Although there is more information in each chapter, I am focusing on key parts that will be questions on the MC and FR sections. Please show all work on each problem, including appropriate units!!

1. A radio broadcasts at a frequency of 107.9 MHz. a. How many seconds per cycle are there? b. What is the broadcast frequency in gigahertz?

2. Which of the following is less: a. 8.7 g/mL or 6.1 µg/µL b. 4 x 105 kg/cm3 or 4 x 10-1 mg/cm3

3. Sulfur and oxygen can react to form both sulfur dioxide and sulfur trioxide. In sulfur dioxide, there are 32.06 g of sulfur and 32.00 g of oxygen. In sulfur trioxide, 32.06 g of sulfur are combined with 48.00 g of oxygen.

a. What is the ratio of the weights of oxygen that combine with 32.06 g of sulfur? b. How do these data illustrate the law of multiple proportions?

4. How many protons, neutrons and electrons are n each of the following? a. 16O-2 b. 122Sb+2 c. 56Fe+3 d. 184W

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5. Name the following compounds: a. PbI2 d. Fe(IO4)3 g. HBr

b. LiH e. NI3 h. HNO2

c. Cr(OH)3 f. P4O10 i. NaHSO3

6. Provide formulas for each of the following names: a. Calcium phosphate d. dinitrogen tetroxide g. nitric acid

b. Manganese dioxide e. potassium permanganate h. hydrocyanic acid

c. Lithium aluminum f. sulfurous acid i. barium chloride hydride

7. Bauxite, the principle ore used in the production of aluminum cans, has a molecular formula of Al2O3 * 2H2O.

a. Determine the molar mass of bauxite b. How many grams of Al are in 0.58 moles of bauxite? c. How many atoms of Al are in 0.58 moles of bauxite? d. What is the mass in grams of 2.1 x 1024 molecules of bauxite?

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8. The analysis of a rocket fuel showed that it contained 87.4% nitrogen and 12.6% hydrogen by mass. Mass spectral analysis showed the fuel to have a molar mass of 32.05 g. What are the empirical and molecular formulas of the fuel?

9. The following reaction was performed: Fe2O3 (s) + 2 X (s) 2 Fe + X2O3 (s) It was found that 79.847 g of Fe2O3 reacted with “X” to form 55.847 g of Fe and 50.982 g of X2O3. Identify element X.

10. A reaction combines 64.81 g of silver nitrate in solution with 92.67 g of potassium bromide in solution.

a. Write the balanced equation for the reaction (including phases) b. How much silver bromide is precipitated? c. Which reactant is limiting? Which is excess? d. How much of the excess is left over? e. If the actual yield of silver bromide were 14.77 g, what is the percent yield?

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11. Calculate the concentration of each ion in a 0.25 M Na3PO4 solution?

12. Describe how you would prepare a 750 mL solution that is 0.35 M BaSO4.

13. A solution of ammonium acetate was made by dissolving 3.85 g of ammonium acetate in enough water to make 500. mL of solution. Calculate the solute concentration.

14. A solution contains Ag+, Pb+2 and Fe+3. If you want to precipitate the Pb+2 selectively, what anion would you choose?

15. What mass of Mg(OH)2 is produced when 100. mL of 0.42 M Mg(NO3)2 is added to excess NaOH solution.

16. What mass of CaCO3 is produced when 250. mL of 6.0 M H2CO3 is added to 750 mL of 1.0 M CaF2?

17. What volume of 0.1379 M HCl is required to neutralize 10.0 mL of 0.2789 M NaOH solution?

18. A titration is done using 0.1302 M NaOH to determine the molar mass of an acid. The acid contains one acidic hydrogen per molecule. If 1.863 g of the acid require 70.11 mL of the NaOH solution, what is the molar mass of the acid?

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19. Determine the oxidation number for each atom in the following: a. Cr2O7-2 b. NaClF4

20. Balance the following redox reaction (acidic solution). Identify the oxidizing agent and reducing agent.

Cr+3 + XeF6 Cr2O7-2 + Xe + F-

21. Balance the following redox reaction that takes place in a basic solution. Co(OH)3 + Sn Co(OH)2 + HSnO2

22. List the regions of the electromagnetic spectrum from high frequency to low frequency and the approximate wavelengths of radiation associated with the visible light colors.

