Spring 2004 Final Exam Review Problems

Spring 2012 Final Exam Review Problems

Chapter 9

1. How many moles of oxygen gas will react with excess sulfur according to produce 1.25 mol of sulfur trioxide according to the following equation? __1__ S8 + __12__ O2  __8__SO3

A 0.833 mol C 1.25 mol B 1.88 mol D 10.0 mol

2. What is the molar mass of iron (III) sulfate, Fe2(SO4)3?

A 104.0 g/mol C 312.0 g/mol B 335.7 g/mol D 399.9 g/mol

3. Given the reaction 2 NO + O2  2 NO2, if 6.5 L of O2 react at STP, how many liters of NO2 are produced?

A 6.5 L C 3.2 L B 26 L D 13 L

4. Given the reaction Zn + 2 HCl  ZnCl2 + H2, if 2.0 mol Zn and 5.0 mol of HCl are allowed to react:

A Zn is the limiting reactant C HCl is the limiting reactant B 1.0 mol of ZnCl2 is produced D 5.0 mol of H2 is produced

5. Given the reaction CaCO3  CaO + CO2, if 50.0 g of CaCO3 react to produce 20.0 g of CO2, what is the percent yield of CO2?

A 66.7% C 40.0% B 90.9% D 250%

6. What is the molarity of a solution containing 27.5 grams of NaOH in a 100. mL solution?

A 0.275 M C 0.688 M B 6.88 M D 275 M

7. What is the mass, in grams, of 250 mL of a 0.100 M solution of KNO3?

A 2.53 grams C 253 grams B 40.5 grams D 4.05 grams

8. Concentrated hydrochloric acid, HCl, has a molarity of 12.0 M. If 15.0 mL of concentrated HCl is diluted to a total volume of 250 mL, what is the molarity of the diluted acid?

A 2.00 M C 0.72 M B 7.2 M D 0.200 M 9. When sulfuric acid, H2SO4, reacts with potassium hydroxide, KOH, the products of the reaction are water and potassium sulfate, K2SO4. If 10.9 mL of 3.0 M KOH reacts with excess H2SO4, how many grams of potassium sulfate could be produced according the balanced equation shown below?

H2SO4 + 2 KOH  2 H2O + K2SO4

A 5.70 grams C 10.4 grams B 114 grams D 2.85 grams

Chapter 10 10. What is the frequency of radiation whose wavelength is 5.89 x 10 - 9 m?

A 1.96 x 10 – 17 s-1 C 1.77 x 10 1 s-1 B 5.09 x 10 16 s-1 D 1.77 x 10 18 s-1

11. Which of the following is not a type of electromagnetic radiation?

A X-rays C Gamma rays B Radiowaves D Alpha waves

12. How many electrons can be held in the 2nd energy level?

A 2 C 8 B 18 D 32

13. Which element is represented by the following electron configuration? 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p4

A Thallium C Polonium B Bismuth D Astatine

14. Which of the following is the correct noble gas configuration for Barium?

A [Kr]5s2 C [Xe]5s2 B [Xe]6s1 D [Xe]6s2

15. Which element is represented by the following noble gas configuration? [Kr]5s24d105p4

A Tellurium C Bromine B Selenium D Indium

16. What part of the following electron configuration is not in the correct order? 1s22s22p63s23p64s24d104p6

A 3p6 C 4d10 B 4p6 D 4s2 17. How many orbitals does each “d” sublevel contain?

A 1 C 3 B 5 D 7

18. What is the maximum number of electrons that each “p” sublevel can hold?

A 2 C 6 B 10 D 14

19. Put the following elements in order of decreasing atomic radii: Fe, S, F, Ba, Cl, Ca

A F, Cl, S, Fe, Ba, Ca C Ba, Ca, Fe, S, Cl, F B F, Cl, S, Fe, Ca, Ba D Cl, Ca, F, Fe, Ba, S

