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Chemistry Benchmark 1 Review Completion Complete each statement. 1. Chemistry is the study of _____________________ and the changes that it undergoes. 2. A(n) ______________________ is a set of controlled observations that test the hypothesis. 3. 100.00 meters 50.000 centimeters 1.0000 kilometer = ____________________ meters. 4. A process that involves one or more substances changing into new substances is known as a ____________________ change. 5. Cutting a sheet of paper is an example of a ____________________ change. 6. A ____________________ property enables a substance to combine with or change into one or more substances. 7. Sugar is a ____________________ form of matter with a definite shape and volume. 8. A ____________________ is a subatomic particle that has mass nearly equal to that of a proton, but it carries no electrical charge. 9. Atoms with the same number of protons but different number of neutrons are called ____________________. 10. An alpha particle is _____________________ charged with two protons and neutrons. 11. Democritus believed that matter is made up of tiny individual particles known as a(n) ____________________. 12. The number of protons in an atom is called the ____________________ of the element. 13. The ____________________ principle states that a maximum of two electrons may occupy a single atomic orbital, but only if the electrons have opposite spins. 14. The arrangement of electrons in an atom is called the ____________________ of an atom. 15. The group 2A elements are known as ____________________ metals. 16. Elements that have physical and chemical properties of both metals and nonmetals are known as ____________________. Short Answer 17. Explain the difference between mass and weight. 18. Explain how hypothesis and theory are different. Use the figure below to answer the question. 19. Infer a qualitative measurement that can be made from the scene shown. 20. Infer a quantitative measurement that can be made from the scene shown. 21. What must be immediately done if chemicals come in contact with the eyes or skin while performing an experiment in the laboratory? 22. Evaluate this dimensional analysis setup. A paperclip is 3.2 cm long. How many paperclips would fit in a football field (100 yards) if 1 inch = 2.54 cm? 23. What two things does a conversion factor do? 24. The data for two different measurements are shown below. Which experiment was more accurate? Explain your answer. Sample Measured value Accepted value Distance 54,700 m 57,900 m Mass 61.3 g 65.7 g A student conducts an experiment to determine the effect of adding salt on the boiling temperature of water. The results are shown below. Sample Amount of Salt Boiling Temperature Sample 1 0g 100.0° C Sample 2 2g 102.3° C Sample 3 5g 104.8° C Sample 4 10 g 107.5° C 25. The student graphs this data using the axes shown. Is this graph correct? Explain your answer. 26. Define a base unit. 27. The distance between the earth and the sun is 90.0 million miles. Calculate this distance in meters up to three significant digits. 28. Convert 600 mg to grams. 29. How many significant digits are there in 6.023 1023 molecules? 30. Identify both a physical change and a chemical change that could be done to a piece of paper. 31. Distinguish between element and compound. 32. Distinguish between homogeneous and heterogeneous mixtures. Give an example of each one. 33. Compare and contrast mass number and atomic mass. 34. What is the average atomic mass of this element? Isotope Mass (amu) Percent Abundance Phosphorus-29 29 5% Phosphorus-31 31 71% Phosphorus-32 32 24% 35. What is the average atomic mass of this element? Isotope Mass (amu) Percent Abundance Silver-105 105 48% Silver-108 108 43% Silver-109 109 9% 36. Write the chemical symbol for the isotope of cobalt with 37 neutrons. 37. Element X has an average atomic mass of 64.32 amu. If this element consists of only two isotopes, X-64 and X-65, which isotope is present in the greater abundance? Explain how you can tell. 38. Define an atom. 39. What do you understand by the term atomic mass unit (amu)? 40. How are atomic number and mass number denoted in the chemical symbol of the isotope of an element? Express the shortened notation for an isotope of element X with atomic number 92 and atomic mass 238. 41. Identify the element containing 34 protons. 42. What were the main flaws in Dalton’s atomic theory? 43. Summarize the relationship between wavelength, frequency, and energy of a wave. 44. A student records the following electron configuration for the element Arsenic (As). Evaluate this student’s answer. 