1. Chemistry 122 Review Chapter 9

2. Organic Chemistry - Vocabulary Organic, cracking, hydrocarbon, refining, reforming, saturated, hydrogenation, aromatic, phenyl, functional group Organic, cracking, hydrocarbon, refining, reforming, saturated, hydrogenation, aromatic, phenyl, functional group

3. Organic Chemistry - Structures Alkanes: single bonded carbons. General formula C n H 2n+2 Alkanes: single bonded carbons. General formula C n H 2n+2 If branches: (# of location) - (branch name) (parent chain) If branches: (# of location) - (branch name) (parent chain) Parent chain is always longest chain Parent chain is always longest chain Cycloalkanes: Single C-C bonds that form ring. Formula of C n H 2n Cycloalkanes: Single C-C bonds that form ring. Formula of C n H 2n

4. Organic Chemistry - Structures Alkenes - hydrocarbons with one or more double carbon-carbon bonds (C=C). General form: C n H 2n Alkenes - hydrocarbons with one or more double carbon-carbon bonds (C=C). General form: C n H 2n Alkynes - hydrocarbons with one or more triple carbon-carbon bonds (C=C). General form: C n H 2n-2 Alkynes - hydrocarbons with one or more triple carbon-carbon bonds (C=C). General form: C n H 2n-2 Benzene - Formula C 6 H 6 Benzene - Formula C 6 H 6

5. Organic Chemistry - Structures Organic Halides - organic compounds that contain one or more halogen atoms Organic Halides - organic compounds that contain one or more halogen atoms Aldehydes and Ketones - Both contain the carbonyl functional group (C=O) Aldehydes and Ketones - Both contain the carbonyl functional group (C=O) In aldehydes the carbonyl group is on the end of the chain, in ketones it is not at the end of the chain. In aldehydes the carbonyl group is on the end of the chain, in ketones it is not at the end of the chain.

6. Organic Chemistry - Structures Carboxylic acids - Contain both carbonyl (C=O) and hydroxyl (OH) groups Carboxylic acids - Contain both carbonyl (C=O) and hydroxyl (OH) groups O O || || Esters - Contain -C-O-R Esters - Contain -C-O-R Amide - has a carbonyl group bonded to a nitrogen Amide - has a carbonyl group bonded to a nitrogen Amine - has a nitrogen bonded to one or more carbons Amine - has a nitrogen bonded to one or more carbons

7. Examples to Try…. 3-ethyl-2,4-dimethylhexane 3-ethyl-2,4-dimethylhexane cyclopentane cyclopentane CH 2 =CH-CH 2 -CH 3 CH 2 =CH-CH 2 -CH 3 1,2-dimethylbenzene 1,2-dimethylbenzene CH 3 -CH-CH 2 -CH 2 -CH 3 CH 3 -CH-CH 2 -CH 2 -CH 3

8. Examples to Try…. C 2 H 5 Br C 2 H 5 Br CH 3 -CH 2 -OH CH 3 -CH 2 -OH 1,2-ethanediol 1,2-ethanediol

9. Chemistry 122 Review Chapter 10

10. Vocabulary Chemical system, energy, exothermic, endothermic, specific heat capacity, volumetric heat capacity, phase change, enthalpy, fusion, vaporizing, condensation, molar enthalpy, heating curve Chemical system, energy, exothermic, endothermic, specific heat capacity, volumetric heat capacity, phase change, enthalpy, fusion, vaporizing, condensation, molar enthalpy, heating curve

11. Main Formulas The heat change in a chemical system may be quantified using either of the following equations: The heat change in a chemical system may be quantified using either of the following equations: q = m c s  t or q = v c v  t q = m c s  t or q = v c v  tWhere: q = quantity of heat flowing to or from the system (J or kJ) m = mass of the substance (g) v = volume of the substance (L) c s = specific heat capacity (J / g o C ) c v = volumetric heat capacity (KJ / L o C)  t = t final – t initial = change in temperature ( o C)

12. Main Formulas Enthalpy change can be calculated using the following: Enthalpy change can be calculated using the following:Equation:  H = n H or  H = m H  H = n H or  H = m H MWhere:  H = enthalpy (energy) change for the phase change (KJ) n = moles of the substance undergoing the phase change (mol) H = molar enthalpy for the substance undergoing the phase change (KJ / mol) from Table 10.3 p.347. m = mass of the substance undergoing the phase change (g) M = molar mass of the substance undergoing the phase change (g / mol)

