* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Practice Test_final_161_F2015
Survey
Document related concepts
State of matter wikipedia , lookup
Equilibrium chemistry wikipedia , lookup
Rate equation wikipedia , lookup
Host–guest chemistry wikipedia , lookup
Electron configuration wikipedia , lookup
Coupled cluster wikipedia , lookup
Electrochemistry wikipedia , lookup
Heat transfer physics wikipedia , lookup
Marcus theory wikipedia , lookup
George S. Hammond wikipedia , lookup
Equation of state wikipedia , lookup
Transition state theory wikipedia , lookup
Transcript
CHEM161 FINAL EXAM (PRACTICE) ____ 1. A 19.0-g sample of lithium is completely burned in air to form lithium oxide. The mass of lithium oxide must be A) less than 19.0 g. B) greater than 19.0 g. C) equal to 19.0 g. D) all of the above. E) none of the above. ____ 2. A sample that cannot be separated into two or more substances by physical means is A) a heterogeneous mixture. B) a compound. C) either a compound or an element. D) an element. E) a homogeneous mixture. ____ 3. Which of the following is an example of a chemical change? A) silver tarnishing B) iodine sublimating C) alcohol boiling D) sucrose dissolving E) sodium chloride melting ____ 4. Two students determined the volume of a glass container three separate times (see table below). The true volume of the container is 24.20 mL. Which statement correctly describes the students’ results? Student A 24.3 mL 24.4 mL 24.5 mL Student B 24.89 mL 24.87 mL 24.88 mL A) Student A’s results are the most accurate. Student B’s results are the most precise. B) Student A’s results are the most accurate and precise. C) Student B’s results are the most accurate and precise. D) Student A’s results are the most precise. Student B’s results are the most accurate. E) The precision and accuracy of the two data sets are identical. ____ 5. Express the result of the following calculation in scientific notation: 0.0263 cm2 ÷ 88.2 cm A) B) C) D) E) ____ 6. What is the best answer to the following expression involving a sum of measurements? (85.430 cm + 0.400 cm + 31.3 cm) A) B) C) D) E) 117 cm 117.1300 cm 117.13 cm 117.130 cm 117.1 cm ____ 7. The melting point of nitrogen is 63 K. What is this temperature in degrees Celsius? A) 63°C B) –336°C C) –63°C D) –210.°C E) 483°C ____ 8. A particular sheet of paper measures paper in cm2? (2.54 cm = 1 in exactly) A) 1.1 102 cm2 B) 4.4 101 cm2 C) 2.8 102 cm2 D) 1.7 101 cm2 E) 6.8 cm2 ____ 9. A 4.06 cm3 sample of solid sodium metal has a density of 0.968 g/cm3. What volume does this sample of sodium occupy in its liquid state? The density of liquid sodium is 0.927 g/cm3. A) 4.24 cm3 B) 3.89 cm3 C) 4.52 cm3 D) 3.64 cm3 E) 0.257 cm3 ____ inches. What is the surface area of one side of the 10. The average speed of oxygen molecules at 690°C is 1.60 105 cm/s. Which of the following calculations would convert this speed to units of miles per hour? A) B) C) D) E) ____ 11. Which one of the following lists gives the correct symbols for the elements phosphorus, potassium, silver, chlorine, and sulfur? A) P, Po, Ag, Cl, S B) K, Ag, Po, Cl, S C) P, K, Ag, Cl, S D) Ph, K, Ag, S, Cl E) Ph, Po, Ag, Cl, S ____ 12. Which of the following conclusions regarding Rutherford’s gold foil experiment is not consistent with the observations? A) The nucleus occupies only a small portion of the space of an atom. B) Most alpha particles travel straight through the gold foil. C) The nucleus occupies a large amount of the atom space. D) The nucleus, like the alpha particles used to bombard the gold foil, is