1. Outcomes – February 23-24 What level of thinking is: Determining whether the law of conservation of mass was obeyed in a chemical reaction when balancing equations? Differentiating between types of reactions? Judging if a metal will be replaced with another element in a single replacement reaction

2. Bellwork • Balance the equation: Pb(OH)2 + HCl H2O + PbCl2 • Take out the Unit 8 Part 3 packet (the one you got two days ago) • Begin to read Section 9.2 in the textbook

3. Page 7 • 1. Two moles of potassium iodide (aqueous) plus lead (II) nitrate (aqueous) YIELDS lead (II) iodide (solid) plus two moles of potassium nitrate (aqueous)

4. 2. Six moles of aqueous hydrochloric acid plus two moles of solid aluminum YIELDS two moles of aluminum chloride (aqueous) and three moles Hydrogen gas

5. Page 7 continued • 3. a. KI, Pb(NO3)2 b. HCl, Al • 4. a. PbI2, KNO3 b. AlCl3, H2 • 10. The subscripts tell you how many atoms of the element are in the compound. • If a subscript is outside of the parentheses, then you distribute (multiply) the subscript to the subscripts of the elements within the parentheses. • 10.c. We would say that there are two nitrates (NO3) in the compound

6. Page 9 • 1. a. Reactants: 1 atom Mg; • Products: 1 atom Mg • b. Ag (silver) • c. Mg + Ag2S  MgS + 2Ag • 2. Step 1. Fe(s) + O2  Fe2O3 • Step 2 . Fe: 1, O: 2 • Step 3. Fe:2, O:3 • Step 4. 4Fe(s) + 3O2  2Fe2O3 • Step 5. Done • Step 6. Done

7. Page 9 • 3. a. We need to write the coefficients in the lowest possible ratio. (Step 5)

8. b. MgNO32 should be  Mg(NO3)2 • Mg(NO3)2 + 2K  Mg + 2KNO3 - already balanced

9. c. AlCl3 + 3AgNO33AgCl + Al(NO3)3 --- coefficients • Now it’s balanced!

10. Independent Practice • Page 11 – Reactivity Series • Balancing Equations IP worksheet