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Midterm Review Sample Content Questions Metric Units Solve the following conversions by dimensional analysis. On the line to the left of the problem, identify the number of significant figures in the value provided. ______1. 1550 kg of water = __________ cm3 ______2. 4.570 x 10-8 Mg Au = ____________ mg ______3. 0.0008500 Mm = ___________ cm ______4. 6.7 x 104 μg = __________ g Solve the following and answer in correct significant figures and units. 5. 45 m3 ÷ 7.0 m = ___________ 6. 255 g ÷ 20.0 mL = _____________ 7. 800.0 m2 x 20 m = ____________ 8. 1.355 cm + 55.2 cm = _____________ Matter and Changes 9. Which of the following signs of a chemical reaction could potentially occur in a physical change too: color change, temperature change, gas evolution, formation of a precipitate, new substance forms. List any/all that apply and what conditions must occur for them to be considered physical by providing an example. 10. What is the significance of all physical and chemical changes and the law of conservation of matter? 11. What are properties – chemical vs. physical? Give a few examples of both chemical and physical properties. 12. What is meant by the following: “density is a constant”? 13. How does an increase in temperature affect the density of most substances? 14. The density of lead is 11.3 g/cm3. What is the volume in Liters of 4576 kg of lead? The Atom 15. Identify the number of electrons, neutrons, protons in the following: # electrons # neutrons # protons A. lead – 204 B. 178 O C. P3D. calcium ion E. arsenide ion 16. What is the subatomic particle that varies in an isotope? Which varies in an ion? 17. Which of the ions in problem 15 are anions? How would you recognize an anion? 18. What is the significance of Rutherford’s gold foil experimentation? 19. What is the significance of the Plum pudding model of the atom? 20. Bohr is known for the “planetary model” of the atom – what does this mean? 21. What is the most accepted theory of the atom used in chemistry today? Nuclear Chemistry 22. Identify the following reactions as alpha, beta, and/or gamma radiation. A. B. + 10n → 23992U + 59 0 26Fe → 27Co + -1e 238 92U 0 0 59 C. D. → 42He + 22286Rn 0 36 17Cl → -1e + 18Ar 226 36 88Ra 23. Balance the following nuclear reactions by supplying the missing atom or particle. A. 23993Np → ______ + 0-1e B. 232 C. 40 D. 90Th 20Ca → + 4 238 2He 92U + _________ → 70 30Zn + 410n + 2_____ 4_____ → 42He + 2 01e 24. What criteria are used to determine if an isotope is radioactive? 25. Identify how you know if a nucleus is radioactive? 26. What is the most penetrating radiation – alpha, beta, or gamma? Nomenclature 27. Provide the name for the following compounds. A. H2S (g) E. ZnCrO4 B. H2SO3 (aq) F. HNO3 (aq) C. K3PO4 G. Fe(OH)3 D. SnCO3 H. HClO4 I. HBr 28. Write the formula for the following compounds. A. ammonia E. cadmium oxalate B. chromium (III) cyanide F. lithium oxide C. acetic acid G. sulfur dioxide D. silver nitrite H. cobalt (II) chloride heptahydrate 29. How do you know if a substance is molecular “covalent” or ionic by its formula? 30. What are the seven diatomic nonmetal molecules? Quantum Mechanics and Periodicity 31. What is the electron configuration for copper? 32. What is the electron configuration for palladium? How many valence electrons does it contain? 33. What is the Aufbau diagram for phosphorus? How many lone electrons does phosphorus contain? 34. What electron configuration is expressed by the following quantum numbers? n=4 l= 2 m l = -1 ms = +1/2 35. Identify which of the following sets of quantum numbers cannot occur for an electron. Identify the error and why it is incorrect. If it is correct identify the proper configuration value, i.e. 3d2. a. n=3 l= 3 m l = -2 ms = +1/2 c. n=3 l= 2 m l = -1 ms = -1/2 b. n=2 l= 1 m l = -0 ms = -1/2 d. n=5 l= 3 m l = +3 ms = -1/2 36. How many electrons maximum can a d sublevel hold? 37. What is the ionic charge for Barium? What electrons will barium lose to become a cation? 38. What is ionization energy? For aluminum where would you notice a significant rise in ionization energy – from 1st IE to 2ndIE, 2nd IE to 3rdIE, 3rd IE to 4thIE? Explain how you know. 39. What is the trend for atomic radius across a period? Down a group? 40. Who is the most electronegative atom on the periodic table? What does electronegativity mean? Use the image shown to answer the corresponding question. Percent Error 42. Suppose a student measures the mass and volume of a sample of lead in the lab. The mass is recorded as 85.0 g and the volume is measured and calculated to be 7.10 cm3. The theoretical density of lead is 11.3 g/cm3. Calculate the percent error for this experiment. Light Energy 43. Calculate the energy in a light wave if the wavelength is 2.5 x 10-10 meters.