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Interim Exam - Review 1. A sample of a substance is heated strongly in a crucible and the sample increases in mass. This is evidence that the substance has 1. 2. 3. 4. 5. melted. sublimed. evolved a gas. expanded undergone a chemical change. 8. A pure substance that contains more than one type of atom is called a(n) 1. allotrope. 3. element. 5. isomer. 9. In a chemical change, the total mass of the product(s) is 1. 2. 3. 4. 5. 2. A chemical property of sulfur is that it is 1. solid. 3. odorless. 5. brittle. 2. yellow. 4. combustible. 1. has been known for many centuries. 2. combines with oxygen to form a gas. 3. cannot be chemically decomposed into two or more substances. 4. is formed when wood is heated without the presence of air. 5. can be found in many pure forms. 4. An element is identified most accurately by its 1. element 3. compound 5. none of the above 1. any proportion 3. definite proportions 5. one proportion only 2. Cu2+ 3. Cu(II) 1. filtration 3. boiling 5. decomposition 4. Cu(aq) 5. CuO 2. baking a cake. 4. breaking glass. 1. 2. 3. 4. 5. a change in color. a change of state. a change in density. a change in the number of atoms. the formation of a new pure substance. H-Chem 2015-16 2. chlorination 4. distillation 14. Ernest Rutherford concluded from experiments that they indicated nuclei of atoms are relatively 7. A chemical change involves 1. 2. 3. 4. 5. soluble in water different in properties the same size as every other particle the same in properties as every other particle the same phase as every other particle 13. Sea water is made salt–free by 6. An example of a chemical change is 1. grinding rock. 3. heating water. 5. melting ice. 2. equal proportions 4. constant proportions 12. A substance is considered to be homogeneous if every particle is 1. 2. 3. 4. 5. 5. Which of the following notations correctly indicates that the substance copper is in the solid state? 2. solution 4. pure substance 11. A mixture consists of two or more components in mass and color volume and odor color and conductivity density and color density and conductivity 1. Cu(s) less than that of the reactants. a function of the rate of reaction. the same as that of the reactants. more than that of the reactants. less if a catalyst is present. 10. A homogeneous mixture is a(n) 3. Carbon is classified as an element rather than as a compound because it 1. 2. 3. 4. 5. 2. compound. 4. solution. Page 1 far apart and positively charged far apart and negatively charged close together and positively charged close together and negatively charged close together and neutral Dr. Powell 15. The nucleus of an atom 1. 2. 3. 4. 5. 20. The number of neutrons in one atom of an element is is electrically neutral is the densest portion of the atom occupies most of the atom’s volume is a low fraction of the atom’s mass is large compared to the size of the atom 1. 2. 3. 4. 5. the same in each isotope the same as the atomic number equal to the number of protons in the nucleus equal to the mass number minus the atomic number equal to the number of electrons minus the number of protons 21. Naturally occurring gallium is 60% 69Ga and 40% 71Ga by mass. Based on this data the atomic mass of this element is 1. 39.0 1. A 3. C 5. None of the above 2. B 4. D 1. 1.0 1. 2. 3. 4. 5. the mass of the electron the existence of the neutron that the electron carries a negative charge that the atom has a concentrated central mass that the atom has very little open space 92U 1. 2. 3. 4. 5. ® 14156Ba + 9236Kr + 310n what is the mass number of uranium, U? 1. 92 2. 143 3. 233 4. 235 19 protons, 20 neutrons, 20 electrons 19 protons, 20 neutrons, 18 electrons 20 protons, 19 neutrons, 19 electrons 39 protons, 39 neutrons, 39 electrons 19 protons, 39 neutrons, 18 electrons H-Chem 2015-16 2. 2.0 3. 3.0 4. 4.0 5. 6.0 protons neutrons neutrons and protons valence electrons and protons kernel electrons 9 protons, 19 neutrons, 9 electrons 9 protons, 9 neutrons, 19 electrons 19 protons, 19 neutrons, 9 electrons 19 protons, 19 neutrons, 10 electrons 9 protons, 10 neutrons, 9 electrons 25. An element with an atomic number of 12 and a mass number of 25 contains 5. 