13. Main Formulas Calculating total energy: Calculating total energy:  E tot = sum of the parts of the heating curve = a + b + c + d + e = q ice +  H fus + q water +  H vap + qsteam

14. Main Formulas  H system = - q calorimeter  H system = - q calorimeter

15. Problems to Try…. When 150. L of water (in a hot water heater) at 10.0 o C is heated to 65.0 o C, how much energy is required? When 150. L of water (in a hot water heater) at 10.0 o C is heated to 65.0 o C, how much energy is required? If 500.0 g of freon-12, CCl 2 F 2, was turned from a liquid to a gas at SATP, what is the expected enthalpy change,  H? If 500.0 g of freon-12, CCl 2 F 2, was turned from a liquid to a gas at SATP, what is the expected enthalpy change,  H? Calculate the total energy released when 1.0 kg of molten iron, Fe (l), at 1700 o C, cools to solid iron, Fe (s), at 80 o C. The specific heat capacity of liquid iron is 0.20 J/g o C and that of solid iron is 0.11 J/g o C. The molar enthalpy of solidification of iron is -15 KJ/mol at 1535 o C. Calculate the total energy released when 1.0 kg of molten iron, Fe (l), at 1700 o C, cools to solid iron, Fe (s), at 80 o C. The specific heat capacity of liquid iron is 0.20 J/g o C and that of solid iron is 0.11 J/g o C. The molar enthalpy of solidification of iron is -15 KJ/mol at 1535 o C.

16. Problems to Try…. In a calorimetry experiment, 4.24 g of lithium chloride is dissolved in 100 mL of water at an initial temperature of 16.3 o C. The final temperature of the solution is 25.1 o C. Calculate the molar enthalpy of solution for lithium chloride In a calorimetry experiment, 4.24 g of lithium chloride is dissolved in 100 mL of water at an initial temperature of 16.3 o C. The final temperature of the solution is 25.1 o C. Calculate the molar enthalpy of solution for lithium chloride

17. Chemistry 122 Review Chapter 14

18. Vocabulary: equilibrium, Le Chatelier’s Principle Vocabulary: equilibrium, Le Chatelier’s Principle Types of changes: Types of changes: –concentration –temperature –pressure/volume (gases only)

19. Concentration changes addition of reactant  shifts equilibrium to the RIGHT addition of reactant  shifts equilibrium to the RIGHT removal of product  shifts equilibrium to the RIGHT removal of product  shifts equilibrium to the RIGHT addition of product  shifts equilibrium to the LEFT addition of product  shifts equilibrium to the LEFT removal of reactant  shifts equilibrium to the LEFT removal of reactant  shifts equilibrium to the LEFT Example : CaCO 3 (s)CaO (s) + CO 2 (g) + heat Example : CaCO 3 (s)CaO (s) + CO 2 (g) + heat What will happen to the equilibrium reaction above if: What will happen to the equilibrium reaction above if: –the concentration of CaCO 3 increases? SHIFT RIGHT to decrease concentration of CaCO 3 SHIFT RIGHT to decrease concentration of CaCO 3 –the concentration of CaCO 3 decreases? SHIFT LEFT to increase concentration of CaCO 3 SHIFT LEFT to increase concentration of CaCO 3 –the concentration of CaO (or CO 2 ) increases? SHIFT LEFT to decrease concentration of CaO (or CO 2 ) SHIFT LEFT to decrease concentration of CaO (or CO 2 ) –the concentration of CaO (or CO 2 ) decreases? SHIFT RIGHT to increase concentration of CaO (or CO 2 ) SHIFT RIGHT to increase concentration of CaO (or CO 2 )

20. Temperature changes Heat energy is treated as though it were a reactant or product Heat energy is treated as though it were a reactant or product Heat is added by heating and removed by cooling the container Heat is added by heating and removed by cooling the container reactants + energy products ENDOTHERMIC reactants + energy products ENDOTHERMIC reactantsproducts + energy EXOTHERMIC reactantsproducts + energy EXOTHERMIC Example : Example : 2 NaCl (s) + H 2 SO 4 (l) + energy 2 HCl (g) + Na 2 SO 4(s) 2 NaCl (s) + H 2 SO 4 (l) + energy 2 HCl (g) + Na 2 SO 4(s) What will happen to the equilibrium reaction above if: What will happen to the equilibrium reaction above if: –the reaction vessel is heated? SHIFT RIGHT to decrease energy on reactants side SHIFT RIGHT to decrease energy on reactants side –the reaction vessel is cooled? SHIFT LEFT to increase energy on reactants side SHIFT LEFT to increase energy on reactants side

