Chemistry_Electron_in Chemistry_Obj6bcde Some questions (c) 2012 by STAAR Test Maker. Some questions (c) 2012 by Region 10 Educational Service Center. Page 2 GO ON 1 Which form of electromagnetic radiation is more energetic than ultraviolet rays? A Violet light B Infrared radiation C Xrays D Microwaves 2 Which of these is the least energetic form of electromagnetic radiation? F Visible light G Microwaves H Gamma rays J 3 Radio waves Which of the following statements about electromagnetic radiation is true? A Electromagnetic waves with high frequency are more energetic than electromagnetic waves with low frequency. B All electromagnetic radiation carries the same amount of energy. C Electromagnetic waves with long wavelength are more energetic than electromagnetic waves with short wavelength. D Electromagnetic radiation in a vacuum can change frequency to become more or less energetic. Page 3 GO ON 4 Which of the following is the correct 5 Which pair of elements and/or ions edot diagram? are isoelectronic with each other? F A Be & Ne B K+ & Ar C Na+1 & Cl1 D P & K G 6 Which particles are represented by the dots in Lewis valence edot structures? F H core electrons G valence electrons H protons J all electrons J 7 Which element has the ground state electronic configuration, 1s2 2s2 2p6 3s2 3p6 4s1 ? A calcium B potassium C phosphorus D bromine Page 4 GO ON 8 What is the ground state electron configuration for arsenic? F 1s2 2s2 2p6 3s2 3p6 3d104s2 4p 3 G 1s2 2s2 2p6 3s2 3p6 4s2 4p3 4d10 H 1s2 2s2 2p6 3s2 3p6 3d104s2 4p 6 J 1s2 2s2 2p6 3s2 3p6 4s2 4p 3 Page 5 GO ON 9 Which species has the same electron configuration as a Cl ion? A F B Ar C S D Br 10 Which species does not have a noble gas electron configuration? F Na+ G S H Mg2+ J 11 Ar Which electron configuration is correct for a sodium ion? A 2−8−1 B 2−8 C 2−8−2 D 2−7 Page 6 GO ON 12 Which ion has the same electron configuration as an atom of He? F O2 G Ca2+ H H J 13 Na+ Which particle has the same electron configuration as a potassium ion? A Fluoride ion B Neon atom C Argon atom D Sodium ion 14 Which electron configuration represents an atom in an excited state? F 2−2−1 G 2−2 H 2−8−1 J 2−8 Page 7 GO ON 15 Which electron configuration represents an atom in an excited state? A 2−7 B 2−0−1 C 2−8 D 2−2 16 Which electron configuration represents an atom in an excited state? F 2−8−2 G 2−8−1 H 2−7−2 J 17 2−8 An atom with the electron configuration of 2−8−13−2 has an incomplete — A second principal energy level. B 4s sublevel. C 2p sublevel. D third principal energy level. Page 8 GO ON 18 An atom with the electron configuration 2−8−8−2 has an incomplete — F third principal energy level. G 2s sublevel. H second principal energy level. J 19 3s sublevel. Which electron configuration represents a strontium atom in an excited state? A 2−8−18−8−2 B 2−8−18−7−3 C 2−8−18−7−1 D 2−8−18−8−1 20 Which electron configuration represents an atom in an excited state? F 2−6−2 G 2−7 H 2−8−8−2 J 2−8−1 Page 9 GO ON 21 Which electron configuration represents an atom of an element having a completed third principal energy level? A 2−8−6−2 B 2−8−2 C 2−8−18−2 D 2−8−10−2 22 A fluoride ion (F) has the same electron configuration as — F Na+. G Cl. H Na. J 23 Cl. Which electron configurations represent the first two elements in Group 17 of the Periodic Table? A 2−1 and 2−2 B 2−2 and 2−3 C 2−8 and 2−8−7 D 2−7 and 2−8−7 Page 10 GO ON 24 Which is the electron configuration of a neutral atom in the ground state with a total of six valence electrons? F 2−6 G 2−4 H 2−8−8 J 25 2−8 Which element has an atom with the electron configuration 2−8−8−2? A Ni B Mg C Ca D Ge 26 The electrondot symbol below represents an ion of element X. Which of the following could be element X? F K G N H I J H Page 11 GO ON 27 Which is the correct electrondot symbol for the fluoride ion? A B C D 28 The electrondot symbol X: would best represent — F Na. G Cl. H Ne. J 29 Mg. Which electrondot symbol represents an atom of the element