236 1. 2. 3. 4. 5. 19. How many protons, neutrons, and electrons are there in potassium ions, 3919K+? 1. 2. 3. 4. 5. 5. 71.0 24. An atom of fluorine, 199F, contains 18. In the fission reaction, + 4. 70.0 23. The atomic mass of an element is closely related to the number of its 17. Rutherford's alpha–particle bombardment of gold foil helped develop our current model of the atom by determining 10n 3. 69.8 22. If a new standard for relative atomic masses were chosen in which the most common atom of oxygen, “O”, had a mass of 48 the relative atomic mass of hydrogen as compared to the current stadard would be 16. Which is true? 1. 2. 3. 4. 5. 2. 69.0 12 protons, 13 neutrons, 12 electrons 12 protons, 13 neutrons, 13 electrons 13 protons, 12 neutrons, 13 electrons 13 protons, 13 neutrons, 13 electrons 13 protons, 12 neutrons, 12 electrons 26. The atomic mass unit is defined as 1. 2. 3. 4. 5. Page 2 the mass of a carbon atom. 1/12 of the mass of the carbon atom. 12 g. one microgram. the mass of a hydrogen atom. Dr. Powell 27. An ion containing 11 protons, 12 neutrons, and 10 electrons has approximately the same mass as 1. 13 protons 3. 22 neutrons 5. 33 protons 33. Which statement is true? All isotopes of the same element have 2. 21 protons 4. 23 neutrons 1. 2. 3. 4. 5. 28. Atoms of an element all have the same number of 1. 2. 3. 4. 5. protons neutrons nuclear particles neutrons plus protons total subatomic particles 34. Boron has two common isotopes, 105B and 115B. The relative atomic mass of boron is 10.8. The percent 105B in an average sample of boron is 1. 20% 35. The atom 29. Which property of the elements always increases with increasing atomic number? 1. 2. 3. 4. 5. 1. Atomic diameter Electronegativity Number of valence electrons Nuclear charge Number of protons 1. 3. 5. 2. 3. 50% 4. 67% 5. 80% is an isotope of 3014Si 3. 2716S 4. 6530Zn 5. 45Rh 2814X, 2815X, 2816X 2. 4. 126X, 168X, 2010X 11X, 21X, 31X 3818X, 3919X, 4020X 128X, 164X, 200X 37. Deuterium, 21D, is an isotope of 1. the same element can have a different number of neutrons 2. the same element can have a different mass number 3. different elements can have the same number of electrons 4. different elements can have a different number of protons 5. different elements can have the same number of neutrons 1. lithium 3. dubnium 5. hydrogen 1. Chlorine nuclei are smaller than chlorine atoms 2. All chlorine atoms have the same nuclear charge 3. Some naturally occurring chlorine nuclei have 19 protons 4. Some naturally occurring chlorine nuclei have 20 neutrons 5. All chlorine atoms have the same number of protons 2. helium 4. oxygen 38. The symbol 1. 2. 3. 4. 5. 31. Which is false concerning nuclei of chlorine? indicates this isotope consists of A B C D None of the above correctly represent this isotope. 39. The number of neutrons in an atom of 1. 2. 3. 4. 5. 32. Which particle consists of 13 protons, 14 neutrons, and 10 electrons? 2. Silicon atom 4. Phosphide ion 94Be is 4 5 9 13 The number of neutrons cannot be determined from the information given. 40. The chlorine atom, 3517Cl, has the same number of neutrons as 1. H-Chem 2015-16 2715P 2. 40% 3015X 36. Which set represents isotopes of the same element? 30. Which is of these statements is false? Neutral atoms of 1. Cobalt atom 3. Aluminum ion 5. Nitrogen isotope the same number of neutrons the same number of protons different numbers of electrons the same mass the same nuclear structure Page 3 3516S 2. 3717Cl 3. 3618Ar 4. 4020Ca 5. 189F Dr. Powell 41. Which of the following statements about the elements 24 11X and 2512Y is correct? 1. 2. 3. 4. 5. 48. Experimental evidence indicates that the nucleus of an atom They are isotopes of the same element They are non–metals They are members of the same chemical family They have the same number of neutrons per atom The have the same electron configuration 1. 2. 3. 4. 5. 