21. Pressure/volume changes only affects systems involving gases only affects systems involving gases consider: the total amount in moles of gas reactants and the total amount in moles of gas products consider: the total amount in moles of gas reactants and the total amount in moles of gas products if # moles of gas reactants = # moles of gas products : if # moles of gas reactants = # moles of gas products : –no affect on equilibrium if # moles of gas reactants  # moles of gas products: if # moles of gas reactants  # moles of gas products: –an increase in pressure (decrease in volume) will shift equilibrium to the side with fewer moles of gas –a decrease in pressure (increase in volume) will shift equilibrium to side with more moles of gas

22. Pressure/volume changes Example: Example: 2 SO 2 (g) + O 2 (g) 2 SO 3 (g) + energy 2 SO 2 (g) + O 2 (g) 2 SO 3 (g) + energy # moles of gas reactants # moles of gas products # moles of gas reactants # moles of gas products = 3 = 2 = 3 = 2 What will happen to the equilibrium reaction above if: What will happen to the equilibrium reaction above if: –the pressure inside the reaction vessel increases? SHIFT RIGHT to side with less moles of gas (products) SHIFT RIGHT to side with less moles of gas (products) –The pressure inside the reaction vessel decreases? SHIFT LEFT to side with more moles of gas (reactants) SHIFT LEFT to side with more moles of gas (reactants)

23. Example Given: Given: N 2 (g) + 3 H 2 (g) 2 NH 3 (g) + heat N 2 (g) + 3 H 2 (g) 2 NH 3 (g) + heat How will this equilibrium respond to the following changes? How will this equilibrium respond to the following changes? (a) A decrease in temperature? (a) A decrease in temperature? (b) A decrease in pressure? (b) A decrease in pressure? (c) An increase in nitrogen? (c) An increase in nitrogen? (d) A decrease in ammonia? (d) A decrease in ammonia? Answers: (a) RIGHT (b) LEFT (c) RIGHT (d) RIGHT

24. Chemistry 122 Review Chapter 7

25. Vocabulary Limiting reagent, excess reagent, gravimetric, solute, solvent Limiting reagent, excess reagent, gravimetric, solute, solvent

26. Steps to Stoichiometry Step 1: write a balanced chemical equation and list the measurement and conversion factors for the given and required substances Step 1: write a balanced chemical equation and list the measurement and conversion factors for the given and required substances Step 2: convert the given measurement to an amount in moles by using the appropriate conversion factor. Step 2: convert the given measurement to an amount in moles by using the appropriate conversion factor. Step 3: Calculate the amount of the required substance by using the mole ratio from the balanced equation Step 3: Calculate the amount of the required substance by using the mole ratio from the balanced equation Step 4: Convert the calculated amount to the final required quantity by using the appropriate conversion factor or the ideal gas law. Step 4: Convert the calculated amount to the final required quantity by using the appropriate conversion factor or the ideal gas law.

27. Try This….. If 300g of propane burns in a gas barbecue, what volume of oxygen at SATP is required for the reaction? If 300g of propane burns in a gas barbecue, what volume of oxygen at SATP is required for the reaction? Calculate the mass of lead (II) chloride precipitate produced when 2.57g of sodium chloride in solution reacts in a double replacement reaction with excess aqueous lead (II) nitrate. Calculate the mass of lead (II) chloride precipitate produced when 2.57g of sodium chloride in solution reacts in a double replacement reaction with excess aqueous lead (II) nitrate.

28. Exam Format Matching (definitions and structures) – 12 marks Matching (definitions and structures) – 12 marks Definitions – 10 marks Definitions – 10 marks Organic naming and drawing structures – 30 marks Organic naming and drawing structures – 30 marks Calculations – 40 marks Calculations – 40 marks Short answer – 8 marks Short answer – 8 marks Total: 100 marks Total: 100 marks