Classes of Chemical Reactions
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1 Classes of Chemical Reactions Reactions in aqueous media Precipitation reactions Acid-Base reactions Oxidation-Reduction reactions Reversible reactions Classes of Chemical Reactions Water (H 2 O), a unique solvent most abundant liquid medium for biochemical reactions solvent of high polarity O H H +
2 Classes of Chemical Reactions The solubility of ionic compounds: dissociation Na + Cl - Cl - Cl - NaCl Na + Na + O H H + Na + Cl - Classes of Chemical Reactions O H H +
3 Classes of Chemical Reactions electrolytes: a substance that conducts an electric current when dissolved in water Acids are donors of H + (this is a definition) or HBr! H 3 O + + Br HBr! H + + Br O H H + Equations for Aqueous Ionic Reactions molecular equation: 2AgNO 3 + Na 2 CrO 4! Ag 2 CrO 4 (s) + 2NaNO 3 total ionic equation: 2Ag + + 2NO 3 + 2Na + + CrO 42! Ag 2 CrO 4 (s) + 2Na + + 2NO 3 net ionic equation: 2Ag + + CrO 42! Ag 2 CrO 4 (s)
4 Classes of Chemical Reactions Precipitation Reactions Driving Force for Precipitation Reactions: INSOLUBILITY Some ions combine to form insoluble products 2Al CO 32! Al 2 (CO 3 ) 3 (s) No reaction in this case: KCl + NaBr: K + + Cl - + Na + + Br -! same ions no precipitate Classes of Chemical Reactions Precipitation Reactions Table 4.1. Solubility Principles SOLUBLE 1. all common compounds of Group 1A ions and NH 4 + are soluble 2. all common NO 3 -, CH 3 CO 2 -, and ClO 4 - are soluble 3. all halides, except Ag +, Pb 2+, Cu +, and Hg 2 2+ are soluble 4. all common SO 4 2- are soluble, except Ca 2+, Sr 2+, Ba 2+, and Pb 2+ INSOLUBLE 1. all common metal hydroxides are insoluble, except alkali and alkaline earth 2. all common CO 3 2- and PO 4 3- are insoluble, except alkali and NH all common sulfides (S 2- ) are insoluble, except alkali
5 Classes of Chemical Reactions Acid-Base Reactions Acid - a substance that is a donor of H + : HX! H + + X Base - a substance that is a donor of OH : MOH! M + + OH Classes of Chemical Reactions Acid-Base Reactions STRONG ACIDS Hydrochloric acid, HCl WEAK ACIDS Hydrofluoric acid, HF Hydrobromic acid, HBr Phosphoric acid, H 3 PO 4 Hydroiodic acid, HI Acetic acid, CH 3 CO 2 H Nitric acid, HNO 3 Carbonic acid, H 2 CO 3 Sulfuric acid, H 2 SO 4 Perchloric acid, HClO 4
6 Classes of Chemical Reactions Acid-Base Reactions STRONG BASES WEAK BASES Sodium Hydroxide, NaOH Ammonia, NH 3 Potassium Hydroxide, KOH Calcium Hydroxide, Ca(OH) 2 Strontium Hydroxide, Sr(OH) 2 Barium Hydroxide, Ba(OH) 2 Cesium Hydroxide, CsOH NH 3 + H 2 O! NH OH Classes of Chemical Reactions Acid-Base Reactions Driving Force for Acid-Base Reactions: FORMATION OF WATER Ba OH + 2H + + 2Cl! Ba Cl + 2H 2 O
7 Classes of Chemical Reactions Acid-Base Reactions Driving Force for Acid-Base Reactions: FORMATION OF WATER Ba OH + 2H + + 2Cl! Ba Cl + 2H 2 O Ba(OH) 2 + 2HCl! BaCl 2 + 2H 2 O Classes of Chemical Reactions Acid-Base Reactions Driving Force for Acid-Base Reactions: FORMATION OF WATER Ba OH + 2H + + 2Cl! Ba Cl + 2H 2 O Ba(OH) 2 + 2HCl! BaCl 2 + 2H 2 O OH + H +! H 2 O neutralization reaction
8 Classes of Chemical Reactions Acid-Base Reactions Acid-Base Titrations: one solution of known concentration is used to determine the concentration of another solution HCl + NaOH! NaCl + H 2 O Classes of Chemical Reactions Acid-Base Reactions Acid-Base Titrations: one solution of known concentration is used to determine the concentration of another solution HCl + NaOH! NaCl + H 2 O
