Structure for the following atoms: K, Al, Si, O, S, N. 2.) Ionic Bonds happen mainly between ….. 3.) Describe how Ionic Bonds form. 4.)Solve the following equation; 214 84 Po + 2 4 2 He + 2 0 -1 e → _____ 239 92 U + 4 2 He → _____ + 1 0 n 9 4 Be + 1 1 H → _____ + 4 2 He