Chemistry Exam Review

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Lawrence Fox
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1 Chemistry Exam Review This exam review was compiled using the NC Essential Standards. You need to answer each question. You will receive multiple grades for your work. If you study everything on the exam review, you should have no problem with the final exam. If you turn in this copy unmarked as well as the exam strategies you will receive 5 extra points on your grade Standard 1.1: Analyze the structure of atoms and ions. (11-14% of MC) 1. Describe the location of protons, neutrons and electrons in the atom. Describe their charge and relative masses when compared with one another. 2. What does the atomic structure and mass number tell us about the atom? What are their symbols? 3. Draw the Bohr model for the Al atom. Fill in the number of protons, neutrons and electrons. It is an aluminum atom with a mass number of Define the following terms: a) atom b) molecule c) element d) compound e) mixture 5. Describe today's model of the atom (the quantum mechanical model). 6. Define: (a) quantum number (b) suborbital (c) spin 7. The atomic number of an element is 10. What is the electron configuration? 8. What is the electron configuration of krypton? 9. What is the electron configuration of sodium (use the noble gas configuration)? 10. What are the symbols for the following: a) carbon-12 b) hydrogen-1 c) alpha particle d) beta particle e) gamma radiation f) carbon What is an isotope? 12. What is carbon-14 dating and how is it done? 13. Explain the penetrating power of alpha, beta, and gamma decay. 14. Name 3 ways that radiation can be detected. 15. What are fission and fusion? Give common examples of how they are used or where they are found. 16. A sample initially contains 248 g of strontium-90, which has a half-life of 29 years. What is the amount of strontium-90 left after 52 years? 17. Nitrogen-13 emits beta radiation and decays to another element with a half-life of 10 min. How long is 3 half-lives? Write the equation for this decay reaction. How many grams of the isotope (nitrogen-13, t 1/2 = 10 min.) at the end of 3 half-lives? Complete the following reactions: Al + 4 He 30 Si +? Si 0 e +?

2 Chm 1.2 Understand the bonding that occurs in simple compounds in terms of bond type, strength and properties. (13-14% of MC) 20. Name CBr 4. What kind of molecule is this? Explain its shape. Why does it have this shape? 21. Name Al(NO 3 ) 3. What bond holds this together? 22. Name Cu 2 S. What type of bond is this? 23. Write the formula for aluminum hydrogen carbonate. 24. What is the name of the compound with the chemical formula CrCl 3? 25. Write the formula for lead (IV) chromate. 26. Write the formula for dinitrogen tetrahydride. What type of compound is this? 27. Write the formula for zinc hydrogen sulfate. 28. How does an S 2- ion differ from an electrically neutral sulfur atom? 29. If two oxygen atoms combine chemically, what kind of bond is formed between them? (be specific as possible). 30. What do the ions K +, Ca 2+, and Cl have in common? *Chm 1.3 Understand the physical and chemical properties of atoms based on their position in the periodic table (4-10% multiple choice; Constructed response 1-4%) 31. Describe the properties of metals. Where are they located on the periodic table? 32. Describe the properties of nonmetals. Where are they located on the periodic table? 33. What are the semi-metals/metalloids? Where are they located on the periodic table? 34. Explain why fluorine has a smaller atomic radius than both oxygen and chlorine. 35. In general, would you expect nonmetals to have large electron affinities than metals? Why or why not? 36. Which have larger ionic sizes, metals or nonmetals? Why? 37. What element has the largest electronegativity? 38. What is electronegativity? 39. What is ionization energy? 40. Why are the noble gases sometimes called inert gases? 41. What are the most active metals? What are the most active nonmetals? 42. Label the families of the elements on a periodic table which you sketch. 43. What are the trends of atomic size, ionic size, electronegativity, and ionization energy? Show the trends on a table you create. *Chm 2.1 Understand the relationship among pressure, temperature, volume and phase. (MC 14-19%; CR 0-2%)

3 Temperature 44. Label the following phase diagram. Label: a) specific heat of a solid b) specific heat of a liquid c) specific heat of a gas d) heat of solidification e) heat of vaporization f) heat of condensation g) melting point h) freezing point i) boiling point j) gas k) liquid l) solid Energy 45. What happens to the temperature when a substance melts? 46. Define: exothermic and endothermic 47. What is the kinetic molecular theory of gases? 48. Define: a) pressure b) volume c) temperature 49. What does Boyle's law state, what equation accompanies it, and what does a graph of P vs. V look like? 50. A gas with a volume of 4.0L at a pressure of 0.90 atm is allowed to expand until the pressure drops to 0.20 atm. What is the new volume? 51. What is Charles' law, what equation accompanies it, and what type of graph do you get with V vs. T? 52. Five liters of air at -50 degrees C are warmed to 100 degrees C. What is the new volume if the pressure remains constant? 53. What is Gay-Lussac's law, what equation accompanies it, and what does a graph of P vs. T look like? 54. What is Dalton's law of partial pressures? 55. A gas mixture containing oxygen, nitrogen and carbon dioxide has a pressure of 250 mmhg. If P O2 = 50 mmhg, and P N2 = 175 mmhg, what is the P CO2? 56. What is the formula for the ideal gas law? 57. Determine the volume occupied by mole of a gas at 15 degrees C if the pressure is 622 mmhg. 58. What is the formula for the combined gas law? 59. A 5.0 L air sample at a temperature of -50 degrees C has a pressure 800 mmhg. What will be the new pressure if the temperature is raised to 100 degrees C and the volume expands to 7.0 L. For the next two problems put all the temperatures in Kelvin and Celsius K degrees C