in Period 4 with the highest first ionization energy? A B C D Page 12 GO ON 30 Which is the correct electrondot diagram of an atom of sulfur in the ground state? F G H J 31 Which electrondot symbol represents an atom of chlorine in the ground state? A B C D Page 13 GO ON 32 Atom X has an electron configuration of 2−8−2. Which electrondot symbol correctly represents this atom? F G H J 33 Which is the electrondot symbol for an atom with an electron configuration of 2−5? A B C D Page 14 GO ON 34 Which electrondot symbol correctly represents an atom of its given element? F G H J 35 Which Lewis electrondot diagram is drawn correctly for the atom it represents? A B C D Page 15 GO ON 36 Which Lewis electrondot diagram is correct for a S2 ion? F G H J 37 An atom in the ground state contains a total of 5 electrons, 5 protons, and 5 neutrons. Which Lewis electrondot diagram represents this atom? A B C D Page 16 GO ON 38 Which Lewis electrondot diagram represents an atom of a Group 13 element in the ground state? F G H J 39 How does the ground state electron configuration of the hydrogen atom differ from that of a ground state helium atom? A Hydrogen contains a completely filled orbital. B Hydrogen has two electrons in a lower energy level. C Hydrogen contains a halffilled orbital. D Hydrogen has one electron in a higher energy level. Page 17 GO ON 40 Which orbital notation correctly represents the outermost principal energy level of a nitrogen atom in the ground state? F G H J 41 Which is the correct orbital notation for the electrons in the second principal energy level of a beryllium atom in the ground state? A B C D Page 18 GO ON 42 Which orbital notation correctly represents the outermost principal energy level of a sulfur atom in the ground state? F G H J 43 Which is the orbital notation for the electrons in the third principal energy level of an argon atom in the ground state? A B C D Page 19 GO ON 44 In an atom of lithium in the ground state, what is the total number of orbitals that contain only 1 electron? F 4 G 2 H 3 J 45 1 What is the total number of partially occupied 2p orbitals in a nitrogen atom in the ground state? A 2 B 1 C 3 D 5 Page 20 GO ON 46 Which orbital notation represents the valence electrons of a phosphorus atom in the ground state? F G H J 47 The diagram below represents the orbital notation of an atom's valence shell in the ground state. The diagram could represent the valence shell of — A Al. B Cl. C Li. D Si. Page 21 GO ON 48 Which orbital notation correctly represents the outermost principal energy level of a noble gas in the ground state? F G H J 49 Which atom in the ground state has three halffilled orbitals? A Si B Al C Li D P Page 22 GO ON 50 The orbital notation of an atom in the ground state is shown below. Which atom is represented by this notation? F C G Be H N J 51 B Which orbital notation represents a noble gas in the ground state? A B C D Page 23 GO ON 52 What is the electron configuration for Be2+ ions? F 1s2 2s1 G 1s2 2s2 H 1s1 J 53 1s2 A neutral atom of an element has an electron configuration of 2−8−2. What is the total number of p electrons in this atom? A 6 B 12 C 10 D 2 54 Which is the electron configuration of an atom in an excited state? F 1s1 2s1 G 1s2 2s1 H 1s2 2s2 2p2 J 1s2 2s2 2p1 Page 24 GO ON 55 Which sublevel configuration correctly represents a completely filled third principal energy level? A 3s2 3p6 3d8 B 3s2 3p6 3d5 C 3s2 3p6 3d10 D 3s2 3p2 3d10 56 Which electron configuration represents an atom in an excited state? F 1s2 2s2 2p6 4s1 G 1s2 2s1 H 1s2 2s2 2p6 3s2 3p3 J 57 1s2 2s2 2p6 Which is the electron configuration for a neutral atom in the ground state? A 1s2 2s2 2p6 3s1 B 1s2 2s2 2p4 3s1 C 1s2 2s2 3s1 D 1s2 2s2 2p6 3p1 Page 25 GO ON 58 Which is a possible electron configuration for argon in an excited state? F 1s2 2s2 2p7 3s2 3p5 G 1s2 2s2 2p6 3s2 3p5 4s1 H 1s2 2s3 2p5 3s2 3p6 J 59 1s2 2s2 2p6 3s1 3p7 Which electron configuration represents an atom in