Tuesday, October 5

Like always, class started with a quick recap of last night's blog and yesterday's lesson. Mr. Henderson gave us a heads up on coming up assignments and a little of whats going to happen this week. He reminded us that we have several webassign assignments and labs that were due.

After that, Mr. Henderson told us to open up to page seven, where we would learn how to name ionic compounds. We were given a set of chemical formulas and names of ionic compounds. We were told to find patterns in them. In the chemical formula, we found that the subscripts on the formula give info about the charges on the ions. He said that they followed the principle of electrical neutrality, which means that the sum of all positively charged ions always equal the sum of all the negatively charged ions. In the names of the ionic compound we found that they were made up of two words. The first part was metal, which was then followed by a non-metal. The first word was always the actual name of th

e metal, while the second word ended with -ide. Also, we found that in ionic compounds di- and tri- were not used. Then, we were given problems five and six to solve. On problem five we were given four chemical formulas, which we were suppose to name. The answers to problem five were:

NaBr-Sodium Bromide BaO- Barium Oxide CaF2-Calcium Fluoride Al₂S3-Aluminum Sulfide

On problem six we were give names of four ionic compound, which we were suppose to write the chemical formula. The answers to problem six were:

potassium chloride- KCl sodium sulfide-Na₂S

calcium bromide- CaBr₂ aluminum fluoride- AlF₃

After we were done with page seven, we moved to page eight. On this page, we had to name ionic compounds, but they were different than the ones on page seven. They had roman numerals next to their names. The roman numerals represented the charge of the metals. Also, all the metals were transition metals and Pb+Sn. All these metals could posses different types of charges. For example, iron could have 2, 3, or 5 charges and rarely 4 or 6 charges. Afterwards, we were given problems six and seven to complete. Problem six was similar to problem five on page seven and problem seven was similar to problem six on page seven. The answers to problem six were:

FeBr₃- iron (III) bromide

NiS- nickel (II) sulfide

CoCl₂- cobolt (II) chloride

FeBr₂- iron (II) bromide

AuCl₃- gold (III) chloride

SnF₂- tin (II) fluoride

The answers to problem seven were:

copper (I) chloride- CuCl iron (III)oxide- Fe₂O₃

tin (IV) fluoride- SnF₄ iron (II)sulfide- FeS

After answering the problems on page eight, class ended. For homework, we were given a choice to do some of the work at home or to work on it at the computer lab tomorrow. If you require a more detailed explanation on how to name ionic compounds, I recommend you check out this website.

http://chemistry.about.com/od/nomenclature/a/nomenclature-ionic-compounds.htm