Unit Review

Today we began class by stamping pg 14 and going over the answers.
The answers are as followed:

a) magnesium iodine
b) cobalt (II) sulfide
c) copper (I) sulfide
d) Calcium oxide
e) aluminum chloride
f) manganese (IV) oxide
g) Barium Fluoride
h) Sodium Sulfate
i) Iron (II) Carbonate
j) Calcium Phosphide
k) Manganese (IV)Oxide
l) Aluminum Sulfate
m) Mercury (II) Oxide

Rules to remember when naming ions
-write the cation (first part of name)first,then the anion.
-Make sure to drop the ending of the anion(second part of name) and add -ide. ex: Calcium chlorine turns into calcium chloride.
-When given a polyatomic ion look up the name
-When given a transition metal, determine the number of electrons lost and indicate the charge using roman numerals.

ex: FeCl3 (This means we have 1 Fe and 3 Cl)
Look up the charge of Cl, it's -1

Fe
Cl-1
Cl-1 = -3
Cl-1
Because there are 3 Cl's with a -1 charge, there is an overall -3 charge
Next you determine what charge you would need in order for the ion to be neutral.
In this example you need a +3 charge, so the new name becomes: Iron (III) Chloride

Next we reviewed the entire unit as a class, by filling in the Review & Topic outline pages 1 and 2.
Some of the material we reviewed included:
-Whether an element will gain or lose and election and the amount it will gain/lose.
-Completing an orbital diagram and the electron configuration
-How to write the formula of 2 given ions
-How to name the compounds when given the formula
-Naming polyatomic ions
-Naming transition metals in a formula

Homework
Study for the test tomorrow!
Webassigns due Thursday at 11:59pm