Test Bank For Chemistry: An Atoms First Approach, 2Nd Edition By Steven S. Zumdahl | Complete Chapter 1-21

Chapter 1 - Chemical Foundations 1. Consider the element indium, atomic number 49, atomic mass 114.8 g. The nucleus of an atom of indium-112 contains: a. 49 protons, 63 neutrons, 49 electrons. b. 49 protons, 49 neutrons. c. 49 protons, 49 alpha particles. d. 49 protons, 63 neutrons. e. 49 protons, 112 neutrons. ANSWER: d POINTS: 1 2. A hypothetical element consists of two isotopes of masses 78.95 amu and 80.95 amu with abundances of 32.9% and 67.1%, respectively. What is the average atomic mass of this element? a. 79.95 amu b. 78.95 amu c. 79.6 amu d. 80.3 amu e. 80.95 amu ANSWER: d POINTS: 1 3. Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.23% abundance), X-29 (28.976 amu, 4.67% abundance), and X-30 (29.974 amu, 3.10% abundance). Calculate the atomic weight of X. a. 28.09 amu b. 48.63 amu c. 27.16 amu d. 28.97 amu e. 86.93 amu ANSWER: a POINTS: 1 4. The atomic mass of rhenium is 186.2. Given that 37.1% of natural rhenium is rhenium-185, what is the other stable isotope? a. b. c. d. e. ANSWER: b POINTS: 1 5. Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.23% abundance), X-29 Copyright Cengage Learning. Powered by Cognero. Page 1 Chapter 1 - Chemical Foundations (28.976 amu, 4.67% abundance), and X-30 (29.974 amu, 3.10% abundance). What is the identity of element X? a. Cu b. Al c. Ni d. Si e. Sr ANSWER: d POINTS: 1 6. What is the mass of 6 atom(s) of copper in grams? a. 381.3 g b. 1.58 × 1021 g c. 6.38 × 10–24 g d. 6.022 × 1023 g e. 6.33 × 10–22g ANSWER: e POINTS: 1 7. You have a sample of zinc (Zn) and a sample of aluminum (Al). You have an equal number of atoms in each sample. Which of the following statements concerning the masses of the samples is true? a. The mass of the zinc sample is more than twice as great as the mass of the aluminum sample. b. The mass of the zinc sample is more than the mass of the aluminum sample, but it is not twice as great. c. The mass of the aluminum sample is more than twice as great as the mass of the zinc sample. d. The mass of the aluminum sample is more than the mass of the zinc sample, but it is not twice as great. e. The masses of each sample are equal. ANSWER: a POINTS: 1 8. has _____. a. 20 protons, 20 neutrons, and 18 electrons b. 22 protons, 20 neutrons, and 20 electrons c. 20 protons, 22 neutrons, and 18 electrons d. 22 protons, 18 neutrons, and 18 electrons e. 20 protons, 20 neutrons, and 22 electrons ANSWER: a POINTS: 1 9. Which of the following statements is (are) true? a. and have the same number of neutrons. b. and are isotopes of each other because their mass numbers are the same. Copyright Cengage Learning. Powered by Cognero. Page 2 Chapter 1 - Chemical Foundations c. has the same number of electrons as . d. A and B e. A and C ANSWER: e POINTS: 1 10. A species with 12 protons and 10 electrons is _____. a. Ne2+ b. Ti2+ c. Mg2+ d. Mg e. Ne2– ANSWER: c POINTS: 1 11. The numbers of protons, neutrons, and electrons in K + are: a. 20 p, 19 n, 19 e. b. 20 p, 19 n, 20 e. c. 19 p, 20 n, 20 e. d. 19 p, 20 n, 19 e. e. 19 p, 20 n, 18 e. ANSWER: e POINTS: 1 12. An ion is formed: a. by either adding or subtracting protons from the atom. b. by either adding or subtracting electrons from the atom c. by either adding or subtracting neutrons from the atom. d. all of the above are true. e. two of the above are true. ANSWER: b POINTS: 1 13. All of the following are true except: a. ions are formed by adding electrons to a neutral atom. b. ions are formed by changing the number of protons in an atom's nucleus. Copyright Cengage Learning. Powered by Cognero. Page 3 Chapter 1 - Chemical Foundations c. ions are formed by removing electrons from a neutral atom. d. an ion has a positive or negative charge. e. metals tend to form positive ions. ANSWER: b POINTS: 1 14. The formula of