positively charged. E) Wide angle deflections result from a collision of an alpha particle and a gold atom nucleus. ____ 13. Which nuclide has the same number of protons as A) ? B) C) D) E) ____ 14. Which of the following statements about different elements is incorrect? A) Potassium is an alkali metal. B) Fluorine is a halogen. C) Aluminum is a transition element. D) Barium is an alkaline earth metal. E) Helium is a noble gas. ____ 15. What is the formula of magnesium nitrite? A) Mg(NO2)2 B) Mg3N2 C) Mg2(NO2)2 D) Mg2N3 E) Mg(NO2)3 ____ 16. Which is a correct balanced chemical equation corresponding to the following description of a chemical reaction? Hydrochloric acid reacts with magnesium metal to produce aqueous magnesium chloride and hydrogen gas. A) 2HCl(aq) + Mg(s) MgCl2(aq) + 2H(g) B) 2HCl(aq) + Mg(s) MgCl2(aq) + H2(g) C) 2HCl(aq) + Mg(s) MgCl(aq) + H2(g) D) 2HCl(aq) + Mg(aq) MgCl2(s) + H2(g) E) HCl(aq) + Mg(s) MgCl(aq) + H(g) ____ 17. Which of the following chemical equations is not balanced? A) NH4NO3 N2O + 2H2O B) C12H22O11 12C + 11H2O C) 2NH4SCN + Ba(OH)2 • 8H2O 2NH3 + 10H2O + Ba(SCN)2 D) (NH4)2Cr2O7 N2O + Cr2O3 + 4H2O E) 2Mg + CO2 2MgO + C ____ 18. The formula mass of zinc acetate trihydrate, Zn(CH3COO)2 • 3H2O, is A) 321 amu. B) 184 amu. C) 268 amu. D) 238 amu. E) 114 amu. ____ 19. How many molecules are there in 192 g of citric acid, C6H8O7? A) (6.02 1023) / 192 B) 192 C) 6.02 1023 D) 96.0 E) 192 (6.02 1023) ____ 20. What is the percent by mass oxygen in (NH4)2SO3? A) 41.3 % B) 20.7 % C) 54.0 % D) 42.0 % E) 1.00 % ____ 21. A compound composed of only C and F contains 17.39 % C by mass. What is its empirical formula? A) CF3 B) CF C) C2F D) CF4 E) CF2 ____ 22. The empirical formula of styrene is CH. An experimental determination of the molar mass of styrene by a student yields the value of 104 g/mol. What is the molecular formula of styrene? A) C5H10 B) CH C) C8H8 D) C3H8 E) C6H9 ____ 23. Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows: Cu2S(s) + O2(g) 2Cu(s) + SO2(g) If 0.680 kg of copper(I) sulfide reacts with excess oxygen, what mass of copper metal may be produced? A) 0.680 kg B) 0.136 kg C) 0.271 kg D) 0.543 kg E) 1.36 kg ____ 24. Which of the following solutions would be expected to be the best conductor of an electric current at room temperature? A) 0.10 M Na2SO4 B) 1.0 M CH3COOH C) 0.10 M NaCl D) 0.10 M CO(NH2)2 E) 0.10 M CH3COOH ____ 25. Identify the spectator ion(s) in the following reaction. Cu(OH)2(s) + 2H+(aq) + 2Cl–(aq) Cu2+(aq) + 2Cl–(aq) + 2H2O(l) A) B) C) D) E) Cu2+ and Cl– Cu2+ Cu(OH)2 Cl– H+ and Cl– ____ 26. Which of the following is a weak electrolyte in aqueous solution? A) Mg(OH)2 B) NH3 C) LiOH D) RbOH E) Sr(OH)2 ____ 27. All the following are oxidation–reduction reactions except A) H2(g) + F2(g) 2HF(g). B) Ca(s) + H2(g) CaH2(s). C) 2K(s) + 2H2O(l) 2KOH(aq) + H2(g). D) 6Li(s) + N2(g) 2Li3N(s). E) Mg3N2(s) + 6H2O(l) 3Mg(OH)2(s) + 2NH3(g). ____ 28. What is the oxidation number of each O in BaFeO4? A) +6 B) +2 C) -2 D) +3 E) 0 ____ 29. A 29.0-g sample of NaOH is dissolved in water, and the solution is diluted to give a final volume of 1.60 L. The molarity of the final solution is A) 18.1 M. B) 0.453 M. C) 0.725 M. D) 0.0552 M. E) 0.862 M. ____ 30. What mass of oxalic acid dihydrate, H2C2O4 · 2H2O, is required to prepare 250.0 mL of a 1.32 M solution of oxalic acid? A) 126 g B) 41.6 g C) 119 g D) 166 g E) 29.7 g ____ 31. What is the final concentration of HCl in a solution prepared by addition of 930.0 mL of 8.77 M HCl to 468.0 mL of 3.22 M HCl? Assume volumes are additive. A) 6.00 M