an excited state? A 1s2 2s2 2p6 B 1s2 2s2 C 1s2 2s2 3s1 D 1s2 2s2 2p6 3s1 60 Which electron configuration represents a potassium atom in an excited state? F 1s2 2s2 2p6 3s2 3p6 4s1 G 1s2 2s2 2p6 3s2 3p3 H 1s2 2s2 2p6 3s1 3p4 J 1s2 2s2 2p6 3s2 3p5 4s2 Page 26 GO ON 61 Which is the electron configuration of an atom in the ground state? A 1s2 2s2 2p5 3s2 B 1s2 2s1 2p2 C 1s2 2s2 2p6 3s1 D 1s2 2s2 3s1 62 In the electrondot symbol the dots represent electrons located in — F s, p, and d sublevels. G p sublevels, only. H s and p sublevels, only. J 63 s sublevels, only. What is the correct electron configuration of an O2 ion? A 1s2 2s2 2p3 B 1s2 2s2 2p2 C 1s2 2s2 2p6 D 1s2 2s2 2p5 Page 27 GO ON 64 Which is the electrondot symbol for an atom with an electron configuration of 1s2 2s2 2p3 ? F G H J 65 Atom X has an electron configuration of 1s2 2s2 2p6 3s2 . Which electrondot symbol correctly represents this atom? A B C D Page 28 GO ON 66 Which is the electron configuration of an element with a completely filled third principal energy level? F [Ar]3d10 4s2 G [Ar]3d8 4s2 H [Ne]3s2 3p6 J 67 [Ne]3s2 Which electron configurations represent the first two elements in Group 17 (7A) of the Periodic Table? A 1s2 2s2 2p5 and [Ne]3s2 3p5 B 1s2 2s1 and 1s2 2s2 C 1s2 2s2 2p6 and [Ne]3s2 3p5 D 1s2 2s2 and 1s2 2s2 2p1 68 An atom with the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 has an incomplete — F 2s sublevel. G 2nd principal energy level. H 3rd principal energy level. J 3s sublevel. Page 29 GO ON 69 If the electron configuration of an atom of element X is 1s2 2s2 2p4 , which of the following is the electrondot symbol for this element? A B C D 70 A Mg2+ ion has the same electron configuration as — F Ar0 . G Na0 . H F . J 71 Ca2+. Which sublevels are occupied in the outermost principal energy level of an argon atom in the ground state? A 2p and 3d B 2s and 3p C 3s and 3p D 3s and 3d Page 30 GO ON 72 Which electron configuration represents an atom in an excited state? F 1s2 3p1 G 1s2 2s2 2p6 H 1s2 2s2 2p5 J 73 1s2 2s2 Which is the electron configuration of a A 1s2 B 1s2 2s1 C 1s2 2s2 H atom in the ground state? D 1s1 74 What is the electron configuration of a fluoride ion (F) in the ground state? F 1s2 2s2 2p4 G 1s2 2s2 2p6 H 1s2 2s2 2p5 J 1s2 2s2 2p7 Page 31 GO ON 75 An atom with the electron configuration 1s2 2s2 2p6 3s2 3p6 3d5 4s2 has an incomplete — A third principal energy level. B 2p sublevel. C 4s sublevel. D second principal energy level. 76 Which electron configuration is possible for a nitrogen atom in the excited state? F 1s2 2s2 2p2 G 1s2 2s2 2p2 3s1 H 1s2 2s2 2p3 J 77 1s2 2s2 2p4 Which is the configuration of an atom in the ground state? A 1s2 2s2 2p6 3p3 B 1s2 2s2 2p6 3s2 C 1s2 2s2 2p5 3s2 D 1s2 2s2 2p5 3p3 Page 32 GO ON 78 An atom in the excited state can have an electron configuration of — F 1s2 2s2 2p6 . G 1s2 2p1 . H 1s2 2s2 . J 79 1s2 2s2 2p5 . What is the electron configuration of a Mn atom in the ground state? A 1s2 2s2 2p6 3s2 3p6 3d5 4s2 B 1s2 2s2 2p6 3s2 C 1s2 2s2 2p6 3s2 3p6 3d7 D 1s2 2s2 2p6 3s2 3p6 3d5 4s1 4p1 80 Which electron configuration represents an atom in the excited state? F 1s2 2s2 2p5 3s1 G 1s2 2s2 2p6 3s1 H 1s2 2s2 2p6 3s2 3p1 J 1s2 2s2 2p6 3s2 Page 33 GO ON 81 Which electron configuration represents an atom of lithium in an excited state? A 1s1 2s2 B 1s1 2s1 C 1s2 2s2 D 1s2 2s1 82 A sample of lead is found to contain 83 Determine the element according to three isotopes: 23.5% of the the mass abundance data in the sample has a mass of 204 amu, table. 24.1% has a mass of 207 amu, and Mass 24 25 26 the remainder has a mass of 208 amu. What is the average atomic mass of lead? F 206.3 amu G 207.2 amu H 206.8 amu J 82.0 amu Page 34 A aluminum B chromium C magnesium Abundance 78.98% 10.03% 11.00% D sodium GO ON 84 The following table shows the mass 85 Boron has the average atomic mass and abundance of three isotopes of of 10.81 and has two naturally element J. Which set up would occurring isotopes. Which isotope of calculate the average atomic mass boron is more abundant? of element J correctly? A Boron10 is more abundant. B Boron11 is more abundant. C Boron10 and boron11 have Isotope A B C F Mass Number (grams) Z Y W Percent Abundance (%) 15 50 35 the same abundance. D There is not enough information to make that determination. 