Lesson Review: Socrative Teacher Code: LR2E0KJH
1. Review the previous lesson.
2. Discussion of the nature of chemical reactions
4. Analyze results.
1. Observe and describe the reactants and products of a chemical reaction.
2. Determine the percent yield of the reaction.
3. Explain whether or not mass was conserved.
4. Evaluate how to improve the experiment.
Weebly Links: Chemical Reactions
Textbook Readings: 1.1; p. 6-8
Mission 1: Here We Go Again! As we've been talking about, chemical reactions summarize chemical change and are represented by chemical equations. Reactants are on the left and products are on the right. Equations are balanced using coefficients to ensure that mass is conserved (we can't break that law, y'all). State symbols are used to denote the state of matter each reactant and product are in at the time of reaction.
Reminder: (s) = solid (l) = liquid (g) = gaseous (aq) = aqueous (dissolved in water)
Having said all that, let's take a look at the reaction of copper metal in aqueous silver nitrate. It's on the board and you should have it in your notes.
Mission 2: See, What Had Happened Was...Well, what happened? What did you see? What should you have seen? Did you understand what happened and why? We were supposed to get a certain amount of silver. Did we get it? Why or why not? What's the problem? Aren't reactions supposed to work?
Guess we need to talk about that a little more then, right? How would you evaluate this demonstration? How would you improve it and why? If you were doing this with my grade 10s, how would you do it?
Homework: We're going to wrap up Section 1.1 and move back to Section 1.2. Be sure to read pages 10-14 (again) and focus on how matter changes states (or phases) via changes in temperature and/or pressure, and how to read a phase diagram (p. 13).
Next Class: Empirical & Molecular Formulas