Today you will be using computers to research a topic. You are required to make your own notes on the following. YOU MUST include diagrams and drawings where given to act as visuals. These notes will be for marks so use pencil crayons and add colour to your work. Please make sure to include a title and date on the top of every new page. Only PARTS A and B will be marked. These notes are due tomorrow .
NEATLY make your own notes on the following:
PART A
1. Click on : http://www.wwnorton.com/college/chemistry/gilbert2/chemtours/chemtour.asp#9 and scroll down/select
Ch. 10, click on “ Intermolecular Forces Tutorial ”. Using the play (triangle), navigate through these questions.

What are intermolecular forces (IMF)? Which macroscopic properties do they determine? Push play to continue.

Draw two water molecules illustrating intra and intermolecular forces. Push play to continue.

What is an ionic bond? What is the IMF for ionic compounds? Push play to continue.

How can the strength of ion-ion forces be determined? Give an example and explain. Push play to continue.

What IMF act between two polar molecules? Give an example. Push play to continue.

What happens to the IMF when the polarity of the molecule increases? Push play to continue.

What is hydrogen bonding? When does it occur? Give an example. Push play to continue.

What are dispersion forces? Give an example.

What is an induced dipole? Give an example. Push play to continue.

Rank all IMF from stronger  weaker IMF.

What does miscible and immiscible mean? What determines if substances will be soluble in other substances?

What are ion-dipole forces? Give an example. Push play to continue.
Questions : a. Rank the following substances from strongest to weakest IMF. (He, NH
3
, NF
3
, NaCl) b. Rank the following substances from strongest to weakest IMF. (HF, F
2
, FCl) c. Rank the following substances from strongest to weakest IMF. (NaCl, MgCl
2
, AlCl
3
, MgS, NaBr) d. Are ammonia (NH
3
) and water (H
2
O) miscible? Push play to continue. e. Would you expect KBr to be a solid, liquid or gas at room temperature?
PART B
1. Click on the following :

What are non-polar and polar bonds? Give an example of each.

Explain how symmetry is involved in determining if bonds are polar or non-polar. Give examples.
2. Explain why the following are polar or non-polar molecules: H
2
, NCl
3
,
CO
2
, AlCl
3
, CH
4
, HCN, H
2
O, NH
3
.
Draw partial charges as part of your explanation.
PART C
These websites are for your information only, to give you supplementary information needed to gain a better understanding of Intra/Intermolecular forces …Take a look through them  http://members.aol.com/profchm/intermol.html
1. If you are curious to read about formal charges click on this link: http://www.cornellcollege.edu/chemistry/chemstds/fcharge.shtml
2. Close off this window and make sure you are back onto the http://www.wwnorton.com/chemistry/overview/ch7.htm
website and click on “ Expanded Valence Shell Tutorial ” (in green). Briefly, make your own notes on what this is. Check out the formal charges section too.
Formal charges are used to determine the exact Lewis structures. Check out the formula FC = # VE initially on the central atom
– (nonbonding electrons on the central atom + # of bonds on the central atom)
3. Use FC’s to determine the Lewis structure of AsO
3
3, AsO
4
3. Is NF
5
a legitimate molecule? Try drawing the shape.
What is its formal charge on Nitrogen?

Determination of Formal Charge
1. Count the valence electrons that "belong" to each atom.

Unshared pairs belong entirely to the atom on which they reside.

Shared pairs of electrons are divided evenly between the atoms by which they are shared: half "belong" to one atom, and half "belong" to the other. (This way of counting electrons is different than that used for counting octets.
When you count for an octet, shared pairs are counted twice, once for each of the sharing atoms.)
2. Compare the number of valence electrons that "belong" to each atom to the number of valence electrons brought into bonding by that atom.

Carbon always brings 4 valence electrons into bonding.

Nitrogen always brings 5 valence electrons into bonding.

Oxygen always brings 6 valence electrons into bonding.

The halogens always bring 7 valence electrons into bonding.

Hydrogen always brings 1 valence electron into bonding.
3. If the number of valence electrons brought into bonding is different from the number that "belong" to the atom, the atom has a formal charge.

If the number of electrons that "belong" is one more than the number brought into bonding, the formal charge is -
1.

If the number of electrons that "belong" is one less than the number brought into bonding, the formal charge is
+1 .
 etc.

If the number of electrons that "belong" is the same as the number brought into bonding, the formal charge is 0 .
4. The sum of the formal charges is the charge of the species.

If the sum of the formal charges is 0 , the species is a molecule.

If the sum of the formal charges is not 0 , the species is an ion.