42. If Z represents the atomic number of an element and A represents its mass number, then the number of neutrons in one atom of the element is 1. A 2. A + Z 3. A – Z 4. Z – A 5. Z 49. How many nucleons does 2512Mg contain? 1. 12 2. 32 3. 39 4. 57 21H 5. 82 1. They are positive subatomic particles and are found in the nucleus. 2. They are positive subatomic particles and are found surrounding the nucleus. 3. They are negative subatomic particles and are found in the nucleus. 4. They are negative subatomic particles and are found surrounding the nucleus. 5. They are negative subatomic particles and are equally distributed throughout the atom 24595Am 1. + ? ® 24597Bk + 4 10n 42He 2. 2 11H 3. 4 11H 4. 4 0-1e 5. 2 42He 52. Radioactive plutonium, 21484Pu, emits an alpha particle and changes to a new element, “X”. This new element emits a beta particle and is converted to element, “Y”. Which are representations of elements X and Y? 1. 3. 5. 21082X and 21083Y and 21181Y 21083X and 21184Y 2. 4. 21280X 21282X 21080X and 21081Y and 21081Y 53. Bismuth, 83Bi, emits a beta particle. Which is correct? I. Lead, 82Pb, is formed. II. Polonium, 84Po, is formed. III. The mass number increases. IV. The mass number decreases. 1. charge of +1 and mass of 1 amu 2. charge of +1 and mass of amu 1. I only 3. I and IV 5. II and IV only 3. charge of –1 and mass of 1 amu 4. charge of –1 and mass of amu 2. II only 4. II and III only 54. What is “X” in the equation? 21083Bi ® "X" + 0–1e 1. H-Chem 2015-16 2. proton 4. electron Which is necessary to complete the equation? 47. What is the charge and mass of a proton? 5. neutral charge and mass of 1 amu 5. 49 51. Consider the nuclear reaction 45. Which statement best describes electrons? 1. 1 2. 11 3. 12 4. 23 5. It is impossible to tell 4. 37 + 31H ®42He + X 1. triton 3. neutron 5. deuteron 2. isotope 4. nucleon 46. A neutral atom contains 12 neutrons and 11 electrons. The number of protons in this atom is 3. 25 the missing particle, X, is probably a(n) 44. Which is a synonym for the term “nuclide”? 1. ion 3. electron 5. neutrino 2. 13 50. Consider the nuclear equation below: 43. How many neutrons are in a 5725Mn7+ ion? 1. 25 contains most of the mass of the atom contains a small percentage of the mass of the atom has no charge has a negative charge contains most of the volume of the atom Page 4 20983Bi 2. 21082Pb 3. 21084Po 4. 21183Bi 5. 20982Pb Dr. Powell 55. The equation, E = mc2, computes the quantity of energy 1. 2. 3. 4. 5. required to start a nuclear reaction generated during a nuclear reaction necessary to moderate a nuclear reactor evolved during radioisotope production stored in electromagnetic radiation has a half-life of 8 hours. Starting with 1.00 gram of the isotope, how much would remain at the end of 24 hours? 2. 0.333 gram 4. 0.125 gram 61. Which statements are correct? I The emission of a beta–particle reduces the ratio of neutrons to protons in the nucleus. II That the 168O isotope is stable is a reasonable prediction. III Radioactive tracers can be used to determine reaction mechanisms. IV 90Sr (t½ = 28 y) is more stable than 60Co (t ½ = 5.3 y). man–made radioactive products of nuclear fission found in naturally occurring uranium nonmetals 57. A radioactive isotope contains nuclei which 1. 2. 3. 4. 5. 21082Pb 1. 0.500 gram 3. .250 gram 5. 0.000 gram 56. All of the elements in the seventh row of the Periodic Table are 1. 2. 3. 4. 5. 60. 1. II 3. II and IV 5. All are correct have unpredictable properties give off radio waves when heated undergo change only when energy is absorbed spontaneously change, liberating energy are completely stable 2. I and II 4. II, III and IV 62. A sample of an ore contains 100. milligrams of radioactive phosphorus–32 with a half-life of 14.3 days. How many milligrams of 32P remain in the sample after 28.6 days? The symbol for the milligram is mg. 58. The diagram below represents radioactive emanations passing through an electric field. 1. 0.00 mg 3. 50.0 mg 5. 200 mg 2. 25.0 mg 4. 