The Creation of Magnesium Oxide

On block day we started a lab. First we had to find the balanced equation for magnesium and oxygen reacting to form magnesium oxide. Using the stoichiometry format, we had to calculate the mass of magnesium needed to form 0.60 grams of magnesium oxide. It turned out to be 0.36 grams of magnesium. After cutting the needed amount, it was put into a crucible and put on a fire to burn. It took a long time and I was getting impatient.

This was the end result and my group got an percent error of 33% a little much...but it's ok! I'm just looking forward to the three day weekend! =)

Stoichiometry

Stoichiometry! What a difficult and confusing subject. Changing grams to moles to grams to moles gets too complex. I didn't get it at all at first, but after a few more practice problems and I think I have the hang of it now. I hope I don't forget how to do those problems, or else that won't be very good since the test is soon. It's even going to be an extra credit problem!

There is a total of seven steps to these types of problems. Starting with the given, changing g x to mol x, then mol x to mol y to g y, cancel, and box your answer with the units! Just typing that gets me confused, but when I go to write it down, hopefully I will understand it more.

BOOM BOOM REACTIONS!

I have learned how to balance...CHEMICAL EQUATIONS! There are so many types of reactions, but we only have learned about single replacement, double replacement, combustion, and synthesis. To increase a reactions rate you have to increase the temperature, surface area, or concentration. Catalysts also speed up the reaction rate without being sucked into the reaction.

Some reactions that happen every day is iron turning into rust! I also saw one first hand when Mr.Olson smashed cannon balls covered in aluminum foil creating sparks. My favorite was the gas turning into flame, but I kept thinking the roof was going to burn down.

Acids and Bases

Acids and bases are quite the opposites. Acids have a pH of 0 to 6, 7 is neutral, and 8 to 14 is a base. Some examples of strong acids are hydrochloric acid and nitric acid, weak ones are acetic acid and hydro fluoric acid. Some strong bases are sodium hydroxide and calcium hydroxide and some weak ones are ammonia and methylamine!

Acids are proton donors and bases accept protons. Acids have high hydrogen concentrations, while bases have high oxide concentrations!

Solutions!

Earlier we learned about chemical solutions. There are two general types, homogeneous and heterogeneous. Homogeneous solutions look the same throughout, whereas heterogeneous ones are not. Solutions are dilute, with little solute or concentrated, having a lot of solute. Using the molarity equation, molarity=mol/L, I can measure a solution's concentration.

These solutions are very rainbowy and pretty. They are made by mixing different chemicals together!

We also learned how to calculate parts per million and hundred from having the grams of the solute and solution.