water, H2O, suggests: a. there is twice as much mass of hydrogen as oxygen in each molecule. b. there are two hydrogen atoms and one oxygen atom per water molecule. c. there is twice as much mass of oxygen as hydrogen in each molecule. d. there are two oxygen atoms and one hydrogen atom per water molecule. e. none of these. ANSWER: b POINTS: 1 15. NaHCO3 is the active ingredient in baking soda. How many grams of oxygen are in 0.33 g of NaHCO3? a. 0.063 g b. 0.012 g c. 3.93 × 103 g d. 0.021 g e. 0.19 g ANSWER: e POINTS: 1 16. Phosphorus has the molecular formula P4, and sulfur has the molecular formula S8. How many grams of phosphorus contain the same number of molecules as 4.26 g of sulfur? a. 2.06 g b. 0.486 g c. 4.11 g d. 4.26 g e. none of these ANSWER: a POINTS: 1 17. What is the subscript of barium in the formula of barium phosphate? a. 3 b. 4 c. 1 d. 0 e. 2 ANSWER: a Copyright Cengage Learning. Powered by Cognero. Page 4 Chapter 1 - Chemical Foundations POINTS: 1 18. The __________ in a chemical equation represent the number of atoms in a particular molecule or formula unit. ANSWER: subscripts POINTS: 1 Copyright Cengage Learning. Powered by Cognero. Page 5 Chapter 2 - Atomic Structure and Periodicity Chapter_2_Atomic_Structure_and_Periodicity 1. When ignited, a uranium compound burns with a green flame. The wavelength of the light given off by this flame is greater than that of _____. a. red light b. infrared light c. radio waves d. ultraviolet light e. none of these ANSWER: d POINTS: 1 2. Which form of electromagnetic radiation has the longest wavelengths? a. Gamma rays b. Microwaves c. Radio waves d. Infrared radiation e. X-rays ANSWER: c POINTS: 1 3. Which of the following frequencies corresponds to light with the longest wavelength? a. 3.00 × 1013 s –1 b. 4.12 × 105 s –1 c. 8.50 × 1020 s –1 d. 9.12 × 1012 s –1 e. 3.20 × 109 s –1 ANSWER: b POINTS: 1 4. Which of the following are incorrectly paired? a. Wavelength – λ b. Frequency – ν c. Speed of light – c d. Hertz – s–1 e. X-rays – shortest wavelength ANSWER: e POINTS: 1 Copyright Cengage Learning. Powered by Cognero. Page 1 Chapter 2 - Atomic Structure and Periodicity 5. When a strontium salt is ignited, it burns with a red flame. The frequency of the light given off by this flame is greater than _____. a. yellow light b. infrared light c. ultraviolet light d. radio waves e. x-rays ANSWER: b POINTS: 1 6. A line in the spectrum of atomic mercury has a wavelength of 258 nm. When mercury emits a photon of light at this wavelength, the frequency of this light is: a. 8.61 × 10–16 s –1 b. 7.70 × 10–19 s –1 c. 1.16 × 1015 s –1 d. 77.3 s–1 e. none of these ANSWER: c POINTS: 1 7. What is the wavelength of a photon of red light (in nm) whose frequency is 4.58 × 1014 Hz? a. 655 nm b. 1.53 × 106 nm c. 153 nm d. 458 nm e. None of these ANSWER: a POINTS: 1 Copyright Cengage Learning. Powered by Cognero. Page 2 Chapter 2 - Atomic Structure and Periodicity 8. Yellow light can have a wavelength of 576 nm. The energy of a photon of this light is: a. 1.14 × 10–31 J. b. 5.76 × 10–7 J. c. 3.45 × 10–19 J. d. 5.20 × 1014 J. e. 2.90 × 1018 J. ANSWER: c POINTS: 1 9. Which one of the following types of radiation has the shortest wavelength, the greatest energy, and the highest frequency? a. Ultraviolet radiation b. Infrared radiation c. Visible red light d. Visible blue light e. None, because short wavelength is associated with low energy and low frequency, not high energy and high frequency ANSWER: a POINTS: 1 10. What is the energy of a photon of blue light that has a wavelength of 479 nm? a. 4.79 × 10–7 J b. 4.15 × 10–19 J c. 6.26 × 1014 J d. 9.52 × 10–32 J e. 2.41 × 1018 J ANSWER: b POINTS: 1 11. How many of the following is/are incorrect? i. The importance of the equation E = mc 2 is that energy has mass. ii. Electromagnetic radiation can be thought of as a stream of particles called photons. iii. Electromagnetic