Monday, November 8

Mr. Henderson started class today by examining what the rest of this week looks like. We will be learning a new topic for the next couple of days preceding the test, followed by the test Friday. He told us that the test Friday will be composed of: 14 multiple choice questions, 1 double-sided page of writing and balancing equations, no math work, and a section on identifying the reaction type. Mr. H said that what is going to make this test difficult is that it requires a lot of unit 2 work -- writing equations and such. But, we have a very resourceful tool to help us review, this blog! Mr. H walked us through Brooke's blog and talked about how helpful it will be to study for the test. To review, we can also use the Delicious websites created by the class (which, reminder, are due on Thursday!).

We then moved on to the new topic of today, Dissociation and Hydration. He begun this by doing page 11 in our packets. The first small section of this page was identifying a compound as being either ionic or molecular. An ionic compound is one which consists of a cation (metal) and anion (nonmetal), while a molecular compound consist of, normally, two anions. A good, common example of a molecular compound are those hydrocarbons Mr. H keeps talking about. These are the answers to the first part of page 11 ("i" for ionic and "m" for molecular):

1.

a. NaCl I

b. CO2 M

c. NaNO3 I

d. D2H5OH M

e. NH4Cl I

f. C6H12O6 M

If you need extra help distinguishing between the two types of compounds, this is very helpful: http://www.buzzle.com/articles/ionic-compounds-vs-molecular-compounds.html

The following section of the packet introduces a new topic to us, dissociation/hydration. We were supposed to find what the compound looked like after it had dissolved in water (after being broken up into individual ions by the water). The first few problems/answers are:

a. KF(s) -> K+(aq) + F-(aq)

b. CaCl2(s) -> Ca2+(aq) + 2Cl(aq)

c. Na2SO4(s) -> 2Na+(aq) + SO42-(aq)

One of the most difficult things to remember is that Uncle HONClBrIF does not apply to these ions because they're not considered to be "by themselves", but "with" water.

As should be obvious by now, all we are doing is splitting the compound into the ions of which it is made up. But then it gets a little more trickey; we are asked to perform the same type of equation, they give us the name and expect us to derive the formula from that. For example the first question asks what happens when you put lithium phosphate in water:

First, we figure out that the formula for lithium phosphate is Li3PO4

Next, we figure out that the ions of which it is mad up are Li+ and PO43-

Then, we balance the equation to get something which looks like this -- Li3PO4(s) -> 3Li+ + PO43-

After doing a couple more problems like this one, we moved onto yet another new topic. This is the topic of electrolytic (E) and non-electrolytic (NE) solutions. What makes a solution electrolytic is if it is created by ionic compounds, a cation and an anion.

Answers to the last section:

a. NaCl E

b. SO3 NE

c. C2H5OH NE

d. KF E

e. BaCl2 E

f. C12H22O11 NE

He demonstrated this concept through a conductivity test. If, when the wires were placed in the solution, it caused the lightbulb to light, then the solution is electrolytic. This also implies that it contains an ionic compound. He used a video (from the blog) to demonstrate this:

http://g.web.umkc.edu/gounevt/Animations/Animations211/StrongWeakNonElelytes.swf

After this, we moved on to Lab CR2, the Chemical Dropout Lab. We mixed various substances, observing whether or not they each created a precipitate. If a solid developed, or the mixture became cloudy, we knew that a precipitate had been formed.

This picture shows perfectly what precipitates look like.

Overall, today was a very intense day. We were introduced to many new concepts, but luckily Mr. Henderson is explaining them very well and we have many review tools at our fingertips.