B) 0.00858 M C) 12.0 M D) 6.91 M E) 5.08 M ____ 32. In a volumetric analysis experiment, an acidic aqueous solution of methanol (CH3OH) is titrated with a solution of potassium dichromate (K2Cr2O7) according to the following balanced chemical equation: 2K2Cr2O7(aq) + 8H2SO4(aq) + 3CH3OH(aq) 2Cr2(SO4)3(aq) + 11H2O(l) + 3HCOOH(aq) + 2K2SO4(aq) It required 43.91 mL of 0.0435 M K2Cr2O7 to reach the endpoint. What mass of CH3OH was present initially? A) 0.0918 g B) 2.09 g C) 0.929 g D) 0.0612 g E) 0.0408 g ____ 33. A flexible vessel contains 32.00 L of gas at a pressure of 1.59 atm. Under conditions of constant temperature and moles of gas, what is the volume of the gas when the pressure of the vessel is decreased by a factor of three? A) 96.1 L B) 10.7 L C) 0.0104 L D) 32 L E) 4.80 L ____ 34. How many moles of gas are in a gas sample occupying 0.738 L at 135 mmHg and 30°C? A) B) C) D) E) 190 mol 4.01 mol 40.5 mol 0.00527 mol 0.000433 mol ____ 35. The density of a gas is 1.96 g/L at STP. What is its molar mass? A) 65.2 g/mol B) 58.9 g/mol C) 11.4 g/mol D) 22.4 g/mol E) 43.9 g/mol ____ 36. What is the total volume of gases produced at 819 K and 1.00 atm pressure when 320 g of ammonium nitrite undergoes the following decomposition reaction? NH4NO2(s) N2(g) + 2H2O(g) A) B) C) D) E) 3 22.4 L 22.4 L 15 22.4 L 5 22.4 L 45 22.4 L ____ 37. Which of the following is included as a postulate in the kinetic molecular theory of an ideal gas? A) Collisions between molecules are all elastic. B) All molecules move randomly in zigzag directions. C) The distance between gas molecules is small compared with the size of the molecule. D) All the molecules have the same velocity. E) In an average collision between molecules, both molecules have the same kinetic energy. ____ 38. Which of the following gases will have the slowest rate of effusion at constant temperature? A) H2 B) F2 C) Ne D) SO3 E) CF4 ____ 39. Real gases deviate from ideal behavior for two reasons: (1) real gas molecules have intermolecular forces, and (2) real gas molecules have A) pressures within the chemical bonds. B) nonzero molecular volumes. C) ionization energies. D) molecular vibrations. E) a distribution of molecular speeds. ____ 40. Given the thermochemical equation 2Al(s) + O2(g) Al2O3(s); H = –1676 kJ find H for the following reaction. 2Al2O3(s) 4Al(s) + 3O2(g) A) B) C) D) E) ____ 838 kJ 1676 kJ –1676 kJ 3352 kJ –838 kJ 41. What mass of hydrogen is consumed when 587.9 kJ of energy is evolved from the combustion of a mixture of H2(g) and O2(g)? H2(g) + O2(g) H2O(l); H° = –285.8 kJ A) B) C) D) E) 4.147 g 2.073 g 0.2412 g 6.162 g 2.131 g ____ 42. The quantity of heat required to raise the temperature of a sample of a substance by 1°C is the sample’s A) work. B) calorimetry. C) heat capacity. D) specific heat. E) enthalpy. ____ 43. A 100 g sample of each of the following metals is heated from 35C to 45C. Which metal absorbs the lowest amount of heat energy? Metal copper magnesium mercury silver lead A) B) C) D) E) ____ Specific Heat 0.385 J/(g°C) 1.02 J/(g°C) 0.138 J/(g°C) 0.237 J/(g°C) 0.129 J/(g°C) lead magnesium silver mercury copper 44. Exactly 105.2 J will raise the temperature of 10.0 g of a metal from 25.0°C to 60.0°C. What is the specific heat capacity of the metal? A) 0.301 J/(g°C) B) C) D) E) ____ 3.33 J/(g°C) 29.3 J/(g°C) 25.2 J/(g°C) none of these 45. Given: Pb(s) + PbO2(s) + 2H2SO4(l) 2PbSO4(s) + 2H2O(l); H° = –509.2 kJ SO3(g) + H2O(l) H2SO4(l); H° = –130. kJ determine H° for the following thermochemical equation. Pb(s) + PbO2(s) + 2SO3(g) 2PbSO4(s) A) B) C) D) E) 