1s22s22p63s23p64s24d104p3 45. Explain why it is only possible for two electrons to exist in the same orbital. 46. Use the model of the atom shown to identify the correct element. Write the electron configuration and orbital diagram for this element. 47. Which rule for filling of orbitals by electrons in the element Silicon is being violated in the orbital diagram shown? Justify your answer. 48. Which rule for the filling of orbitals in the element Phosphorus is being violated in the orbital diagram shown? Justify your answer. 49. Which rule for the filling of orbitals by electrons in the element Magnesium is being violated? Justify your answer. 50. Define a photon. What is the formula used to calculate the energy of a photon? 51. Why does a piece of iron appear red when heated sufficiently and blue at a higher temperature? 52. What is the ground state electron configuration of chlorine and the number of valence electrons in it? 53. How many valence electrons are present in cesium? Write the electron configuration of cesium if the atomic number is 55. 54. Write the noble gas form of the electron configuration and the electron dot structure of sodium and oxygen. 55. Write the noble gas form of the electron configuration and the electron dot structure of selenium and phosphorus. 56. A student makes the following statement: “It’s easy to tell which energy level an element is in - you just count down which row it is in, and that’s the energy level.” Is this student correct? Explain how you came to your conclusion. 57. Explain what is meant by the “octet rule.” Does it hold true for the modern periodic table? 58. Label the blank periodic table with the following terms. A: metalloids B: element with the highest electronegativity C: alkali metals D: lanthanide series E: element with the greatest atomic radius F: noble gases G: halogens 59. Explain the significance of the stair-step line located near the right-hand side of the periodic table 60. Do the figures in this partial periodic table demonstrate the trend in atomic radius, ionic radius, or neither of these? Relate your answer to the structure of atoms across the periodic table. 61. Place these five elements in order of electronegativity, with the highest electronegativity first. 62. Identify the representative elements from the list given below. Na, Ca, Sc, Co, Ni, Si, N, Se, Cl, Ge 63. Why is argon placed before potassium in the modern periodic table? 64. Why do elements in the same group have similar properties? 65. Why is the size of a sodium ion (Na+) less than that of a sodium atom (Na)? 66. List the general electron configuration and location of the s, p, d, and f-block elements in the periodic table. 67. Use the periodic table to write the names of the third alkali metal and the first transition metal. Problem 68. A vessel contains 30 mL of water. A sample of 5.0 g of copper metal is dropped into this vessel, raising the level of water in it to 40 mL. What is the density of the copper sample? 69. When a 5.00-g metal piece, A, was immersed in 38.0 mL of water, the water level rose to 50.0 mL. Similarly, when a 5.00-g metal piece, B, was immersed in 38.0 mL of water, the level of water rose to 60.0 mL. Compare the density of the metal pieces, A and B. 70. Calculate the area of a rectangular piece of land with a length of 8.0 105 cm and a width of 4.0 103 cm. Express your answer in meters. 71. Complete the following table: Element Number of protons Sodium Phosphorus 15 Cobalt 27 Bromine Silver Number of electrons 11 Number of neutrons 12 Atomic number Mass number 31 32 35 80 61 47 72. An element X has two naturally occurring isotopes: X-79 (abundance = 50.69%, mass = 78.918 amu) and X-81 (abundance = 49.31%, mass = 80.917 amu). Calculate the weighted atomic mass of X. Also, identify the unknown element which exists as a reddish-brown gas and is a liquid at room temperature. 73. An element X has three naturally occurring isotopes: X-24, X-25, and X-26. The atomic mass of X-25 is 24.986 amu and the relative abundance is 10.00 %. The atomic mass of X-26 is 25.982 amu and the relative abundance is 11.01 %.Given that the weighted atomic mass of the element X is 24.305, calculate the mass contribution due to the isotope X-24 and identify the element. 74. Calculate the number of protons, electrons, and neutrons in an atom of the element Pb with mass number 207 and atomic number 82. 75. Fluorine (F) contains 9 proton and 10 neutrons. Calculate its mass in amu for 81 atoms. (Given: mass of a proton = 1.007276 amu, mass of a neutron = 1.008665 amu). 76. Lead contains 82 protons and 125 neutrons. Write the shortened notation of the element with its symbol, atomic number, and mass number. 77. How many sublevels and orbitals are possible in the third energy level? 