Net Ionic Equations

AP Chemistry Name Net Ionic Equations Period Unit 1 - _ _ CHEMICAL Date _ REACTIONS Part 1: Mini-Lab 1. Put on goggles & tie hair back. 2. Obtain a 100 rnL beaker. Put 20 mL of HCl in the beaker (from the bottle up front). 3. Obtain a small piece of zinc (from the front). 4. Put the zinc into the beaker with the acid, then record your observations. Observations: i \ -\.M~cdcv~r-- -- \0v\c.blt Questions: 1. Did a chemical reaction take place? How do you know? Yf_.5 I'\, --W'M~ ~ -~\1/l~ i::, c-.- 'c,v\ f>.-- rwf·,+1-¥- -~ ~ Si~n aF~ ~· _ '-<'f\-t- ~ 2. The formula for the reaction is: Zn (s) + 2 HCl (aq) ➔ ZnCh (aq) + H2 (g) Lor S~ Draw a particulate diagram of the reactants and the products (the before and the after of the chemical reaction) in the boxes below: Products Reactants cO 3. Check your diagrams for law of conservation of mass. There should be the same amount of each type of atom on either side of the arrow. 4. Compare your two diagrams. Are there any components that do not change from the beginning to the end? Which one? (Yes, there should only be one!) u- 5. Below I've rewritten the orig111al equation, but I've separated out the ionic aqueous substances into their ions. This is because ionic compounds always Zn (s) + 2 H+ (aq) + 2 c1- (aq) ➔ d j s.S:o-CA o,M when they dissolve in water. Zn2+ (aq) + 2 c1- (aq) + H2 (g) Look at the ion you identified in number 4-how does it compare on either side of the equation? Part 2: Modeling Chemical Reactions 1B IA Reacrion 1 D D • • D D D D 1. Which beakers contain solid, insoluble substances? How do .. you know? JC: \G1 + D D 6 6 D ?,,,,A , 7-. C- 1 3A 1 3C. £c)·,ol ,'s cll.-VV\~ • ~lo~ 8oSb Which beakers contain solutions of ionic substances? How do you know? 2. '<:_ 2A 2B + Reaction 2 0 2C '\ D □ D D D D 0 0 □ O D D •□ ~(? O A,\\ D O e D D D e e □ h..,+ ?,~ ft 3Pr $htSW5 c>1so6~.el_ ,~s «; :rn 3A Reaction 3 ID 3C ti) IC. + □ □ u t:,. t:,. t:,. 0 t:; D 6 D •u 6 D D • • 3. Which reactions produce a gas? ±\: 3 D D • n 1• 4. The reactions shown in the beaker are the following three reactions: Zn (s) + 2 I-ICl (aq) ➔ ZnCh (aq) + I-I2 (g) ::d:-3 Zn (s) + Cu(N03)2 (aq) ➔ Zn(N03)2 (aq) + Cu (s) # 2 Zn(N03)2 (aq) + Na2C03 (aq) ➔ ZnC03 (s) + 2 NaN03 (aq) n: \ Match the three reactions to the equations above. 5. Each reaction has some ions that do not change from the beginning to the end. These are called spectator ions. Identify the shape that represents the spectator ion in each reaction. Reaction 1: 6,. Reaction 2: tJ Reaction 3: [] 6. We can also identify spectator ions by the chemical equation. To do this, we must first break apart ionic compounds into their ions, to represent their dissociation in water. Full Equation: Zn (s) + 2 HCl (aq) ➔ ZnCh (aq) + Hz (g) Zn (s) + 2 H+ (aq) + 2 c1- (aq) ➔ Zn2+ (aq) + 2 c1- (aq) + I-I2 (g) Ionic Equation: From the ionic equation we see that c1- doesn't change, so c1- is our spectator ion. Try it for the other two reactions. Full Equation: Zn (s) + Cu(N03)2 (aq) Ionic Equation: ~ (s°"J Ionic Equation: Spectator Ion: Zn(N03)2 (aq) + Cu (s) .J 2 ND.3 - ~ "2:-n-+ 2 -+-ZND~ - -r ~t.s') Nob- Spectator Ion: Full Equation: -I C-t-t'Z ➔ zn(N03)2 (aq) + Na2C03 (aq) l--v,_.z,,l/\/05- N K -t.. I f- --Z No-.. .- ➔ ZnC03 (s) + 2 NaN03 (aq) 4- C0_3-~ _.:, z-.,,.,C03 Cs') .,_ zNo..• -1 -Z /VDJ-