4 62. Phase diagrams You should be able to identify state of matter using unlabeled phase diagram. Identify the triple point and critical point. 63. Distinguish between an endothermic and exothermic reaction. 64. When 435 J of heat energy is added to 3.4 g of olive oil at 21 degrees C, the temperature increases to 85 degrees C. What is the specific heat of olive oil? *Chm 2.2 Analyze chemical reactions in terms of quantities, product formation and energy (MC 14-19% ; CR 0-2%) 65. Define: a) atomic mass b) gram-atomic mass c) molecular mass d) gram molecular mass 66. Calculate the % composition of C 3 H Calculate the mass of carbon in 82 g of C 2 H What is the empirical formula of a compound that is 71.71% Cl, 16.16% O, and 12.12% C? 69. Determine the empirical formula of a compound that is 25.9% nitrogen and 74.1% oxygen? Use the reaction below to determine the answers to the following three problems: 5C + 2 SO 2 CS CO 70. How many moles of CS 2 form when 6.30 mole of C reacts? 71. How many grams of carbon monoxide is formed when 20.0g of carbon is used? 72. How many grams of carbon disulfide is formed when 2.6 moles of SO 2 are used? 73. Calculate the volume of 9.6 moles of helium at STP. 74. Calculate the volume of 3.2 g of carbon dioxide gas at STP. 75. Calculate the mass of 18.0 L of CH 3 at STP. Using the following reaction, calculate the following two problems at STP. Remember to balance all reactions.

5 H 2 + O 2 H 2 O 76. If 2.0 L of hydrogen reacts with oxygen, what volume of oxygen must be used for a complete reaction? 77. What volume of water would be produced (using information from the previous problem)? Chm 3.1 Understand the factors affecting rate of reaction and chemical equilibrium. (MC 7-12%) 78. What are the factors that affect reaction rates (describe each and how they work)? 79. What is dynamic equilibrium? 80. What is LeChatlier's principle? 81. What happens to the reaction below when, A (g) + B (g) 3C (g) + energy a) the concentration of A is increased? b) The concentration of C is increased? c) The temperature is increased?5) d) The pressure is decreased? Write the Keq expression for each of the next three problems: (none are solids or pure liquids) 82. 2HBr H 2 + Br SO 3 2SO 2 + O PCl 5 PCl 3 + Cl 2 *Chm 3.2 Understand solutions and the solution process. (MC 12-17%; CR 0-3) 85. Write the formulas for the following acids, bases and salts. Identify them as acids, bases and salts. a) sodium chloride c) sulfuric acid e) ammonia g) sodium hydroxide b) acetic acid d) sodium bicarbonate f) potassium hydroxide 86. Define the terms acid and base according to the following theories: a) Arrhenius theory b) Bronsted-Lowry theory c) Lewis theory 87. Describe all the properties of acids and be sure to include how they affect indicators and ph. 88. Describe all the properties of bases and be sure to include how they affect indicators and ph. 89. Describe all the properties of salts and be sure to include how they affect indicators and ph.

6 90. Define: a) molarity b) dilutions c) acid/base titrations and ionization 91. What are the effects of concentration on the boiling point and freezing point of a solution? 92. Write the equation for the equilibrium of water. 93. Describe the ph scale and identify where acids and bases are located on the scale. 94. What are the factors that affect solubility? 95. A salt solution has a volume of 2.0L and contains 0.70 mol of NaCl. What is the molarity of the solution? 96. An aqueous solution has a volume 2.0L and contains 36.0 g of glucose. If the molar mass of glucose is 180g, what is the molarity of the solution? 97. You need 250mL of 0.20 M NaCl, but the only supply of sodium chloride you have is a solution of 1.0M NaCl. How do you prepare the required solution?

Chemistry Final Exam: Practice Problems

Chemistry Final Exam: Practice Problems 1. Key Vocabulary/Terms: atomic number element compound kinetic theory acid base salt vaporization condensation evaporation boiling sublimation energy level valence