78. Write the ground state electron configuration of sulfur and draw its electron-dot structure. 79. Two elements A and B have atomic numbers 8 and 17 respectively. Identify their groups in the periodic table. 80. An element has similar chemical properties as oxygen and selenium. It has an atomic number greater than krypton but less than iodine. Use the periodic table to identify the element. 81. Identify the element having the largest size and the element having the highest electronegativity from the list of electron configurations given below: a. [Ne] 3s23p3 b. [Ne] 3s23p4 c. [Ne] 3s23p5 d. [Ne] 3s23p34s23d3 82. Arrange the elements given below in the increasing order of their atomic size. Element A 1s22s22p6 Element B 1s22s2 Element C 1s22s22p63s1 Element D 1s22s22p3 Chemistry Benchmark 1 Review Answer Section COMPLETION 1. ANS: matter PTS: NAT: KEY: 2. ANS: 1 DIF: 1 B.2 STA: ABC 1.1 Chemistry | Matter experiment PTS: OBJ: STA: KEY: 3. ANS: 1 DIF: 1 REF: Page 11 1.3.2 Compare and contrast types of data. NAT: G.2 ABC 1.1 TOP: Compare and contrast types of data. Theory | Scientific law MSC: 1 1100.5 PTS: OBJ: STA: KEY: 4. ANS: 1 DIF: 1 REF: Page 26 2.1.2 Explain how adding a prefix changes a unit. NAT: UCP.1 ABC 1.1 TOP: Explain how adding a prefix changes a unit. Meter | Kilometer | Centimeter MSC: 2 chemical PTS: OBJ: NAT: TOP: KEY: 5. ANS: 1 DIF: 1 REF: Page 62 3.2.2 Define chemical change and list several indications that a chemical change has taken place. UCP.3 | B.3 STA: ABC 10.1 Define chemical change and list several indications that a chemical change has taken place. Chemical change MSC: 1 physical PTS: OBJ: NAT: TOP: KEY: 6. ANS: 1 DIF: 1 REF: Page 61 3.2.1 Define physical change and list several common physical changes. UCP.3 | B.2 STA: ABC 10.1 Define physical change and list several common physical changes. Physical change MSC: 2 chemical PTS: OBJ: NAT: KEY: 7. ANS: 1 DIF: 1 REF: Page 57 3.1.2 Distinguish between physical and chemical properties. B.2 STA: ABC 10.1 TOP: Distinguish between physical and chemical properties. Chemical property MSC: 1 solid PTS: OBJ: STA: KEY: REF: Page 7 OBJ: 1.2.1 Define chemistry and matter. TOP: Define chemistry and matter. MSC: 1 1 DIF: 1 REF: Page 58 3.1.3 Differentiate among the physical states of matter. NAT: B.2 ABC 10.1 TOP: Differentiate among the physical states of matter. Solids MSC: 2 8. ANS: neutron PTS: OBJ: NAT: TOP: KEY: 9. ANS: PTS: OBJ: NAT: TOP: KEY: 10. ANS: 1 DIF: 1 REF: Page 96 4.2.2 Describe the structure of the nuclear atom, including the locations of the subatomic particles. B.1 | G.3 STA: ABC 10.1 | ABC 10.2 Describe the structure of the nuclear atom, including the locations of the subatomic particles. Neutron MSC: 1 isotopes 1 DIF: 1 REF: Page 100 4.3.2 Define an isotope and explain why atomic masses are not whole numbers. B.1 STA: ABC 10.1 | ABC 10.2 Define an isotope and explain why atomic masses are not whole numbers. Isotopes MSC: 1 positively PTS: 1 DIF: 1 REF: Page 106 OBJ: 4.4.2 Characterize alpha, beta, and gamma radiation in terms of mass and charge. NAT: B.1 | B.6 STA: ABC 10.1 | ABC 10.2 TOP: Characterize alpha, beta, and gamma radiation in terms of mass and charge. KEY: Alpha radiations MSC: 1 11. ANS: atomos atom PTS: OBJ: NAT: TOP: KEY: 12. ANS: 1 DIF: 1 REF: Page 88 4.1.1 Compare and contrast the atomic models of Democritus and Dalton. G.3 | UCP.2 | B.1 | B.2 STA: ABC 10.1 Compare and contrast the atomic models of Democritus and Dalton. Atom MSC: 1 atomic number PTS: OBJ: NAT: TOP: KEY: 13. ANS: 1 DIF: 1 REF: Page 98 4.3.1 Explain the role of atomic number in determining the identity of an atom. B.1 STA: ABC 10.1 Explain the role of atomic number in determining the identity of an atom. Atomic number MSC: 1 Pauli exclusion PTS: 1 DIF: 1 REF: Page 136 OBJ: 5.3.1 Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron configurations using orbital diagrams and electron configuration notation. NAT: B.6 STA: ABC 10.1 | ABC 10.2 TOP: Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron configurations using orbital diagrams and electron configuration notation. KEY: Pauli exclusion principle MSC: 1 14. ANS: electron configuration PTS: 1 DIF: 1 REF: Page 135 OBJ: 5.3.1 Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron configurations using orbital diagrams and electron configuration notation. NAT: B.6 STA: ABC 10.2 TOP: Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron configurations using orbital diagrams and electron configuration notation. KEY: Electron configuration MSC: 1 15. ANS: alkaline earth PTS: OBJ: NAT: TOP: KEY: 16. ANS: 1 DIF: 1 REF: Page 155 6.1.1 Trace the development and identify key features of the periodic table. G.3 | B.1 | UCP.1 STA: ABC 10.1 Trace the development and identify key features of the periodic table. Alkaline earth metals MSC: 1 metalloids PTS: OBJ: NAT: TOP: KEY: 1 DIF: 1 REF: Page 158 6.1.1 Trace the development and identify key features of the periodic table. G.3 | B.1 | UCP.1 STA: ABC 10.1 Trace the development and identify key features of the periodic table. Metalloids MSC: 1 SHORT ANSWER 17. ANS: Mass is a measurement of the amount of matter in a substance, while weight is a measure of gravity’s effect on that mass. PTS: 1 DIF: Bloom's Level 2 NAT: UCP.2 | E.2 STA: ES 9.1 18. ANS: A hypothesis is a prediction of the outcome of one experiment. A theory is a description of how a process is believed to occur and is based on the results of many different experiments. PTS: 1 DIF: Bloom's Level 4 NAT: UCP.2 | A.2 STA: ABC 1.1 19. ANS: Answers should be descriptions of object without using numbers (counting or measuring). PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3 | A.1 | A.2 STA: ABC 10.1 20. ANS: Answers should include a numerical value obtained from measurement or counting. PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3 | A.1 | A.2 STA: ABC 10.1 21. ANS: Flush the area immediately with large quantities of water and inform the teacher of the spill and the chemical. PTS: 1 DIF: 1 REF: Page 16 OBJ: 1.4.2 Apply knowledge of laboratory safety. NAT: A.1 | A.2 STA: ABC 3.1 TOP: Apply knowledge of laboratory safety. KEY: Laboratory safety MSC: 1 22. ANS: The second conversion factor, 1 inch = 2.54 cm, is reversed. It needs to be arranged so that the unit in the denominator of one fraction can cancel out the unit in the numerator of the next fraction, and so on. PTS: 1 DIF: Bloom's Level 6 STA: ABC 1.1 23. ANS: 1. cancels one unit 2. introduces a new unit NAT: UCP.2 PTS: 1 DIF: Bloom's Level 2 NAT: UCP.2 STA: ABC 1.1 24. ANS: The distance measurement has an error of 5.53%. The mass measurement has an error of 6.70%. Therefore, distance was measured more accurately. PTS: 1 DIF: Bloom's Level 6 NAT: UCP.2 | UCP.3 STA: ABC 1.1 25. ANS: The independent variable should be placed on the X axis, and the dependent variable on the Y axis. This graph is correct as shown. PTS: 1 DIF: Bloom's Level 6 NAT: UCP.2 STA: ABC 1.1 26. ANS: A base unit is a defined unit in a system of measurement that is based on an object or event in the physical world. It is independent of other units. PTS: 1 DIF: 1 REF: Page 26 OBJ: 2.1.1 Define SI base units for time, length, mass, and temperature. NAT: UCP.1 STA: ABC 1.1 TOP: Define SI base units for time, length, mass, and temperature. KEY: Base unit MSC: 1 27. ANS: 1.44 1011m PTS: 1 DIF: 1 REF: Page 34 OBJ: 2.2.2 Use dimensional analysis to convert between units. NAT: UCP.1 STA: ABC 1.1 TOP: Use dimensional analysis to convert between units. KEY: Miles | Meter MSC: 3 28. ANS: 1mg = 1/ 1000 g 600 mg = 0.6 g PTS: OBJ: STA: KEY: 29. ANS: 1 DIF: 1 REF: Page 34 2.2.2 Use dimensional analysis to convert between units. NAT: UCP.1 ABC 1.1 TOP: Use dimensional analysis to convert between units. Gram | Milligram MSC: 3 There are four significant digits in 6.023 1023 molecules. PTS: 1 DIF: 1 REF: Page 39 OBJ: 2.3.2 Use significant figures and rounding to reflect the certainty of data. NAT: E.2 | G.2 STA: ABC 1.1 TOP: Use significant figures and rounding to reflect the certainty of data. KEY: Significant figures | Molecules MSC: 2 30. ANS: A physical change might be ripping it, crumpling it, or writing on it with pencils or pens. A chemical change might be burning it or letting it rot. PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3 | B.2 | B.3 STA: ABC 10.1 31. ANS: An element is the smallest piece of matter that retains its physical and chemical properties, and is made up of only one type of atom. A compound is made of more than one different element chemically joined together. A compound can be broken into smaller pieces by chemical means. PTS: 1 DIF: Bloom's Level 2 NAT: UCP.2 STA: ABC 10.1 32. ANS: A homogeneous mixture is a combination of substances in varying proportions where the individual substances cannot be distinguished. Every part of the mixture has the same composition as any other part, such as in a beverage made from powdered mix. In a heterogeneous mixture, the different substances can be distinguished. Parts of the mixture have different compositions, as in a chocolate-chip cookie. PTS: 1 DIF: Bloom's Level 3 NAT: UCP.2 STA: ABC 10.1 33. ANS: Mass number is the total number of neutrons and protons in an individual atom. It is an integer number. Atomic number, or average atomic number, is the weighted average mass of all of the different isotopes found in a sample of an element. Because