1. Chemistry Tri B Final Review Final Review Chapter 8 Shape it Chapter 9 Reactionary Chapter 10 Stoich it Chapter 11 Stoich Master Chapter 12 Feel the heat Chapter 13 Passing Gas Work it 200 400 600 800 1000

2. Chapter 8 200 200 What are the shapes of CO 2 and H 2 O molecules? Are they polar or non- polar? –CO 2 linear, non polar –H 2 O bent, polar

3. Chapter 8 400 400 What are the shapes of BCl 3 and CH 4 Are they polar or non-polar? –BCl 3 trigonal planar, non-polar –CH 4 tetrahedral, non-polar

4. Chapter 8 600 600 What is the shape of NH 3 and SO 2 ? Are they polar or non-polar –NH 3 pyramidal, polar –SO 2 bent, polar

5. Chapter 8 800 800 What is an ionic bond? What is a non- polar covalent bond? A polar covalent bond? –Metal to nonmetal transfer of e- –Non-metal to non-metal with similar or same EN (equal sharing of electrons) –Non-metal to non-metal with different EN (unequal sharing of electrons)

6. Chapter 8 1000 1000 Write the formulas for magnesium fluoride, zinc oxide, oxygen, hydrogen fluoride. Indicate if they are ionic, polar or non-polar covalent. Write the polyatomic ions for hydroxide, nitrate, carbonate, sulfate and phosphate. –MgF 2 ionic –ZnO ionic –O 2 non-polar covalent –HF polar covalent –OH - NO 3 - CO 3 -2 SO 4 -2 PO 4 -3

7. Chapter 9 200 200 What is the formula for Iron III oxide? Lead II Sulfate? What is the name of Sn(CO 3 ) 2, Cr(OH) 3, KNO 3 –Fe 2 O 3 –PbSO 4 –Tin IV Carbonate –Chromium III hydroxide –Potassium nitrate

8. Chapter 9 400 400 Name the type of reaction HCl + Mg(OH) 2  MgCl 2 + H 2 O Hydrogen + oxygen produces water H 2 O 2  H 2 O + O 2 NaOH + Li  LiOH + Na –Double Replacement –Direct Combination (syn) –Decomposition –Single Replacement

9. Chapter 9 600 600 State the Law of Conservation of Matter. How does it apply to balancing a chemical equation –Matter is neither created or destroyed –Must have the same number and types of atoms on either side of the  sign.

10. Chapter 9 800 800 How are ionic formulas balanced? How are equations balanced? Name the molecular compound N 3 F 4, CO, P 2 O 5. –Subscripts –Coefficients –Trinitrogen tetrafluoride, carbon monoxide, diphosphorus pentaoxide

11. Chapter 9 1000 1000 What do you call a solid formed in a chemical reaction that separates from the solution? –A precipitate

12. Chapter 10 200 200 What is a formula mass? What is the formula mass of carbonate? What is the molar mass? What is the molar mass of carbon dioxide? –Sum of all the atoms in a formula –60.01amu –Same as formula mass but expressed as g/mol –44.01g/mol

13. Chapter 10 400 400 How many Be 2+ ions are in 2.0 mol of BeO? How many water molecules are there in 0.5 moles of water? –1.2 x 10 24 ions –3 x 10 23 molecules

14. Chapter 10 600 600 How many grams of water are in 3.000 moles of water? (the molar mass of water is 18.02g/mol) How many moles in 22.5g of water? –54.06g water –1.25mols water

15. Chapter 10 800 800 What is an empirical formula? If the empirical formula is CH 4 and the molar mass is 64.2g/mol what is the molecular formula? –Smallest whole number ratio (simplest terms) –C 4 H 16

16. Chapter 10 1000 1000 What is the branch of chemistry called that deals with mass relationships among reactants and products? What is an Activity Series used for? –Stoichiometry –Determine if a chemical reaction will occur

17. Chapter 11 200 200 Given the equation N 2 + 3H 2  2NH 3 what is the Molar Ratio of N 2 to NH 3 ? How many moles of hydrogen would be needed to make 6 moles of ammonia? –1:2 –9 moles