15 + 50 + 35 / 3 = Average atomic mass of J G Mass Z + Mass Y + Mass W / 3 = Average atomic mass of J H (Mass Z x 0.15) + (Mass Y x 0.50) + (Mass W x 0.35) = Average atomic mass of J J 86 What is the average atomic mass of neon? Isotope (Mass Z + 0.15) + (Mass Y + 0.50) + (Mass W +0.35) = Ne‐ 20 Ne‐ 21 Ne‐ 22 Average atomic mass of J F Mass number (grams) 20 21 22 Percent Abundance (%) 90.48 0.27 9.25 10.50 amu G 20.19 amu H 21.00 amu J Page 35 2018.77 amu GO ON 87 Analysis of an unknown element by 90 When given the following mass spectrometry determines that information, what is the molar mass 59.0% of the sample has an atomic of element "J"? mass of 79.0 amu, while the Isotope remainder has a mass of 81.0 amu. What is the average atomic mass of J 26 J 30 J 36 this unknown substance? Record your answer and fill in the F bubbles on your answer document. 88 Percentage (%) 33.3 26.7 40.0 30.7 amu Be sure to use the correct place G 31.1 amu value. H 33.3 amu J Mass Number 26 30 36 3106. amu Of the three isotopes of carbon, C 14 is the rarest, comprising only 0.1% of all carbon atoms. If the average atomic mass of carbon is 12.01 amu and the two remaining 91 There are two common isotopes of isotopes contain 6 and 7 neutrons, lithium: Li6 and Li7. If the average respectively, what is the relative atomic mass of lithium is abundance of carbon13? 6.94 amu, what is the relative abundance of the larger isotope? Record your answer and fill in the Round your answer to the nearest bubbles on your answer document. percent. Be sure to use the correct place value. Record your answer and fill in the bubbles on your answer document. Be sure to use the correct place 89 Two stable isotopes of silver exist, value. the smallest with 60 neutrons. If the average atomic mass of silver is 107.87 amu, how many neutrons does the larger isotope have? Record your answer and fill in the bubbles on your answer document. Be sure to use the correct place value. Page 36 GO ON 92 Isotopic analysis of copper reveals that 24.50% of copper atoms contain 36 neutrons, whereas 75.50% of copper atoms have 34 neutrons. What is the average atomic mass of copper? Report your answer with four significant figures. Record your answer and fill in the bubbles on your answer document. Be sure to use the correct place value. Page 37 GO ON 93 Forty percent of the atoms of an element have a mass of 16 amu. Sixty percent of the atoms have a mass of 18 amu. What is the average atomic mass, in amu, of this element? Record your answer and fill in the bubbles on your answer document. Record your answer and fill in the bubbles on your answer document. Be sure to use the correct place value. 94 The table below gives information about two isotopes of element X. What is the average atomic mass, in amu, of element X? Express your answer to the correct number of significant figures. Record your answer and fill in the bubbles on your answer document. Record your answer and fill in the bubbles on your answer document. Be sure to use the correct place value. Page 38 GO ON 95 A sample of element X contains 90 percent 35 X atoms, 8.0 percent 37 X atoms, and 2.0 percent 38 X atoms. The average atomic mass is closest to — A 38 amu. B 32 amu. C 37 amu. D 35 amu. 96 The average atomic mass of chlorine is 35.5 amu. Which mixture of isotopes (shown as percents) produces this average mass? F 75% 35 Cl and 25% 37 Cl G 75% 12 C and 25% 13 C H 50% 35 Cl and 50% 37 Cl J 97 50% 12 C and 50% 13 C If 75.0% of the atoms of an element each have a mass of 35.0 amu, and 25.0% of the atoms each have a mass of 37.0 amu, what is the average atomic mass of the