The Activity Series

1. The Activity Series Text Reference: 3.3 (pg. 125 - 128)

2. Definition • The activity series of metals is an empirical tool used to predict products in displacement reactions and reactivity of metals with water and acids in replacement reactions and ore extraction. • Example - 2 Mg (s) + TiCl4 (l) → Ti (s) + 2 MgCl2 (s) • Magnesium is used to produce Titanium from Titanium Tetrachloride. The reaction happens as Mg is higher in the Activity Series table than Ti

3. Let’s look at several reactions: Fe + CuSO4  Cu + Fe2(SO4)3 Li + H2O  LiOH + H2 Such experiments reveal trends. The activity series ranks the relative reactivity of metals. Metals near the top are most reactive and will displace metals near the bottom. Q: Which of these will react? Fe + CuSO4  Ni + NaCl  Li + ZnCO3  Al + CuCl2  Cu + Fe2(SO4)3 NR (no reaction) Zn + Li2CO3 Cu + AlCl3

4. cold H2O hot H2O H is the only nonmetal listed. H2 may be displaced from acids or can be given off when a metal reacts with H2O (producing H2 + metal hydroxide). The reaction with H2O depends on metal reactivity & water temp. Q: will Mg react with H2O? steam A: No for cold, yes if it is hot/steam Mg + H2O  H2 + Mg(OH)2 acid Q: Zn + HCl  H2 + ZnCl2 Complete these reactions: Al + H2O(steam)  Cu + H2O  Ca + H2SO4  Na + H2O  H2 + Al(OH)3 NR H2 + CaSO4 H2 + NaOH

5. Other Activity Series Information • All metals will have a specific place in the activity series. For simplicity, only the most common metals are shown. • The metals near the top of the activity series are more reactive because their valence electrons are more easily removed. • On tests and exams the activity series may appear as K, Na, … Ag, Au; you must remember that K is reactive, Au is not. • If the valence of a metal is not indicated in the question, use its most common valence (in bold on your periodic table) to determine the correct chemical formula.

6. The formation and behavior of oxides can also be predicted via the activity series. Complete these reactions: Ca + O2  Au + O2  Fe2O3+ H2 Oxides Oxides form via the addition of oxygen: K + O2  K2O Oxides plus H2 (with heat) will change to metal and H2O: NiO + H2  Ni + H2O heat CaO Oxides decompose with heat: HgO  Hg+O2 NR heat heat Fe + H2O

7. How can you remember the Activity Series Order? • Potassium > Sodium > Calcium > Magnesium > Aluminum > Zinc > Iron > Tin > Lead > Hydrogen > Copper > Mercury > Silver. • Popular Scientists Can Make A Zoo In The Low Humid Country More So • ……your turn

8. Homework ACTIVITY LAB tomorrow. Review Displacement and Activity Series concept. Review page 131 in textbook and come to class on Monday prepared to tell me what your steps are {you must have them written down to proceed}

9. Activity series lab • On the next slide, place a check in the corner of boxes where you think reactions will take place. • Get a plastic spot plate. • Combine chemicals specified in the chart. Figure out a way to keep track of the chemicals. Use a ¼ scoop for solids (the less, the better). Use 1 squeeze of an eyedropper for solutions. • Write chemical equations for chemicals that reacted. Write NR where there was no reaction. • Dump used chemicals into the large funnel at the front of the room (use a squirt bottle to rinse remaining chemicals into the funnel). Wash the spot plate and glass rod very well. Dry & return.

10.    Mg + AgNO3  Ag+ Mg(NO3)2 Cu + AgNO3  Ag+ Cu(NO3)2 Zn + AgNO3  Ag+ Zn(NO3)2 AgNO3   Mg + H2SO4  H2 + MgSO4 Zn + H2SO4  H2 + ZnSO4 H2SO4 NR   Mg+ Fe(NO3)3  Fe+ Mg(NO3)2 Zn+ Fe(NO3)3  Fe+ Zn(NO3)2 Fe(NO3)3 NR   Mg + CuCl2  Cu + MgCl2 Zn + CuCl2  Cu + ZnCl2 CuCl2 NR