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Chapter 10 Chemical Reactivity

Chapter 10 Chemical Reactivity. Four Common Reaction Types : 1) Combination 2) Decomposition 3) Single-replacement 4) Double-replacement But first! Let’s look at polyatomic ions. Compounds Containing Polyatomic Ions.

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Chapter 10 Chemical Reactivity

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  1. Chapter 10Chemical Reactivity

  2. Four Common Reaction Types: 1) Combination 2) Decomposition 3) Single-replacement 4) Double-replacement But first! Let’s look at polyatomic ions

  3. Compounds Containing Polyatomic Ions • Polyatomic ions: single ions containing > one atom covalently bonded • Often look for parentheses Ca(OH)2 • Name & charge of polyatomic ion does notD • Note: no ( ) for single polyatomic group

  4. Memorize Common Polyatomic Ions

  5. Patterns for Polyatomic Ions • Elements in same column form similar • polyatomic ions - same # O’s &same charge:

  6. Periodic Pattern of Polyatomic Oxyanions: the -ate groups

  7. Patterns for Polyatomic Ions • If polyatomic ion starts with an H • add “hydrogen” prefix before name • and add +1 to charge CO32−= carbonate HCO3− = hydrogen carbonate

  8. Patterns for Polyatomic Oxyanions • -ate ion e.g. Chlor______= ClO3− • -ate ion +1 ex O same charge, _____prefix • e.g. ______________= ClO4− • -ate ion –1 O same charge, _____suffix • e.g. Chlor______= ClO2− • -ate ion –2 O same charge, • e.g. _______________= ClO− • ______prefix, • ______ suffix

  9. Naming ionic compounds containing a polyatomic ion e.g. Na2SO4 • 1. Identify the ions Na = Na+ because in Group 1A SO4 = SO42− a polyatomic ion • 2. Name the cation Na+ = sodium, metal with invariant charge • Name the anion SO42− = • 4. Write cation name followed by name of anion

  10. Fe(NO3)3 • Identify ions • NO3= NO3− a polyatomic ion Fe = Fe3+ to balance charge of 3 NO3− ions • 2. Name cation Fe3+ = iron(III), metal with variable charge • Name anion NO3− = • 4. Write cation name followed by anion name

  11. Practice — What are the formulas for compounds made from the following ions? aluminum ion with a sulfate ion chromium(II) with hydrogen carbonate

  12. Four Common Reaction Types: 1) Combination Elem + elem one prod Elem + Cmpnd one prod Cmpnd + Cmpnd one prod

  13. Four Common Reaction Types: 1) Combination Elem + elem one prod metalelement + elementalO2 ionic metal oxide e.g. 4Al(s) + 3O2(g)  2Al2O3(s) lattice E (solid)

  14. Four Common Reaction Types: 1) Combination Elem + elem one prod Non-metalelement+ elem.O2 covalent oxide e.g. Combustion rxtn: S(s) + O2(g)  SO2(g) volatile product  gas

  15. Four Common Reaction Types: 1) Combination Compound + Compound  one product e.g. metal oxide + CO2 or SO3 What practical environmental applications for these 2 rxtns can you think of?

  16. Hydrates • ionic compounds containing a specific # of waters surrounding each formula unit • Water of hydration “driven off” by heating Cobalt (II) chloride _______________ CoCl2 Cobalt (II) chloride _______________ CoCl2. 6H2O

  17. Hydrates • In formula, attached H2O’s follow a ∙ • CoCl2∙6H2O

  18. Hydrates • attached waters indicated by prefix+hydrate after name of ionic compound • CoCl2∙6H2O = • CaSO4∙½H2O =

  19. Anhydrous salts are ____________________ = absorb ________even from atmosphere Used as __________________

  20. Practice What is the formula of magnesium sulfate heptahydrate? What is the name of NiCl2•6H2O?

  21. Solutions • Homogeneous mixtures = solutions • Part of solution that D’s state = the solute • Part that keeps its state = the solvent • if both parts in same state, major part is the solvent 22

  22. What Happens When a Solute Dissolves? When solute & solvent mix, there are attractive forces btwnsolute & solvent molecules If attractions btwnsolute and solvent are strong enough, the solute will dissolve 23