element? A 35.5 amu B 37.0 amu C 36.0 amu D 35.0 amu Page 39 GO ON 98 Element X has two isotopes. If 72.0% of the element has an atomic mass of 84.9 atomic mass units, and 28.0% of the element has an atomic mass of 87.0 atomic mass units, the average atomic mass of element X is equal to which of the following? F (72.0 − 84.9) × (28.0 + 87.0) G (72.0 + 84.9) × (28.0 + 87.0) H J 99 + (72.0 × 84.9) + (28.0 × 87.0) The average atomic mass of element A is 63.6 atomic mass units. The only naturally occurring isotopes of element A are A63 and A65. What is the percent abundance of A63 in a naturally occurring sample of element A to the nearest whole number percentage? Record your answer and fill in the bubbles on your answer document. Be sure to use the correct place value. Page 40 GO ON 100 A 100.00gram sample of naturally occurring boron contains 19.78 grams of boron10 (atomic mass = 10.01 atomic mass units) and 80.22 grams of boron11 (atomic mass = 11.01 atomic mass units). Which numerical setup can be used to determine the average atomic mass of naturally occurring boron? F G H (0.1978)(10.01) + (0.8022)(11.01) J 101 (0.8022)(10.01) + (0.1978)(11.01) Which value of an element is calculated using both the mass and the relative abundance of each of the naturally occurring isotopes of the element? A Atomic number B Atomic mass C Halflife D Molar volume Page 41 GO ON 102 The atomic mass of titanium is 47.88 atomic mass units. This atomic mass represents the — F weighted average mass of the most abundant isotope of Ti. G total mass of all the protons and neutrons in an atom of Ti. H total mass of all the protons, neutrons, and electrons in an atom of Ti. J 103 weighted average mass of all the naturally occurring isotopes of Ti. The relative abundance of the three most common isotopes of titanium is shown below. Most Common Isotopes of Titanium Based on this data, what is the average atomic mass, in amu, of titanium? A 47.87 B 46.95 C 47.46 D 47.68 Page 42 GO ON 104 When light passes from air to a new medium such as water, the speed of light decreases but the frequency of the light remains constant. If green light has a wavelength of 495 nm in air (c=3.00x10^8 m/s), what will be the wavelength of that light in water where the speed of light is reduced to 2.25x10^8 m/s? F 495 nm G 659 nm H 219 nm J 105 371 nm A particular nuclear process releases a single gamma ray photon with an energy of 4.75x10^14 joules. What is the frequency of this radiation? A 1.43 x 10^5 Hz B 7.17 x 10^19 Hz C 1.39 x 10^20 Hz D 2.15 x 10^28 Hz Page 43 GO ON 106 The energy required to remove an electron from a particular energy level in a hydrogen atom (the ionization energy) is given by the equation below. What is the minimum wavelength of light that is capable of removing an electron from the third energy level of a hydrogen atom? F 242 nm G 365 nm H 821 nm J 107 124 nm On the AM radio dial, frequencies 109 In the Lunar Laser Ranging are measured in kilohertz. What is experiment, a highpower pulsed the approximate wavelength of a laser with a frequency of radio wave from 1030AM on the 5.64x1014 Hz is reflected off a radio dial? small mirror left on the moon's A 2000 to 3000 cm surface by Apollo astronauts. What B 200 to 300 km C 2 to 3 km D 200 to 300 m is the wavelength of this laser light in nanometers? (1nm = 109m) Record your answer and fill in the bubbles on your answer document. 