23. A carbon-oxygen double bond in a certain organic molecule absorbs radiation that has a frequency of 6.0 x 1013 s-1. a. to what region of the spectrum does this radiation belong? b. what is the wavelength of the radiation c. what is the energy of this radiation per photon? Per mole of photons? d. a carbon-oxygen bond in a different molecule absorbs radiation with a frequency equal to 5.4 x 1013 s-1. Does this radiation give more or less energy?

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24. Calculate the wavelength of light that must be absorbed by a hydrogen atom in its ground state to reach the excited state of ΔE = + 2.914 x 10-18J.

25. Calculate the wavelength of light emitted in the spectral transition from n=4 to n=2.

26. Which of the following sets of quantum numbers are allowed? a. n=4, l=7, ml=0 b. n=7, l=0, ml=1 c. n=7, l=5, ml=-3 d. n=3, l=-1, ml=0 e. n=0, l=0, ml=0

27. What is the electron configuration of calcium? How barium compare?

28. How many half-filled orbitals does each of the following have in the ground state? a. O b. B c. Mn

29. An element “X” combines with calcium to give a salt CaX2. The element has the highest energy electrons in the 4p. What is “X”

30. Order the following groups from smallest to largest radius. a. Ar, Cl-, K+, S-2 b. Na, Mg, Ar, P

31. Which of the following will have the most exothermic electron affinity? The least? a. Ge, Si, C b. Cl, Cl-, Cl+

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32. Using the periodic table, place the following in order from the lowest to the highest

electronegativity: F, Nb, N, Si, Rb, Ca, N, F

33. Place the following in order of increasing polarity: NaBr, I2, H2O, MnO2, CN-

34. Which of the following molecules would you expect to have a dipole moment of zero? Describe the dipole orientation of the other two molecules. a. KI b. CF4 H2Se

35. List four ions that are isoelectronic with argon and have charges from +2 to -2. Arrange them in order of increasing ionic radius.

36. Predict formulas of the binary compounds formed from the following sets of atoms a. Mg and N ________________________ b. Na and F ________________________ c. Ca and S ________________________ d. Sr and Te ________________________

37. Place the following in an order of increasing ionic size. Use shorthand notation to list

the core electron configuration for each of the ions. a. Ba+2, Te-2, Cs+, I-

38. Using the bond energy values listed in Table 8.4 of your text, calculate ΔH for the following: HCN(g) + 2 H2(g) CH3NH2(g)

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39. Draw the Lewis dot structures for the following. Then, determine the molecular geometry of each. Finally, indicate which molecules or ions are polar.

a. SeF6 d. CF3Cl g. IF4

b. N2O e. SCl4 h. SnCl5

c. ClO- f. H2Se i. TlCl2

40. The condensed formula for urea is H2NCONH2. a. Draw the Lewis structure b. How many σ bonds are there? c. How many π bonds are there? d. What is the hybridization at the carbon? e. How are the nitrogen atoms hybridized? f. What is the N-C-N bond angle expected to be? g. How many lone pairs of electrons are there?

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41. A diver at a depth of 100 ft (pressure approximately 3 atm) exhales a small bubble of air with a volume equal to 100 mL. What will be the volume of the bubble at the surface.

42. The volume of a gas (held at constant pressure) is to be used “as a thermometer”. If the volume at 0.0oC is 75.0 cm3, what is the temperature when the volume is 56.7 cm3?

43. If a 16.6 L sample of gas contains 9.2 moles of F2, how many moles of gas would there be in a 750 mL sample at the same temperature and pressure?

44. A weather balloon is filled with 0.285 m3 of helium on the ground at 180C and 756 toor. What will the volume of the balloon be at an altitude of 10 km where the temperature is -480C and the pressure is 0.14 atm?

45. A 10.5 g sample of CO2 gas occupies a volume of 7.00 L at a pressure of 1.5 atm. What must be the temperature of the gas?

