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Chemi1100pretest1 Multiple Choice Identify the choice that best completes the statement or answers the question. ____ 1. Accordingly to the periodic law the properties of elements repeat at regular intervals when the elements are arranged in order of a. their increasing atomic mass. b. their increasing atomic size. c. their increasing number of neutrons in the nucleus. d. their increasing number of isotopes. e. their increasing number of protons in the nucleus. ____ 2. a. b. c. d. e. Which electrons have the greatest influence on the properties of elements? those electrons in s orbitals those electrons in d orbitals core electrons the outermost electrons none of these ____ 3. a. b. c. d. e. Cr Ga Sn Sb Li ____ ____ is a d-transition metal. 4. a. b. c. d. e. Rb Ho Co Ru Bi 5. a. b. c. d. e. Cl Sr Co K N ____ 6. a. b. c. d. e. What would be the outer electron configuration of group VIA (O, S, Se, . . .)? ns2np6 ns2np2 ns2np4 np6 ns0np6 ____ 7. What would be the outer electron configuration of alkaline earth metals? a. ns2np2 b. np2 c. ns0np2 ____ Which one of the following is an inner transition (f-transition) element? Which of the following is not a representative element? d. nd2 e. ns2 ____ ____ ____ ____ ____ 8. Choose the term that best describes all members of this series of elements: Xe, Rn, He, Ne, Kr a. b. c. d. e. metalloids noble gases alkaline earth metals alkali metals representative elements 9. a. b. c. d. e. Al Si P S Cl Which element has the largest atomic radius? 10. Arrange the following elements in order of increasing atomic radii. K, Na, Mg, Cs, Cl a. b. c. d. e. Na < Mg < Cl < K < Cs Cl < Mg < Na < K < Cs Cs < K < Cl < Mg < Na Cl < Mg < Cs < K < Na Cl < Mg < Na < Cs < K 11. a. b. c. d. e. Cs Rb Ca Ba Na Which element has the lowest first ionization energy? 12. a. b. c. d. e. Which of the following elements has the most negative electron affinity? Si P S Se Te ____ 13. a. b. c. d. e. Which one of the following species is not isoelectronic with neon? Mg2+ Na+ O2 Si2+ Al3+ ____ 14. Which ion has the largest radius? + a. Li b. Na+ c. Be2+ d. Mg2+ e. Al3+ ____ 15. a. b. c. d. e. ____ 16. Simple positively charged ions are always ____ than the neutral atoms from which they are formed. smaller larger isoelectronic the same size more anionic Arrange the following elements in order of decreasing electronegativities. Al, Cs, Mg, Na, P a. b. c. d. e. P > Al > Mg > Na > Cs Cs > Na > Mg > Al > P Al > Mg > Na > Cs > P P > Al > Mg > Cs > Na P > Cs > Na > Mg > Al ____ 17. a. b. c. d. e. Which of the following pairs of elements would be expected to form an ionic compound? S / F H / C Rb / Cl As / Br C / I ____ 18. a. b. c. d. e. Which of the following oxides does not give an acidic solution when dissolved in water? SO2 CO2 N2O5 P4O10 Na2O ____ 19. a. b. c. d. e. An amphoteric compound exhibits acidic properties. acidic and basic properties. metallic properties. basic properties. ionic properties. ____ 20. a. b. c. d. e. Atoms consist of three fundamental particles. What are these particles and their charges? proton (+1), neutron (neutral) and electron (1) proton (1), neutron (+1) and electron (neutral) proton (+1), neutron (1) and electron (neutral) proton (neutral), neutron (+1) and electron (1) proton (1), neutron (neutral) and electron (+1) ____ 21. a. b. c. d. One of the following does not describe solids. Which one is it? Particles in definite positions. Definite shape. Easily compressed. Relatively high