108 The bright red line from the emission spectrum of hydrogen Be sure to use the correct place value. has a wavelength of 657nm. What is the energy, in joules, of a single photon of this light? F 3.03 x 10^19 J G 4.35 x 10^40 J H 3.03 x 10^28 J J 4.56 x 10^14 J Page 44 GO ON 110 A typical cell phone uses 112 The government, through the FCC wavelengths of 0.36 meters. How (Federal Communications much energy does this wave have? Commission), has set rules and F 2.4 X 1034 J guidelines for the use of radio G 5.5 X 1025 J wireless frequency "traffic". A equipment to better control wireless server gives off 3.3 X 10 H 1.1 X 108 J J 24 joules of energy. What is the 8.3X108 J wavelength of this server in meters? F 2.2 X 1057 m G 6.0 X 1052 m 111 A microwave can have a frequency H 5.0 X 109 m of 3.8 X 1010Hz. How much J energy does this microwave give 9.1 X1031 m off in joules? A 5.7 X 1043 J B 1.14 X 1019 J C 2.5 X1023 J D 1.7 X 1044 J 113 Red lights on a traffic light have a frequency of 4.3 X 1015 Hz. What is the red light’s wavelength in meters? A 1.5 X 1049 meters B 7.0 X 108 meters C 1.4 X 107 meters D 1.3 X 1024 meters Page 45 GO ON 114 Radar detectors use radio waves 116 NASA's SWIFT satellite is designed to measure the speed of moving to collect information regarding vehicles. Radar detectors have a long duration gammaray bursts wavelength of 1.8 meters. What is that occur when supernovae, occur the frequency of waves from a in distant galaxies. If SWIFT detects radar detector? a gammaray burst with a F frequency of 3.5x1020 Hz, how 3.7 X 1034 Hz much energy (in picojoules) does G 6.0 X 109 Hz one single photon of this light carry? (1pJ=1012J) H 5.4 X 108 Hz J 1.7 X 108 Hz Record your answer and fill in the bubbles on your answer document. Be sure to use the correct place value. 115 Our Sun (a Class G2 yellow dwarf) emits most of its energy in the visible spectrum, with light of wavelength of 483 nm being the most intense. How much energy does a mole of photons of this light carry? Round your answer to the nearest kilojoule. 117 A local radio station broadcasts a signal that is composed of radio waves with a wavelength of 3.04 meters. Determine the frequency of this signal in megahertz, the same unit used on the FM radio dial. (1MHz = 106 Hz) Record your answer and fill in the bubbles on your answer document. Record your answer and fill in the Be sure to use the correct place bubbles on your answer document. value. Be sure to use the correct place value. Page 46 GO ON 118 A typical microwave oven heats food through a process called dielectric heating; photons of non ionizing radiation are emitted that excite polarized molecules like water and fat. Each photon of light has an energy of 1.62x1024J. What is the wavelength (in mm) of the radiation emitted by a microwave oven? Record your answer and fill in the bubbles on your answer document. Be sure to use the correct place value. Page 47 GO ON 119 How much energy, in Joules, does one microwave with wavelength of 9.0 centimeters carry? A 6.0 × 1033 B 2.2 × 1024 C 2.2 × 1026 D 6.0 × 1035 120 The diagram below represents an excited neon atom emitting a photon, with frequency 4.03 × 1014 hertz (Hz), as one of its electrons moves from an excited state to the ground state. What was the change in energy, in Joules, when the electron moved from the excited state to the ground state? F 2.67 × 1019 G 2.48 × 1015 H 6.63 × 1034 J 7.44 × 107 Page 48 GO ON Directions: Read the information below about the decay of radioactive cobalt60 and answer any questions that follow. An atom of a radioactive isotope of cobalt, 60 Co, typically emits two gamma rays in quick succession when decaying to 60 Ni. These gamma rays predictably have the following frequencies. Frequency of first emitted gamma ray = 2.82 × 1014 MHz Frequency of second emitted gamma ray = 3.21 × 1014 MHz 121 How much longer is the wavelength of the first gamma ray than the wavelength of the second gamma ray emitted by a radioactive 60 Co atom? A 1.26 × 1013 meters B 1.26 × 107 meters C 8.28 × 1013 meters D 8.28 × 107 meters Page 49 GO ON 122 What is the difference in energy, in megaelectron volts (MeV), between the second and first gamma ray emitted by a cobalt60 atom? 1 eV = 1.60 × 1019 Joules Express your answer to the appropriate number of significant figures. Record your answer and fill in the bubbles on your answer document. Record your answer and fill in the bubbles on your answer document. Be sure to use the correct place value. Directions: The table below shows the most