75.0 mg 63. How long will it take a sample of 6.000 × 1020 atoms of 42K, with a half life of 12.4 h, to decrease to 1.875 × 1019 atoms ? 1. 0.3875 h 3. 12.4 h 5. 397 h Which type of emanation is represented by the arrow labeled 1? 1. alpha particle 3. positron 5. neutron 2. beta particle 4. gamma ray 64. The activity of a sample of La–140 goes from 640. cpm to 40.0 cpm in 160. hours. What is its half-life? 1. 2560. h 3. 160. h 5. 10.0 h 59. In which list can all particles be accelerated by an electric field? 1. 2. 3. 4. 5. alpha particles, beta particles, and neutrons alpha particles, beta particles, and protons alpha particles, protons, and neutrons beta particles, protons, and neutrons neutrons, beta particles, and positrons H-Chem 2015-16 2. 2.48 h 4. 62.0 h 2. 640. h 4. 40.0 h 65. Mendeleevium–256 emits at a rate of 100. dps after 2.00 hours of experimenting. If the half–life is 30.0 minutes, what was the original count rate in dps? 1. 100. 3. 1500. 5. 3.28 x 106 Page 5 2. 400. 4. 1,600. Dr. Powell 66. A nuclear reaction occurs, and the reactants have more mass than the products. This mass difference represents 1. 2. 3. 4. 5. 73. Given the reaction: 94Be the energy lost to heat and sound the energy used to bind the nucleons the uncertain mass of the neutrino the kinetic energy of the final products the potential energy of the electrostatic force 1. 2. 3. 4. breaking the bonds in the original molecules forming new bonds the mass defect the high energy of large molecules with which fusion usually occurs 5. the drop of energy level of the electrons in the atoms involved 68. An increase in the average kinetic energy of a sample of copper atoms occurs with an increase in 1. 2. 3. 4. 5. 75. I. An atom of 2311Na has 12 neutrons 2. temperature 4. volume BECAUSE II. the number of neutrons is the difference between the mass number and the atomic number. 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I 2. 10°C to 1°C 4. 60°C to 50°C 2. gas 4. vapor 76. I. An atom of 23Na has 23 electrons BECAUSE 71. Which equation represents sublimation? 1. I2(s) ® I2(g) 3. CO2(l) ® CO2(g) 5. O2(g) ® O2(s) II. the number of protons equals the number of electrons in a neutral atom. 2. NH3(g) ® NH3(l) 4. H2O(s) ® H2O(l) 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I 72. A phase change from the solid directly to the gaseous state is called 1. fusion 3. sublimation 5. deposition H-Chem 2015-16 natural transmutation artificial transmutation fission fusion oxidation-reduction 1. 23892U ® 23490Th + 42He 2. 23490Th ® 23491Pa + 0–1e 3. 21884Po ® 21482Pb + 42He 4. 94Be + 42He ® 126C + 10n 5. none of the above 70. The state of matter which exhibits definite volume but not a definite shape is 1. liquid 3. solid 5. aqueous + 42He 74. Which equation represents artificial transmutation? 69. Which change in the temperature of a 1-gram sample of water would cause the greatest increase in the average kinetic energy of its molecules? 1. 1°C to 10°C 3. 50°C to 60°C 5. 500°C to 501°C 63Li Which type of reaction is represented? 67. Fusion reactions release energy due to 1. concentration 3. pressure 5. density + 11H 2. boiling 4. chemical change Page 6 Dr. Powell 77. I. A sodium atom becomes a positive ion when it loses an electron 80. I. Chemical properties are more similar for sodium and magnesium than for sodium and lithium BECAUSE BECAUSE II. electrons have a positive charge. II. sodium and magnesium are in the same period. 1. 2. 3. 4. 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I 81. I. Cl– is a negatively charged ion 78. I. Potassium and carbon exhibit similar properties BECAUSE BECAUSE II. they are in the same period. II. it has gained an electron and has more electrons than protons. 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I 79. I. Isotopes of different elements can have the same mass number 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I 82. I. Na+ is a positively charged ion BECAUSE BECAUSE II. they can have the same number of neutrons. II. it has less electrons than protons. 1. 2. 3. 4. 