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

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Luke Wilson
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1 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 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 10 5 kg/cm 3 or 4 x 10-1 mg/cm 3 3. Sulfur and oxygen can react to form both sulfur dioxide and sulfur trioxide. In sulfur dioxide, there are g of sulfur and g of oxygen. In sulfur trioxide, g of sulfur are combined with g of oxygen. a. What is the ratio of the weights of oxygen that combine with 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. 16 O -2 b. 122 Sb +2 c. 56 Fe +3 d. 184 W

2 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 molecules of bauxite? 2

3 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 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 g of Fe2O3 reacted with X to form g of Fe and g of X2O3. Identify element X. 10. A reaction combines g of silver nitrate in solution with 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 g, what is the percent yield? 3

4 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 BaSO 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 M HCl is required to neutralize 10.0 ml of M NaOH solution? 18. A titration is done using M NaOH to determine the molar mass of an acid. The acid contains one acidic hydrogen per molecule. If g of the acid require ml of the NaOH solution, what is the molar mass of the acid? 4

5 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 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 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 s -1. Does this radiation give more or less energy? 5

6 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 = x J. 25. Calculate the wavelength of light emitted in the spectral transition from n=4 to n= 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 + 6

7 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 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 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) 7

8 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? 8

9 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 0.0 o C is 75.0 cm 3, what is the temperature when the volume is 56.7 cm 3? 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 m 3 of helium on the ground at 18 0 C and 756 toor. What will the volume of the balloon be at an altitude of 10 km where the temperature is C 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 26 0 C 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. 9

10 48. A 27.7 ml sample of CO2 was collected over water at C and 1.00 atm. What is the pressure due to the CO2? (the vapor pressure of water at C 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 10

11 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 0 o C is added to 100 g of water at 75 o C? 11

12 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 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 0 o C in water is 8.21 x 10-4 mol/l, if the N2 pressure above the water is atm. What is the solubility at 1 atm of N2 and 0 0 C? What is the Henry s Law constant for nitrogen? g of NaCl are added to 180 g of water at 38 0 C. Calculate the vapor pressure of the solution at 38 0 C? The molar mass for NaCl is 58 g/mol and the vapor of water at 38 0 C is 50. torr. 66. Calculate the vapor pressure of a solution of g MgCl2 in ml of water at C. The density of water is g/m? and the vapor pressure is torr. 67. A solution is made by mixing acetone (C3H6O) and methanol (CH3OH) in a closed container at 25 0 C. The acetone mole fraction in the liquid is Assume ideal behavior for both the liquid and gass phase. What is the mole fraction in the gas phase above the solution at 25 0 C. (vapor pressure at 25 0 C for pure acetone and pure methanol are 270 torr and 140 torr respectively) 12

13 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 C. What is the molar mass of the unknown solute. The Kb for benzene is C/m, the normal boiling point for benzene is C and the density of benzene is 0.879g/mL. 69. The osmotic pressure of blood is 7.65 atm at 37 0 C. How much glucose, C6H12O6 should be used per liter for an intravenous injection having the same osmotic pressure as blood? 13

3. Which of the following compounds is soluble? The solubility rules are listed on page 8.

3. Which of the following compounds is soluble? The solubility rules are listed on page 8. 1. Classify the following reaction. Sb 2 O 3 + 3 Fe 2 Sb + 3 FeO a) Combination reaction b) Decomposition reaction c) Neutralization reaction d) Single-replacement reaction e) Double-replacement reaction