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Fundamentals of Chemistry Final Exam Practice Test: 1. Which of the following is classified as a chemical change? a) making ice cubes b) cutting a cake c) melting iron d) baking a cake 2. Round 9.8756 to three significant figures: a) 9.87 b) 9.88 c) 9.86 d) 9.9 3. How many valence electrons do halogens have? a) 2 b) 8 c) 5 d) 7 4. The elements that have the highest ionization energy are on which side of the periodic table? a) the top right b) the top left c) the bottom right d) the bottom left 5. The number 0.0045978 in scientific notation is: a)4.5978 x 10^3 b) 4.5978 x 10^-2 c) 4.5978 x 10^-3 d) 4.5978 x 10^2 6. If an element has an atomic mass of 52, and there are 24 protons, how many neutrons are there? a. 24 b. 28 c. 25 d. 32 7. An ionic bond has a difference in electronegativity of: a. >1.9 c. 0.5-1.9 b.<0.5 d. 0.9-1.5 8. The fact that atoms are most stable when they have a full valence shell is known as: a. the covalence theory b. the octet rule c. the atomic theory d. Dalton’s rule 9. The mass of a sample is 6.00 g and its volume is 3.0 L. The density of the sample is: a. 0.50 g/L b. 0.500 g/L c. 2.00 g/L d. 2.0 g/L 10. The Law of Conservation of Energy states: a.energy can’t be created b. energy can’t be destroyed c. both a and b d. neither a nor b 11. Gases differ from liquids in that they: a.have no definite shape b. have no definite volume c. are uncompressible d.have definite shape 12. Which orbital is lowest in energy? a. 1s c. 3s d. 2s d. 2p 13. Alpha emission involves the release of what? a. the nucleus of a hydrogen atom b. an electron c. the nucleus of a helium atom d. a neutron 17. One mole of methane gas occupies 20.0L at 1.00 atm pressure. What is the temperature of the gas in kelvins? a. 244 K b. 368 K c. 543 K d.273 K 20. A gas has a volume of 0.50 L and a pressure of 1.0 atm at 393 K. When the gas is heated to 500 K, its volume expands to 3.0 L. What is the new pressure of the gas in the container? a. 0.54 atm b. 0.28 atm c. 0.34 atm d. 0.21 atm 21. If 3.3 g of a gas at 40 degrees Celsius and 1.15 atm pressure occupies a volume of 1.0 L, what is the mass of one mole of the gas? a. 62 g/mol b. 45 g/mol c. 74 g/mol d.52 g/mol 22. To a tank containing nitrogen gas at 2.0 atm and oxygen gas at 1.0 atm, we add an unknown quantity of carbon dioxide gas until the total pressure in the tank is 4.6 atm. What is the partial pressure of carbon dioxide? a. 1.3 atm b. 4.6 atm c. 2.0 atm d. 1.6 atm 23. Which of the following types of intermolecular forces is the strongest? a. hydrogen bonds b. dispersion forces c. dipole-dipole forces 24. What is the molecular weight of KCl? a. 76.8 amu b. 74.6 amu c. 82.3 amu d. 67.5 amu 25. Calculate the number of grams in 1.77 mol of NO2: a. 81.4 g b. 5.34 g c. 6.8 g d. 112.4 g 26. How many grams of NaOH are needed to make 2.0 L of 0.15 M solution of NaOH made? a. 6 g b. 8 g c. 10 g d. 12 g 27. If we have 6.0 M HCl solution, what volume of this is needed to make 200mL of 3.5 M solution? a. 0.12 L b. 1.2 L c. 12 L d. 120 L 28. What is the pH of a phosphate buffer solution containing 1.0 M of NaH2PO4 and 0.50 M Na2HPO4? H2PO4– + H2O HPO4-2 + H3O + pKa=7.21 a. 6.95 b. 8.34 c. 6.91 d. 7.26 29. What is the pOH of a soltution with a pH=5.3? a. 11.7 b. 8.7 c. 6.3 d. 5.3 30. Which of the following is a colligative property? a. boling point b. freezing point depression c. boiling depression 32. If you remove a reactant from a reaction at equilibrium, which direction will the reaction shift? a. right b. left c. neither 33. What is the [H3O ] for a solution with [OH– ] of 5.0 x 10–7 M? + a. 14.99 x 10–8 M b 2.40 x 10–8 M c. 1.99x 10–8 M 35. KOH is a: a. strong acid b. weak acid c. strong base d. weak base 36. When are Arrhenius acid and base definitions useful? a. in aqueous solutions only b. in all solutions c. all the time 37. H2SO4 is: a. monoprotic b. diprotic c. triprotic d. polyprotic 39. The atomic number is equal to: a. the number of neutrons b. the number of protons c. the atomic mass d. the number of isotopes 40. An isotope has the same number of protons, but different numbers of neutrons. a. false b. true 41. The atomic number of Boron is: a. 3 b. 5 c. 10 d. 11 42. A reaction that gives off heat is called: a. endothermic b. enterthermic c. exothermic d. intrathermic 43. Water is capable of which intermolecular forces: a. dispersion b. dipole-dipole c. hydrogen bonds d. all of the above 44. Magnesium likes to: a. gain 1 electron b. lose 1 electron c. gain 2 electrons d. lose 2 electrons 45. The most common isotope of carbon has atomic weight of: a. 12 b. 11 c. 13 d. 14 46. Calories and Joules measure what? a. temperature b. mass c. energy d. volume 47. Polar solutions are more like to dissolve: a. nonpolar substances b. polar substances c. neither 48. How many electrons can the p orbital hold if full? a. 2 b. 3 c. 5 d. 6 49. Halogens like to lose ____ electrons in order to have a noble gas electron configuration? a. 1 b. 2 c. 3 d. 4 50. 30 grams is the same as: a. 0.30 kg b. 3.0 kg c. 0.003 kg d. 0.030 kg Answer key: 1. d 2. b 3. d 4. a 5. c 6. b 7. a 8. b 9. d 10. c 11. a 12. a 13. c 14. c 15. a 16. b 17. a 18. a 19. b 20. d 21. c 22. d 23. a 24. b 25. a 26. d 27. a 28. c 29. b 30. b 31. a 32. a 33. c 34. a 35. c 36. a 37. b 38. c 39. b 40. b 41. b 42. c 43. d 44. d 45. a 46. c 47. c 48. d 49. a 50. d
"46050_2007 - practice exam 2"