common frequencies of photons released by different metal ion samples when passed through a flame. Use the information in this table to answer any questions that follow. Page 50 GO ON 123 Gabriel performed a flame test on a sample of an unknown salt and observed a yellow flame. Most of the photons emitted by the flame had an approximate wavelength of 590 nanometers. Which metal ion was most likely present in Gabriel's salt sample? A Mn2+ B Zn2+ C Li+ D Na+ 124 Pamela performed a flame test on a sample of an unknown salt and observed a blue flame that emitted many photons with a wavelength of 475 nanometers. Which metal ion was most likely present in Pamela's salt sample? F Li+ G Mn2+ H Zn2+ J Cu+ Page 51 GO ON 125 A chemist performed a flame test on a sample of an unknown metal chloride and observed a red flame. Most of the photons emitted by the sample had a wavelength of 6.8 × 107 meters. Which metal ion was most likely present in the sample? A Mn2+ B Na+ C Li+ D Cu+ 126 A chemist performed a flame test on a sample of an unknown metal nitrate and observed a bluish green flame. Most of the photons emitted by the sample had a wavelength of 5.00 × 107 meters. Which metal ion was most likely present in the sample? F Cu+ G Li+ H Mn2+ J Zn2+ Page 52 GO ON 127 Mediumwave AM radio is broadcast on the frequency band from 520. kHz to 1610 kHz. What is the maximum wavelength of a mediumwave AM radio wave? A 186 m B 1.73 mm C 5.37 mm D 577 m 128 What is the frequency, in megahertz, of an infrared wave with a wavelength of 210 micrometers? F 1.4 × 106 G 1.4 × 1012 H 1.4 × 108 J 129 1.4 × 1014 What is the wavelength, in nanometers, of an Xray with a frequency of 6.0 × 1017 Hz? Express your answer to the appropriate number of significant figures. Record your answer and fill in the bubbles on your answer document. Record your answer and fill in the bubbles on your answer document. Be sure to use the correct place value. Page 53 GO ON 130 What is the frequency, in hertz, of an ultraviolet wave with a wavelength of 3.0 × 108 meters? F 1.0 G 9.0 × 1016 H 1.0 × 1016 J 131 9.0 What is the wavelength of a radio wave with a frequency of 1.2 × 106 Hz? A 4.0 × 103 meters B 3.6 × 102 meters C 3.6 × 1014 meters D 2.5 × 102 meters Page 54 GO ON 132 The energy of violet light is 134 Which of the following waves would approximately twice that of red have the lowest energy? light. How do the wavelengths of F violet and red light compare? F The wavelength of violet light is G sometimes greater than and sometimes less than that of H red light. G The wavelength of violet light is the same as that of red light. J All three waves have the same energy. H The wavelength of violet light is approximately twice that of red light. J 135 Radio station A broadcasts a signal The wavelength of violet light is with a frequency of 98.7 MHz, and approximately half that of red radio station B broadcasts a signal light. with a frequency of 100.3 MHz. What can be said about the 133 As electrons fall from high energy orbitals to lower orbitals, energy is relationship of signal A to signal B? A same energy. released in the form of electromagnetic radiation. The B farther the electron falls, the more energy is released. Which of the following electronic transitions A C B an electron falling from the 3rd Signal A has a shorter wavelength than signal B. D Signal A has a longer wavelength than signal B. an electron falling from the 6th to the 2nd energy level Signal A has more energy than signal B. would produce a wave with the lowest frequency? Signal A and signal B have the E Signal A and signal B have the same wavelength. to the 2nd energy level C an electron falling from the 5th to the 2nd energy level D an electron jumping from the 1st to the 2nd energy level Page 55 GO ON 136 Which of the following choices lists 138 Which two factors of the electromagnetic radiation in order electromagnetic radiation have an from shortest wavelength to inverse relationship? longest wavelength? F F G energy and frequency Xrays, microwaves, visible light, infrared amplitude and nodes H frequency and wavelength G Xrays, visible light, infrared, J microwaves wavelength and energy H microwaves, infrared, visible light, Xrays J infrared, visible light, microwaves, Xrays 139 Different types of waves are found in the electromagnetic spectrum. 