18. Chapter 11 400 400 Given the combustion reaction of CH 4 + 2O 2  CO 2 + 2H 2 O What is the molar ratio of oxygen to water? How many grams of methane would be needed to produce 2.000 moles of carbon dioxide? –2:2 or 1:1 –32.10 g methane

19. Chapter 11 600 600 Given the reaction 2FeBr 3 + 3Ca  3CaBr 2 + 2Fe Which would limit the reaction 80.g of FeBr 3 or 20.g of Ca? How many moles of Fe would be produced? – FeBr 3. –0.27 mol

20. Chapter 11 800 800 What is the formula for %yield? Given MgO + H 2 O  Mg(OH) 2 Which would limit the reaction 20.g of MgO or 20.g of H 2 O? What would the % yield be if 24.0g of Mg(OH) 2 were produced? –Actual(measured) / Expected(calculated) x 100 –MgO –83%

21. Chapter 11 1000 1000 What volume of oxygen at STP is required to burn 500.g of glucose? If 600.g of CO 2 are produced what is the % yield? C 6 H 12 O 6 + 6O 2  6CO 2 + 6H 2 O –373L –81.9%

22. Chapter 12 200 200 What is the amount of heat required to raise the temperature of one gram of a substance by 1°C called? What are the units for specific heat? –specific heat –J/g* o C

23. Chapter 12 400 400 What is the sign of an exothermic rxn? What happens to the temperature of the surroundings during an exothermic rxn? –negative –It increases

24. Chapter 12 600 600 Standard pressure is? How much heat is transferred when 9.22g of glucose reacts with excess oxygen C 6 H 12 O 6 + 6O 2  6CO 2 + 6H 2 O delta H= -2803kj –1atm –144kj

25. Chapter 12 800 800 Use Hess’s Law to calculate the delta H net of the equation 2S + 2O 2  2SO 2 Given the equations 2SO 2 + O 2  2SO 3. Delta H = -196kj 2S + 3O 2  2SO 3. Delta H = -790kj –-594kj

26. Chapter 12 1000 1000 What do you do to the sign of the delta H in calculating a net equation if you have doubled the coefficients? –Double it.

27. Chapter 13 200 200 What is the conversion factor between atm and mmHg? –1atm = 760mmHg

28. Chapter 13 400 400 Convert.75atm to mmHg? Convert 825mmHg to atm –570mmHg –1.09atm

29. Chapter 13 600 600 What is standard temperature? When do gases diffuse fastest, hot or cold temps? Which is more dense a liquid or a gas of the same substance? –0C or 273K –Hot. Higher temp higher KE faster movement! –liquid

30. Chapter 13 800 800 If you decrease the pressure on a container what will happen to the volume? Which gas will diffuse faster CO or CO 2 explain your answer. What will be the new pressure on a container that was 2L at 1atm if the volume was changed to 1L? –It increases –CO the gas molecules are smaller –2atm

31. Chapter 13 1000 1000 True or false. When gas particles collide they transfer energy to each other. Explain your answer –False. Collisions are perfectly elastic.

32. Work it 200 200 If the empirical formula is XY 4, which are possible molecular formulas? X 2 Y 4, X 3 Y 6, X 2 Y 8 or X 5 Y 10 –X2Y8–X2Y8

33. Chapter Work it 400 400 Write the balance equation for gaseous oxygen reacting with gaseous hydrogen to create liquid water? Convert 64g of O 2(g) to liters –O 2(g) + 2H 2(g)  2H 2 O (l). –45L

34. Chapter Work it 600 600 How much heat is transferred if 150.g of manganese (IV) oxide react given 2MnO 2  2MnO + O 2. H= +264Kj Is this reaction endo or exothermic? C  CaC 2 + CO  H = 464.8kJ –228kj absorbed –endo

35. Chapter Work it 800 800 What is the empirical formula for a compound containing 2.128g Cl and 1.203 g Ca? –CaCl 2.

36. Chapter Work it 1000 1000 What is the molecular formula for a substance containing 54.1% Ca, 43.2% O and 2.7% H? –Ca(OH) 2

37. Final Jeopardy Aluminum reacts spontaneously with bromine to produce AlBr 3. If 45.0 g of Al react with 45.0 g of Bromine, which is the limiting reactant? What is the percent yield if 31.0g of AlBr 3 are actually produced? –Bromine –61.9%