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Home , Isotopes of lithium, Period 4 element

NAME MIDTERM REVIEW

1. During a laboratory activity, a student combined two solutions. In the laboratory report, the student wrote “A yellow color appeared.” The statement represents the student’s recorded A) conclusion B) observation C) hypothesis D) inference 2. Which of the following statements contained in a student's laboratory report is a conclusion? A) A gas is evolved. B) The gas is insoluble in water. C) The gas is . D) The gas burns in air. 3. The diagram below represents a portion of a 100-milliliter graduated cylinder.

What is the reading of the meniscus? A) 35.0 mL B) 36.0 mL C) 44.0 mL D) 45.0 mL 4. An aluminum sample has a mass of 80.01 g and a of 2.70 g/cm3. According to the data, to what number of significant figures should the calculated volume of the aluminum sample be expressed? A) 1 B) 2 C) 3 D) 4 5. A student in a laboratory determined the boiling point of a substance to be 71.8°C. The accepted value for the boiling point of this substance is 70.2°C. What is the percent error of the student's measurement? A) 1.60% B) 2.28% C) 2.23% D) 160.% MIDTERM REVIEW

6. Base your answer to the following question on the information below.

A method used by ancient Egyptians to obtain from copper(I) sulfide ore was heating the ore in the presence of air. Later, copper was mixed with to produce a useful alloy called bronze. Calculate the density of a -gram sample of bronze that has a volume of cubic centimeters. Your response must include a correct numerical setup and the calculated result.

7. Compared to the charge of a , the charge of an 14. As a result of the foil experiment, it was concluded has that an A) a greater magnitude and the same sign A) contains , , and B) a greater magnitude and the opposite sign B) contains a small, dense nucleus C) the same magnitude and the same sign C) has positrons and orbitals D) the same magnitude and the opposite sign D) is a hard, indivisible sphere 8. Which particle has no charge? 15. The gold foil experiment led to the conclusion that each atom in the foil was composed mostly of empty space A) electron B) because most alpha particles directed at the foil C) positron D) proton A) passed through the foil 9. What is the overall charge of an ion that has 12 protons, 10 electrons, and 14 neutrons? B) remained trapped in the foil C) were deflected by the nuclei in gold A) 2– B) 2+ C) 4– D) 4+ D) were deflected by the electrons in gold atoms 10. Which particles have approximately the same mass? 16. All atoms have the same A) an electron and an A) B) an electron and a proton B) mass number C) a neutron and an alpha particle C) number of neutrons plus the number of electrons D) a neutron and a proton D) number of neutrons plus the number of protons 11. Which phrase describes an atom? 17. Which represents the electrons in A) a negatively charged nucleus surrounded by an atom of Ga in an excited state? positively charged protons A) 2-8-17-3 B) 2-8-17-4 B) a negatively charged nucleus surrounded by C) 2-8-18-3 D) 2-8-18-4 positively charged electrons C) a positively charged nucleus surrounded by 18. Which quantity represents the number of protons in an negatively charged protons atom? D) a positively charged nucleus surrounded by A) atomic number negatively charged electrons B) oxidation number 12. An ion that consists of 7 protons, 6 neutrons, and 10 C) number of neutrons electrons has a net charge of D) number of electrons A) 4– B) 3– C) 3+ D) 4+ 19. What is the charge of the nucleus of an atom? 13. Which subatomic particles are located in the nucleus of A) 0 B) –2 C) +8 D) +16 a atom? 20. The notation for the nuclide 13755Cs gives information A) protons, only about B) neutrons, only A) mass number, only C) protons and neutrons B) atomic number, only D) protons and electron C) both mass number and atomic number D) neither mass number nor atomic number MIDTERM REVIEW

21. An atom of any element must contain 29. The nucleus of an atom of -58 contains A) an equal number of protons and neutrons A) 27 protons and 31 neutrons B) an equal number of protons and electrons B) 27 protons and 32 neutrons C) more electrons than neutrons C) 59 protons and 60 neutrons D) more electrons than protons D) 60 protons and 60 neutrons 22. In an atom of -40, the number of protons 30. -37 can be represented as