20. Put the following elements in order of increasing electronegativity: Rb, O, Ca, Sr, Mn

A Rb, Sr, Ca, Mn, O C Rb, O, Ca, Sr, Mn B O, Mn, Ca, Sr, Rb D Rb, Ca, Sr, Mn, O

21. Which of the following elements has the smallest ionization energy: C, Se, K, or Sc?

A C C Se B K D Sc

22. What is the electron configuration for Arsenic?

A 1s22s22p63s23p64s23d104p3 B 1s22s22p63s23p64s23d94p4 C 1s22s22p63s23p64s13d104p4 D 1s22s22p63s23p64s23d104p6

23. Put the following in order of decreasing ionic radii: N - 3, F - 1, Na + 1, Mg + 2, O - 2.

A N - 3, F - 1, Na + 1, Mg + 2, O - 2 B N - 3, O - 2, F - 1, Na + 1, Mg + 2 C Mg +2, Na + 1, F - 1, O - 2, N - 3 D N - 3, O - 2, Mg + 2, F - 1, Na + 1

24. How many unshared electrons will Silicon have in its orbital notation?

A 0 C 1 B 2 D 3

Chapter 11

-3 25. How many valence electrons does C2ClO3 contain?

A 32 C 36 B 33 D 29 26. What is the electron configuration for sulfide ion, S-2?

A 1s22s22p63s23p3 C 1s22s22p63s23p4 B 1s22s22p63s23p6 D 1s22s22p63s23p1

According to the Lewis diagram above, a nitrogen molecule has a –

A bent structure and a double bond B polar structure and a triple bond C linear structure and a triple bond D circular structure and an ionic bond

28. Which of the following elements is not an exception to the octet rule?

A Hydrogen C Beryllium B Boron D Carbon

29. Which of the following compounds is considered ionic?

A CO C H2O B NaCl D F2

30. The bond between carbon and chlorine is polar. Carbon tetrachloride is a molecule with a tetrahedral shape. This molecule is

A polar C nonpolar B ionic D metallic

31. Methane, CH4, contains what type of intermolecular forces?

A hydrogen bonding C dipole-dipole interactions B dispersion forces D nonpolar covalent bonding

32. The bond that exists between nitrogen and fluorine is

A ionic C covalent B polar covalent D nonpolar ionic

33. When drawing structural formulas, two lines between atoms (as in O = C = O) represents

A 2 electrons in a single bond B 2 electrons in a double bond C 4 electrons in a double bond D 4 electrons in a single bond 34. The bond in the molecule hydrogen bromide, HBr, is considered to be

A nonpolar covalent C polar covalent B ionic D metallic

35. Which of the following ions or molecules would have resonance structures?

-1 -1 A ClO3 C NO2 -3 B PO4 D O2

36. How many valence electrons would an atom of aluminum gain or lose when forming a bond?

A gain 3 C lose 3 B gain 5 D lose 5

-2 37. What is the VSEPR shape for SO3 ?

A trigonal planar C bent B tetrahedral D trigonal pyramidal

Chapter 12

38. The average kinetic energy of water molecules is greatest in:

A steam at 200oC C liquid water at 90oC B liquid water at 273 K D ice at 0oC

39. An increase in the temperature of a contained liquid:

A causes the vapor pressure above the liquid to increase. B decreases the vapor pressure above a liquid. C causes fewer particles to escape the surface of the liquid D has no effect on the kinetic energy of the liquid

40. A pressure of 2.5 atm is equivalent to

A 41 kPa C 1900 mm Hg B 3.0 x 102 torr D 2.5 kPa

41. At 80 K, the particles of a gas have:

A twice the average kinetic energy of the same particles at 40 K B half the average kinetic energy of the same particles at 40 K C one-fourth the average kinetic energy of the same particles at 20 K D none of these

42. Compared with gases, liquids:

A have stronger attractions between particles B have more space between their particles C are much less dense D are more easily compressed o o 43. Helium gas is collected over water at 25 C (Pwater at 25 C = 23.8 mm Hg). What is the partial pressure of the helium, given the barometric pressure is 750.0 mm Hg?

A 773.8 mm Hg C 750.0 mm Hg B 726.2 mm Hg D 701.2 mm Hg

44. A 1.0 mol sample of gas is at a temperature of 20oC and a pressure of 1.2 atm. What is the volume occupied by the gas? (R = 0.0821 L atm/K mol)?