radiation exhibits wave properties. iv. Energy can only occur in discrete units called quanta. a. 0 b. 1 c. 2 d. 3 e. 4 ANSWER: a POINTS: 1 Copyright Cengage Learning. Powered by Cognero. Page 3 Chapter 2 - Atomic Structure and Periodicity 12. From the following list of observations, choose the one that most clearly supports the following conclusion:electrons have wave properties. a) emission spectrum of hydrogen b) the photoelectric effect c) scattering of alpha particles by metal foil d) diffraction e) cathode "rays" Reference: Ref 2-1 a. observation a b. observation b c. observation c d. observation d e. observation e ANSWER: d POINTS: 1 13. From the following list of observations, choose the one that most clearly supports the following conclusion: electromagnetic radiation has wave characteristics. a) emission spectrum of hydrogen b) the photoelectric effect c) scattering of alpha particles by metal foil d) diffraction e) cathode "rays" Reference: Ref 2-1 a. observation a b. observation b c. observation c d. observation d e. observation e ANSWER: d POINTS: 1 Copyright Cengage Learning. Powered by Cognero. Page 4 Chapter 2 - Atomic Structure and Periodicity 14. From the following list of observations, choose the one that most clearly supports the following conclusion: electrons in atoms have quantized energies. a) emission spectrum of hydrogen b) the photoelectric effect c) scattering of alpha particles by metal foil d) diffraction e) cathode "rays" Reference: Ref 2-1 a. observation a b. observation b c. observation c d. observation d e. observation e ANSWER: a POINTS: 1 15. From the following list of observations, choose the one that most clearly supports the following conclusion: spacing between atoms in a crystal is on the same order as the de Broglie wavelength of accelerated electrons. a) emission spectrum of hydrogen b) the photoelectric effect c) scattering of alpha particles by metal foil d) diffraction e) cathode "rays" Reference: Ref 2-1 a. observation a b. observation b c. observation c d. observation d e. observation e ANSWER: d POINTS: 1 Copyright Cengage Learning. Powered by Cognero. Page 5 Chapter 2 - Atomic Structure and Periodicity 16. Consider an atom traveling at 1% of the speed of light. The de Broglie wavelength is found to be 1.39 × 10– 3 pm. Which element is this? a. H b. Mo c. C d. Ti e. P ANSWER: b POINTS: 1 17. The four lines observed in the visible emission spectrum of hydrogen tell us that: a. The hydrogen molecules they came from have the formula H4. b. We could observe more lines if we had a stronger prism. c. There are four electrons in an excited hydrogen atom. d. Only certain energies are allowed for the electron in a hydrogen atom. e. The spectrum is continuous. ANSWER: d POINTS: 1 18. When a hydrogen electron makes a transition from n = 3 to n = 1, which of the following statements is true? I. Energy is emitted. II. Energy is absorbed. III. The electron loses energy. IV. The electron gains energy. V. The electron cannot make this transition. a. I, IV b. I, III c. II, III d. II, IV e. V ANSWER: b POINTS: 1 Copyright Cengage Learning. Powered by Cognero. Page 6 Chapter 2 - Atomic Structure and Periodicity 19. In Bohr's atomic theory, when an electron moves from one energy level to another energy level more distant from the nucleus: a. Energy is emitted. b. Energy is absorbed. c. No change in energy occurs. d. Light is emitted. e. None of these. ANSWER: b POINTS: 1 20. Which of the following is incorrect? a. The emission spectrum of hydrogen contains a continuum of colors. b. Diffraction produces both constructive and destructive interference. c. All matter displays both particle and wavelike characteristics. d. Niels Bohr developed a quantum model for the hydrogen atom. e. The lowest possible energy state of a molecule or atom is called its ground state. ANSWER: a POINTS: 1 21. Consider the