3.77 103 kJ –521 kJ –3.77 103 kJ –639 kJ –769 kJ ____ 46. Which of the following species does not have a standard enthalpy of formation equal to zero at 25°C? A) Cl2(l) B) N2(g) C) Fe(s) D) H+(aq) E) S8(s) ____ 47. What is the frequency of a photon having a wavelength of 954.9 nm? ( ) A) 3.14 10–4 Hz B) 1.44 1027 Hz C) 3.14 1014 Hz D) 2.08 10–37 Hz E) 2.08 10–19 Hz ____ 48. When an electron in an atom makes a transition from n = 6 to n = 4, which of the following statements is/are correct? I. II. III. IV. V. Energy is emitted. Energy is absorbed. The electron loses energy. The electron gains energy. The electron cannot make this transition. A) I and III B) I and IV C) II and IV , D) II and III E) III ____ 49. What is the frequency of light emitted when the electron in a hydrogen atom undergoes a transition from level ( ) A) B) C) D) E) ____ 50. Which of the following combinations of quantum numbers is permissible? A) n = 1, l = 2, ml = 0, ms = B) n = 3, l = 2, ml = 1, ms = C) n = 3, l = 3, ml = 1, ms = D) n = 2, l = 1, ml = –1, ms = 0 E) n = 4, l = 3, ml = 4, ms = CHEM161 FINAL EXAM (PRACTICE) Answer Section 1. ANS: B PTS: 1 DIF: easy REF: 1.3 OBJ: Apply the law of the conservation of mass. (Example 1.1) TOP: general concepts | matter 2. ANS: C PTS: 1 DIF: easy REF: 1.4 OBJ: Describe the classifications of matter: elements, compounds, and mixtures (heterogeneous and homogeneous). TOP: general concepts | matter KEY: states of matter MSC: general chemistry 3. ANS: A PTS: 1 DIF: easy REF: 1.4 OBJ: Understand the difference between chemical changes (chemical reactions) and physical changes. TOP: general concepts | matter KEY: physical and chemical change MSC: general chemistry 4. ANS: A PTS: 1 DIF: easy REF: 1.5 OBJ: Define and use the terms precision and accuracy when describing measured quantities. TOP: general concepts | measurement 5. ANS: D PTS: 1 DIF: easy REF: 1.5 OBJ: Know how to represent numbers using scientific notation. TOP: general concepts | measurement KEY: significant figures | scientific notation MSC: general chemistry 6. ANS: E PTS: 1 DIF: easy REF: 1.5 OBJ: Use significant figures in calculations. (Example 1.2) TOP: general concepts | measurement KEY: significant figures MSC: general chemistry 7. ANS: D PTS: 1 DIF: easy REF: 1.6 OBJ: Convert from one temperature scale to another. (Example 1.3) TOP: general concepts | measurement KEY: SI unit | temperature MSC: general chemistry 8. ANS: C PTS: 1 DIF: difficult REF: 1.7 OBJ: Define and provide examples of derived units. TOP: general concepts | measurement MSC: general chemistry 9. ANS: A PTS: 1 DIF: difficult REF: 1.8 OBJ: Use density to relate mass and volume. TOP: general concepts | measurement 10. ANS: C PTS: 1 DIF: moderate REF: 1.8 OBJ: Apply dimensional analysis to solving numerical problems. TOP: general concepts | measurement KEY: factor label method MSC: general chemistry 11. ANS: C PTS: 1 DIF: easy REF: 2.1 OBJ: Recognize the atomic symbols of the elements. TOP: early atomic theory | atomic theory of matter KEY: atomic symbol MSC: general chemistry 12. ANS: C PTS: 1 DIF: easy REF: 2.2 OBJ: Describe Rutherford's experiment that led to the nuclear model of the atom. