Monday, we started with the Naming Ionic Compounds worksheet. This worksheet walked us through naming Ionic Compounds. At first I was confused because I didn't even know what a cation or anion was. I understood what a cation and anion as after Dr. Finnan did some problems on the board. After hearing the problem spoken out-loud, I realized that every ionic compound has a metal. That realization led to me realizing that the metal in the ionic compound is the cation. If the metal is the cation, the other element in the compound, the nonmetal, must be the anion. As we completed the worksheet, I began to catch on and I now understand that a cation is the metal in the compound, and the anion is the nonmetal. For the mist part, this worksheet made sense to me. The main idea I took away from it was that in order to be in existence, the compounds must have a total charge of 0. So if that involves saying it's Fe (II) and not Fe(III) then it's really important to list those factors so we know the total charge is 0.
Also on Monday, Dr. Finnan also showed us the oxidation of copper. Dr. Finnan held a burner next to copper that was already oxidized. The heat of the burner turned the copper touching the flame into pure copper. When Dr. Finnan removed the burner, the pure copper that was made was so hot, it reacted with the oxygen in the air, causing it to oxidize.
On Tuesday, we practiced even more naming. We completed Unit 6 Worksheet 3. This worksheet was practice on naming ionic compounds. Something new introduced in this worksheet was creating the formula given the name. This wasn't very difficult. The elements are given in the name. However, the total charge of the compound must be 0. That was a rule I learned on Monday, so I applied it to the problems on the worksheet, and it worked and it made sense. The rule of the net charge being 0 is very important and it can change the formula of the compound. For example the ionic compound silver sulfide. From the name we know the compound involves Silver, Ag, and Sulfur, S. Sulfur has a charge of 2-. Silver has a charge of 1+. The formula for this compound isn't just AgS. That would mean the net charge is 1-. The name is Ag2S. If we have two silver atoms, both with a charge of 1+, then they cancel out the Sulfur atom with a charge of 2-.
On Wednesday, we were introduced to Polyatomic Ions. Polyatomic ions are ions with more than two elements in them. We learned about polyatomic ions in the Polyatomic ions worksheet. Every polyatomic ion has a special name. There isn't really a trick to figuring them out, you just have to memorize them. At first it was difficult to understand these. I didn't really understand that every polyatomic ion has its own name. I was confused because I was trying to separate the polyatomic ion into the elements it consisted of, to name them separately. I now understand that the polyatomic ion in the compound can't be separated, it has its own specific name. I came to this realization by looking at the formulas for some polyatomic ions. Like BaSO4. The Ba represents Barium. The SO4, is a polyatomic ion with the name sulfate. All you have to do is match the polyatomic formula in the compound with its name. You can't separate the Oxygen form the Sulfur. Together, they create the polyatomic ion sulfate. So the full name of the compound BaSO4 is Barium Sulfate. A difficult component to naming polyatomic compounds is recognizing the polyatomic ion in the compound. There isn't really a trick to this. Once you realize the compound is polyatomic, you just have to check and see what polyatomic is in the compound by looking at the elements involved in the formula.
On Thursday, we focused on naming Molecular Compounds. We completed the Naming Molecular Compounds worksheet. Molecular compounds are between nonmetals, they have covalent bonds. The important thing to remember with naming molecular compounds is that the elements get prefixes. For example, N2O4 is Dinitrogen tetraoxide. The di represents that there are two Nitrogen and the tetra represents there are 4 Oxygen. There are some rules for naming molecular compounds. The second element always ends in -ide, for example, oxide, fluoride, iodide. Second, if the first element listed in the compound has only one atom, it doesn't need the prefix mono, it is implied that the first element has only one atom if it doesn't have a prefix. For example, CO2 is not monocarbon dioxide, it is just Carbon dioxide. Thirdly, there are never two vowels. So it's not monooxide, it's just monoxide. You drop an o. It did not take very long for me o understand this. You just match the prefix with the number of atoms. The difficult part was remembering and recognizing that the prefixes only happen in molecular compounds. Any compound with a metal is not molecular, so it does not have the prefixes.
Reviewing on how to name compounds
On this whiteboard, it is important to note the atoms versus ions. The LiClO3 compound has five atoms. 1 Li, 1 Cl, and 3 O. However, there are only 2 ions. Li and ClO3. ClO3 is the polyatomic ion Chlorate, so you can't separate it into Cl and O3, they have to be together. You can separate Lithium because it is not part of the polyatomic ion.
Prefixes for molecular compounds
On Friday we got the review guide for Unit 6. I understood what was on there and I hope I did well on Monday's test.
This week in science was busy. At first, naming compounds was difficult for me. I didn't understand that the net charge had to be 0. I eventually figured that out and it became much easier. Sometimes you have to change the formula to make the net charge 0 by adding an atom. The difference between covalent and ionic bonds is the metal element in an ionic bond. Covalent bonds, or molecular compounds, get prefixes, and always end in -ide. Compounds with polyatomic ions, aren't that difficult. You just match the polyatomic ion with its name on the blue sheet Dr. Finnan gave us. Those wee the main ideas from week 7 and I look forward to week 8.
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