it is a weighted average, atomic mass is usually a decimal number. PTS: 1 DIF: Bloom's Level 2 STA: ABC 10.1 | ABC 10.2 34. ANS: (29*.05)+(31*.71)+(32*.24) = 31.14 amu NAT: UCP.2 | B.1 PTS: 1 DIF: Bloom's Level 3 STA: ABC 10.1 | ABC 10.2 35. ANS: (105*.48)+(108*.43)+(109*.09) = 106.65 amu NAT: UCP.2 | B.1 PTS: 1 DIF: Bloom's Level 3 STA: ABC 10.1 | ABC 10.2 36. ANS: NAT: UCP.2 | B.1 PTS: 1 DIF: Bloom's Level 3 STA: ABC 10.1 | ABC 10.2 NAT: B.1 37. ANS: The more abundant isotope would be X-64. With only two isotopes, one can be certain that the weighted average atomic mass will be closer to the isotope in greater abundance. Since the average mass is 64.32, which rounds to 64, isotope X-64 must be more abundant than X-65. PTS: 1 DIF: Bloom's Level 4 NAT: UCP.2 STA: ABC 10.1 | ABC 10.2 38. ANS: An atom is the smallest particle of an element that retains the properties of the element. PTS: 1 DIF: 1 REF: Page 90 OBJ: 4.1.2 Define an atom. NAT: B.1 STA: ABC 10.1 TOP: Define an atom. KEY: Atom MSC: 1 39. ANS: The atomic mass unit measures the mass of an atom relative to the mass of carbon-12 atom, which is taken as a standard. One atomic mass unit is defined as 1/12 the mass of a carbon-12 atom. PTS: 1 DIF: 1 REF: Page 102 OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number. NAT: B.1 STA: ABC 10.1 | ABC 10.2 TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number. KEY: Atomic mass unit MSC: 2 40. ANS: The atomic number is written as the subscript in the chemical symbol of an element and the mass number is written as the superscript in the chemical symbol of an element. The notation for an isotope of element X is denoted as . PTS: 1 DIF: 2 REF: Page 98 | Page 100 OBJ: 4.3.2 Define an isotope and explain why atomic masses are not whole numbers. NAT: B.1 STA: ABC 10.1 | ABC 10.2 TOP: Define an isotope and explain why atomic masses are not whole numbers. KEY: Atomic number | Mass number | Isotopes MSC: 3 41. ANS: The element containing 34 protons is Selenium (Se). PTS: 1 DIF: 1 REF: Page 98 OBJ: 4.3.1 Explain the role of atomic number in determining the identity of an atom. NAT: B.1 STA: ABC 10.1 | ABC 10.2 TOP: Explain the role of atomic number in determining the identity of an atom. KEY: Atomic number MSC: 1 42. ANS: There were two main flaws in Dalton’s atomic theory. a. Atoms are not indivisible. They are divisible into several subatomic particles. b. All atoms of a given element may not have identical properties as their masses may vary slightly. PTS: OBJ: NAT: TOP: KEY: 1 DIF: 2 REF: Page 90 4.1.1 Compare and contrast the atomic models of Democritus and Dalton. G.3 | UCP.2 | B.1 | B.2 STA: ABC 10.1 | ABC 10.2 Compare and contrast the atomic models of Democritus and Dalton. Dalton's atomic theory MSC: 2 43. ANS: As the amount of energy carried by a wave increases, the individual waves get closer together, increasing their frequency but decreasing their wavelength. PTS: 1 DIF: Bloom's Level 3 NAT: UCP.2 | B.6 STA: ABC 10.2 | ABC 10.3 44. ANS: The “d10” should be preceded by a 3; although the first set of d-block elements are in the fourth period, these electrons are actually contained in the third energy level due to the overlapping of energy levels and orbitals. PTS: 1 DIF: Bloom's Level 6 NAT: UCP.2 | B.1 STA: ABC 10.2 | ABC 10.3 45. ANS: Electrons have a spin. In any given orbital, only two electrons can exist because one will spin in an “upward” direction while the other one spins in a “downward” direction. A pair of electrons can only exist in an orbital if they are spinning in opposite directions. PTS: 1 DIF: Bloom's Level 3 NAT: B.1 STA: ABC 10.2 | ABC 10.3 46. ANS: The element is Silicon. The electron configuration is 1s2s222p63s23p6. The orbital diagram is shown below. PTS: 1 DIF: Bloom's Level 5 NAT: UCP.2 | B.1 STA: ABC 10.2 | ABC 10.3 47. ANS: This violates the Aufbau principle, which states that electrons must fill in the orbital with the lowest amount of energy before filling any orbitals with a greater amount of energy. In the diagram shown, electrons are placed in the 3p orbitals before the 3s is filled. PTS: 1 DIF: Bloom's Level 4 NAT: UCP.2 | B.1 STA: ABC 10.2 | ABC 10.3 48. ANS: This is violating Hund’s rule. According to Hund’s rule, single electrons must occupy the orbitals within the same energy level and type of orbital before two electrons are allowed to occupy the same orbital. Here, two electrons occupy the first 3p orbital before the other two orbitals have one electron. PTS: 1 DIF: Bloom's Level 4 NAT: UCP.2 | B.1 STA: ABC 10.2 | ABC 10.3 49. ANS: The Pauli exclusion principle is being violated. The Pauli exclusion principle requires that if two electrons occupy the same orbital, they must have opposite