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I H-Chem 2015-16 Page 7 I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I Dr. Powell 83. I. An element with an atomic number of “A” and a mass number of “Z” has A number of neutrons 86. I. Sodium is a metal BECAUSE BECAUSE II. sodium is a solid at room temperature. II. all elements have the same number of neutrons as protons. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I 1. 2. 3. 4. 87. I. When I2(s) is heated a purple gas is formed 84. I. Most of the alpha particles in Rutherford’s gold foil experiment were deflected BECAUSE II. solid iodine sublimes at standard pressure. BECAUSE 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I II. the nucleus makes up most of the mass of an atom. 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I 88. I. Beta particles are affected by an electric field BECAUSE 85. I. The atomic mass of chlorine is 35.45 II. beta particles are high energy electrons. BECAUSE II. the most abundant isotope of chlorine has 17 protons. 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I H-Chem 2015-16 Page 8 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I Dr. Powell 89. I. In the detonation of a nuclear weapon, a small amount of mass is gained BECAUSE 92. What would the correct equation for determining percent error be in a theoretical experiment where the experimental value is determined as J and the accepted value is J? 1. II. the mass defect is regained according to the formula E=mc2. 2. 1. 2. 3. 4. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I 90. I. In order to mix an acid with water, one should quickly pour the water into the acid 3. 4. 5. none of the above 93. Test tubes containing nonflammable fluids being heated should be pointed at the nearest 1. sink 3. floor 5. desktop BECAUSE II. pouring the acid into the water is too dangerous, since it increases one’s chances of spilling acid. I is TRUE, II is FALSE I is FALSE, II is TRUE I and II are BOTH FALSE I and II are BOTH TRUE but II IS NOT a correct explanation of I 5. I and II are BOTH TRUE and II IS a correct explanation of I 94. Which device is preferred to remove a spill of a large quantity of a caustic chemical from clothing? 1. 2. 3. 4. 5. 1. 2. 3. 4. a fire blanket a safety shower an eye-wash facility an approved fire extinguisher an externally-vented fume hood 95. In the laboratory, never dip a stirring rod into a reagent bottle because 1. 2. 3. 4. the bottle may tip the rod might break the rod may puncture the bottle the contents of the bottle may become contaminated 5. the amount of liquid remaining on the rod is too small to be used 91. Through experimentation, a student determined the vapor pressure of water at 60°C to be 140.2 torr. If the actual vapor pressure of water at 60°C is 149.4 torr, what is the student's percent error? 1. .0616% 3. 6.16% 5. 6.56% 2. wall 4. ceiling 2. .0656% 4. –6.16% 96. Two samples are massed using different balances. What is the total mass of the samples to the correct number of significant digits? 1. 3. 5. H-Chem 2015-16 Page 9 2. 4. Dr. Powell 97. How many 100 mg tetracycline capsules can be made from 1 kg of tetracycline? 1. 10 3. 1,000 5. 100,000 99. Which is the proper reading for the buret? 2. 100 4. 10,000 98. An unknown mass of an element reacts completely with 1.811 g of sulfur and 3.613 g of oxygen to produce 7.124 g of a compound containing the element, S, and O. What additional information is required to determine the unknown mass? 1. 2. 3. 4. 5. The formula of the product. The balanced reaction equation. The molar mass of the unknown element. The electron configuration of the unknown element. No additional information is needed. 1. 21.55 mL 3. 22.3 mL 5. 22.60 mL 2. 21.7 mL 4. 22.45 mL 100. Which should be used to accurately measure 185 mL of an aqueous solution? A 250 mL 1. beaker 3. volumetric flask 5. pipet 2. Florence flask 4. graduated cylinder 101. Which apparatus delivers 50.00 mL of liquid most accurately? 1. 2. 3. 4. 5. H-Chem 2015-16 Page 10 50 mL buret 50 mL beaker 50 mL test tube 50 mL graduated cylinder 50 mL flask Dr. Powell