densities. e. Particles compact. ____ 22. a. b. c. d. e. All of the following are properties of antimony. Which one is not a physical property? It is a solid at room temperature. It has both yellow and gray forms (allotropes) in the solid state. It burns in an atmosphere of chlorine. It is one of the few substances that expands upon freezing. The gray form melts at 631C. ____ 23. The following statements describe some physical and chemical properties of sucrose (table sugar). Which response includes all that describe chemical properties, and none that describe physical properties? I. It is a colorless solid. II. It chars or blackens when heated gently. III. Its density is 1.6 g/mL. IV. It ignites and burns with a yellow flame when heated strongly. V. It is usually in the form of small crystals although it can occur as a powder. a. b. c. d. e. I, III, and IV II and IV II, IV, and V I and V another combination is the answer ____ 24. a. b. c. d. e. Which of the following is not an intensive property of matter? color density melting point weight boiling point ____ 25. Which response includes all of the following that involve chemical changes, and none that involve physical changes? I. converting milk to cheese II. converting water to steam III. composting leaves IV. burning of gasoline V. melting wax a. b. c. d. e. II and V I, III, and IV I, II, and III IV and V III, IV, and V ____ 26. a. b. c. d. e. Which mixture is incorrectly labeled? homogeneous / sugar dissolved in water homogeneous / sand stirred into water heterogeneous / orange juice with pulp heterogeneous / chocolate chip cookie heterogeneous / concrete sidewalk ____ 27. What is the symbol for the element potassium? a. b. c. d. e. K P Pt W Po ____ 28. a. b. c. d. e. Water is always 11.1% hydrogen and 88.9 % oxygen by mass. This is a statement of the Law of Conservation of Matter. Law of Definite Proportions. Law of Multiple Proportions. Law of Conservation of Matter and Energy. none of these. ____ 29. Below is a list of physical properties and the fundamental unit used in the SI system to measure each. Which unit is not the correct fundamental unit for the property? a. b. c. d. e. physical property / unit length / meter time / second mass / gram temperature / kelvin electric current / ampere ____ 30. Below is a list of common prefixes used in the SI and metric systems. Included with each is an abbreviation and meaning. Which set contains an error? a. mega- M 106 b. decid 101 c. centi- c 102 d. micro- m 106 e. kilok 103 ____ 31. a. b. c. d. e. Which of the following is equivalent to 10 cm? 1m 0.1 dm 100 mm 1000 m 1 mm ____ 32. a. b. c. d. e. Which of the following numbers has 4 significant figures? 0.04309 0.0430 0.0431 0.43980 0.043090 ____ 33. The sum 2.834 + 5.71520 + 2.12 + 178.1 + 250.2619 expressed to the proper number of significant figures is: a. 439 b. 439.0 c. 439.03 d. 439.031 e. 439.0311 ____ 34. Perform the indicated mathematical operations and express the answer in scientific notation rounded off to the proper number of significant figures: (8.001 102) (2.88 103 2.4 103) = a. b. c. d. e. 9.6 102 9.60 108 9.601 108 9.6 108 9.6 102 ____ 35. If 5.76 1013 neon atoms (spherical) were laid in a line, each touching the next, the line would measure 2.54 miles. What is the diameter of a neon atom in Å? (1 Å=1x10 10 m) a. 0.92 Å b. 0.71 Å c. 1.86 Å d. 1.44 Å e. 1.74 Å ____ 36. a. b. c. d. e. ____ 37. At 25C, one milliliter of mercury has a mass of 13.6 grams. How many liters of mercury are required to have a mass of 500 