spin directions. This is generally shown by having arrows pointing either up or down in the orbital diagrams. Here, the two electrons in the 3s orbital are spinning the same direction, as indicated by the arrows pointing the same direction. PTS: 1 DIF: Bloom's Level 4 NAT: UCP.2 | B.1 STA: ABC 10.2 | ABC 10.3 50. ANS: A photon is a particle of electromagnetic radiation that has no mass and carries a quantum of energy. The energy of a photon can be calculated using the formula Equantum h , where E is energy of the photon, h is Planck’s constant, and is frequency of the photon. PTS: 1 DIF: 1 REF: Page 123 OBJ: 5.1.1 Compare the wave and particle models of light. NAT: B.1 STA: ABC 10.2 | ABC 10.3 TOP: Compare the wave and particle models of light. KEY: Photon | Energy levels MSC: 1 51. ANS: A piece of iron appears red when heated sufficiently and blue at a higher temperature, because the kinetic energy of iron increases when it is heated. With an increase in the amount of energy, different colors of light are emitted. These colors correspond to different frequencies and wavelengths. PTS: 1 DIF: 1 REF: Page 122 OBJ: 5.1.2 Define a quantum of energy and explain how it is related to an energy change of matter. NAT: B.6 STA: ABC 10.1 TOP: Define a quantum of energy and explain how it is related to an energy change of matter. KEY: Quantum MSC: 2 52. ANS: The ground state electron configuration of chlorine is 1s22s22p63s23p5. It has 7 valence electrons. PTS: 1 DIF: 1 REF: Page 138 OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence electrons. NAT: B.1 | B.6 STA: ABC 10.2 | ABC 10.3 TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons. KEY: Valence electrons | Electron configuration MSC: 2 53. ANS: There is only one valence electron in cesium. The electron configuration of cesium with atomic number 55 is [Xe]6s1. PTS: 1 DIF: 1 REF: Page 140 OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence electrons. NAT: B.1 | B.6 STA: ABC 10.2 | ABC 10.3 TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons. KEY: Valence electrons | Electron configuration MSC: 1 54. ANS: a. The noble gas form of the electron configuration of sodium is [Ne]3s1. Its electron dot structure is b. The noble gas form of electron configuration of oxygen is [He]2s22p4. Its electron dot structure is PTS: 1 DIF: 2 REF: Page 138 | Page 140 OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence electrons. NAT: B.1 | B.6 STA: ABC 10.1 | ABC 10.2 TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons. KEY: Electron configuration | Electron-dot structure MSC: 2 55. ANS: a. The noble gas form of the electron configuration of selenium is [Ar]4s24p4. Its electron-dot structure is b. The noble gas form of the electron configuration of phosphorus is [Ne]3s23p5. Its electron-dot structure is . PTS: 1 DIF: 2 REF: Page 138 OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence electrons. NAT: B.1 | B.6 STA: ABC 10.1 | ABC 10.2 TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons. KEY: Electron configuration | Electron-dot structure MSC: 2 56. ANS: No, the student is not correct. We know from writing electron configurations (Chapter 5) that elements in each row of the d-block are actually contained in the energy level of the previous row; therefore one cannot merely count down the rows. Periods and energy levels are not the same thing. One should also be careful to not claim that the top row of the d-block is energy level 1 because it is the first row of that section. PTS: 1 DIF: Bloom's Level 6 NAT: B.1 | B.6 STA: ABC 10.1 57. ANS: The octet rule states that most elements would like to have eight electrons in their outer energy level to become stable like the closest noble gas. PTS: 1 STA: ABC 10.1 58. ANS: DIF: Bloom's Level 4 NAT: B.2 PTS: 1 DIF: Bloom's Level 1 NAT: UCP.2 | B.2 STA: ABC 10.1 59. ANS: The stairstep line separates the metals from the nonmetals on the periodic table. Elements that are adjacent to this line are considered metalloids and have some properties of metals and some properties of nonmetals. PTS: 1 STA: ABC 10.1 DIF: Bloom's Level 3 NAT: UCP.2 | B.2 60. ANS: These show the atomic radius change. As electrons are added to the outer energy levels of an atom (as one moves across the periodic table), the size of the atom decreases. This is because the additional positive charge in the nucleus attracts the electrons more strongly and no additional shielding effect occurs across the period. PTS: 1 STA: ABC 10.1 61. ANS: B, D, C, E, A DIF: Bloom's Level 4 PTS: 1 DIF: Bloom's Level 4 STA: ABC 10.1 62. ANS: Na, Ca, N, Si, Se, Cl, Ge NAT: UCP.2 | B.1 | B.2 NAT: UCP.2 | B.2 PTS: 1 DIF: 1 REF: Page 154 OBJ: 6.1.1 Trace the development and identify