A) equals the number of electrons A) 1735Cl B) 2037Cl C) 3520Cl D) 3717Cl B) equals the number of neutrons 31. The atomic masses and the natural abundances of the C) is less than the number of electrons two naturally occurring of are shown D) is greater than the number of electrons in the table below. 23. An atom contains 22 neutrons and 40 . What is the total number of protons in the atom? A) 18 B) 22 C) 40 D) 62 24. Which quantity can vary among atoms of the same element? A) mass number B) atomic number C) number of protons D) numbers of electrons Which numerical setup can be used to determine the 25. What is the mass number of a carbon atom that contains of lithium? six protons, eight neutrons, and six electrons? A) (0.075)(6.02 u) + (0.925)(7.02 u) A) 6 B) 8 C) 14 D) 20 B) (0.925)(6.02 u) + (0.075)(7.02 u) 26. In which list are the elements arranged in order of C) (7.5)(6.02 u) + (92.5)(7.02 u) increasing atomic mass? D) (92.5)(6.02 u) + (7.5)(7.02 u) A) Cl, K, Ar B) Fe, Co, Ni 32. The atomic mass of an element is the weighted average C) Te, I, Xe D) Ne, F, Na of the 27. The table below shows the number of subatomic A) number of protons in the isotopes of that element particles in atom X and in atom Z. B) number of neutrons in the isotopes of that element C) atomic numbers of the naturally occurring isotopes of that element D) atomic masses of the naturally occurring isotopes of that element 33. Element X has two isotopes. If 72.0% of the element has an isotopic mass of 84.9 atomic mass units, and 28.0% of the element has an isotopic mass of 87.0 atomic mass units, the average atomic mass of element Atom X and atom Z are isotopes of the element X is numerically equal to A) aluminum B) carbon A) C) D) B) 28. Atoms of different isotopes of the same element differ C) in their total number of D) A) electrons B) neutrons C) protons D) valence electrons MIDTERM REVIEW

34. An orbital is defined as a region of the most probable 42. In the wave-mechanical model of the atom, orbitals are location of regions of the most probable locations of A) an electron B) a neutron A) protons B) positrons C) a nucleus D) a proton C) neutrons D) electrons 35. What is the total number of valence electrons in an 43. Which of atomic models is listed in historical atom of in the ground state? order from the earliest to the most recent? A) 8 B) 2 C) 14 D) 4 A) hard-sphere model, wave-mechanical model, 36. Compared to an electron in the first of an electron-shell model atom, an electron in the third shell of the same atom has B) hard-sphere model, electron-shell model, wave-mechanical model A) less mass B) less energy C) electron-shell model, wave-mechanical model, C) more mass D) more energy hard-sphere model 37. What is the electron configuration of a atom in D) electron-shell model, hard-sphere model, the ground state? wave-mechanical model A) 2–4 B) 2–6 C) 2–8–4 D) 2–8–6 38. How many electrons are in the outermost principal (shell) of an atom of carbon in the ground state? A) 6 B) 2 C) 3 D) 4 39. Which electron configuration represents an atom in an excited state? A) 2–7 B) 2–6–2 C) 2–8–1 D) 2–8–8–2 40. As an electron in an atom moves from the ground state to the excited state, the electron A) gains energy as it moves to a higher energy level B) gains energy as it moves to a lower energy level C) loses energy as it moves to a higher energy level D) loses energy as it moves to a lower energy level 41. During a flame test, ions of a specific metal are heated in the flame of a gas burner. A characteristic color of light is emitted by these ions in the flame when the electrons A) gain energy as they return to lower energy levels B) gain energy as they move to higher energy levels C) emit energy as they return to lower energy levels D) emit energy as they move to higher energy levels MIDTERM REVIEW

Base your answers to questions 44 and 45 on the information and the bright-line spectra represented below.

Many advertising signs depend on the production of light emissions from gas-filled glass tubes that are subjected to a high-voltage source. When light emissions are passed through a spectroscope, bright-line spectra are produced.

44. Identify the two gases in the unknown mixture.

45. Explain the production of an emission spectrum in terms of the energy states of an electron.

46. Draw the electron-dot (Lewis) structure of an atom of 50. Which two characteristics are associated with ? chlorine. A) low first ionization energy and low

B) low first ionization energy and high electronegativity C) high first ionization energy and low electronegativity D) high first ionization energy and high 47. The elements on the are arranged in electronegativity order of increasing 51. What is a property of most metals? A) atomic number B) mass number A) They tend to gain electrons easily when bonding. C) number of isotopes D) number of moles B) They tend to lose electrons easily when 48. Which two elements have the most similar chemical bonding. properties? C) They are poor conductors of heat. A) Be and Mg B) Ca and Br D) They are poor conductors of electricity. C) Cl and Ar D) Na and P 52. The element in 4 and Group 1 of the Periodic 49. A solid element that is malleable, a good conductor of Table would be classified as a electricity, and reacts with oxygen is classified as a A) metal B) A) metal B) metalloid C) D) C) noble gas D) nonmetal MIDTERM REVIEW

