Review for End of Course Exam Honors Chemistry
Review for End of Course Exam Honors ChemistryDirections: Answer each question to the best of your ability. This covers all the material on your final exam. You should use a separate piece of paper where necessary. No notes are allowed on the test but you will have the periodic table.1. What is the pH of a system if [H+] = 1.0 x 10-7M?What is the pH of a system if [H+] = 1.0 x 10-8M?What is the pH of a system if [H+] = 1.0 x 10-10M?When the [H+] goes down, the pH goes _____.When the [H+] goes up, the pH goes _____.2. Name the seven strong acids. What do you call any other acid? What differentiates a strong acid?3. For the reactionN2O4 (g) 2 NO2 (g) Ho = 58.0 kjHow does the equilibrium shift whenN2O4 is addedN2O4 is removedHeat is addedA catalyst is addedHeat is removedIncreasing the volume?4. Sketch a reaction energy profile for the above reaction. Show the energy of the reactants, energy of the products, activation energy and Hrxn. What would look different if a catalyst were used for the reaction?5. What was Rutherford’s experiment? What three things did he discover about the structure of an atom?6. How many protons, electrons, and neutrons in73Li3919K6329Cu7. What is a likely isotope for 8a? What is the same for isotopes? What is different for isotopes?8. If the density of a substance is 4.80 g/cm3, what mass would a volume of 30.00 cm3 of the substance have? What is the best way to report this answer?9. What is required to protect a human from the following types of radiation?alphabetagamma10. How many grams of a 10.0g sample 18F will remain after 330 minutes if the half-life for fluorine-18 is 110 minutes?11. The half-life for strontium-90 is 28.8 years. How long will it take for a 8.0 mg sample to decay to 0.50 mg?12. Complete the following nuclear reactions.146C 147N + _______11854Xe o+1e + _______11854Xe + o-1e ______23994Pu _____ + 23592U13. Name the type of decay in each part of #12.14. Balance the following chemical equations.a) K3PO4 + AgNO3 Ag3PO4 + KNO3b) N2 + H2 NH3c) H2 + Br2 HBrd) C2H4 + O2 H2O + CO215. How many molecules are in one mole H2O? How many molecules are in one gram of H2O? How many grams in one mole of H2O?16. Complete the following reactions. Utilize the type of reaction to help.Zn + HCl AgNO3 + KBr Mg + O2 HI C3H8 + O2 17. What are the charges of the ions formed in 16c? When the ions come together to form a compound, what is required of the charges?18. What are the most common charges for groups 1, 2, and 13-18 on the periodic table?19. Sketch a rough outline of a periodic table. Locate the following.a) alkali metalsg) s-blockm) metalloid/semimetalsb) halogensh) d-blockc) alkaline earth metalsi) p-blockd) noble gasesj) f-blocke) transition metalsk) metalsf) inner transition metalsl) nonmetals20. Which is more reactive?S or Cl?Na or Rb?F or Br?Na or Mg?21. In period 3, which element is the smallest (atomic radius)? Which element is the largest? Why?22. Which elements are most easily ionized (smallest ionization energy)?23. In group 2, which element is the smallest (atomic radius)? Which element is the largest? Why?24. If a reaction is exothermic, what happens to its surroundings? If a reaction is endothermic, what happens to its surroundings?25. How much heat is required to vaporize 25.0 g of liquid water at 100.0oC?26. How much heat is released when 25.0g of water freezes at 0.0oC?27. A piece of aluminum (specific heat = 0.902 j/goC) is heated to 87.5oC. It is then placed in a Styrofoam cup with 150.0g of water at 20.00oC. The final temperature of the aluminum and the water is 25.3oC. The specific heat of water is 4.184j/goC. What is the mass of the piece of aluminum? Why does calorimetry work?28. 3 BaCl2 (aq) + 2 (NH4)3PO4 (aq) 6 NH4Cl (aq) + Ba3(PO4)2 (s) How many grams of barium phosphate will precipitate when 34.0 grams of barium chloride react with ammonium phosphate?What is the percent yield if only 25.4 g actually precipitate?How many moles of ammonium chloride are in the resulting solution when 25.0g of ammonium phosphate react with barium chloride?How many moles of barium chloride react when 25.0 mL of a 2.0 M solution of barium chloride are used in the reaction?How much ammonium phosphate should you dissolve in water in order to have 0.534 moles in the reaction?29. How many molecules of SO3 are in 35.0 L of the gas at STP?30. Define reaction rate.31. What are four ways to increase the rate of an endothermic reaction?32. What is the molarity of a solution of copper (II) nitrate when 50.0g of copper (II) nitrate are dissolved in 250.0mL?33. What is the volume of a 0.450 mole sample of SO2 gas at 35.0oC and 1.33 atm?34. What is ionic bonding? What kinds of elements would make compounds that involve ionic bonding? Which electrons are involved? What happens to the metals? What happens to the nonmetals?35. What is a covalent bond? What kinds of elements make compounds that contain covalent bonds? 36. Write Lewis dot structures fora) NH3g) H2NNH2b) H2Oh) PCl3c) CO2i) PCl5d) N2j) SF4e) H3CCH3k) SF6f) HCCH37. How many domains and what is the molecular structure fora) H2Oe) which of these molecules are polar? Show the (+) end and the (-) end.b) PCl3c) SF4d) SF638. What are the angles and what does each structure look like? lineartrigonal planartrigonal pyramidaltetrahedral39. What can make the angles in a molecular structure slightly different from the usual value?40. What are the three types of intermolecular forces?What kinds of molecules have each of the intermolecular forces?What makes each force larger? (bond polarity, molar mass--#electrons?)Which is strongest? What is required for this intermolecular force?When intermolecular forces are strong, how are physical characteristics of the molecules different? Compare the boiling points of H2O and H2S. Explain the difference.41. What is the complete electron configuration for?a) Nad) Cl-1b) K+1e) Pc) Fef) Ar42. What determines the average kinetic energy of a gas?43. a) If the temperature of a gas increases and the volume is constant, what happens to the pressure?b) If the pressure of a gas increases and the temperature is constant, what happens to the volume?c) If the number of gas molecules increases and the temperature and volume are constant, what happens to the pressure?44. Draw two balloons of the same size. Label them 1.0 L each. One balloon contains 1.0 mole of H2 and the second balloon contains 1.0 mole of O2. The balloons have the same temperature of 298 pare the pressure in each pare the mass in each balloon.45. What are the seven diatomic molecules on the periodic table? What does it mean to be diatomic? ................
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