kg of mercury? a. 500 L b. 25.2 L c. 42.1 L d. 13.6 L e. 36.8 L ____ 38. A metal cube having a mass of 112 grams is dropped into a graduated cylinder containing 30.00 mL of water. This causes the water level to rise to 39.50 mL. What is the density of the cube? a. 2.86 g/mL b. 11.8 g/mL c. 10.8 g/mL d. 3.74 g/mL e. 10.6 g/mL ____ 39. a. b. c. d. e. ____ 40. Gallium, a metal, has a freezing point near room temperature so it can be melted by holding it in your hands. If gallium's melting point is 302.8 K, what is that temperature in C? What is the area in square millimeters of a rectangle that is 8.632 cm long and 26.41 mm wide? 2280 mm2 3.060 mm2 22.80 mm2 0.3060 mm2 30.60 mm2 The density of mercury is 13.6 g/cm3. What is the mass of 6.50 cm3 of mercury? 0.478 g 88.4 g 18.9 g 2.38 g 1.10 102 g a. b. c. d. e. 0.0C 575.8C 302.8C 39.8C 29.8C ____ 41. If a sample of butane, C4H10, contains a total of 8.0 103 atoms of carbon, how many molecules of butane are in the sample? a. 6.0 103 b. 3.0 103 c. 8.0 103 d. 1.1 104 e. 2.0 103 ____ 42. Each response below lists an ion by name and by chemical symbol or formula. Also each ion is classified as monatomic or polyatomic and as a cation or anion. Which response contains an error? a. hydroxide / OH / monatomic / anion b. carbonate / CO32 / polyatomic / anion c. ammonium / NH4+ / polyatomic / cation d. magnesium / Mg2+ / monatomic / cation e. sulfite / SO32 / polyatomic / anion ____ 43. a. b. c. d. e. What is the formula for ammonium fluoride? AlF Al2F3 NH3F NH4F2 NH4F ____ 44. a. b. c. d. e. What is the formula for aluminum oxide? Al2O3 Ag2O3 AlO3 AlO AlO2 ____ 45. a. b. c. d. e. Calculate the number of moles of oxygen atoms in 35.2 grams of oxygen. 2.20 moles 4.42 moles 0.54 moles 2.57 moles 1.13 moles ____ 46. a. b. c. d. e. Determine the number of sulfur atoms in 27.1 g of molecular sulfur (S 8). 0.845 5.27 1023 5.09 1023 2.07 1023 0.106 ____ 47. a. b. c. d. e. Calculate the formula weight of NaHSO4. 193 amu 104 amu 120 amu 215 amu 185 amu ____ 48. a. b. c. d. e. What is the mass in grams of 5.00 1012 water molecules? 1.50 1010 g 1.67 1035 g 2.17 1012 g 6.69 109 g 4.61 1013 g ____ 49. a. b. c. d. e. Which of the following has no charge? nucleus neutron proton electron alpha particle ____ 50. In interpreting the results of his "oil drop" experiment in 1909, Robert Millikan was able to determine ____. a. the charge on a proton b. that electrically neutral particles (neutrons) are present in the nuclei of atoms c. that the masses of protons and neutrons are nearly identical d. the charge on an electron e. the extremely dense nature of the nuclei of atoms ____ 51. In the Rutherford gold foil experiment, the fact that most of the alpha particles were not deflected as they passed through the gold foil indicates that a. the nucleus is positively charged. b. the atom is mostly empty space. c. atoms are solid spheres touching each other in the solid state. d. gold is very dense. e. none of these is correct. ____ 52. a. b. c. d. e. ____ 53. The atomic number of an element gives the number of ____ and ____ in the atom while the mass number gives the total number of ____ and ____. a. neutrons; protons; neutrons; electrons b. neutrons; electrons; protons; electrons c. neutrons; electrons; neutrons; protons d. protons; electrons; neutrons; electrons e. protons; electrons; neutrons; protons The number of electrons in a neutral atom of an element is always equal to the ____ of the element. mass number atomic number atomic mass unit isotope number Avogadro's number ____ 54. a. b. c. d. e. Isotopes are atoms of the same element that have different numbers of electrons. have different numbers of protons. have different atomic numbers. have different numbers of neutrons. have different nuclear charges. ____ 55. a. b. c. d. e. Give the number of protons, neutrons, and electrons in an atom of the 90Sr isotope. 