CHEMISTRY MIDTERM EXAM REVIEW: FALL SEMESTER MIDTERM WILL INCLUDE: 1. DISTRICT MIDTERM 50 MULTIPLE CHOICE QUESTIONS (50 POINTS) 2. DISTRICT CONSTRUCTED RESPONSES (2O POINTS) 3. TEACHER PORTION: 15 MULTIPLE CHOICE QUESTIONS (30 POINTS) Define the following: 1. Independent variable- Unit 1: INTRO TO CHEM 2. Dependent variable- Read the scenario below and answer the questions that follow: Bart thinks that if mice are exposed to microwaves, then they will live longer than normal. He takes 50 mice and microwaves them for 10 seconds. Another 50 mice are set aside and not put in the microwave. He found that the average life span of the microwaved mice was 16 months, the average life span of the second group was 22 months. 3. What is the independent variable in the situation above? 4. What is the dependent variable in the situation above? Unit 2: Math Skills Convert the following using dimensional analysis: King Henry Died By Drinking Chocolate Milk 5. 100 m = km 6. 23 g = kg 7. 12.3 ml = L Fill in the following equivalents: 8. 1 milliliter = cm 3 or L Convert to Scientific Notation: 9. 1999= 10. 1,360,000= Convert from Scientific Notation 11. 3.4 X 10 3 = 12. 2.415 X 10-3 = 1
Determine the number of significant digits in the following: 13. 1000.00 = 14. 0.0023 = 15. 0.000020 = 16. 213.12 = Calculate the following and put your answer in the correct number of significant digits. 17. 2.12 + 2.1 = 18. 2.013/0.01 = Define the following: 19. Accurate- 20. Precise- In the blanks provided: Put an A or Accurate, P for Precise, B for Both or N for None: 21. Jimmy knows the mass of a ring is 4.3 g. He measured it 3 times. Here is the data: 4.3, 4.3, 4.3 22. Jimmy knows the mass of a rock is 12.3 g. He measured it 3 times. Here is the data: 12.4, 12.5, 12.6 23. Jimmy knows the length of a piece of paper is 11.0 cm. He measured it 3 times. Here is the data: 2.5, 7.78, 12.5 DEFINE the following and GIVE EXAMPLES: 24. Element- UNIT 3: Matter 25. Compound 4 Examples 26. Mixture- 27. Heterogeneous mixture- 28. Homogeneous mixture- 29. Solution 30. Pure substance- 2
31. Impure substance: 4 examples: 32. Fill in the triangle with the classification of matter: (Homogeneous, Heterogeneous, Compound, Pure, Impure, Substance, Element) Can be separated physically: Can be separated chemically: 32. Physical change- 33. Physical change- 33. Chemical change- 34. Physical property- 35. Chemical Property- 36. Density- 37. Formula for density = 38. Fill in the table below: Mass Volume Density Identity of substance *use table of densities below Substance 1 25.00 g 16.31cm 3 Substance 2 346.5g 44.00cm 3 Substance 3 10.8 g 4.0 cm 3 Element Density Aluminum 2.7g/cm 3 Rubidium 1.532 g/cm 3 Iron 7.874g/cm 3 3
39. Is density intensive or extensive? 40. Explain your answer. UNIT 4: ATOMS Discuss the atomic theories for: 41. Dalton- 42. Thompson- 43. Rutherford- 44. Bohr- 45. Define Isotope- 46 How many protons, neutrons and electrons in Carbon-13? 45. What is the mass number of Carbon-13? 47. Draw the Bohr model for Carbon 12, Carbon -13, and Carbon -14. Which isotope is most common? Explain why. 48. Fill in the table below: Unit 5: Periodic Table & e-config Element Family # of valence e- predicted charge Lithium Gold Neon Chlorine Aluminum Beryllium 49. What is the trend for ionization in energy in a group and in a period? 4
50. Circle the element the pair that has the higher ionization energy. Lithium or Sodium Nitrogen or Carbon 51. What is the trend for atomic size in a group and in a period? 52. Circle the element in the pair that has the larger atomic radius. Lithium or Sodium Nitrogen or Carbon 53. Circle the element which has greater reactivity? Lithium or Sodium Oxygen or Sulfur 54. Circle which elements will have similar chemical properties? 55. Explain why you circled these elements: 56. Which groups are the representative elements? 57. Fill in the following on the periodic table below: A. Label the names of the families B. Put the trends (increase or decrease) in the blanks by the arrows C. Label the number of valence electrons for all the representative elements D. Label the predicted ionic charge for all the representative elements. E. Label the s, p, d, and f blocks. F. Any s sublevel can hold up to electrons. p can hold electrons. d can hold electrons. f can hold electrons. 1. - 2. 3. Metal Trend 1. 2. 3. Define the following: Non Metal Trend 5
58. Define Valence electron- 59. Electrons found on the outside orbitals used in forming bonds are known as: 60. What is the electron configuration for Neon? 61. Write the ground state electron configuration (abbreviated version) for Chlorine: 62. Fill in the orbitals using arrows for Oxygen. Use Hund, Pauli, and Aufbau rules: 1s 2s 2p 63. What is the maximum number of electrons in each sublevel? s p d f Unit 6: IONS & BONDING Draw a Lewis dot Structure to show the bonding of Carbon with 4 Hydrogens. Define the following: 64. Cation- 65. Anion- 66. Ionic bond- 67. Covalent bond- 68. Ionic (I) or Covalent (C)? a. NaCl b. CO c. LiBr d. SO 4 69. Circle the elements that would form a bond by sharing electrons : Lithium Gold Nitrogen Sulfur Potassium 70. Explain why you circled these items above: 71. What type of compound(s) requires prefixes when naming them? 72. What type of compound(s) has the following endings ide, -ate, or - ite? 73. When naming compound(s) when are roman numerals needed? 6
74. What type of compound(s) can end in ide? 75. Describe the difference between Li and Li +1 : 76. Describe the difference between S and S -2 : 77. Fill in the table below: Isotope Atomic # Mass # Proton # Neutron # Electron # Charge Carbon 6 7 5 78. Name the following: a. NaCl = c. Be(NO 3 ) 2 = e. CuCl= b. CO= d. SO 4 = f. AuCl 2 = 79. Write formulas for the following: a. Li +1 bonds with Br -1 e. Mg +2 bonds with Cl -1 b. Ca +2 bonds with PO 4-3 f. H +1 bonds with SO 4-2 c. Copper (I) Chloride g. Sodium Nitrate d. Carbon Dioxide h. Dinitrogen Trioxide Unit 7: Moles 80. List three different quantities that are equivalent to one mole. 81. Calculate the molar mass of Ba(ClO 3 ) 2. 82. Convert 45 moles of NaCl to grams. 7
83. If CO 2 has a molar mass of 44 g/mol, what is the number of moles in 12.2 grams of CO 2. 84. If there are 25.6 g Ba(PO 3 ) 2, how much would this be in moles. 85. How many atoms are in 23.0 g iron (III) chloride, FeCl 3? 86. Calculate the % Nitrogen in Ca(NO 3 ) 2. 87. Define empirical formula: 88. List the directions on how to calculate empirical formulas. 1. 2. 3. 89. What is the empirical formula for 69.4 g Carbon, 135.5 grams Hydrogen and 21.6 g Oxygen. 90. Define molecular formula: 91. What is the formula for calculating molecular? 92. What is the molecular formula of this compound (Question # 89 ) if it has a molecular mass of 74.0 g/mol 93. Law of conservation of mass states: 8