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. TOP: early atomic theory | atomic theory of matter ANS: E PTS: 1 DIF: easy REF: 2.3 OBJ: Write the nuclide symbol for a given nuclide. TOP: early atomic theory | atomic theory of matter KEY: nuclear structure MSC: general chemistry ANS: C PTS: 1 DIF: easy REF: 2.5 OBJ: Find the main-group and transition elements on the periodic table. TOP: early atomic theory | periodic table MSC: general chemistry ANS: A PTS: 1 DIF: easy REF: 2.8 OBJ: Write the formula of an ionic compound from its name. (Example 2.5) TOP: early atomic theory | chemical substance KEY: nomenclature of simple compound | ionic compound MSC: general chemistry ANS: B PTS: 1 DIF: moderate REF: 2.9 OBJ: Write chemical equations using appropriate phase labels,symbols of reactions conditions, and the presence of a catalyst. TOP: early atomic theory | chemical equation KEY: balancing chemical equation MSC: general chemistry ANS: D PTS: 1 DIF: easy REF: 2.10 OBJ: Determine if a chemical reaction is balanced. TOP: early atomic theory | chemical equation KEY: balancing chemical equation MSC: general chemistry ANS: D PTS: 1 DIF: easy REF: 3.1 OBJ: Calculate the formula mass from a formula. (Example 3.1) TOP: stoichiometry | mass and moles of substance KEY: formula mass MSC: general chemistry ANS: C PTS: 1 DIF: easy REF: 3.2 OBJ: Calculate the number of molecules in a given mass of substance. (Example 3.6) TOP: stoichiometry | mass and moles of substance KEY: mole | mole calculations MSC: general chemistry ANS: A PTS: 1 DIF: easy REF: 3.3 OBJ: Calculate the percentage composition of the elements in a compound. (Example 3.7) TOP: stoichiometry | determining chemical formulas ANS: A PTS: 1 DIF: easy REF: 3.5 OBJ: Determine the empirical formula from the percentage composition. (Example 3.11) TOP: stoichiometry | determining chemical formulas KEY: empirical formula MSC: general chemistry ANS: C PTS: 1 DIF: easy REF: 3.5 OBJ: Understand the relationship between the molecular mass of a substance and its empirical formula mass. TOP: stoichiometry | determining chemical formulas KEY: molecular formula MSC: general chemistry ANS: D PTS: 1 DIF: easy REF: 3.7 OBJ: Relate the quantities of two reactants or two products. (Example 3.14) TOP: stoichiometry | stoichiometry calculation KEY: amounts of substances MSC: general chemistry ANS: A PTS: 1 DIF: easy REF: 4.1 OBJ: Compare the properties of solutions that contain strong electrolytes and weak electrolytes. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. TOP: MSC: ANS: OBJ: TOP: KEY: ANS: OBJ: TOP: KEY: ANS: OBJ: TOP: KEY: ANS: OBJ: TOP: ANS: OBJ: TOP: MSC: ANS: OBJ: TOP: MSC: ANS: OBJ: TOP: MSC: ANS: OBJ: TOP: MSC: ANS: OBJ: ANS: OBJ: KEY: ANS: OBJ: KEY: ANS: OBJ: TOP: MSC: chemical reactions | ions in aqueous solution KEY: electrolyte general chemistry D PTS: 1 DIF: easy REF: 4.2 From the complete ionic equation, write the net ionic equation. chemical reactions | ions in aqueous solution ionic equation | net ionic equation MSC: general chemistry B PTS: 1 DIF: easy REF: 4.4 Distinguish between a strong base and a weak base and the solutions they form. chemical reactions | types of chemical reactions acid-base reaction | weak base MSC: general chemistry E PTS: 1 DIF: easy REF: 4.5 Define an oxidation-reduction reaction. chemical reactions | types of chemical reactions oxidation-reduction reaction MSC: general chemistry C PTS: 1 DIF: moderate REF: 4.5 Learn the oxidation-number rules. chemical reactions | types of chemical reactions B PTS: 1 DIF: easy REF: 4.7 Calculate the molarity from mass and volume. (Example 4.9) chemical reactions | working with solutions KEY: concentration general chemistry B PTS: 1 DIF: moderate REF: 4.7 Use molarity as a conversion factor. (Example 4.10) chemical reactions | working with solutions KEY: concentration general chemistry D PTS: 1 DIF: difficult REF: 4.8 Perform calculations associated with dilution. chemical