38 p; 38 n; 38 e 38 p; 90 n; 38 e 52 p; 38 n; 52 e 38 p; 52 n; 38 e 90 p; 38 n; 90 e Chapter 4 Values The following values may be useful for solving some of the problem(s) below. speed of light = 3.00 108 m/s Planck's constant = 6.63 1034 Js 1 joule = 1 kgm2/s2 1 Ångstrom = 1 1010 m ____ 56. a. b. c. d. e. What is the wavelength of yellow light having a frequency of 5.17 1014 Hz? 3.60 1010 m 1.55 1023 m 6.45 1028 m 5.80 107 m 2.72 106 m ____ 57. a. b. c. d. e. What is the energy, in J/photon, of ultraviolet light with a frequency of 2.70 1016 Hz? 6.00 108 J/photon 8.00 106 J/photon 2.46 1018 J/photon 4.07 1019 J/photon 1.79 1017 J/photon ____ 58. a. b. c. d. e. Calculate the energy (J/photon) of a photon of wavelength 3.65 106 m. 5.45 1020 J 1.82 1028 J 1.22 1014 J 6.05 1037 J none of these ____ 59. a. b. c. d. e. The Rydberg equation is an empirical equation that describes mathematically ____. the lines in the emission spectrum of hydrogen the results of the oil drop experiment the results of the cathode ray experiments the Bohr model of the atom the possible paths of two isotopes of the same element in a mass spectrometer ____ 60. What is the velocity of a neutron of mass 1.67 1027 kg that has a de Broglie wavelength of 2.05 Å? a. b. c. d. e. 19 m/s 1.94 103 m/s 8.13 107 m/s 1.93 104 m/s 5.16 104 m/s ____ 61. a. b. c. d. e. What statement regarding quantum numbers is false? The spin quantum number has values of either +1 or 1. The principle quantum number has only integer values. The angular momentum quantum number also has letter designations. The magnetic quantum number has its values restricted by the l quantum number. The magnetic quantum number is represented by ml. ____ 62. I. II. III. Which response lists all the true statements about the four quantum numbers? n = principal quantum number, n = 1,2,3, . . . l = angular momentum quantum number, l = 0,1,2,3, . . ., (n1) ml = magnetic quantum number, ml = 0, 1, . . ., l IV. ms = spin quantum number, ____ ____ ____ a. b. c. d. e. I, II, and IV I, II, and III I and III II and III II, III, and IV 63. a. b. c. d. e. 8 2 16 18 25 64. a. b. c. d. e. 1 2 0 2 3 The third energy level or shell of an atom can hold a maximum of ____ electrons. Which of the following is not a valid magnetic quantum number for the 3d set of orbitals? 65. What is the value of the angular momentum quantum number, l, for the following orbital? a. b. c. d. e. ms = ± 1 0 1 2 ____ 66. All orbitals of a given degenerate set must be singly occupied before pairing begins in that set is a statement of ____. a. the Heisenberg Uncertainty Principle b. the Bohr Theory c. the Aufbau Principle d. Planck's Theory e. Hund's Rule ____ 67. Which element has the electron configuration below? 1s22s22p63s23p63d104s24p3 a. b. c. d. e. V Ca P As Se ____ 68. a. b. c. d. e. What is the electron configuration of tin, Sn? [Kr]5s23d103f145p4 [Kr]5s23d104d145p4 [Kr]5s23d104f145p2 [Kr]5s24d105p2 [Xe]5s24d105p2 ____ 69. a. b. c. d. e. What is the electron configuration of the iron(III) ion? Fe [Ar]4s23d3 Fe3+[Ar]3d5 Fe2+[Ar]4s23d3 Fe2+[Ar]3d5 Fe3+[Kr]3d5 ____ 3+ Which of the following sets of quantum numbers could represent the highest energy electron in V2+? 