Lessons 21 and 22

(I'll just combine the two into one summary.)

In Lesson 21, we learned more about ionic compounds, diving further into understanding how they work with a simple card game in which one has 8 cards, all numbered 1 to 7, with a goal to make a total # of 8 "valence electrons" out of two, three, or four cards whilst also creating an ionic compound between a metal and a nonmetal. While the game was easy, repeatedly drawing a card with a 7 from it on the deck was awful, haha. In Lesson 22, we played another card game, this time centered around polyatomic ions. Polyatomic ions are just what their name suggests: ions with multiple atoms in them. They have a charge. Common polyatomic ions include CO3 (carbonate), NH4 (ammonium), OH (hydroxide), and SO4 (sulfate). The goal of our second game was to create a polyatomic compound with two, three, four, or five cards. The compounds had to include a positively-charged cation (which was usually a single element) and a negatively-charged anion (which was usually the polyatomic ions.) We had to snatch up more cards if needed to balance out our own compounds.

Lesson 21 Problems:
1.) Explain how to use the periodic table to determine the charges on ions. As you get closer to the noble gases on the table, your charge becomes more and more negative. As you get closer to group 1A, your charges become more positive.

7.) Predict the formulas for ionic compounds between the following metals and nonmetals:
A.) Al and Br Al3Br
B.) Al and S AlS2
C.) Al and As AlAs
D.) Na and S NaS2
E.) Ca and S CaS
F.) Ga and S GaS2


Lesson 22 Problems:
1.) What is a polyatomic ion? A polyatomic ion is an ion that has multiple atoms in it. It has a charge, and that charge is usually negative.

3.) Write the names of the following compounds:
A.) NH4Cl Ammonium chloride
B.) K2SO4 Potassium sulfate
C.) Al(OH)3 Aluminum hydroxide
D.) MgCO3 Magnesium carbonate