53. In which section of the Periodic Table are the most active metals located? A) upper right corner B) lower right corner C) upper left corner D) lower left corner 54. The element sulfur is classified as a A) metal B) metalloid C) nonmetal D) noble gas 55. Which element has chemical properties that are most similar to the chemical properties of ? A) B) chlorine C) D) oxygen 56. What are two properties of most ? A) high ionization energy and poor electrical conductivity B) high ionization energy and good electrical conductivity C) low ionization energy and poor electrical conductivity D) low ionization energy and good electrical conductivity 57. Which property is characteristic of nonmetals? A) They have a high electronegativity. B) They lose electrons easily. C) They have a low first ionization energy. D) They are good conductors of electricity. 58. The table below shows some properties of elements A, B, C, and D.

Which element is most likely a nonmetal? A) A B) B C) C D) D MIDTERM REVIEW

59. Which statement explains why neon is a Group 18 67. What is the total number of valence electrons in a element? atom in the ground state? A) Neon is a gas at STP. A) 8 B) 2 C) 18 D) 20 B) Neon has a low . 68. Which symbol represents a particle with a total of 10 C) Neon atoms have a stable electrons? configuration. 3+ 3+ D) Neon atoms have two electrons in the first shell. A) N B) N C) Al D) Al 60. An atom of argon in the ground state tends not to bond 69. The atoms of the elements in Group 2 have the same with an atom of a different element because the argon A) mass number atom has B) atomic number A) more protons than neutrons C) number of protons B) more neutrons than protons D) number of valence electrons C) a total of two valence electrons 70. What is the net charge of an ion that has 8 protons, 9 D) a total of eight valence electrons neutrons, and 10 electrons? 61. Which element is a noble gas? A) 1+ B) 2+ C) 1- D) 2- A) B) chlorine 71. When an atom of lithium loses an electron, the atom C) D) becomes a 62. Which group on the Periodic Table has elements with A) negative ion with a radius smaller than the radius atoms that tend not to bond with atoms of other of the atom elements? B) negative ion with a radius larger than the radius of A) Group 1 B) Group 2 the atom C) Group 17 D) Group 18 C) positive ion with a radius smaller than the radius of the atom 63. Which list of elements consists of , only? D) positive ion with a radius larger than the radius of A) B, Al, Ga B) C, N, P the atom C) O, S, Se D) Si, Ge, As 72. Compared to a phosphorus atom, a P3– ion has 64. Pure is chemically classified as a metalloid A) more electrons and a larger radius because silicon B) more electrons and a smaller radius A) is malleable and ductile C) fewer electrons and a larger radius B) is an excellent conductor of heat and electricity D) fewer electrons and a smaller radius C) exhibits metallic and nonmetallic properties 73. What is the total number of electrons in a S2– ion? D) none of the above A) 10 B) 14 C) 16 D) 18 65. Which element has the greatest density at STP? 74. An atom of which element has the largest atomic A) calcium B) carbon radius? C) chlorine D) copper A) Fe B) Mg C) Si D) Zn 66. Which Lewis electron-dot diagram represents a 75. As atomic number increases within Group 15 on the nitrogen atom in the ground state? Periodic Table, A) B) A) decreases, only C) D) B) increases, only C) decreases, then increases D) increases, then decreases MIDTERM REVIEW

76. Which statement describes the general trends in 83. Given four particle models: electronegativity and first ionization energy as the elements in Period 3 are considered in order from Na to Cl? A) Electronegativity increases, and first ionization energy decreases. B) Electronegativity decreases, and first ionization energy increases. C) Electronegativity and first ionization energy both increase. D) Electronegativity and first ionization energy both decrease. 77. Which general trend is demonstrated by the Group 17 Which two models can be classified as elements? elements as they are considered in order from top to A) I and II B) I and IV bottom on the Periodic Table? C) II and III D) II and IV A) a decrease in atomic radius 84. A substance is classified as either an element or a B) a decrease in electronegativity C) an increase in first ionization energy A) compound D) an increase in nonmetallic behavior B) solution C) heterogeneous mixture 78. Based on Reference Table S, atoms of which of these D) homogeneous mixture elements have the strongest attraction for the electrons in a chemical bond? 85. Matter is classified as a A) Al B) Si C) P D) S A) substance, only 79. Which atom in the ground state requires the least B) substance or as a mixture of substances amount of energy to remove its valence electron? C) homogenous mixture, only D) homogenous mixture or as a heterogeneous A) lithium atom B) atom mixture C) atom D) atom 86. Which type of matter is composed of two or more 80. The amount of energy required to remove the outermost elements that are chemically combined in a fixed electron from a gaseous atom in the ground state is proportion? known as A) solution A) first ionization energy B) compound B) activation energy C) homogeneous mixture C) conductivity D) heterogeneous mixture D) electronegativity 87. Which substance can not be decomposed by a chemical 81. Which has the most metallic change? properties? A) AlCl3 B) H2O C) HI D) Cu A) As B) Br C) Ge D) Sc 88. Which substance represents a compound? 82. In which group of the Periodic Table do most of the elements exhibit both positive and negative oxidation A) C(s) B) Co(s) states? C) CO(g) D) O2(g) A) 17 B) 2 C) 12 D) 7 89. Which substance can be decomposed by a chemical change? A) Co B) CO C) Cr D) Cu MIDTERM REVIEW

