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Why do chemists like (NO 3 - )’s so much?

Why do chemists like (NO 3 - )’s so much?. Because they’re cheaper than day rates!!!. REACTIONS (CONTINUED..). Single Displacement Reactions. By the end of this lesson you will be able to:. Demonstrate an understanding of the activity series for metals and halogens

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Why do chemists like (NO 3 - )’s so much?

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  1. Why do chemists like (NO3-)’s so much? Because they’re cheaper than day rates!!!

  2. REACTIONS (CONTINUED..) Single Displacement Reactions

  3. By the end of this lesson you will be able to: • Demonstrate an understanding of the activity series for metals and halogens • Predict products of a single displacement reaction

  4. Single Displacement Reactions -One element in a compound is displaced (or replaced) by another element. Two types exist • A metal replacing a metal cation in a compound. (2 metals switching spots) • A non-metal (halogen) replacing an anion in a compound. (2 non-metals switching spots)

  5. Example of Type 1: A metal replacing a cation (metal) • Predict the products of the single displacement reaction below: • Mg(s) + HCl(aq) MgCl2(aq) + H2(g) • Rules: • Treat hydrogen as a metal • Treat acids as ionic compounds (HCl = H+Cl-) • Treat Water as ionic (H2O = H+OH-)

  6. Example of Type 1: A metal replacing a cation (metal) • Predict the products of the single displacement reaction below: • Na(s) + H2O(l) NaOH(aq) + H2(g) • Rules: • Treat hydrogen as a metal • Treat acids as ionic compounds (HCl = H+Cl-) • Treat Water as ionic (H2O = H+OH-) • http://www.youtube.com/watch?v=eCk0lYB_8c0 • http://www.youtube.com/watch?v=hqbwPxZsgHs&NR=1

  7. Example of Type 2: A non-metal replacing a anion. • Predict the products of the single displacement reaction below: • F2(g) + NaCl(aq) NaF(aq) + Cl2(g)

  8. Activity Series and Single Displacement Reactions Example: If we have the following reactions, which one will take place? • Fe(s) + CuSO4(aq) → Cu(s) + FeSO4(aq) or • Cu(s) + FeSO4(aq) → Fe(s) + CuSO4(aq) Will the reaction: Li + H2O  LiOH(s) + H2(g) The activity series is used to determine if a single displacement reaction will occur. (ref. pg.

  9. No, Ni is below Na Yes, Li is above Zn Yes, Al is above Cu Yes, Fe is above Cu We have looked 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. It allows us to predict if certain chemicals will undergo single displacement reactions when mixed: metals near the top are most reactive and will displacing 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

  10. cold 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? hot 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

  11. Activity Series of Metals (p.130)

  12. The more reactive metals are at the top of the activity series. • The less reactive metals are at the bottom. • A reactive metal will displace or replace any metal in a compound that is below in the activity series. • So, sometimes, reactions will NOT occur!

  13. 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.

  14. Reactivity Increases Reactivity decreases Activity Series for halogens Activity Series of Halogens • A reactive halogen will displace or replace any halogen in a compound that is below in the activity series. • So, sometimes, reactions will NOT occur! • This activity series mirrors the position of the halogens in the periodic table. F > Cl > Br > I

  15. Using the Activity Series Note: If there is no reaction, write NR. Examples: 1) Cu(s) + MgSO4(aq) → 2) Zn(s) + FeCl2(aq) → 3) K(s) + H2O(l) → 4) Cl2 + 2NaI → 5) I2 + LiCl → • Steps: • Identify if the reaction will involve metals or halogens. • Select the appropriate reactivity series (metal or halogen) • Perform the switch • If there is no reaction, write NR.

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