key features of the periodic table. NAT: G.3 | B.1 | UCP.1 STA: ABC 10.1 TOP: Trace the development and identify key features of the periodic table. KEY: Metals MSC: 2 63. ANS: In the modern periodic table, the elements are placed in the order of their increasing atomic numbers. The atomic number of argon is 18 while the atomic number of potassium is 19. Therefore, argon is placed before potassium in the modern periodic table. PTS: 1 DIF: 1 REF: Page 153 OBJ: 6.1.1 Trace the development and identify key features of the periodic table. NAT: G.3 | B.1 | UCP.1 STA: ABC 10.1 TOP: Trace the development and identify key features of the periodic table. KEY: Atomic number MSC: 2 64. ANS: Elements in the same group have the same electron configuration and number of valence electrons. Valence electrons determine the properties of elements. Therefore, properties of elements in the same group are similar. PTS: 1 DIF: 1 REF: Page 159 OBJ: 6.2.1 Explain why elements in the same group have similar properties. NAT: UCP.1 | B.1 | B.2 STA: ABC 10.1 TOP: Explain why elements in the same group have similar properties. KEY: Groups | Electron configuration MSC: 2 65. ANS: The loss of an electron from a sodium atom results in a smaller radius. The electrostatic repulsion between the remaining number of electrons decreases thus allowing them to be pulled closer to the nucleus. Therefore, the size of a sodium ion (Na+) is less than that of a sodium atom (Na). PTS: OBJ: NAT: TOP: 1 DIF: 2 REF: Page 165 6.3.2 Relate period and group trends in atomic radii to electron configuration. UCP.1 | B.1 | B.2 STA: ABC 10.1 Relate period and group trends in atomic radii to electron configuration. KEY: Atomic size | Ionic radius MSC: 2 66. ANS: The general electron configuration and locations of the block elements are: a. ns0-2 for s-block elements in groups 1 and 2. b. ns0-2 and np0-6 for p-block elements in groups 13, 14, 15, 16, 17, and 18. c. (n–1)d0-10 and ns0-2 for d-block elements in groups 3, 4, 5, 6, 7, 8, 9, 10, 11, and 12. d. (n–2)f0-14, (n–1)d0-10, np0-6, and ns0-2 for f-block elements in lanthanide and actinide groups. PTS: 1 DIF: 2 REF: Page 161 OBJ: 6.2.2 Identify the four blocks of the periodic table based on electron configuration. NAT: UCP.1 | B.1 STA: ABC 10.1 TOP: Identify the four blocks of the periodic table based on electron configuration. KEY: Electron configuration MSC: 1 67. ANS: Potassium is the third alkali metal and scandium is the first transition metal in the periodic table. PTS: OBJ: NAT: TOP: KEY: 1 DIF: 1 REF: Page 156 6.1.1 Trace the development and identify key features of the periodic table. G.3 | B.1 | UCP.1 STA: ABC 10.1 Trace the development and identify key features of the periodic table. Alkali metals | Transition metals MSC: 1 PROBLEM 68. ANS: 0.5 g/mL PTS: 1 DIF: 1 REF: Page 28 OBJ: 2.1.3 Compare the derived units of volume and density. STA: ABC 1.1 TOP: Compare the derived units of volume and density. KEY: Mass | Density | Volume MSC: 3 NOT: Density = mass / volume. The volume of the copper sample is = 40 mL - 30 mL = 10 mL. 69. ANS: Metal A has a greater density than metal B. The density of metal A = 0.417 g/mL. The density of metal B = 0.227 g/mL. PTS: 1 DIF: 2 REF: Page 29 OBJ: 2.1.3 Compare the derived units of volume and density. TOP: Compare the derived units of volume and density. MSC: 3 NOT: Density = mass / volume 70. ANS: 3.2 105 m2 PTS: OBJ: STA: KEY: NOT: 71. ANS: STA: ABC 1.1 KEY: Mass | Density | Volume 1 DIF: 2 REF: Page 35 2.2.2 Use dimensional analysis to convert between units. NAT: UCP.1 ABC 1.1 TOP: Use dimensional analysis to convert between units. Meter | Centimeter | Area MSC: 3 Area = length * width. 1m = 100 cm. Element Sodium Phosphorus Cobalt Bromine Silver Number of protons 11 35 47 Number of electrons Number of neutrons 15 27 16 45 47 Atomic number 11 15 27 35 Mass number 23 59 108 PTS: 1 DIF: 3 REF: Page 98 | Page 99 | Page 100 OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number. NAT: B.1 STA: ABC 10.1 | ABC 10.2 TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number. KEY: Composition of elements MSC: 3 NOT: Atomic number = number of protons = number of electrons. Mass number = number of protons + number of neutrons. 72. ANS: 79.904 amu Bromine PTS: 1 DIF: 3 REF: Page 102 | Page 103 OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number. NAT: B.1 STA: ABC 10.1 | ABC 10.2 TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number. KEY: Atomic mass of isotopes MSC: 3 NOT: Weighted atomic mass of element X = mass contribution of X-79 + mass contribution of X-81. Mass contribution of each isotope = (mass in amu of the isotope) * (percent abundance). 