90. What is the chemical formula for (III) oxide? 99. The bonds in BaO are best described as

A) FeO B) Fe2O3 A) covalent, because valence electrons are shared C) Fe3O D) Fe3O2 B) covalent, because valence electrons are transferred 91. What is the total number of different elements present C) ionic, because valence electrons are shared in ? D) ionic, because valence electrons are transferred A) 7 B) 9 C) 3 D) 4 92. What is the IUPAC name for the compound ZnO? A) oxide B) zinc oxalate C) zinc peroxide D) zinc hydroxide 93. Which is a binary compound?

A) CaCl2 B) KOH C) NaNO3 D) MgSO4

94. The correct name for the compound NaClO3 is sodium A) chloride B) chlorate C) perchlorate D) chlorite 95. Given the balanced equation representing a reaction: Cl2 Cl + Cl What occurs during this reaction? A) A bond is broken as energy is absorbed. B) A bond is broken as energy is released. C) A bond is formed as energy is absorbed. D) A bond is formed as energy is released. 96. Which term indicates how strongly an atom attracts the electrons in a chemical bond? A) alkalinity B) atomic mass C) electronegativity D) activation energy 97. Which bond is least polar? A) As–Cl B) Bi–Cl C) P–Cl D) N–Cl 98. Given the electron dot diagram:

The electrons in the bond between hydrogen and fluorine are more strongly attracted to the atom of A) hydrogen, which has the higher electronegativity B) fluorine, which has the higher electronegativity C) hydrogen, which has the lower electronegativity D) fluorine, which has the lower electronegativity MIDTERM REVIEW

100. The data table below represents the properties determined by the analysis of substances A, B, C, and D.

Which substance is an ionic compound? A) A B) B C) C D) D

101. The chemical bonding in sodium phosphate, Na3PO4 , 106. The ability to conduct electricity in the solid state is a is classified as characteristic of metallic bonding. This characteristic is best explained by the presence of A) ionic, only B) metallic, only A) high ionization energies C) both covalent and ionic B) high D) both covalent and metallic C) mobile electrons 102. Given a formula for oxygen: D) mobile protons 107. The electronegativity difference between the atoms in a molecule of HCl can be used to determine What is the total number of electrons shared between A) the entropy of the atoms the atoms represented in this formula? B) the atomic number of the atoms A) 1 B) 2 C) 8 D) 4 C) the first ionization energy of the atoms D) the polarity of the bond between the two 103. The bond between Br atoms in a Br2 molecule is atoms A) ionic and is formed by the sharing of two valence 108. Which formula represents a molecule with the most electrons polar bond? B) ionic and is formed by the transfer of two valence electrons A) CO B) NO C) HI D) HCl

C) covalent and is formed by the sharing of two 109. Why is a molecule of CO2 nonpolar even though the valence electrons bonds between the carbon atom and the oxygen atoms D) covalent and is formed by the transfer of two are polar? valence electrons A) The shape of the CO2 molecule is symmetrical. 104. Which terms describe a substance that has a low B) The shape of the CO2 molecule is asymmetrical. melting point and poor electrical conductivity? C) The CO2 molecule has a deficiency of electrons. A) covalent and metallic D) The CO2 molecule has an excess of electrons. B) covalent and molecular 110. At STP, fluorine is a gas and is a liquid C) ionic and molecular because, compared to fluorine, bromine has D) ionic and metallic A) stronger covalent bonds 105. Which element consists of positive ions immersed in a B) stronger intermolecular forces "sea" of mobile electrons? C) weaker covalent bonds A) sulfur B) nitrogen D) weaker intermolecular forces C) calcium D) chlorine 111. Which of these substances has the strongest intermolecular forces?