A 20 L C 30 L B 40 L D 50 L

45. Increasing the volume of a given amount of gas at constant temperature causes the pressure to decrease because:

A the molecules are striking a larger area with the same force B there are fewer molecules C the molecules are moving more slowly D there are more molecules

46. A gas occupies a volume of 2.50 L at a pressure of 350.0 kPa. If the temperature remains constant, what volume would the gas occupy at 1750 kPa?

A 5.00 L C 0.500 L B 12.5 L D 1.40 x 102 L

47. A sample of chlorine gas has a pressure of 7.25 kPa at 20.0oC. What will its pressure be at 60.0oC if its volume remains constant?

A 2.42 kPa C 8.24 kPa B 21.8 kPa D 6.38 kPa

48. What is the mass, in grams, of 0.125 L of CO2 gas at STP?

A 0.246 g C 2.80 g B 181 g D 4.11 g

49. If a sample of oxygen occupies a volume of 2.15 L at a pressure of 58.0 kPa and a temperature of 25oC, what volume would this sample occupy at 101.3 kPa and 0.0oC?

A 1.35 L C 1.13 L B 4.10 L D 3.44 L

50. Among the gases listed, which would have the fastest rate of effusion?

A NH3 C CH4 B SO2 D NO2 Chapter 16 51. What is the pH of a solution with an [OH-1] = 4.5 x 10-8?

A 7.35 C 6.65 B 8.65 D 5.35

52. Which of the following concentrations or pH values would be for an acidic solution?

A pH = 7.4 C [H+1] = 2.0 x 10-10 B pOH = 9.3 D [OH-1] = 4.2 x 10-5

53. Which of the following is not a strong acid?

A HNO3 C H2SO4 B HF D HBr

54. What is the pH of a 0.001 M HCl solution?

A 0.001 C 4 B 3 D 5

55. What is the pH of a 0.025 M Sr(OH)2 solution?

A 1.3 C 1.60 B 12.40 D 12.70 Spring Final Exam Review Problems Part II

-1 1. For each of the following Lewis molecules and ions: NO3 , PCl3 and SO2Cl2  Determine the number of valence electrons.  Draw the Lewis dot structure. If necessary, draw all possible resonance structures.  Determine if it is polar or nonpolar.  Determine the VSEPR shape.  Tell the strongest type of intermolecular force.

2. How many grams of dinitrogen tetrafluoride, N2F4, can be produced by the reaction of 5.8 grams of ammonia, NH3, and 9.5 grams of fluorine gas, F2? What is the limiting reactant? What is the excess reactant? How much excess remains at the end of the reaction? What is the percent yield of N2F4 if the actual yield is 4.8 g N2F4? 2 NH3 + 5 F2  1 N2F4 + 6 HF

3. How many milliliters of hydrogen gas, H2, will be produced when 25.0 mL of 1.00 M HCl reacts with excess magnesium at STP? Mg (s) + 2 HCl (aq)  MgCl2 (aq) + H2 (g) o 4. Helium gas, He, collected over water at 22 C and a total pressure of 1.00 atm occupied a vessel whose volume was 2.54 L. What is the partial pressure of He at 22oC? What volume, in mL, would this gas occupy if it were cooled to liquid-nitrogen temperature (-197oC) and 125 kPa?

5. If it takes 4.67 times as long for 0.75 moles of an unknown gas to effuse as it takes the same number of moles of hydrogen gas, H2, to effuse under the same conditions, what is the molar mass of the unknown gas?

-8 6. How much energy, in Joules, would be produced when a particle of light has a wavelength of 8.23 x 10 m? (Hint: you must use the c = w x f equation and the E = h x f equations).

7. Draw the orbital notation for Gallium. Be sure to label each sublevel appropriately. Also, determine the number of shared and unshared pairs of electrons in Gallium. Also write the electron configuration for Gallium and the noble gas configuration for Gallium.

-1 -6 +1 8. A solution has an [OH ] = 6.4 x 10 . Determine the pH, pOH, [H ]. Is this solution acidic, basic, or neutral?