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Understanding Ion Transfer and Electron Transfer Reactions in Chemistry

Explore examples of ion transfer reactions in water treatments to understand the rearrangement of ions. Learn about solubility rules and evidence of reactivity in chemical reactions involving ions and salts. Discover electron transfer in batteries and corrosion processes.

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Understanding Ion Transfer and Electron Transfer Reactions in Chemistry

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  1. Transfer of ions • examples: water treatments and water purification • starting from soluble ionic salts, just a simple rearrangement of ions • the driving force for the reaction, is the formation of a (s), (l),or (g) • evidence for chemical reactivity is observed if: • a solid precipitate is seen forming • the (l) symbol for a molecule is written into the balance equation • as in the case for a acid-base neutralization reaction • gaseous bubbles are produced in the reaction mixture

  2. Cu2+ SO42- Na+ NO3- H+ Cl- Ag+ NO3- 2Na+ CO32- Cu2+ SO42- Cu(NO3)2 (aq) CuCl2 (aq) Cu(NO3)2 (aq) Cu(CO3)2 (s) Na2SO4 (aq) H2SO4 (aq) Ag2SO4 (s) Na2SO4 (aq) Na+ NO3- Na2CO3 (aq) NaNO3 (aq) NaCl (aq) Cu(NO3)2 (aq) AgNO3(aq) HNO3 (aq) H+ Cl- HNO3 (aq) H2CO3 = CO2 + H2O AgCl (s) NaCl (aq) Ag+ NO3- Ag2CO3 (s) NaNO3 (aq) 2Na+ CO32- (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) (aq) 1. Write correct ions and ionic salt formulas 2. Apply solubility rules to determine if salts are Soluble (aq) or insoluble (s) in water

  3. Water wedges in between K+ Cl– NaCl dissolves Cl– K+ Solubility Rules for Ionic Salts in H2O • Thus • All ionic salts of group I ions, • Li+, Na+, K+ are solubule in water • All ionic salts of nitrate ion, • NO3_ are solubule in water • All ionic salts of ammonium ion, • NH4+ are solubule in water This solubility separation is called solvation-dissociation

  4. Acids (l) (l) H+ ClO4- (aq) 2H+ SO42-(aq) H+ Cl-(aq) H+ NO3-(aq) Weak Acids Weak Electrolytes Stay as liquids Stay molecular • often have H listed first in their chemical formula • Strong Acids (strong electrolytes)

  5. silver (I) chloride + sodium nitrate Ag+ (NO3)– Na+ Cl- Ag+ Cl- Na+ (NO3)– silver (I) nitrate + sodium chloride Ag NO3 Na Cl Ag Cl Na NO3 (aq) (aq) (s) (aq) 1. Write correct ion and ionic salt formulas 2. Apply solubility rules to determine if salts are Soluble (aq) or insoluble (s) in water

  6. barium phosphate + sodium chloride Na+ (PO4)3- Ba2+ Cl- Ba2+ (PO4)3- Na+ Cl- soduim phosphate + barium chloride Na3PO4 BaCl2 Ba3(PO4)2 NaCl (aq) (aq) (s) (aq) 1. Write correct ion and ionic salt formulas 2. Apply solubility rules to determine if salts are Soluble (aq) or insoluble (s) in water

  7. Transfer of electrons • examples: batteries, corrosion, metabolism • starting from an ionic salt and an element, an element and salt are produced. • the driving force for the reaction is the transfer of electrons which may result in the formation of a (s), (l),or (g) • evidence for chemical reactivity is observed if: • a solid precipitate is seen forming • the (l) symbol for a molecule is written into the balance equation • as in the case for a acid-base neutralization reaction • gaseous bubbles are produced in the reaction mixture

  8. hydrogen gas + magnesium chloride H+ Cl- Mg H2 Mg2+ Cl- hydrochloric acid + magnesium metal HCl Mg H2 MgCl2 (aq) (s) (g) (aq) 1. Write correct ion and ionic salt formulas 2. Apply solubility rules to determine if salts are Soluble (aq) or insoluble (s) in water

  9. silver metal + sodium nitrate Ag+ NO3- Cu Ag Cu2+ NO3- hydrochloric acid + copper metal AgNO3 Cu Ag Cu(NO 3)2 (aq) (s) (s) (aq) 1. Write correct ion and ionic salt formulas 2. Apply solubility rules to determine if salts are Soluble (aq) or insoluble (s) in water

  10. Mgo lost electrons (s) (s) (g) magnesium metal solid oxygen gas magnesium oxide solid ionic salt Oxygen gained electrons Mg O Mg 2+ O2O O2– What reactant was oxidized? What reactant was reduced?

  11. Iron metal lost electrons (s) 4 3 2 iron metal solid (g) (s) oxygen gas iron (III) oxide solid TM ionic salt Oxygen gained electrons Fe 3+ Fe 3+ Fe O O2– O2– O2– O2O What reactant was oxidized? What reactant was reduced?

  12. Combination - Synthesis (the REDOX process defined) iron metal chlorine gas forms iron (II) chloride 1 1 1 Analyzing the half reactions Oxidation OIL Reduction RIG Cl2o + 2e- 2Cl – Feo Fe 2+ + 2e- Fe(s) + Cl2(g) FeCl2 (s) the electrons on the reactant side cancel the electrons on the product side Fe 2+ Cl – Cl – 1 1 1 1 combining both half reactions 1 Fe(s) + 1 Cl2(g) 1 FeCl2 (s)

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