A) H2O B) H2S C) H2Se D) H2Te MIDTERM REVIEW

112. Which electron-dot structure represents a non-polar 120. Given the reaction: molecule? A) B)

Which type of reaction is represented? C) D) A) natural transmutation B) artificial transmutation C) fission D) fusion 113. Given the equation representing a in which X represents a nuclide: 121. What is one benefit associated with a nuclear fission reaction? A) The products are not radioactive. B) Stable isotopes are used as reactants. Which nuclide is represented by X? C) There is no chance of biological exposure. A) B) D) A large amount of energy is produced. C) D) 122. Which statement best describes what happens in a 114. Which nuclear emission has the greatest mass and the fission reaction? least penetrating power? A) Heavy nuclei split into lighter nuclei. A) an alpha particle B) a beta particle B) Light nuclei form into heavier nuclei. C) a neutron D) a positron C) Energy is released and less stable elements are formed. 115. Which particle has the least mass? D) Energy is absorbed and more stable elements are A) alpha particle B) beta particle formed. C) neutron D) proton 123. Given the balanced equation representing a nuclear 116. Which particle is emitted when an atom of 85Kr reaction: spontaneously decays? 2 3 4 1 A) an alpha particle B) a beta particle 1H + 1H 2He + 0n Which phrase identifies and describes this reaction? C) a neutron D) a proton A) fission, mass converted to energy 117. Which statement best describes gamma radiation? B) fission, energy converted to mass A) It has a mass of 1 and a charge of 1. C) fusion, mass converted to energy B) It has a mass of 0 and a charge of –1. D) fusion, energy converted to mass C) It has a mass of 0 and a charge of 0. 124. In which type of reaction do two lighter nuclei D) It has a mass of 4 and a charge of +2. combine to form one heavier nucleus? 118. What is the total number of years that must pass A) combustion B) reduction before only 25.00 grams of an original 100.0-gram sample of C-14 remains unchanged? C) nuclear fission D) A) 2865 y B) 5730 y 125. Given the nuclear equation: C) 11 460 y D) 17 190 y Which particle is represented by ? 119. What is the half-life of a radioisotope if 25.0 grams of an original 200.-gram sample of the remains A) B) C) D) unchanged after 11.46 days? A) 2.87 d B) 3.82 d C) 11.46 d D) 34.38 d MIDTERM REVIEW

126. Given the equation: 128. The radioactive isotope carbon-14 can be used for A) determining the age of a sample B) determining medical disorders When the equation is balanced correctly, which C) controlling fission reactions particle is represented by X? D) controlling speeds of neutrons A) B) C) D) 129. Which radioactive isotope is used in geological dating? 127. What is a problem commonly associated with nuclear power facilities? A) -238 B) -131 C) cobalt-60 D) -99 A) A small quantity of energy is produced. B) Reaction products contribute to acid rain. 130. Which radioisotope is used to treat thyroid disorders? C) It is impossible to control nuclear fission. A) Co-60 B) I-131 D) It is difficult to dispose of wastes. C) C-14 D) U-238 Answer Key midterm review

1. B 36. D 61. A 97. D 2. C 37. D 62. D 98. B 3. A 38. D 63. D 99. D 4. C 39. B 64. C 100. D 5. B 40. A 65. D 101. C 6. 41. C 66. C 102. D 42. D 67. B 103. C 43. B 68. D 104. B 7. D 44. Allow credit for A 69. D 105. C 8. B and D. 70. D 106. C 9. B 45. Acceptable responses: 71. C 107. D 10. D Energy is released 72. A 108. D 11. D when an electron falls from a high state 73. D 109. A 12. B (excited) to a low 74. B 110. B 13. C state (ground), excited 75. B 111. A 14. B state to ground state, high energy to low 76. C 112. B 15. A energy. 77. B 113. B 16. A 46. 78. D 114. A 17. B 79. C 115. B 18. A 80. A 116. B 19. C 81. D 117. C 20. C 82. A 118. C 21. B 83. C 119. B 22. A 47. A 84. A 120. B 23. A 48. A 85. B 121. D 24. A 49. A 86. B 122. A 25. C 50. A 87. D 123. C 26. A 51. B 88. C 124. D 27. B 52. A 89. B 125. A 28. B 53. D 90. B 126. B 29. A 54. C 91. C 127. D 30. D 55. B 92. A 128. A 31. A 56. A 93. A 129. A 32. D 57. A 94. B 130. B 33. C 58. C 95. A 34. A 59. C 96. C 35. D 60. D