70. n l ml ms 4 0 0 4 1 1 3 2 1 3 1 0 + 4 2 1 a. b. c. d. e. ____ 71. a. b. c. d. Which of the following atoms has the greatest number of unpaired electrons in its ground state? Fe N S Ti e. Cu Chemi1100pretest1 Answer Section MULTIPLE CHOICE 1. ANS: 2. ANS: 3. ANS: 4. ANS: 5. ANS: 6. ANS: 7. ANS: 8. ANS: 9. ANS: 10. ANS: 11. ANS: 12. ANS: 13. ANS: 14. ANS: 15. ANS: 16. ANS: 17. ANS: 18. ANS: 19. ANS: 20. ANS: 21. ANS: 22. ANS: 23. ANS: 24. ANS: 25. ANS: 26. ANS: Elements 27. ANS: Elements 28. ANS: Elements 29. ANS: 30. ANS: 31. ANS: 32. ANS: 33. ANS: 34. ANS: 35. ANS: Analysis) 36. ANS: Analysis) E D A B C C E B A B A C D B A A C E B A C C B D B B PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: More About the Periodic Table More About the Periodic Table More About the Periodic Table More About the Periodic Table More About the Periodic Table More About the Periodic Table More About the Periodic Table More About the Periodic Table Atomic Radii Atomic Radii Ionization Energy Electron Affinity Ionic Radii Ionic Radii Ionic Radii Electronegativity Electronegativity Oxygen and the Oxides Oxygen and the Oxides Chemistry – A Molecular View of Matter States of Matter Chemical and Physical Properties Chemical and Physical Properties Chemical and Physical Properties Chemical and Physical Changes Mixtures, Substances, Compounds, and A PTS: 1 TOP: Mixtures, Substances, Compounds, and B PTS: 1 TOP: Mixtures, Substances, Compounds, and C D C A B D B PTS: PTS: PTS: PTS: PTS: PTS: PTS: 1 1 1 1 1 1 1 TOP: TOP: TOP: TOP: TOP: TOP: TOP: Measurements in Chemistry Measurements in Chemistry Measurements in Chemistry Use of Numbers Use of Numbers Use of Numbers The Unit Factor Method (Dimensional A PTS: 1 TOP: The Unit Factor Method (Dimensional 37. ANS: Analysis) 38. ANS: 39. ANS: 40. ANS: 41. ANS: 42. ANS: 43. ANS: Compounds 44. ANS: Compounds 45. ANS: 46. ANS: 47. ANS: Moles 48. ANS: Moles 49. ANS: 50. ANS: 51. ANS: 52. ANS: 53. ANS: 54. ANS: 55. ANS: 56. ANS: 57. ANS: 58. ANS: 59. ANS: 60. ANS: 61. ANS: Atom 62. ANS: 63. ANS: 64. ANS: 65. ANS: 66. ANS: 67. ANS: 68. ANS: 69. ANS: 70. ANS: 71. ANS: E PTS: 1 TOP: The Unit Factor Method (Dimensional B B E E A E PTS: PTS: PTS: PTS: PTS: PTS: 1 1 1 1 1 1 TOP: TOP: TOP: TOP: TOP: TOP: Density and Specific Gravity Density and Specific Gravity Heat and Temperature Chemical Formulas Ions and Ionic Compounds Names and Formulas of Some Ionic A PTS: 1 TOP: Names and Formulas of Some Ionic A C C PTS: PTS: PTS: 1 1 1 TOP: TOP: TOP: The Mole The Mole Formula Weights, Molecular Weights, and A PTS: 1 TOP: Formula Weights, Molecular Weights, and B D B B E D D D E A A B A PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: 1 1 1 1 1 1 1 1 1 1 1 1 1 TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: Fundamental Particles The Discovery of Electrons Rutherford and the Nuclear Atom Atomic Number Mass Number and Isotopes Mass Number and Isotopes Mass Number and Isotopes Electromagnetic Radiation Electromagnetic Radiation Electromagnetic Radiation Atomic Spectra and the Bohr Atom The Wave Nature of the Electron The Quantum Mechanical Picture of the A D E D E D D B C A PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: 1 1 1 1 1 1 1 1 1 1 TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: Quantum Numbers Atomic Orbitals Atomic Orbitals Atomic Orbitals Electron Configurations Electron Configurations Electron Configurations Electron Configurations Electron Configurations Paramagnetism and Diamagnetism