following portion of the energy-level diagram for hydrogen: n = 4 –0.1361 × 10–18 J n = 3 –0.2420 × 10–18 J n = 2 –0.5445 × 10–18 J n = 1 –2.178 × 10–18 J For which of the following transitions does the light emitted have the longest wavelength? Reference: Ref 2-2 a. n = 4 to n = 3 b. n = 4 to n = 2 c. n = 4 to n = 1 d. n = 3 to n = 2 e. n = 2 to n = 1 ANSWER: a POINTS: 1 Copyright Cengage Learning. Powered by Cognero. Page 7 EMAIL ME: For help with report, Assignment, Essay and thesis writing Chapter 2 - Atomic Structure and Periodicity 22. Consider the following portion of the energy-level diagram for hydrogen: n = 4 –0.1361 × 10–18 J n = 3 –0.2420 × 10–18 J n = 2 –0.5445 × 10–18 J n = 1 –2.178 × 10–18 J In the hydrogen spectrum, what is the wavelength of light associated with the n = X to n = 1 electron transition? Reference: Ref 2-2 a. 1.99 × 10–25 nm b. 3.65 × 102 nm c. 8.22 × 106 cm d. 1.63 × 10–18 m e. 1.22 × 10–7 m ANSWER: e POINTS: 1 23. What is the wavelength of light that is emitted when an excited electron in the hydrogen atom falls from n = 5 to n = 4? a. 2.47 × 105 m b. 4.05 × 10–6 m c. 4.90 × 10–20 m d. 1.46 × 10–6 m e. none of these ANSWER: b POINTS: 1 24. The energy of the light emitted when a hydrogen electron goes from n = 2 to n = 1 is what fraction of its ground-state ionization energy? a. 3/4 b. 1/2 c. 1/4 d. 1/8 e. 1/9 ANSWER: a POINTS: 1 Copyright Cengage Learning. Powered by Cognero. Page 8 Chapter 2 - Atomic Structure and Periodicity 25. The wavelength of light associated with the n = 2 to n = 1 electron transition in the hydrogen spectrum is 1.216 × 10–7 m. By what coefficient should this wavelength be multiplied to obtain the wavelength associated with the same electron transition in the Li2+ ion? a. 1/9 b. 1/7 c. 1/4 d. 1/3 e. 1 ANSWER: a POINTS: 1 26. In an investigation of the electronic absorption spectrum of a particular element, it is found that a photon having λ = 500 nm provides just enough energy to promote an electron from the second quantum level to the third. From this information, we can deduce _____. a. the energy of the n = 2 level b. the energy of the n = 3 level c. the sum of the energies of n = 2 and n = 3 d. the difference in energies between n = 2 and n = 3 e. all of these ANSWER: d POINTS: 1 27. Which of the following is a reasonable criticism of the Bohr model of the atom? a. It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus. b. It does not adequately predict the line spectrum of hydrogen. c. It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen. d. It does not adequately predict the ionization energy of the first energy level electrons for one-electron species for elements other than hydrogen. e. It shows the electrons to exist outside of the nucleus. ANSWER: c POINTS: 1 Copyright Cengage Learning. Powered by Cognero. Page 9 Chapter 2 - Atomic Structure and Periodicity 28. Which of the following statements is (are) true? I. An excited atom can return to its ground state by absorbing electromagnetic radiation. II. The energy of an atom is increased when electromagnetic radiation is emitted from it. III. The energy of electromagnetic radiation increases as its frequency increases. IV. An electron in the n = 4 state in the hydrogen atom can go to the n = 2 state by emitting electromagnetic radiation at the appropriate frequency. V. The frequency and wavelength of electromagnetic radiation are inversely proportional to each other. a. II, III, IV b. III, V c. I, II, III d. III, IV, V e. I, II, IV ANSWER: d POINTS: 1 29. Which of the following best describes an orbital? a. Space where electrons are unlikely to be found in an atom b. Space which may contain electrons, protons, and/or neutrons c. The space in an atom where an electron is most likely to be found d. Small, walled spheres that contain electrons e. A single space within an atom that contains all electrons of that atom