reactions | working with solutions KEY: diluting solutions general chemistry A PTS: 1 DIF: moderate REF: 4.10 Calculate the quantity of substance in a titrated solution. (Example 4.14) chemical reactions | quantitative analysis KEY: volumetric analysis general chemistry A PTS: 1 DIF: easy REF: 5.2 Use Boyle's law. (Example 5.2) TOP: phases | gas D PTS: 1 DIF: easy REF: 5.3 Use the ideal gas law. (Example 5.6) TOP: phases | gas ideal gas law | calculations with the ideal gas law MSC: general chemistry E PTS: 1 DIF: easy REF: 5.3 Determine the molecular mass of a vapor. (Example 5.8) TOP: phases | gas ideal gas law | gas density MSC: general chemistry E PTS: 1 DIF: moderate REF: 5.4 Solving stoichiometry problems involving gas volumes. (Example 5.9) phases | gas KEY: ideal gas law | stoichiometry and gas volumes general chemistry 37. ANS: A PTS: 1 DIF: easy REF: 5.6 OBJ: List the five postulates of the kinetic theory. TOP: phases | gas KEY: kinetic theory of an ideal gas | postulates of kinetic theory MSC: general chemistry 38. ANS: E PTS: 1 DIF: easy REF: 5.7 OBJ: Calculate the ratio of effusion rates of gases. (Example 5.13) TOP: phases | gas KEY: molecular speed | effusion MSC: general chemistry 39. ANS: B PTS: 1 DIF: easy REF: 5.8 OBJ: Explain how and why a real gas is different from an ideal gas. TOP: phases | gas KEY: real gases MSC: general chemistry 40. ANS: D PTS: 1 DIF: easy REF: 6.4 OBJ: Manipulate a thermochemical equation using these rules. (Example 6.3) TOP: thermochemistry | heats of reaction KEY: thermochemical equation | enthalpy of reaction MSC: general chemistry 41. ANS: A PTS: 1 DIF: easy REF: 6.5 OBJ: Calculate the heat absorbed or evolved from a reaction given its enthalpy of reaction and the mass of a reactant or product. (Example 6.4) TOP: thermochemistry | heats of reaction 42. ANS: C PTS: 1 DIF: easy REF: 6.6 OBJ: Define heat capacity and specific heat. TOP: thermochemistry | heats of reaction KEY: calorimetry | heat capacity MSC: general chemistry 43. ANS: A PTS: 1 DIF: easy REF: 6.6 OBJ: Relate the heat absorbed or evolved to the specific heat, mass, and temperature change. TOP: thermochemistry | heats of reaction 44. ANS: A PTS: 1 DIF: easy REF: 6.6 OBJ: Calculate using this relation between heat and specific heat. (Example 6. 5) TOP: thermochemistry | heats of reaction KEY: calorimetry | specific heat MSC: general chemistry 45. ANS: E PTS: 1 DIF: moderate REF: 6.7 OBJ: Apply Hess's law to obtain the enthalpy change for one reaction from the enthalpy changes of a number of other reactions. (Example 6.7) TOP: thermochemistry | heats of reaction KEY: Hess's law MSC: general chemistry 46. ANS: A PTS: 1 DIF: easy REF: 6.8 OBJ: Define standard state and reference form. TOP: thermochemistry | heats of reaction KEY: standard enthalpies of formation MSC: general chemistry 47. ANS: C PTS: 1 DIF: easy REF: 7.1 OBJ: Relate the wavelength, frequency, and speed of light. (Examples 7.1 and 7.2) TOP: atomic theory | light KEY: electromagnetic radiation MSC: general chemistry 48. ANS: A PTS: 1 DIF: easy REF: 7.3 OBJ: Relate the energy of a photon to the associated energy levels of an atom. TOP: atomic theory | light 49. ANS: E PTS: 1 DIF: moderate REF: 7.3 OBJ: TOP: MSC: 50. ANS: OBJ: TOP: MSC: Determine the wavelength or frequency of a hydrogen atom transition. (Example 7.4) atomic theory | light KEY: Bohr theory | atomic line spectra general chemistry B PTS: 1 DIF: easy REF: 7.5 Apply the rules for quantum numbers. (Example 7.6) atomic theory | quantum mechanics KEY: quantum numbers general chemistry