  23. Table Salt Dissolving in Water Each ion is attracted to surrounding water molecules & pulled off & away from crystal. ion is surrounded by water molecules, = ________________ Solvated ion lower in E than ions in crystal lattice

  24. Table Salt Dissolving in Water Result: soltn with free moving charged particles - can conduct electricity 25

  25. Dissociation and Ionization • Dissociation: ionic compounds dissolve in water, anions & cations are separated: Na2S(s) 2 Na+(aq) + S2-(aq) H2O(l) • Compounds w/ polyatomic iondissociating, polyatomic group stays together as one ion: Na2SO4(s) H2O(l) 26

  26. Non-electrolyte solutions: whole molecules dissolved in water Generally, molecular compounds do _____________when they dissolve • exception is 27

  27. Salt vs. Sugar Dissolved in Water ionic compounds dissociate into ions when they dissolve molecular compounds do not dissociate when they dissolve

  28. Acids and Bases • Acids: molecular compounds that ionize when dissolved in water • molecules ripped apart when attracted by water • acids ionize 29

  29. Acids and Bases in Solution • Acids ionize in water  H+ ions H from acid molecule _____________ion, (we use H+& H3O+interchangeably) 30

  30. Dissociation and Ionization • When strong acids dissolve in water, the molecule ionizes into H+ (actually H3O+) & anions H2SO4(aq) 31

  31. Acids and Bases • Bases: ionic compounds that dissociate when dissolved in water OH-anion +a metal cation KOH(s) + H2O (l)  32

  32. Common Reaction Types: 1) Combination Group I & II Metal oxides + H2O  a base(aq) Na2O(s) + H2O(l)  Na+(aq) + OH-(aq) water is both a reactant and solvent Other metal oxides are more inert

  33. Common Reaction Types: 1) Combination H with non-metal + H2O  an acid (aq) Water pops H+ off & leaves a solvated anion

  34. Only name as an acid • if molecule is dissolved in water -(aq) subscript • hydrochloric acid vs. hydrogen chloride gas

  35. Common Reaction Types: Note: not every compound with H atoms will donate them as an acid.

  36. Acids • Sour taste • Dissolve many metals • - e.g. Zn, Fe, Mg; • - but not Au, Ag, Pt • Formula generally starts with H • e.g. 37

  37. Reaction of Acids with Metals H2 gas 38

  38. Acids • Organic (carboxylic) acids: • -COOH functional group Organic? That’s totally “cooh” with me! 39

  39. Acids • Binary acids H+cationand non-metal anion • Oxyacids have H+cation & ________________ 40

  40. Naming Binary Acids Write a hydro prefix Follow with non-metal name Changeending on non-metal name to –ic Write acid at end of name 41

  41. Naming Binary Acids 42

  42. Example: HCl(aq) • Identify non-metal anion Cl = Cl−, chloride because Group 7A • 2. anion D to –icsuffix • Cl− = chloride  • 3. Add hydro- prefix to anion • 4. Add word acid to end: 43

  43. Naming Oxyacids • If polyatomic ion name ends in –ate, then change ending to ____suffix • If polyatomic ion name ends in –ite, then change ending to ______suffix • Write word acid at end of all names 44

  44. Naming Oxyacids 45

  45. Example: Naming oxyacids HNO3(aq) • 1. ID anion NO3= NO3−= nitrate • –ate suffix, D to –ic. • –ite suffix, D to -ous • NO3−= nitrate  • Write anion name followed by “acid” 46

  46. Example: Naming oxyacids HNO2(aq) • 1. ID anion NO3= NO3−= nitrite • –ate suffix, D to –ic. • –ite suffix, D to -ous • NO3−= nitrite  • Write anion name followed by “acid” 47

  47. Example: Naming oxyacids H2SO4(aq) • 1. ID anion SO4 = SO42− = sulfate • –ate suffix, D to –ic. • –ite suffix, D to -ous • SO42− = sulfate  • Write anion name followed by “acid” 48

  48. Example: Naming oxyacids H2SO3(aq) • ID the anion SO3 = SO32− = sulfite • –ate suffix, D to –ic. • –ite suffix, D to -ous • SO32− = sulfite  • Write anion name followed by “acid” 49

  49. Name the Following H2S HClO3 H3PO3 50

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