137 Wave A and wave B are similar waves that are being compared. If the wavelength in wave B is List the waves in order of increasing wavelengths. A gamma rays, Xray, ultraviolet doubled, how would its frequency waves, infrared, microwaves, change? and radio waves A Wave B's frequency would be B infrared, gamma rays, doubled. B C ultraviolet waves, and Xray Wave B's frequency would be cut in half. Wave B's frequency would be multiplied by a factor of four. D Wave B's frequency would be cut by a fourth. radio waves, microwaves, C infrared, ultraviolet waves, microwaves, radio waves, gamma rays, and Xray D ultraviolet waves , Xray, gamma rays, infrared, microwaves, and radio waves Page 56 GO ON 140 What is the electromagnetic spectrum? F It is the range of wavelengths and frequencies that can be detected by the human eye. G It is a measure of the absorption of radiation as a function of frequency or wavelength. H It is a range containing all of the possible frequencies and wavelengths of electromagnetic radiation. J It is a spectrum of frequencies of electromagnetic radiation emitted by the element's atoms when they are returned to a lower energy state. Page 57 GO ON 141 Two photons of electromagnetic radiation, A and B, are propagating in a vacuum. If photon A is less energetic than photon B, which of the following is true? A A has higher frequency and longer wavelength than B. B A has higher frequency and shorter wavelength than B. C A has lower frequency and longer wavelength than B. D A has lower frequency and shorter wavelength than B. 142 Electromagnetic radiation propagates at a speed of 3.0 × 108 meters per second — F in all mediums. G only if it is in the form of gamma rays. H only if it is in the form of visible light. J 143 in a vacuum. Visible light occupies the range of wavelengths from 380 to 790 nanometers in the electromagnetic spectrum. Which of the following kinds of electromagnetic radiation has shorter wavelength than visible light? A Infrared radiation B Microwaves C Radio waves D Xrays Page 58 GO ON 144 Due to the Doppler Effect, waves from an approaching source (moving toward the observer) are observed as having a shorter wavelength than when they were emitted. Which of the following pairs could represent the kind of radiation emitted from a source rapidly approaching Earth and the kind of radiation it is detected as on Earth? F Emitted as yellow light, observed as blue light G Emitted as a gamma ray, observed as ultraviolet light H Emitted as a microwave, observed as a radio wave J 145 Emitted as ultraviolet light, observed as infrared radiation Due to the Doppler Effect, waves from a receding source (moving away from the observer) are observed as having a longer wavelength than when they were emitted. Which of the following pairs could represent the kind of radiation emitted from a source moving away from Earth and the kind of radiation it is detected as on Earth? A Emitted as yellow light, observed as ultraviolet light B Emitted as a radio wave, observed as infrared radiation C Emitted as an Xray, observed as a gamma ray D Emitted as red light, observed as a microwave Page 59 GO ON 146 Which graph most accurately displays the relationship between the energy and frequency of a photon? Page 60 GO ON F G H J Page 61 GO ON Page 62 GO ON 147 Which graph correctly displays the relationship between wavelength, in meters, and frequency, in hertz, in the electromagnetic spectrum? A B C Page 63 GO ON D Page 64 BE SURE YOU HAVE RECORDED ALL OF YOUR ANSWERS ON YOUR ANSWER DOCUMENT STOP
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