46. A hydrocarbon was analyzed to be 85.7% C and 14.3% H. At 260C and 745 torr pressure a sample with a volume of 1.13 L had a mass of 1.904g. Determine the molecular formula.

47. An unknown gas has a density of 7.06 g/L at a pressure of 1.50atm and 280 K. Calculate the molar mass of the gas.

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48. A 27.7 mL sample of CO2 was collected over water at 25.00C and 1.00 atm. What is the pressure due to the CO2? (the vapor pressure of water at 25.00C is 23.8 torr). What will the volume of CO2 be at the same temperature and pressure after removing the water vapor?

49. A gaseous mixture of O2, H2 and N2 has a total pressure of 1.50 atm and contains 8.20 g of each gas. Find the partial pressure of each gas in the mixture.

50. Calculate the root mean square speed of O2 gas molecules at 300 K.

51. What happens to the average kinetic energy of a mole of an ideal gas if: a. The volume is doubled resulting in a decrease in pressure at a constant

temperature b. The temperature is increased at a constant pressure? c. Absolute zero is obtained?

52. What are the relative rates of diffusion for methane (CH4) and oxygen (O2)? If O2 travels 1.00 m in a certain amount of time, how far will the methane be able to travel under the same conditions?

53. Which gas would effuse faster, Ar or O2? How much faster?

54. Define the terms in your own words: a. dipole-dipole forces b. hydrogen bonding c. London Dispersion forces

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55. Of HF, HCl and HBr, which has the highest boiling point? Why? Which has the lowest

boiling point?

56. Which would you expect to have a lower melting point, C3H8 or CH3OH? Why?

57. Which would have greater surface tension N2(l) or Br2(l)? Why?

58. Classify the following as either ionic, molecular or atomic crystalline solids: a. dry ice b. graphite c. CaF2 d. MnO2 e. Naphthalene, C10H8

59. Why is iron relatively soft, ductile and malleable, while high carbon steeles are much stronger and less malleable?

60. On the top of one of the peaks of the Rocky Mountains, the pressure of the atmosphere is 550 torr. Determine the boiling point of water at this location.

61. Isopropanol, C3H8O is also known as rubbing alcohol. The heat of vaporization is 42.1 kJ/mole. How much heat is needed to evaporate 25 g of isopropanol?

62. What is the final temperature when 10 g of water at 0oC is added to 100 g of water at 75oC?

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63. Sodium chloride dissolves easily in distilled water to make a solution. Calculate the molarity, molality, mass percent and mole fraction of sodium chloride if 54.76 g of NaCl dissolves in 250. mL of water. Assume the density of water is 1.00 g/ml.

64. The solubility of nitrogen at 0oC in water is 8.21 x 10-4mol/L, if the N2 pressure above the water is 0.790 atm. What is the solubility at 1 atm of N2 and 00C? What is the Henry’s Law constant for nitrogen?

65. 58 g of NaCl are added to 180 g of water at 380C. Calculate the vapor pressure of the solution at 380C? The molar mass for NaCl is 58 g/mol and the vapor of water at 380C is 50. torr.

66. Calculate the vapor pressure of a solution of 40.27 g MgCl2 in 500.3 mL of water at 25.00C. The density of water is 0.9971 g/m? and the vapor pressure is 23.756 torr.

67. A solution is made by mixing acetone (C3H6O) and methanol (CH3OH) in a closed container at 250C. The acetone mole fraction in the liquid is 0.50. Assume ideal behavior for both the liquid and gass phase. What is the mole fraction in the gas phase above the solution at 250C. (vapor pressure at 250C for pure acetone and pure methanol are 270 torr and 140 torr respectively)

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68. A 7.45 g unknown solute was dissolved into 87.9 g of benzene. The boiling point of the mixture was measured to be 83.80C. What is the molar mass of the unknown solute. The Kb for benzene is 2.530C/m, the normal boiling point for benzene is 80.10C and the density of benzene is 0.879g/mL.

69. The osmotic pressure of blood is 7.65 atm at 370C. How much glucose, C6H12O6 should be used per liter for an intravenous injection having the same osmotic pressure as blood?