9 Acid-Base Titrations Practice Problem ml of an HCl solution of unknown concentration required ml of M standard NaOH solution to reach the endpoint. What is the concentration of the HCl solution? Acid-Base Titrations Practice Problem ml of an HCl solution of unknown concentration required ml of M standard NaOH solution to reach the endpoint. What is the concentration of the HCl solution? HCl + NaOH! NaCl + H 2 O
10 Acid-Base Titrations Practice Problem ml of an HCl solution of unknown concentration required ml of M standard NaOH solution to reach the endpoint. What is the concentration of the HCl solution? HCl + NaOH! NaCl + H 2 O n(hcl) = n(naoh) = L " mol/l = mol Acid-Base Titrations Practice Problem ml of an HCl solution of unknown concentration required ml of M standard NaOH solution to reach the endpoint. What is the concentration of the HCl solution? HCl + NaOH! NaCl + H 2 O n(hcl) = n(naoh) = L " mol/l = mol mol L = mol/l
11 Oxidation-Reduction Red + Ox! Products e electrons reducing agent: loses electrons oxidizing agent: gains electrons Oxidation-Reduction Red + Ox! Products e electrons reducing agent: loses electrons oxidizing agent: gains electrons 2Mg + O 2! 2MgO Mg 2+ O 2
12 Oxidation-Reduction Red + Ox! Products e electrons reducing agent: loses electrons oxidizing agent: gains electrons 2Mg + O 2! 2MgO 4 electrons Mg 2+ O 2 Oxidation-Reduction Red + Ox! Products e electrons reducing agent: gets oxidized oxidizing agent: gets reduced 2Mg + O 2! 2MgO 4 electrons Mg 2+ O 2
13 Oxidation-Reduction + #+ Cl Cl H H H Cl #$ non-polar covalent bond: electrons distributed evenly polar covalent bond: electrons distributed unevenly OXIDATION STATE: A MODEL, compounds treated as if electrons were transferred completely, not actually shared Cl H Oxidation-Reduction redox reactions are characterized by change in oxidation state H 2 + Cl 2! 2HCl +1-1 Cl H
14 Oxidation-Reduction redox reactions are characterized by change in oxidation state H 2 + Cl 2! 2HCl reducing agent: loses electrons oxidizing agent: gains electrons +1-1 Cl H Oxidation Number (State): General For an atom in its elemental form equals 0 (H 2, N 2 ) For monoatomic ion equals the ion charge (Ag +, S 2- ) The sum of O.N. for the atoms in a compound is zero (HCl) The sum of O.N. for the atoms in a polyatomic ion equals the ion charge ClO +1-2
15 Oxidation Number (State): General Rules for assigning an oxidation number 1. For Group 1A +1 in all compounds 2. For Group 2A +2 in all compounds 3. For hydrogen +1 in combination with nonmetals -1 in combination with metal and B 4. For fluorine -1 in all compounds 5. For oxygen -2 in all compounds except F and peroxides 6. For Group 7A (halogens) -1 except with O and halogens lower in the group Oxidants and Reducing Agents AgNO 3 + NaCl! AgCl(s) + NaNO 3
16 Oxidants and Reducing Agents AgNO 3 + NaCl! AgCl(s) + NaNO Oxidants and Reducing Agents AgNO 3 + NaCl! AgCl(s) + NaNO 3 +5 NOT a redox reaction +5
17 Oxidants and Reducing Agents AgNO 3 + NaCl! AgCl(s) + NaNO 3 +5 NOT a redox reaction +5 2Al + 3H 2 SO 4! Al 2 (SO 4 ) 3 + 3H 2 Oxidants and Reducing Agents AgNO 3 + NaCl! AgCl(s) + NaNO 3 +5 NOT a redox reaction Al + 3H 2 SO 4! Al 2 (SO 4 ) 3 + 3H
18 Oxidants and Reducing Agents AgNO 3 + NaCl! AgCl(s) + NaNO 3 +5 NOT a redox reaction a redox reaction 2Al + 3H 2 SO 4! Al 2 (SO 4 ) 3 + 3H Balancing Redox Reactions
19 Balancing Redox Reactions Balancing Redox Reactions