73. ANS: 23.985 amu Magnesium PTS: 1 DIF: 3 REF: Page 102 | Page 103 OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number. NAT: B.1 STA: ABC 10.1 | ABC 10.2 TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number. KEY: Atomic mass of isotopes MSC: 3 NOT: Weighted atomic mass of element X = mass contribution of X-24 + mass contribution of X-25 + mass contribution of X-26. Mass contribution = (mass of the isotope in amu) * (percent abundance). 74. ANS: Number of protons = atomic number = 82. Number of electrons = number of protons = 82. Number of neutrons = mass number – atomic number = 125. PTS: 1 DIF: 2 REF: Page 98 | Page 101 OBJ: 4.3.1 Explain the role of atomic number in determining the identity of an atom. NAT: B.1 STA: ABC 10.1 | ABC 10.2 TOP: Explain the role of atomic number in determining the identity of an atom. KEY: Atomic number MSC: 3 NOT: Atomic number = number of protons = number of electrons. 75. ANS: 1551.32 amu PTS: 1 DIF: 2 REF: Page 102 OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number. NAT: B.1 STA: ABC 10.1 | ABC 10.2 TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number. KEY: Mass of individual atoms MSC: 3 NOT: The mass of an atom depends on the number of protons and neutrons. It is expressed in atomic mass units (amu). 76. ANS: PTS: 1 DIF: 1 REF: Page 100 OBJ: 4.3.2 Define an isotope and explain why atomic masses are not whole numbers. NAT: B.1 STA: ABC 10.1 | ABC 10.2 TOP: Define an isotope and explain why atomic masses are not whole numbers. KEY: Chemical symbol and notation MSC: 3 NOT: Isotopes are written with a shortened type notation. The notation includes the chemical symbol, atomic number and mass number. The atomic mass and the atomic number are written to the left of the chemical symbol. The atomic mass is denoted as a superscript and the atomic number is denoted as a subscript. 77. ANS: There are three sublevels and nine orbitals possible in the third energy level. PTS: 1 DIF: 2 REF: Page 134 OBJ: 5.2.3 Identify the relationships among a hydrogen atom's energy levels, sublevels, and atomic orbitals. NAT: B.6 STA: ABC 10.1 | ABC 10.2 TOP: Identify the relationships among a hydrogen atom's energy levels, sublevels, and atomic orbitals. KEY: Energy levels | Sublevels | Atomic orbitals MSC: 2 NOT: The number of sublevels is equal to the types of orbitals. The number of orbitals is equal to all the integers ranging from positive to negative values. 78. ANS: The ground state electron configuration of sulfur is [Ne]3s23p4. Its electron dot structure is PTS: 1 DIF: 2 REF: Page 138 OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence electrons. NAT: B.1 | B.6 STA: ABC 10.1 | ABC 10.2 TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons. KEY: Electron-dot structure | Valence electrons MSC: 3 79. ANS: Element A belongs to group 6A and element B belongs to group 7A in the periodic table. PTS: 1 DIF: 1 REF: Page 159 OBJ: 6.2.1 Explain why elements in the same group have similar properties. NAT: UCP.1 | B.1 | B.2 STA: ABC 10.1 TOP: Explain why elements in the same group have similar properties. KEY: Groups MSC: 1 NOT: Groups indicate the number of valence electrons. 80. ANS: Tellurium PTS: 1 DIF: 1 REF: Page 157 OBJ: 6.1.1 Trace the development and identify key features of the periodic table. NAT: G.3 | B.1 | UCP.1 STA: ABC 10.1 TOP: Trace the development and identify key features of the periodic table. KEY: Periodic table MSC: 2 NOT: Elements are arranged in the increasing order of their atomic numbers. Elements in groups have similar properties. 81. ANS: The element having the largest size has an electron configuration of [Ne] 3s23p34s23d3. The element having the highest electronegativity has an electron configuration of [Ne] 3s23p5. PTS: 1 DIF: 2 REF: Page 163 | Page 168 OBJ: 6.3.2 Relate period and group trends in atomic radii to electron configuration. NAT: UCP.1 | B.1 | B.2 STA: ABC 10.1 TOP: Relate period and group trends in atomic radii to electron configuration. KEY: Electron configuration | Atomic size | Electronegativity MSC: 2 NOT: The size of the atom depends on the number of shells in an atom. Electronegativity increases across a period. 82. ANS: The arrangement of elements in the increasing order of their atomic size is B < A < D < C. Element B is the smallest and Element C is the largest. PTS: 1 DIF: 1 REF: Page 163 OBJ: 6.3.2 Relate period and group trends in atomic radii to electron configuration. NAT: UCP.1 | B.1 | B.2 STA: ABC 10.1 TOP: Relate period and group trends in atomic radii to electron configuration. KEY: Atomic size | Electron configuration MSC: 2 NOT: The size of an atom depends upon the number of shells in an atom. In the same period, the atomic size decreases from left to right.