20 Balancing Redox Reactions Balancing Redox Reactions
21 Balancing Redox Reactions Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent
22 Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent
23 Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent Step 3. Determine the number of electrons: (a) gained by the oxidant Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent Step 3. Determine the number of electrons: (a) gained by the oxidant (3)
24 Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent Step 3. Determine the number of electrons: (a) gained by the oxidant (3), and (b) lost by the reducing agent Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent Step 3. Determine the number of electrons: (a) gained by the oxidant (3), and (b) lost by the reducing agent (1)
25 Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent Step 3. Determine the number of electrons: (a) gained by the oxidant (3), and (b) lost by the reducing agent (1) Step 4. (the key step) Assign coefficients to match the number of electrons lost and gained. Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent Step 3. Determine the number of electrons: (a) gained by the oxidant (3), and (b) lost by the reducing agent (1) Step 4. (the key step) Assign coefficients to match the number of electrons lost and gained. K 2 Cr 2 O 7 + 6HI! KI + CrI 3 + 3I 2 + H 2 O
26 Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent Step 3. Determine the number of electrons: (a) gained by the oxidant (3), and (b) lost by the reducing agent (1) Step 4. (the key step) Assign coefficients to match the number of electrons lost and gained. Step 5. Complete balancing by inspection (by guessing) K 2 Cr 2 O 7 + 6HI! KI + CrI 3 + 3I 2 + H 2 O Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent Step 3. Determine the number of electrons: (a) gained by the oxidant (3), and (b) lost by the reducing agent (1) Step 4. (the key step) Assign coefficients to match the number of electrons lost and gained. Step 5. Complete balancing by inspection (by guessing) K 2 Cr 2 O 7 + 6HI! 2KI + 2CrI 3 + 3I 2 + 7H 2 O
27 Balancing Redox Reactions Step 2. Find and the oxidant and reducing agent Step 3. Determine the number of electrons: (a) gained by the oxidant (3), and (b) lost by the reducing agent (1) Step 4. (the key step) Assign coefficients to match the number of electrons lost and gained. Step 5. Complete balancing by inspection (by guessing) K 2 Cr 2 O HI! 2KI + 2CrI 3 + 3I 2 + 7H 2 O READ SECTION 4.6: The activity series of the metals
28 READ (!) SECTION 4.6: The activity series of the metals Reversible Reactions CaCO 3! CaO + CO 2 CaO + CO 2! CaCO 3 CaCO 3 CaO + CO 2 equilibrium system
29 Practice Problem (4.70) Identify the oxidizing agent and the reducing agent in each of the following: 8H + + 6Cl + Sn + 4NO 3! SnCl NO 2 + 4H 2 O Practice Problem (4.70) Identify the oxidizing agent and the reducing agent in each of the following: 8H + + 6Cl + Sn + 4NO 3! SnCl NO 2 + 4H 2 O 2MnO Cl + 16H +! 5Cl 2 + 2Mn H 2 O
30 Practice Problem (4.75) Use the oxidation number method to balance the following equations by placing coefficients. Identifiy the reducing and oxidizing agents: (b) I 2 + Na 2 S 2 O 3! Na 2 S 4 O 6 + NaI Practice Problem (4.83) Balance the following redox reaction and classify it as a combination, decomposition, or displacement reaction: (a) Ca + H 2 O! Ca(OH) 2 + H 2 (b) NaNO 3! NaNO 2 + O 2 (c) C 2 H 2 + H 2! C 2 H 6
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